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The condensed electron configuration of silicon 14 is

(N3) 3s2 sp2

Place the following in order of increasing standard molar entropy. H2O (l) H2O (g) H2O (s)

(s) < (l) < (g)

Given w = 0, an endothermic reaction has the following.

+ ΔH and +ΔE *

Draw the best Lewis structure for the free radical, NO2. What is the formal charge on the N?

Determine the oxidation state of P in PO3 3-

Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)

+91 V

Draw the best Lewis structure for Cl3-. What is the formal charge on the central CL atom?

-1

What is Δn for the following equation in relating Kc to Kp? 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

-1

A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = ?

-1.24 x 10³ kJ/mol

The combustion of titanium with oxygen produces titanium dioxide: Ti (s) + O2 (g) → TiO2 (s) When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00°C to 91.60°C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is __________ kJ/mol.

-1.52 x 10⁴

The temperature rises from 25.00 °C to 29.00 °C in a bomb calorimeter when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate ΔErxn for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the calorimeter is 4.90 kJ/°C . The molar mass of sugar is 342.3 g/mol.

-1.92 x 10³ kJ/mole

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2 (l) → 2H2O (l) + O2 (g) H = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

-11.5 kJ

When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written. 2 CH4(g) + 3 Cl2(g) → 2 CHCl3(l) + 3 H2(g)

-1420kJ

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O2(g) → 2 HgO(s) P(Hg) = 0.025 atm, P(O2) = 0.037 atm ΔG° = -180.8 kJ

-154.4 kJ

What is Δn for the following equation in relating Kc to Kp? N2(g) + 3 H2(g) 2 NH3(g)

-2

Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L·atm)

-24.1 kJ

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm, P(CO2) = 2.1 atm ΔG°rxn = ?

-25.0 kJ

A 4.98 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 4.25 kJ/°C. If the temperature rose from 29.5°C to 69.8°C, determine the value of ΔH°comb for aniline.

-3.20 x 10³ kJ/mol

Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I(aq)

-3.3 x 102 kJ

Calculate the work, w, gained or lost by the system when a gas expands from 15 L to 40 L against a constant external pressure of 1.5 atm. 101.3 L · atm = 101 J

-3.8 kJ

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m.

-30.0 °C

At constant pressure, the combustion of 15.0 g of C2H6(g) releases 777 kJ of heat. What is ΔH for the reaction given below? 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l).

-3120 kJ

Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.0 25 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00°C to 35.75°C. If the specific heat of the solution is 4.18 J/(g · °C), calculate ΔH for the reaction, as written. 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) ΔH= ?

-360 kJ

In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is __________.

-40.5

When 1.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 33.10°C. If the specific heat of the solution is 4.18 J/(g · °C), calculate ΔH for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g)

-431 kJ

Calculate the change internal energy (ΔE) for a system that is giving off 45.0 kJ of heat and is performing 855 J of work on the surroundings.

-45.9 kJ

A balloon is inflated from 0.0100 L to 0.500 L against an external pressure of 10.00 atm. How much work is done in joules? 101.3 J = 1 L x atm

-496 J

What is △n for the following equation in relating Kc to Kp? P4(s) + 5 O2(g) ⇌ P4O10(s)

-5

Determine ΔG°rxn using the following information. FeO(s) + CO(g) → Fe(s) + CO2(g) ΔH°= -11.0 kJ; ΔS°= -17.4 J/K

-5.8 kJ

A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.00°C and the temperature of the resulting solution was recorded as 37.00°C, determine the ΔH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCl. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water.

-55.7 kJ/mol NaOH

The value of ΔG° at 141.0°C for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3 Cl2 (g) → 2 PCl3 (g) is __________ kJ/mol. At 25.0°C for this reaction, ΔH° is -720.5 kJ/mol, ΔG° is -642.9 kJ/mol, and ΔS° is -263.7 J/K.

-612.3

Use the ΔH°f information provided to calculate ΔH°rxn for the following: ΔH°f (kJ/mol) SO2Cl2(g) -364 H2O(l) -286 HCl(g) -92 H2SO4(l) -814 SO2Cl2 (g) + 2 H2O(l) → 2 HCl(g) + H2SO4(l) ΔH°rxn = ?

-62 kJ

Two solutions, initially at 24.69°C, are mixed in a coffee cup calorimeter (Ccal = 105.5 J/°C). When a 200.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.100 M NaCl solution, the temperature in the calorimeter rises to 25.16°C. Determine the DH°rxn, in units of kJ/mol AgCl. Assume that the density and heat capacity of the solutions is the same as that of water.

-64 kJ/mol AgCl

Phosphorous and chlorine gases combine to produce phosphorous trichloride: P2 (g) + 3 Cl2 (g) → 2PCl3 (g) ΔG° at 298 K for this reaction is -642.9 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.5 atm P2, 1.6 atm Cl2, and 0.65 atm PCl3is __________.

-649.5

Two solutions, initially at 24.60°C, are mixed in a coffee cup calorimeter (Ccal = 15.5 J/°C). When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution, the temperature in the calorimeter rises to 25.30°C. Determine the DH°rxn for the reaction as written below. Assume that the density and heat capacity of the solutions is the same as that of water. NaCl (aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) DH°rxn = ?

-69 kJ

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 3N2O(g) + 3NO2(g) → 9 NO(g)

-69.0 kJ

When 0.455 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is 4.18 J/(g · °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene.

-7060 kJ/mol

Estimate ΔG°rxn for the following reaction at 387 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH°= -158.0 kJ; ΔS°= -219.9 J/K

-72.9 kJ

The value of ΔG° at 100.0 °C for the formation of calcium chloride from its constituent elements: Ca (s) + Cl2 (g) → CaCl2 (s) is __________ kJ/mol. At 25.0°C for this reaction, ΔH° is -795.8 kJ/mol, ΔG° is -748.1 kJ/mol, and ΔS° is -159.8 J/K.

-736.1

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 ml of solution having a density of 1.25 g/ml by 7.80°C? (The specific heat of the solution is 3.74 joules/gramK.)

-9.12 kJ

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O DH = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

-94.6 kJ

A mixture of 1.0 mol Ne and 1.0 mol He at STP in rigid container.

...

Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.

...

Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN.

...

Determine the electron geometry, molecular geometry and polarity of SF6 .

...

Give the approximate bond angle for a molecule with a tetrahedral shape.

...

Give the approximate bond angle for a molecule with a trigonal planar shape.

...

How many subshells are there in the shell with n=4

...

Identify the number of electron groups around a molecule with a tetrahedral shape.

...

Identify the shape that goes with sp3d.

...

List in decreasing boiling point order CH3CH2CH3 Ar CH3CN

...

Look over math problems

...

Place the following in order of increasing strengths of intermolecular forces CH4 CH3CH2CH3 CH3CH3

...

The orbital hybridization of carbon atom in C2H2 is

...

What element is undergoing oxidation in the following reaction Zn + 2AgNo3 → Zn (NO3)2 + 2Ag

...

What period 3 electron has the following ionization energies 1012 1900 2910 2960 6270 22,200

...

Which contains an ionic bond SiF5 NH4NO3 C2Br4 CO2 OCl2

...

Which of the following compounds are insoluble in water NaC2H3O2 SrSo4 BaS AlPO4

...

which of these sets of quantum numbers represents a 4d orbital A) N=4 L=2 ml= 2+ B) N=4 L=3 ml=+3 C) N=4 l=1 ml=0 D) N=4 l=2 ml=+3

...

In the best Lewis structure for NO+ what is the formal charge on the N atom?

Calculate the mole fraction of MgCl2 in an aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.

0.00841

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(g) + H2O(g) ⇌ C2H5OH(g) Kc = 9.0 × 103 [C2H4]eq = 0.015 M [C2H5OH]eq = 1.69 M

0.013 M

Calculate the value of [N2]eq if [H2]eq = 2.0 M, [NH3]eq = 0.5 M, and Kc = 2. N2(g) + 3 H2(g) ⇌ 2 NH3(g)

0.016 M

Calculate the mole fraction of total ions in an aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.

0.0252

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Al(s) Al3+(aq, 0.115 M) Al3+(aq, 3.89 M) Al(s)

0.030 V

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution.

0.0337 M *

Consider the following reaction: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g) A reaction mixture initially contains 0.50 M CH4 and 0.75 M H2S. If the equilibrium concentration of H2 is 0.44 M, find the equilibrium constant (Kc) for the reaction.

0.038

A solution is 0.0433 m LiF. What is the molarity of the solution if the density is 1.10 g/mL?

0.0476 M

Calculate P [NO]eq, if P [NOCl]eq = 0.33 atm, P [Cl2]eq = 0.50 atm, and Kp = 1.9 x 10-2. 2 NOCl(g) 2 NO(g) + Cl2(g)

0.064 atm

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Fe(s) Fe3+(aq, 0.0011 M) Fe3+(aq, 2.33 M) Fe(s)

0.066 V

Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) + SO2(g) A reaction mixture initially contains 0.86 atm NO and 0.86 atm SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118.

0.084 atm

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Cu(s) Cu2+(aq, 0.0032 M) Cu2+(aq, 4.48 M) Cu(s)

0.093 V

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 M, [H2]eq = 1.1 M, [NH3]eq = 0.47 M. N2(g) + 3 H2(g) ⇌ 2 NH3(g)

0.11

Consider the following reaction: 2 H2O(g) + 2 SO2(g) ⇌ 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6.

0.12 M

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0. 45 mol of I2 and 0. 45 mol of Cl2 are initially mixed in a 2.0-L flask?

0.14 M

5) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?

0.145 /44 = 0.00330 moles of CO2 IDK

Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.2 atm. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 M/atm.

0.18 M

At a certain temperature, Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). If a 3.00-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?

0.185 mol

Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O (g)

0.198 g CO2 *

An aqueous solution is 0.387 M in HCl. What is the molality of the solution if the density is 1.23 g/mL?

0.318 m

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 M O2 at 25°C. The Henry's law constant for oxygen in water at 25°C is 1.3 × 10-3 M/atm.

0.32 atm

How many moles of CO are contained in a 5.00 L tank at 155°C and 2.80 atm?

0.399 moles

Calculate the molality of a solution formed by dissolving 27.8 g of LiI in 500.0 mL of water.

0.415 m

Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H2O.

0.454 m

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

0.724 mol O2 *

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

0.74 °C

Consider the following reaction: CO2(g) + C(graphite) ⇌ 2 CO(g) A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO. Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.

0.83 atm

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) Sn2+(aq, 1.8 M) Ag+(aq, 0.055 M) Ag(s)

0.86 V

The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + B(g) ⇌ AB(g) Kc = 0.24 AB(g) + A(g) ⇌ A2B(g) Kc= 3.8 2 A(g) + B(g) ⇌ A2B(g)

0.91

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Sn(s) + 2 Ag(aq) → Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e → Sn(s) Ag(aq) + e → Ag(s) E° = -0.14 V E° = +0.80 V

0.94 V

How many lone pairs of electrons are on the As atom in AsCl3

How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3

How many of the following molecules have sp3 hybridization on the central atom? XeCl4 CH4 SF4 C2H2

What is Δn for the following equation in relating Kc to Kp? N2O4(g) ⇌ 2NO2(g)

What is △n for the following equation in relating Kc to Kp? KClO3 (s) ⇌ KClO (s) + O2(g)

10) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2.

1. Determine which is the limiting reactant. 4.000 mol C8H18 x 16/2 =32 mol CO2 4.000 mol O2 x 16/25=2.56 mol CO2 -Limiting reactant is O2 because it created LESS CO2. 2) Find theoretical yield of CO2: 2.56 mol CO2 x molar mass of CO2= 2.56 x 44=112.64 g 3) Find percent yield: Percent yield=[actual yield/theoretical yield ] x100% Percent yield=[28.16/112.64 ]x100%= 25 %

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) Sn2+(aq, 0.022 M) Ag+(aq, 2.7 M) Ag(s)

1.01 V

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

1.1 x 10⁻⁷²

Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) → ClO(g) + O2(g) ΔG° = - 34.5 kJ

1.12 x 10⁶

How many molecules of CO2 are contained in a 10.0 L tank at 7.53 atm and 485 K?

1.14 × 1024 molecules

Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6). 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ

1.19 x 104 kJ/kg CO₂

How many atoms of exygen are contained in 47.6 g of Al2(CO3)3? The molar mass of the compound is 233.99 g/mol

1.1O x 1O^24 O atoms

Consider the following reaction: CuS(s) + O2(g) ⇌ Cu(s) + SO2(g) A reaction mixture initially contains 2.9 M O2. Determine the equilibrium concentration of O2 if Kc for the reaction at this temperature is 1.5.

1.2 M

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Pb(s) + Br2(l) → Pb2+(aq) + 2 Br(aq) Pb2+(aq) + 2 e → Pb(s) E° = -0.13 V Br2(l) + 2 e → 2 Br(aq) E° = +1.07 V

1.20 V

How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 mL of 0.140 M sucrose solution?

1.21 × 1021 molecules C12H22O11 *

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)

1.3 x 10⁻¹⁶

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3 Cl2(g) + 2 Fe(s) → 6 Cl(aq) + 2 Fe3+(aq) Cl2(g) + 2 e → 2 Cl(aq) Fe3+(aq) + 3 e → Fe(s) E° = +1.36 V E° = -0.04 V

1.40 V

Kc is 1.67 × 1020 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O42-(aq) ⇌ [Fe(C2O4)3]3-(aq). If 0. 0200 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

1.44 x 10⁻²² M

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0 °C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.

1.51 kg

A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

1.65 x 10⁻²

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86°C/m and Kb = 0.512°C/m.

1.65° C

How much energy is required to decompose 765 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful. 4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°rxn = +1207 kJ

1.68 x 10³ kJ

How much energy is required to decompose 765 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful. 4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°rxn = +1207 kJ

1.68 × 103 kJ *

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl)eq = 0.22 atm, P(NO)eq = 0.10 atm, P(Cl2)eq = 0.081 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

1.7 x 10⁻²

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C. What is the specific heat of benzene?

1.72 J/g°C

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PCl5]eq = 0.56 M, [PCl3]eq = 0.23 M, [Cl2]eq = 4.4 M. PCl5(g) ⇌ PCl3(g) + Cl2(g)

1.8

Determine the equilibrium constant for the following reaction at 498 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH° = -304.2 kJ; ΔS° = -414.2 J/K

1.87 x 10¹⁰

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g). 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc=1.7 x 10⁸ [SO2]eq = 0.0034 M [O2]eq = 0.0018 M

1.9 M

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO2(g). NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g) [NH3]eq = 2.9 × 10-3 M Kc = 1.58 × 10-8

1.9 x 10⁻³

10) A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K?

10.2 atm ????

A solution is prepared by dissolving 98.6 g of NaCl in enough water to form 875 mL of solution. Calculate the mass % of the solution if the density of the solution is 1.06 g/mL.

10.6 %

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

10.9 g H2O *

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

10.9 moles H2O *

Using the following equation for the combustion of octane, calculate the amount of moles of oxygen that reacts with 100.0 g of octane. The molar mass of octane is 114.33 g/mole. The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

10.93 moles

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water.

108C

Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water. The vapor pressure of pure water at 55°C is 118.1 torr.

115 torr

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.

12.8 M

What is the approximate bond angle for a molecule with a trigonal planar shape

120

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. CaCO3(s) → CaO(s) + CO2(g) P(CO2) = 0.033 atm ΔG° =+131.1 kJ

122.6 kJ

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. 2 HD(g) ⇌ H2(g) + D2(g) Kc = 0.28 2 H2(g) + 2 D2(g) ⇌ 4 HD(g)

Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K

13.0

The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C. What mass of sucrose (molar mass= 342.30 g/mol) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512°C/m.

130 g sucrose

Determine ΔG°rxn using the following information. CaCO3(s) → CaO(s) + CO2(g) ΔH°= +179.2 kJ; DS°= +160.2 J/K

131.4 kJ

The specific heat capacity of liquid mercury is 0.14 J/gK. How many joules of heat are needed to raise the temperature of 5.00 g of mercury from 15.0°C to 36.5°C?

15 J

A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rises from 25.0 to 62.3°C, determine the heat capacity of the calorimeter. The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = -1235 kJ

15.7 kJ/°C

According to the following thermochemical equation, what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO2. SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ

150 g

How much energy is required to vaporize 158g of butane (C4H10) at its boiling point, if its DHvap is 24.3 kJ/mol

158g x 1mol/58g= 2.72 mol (24.3 kJ/mol)= 66.1kJ

How many orbitals are there in the fourth shell, n=4

Calculate the amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 K to 385.0 K. The specific heat capacity of ethanol is 2.42 J/g°C.

16.6 kJ

Estimate ΔG°rxn for the following reaction at 775 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH°= -304.2 kJ; ΔS°= -414.2 J/K

17 kJ

What mass of CuCl2 is contained in 75.85 g of a 22.4% by mass solution of CuCl2 in water?

17.0 g

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl, if the solution has a density of 1.20 g/mL.

17.5 m

Calculate the mass percent composition of lithium in Li3PO4

17.98%

How much heat is absorbed when 45.00 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation? 5 C(s) + 2 SO2(g) → CS2(l) + 4 CO(g) ΔH° = 239.9 kJ

179.8 kJ

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current? Ag(aq) + e → Ag(s)

19.6 g

According to the following thermochemical equation, what mass of H2O (in g) must form in order to produce 975 kJ of energy? SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ

191 g

Consider the molecule below. Determine the hybridization at each of the 3 labeled atoms.

1=sp2, 2=sp3, 3=sp3

Consider the molecule below. Determine the molecular geometry at each of the 3 labeled atoms.

1=trigonal planar, 2=tetrahedral, 3=trigonal pyramidal

Give the complete electronic configuration for Ca2+

1s2,2s2,2p6,3s2,3p6

Give the complete electronic configuration for Br-

1s2,2s2,2p6,3s3,3p6,4s2,3d1O,4p6

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Fe2+(aq) + K(s) → Fe(s) + K+(aq)

How many of the following molecules are polar? XeO2 SiCl2Br2 C2Br2 SeCl6

How many of the following molecules have sp hybridization on the central atom? C2Cl2 CO2 O3 H2O

How many of the following molecules have sp3d hybridization on the central atom? SiCl4 BrF5 AsF5 BrF3

Identify the number of electron groups around a molecule with sp hybridization

What is Δn for the following equation in relating Kc to Kp? CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g)

Identify the bonding pairs and lone pairs of electrons in water

2 bonding pairs and 2 lone pairs

Identify the number of bonding pairs and lone pairs of electrons in water

2 bonding pairs and 2 lone pairs

A double covalent bond contains _____ of electrons

2 pairs

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [ O2]eq = 4.1 M, [ N2O]eq = 3.3 × 10-18 M. 2 N2(g) + O2(g) ⇌ 2 N2O(g)

2.0 x 10⁻³⁷

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d= 0.792 g/mL) and 387 mL of CH3CH2CH2OH (d= 0.811 g/mL).

