Chemistry II Lecture Final
Which one of the following will form an acidic solution in water? NaF KNO3 NH4Cl LiI None of the above solutions will be acidic.
NH4Cl
Which of the following molecules is polar? SF6 CCl4 BF3 NO2 CO2
NO2
What is the electron geometry (or electron arrangement) around an atom in a molecule or ion which is surrounded by one lone pair of electrons and four single bonds. trigonal bipyramidal see-saw or distorted tetrahedron T-shaped linear trigonal planar
Triagonal bipyramidal
When the concentrations of the reactants are increased, the rate of the reaction increases. This is best explained by an increase in the fraction of molecules that have enough energy to react. an increase in the rate constant. an increase in the average potential energy of the molecules. an increase in the frequency of the molecular collisions. an increase in the kinetic energy of the molecules.
an increase in the frequency of the molecular collisions.
The boiling point of a liquid is: always the temperature at which the vapor pressure equals 760 mmHg (1 atm). always the temperature at which the liquid phase of a substance is in equilibrium with the vapor phase. always the temperature at which the vapor pressure equals the pressure exerted on the liquid. always equal to the vapor pressure of the liquid at a given temperature. independent of the pressure exerted on the liquid.
always the temperature at which the vapor pressure equals the pressure exerted on the liquid.
For a reaction, what generally happens if the temperature is increased? a decrease in k occurs, which results in a slower rate an increase in k occurs, which results in a slower rate there is no change with k or the rate a decrease in k occurs, which results in a faster rate an increase in k occurs, which results in a faster rate
an increase in k occurs, which results in a faster rate
Identify oxidation. increase in oxidation number loss of electrons decrease in oxidation number gain of electrons both A and B
both A and B
If a reaction is zero-order in a reactant, when the concentration of the reactant is decreased by a factor of 2, the reaction rate will quadruple. decrease by a factor of 1/2. remain constant. decrease by a factor of 1/4. double.
remain constant
Which one of the following has a definite shape and volume? solid all of the above none of the above liquid gas
solid
The oxidation numbers of nitrogen in N2O and N2F4 are, respectively,
+1 and +2.
The oxidation number of chromium in sodium chromite, NaCrO2, is
+3.
Which of the following amounts of solute, dissolved in 1.0 kg of water, creates a solution with the lowest freezing temperature? (assuming ideal behavior) 0.0015 mol of sulfuric acid, H2SO4 0.0015 mol of H2SO3 0.0030 mol of ethanol, C2H5OH 0.0030 mol of methanol, CH3OH 0.0015 mol of sucrose, C12H22O11
0.0015 mol of sulfuric acid, H2SO4
Which of the following solutes, dissolved in 1.0 kg of water, creates a solution that boils at the highest temperature? 0.010 mol H3PO4 0.010 mol HClO4 0.010 mol H2SO4 0.010 mol HCl 0.010 mol HF
0.010 mol H2SO4
Which of the following solutes in aqueous solution would be expected to exhibit the smallest freezing-point lowering (assuming ideal behavior)? 0.1 m NaCl 0.2 m CH3COOH 0.05 m Al2(SO4)3 0.1 m MgCl2 0.25 m NH3
0.1 m NaCl
Which solution has the highest pH? 0.10 M HBr(aq) 0.10 M HI(aq) 0.10 M HF(aq) 0.10 M HCl(aq) 0.10 M HClO4(aq)
0.10 M HF(aq)
Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. 0.100 m MgCl2 0.100 m AlCl3 0.100 m C6H12O6 0.100 m NaCl They all have the same boiling point.
0.100 m AlCl3
Which of the following solutions would have the highest osmotic pressure? 0.15 M MgBr2 0.15 M NaCl 0.20 M C12H22O11 0.20 M C6H12O6 0.20 M CH3OH
0.15 M MgBr2
Which of the following forces is/are responsible for capillary action, a property of liquids? 1. attractive forces between the liquid and the capillary material 2. surface tension of the liquid 3. viscosity of the liquid
1 and 2
Which of the following concerning molecular geometry and dipole moments is/are correct? 1. Only molecules with polar bonds may have a permanent dipole moment. 2. All molecules with polar bonds have a permanent dipole moment. 3. All square planar molecules are nonpolar.
