Zach and Parker's Guide to Chem 1301

Ionization energy is the energy needed to remove an electron from an ion or an atom.

Define Ionization energy

Paramagnetic is when an unpaired electron is attracted by an external magnetic field.

Define Paramagnetic

D

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

E

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

9.6 g

How many grams of CH3OH must be added to water to prepare 150mL of a solution that is 2.0 M CH3OH?

39.0 g

How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?

D

How many grams of KCl(s) are produced from the thermal decomposition of KClO3(s) which produces 50.0 mL of O2(g) at 25°C and 1.00 atm pressure according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)? A) 0. 167 g B) 0. 304 g C) 0. 152 g D) 0. 102 g

2.75 g

How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?

E

112) Identify the compound with covalent bonding. A) Li B) S C) He D) NaCl E) H2O

A

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? A) 71 g/mol B) 59 g/mol C) 5.9 g/mol D) 44 g/mol

D

A balloon contains 0.76 mol N2, 0.18 mol O2, 0.031 mol He and 0.026 mol H2 at 7 49 mm Hg. What is the partial pressure of O2? A) 23 mm Hg B) 20 mm Hg C) 570 mm Hg D) 140 mm Hg

4,000,000,000 bytes

A flash drive contains 4 gigabytes. How many bytes does it contain?

16.3 L

A mass of mercury occupies 0.950L. What volume would an equal mass of ethanol occupy? The density of mercury is 13.546g/mL and the density of ethanol is 0.789 g/mL.

No. The vaporized isopropyl alcohol is just in a different physical state. It still has mass and therefore the gas plus the remaining liquid and container have the same total mass after the vaporization of some of the isopropyl alcohol.

A sample of liquid isopropyl alcohol is placed in a sealed container. Some of the volatile isopropyl alcohol vaporizes. Does the mass of the sealed container and its contents change during the vaporization? Explain.

A

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution? A) 0. 274 M B) 3.65 M C) 0. 356 M D) 2.81 M

C

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP? a. 3.8atm b. 0.59atm c. 1.7atm d. 1.9atm e. 1.1atm

hydrosulfuric acid

An aqueous solution of H2S is named ________.

54

An atom of 131Xe contains __________ electrons.

17O2-

An ion has 8 protons, 9 neutrons, and 10 electrons. The symbol for the ion is __________.

C

At atmospheric pressure, dry ice ________. a. freezes b. deposits c. sublimes d. melts e. boils

A

Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 10.0 g of Fe2O3. ________ MgO(s) + ________ Fe(s) → ________ Fe2O3(s) + ________ Mg(s) A) 7.57 g B) 0.841 g C) 0.312 g D) 2.52 g

1 C9H20 + 14 O2 → 10 H2O + 9 CO2

Balance the following equation. _____ C9H20 + _____ O2 → _____ H2O + _____ CO2

The large increase in ionization energy between IE6 and IE7 shows that there are 6 valence electrons in this element. The only period 3 element that contains 6 valence electrons is S.

Below is a list of successive ionization energies (in kJ/mol) for a period 3 element. Identify the element and explain how you came to that conclusion. IE2 = 2250 IE3 = 3360 IE4= 4560 IE5= 7010 IE6= 8500 IE7 = 27,100

D

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H2O (l) → Ca(OH)2 (s) A 4.50-g sample of CaO is reacted with 4.34 g of H2O. How many grams of water remain after the reaction is complete? A) 0.00892 B) 0.161 C) 0.00 D) 2.90 E) 1.04

D

Calculate the kinetic energy of a 150 g baseball moving at a speed of 39. m/s ( 87 mph). A) 5.8 × 103 J B) 1.1 × 105 J C) 5.8 J D) 1.1 × 102 J

56.11%

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

D

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 A) +6.1 kJ B) +3.8 kJ C) -6.1 kJ D) -3.8 kJ

1. 10^3 2. 10^-2 3. 10^-3 4. 10^-9 5. 10^-6 6. 10^-1 7. 10^6

Conversion Factors 1. kilo- 2. centi- 3. milli- 4. nano- 5. micro- 6. deci- 7. mega-

E

Define triple point. a. The temperature, pressure, and density for a gas. b. The temperature at which the boiling point equals the melting point. c. The temperature that is unique for a substance. d. The temperature at which the solid and liquid co-exist. e. The temperature and pressure where solid, liquid, and gas are equally stable and in equilibrium.

