General Chemistry I Final Exam Questions - 1986 Verified Questions

Course Introduction

General Chemistry I Final Exam Questions

General Chemistry I introduces the fundamental concepts and principles of chemistry, providing a solid foundation for further study in the sciences. Topics covered include atomic structure, chemical bonding, stoichiometry, chemical reactions, thermochemistry, and properties of gases, liquids, and solids. Emphasis is placed on quantitative problem-solving, laboratory techniques, and developing critical thinking skills to understand the behavior of matter at the molecular and atomic levels. This course is designed for students pursuing studies in science, engineering, health professions, and related fields.

Recommended Textbook

Chemical Principles 6th Edition by Professor Peter Atkins

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Page 2

Chapter 1: The Quantum World

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Q1) The planet Mercury has a maximum intensity of solar radiation of 3700 nm on the sunlit side.What is the temperature of the surface of Mercury on the sunlit side? The empirical value of the constant in Wien's law is 2.9 K·mm.

A)510^oC

B)780^oC

C)1100^oC

D)290^oC

E)543^oC

Answer: A

Q2) When a mole of photons possesses an energy of 2.4 * 10⁷ J,what is its frequency in /sec?

A)1.6 * 10^-15J/mol

B)6.1 * 10^-16J/mol

C)6.1 * 10¹⁶J/mol

D)1.6 * 10⁵J/mol

E)4.2 * 10¹⁶J/mol

Answer: C

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) How many unpaired electrons are in a chromium atom?

A)0

B)5

C)6

D)4

E)3

Answer: C

Q2) Which of the following is likely to form ions two units lower in charge than expected from the group number?

A)Hg

B)Cd

C)Sb

D)Ge

E)Zn

Answer: C

Q3) When an electron is added to a gaseous chlorine atom,349 kJ.mol^-¹ of energy is released.What is the ionization energy of a gaseous chloride ion?

Answer: +349 kJ.mol^-¹

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Page 4

Chapter 3: Chemical Bonds

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Q1) Which of the following statements is true?

A)The electronegativity of an atom is defined as electron affinity of the atom.

B)The electronegativity of an atom depends only on the value of the ionization energy of the atom.

C)Atoms with high ionization energies and high electron affinities have low electronegativities.

D)Atoms with low ionization energies and low electron affinities have low electronegativities.

E)Atoms with low ionization energies and low electron affinities have high electronegativities.

Answer: D

Q2) The electronegativity of an element can be expressed as ½(I + E_a)where I is the ionization energy and E_a is the electron affinity. A)True

B)False

Answer: True

Q3) List the chalcogens in order of increasing electronegativity. Answer: tellurium < selenium < sulfur < oxygen.

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Page 5

Chapter 4: Molecular Shape and Structure

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Q1) Which of the following is polar?

A)NON

B)XeF₂

C)XeO₂

D)ICl₄^-

E)I₃^-

Q2) Which of the following has bond angles of 180S1U1P1\(\circ\)S1S1P0?

A)I₃^-0

B)ClO₂^-

C)O₃

D)NH₂^-

E)HO₂^-

Q3) All the following are paramagnetic except

A)O₂⁺.

B)O₂^-.

C)N₂²⁺.

D)N₂²^-

E)O₂.

Q4) Name all the angles in a trigonal planar geometry.

Q5) What is the ground-state electron configuration of O₂^-?

Page 6

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Chapter 5: The Properties of Gases

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Q1) Ideal gases and real gases behave most similarly under which of the following conditions?

A)Low temperatures and low pressures.

B)Low temperatures and high pressures.

C)High pressures and low molar masses.

D)High temperatures and high pressures.

E)High temperatures and low pressures.

Q2) A pressure of 2.50 * 10⁵ kg.m^-¹.s^-² corresponds to

A)1.00 atm

B)760 mmHg

C)253 kPa

D)2.50 * 10⁵ Torr

E)2.50 Pa

Q3) What is the density of xenon gas at 750 kPa and 25S1U1P1\(\circ\)S1S1P0C?

A)5.30 g.L^-¹

B)0.392 g.L^-¹

C)39.7 g.L^-¹

D)79.5 g.L^-¹

E)19.9 g.L^-¹

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Chapter 6: Liquids and Solids

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Q1) What is the coordination number of magnesium in MgO? The ionic radii of Mg²⁺ and O^2-are 72 and 140 pm,respectively.

