General Chemistry I Mock Exam - 1986 Verified Questions

General Chemistry I Mock Exam

Course Introduction

General Chemistry I provides an introduction to the fundamental concepts of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, and thermochemistry. Students will explore the properties and behavior of elements and compounds, learn to interpret the periodic table, and develop problem-solving skills through quantitative and qualitative analysis. The course lays the groundwork for understanding chemical reactions and the scientific principles that govern the composition and changes of matter, preparing students for further study in chemistry and related scientific disciplines.

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 metals has the lowest work function?

A)Be

B)Sr

C)Li

D)Rb

Answer: D

Q2) What is the frequency of a photon that has an energy of 5.4 * 10^-18 J?

A)1.6 * 10^-34Hz

B) (1 .2 * 10¹⁶Hz)

C)1.2 * 10^-¹⁶Hz

D)(8.1 * 10¹⁵Hz)

E)8.1 *10¹⁵Hz

Answer: E

Q3) All the orbitals of a given shell of He⁺ are degenerate regardless of the value of the orbital angular momentum.

A)True

B)False

Answer: True

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Page 3

Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) Which set of quantum numbers,n,l,m_l,could correspond to one of the highest energy electrons in Zr?

A)4,2,-2

B)4,2,+3

C)3,2,-2

D)4,3,-2

Answer: A

Q2) Which of the following atoms has the highest electron affinity?

A)Ar

B)P

C)Al

D)Si

Answer: D

Q3) Write the ground-state electron configuration of a europium atom.

A)[Xe]5d⁷6s²

B)[Xe]4f²5d⁵6s²

C)[Xe]4f⁹

D)[Xe]4f⁷6s²

E)[Xe]4f⁵5d²6s²

Answer: D

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Chapter 3: Chemical Bonds

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Q1) For dinitrogen monoxide,the arrangement of the atoms is N-N-O.In the Lewis structure with a single bond between NN and a triple bond between NO,the formal charges on N,N,and O,respectively,are

A)(-1,+1,0.)

B)0,0,0.

C)0,+1,-1.

D)0,-1,+1.

E)(-2,+1,+1.)

Answer: E

Q2) The Madelung constant is different for all crystals.

A)True

B)False

Answer: True

Q3) Predict the N-O bond lengths in NO₂^-,given the N-O and N=O bond lengths of 140 and 120 pm,respectively.

Answer: Both ~ 130 pm

Q4) Draw the Lewis structure of xenon difluoride and give the number of lone pairs electrons around the central atom.

Answer: Three

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Chapter 4: Molecular Shape and Structure

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Q1) Draw the Lewis structure of formamide,NH₂CHO,and give the number of lone pairs of electrons,and the number of \(\sigma\)- and \(\pi\)-bonds.

Q2) The molecules OF₂ and O₃ both have bent shapes.What is the hybridization of the central atom in OF₂ and O₃,respectively?

A)sp³ and sp²

B)both sp³

C)both sp²

D)sp³ and sp

E)both sp

Q3) What is the shape of ClF₃?

A)Tetrahedral

B)Seesaw

C)Trigonal bipyramidal

D)T-shaped

E)Square planar

Q4) Name all the angles in a trigonal planar geometry.

Q5) Predict the HNH bond angle in NH₂^-

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

Q7) Predict the electron arrangement in ClF₃.

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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 STP?

A)44.8

B)6.00

C)22.4

D)134

E)67.2

Q2) What is the pressure inside a system when the system-side column in an open mercury manometer is 75.0 mm lower than the atmosphere side when the atmospheric pressure is 735 mmHg?

A)820 kPa

B)10.0 kPa

C)88.0 kPa

D)75 kPa

E)108 kPa

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Chapter 6: Liquids and Solids

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Q1) In the rock-salt structure (NaCl),the cations occupy all the octahedral holes.True or false?

A)True

B)False

Q2) How many atoms are there in a primitive cubic unit cell?

A)1

B)2

C)3

D)8

E)4

Q3) Which of the following has the highest boiling point?

A)CH₃CH₂CH₂CH₂CH₂Br

B)CH₃CH₂CH₂CH₂CH₂I

C)CH₃CH₂CH₂CH₂CH₃

D)CH₃CH₂CH₂CH₂CH₂F

E)CH₃CH₂CH₂CH₂CH₂Cl

Q4) Isotropic liquids have viscosities that are the same in every direction.True or false?

A)True

B)False

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Chapter 7: Inorganic Materials

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Q1) Resistance in a material is defined as:

A)R = \(\kappa\).A² / l

B)R = \(\kappa\).A / l

C)R = \(\kappa\).l / A

D)R = \(\kappa\).A / l²

E)R = \(\kappa\)².A / l

Q2) What is the minimum pressure and temperature for diamond formation?