2.01 m

What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?

2.02 g

For a process at constant pressure, 49,600 calories of heat are released. This quantity of heat is equivalent to ___ J

2.08 x 10⁵J

Determine the equilibrium constant for the following reaction at 549 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH° = -94.9 kJ; ΔS°= -224.2 J/K

2.08 x 10⁻³

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2 NO2(g) Kc=1.46 2 N2O4(g) ⇌ 4 NO2(g)

2.13

The reaction below has a Kc value of 1.0 × 1012. What is the value of Kp for this reaction at 500 K? 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

2.4 x 10¹⁰

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I(aq)

2.4 x 10⁵⁸

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.

2.41 m

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) / Mg2+(aq, 2.74 M) //Cu2+(aq, 0.0033 M) / Cu(s)

2.62 V

The specific heat capacity of solid copper metal is 0.385 J/gK. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0°C to 77.5°C?

2.66 x 10⁴J

According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol. Fe3O4(s) → 3 Fe(s) + 2 O2(g) ΔH°rxn = +1118 kJ

2.66 x 10⁵ kJ

The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol) solution is 102.5°C. Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512°C/m.

2.7

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq) Mg2+(aq) + 2 e → Mg(s) E° = -2.38 V E° = +0.34 V Cu2+(aq) + 2 e → Cu(s)

2.72 V

How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.60 atm) according to the following reaction? Assume that there is excess Xe.

2.75 × 1023 molecules XeF6

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3 H2O → ICl + HIO3 + 5 HCl

2.78 × 1024 molecules HCl ?

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(CO)eq = 6.8 × 10-11 atm, P(O2)eq = 1.3 × 10-3 atm, P(CO2)eq = 0.041 atm. 2 CO(g) + O2(g) ⇌ 2 CO2(g)

2.8 x 10²⁰

According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO2 if there is plenty of water present? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

2.81 moles NO *

Calculate the amount of heat (in kJ) necessary to raise the temperature of 47.8 g benzene by 57.0 K. The specific heat capacity of benzene is 1.05 J/g°C

2.86 kJ

What pressure will 2.6 x 1023 molecules of H2 exert in a 3.9 L container at 45°C?

2.9 atm

Give the number of valence electrons for CH2Cl2

How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6 Li(s) + N2(g) → 2 Li3N(s)

20.3 g Li3N *

Calculate the molar mass of Al(C2H3O2)3

204.13 g/mol

Give the number of valence electrons for XeI2

22 electrons

Which of the following samples will have the greatest volume at STP?

22 g He

A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 torr, what is the molar mass of the unknown compound?

223 g/mol

Which of the following samples would have the greatest volume? 22g Cl2 22g Ne 22g He 22g O2

22g He

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔGorxn for the following reaction. 3 NO(g) → N2O(g) + NO2(g)

23.0 kJ

Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water. The vapor pressure of pure water at 25°C is 23.8 torr.

23.1 torr

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 23.0°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g · °C), calculate the final temperature of the solution. Ca2+(aq) + 2 F-(aq) → CaF2(s) ΔH° = -11.5 kJ

23.55°C

According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g/mol. B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) ΔH°rxn = -1396 kJ

238 kJ

What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

24.5 g

Consider the following reaction: Xe(g) + 2 F2(g) → XeF4(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2. If the equilibrium pressure of Xe is 0.34 atm, find the equilibrium constant (Kp) for the reaction.

A 4.55 L sample of water contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL.

25.3 ppm

At 1 atm pressure, the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol. To the correct number of significant figures, how much heat is required to melt 4.50 mol of gallium at 1 atm pressure?

27 kJ

Give the number of core electrons for Se

Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 atm.

28.0 K 4

Calculate the mass percent composition of sulfur in Al2(SO4)3

28.12%

1) What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 7.6 L at 3.8 atm?

29 L

A 5.00-g sample of liquid water at 25.0 C is heated by the addition of 84.0 J of energy. The final temperature of the water is __________ °C. specific heat capacity of water is 4.18 J/gK

29.0

Give the number of valence electrons for CH2Cl2

2O valence electrons

How many of the following molecules are polar? PCl5 COS XeO3 SeBr2

How many of the following molecules are polar? XeCl2 COF2 PCl4F SF6

How many unpaired electrons are present in the ground state As atom

What is △n for the following equation in relating Kc to Kp? 2 Na(s) + 2 H2O(l) ⇌ 2 NaOH(aq) + H2(g)

How many bonding pairs and lone pairs of electrons are in N2

3 bonding and 2 lone

A triple covalent bond contains ___ pairs of electrons

3 pairs

Predict the charge that Aluminum would have

For the reaction: N2(g) + 2 O2(g) ⇌ 2 NO2(g), Kc = 8.3 × 10-10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

3.0 x 10¹⁰ M

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. N2O4(g) ⇌ 2 NO2(g) Kc = 1.46 3 N2O4(g) ⇌ 6 NO2(g)

3.11

Nickel can be plated from aqueous solution according to the following half reaction. How long would it take (in min) to plate 29.6 g of nickel at 4.7 A? Ni2+(aq) + 2 e → Ni(s)

3.5 x 10² min

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M, [HI]eq = 5.6 × 10-16 M, [Cl2]eq = 0.0019 M. 2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(g)

3.5 x 10⁻³²

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O (g)

3.50 moles O2 *

A 1.00 L sample of water contains 0.0036 g of Cl ions. Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g/mL.

3.6 ppm

The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 500 K? N2(g) + 3 H2(g) ⇌ 2 NH3(g)

3.6 x 10⁻²

Consider the following reaction: COCl2(g) ⇌ CO(g) + Cl2(g) A reaction mixture initially contains 1.6 M COCl2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 × 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6.

3.7 x 10⁻² M

What mass of NaCl is contained in 24.88 g of a 15.00% by mass solution of NaCl in water?

3.73 g

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

3.95 J/g°C

Using the following equation for the combustion of octane, calculate the amount of grams of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g/mole. The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

307.9 g

A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C.

308 K

A 50.0-g sample of liquid water at 25.0°C is mixed with 29.0 g of water at 45.0°C. The final temperature of the water is __________°C.

32.3

Calculate the change in internal energy (ΔE) for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 24.0 L in volume at 1.00 atm. (Remember that 101.3 J = 1 L·atm)

34.2 kJ

Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K

34.6 kJ

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = -28.0 kJ P(O2) = 0.41 atm, P(O3) = 5.2 atm

341 kJ

For a given reaction, ΔH = -19.9 kJ/mol and ΔS = -55.5 J/Kmol. The reaction will have ΔG = 0 at __________ K. Assume that ΔH and ΔS do not vary with temperature.

359

The specific heat of copper is 0.385 J/(g · °C). If 34.2 g of copper, initially at 24.0°C, absorbs 4.689 kJ, what will be the final temperature of the copper?

380 °C

How many moles of KF are contained in 244 mL of 0.135 m KF solution? The density of the solution is 1.22 g/mL.

4.02 x 10⁻² mol KF

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

4.09 x 10⁻³

What pressure (in atm) will 0.44 moles of CO2 exert in a 2.6 L container at 25°C?

4.1 atm

What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C?

4.1 atm

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

4.1 x 10²kJ

What mass of ethane (CH3CH3) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g/mL.

4.25 g

How many moles of CH3CH2OH are contained in 548 mL of 0.0788 M CH3CH2OH solution?

4.32 × 10-2 mol *

The reaction below has a Kp value of 41. What is the value of Kc for this reaction at 400 K? N2(g) + 3 H2(g) ⇌ 2 NH3(g)

4.4 x 10⁴

Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H2CO3 → H2O + CO2

4.40 g *

The decomposition of ammonia is: 2 NH3(g) → N2(g) + 3 H2(g). If Kp is 1.5 × 103 at 400°C, what is the partial pressure of ammonia at equilibrium when N2 is 0. 10 atm and H2 is 0.15 atm?

4.7 x 10⁻⁴

Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

4.82 x 103 kJ *

4.82 x 10³ kJ

What volume of benzene (C6H6, d= 0.88 g/mL, molar mass = 78.11 g/mol) is required to produce 1.5 x 103 kJ of heat according to the following reaction? 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ

42 mL

The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?

429 J

How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution?

43.83 g *

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M, [I2]eq = 0.39 M, [HI]eq = 1.6 M. H2(g) + I2(g) ⇌ 2 HI(g)

3) How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol.

47.6 g Al2(CO3)3 x (mol Al2(CO3)3 / 233.9 g) x ( 6.0223 x 10^23/ mol Al2(CO3)3) x ( 9 atom O / Al2(CO3)3 atom)

Below what temperature does the following reaction become nonspontaneous? 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔH = +136.5 kJ; ΔS = +287.5 J/K

475 K

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 14.25 kJ/°C. If the initial temperature was 32.9°C, use the information below to determine the value of the final temperature of the calorimeter. 4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 NO2(g) ΔH°rxn= -1.28 x 104 kJ

48.7 °C

How much energy is required to vaporize 48.7g of dichloromethane (CH2CL2) at its boiling point, if its DHvap is 31.6kJ/mol?

48.7g x 1mol/84g = 0.58mol(31.6 kJ/mol) =18.1 kJ

Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm.

49.4 mg

How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

49.7 g O2 *

How many different values of ml are possible in the 2p sub level?

How many signification figures are in 20.300m?

What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5 atm, if the F2 has a volume of 25.0 mL at 1.2 atm?

5.5 mL

Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 M/atm.

5.7 x 10⁻⁴

The reaction below has a Kp value of 3.3 x 10-5. What is the value of Kc for this reaction at 700 K? 2 SO3(g) ⇌ 2 SO2(g) + O2(g)

5.7 x 10⁻⁷

Estimate ΔG°rxn for the following reaction at 449.0 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH°= -94.9 kJ; ΔS°= -224.2 J/K

5.8 kJ

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?

50.0 g Al, C Al =0.903 J/g°C

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed?

54.93 g ?

According to the following reaction, how much energy is evolved during the reaction of 2.50 L B2H6 and 5.65 L Cl2 (Both gases are initially at STP)? The molar mass of B2H6 is 27.67 g/mol. B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) ΔH°rxn = -1396 kJ

58.7 kJ

Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.

59 M/atm

A 6.50-g sample of copper metal at 25.0°C is heated by the addition of 84.0 J of energy. The final temperature of the copper is __________°C. The specific heat capacity of copper is 0.38 J/gK.

59.0

Draw the Lewis structure for SO42-. How many equivalent resonance structures can be drawn?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I2(s) + Fe(s) → Fe3+(aq) + I(aq)

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Mg(s) + Al3+(aq) → Al(s) + Mg2+(aq)

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) ⇌ 2 HBr(g) Kc = 3.8 × 104 4 HBr(g) ⇌ 2 H2(g) + 2 Br2(g)

6.0 x 10⁻¹⁰

How many moles of KF are contained in 347 g of water in a 0.175 m KF solution?

6.07 x 10⁻² mol KF

6.1 x 10⁻⁶

A compound is found to have a molar mass of 598 g/mol. If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C, what is the osmotic pressure of the resulting solution?

6.36 torr

Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K

6.762 x 10³ K

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter. 4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 NO2(g) ΔH°rxn= -1.28 x 104 kJ

6.84 kJ/°C

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4 (g) → 2 NO2 (g) A 1.000-L flask is charged with 3.00 × 10-2 mol of N2O4. At equilibrium, 2.36 × 10-2 mol of N2O4 remains. Keq for this reaction is __________.

6.94 x 10⁻³

Using the following equation for the combustion of octane, calculate the amount of moles of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g/mole. The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

6.997 moles

How much heat is absorbed/released when 35.00 g of NH3(g) reacts in the presence of excess O2(g) to produce NO(g) and H2O(l) according to the following chemical equation? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l) ΔH° = 1168 kJ

600.1 kJ of heat absorbed

Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH = -11.0 kJ; ΔS = -17.4 J/K

632 K

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl3 (g) + Cl2 (g) → PCl5 (g) An equilibrium mixture at 450 K contains PPCl3 = 0.124 atm, PCl2 = 0.157 atm, and PPCl5 = 1.30 atm. What is the value of Kp at this temperature?

66.7

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 9 NO(g) → 3N2O(g) + 3NO2(g)

69.0 kJ

Determine DHsolute for KBr if the DHsolution (KBr) = +19.9 kJ/mol and the ΔHhydration(KBr)=-670. kJ/mol.

690 kJ/mol

Give the valence electrons for Cl

Determine the equilibrium constant for the following reaction at 298 K. SO3(g) + H2O(g) → H2SO4(l) ΔG° = -90.5 kJ

7.31 x 10¹⁵

The Kp for the reaction below is 1.49 × 108 at 100.0°C: CO (g) + Cl2 (g) → COCl2 (g) In an equilibrium mixture of the three gases, PCO = PCl2 = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is __________ atm.

7.34

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.7 × 10⁶ SO3(g) ⇌ 1/2 O2(g) + SO2(g) Kc=X

7.7 x 10⁻⁴

4) Determine the empirical formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen.

70.79 g C * (1 mol C/12.01 g C) = 5.89 mol C 8.91 g H * (1 mol/1.01 g H) = 8.82 mol H 4.59 g N * (1 mol/ 14.0 g N) = 0.328 mol N 15.72 g O * (1 mol/16.0 g O) = 0.983 mol O 5.89 mol C/0.328 = 18 C 8.82 mol H/0.328 = 27 H 0.328 mol N/0.328 = 1 N 0.983 mol O/0.328 = 3 O C18H27O3N = empirical formula

How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ

753 kJ

) How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ

769 kJ

How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ

769 kJ *

The Lewis dot symbol for the chloride ion is

8 dots

The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + 2B(g) ⇌ AB2(g) Kc= 50 AB2(g) + B(g) ⇌ AB3(g) Kc=X A(g) + 3B(g) ⇌ AB3(g) Kc= 478

8.1

An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0. 0100 M O2. At this temperature, Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). What is the equilibrium concentration of CO?

8.4 x 10⁻⁴

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2 SO2 + O2 (g) → 2 SO3 (g) At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is __________ atm.

82.0

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.

82.6°C

The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C?

840 J

A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ/°C. Using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°C. The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = -1235 kJ

85.7 °C

According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)

86.1 mL *

What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385 K?

86.7 g

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g) ⇌ 2 NO2(g) [N2O4]eq = 0.039 M Kc= 0.21

9.0 x 10⁻² M

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution. Calculate the mass % of KBr in the solution if the density is 1.12 g/mL.

9.31%

How many C2H4 molecules are contained in 45.8 mg of C2H4? The molar mass of C2H4 is 28.5 g/mol

9.83 x 1O^2O C2H4 molecules

Using the following thermochemical equation, determine the amount of heat produced from the combustion of 24.3 g benzene (C6H6). The molar mass of benzene is 78.11 g/mole. 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ

977 g C₆H₆

According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)

99.8 g S *

A student is preparing to perform a series of calorimetry experiments. She first wishes to determine the calorimeter constant (Ccal) for her coffee cup calorimeter. She pours a 50.0 mL sample of water at 345 K into the calorimeter containing a 50.0 mL sample of water at 298 K. She carefully records the final temperature of the water as 317 K. What is the value of Ccal for the calorimeter?

99J/K

Estimate the enthalpy change for the reaction 2CO + O2 ® 2CO2 given the following bond energies. BE(CºO) = 1074 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol A) +2380 kJ/mol D) -561 kJ/mol B) +1949 kJ/mol E) -744 kJ/mol C) +744 kJ/mol

= [2(CO) + O2] - [2(CO2)] = 2(1074) + 499 - 4(802) = -561 kJ/mol

1) No two electrons can have the same four quantum number is known as A) Pauli exclusion principle B) Hund's rule C) Aufbau principle D) Heisenberg uncertainty principle

10) Calculate the wavelength (in nm) of a the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz. A) 633 nm B) 158 nm C) 142 nm D) 704 nm E) 466 nm

12) Use Lewis theory to determine the chemical formula for the compound formed between Ca and N. A) Ca3N2 3 B) Ca2N3 C) CaN2 D) CaN

13) Identify the element that has a ground state electronic configuration of [Kr]5s24d5. A) Tc B) Mn C) Nb D) Ru

14) Consider the molecule below. Determine the molecular geometry at each of the 3 labeled atoms. A) 1=trigonal planar, 2=tetrahedral, 3=trigonal pyramidal B) 1=tetrahedral, 2=tetrahedral, 3=tetrahedral C) 1=trigonal planar, 2=tetrahedral, 3=tetrahedral D) 1=tetrahedral, 2=tetrahedral, 3=trigonal planar E) 1=trigonal planar, 2=trigonal pyramidal, 3=trigonal pyramidal

15) Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO2 SeCl6 SeF2 A) SeCl6 < SeF2 < SeO2 B) SeF2 < SeO2 < SeCl6 C) SeF2 < SeCl6 < SeO2 D) SeO2 < SeF2 < SeCl6 E) SeCl6 < SeO2 < SeF2

17) Place the following in order of decreasing magnitude of lattice energy. K2O Rb2S Li2O A) Li2O > K2O > Rb2S B) Li2O > Rb2S > K2O C) Rb2S > K2O > Li2O D) Rb2S > Li2O > K2O E) K2O > Li2O > Rb2S

17) Which of the following occur as the wavelength of a photon increases? A) the frequency decreases B) the energy increases C) the speed decreases D) Planck's constant decreases E) None of the above occur as the wavelength of a photon increases.

19) Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm. A) 4.85 × 10-19 J B) 2.06 × 10-19 J C) 1.23 × 10-19 J D) 8.13 × 10-19 J E) 5.27 x 10-19 J

2) Choose the orbital diagram that represents the ground state of N. A) B) C) D) E)

2) Give the approximate bond angle for a molecule with a tetrahedral shape. A) 109.5° B) 180° C) 120° D) 105°

2) Place the following types of electromagnetic radiation in order of increasing frequency. visible light microwaves X-rays A) microwaves < visible light < X-rays B) X-rays < visible light < microwaves C) microwaves < X-rays < visible light D) X-rays < microwaves < visible light E) visible light < X-rays < microwaves

2) Which of the following represent the Lewis structure for N? A) B) C) D) E)

21) How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3 A) 1 B) 2 C) 3 D) 4 E) 0

22) Choose the compound below that should have the highest melting point according to the ionic bonding model. A) AlN B) MgO C) NaF D) CaS E) RbI

23) How many valence electrons does an atom of Ba possess? A) 2 B) 1 C) 8 D) 6 E) 3

24) Determine the shortest frequency of light required to remove an electron from a sample of Ti metal if the binding energy of titanium is 3.14 × 103 kJ/mol. A) 7.87 x 1015 Hz B) 4.74 x 1015 Hz C) 2.11 x 1015 Hz D) 1.27 x 1015 Hz E) 6.19 x 1015 Hz

24) How many valence electrons does an atom of Ti possess? A) 2 B) 4 C) 6 D) 8 E) 0

25) Which of the following statements is TRUE? A) An ionic bond is much stronger than most covalent bonds. B) An ionic bond is formed through the sharing of electrons. C) Ionic compounds at room temperature typically conduct electricity. D) Once dissolved in water, ionic compounds rarely conduct electricity. E) None of the above are true.

27) Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s. A) 1.99 × 10-10 m B) 5.03 × 10-10 m C) 1.81 × 10-10 m D) 5.52 × 10-9 m E) 2.76 × 10-9 m

27) Determine the electron geometry, molecular geometry and polarity of TeCl6. A) eg=octahedral, mg=octahedral, nonpolar B) eg=trigonal bipyramidal, mg=trigonal bipyramidal, nonpolar C) eg=octahedral, mg=square planar, polar D) eg=trigonal bipyramidal, mg=see-saw, polar E) eg=tetrahedral, mg=trigonal pyramidal, polar

28) Place the following elements in order of increasing electronegativity. Sr N Na A) Sr < Na < N B) Na < N < Sr C) Sr < N < Na D) N < Sr < Na E) N < Na < Sr

3) Choose the valence orbital diagram that represents the ground state of Zn. A) B) C) D) E)

3) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. A) eg=trigonal planar, mg=trigonal planar B) eg=tetrahedral, mg=trigonal planar C) eg=tetrahedral, mg=trigonal pyramidal D) eg=trigonal planar, mg=bent E) eg=trigonal bipyramidal, mg= trigonal bipyramidal

33) Place the following in order of decreasing dipole moment. I. cis-CHCl=CHCl II. trans-CHCl=CHCI III. cis-CHF=CHF A) III > I > II B) II > I > III C) I > III > II D) II > III > I E) I = III > II

33) Place the following in order of increasing radius. Ca2+ S2- Cl- A) Ca2+ < Cl- < S2- B) Cl- < Ca2+ < S2- C) S2- < Cl- < Ca2+ D) Ca2+ < S2-< Cl- E) Cl- < S2- < Ca2+

33) Which of the following transitions (in a hydrogen atom) represent absorption of the smallest frequency photon? A) n = 5 to n = 6 B) n = 5 to n = 4 C) n = 4 to n = 1 D) n = 1 to n = 3 E) n = 1 to n = 2

34) Choose the transition (in a hydrogen atom) below that represents the absorption of the shortest wavelength photon. A) n = 1 to n = 2 B) n = 2 to n = 3 C) n = 4 to n = 5 D) n = 6 to n = 3 E) n = 3 to n = 1

34) Using periodic trends, place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl A) Sb-Cl > As-Cl > P-Cl B) As-Cl > Sb-Cl > P-Cl C) Sb-Cl > P-Cl > As-Cl D) P-Cl > As-Cl > Sb-Cl E) Sb-Cl > P-Cl > As-Cl

37) What are the possible orbitals for n = 3? A) s, p, d B) s, p, d, f C) s D) s, p

38) Identify the shape that goes with sp3d. A) trigonal bipyramidal B) octahedral C) tetrahedral D) trigonal planar

39) A molecule containing a central atom with sp3d2 hybridization has a(n) __________ electron geometry. A) octahedral B) trigonal bipyramidal C) tetrahedral D) trigonal planar E) trigonal pyramidal

4) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom. A) n = 3, l = 1, ml = 1, ms = + B) n = 3, l = 0, ml = 1, ms = - C) n = 3, l = 2, ml =1 , ms = + D) n = 2, l = 1, ml = 1, ms = - E) n = 3, l =2 , ml = 1, ms = -

42) Give the number of valence electrons for XeI2. A) 22 B) 20 C) 18 D) 24

42) How many orbitals are contained in the third principal level (n=3) of a given atom? A) 9 B) 3 C) 18 D) 7 E) 5

44) Draw the Lewis structure for BrF5. What is the hybridization on the Br atom? A) sp3d2 B) sp3d C) sp3 D) sp2 E) sp

45) Choose the diamagnetic species from below. A) Sn2+ B) Br C) P D) Cr E) None of the above are diamagnetic.

46) Which of the following quantum numbers describes the orientation of an orbital? A) magnetic quantum number B) principal quantum number C) angular momentum quantum number D) spin quantum number E) Schrödinger quantum number

48) Choose the best Lewis structure for NO3⁻. A) B) C) D) E)

49) Choose the best Lewis structure for SO42⁻. A) B) C) 12 D) E)

49) Give the ground state electron configuration for Br-. A) [Ar]4s23d104p6 B) [Ar]4s23d104p5 C) [Ar]4s24p6 D) [Ar]4s24d104p6 E) [Ar]4s23d104p4

5) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Sr atom. A) n = 5, l = 0, ml = 0, ms = - B) n = 4, l = 1, ml = 1, ms = - C) n = 5, l = 1, ml = 0, ms = + D) n = 4, l = 1, ml = -1, ms = + E) n = 5, l = 1, ml =1 , ms = -

5) Identify the color that has a wavelength of 460 nm. A) blue B) green C) red D) yellow

50) How many of the following molecules have sp3d hybridization on the central atom? SiCl4 BrF5 AsF5 BrF3 A) 2 B) 0 C) 4 D) 1 E) 3

50) If two electrons in the same atom have the same value of "l", they are A) in the same sublevel, but not necessarily in the same level. B) in the same level, but different sublevel. C) in the same orbital. D) in different levels and in different shaped orbitals. E) None of the above

7) Determine the electron geometry (eg) and molecular geometry (mg) of PF5. A) eg=trigonal bipyramidal, mg=trigonal bipyramidal B) eg=octahedral, mg=octahedral C) eg=trigonal bipyramidal, mg=tetrahedral D) eg=tetrahedral, mg=trigonal pyramidal E) eg=trigonal planar, mg=octahedral

7) Which of the following represent the Lewis structure for S2⁻? A) B) C) D) E)

7) Which of the following statements is TRUE? A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. 3 B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers. D) Two electrons in the same orbital can have the same spin. E) None of the above are true.

8) Give the ground state electron configuration for Se. A) [Ar]4s23d104p4 B) [Ar]4s24d104p4 C) [Ar]4s23d104p6 D) [Ar]4s23d10 E) [Ar]3d104p4

Which response includes all the molecules below that do not follow the octet rule? (1) H2S (2) BCl3 (3) PH3 (4) SF4 A) (2) and (4) B) (2) and (3) C) (1) and (2) D) (3) and (4) E) (1) and (4)

A) (2) and (4)

BeF4 2- is called the fluoberyllate ion. The formal charge on the beryllium atom in this ion is A) -2 B) -1 C) 0 D) +1 E) +2

A) -2 https://www.youtube.com/watch?v=oIEwNZawHeU

The number of lone electron pairs in the NH4 + ion is ___. A) 0 B) 1 C) 2 D) 3 E) 4

A) 0

Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to give a formal charge of zero? A) 0 B) 1 C) 2 D) 3 E) 4

A) 0 https://www.youtube.com/watch?v=ZlHIQhJlWNs

Calculate the value of [N2]eq of [H2]eq = 2.0M, [NH3]eq = 0.5M, and Kc = 2. N2(g) + 3 H2(g) <---> 2 NH3(g) A) 0.016 M B) 0.031 M C) 0.062 M D) 0.40 M E) 62.5 M

A) 0.016 M

The reaction below has a Kp value of 3.3 x 10-5. What is the value of Kc for this reaction at 700 K? 2SO3(g) <--> 2SO2(g) _ O2(g) A) 5.7 x 10-7 B) 1.7 x 106 C) 3.3 x 10-5 D) 3.0 x 104 E) 1.9 x 10-3

A) 5.7 x 10-7

Which of the following is a useful guideline for the application of formal charges in neutral molecules? A) A Lewis structure in which there are no formal charges is preferred. B) Lewis structures with large formal charges (e.g., +2,+3 and/or -2,-3) are preferred. C) The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms

A) A Lewis structure in which there are no formal charges is preferred

Which compound has the longest carbon-carbon bond length?

A) CH2CH2 B) CH3CH3 C) HCCH D) all bond lengths are the same

Which of the following compounds is ethanol?

A) CH3CO2CH3 B) CH3CO2H C) C2H5OH D) C2H6 E) CH3OCH3

section 9.2 1. Which one of the following is most likely to be an ionic compound? A) CaCl2 B) CO2 C) CS2 D) SO2 E) OF2

A) CaCl2

Choose the statement that is true A) Core electrons effectively shield outer electrons from nuclear charge B) Cored electrons are the easiest of all electrons to remove C) Valence electrons are most difficult of all electrons to remove D) Outer electrons efficiently shield one another form the nuclear charge

A) Core electrons effectively shield outer electrons from nuclear charge

In which of the following reactions will Kc = Kp? A) H2(g) + I2(g) <--> 2HI(g) B) CH4(g) + H2O(g) <--> CO(g) + 3H2(g) C) N2O4(g) <--> 2NO2(g) D) CO(g) + 2H2(g) <--> CH3OH(g) E) N2(g) + 3H2(g) <--> 2NH3(g)

A) H2(g) + I2(g) <--> 2HI(g)

For which of these species does the best Lewis structure have two or more equivalent resonance structures? A) HCO2 - B) SCN- C) CNO- D) N3 - E) CO2

A) HCO2

Identify the compound with the highest percent ionic character

A) IBr B) HCl C) HF D) LiF

Identify the compound with the smallest percent ionic character

A) IBr B) HF C) HCl D) LiF

Which of these contains an ionic bond? A) KBr B) Ne C) CO D) H2O E) O2

A) KBr

Which of the following solids would have the lowest melting point? A) KI B) KBr C) KCl D) KF

A) KI

Which one of the following compounds utilizes both ionic and covalent bonding? A) Na2SO4 B) AlCl3 C) PO4 3- D) NH4 + E) CaO

A) Na2SO4

Which of the following solids would have the highest melting point? A) NaF B) NaCl C) NaBr D) NaI

A) NaF

Which of the following ionic solids would have the largest lattice energy? A) SrO B) NaF C) CaBr2 D) CsI E) BaSO4

A) SrO The larger the lattice energy, the more stable the solid and the more tightly held the ions. It takes more energy to melt such a solid, and so the solid has a higher melting point than one with a smaller lattice energy.

Give the direction of the reaction, if K >>1. A) The forward reaction is favored. B) The reverse reaction is favored. C) Neither direction is favored. D) If the temperature is raised, then the forward reaction is favored. E) If the temperature is raised, then the reverse reaction is favored.

A) The forward reaction is favored.

Define electronegativity: A) an atoms ability to attract electrons that are shared in a chemical bond B) an atoms ability to form an ionic bond with another atom C) an atoms ability to donate valence electrons to another atom D) an atoms ability to form a cation E) an atoms ability to form double and triple bonds

A) an atoms ability to attract electrons that are shared in a chemical bond

Classify the Ca — Cl bond in CaCl2 as ionic, polar covalent, or nonpolar covalent. A) ionic B) polar covalent C) nonpolar covalent

A) ionic

A covalent bond is best described as

A) the transfer of electrons B) a bond between two polyatomic ions C) a bond between a metal and a nonmetal D) the sharing of electrons between atoms E) a bond between a metal and a polyatomic ion

Calculate the value of [N2]eq if [H2]eq = 2.0M, [NH3]eq = 0.5M, and Kc = 2. N2(g) + 3H2(g) <--> 2NH3(g) A)0.016 M B) 0.031 M C) 0.062 M D) 0.40 M E) 62.5 M

A)0.016 M

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of CO2 (g). NH2COONH4(s)↔ 2 NH3 (g) + CO2(g) Kc= 1.58×10^-8 [NH3]eq= 2.5×10^-3 A. 2.5×10^-3 M B. 0.053 M C. 4.0×10^-11 M D. 0.022 M E. 6.3×10^-6 M

A. 2.5×10^-3 M

The half- life of the reaction A→B is independent of concentration, it's rate constant is equal to 1.12×10^-3 and the initial concentration of A is 0.100 M. What is the half life in seconds? A. 619 B. 378 C. 37.8 D. 8930 E. 525

A. 619

Identify a homogeneous catalyst. A. H2SO4(aq) with concentrated HCl(aq) B. Pd in H2 gas C. SO2 gas over vanadium oxide D. N2 and H2 gas catalyzed by Fe E. Pt with methane gas

A. H2SO4(aq) with concentrated HCl(aq)

Give the characteristics of a first order reaction having only one reactant. A. The rate of reaction is directly proportional to the concentration of the reactants. B. The rate of the reaction is not proportional to the concentration of the reactant. C. The rate of the reaction is proportional to the square root of the concentration of the reactant. D. The rate of the reaction is proportional to the natural log of the concentration of the reactant. E. The rate of the reaction is proportional to the square of the concentration of the reactant.

A. The rate of the reaction is directly proportional to the concentration of the reactant.

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? ∆H°= +35.9kJ Fe3O4(s) +CO(g) ↔ 3 FeO(s) + CO2(g) A. the reaction will shift to the right in the direction of products. B. the reaction will shift to the left in the direction of the reactants. C. the equilibrium constant will decrease D. the equilibrium constant will increase E. no effect will be observed

A. the reaction will shift to the right in the direction of products

Which substance below has the strongest inter molecular forces?

A2X,DHvap=39.6 kJ/mol Pick the one with the highest Hvap

What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) / Sn2+(aq) // Ag+(aq) / Ag(s)

Ag ⁺ (aq)

What is the oxidizing agent in the redox reaction represented by the following cell notation? Ni(s) / Ni2+(aq) // Ag+(aq) / Ag(s)

Ag⁺ (aq)

Use Lewis theory to determine the chemical formula for the compound formed between Al and O

Al2O3

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Al and F2 in the balanced reaction? Al(s) + F2(g)→ Al3+(aq) + F-(aq)

Al=2, F₂=3

Which of the following processes is endothermic?

An atom absorbs a photon. *

Define an Anion and Cation

Anion- Atom that has gained an electron Cation- Atom that has lost an electron

Place the following in order of decreasing IE1 Cs Mg Ar

Ar> Mg > Cs

Choose the compound below that contains at least one polar covalent bond, but is nonpolar.

AsCl5

Which one of the following exhibits dipole-dipole attraction between molecules?

AsH3

11) Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz. A) 229 nm B) 436 nm C) 206 nm D) 485 nm E) 675 nm

11) Use Lewis theory to determine the chemical formula for the compound formed between Al and O. A) Al3O2 B) Al2O3 C) AlO2 D) Al2O E) AlO

13) Calculate the energy of the green light emitted per photon, by a mercury lamp with a frequency of 5.49 × 1014 Hz. A) 2.75 × 10-19 J B) 3.64 × 10-19 J C) 5.46 × 10-19 J D) 1.83 × 10-19 J E) 4.68 × 10-19 J

15) How many unpaired electrons are present in the ground state P atom? A) 0 B) 3 C) 1 D) 2 E) 4

16) Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF3 OF2 PF4⁺ A) PF3 < OF2 < PF4⁺ B) OF2 < PF3 < PF4⁺ C) OF2 < PF4⁺ < PF3 D) PF4⁺ < OF2 < PF3 E) PF4⁺ < PF3 < OF2

18) Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl A) RbBr > NaF > KCl B) NaF > KCl > RbBr C) KCl > NaF > RbBr D) NaF > RbBr > KCl E) RbBr > KCl > NaF

20) Place the following in order of increasing magnitude of lattice energy. MgO LiI CaS A) CaS < MgO < LiI B) LiI < CaS < MgO C) MgO < CaS < LiI D) LiI < MgO < CaS E) MgO < LiI < CaS

22) How many of the following molecules are polar? XeCl2 COF2 PCl4F SF6 A) 0 B) 3 C) 1 D) 2 E) 4

23) Choose the compound below that should have the highest melting point according to the ionic bonding model. A) SrI2 B) MgF2 C) CaCl2 D) SrF2 E) SrBr2

25) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2. A) eg=tetrahedral, mg=bent, polar B) eg=trigonal planar, mg=bent, polar C) eg=linear, mg=linear, nonpolar D) eg=tetrahedral, mg=tetrahedral, nonpolar E) eg=trigonal pyramidal, mg=trigonal pyramidal, polar

25) Determine the longest wavelength of light required to remove an electron from a sample of potassium metal if the binding energy for an electron in K is 1.76 × 103 kJ/mol. A) 147 nm B) 68.0 nm C) 113 nm D) 885 nm E) 387 nm

28) Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m/s. A) 7.60 × 10-36 m B) 1.32 × 10-34 m C) 2.15 × 10-32 m D) 2.68 × 10-34 m E) 3.57 × 10-32 m

28) Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3. A) eg=trigonal planar, mg=trigonal planar, nonpolar B) eg=tetrahedral, mg=trigonal pyramidal, polar C) eg=trigonal planar, mg=trigonal pyramidal, polar D) eg=trigonal bipyramidal, mg=trigonal planar, nonpolar E) eg=octahedral, mg=tetrahedral, nonpolar

28) How many valence electrons do the alkali metals possess? A) 1 B) 2 C) 7 D) 6 E) 8

3) Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves A) radio waves > microwaves > ultraviolet light B) ultraviolet light > microwaves > radio waves C) radio waves > ultraviolet light > microwaves D) ultraviolet light > radio waves > microwaves E) microwaves > radio waves > ultraviolet light

3) Which of the following represent the Lewis structure for Cl? A) B) C) D) E)

30) Choose the bond below that is most polar. A) C-N B) C-F C) C-O D) C-C E) F-F

30) Choose the compound below that contains at least one polar covalent bond, but is nonpolar. A) HCN B) CF4 C) SeBr4 D) ICl3 E) Both B and C are nonpolar and contain a polar covalent bond.

31) It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen making the assumption that ionization is the transition from n=1 to n=∞. A) -2.18 × 10-18 J B) +2 .18 × 10-18 J C) +4.59 × 10-18 J D) -4.59 × 10-18 J E) +4.36 x 10-18 J

34) Place the following in order of increasing radius. Br- Na+ Rb+ A) Br- < Rb+ < Na+ B) Na+ < Rb+ < Br- C) Rb+ < Br- < Na+ D) Br- < Na+ < Rb+ E) Rb+ < Na+ < Br-

35) Using periodic trends, place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S A) Si-P < Si-Cl < Si-S B) Si-P < Si-S < Si-Cl C) Si-S < Si-Cl < Si-P D) Si-Cl < Si-P < Si-S E) Si-Cl < Si-S < Si-P

35) Which of the following transitions represent the emission of a photon with the largest energy? A) n = 2 to n = 1 B) n = 3 to n = 1 C) n = 6 to n = 3 D) n = 1 to n = 4 E) n = 2 to n = 5

36) Choose the statement that is TRUE. A) Outer electrons efficiently shield one another from nuclear charge. B) Core electrons effectively shield outer electrons from nuclear charge. C) Valence electrons are most difficult of all electrons to remove. D) Core electrons are the easiest of all electrons to remove. 8 E) All of the above are true.

