Physical Chemistry I Review Questions - 1986 Verified Questions

Physical Chemistry I Review Questions

Course Introduction

Physical Chemistry I provides an in-depth introduction to the fundamental principles governing chemical systems at the molecular level. This course covers topics such as thermodynamics, chemical equilibria, phase transitions, and the properties of gases, liquids, and solids. Students will explore concepts including the laws of thermodynamics, enthalpy, entropy, free energy, and their applications to biological and chemical processes. Emphasis is placed on quantitative problem-solving and the development of a molecular understanding of macroscopic phenomena, preparing students for advanced coursework in chemistry 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) What does the term "black body" signify for an object?

A)The object is white hot.

B)The object is black to human sight.

C)The object absorbs and emits all wavelengths

D)The object absorbs certain wavelengths of light preferentially.

E)There is no significance to the name.

Answer: C

Q2) What is the energy of a mole of photons with a frequency of 3.2 *10¹⁶ Hz?

A)1.3 * 10⁷J/mol

B)1.3 * 10^-7J/mol

C)3.2 * 10¹⁶J/mol

D)7.7 *10^-⁸J/mol

E)7.7 * 10⁸J/mol

Answer: A

Q3) In everyday life,we have no difficulty in measuring both the velocity and position of objects.

A)True

B)False Answer: True

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) An aluminum atom contains how many unpaired electrons?

A)7

B)6

C)5

D)4

E)3

Answer: E

Q2) Which atom has the highest first ionization energy?

A)Mg

B)Ca

C)Sr

D)Ba

Answer: A

Q3) Write the ground-state electron configuration of FeS1U1P13+S1S1P0.

A)[Ar]3dS1U1P15S1S1P04sS1U1P12S1S1P0

B)[Ar]3dS1U1P13S1S1P04sS1U1P12S1S1P0

C)[Ar]3dS1U1P13S1S1P04sS1U1P10S1S1P0

D)[Ar]3dS1U1P16S1S1P04sS1U1P11S1S1P0

E)[Ar]3dS1U1P13S1S1P04sS1U1P13S1S1P0

Answer: B

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Chapter 3: Chemical Bonds

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Sample Questions

Q1) Because of the octet rule,the gaseous O²^- ion is stable.

A)True

B)False

Answer: False

Q2) Estimate the CN bond length in urea,NH₂CONH₂.Given: covalent radii (pm)of C-,77; C=,67; N-,75; N=,60; O-,74; O=,60; H,37.

A)71 pm

B)127 pm

C)76 pm

D)152 pm

E)142 pm

Answer: D

Q3) How many electrons are in the expanded valence in XeO₄?

Answer: 16

Q4) Why are the N-O bond lengths in NO₃^- the same?

Answer: The explanation is resonance.

Q5) List the chalcogens in order of increasing electronegativity.

Answer: tellurium < selenium < sulfur < oxygen.

Q6) If dinitrogen oxide has a dipole moment,what is the arrangement of atoms?

Answer: N-N-O

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Chapter 4: Molecular Shape and Structure

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Sample Questions

Q1) What is the shape of XeF₄?

A)Square planar

B)Tetrahedral

C)Trigonal bipyramidal

D)Seesaw

E)T-shaped

Q2) How many lone pairs of electrons are there in the Lewis structure of azidocarbonamide,H₂NC(O)NNC(O)NH₂?

A)8

B)12

C)10

D)16

E)6

Q3) For A₂,the LCAO-MO,\(\varPsi\) = c_A\(\varPsi\) _A + c_B\(\varPsi\) _B,has c_A = c_B.

A)True

B)False

Q4) What is the ground-state electron configuration of O₂^-?

Q5) Name all the angles in a trigonal planar geometry.

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Chapter 5: The Properties of Gases

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Q1) Helium,H₂,and neon all have very small values of the van der Waals coefficient "a",whereas Cl₂,xenon,and water have large values.Which gases would you expect to be able to be liquefied by expansion?

Q2) Consider two cylinders of gas,both with a volume of 25 L and at 1 atm and 25S1U1P1\(\circ\)S1S1P0C.If one cylinder contains nitrogen gas and the other argon,which of the following statements are true and which are false.

