General Chemistry I Chapter Exam Questions - 1986 Verified Questions

Course Introduction

General Chemistry I Chapter Exam Questions

General Chemistry I offers a comprehensive introduction to the fundamental principles of chemistry, focusing on the structure of matter, atomic theory, chemical bonding, stoichiometry, states of matter, and basic thermochemistry. This course emphasizes the quantitative and qualitative analysis of chemical reactions, the periodic properties of elements, and the behavior of solutions. Laboratory components provide practical experience in experimental techniques, data analysis, and the application of theoretical concepts to real-world scenarios. General Chemistry I lays the foundational knowledge necessary for advanced study in chemistry and related scientific fields.

Recommended Textbook

Chemical Principles 6th Edition by Professor Peter Atkins

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20 Chapters

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Page 2

Chapter 1: The Quantum World

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Q1) Of the following,which is a Balmer series visible band?

A)954.6 nm

B)656.3 nm

C)401.2 nm

D)121.6 nm

E)97.3 nm

Answer: B

Q2) What is the frequency of a photon that has an energy of 5.4 * 10^-18 J?

A)1.6 * 10^-34Hz

B) (1 .2 * 10¹⁶Hz)

C)1.2 * 10^-¹⁶Hz

D)(8.1 * 10¹⁵Hz)

E)8.1 *10¹⁵Hz

Answer: E

Q3) The four \(\pi\) electrons of 1,3-butadiene can be modeled as particles in a box.If the length of 1,3-butadiene (L)is 0.56 nm,calculate the energy of the lowest energy transition.

Answer: 9.6 * 10^-¹⁹ J

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) Which of the following species is isoelectronic with Kr?

A)K⁺

B)Cl^-

C)Ar

D)Xe

E)Sr²⁺

Answer: E

Q2) Consider the following ground-state electronic configurations.Which atom has both the highest first ionization energy and the highest electron affinity?

A)[Ne] 3s²3p⁵

B)[Ne] 3s²3p³

C)[Ne] 3s²3p¹

D)[Ne] 3s²3p⁴

Answer: A

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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Chapter 3: Chemical Bonds

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Q1) Which of the following metal ions has the ground-state electron configuration [Ar]3d⁶?

A)Ni³⁺

B)Fe²⁺

C)Mn²⁺

D)Cu⁺

E)Ca²⁺

Answer: B

Q2) Which of the following has resonance structures?

A)XeOF₂

B)N₂H₄

C)CH₃CONH^-

D)H₂CO

Answer: C

Q3) What is the formal charge on the Xe atom in XeF₄?

A)0

B)(-4)

C)+2

D)+4

Answer: A

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Chapter 4: Molecular Shape and Structure

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Q1) What is the shape of SO₃²^-?

A)T-shaped

B)Trigonal pyramidal

C)Seesaw

D)Tetrahedral

E)Trigonal planar

Q2) What is the shape of IF₄⁺?

A)Tetrahedral

B)Seesaw

C)Trigonal bipyramidal

D)Square planar

E)T-shaped

Q3) Which of the following has bond angles of 90S1U1P1\(\circ\)S1S1P0,120S1U1P1\(\circ\)S1S1P0,and 180S1U1P1\(\circ\)S1S1P0?

A)PF₆^-

B)IF₅

C)XeF₄

D)ICl₄^-

E)SF₄

Q4) Predict the electron arrangement in IF₅.

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Chapter 5: The Properties of Gases

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Q1) A Group 17 or Group 18 gas has a density of 2.92 g.L^-¹ at 1.00 atm and 25S1U1P1\(\circ\)S1S1P0C.The gas is

A)helium

B)neon

C)fluorine

D)argon

E)chlorine

Q2) How many liters of carbon dioxide measured at 25.0S1U1P1\(\circ\)S1S1P0C and 821 Torr would be produced by the combustion of 319 g of glucose,C₆H₁₂O₆?

A)3.37 L

B)40.1 L

C)241 L

D)20.2 L

Q3) A sample of nitrogen gas collected at 24S1U1P1\(\circ\)S1S1P0C and 745 Torr has a vapor pressure of 745 Torr.True or false?