1 only
A single covalent bond contains __________ of electrons. 4 pairs 0 pairs 3 pairs 1 pair 2 pairs
1 pair
Which of the following concerning solutions is/are correct? 1. The solvent in a mixture of gases is generally considered to be the substance in greater amount. 2. The solid dissolved in a solution is known as the solute. 3. Solid solutions are called alloys.
1, 2, and 3
Which of the following concerning intermolecular forces is/are correct? 1. Intermolecular forces depend in part on the shape of a molecule. 2. London forces contribute to the net forces of attraction found in all molecular solids and liquids. 3. Hydrogen bonding is a special category of dipole-dipole attractions.
1, 2, and 3.
For which of the following values of the equilibrium constant does the reaction mixture contain mostly reactants? 10^0 10^1 10^-9 10^-1 10^9
10^-9
What is the overall order of the following reaction, given the rate law? X + 2 Y → 4 Z Rate = k[X][Y] 3rd order 5th order 1st order 0th order 2nd order
2nd order
For a dilute solution of (NH4)3PO4, the van't Hoff factor (i) would be approximately 4. 2. 3. 1. 5.
4
Give the number of valence electrons for ICl5. 40 44 36 46 42
42
In the I3- ion, how many electron groups surround the central atom? 5 3 6 4 2
5
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4. eg=octahedral, mg=square planar eg=tetrahedral, mg=bent eg=tetrahedral, mg=tetrahedral eg=linear, eg=linear eg=trigonal bipyramidal, mg=tetrahedral
???
Which of the following statements is incorrect concerning a catalyst? A catalyst decreases the activation energy of a reaction. A catalyst may appear in the rate law for a reaction. A catalyst alters the equilibrium distribution of reactants and products. There is no net consumption of a catalyst in a reaction. A catalyst provides an alternative reaction mechanism.
A catalyst alters the equilibrium distribution of reactants and products.
Which statement concerning the cathode in an electrochemical cell is correct? Metal ions may be deposited as metal atoms on the cathode during cell discharge. When connected to an external circuit, the cathode develops a positive charge. Reduction occurs at the cathode during cell discharge. Positive ions flow towards the cathode during cell discharge. All of the above.
All of the above.
Which of the following is TRUE? An neutral solution does not contain any H3O+ or OH- A neutral solution contains [H2O] = [H3O] A basic solution does not contain H3O+ An acidic solution has [H3O] > [OH] None of the above are true.
An acidic solution has [H3O] > [OH]
Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution? Br- HF H2SO3 H3O+ HNO3
Br-
Which compound has the lowest standard enthalpy of vaporization at 25°C? C6H14 C8H16 C5H12 C8H18 C7H16
C5H12
Which of the following bases is the WEAKEST? The base is followed by its Kb value. C5H5N, 1.7 × 10-9 (CH3CH2)3N, 5.2 × 10-4 NH3, 1.76 × 10-5 HOCH2CH2NH2, 3.2 × 10-5 Since these are all weak bases, they have the same strength.
C5H5N, 1.7 × 10-9
Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution. CH3CH2OCH2CH3, Kb = 1.79°C/m C6H6, Kb = 5.12°C/m CHCl3, Kb = 4.70°C/m CCl4, Kb = 29.9°C/m CH3CH2OH, Kb = 1.99°C/m
CCl4, Kb = 29.9°C/m
Identify the acid that is in vinegar. H2SO4 HF CH3COOH H2CO3 HNO3
CH3COOH
Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force. None of the above compounds exhibit hydrogen bonding. C2H6 CH2F2 CH3OH SCl2
CH3OH
Which molecule or compound below contains a pure covalent bond? NaCl PF3 Li2CO3 Cl2 SCl6
Cl2
Which of the following is an ionic solid? SiO2(s) Ne(s) Na(s) CsF(s) CO2(s)
CsF(s)
What is the strongest type of intermolecular force present in H2? dipole-dipole dispersion hydrogen bonding ion-dipole none of the above
Dispersion
Which of the following statements is TRUE? Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction. Dynamic equilibrium indicates that the amount of reactants and products are equal. The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction. A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products. All of the above are true.
Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCl is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing? Na+ OH- Na- F- none of these
F-
Place the following compounds in order of increasing strength of intermolecular forces. CO2 F2 NH2CH3
F2 < CO2 < NH2CH3
Identify the diprotic acid. HNO3 HCl HClO4 CH3COOH H2SO4
H2SO4
Identify the strongest acid. H2O H2S H2Te H2Se not enough information is available
H2Te MAYBE (NOT H2O)
Which of the following is NOT a conjugate acid-base pair? NH4+/NH3 H2SO3/HSO3- H3O+/OH- C2H3O2-/HC2H3O2 All of the above are conjugate acid-base pairs.
H3O+/OH-
Place the following in order of increasing acid strength. HBrO2 HBrO3 HBrO HBrO4
HBrO HBrO2 HBrO3 HBrO4
Which of the following is a WEAK acid? HNO3 HCO2H H2SO4 HCl HClO4
HCO2H
Rank the following in order of decreasing acid strength in aqueous solution: HCl, HOCl, HOBr, HOI.
HCl > HClO > HBrO > HIO
Which of the following acids is the STRONGEST? The acid is followed by its Ka value. HCHO2, 1.8 × 10-4 HCN, 4.9 × 10-10 HF, 3.5 × 10-4 HClO2, 1.1 × 10-2 HNO2, 4.6 × 10-4
HClO2, 1.1 × 10-2
Identify the strongest acid. HClO HClO3 HClO4 HClO2 Not enough information is given.
HClO4
Which of the following pairs of species is not a conjugate acid-base pair? HOCl, OCl- HNO2, NO2+ O2-, OH- HSO4-, SO42- H2CO3, HCO3-
HNO2, NO2+
What is the conjugate base of H2PO4- ? HPO42- OH H3O+ PO43- H3PO4
HPO42-
What is the conjugate base of H2PO4-(aq)? PO43- H3O+ HPO42- H3P H3PO4
HPO42-
Why does hydrogen fluoride have an unusually high normal boiling point compared to the other hydrogen halides? The H-F bond in hydrogen fluoride is very strong. Hydrogen fluoride has very strong London dispersion forces. Hydrogen fluoride is capable of forming hydrogen bonds. Hydrogen fluoride is ionic. Hydrogen fluoride is covalent.
Hydrogen fluoride is capable of forming hydrogen bonds.
Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 M sucrose II. 0.00095 M glucose III. 0.0060 M glycerin
I > III > II
How does the solubility of a gas in a solvent depend on pressure and temperature? Increasing the partial pressure of the gas while increasing the temperature increases the solubility of the gas. Decreasing the partial pressure of the gas while decreasing the temperature increases the solubility of the gas. Increasing the partial pressure of the gas while decreasing the temperature increases the solubility of the gas. Decreasing the partial pressure of the gas while increasing the temperature increases the solubility of the gas. Gas solubility is unaffected by pressure or temperature.
Increasing the partial pressure of the gas while decreasing the temperature increases the solubility of the gas.
Identify the type of solid for AgCl. metallic atomic solid ionic solid nonbonding atomic solid networking atomic solid molecular solid
Ionic solid
For a specific reaction, which of the following statements can be made about the equilibrium constant? It can be changed by the addition of a catalyst. It increases when the concentration of one of the products is increased. It increases when the concentration of one of the reactants is increased. It always remains the same. It changes with changes in the temperature.
It changes with changes in the temperature.
Which of the following salts will produce a neutral solution when added to pure water? LiHCO3 NH4NO3 Na2SO4 RbNO2 KNO3
KNO3 Maybe (NOT RbNO2)
The strongest intermolecular forces present in a sample of pure I2 are London forces. dipole-dipole forces. metallic bonds. covalent network bonds. covalent bonds.
