General Chemistry II Exam Review
Course Introduction
General Chemistry II builds upon fundamental concepts introduced in General Chemistry I, delving deeper into chemical reactions, equilibria, thermodynamics, kinetics, acids and bases, electrochemistry, and coordination chemistry. The course emphasizes problem-solving, quantitative reasoning, and laboratory techniques pertinent to chemical analysis. Students explore topics such as solubility, entropy, enthalpy, Gibbs free energy, reaction rates, buffer systems, and the properties of solutions. Through lectures, laboratory experiments, and collaborative activities, learners develop a comprehensive understanding of chemical principles and their applications in real-world contexts, providing a strong foundation for advanced studies in chemistry and related fields.
Recommended Textbook
Chemistry A Molecular Approach 4th Edition by Nivaldo J. Tro
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Page 2
Chapter 1: Matter, measurement, and Problem Solving
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169 Verified Questions
169 Flashcards
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Sample Questions
Q1) Household ammonia is an example of A) a compound.
B) an element.
C) a heterogeneous mixture.
D) a homogeneous mixture.
Answer: D
Q2) Round off 00507506 to four significant figures.
A) 0051
B) 5076
C) 5100
D) 5.075 × 10<sup>5</sup>
Answer: D
Q3) Identify a unit that is used for area.
A) L<sup> </sup>
B) yd
C) yd<sup>2</sup>
D) Kelvin
E) m
Answer: C
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Page 3
Chapter 2: Atoms and Elements
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Sample Questions
Q1) Rutherford proposed the
A) atomic bomb.
B) hydroelectric.
C) First Law of Conservation.
D) theory of explosives.
E) nuclear theory.
Answer: E
Q2) Calculate the mass (in g)of 2.1 × 10<sup>24</sup> atoms of W.
A) 3.9 × 10<sup>2</sup> g
B) 2.4 × 10<sup>2</sup> g
C) 3.2 × 10<sup>2</sup> g
D) 1.5 × 10<sup>2</sup> g
E) 6.4 × 10<sup>2</sup> g
Answer: E
Q3) Which element has the chemical symbol,Rn?
A) radium
B) radon
C) rhenium
D) rhodium
Answer: B
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Chapter 3: Molecules,compounds,and Chemical Equations
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Sample Questions
Q1) Which of the following exists as a polyatomic molecule?
A) neon
B) carbon
C) phosphorus
D) lithium
E) argon
Answer: C
Q2) An ionic bond is best described as
A) the sharing of electrons.
B) the transfer of electrons from one atom to another.
C) the attraction that holds the atoms together in a polyatomic ion.
D) the attraction between two nonmetal atoms.
E) the attraction between two metal atoms.
Answer: B
Q3) Give the mass percent of carbon in C<sub>14</sub>H<sub>19</sub>NO<sub>2</sub>.
A) 72.07%
B) 8.21%
C) 6.00%
D) 13.72%
Answer: A
Page 5
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Chapter 4: Chemical Quantities and Aqueous Reactions
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Sample Questions
Q1) Determine the oxidation state of nitrogen in LiNO<sub>3</sub>.
A) +5
B) +3
C) -1
D) +2
E) -4
Q2) The titration of 25.0 mL of an unknown concentration H<sub>2</sub>SO<sub>4</sub> solution requires 83.6 mL of 0.12 M LiOH solution.What is the concentration of the H<sub>2</sub>SO<sub>4</sub> solution (in M)?
A) 0.20 M
B) 0.40 M
C) 0.10 M
D) 0.36 M
E) 0.25 M
Q3) The mixing of which pair of reactants will result in a precipitation reaction?
A) Mg(NO<sub>3</sub>)<sub>2</sub>(aq) + K<sub>2</sub>CO<sub>3</sub>(aq)
B) Na<sub>2</sub>SO<sub>4</sub>(aq) + Cu(NO<sub>3</sub>)<sub>2</sub>(aq)
C) LiClO<sub>4</sub>(aq) + (NH<sub>4</sub>)<sub>2</sub>S(aq)
D) NH<sub>4</sub>Cl(aq) + NH<sub>4</sub>I(aq)
Q4) Describe the greenhouse effect.
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Chapter 5: Gases
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Sample Questions
Q1) The rate of effusion of two different gases is known as
A) Avogadro's Law.
B) Graham's Law.
C) Charles's Law.
D) Boyle's Law.
E) Dalton's Law.
Q2) Which of the following would have a density of 0.172 g/L at 7.0°C and 0.987 atm?
A) Ar<sub> </sub>
B) He<sub> </sub>
C) Ne
D) Rn
E) SO<sub>2</sub>
Q3) Give the temperature and pressure at STP.
