General Chemistry I Exam Questions - 2075 Verified Questions

Course Introduction

General Chemistry I Exam Questions

General Chemistry I introduces students to the fundamental principles of chemistry, focusing on the structure and behavior of matter. Topics include atomic and molecular structure, chemical bonding, stoichiometry, chemical reactions, thermochemistry, and the properties of gases, liquids, and solids. The course emphasizes problem-solving and laboratory skills, providing a foundation for understanding chemical processes in both everyday life and advanced scientific contexts. Students engage in both theoretical concepts and practical experiments to deepen their comprehension of core chemical principles.

Recommended Textbook Chemistry and Chemical Reactivity 9th Edition by John C. Kotz\New folder

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Page 2

Chapter 1: Basic Concepts of Chemistry

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Q1) One of the following is \(\underline{\text{ not }}\) a description of \(\underline{\text{ gases. }}\)Which one is it?

A) easily compressed

B) particles in definite positions

C) relatively low densities

D) fills any container completely

E) expands infinitely on heating

Answer: B

Q2) Which of the following are likely to form a homogeneous mixture?

1) milk and ice cream blended together with chocolate syrup

2) an egg combined with milk and mixed with a whisk

3)1 gram table salt combined with 250 mL of water

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Answer: C

Q3) The ________ of a substance is defined as its mass per unit volume.

Answer: density

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Chapter 2: Mathlets Review: The Tools of Quantitative Chemistry

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Q1) A cylinder has a radius of 2.38 mm and a height of 175 mm.Calculate the volume of the cylinder in liters.(Volume = \(\pi\)r²h)

A) 3.11 \(\times\) 10^-3 L

B) 3.11 \(\times\) 10^-2 L

C) 0.311 L

D) 3.11 L

E) 3.11 \(\times\) 10³ L

Answer: A

Q2) A piece of metal (mass = 17.676 g)is placed in 11.00 mL of chloroform (d = 1.498 g/mL)in a 25-mL graduated cylinder.The chloroform level increases to 15.46 mL.The best value for density of this metal from these data is

A) 1.14 g/mL.

B) 2.65 g/mL.

C) 3.963 g/mL.

D) 5.94 g/mL.

E) 3.96 g/mL.

Answer: E

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Page 4

Chapter 3: Atoms, molecules, and Ions

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Q1) A neutral atom of the isotope ¹⁹⁷Au contains

A) 197 neutrons and 276 electrons.

B) 79 protons and 197 neutrons.

C) 197 protons and 118 electrons.

D) 197 protons,79 neutrons,and 197 electrons.

E) 79 protons and 118 neutrons.

Answer: E

Q2) What is the charge on the copper ion in Ga₃P?

A) 3-

B) 1-

C) 0

D) 1+

E) 3+

Answer: D

Q3) William Crookes was this first to observe particles produced from a cathode ray tube.These particles eventually became known as ________.

Answer: electrons

Q4) Oxygen and ________ are the two most abundant elements in the Earth's crust. Answer: silicon

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Chapter 4: Chemical Reactions

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Q1) A precipitate will form when aqueous Pb(NO₃)₂ is added to an aqueous solution of ____.

A) Cu(NO₃)₂

B) NaI

C) NaCH₃CO₂

D) Pb(ClO₄)₂

E) KNO₃

Q2) Which species in the reaction below undergoes reduction? H₂O(g)+ CO(g)\(\to\) H₂(g)+ CO₂(g)

A) H₂O

B) CO

C) H₂

D) CO₂

E) None

Q3) Nitric acid is the product of the reaction of ____ and H₂O.

A) SO₃

B) NO₂

C) N₂

D) NH₃

E) N₃^-

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Chapter 5: Stoichiometry: Quantitative Information About Chemical Reactions

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Q1) An impure sample of benzoic acid (C₆H₅COOH,122.12 g/mol)is titrated with 0.8067 M NaOH.A 5.109-g sample requires 36.97 mL of titrant to reach the endpoint.What is the percent by mass of benzoic acid in the sample?

C₆H₅COOH(aq)+ NaOH(aq)\(\to\)NaC₆H₅COO(aq)+ H₂O(l)

A) 0.02442 %

B) 2.982 %

C) 100.0 %

D) 24.42 %

E) 71.29 %

Q2) A 50.00-mL sample of a weak monoprotic acid is titrated with 0.0955 M NaOH.At the endpoint,it is found that 32.56 mL of titrant was used.What was the concentration of the weak acid?