38) What value of l is represented by a d orbital? A) 1 B) 2 C) 0 D) 3

40) Draw the Lewis structure for OF2. What is the hybridization on the O atom? A) sp B) sp3 C) sp2 D) sp3d E) sp3d2

40) Place the following in order of increasing IE1. N F As A) N < As < F B) As < N < F C) F < N < As D) As < F < N E) F < N < As

41) Choose the best Lewis structure for CH2Cl2. A) B) C) D) E)

43) How many sublevels are contained in the second shell (n=2) of a given atom? A) 1 B) 2 C) 9 D) 4 E) 3

45) Draw the Lewis structure for BrCl3. What is the hybridization on the Br atom? A) sp3d2 B) sp3d C) sp3 D) sp2 E) sp

46) Choose the paramagnetic species from below. A) Ti4+ B) O C) Ar D) All of the above are paramagnetic. E) None of the above are paramagnetic.

47) Choose the best Lewis structure for BF3. A) B) C) D) 11 E)

47) Consider the molecule below. Determine the hybridization at each of the 3 labeled atoms. A) 1=sp2, 2=sp3, 3=sp2 B) 1=sp2, 2=sp3, 3=sp3 C) 1=sp3, 2=sp3, 3=sp3 D) 1=sp3, 2=sp3, 3=sp2 E) 1=sp, 2=sp2, 3=sp2

47) How many different values of ml are possible in the 4f sublevel? A) 1 B) 7 C) 3 D) 5 E) 2

50) Give the ground state electron configuration for Mg2+. A) 1s22s22p63s2 B) 1s22s22p6 C) 1s22s22p63s23p2 D) 1s22s22p63s23p6 E) 1s22s22p63s1

6) Give the set of four quantum numbers that represent the last electron added (using the Aufbau principle) to the Zn atom. A) n = 4, l = 3, ml = 3, ms = - B) n = 3, l = 2, ml = 2, ms = - C) n = 3, l = 1, ml = 1, ms = + D) n = 3, l = 3, ml = 2, ms = - E) n = 4, l = 2, ml = 0, ms = +

8) Use Lewis theory to determine the chemical formula for the compound formed between Ca and N. A) CaN B) Ca3N2 C) CaN2 D) Ca2N E) Ca2N3

8) Which of the following types of electromagnetic radiation has the shortest wavelength? A) blue B) violet C) orange D) green E) yellow

9) Determine the electron geometry (eg) and molecular geometry (mg) of BrF3. A) eg=trigonal planar, mg=trigonal planar B) eg=trigonal bipyramidal, mg= T-shape C) eg=trigonal planar, mg=bent D) eg=trigonal bipyramidal, mg=see-saw E) eg=tetrahedral, mg=trigonal pyramidal

9) Give the ground state electron configuration for I. A) [Kr]5s24d105p6 B) [Kr]5s24d105p5 C) [Kr]4d105p6 D) [Kr]5s25p6 E) [Kr]5s25d105p6

What is delta n for the following equation in relating Kc to Kp? 2SO2(g) + O2(g) <--> 2SO3(g) A) 3 B) -1 C) -2 D) 2 E) 1

B) -1

Use bond energies to estimate the enthalpy change for the reaction of one mole ofCH4 with chlorine gas to give CH3Cl and hydrogen chloride. BE(C-H) = 414 kJ/mol BE(C-Cl) = 326 kJ/mol BE(H-Cl) = 432 kJ/mol BE(Cl-Cl) = 243 kJ/mol A) -106 kJ/mol D) +106 kJ/mol B) -101 kJ/mol E) +331 kJ/mol C) +101 kJ/mol

B) -101 kJ/mol

The number of lone electron pairs in the N2 molecule is ___. A) 1 B) 2 C) 3 D) 4 E) 5

B) 2 :N:::N: Two pair. One lone pair on each N

Determine the value of Kp for the following reaction if equilibrium concentrations are as follows: P(CO)eq= 6.8 x 10-11atm, P(O2)eq =1.3 x 10-3atm, P(CO2)eq= 0.041atm 2CO(g) + O2(g) <--> 2CO2(g) A) 3.6 x 10-21 B) 2.8 x 1020 C) 4.6 x 1011 D) 2.2 x 10-12 E) 3.6 x 10-15

B) 2.8 x 1020

The reaction below has a Kc value of 41. What is the value of Kp for this reaction at 500K? N2(g) + 3H2(g) <--> 2NH3(g) A) 2.4 x 10-2 B) 4.4 x 104 C) 41 D) 2.3 x 10-5 E) 1.9 x 104

B) 4.4 x 104

section 9.8 Each of the three resonance structures of NO3 - has how many lone pairs of electrons? A) 7 B) 8 C) 9 D) 10 E) 13

B) 8 resonance structures are just 3 different ways of writing the lewis structure https://www.youtube.com/watch?v=MWDL5WCZBzE

B) 9.0 x 10-2 M

Which one of the following compounds utilizes both ionic and covalent bonding? A) CO3 2- B) Al2(SO4)3 C) CO2 D) C6H12O6 E) MgCl2

B) Al2(SO4)3

Which of the following is a Noble Gas? A) N B) Ar C) K D) O E) Br

B) Ar

Which one of the following molecules has an atom with an expanded octet? A) HCl B) AsCl5 C) ICl D) NCl3 E) Cl2

B) AsCl5 https://www.youtube.com/watch?v=T5BKsjRXUog As has ten octants

Which one of the following is most likely to be an ionic compound? A) NCl3 B) BaCl2 C) CO D) SO2 E) SF4

B) BaCl2

Which of the elements listed below would most likely form a nonpolar covalent bond when bonded to bromine? A) Rb B) Br C) C D) O E) H

B) Br

Arrange the following bonds in order of increasing ionic character B — C C — N C — O C — C

B) C — C < B — C < C — N < C — O

2. Which one of the following is most likely to be an ionic compound? A) ClF3 B) FeCl3 C) NH3 D) PF3 E) SO3

B) FeCl3

9.5 Which of the elements listed below would most likely form a polar covalent bond when bonded to oxygen? A) Mg B) H C) Al D) O E) Na 0.0-0.4 nonpolar 0.5-1.8 polar 1.8 higher ionic

B) H The bond in HF is called a polar covalent bond, or simply a polar bond, because the electrons spend more time in the vicinity of one atom than the other. also they are non metal Experimental evidence indicates that in the HF molecule the electrons spend more time near the F atom

Arrange the elements C, O, and H in order of increasing electronegativity A) C < O < H B) H < C < O C) C < H < O D) O < C < H E H < O < C

B) H < C < O

List all types of bonding present in the ion SO4 2- I. ionic bond II. polar covalent bond III. nonpolar covalent bond A) I only B) II only C) III only D) I and II E) II and III

B) II only

List all types of bonding present in the molecule SO3 I. ionic bond II. polar covalent bond III. nonpolar covalent bond A) I only B) II only C) III only D) I and II E) II and III

B) II only

Express the equilibrium constant for the following reaction. 2CH3Cl(g) + Cl2(g) <---> 2CH2Cl2(g) + H2(g) A) K= [CH2Cl2][H2] / [CH3Cl][Cl2] B) K= [CH2Cl2]2[H2] / [CH3Cl]2[Cl2] C) K= [CH3Cl]2[H2] / [CH2Cl2]2[H2] D) K= [CH3Cl][Cl2] / [CH2Cl2][H2] E) K= [CH3Cl]1/2[Cl2] / [CH2Cl2]1/2[H2]

B) K= [CH2Cl2]2[H2] / [CH3Cl]2[Cl2]

Which one of the following is most likely to be a covalent compound? A) CsOH B) NF3 C) Sr(NO3)2 D) CaO E) LiF

B) NF3

The Lewis structure reveals a double bond in which of the following molecules? A) Br2 B) O2 C) N2 D) H2 E) CH4

B) O2 When oxygen binds with only another oxygen, a double bond (=) forms because both single electrons from both oxygens come together to create 2 bonds between the oxygens.

Arrange the elements F, P, and Cl in order of increasing electronegativity A) F < P < Cl B) P < Cl < F C) Cl < P < F D) P < F < Cl E) Cl < F < P

B) P < Cl < F to the right and up are the most electronegativity

Which of the elements listed below is most likely to exhibit an expanded octet in its compounds? A) O B) S C) Na D) C E) N

B) S

The Lewis dot symbol for the S 2- ion is A) S •• •• : : B) S •• •• : : 2- C) S2- D) —S • • — 2- E) S •• • : —

B) S •• •• : : 2- see pdf u read the group number and add 2 electrons bc of the negative 2

In which of the following reactions will Kc = Kp? A) 4NH3(g) + 3O2(g) <--> 2N2(g) + 6H2O(g) B) SO3(g) + NO(g) <--> SO2(g) + NO2(g) C) 2N2(g) + O2(g) <--> 2N2O(g) D) 2SO2(g) + O2(g) <--> 2SO3(g) E) None of the above reaction have Kc=Kp.

B) SO3(g) + NO(g) <--> SO2(g) + NO2(g)

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? CO2(g) + 2H2O(l) <--> CH4(g) + 2O2(g) delta H= +890kJ A) The reaction will shift to the left in the direction of reactants. B) The equilibrium constant will decrease. C) The equilibrium constant will increase. D) The reaction will shirt to the right in the direction of products. E) No effect will be observed.

B) The equilibrium constant will decrease.

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? C3H8(g) + 5O2(g) <--> 3CO2(g) + 4H20(l) delta H=-2220kJ A) The reaction will shirt to the right in the direction of products. B) The reaction will shift to the left in the direction of reactants. C) The equilibrium constant will increase. D) The equilibrium constant will decrease. E) No effect will be observed.

B) The reaction will shift to the left in the direction of reactants.

Give the direction of the reaction, if K <<1. A) The forward reaction is favored. B) The reverse reaction is favored. C) Neither direction is favored. D) If the temperature is raised, then the forward reaction is favored. E) If the temperature is raised, then the reverse reaction is favored.

B) The reverse reaction is favored.

The electron dot formula for O2 shows A) a single covalent bond D) a total of 8 x 2 = 16 electron dots B) a double covalent bond E) a total of 32 electron dots C) an ionic bond

B) a double covalent bond

Section: 9.3 Complete this statement: Coulomb's law states that the magnitude of the force of interaction between two charged bodies is A) directly proportional to the product of the charges on the bodies and directly proportional to the distance separating them. B) directly proportional to the product of the charges on the bodies, and inversely proportional to the square of the distance separating them. C) inversely proportional to the product of the charges on the bodies, and directly proportional to the square of the distance separating them. D) directly proportional to the sum of the charges on the bodies, and inversely proportional to the square of the distance separating them.

B) directly proportional to the product of the charges on the bodies, and inversely proportional to the square of the distance separating them.

Classify the C — Cl bond in CCl4 as ionic, polar covalent, or nonpolar covalent A) ionic B) polar covalent C) nonpolar covalent

B) polar covalent

Classify the O — H bond in CH3OH as ionic, polar covalent, or nonpolar covalent. A) ionic B) polar covalent C) nonpolar covalent

B) polar covalent

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. 2 SO2(g) +O2(g) → 2 SO3(g) A. -(1/2)∆[SO3]/∆t B. +(1/2)∆[SO3]/∆t C. +2∆[SO3]/∆t D. ∆[SO3]/∆t E. not enough information

B. +(1/2)∆[SO3]/∆t

Calculate the freezing point of a solution of 500.0g of ethylene glycol (C2H6O2) dissolved in 600.0g of water. Kf= 1.86°C/m and Kb= 0.512°C/m. A. 70.2°C B. -25.0°C C. -8.32°C D. -30.0°C E. 8.32°C

B. -25.0°C

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g)↔ I2(g) + Cl2 (g) What is the equilibrium concentration of ICl, if 0.45 mol I2 and 0.45 mol of Cl2 are initially mixed in a 2.0 L flask? A. 0.14 M B.0.27 M C. 0.34 M D. 0.17 M E. none of the above

B. 0.27 M

Determine the boil point of a solution that contains 78.8g of naphthalene (C10H8, molar mass 128.16 g/mol) dissolved in 722 mL (d= 0.877g/mL). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m. A. 2.5°C B. 82.6°C C. 80.4°C D. 2.2°C E. 82.3°C

B. 82.6°C

Which if the following statements is TRUE? A. If Q<K, it means the reverse reaction will proceed to form more reactants. B. If Q=K, it means the reaction is at equilibrium. C. If Q>K, it means the forward reaction will proceed to form more products. D. none of the above E. all of the above

B. If Q=K, it means the reaction is at equilibrium

The scattering of light by collodial dispersion is known as A. Brownian motion B. Tyndall effect C. Micelle repulsion D. an aerosol E. an emulsion

B. Tyndall effect

Place the following substances in order of decreasing vapor pressure at a given temperature. BeF2 CH3OH OF2

BEF2>OF2>CH3OH

Place the following in order of increasing radius Ba2+ Te2- I-

Ba2+ < I- , Te2-

Use the Lewis theory to determine the chemical formula for the compound formed between Ba and N

Ba3N2

What is the difference between bomb calorimetry and coffee cup calorimetry

Bomb calorimetry is performed at constant volume whereas coffee cup is performed at constant pressure

Which contains a pure covalent bond PCl3 SCl6 NaCl Li2CO3 Br2

Br2

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Br2 and OH in the balanced reaction? Br2(l) → BrO3(aq) + Br(aq)

Br₂=3, OH=6

1) Give the approximate bond angle for a molecule with a trigonal planar shape. A) 109.5° B) 180° C) 120° D) 105°

10) Determine the electron geometry (eg) and molecular geometry (mg) of ICl2⁻. A) eg=tetrahedral, mg=bent B) eg=tetrahedral, mg=trigonal pyramidal C) eg=trigonal bipyramidal, mg=linear D) eg=trigonal bipyramidal, mg=trigonal planar E) eg=octahedral, mg=linear

10) Give the ground state electron configuration for Sr. A) [Kr]5s24d2 B) [Kr]5s24d105p2 C) [Kr]5s2 D) [Kr]5s25d105p2 E) [Kr]5s24d10

12) Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm. A) 2.20 × 1014 s-1 B) 1.98 × 1014 s-1 C) 4.55 × 1014 s-1 D) 5.05 × 1014 s-1 E) 3.32 × 1014 s-1

13) Use Lewis theory to determine the chemical formula for the compound formed between K and I. A) KI2 B) K2I C) KI D) K2I2

14) Calculate the energy of the orange light emitted per photon, by a neon sign with a frequency of 4.89 × 1014 Hz. A) 3.09 × 10-19 J B) 6.14 × 10-19 J C) 3.24 × 10-19 J D) 1.63 × 10-19 J E) 5.11 × 10-19 J

14) Identify the element that has a ground state electronic configuration of [Ar]4s23d104p1. A) Al B) In C) Ga D) B

14) Which of the following reactions is associated with the lattice energy of Li2O (ΔH°latt)? A) Li2O(s) → 2 Li⁺ (g) + O2⁻ (g) B) 2 Li⁺ (aq) + O2⁻ (aq) → Li2O(s) C) 2 Li⁺ (g) + O2⁻ (g) → Li2O(s) D) Li2O(s) → 2 Li⁺ (aq) + O2⁻ (aq) E) 2 Li(s) + 1/2O2(g) → Li2O(s)

16) How many unpaired electrons are present in the ground state Kr atom? A) 1 B) 2 C) 0 D) 3 E) 5

17) Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N2O NCl3 NO2⁻ A) NCl3 > NO2⁻ > N2O B) NO2⁻ > N2O > NCl3 C) N2O > NO2⁻ > NCl3 D) NCl3 > N2O > NO2⁻ E) N2O > NCl3 > NO2⁻

18) Write out the orbital diagram that represents the ground state of As. How many unpaired electrons are there? A) 0 B) 4 C) 3 D) 2 E) 1

19) Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS A) MgO < CaO < SrS B) SrS < MgO < CaO C) SrS < CaO < MgO D) CaO < MgO < SrS E) CaO < SrS < MgO

20) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO3. A) eg=tetrahedral, mg=trigonal pyramidal, polar B) eg=tetrahedral, mg=tetrahedral, nonpolar C) eg=trigonal planar, mg=trigonal planar, nonpolar D) eg= trigonal bipyramidal, mg=trigonal planar, polar E) eg=trigonal pyramidal, mg=bent, nonpolar

20) How many of the following elements have 1 unpaired electron in the ground state? B Al S Cl A) 1 B) 2 C) 3 D) 4

20) How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy? A) 3.37 × 1019 photons B) 3.06 × 1030 photons C) 1.80 × 1024 photons D) 4.03 × 1028 photons E) 2.48 × 1025 photons

23) How many of the following molecules are polar? XeO2 SiCl2Br2 C2Br2 SeCl6 A) 1 B) 4 C) 2 D) 3 E) 0

24) Choose the compound below that should have the lowest melting point according to the ionic bonding model. A) LiF B) NaCl C) CsI D) KBr E) RbI

29) Determine the electron geometry, molecular geometry and polarity of HBrO2 . A) eg=trigonal bipyramidal, mg=trigonal planar, nonpolar B) eg=octahedral, mg=square planar, nonpolar C) eg=tetrahedral, mg=bent, polar D) eg=tetrahedral, mg=linear, nonpolar E) eg=linear, mg=linear, polar

29) Determine the velocity of a marble (m = 8.66 g) with a wavelength of 3.46 × 10-33 m. A) 45.2 m/s B) 11.3 m/s C) 22.1 m/s D) 38.8 m/s E) 52.9 m/s

29) Give the complete electronic configuration for Mn. A) 1s22s22p63s23p64s24d5 B) 1s22s22p63s23p64s13d6 C) 1s22s22p63s23p64s23d5 D) 1s22s22p63s23p64s24p5

30) Place the following elements in order of increasing atomic radius. P Ba Cl A) Ba < P < Cl B) P < Cl < Ba C) Cl < P < Ba D) Cl < Ba < P E) Ba < Cl < P

31) Choose the bond below that is most polar. A) H-I B) H-Br C) H-F D) H-Cl E) C-H

31) Choose the compound below that contains at least one polar covalent bond, but is nonpolar. A) GeH2Br2 B) SCl2 C) AsCl5 D) CF2Cl2 E) All of the above are nonpolar and contain a polar covalent bond.

