Foundations of Chemistry Test Preparation - 1986 Verified Questions

Foundations of Chemistry Test Preparation

Course Introduction

Foundations of Chemistry provides an essential introduction to the fundamental principles of chemical science. The course covers atomic and molecular structure, chemical bonding, stoichiometry, the periodic table, states of matter, chemical reactions, thermochemistry, and the properties of solutions. Emphasis is placed on the scientific method, problem-solving skills, laboratory techniques, and real-world applications of chemistry, preparing students for advanced study in science, engineering, and health-related fields.

Recommended Textbook

Chemical Principles 6th Edition by Professor Peter Atkins

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20 Chapters

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Chapter 1: The Quantum World

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Q1) 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

Q2) Light of wavelength 242 nm ionizes a sodium ion in the gas phase; what is the ionization energy of sodium?

A)8.20 kJ.mol^-¹

B)988 kJ.mol^-¹

C)198 kJ.mol^-¹

D)494 kJ.mol^-¹

E)247 kJ.mol^-¹

Answer: D

Q3) A node is a point at which the wavefunction becomes zero.

A)True

B)False

Answer: False

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) Which of the following has the largest radius?

A)P³

B)Cl^-

C)K⁺

D)Cl

E)N³

Answer: A

Q2) What is the ground-state electron configuration of Nb?

A)[Kr]4d⁴5s¹

B)[Kr]4d⁵5s²

C)[Kr]5d³4s²

D)[Kr]5d³5s²

E)[Kr]4d³5s²

Answer: E

Q3) Which atom has the highest second ionization energy?

A)Cs

B)Na

C)Li

D)K

Answer: C

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Chapter 3: Chemical Bonds

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Q1) Which of the following has the highest melting point?

A)KF

B)KI

C)RbF

D)KBr

E)KCl

Answer: A

Q2) Write three Lewis structures for the cyanate ion,NCO^-,where the arrangement of atoms is N-C-O.In the most plausible structure,

A)there is a triple bond between N and C.

B)there are two double bonds.

C)there is a triple bond between C and O.

D)the formal charge on O is +1.

E)the formal charge on N is -1.

Answer: A

Q3) Write all possible Lewis structures of sulfur dioxide.Which structure is most feasible?

Answer: The structure with the expanded valence is favored.

Q4) 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 SO₃²^-?

A)T-shaped

B)Trigonal pyramidal

C)Seesaw

D)Tetrahedral

E)Trigonal planar

Q2) All the following have a linear shape except

A)BeCl₂.

B)O₃.

C)I₃^-.

D)XeF₂.

E)CS₂.

Q3) Both C₂ and C₂² are diamagnetic.True or false?

A)True

B)False

Q4) Predict the HNH bond angle in NH₂^-

Q5) How many peaks would you predict for the photoelectron spectrum of water using 1)the molecular orbital model and 2)the VSEPR model?

Q6) Predict the electron arrangement in ClF₃.

Q7) Predict the electron arrangement in IF₅.

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Chapter 5: The Properties of Gases

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Sample Questions

Q1) Which of the following gases effuses slowest?

A)Fluorine

B)Carbon dioxide

C)Chlorine

D)Carbon monoxide

E)Nitrogen

Q2) How many atoms of argon occupy 20.00 mL if the temperature is 200°C and the pressure is 2.00 × 10-3 Torr?

A)2.01 * 10¹⁷

B)6.02 * 10^-17

C)3.10 * 10¹⁷

D)2.44 * 10¹⁹

E)2.80 * 10^-¹¹

Q3) Calculate the density of camphor,C₁₀H₁₆O,at

80S1U1P1\(\circ\)S1S1P0C and 12 Torr.

A)8.2 * 10^-⁴ g.L^-¹

B)0.083 g.L^-¹

C)0.37 g.L^-¹

D)0.62 g.L^-¹

E)6.8 * 10^-3 g.L^-¹

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Chapter 6: Liquids and Solids

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Q1) What are all the intermolecular forces that are responsible for the existence of ice?

A)Dipole-dipole and London forces

B)London forces

C)Dipole-dipole,London forces,and hydrogen bonding

D)Dipole-dipole and ion-ion

E)Hydrogen bonding and dipole-dipole

Q2) How many octahedral holes are there in a face-centered cubic unit cell?

A)6

B)13

C)12

D)4

E)8

Q3) An amorphous solid is one in which the atoms,ions,or molecules lie in a random jumble with no order.True or false?

A)True

B)False

Q4) How many atoms are there in a face-centered cubic unit cell?

Q5) Metals with a hexagonal close-packed structure have/do not have slip planes and as a result are malleable/brittle.

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Chapter 7: Inorganic Materials

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Q1) What element besides iron and carbon is necessary to produced stainless steel?

A)Chromium.

B)Vanadium.

C)Phosphorus.

D)Sulfur.

E)Zinc.

Q2) How do luminescent materials release light?

A)By returning from an excited state to a lower,but still excited state.

B)By the absorption of any wavelength radiation.

C)By the absorption of light photons.

D)By returning from an excited state to a lower energy state.

