Principles of Chemistry Question Bank - 1986 Verified Questions

Principles of Chemistry Question

Bank

Course Introduction

Principles of Chemistry introduces students to the fundamental concepts and theories that form the foundation of chemical science. Topics include atomic and molecular structure, stoichiometry, chemical bonding, states of matter, thermodynamics, chemical equilibrium, acids and bases, and kinetics. Through a combination of lectures, laboratory experiments, and problem-solving exercises, students develop essential skills in scientific reasoning, laboratory techniques, and the application of chemical principles to real-world problems in science and engineering. This course serves as a prerequisite for advanced study in chemistry, biology, and related fields.

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Chemical Principles 6th Edition by Professor Peter Atkins

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1986 Verified Questions

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Page 2

Chapter 1: The Quantum World

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Sample Questions

Q1) Calculate the velocity of an oxygen molecule,given that it has a de Broglie wavelength of 0.0140 nm.

A)890.m.s^-¹

B)3.00 * 10⁸ m.s^-¹

C)1780 m.s^-¹

D)445 m.s^-¹

E)8.90 m.s^-¹

Answer: A

Q2) What is the wavelength of a radio station transmitting at 99.1 MHz?

A)330 nm

B)303 nm

C)0.00303 m

D)3.03 m

E)0.330 m

Answer: D

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

A)True

B)False

Answer: False

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Page 3

Chapter 2: Quantum Mechanics in Action: Atoms

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Sample Questions

Q1) All the following are non-metals except A)C.

B)S.

C)Ga.

D)Se.

E)Cl.

Answer: C

Q2) How many nodal planes are present in an f-orbital?

A)2

B)3

C)7

D)4

E)5

Answer: B

Q3) In each pair,which ionization reaction is larger?

(a)I₃ of B; or I₃ of Be

(b)I₄ of C; or I₃ of B

Answer: (a)I₃ of Be

(b)I₄ of C

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Page 4

Chapter 3: Chemical Bonds

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Sample Questions

Q1) Use the bond enthalpies given to estimate the heat released when 2-methyl-1-propene,(CH₃)₂C=CH₂,reacts with HBr to give (CH₃)₂CBrCH₃.Bond enthalpies (kJ.mol^-¹): C-H,412; C-C,348; C=C,612; C-Br,276; H-Br,366.

A)58 kJ.mol^-¹

B)507 kJ.mol^-¹

C)317 kJ.mol^-¹

D)288 kJ.mol^-¹

E)181 kJ.mol^-¹

Answer: A

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

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Page 5

Chapter 4: Molecular Shape and Structure

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Sample Questions

Q1) Which of the following has bond angles slightly less than 109S1U1P1\(\circ\)S1S1P0?

A)NO₂^-

B)I₃^-

C)HOCl

D)O₃

E)CH₂^-

Q2) Which of the following is paramagnetic?

A)N₂

B)N₂²⁺

C)O₂²^-

D)N₂²^-

E)NO⁺

Q3) For HF,the LCAO-MO,\(\varPsi\) = c_H\(\varPsi\) _H + c_F\(\varPsi\) _F,has c_H = c_F.

A)True

B)False

Q4) Draw the Lewis structure of formamide,NH₂CHO,and give the number of lone pairs of electrons,and the number of \(\sigma\)- and \(\pi\)-bonds.

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Page 6

Chapter 5: The Properties of Gases

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Sample Questions

Q1) The empirical formula of a gas is CH₃O.If 2.77 g of the gas occupies 1.00 L at exactly 0S1U1P1\(\circ\)S1S1P0C at a pressure of 760 Torr,what is the molecular formula of the gas?

A)C₄H₁₂O₄

B)C₂H₆O₂

C)C₅H₁₅O₅

D)CH₃O

E)C₃H₉O₃

Q2) The height of water in a water barometer is 883 cm at 20S1U1P1\(\circ\)S1S1P0C.The density of water at 20S1U1P1\(\circ\)S1S1P0C is 0.998 g.cm^-³.What is the pressure?

