General Chemistry II Test Questions - 2075 Verified Questions

General Chemistry II Test Questions

Course Introduction

General Chemistry II is a continuation of the foundational principles introduced in General Chemistry I, focusing on chemical kinetics, equilibrium, acid-base chemistry, thermodynamics, and electrochemistry. Students explore the behavior of solutions, reaction mechanisms, and the principles governing the direction and spontaneity of chemical reactions. The course also covers coordination compounds, nuclear chemistry, and selected topics in organic and transition element chemistry. Emphasis is placed on problem-solving, laboratory techniques, and real-world applications to reinforce theoretical concepts and develop practical laboratory skills.

Recommended Textbook Chemistry and Chemical Reactivity 9th Edition by John C. Kotz\New folder

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Chapter 1: Basic Concepts of Chemistry

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Sample Questions

Q1) Properties,such as color and density,which can be observed or measured without changing the composition of a substance are called ________ properties.

Answer: physical

Q2) Which of the following are likely to form a homogeneous mixture?

1) milk and ice cream blended together with chocolate syrup

2) an egg combined with milk and mixed with a whisk

3)1 gram table salt combined with 250 mL of water

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Answer: C

Q3) Which of the following are extensive properties: mass,volume,and/or density?

A) mass only

B) volume only

C) density only

D) mass and volume

E) volume and density

Answer: D

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Chapter 2: Mathlets Review: The Tools of Quantitative Chemistry

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Sample Questions

Q1) What volume of a pure liquid (density 0.710 g/mL)has a mass of 0.290 kg?

A) 4.08 \(\times\) 10² mL

B) 2.45 \(\times\) 10^-3 mL

C) 2.06 \(\times\) 10^-1 mL

D) 2.45 mL

E) 4.08 \(\times\) 10^-1 mL

Answer: A

Q2) Convert 0.440 ng to milligrams and express the answer in scientific notation using the correct number of significant figures.

A) 4.40 \(\times\) 10^-5 mg

B) 4.40 \(\times\) 10^-7 mg

C) 4.4 \(\times\) 10^-7 mg

D) 0.440 \(\times\) 10^-8 mg

E) 0.440 \(\times\) 10^-7 mg

Answer: B

Q3) Assuming the density of water is 1.00 g/cm³,the mass of 1.0 cubic meter (m³) of water is ________ grams.

Answer: 1.0 \(\times\) 10⁶

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Chapter 3: Atoms, molecules, and Ions

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Sample Questions

Q1) Naturally occurring element X exists in three isotopic forms: X-28 (27.979 u,77.03% abundance),X-29 (28.976 u,8.00% abundance),and X-30 (29.974 u,14.97% abundance).Calculate the atomic weight of X.

A) 29.64 u

B) 28.36 u

C) 29.05 u

D) 29.60 u

E) 27.38 u

Answer: B

Q2) The masses of isotopes and their abundances are determined experimentally using A) a mass spectrometer.

B) an analytical balance.

C) a centrifuge.

D) filtration followed by distillation.

E) electrolysis.

Answer: A

Q3) The building blocks of atoms (neutrons,protons,and electrons)are called ________ particles.

Answer: subatomic

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Page 5

Chapter 4: Chemical Reactions

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Sample Questions

Q1) Which of the following is a \(\underline{\text{ weak base }}\) in aqueous solution?

A) LiCl

B) LiOH

C) NH₃

D) HBr

E) Ca(OH)₂

Q2) Which equation best represents the \(\underline{\text{ net ionic reaction }}\) that occurs when an aqueous solution of barium bromide is mixed with an aqueous solution of sodium sulfate?

A) 2H⁺(aq)+ 2Br^-(aq)\(\to\) 2HBr(g)

B) Ba²⁺(aq)+ SO₄^2-(aq)\(\to\) BaSO₄(s)

C) Ba²⁺(aq)+ 2Br^-(aq)+ 2Na⁺(aq)+ SO₄^2-(aq)\(\to\) BaSO₄(s)+ 2NaBr(aq)

D) BaBr₂(aq)+ Na₂SO₄(aq)\(\to\)

BaSO₄(s)+ 2NaBr(aq)

E) No net reaction occurs.

Q3) _____-oxides produce acids when reacted with water.