A)4

B)2

C)8

D)6

E)12

Q2) Estimate the density of cesium iodide from its crystal structure.The ionic radii of Cs⁺ and Cl^- are 170 and 220 pm,respectively.

A)7.25 g.cm^-3

B)18.9 g.cm^-3

C)9.44 g.cm^-3

D)4.72 g.cm^-3

E)3.77 g.cm^-3

Q3) Butane and 2-propanone have approximately the same boiling points.True or false?

A)True

B)False

Q4) Which has the higher boiling point,1,1-dichloroethene or cis-dichloroethene?

Q5) How many atoms are there in a face-centered cubic unit cell?

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Chapter 7: Inorganic Materials

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Q1) Brass is an example of what kind of metal?

A)A pure elemental metal.

B)An ionic metal.

C)An alloy.

D)An amalgam.

E)None of the above.

Q2) How is boron nitride related to graphite?

A)It has the same melting point.

B)Both are molecular solids.

C)Both have octagonal planes of atoms.

D)It is isoelectronic.

E)There is no direct relationship.

Q3) What does "sintering" mean?

A)Mixing finely divided metal powders and pressing in a mold.

B)Mixing molten metals and pressing in a mold.

C)Mixing finely divided metal powders in a stream of oxygen.

D)Mixing molten metals in a stream of oxygen.

E)Adding one metal on top of another metal.

Q4) To what two chemicals are most glasses not resistant?

Q5) What contaminant causes the red "terra cotta" color in most ceramics?

Page 9

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Chapter 8: Thermodynamics: The First Law

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Q1) What is the standard enthalpy of formation of Br₂(l)?

A)a positive value.

B)a negative value.

C)zero.

D)a positive value if it is forming from ions or a solid.

E)a negative value if it is forming from ions or a solid.

Q2) All bond enthalpies are positive.

A)True

B)False

Q3) The enthalpy of sublimation of a substance is related to its enthalpy of vaporization and enthalpy of fusion by the equation,\(\Delta\)H_sublimation = \(\Delta\)H_vaporization - \(\Delta\)H_fusion.True or false?

A)True

B)False

Q4) Combustion reactions can be exothermic or endothermic.

A)True

B)False

Q5) What equation corresponds to the standard enthalpy of formation of gaseous hydrogen atoms,which,at 298 K is +217 kJ.mol^-1?

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Chapter 9: Thermodynamics: The Second and Third Laws

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Q1) Rank the standard molar entropy of the following from lowest to highest.

1. H₂O(l)

2. H₂O(g)

3. H2O₂(l)

4. H₂O₂(aq)

A)4 < 1 < 3 < 2

B)1 < 3 < 4 < 2

C)3 < 1 < 4 < 2

D)2 < 4 < 3 < 1

E)1 < 3 < 2 < 4

Q2) Which of the following would have the largest calculated value of the residual entropy?

A)C₆H₅Cl(s)(chlorobenzene)

B)CO(s)

C)N₂O(s)

D)FClO₃(s)

E)CCl₄(s)

Q3) For He(g,10 atm)\(\rightarrow\) He(g,1 atm),is the entropy change positive or negative?

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Page 11

Chapter 10: Physical Equilibria

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Q1) What happens to the boiling point of water in a pressure cooker when compared to its boiling point at 1 atm of pressure?

Q2) Using a mass of 500.0 g of water,what is the molality of NaClO₄ in a solution made using 125 g of sodium perchlorate monohydrate?

A)1.78 m

B)3.56 m

C)0.900 m

D)2.04 m

E)0.250 m

Q3) What is the molality of carbon tetrachloride in a solution of toluene,given that the mole fraction is 0.200?

Q4) Of the following five materials,which has the lowest freezing point and the highest boiling point?

A)1.5 m magnesium phosphate

B)2.0 m potassium chloride

C)1.0 m sodium chloride

D)1.5 m aluminum nitrate

E)1.5 m calcium chloride

Q5) What is the vapor pressure of carbon disulfide at its normal boiling point?

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Chapter 11: Chemical Equilibria

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Q1) Calculate the vapor pressure of chloroform,CHCl₃(l),at 25°C.The standard free energies of formation of CHCl₃(l)and CHCl₃(g)are -71.84 and -70.12 kJ.mol^-1 at 25°C,respectively.