London forces
Based on the formulas of the following solutes, which compound would have the smallest van't Hoff factor (i)? Ca(NO3)2(aq) K2SO4(aq) Th(SO4)2(aq) Al2(SO4)3(aq) MgSO4(aq)
MgSO4(aq)
In a table of standard reduction potentials, the strongest reducing agents are the _______ species in the half-reactions with the _______ E° values. reduced, most negative oxidized, most positive reduced, most positive oxidized, most negative none of these
NOT oxidized, most positive
Identify the base that is in baking soda. NH3 NaHCO3 NaOH Na2CO3 KOH
NaHCO3
Which of the following is a correct statement of Henry's law? The concentration of a gas in solution is directly proportional to the mole fraction of solvent. The concentration of a gas in solution is inversely proportional to temperature. The concentration of a gas in solution is independent of pressure. The concentration of a gas in a solution is inversely proportional to pressure. none of these
None of these. Why???
Which one of the following statements provides the best evidence that all the carbon compounds listed below have tetrahedral molecular geometries instead of square planar molecular geometries? Only one CH4 compound is known and it is nonpolar. Only one CH3F compound is known and it is polar. Only one CH2F2 compound is known and it is polar. Only one CF4 compound is known and it is nonpolar. Only one CHF3 compound is known and it is polar.
Only one CH2F2 compound is known and it is polar.
Which one of the following salts, when dissolved in water, produces the solution with the highest pH? CsClO4 KHCO3 CH3CH3NH3Cl RaO
RaO
Which of the following statements is true in a reaction system at equilibrium? The equilibrium constant is zero. The number of collisions per unit time between reactants is equal to the number of collisions per unit time between products. Reactants are reacting to form products at the same rate as products are reacting to form reactants. Reactants and products are present in equimolar amounts. The product of the concentrations of the products divided by the product of the concentrations of the reactants is always a constant.
Reactants are reacting to form products at the same rate as products are reacting to form reactants.
Which molecule is polar? C2H4 CS2 C6H6 SO2 CF4
SO2
Which of the following substances has the weakest intermolecular forces? I2 C8H18 SiH4 CH3CH2CH2CH2OH SbCl3
SiH4
Place the following elements in order of increasing electronegativity. Sr N Na
Sr < Na < N
Which of the following statements is true for a voltaic (galvanic) cell? The electron flow is from the anode to the cathode. The electron flow is from the positive electrode to the negative electrode. The electron flow is from the negative cathode to the positive anode. The electron flow is through the salt bridge. The electron flow is from the oxidizing agent to the reducing agent through an external circuit.
The electron flow is from the anode to the cathode.
Give the direction of the reaction, if K >> 1. Neither direction is favored. The forward reaction is favored. The reverse reaction is favored. If the temperature is raised, then the reverse reaction is favored. If the temperature is raised, then the forward reaction is favored.
The forward reaction is favored.
Give the reason that antifreeze is added to a car radiator. The freezing point is elevated and the boiling point is lowered. The freezing point and the boiling point are elevated. The freezing point is lowered and the boiling point is elevated. None of the above. The freezing point and the boiling point are lowered.
The freezing point is lowered and the boiling point is elevated.
Which of the following sets of conditions favors maximum solubility of solute in solvent? The intermolecular forces between solute and solvent molecules are much weaker than the intermolecular forces between solute molecules, but much stronger than the intermolecular forces between solvent molecules. The intermolecular forces between solute and solvent molecules are much stronger than the intermolecular forces between solute molecules or the intermolecular forces between solvent molecules. The intermolecular forces between solute and solvent molecules are much stronger than the intermolecular forces between solvent molecules, but much weaker than the intermolecular forces between solute molecules. The intermolecular forces between solute and solvent molecules are much stronger than the intermolecular forces between solute molecules, but much weaker than the intermolecular forces between solvent molecules. The intermolecular forces between solute and solvent molecules are much weaker than the intermolecular forces between solute molecules or the intermolecular forces between solvent molecules.