A) 0°C and 1.00 atm
B) 0K and 760 torr
C) 25°C and 760 in Hg
D) 300 K and 1 torr Hg
E) 0°C and 1 mm Hg
Q4) Why does HOT air rise?
Q5) Define effusion.
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Chapter 6: Thermochemistry
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Sample Questions
Q1) When 50.0 mL of 0.400 M Ca(NO<sub>3</sub>)<sub>2</sub> is added to 50.0 mL of 0.800 M NaF,CaF<sub>2</sub> precipitates,as shown in the net ionic equation below.The initial temperature of both solutions is 22.0°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. Ca<sup>2+</sup>(aq)+ 2 F<sup>-</sup>(aq) CaF<sub>2</sub>(s) H° = -11.5 kJ
A) 21.45°C
B) 22.55°C
C) 23.10°C
D) 23.65°C
Q2) Give the units of specific heat capacity.
A) Jg/°F
B)( <sup>J</sup>/g °C)
C) J/mole °C
D) g/°C
E) gmole °F
Q3) Describe the energy changes that occur when a book is held 6 ft off the floor and then dropped.
Q4) Define chemical energy.
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Chapter 7: The Quantum-Mechanical Model of the Atom
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Sample Questions
Q1) A sunburn is caused by overexposure to ________ radiation.
A) ultraviolet
B) gamma
C) microwave
D) x-ray
E) radio
Q2) The number of cycles that pass through a stationary point is called
A) wavelength.
B) amplitude.
C) frequency.
D) area.
E) median.
Q3) How many photons are contained in a burst of yellow light (589 nm)from a sodium lamp that contains 623 kJ of energy?
A) 2.10 × 10<sup>13</sup> photons
B) 3.06 × 10<sup>30</sup> photons
C) 1.85 × 10<sup>24</sup> photons
D) 4.03 × 10<sup>28</sup> photons
E) 2.48 × 10<sup>25</sup> photons
Q4) Define diffraction.
9
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Chapter 8: Periodic Properties of the Elements
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Sample Questions
Q1) 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.
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 is true.
Q2) List the noble gas that has the highest ionization energy.
Q3) How many of the following species are diamagnetic? Cs Zr<sup>2</sup> Al<sup>3</sup> Hg<sup>2</sup>
A) 1
B) 3
C) 0
D) 2
E) 4
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Page 10
Chapter 9: Chemical Bonding I: Lewis Theory
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Sample Questions
Q1) Choose the bond below that is most polar.
A) H-Cl
B) H-P
C) H-F
D) H-Si
E) As-H
Q2) Which of the following processes is endothermic?
A) the reaction associated with the lattice energy of LiI.
B) the reaction associated with the ionization energy of potassium.
C) the reaction associated with the heat of formation of SrO.
D) the formation of CO<sub>2</sub> from its elements in their standard states.
E) None of the above is endothermic.
Q3) Give the complete electronic configuration for Ca<sup>2+</sup>.
A) 1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>4p<sup>6</sup>
B) 1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>
C) 1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>5</sup>
D) 1s<sup>2</sup>2s<sup>2</sup>3p<sup>6</sup>4s<sup>2</sup>5p<sup>6</sup>
E) 1s<sup>2</sup>2s<sup>2</sup>p<sup>6</sup>3s<sup>2</sup>p<sup>6</sup>
Q4) Define bond energy.
Q5) List the least electronegative atom.
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Chapter 10: Chemical Bonding Ii: Molecular Shapes,valence
Bond Theory,
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Sample Questions
Q1) Give the hybridization for the Br in BrO<sub>4</sub> .
A) sp
B) sp<sup>3</sup>d<sup>2</sup>
C) sp<sup>3</sup>d
D) sp<sup>3</sup>
E) sp<sup>2</sup>
Q2) Choose the compound below that contains at least one polar covalent bond,but is nonpolar.
A) HCN
B) CBr<sub>4</sub>
C) SeBr<sub>4</sub>
D) ICl<sub>3</sub>
E) Both B and C are nonpolar and contain a polar covalent bond.
Q3) Determine the electron geometry (eg)and molecular geometry (mg)of the underlined carbon in CH<sub>3</sub>F.
A) eg = tetrahedral, mg = tetrahedral
B) eg = linear, mg = trigonal planar
C) eg = trigonal planar, mg = tetrahedral
D) eg = linear, mg = bent
E) eg = tetrahedral, mg = trigonal planar
Page 12
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Chapter 11: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) How much energy must be removed from a 125 g sample of benzene (molar mass = 78.11 g/mol)at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful.