A)0.499 atm

B)0.000255 atm

C)0.813 atm

D)1.0 atm

E)0.97 atm

Q2) Consider the following reaction at a certain temperature:

Ni(s)+ 4CO(g) Ni(CO)₄(g)

Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)₄(g)are 1.25 and 6.65 atm over 1.00 kg of nickel.

Q3) For the reaction 2NOCl(g) 2NO(g)+ Cl₂(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

Q4) For a pure solid or liquid,the molar free energy always has its standard value.

A)True

B)False

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13

Chapter 12: Acids and Bases

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Q1) Which of the following is the strongest base?

A)methylamine (pK_b = 3.44)

B)morphine (pK_b = 5.79)

C)urea (pK_b = 13.90)

D)ammonia (pK_b = 4.75)

E)pyridine (pK_b = 8.75)

Q2) A flask of 0.25 M HBrO(aq)has what pH? (pK_a = 8.69)

A)5.90

B)0.60

C)8.10

D)4.65

E)9.30

Q3) Which of the following is the weakest acid?

A)HCN (pK_a = 9.31)

B)HIO₃ (pK_a = 0.77)

C)HF (pK_a = 3.45)

D)CH₃COOH (pK_a = 4.75)

E)HNO₂ (pK_a = 3.37)

Q4) Write the autoprotolysis reaction for liquid ammonia.

Q5) What is the conjugate acid of O^2-?

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Chapter 13: Aqueous Equilibria

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Q1) Calculate the value of the equilibrium constant for the reaction AgCl(s)+ 2NH₃(aq) Ag(NH₃)₂+(aq)+ Cl^-(aq)

Given K_sp = 1.6 * 10^-¹⁰ for silver chloride and K_f = 1.6 * 10⁷ for the ammonia complex of Ag⁺ ions,Ag(NH₃)²⁺.

A)1.0 * 10^-¹⁷

B)6.3 * 10⁹

C)6.3 * 10^-⁸

D)1.0 * 10¹⁷

E)2.6 * 10^-³

Q2) If you wish to increase the solubility of silver benzoate,a preservative,you would

A)add sodium hydroxide.

B)decrease the pH.

C)add sodium acetate.

D)add sodium benzoate.

E)add silver nitrate.

Q3) What is the main factor that directly determines the pH of any buffer?

Q4) What is the main factor that determines the pH of any buffer?

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Chapter 14: Electrochemistry

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Q1) If the standard potentials for the couples Cu²⁺/Cu,Ag⁺/Ag,and Fe²⁺/Fe are +0.34,+0.80,and -0.44 V,respectively,which is the strongest reducing agent?

A)Fe

B)Ag

C)Ag⁺

D)Cu

E)Fe²⁺

Q2) When the Ag(s)|AgCl(s)|Cl^-(aq)electrode acts as a cathode,the reaction is

A)Ag⁺(aq)+ e^-\(\rightarrow\) Ag(s).

B)Ag(s)+ Cl^-(aq)\(\rightarrow\) AgCl(s)+ e^-

C)Ag(s)\(\rightarrow\) Ag⁺(aq)+ e^-

D)2AgCl(s)+ 2e^-\(\rightarrow\) 2Ag⁺(aq)+ Cl₂(g).

E)AgCl(s)+ e^- \(\rightarrow\) Ag(s)+ Cl^-(aq).

Q3) What current is required to produce 91.6 g of chromium meta from chromium(VI)oxide in 12.4 hours?

Q4) The half-reaction that occurs at cathode when 1 M AgNO₃(aq)is electrolyzed is __________________.

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Chapter 15: Chemical Kinetics

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Q1) Consider the mechanism

ClO^-(aq)+ H₂O(l) HOCl(aq)+ OH^-(aq)K,fast I^-(aq)+ HOCl(aq)\(\rightarrow\) HOI(aq)+ Cl^-(aq)k,slow HOI(aq)+ OH^-(aq)\(\rightarrow\)OI^-(aq)+ H₂O(l)k,fast

Draw the reaction profile for this mechanism.

Q2) Consider the reaction 2N₂O₅(g)\(\rightarrow\) 4NO₂(g)+ O₂(g)

Rate = k[N₂O₅]

Calculate the time for the concentration of N₂O₅ to fall to one-fourth its initial value if the half-life is 133 s.