The intermolecular forces between solute and solvent molecules are much stronger than the intermolecular forces between solute molecules or the intermolecular forces between solvent molecules.
What will happen if a small amount of hydrochloric acid is added to a 0.1 M solution of HF? The percent ionization of HF will decrease. Ka for HF will increase. Ka for HF will decrease. The percent ionization of HF will remain unchanged. The percent ionization of HF will increase.
The percent ionization of HF will decrease.
Which of the following statements is incorrect? The rates of most chemical reactions change with time. The rate constant for a reaction can be changed by changing the temperature. The rate constant is dependent on the reactant concentrations. In a series of step-wise reactions, the rate-determining step is the slowest one. The rate of a catalyzed reaction is dependent on the concentration of the catalyst.
The rate constant is dependent on the reactant concentrations.
Which of the following statements is always true? Exothermic reactions have lower activation energies than endothermic reactions. The rate of a catalyzed reaction is independent of the concentration of the catalyst. The rate for a reaction depends on the concentrations of all the reactants. The rate constant is independent of the concentrations of the reacting species. The rate law can be determined from the stoichiometric equation.
The rate constant is independent of the concentrations of the reacting species.
Given the following rate law, how does the rate of reaction change if the concentration of X is doubled? Rate = k [X][Y]2 The rate of reaction will increase by a factor of 2. The rate of reaction will decrease by a factor of 2. The rate of reaction will increase by a factor of 4. The rate of reaction will increase by a factor of 5. The rate of reaction will remain unchanged.
The rate of reaction will increase by a factor of 2
Give the characteristic of a zero order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant. The rate of the reaction is proportional to the square root of the concentration of the reactant.
The rate of the reaction is not proportional to the concentration of the reactant
Which of the following statements is TRUE? The solubility of a gas is highly dependent on both pressure and temperature. The solubility of a gas is highly dependent on pressure. The solubility of a gas is highly dependent on temperature. The solubility of a gas is not dependent on either temperature or pressure. None of the above.
The solubility of a gas is highly dependent on both pressure and temperature.
A cucumber is placed in a concentrated salt solution. What is most likely to happen? Water will flow from the solution to the cucumber. No change will occur. Salt will flow into the cucumber. Salt will precipitate out. Water will flow from the cucumber to the solution.
Water will flow from the cucumber to the solution.
Which of the following represents a dynamic equilibrium? a stoppered flask half full of water a coin spinning in mid-air two people of equal mass balanced on the ends of a seesaw an open pan of boiling water an object traveling at a constant speed
a stoppered flask half full of water
The rates of most chemical reactions are sensitive to a change in the temperature of the reaction system. The increase in rate as the temperature increases is best explained by an increase in the collision frequency. an increase in the number of high-energy molecules. a decrease in the collision frequency. an increase in the activation energy. a decrease in the activation energy.
an increase in the number of high-energy molecules.
A solution containing less than the equilibrium amount is called __________. a saturated solution an unsaturated solution a dilute solution a concentrated solution a supersaturated solution
an unsaturated solution
Which of the following conversions is not an oxidation-reduction reaction? conversion of Mn2O3 to MnO2 conversion of K to KCl conversion of NaBr to Br2 conversion of CaCO3 to CaO conversion of VO2+ to VO2+
conversion of CaCO3 to CaO
The forces between polar molecules is known as __________. ion-dipole forces dipole-dipole forces hydrogen bonding ionic forces dispersion forces
dipole-dipole
The strongest intermolecular forces between molecules of PH3 are hydrogen bonds. covalent bonds. ionic bonds. London forces. dipole-dipole attractions.