35) Place the following in order of decreasing radius. Te2- F- O2- A) F- > O2- > Te2- B) F- > Te2- > O2- C) Te2- > O2- > F- D) Te2- > F- > O2- E) O2- > F- > Te2-

36) For n = 3 what are the possible sublevels? A) 0 B) 0, 1 C) 0, 1, 2 D) 0, 1,2, 3

36) Which molecule or compound below contains a pure covalent bond? A) Li2CO3 B) SCl6 C) Cl2 D) PF3 E) NaCl

39) Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error? A) n = 2, l = 1 , ml = -1 B) n = 4, l = 2, ml =0 C) n = 3, l =3 , ml = -2 D) n = 1, l = 0, ml =0 E) n = 3, l = 0, ml =0

39) What period 3 element having the following ionization energies (all in kJ/mol)? IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200 A) Si B) S C) P D) Cl E) Mg

4) Identify the color that has a wavelength of 700 nm. A) blue B) green C) red D) yellow

4) Which of the following represent the Lewis structure for Mg? A) B) C) D) E)

41) Draw the Lewis structure for SO3. What is the hybridization on the S atom? A) sp B) sp3 C) sp2 D) sp3d E) sp3d2

41) Place the following in order of decreasing IE1. Cs Mg Ar A) Cs > Mg > Ar B) Mg > Ar > Cs C) Ar > Mg > Cs D) Cs > Ar > Mg E) Mg > Cs > Ar

43) Choose the best Lewis structure for XeI2. A) B) C) D) E)

47) How many of the following species are paramagnetic? Sc3+ Br- Mg2+ Se A) 0 B) 2 C) 1 D) 4 E) 3

48) How many different values of l are possible in the third principal level? A) 1 B) 2 C) 3 D) 0 E) 4

48) How many of the following molecules have sp hybridization on the central atom? C2Cl2 CO2 O3 H2O A) 0 B) 1 C) 2 D) 3 E) 4

50) Choose the best Lewis structure for PO43⁻. A) B) C) D) E)

6) Which of the following visible colors of light has the largest frequency? A) green B) red C) blue D) yellow E) orange

9) Use Lewis theory to determine the chemical formula for the compound formed between Rb and S. A) RbS B) RbS2 C) Rb2S D) Rb2S3 E) Rb3S2

9) Which of the following types of electromagnetic radiation has the smallest frequency? A) yellow B) blue C) orange D) green E) purple

The Lewis structure for CS2 is:

What element is being oxidized in the following redox reaction? MnO4 (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

What is delta n for the following equation in relating Kc to Kp? N2(g) + 3H2(g) <--> 2NH3(g) A) 4 B) -4 C) -2 D) 2 E) 1

C) -2

9.9 What is total number of lone pairs in the best Lewis structure for SOF4 that exceeds the octet rule (S is the central atom)? A) 0 B) 2 C) 14 D) 16 E) 18

C) 14 https://www.youtube.com/watch?v=nzmQkngRGiw

Assuming the octet rule is obeyed, how many covalent bonds will an oxygen atom form to give a formal charge of zero? A) 0 B) 1 C) 2 D) 3 E) 4

C) 2

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq= 3.6M, [O2]eq= 4.1M, [N2O]eq= 3.3 x 10-18M. 2N2(g) + O2(g) <--> 2N2O(g) A) 2.2 x 10-19 B) 4.5 x 1018 C) 2.0 x 10-37 D) 5.0 x 1036 E) 4.9 x 10-17

C) 2.0 x 10-37

Determine the value of Kc for the following raction if the equilibrium concentrations are as follows: [H2]eq = 0.14M, [I2]eq = 0.39M. [HI]eq = 1.6M. H2(g) + I2(g) <--> 2HI(g) A) 2.1 x 10-2 B) 29 C) 47 D) 3.4 x 10-2 E) 8.7 x 10-2

C) 47

Calculate the energy change for the reaction K(g) + Br(g) ->K+(g) + Br- (g) A) -1,092 kJ/mol D) 1,092 kJ/mol B) -95 kJ/mol E) 1,187 kJ/mol C) 95 kJ/mol

C) 95 kJ/mol You need two reactions K(g) ----> K+(g) + e- IE = 419 kJ/mol Br(g) + e- ----> Br-(g) EA = -324 kJ/mol (this releases energy) 419-324=95

Which of the following covalent bonds is the most polar (i.e., highest percent ionic character)? A) Al — I B) Si — I C) Al — Cl D) Si — Cl E) Si — P

C) Al — Cl

Arrange the elements Ba, Br, and Ga in order of increasing electronegativity A) Ba < Br < Ga D) Ga < Ba < Br B) Br < Ga < Ba E) Ga < Br < Ba C) Ba < Ga < Br

C) Ba < Ga < Br

Which one of these polar covalent bonds would have the greatest percent ionic character? A) H — Br B) H — Cl C) H — F D) H — I

C) H — F ionic bonds have electronegative greater then 2.0 H-F are the highest of the polar covalents An ionic bond forms when the electronegativity difference between the two bonding atoms is 2.0 or more. This rule applies to most but not all ionic compounds. Sometimes chemists use the quantity percent ionic character to describe the nature of a bond

Arrange the following bonds in order of increasing ionic character H — Cl C — H H — H O — H A) H — Cl < C — H < H — H < O — H B) H — H < C — H < O — H < H — Cl C) H — H < C — H < H — Cl < O — H D) C — H < O — H < H — Cl < H — H E) C — H < H — Cl < O — H < H — H

C) H — H < C — H < H — Cl < O — H

List all types of bonding present in the molecule S8 I. ionic bond II. polar covalent bond III. nonpolar covalent bond A) I only B) II only C) III only D) I and II E) II and III

C) III only

Which of the following statements is TRUE? A) If Q< K, it means the reverse reaction will proceed to form more reactants. B) If Q >K, it means the forward reaction will proceed to form more products. C) If Q = K, it mean the reaction is at equilibrium. D) All the above are true. E) None of the above are true.

C) If Q = K, it mean the reaction is at equilibrium.

Which of the following ionic solids would have the largest lattice energy? A) KF B) KI C) LiF D) LiI E) NaF

C) LiF

Which of the following solids would have the highest melting point? A) NaI B) NaF C) MgO D) MgCl2 E) KF

C) MgO

The Lewis structure reveals a triple bond in which of the following molecules? A) Br2 B) O2 C) N2 D) H2 E) CH4

C) N2 A step-by-step explanation of how to draw the N2 Lewis Dot Structure (Nitrogen Gas). For the N2 Lewis structure, calculate the total number of valence electrons for the N2 molecule (N2 has 10 valence electrons

The Lewis structure reveals an unpaired electron (free radical) in which of the following species A) NO3 - B) N2O C) NO2 D) NO2 - E) HNO3

C) NO2

Arrange the following bonds in order of increasing ionic character C — F O — F H — F Na — F A) C — F < O — F < H — F < Na — F B) C — F < H — F < O — F < Na — F C) O — F < C — F < H — F < Na — F D) H — F < C — F < O — F < Na — F E) Na — F < H — F < C — F < O — F

C) O — F < C — F < H — F < Na — F

Which one of the following compounds does not follow the octet rule? A) NF3 B) CF4 C) PF5 D) AsH3 E) HCl

C) PF5 https://www.youtube.com/watch?v=aqDYtjhSdBE

What type of chemical bond holds the atoms together within a water molecule? A) Ionic bond C) Polar covalent bond B) Nonpolar covalent bond D) Coordinate covalent bond

C) Polar covalent bond

Which of these is a Chemical property? A) Less dense than air B) Gaseous at room temperature C) Reacts explosively with oxygen D) Colorless E) Tasteless

C) Reacts explosively with Oxygen

Which one of the following is most likely to be a covalent compound? A) KF B) CaCl2 C) SF4 D) Al2O3 E) CaSO4

C) SF4

Which of the following is true A) dispersion forces are generally stronger than dipole dipole forces B) Hydrogen bonds are stronger than covalent bonds C) Vapor pressure increases with temperature D) Intermolecular forces hold the atoms in molecules together

C) Vapor pressure increases with temperature

Which of these is a property of a gas A) constant shape B) constant volume C) easily compressed D) high density

C) easily compressed

Express the equilibrium constant for the following reaction. 16 CH3Cl(g)+ 8 Cl2(g)↔ 16 CH2Cl2(g)+8H2(g) A. K=[CH2Cl2][H2]/[CH3Cl][Cl2] B. K=[CH3Cl][Cl2]/[CH2Cl2][H2] C. K=[CH2Cl2]^16 [H2]^8 / [CH3Cl]^16 [Cl2]^8 D. K=[CH3Cl]^16 [Cl2]^8 / [CH2Cl2]^16 [H2]^8

C. K=[CH2Cl2]^16 [H2]^8 / [CH3Cl]^16 [Cl2]^8

What is the overall rate law for the three step mechanism? Cl2(g)↔ 2 Cl(g) fast Cl(g) + CHCl3(g)→HCl(g) + CCl3(g) slow Cl(g) +CCl3(g)→CCl4(g) fast A. k[Cl2][CHCl3] B. k[Cl][CHCl3] C. k[Cl2]^1/2 [CHCl3] D. k [Cl2][CHCl3)^1/2 E. none of the above

C. k[Cl2]^1/2 [CHCl3]

Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.

C1 = bent, C2 = trigonal planar

Consider the molecule below. Determine the hybridization at each of the 2 labeled carbons.

C1 = sp2, C2 = sp3

Determine the molecular formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen

C18H27NO3

Estimate the enthalpy change for the combustion of one mole of acetylene, C2H2, to form carbon dioxide and water vapor. BE(C-H) = 456 kJ/mol BE(CºC) = 962 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol BE(O-H) = 462 kJ/mol

C2H2 + (5/2)O2 → 2CO2 + H2O 962 + (2)(456) + (5/2)499 = (2)(2)(802) + (2)(462) + E E = - 1,010.5 kJ/mol ≈ - 1,010 kJ/mol

Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145. mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?

C3H6O

In which of the following molecules is hydrogen bonding likely to be the most significant compound of the total inter-molecular forces? CH4 C5H11OH C6H13NH2 CH3OH CO2

C6H13NH2

Determine the molecular formula of a compound that is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen. The molecular weight is 194.19 g/mol

C8H1ON4O2

Choose the compound that contains at least one polar covalent bond but is nonpolar. ICl3 HCN SeF4 CCl4

CCl4

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

CCl₄ kb=29.9°C/m

Choose the bond that is the most polar NO CN ClCl CF CC

Choose the compound below that contains at least one polar covalent bond, but is nonpolar.

CF4

Place the following in order of decreasing strength of intermolecular forces CH3CH2CH2CH2CH2CH3 (CH3)3 CCH3 (CH3)3CCH2CH3

CH3CH2CH2CH2CH2CH3 > (CH3)3CCH2CH3 > (CH3)3 CCH3

Which of the following exhibits hydrogen bonding CH3I CH3NH2 CH3OCH3 HBr

CH3NH2

Which one of the following substances will have a hydrogen bonding as one of its intermolecular forces?

CH3NH2

Choose the one that exhibits hydrogen boning as its strongest C2H6 CH2Br2 CH3OH SBr2

CH3OH

Of the following substances, only_______ has London dispersion forces as its only intermolecular force CH3OH NH3 H2S CH4 HCL

CH4

Which of the following processes have a ΔS > 0?

CH₄(g) +H₂O(g) → CO(g) +3H₂

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

CL2- because dispersion

Place the following in order of increasing molar entropy at 298 K. NO CO SO

CO < NO < SO

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS2 CF4 SCl2

CS2 > CF4 > SCl2

Determine which of these following pairs of reactants will result in a spontaneous reaction at 25°C.

Ca(s) + Mg2+(aq)

What is the formula for calcium phosphate?

Ca3(PO4)2

What element is defined by the following information? Protons-20 Neutrons-10 Electrons-20

Calcium

Global warming is thought to be caused by an increase of what gas?

Carbon Dioxide

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cd and Ag+ in the balanced reaction? Cd(s) + Ag+(aq) → Ag(s) + Cd2+(aq)

Cd=1, Ag=2

Which Gas Law refers to the relationship between volume and temperature

Charles

The volume of a gas is proportional to the temperature of a gas is known as

Charles's Law

What element is being reduced in the following redox reaction? Cr(OH)4(aq) + ClO(aq) → CrO42-(aq) + Cl(aq)

What element is being reduced in the following redox reaction? H2O2(l) + ClO2(aq) → ClO2(aq) + O2(g)

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of ClO2 and H2O in the balanced reaction? H2O2(l) + ClO2(aq) → ClO2(aq) + O2(g)

ClO₂=2, H₂O=2

What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) / Fe3+(aq) // Cl2(g) / Cl(aq) Pt

Cl₂ (g)

Place the following in order of decreasing molar entropy at 298 K. H2 Cl2 F2

Cl₂ < F₂ < H₂

19) Determine the volume of H2S (at 375 K and 1.20 atm) needed to produce 55.0 g of S. Assume that there is excess SO2 present. 2 H2S(g) + SO2(g) 3 S(s) + 2 H2O(g)

Conversions to find (n) number of moles 55gS/32.07= 1.175 because its a 3/2 ratio in the equation 1.175/1.5= 1.143 moles pv=nRt v=nRt/p v=(1.143)(.08206)(375)/1.2= 29.3L

What element is being oxidized in the following redox reaction? Cr(OH)4(aq) + ClO(aq) → CrO42-(aq) + Cl(aq)

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cr(OH)4 and ClO in the balanced reaction? Cr(OH)4(aq) + ClO(aq) → CrO42-(aq) + Cl(aq)

Cr(OH)₄=2, ClO=3

Write the formula for copper (II) sulfate pentahydrate

CuSO4 5H2O

10) Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br. A) MgBr B) Mg2Br3 C) Mg3Br2 D) MgBr2 E) Mg2Br

11) Determine the electron geometry (eg) and molecular geometry (mg) of XeF2. A) eg=trigonal bipyramidal, mg=bent B) eg=linear, mg=linear C) eg=tetrahedral, mg=linear D) eg=trigonal bipyramidal, mg=linear E) eg=tetrahedral, mg=bent

11) Give the ground state electron configuration for Pb. A) [Xe]6s26p2 B) [Xe]6s25d106p2 C) [Xe]6s25f146d106p2 D) [Xe]6s24f145d106p2 E) [Xe]6s25f145d106p2

13) Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons. A) C1 = tetrahedral, C2 = linear B) C1 = trigonal planar, C2= bent C) C1 = bent, C2 = trigonal planar D) C1 = trigonal planar, C2 = tetrahedral E) C1 = trigonal pyramidal, C2 = see-saw

15) Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm. A) 1.46 × 1014 s-1 B) 6.86 × 1014 s-1 C) 4.33 × 1014 s-1 D) 6.17 × 1014 s-1 E) 1.62 × 1014 s-1

15) Which of the following reactions is associated with the lattice energy of CaS (ΔH°latt)? A) Ca(s) + S(s) → CaS(s) B) CaS(s) → Ca(s) + S(s) C) Ca2⁺ (aq) + S2⁻ (aq) → CaS(s) D) Ca2⁺ (g) + S2⁻ (g) → CaS(s) E) CaS(s) → Ca2⁺ (aq) + S2⁻ (aq)

16) Which of the following occur as the energy of a photon increases? A) the frequency decreases. B) the speed increases. C) the wavelength increases D) the wavelength gets shorter. E) None of the above occur as the energy of a photon increases.

17) How many unpaired electrons are present in the ground state Ge atom? A) 0 B) 3 C) 1 D) 2 E) 4

18) Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS2 CF4 SCl2 A) CS2 = SCl2 > CF4 B) SCl2 > CF4 > CS2 C) CF4 > CS2 > SCl2 D) CS2 > CF4 > SCl2 E) CF4 > CS2 > SCl2

19) How many of the following elements have 2 unpaired electrons in the ground state? C O Ti Si A) 1 B) 2 C) 3 D) 4

21) How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy? A) 5.67 × 1023 photons B) 2.01 × 1024 photons C) 1.25 × 1031 photons D) 4.99 × 1023 photons E) 7.99 × 1030 photons

21) Identify the number of valence electrons for Mn. A) 8 B) 7 C) 5 D) 2

22) How much energy (in kJ) do 3.0 moles of photons all with a wavelength of 655 nm, contain? A) 183 kJ B) 303 kJ C) 394 kJ D) 548 kJ E) 254 kJ

24) How many of the following molecules are polar? PCl5 COS XeO3 SeBr2 A) 2 B) 0 C) 1 D) 3 E) 4

26) How many valence electrons does an atom of Al possess? A) 1 B) 2 C) 5 D) 3 E) 8

26) Place the following elements in order of increasing electronegativity. K Cs P A) P < K < Cs B) K < P < Cs C) Cs < P < K D) Cs < K < P E) P < Cs < K

29) List the following compounds in decreasing electronegativity difference. Cl2 HCl NaCl A) NaCl > Cl2 > HCl B) Cl2 > HCl > NaCl C) HCl > NaCl > Cl2 D) NaCl > HCl > Cl2

30) Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of 1.33 × 10-35 m. A) 8.81 m/s B) 12.3 m/s C) 2.21 m/s D) 4.98 m/s E) 6.44 m/s

31) Place the following elements in order of decreasing atomic radius. Xe Rb Ar A) Ar > Xe > Rb B) Xe > Rb > Ar C) Ar > Rb > Xe D) Rb > Xe > Ar E) Rb > Ar > Xe

32) Choose the bond below that is least polar. A) P-F B) C-Br C) C-F D) C-I E) C-Cl

34) Determine the electron geometry, molecular geometry and polarity of N2O (N central). A) eg=linear, mg=linear, nonpolar B) eg=tetrahedral, mg=linear, nonpolar C) eg=tetrahedral, mg=bent, polar D) eg= linear, mg=linear, polar E) eg=trigonal planar, mg=bent, polar

35) A molecule containing a central atom with sp3 hybridization has a(n) __________ electron geometry. A) linear B) trigonal bipyramidal C) octahedral D) tetrahedral E) bent

37) Identify the number of electron groups around a molecule with a tetrahedral shape. A) 1 B) 2 C) 3 D) 4

37) Which molecule or compound below contains a polar covalent bond? A) C2H4 B) ZnS C) LiI D) NCl3 E) AgCl

37) Which reaction below represents the first ionization of O? A) O+ (g) + e- → O(g) B) O(g) + e- → O- (g) C) O- (g) → O(g) + e- D) O(g) → O+ (g) + e- E) O- (g) + e- → O2- (g)

39) Choose the best Lewis structure for BeF2. A) B) C) D) E)

4) Determine the electron geometry (eg) and molecular geometry (mg) of CO32⁻. A) eg=tetrahedral, mg=tetrahedral B) eg=tetrahedral, mg=trigonal pyramidal C) eg=trigonal planar, mg=bent D) eg=trigonal planar, mg=trigonal planar E) eg=tetrahedral, mg=trigonal planar

40) Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. A) n = 2, l = 2, ml =-1 B) n = 2, l = 2, ml =0 C) n = 3, l = 2, ml =-3 D) n = 4, l = 3, ml =-2 E) n = 4, l = 2, ml =+4

42) Draw the Lewis structure for BrO4⁻. What is the hybridization on the Br atom? A) sp B) sp3d2 C) sp3d D) sp3 E) sp2

42) Place the following in order of increasing IE1. K Ca Rb A) Ca < K < Rb B) Rb < Ca < K C) Ca < Rb < K D) Rb < K < Ca E) K < Ca < Rb

44) Choose the best Lewis structure for ICl5. A) B) C) D) E)

44) Which of the following statements are TRUE? A) We can sometimes know the exact location and speed of an electron at the same time. B) All orbitals in a given atom are roughly the same size. C) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. E) All of the above are true.

