General Chemistry II Question Bank - 1830 Verified Questions

General Chemistry II Question Bank

Course Introduction

General Chemistry II is a continuation of introductory chemistry, focusing on advanced concepts such as chemical kinetics, chemical equilibrium, acid-base equilibria, thermodynamics, electrochemistry, and an introduction to coordination chemistry. The course deepens students' understanding of chemical processes and reactions, examining how molecular structure influences physical and chemical properties. Laboratory components reinforce principles through practical experiments involving qualitative and quantitative analysis. This course is essential for students in science, engineering, and health-related fields who require a comprehensive foundation in chemistry for further studies.

Recommended Textbook

Principles of General Chemistry 2nd Edition by Martin Silberberg

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23 Chapters

1830 Verified Questions

1830 Flashcards

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Page 2

Chapter 1: Keys to the Study of Chemistry

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66 Verified Questions

66 Flashcards

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Sample Questions

Q1) Use the relationship between temperatures in Celsius and Fahrenheit to calculate the temperature at which a.the numerical value is the same on both scales. b.the Fahrenheit number is exactly twice the Celsius number.

Answer: a.40.°F = - 40.°C

b.320.°F = 160.°C

Q2) When applying the scientific method,a model or theory should be based on experimental data.

A)True

B)False

Answer: True

Q3) The ripening of fruit,once picked,is an example of physical change.

A)True

B)False

Answer: False

Q4) Briefly explain the relationship between hypothesis and experiment in the scientific method.

Answer: A hypothesis should be capable of leading to a prediction which is testable by experiment.If the experimental result differs from the prediction,the hypothesis should be modified.

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Chapter 2: The Components of Matter

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Sample Questions

Q1) Which of the following ions occurs commonly?

A)N³⁺

B)S⁶⁺

C)O^2-

D)Ca⁺

E)Cl⁺

Answer: C

Q2) What is the name of IF₇?

A)iodine fluoride

B)iodic fluoride

C)iodine heptafluoride

D)heptafluoroiodide

E)heptafluorine iodide

Answer: C

Q3) Ionic compounds may carry a net positive or negative charge.

A)True

B)False

Answer: False

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4

Chapter 3: Stoichiometry of Formulas and Equations

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Sample Questions

Q1) Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂ and 0.226 g H₂O.If its molar mass is between 158 and 167 g/mol,what is its molecular formula?

A)C₄H₆O₇

B)C₆H₈O₅ C)C₇H₁₂O₄

D)C₄H₃O₂

E)C₈H₆O₄

Answer: E

Q2) Sodium bromate is used in a mixture which dissolves gold from its ores.Calculate the mass in grams of 4.68 mol of sodium bromate.

A)706 g

B)482 g

C)383 g

D)32.2 g

E)0.0310 g

Answer: A

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Chapter 4: Three Major Classes of Chemical Reactions

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Sample Questions

Q1) In both of the following reactions,a precipitate is formed.Complete and balance the equations,showing the phases of the products.

a.AgNO₃(aq)+ CaCl₂(aq) \(\to\) b.NaOH(aq)+ Fe(NO₃)₃(aq)\(\to\)

Q2) Select the classification for the following reaction. H₂CO₃(aq) \(\to\) H₂O(l)+ CO₂(g)

A)combination

B)decomposition

C)displacement

D)acid-base

E)None of these choices is correct.

Q3) In the following reaction,what ions,if any,are spectator ions?

Pb(NO₃)₂(aq)+ 2NaCl(aq) \(\to\) PbCl₂(s)+ 2NaNO₃(aq)

A)Pb²⁺(aq),Cl^-(aq)

B)Na⁺(aq),NO₃^-(aq)

C)Pb²⁺(aq),NO₃^-(aq)

D)Na⁺(aq),Cl^-(aq)

E)There are no spectator ions.

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Page 6

Chapter 5: Gases and the Kinetic-Molecular Theory

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Sample Questions

Q1) "The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ Law.