A)88.3 kPa

B)8.81 * 10³ Pa

C)101 kPa

D)8.64 * 10³ Pa

E)86.4 kPa

Q3) If it takes 15 s for a certain sample of neon to effuse through a porous barrier,it will take ________________________________ (15 s,greater than 15 s,less than 15 s)for the same amount of nitrogen gas to effuse through the barrier under the same conditions.

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Chapter 6: Liquids and Solids

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Sample Questions

Q1) Which answer best accounts for the Na⁺ ions present in the NaCl unit cell?

A)1 center atom + 1/8 * 24 corner atoms

B)1 center atom + 1/2 * 6 face atoms

C)1 center atom + 1/8 * 8 corner atoms

D)1 center atom + 1/4 * 12 edge atoms

E)1/8 * 8 corner atoms + 1/2 * 6 face atoms

Q2) Which of the following can form intermolecular hydrogen bonds?

A)NH₂CH₂COOH

B)SiH₄

C)CH₃COCH₃

D)H₂CO

E)CH₃Cl

Q3) How many atoms are there in a primitive cubic unit cell?

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

Page 8

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Chapter 7: Inorganic Materials

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Sample Questions

Q1) Steel is often produced through what is called the basic oxygen process.

A)True

B)False

Q2) What is the diameter range of a nano-tube?

A)A few angstroms.

B)A few nanometers.

C)A few microns.

D)No more than 5 angstroms.

E)No more than 5 microns.

Q3) delocalized pi-bonds are the reason carbon nano-tubes conduct electricity.

A)True

B)False

Q4) Portland cement is made from what materials?

A)Oxides.

B)Sand and clay.

C)Crushed limestone

D)Only B and C,above.

E)A,B,and C,above.

Q5) A metal sample can be considered a sea of __________________ (protons,electrons,neutrons)in an array of cations.

Page 9

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Chapter 8: Thermodynamics: The First Law

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Sample Questions

Q1) A reaction known to release 2.00 kJ of heat takes place in a calorimeter containing 0.200 L of solution and the temperature rose by 4.46S1U1P1\(\circ\)S1S1P0C.When 100 mL of nitric acid and 100 mL of sodium hydroxide were mixed in the same calorimeter,the temperature rose 2.0S1U1P1\(\circ\)S1S1P0C.What is the heat output for the neutralization reaction?

A)0.0186 kJ^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

B)0.448 kJ^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

C)0.816 kJ^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

D)17.9 kJ^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

E)0.901 kJ^-1.(S1U1P1\(\circ\)S1S1P0C)^-1

Q2) What mass of ethanol,C₂H₅OH(l),must be burned to supply 500 kJ of heat? The standard enthalpy of combustion of ethanol at 298 K is -1368 kJ.mol^-1

A)126 g

B)2.74 g

C)16.8 g

D)10.9 g

E)29.7 g

Q3) Work is reported in joules; and 1 joule = ____________

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Page 10

Chapter 9: Thermodynamics: The Second and Third Laws

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Sample Questions

Q1) The experimental value of the molar entropy of 1 mol NO at 0 K is about 5 JK^-1.We can conclude that in the crystal the molecules of NO are arranged randomly.

A)True

B)False

Q2) Calculate the normal boiling point of chloroform,given that the standard entropy and enthalpy of vaporization of chloroform is +93.7 J.K^-1.mol^-1 and 31.4 J.K^-1.mol^-1

Q3) For the reaction 2NH₃(g) 3H₂(g)+ N₂(g),K_P = 1.47 *10^-6 at 298 K.Estimate the temperature at which K_P = 0.0100.

Q4) Calculate the standard entropy for the following reaction from standard molar entropies.

NH₄ClO₄(s)+ Al(s)\(\rightarrow\) NH₄Cl(s)+ Al₂O₃_(s)

Q5) All the halogens exist as diatomic molecules at room temperature and 1 bar.Under these conditions,which of the halogens,F to I,has the smallest molar entropy?

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Page 11

Chapter 10: Physical Equilibria

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Q1) A plot of ln(vapor pressure)versus 1/T for methanol gives a straight line with an intercept of 13.6.The enthalpy of vaporization of methanol is

A)113 kJ.mol^-1

B)13.6 kJ.mol^-1

C)611 kJ.mol^-1

D)1.64 kJ.mol^-1

E)Not enough information given to calculate.