45) Give the number of valence electrons for SF4. A) 28 B) 30 C) 32 D) 34

48) How many of the following species are diamagnetic? Cs Zr2+ Al3+ Hg2+ A) 1 B) 3 C) 0 D) 2 E) 4

49) How many different values of ml are possible in the 3d sublevel? A) 2 B) 1 C) 3 D) 5 E) 7

5) Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1. A) eg=tetrahedral, mg=tetrahedral B) eg=tetrahedral, mg=trigonal pyramidal C) eg=trigonal planar, mg=bent D) eg=trigonal planar, mg=trigonal planar E) eg=tetrahedral, mg=trigonal planar

5) Which of the following represent the Lewis structure for Br⁻? A) B) C) D) E)

7) Which of the following visible colors of light has the longest wavelength? A) blue B) green C) yellow D) red E) violet

8) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN. A) eg=tetrahedral, mg=tetrahedral B) eg=linear, mg=trigonal planar C) eg=trigonal planar, mg=bent D) eg=linear, mg=linear E) eg=trigonal planar, mg=trigonal planar

In a reaction mixture containing only reactants, what is the value of Q? A) -1 B) - C) infinity D) 0 E) It cannot be determined without concentrations.

D) 0

In a reaction mixture containing only reactants, what is the value of Q? A) -1 B) 1 C) infinity D) 0 E) It cannot be determined without concentrations.

D) 0

Calculate P[NO]eq, if P[NOCl]eq= 0.33atm, P[Cl2]eq= 0.50atm, and Kp= 1.9 x 10-2 2NOCl(g) <--> 2NO(g) + Cl2(g) A) 1.7 atm B) 0.0042 atm C) 0.30 atm D) 0.064 atm E) 0.087 atm

D) 0.064 atm

Determine the value of Kc for the following reaction if equilibrium concentrations are as follows: [N2]eq= 1.5M, [H2]eq= 1.1M, [NH3]eq= 0.47M N2(g) + 3H2(g) <--> 2NH3(g) A) 3.5 B) 0.28 C) 9.1 D) 0.11 E) 0.78

D) 0.11

The total number of lone pairs in NCl3 is A) 6 B) 8 C) 9 D) 10 E) 13

D) 10 N has five valence e⁻ (group 15). It uses three of these e⁻ to form the three N:Cl σ bonds. The remaining two e⁻s form a lone pair so that's one lp! (NCl3 is an AX3E system and like NH3 trigonal pyramidal.) Cl is [Ne] 3s^2 3p^5; the e⁻ from N completes the p shell and forms a bp. That leaves the 3^s2 and two 3p^4 to form three lp per Cl substituent. Hence the total number of lp = 1 (:N) + 3×3 ("Cl:::") for a total of 10 (1st answer) https://www.youtube.com/watch?v=yHMEvt1tcsc

105. Use the bond enthalpy data given to estimate the heat released when 25.0 g of acetylene gas, C2H2, burns in excess oxygen to yield carbon dioxide and water vapor at 25°C. BE(C-C) = 347 kJ/mol BE(CºC) = 812 kJ/mol BE(C=O in CO2) = 799 kJ/mol BE(C-H) = 414 kJ/mol BE(O-H) = 460 kJ/mol BE(O=O) = 498.7 kJ/mol

D) 1180 kJ

The number of lone electron pairs in the ClO4 - ion is ___. A) 3 B) 4 C) 6 D) 12 E) 24

D) 12 https://www.google.com/search?q=ClO4+lewis+structure&biw=1242&bih=585&tbm=isch&imgil=ZA4NAGXOYGBtoM%253A%253BKAjzwafRZZ8YhM%253Bhttp%25253A%25252F%25252Fwww.youtube.com%25252Fwatch%25253Fv%2525253DbXEMU2fMMus&source=iu&pf=m&fir=ZA4NAGXOYGBtoM%253A%252CKAjzwafRZZ8YhM%252C_&usg=__Vwuq4Le9orGmtH2kCSjt8WXiVkk%3D&ved=0CCcQyjc&ei=OlBJVYCqJIO1yQTtlIDQDA#imgrc=ZA4NAGXOYGBtoM%253A%3BKAjzwafRZZ8YhM%3Bhttp%253A%252F%252Fi.ytimg.com%252Fvi%252FbXEMU2fMMus%252Fmaxresdefault.jpg%3Bhttp%253A%252F%252Fwww.youtube.com%252Fwatch%253Fv%253DbXEMU2fMMus%3B1365%3B773

section 9.6 The total number of valence electrons in the molecule CO2 is A) 4 B) 10 C) 14 D) 16 E) 20

D) 16

Use the bond enthalpy data given to estimate the heat released when 50.0 g of propane gas, C3H8, burns in excess oxygen to yield carbon dioxide and water vapor at 25°C. BE(C-C) = 347 kJ/mol BE(C=O in CO2) = 799 kJ/mol BE(C-H) = 414 kJ/mol BE(O-H) = 460 kJ/mol BE(O=O) = 498.7 kJ/mol

D) 2240 kJ

In which orbital below would an electron be closest to the nucleus? A) 2p B) 3p C)4s D) 2s E) 5d

D) 2s

9.7 Assuming the octet rule is obeyed, how many covalent bonds will a nitrogen atom form to give a formal charge of zero? A) 0 B) 1 C) 2 D) 3 E) 4 https://www.youtube.com/watch?v=vOFAPlq4y_k

D) 3 http://guweb2.gonzaga.edu/faculty/cronk/chemistry/L00-index.cfm?L00resource=formal-charge Formal charge = number of valence electrons - (number of lone-pair electrons + 1/2 number of bonding electrons)

The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 500K? N2(g) + 3H2(g) <--> 2NH3(g) A) 15 B) 61 C) 28 D) 3.6 x 10-2 E) 1.9 x 10-2

D) 3.6 x 10-2

The total number of bonding electrons in a molecule of formaldehyde (H2CO) is A) 3 B) 4 C) 6 D) 8 E) 18

D) 8 https://www.youtube.com/watch?v=-RJKFO8WKsQ remember H only needs 2

34) Which statement is true for a catalyst?

D) A catalyst increases rate by providing a reaction path which has lower activation energy.

The Lewis dot symbol for the calcium ion is

D) Ca2+

List all types of bonding present in the compound CaCO3 I. ionic bond II. polar covalent bond III. nonpolar covalent bond A) I only B) II only C) III only D) I and II E) II and III

D) I and II

List all types of bonding present in the compound NH4NO3 I. ionic bond II. polar covalent bond III. nonpolar covalent bond A) I only B) II only C) III only D) I and II E) II and III

D) I and II E) II and III

Express the equilibrium constant for the following reaction. P4(s) + 5O2(g) <--> P4O10(s) A) K= [P4][O2]5 / [P4O10] B) K= [P4O10] / [P4][O2]5 C) K= [O2]-5 D) K= [O2]5 E) K= [P4O10] / [P4][O2]1/5

D) K= [O2]5

Which of the following is an alkali metal? A) Zn B) Ca C) F D) Li E) Xe

D) Li

Which of the following contains the fewest atoms? A) 3.22 g K B) 3.22 g Na C) 3.22 g Ca D) 3.22 g Rb E) 3.22 g Li

D) Lithium

Which one of the following compounds utilizes both ionic and covalent bonding? A) C10H22O B) NH3 C) Na2S D) NH4NO3 E) K3N

D) NH4NO3

Which of the following substances will display an incomplete octet in its Lewis structure? A) CO2 B) Cl2 C) ICl D) NO E) SO2

D) NO

9.4 Which one of the following is most likely to be a covalent compound? A) Rb2O B) BaO C) SrO D) SeO2 E) MnO2

D) SeO2 Covalent compounds are compounds that contain only covalent bonds. The structures we use to represent covalent compounds, such as H2 and F2, are called Lewis structures.

Which of the bonds below would have the greatest polarity (i.e., highest percent ionic character)? A) Si — P B) Si — S C) Si — Se D) Si — Cl E) Si — I

D) Si — Cl

Which of the elements listed below would most likely form an ionic bond when bonded to chlorine? A) H B) Br C) O D) Sr E) N

D) Sr

Which of the following transitions represent emission of the longest wavelength photon A) n=4 to n=2 B) n=1 to n=2 C) n=3 to n=2 D) n=3 to n=4 E) n=5 to n=4

D) n=5 to n=4

Express the equilibrium constant for the following reaction: P4(s)+ 5 O2(g)↔ P4O10(s) A. [P4O10]/[O2]^5 [P4] B. [P4O10]/[O2]^5 C. [O2]^5 D. 1/[O2]^5 E. none of the above

D. 1/[O2]^5

Identify the methods used to monitor a reaction as it occurs in the reaction flask. A. polarimeter B. spectrometer C. pressure measurement D. all of the above E. none of the above

D. all of the above

A plot of concentration of reactant A v. time produces a plot with a curved line (not a straight line plot). What can you state about the reaction order for [A]? A. 0th order B. 1st order C. 2nd order D. not 0th order E. not 1st order

D. not 0th order

Give the direction of the reaction, if the only information you know is K<<1. A. the forward reaction is favored B. if the temperature is raised, then the reverse reaction is favored. C. if the temperature is raised, then the forward reaction is favored. D. the reverse reaction is favored E. not enough information

D. the reverse reaction is favored

Define a liquid

Definite volume and no definite shape

What is the strongest type of intermolecular force present in CHCl3

Dipole-dipole

1) Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays radio waves A) gamma rays < radio waves < ultraviolet light B) radio waves < ultraviolet light < gamma rays C) radio waves < gamma rays < ultraviolet light D) ultraviolet light < gamma rays < radio waves E) gamma rays < ultraviolet light < radio waves

1) Which of the following statements is TRUE? A) A covalent bond is formed through the transfer of electrons from one atom to another. B) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." C) It is not possible for two atoms to share more than two electrons. D) Single bonds are shorter than double bonds. E) A covalent bond has a lower potential energy than the two separate atoms.

12) Determine the electron geometry (eg) and molecular geometry (mg) of XeF4. A) eg=tetrahedral, mg=tetrahedral B) eg=linear, eg=linear C) eg=tetrahedral, mg=bent D) eg=trigonal bipyramidal, mg=tetrahedral E) eg=octahedral, mg=square planar

12) Give the ground state electron configuration for Cd. A) [Kr]5s25d10 B) [Kr]5s24d105p2 C) [Kr]4d10 D) [Kr]5s24d8 E) [Kr]5s24d10

16) Which of the following reactions is associated with the lattice energy of RbI (ΔH°latt)? A) Rb(s) +1/2I2(g) → RbI(s) B) RbI(s) → Rb⁺ (g) + I⁻ (g) C) RbI(s) → Rb(s) + I2(g) D) RbI(s) → Rb⁺ (aq) + I⁻ (aq) E) Rb⁺ (g) + I⁻ (g) → RbI(s)

18) Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. A) 3.54 × 10-19 J B) 4.27 × 10-19 J C) 2.34 × 10-19 J D) 6.45 × 10-19 J E) 2.83 × 10-19 J

19) Place the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H2O H3O⁺ A) H2O < H3O⁺ < HCN B) H3O⁺ < H2O < HCN C) HCN < H3O⁺ < H2O D) H2O < HCN < H3O⁺ E) H2O < H3O⁺ < HCN

21) Place the following in order of decreasing magnitude of lattice energy. KF MgS RbI A) RbI > KF > MgS B) RbI > MgS > KF C) MgS > RbI > KF D) KF > RbI > MgS E) MgS > KF > RbI

22) How many valence electrons does an atom of S have? A) 3 B) 1 C) 2 D) 4 E) 6

23) What total energy (in kJ) is contained in 1.0 mol of photons all with a frequency of 2.75 × 1014 Hz? A) 182 kJ B) 219 kJ C) 457 kJ D) 326 kJ E) 110 kJ

25) How many valence electrons does an atom of Cu possess? A) 2 B) 9 C) 11 D) 3 E) 1

26) Determine the electron geometry, molecular geometry and polarity of SF6 . A) eg=trigonal bipyramidal, mg=trigonal bipyramidal, nonpolar B) eg=tetrahedral, mg=tetrahedral, polar C) eg=trigonal bipyramidal, mg=see-saw, polar D) eg=octahedral, mg=trigonal bipyramidal, nonpolar E) eg=octahedral, mg=octahedral, nonpolar

26) Which of the following statements is TRUE? A) The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All of the above are true.

27) How many valence electrons do the halogens possess? A) 5 B) 6 C) 2 D) 1 E) 7

27) Place the following elements in order of decreasing electronegativity. S Cl Se A) Se > S > Cl B) Cl > Se > S C) Se > Cl > S D) S > Cl > Se E) Cl > S > Se

32) Place the following in order of increasing atomic radius. As O Br A) As < Br < O B) O < As < Br C) Br < As < O D) As < O < Br E) O < Br < As

32) Place the following in order of increasing dipole moment. I. BCl3 II. BIF2 III. BClF2 A) I < II = III B) II < III < I C) I < II < III D) II < I < III E) I < III < II

32) Which of the following transitions (in a hydrogen atom) represent emission of the longest wavelength photon? A) n = 1 to n = 2 B) n = 3 to n = 1 C) n = 3 to n = 4 D) n = 4 to n = 2 E) n = 5 to n = 4

33) Using periodic trends, place the following bonds in order of increasing ionic character. S-F Se-F O-F A) Se-F < S-F < O-F B) S-F < Se-F < O-F C) O-F < Se-F < S-F D) Se-F < O-F < S-F E) O-F < S-F < Se-F

36) A molecule containing a central atom with sp3d hybridization has a(n) __________ electron geometry. A) tetrahedral B) linear C) octahedral D) trigonal planar E) trigonal bipyramidal

38) Which molecule or compound below contains an ionic bond? A) CO2 B) C2Cl4 8 C) SiF4 D) OCl2 E) NH4NO3

38) Which reaction below represents the second ionization of Sr? A) Sr(g) → Sr+ (g) + e- B) Sr2+ (g) + e- → Sr+ (g) C) Sr+ (g) + e-⁻ → Sr(g) D) Sr- (g) + e- → Sr2- (g) E) Sr+ (g) → Sr2+ (g) + e-

40) Choose the best Lewis structure for OCl2. A) B) C) D) E)

41) Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. A) n = 4, l = 4, ml =0 B) n = 3, l = 2, ml =+3 C) n = 4, l = 0, ml =-1 D) n = 3, l = 1, ml = -2 E) n = 5, l = 3, ml =-3

43) Draw the Lewis structure for SF6. What is the hybridization on the S atom? A) sp B) sp2 C) sp3 D) sp3d E) sp3d2

43) Place the following in order of decreasing metallic character. P As K A) P > As > K B) As > P > K C) K > P > As D) As > K > P E) K > As > P

44) Choose the paramagnetic species from below. A) Ca B) O2- C) Cd2+ D) Zn E) Nb3+

45) Which of the following quantum numbers describes the shape of an orbital? A) principal quantum number B) magnetic quantum number C) spin quantum number D) Schrödinger quantum number E) angular momentum quantum number

46) Choose the best Lewis structure for SF4. A) B) C) D) E)

46) Consider the molecule below. Determine the hybridization at each of the 2 labeled carbons. A) C1 = sp3, C2 = sp3d B) C1 = sp, C2 = sp2 C) C1 = sp2, C2 = sp3d D) C1 = sp3d, C2 = sp3d2 E) C1 = sp2, C2 = sp3

49) How many of the following molecules have sp3 hybridization on the central atom? XeCl4 CH4 SF4 C2H2 A) 0 B) 4 C) 3 D) 2 E) 1

6) Determine the electron geometry (eg) and molecular geometry (mg) of SiF4. A) eg=tetrahedral, mg=trigonal pyramidal B) eg=octahedral, mg=square planar C) eg=trigonal bipyramidal, mg=trigonal pyramidal D) eg=tetrahedral, mg=bent E) eg=tetrahedral, mg=tetrahedral

6) Which of the following represent the Lewis structure for Ca2⁺? A) B) C) D) 2 E)

Which of the following Lewis structures is incorrect?

Which of the following reactions would have the smallest value of K at 298 K?

E cell = -0.030 V

The formal charge on the bromine atom in BrO3 - drawn with three single bonds is A) -2 B) -1 C) 0 D) +1 E) +2

E) +2 https://www.youtube.com/watch?v=arkf8YDSgMM

The reaction below has a Kc value of 1.0 x 1012. What is the value of Kp for this reaction at 500K? 2SO2(g) + O2(g) <--> 2SO3(g) A) 4.2 x 10-11 B) 1.0 x 1012 C) 2.4 x 10-12 D) 4.1 x 1013 E) 2.4 x 1010

E) 2.4 x 1010

Assuming the octet rule is obeyed, how many covalent bonds will a carbon atom form to give a formal charge of zero? A) 0 B) 1 C) 2 D) 3 E) 4

E) 4

The covalent bond with the greatest polarity would form in which of the atom pairs below? A) Br — Br B) S — O C) C — P D) C — O E) B — O

E) B — O

Which one of the following molecules has an atom with an incomplete octet? A) NF3 B) H2O C) AsCl3 D) GeH4 E) BF3

E) BF3 https://www.youtube.com/watch?v=JecuOoa12gQ B is incomplete

A nonpolar covalent bond (i.e., pure covalent) would form in which one of the following pairs of atoms? A) Na — Cl B) H — Cl C) Li — Br D) Se — Br E) Br — Br

E) Br — Br non polar = 0.0-0.4

The Lewis structure reveals only single bonds in which of the following species? A) CO2 B) CO C) CO3 2- D) Cl2CO E) CCl4

E) CCl4

Which of the elements listed below would most likely form an ionic bond when bonded to oxygen? A) Cl B) C C) O D) H E) Ca

E) Ca

Which one of the following ionic solids would have the largest lattice energy? A) NaCl B) NaF C) CaBr2 D) CsI E) CaCl2

E) CaCl2 https://www.youtube.com/watch?v=EwnU8RalZOw lattice energy increas when u go up the table n decrease when you go down

Which of these is a chemical change? A) Water is vaporized B) Powdered lemonade is stirred into water C) Paper is shredded D)Salt is dissolved in water E) Methane gas is burned

E) Methane burned

Which one of the following compounds does not follow the octet rule? A) NF3 B) CO2 C) CF4 D) Br2 E) NO

E) NO

Which molecule has a Lewis structure that does not obey the octet rule? A) N2O B) CS2 C) PH3 D) CCl4 E) NO2

E) NO2 n is messing octants http://www.kentchemistry.com/links/bonding/LewisDotTutorials/NO2.htm

Calculate the energy change for the reaction K(g) + I(g) --> K+(g) + I - (g) given the following ionization energy (IE) and electron affinity (EA) values A) -124 kJ/mol D) 1429 kJ/mol B) -715 kJ/mol E) None of these C) 715 kJ/mol

E) None of these

A polar covalent bond would form in which one of the following pairs of atoms? A) Cl — Cl B) Si — Si C) Ca — Cl D) Cr — Br E) P — Cl

E) P — Cl polar covalent bond are non metal

Which of the following transitions represent absorption of the smallest frequency photon A) n=1 to n=2 B) n=1 to n=3 C) n=3 to n=2 D) n=3 to n=4 E) n=5 to n=4

E) n=5 to n=4

What are the units of k in a second order reaction? A. M^2/s B. M C. 1/M D.M/s E. (M^-1)(s^-1)

E. (M^-1)(S^-1)

If a reaction mixture initially contains 0.130 M CO and 0.130 M H2O, what will the equilibrium concentration of CO2 (g) be? CO(g) + H2O ↔ CO2(g) +H2(g) Kc= 102 A. 0.110 B. 0130 C. 0.100 D. 11.2 E. 0.118

E. 0.118

What data should be plotted to show that experimental concentration data fits second- order reaction? A. ln [reactant] v. time B. in (k) v. 1/T C. [reactant] v. time D. in (k) v. Ea E. 1/[reactant] v. time

E. 1/[reactant] v. time

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g)↔ 2 H2O(g) + 2 SO2(g) A. The equilibrium constant will increase B. the reaction will shift to the right in the direction of the products. C. No effect will be observed D. The equilibrium constant will decrease E. The reaction will shift to the left in the direction of the reactants

E. The reaction will shift to the left in the direction of reactants

What would I need to plot to give me s straight line with a slope equal to -Ea/R, for A→B? A. in[A] v. time B. [A] v. time C. 1/[A] v. time D. In k v. time E. In k v. 1/T

E. ln k v. 1/T

Place the following compounds in order of increasing strength of intermolecular forces CO2 F2 NH2CH3

F2<CO2<NH2CH3

What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s) Fe3+(aq) Cl2(g) Cl(aq) Pt

Fe (s)

Determine the cell notation for the redox reaction given below. 3 Cl2(g) + 2 Fe(s) → 6 Cl(aq) + 2 Fe3+(aq)

Fe(s) / Fe3+(aq) // Cl2(g) / Cl(aq) Pt

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

Fe3+(aq) + Ni(s)

22) A 0.286-g sample of gas occupies 125 mL at 60. cm of Hg and 25°C. What is the molar mass of the gas?

