Physical Science Chemistry Practice Questions - 1986 Verified Questions

Physical Science Chemistry

Practice Questions

Course Introduction

Physical Science Chemistry explores the fundamental concepts of chemistry within the broader context of physical science. The course covers key topics such as atomic structure, chemical bonding, states of matter, chemical reactions, and the periodic table. Students will learn how chemical principles apply to everyday life and various scientific fields, as well as develop skills in laboratory techniques, scientific reasoning, and problem-solving. Through a combination of lectures, experiments, and projects, the course provides a strong foundation for further study in chemistry and related sciences.

Recommended Textbook

Chemical Principles 6th Edition by Professor Peter Atkins

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20 Chapters

1986 Verified Questions

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Page 2

Chapter 1: The Quantum World

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Q1) Which of the following statements regarding electromagnetic radiation is true?

A)Electromagnetic radiation with a wavelength of 400 nm travels faster than that with a wavelength of 600 nm.

B)The frequency of electromagnetic radiation determines how fast it travels.

C)Electromagnetic radiation with a wavelength of 400 nm has a frequency that is smaller than that with a wavelength of 600 nm.

D)Electromagnetic radiation with a wavelength of 600 nm travels faster than that with a wavelength of 400 nm.

E)Electromagnetic radiation with a wavelength of 600 nm has a frequency that is smaller than that with a wavelength of 400 nm.

Answer: E

Q2) What is the frequency of radiation with a wavelength of 2.0 m?

A)1.5 * 10⁸ /sec

B)3.0 * 10⁸ /sec

C)7.0 * 10^-9 /sec

D)7.0 * 10⁸ /sec

E)1.5 * 10^-8 /sec

Answer: A

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Page 3

Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) Which of the following has the smallest radius?

A)P⁺⁵

B)P^3-

C)N⁺⁵

D)N

E)N³

Answer: C

Q2) Which atom has the lowest electron affinity?

A)Al

B)Si

C)P

D)S

Answer: A

Q3) Which of the following has the smallest atomic radius?

A)Cl

B)P

C)S

D)Si

E)Al

Answer: A

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Chapter 3: Chemical Bonds

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Sample Questions

Q1) How many lone pairs of electrons are found in the Lewis structure of hydrazine,H₂NNH₂?

A)8

B)4

C)1

D)0

E)2

Answer: E

Q2) Which of the following compounds is the least stable?

A)CH₄

B)SnH₄

C)SiH₄

D)GeH₄

E)PbH₄

Answer: E

Q3) In the "best" Lewis structure of XeO₄,there are two double bonds and the formal charge on Xe is zero.

A)True

B)False

Answer: False

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Chapter 4: Molecular Shape and Structure

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Sample Questions

Q1) What is the shape of the molecule AX₄E₂?

A)Octahedral

B)Tetrahedral

C)Seesaw

D)Square planar

E)Square pyramidal

Q2) What is the approximate NNC bond angle in azidocarbonamide,H₂NC(O)NNC(O)NH₂?

A)118S1U1P1\(\circ\)S1S1P0

B)180S1U1P1\(\circ\)S1S1P0

C)90S1U1P1\(\circ\)S1S1P0

D)107S1U1P1\(\circ\)S1S1P0

E)109S1U1P1\(\circ\)S1S1P0

Q3) How many \(\sigma\)- and \(\pi\)-bonds are present in diazomethane,CH₂NN?

Q4) The molecule cis-dichloroethene is nonpolar.

A)True

B)False

Q5) What is the bond order in the OH radical?

Q6) Name all the angles in a trigonal planar geometry.

Page 6

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Chapter 5: The Properties of Gases

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Q1) Ammonium nitrate can decompose according to the following equation: NH₄NO₃(s)\(\rightarrow\) N₂O(g)+ 2H₂O(g)

How many liters of gas are produced by decomposition of 160 g of ammonium nitrate at -25S1U1P1\(\circ\)S1S1P0C and 86.0 kPa?

A)48.0

B)14.5

C)57.6

D)173

E)144

Q2) In a gas,temperature is proportional to the square root of the average speed of the molecules.True or false?

A)True

B)False

Q3) What is the molar volume of a nitrogen gas at -27.0^oC and 1 atm?