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Chapter 5: Stoichiometry: Quantitative Information About Chemical Reactions

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Q1) A solution of sodium oxalate (Na₂C₂O₄)in acidic solution is titrated with a solution of potassium permanganate (KMnO₄)according to the following balanced chemical equation: 2KMnO₄(aq)+

8H₂SO₄(aq)+ 5Na₂C₂O₄(aq)\(\to\) 2MnSO₄(aq)+ 8H₂O(l)+ 10CO₂(g)+ 5Na₂SO₄(aq)+ K₂SO₄(aq)

What volume of 0.0388 M KMnO₄ is required to titrate 0.134 g of Na₂C₂O₄ dissolved in 20.0 mL of solution?

A) 1.38 mL

B) 3.45 mL

C) 10.3 mL

D) 25.8 mL

E) 20.0 mL

Q2) The numbers preceding the formulas in chemical equations are referred to as the ________ coefficients.

Q3) The pH of purified water (or of a neutral solution)is _____.

Page 7

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Chapter 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

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Sample Questions

Q1) How much energy is needed to convert 57.5 grams of ice at 0.00°C to liquid water at 75.0°C?

Specific heat capacity (ice)= 2.10 J/g°C

Specific heat capacity (liquid water)= 4.18 J/g°C

Heat of fusion = 333 J/g

Heat of vaporization = 2258 J/g

A) 18.0 kJ

B) 2.06 kJ

C) 28.2 kJ

D) 37.2 kJ

E) 148 kJ

Q2) What is the minimum mass of ice at 0.0 S1U1P1\(\circ\)S1S1P0C that must be added to 1.00 kg of water to cool the water from 28.0 S1U1P1\(\circ\)S1S1P0C to 12.0

S1U1P1\(\circ\)S1S1P0C? (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g.K,liquid water = 4.184 J/g.K)

A) 175 g

B) 201 g

C) 244 g

D) 299 g

E) 1140 g

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Chapter 7: The Structure of Atoms

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Sample Questions

Q1) The n = ____ shell is the lowest that may contain s-orbitals.

A) 1

B) 2

C) 3

D) 4

E) 5

Q2) In Bohr's atomic theory,when an electron moves from one energy level to another energy level more distant from the nucleus,

A) energy is absorbed.

B) light is emitted.

C) energy is emitted.

D) no change in energy occurs.

E) none of these

Q3) The ____ of a photon of light is ____ proportional to its frequency and ____ proportional to its wavelength.

A) energy,directly,inversely

B) energy,inversely,directly

C) velocity,directly,inversely

D) intensity,inversely,directly

E) amplitude,directly,inversely

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Chapter 8: The Structure of Atoms and Periodic Trends

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Sample Questions

Q1) Which element has the ground state electron configuration [Ar]3d¹⁰4s¹?

A) Cu

B) Zn

C) Ge

D) Ag

E) Cd

Q2) The element ________ has the following electron configuration: [Rn]5f¹²7s².

Q3) What is the maximum number of electrons that can occupy \(\underline{\text{ one }}\) d orbital?

A) 1

B) 2

C) 6

D) 10

E) 14

Q4) Electron ________ is defined as the energy change for a process in which a gas phase atom acquires an electron.

Q5) The f-block elements are also referred to as the ________ and actinides.

Q6) Explain the difference between paramagnetic and ferromagnetic.

Page 10

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Chapter 9: Bonding and Molecular Structure

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Q1) The molecular geometry of a molecule whose central atom has four single bonds and one lone pair of electrons is ________.

Q2) What is the electron-pair geometry around an atom in a molecule or ion which is surrounded by zero lone pairs of electrons and five single bonds.

A) trigonal bipyramidal

B) see-saw or distorted tetrahedron

C) T-shaped

D) linear

E) trigonal planar

Q3) What is the bond angle in a trigonal planar molecule or ion?

A) 109°

B) 180°

C) 90°

D) 72°

E) 120°

Q4) In PCl₅,the Cl-P-Cl bond angle between an axial and an equatorial chlorine atom is ________ degrees.

Q5) If a molecule has a positive and negative end,the molecule is said to have a(n)________ moment.

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Chapter 10: Bonding and Molecular Structure: Orbital

Hybridization and Molecular Orbitals

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Sample Questions

Q1) What is the maximum number of hybridized orbitals that can be formed by a fluorine atom?

A) 1

B) 2

C) 3

D) 4

E) 6

Q2) In valence bond theory,each sigma bond in CH₄ is formed from the overlap of a hydrogen atom's 1s orbital with a(n)________ hybridized orbital on the carbon atom.

Q3) Which of the following characteristics apply to NCl₃?