First convert the pressure 60cmHg (10mm) = 600mmHg 600mmHg/760mmHg= .7894 Second convert temperature 25+273=298 Third convert volume 125/1000=.125 pv=nRt n=pv/Rt (.7894)(.125)/(.08206)(298)= .00403 Lastly divide by the sample number .286/.00403= 71

Go back over the tests

For the problems that can't be typed in quizlet

32) Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction?

Generally, no. The relationship between the activation energies of the forward and reverse reactions are related by the relative energies of the reactants and products. If the reactants are higher in energy than the products, the activation energy for the forward reaction will be smaller than the activation energy for the reverse reaction and vice versa.

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) Pb2+(aq) H+(aq) H2(g) Pt

H+

Place the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H2O H3O⁺

H2O < H3O⁺ < HCN

Place the following in order of decreasing boiling point H2O N2 CO

H2O > CO > N2

Place the following substances in order of decreasing boiling point. H2O N2 CO

H2O>CO>N2

Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite

H2SO3(aq)+2LiOH (aq) → 2H2O(l)+Li2SO3(aq)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H and Fe3+ in the balanced reaction? Fe2+(aq) + MnO4(aq) → Fe3+(aq) + Mn2+(aq)

H=8, Fe³⁺=5

Choose the substance with the highest viscosity.

HOCH2CH2CH2CH2OH

Choose the substance with the highest surface tension.

HOCH2CH2OH

What is the empirical formula for Hg2(NO3)2?

HgNO3

Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point?

Highest Dipole point CH3CN-3.9

How many electron domains does the central atom have in NO2-? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6

How many electron domains does the central atom have in PCl3? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4 (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

H₂C₂O₄ =5, H₂O =8

Place the following in order of increasing dipole moment. I. BCl3 II. BIF2 III. BClF2

I < III < II

Place the following in order of decreasing dipole moment. I. cis-CHCl=CHCl II. trans-CHCl=CHCI III. cis-CHF=CHF

III > I > II

The equilibrium constant, Kp, equals 3.40 at 25°C for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 5.00 atm of each gas, in what direction will the system shift to reach equilibrium?

It will shift right

Determine the oxidation states of both K and O in KO2

K +1, O -1/2

37) Express the equilibrium constant for the following reaction. 2 Na(s) + 2 H2O(l) 2 NaOH(aq) + H2(g)

K = [H2][NaOH]2

Choose the substance with the highest boiling point.

At a certain temperature, nitrogen and hydrogen react to form ammonia: N2(g) + 3 H2(g) ⇌ 2 NH3(g). When initial amounts of N2, H2, and NH3 are mixed, the concentration of NH3 increases. Which statement below is TRUE?

Kc >Q

The VSEPR model predicts H-O-H bond angle in H3O+ would be

Less than 109.5 but greater than 90

17) Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2)2(aq) 2 LiC2H3O2(aq) + Fe(s)

Li whyyyyy

Identify the spectator ions in the following molecular equation LiCl (aq) + AgNO3 (aq) → AgCl (s) + LiNO3(aq)

Li + and NO3-

Determine the reducing agent in the following reaction 2Li + Fe (C2H3O2)2 → LiC2H3O2 + Fe

Lithium

The intermolecular force responsible for the fact that CH4 has the lowest boiling point in the set CH4, SiH4,GeH4, SnH4 is/are

London dispersion forces

24) Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 × 10-3 M/s, what is the rate of formation of SO3? 2 SO2(g) + O2(g) 2 SO3(g)

Look at equation, coefficient for SO3 is 2 Multiply: (3.56 × 10-3 M/s) (2) = 7.12 × 10-3 M/s

Determine the redox reaction represented by the following cell notation. Mg(s) / Mg2+(aq) // Cu2+(aq) / Cu(s)

Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq)

Which of the following substances should have the highest melting point?

MgO

What element is being reduced in the following redox reaction? MnO4 (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

49) What will happen to the following endothermic reaction in equilibrium if the temperature is raised? N2O4(g) 2NO2(g)

More NO2 will be produced.

What element is being oxidized in the following redox reaction? Zn2+(aq) + NH4+(aq) → Zn(s) + NO3(aq)

What would the Lewis structure for N look like?

N with 5 dots around it

Choose the bond below that is the strongest n-n N-N double bond N-N triple bond N-C C-C

N-N triple bond

Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25°C.

N2 + 3H2 ---> 2NH3 moles of N2 = 6.50 / 28 = 0.232 mol moles of H2 = 3*0.232 = 0.696 mol moles of NH3 = 2*0.232 = 0.464 mol so heat released = 0.464*3*393 - (0.232*941.4 + 0.696*436.4) = 24.9 k

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N2O NCl3 NO2⁻

N2O > NO2⁻ > NCl3

Determine the molecular formula of a compound that has a molar mass of 92. g/mol and an empirical formula of NO2

N2O4

place in order of increasing strength of forces CS2 Cl2 NH2CH3

NH2CH3 > CS2 > Cl2

Place in order of increasing bond length NO2- NO3- NO

NO < NO2- < NO3-

16) Determine the oxidation state of Cl in NaClO3.

Na Cl O 1 x 3(-2) 1 + x + -6 x+-5 x=5

Place the following in order of decreasing standard molar entropy. NaCl(s) Na3PO4 (aq) NaCl (aq)

Na₃PO₄ > NaCl (aq) > NaCl (s)

Which of the following gas samples would be most likely to behave ideally under the stated conditions?

Ne at STP

A student performs an experiment to determine the density of a sugar solution. she obtains the following results: 1.11g/ml, 1.81g/ml, 1.95g/ml, 1.75g/ml. If the actual value for the density is 1.75 are her results accurate or precise?

Neither accurate or precise.

Isotopes differ in the number of what particle?

Neutrons

What is the reducing agent in the redox reaction represented by the following cell notation? Ni(s) / Ni2+(aq) // Ag+(aq) / Ag(s)

Ni (s)

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

No effect will be observed

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? CuS(s) + O2(g) ⇌ Cu(s) + SO2(g)

No effect will be observed

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? CuS(s) + O2(g) ⇌ Cu(s) + SO2(g)

No effect will be observed

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO2(g) + C(graphite) ⇌ 2 CO(g)

No effect will be observed since C is not included in the equilibrium expression

Place the following in order of decreasing molar entropy at 298 K. HCl, N2H4, Ar

N₂H₄> HCl >Ar

Place the following in order of decreasing standard molar entropy N₂O₄ (g), NO (g), NO₂ (g)

N₂O₄ > NO₂ >NO

What element is being oxidized in the following redox reaction? H2O2(l) + ClO2(aq) → ClO2(aq) + O2(g)

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force HF CO NaCl O2

The density of a gas is 1.43 g/mole at STP. What is the gas?

O2 ?????

Place the following in order of decreasing boiling point N2 O2 H2

O2> N2> H2

Using Lewis structures and formal charge, which of the following ions is most stable? OCN- ONC- NOC-

OCN-

Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF3 OF2 PF4⁺

OF2 < PF3 < PF4⁺

freezing

Of the following, __ is an exothermic process (A) melting (B) subliming (C) freezing (D) boiling

For the isomerization reaction: butane ⇌ isobutane Kp equals 25 at 500°C. If the initial pressures of butane and isobutane are 20. atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?

P(butane) = 0.77 atm and P(isobutane) = 19.2 atm

The equilibrium constant, Kp, equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0. 145 atm of trans-2-butene, what is the equilibrium pressure of each gas?

P(cis-2-butene) = 0. 0898 atm and P(trans-2-butene) = 0. 305 atm

Determine the empirical formula for a compound that is found to contain 1O.15 mg P and 34.85 mg Cl

PCl3

Which contains at least one polar covalent bond? Pcl5 C2H4 AgI ZnS LiI

PCl5

No two electrons can have the same four quantum numbers is known as

Pauli exclusion principle

What is undergoing oxidation in the redox reaction represented by the following cell notation? Pb(s) Pb2+(aq) H+(aq) H2(g) Pt

Pb (s)

Determine the cell notation for the redox reaction given below. Pb(s) + 2H(aq) → Pb2+(aq) + H2(g)

Pb(s) / Pb2+(aq) // H+(aq) / H2(g) Pt

Identify the greatest currently used source of energy in the US

Petroleum

Determine the number of protons, neutrons, and electrons in the follow: ⁴⁵₂₂X

Protons-22 Neutrons-23 Electrons-22

35) A reaction follows the following two-step mechanism. 2A A2 Slow A2 + B A2B Fast Overall: 2A + B = A2B What is the rate law?

Rate = k[A]2

36) Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO2 + Cl2 2NO2Cl (overall reaction) Mechanism NO2 + Cl2 NO2Cl + Cl slow NO2 + Cl NO2Cl fast

Rate = k[NO2][Cl2]

Place the following elements in order of decreasing atomic radius Xe Rb Ar

Rb>Xe>Ar

Which of the visible colors of light has the longest wavelength?

Red

For which reaction will Kp = Kc?

S (s) + O2 (g) ⇌ SO2 (g)

Place the following substances in order of increasing vapor pressure at a given temperature SF6 SiH4 SF4

SF4<SF6<SiH4

Place the following in order of increasing molar entropy at 298 K. CO2, C3H8, SO

SO <CO₂ <C₃H₈

Choose the one that exhibits dipole-dipole forces CF4 SO2 H2 BCl3 NH3

SO2

Chose the paramagnetic species from below Ar Se Ti4+

Which of the following elements can form compounds with an expanded octet? Li C F Se

Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO2 SeCl6 SeF2

SeCl6 < SeF2 < SeO2

What is a covalent bond?

Sharing of electrons between two atoms

Place the following bonds in order of increasing ionic character SiP SiCl SiS

SiP < SiS < SiCl

A piece of iron (C=0.449 J/g°C) and a piece of gold (C=0.128 J/g°C) have identical masses. If the iron has an initial temperature of 498 K and the gold has an initial temperature of 298 K, which of the following statements is TRUE of the outcome when the two metals are placed in contact with one another? Assume no heat is lost to the surroundings.

Since the two metals have the same mass, the thermal energy contained in each metal after equilibrium will be the same

What is the reducing agent in the redox reaction represented by the following cell notation? Sn(s) / Sn2+(aq) // Ag+(aq) / Ag(s)

Sn (s)

Determine the cell notation for the redox reaction given below. Sn(s) + 2 Ag(aq) → Sn2+(aq) + 2 Ag(s)

Sn(s) / Sn2+(aq) // Ag+(aq) / Ag(s)

Choose the diamagnetic species from below N I Cr Sn2+

Sn2+

Determine which of the following other pairs of reactants will result in a spontaneous reaction at 25°C.

Sn4+(aq) + Mg(s)

14) Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO3(aq) AgBr(s) + KNO3(aq)

Spectator ion: one that exists in both the reactant and the product K+ & NO3- cannot be Ag because its aqueous in reactants and solid in products

18) To what volume will a sample of gas expand if it is heated from 50.0°C and 2.33 L to 500.0°C?

T1 = 50 + 273 = 323 K T1 = 500 + 273 = 773 K at constant pressure V1/T1 = V2 / T2 ( Charles' law) 2.33/ 323 = V2 / 773 V2 = 5.58 L

When energy is transferred from the system to the surrounding in a thermochemical reaction

The energy released by the system is equal to the energy absorbed by the surrounding

Which of the following processes is exothermic?

The formation of dew in the morning. *

What does the magnetic quantum number ml describe

The orientation of the region in space an electron occupies with respect to an applied magnetic field

Define specific heat capacity

The quantity heat required to raise the temperature of 1 gram of a substance by 1 C

Consider the following reaction at equilibrium. What effect will removing H2O have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

The reaction will shift in the direction of products

44) Consider the following reaction at equilibrium. What effect will adding more H2S have on the system? 2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g)

The reaction will shift in the direction of products.

43) Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system? SO2(g) + NO2(g) SO3(g) + NO(g)

The reaction will shift in the direction of reactants.

Consider the following reaction at equilibrium. What effect will adding more H2S have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

The reaction will shift in the direction of the products

Consider the following reaction at equilibrium. What effect will removing NO2 have on the system? SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

The reaction will shift in the direction of the reactants

46) Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g)

The reaction will shift to the left in the direction of reactants.

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? CO2(g) + 2 H2O(l) ⇌ CH4(g) + 2 O2(g) ΔH° = +890 kJ

The reaction will shift to the left in the direction of the reactants

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ

The reaction will shift to the left in the direction of the reactants

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

The reaction will shift to the left in the direction of the reactants

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2 F2(g) → XeF4(g)

The reaction will shift to the left in the direction of the reactants

45) Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g)

The reaction will shift to the right in the direction of products.

Consider the following reaction at equilibrium. What effect will adding CO2 have on the system? CO2(g) + C(graphite) ⇌ 2 CO(g)

The reaction will shift to the right in the direction of the products

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

The reaction will shift to the right in the direction of the products

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? Fe3O4(s) + CO(g) ⇌ 3 FeO(s) + CO2(g) ΔH°= +35.9 kJ

The reaction will shift to the right in the direction of the products

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2 F2(g) → XeF4(g)

The reaction will shift to the right in the direction of the products

Which of the following is TRUE if ΔEsys = - 95 J?

The system is losing 95 J, while the surroundings are gaining 95 J.

Which of the following processes is endothermic?

The vaporization of rubbing alcohol. *

Use bond energies to estimate the enthalpy of formation of HBr(g). BE(H-H) = 436 kJ/mol BE(Br-Br) = 192 kJ/mol BE(H-Br) = 366 kJ/mol A) +262 kJ/mol D) -52 kJ/mol B) +104 kJ/mol E) -104 kJ/mol C) +52 kJ/mo

This is a Hess's Law problem: Products - Reactants On the product side, you have 2 H-Br bonds On the reactant side, you have 1 H-H bond and 1 Br-Br bond So, the math expression would be 366x2 - 436 -192 = 104 kJ This reaction produced 2 mol HBr, so 104 kJ = 2 mol The enthalpy of formation = -52 kJ/mol

The standard enthalpy of formation of ammonia at 25°C is -46.3 kJ/mol. Estimate the N-H bond enthalpy at this temperature. (Given: BE(NºN)=941.4 kJ/mol, BE(H-H) = 436.4 kJ/mol) A) 360 kJ/mol D) 459 kJ/mol B) 383 kJ/mol E) 475 kJ/mol C) 391 kJ/mol

To find the bond enthalpy, you subtract the energy of the bonds formed (since they release energy) and add the energy of the bonds broken (since you need to supply energy). 1/2 an N2 bond is 941/2 = 470.5 kJ/mol 3/2 H2 bonds = 3×436/2 = 654 kJ/mol Total energy = bonds broken-bonds formed = (470.5 + 654) - 3(N-H) Total energy = -46.3 kJ/mol Therefore, -3(N-H) + 1124.5 = -46.3 3(N-H) = 1124.5 + 46.3 = 1170.8 (N-H) = 1170.8/3 = 390.2667 ≈ 390 kJ/mol Remember: total energy of reaction = (total energy of bonds broken) - (total energy of bonds formed)

...

Two or more substances in variable proportions, where the composition is variable throughout

21) The volume of 350. mL of gas at 25°C is decreased to 135 mL at constant pressure. What is the final temperature of the gas?

V1/T1=V2/T2 .35/25=.135/T2 T2= 9.6

Le Chatelier's principle

When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes disturbance.

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Zn and H+ in the balanced reaction? Zn2+(aq) + NH4+(aq) → Zn(s) + NO3(aq)

Zn=4 H=10

Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation: C6H12 ⇌ CH3C5H9 If Kc = 0.143 at 25°C for this reaction, find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 M and 0. 075 M, respectively.

[C6H12] = 0. 241 M, [CH3C5H9] = 0. 034 M

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250° 0. 125 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?