H<sub>vap</sub> = 33.9 kJ/mol
H<sub>fus</sub> = 9.8 kJ/mol
C<sub>liq</sub> = 1.73 J/g°C
C<sub>gas </sub>= 1.06 J/g°C
C<sub>sol</sub> = 1.51 J/g°C
T<sub>melting </sub>= 279.0 K
T<sub>boiling</sub> = 353.0 K
A) 38.9 kJ
B) 95.4 kJ
C) 67.7 kJ
D) 54.3 kJ
E) 74.4 kJ
Q2) Define viscosity.
Q3) Why is the H<sub>vap</sub> higher than H<sub>fus </sub>for a given compound?
Q4) Define boiling point of a liquid.
Q5) Define dynamic equilibrium.
Q6) Define volatile.
Page 13
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Chapter 12: Solids and Modern Materials
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Sample Questions
Q1) Identify a use for ceramics.
A) beakers
B) bridges
C) furniture
D) wooden decks
E) bricks
Q2) Identify the technique that determines the arrangement of atoms and measures the distance between them.
A) x-ray diffraction
B) ultraviolet
C) nuclear magnetic resonance
D) infrared
E) atomic absorption
Q3) Identify an element that is NOT in silicate ceramics.
A) oxygen
B) silicon
C) aluminum
D) carbon
E) hydrogen
Q4) Describe the difference between the conduction band and the valence band.
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Chapter 13: Solutions
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Sample Questions
Q1) ______ is burped up from the bottom of a water-filled volcanic crater.
A) Carbon monoxide
B) Oxygen
C) Nitrogen
D) Hydrogen
E) Carbon dioxide
Q2) Determine H<sub>solute</sub> for KBr if the H<sub>solution </sub>(KBr)= +19.9 kJ/mol and the H<sub>hydration</sub>(KBr)= -670.kJ/mol.
A) +650 kJ/mol
B) -650 kJ/mol
C) +690 kJ/mol
D) -710 kJ/mol
E) -690 kJ/mol
Q3) A solid can be purified through what technique?
A) recrystallization
B) dilution
C) dissolution
D) boiling
E) melting
Q4) Define osmosis.
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Chapter 14: Chemical Kinetics
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Sample Questions
Q1) In the hydrogenation of double bonds,a catalyst is needed.In the third step,the reactants react to form the product.This step is known as
A) adsorption.
B) diffusion.
C) reaction.
D) desorption.
E) none of the above
Q2) Given the following rate law,how does the rate of reaction change if the concentration of X is doubled? Rate = k[X][Y]<sup>3</sup>
A) The rate of reaction will increase by a factor of 2.
B) The rate of reaction will increase by a factor of 8.
C) The rate of reaction will increase by a factor of 6.
D) The rate of reaction will decrease by a factor of 2.
E) The rate of reaction will remain unchanged.
Q3) Define activation energy.
Q4) Define half-life.
Q5) Define the frequency factor.
Q6) Explain what the exponential factor in the Arrhenius equation represents.
Q7) Explain how the order of a reaction can be determined.
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) The reaction below has a K<sub>p</sub> value of 41.What is the value of K<sub>c</sub> for this reaction at 400 K? N<sub>2</sub>(g)+ 3 H<sub>2</sub>(g) 2 NH<sub>3</sub>(g)
A) 3.8 × 10<sup>-2</sup>
B) 4.4 × 10<sup>4</sup>
C) 26
D) 2.3 × 10<sup>-5</sup>
E) 41
Q2) Determine the value of K<sub>c</sub> for the following reaction if the equilibrium concentrations are as follows: [P<sub>4</sub>O<sub>10</sub>]<sub>eq </sub>= 2.000 moles,[P<sub>4</sub>]<sub>eq</sub> = 3.000 moles,[O<sub>2</sub>]<sub>eq</sub> = 4.000 M P<sub>4</sub>O<sub>10</sub>(s) P<sub>4</sub>(s)+ 5 O<sub>2</sub>(g)
A) 20.00
B) 4.000
C) 1.320
D) 1536
E) 1024
Q3) How is the reaction quotient different from an equilibrium constant for a given reaction?
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Chapter 16: Acids and Bases
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Sample Questions
Q1) Determine the pH of a 0.62 M NH<sub>4</sub>NO<sub>3</sub> solution at 25°C.The K<sub>b</sub> for NH<sub>3</sub> is 1.76 × 10<sup>-5</sup>.
A) 2.48
B) 9.27
C) 11.52
D) 4.73
E) 9.45
Q2) Determine the pOH of a 0.00598 M HClO<sub>4</sub> solution.