1)polar bonds

2)nonpolar molecule

3)triangular-planar molecular shape

4)sp² hybridized N atom

A) 1 only

B) 1 and 2

C) 3 and 4

D) 1,2,and 3

E) 1,2,3,and 4

Page 12

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Chapter 11: Gases and Their Properties

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Sample Questions

Q1) How long will it take 10.0 mL of Ne gas to effuse through a porous barrier if it has been observed that 125 minutes are required for 10.0 mL of Ar gas to effuse through the same barrier?

A) 1.41 min.

B) 31.9 min.

C) 63.1 min.

D) 88.8 min.

E) 176 min.

Q2) The ideal gas law can be modified to correct for the errors arising from nonideality.The modified equation is known as the ________ equation of state for a real gas.

Q3) What volume of gaseous water,H₂O,has the same \(\underline{\text{moles }}\) of gas as 10.0 L of xenon gas at the same temperature and pressure?

A) 40.0 L

B) 2.50 L

C) 10.0 L

D) 3.33 L

E) 30.0 L

Q4) What are two ways in which real gases differ from ideal gases?

Page 13

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Chapter 12: Intermolecular Forces and Liquids

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Sample Questions

Q1) Place the following cations in order from the most negative to the least negative hydration enthalpy: Cs⁺,Na⁺,and Rb⁺.

A) Cs⁺ < Rb⁺ < Na⁺

B) Cs⁺ < Na⁺ < Rb⁺

C) Na⁺ < Rb⁺ < Cs⁺

D) Na⁺ < Cs⁺ < Rb⁺

E) Rb⁺ < Na⁺ < Cs⁺

Q2) Which of the following boils at the \(\underline{\text{ highest }}\) temperature?

A) C₅H₁₂

B) C₆H₁₄

C) C₇H₁₆

D) C₈H₁₈

E) C₉H₂₀

Q3) A molecule will \(\underline{\text{always }}\) be polar if it ___.

A) has polar bonds

B) contains both carbon and chlorine

C) consists of more than three atoms

D) is diatomic with different electronegativities

E) contains atoms with different electronegativities

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Chapter 13: The Chemistry of Solids

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Sample Questions

Q1) The metal chromium crystallizes in a body-centered cubic lattice.If the density of chromium is 7.14 g/cm³,what is the unit cell edge length?

A) 289 pm

B) 77.0 pm

C) 77.5 pm

D) 61.1 pm

E) 230 pm

Q2) Chromium (atomic mass 52.00 g/mol)crystallizes in a body-centered cubic unit cell.If the length of an edge of the unit cell is 289 pm,what is the density (in g/cm³)of chromium?

A) 3.58 g/cm³

B) 7.15 g/cm³

C) 13.7 g/cm³

D) 14.3 g/cm³

E) 21.3 g/cm³

Q3) Above a substance's ________ temperature,it is not possible to compress the substance into the liquid phase.If enough pressure is applied the substance will become a supercritical fluid.

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Chapter 14: Solutions and Their Behavior

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Sample Questions

Q1) What volume of a 0.771 M solution of CaCl₂ contains 1.28 g of solute?

A) 66.8 mL

B) 15.0 mL

C) 1.66 mL

D) 8.89 mL

E) 85.0 mL

Q2) What partial pressure of oxygen gas is required in order for 0.00392 g of the gas to dissolve in 23.7 mL of pure water? The Henry's law constant for oxygen gas is 1.3 \(\times\) 10^-3 M atm^-1.

A) 2.2 \(\times\) 10^-7 atm

B) 4.0 \(\times\) 10⁰ atm

C) 1.6 \(\times\) 10^-7 atm

D) 2.5 \(\times\) 10^-1 atm

E) 4.2 \(\times\) 10^-2 atm

Q3) What is the definition of molality?

A) moles of solute per kg of solvent

B) grams of solute per kg of solution

C) grams of solute per liter of solution

D) moles of solute per liter of solvent

E) moles of solute per liter of solution

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Chapter 15: Chemical Kinetics: the Rates of Chemical Reactions

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Q1) Consider the exothermic combustion of coal.Which of the following could increase the rate of reaction?

A) using smaller pieces of coal

B) increasing the concentration of oxygen

C) lowering the temperature

D) both (a)and (b)are correct

E) choices (a),(b)and (c)are all correct

Q2) In general,as temperature increases,the rate of a chemical reaction

A) decreases due to fewer collisions with proper molecular orientation.

B) increases for exothermic reactions,but decreases for endothermic reactions.

C) increases due to a greater number of effective collisions.

D) remains unchanged.

E) decreases due to an increase in the activation energy.

