Chemical Fundamentals Exam Preparation Guide - 1986 Verified Questions

Course Introduction

Chemical Fundamentals

Exam Preparation Guide

Chemical Fundamentals provides a foundational understanding of the basic principles of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, and the properties of gases, liquids, and solids. The course emphasizes the role of chemical reactions and equations, introduces the periodic table, and explores concepts such as solution chemistry and thermodynamics. Through both theoretical learning and practical laboratory exercises, students develop critical analytical and problem-solving skills essential for further studies in chemistry and related scientific disciplines.

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 energy in joules does a photon with a frequency of 5.0 * 10¹⁴ /sec have?

A)1.3 * 10^-19

B)3.3 * 10^-19

C)6.6 * 10^-¹⁹

D)6.6 * 10¹⁹

E)3.3 * 10¹⁹

Answer: B

Q2) The zero-point energy in 1,3-butadiene is larger than in 1,3,5,7-octatetraene.

A)True

B)False

Answer: True

Q3) In a one-dimensional particle in a box,for n = 6,how many wavelengths equal the size of the box?

Answer: B

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) Which of the following species is isoelectronic with Ra²⁺?

A)I^-

B)Kr

C)Xe

D)Rn

E)Fr

Answer: D

Q2) Write the ground-state electron configuration of In⁺.

A)[Kr]4d⁷5s²5p³

B)[Kr]4d⁸5s¹5p³

C)[Kr]4d⁵5s¹5p⁶

D)[Kr]4d¹⁰5s²

E)[Kr]4d¹⁰5s¹5p¹

Answer: D

Q3) Nodal planes in orbitals can be accounted for by the wavelike behavior of electrons.

A)True

B)False

Answer: True

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Chapter 3: Chemical Bonds

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Q1) How many electrons are in the expanded valence in XeOF₂?

A)14

B)12

C)8

D)10

E)6

Answer: B

Q2) How many valence electrons are present in W⁴⁺?

Answer: 2

Q3) 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

Q4) List the chalcogens in order of increasing electronegativity.

Answer: tellurium < selenium < sulfur < oxygen.

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Chapter 4: Molecular Shape and Structure

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Q1) Which of the following molecules is (are)polar?

(a)AsCl₄⁺

(b)I₃⁺

(c)I₃^-

(d)N₃^-

(e)S₃²^-

A)(b)and (e)

B)(b)and (c)

C)(c)and (e)

D)only (e)

Q2) Which of the following is polar?

A)CO₃²^-

B)O₃

C)XeF₂

D)I₃^-

E)NON

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

Q4) The electron arrangement and shape in IF₄⁺,respectively,are

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Chapter 5: The Properties of Gases

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Q1) What volume is occupied by 50.0 g of chlorine gas at 10.00°C at a pressure of 755 Torr?

A)1.53 L

B)8.2 L

C)16.4 L

D)0.64 L

E)181 L

Q2) Consider both nitrogen and chlorine as ideal gases.

(a)What is the molar kinetic energy of nitrogen gas at 25S1U1P1\(\circ\)S1S1P0C?

(b)At 25S1U1P1\(\circ\)S1S1P0C,the molar kinetic energy of chlorine gas is ___________________________(equal to,greater than,less than)the molar kinetic energy of nitrogen.

Q3) A sample of gas with a volume of 750 mL exerts a pressure of 98.0 kPa at 30S1U1P1\(\circ\)S1S1P0C.What pressure will the sample exert when it is compressed to 250 mL and cooled to -25S1U1P1\(\circ\)S1S1P0C?

A)353 kPa

B)241 kPa

C)359 kPa

D)39.9 kPa

E)26.7 kPa

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Chapter 6: Liquids and Solids

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Q1) 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

Q2) All the following are units of surface tension except

A)mJ.m^-2.

B)N.m.

C)J.m^-2

D)mN.m^-1.

E)kg.s^-2.

Q3) Which of the following is the strongest intermolecular force between molecules?

A)Dipole-dipole (stationary)

B)Hydrogen bonding

C)Dipole-dipole (rotating)

D)London

E)Ion-dipole

Q4) Which has the higher boiling point,HCl or HI?

Page 8

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Chapter 7: Inorganic Materials

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Q1) Why is gravel often used as a filler in concrete?

A)Because it is hard.

B)Because it is inexpensive.

C)It is easily deformable.

D)Because it is a granite.

E)Gravel is not a filler in concrete.

Q2) Paramagnetism is a weaker phenomenon than ferromagnetism.

A)True

B)False

Q3) Which mineral is a common form of crystalline calcium carbonate?.

A)Carbonite.

B)Calcite.

C)Aragonite.

D)B and C,above.

E)A and C,above.

Q4) To what two chemicals are most glasses not resistant?

Q5) Atom arrangements that move relative to one another along set two-dimensional surfaces are called what?