(a)The temperature of the gases is different.

(b)The average molecular speed of the gases is the same.

(c)The average kinetic energy of the gases is the same.

Q3) The main composition of dry air at sea level is about 75.5% nitrogen,23.1% oxygen,and 1.3% argon.In a 1.00-g sample of dry air at 1.00 atm,calculate the partial pressure of argon gas.

Q4) What is the density of helium gas at 750 kPa and 25S1U1P1\(\circ\)S1S1P0C?

A)2.42 g.L^-¹

B)1.21 g.L^-¹

C)0.605 g.L^-¹

D)0.161 g.L^-¹

E)0.0120 g.L^-¹

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Page 7

Chapter 6: Liquids and Solids

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Q1) The ability of water to "wet" paper is due to hydrogen bonding between water molecules and surface molecules in the paper.True or false?

A)True

B)False

Q2) Tetrabromomethane has a higher boiling point than tetrachloromethane.True or false?

A)True

B)False

Q3) 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

Q4) Gold has a face-centered cubic unit cell.If the edge length of the unit cell is 407 pm,what is the atomic radius of gold?

Q5) Which has the higher boiling point,1,1-dichloroethene or cis-dichloroethene?

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Chapter 7: Inorganic Materials

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Sample Questions

Q1) How is pig iron produced?

A)In a charcoal fire.

B)Through multiple heatings.

C)In a blast furnace.

D)Through molten mixing with other metals.

E)It is naturally occuring.

Q2) Malleability refers to a metal's ability to be hammered into a specific shape.

A)True

B)False

Q3) What best describes alnico?

A)A metal alloy.

B)A ferromagnetic alloy.

C)A non-metallic alloy.

D)An anti-ferromagnetic alloy.

E)An iron-containing alloy.

Q4) How is bonding in solids best described?

A)Bands of atomic orbitals.

B)Bands of molecular orbitals.

C)A conduction band overlapping a valence band.

D)A conduction band overlapping a band gap.

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Chapter 8: Thermodynamics: The First Law

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Q1) When nitrogen gas expands from 3.00 to 6.00 L and 2.00 kJ of energy is transferred as heat to the nitrogen in a cylinder fitted with a piston at an external pressure of 2.00 atm,against this constant pressure,what is \(\Delta\)U for the process?

A)(-0.608 kJ)

B)+2.61 kJ

C)(-2.61 kJ)

D)0

E)+1.39 kJ

Q2) What equation corresponds to the standard enthalpy of formation of gaseous hydrogen atoms,which,at 298 K is +217 kJ.mol^-1?

Q3) 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

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) The standard free energy of formation of benzene,C₆H₆(l),is +124.3 kJ.mol^-1 at 298 K.This means that at 298 K benzene is thermodynamically unstable even though it can be kept indefinitely without decomposing.Explain.

Q2) Which of the following has the largest molar entropy?

A)H₂(g)

B)KF(aq)

C)CO₂(s)

D)CaO(s)

E)He(l)

Q3) Which of the following statements is true?

A)The molar entropy does not depend on the structure of the compound.

B)The molar entropy of H₂O(l)is about the same as the molar entropy of ice.

C)An isothermal process that leads to a decrease in free energy is spontaneous.

D)If \(\Delta\)G_rS1U1P1\(\circ\)S1S1P0> 0,then the reaction is spontaneous.

E)All processes that give positive changes in energy are spontaneous.

Q4) What is the change in entropy when the pressure of an ideal gas is increased at constant temperature? Choose from +,0,-.

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11

Chapter 10: Physical Equilibria

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Sample Questions

Q1) Consider the phase diagram for sulfur in the text on page 316.Monoclinic sulfur is denser than rhombic sulfur.

A)True

B)False

Q2) Which of the following has the smallest freezing point depression and the smallest boiling point elevation?

A)2.0 m potassium chloride

B)1.5 m magnesium phosphate

C)1.0 m sodium chloride

D)1.5 m aluminum nitrate

E)Both A and C

Q3) For AlF₃,the lattice enthalpy is 5220 kJ.mol^-1 and the enthalpy of solution is -27 kJ.mol^-1 at 25S1U1P1\(\circ\)S1S1P0C.Calculate the enthalpy of hydration of AlF₃ at this temperature.