Q2) The vapor pressure of benzene at 25S1U1P1\(\circ\)S1S1P0C is 94.6 Torr and its enthalpy of vaporization is 30.8 kJ.mol^-1.Estimate the normal boiling point of benzene.Assume the enthalpy of vaporization is independent of temperature.

A)640 K

B)358 K

C)470 K

D)624 K

E)Not enough information given.

Q3) The normal boiling point of ethanol is 78S1U1P1\(\circ\)S1S1P0C.If the vapor pressure of ethanol is 13.3 kPa at 34.9S1U1P1\(\circ\)S1S1P0C,calculate the enthalpy of vaporization of ethanol.

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12

Chapter 11: Chemical Equilibria

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Sample Questions

Q1) The equilibrium constant,K,for the reaction 2HgO(s) 2Hg(l)+ O₂(g) Is 1.2 * 10^-30.Calculate K for the reaction 1/2O₂(g)+ Hg(l) HgO(s).

A)-1.1 * 10^-15

B)8.3 * 10²⁹

C)4.2 * 10²⁹

D)9.1 * 10¹⁴

E)1.1 * 10^-15

Q2) Consider the reaction 3Fe(s)+ 4H₂O(g) 4H₂(g)+ Fe₃O₄(s)

If the volume of the container is reduced,

A)the equilibrium constant increases.

B)more H₂(g)is produced.

C)no change occurs.

D)more H₂O(g)is produced.

E)more Fe(s)is produced.

Q3) At the normal boiling point of chlorine,238.5 K, H of vaporization is 20.4 kJ.mol^-1.For the reversible vaporization of 1 mol of chlorine at 238.5 K and a constant pressure of 1 atm,determine q, S,and G.

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Page 13

Chapter 12: Acids and Bases

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Sample Questions

Q1) Which of the following produces the strongest conjugate base?

A)HF (pK_a = 3.45)

B)HClO (pK_a = 7.53)

C)HCOOH (pK_a = 3.75)

D)CH₃COOH (pK_a = 4.75)

E)HIO (pK_a = 10.64)

Q2) What is the pH of 0.025 M (CH₃)₃N(aq)(K_b = 6.5 * 10^-5)?

A)11.91

B)12.40

C)11.11

Q3) The pH of 0.010 M aniline(aq)is 8.32.What is the percentage aniline protonated?

A)2.1%

B)0.69%

C)0.021%

D)0.12%

E)0.21%

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

Page 14

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Chapter 13: Aqueous Equilibria

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Sample Questions

Q1) Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH₃(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

Q2) 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

Q3) Which of the following mixtures gives a buffer with a pH greater than 7.0? For HCNO,K_a = 2.2 * 10^-4 and for NH₃,K_b = 1.8 * 10F1F1F1S1^-5.

A)10 mL of 0.1 M NH₃(aq)+ 10 mL of 0.1 M HCl(aq)

B)10 mL of 0.1 M HCNO(aq)+ 10 mL 0f 0.1 M NaOH(aq)

C)10 mL of 0.1 M HCNO(aq)+ 5.0 mL of 0.1 M NaOH(aq)

D)10 mL of 0.1 M NH₃(aq)+ 10 ml of 0.1 M HCNO(aq)

E)10 mL of 0.1 M NH₃(aq)+ 5.0 mL of 0.1 M HCl(aq)

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

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Chapter 14: Electrochemistry

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Sample Questions

Q1) What reaction occurs at the cathode in the following cell diagram?

Cd(s)|CdSO₄(aq)|Hg₂SO₄|Hg(l)

Q2) 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⁺

Q3) The galvanic cell shown above uses the half-cells Mg²⁺/Mg and Zn²⁺/Zn,and a salt bridge containing KCl(aq).The voltmeter gives a positive voltage reading.Identify A and write the half-reaction that occurs in that compartment.Does the size of the electrode A increase or decrease during operation of the cell? What is the voltmeter reading?

Q4) What current is required to produce 91.6 g of chromium meta from chromium(VI)oxide in 12.4 hours?