[PCl5] = 0.0 0765 M, [PCl3] = 0. 117 M, and [Cl2] = 0. 117 M

crystalline solids

__ have highly ordered structures.

viscosity

__ increases as temperature decreases, increases as molecular weight increases, and increases as intermolecular forces increase

surface tension

__ is the energy required to expand the surface area of a liquid by a unit amount of area.

water

__ is the most common solvent among liquid solutions

condensation

__ must exist in equilibrium with the evaporation process when a measurement of vapor pressure is made

supersaturated

__ solutions are very unstable

suspension

a __ is a mixture containing particles that settle out if left undisturbed

exothermic

a __ reaction releases heat to its surroundings

endothermic reaction

a __ requires added energy to proceed

a certain solid substance that is brittle, has a high melting point, and it nonconducting unless melted is most likely to be: (A) I2 (B) NaCl (C) CO2 (D) Cu

endothermic, positive

a chemical reaction that absorbs heat from the surroundings is said to be __ and has a __ value of △H at constant pressure

water will flow from the cucumber to the solution

a cucumber is placed in a concentrated salt solution. what will most likely happen?

solute

a dilute solutions contains small amounts of __

exothermic

a negative △H corresponds to an __ process

metallic

a solid has a very high melting point, great hardness, and poor electrical conduction. this is a __ solid

supersaturated

a solution with a concentration higher than the solubility is __

all of the following statements about enthalpy are true except (A) the enthalpy of a substance depends on its temperature, physical state, and composition (B) under constant pressure, the enthalpy change for a reaction is equal to the amount of heart absorbed or released (C) there is generally a very large numerical difference between the energy and enthalpy of a substance (D) enthalpy is represented by the capital letter H

The vertical height of a wave is called

amplitude

an atom of which element below has the most unpaired electrons? (A) Ba (B) Na (C) P (D) F (E) O

determines the shape of the orbital

angular momentum quantum number (l)

decreases

as temperature increases, the solubility of a gas in water __

For a given reaction, ΔH = + 35.5 kJ/mol and ΔS = + 83.6 J/Kmol. The reaction is spontaneous at __________. Assume that ΔH and ΔS do not vary with temperature.

at T> 425 K

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g). If initial concentrations are [SO2] = 6.00 M, [O2] = 0.45 M, and [SO3] = 9.00 M, the system is

at equilibrium

Which of the following is not a major contributor to energy consumption?

atmospheric

Instrument used to measure atmospheric pressure

barometer

below are some elements with their number of valence electrons. which is incorrect? (A) Be---2 (B) Br---5 (C) Li--- 1 (D) Al---3 (E) C---4

will have decreased

consider pure water separated from an aqueous sugar solution by a semipermeable membrane, which allows water to pass freely but not sugar. After some time has passed, the concentration of sugar solution:

a long-range repeating pattern of atoms, molecules, or ions

crystalline solids differ from amorphous solids in that crystalline solids have__

way to separate a mixture by pouring off the water into another container

decanting

Determine the name for N2O5

dinitrogen pentoxide

way to separate a mixture by heating it to foil off more liquid

distillation

Determine the electron geometry (eg) and molecular geometry (mg) of ICl2-

eg = trigonal bipyramidal mg = linear

Determine the electron geometry (eg) and molecular geometry (mg) of PF5

eg = trigonal bipyramidal mg = trigonal bipyramidal

Determine the electron geometry (eg) and molecular geometry (mg) of BCl3

eg = trigonal planar mg = trigonal planar

Determine the electron geometry (eg) and molecular geometry (mg) of Co32-

eg = trigonal planar mg = trigonal planar

Determine the electron geometry (eg) and molecular geometry (mg) of the underline atom H2C*O

eg = trigonal pyramidal mg = trigonal planar

Determine the electron geometry, molecular geometry and polarity of N2O (N central).

eg= linear, mg=linear, polar

Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O

eg= tetrahedral mg = bent sp3

Determine the electron geometry, molecular geometry and polarity of TeCl6.

eg=octahedral, mg=octahedral, nonpolar

Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.

eg=octahedral, mg=square planar

Determine the electron geometry, molecular geometry and polarity of HBrO2 .

eg=tetrahedral, mg=bent, polar

Determine the electron geometry (eg) and molecular geometry (mg) of SiF4.

eg=tetrahedral, mg=tetrahedral

Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3.

eg=tetrahedral, mg=trigonal pyramidal, polar

Determine the electron geometry (eg) and molecular geometry (mg) of BrF3.

eg=trigonal bipyramidal, mg= T-shape

Determine the electron geometry (eg) and molecular geometry (mg) of ICl2⁻.

eg=trigonal bipyramidal, mg=linear

Determine the electron geometry (eg) and molecular geometry (mg) of XeF2.

eg=trigonal bipyramidal, mg=linear

Determine the electron geometry (eg) and molecular geometry (mg) of PF5.

eg=trigonal bipyramidal, mg=trigonal bipyramidal

Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2.

eg=trigonal planar, mg=bent, polar

Determine the electron geometry (eg) and molecular geometry (mg) of CO32⁻.

eg=trigonal planar, mg=trigonal planar

Determine the electron geometry (eg) and molecular geometry(mg) of BCl3.

eg=trigonal planar, mg=trigonal planar

Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO3.

eg=trigonal planar, mg=trigonal planar, nonpolar

dispersion forces

elemental iodine (I2) is a solid at room temperature. what is the major attractive force that exists among different I2 molecules in the solid?

endothermic

endothermic or exothermic? 2h2o + 572 KJ --> 2h2 + o2

exothermic

endothermic or exothermic? 2no + o2 --> 2no2 △H= -113 KJ

exothermic

endothermic or exothermic? 2s + 3o2 --> 2so3 △H= -791 KJ

endothermic

endothermic or exothermic? c + h2o + 113KJ --> co + h2

exothermic

endothermic or exothermic? c3h8 + 5o2 --> 3co2 + 4h2o + 2043KJ

When heat is absorbed by the system from the surroundings, the process is said to be ____ and the sign of the process is ____

endothermic, positive

mixture is poured through filter paper in a funnel

filtration

Place the following types of electromagnetic radiation in order of decreasing energy. gamma rays radio rays microwaves

gamma rays > microwaves > radio waves

how many electron domains does the central atom have in BeBr2? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6

how many electron domains does the central atom have in H2O? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6

how many electron domains does the central atom have in XeF2? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6

how many electron domains does the central atom have in XeF4? (A) 2 (B) 3 (C) 4 (D) 5 (E) 6

how many lone pairs of electrons are in the outer shell of the central nitrogen atom of NH3? (A) 4 (B) 3 (C) 2 (D) 1 (E) 0

how many valence electrons does a phosphorus atom have?

9.10 enthanples

https://www.youtube.com/watch?v=0mLFSDId6pQ

What is the strongest type of intermolecular force present in NH2CH3

hydrogen bonding

dipole-dipole attraction

hydrogen bonding is a special case of __

Hess's law statement

if a reaction takes place in steps, the △H for the reaction will be the sum of △Hs for the individual steps

the mole fraction of 0.1

in a 0.1 molar solution of NaCl in water, what will be the closest to 0.1?

more than the energy required to break apart the reactants

in a combustion reaction, an exothermic reaction, the energy released as the products form is_

strong enough to hold molecules relatively close together but NOT strong enough to keep molecules from moving past each other

in liquids, the attractive intermolecular forces are__

liquid carbon only

in what form or forms does carbon exist at 6000K and 10fifth atm?

in which of the following groups of substances would dispersion forces be the only significant force of attraction: I--Cl2 II--HF III--H20 IV--CCl4 V--KNO2 (A) I, III, V (B) I, II, IV (C) I, IV (D) II, V

Give the change in condition to go from a liquid to a gas

increase heat or reduce pressure

On the electromagnetic spectrum visible light is immediately between these two other wavelengths.

infrared and ultraviolet

Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (MCP) according to the equation: C6H12 ⇌ MCP If Kc = 0.143 at 25°C for this reaction, predict the direction in which the system will shift if the initial concentrations of C6H12 and MCP are 0. 0400 M and 0. 0200 M, respectively. The system will shift

left

Slope is located in

liquid

specifies the orientation of the orbital

magnetic quantum number (ml)

extreme brittleness

metallic solids do NOT exhibit __

colloid

milk is an example of a __

suspension

muddy water from a creek after a heavy rain is an example of a __

What are the possible values of n and l or an electron in a 3d orbital A) n=1,2,3 and l=-2,-1,0,+1,+2 B) n=4 and l= -2,-1,0,+1,+2 C) n=3 and l=2 D) n=1,2,3 and l=2

n=3 and l=2

What are the correct values for a 4f sublevel

n=4 l=3 ml=-3,-2,-1,0,+1,+2,+3

Which of these transitions would be seen as green if the transistions were n=6 to n=2; n=5 to n=2; n=4 to n=2, and n=3 to n=2

n=4 to n=2

A molecule containing a central atom with sp3d2 hybridization has a(n) __________ electron geometry.

octahedral

of the following substances, only __ has hydrogen bonding as its strongest intermolecular force: (A) CH3CH2Cl (B) NH3 (C) H2S (D) CH4

of the following △Hf is not zero for (A) O2 (g) (B) C(graphic) (C) N2 (g) (D) F2 (s)

dispersion, dipole- dipole, hydrogen bonding

order the intermolecular forces from weakest to strongest:

substance that causes the oxidation of another substance

oxidizing agent

Identify the greatest source of energy in the U. S.

petroleum

The compound ClF contains

polar bonds with partial negative charges on the F atoms

Energy that is associated with the position or composition of an object is called

potential energy *

gases

pressure will increase solubility of __ in liquids

integer that determines the overall size and energy of an orbital

principle quantum number (n)

made up of only one component and its composition is invariant

pure substance

Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as gaining heat from the surroundings?

q = +, w = -

Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as losing heat to the surroundings?

q = - , w = -

How much energy is required to heat 36.0g H2O from a liquid at 65°C to a gas at 115°C? DHvap= 40.7 kJ/mol C liq= 4.18J/g°C C gas= 2.01 J/g°C C sol= 2.09 J/g°C T melting= 0°C T boiling= 100°C

q liq= 4.18J/g°c(36g)(100°c-65°c) = 5.266 kJ 36g x 1 mol/18g= 2 mol q= 2 mol x 40.7 kJ/mol= 81.4 kJ q gas= 2.01J/g°c(36g)(115-100°c)= 1.0854 kJ 5.266+81.4+1.0854= 87.7kJ

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

raising T, adding SO₃ and removing O₂

substance that causes the reduction of another substance

reduction agent

viscosity

several liquids are compared by adding them to series of 50ml graduated cylinders, then dropping a steel ball of uniform size and mass into each. the time required for the ball to reach the bottom of the cylinder is noted. this is a method used a compare the differences in a property of liquids known as __

Draw the Lewis structure for SO3. What is the hybridization on the S atom?

sp2

Draw the Lewis structure for BrO4⁻. What is the hybridization on the Br atom?

sp3

Draw the Lewis structure for OF2. What is the hybridization on the O atom?

sp3

Draw the Lewis structure for BrCl3. What is the hybridization on the Br atom?

sp3d

Give the hybridization for the Br in BrCl3

sp3d

Draw the Lewis structure for BrF5. What is the hybridization on the Br atom?

sp3d2

Draw the Lewis structure for SF6. What is the hybridization on the S atom?

sp3d2

What is the molecular geometry of ClF4-

square planar

What kind of electrolyte and acid is HCl

stronger electrolyte and strong acid

List the traits of a nonmetal

tend to gain electrons poor conductors of heat found in the upper right hand corner of the periodic table poor conductors of electricity

A molecule containing a central atom with sp3 hybridization has a(n) __________ electron geometry.

tetrahedral

Determine the electron geometry, molecular geometry, and polarity of N2O

tetrahedral bent polar

joule

the SI unit of heat and energy is the __

enthalpy change

the __ for a reaction is determined by subtracting the enthalpy of the reactants from the enthalpy of products

standard state

the __ of an element is defined by the most stable form of the element under standard conditions

specific heat

the amount of heat needed to raise the temperature of 1g of a substance by 1 degree C

Brownian motion

the erratic movement of colloid particles is called __

the only noble gas without eight valence electrons is (A) Ar (B) Ne (C) He (D) Kr (E) All noble gases have eight valence electrons

life dissolves like

the phrase "__" refers to the fact that polar solvents dissolve polar solutes and non polar solvents dissolves on non polar solutes

endpoint

the point in a titration at which the indicator changes is called the __

a liquid becomes a gas

the process of evaporation happens when what occurs?

solvation

the process of solute particles being surrounded by solvent particles is known as

Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system? SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

the reaction will shift in the direction of reactants

less than

the surface tension of water is great than the surface tension of cooking oil because the unattractive forces between the molecules of cooking oil is __ the attractive forces between the molecules of water

the total number of lone pairs of electrons in the N2 molecule is (A) 1 (B) 2 (C) 3 (D) 4

the total number of valence electrons (available electrons) for C4H5Cl2FO molecule is (A) 42 (B) 44 (C) 46 (D) 48 (E) 50

Determine the name for TICO3. Remember that titanium forms several ions.

titanium (II) carbonate

mass of solvent, total volume of solution, chemical formula of solute

to express a solution concentration in molarity, you need to know:

A molecule containing a central atom with sp3d hybridization has a(n) __________ electron geometry.

trigonal bipyramidal

What is the molecular geometry of SbCl3

trigonal planar

Determine the electron geometry, molecular geometry, and polarity of SO2

trigonal planar bent polar

Identify the shortest bond c-c single bond c-c double bond c-c triple bond

triple bond

temperatures<3500K and pressures> 10fifth atm

under what conditions is diamond most likely to form?

The element that corresponds to the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d3

vanadium

Given a constant amount of gas and constant pressure, the relationship between temperature and volume is

volume is proportional to the absolute temperature

capillary action

what does not affect the viscosity of a liquid?

triple point

what is defined as the combination of pressure and temperature at which all three states of matter can coexist as equilibrium?

adhesive forces

what is responsible for capillary action?

what is the hybridization of the I central atom in I3- molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the hybridization of the boron atom in BF3 molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the hybridization of the carbon atom in CO2 molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the hybridization of the nitrogen atom in NH3 molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the hybridization of the oxygen atom in H3O+ molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the hybridization of the sulfur atom in SF6 molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the hybridization of the sulfur atom in SO3 2- molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the hybridization of the xenon atom in XeF4 molecules? (A) sp (B) sp2 (C) sp3 (D) sp3d (E) sp3d2

what is the molecular geometry of AsF5? (A) trigonal bipyramidal (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of AsH3? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of BBr3? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of BeBr2? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of CCl4? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of ClF3? (A) octahedral (B) square pyramidal (C) square planar (D) trigonal bipyramidal (E) linear

what is the molecular geometry of ClO2-? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of PCl3? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of PH4+? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal

what is the molecular geometry of SF4? (A) octahedral (B) seesaw (C) t-shaped (D) trigonal bipyramidal (E) linear

what is the molecular geometry of SiCl62-? (A) octahedral (B) square pyramidal (C) square planar (D) trigonal bipyramidal (E) linear

what is the molecular geometry of TeF6? (A) octahedral (B) square pyramidal (C) square planar (D) trigonal bipyramidal (E) linear

what is the molecular geometry of XeF2? (A) octahedral (B) square pyramidal (C) square planar (D) trigonal bipyramidal (E) linear

what is the molecular geometry of XeF4? (A) octahedral (B) square pyramidal (C) square planar (D) trigonal bipyramidal (E) linear

what is the symbol for enthalpy?

decreases, increases, decreases, increases

when a nonvolatile solute is added to a solvent, the solution vapor pressure __, the boiling point __, the freezing point __, and the osmotic pressure across a semipermeable membrane __.

a hydrogen from one molecule and an oxygen from the other molecule

when a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction?

the cohesive force is greater than the adhesive force

when the liquid metal mercury is placed in a small tube, the meniscus actually curves upward just the opposite of water. the reason for this is that...

which of the collowing should be immiscible with benzene (C6H6)? (A) C6H14 (B) Br2 (C) CH3CH2OH (D)C3H8

which of the fallowing statements is false? (A) diamond is a covalent crystal (B) solid ionic crystal are good electrical conductors (C) molecular crystals are fairly soft (D) metallic crystals are usually good electrical conductors

which of the follow statements regarding water are true? (A) hydrogen bonds are stronger than covalent bonds (B) only covalent bonds are broken when ice melts (C) only hydrogen-bonds are broken when ice melts (D) liquid water is less dense than solid water

which of the following is most soluble in water? (A) CH3OH (B) CH3CH2OH (C) CH3CH2CH2OH (D)CH3CH2CH2CH2CH2OH

which of the following is not part of the kinetic-molecular theory? (a) atoms are neither created nor destroyed by ordinary chemical reactions (b) attractive and repulsive forces between gas molecules are negligible (c) gases consist of molecules in continuous, random motion (d) collisions between gas molecules do not result in the loss of energy

which of the following is paired incorrectly? (A) crystalline solids-- highly regular arrangement of their components (B) amorphous solids-- considerable disorder in their structures (C) unit cell-- the smallest repeating unit in a lattice (D) molecular solids-- good conductors of heat

which of the following species has sp3 hybridization at the central atom? (A) PF5 (B) NH3 (C) SF6 (D) HF (E) CF4

which of the following species has sp3d hybridization at the central atom? (A) PF5 (B) NH3 (C) SF6 (D) HF (E) CF4

which of the following statements about bonds and energy is correct? (A) bond breaking and bond formation both release energy (B) bond breaking and bond formation both require energy (C) bond breaking requires energy and bond formation releases energy (D) bond breaking releases energy and bond formation requires energy

which of the following statements is not true regarding enthalpy? (A) the change in enthalpy is positive for a process that absorbs heat (B) enthalpy is a state function (C) enthalpy is an extensive property (D) the enthalpy of a system can be measured

which one of the following is an exothermic process? (A) ice melting (B) water evaporating (C) boiling soup (D) condensation of water vapor

which statement regarding water is true? (A) energy is required in order to break down the crystal lattice of ice to a liquid (B) hydrogen bonds are stronger than covalent bonds (C) liquid water is less dense than solid water (D)only covalent bonds are broken when ice melts

For a particular process that is carried out at constant pressure, q = 145 kJ and w = - 35 kJ. Therefore, DE= and DH=

ΔE = 110 kJ and ΔH = 145 kJ.

When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C, 169.5 kJ are absorbed and PΔV for the vaporization process is equal to 14.5 kJ then ΔE = X and ΔH = X

ΔE= 155.0 kJ and ΔH = 169.5 kJ.

Which of the following relationships is correct at constant T and P?

ΔG is proportional to -ΔSuniv

When 10.00 moles of H2(g) reacts with 5.000 mol of O2(g) to form 10.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 683.0 kJ of heat are released during this reaction, and PΔV is equal to - 37.00 kJ, then ΔE° = X and ΔH° = X

ΔH° = - 683.0 kJ and ΔE° = - 646.0 kJ.

Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 398 K. Predict whether or not this reaction will be spontaneous at this temperature. 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g) ΔH = -1267 kJ

ΔSsurr = +3.18 kJ/K, reaction is spontaneous

Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 355 K. Predict whether or not this reaction will be spontaneous at this temperature. 2 NO(g) + O2(g) → 2 NO2(g) ΔH = -114 kJ

ΔSsurr = +321 J/K, reaction is spontaneous

Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 298 K. Predict whether or not this reaction will be spontaneous at this temperature. N2(g) + 2 O2(g) → 2 NO2(g) ΔH = +66.4 kJ

Finished work

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