A)Charles'

B)Boyle's

C)Amontons'

D)Avogadro's

E)Gay-Lussac's

Q2) "The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure" is a statement of _____________ Law.

A)Charles' B)Boyle's

C)Amontons'

D)Avogadro's E)Dalton's

Q3) Aluminum metal shavings (10.0 g)are placed in 100.mL of 6.00 M hydrochloric acid.What is the maximum volume of hydrogen,measured at STP,which can be produced?

2Al(s)+ 6HCl(aq) \(\to\) 2AlCl₃(aq)+ 3H₂(g)

Q4) State Avogadro's Law.

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Chapter 6: Thermochemistry: Energy Flow and Chemical Change

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Sample Questions

Q1) A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings.If the initial internal energy,E,is 61.2 kJ,what is the final value of E?

A)32.7 kJ

B)46.5 kJ

C)75.9 kJ

D)82.8 kJ

E)89.7 kJ

Q2) Natural gas,or methane,is an important fuel.Combustion of one mole of methane releases 802.3 kilojoules of energy.How much energy does that represent in kilocalories?

A)1.92 \(\times\) 10^-1 kcal

B)1.92 \(\times\) 10² kcal

C)3.36 \(\times\) 10³ kcal

D)1.92 \(\times\) 10⁵ kcal

E)3.36 \(\times\) 10⁶ kcal

Q3) The standard heat (enthalpy)of formation of graphite is zero.

A)True

B)False

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Page 8

Chapter 7: Quantum Theory and Atomic Structure

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Sample Questions

Q1) A photon has an energy of 5.53 \(\times\) 10^-17 J.What is its frequency in s^-1?

A)3.66 \(\times\) 10^-50 s^-1

B)1.20 \(\times\) 10^-17 s^-1

C)3.59 \(\times\) 10^-9 s^-1

D)2.78 \(\times\) 10⁸ s^-1

E)8.35 \(\times\) 10¹⁶ s^-1

Q2) If the energy of a photon is 1.32 \(\times\) 10^-18 J,what is its wavelength in nm?

A)1.50 \(\times\) 10^-7 nm

B)150.nm

C)1.99 \(\times\) 10¹⁵ nm

D)1.99 \(\times\) 10²⁴ nm

E)None of these choices is correct.

Q3) In the Bohr model of the hydrogen atom,the electron moves in a circular path which Bohr referred to as an orbital.

A)True

B)False

Q4) a.Calculate the momentum of a photon of green light,wavelength 515 nm.

b.If this photon is traveling in a vacuum,what is its "mass"?

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Chapter 8: Electron Configuration and Chemical Periodicity

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Sample Questions

Q1) Which of the following elements will form a cation with a +2 charge?

A)Si

B)Sr

C)Ga

D)Cs

E)S

Q2) Which of the following elements has the largest atomic size?

A)S

B)Ca

C)Ba

D)Po

E)Rn

Q3) Elements with ________________ first ionization energies and ___________ electron affinities generally form cations.

A)low,very negative

B)high,positive or slightly negative

C)low,positive or slightly negative

D)high,very negative

E)None of these is generally correct.

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Page 10

Chapter 9: Models of Chemical Bonding

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Sample Questions

Q1) Using appropriate,real examples to illustrate your answer,describe the correlation between bond energy and bond length for a series of varying bond order.

Q2) For which of the following elements (in their normal,stable forms)would it be correct to describe the bonding as involving "electron pooling"?

A)hydrogen B)helium

C)sulfur

D)iodine

E)aluminum

Q3) Bond energy increases as bond order increases,for bonding between a given pair of atoms.

A)True

B)False

Q4) A single covalent bond consists of a single delocalized electron pair.

A)True B)False

Q5) Covalently bonded substances do not necessarily exist as separate molecules. A)True B)False

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Chapter 10: The Shapes of Molecules

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Sample Questions

Q1) Draw Lewis structures,showing all valence electrons,for: a.N

b.Br^- c.O₂ d.SO₄^2-

Q2) Which of the following has no net dipole moment?