dipole-dipole
What is the strongest type of intermolecular force present in CHF3? none of the above ion-dipole dispersion hydrogen bonding dipole-dipole
dipole-dipole
Which of the following is a molecular solid? carborundum, SiC quartz glass hydrogen chloride potassium
hydrogen chloride
Fluids used for an intravenous transfusion must be __________ with bodily fluids. isosmotic neosmotic hyposmotic magnosmotic hyperosmotic
isosmotic
Identify the battery that is in most automobiles. lead-acid storage battery lithium ion battery dry-cell battery fuel cell NiCad battery
lead-acid storage battery
The catalyzed pathway in a reaction mechanism has a __________ activation energy and thus causes a __________ reaction rate. higher, lower higher, higher higher, steady lower, higher lower, steady
lower, higher
A solution of two liquids, A and B, shows negative deviation from Raoult's law. This means that the two liquids have a positive heat of solution. molecules of A interact more strongly with B than A molecules interact with A or B molecules interact with B. molecules of A interact strongly with other A-type molecules. molecules of A interact weakly, if at all, with B molecules. molecules of A hinder the strong interaction between B molecules.
molecules of A interact more strongly with B than A molecules interact with A or B molecules interact with B
The molality of a solution is defined as moles of solute per liter of solution. the gram molecular weight of solute per kilogram of solvent. moles of solute per kilogram of solvent. grams of solute per liter of solution. moles of solute per kilogram of solution.
moles of solute per kilogram of solvent
Which one of the following liquids would you expect to have the highest vapor pressure at room temperature? (all boiling points are normal boiling points) n-pentane, b.p. = 36.1°C methanol, b.p. = 65.0°C carbon tetrachloride, b.p. = 76.7°C acetic acid, b.p. = 118°C mercury, b.p. = 357°C
n-pentane, b.p. = 36.1°C
In general, which of the following type(s) of solid(s) would exhibit the greatest solubility in a nonpolar solvent? network covalent nonpolar molecular ionic metallic polar molecular
nonpolar molecular
What is the electron geometry (or electron arrangement) around an atom in a molecule or ion which is surrounded by one lone pair of electrons and five single bonds. octahedral square pyramidal square planar bent linear
octahedral
In a chemical reaction at constant temperature, the addition of a catalyst provides an alternative reaction pathway with a different activation energy. increases the concentration of the products at equilibrium. affects the equilibrium constant. increases the fraction of molecules with more than a given kinetic energy. decreases the energy released in the chemical reaction.
provides an alternative reaction pathway with a different activation energy
Which of the following solutions has the highest hydroxide-ion concentration? 0.1 M HCl a solution with pH = 5 0.1 M H2SO4 pure water a solution with pOH = 12
pure water
The following reaction is exothermic. Which change will shift the equilibrium to the left? 2 SO2(g) + O2(g) 2 SO3(g) adding argon raising the temperature adding a solid all of the above none of the above
raising the temperature
Which rate law is bimolecular? rate = k [A][B][C][D] rate = k[A][B]2 rate = k [A][A][B] rate = k [A][B] rate = k [A]
rate = k [A][B]
What is the name for the following phase change? I2(s) -------> I2(g) sublimation freezing vaporization condensation melting
sublimation
In a liquid, the energy required to increase the surface of the area by a unit amount is called __________.
surface tension
Identify the location of oxidation in an electrochemical cell. the anode the salt bridge the cathode the socket the electrode
the anode
Define sublimation. the phase transition from liquid to gas the phase transition from liquid to solid the phase transition from gas to liquid the phase transition from gas to solid the phase transition from solid to gas
the phase transition from solid to gas
Identify the rate-determining step. the fast step the slowest step always the second step the faster step always the last step
the slowest step
The fact that the boiling point of a pure solvent is lower than the boiling point of a solution of the same solvent is a direct consequence of the freezing-point depression of the solution. vapor pressure of the solution being higher than the vapor pressure of the pure solvent. osmotic pressure of the solvent being lower than the osmotic pressure of the solution. vapor pressure of the solution being lower than the vapor pressure of the pure solvent. osmotic pressure of the solvent being higher than the osmotic pressure of the solution.
vapor pressure of the solution being lower than the vapor pressure of the pure solvent.
The measure of the resistance to flow of a liquid is London forces. van der Waals forces. viscosity. vapor pressure. surface tension.
viscosity