A) 0.0622 M

B) 3.11 M

C) 0.0955 M

D) 5.87 \(\times\) 10^-5 M

E) 0.147 M

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Chapter 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

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Q1) Many homes are heated using natural gas.The combustion of natural gas converts

A) chemical potential energy to thermal energy.

B) thermal energy to mechanical energy.

C) mechanical energy to chemical potential.

D) electrostatic energy to mechanical energy.

E) gravitational energy to acoustic energy.

Q2) A hot piece of iron is dropped into a beaker containing colder water.Which of the following statements is/are CORRECT?

1)Energy is transferred as heat from the iron to the water.

2)Thermal equilibrium is attained when the iron and the water reach the same temperature.

3)Thermal energy from the iron is converted to electrostatic energy in the water.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Q3) The heat required to convert a solid at its melting point to a liquid is called the heat of ________.

Page 8

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Chapter 7: The Structure of Atoms

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Q1) The size of an electron orbital is often chosen to be the distance within which 90% of the electron density is found.Why is the orbital radius not chosen to be the distance within which 100% of the electron density is found?

Q2) Which of the following statements is/are CORRECT?

1)A diamagnetic substance is strongly attracted to a magnetic field.

2)Substances that retain their magnetism after they are withdrawn from a magnetic field are called ferromagnetic.

3)Most transition metals and all lanthanide metals are ferromagnetic.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 3

E) 1,2,and 3

Q3) How many p orbitals are in the n = 3 shell?

A) 1

B) 6

C) 0

D) 5

E) 3

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Chapter 8: The Structure of Atoms and Periodic Trends

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Q1) What noble gas core precedes the valence shell ground state electron configuration for oxygen (O)?

A) [He]

B) [Kr]

C) [Ar]

D) [Ne]

E) [Rn]

Q2) Which 1+ ion has the ground state electron configuration [Kr]4d¹⁰?

A) Ru

B) Au

C) Ag

D) In

E) Cd

Q3) The element ________ has the following electron configuration: [Rn]5f¹²7s².

Q4) Explain the difference between paramagnetic and ferromagnetic.

Q5) ________ rule states that the most stable arrangement of electrons is that which contains the maximum number of unpaired electrons,all with the same spin direction.

Q6) The f-block elements are also referred to as the ________ and actinides.

Page 10

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Chapter 9: Bonding and Molecular Structure

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Q1) Which of the following has an incomplete octet in its Lewis structure?

A) SO₂

B) F₂

C) NO₂

D) ICl

E) CO₂

Q2) Which of the following molecules or ions will have a Lewis structure most like that of phosphorus trichloride,PCl₃?

A) ClO₃^-

B) SO₃

C) CO₃^2-

D) BF₃

E) Cl₂CO

Q3) Which of the following compounds has polar covalent bonds: CCl₄,Cl₂,HCl,and KCl?

A) CCl₄ only

B) Cl₂ only

C) HCl and KCl

D) Cl₂ and KCl

E) CCl₄ and HCl

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Chapter 10: Bonding and Molecular Structure: Orbital

Hybridization and Molecular Orbitals

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Q1) What is the molecular geometry around an atom that has 2 \(\sigma\) bonds,0 \(\pi\) bonds,and 1 lone pair of electrons?

A) linear

B) trigonal planar

C) tetrahedral

D) bent

E) trigonal pyramidal

Q2) For which of the following molecules or ions does the central atom have sp hybridization: N₃^-,O₃,and SF₃⁺?

A) N₃^- only

B) O₃ only

C) SF₃⁺ only

D) O₃ and SF₃⁺

E) SF₃⁺and N₃^-

Q3) What is the hybridization of the central nitrogen atom in N₂O?

A) sp

B) sp²

C) sp³

D) none

Page 12

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Chapter 11: Gases and Their Properties

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Q1) A gas sample is held at constant pressure.The gas occupies 3.62 L of volume when the temperature is 21.6°C.Determine the temperature at which the volume of the gas is 3.49 L.

A) 295 K

B) 284 K

C) 20.8 K

D) 557 K

E) 306 K

Q2) What are two ways in which real gases differ from ideal gases?

Q3) Which of the following would represent the greatest pressure?

A) 58143 Pa

B) 307 mmHg

C) 11.7 psi

D) 0.624 atm

E) 17.7 in Hg

Q4) The rate of effusion of a gas is inversely proportional to the square root of its

Q5) The ideal gas law can be modified to correct for the errors arising from nonideality.The modified equation is known as the ________ equation of state for a real gas.