A submicroscopic particle that constitutes the fundamental building block of ordinary matter

Define: Atom

Only can be observed while the chemical identity of a substance is changing, such as sodium metals tendency to react with water to form hydrogen gas and sodium hydroxide

Define: Chemical Property

Electrons in completed shells

Define: Core Electrons

Energy is the capacity to do work

Define: Energy

Energy is neither created nor destroyed

Define: Law of Conservation of Energy

Anything that occupies space and has mass

Define: Matter

Something that can be observed without changing the chemical identity of the substance, such as color or scent

Define: Physical Property

Electrons in the outermost shell

Define: Valence Electrons

A molecular formula is the exact number of each type of atom necessary to build a specific molecule. An empirical formula is simply the smallest whole number ratio between atoms in a compound. For example, C2H4 is the molecular formula for ethene. The empirical formula for ethene is CH2, the smallest whole number ratio between the elements.

Describe the difference between a molecular formula and an empirical formula. Give an example.

An ionic compound is formed between a metal and a nonmetal (or polyatomic ions) and is held together through the attraction of opposite charges. An example is NaCl. A molecular compound is usually formed between 2 or more nonmetals and is held together through the sharing of electrons between atoms. An example is CO2.

Describe the difference between ionic and molecular compounds. Give an example of each.

Ions have the loss or gain of electrons; isotopes differ in the number of neutrons

Describe the difference between ions and isotopes.

D

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

A

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.

D

Determine the electron geometry (eg) and molecular geometry (mg) of the underlined atom CH3OCH3. a. eg=tetrahedral, mg=tetrahedral. b. eg=linear, mg=linear. c. eg=trigonal bipyramidal, mg=tetrahedral. d. eg=tetrahedral, mg=bent. e. eg=octahedral, mg=square planar.

C

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

B

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution a. 0.0107 M b. 0.0337 M c. 0.0297 M d. 0.0936 M e. 0.0651 M

B

Determine the molecular formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen. a. C18H27NO2 b. C18H27NO3 c. C17H26NO3 d. C17H27NO3

+7

Determine the oxidation state of Mn in KMnO4.

Water molecules are polar and oil molecules are not polar.

Explain why oil and water do not mix.

B

For a particular process that is carried out at constant pressure, q = 145 kJ and w = -35 kJ. Therefore, A) ΔE=180kJ and ΔH=145kJ. B) ΔE=110kJ and ΔH=145kJ. C) ΔE=145kJ and ΔH=180kJ. D) ΔE=145kJ and ΔH=110kJ.

F, Cl, Br, I

Give an example of a halogen.

1. Mg 2. C 3. K 4. Fe 5. Si

Give the abbreviations for the following 1. magnesium 2. carbon 3. potassium 4. iron 5. silicon

E

Give the approximate bond angle for a molecule with an octahedral shape. A. 109.5° B. 180° C. 120° D. 105° E. 90°

D

How many different values of ml are possible in the 2p sub-level? A) 2 B) 7 C) 1 D) 3 E) 5

A

Give the change in condition to go from a liquid to a gas. a. increase heat or reduce pressure b. increase heat or increase pressure c. cool or reduce pressure d. cool heat or increase pressure e. none of the above

C

Give the complete electronic configuration for Br-. A) 1s2 2s2 p6 3s2 p6 4s2 3d10 4p6 B) 1s2 2s2 2p6 3s2 3p6 4s2 4p6 C) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 D) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 E) 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p6

D

Give the complete electronic configuration for Ca2+. A) 1s2 2s2 p6 3s2 p6 B) 1s2 2s2 2p6 3s2 3p5 C) 1s2 2s2 2p6 3s2 4p6 D) 1s2 2s2 2p6 3s2 3p6 E) 1s2 2s2 3p6 4s2 5p6

C

Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3. A. eg=tetrahedral, mg=trigonal planar, sp2 B. eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 C. eg=tetrahedral, mg=trigonal pyramidal, sp3 D. eg=trigonal pyramidal, mg=tetrahedral, sp3 E. eg=trigonal planar, mg=trigonal planar, sp2

[Kr]4d^10

Give the ground state electron configuration for Cd+2.

C

Give the hybridization for the S in SO3. a. sp b. sp3 c. sp2 d. sp3d e. sp3d2

2

Give the number of core electrons for Mg2+.

C

Give the number of pairs of valence electrons for BF3. A) 8 B) 14 C) 12 D) 16 E) 10

C

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

E

Give the number of valence electrons for SO42-. A) 34 B) 36 C) 28 D) 30 E) 32

D

Give the term for the temperature at which the gas and liquid phases form a supercritical fluid. a. Absolute temperature b. Definite temperature c. Fluid temperature d. Critical temperature e. Solid temperature

358

Given the equation: C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) (not balanced) Determine the number of liters of CO2 formed at STP when 240.0 grams of C2H6 is burned in excess oxygen gas.

