Survey of Chemistry Solved Exam Questions - 2075 Verified Questions

Survey of Chemistry

Solved Exam Questions

Course Introduction

Survey of Chemistry provides a broad overview of the fundamental principles of chemistry, including atomic and molecular structure, chemical bonding, stoichiometry, states of matter, solutions, and basic chemical reactions. The course emphasizes the essential concepts and applications of chemistry in everyday life, introduces laboratory techniques, and fosters scientific literacy. Designed for non-science majors or those seeking a foundational understanding, this course lays the groundwork for further study in the chemical sciences or related fields.

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) An intensive property of a substance is

A) independent of the amount present.

B) dependent on its volume,but not its mass.

C) not affected by its temperature.

D) dependent only on its temperature.

E) dependent only on its mass and volume.

Answer: A

Q2) A \(\underline{\text{ theory }}\) is a ________.

A) mathematical formula that models a pattern of behavior

B) set of quantitative data

C) well-tested unifying principle that explains a body of facts

D) tentative explanation or predication based upon experimental observations

E) set of experiments designed to test a theory

Answer: C

Q3) Potential energy possessed by water at the top of a waterfall is known as ________ energy.

Answer: gravitational

Q4) Substances like hydrogen (H₂) and oxygen (O₂) that are composed of only one type of atom are classified as ________.

Answer: elements

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Chapter 2: Mathlets Review: The Tools of Quantitative Chemistry

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Sample Questions

Q1) How many cubic kilometers equal one cubic meter?

A) 10⁴

B) 10⁹

C) 10^-3

D) 10^-9

E) 10³

Answer: D

Q2) Which of the following is the \(\underline{\text{ smallest }}\) volume?

A) 1.5 \(\times\) 10⁸ pL

B) 1.5 \(\times\) 10⁶ nL

C) 1.5 \(\times\) 10³ \(\mu\)L

D) 1.5 \(\times\) 10^-1 mL

E) 1.5 \(\times\) 10^-5 L

Answer: E

Q3) What is the difference between the accuracy of measurements and the precision of measurements?

Answer: Accuracy is an indicator of how close a measurement,or the average of a set of measurements,is to the correct value.Precision is an indicator of how close two measurements are to each other,or how much numerical spread is present in a set of measurements.

Page 4

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Chapter 3: Atoms, molecules, and Ions

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Sample Questions

Q1) A certain element consists of two stable isotopes.The first has a mass of 14.0031 amu and a percent natural abundance of 99.63%.The second has a mass of 15.001 amu and a percent natural abundance of 0.37%.What is the atomic weight of the element?

A) 13.95 u

B) 14.00 u

C) 14.01 u

D) 14.50 u

E) 19.50 u

Answer: C

Q2) In which ionic compound,NaBr or KBr,is the force of attraction between anions and cations stronger?

Answer: The force of attraction is stronger for NaBr.The electrostatic attraction between anions and cations decreases as the separation of the ions increases.The potassium ion will be farther from the bromide ion than the sodium ion due to its larger ionic radius.

Q3) Pure oxygen can exist as O₂ or O₃.Elements that exist in more than one distinct form are called ________.

Answer: allotropes

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Page 5

Chapter 4: Chemical Reactions

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Sample Questions

Q1) A solution is a homogeneous mixture composed of one or more ____________ dissolved in a solvent.

Q2) A precipitate will form when aqueous nickel(II)chloride is added to an aqueous solution of ____.

A) SrI₂

B) Cu(NO₃)₂

C) KOH

D) Na₂SO₄

E) NaBr

Q3) The oxidation number of nitrogen is highest in which of the following?

A) NH₃

B) N₂

C) HNO₂

D) NaNO₃

E) NO₂^-

Q4) A(n)________ agent gains electrons in an oxidation-reduction reaction.

Q5) _____-oxides produce acids when reacted with water.

Q6) ________ acid is produced in a larger quantity than any other chemical in the United States.This chemical is used in the production of fertilizers,pigments,alcohol,paper and detergents.