A)133 s

B)33.3 s

C)266 s

D)66.6 s

E)533 s

Q3) What is the half-life of a second order reaction?

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Chapter 16: The Elements: the Main Group Elements

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Q1) Which of the following has the largest atomic radius?

A)In

B)Ga

C)Ge

D)Al

Q2) The electron affinities of elements are always positive.

A)True

B)False

Q3) Write an equation for the second ionization energy of magnesium.

Q4) Which of the following statements is false?

A)Oxides of nonmetals are acidic.

B)Elements with intermediate ionization energies form amphoteric oxides.

C)Elements with low ionization energies commonly form ionic oxides.

D)Oxides of main-group metals are acidic.

Q5) Both boric acid and nickel(II)chloride are weak acids in aqueous solutions.Explain.

Q6) Write the reaction for the disproportionation of nitrogen dioxide in water.

Q7) Sodium borohydride is an oxidizing agent.

A)True

B)False

18

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Chapter 17: The Elements: The D Block

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Q1) All of the following ligands are monodentate except A)ammine.

B)cyano. C)aqua.

D)carbonyl.

E)oxalato.

Q2) Which of the following has the largest atomic radius?

A)Ru

B)Pt

C)Mo

D)Cd

E)Zn

Q3) Which of the following complexes is chiral?

A)[Co(en)₃]³⁺

B)[RuCl₃(CN)₃]^3-

C)[Co(NH₃)₆]³⁺

D)trans-[Cr(en)₃]³⁺

Q4) What do all rhodium complexes have in common?

Q5) In the following reaction,what acts as the Lewis acid? MgO(s)+ SO₂(g)\(\rightarrow\) MgSO₃(s)

Page 19

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Chapter 18: Nuclear Chemistry

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Q1) Which of the following is expected to be stable?

A)²⁰⁸Pb

B)⁷Be

C)¹²²Sb

D)⁸⁷Kr

E)²⁴Na

Q2) All of the following are stable except

A)¹⁵O.

B)²⁰Ne.

C)¹⁴N.

D)¹²C.

E)¹⁶O.

Q3) Heavy elements are more likely to give off \(\beta\) radiation. A)True

B)False

Q4) Nuclides that lie above the band of stability are proton rich. A)True

B)False

Q5) Nuclides that lie below the band of stability are proton rich and can form more stable nuclei by _______________,___________________,and

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Chapter 19: Organic Chemistry I

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Q1) All of the following are saturated hydrocarbons except

A)C₄H₁₀.

B)C₃H₄.

C)C₅H₁₂.

D)C₄H₆.

E)C₃H₈.

Q2) When 2-methyl-1-butene reacts with HBr,the reaction occurs in two steps.What is the major product? (Hint: Intermediate carbocations are most stable when formed at tertiary carbons.)

Q3) What type of reaction is that of chlorine and ethylene (the older name for ethene)to form 1,2-dichloroethane?

A)Electrophilic reaction

B)Substitution reaction

C)Nucleophilic reaction

D)Oxidation reaction

Q4) Why do alkanes not react with boiling nitric acid?

Q5) Name the compound CH₃CH=CHCH=CH₂.

Q6) By what type of mechanism do alkanes undergo substitution reactions?

Q7) Name the compound (CH₃)₂CHCCCH₃.

Q8) When 2-methyl-1-butene reacts with HBr,what are the two products formed?

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Chapter 20: Organic Chemistry II

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Q1) Oxidation of secondary alcohols produces A)acids.

B)aldehydes.

C)ketones.

D)Secondary alcohols cannot be oxidized. E)ethers.

Q2) Which of the following produces a silver mirror with Tollens reagent?

A)CH₃COOH

B)CH₃C(O)OCH₃

C)CH₃COCH₃

D)CH₃OCH₃

E)CH₃CHO

Q3) The -OH group occurs in A)aldehydes and alcohols.

B)alcohols only.

C)alcohols,phenols,and carboxylic acids.

D)phenols and ketones.

E)ketones and carboxylic acids.

Q4) Where is the electrophilic site in the compound 2-bromo-2-methylbutane?

Q5) When amines condense with carboxylic acids,what molecule is eliminated?

Page 22

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