A)8kbar,150S1U1P1\(\circ\)S1S1P0C

B)800kbar,15,000S1U1P1\(\circ\)S1S1P0C

C)80 kbar,15,000S1U1P1\(\circ\)S1S1P0C

D)800kbar,1,500S1U1P1\(\circ\)S1S1P0C

E)80kbar,1,500S1U1P1\(\circ\)S1S1P0C

Q3) What is the formula of buckminsterfullerene?

A)C_1-10

B)C₆

C)C₁₀

D)C₆₀

E)Millions of carbon atoms.

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

Q5) To what two chemicals are most glasses not resistant?

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Chapter 8: Thermodynamics: The First Law

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Q1) Given the standard reaction enthalpies below:

N₂(g)+ O₂ \(\rightarrow\) 2NO(g)

\(\Delta\)H° = +180.5 kJ.mol^-1

2NO₂(g)\(\rightarrow\) N₂(g)+ 2O₂(g)

\(\Delta\)H° = -66.4 kJ.mol^-1

Calculate the standard reaction enthalpy for the oxidation of nitric oxide to nitrogen dioxide,shown below:

2NO(g)+ O₂(g)\(\rightarrow\) 2NO₂(g)

A)(+114.1 kJ.mol^-1)

B)(+246.9 kJ.mol^-1)

C)(-114.1 kJ.mol^-1)

D)(-294.6 kJ.mol^-1)

E)(-246.9 kJ.mol^-1)

Q2) For any isothermal process,\(\Delta\)U > 0 for an ideal gas.

A)True

B)False

Q3) What equation corresponds to the standard enthalpy of formation of gaseous hydrogen atoms,which,at 298 K is +217 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) Calculate \(\Delta\)S_surr° at 298 K for the reaction H₂(g)+ F₂(g)\(\rightarrow\) 2HF(g)

\(\Delta\)H_r° = -546 kJ.mol^-1,\(\Delta\)S_r° = +14.1 J.K^-1.mol^-1

A)+14.1 J.K^-1.mol^-1

B)+1820 J.K^-1.mol^-1

C)+1830 J.K^-1.mol^-1

D)(-1830 J.K^-1.mol^-1)

E)(-14.1 J.K^-1.mol^-1)

Q2) All entropies of fusion are positive.

A)True

B)False

Q3) The standard reaction free energy for the oxidation of glucose is -2879 kJ·mol^-1.What is the maximum nonexpansion work obtainable from 125 g glucose,C₆H₁₂O₆(s)?

Q4) 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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Chapter 10: Physical Equilibria

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Q1) 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

Q2) Which of the following liquids freeze at a lower temperature when pressure is applied?

A)Water

B)Acetic acid

C)Benzene

D)Methanol

E)Carbon tetrachloride

Q3) the van't Hoff i of HF differs from that of HCl?

A)True

B)False

Q4) What is the vapor pressure of carbon disulfide at its normal boiling point?

Page 12

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Chapter 11: Chemical Equilibria

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Q1) At 25S1U1P1\(\circ\)S1S1P0C,K = 6.9 * 10⁵ for the reaction

N₂(g)+ 3H₂(g) 2NH₃(g)

Calculate K_c at 25S1U1P1\(\circ\)S1S1P0C for this reaction.

A)2.8 * 10⁴

B)6.8 * 10⁵

C)1.1 * 10³

D)1.7 * 10⁷

E)4.1 * 10⁸

Q2) Consider the reaction

CuSO₄(s)\(\rightarrow\) CuO(s)+ SO₃(g)

If \(\Delta\)GS1U1P1\(\circ\)S1S1P0 = -14.6 kJ at 950S1U1P1\(\circ\)S1S1P0C for this reaction,what is \(\Delta\)G for an SO₃(g)pressure of 20 bar at this temperature.

A)15.9 kJ

B)45.1 kJ

C)-14.6 kJ

D)30.5 kJ

E)-45.1 kJ

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13

Chapter 12: Acids and Bases

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Q1) the pH of 0.10 M and 0.40 M NaHCO₃(aq)solutions is 8.31 for both?

A)True

B)False

Q2) If the value of K_b for pyridine is 1.8 * 10^-9,calculate the equilibrium constant for C₅H₅NH⁺(aq)+ H₂O(l) C₅H₅N(aq)+ H₃O⁺(aq)

A)-1.8 * 10^-9

B)1.8 *10^-16

C)5.6 * 10⁸

D)1.8 * 10^-9

E)5.6 * 10^-6

Q3) Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

A)True

B)False

Q4) Write the autoprotolysis reaction for liquid ammonia.

Q5) Is a 0.1 M aqueous solution of HPO₄^2-acidic,basic,or neutral? Prove your answer using the appropriate equilibrium constants.

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Chapter 13: Aqueous Equilibria

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Q1) At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq)with 0.260 M HCl(aq),

A)the pH is less than 7.

B)[CH₃NH₃⁺] = 0.260 M.

C)the pH is 7.0.

D)[CH₃NH₂] = 0.130 M.

E)the pH is greater than 7.

Q2) What is the pH of an aqueous solution that is 1.0 M HClO (K_a = 3.0 *10^-8)and 0.75 M NaClO?