706

Given the equation: C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) (not balanced) Determine the number of liters of O2 consumed at STP when 270.0 grams of C2H6 is burned.

An ionic compound that contains a polyatomic ion, such as NaNO3, has both ionic bonds (that hold the sodium and nitrate ions together) as well as covalent bonds (that hold the atoms within the nitrate ion together).

How can one compound contain both ionic and covalent bonds? Give an example.

A

How many compounds, of the ones listed below, have hydrogen bonding? CH3CH2CH2NH2; (CH3CH2)2NCH2CH3; CH3CH2NHCH2CH3 a. 2 b. 3 c. 1 d. 0

A

How many mL of O2 gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0. 300 grams of KClO3(s) according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g) A) 90.4 mL B) 40.2 mL C) 181 mL D) 30.1 mL

A

How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 1.38 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq) A) 102 mL B) 25.5 mL C) 51.1 mL D) 43.1 mL

E

How many millimoles of Ca(NO3)2 contain 4.78 × 1022 formula units of Ca(NO3)2? The molar mass of Ca(NO3)2 is 164.10 g/mol. a. 57.0 mmol Ca(NO3)2 b. 20.7 mmol Ca(NO3)2 c. 12.6 mmol Ca(NO3)2 d. 13.0 mmol Ca(NO3)2 e. 79.4 mmol Ca(NO3)2

0.0652 mol

How many moles are there in 3.00 g of ethanol, CH3CH2OH?

A

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl3(g) + 3 H2O(l) → 3 HCl(aq) + B(OH)3(aq) A) 0. 0914 mol B) 0.823 mol C) 0. 274 mol D) 10.9 mol

three

How many significant figures are there in the answer to the following problem? ( 9.992 × 3.200) + 0. 610 = ?

B

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? 5C(s)+2SO2(g)→CS2(l)+4CO(g) ΔH°=239.9kJ A) 898.5 kJ B) 179.8 kJ C) 2158 kJ D) 239.9 kJ

C

Identify a liquid a. No definite shape and no definite volume b. Definite volume and definite shape c. No definite shape and definite volume d. No definite volume and definite shape

D

Identify an ionic bond. A) Electrons are lost. B) Electrons are shared. C) Electrons are gained. D) Electrons are transferred. E) Electrons are pooled.

D

Identify the compound with ionic bonding. A) Li B) He C) H2O D) NaCl E) S

C

Identify the compound with metallic bonding. A) S B) NaCl C) Li D) He E) H2O

C

Identify the correct values for a 2p sublevel. A) n=1,l=0,ml=0 B) n=4,l=-1,ml=-2 C) n=2,l=1,ml=0 D) n=2,l=1,ml=-2 E) n=3,l=1,ml=0

D

Identify the place that has the lowest boiling point of water. a. Death Valley, 282 feet below sea level b. A pressurized passenger jet, 35,000 feet c. New Orleans, sea level d. Mt.Everest,29,035feet e. Denver, Colorado, 5280 feet

A

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube. a. capillary action b. viscosity c. surface tension d. density e. none of the above

C

If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to produce 32.0 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g) A) 81.7 g B) 283 g C) 126 g D) 53.1 g

A

In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be made from 3.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C. A) 1.36 L B) 0. 0975 L C) 1.33 L D) 1.30 L

C

In which set do all elements tend to form anions in binary ionic compounds? A) Li, Na, K B) C, S, Pb C) N, O, I D) K, Fe, Br

Yes. The polarity of a molecule depends on the molecular geometry and whether or not all of the dipoles (polar bonds) cancel one another. If the molecular geometry causes all of the dipoles to cancel, the molecule will be nonpolar. An example is CF4 where there are four polar bonds, but the dipoles sum to 0 making the molecule nonpolar.

Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

1. Combustion 2. Acid-Base 3. Oxidation Reduction 4. Gas Evolution 5. Precipitation

List the following as a combustion, oxidation reduction, precipitation, acid-base, gas evolution: 1) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) 2) H2SO4(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2SO4(aq) 3) Mg(s) + Cu(NO3)2(aq) → Mg(NO3)2(aq) + Cu(s) 4) HCl(aq) + (NH4)2S(aq) → H2S(g) + 2NH4Cl(aq) 5) NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)

Na+ and OH-

List the spectator ions in the following reaction: Ba+2(aq) + 2OH-(aq) + 2 Na+(aq) + CO3-2(aq) → 2 Na+(aq) + 2OH-(aq) + BaCO3 (s)

C

Lithium and nitrogen react to produce lithium nitride: 6Li(s)+N2(g) → 2Li3N(s) How many moles of N2 are needed to react with 0.500 mol of lithium? A) 0.500 B) 3.00 C) 0.0833 D) 1.50 E) 0.167