Q6) What contaminant causes the red "terra cotta" color in most ceramics?

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Chapter 8: Thermodynamics: The First Law

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Q1) For most reactions,the value of \(\Delta\)U is very close to that for \(\Delta\)H.

A)True

B)False

Q2) Give \(\Delta\)H_r values for each of the following reactions from the information below.

\(\Delta\)H_fS1U1P1\(\circ\)S1S1P0(HCl(g))= -92.31 kJ.mol^-1

H-Cl bond enthalpy = +431 kJ.mol^-1

O-H bond enthalpy = +463 kJ.mol^-1

\(\Delta\)H_fS1U1P1\(\circ\)S1S1P0(H₂O(g))= -241.8 kJ.mol^-1

(a)2H(g)+ O(g)\(\rightarrow\)H₂O(g)

(b)H₂(g)+ Cl₂(g)\(\rightarrow\) 2HCl(g)

(c)H(g)+ Cl(g)\(\rightarrow\) HCl(g)

Q3) The temperature of a sample increases at its boiling point until all the liquid has been vaporized.

A)True

B)False

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Chapter 9: Thermodynamics: The Second and Third Laws

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Q1) The molar entropy of silver at 298 K is equal to the area under the curve obtained by plotting (from T = 0 to T = 298 K)

A)C_P versus T.

B)lnC_P versus T.

C)ln(C_P/T)versus T.

D)C_P/T versus T.

E)C_P versus 1/T.

Q2) The reaction

CaO(s)+ H₂O(l) Ca(OH)₂(s)

Is spontaneous at 0^oC.Pedict the sign of the reaction enthalpy and entropy,respectively.

A)(+and-)

B)(-and -)

C)+ and +

D)(- and +)

E)(- and 0)

Q3) The change in molar entropy for vaporization of all liquids is about the same.

A)True

B)False

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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) Why is the vapor pressure of cis-dibromoethene lower than the vapor pressure of trans-dibromoethene?

A)Ion-dipole forces

B)London forces

C)Hydrogen bonding

D)Ion-ion forces

E)Dipole-dipole forces

Q3) Consider the phase diagram for sulfur in the text on page 316.Monoclinic sulfur is denser than rhombic sulfur.

A)True

B)False

Q4) 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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Q1) Given: C(s)+ CO₂(g) 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO₂(g)are 1.22 atm and 0.780 atm,respectively.Calculate the value of K for this reaction.

A)3.13

B)2.00

C)1.91

D)1.56

E)0.640

Q2) For the reaction NH₃(g)+ H₂S(g) NH₄HS(s)

K_c = 9.7 at 900 K.If the initial concentrations of NH₃(g)and H₂S(g)are 2.0 M,what is the equilibrium concentration of H₂S(g)?

A)1.9 M

B)0.20 M

C)1.7 M

D)0.10 M

E)0.32 M

Q3) Consider the reaction

Na⁺(g)+ Cl^-(g) NaCl(s) If the temperature is lowered,the products/reactants are favored.

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Chapter 12: Acids and Bases

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Q1) In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH₄⁺.

A)True

B)False

Q2) All of the following are Lewis bases except

A)OH^-

B)H₂O

C)SO₃

D)Br^-

Q3) Which of the following is the strongest acid?

A)CH₃CH₂OH

B)CH₃COOH

C)CHCl₂COOH

D)CH₂ClCOOH

E)CCl₃COOH

Q4) Strong acids are leveled in water to the strength of the acid H₃O⁺.

A)True

B)False

Q5) What is the conjugate acid of O^2-?

Page 14

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Chapter 13: Aqueous Equilibria

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Q1) What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq)with 0.26 M HClO₄(aq)? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

A)5.72

B)7.00

C)5.57

D)2.16

E)2.01

Q2) At the stoichiometric point in the titration of 0.130 M HCOOH(aq)with 0.130 M KOH(aq),

A)the pH is 7.0.

B)[HCOOH] = 0.0650 M.

C)[HCO₂-] = 0.130 M.

D)the pH is greater than 7.

E)the pH is less than 7.

Q3) In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

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) The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Pb(s)|Pb²⁺(aq)m Cu²⁺(aq)|Cu(s)

Is +0.47 V.What is the standard potential of the Pb²⁺/Pb electrode?

A)-0.26 V

B)+0.81 V

C)-0.81V

D)-0.13 V

E)+0.13 V

Q2) In a working electrochemical cell (+ cell voltage),the electrons flow from the anode through the external circuit to the cathode.

A)True

B)False

Q3) 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^-

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Chapter 15: Chemical Kinetics

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Q1) The activation energy of a reaction is given by

A)+(slope of a plot of lnk vs 1/T)\(\div\) R.

B)-(slope of a plot of lnk vs 1/T)\(\div\) R.