A)2.22 L

B)22.4 L

C)24.6 L

D)20.2 L

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Page 7

Chapter 6: Liquids and Solids

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Sample Questions

Q1) Viscosity usually decreases with increasing temperature.True or false?

A)True

B)False

Q2) Metals with a hexagonal close-packed structure have/do not have slip planes and as a result are malleable/brittle.

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

A)True

B)False

Q4) Which of the following has the largest value of surface tension?

A)H₂O

B)CCl₄

C)CH₃OH (methanol)

D)Hg

E)C₆H₆ (benzene)

Q5) BN 2.I₂ 3.ice 4.SiO₂ 5.Ba 6.C 7.BeCl₂ 8.B

A)2,3,7,and 1,4,6,8

B)1,2,3,and 6,8

C)1,2,4,7,and 5,6,8

D)1,2,4,7,and 6,8

E)2,4,7,and 6,8

Page 8

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Chapter 7: Inorganic Materials

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Sample Questions

Q1) What do the current high temperature superconductors have in common?

A)They are all metals.

B)They are all non-metals.

C)They are all undoped materials.

D)They are ceramic oxides.

E)Nothing.There is nothing in common.

Q2) 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.

Q3) How are atoms in a substitutional alloy arranged?

A)In micro-clusters within the greater solid.

B)In precise,geometric arrays.

C)Those of one element replace those of the major element.

D)Those of one element fit into the interstices formed by the major element.

E)In planes,known as slips.

Q4) Bone is a composite composed of collagen and ______________________ (phosphate salts /carbonate salts / sulfate salts).

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Chapter 8: Thermodynamics: The First Law

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Sample Questions

Q1) The formation of solid calcium oxide from a gas of its ions is an exothermic process and is equal to the reverse of the lattice enthalpy.

A)True

B)False

Q2) The standard enthalpy of formation of NaCl(s)is -411 kJ/mol.In a Born-Haber cycle for the formation of NaCl(s),which enthalpy change(s)is/are endothermic?

A)the lattice enthalpy of NaCl(s)

B)the electron affinity of chlorine

C)the reverse of the lattice enthalpy of NaCl(s)

D)All of the enthalpy changes are endothermic except for the standard enthalpy of formation of NaCl(s).

Q3) An isothermal change is one that occurs at a constant temperature.

A)True

B)False

Q4) What equation corresponds to the standard enthalpy of formation of gaseous hydrogen atoms,which,at 298 K is +217 kJ.mol^-1?

Q5) Work is reported in joules; and 1 joule = ____________

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Chapter 9: Thermodynamics: The Second and Third Laws

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Sample Questions

Q1) Consider the compounds

PCl₅(g),HCN(g),CuO(s),NO(g),NH₃(g),and SO₂(g).

Which compound will have approximately the same stability with respect to its elements if the temperature is raised?

A)CuO(s)

B)NO(g)

C)PCl₅(g)

D)HCN(g)

E)NH₃(g)

Q2) An example of a spontaneous process having \(\Delta\)H ~ 0 is

A)1 L He(1 atm,298 K)+ 1 L Ar(1 atm,298 K)\(\rightarrow\) 2 L He/Ar mixture(1 atm,298 K).

B)evaporation of water at 100S1U1P1\(\circ\)S1S1P0C and 1 atm.

C)a ball rolling from the top of a hill to the bottom of a valley.

D)precipitation of AgBr(s)from a solution of Ag⁺(aq)and Br^-(aq).

E)freezing of water at -10S1U1P1\(\circ\)S1S1P0C.

Q3) For CO₂(g)\(\rightarrow\) CO₂(aq),is the entropy change positive or negative?

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Chapter 10: Physical Equilibria

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Q1) The vapor pressure of methanol at 25S1U1P1\(\circ\)S1S1P0C is 123 Torr and its enthalpy of vaporization is 35.3 kJ.mol^-1.Estimate the normal boiling point of methanol.Assume the enthalpy of vaporization is independent of temperature.

A)450 K

B)342 K

C)315 K

D)373 K

E)Not enough information given.