Q3) Carbon dating may be used to date (once living)materials that are between 100 and 40,000 years old.The half-life of the first-order decay of carbon-14 is 5730 years.What percentage of carbon-14 remains in a sample after 40,000 years.

Q4) Draw the reaction coordinate diagram for an exothermic reaction involving three mechanistic steps.

Q5) Radioactive isotopes decay by ________-order kinetics.

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Chapter 16: Principles of Reactivity: Chemical Equilibria

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Q1) Which of the following statements is/are CORRECT?

1)Product concentrations appear in the numerator of an equilibrium constant expression.

2)A reaction favors the formation of products if K >> 1.

3)Stoichiometric coefficients are used as exponents in an equilibrium constant expression.

A) 1 only

B) 2 only

C) 3 only

D) 2 and 3

E) 1,2,and 3

Q2) The symbol Q is called the ________.

Q3) If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.

Q4) In 1913,the Haber-Bosch process was patented.The product of the Haber-Bosch process is ________.

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Chapter 17: The Chemistry of Acids and Bases

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Q1) Which of the following species \(\underline{\text{ cannot }}\)act as a Lewis base?

A) S^2-

B) H₂S

C) NH₃

D) CH₄

E) SH^-

Q2) What is the pH of the final solution when 25 mL of 0.021 M HCl has been added to 35 mL of 0.036 M HCl at 25°C?

A) 3.3

B) 1.9

C) 1.5

D) 2.7

E) 3.5

Q3) Which is the stronger Brønsted-Lowry acid,Fe(H₂O)₆²⁺ or Fe(H₂O)₆³⁺? Explain.

Q4) When a Lewis acid and a Lewis base combine,the product may be referred to as an acid-base ________.

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Chapter 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria

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Q1) Titration of 0.5083 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 36.95 mL of 0.1067 M NaOH to reach the endpoint.What is the molar mass of the acid?

A) 128.9 g/mol

B) 0.007756 g/mol

C) 190.6 g/mol

D) 1.468 g/mol

E) 2.718 g/mol

Q2) Which of the following conditions is/are met at the equivalence point of the titration of a monoprotic weak base with a strong acid?

1)The moles of acid added from the buret equals the initial moles of weak base.

2)The volume of acid added from the buret must equal the volume of base titrated.

3)The pH of the solution is less than 7.00.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 3

E) 2 and 3

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Chapter 19: Entropy and Free Energy

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Q1) If a cube of ice at 0 S1U1P1\(\circ\)S1S1P0C is placed outside on a warm summer day,the ice will melt spontaneously.What are the signs of \(\Delta\)_rH,\(\Delta\)_rS,and \(\Delta\)_rG for this process?

A) (\(\Delta\)_rH) < 0,\(\Delta\)_rS > 0,\(\Delta\)_rG < 0

B) (\(\Delta\)_rH) < 0,\(\Delta\)_rS < 0,\(\Delta\)_rG < 0

C) (\(\Delta\)_rH) < 0,\(\Delta\)_rS > 0,\(\Delta\)_rG > 0

D) (\(\Delta\)_rH) > 0,\(\Delta\)_rS > 0,\(\Delta\)_rG < 0

E) (\(\Delta\)_rH) > 0,\(\Delta\)_rS < 0,\(\Delta\)_rG > 0

Q2) For any process,the change in entropy of the universe equals the sum of the entropy changes for the system and for the ________.

Q3) Does the formation of complex molecules such as proteins and nucleic acids from more simple molecules contradict the second law of thermodynamics?

Q4) At what temperature (in kelvin units)is the entropy of a pure crystal 0.0 J/K.

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Chapter 20: Principles of Reactivity: Electron Transfer Reactions

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Q1) Given:

2H⁺(aq)+ 2e^- \(\to\) H₂(g); 0.00 V Rb⁺(aq)+ e^- \(\to\) Rb(s); -2.98 V F₂(g)+ 2e^- \(\to\) 2F^-(aq); 2.87 V Al³⁺(aq)+ 3e^- \(\to\) Al(s); -1.66 V Pb²⁺(aq)+ 2e^- \(\to\) Pb(s); -0.13 V

Under standard-state conditions,which is the strongest reducing agent?

A) Al³⁺

B) H⁺

C) Pb²⁺

D) F^-

E) Rb

Q2) Write balanced reduction and oxidation half-reactions for the processes that occur at the cathode and anode of a fuel cell used aboard NASA's space shuttles.

Q3) Explain the function of a salt bridge in a voltaic cell.

Q4) In an electrolytic cell,reduction occurs at the ________ and oxidation occurs at the ________.