A)N₂O

B)NF₃

C)H₂Se

D)TeO₃

E)CH₃Cl

Q3) In order for a non-cyclic triatomic molecule to be bent,VSEPR theory requires that there must be two lone pairs on the central atom.

A)True

B)False

Q4) The molecule AX₂,where A and X are different elements,will have a dipole moment if the molecule is bent.

A)True

B)False

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Chapter 11: Theories of Covalent Bonding

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Sample Questions

Q1) A molecule with the formula AX₄E₂ uses _________ to form its bonds.

A)sp hybrid orbitals

B)sp² hybrid orbitals

C)sp³ hybrid orbitals

D)sp³d hybrid orbitals

E)sp³d² hybrid orbitals

Q2) The nitrosonium ion,NO⁺,forms a number of interesting complexes with nickel,cobalt,and iron.According to molecular orbital theory,which of the following statements about NO⁺ is correct?

A)NO⁺ has a bond order of 2 and is paramagnetic.

B)NO⁺ has a bond order of 2 and is diamagnetic.

C)NO⁺ has a bond order of 3 and is paramagnetic.

D)NO⁺ has a bond order of 3 and is diamagnetic.

E)None of these statements is correct.

Q3) Valence bond theory explains the bonding in diatomic molecules such as HCl without resorting to the use of hybrid orbitals.

A)True

B)False

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Page 13

Chapter 12: Intermolecular Forces: Liquids,solids,and Phase Changes

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Sample Questions

Q1) For the solid forms of the following elements,which one is most likely to be of the molecular type?

A)Xe

B)C

C)Pb

D)S

E)Cr

Q2) Neon condenses due to

A)dipole-dipole forces.

B)London dispersion forces.

C)hydrogen bonding.

D)covalent bonding.

E)intramolecular forces.

Q3) Which of the following factors contributes to a low viscosity for a liquid?

A)low temperature

B)spherical molecular shape

C)hydrogen bonding

D)high molecular weight

E)high boiling point

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Q4) How do the electrical properties of semiconductors differ from those of metals?

Chapter 13: The Properties of Solutions

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Sample Questions

Q1) Which of the following aqueous liquids will have the lowest freezing point?

A)0.5 m C₁₂H₂₂O₁₁ (sucrose)

B)0.5 m Ca(NO₃)₂

C)0.5 m NiSO₄

D)0.5 m Li₃PO₄

E)pure water

Q2) The solubility of the oxidizing agent potassium permanganate is 7.1 g per 100.0 g of water at 25°C.What is the mole fraction of potassium permanganate in this solution?

A)0.0080

B)0.0086

C)0.066

D)0.45

E)0.48

Q3) The solubility of gases in water increases with increase in the pressure of the gas.

A)True

B)False

Q4) A 7.112 M solution of sulfuric acid (H₂SO₄)in water has a density of 1.395 g/mL.What is its molality?

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Page 15

Chapter 14: The Main-Group Elements: Applying Principles of Bonding and Structure

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Sample Questions

Q1) Certain Period 2 elements exhibit behaviors similar to Period 3 elements immediately below and to the right.One of these interesting diagonal relationships occurs between beryllium and aluminum.Which of the following is one of their differences?

A)Some aluminum compounds and all beryllium compounds show significant covalent character in the gas phase.

B)Beryllium forms bridge bonds in its hydrides while aluminum does not.

C)Both form oxides that are impervious to reaction with water.

D)The cations for both strongly polarize nearby electron clouds.

E)Beryllium occurs in nature as the uncombined element,whereas aluminum does not.

Q2) Predict the products for the following set of reactants.

Cl₂(g)+ I^-(aq) \(\to\)

A)ICl

B)ICl₂

C)ICl₃

D)I₂ + Cl^-

E)I + Cl₂^-

Q3) Name the three allotropes of carbon and briefly describe their properties and structures.