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Chapter 12: Intermolecular Forces and Liquids

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Q1) When a water molecule forms a hydrogen bond with another water molecule,which atoms are involved in the interaction?

A) a hydrogen from one molecule and a hydrogen from the other molecule

B) a hydrogen from one molecule and an oxygen from the other molecule

C) an oxygen from one molecule and an oxygen from the other molecule

D) an oxygen and a hydrogen from the same molecule

E) two hydrogens from one molecule and one hydrogen from the other molecule

Q2) What intermolecular force or bond is primarily responsible for the solubility of oxygen (O₂)in water?

A) dipole/dipole force

B) hydrogen bonding

C) dipole/induced dipole force

D) hydrogen bonding-dipole force

E) ion-induced dipole force

Q3) Which of the following substances will have the strongest intermolecular forces?

A) H₂S

B) CO

C) CH₃OH

D) HBr

E) Ar

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Chapter 13: The Chemistry of Solids

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Q1) Niobium crystallizes in a body-centered cubic lattice.If the radius of niobium is 146 pm,what is the unit cell edge length?

A) 337 pm

B) 292 pm

C) 195 pm

D) 146 pm

E) 63.2 pm

Q2) Which one of the following statements is INCORRECT?

A) Polonium is the only metal that has a primitive cubic lattice.

B) The lattice structure of the alkali metals is body-centered cubic.

C) Many metals can crystallize in more than one type of crystal lattice.

D) Metals with a body-centered cubic lattice contain a net of four metal atoms per unit cell.

E) A hexagonal close packed structure is not an example of a cubic unit cell.

Q3) Which of the following compounds is expected to have the strongest ionic bonds?

A) MgO

B) KBr

C) NaI

D) BaO

E) SrS

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Chapter 14: Solutions and Their Behavior

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Q1) Two nonpolar solvents,such as hexane and carbon tetrachloride,may be miscible even though the enthalpy of mixing of these liquids might be small.A reason that mixing occurs is that mixtures have a greater dispersal of energy relative to pure solvents.The tendency toward greater dispersal of energy is a thermodynamic function called ____.

A) entropy

B) enthalpy

C) saturation

D) adhesion

E) cohesion

Q2) What is the freezing point of an aqueous 1.36 m NaCl solution? (K_fp for water is 1.858°C/m.)Assume no ion pairing occurs.

A) 5.1°C

B) 2.5°C

C) -5.1°C

D) 0.0°C

E) -2.5°C

Q3) A surfactant used for cleaning is called a(n)________.

Q4) ________ are colloidal dispersions of one liquid in another liquid.

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Chapter 15: Chemical Kinetics: the Rates of Chemical Reactions

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Q1) The mechanism of a chemical reaction is given below. (CH₃)₃CCl \(\to\) (CH₃)₃C⁺ + Cl^- \(~~~~~~~~\) \(~~~~~~~~\) (slow)

(CH₃)₃C⁺ + OH^- \(\to\)(CH₃)₃COH \(~~~~ ~~\) \(~~~~~~~~\) (fast)

Which of the following statements concerning the reaction is/are CORRECT?

1)The overall balanced reaction is: (CH₃)₃CCl + OH^- \(\to\)(CH₃)₃COH + Cl^-

2)Hydroxide ion is a reaction intermediate.

3)The following rate law is consistent with the mechanism: rate = k[(CH₃)₃CCl]OH^-].

A) 1 only

B) 2 only

C) 3 only

D) 1 and 3

E) 1,2,and 3

Q2) The pre-exponential,A,in the Arrhenius equation is called the ________ factor.

Q3) Radioactive isotopes decay by ________-order kinetics.

Page 17

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Chapter 16: Principles of Reactivity: Chemical Equilibria

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Q1) If the reaction quotient,Q,is equal to K in a gas phase reaction,then

A) the chemical system has reached equilibrium.

B) the temperature must be increased for the reaction to proceed in the forward direction.

C) the reaction will proceed in the forward direction until equilibrium is established.

D) the reaction will proceed in the backward direction until equilibrium is established.

E) the reaction will proceed in the direction that increases the number of gas phase particles.

Q2) Which of the following statements about the reaction quotient,Q,is false?

A) The value of Q can be used to predict equilibrium concentrations.

B) It has the same expression as K_c.

C) Its value is calculated using nonequilibrium concentrations.

D) If Q > K_c,the reaction must move to equilibrium by forming more reactants.

E) If Q < K_c,the reaction must move to equilibrium by forming more products.

Q3) The symbol Q is called the ________.