A)True

B)False

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Chapter 6: Liquids and Solids

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Q1) Metals with a hexagonal close-packed structure have/do not have slip planes and as a result are malleable/brittle.

Q2) Calculate the size of the octahedral holes in the NaCl structure.The ionic radii of Na⁺ and Cl^- are 102 and 181 pm,respectively.

A)142 pm

B)181 pm

C)102 pm

D)91 pm

E)75 pm

Q3) The atomic radius of aluminum is 143 pm.Estimate its density,given that the metal has a close-packed structure.

A)3.87 g.cm^-3

B)5.54 g.cm^-3

C)7.92 g.cm^-3

D)16.3 g.cm^-3

E)2.71 g.cm^-3

Q4) Determine the percentage of the total volume that is empty space in a primitive cubic structure in which all the atoms are identical.

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Chapter 7: Inorganic Materials

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Q1) What contaminant causes the red "terra cotta" color in most ceramics?

Q2) delocalized pi-bonds are the reason carbon nano-tubes conduct electricity.

A)True

B)False

Q3) What is the minimum pressure and temperature for diamond formation?

A)8kbar,150S1U1P1\(\circ\)S1S1P0C

B)800kbar,15,000S1U1P1\(\circ\)S1S1P0C

C)80 kbar,15,000S1U1P1\(\circ\)S1S1P0C

D)800kbar,1,500S1U1P1\(\circ\)S1S1P0C

E)80kbar,1,500S1U1P1\(\circ\)S1S1P0C

Q4) From what do silicates derive their strength?

A)Their covalently bonded network structures.

B)Strong intermolecular forces.

C)Their extensive pi-delocalized systems.

D)From two-dimensional covalent bonding.

E)Nothing,silicates are not generally considered strong.

Q5) Ceramics are not brittle.

A)True

B)False

Q6) To what two chemicals are most glasses not resistant?

Page 9

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Chapter 8: Thermodynamics: The First Law

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Q1) What is the total motional contribution to the molar internal energy of gaseous H₂O at 25S1U1P1\(\circ\)S1S1P0C?

A)6.19 kJ.mol^-1

B)7.43 kJ.mol^-1

C)3.72 kJ.mol^-1

D)12.4 kJ.mol^-1

E)2.48 kJ.mol^-1

Q2) For most reactions,the value of \(\Delta\)U is very close to that for \(\Delta\)H.

A)True

B)False

Q3) Calculate the average H-S bond enthalpy in H₂S(g)given the standard enthalpies of formation for H₂S(g),H(g),and S(g): -20.1,218,and 223 kJ.mol^-1,respectively.

A)340 kJ.mol^-1

B)231 kJ.mol^-1

C)10.1 kJ.mol^-1

D)679 kJ.mol^-1

E)461 kJ.mol^-1

Q4) Work is reported in joules; and 1 joule = ____________

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Chapter 9: Thermodynamics: The Second and Third Laws

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Q1) When barium hydroxide is dissolved in water,the temperature of the solution increases.Which of the following statements regarding this reaction is true?

A)The reaction is spontaneous at all temperatures.

B)The reaction is driven only by the entropy.

C)The reaction is driven only by the enthalpy.

D)The reaction is spontaneous only at low temperatures.

E)The reaction is spontaneous only at high temperatures.

Q2) The dehydrogenation of cyclohexane,C₆H₁₂(l),to form benzene,C₆H₆(l),is not spontaneous.However,the hydrogenation of ethene to form ethane is spontaneous.Calculate the reaction free energy for the coupled reaction

C₆H₁₂(l)+

3CH₂=CH₂(g)\(\rightarrow\)

C₆H₆(l)+ CH₃CH₃(g)

Q3) When calculating the entropy change as a result of transferring heat reversibly to or from a system,the temperature must be constant.

A)True

B)False

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Chapter 10: Physical Equilibria

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Q1) Consider the phase diagrams for water and carbon dioxide given in the text on page 315.Explain the following observations: A thin wire with weights attached is draped over a block of "dry ice," a second wire with weights is draped over a block of ice.The wire cuts through the ice but not through the "dry ice."