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Chapter 15: Organic Compounds and the Atomic Properties of Carbon

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Sample Questions

Q1) Name the three component parts of a nucleotide.

Q2) The most abundant organic chemical on earth is A)glycogen.

B)starch.

C)cellulose.

D)glucose.

E)carbonate.

Q3) The carbon atoms in a molecule of cyclohexane lie in the same plane.

A)True

B)False

Q4) Amino acids in solution can undergo an internal acid-base reaction.

A)True

B)False

Q5) One characteristic of the monomers that form condensation polymers that is not common in monomers which form addition polymers is A)the presence of pi bonds.

B)the presence of two functional groups.

C)the presence of alkyl side chains.

D)the ability to form free radicals.

E)the presence of sulfur atoms.

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Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions

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Sample Questions

Q1) The reaction CH₃NC(g) \(\to\) CH₃CN(g)is first-order with respect to methyl isocyanide,CH₃NC.If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react,what is the rate constant in units of min^-1?

A)-0.135 min^-1

B)0.0279 min^-1

C)0.089 min^-1

D)0.135 min^-1

E)35.8 min^-1

Q2) Sucrose decomposes to fructose and glucose in acid solution.When ln [sucrose] is plotted vs.time,a straight line with slope of -0.208 hr^-1 results.What is the rate law for the reaction?

A)Rate = 0.208 hr^-1 [sucrose]²

B)Rate = 0.208 hr^-1 [sucrose]

C)Rate = 0.0433 hr [sucrose]²

D)Rate = 0.0433 hr [sucrose]

E)Rate = 0.208 mol L^-1hr^-1 [sucrose]⁰

Q3) The units of the rate constant depend on the order of the reaction.

A)True

B)False

Page 18

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Chapter 17: Equilibrium: the Extent of Chemical Reactions

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Sample Questions

Q1) For a gas-phase equilibrium,a change in the pressure of any single reactant or product will change K_p.

A)True

B)False

Q2) Although a system may be at equilibrium,the rate constants of the forward and reverse reactions will in general be different.

A)True

B)False

Q3) Once a reaction system reaches equilibrium,the concentrations of reactions and products no longer change.

A)True

B)False

Q4) When a reaction system reaches equilibrium,the forward and reverse reactions stop. A)True

B)False

Q5) For some gas-phase reactions,K_p = K_c.

A)True

B)False

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Page 19

Chapter 18: Acid-Base Equilibria

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Sample Questions

Q1) Which of the following is the strongest acid?

A)CH₃COOH

B)HF

C)H₃PO₄

D)H₂SO₃

E)HI

Q2) What is the [OH^-] for a solution at 25°C that has [H₃O⁺] = 2.35 \(\times\) 10^-3 M?

A)4.26 \(\times\) 10^-5 M

B)2.35 \(\times\) 10^-11 M

C)4.26 \(\times\) 10^-12 M

D)2.35 \(\times\) 10^-17 M

E)None of these choices is correct.

Q3) A 1.25 M solution of the weak acid HA is 9.2% dissociated.What is the pH of the solution?

A)0.64

B)0.94

C)1.13

D)2.16

E)None of these choices is correct.

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Chapter 19: Ionic Equilibria in Aqueous Systems

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Sample Questions

Q1) Which of the following substances has the greatest solubility in water?

A)PbI₂,K_sp = 7.9 \(\times\) 10^-9

B)BaF₂,K_sp = 1.5 \(\times\) 10^-6

C)Ca(OH)₂,K_sp = 6.5 \(\times\) 10^-6

D)Zn(IO₃)₂,K_sp = 3.9 \(\times\) 10^-6

E)Ag₂SO₄,K_sp = 1.5 \(\times\) 10^-5

Q2) A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

A)0.025 mol HCl

B)0.063 mol HCl

C)0.082 mol HCl

D)0.50 mol HCl

E)1.0 mol HCl

Q3) The equivalence point in a titration is defined as the point when the indicator changes color.