Q5) 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 Cu²⁺(aq)?

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Chapter 15: Chemical Kinetics

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Sample Questions

Q1) Given:

CH₄(g)+ Cl₂(g)\(\rightarrow\) CH₃Cl(g)+ HCl(g)

The rate law for this elementary process is

A)rate = k[Cl₂].

B)k[CH₃Cl][HCl].

C)rate = k[CH₄][Cl₂].

D)rate = k[CH₄].

E)rate = k[CH₄]².

Q2) It is important to distinguish between the reaction rate and the rate constant.The units of reaction rate are Ms^-1.

A)True

B)False

Q3) A reaction has k = 8.39 M^-1.s^-1.How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

A)5.42 s

B)2.00 s

C)1.42 s

D)8.39 s

E)4.00 s

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Page 17

Chapter 16: The Elements: the Main Group Elements

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Sample Questions

Q1) Which of the following pairs of elements both have acidic oxides?

A)Ca and As

B)Mg and Al

C)B and Li

D)In and Sn

E)P and Se

Q2) All of the following contain silicates in various forms except A)asbestos. B)mica.

C)talc.

D)molecular sieves. E)alum.

Q3) Order the following ions according to their radii from largest to smallest: H^-,Cl^-,^-.

Q4) Sulfur does not react directly with A)chlorine. B)chlorine and bromine.

C)fluorine. D)fluorine and chlorine. E)iodine.

Page 18

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Chapter 17: The Elements: The D Block

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Q1) What do all rhodium complexes have in common?

Q2) What is the formula of the compound formed when potassium dichromate is dissolved in aqueous base?

A)K₂CrO₄

B)K₂Cr₂O₇

C)CrO₃

D)Cr(OH)₃

Q3) What is the name of the complex Na[Co(NH₃)₃Cl₃]?

A)Sodium triamminetrichlorocobaltate(II)

B)Sodium triamminetrichlorocobalt(III)

C)Sodium tris(aminechloro)cobaltate(II)

D)Sodium triamminetrichlorocobalt(II)

E)Sodium trichlorotriamminecobalt(III)

Q4) 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.

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Chapter 18: Nuclear Chemistry

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Sample Questions

Q1) How many nucleons does boron-11 contain?

A)6

B)10

C)5

D)11

E)16

Q2) Nuclides that lie below the band of stability decay by positron emission,electron capture,or proton emission.

A)True

B)False

Q3) What nuclide undergoes \(\alpha\) decay to produce the daughter nuclide polonium-218 (Z = 84)?

A)radon-222

B)radium-226

C)polonium-222

D)polonium-214

E)radon-226

Q4) The rate of nuclear decay does not depend on temperature. A)True

B)False

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Chapter 19: Organic Chemistry I

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Q1) How many of the structural isomers of C₆H₁₄ have only primary and tertiary hydrogens?

A)1

B)2

C)3

D)4

E)5

Q2) What type of reaction is the reaction of ethene with bromine water resulting in the formation of 1,2-bromoethane?

A)Redox reaction.

B)Nucleophilic reaction.

C)Substitution reaction.

D)Oxidation reaction.

Q3) Treating benzoic acid with both nitric acid and concentrated sulfuric acid results in what product?

A)ortho-nitrobenzoic acid

B)meta-nitrobenzoic acid

C)para-nitrobenzoic acid

D)meta- and para-nitrobenzoic acids

Q4) Name the compound (CH₃)₂CHCCCH₃.

Page 21

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Chapter 20: Organic Chemistry II

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Q1) Ethers are less volatile than alcohols of the same molar mass.

A)True

B)False

Q2) Both C₆H₅OH and C₆H₅CH₂OH are weak acids with K_a values about 10^-10

A)True

B)False

Q3) Acetic acetyl chloride reacts with methylamine to produce

Q4) 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.

Q5) What is the product of the reaction

C₅H₉CH₂CH₂Br + NaCN \(\rightarrow\)

Q6) Where is the electrophilic site in the compound 2-bromo-2-methylbutane?

Q7) In the reaction of CH₃CH₂COOH with CH₃NH₂,what molecule is eliminated? Page 22

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Page 23