Q4) Water and acetone,CH₃COCH₃,both freeze at a higher temperature under pressure.

A)True

B)False

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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Sample Questions

Q1) For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction,\(\Delta\)HS1U1P1\(\circ\)S1S1P0 = 92.38 kJ.mol^-1.

A)193 K

B)353 K

C)466 K

D)492 K

E)219 K

Q2) Consider the reaction CO(g)+ 2H₂(g) CH₃OH(g)

At room temperature,K is approximately 2 * 10⁴,but at a higher temperature K is substantially smaller.Which of the following is true?

A)The reaction is endothermic.

B)The value of K_c for this reaction is smaller at all temperatures.

C)At the higher temperature,more CH₃OH(g)is produced.

D)The reaction is exothermic.

E)The reaction becomes spontaneous at higher temperatures.

Q3) Consider the reaction

Na⁺(g)+ Cl^-(g) NaCl(s)

If the temperature is lowered,the products/reactants are favored.

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Page 13

Chapter 12: Acids and Bases

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Q1) The amino acid methionine,HOOC-CH(CH₂CH₂SCH₃)NH<sub>3</s ub>⁺,has pK_a1 = 2.2 and pK_a2 = 9.1.If this amino acid is represented by H₂L⁺,the major species at pH 6 is

A)HL

B)H₂L⁺

C)L^-

D)HL and L^-

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) All of the following acids have the same strength in water except A)HNO₃

B)HClO₃

C)HBr

D)HF

Q4) Write the autoprotolysis reaction for liquid ammonia.

Page 14

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Chapter 13: Aqueous Equilibria

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Q1) Consider the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq),with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

Q2) What is the main factor that determines the pH of any buffer?

Q3) A buffer solution contains 0.25 M NaNO₂(aq)and 0.80 M HNO₂(aq)(pK_a = 3.37).What is the pH after 0.10 mol HBr are added to 1.00 L of this buffer?

A)11.41

B)4.15

C)2.59

D)9.85

E)3.37

Q4) Which of the following water-insoluble salts is more soluble in 1.0 M HClO₄(aq)?

A)AgBr

B)PbF₂

C)Hg₂Br₂

D)PbI₂

E)AgClO₄

Page 15

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Chapter 14: Electrochemistry

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Q1) Consider the following cell: Zn(s)|Zn²⁺(aq,0.10 M)m|Cu²⁺(aq,0.10 M)|Cu(s)

At equilibrium,what is the concentration of Zn²⁺(aq)?

Q2) If the standard potential for Ti³⁺(aq)/Ti²⁺(aq)is -0.37 V and the standard potential for Ti²⁺(aq)/Ti(s)is -1.63 V,calculate the standard potential for Ti³⁺(aq)+ 3e^- \(\rightarrow\) Ti(s).

A)-1.19 V

B)-0.40 V

C)-2.00 V

D)-1.26 V

E)-1.21 V

Q3) If the standard free energy change for combustion of 1 mole of CH₄(g)is -818 kJ.mol^-¹,calculate the standard voltage that could be obtained from a fuel cell using this reaction.

A)-1.06 V

B)+0.53 V

C)+4.24 V

D)+8.48 V

E)+1.06 V

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Page 16

Chapter 15: Chemical Kinetics

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Q1) Consider the reaction 2A \(\rightarrow\)B,Rate = k[A]²

If the rate of disappearance of A is followed,derive the experimental rate constant.

Q2) Consider the following mechanism for the destruction of ozone. O₃ + NO \(\rightarrow\) NO₂ + O₂ NO₂ + O \(\rightarrow\) NO + O₂

What is the catalyst in this reaction?

Q3) A second-order reaction has a rate constant of 1.25 M^-1.s^-1.If the initial reactant concentration is 1.0 M,calculate the time required for 90% reaction.

A)1.3 s

B)7.2 s

C)0.13 s

D)17 s

E)0.89 s

Q4) The rates of first-order and second-order reactions do not change with elapsed time.