E)Through an applied electric voltage.

Q3) What properties are usually associated with high carbon steel?

A)Hardness and brittleness.

B)Ductility and low hardness.

C)Ductility and high hardness.

D)Low hardness and high brittleness.

E)Corrosion resistance and high malleability.

Q4) What contaminant causes the red "terra cotta" color in most ceramics?

Q5) 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) A piece of a newly synthesized material of mass 25.0 g at 80.0S1U1P1\(\circ\)S1S1P0C is placed in a calorimeter containing 100.0 g of water at 20.0S1U1P1\(\circ\)S1S1P0C.If the final temperature of the system is 24.0S1U1P1\(\circ\)S1S1P0C,what is the specific heat capacity of this material?

A)0.30 J.g^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

B)7.46 J.g^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

C)1.19 J.g^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

D)4.76 J.g^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

E)0.84 J.g^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

Q2) Calculate the change in internal energy when 2.50 kJ of energy is transferred as heat to 1.50 mol N₂ at 298 K and 1 atm at constant pressure.

A)+2.14 kJ

B)(-1.79 kJ)

C)+2.50 kJ

D)(-2.50 kJ)

E)+1.79 kJ

Q3) When a gas expands into a vacuum,w = 0.

A)True

B)False

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Chapter 9: Thermodynamics: The Second and Third Laws

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Q1) 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)

Q2) Predict the sign (+,-,0)of the entropy change when a glass of water reversibly loses 200 J of energy at 25°C.

Q3) A piece of equipment must be capable of containing water at temperatures well above its normal boiling point.If the piece of equipment withstands an internal pressure of no more than 10.0 atm,calculate the highest temperature at which the system can be safely operated.

Q4) Which of the following would probably have a positive \(\Delta\)S value?

A)He(g,2 atm)\(\rightarrow\) He(g,10 atm)

B)H₂(g)+ I₂(s)\(\rightarrow\) 2HI(g)

C)2Ag(s)+ Br₂(l)\(\rightarrow\) 2AgBr(s)

D)O₂(g)\(\rightarrow\) O₂(aq)

E)2NO₂(g)\(\rightarrow\)N₂O₄(g)

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Chapter 10: Physical Equilibria

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Q1) Water and acetone,CH₃COCH₃,both freeze at a higher temperature under pressure.

A)True

B)False

Q2) Which of the following has the highest vapor pressure?

A)H₂O

B)CH₃CH₂OH

C)CH₃CH₂OCH₂CH₃

D)CH₃OH

E)CH₃CH₂COOH

Q3) Which of the following 1.0 M solutions contains the most particles?

A)Ethylene glycol

B)Potassium chloride

C)Magnesium sulfate

D)Glucose

E)Sodium sulfate

Q4) Consider the phase diagram for sulfur in the text on page 316.Monoclinic sulfur is denser than rhombic sulfur.

A)True

B)False

Page 12

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Chapter 11: Chemical Equilibria

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Q1) Calculate \(\Delta\)G at 298 K for the reaction C₂H₅OH(l)\(\rightarrow\)C₂H₅OH(g, 0.0263 bar)

Given \(\Delta\)GS1U1P1\(\circ\)S1S1P0 = 6.2 kJ at 298 K.

A)6.2 kJ

B)15 kJ

C)2.8 kJ

D)-2.8 kJ

E)-15 kJ

Q2) Consider the reaction 2CuBr₂(s)\(\rightarrow\)2CuBr(s)+ Br₂(g)

If the equilibrium vapor pressure of Br₂(g)is 1.43 * 10^-5 Torr at 298 K,what is \(\Delta\)G at this temperature when Br₂(g)is produced at a pressure of 7.50 * 10^-8 Torr.

A)-5.65 kJ

B)13.0 kJ

C)5.65 kJ

D)-3.42 kJ

E)-13.0 kJ

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Chapter 12: Acids and Bases

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Q1) For a solution labeled "0.10 M H₂SO₃(aq)," pK_a1 = 1.81 and pK_a2 = 6.91,which of the following is true?

A)[H⁺] = 0.2 M.

B)The pH is 1.0.

C)The pH ~1.5.

D)The pH is 0.70.

E)The pH ~ 4.4.

Q2) The pH of 0.800 M aqueous benzenesulfonic acid is 0.51.What is the value of K_a for benzenesulfonic acid?

A)0.19

B)0.12

C)0.90

D)0.44

E)0.51

Q3) Which of the following 0.10 M aqueous solutions has the lowest pH?

A)B(OH)₃

B)HIO

C)C₂H₅NH₃Cl

D)C₆H₅OH

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Chapter 13: Aqueous Equilibria

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Q1) Choose the effective pH range of a HF/NaF buffer.For HF,K_a = 3.5 * 10^-4.

A)6.0-8.0

B)9.6-11.6

C)5.0-7.0

D)0.7-2.7

E)2.5-4.5

Q2) If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq)and 0.155 M NaHClO(aq),the final concentrations of HClO(aq)and ClO^-(aq),respectively,are

A)0.190 M and 0.155 M.