C

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+O2(g) → 2MgO(s) When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is __________ g. A) 4.00 B) 0.165 C) 6.63 D) 13.3 E) 3.32

1

Number of unpaired electrons in Na

2

Number of unpaired electrons in Ti2+

0

Number of unpaired electrons in Zn2+

B

Of the following elements, which has the highest electronegativity? A) Ti B) Cl C) Se D) S

A

Of the following elements, which has the lowest electronegativity? A) Ba B) Sr C) I D) At

A

Of the following, which element has the highest first ionization energy? A) carbon B) boron C) beryllium D) lithium

E

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

C

Place the following substances in order of decreasing boiling point. H2O N2 CO a. CO>H2O>N2 b. N2>CO>H2O c. H2O>CO>N2 d. CO>N2>H2O e. N2>H2O>CO

A

Place the following substances in order of increasing vapor pressure at a given temperature. NF3 NH3 BCl3 a. NH3 < NF3 < BCl3 b. NF3 < NH3 < BCl3 c. BCl3 < NF3 < NH3 d. NH3 < BCl3 < NF3 e. BCl3 < NH3 < NF3

B

Predict the actual bond angles in BrF3 using the VSEPR theory. a. more than 120° b. between 109° and 120° c. between 90° and 109° d. exactly 90° e. less than 90°

rubidium sulfide

Rb2S is named ____________.

Protons

The atomic number is equal to the number of

35

The atomic number of an atom of 80Br is __________.

Li2O2

The chemical formula for lithium peroxide is __________.

HNO2 (aq)

The chemical formula for nitrous acid is _________.

copper(II) iodate

The compound, Cu(IO3)2, is named ___________.

E

The density of krypton gas at 1.21 atm and 50.0°C is __________ g/L. A) 0.0456 B) 0.262 C) 0.295 D) 7.65 E) 3.82

Avogadro's number

The number, 6.022 x 1023 is called ________.

C

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? A) 7.7 × 102 J B) 0.0013 J C) 15 J D) 36 J E) 1.7 J

A

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

D

Use the molecular orbital diagram shown to determine which of the following are paramagnetic. a. O22− b. Ne22+ c. O22+ d. F22+ e. None of the above are paramagnetic

E

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 4SO3(g) →4S(s)+6O2(g) ΔH°rxn= ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g)→ 2 SO3(g) ΔH°rxn = -197.8 kJ A) -494.6 kJ B) -692.4 kJ C) -293.0 kJ D) -791.4 kJ E) 1583 kJ

A

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 A) 307.9 g B) 792.3 g C) 260.1 g D) 800.1 g

C

What is the charge on the Cr ions in Cr2O3? a. 2− b.1+ c.3+ d.2+ e.6+

B

What is the chemical formula for iron(III) sulfate? A) Fe3S B) Fe2(SO4)3 C) Fe2S3 D) Fe3SO4

0.29 M

What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Mg

What is the identity of element Q if the ion Q2+ contains 10 electrons?

60.5 g

What is the mass of 0.500 mol of dichlorodifluoro methane, CCl2F2?

D

What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C? A) 0.681 atm B) 0. 510 atm C) 1.16 atm D) 1.66 atm

Covalent Bonding

What type of bonding is found in the compound O F2?

D

When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed? AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq) A) 3.31 g B) 6.44 g C) 2.24 g D) 1.07 g

C

When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride? A) 9.40 g B) 18.8 g C) 8.44 g D) 11.9 g

A

Which element has the highest first electron affinity? A) O B) Mg C) Na D) Ne

C

Which ionization process requires the most energy? A) F(g)→ F+(g)+e- B) O+(g)→ O2+(g)+e- C) F+(g)→ F2+(g)+e- D) O(g)→ O+(g)+e-

He

Which noble gas has the highest ionization energy?

E

Which of the following are examples of extensive properties? a. Temperature b. Density c. Color d. Taste e. Mass

c

Which of the following is the lowest temperature? a. 42C b. 318K c. 57F d. All these temperatures are all equal

A

Which one of the following compounds contains ionic bonds? A) SrO B) SiO2 C) PBr3 D) HBr

Since elements in the same group have the same number of valence electrons (similar electron configurations) they tend to have similar chemical reactivity, since chemical reactions typically involve valence electrons.

Why do elements in the same group tend to have similar chemical properties?

The average atomic mass of silver is 107.9 amu, but there are no atoms of silver that weigh 107.9 amu. One isotope sighs more and another weighs less.

Why doesn't a mass spectrum of silver have a peak at 107.9 amu?