Q2) The vapor pressure of water at 37S1U1P1\(\circ\)S1S1P0C is 47.1 Torr and its enthalpy of vaporization is 44.0 kJ.mol^-1.Estimate the vapor pressure of water at 87S1U1P1\(\circ\)S1S1P0C.Assume that the enthalpy of vaporization of water is independent of temperature.

A)112 Torr

B)256 Torr

C)713 Torr

D)52 Torr

E)504 Torr

Q3) Which liquid would you expect to be the more volatile,CH₃CHO or CH₃OCH₃?

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Page 12

Chapter 11: Chemical Equilibria

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Sample Questions

Q1) At 25S1U1P1\(\circ\)S1S1P0C,\(\Delta\)GS1U1B1rS1U1B0S1U1P1oS1S1P0 for the reaction

2SOS1U1B12S1U1B0(g)+ OS1U1B12S1U1B0(g) ?S1U1B02SOS1U1B13S1U1B0(g)is -141.74 kJ·molS1U1P1-1S1S1P0.Calculate the value of KS1U1B1cS1U1B0 for this reaction.

A)1.74 * 10S1U1P126S1S1P0

B)7.01 * 10S1U1P124S1S1P0

C)2.65 * 10S1U1P112S1S1P0

D)6.56 * 10S1U1P113S1S1P0

Q2) 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.

Q3) At equilibrium,Q = K and \(\Delta\)G°_r = 0. A)True B)False

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Chapter 12: Acids and Bases

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Sample Questions

Q1) HBrO(aq),in a 0.25 M solution,has a pK_a = 8.69.What is its pH?

A)0.60

B)4.65

C)5.90

D)8.10

E)9.30

Q2) Which of the following is the conjugate acid of H₂PO₄^-?

A)PO₄³^-

B)OH^-

C)H₃PO₄

D)H₂PO₄^-

E)HPO₄²^-

Q3) All of the following are Lewis bases except

A)OH^-

B)H₂O

C)SO₃

D)Br^-

Q4) What is the conjugate acid of O^2-?

Q5) Write the autoprotolysis reaction for liquid ammonia.

Page 14

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Chapter 13: Aqueous Equilibria

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Sample Questions

Q1) Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)₂(s)in water at 25S1U1P1\(\circ\)S1S1P0C is 0.011 M.

A)1.5 * 10^-8

B)1.1 * 10^-5

C)2.7 * 10^-6

D)5.3 * 10^-6

E)1.2 * 10^-4

Q2) A certain weak acid has a K_a of 2.0 * 10^-⁵.What is the equilibrium constant for the reaction of this acid with a strong base?

Q3) Which of the following indicators would be most suitable for the titration of 0.10 M lactic acid with 0.10 M KOH(aq)? For lactic acid,pK_a = 3.08.

A)Methyl orange (pK_In = 3.4)

B)Thymol blue (pK_In = 1.7)

C)Alizarin yellow (pK_In = 11.2)

D)Bromophenol blue (pK_In = 3.9)

E)Phenol red (pK_In = 7.9)

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

Q5) What is the main factor that directly determines the pH of any buffer?

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Chapter 14: Electrochemistry

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Q1) If the standard potential for Cu²⁺(aq)/Cu⁺(aq)is 0.15 V and the standard potential for Cu²⁺(aq)/Cu(s)is 0.34 V,calculate the standard potential for Cu⁺(aq)+ e^- \(\rightarrow\) Cu(s).

A)+0.32 V

B)+0.64 V

C)+0.53 V

D)+0.83 V

E)+0.49 V

Q2) The half-reaction that occurs at cathode when 1 M AgNO₃(aq)is electrolyzed is __________________.

Q3) Which species will reduce Br₂ but not V³⁺?

A)Ce

B)Zn

C)Cu

D)Cr²⁺

E)Al

Q4) In order to convert hydrazine,N₂H₄,to nitric acid, A)an oxidizing agent is required.

B)a reducing agent is required.

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Chapter 15: Chemical Kinetics

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Q1) The reaction 2NO(g)+ O₂(g)\(\rightarrow\)2NO₂(g)has \(\Delta\)H_rS1U1P1\(\circ\)S1S1P0= -114 kJ.mol^-1.A possible mechanism for this reaction is 2NO(g) N₂O₂(g)

Rapid equilibrium,K

N₂O₂(g)+ O₂(g)\(\rightarrow\)2NO₂(g) Slow,k

If the activation energy for the reverse reaction is 225 kJ.mol^-1,what is the activation energy for the forward reaction?