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Chapter 17: The Chemistry of Acids and Bases

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Q1) What is the hydronium-ion concentration of a 0.25 M solution of HCN (K_a = 4.9 \(\times\) 10^-10)at 25°C?

A) 1.6 \(\times\) 10^-4 M

B) 3.3 \(\times\) 10^-6 M

C) 2.1 \(\times\) 10^-6 M

D) 1.1 \(\times\) 10^-5 M

E) 4.4 \(\times\) 10^-5 M

Q2) All of the following compounds are acids containing chlorine.Which compound is the weakest acid?

A) HCl

B) HClO

C) HClO₂

D) HClO₃

E) HClO₄

Q3) When a Lewis acid combines with a Lewis base,the base supplies both electrons to the bond.This type of chemical bond is called a(n)________ covalent bond.

Q4) Write a net ionic equation for the neutralization reaction of hydrochloric acid and potassium hydroxide.Identify the spectator ion(s).

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Chapter 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria

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Q1) What is the pH of an aqueous solution composed of 0.64 M NH₄⁺ and 0.20 M NH₃? (K_a of NH₄⁺ = 5.6 \(\times\) 10^-10)

A) 4.80

B) 8.75

C) 9.20

D) 9.25

E) 9.76

Q2) What is the maximum hydroxide-ion concentration that a 0.027 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂,K_sp = 1.8 \(\times\) 10^-11.

A) 4.2 \(\times\) 10^-6

B) 1.7 \(\times\) 10^-4

C) 1.2 \(\times\) 10^-8

D) 6.7 \(\times\) 10^-9

E) 2.6 \(\times\) 10^-5

Q3) For a monoprotic acid titration,the ________ point in a titration is the point where the moles of strong base added equals the moles of acid initially present.

Page 20

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Chapter 19: Entropy and Free Energy

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Q1) ________ changes only occur in the direction that leads toward chemical equilibrium.

Q2) For the process Br₂(l)\(\to\) 2Br(g),

A) (\(\Delta\)H) is + and \(\Delta\)S is + for the reaction.

B) (\(\Delta\)H) is + and \(\Delta\)S = 0 for the reaction.

C) (\(\Delta\)H) is - and \(\Delta\)S is - for the reaction.

D) (\(\Delta\)H) is - and \(\Delta\)S is + for the reaction.

E) (\(\Delta\)H) is + and \(\Delta\)S is - for the reaction.

Q3) When a real gas is compressed from low pressure to a higher pressure,its temperature increases.Predict the signs \(\Delta\)H and \(\Delta\)S.

A) (\(\Delta\)H) < 0 and \(\Delta\)S < 0

B) (\(\Delta\)H) < 0 and \(\Delta\)S > 0

C) (\(\Delta\)H) > 0 and \(\Delta\)S < 0

D) (\(\Delta\)H) > 0 and \(\Delta\)S > 0

E) (\(\Delta\)H) < 0 and \(\Delta\)S = 0

Q4) In any chemical process,energy must be conserved.This is a statement of the ________ law of thermodynamics.

Q5) The total entropy of the universe is always increasing.This is a statement of the ________ law of thermodynamics.

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Chapter 20: Principles of Reactivity: Electron Transfer Reactions

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Q1) Write a balanced chemical equation for the overall reaction represented by the cell notation below.

Al(s)| Al³⁺(aq)|| Br^-(aq)| Br₂(g)| Pt(s)

A) 2Al(s)+ 3Br₂(g)\(\to\) 2Al³⁺(aq)+ 6Br^-(aq)

B) Al(s)+ Al³⁺(aq)\(\to\)Br^-(aq)+ Br₂(g)

C) 2Al³⁺(aq)+ 6Br^-(aq)\(\to\) 2Al(s)+ 3Br₂(g)

D) Al(s)+ 3Br₂(g)\(\to\) Al³⁺(s)+ 2Br^-(aq)

E) Al(s)+ 2Br^-(aq)\(\to\) Br₂(g)+ Al³⁺(aq)

Q2) When a secondary battery provides electrical energy,it is acting as a voltaic cell.When the battery is recharging,it is operating as a(n)________ cell.

Q3) Which of the following statements concerning a voltaic cell is/are correct?

1)Reduction occurs at the cathode.

2)A spontaneous reaction generates an electric current in a voltaic cell.

3)Without a salt bridge charge buildup will cause the cell reaction to stop.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

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Chapter 21: Environmental Chemistry Earths

Environment,energy,and Sustainability

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Q1) Most hydrogen gas is produced industrially by A) electrolysis.