A)7.64

B)7.40

C)6.36

D)7.52

E)6.60

Q3) In the titration of 0.300 M H₃PO₄(aq)with 0.300 M NaOH(aq),the first stoichiometric point occurs at pH < 7 whereas in the titration of 0.300 M HCOOH(aq)with 0.300 M NaOH(aq)the stoichiometric point occurs at pH > 7.Explain.

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) In the cell shown above,A is a standard Ag⁺/Ag electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is +0.80 V,which electrode is negative?

Q2) 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^-

Q3) The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Ag(s)|AgCl(s)|Cl^-(aq)m Cu²⁺(aq)|Cu(s)

Is +0.12 V.What is the standard potential of the AgCl/Ag,Cl^- electrode?

A)-0.46 V

B)-0.22 V

C)+0.24 V

D)+0.46 V

E)+0.22 V

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Chapter 15: Chemical Kinetics

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Q1) 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

Q2) Technetium-99m,used to image the heart and brain,has a half-life of 6.00 h.What fraction of technetium-99m remains in the body after 1 day?

A)0.0625

B)0.250

C)0.0313

D)0.125

Q3) 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

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) What is the shape of BrF₅?

A)Seesaw

B)Square planar

C)Square pyramidal

D)Octahedral

E)Trigonal bipyramidal

Q2) The formula of diborane is

A)BH₃.

B)B₂H₆.

C)B₂H₄.

D)B₂H₂.

E)B₂H.

Q3) Which of the following concentrated acids can be safely transported in passivated lead containers?

A)HClO₄

B)H₂SO₄

C)HI

D)HCl

E)HNO₃

Q4) Which of the alkaline earth metals does not form a saline hydride?

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Chapter 17: The Elements: The D Block

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Q1) Complexes with coordination number 4 are either tetrahedral or octahedral.

A)True

B)False

Q2) What is the oxidation number of iron in K₃[Fe(CN)₆]?

A)+3

B)+2

C)+9

D)+6

Q3) Comparing [Co(CN)₆]^3- with [CoCl₆]^4-,which of the following statements is true?

A)[Co(CN)₆]^3-has more d-electrons than [CoCl₆]^4-.

B)[Co(CN)₆]^3- is paramagnetic while [CoCl₆]^4- is diamagnetic.

C)Both complexes are paramagnetic.

D)[Co(CN)₆]^3- is diamagnetic while [CoCl₆]^4- is paramagnetic.

E)[Co(CN)₆]^3- has the same number of d-electrons as [CoCl₆]^4-.

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Chapter 18: Nuclear Chemistry

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Q1) The binding energy of a nucleus is

A)the energy evolved when a nucleus breaks up into fundamental particles.

B)the energy released when protons and neutrons come together to form a nucleus.

C)related to the number of electrons in a nucleus.

D)the energy required to eject one neutron from the nucleus.

E)related to the mass lost in a chemical reaction.

Q2) The nuclear binding energy for lithium-7 is the energy released in the nuclear reaction

A)3¹H + 7n \(\rightarrow\) ⁷Li.

B)⁶Li + n \(\rightarrow\) ⁷Li.

C)3¹H + 4\(\beta\) \(\rightarrow\) ⁷Li.

D)3¹H + 4n \(\rightarrow\) ⁷Li.

E)7¹H \(\rightarrow\) ⁷Li.

Q3) All the following are predicted to be unstable except

A)Ca-40

B)N-16

C)Na-24

D)O-15

Q4) One becquerel is equal to _________________________ and one curie is equal to _________________________.

Page 20

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Chapter 19: Organic Chemistry I

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Q1) How many different monochlorination products are formed when n-butane reacts with chlorine gas under the influence of UV light?

A)5

B)1

C)3

D)2

E)4

Q2) The product of the reaction of 2-butene with Cl₂ is

A)3,3-dichlorobutane.

B)2,3-dichlorobutane.

C)butane.

D)2-chlorobutane.

E)2,2-dichlorobutane.

Q3) Which of the following forms ortho- and meta-products upon nitration?

A)Phenol

B)Benzoic acid

C)Nitrobenzene

D)Cyanobenzene (benzonitrile)

Q4) Name the compound CH₃CH=CHCH=CH₂.

Q5) When 2-methyl-1-butene reacts with HBr,what are the two products formed?

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Chapter 20: Organic Chemistry II

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Q1) The \(\alpha\) helix results from the pairing of specific bases by hydrogen bonding.Which pairs form hydrogen bonds?

A)AT and GC

B)AC and GC

C)GT

D)AT,GC,AC,and GT

E)AC

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) What is the product of the reaction C₆H₅COCl + CH₃NH₂ \(\rightarrow\)

Q4) Acetic acetyl chloride reacts with methylamine to produce

Q5) Amines react with both carboxylic acids and acid chlorides to produce amides. A)True

B)False

Q6) 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 2.5?

Q7) When amines condense with carboxylic acids,what molecule is eliminated?

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