A)Because an intermediate is involved,the forward activation energy cannot be calculated with the given information.

B)111 kJ.mol^-1

C)339 kJ.mol^-1

D)114 kJ.mol^-1

E)55.5 kJ.mol^-1

Q2) For a zero-order reaction,the rate constant has the same units as the rate of reaction.

A)True

B)False

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) All of the following react with water to form hydrogen and a hydroxide except A)Mg.

B)Na.

C)Ca.

D)K.

E)Be.

Q2) Aqueous solutions of phosphine,PH₃,

A)are neutral.

B)contain the PH₂^-(aq)ion exclusively.

C)are basic.

D)readily form PH₄⁺(aq). E)cannot exist.

Q3) The starting material for the production of sulfuric acid by the contact process is A)H₂S(g).

B)H₂S₂O₇(l).

C)S(g).

D)SO₃(g).

E)SO₂(g).

Q4) Write the reaction for the disproportionation of nitrogen dioxide in water.

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Chapter 17: The Elements: The D Block

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Q1) The cationic complex [Co(OH₂)₆]²⁺ should have how many unpaired electrons?

A)0

B)1

C)2

D)3

E)4

Q2) One mole of cis-tetraamminedichlororhodium(III)chloride dissolves in water to give

A)3 moles of ions.

B)2 moles of ions.

C)1 mole of ions.

D)6 moles of ions.

Q3) Which of the following pairs have about the same atomic radius?

A)Cu and Ag

B)Co and Rh

C)Fe and Ru

D)Mn and Tc

E)Ru and Os

Q4) Why is \(\Delta\)_T is always greater than \(\Delta\)_O?

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Chapter 18: Nuclear Chemistry

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Q1) Cobalt-60,used in the radiation treatment of cancer,is produced by absorption of 2 neutrons and emission of a \(\beta\)particle.What is the starting nuclide?

A)⁵⁸Mn

B)⁵⁸Ni

C)⁵⁸Fe

D)⁵⁹Co

E)⁵⁹Fe

Q2) The nuclide ⁷Be decays by electron capture.

A)True

B)False

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

A)²²²Rn

B)¹¹Li

C)²³⁵U

D)¹¹⁴Cs

E)²²⁶Ra

Q4) In the following equations,fill in the missing species. (a)⁴¹Ca + ___ \(\rightarrow\) ⁴¹K (b)¹⁵O \(\rightarrow\)¹⁵N + ___

Q5) Why does the band of stability curve upward at high atomic number?

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Chapter 19: Organic Chemistry I

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Q1) Name the compound CH₃CH=CHCH=CH₂.

Q2) With which of the following do alkanes react?

A)Boiling nitric acid

B)The strong oxidizing agent KMnO₄

C)Boiling aqueous sodium hydroxide to give alcohols

D)Concentrated sulfuric acid

E)Oxygen to give carbon dioxide and water

Q3) 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.

Q4) Heptane,with the formula,C₇H₁₆,can have how many isomeric structures?

A)4

B)5

C)6

D)7

E)9

Page 21

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Chapter 20: Organic Chemistry II

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Q1) When terephthalic acid ethylene glycol reacts to form the polyester Dacron,the first reaction product has

A)a free carboxyl and a free hydroxyl group.

B)2 free carboxyl groups.

C)2 free hydroxyl groups

D)2 free ester groups.

E)a free ester group and a free hydroxyl group.

Q2) Which of the following is a peptide bond?

A)(-C(O)O-)

B)(-CONH-)

C)(-C-NH-)

D)(-C=N-)

E)(-C(O)-)

Q3) Complete hydrolysis of a hexapeptide yielded Arg,Tyr,Val,Phe,Cys.After partial hydrolysis,the fragments Tyr-Cys,Arg-Phe,Cys,Val-Arg,and Phe-Tyr were obtained.What are the possible sequences in the hexapeptide?

Q4) Ethers are less volatile than alcohols of the same molar mass.

A)True

B)False

Q5) What reactants could be used to synthesize CH₃CONH₂?

Page 22

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