A)True

B)False

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Chapter 16: The Elements: the Main Group Elements

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Q1) Which of the following reactions does not occur?

A)2Br^-(aq)+ Cl₂(g)\(\rightarrow\) Br₂(l)+ 2Cl^-(aq)

B)2I^-(aq)+ Cl₂(g)\(\rightarrow\) I₂(aq)+ 2Cl^-(aq)

C)Cl₂(g)+ H₂O(aq)\(\rightarrow\) HClO(aq)+ HCl(aq)

D)KI(s)+ H₃PO₄(aq)\(\rightarrow\)

KH₂PO₄(AQ)+ hi(G)

E)2^-(aq)+ Cl₂(g)\(\rightarrow\) F₂(g)+ 2Cl^-(aq)

Q2) All of the following are silicon-oxygen compounds except A)asbestos.

B)quartz.

C)talc.

D)diamond.

E)mica.

Q3) In the reaction

Cu²⁺(aq)+ 4NH₃(aq)\(\rightarrow\) Cu(NH₃)₄²⁺(aq) the Lewis acid is ____________ and the Lewis base is ____________.

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Chapter 17: The Elements: The D Block

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Q1) For which one of the following would it not be possible to distinguish between high-spin and low-spin complexes in octahedral geometry?

A)Cr(II)

B)Co(III)

C)Co(II)

D)Fe(II)

E)Ni(II)

Q2) Which of the following complexes has the smallest d-orbital splitting energy?

A)Co(NH₃)₆³⁺

B)Co(NH₃)₅OH²⁺

C)Co(NH₃)₅CN²⁺

D)Co(NH₃)₅I²⁺

E)Co(NH₃)₅(OH₂)³⁺

Q3) rhodium complexes are high spin?

A)True

B)False

Q4) The ligand 4-cyanopyridine can form _____ complex(es)with penataamminecobalt(III).

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 nuclei is stable?

A)¹²⁰Sn

B)²¹³Fr

C)³⁸Cl

D)²⁴Na

E)¹⁵O

Q2) Nuclides that lie above the band of stability are proton rich.

A)True

B)False

Q3) Which of the following nuclei is most likely to emit a positron?

A)²⁴⁶Am

B)⁵⁹Ni

C)¹¹⁸Sn

D)³³Cl

E)²⁰Ne

Q4) 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?

Q5) The rate of nuclear decay does not depend on temperature.

A)True

B)False

Page 20

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Chapter 19: Organic Chemistry I

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Q1) Alkanes undergo substitution by a radical chain mechanism,even though they are very unreactive?

A)True

B)False

Q2) Which of the following forms a meta-product upon nitration?

A)Benzoic acid

B)Aaniline

C)Phenol

D)Chlorobenzene

Q3) The compound (CH₃)₃CCH₂CH(CH₃)₂ is

A)named as a pentane but is an isomer of heptane.

B)named as a pentane but is an isomer of octane.

C)named as a hexane but is an isomer of octane.

D)named as a pentane but is an isomer of hexane.

E)named as a butane but is an isomer of octane.

Q4) Alkanes react with boiling sulfuric acid because the C-C and C-H bonds are easily attacked.

A)True

B)False

Page 21

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Chapter 20: Organic Chemistry II

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Q1) Which of the following is most volatile?

A)(CH₃)₂C(OH)CH₃

B)(CH₃)₃COH

C)CH₃CH(OH)CH₂CH₃

D)CH₃(CH₂)₃OH E)CH₃CH₂CH₂CH₃

Q2) The major product of the reaction of (CH₃)₂CHCH(Br)CH₃ with concentrated KOH in alcohol solvent is

A)2-methyl-2-butene.

B)3-methyl-1-butene.

C)2-hydroxy-3-methylbutane.

D)pentene.

E)3-methylbuatanol.

Q3) The formula of the polymer methyl methacrylate (Plexiglass)is -(CH₃OC(O)C(CH₃)CH₂)-.What is the monomer used to produce this polymer?

Q4) When amines condense with carboxylic acids,what molecule is eliminated?

Q5) What are the hybridization schemes of the C and N atoms,respectively,in C₆H₅CONHCH₃?

Page 22

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