B) solar energy.

C) steam reforming.

D) bacteria.

E) fuel cells.

Q2) Which of the following is not a greenhouse gas?

A) CO₂

B) CH₄

C) H₂O

D) N₂O

E) N₂

Q3) Many homes are heated using natural gas.The combustion of natural gas converts A) chemical potential energy to thermal energy.

B) thermal energy to mechanical energy.

C) mechanical energy to chemical potential.

D) electrostatic energy to mechanical energy.

E) gravitational energy to acoustic energy.

Q4) Explain why fossil fuels,hydrocarbons produced by natural processes,are considered a nonrenewable energy resource.

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Chapter 22: The Chemistry of the Main Group Elements

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Q1) All of the following elements or compounds react with water to produce hydrogen gas EXCEPT ____.

A) Na(s)

B) MgH₂(s)

C) Ca(s)

D) LiH(s)

E) CaO(s)

Q2) Which of the following nitrogen oxides are free radicals: NO,N₂O,NO₂,and/or N₂O₃?

A) NO and N₂O

B) N₂O and NO₂

C) NO₂ and N₂O₃

D) NO and NO₂

E) N₂O and N₂O₃

Q3) The products of the reaction of calcium hydride and water are

A) CaOH + H₂.

B) Ca₂O + H₂.

C) Ca(OH)₂ + H₂.

D) CaO + H₂.

E) CaOH + O₂.

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Chapter 23: The Chemistry of the Transition Elements

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Q1) Which of the following pairs of coordination compounds are coordination isomers?

A) [Cr(H₂O)₆]SO₄ and [Cr(NH₃)₆]SO₄

B) [Cr(NH₃)₅Cl]SO₄ and [Cr(NH₃)₅SO₄]Cl

C) [Co(NH₃)₄(H₂O)₂]Cl₂ and [Co(NH₃)₂(H₂O)₄]Cl₂

D) [Cr(NH₃)₆](NO₃)₂ and [Fe(NH₃)₆](NO₃)₃

E) [Cr(H₂O)₆]Cl₂ and [Fe(H₂O)₆]Cl₂

Q2) What is the coordination number of the transition metal ion in [Ag(NH₃)₂]Cl?

A) 2

B) 3

C) 4

D) 6

E) 8

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Chapter 24: Carbon: Not Just Another Element

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Q1) Which of the following compounds might be used to reduce a carboxylic acid to an aldehyde?

A) H⁺

B) Cl₂

C) K₂Cr₂O₇

D) KMnO₄

E) NaBH₄

Q2) What is the molecular formula for heptane?

A) C₆H₁₂

B) C₆H₁₄

C) C₇H₁₄

D) C₇H₁₆

E) C₉H₂₀

Q3) Which of the following is \(\underline{\text{ not }}\) an addition polymer?

A) polyvinyl chloride

B) nylon

C) teflon

D) styrofoam

E) polypropylene

Q4) Draw Lewis structures for all possible isomers of C₃H₆O.

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Chapter 25: Biochemistry

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Q1) A phospholipid may include all of the following except

A) ester functional groups.

B) one or more alkene functional groups.

C) a net negative charge.

D) a polar tail.

E) a phosphodiester linkage.

Q2) Which of the following statements concerning polysaccharides is/are correct?

1)Humans do not have enzymes that will break down cellulose.

2)Amylopectin and glycogen are both branched chains of glucose.

3)Amylose starch is a linear polysaccharide.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Q3) The fully protonated form of the amino-acid glycine (R=H)may be simply written as H₂Gly⁺.Write the balanced acid dissociation equilibria (K_a1 and K_a2)for this acid.

Q4) The amide linkages in a protein and also called ___ bonds.

Q5) What is the role of tRNA in protein synthesis?

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Chapter 26: Nuclear Chemistry

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Sample Questions

Q1) A certain radioactive isotope has a rate constant of decay of 2.74 \(\times\)10^-2 min^-1.Calculate the time required for a sample of this isotope to decay to one-fourth of its initial value.

A) 25.3 min

B) 31.6 min

C) 0.0548 min

D) 50.6 min

E) 2.74 min

Q2) What is the charge on a positron?

A) +2

B) +1

C) 0

D) -1

E) -2

Q3) When a nucleus undergoes radioactive decay,its new mass number is

A) always less than its original mass number.

B) never more than its original mass number.

C) never less than its original mass number.

D) always the same as its original mass number.

E) always more than its original mass number.

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