A)True

B)False

Q4) Make a clear distinction between buffer range and buffer capacity.

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Chapter 20: Thermodynamics: Entropy,

Direction of Chemical Reactions

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Sample Questions

Q1) In a spontaneous process,the entropy of the system always increases.

A)True

B)False

Q2) a.Explain what is meant by a spontaneous process.

b.Is a spontaneous process necessarily a rapid one? Explain,and provide a real reaction as an example to illustrate your answer.

Q3) In some spontaneous processes,the entropy of the surroundings decreases.

A)True

B)False

Q4) Which of the following is necessary for a process to be spontaneous?

A)(\(\Delta\)H_sys < 0)

B)(\(\Delta\)S_sys > 0)

C)(\(\Delta\)S_surr < 0)

D)(\(\Delta\)S_univ > 0)

E)(\(\Delta\)G_sys = 0)

Q5) The free energy of a perfect crystal at absolute zero,is zero.

A)True

B)False

Q6) State the second and third laws of thermodynamics.

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Chapter 21: Electrochemistry: Chemical Change and Electrical Work

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Sample Questions

Q1) Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.

Q2) What product forms at the cathode during the electrolysis of molten NaCl in the Downs cell?

A)Na⁺(l)

B)Na(l)

C)Cl^-(l)

D)NaOH(aq)

E)Cl₂(g)

Q3) Which one of the following is not a redox reaction?

A)Al(OH)₄^-(aq)+ 4H⁺(aq) \(\to\) Al³⁺(aq)+ 4H₂O(l)

B)C₆H₁₂O₆(s)+ 6O₂(g) \(\to\)6CO₂(g)+ 6H₂O(l)

C)Na₆FeCl₈(s)+ 2Na(l) \(\to\) 8NaCl(s)+ Fe(s)

D)2H₂O₂(aq) \(\to\) 2H₂O(l)+ O₂(g)

E)CO₂(g)+ H₂(g) \(\to\) CO(g)+ H₂O(g)

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Page 23

Chapter 22: The Transition Elements and Their Coordination Compounds

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Sample Questions

Q1) Which of the following species could exist as isomers?

A)[Co(H₂O)₄Cl₂]⁺

B)[Pt(NH₃)Br₃]^-

C)[Pt(en)Cl₂]

D)[Pt(NH₃)₃Cl]⁺

E)None of these choices is correct.

Q2) A characteristic of ligands is that

A)they are Lewis acids.

B)they are Lewis bases.

C)they are ions.

D)they are electron pair acceptors.

E)they are Brønsted-Lowry acids.

Q3) In the spectrochemical series,which one of the following ligands has the strongest field?

A)H₂O

B)CN^-

C)NH₃

D)OH^-

E)Cl^-

Page 24

Q4) What geometry is particularly common for complexes of d¹⁰ metal ions?

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Chapter 23: Nuclear Reactions and Their Applications

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Sample Questions

Q1) A 55-kg person exposed to thorium-234 receives 7.5 \(\times\) 10⁴ \(\beta\) particles,each with an energy of 1.6 \(\times\) 10^-14 J.How many rads does the person receive?

A)2.1 \(\times\) 10^-19

B)1.2 \(\times\) 10^-17

C)2.2 \(\times\) 10^-9

D)1.2 \(\times\) 10^-9

E)None of these choices is correct.

Q2) After 4 half-lives,the fraction of a radioactive isotope which still remains is approximately one eighth.

A)True

B)False

Q3) An isotope with Z > 83,which lies close to the band of stability,will generally decay through

A)(\(\alpha\) decay.)

B)(\(\beta\) decay.)

C)(\(\gamma\) decay.)

D)positron decay.

E)electron capture.

Q4) Write a complete,balanced equation to represent the beta decay of thallium-207.

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