A) 11.777
B) 6.434
C) 7.566
D) 2.223
E) 3.558
Q3) Determine the pOH of a 0.741 M LiOH solution at 25°C.
A) 0.130
B) 13.87
C) 0.741
D) 13.26
E) 1.48
Q4) What is the autoionization of water?
Page 18
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Chapter 17: Aqueous Ionic Equilibrium
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Sample Questions
Q1) Identify the most common indicator.
A) alizarin
B) thymol blue
C) crystal violet
D) phenolphthalein
E) thymolphthalein
Q2) You wish to prepare an HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> buffer with a pH of 5.14.If the pK<sub>a</sub> of is 4.74,what ratio of C<sub>2</sub>H<sub>3</sub>O<sub>2</sub><sup>-</sup>/HC<sub>2</sub>H<sub>3</ sub>O<sub>2</sub> must you use?
A) 0.10
B) 0.30
C) 0.40
D) 2.51
E) 5.0
Q3) Consider the K<sub>sp</sub> values for two compounds: MZ,K<sub>sp</sub> = 1.5 × 10<sup>-2</sup><sup>0</sup> and MZ<sub>2</sub>,K<sub>sp</sub> = 1.5 × 10<sup>-20</sup>.Why don't these compounds have the same molar solubility?
Q4) Define a buffer.
Page 19
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Chapter 18: Free Energy and Thermodynamics
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Sample Questions
Q1) Which of the following processes has a S > 0?
A) 2 NH<sub>3</sub>(g) + CO<sub>2</sub>(g) NH<sub>2</sub>CONH<sub>2</sub>(aq) + H<sub>2</sub>O(l)
B) lithium fluoride forms from its elements
C) 2 HCl(g) H<sub>2</sub>(g) + Cl<sub>2</sub>(l)
D) cesium chloride dissolves in pure water
E) All of the above processes have a S > 0.
Q2) Determine the equilibrium constant for the following reaction at 655 K. HCN(g)+ 2 H<sub>2</sub>(g) CH<sub>3</sub>NH<sub>2</sub>(g) H° = -158 kJ; S°= -219.9 J/K
A) 3.99 × 10<sup>12</sup>
B) 13.0
C) 2.51 × 10<sup>-13</sup>
D) 3.26 × 10<sup>-12</sup>
E) 3.07 × 10<sup>11</sup>
Q3) Why can't we say that a spontaneous reaction is a fast reaction?
Q4) Why can endothermic reactions be spontaneous?
Q5) Define the third law of thermodynamics.
Q6) How is a nonspontaneous process made spontaneous?
Q7) Define entropy.
Page 20
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Chapter 19: Electrochemistry
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Sample Questions
Q1) Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Br<sub>2 </sub>and OH in the balanced reaction? Br<sub>2</sub>(l) BrO<sub>3</sub> (aq)+ Br (aq)
A) Br<sub>2 </sub>= 1, OH = 2
B) Br<sub>2 </sub>= 2, OH = 5
C) Br<sub>2 </sub>= 3, OH = 3
D) Br<sub>2 </sub>= 3, OH = 6
E) Br<sub>2 </sub>= 1, OH = 6
Q2) What is the shorthand notation that represents the following galvanic cell reaction? Pb(s)+ Cu(NO<sub>3</sub>)<sub>2</sub>(aq) Pb(NO<sub>3</sub>)<sub>2</sub>(aq)+ Cu(s)
A) Pb(s) Pb<sup>2+</sup>(aq) Cu<sup>2+</sup>(aq) Cu(s)
B) Cu(s) Cu<sup>2+</sup>(aq) Pb<sup>2+</sup>(aq) Pb(s)
C) Pb(s) NO<sub>3</sub><sup>-</sup>(aq) NO<sub>3</sub><sup>-</sup>(aq) Cu(s) D) Cu(s) Cu(NO<sub>3</sub>)<sub>2</sub>(aq) Pb(NO<sub>3</sub>)<sub>2</sub>(aq) Pb(s)
Q3) Why is sugar water NOT a good conductor of current?
Q4) What is the difference between a voltaic cell and an electrolytic cell?
Q5) Why are iron nails coated with zinc?
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Chapter 20: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Atoms with Z > ________ are radioactive and decay in one or more steps involving mostly alpha and beta decay.
A) 72
B) 130
C) 83
D) 150
E) 30
Q2) An archaeologist graduate student found a leg bone of a large animal during the building of a new science building.The bone had a carbon-14 decay rate of 14.8 disintegrations per minute per gram of carbon.Living organisms have a decay rate of 15.3 disintegrations per minute.How old is the bone?