Q5) If electric current is passed through a solution of molten KBr,the product at the cathode is ________.

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Chapter 21: Environmental Chemistry Earths

Environment,energy,and Sustainability

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Q1) All of the following are used by various cities and municipalities to disinfect water except ___.

A) Cl₂

B) NaOCl

C) O₃

D) UV-light

E) O₂

Q2) The majority of electricity generated in the United States is produced from ___.

A) wind and solar

B) moving water

C) nuclear fission

D) natural gas

E) coal

Q3) Which of the following water disinfectants persist in water pipes even after the initial disinfection process?

A) Cl₂

B) NaOCl

C) O₃

D) A and B

E) A,B,and C

Page 23

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Chapter 22: The Chemistry of the Main Group Elements

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Q1) The only acid that decomposes silicon dioxide is ____.

A) CF₃CO₂H

B) H₂SO₄

C) HBr

D) HF

E) HClO₄

Q2) Which of the following is the most abundant \(\underline{\text{ metal}}\) on earth?

A) calcium

B) iron

C) copper

D) aluminum

E) zinc

Q3) The active ingredients in "strike anywhere" matches are ____ and the powerful oxidizing agent KClO₃(s).

A) N₂H₄

B) P₄O₁₀

C) Mg₃N₂

D) P₄S₃

E) (HPO₃)₃

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Chapter 23: The Chemistry of the Transition Elements

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Q1) Which of the following d-block ion electron configurations may be high spin \(\underline{\text{ or }}\) low spin when placed in an \(\underline{\text{ octahedral ligand}}\) field?

A) [Ar]3d⁸

B) [Ar]3d³

C) [Ar]3d⁹

D) [Ar]3d⁴

E) [Ar]3d²

Q2) The spectrochemical series is

CN^-> NO₂^-> en > NH₃> H₂O > OH^-> F^->Cl^-> Br>I^-

Which of the following complexes will absorb visible light of the longest wavelength?

A) [Co(H₂O)₆]³⁺

B) [Co(I)₆]^3-

C) [Co(OH)₆]^3-

D) [Co(en)₃]³⁺

E) [Co(NH₃)₆]³⁺

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Chapter 24: Carbon: Not Just Another Element

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Q1) Identify the product(s)of the hydrogenation of cis-2-hexene.

A) 2-hydroxyhexane

B) 2,3-dihydroxyhexane

C) trans-2-hexane

D) carbon dioxide and water

E) hexane

Q2) What is the monomer of Teflon?

A) CH₂CH₂

B) CF₂CF₂

C) CH₂C(CN)₂

D) CH₂CHCN

E) CH₂CHCH₃

Q3) Which of the following is \(\underline{\text{ not }}\) an addition polymer?

A) polyvinyl chloride

B) nylon

C) teflon

D) styrofoam

E) polypropylene

Q4) The molecule 2-chloro-4-methylhexane is made by addition of HCl to an alkene.Write a balanced chemical equation for this reaction.

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Chapter 25: Biochemistry

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Q1) Starch and cellulose are polysaccharides made up long chains of glucose linked by glycosidic bonds.Despite the identical composition,why can humans digest starch but not cellulose?

Q2) Which of the following statements concerning lipids is/are correct?

1)Phospholipids are most prevalent in cell membranes.

2)Triglycerides are formed from fatty acids and glycerol.

3)A major function of lipids in the body is energy storage.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Q3) A compound which contains both a positive and negative charge is called a ____.

Q4) The amide linkages in a protein and also called ___ bonds.

Q5) Which of the following is not a lipid?

A) triglycerides

B) fatty acids

C) glycerol

D) steroids

E) phospholipids

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Chapter 26: Nuclear Chemistry

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Q1) A sample of a radioactive isotope is found to have lost 14.0% of its original activity after 8.67 days.What is the rate constant for decay of this isotope?

A) 0.0174 d^-1

B) 0.227 d^-

C) 1.31 d^-1

D) 0.0151 d^-1

E) 0.514 d^-1

Q2) A certain radioactive isotope has a rate constant of decay of 2.74 \(\times\)10^-2 min^-1.Calculate the time required for a sample of this isotope to decay to one-fourth of its initial value.

A) 25.3 min

B) 31.6 min

C) 0.0548 min

D) 50.6 min

E) 2.74 min

Q3) Explain the treatment named boron neutron capture therapy (BNCT).

Q4) Explain the difference between 1 rad and 1 rem of radiation.

Q5) All isotopes of atomic number greater than ________ are unstable and radioactive.

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