C)-R \(\div\) (slope of a plot of lnk vs 1/T).

D)+(slope of a plot of lnk vs 1/T)* R.

E)-(slope of a plot of lnk vs 1/T)* R.

Q2) For a given first-order reaction,after 2.00 min,20% of the reactants remain.Calculate the rate constant for the reaction.

A)0.0134 s^-1

B)0.000808 s^-1

C)74.6 s^-1

D)0.00582 s^-1

E)0.00186 s^-1

Q3) For a given first-order reaction,after 230 s,33% of the reactants remain.Calculate the rate constant for the reaction.

A)207 s^-1

B)0.00174 s^-1

C)0.00209 s^-1

D)0.000756 s^-1

E)0.00482 s^-1

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Chapter 16: The Elements: the Main Group Elements

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Q1) Which one of the following statements is false?

A)Fluorine can be produced by oxidation of a fluoride ion with chlorine.

B)Bromine can be produced by oxidation of a bromide ion with chlorine.

C)Fluorine is produced by electrolysis of an anhydrous mixture of KF and HF.

D)The most stable form of fluorine at 25S1U1P1\(\circ\)S1S1P0C and 1 atm is F₂(g).

Q2) Which of the following is paramagnetic?

A)N₂

B)N₂O

C)O₂^2-

D)O₃

E)NO

Q3) Magnesium nitride dissolves in water to produce

A)HNO₃(aq)and MgO(s).

B)N₂(g)and MgO(s).

C)NH₃(g)and Mg(OH)₂(s).

D)Mg(NO₃)₂(aq).

E)N₂H₄(l)and Mg(OH)₂(s).

Q4) Both ammonia and phosphine are soluble in water.Which is less soluble? Why?

Q5) 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) In the complex [Fe(CN)₆]^4-,

A)iron is a Lewis acid and cyanide is a Lewis base.

B)Cyanide is a Lewis acid.

C)iron has an oxidation number of +3.

D)Cyanide has an oxidation number of -2.

Q2) Both Cu²⁺(aq)and Zn²⁺(aq)are colorless.

A)True

B)False

Q3) The maximum oxidation states for chromium and manganese are

A)both +7.

B)+7 and +8,respectively.

C)+3 and +4,respectively.

D)+5 and +6,respectively.

E)+6 and +7,respectively.

Q4) Which of the following is diamagnetic?

A)[Fe(OH₂)₆]²⁺

B)[Fe(CN)₆]^3-

C)[Co(OH₂)₆]²⁺

D)[Co(NH₃)₆]³⁺

E)[Cr(NH₃)₆]³⁺

Page 19

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Chapter 18: Nuclear Chemistry

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Q1) What is the element produced when ⁴⁴Ti undergoes electron capture?

A)Ar

B)K

C)Sc

D)V

E)Ca

Q2) Complete the nuclear reaction ⁹⁷Mo + ²H \(\rightarrow\) _____ + 2n

Q3) What is the element produced when ⁸³Sr undergoes positron emission?

A)Kr

B)Br

C)Rb

D)Zr

E)Y

Q4) If a nuclide lies above the band of stability,it should decay by

A)Such nuclides do not decay.

B)\(\beta\)-particle emission.

C)positron emission.

D)neutron emission.

E)\(\alpha\)-particle emission.

Page 20

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Chapter 19: Organic Chemistry I

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Q1) Arenes undergo predominantly addition reactions.

A)True

B)False

Q2) The product of the reaction of 2-butene with HBr is

A)1-bromobutane.

B)2-bromo-2-butene.

C)butane.

D)2-bromo-1-butene.

E)2-bromobutane.

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) Why do alkanes not react with boiling nitric acid?

Q5) Alkanes react with boiling sulfuric acid because the C-C and C-H bonds are easily attacked.

A)True

B)False

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Chapter 20: Organic Chemistry II

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Q1) The systematic name of CH₃CH₂CH(CHO)CH₃ is

A)2-ethylpropanal.

B)2-pentanal.

C)3-methylbutanal.

D)2-pentanone.

E)2-methylbutanal.

Q2) The typical amino acid,NH₂CHRCOOH,has pK_a1 and pK_a2 of 2.4 and 9.8,respectively.What is(are)the major species in an aqueous solution whose pH is 10?

Q3) Amines react with both carboxylic acids and acid chlorides to produce amides. A)True B)False

Q4) Which atom of formaldehyde,H₂CO,is susceptible to attack by a nucleophilic reagent?

Q5) The formula of the polymer methyl methacrylate (Plexiglass)is -(CH₃OC(O)C(CH₃)CH₂)-.What is the monomer used to produce this polymer?

Q6) What is the product of the reaction CH₃CH(NH₂)CH₃ + CH₃CH₂C(O)OCH₃ \(\rightarrow\)

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