A) 53.3 years
B) 275 years
C) 111 years
D) 25 years
E) 83 years
Q3) Explain the concept of "magic numbers."
Q4) Define radioactivity.
Q5) What is the "mass defect"?
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Chapter 21: Organic Chemistry
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Sample Questions
Q1) Which of the following names is correct?
A) 2-methyl-5-heptyne
B) 2-ethyl-5-heptyne
C) 5-ethyl-2-hexyne
D) 4-pentyl-1-pentyne
E) 5-methyl-2-decyne
Q2) ________ is used in welding.
A) Propyne
B) 2-butyne
C) 1-butyne
D) Ethyne
E) 1-pentyne
Q3) Which of the following alkane names is correct?
A) 1,2-dipropylhexane
B) 1-propylnonane
C) 4,5-dipropylpentane
D) 2-methyl-3-ethylheptane
E) All of the above names are correct.
Q4) Which part of HCN,the hydrogen or the cyano group,adds to the O in a C=O bond and why?
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Chapter 22: Biochemistry
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Sample Questions
Q1) Identify the source below that does NOT contain triglycerides.
A) corn oil
B) olive oil
C) whale oil
D) beef fat
E) diesel oil
Q2) Which of the following shows all of the tripeptides that can be formed from one molecule each of alanine (Ala),methionine (Met),and proline (Pro)?
A) AlaMetPro
B) AlaMetPro and AlaProMet
C) AlaMetPro, AlaProMet, ProMetAla, ProAlaMet, MetProAla, MetAlaPro
D) AlaMetPro, AlaProMet, ProAlaMet
E) AlaMetPro, AlaProMet, ProAlaMet, MetProAla
Q3) What is a codon?
Q4) How do cis- and trans-fats differ?
Q5) What is the difference between an -glycosidic linkage and a -glycosidic linkage? What implication does this have for the strength of the intermolecular forces between molecules?
Q6) Why are lipids well-suited as structural components of cell membranes?
Page 24
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Chapter 23: Chemistry of the Nonmetals
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Sample Questions
Q1) Tetraphosphorus decoxide reacts with water to produce phosphoric acid.Write a balanced reaction for this process.
A) P<sub>4</sub>O<sub>10</sub> + 6 H<sub>2</sub>O 4 H<sub>3</sub>PO<sub>4</sub>
B) P<sub>2</sub>O<sub>5</sub> + 3 H<sub>2</sub>O 2 H<sub>3</sub>PO<sub>3</sub>
C) P<sub>4 </sub>+ 3 O<sub>2 </sub><sub>+ </sub>6 H<sub>2</sub>O 4 H<sub>3</sub>PO<sub>4 </sub>
D) P<sub>4</sub>O<sub>10 </sub>+ 4 H<sub>2</sub>O 4 H<sub>2</sub>PO<sub>3</sub>
E) P<sub>4</sub> + 3 O<sub>2</sub><sub> + </sub>6 H<sub>2</sub>O 4 H<sub>3</sub>PO<sub>3</sub>
Q2) Which of the following statements is TRUE?
A) Boron is a large component of Earth's crust.
B) Boron is usually found in its elemental state in the Earth's crust.
C) Due to boron's small size and low electronegativity, it behaves as a semimetal instead of a metal.
D) Boron atoms don't typically bond to one another due to its small atomic radius.
E) There are at least 5 allotropes of elemental boron.
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Chapter 24: Metals and Metallurgy
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59 Verified Questions
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Sample Questions
Q1) Identify the normal crystal structure at room temperature for Cr.
A) body-centered cubic
B) trigonal pyramidal
C) octahedral
D) hexagonal
E) hexagonal closest packed
Q2) Give the components of bronze.
A) copper and tin
B) lead and aluminum
C) nickel and zinc
D) copper and zinc
E) zinc and gold
Q3) Identify the substances which contain a high concentration of a specific mineral.
A) slag
B) minerals
C) ores
D) gangue
E) alloy
Q4) Why is zinc used to coat steel objects?
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Chapter 25: Transition Metals and Coordination Compounds
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Sample Questions
Q1) What is a coordinate covalent bond?
Q2) How many unpaired electrons would you expect for the complex ion: [Co(OH)<sub>6</sub>]<sup>3-</sup>?
A) 1
B) 2
C) 4
D) 0
E) 3
Q3) Identify the transition metal that is the coordinated metal in chlorophyll.
A) magnesium
B) manganese
C) selenium
D) iron
E) silver
Q4) How many d electrons are in W<sub> </sub>O<sub>4</sub><sup>2-</sup>?
A) 0
B) 1
C) 2
D) 3
Page 27
Q5) What is the difference between a weak-field complex and a strong-field complex?
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