Q2) For a one-component system,at the triple point

A)f = 3.

B)f = 2.

C)p = 1.

D)f = 0.

E)f = 1.

Q3) For CaCl₂,the absolute value of the enthalpy of hydration is larger than the lattice enthalpy.This means that for CaCl₂

A)the lattice enthalpy is negative.

B)the enthalpy of solution is endothermic.

C)the solubility increases when the temperature increases.

D)the enthalpy of hydration is positive.

E)the enthalpy of solution is exothermic.

Q4) Calculate the molality of ethanol in a solution of water,given that the mole fraction of ethanol is 0.300.

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Chapter 11: Chemical Equilibria

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Q1) The equilibrium constant for the reaction HNO₂(aq)+ H₂O(l) NO₂\(\rightarrow\)(aq)+ H₃O⁺(aq) is 4.3 * 10^-4 at 25S1U1P1\(\circ\)S1S1P0C.Will nitrous acid spontaneously dissociate when [HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-5 M?

Show your calculations.

Q2) Given: 2SO₂(g)+ O₂(g) 2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g),SO₂(g),and O₂(g)are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

A)1.31

B)0.42

C)0.014

D)0.059

E)0.87

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Chapter 12: Acids and Bases

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Q1) For a solution labeled "0.10 M H₂SO₄(aq),"

A)[HSO₄^-] is greater than 0.10 M.

B)the pH is less than 1.0.

C)[SO₄²^-] = 0.10 M.

D)the pH equals 1.0.

E)the pH is greater than 1.0.

Q2) The pH of 0.10 M pyridine(aq)is 9.13.What is the value of K_bfor pyridine?

A)2.7 * 10^-4

B)7.4 * 10^-10

C)2.7 * 10^-5

D)1.8 * 10^-10

E)1.8 * 10^-9

Q3) Which of the following aqueous solutions gives a pH greater than 7?

A)10^-8 M NH₄Cl

B)None of the solutions gives a pH greater than 7.

C)10^-8 M CH₃COOH

D)10^-8 M HCl

E)10^-8 M HCOOH

Q4) Write the autoprotolysis reaction for liquid ammonia.

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Chapter 13: Aqueous Equilibria

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Q1) The solubility of all except which the following compounds increases as the pH of the solution decreases?

A)CaF₂

B)Na₂CO₃

C)PbSO₃

D)KClO₄

E)CuS

Q2) 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

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) In the cell shown above,A is a standard Zn²⁺/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,which half-reaction occurs in the left-hand cell compartment?

A)Zn²⁺(aq)+ 2e^- \(\rightarrow\) Zn(s)

B)Zn(s)\(\rightarrow\) Zn²⁺(aq)+ 2e^-

Q2) For the cell diagram Pt|H₂(g),H⁺(aq)m Cu²⁺(aq)|Cu(s)

Which reaction occurs at the anode?

A)Cu(s)\(\rightarrow\) Cu²⁺(aq)+ 2e^-

B)2H⁺(aq)+ 2e^-\(\rightarrow\) H₂(g)

C)2H⁺(aq)+ Cu(s)\(\rightarrow\) H₂(g)+ Cu²⁺(aq)

D)Cu²⁺(aq)+ 2e^-\(\rightarrow\) Cu(s)

E)H₂(g)\(\rightarrow\) 2H⁺(aq)+ 2e^-

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

Q4) How many seconds are required to produce 4.99 mg of chromium metal from an acidic solution of potassium dichromate,using a current of 0.234 A?

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Chapter 15: Chemical Kinetics

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Q1) A possible mechanism for the reaction 2NO(g)+ O₂(g)\(\rightarrow\) 2NO₂(g)is: 2NO(g) N₂O₂(g) K₁,k₁',fast N₂O₂(g)+ O₂(g)\(\rightarrow\)2NO₂(g) K₂,slow

Application of the steady-state approximation gives A)[N₂O₂] = 0.

B)k₁[NO]²

-k₂[N₂O₂][O₂] = 0.