B)0.210 M and 0.155 M.

C)0.210 M and 0.165 M.

D)0.190 M and 0.165 M.

E)0.200 M and 0.155 M

Q3) The solubility of silver chloride is greater in 0.01 M NH₃(aq)because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

A)True

B)False

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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) What are the products of the electrolytic reduction of copper from aqueous CuSO₄?

A)H₂(g)and H₂SO₃(aq).

B)Cu(s)and O₂(g).

C)H₂SO₃(aq)and O₂(g).

D)Cu(s)and H₂SO₃(aq).

E)H₂(g)and O₂(g).

Q3) When KI(aq)is electrolyzed at a concentration of 1 M,the product at the anode is I₂.

A)True

B)False

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Chapter 15: Chemical Kinetics

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Q1) For the reaction S₂O₈^2-(aq)+ 3I^-(aq)\(\rightarrow\) 2SO₄2^-(aq)+ I₃^-(aq),rate = k[S₂O₈2^-][I^-].When the reaction is followed under pseudo-first-order conditions with [S₂O₈2^-] = 200 m M and [I^-] = 1.5 m M,the rate constant was 1.82 s^-1.The second order rate constant,k,for the reaction is

A)1.21 * 10³ M^-1.s^-1. B)6.07 * 10³ M^-1.s^-1.

C)9.10 M^-1.s^-1.

D)1.37 * 10^-2 M^-1.s^-1. E)1.82 M^-1.s^-1.

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) For the reaction cyclopropane(g)\(\rightarrow\) propene(g)at 500S1U1P1\(\circ\)S1S1P0C,a plot of ln[cyclopropane] vs t gives a straight line with a slope of -0.00067 s^-1.What is the order of this reaction and what is the rate constant?

Q4) 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) In ClF₃,the number of regions of high electron concentration around the chlorine atom are

A)3

B)4

C)5

D)6

E)2

Q2) How do the saline hydrides react in water?

A)They reduce water and produce O₂(g).

B)They all produce H₃O⁺(aq).

C)They oxidize water and produce O₂(g).

D)Saline hydrides are actually insoluble in water.

E)They reduce water and produce H₂(g).

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

A)In

B)Ga

C)Ge

D)Al

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

Q5) When phosphoric acid is heated it undergoes a ________________ reaction.

Page 18

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Chapter 17: The Elements: The D Block

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Q1) Why is \(\Delta\)_T is always greater than \(\Delta\)_O?

Q2) A ligand is A)a Lewis base.

B)necessary in a complex to balance the charge on the metal ion.

C)used to force octahedral geometry on a metal ion.

D)a Lewis acid.

E)used to precipitate metal ions from aqueous solution.

Q3) Zinc is used to galvanize iron.Explain why a galvanized container should not be used to store sodium hydroxide.

Q4) How many unpaired electrons are predicted for [Mn(CN)₆]^4-?

Q5) How many unpaired electrons are there in [CoBr₄]^2-?

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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 nuclear equation for the disintegration of U-238 produces Th-234.What other nuclide is produced?

A)⁴He

B)neutron

C)positron

D)³He

E)\(\beta\)

Q3) When a positron encounters an electron,both are annihilated and converted to energy.

A)True

B)False

Q4) What is the product of the emission of a \(\beta\) particle from K-40?

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Chapter 19: Organic Chemistry I

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Q1) A mixture of nitric acid and concentrated sulfuric acid is used to convert benzene to nitrobenzene.The nitrating agent in this reaction is

A)HNO₃

B)NO₂^-

C)NO₂⁺

D)NO₃^-

Q2) How many isomeric dichloromethylbenzenes exist?

A)4

B)5

C)6

D)7

Q3) Name the compound

CH₃CH(CH₃)CH(CH₂CH₃)C(CH₃)₃.

A)2,4,4-trimethyl-3-ethylpentane

B)2,2,4-trimethyl-3-ethylpentane

C)Decane

D)1,2-tetramethylpentane

E)2,2-dimethyl-3-ethyl-4-methylpentane

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

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Chapter 20: Organic Chemistry II

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Q1) Which atom of formaldehyde,H₂CO,is a Lewis acid site?

Q2) The formula of the polymer methyl methacrylate (Plexiglass)is -(CH₃OC(O)C(CH₃)CH₂)-.What is the monomer used to produce this polymer?

Q3) Which of the following produces a silver mirror with Tollens reagent?

A)CH₃COOH

B)CH₃C(O)OCH₃

C)CH₃COCH₃

D)CH₃OCH₃

E)CH₃CHO

Q4) The systematic name of CH₃CH₂CH(CHO)CH₃ is

A)2-ethylpropanal.

B)2-pentanal.

C)3-methylbutanal.

D)2-pentanone.

E)2-methylbutanal.

Q5) Kevlar is produced from HOOC-C₆H₄-COOH and H₂N-C₆H₄-NH₂.Write the formula for Kevlar.

Page 22

Q6) What is the product of the reaction C₅H₉CH₂CH₂Br + NaCN \(\rightarrow\)

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