C)[N₂O₂] = (k₁/k₂)[NO]². D)k₁[NO]² -k₁'[N₂O₂]k₂[N₂O₂][O₂] = 0. E)[N₂O₂] = (k₁/k₁')[NO]².

Q2) For the elementary reaction A + 2B \(\rightarrow\) products,rate = k[A][B].

A)True

B)False

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Chapter 16: The Elements: the Main Group Elements

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Q1) The compound BeI₂ is an ionic compound.

A)True

B)False

Q2) Sodium borohydride is an oxidizing agent.

A)True

B)False

Q3) The anhydrous material with the common name "Epsom salts" has what chemical formula?

A)MgSO₄

B)Mg(OH)₂

C)CaSO₄

D)CaCl₂

E)MgCl₂

Q4) Circle the species that has the largest radius: Ca²⁺,S^2-,S,Cl.

Q5) Write the reaction for the disproportionation of nitrogen dioxide in water.

Q6) Write the formula of the hydride ion.

Q7) Write the equation for the production of sulfur by the Claus process,identify the reducing agent,and state the total number of electrons transferred in the reaction.

Page 18

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Chapter 17: The Elements: The D Block

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Q1) Except for scandium and titanium,all the 3d transition metals form divalent ions in aqueous solution.

A)True

B)False

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

A)Ru

B)Pt

C)Mo

D)Cd

E)Zn

Q3) When one mole of trans-tetraamminedichlorocobalt(III)chloride dissolves in water,how many moles of ions does it produce?

A)1 mole of ions.

B)2 moles of ions.

C)3 moles of ions.

D)4 moles of ions.

Q4) Complexes with coordination number 4 are either tetrahedral or octahedral.

A)True

B)False

Q5) Why is \(\Delta\)_T is always greater than \(\Delta\)_O?

Page 19

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Chapter 18: Nuclear Chemistry

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Q1) When a \(\beta\) particle is emitted,the mass number

A)decreases by 4.

B)increases by 1.

C)decreases by 2.

D)decreases by 1.

E)does not change.

Q2) Heavy elements are more likely to give off \(\beta\) radiation.

A)True

B)False

Q3) Which of the following is most likely to undergo \(\alpha\) decay?

A)²⁴Na

B)⁴⁷K

C)¹⁴C

D)²³²Th

E)³H

Q4) The nuclide ⁷Be decays by electron capture.

A)True

B)False

Q5) For the fusion of two deuterium atoms to produce helium-4,the difference in mass between products and reactants is -0.0256 u.What is E per mole of helium?

Page 20

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Chapter 19: Organic Chemistry I

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Q1) The compound 1-chloro-1-pentene

A)can exist as cis and trans isomers.

B)has the formula C₅H₁₁Cl.

C)cannot exist as cis and trans isomers.

D)is an alkyne.

E)has 3 structural isomers.

Q2) Name the compound

CH₃C(CH₃)₂CH₂CH₃.

A)2-isopropylpropane

B)1-methyl-2-propylethane

C)2,2-dimethylbutane

D)1,1-dimethylbutane

E)Hexane

Q3) A racemic mixture is an equal mixture of enantiomers and therefore is optically active.

A)True

B)False

Q4) A dichlorobenzene reacts with HNO₃/H₂SO₄ and produces three mononitrated products.Identify the initial dichlorobenzene.

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Chapter 20: Organic Chemistry II

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Q1) All the following polymers are produced by addition polymerization except A)polyethylene.

B)Dacron. C)PVC.

D)polypropylene.

E)Teflon.

Q2) Predict the product(s)of the reaction of acetic acid with methylamine at 200^oC.

A)CH₃COO^-and CH₃NH₃⁺

B)No reaction occurs.

C)CH₃C(O)OCH₃

D)CH₃CONHCH₃

E)CH₃CONH₂

Q3) Predict the product of the reaction of acetic acid with trimethylamine.

A)CH₃CON(CH₃)₃⁺

B)CH₃CONHCH₃

C)CH₃CON(CH₃)₂

D)CH₃CONH₂

E)No reaction occurs.

Q4) What reactants could be used to synthesize CH₃CONH₂?

Page 22

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