Page 6

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Chapter 5: Stoichiometry: Quantitative Information About Chemical Reactions

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Q1) What mass of Na₂CO₃ is present in 0.250 L of a 0.852 M Na₂CO₃ solution?

A) 22.6 g

B) 26.5 g

C) 90.3 g

D) 31.1 g

E) 361 g

Q2) Transmittance,T,is defined as the intensity of light transmitted through a sample divided by the intensity of light incident on the sample.The absorbance,A,is defined as

A) A = -log T

B) A = log (-T)

C) A = 10^T

D) A = 10^-^T

E) A = 10^-1/^T

Q3) The pH of purified water (or of a neutral solution)is _____.

Q4) The percent yield of a chemical reaction is calculated by dividing the actual yield by the ________ yield and multiplying by 100%.

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

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Sample Questions

Q1) How much heat is liberated at constant pressure if 0.834 g of calcium carbonate reacts with 48.9 mL of 0.668 M hydrochloric acid?

CaCO₃(s)+ 2HCl(aq)\(\to\)CaCl₂(aq)+ H₂O(l)+ CO₂(g); \(\Delta\)_rH° = -15.2 kJ/mol-rxn

A) -0.127 kJ

B) -0.375 kJ

C) -12.7 kJ

D) -0.248 kJ

E) -10.2 kJ

Q2) 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.

Q3) In thermodynamics,a(n)________ is defined as the object,or collection of objects,being studied.The surroundings include everything else.

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Chapter 7: The Structure of Atoms

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Q1) A ________,designated by the Greek symbol \(\varPsi\),describes the wave behavior of an electron in an atom.

Q2) According to Heisenberg's ________ principle,it is impossible to simultaneously measure the exact location and energy of an electron.

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

A) 1

B) 6

C) 0

D) 5

E) 3

Q4) Which type of experiment demonstrates that light has the properties of a particle?

A) nuclear fission

B) electron diffraction

C) light emission from atomic gases

D) mass spectroscopy

E) photoelectric effect

Q5) A point in a standing wave that has zero amplitude is called a(n)________.

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Page 9

Chapter 8: The Structure of Atoms and Periodic Trends

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Sample Questions

Q1) A metal halide forms when strontium reacts with elemental iodine.What is the most likely formula of this metal halide?

A) SrI

B) SrI₂

C) Sr₂I

D) SrI₃

E) Sr₃I₂

Q2) In general,atomic radii

A) decrease down a group and remain constant across a period.

B) decrease down a group and increase across a period.

C) increase down a group and increase across a period.

D) increase down a group and remain constant across a period.

E) increase down a group and decrease across a period.

Q3) According to the building-up principle or aufbau principle,which subshell is typically filled next after the 5p subshell?

A) 6s

B) 5d

C) 3p

D) 6d

E) 5f

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Chapter 9: Bonding and Molecular Structure

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Q1) What are the approximate O-S-O bond angles in SO₃^2-?

A) 90S1U1P1\(\circ\)S1S1P0

B) 109.5S1U1P1\(\circ\)S1S1P0

C) 120S1U1P1\(\circ\)S1S1P0

D) 180S1U1P1\(\circ\)S1S1P0

E) 90S1U1P1\(\circ\)S1S1P0 and 180S1U1P1\(\circ\)S1S1P0

Q2) One might expect PCl₃ to have a trigonal planar molecular geometry since its central atom is surrounded by three outer atoms.However,PCl₃ has a trigonal pyramidal geometry.Explain.

Q3) In PCl₅,the Cl-P-Cl bond angle between an axial and an equatorial chlorine atom is ________ degrees.

Q4) Which of the following molecules or ions are isoelectronic: SO₃,NF₃,NO₃^-,CO₃^{2 -}?

A) SO₃ and NF₃

B) NF₃ and CO₃^2-

C) SO₃,NF₃ and CO₃^2-

D) SO₃,NO₃^- and CO₃^2-

E) SO₃,NF₃,NO₃^-,and CO₃^2-

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Chapter 10: Bonding and Molecular Structure: Orbital

Hybridization and Molecular Orbitals

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Q1) Which of the following statements concerning molecular orbital (MO)bond theory is/are CORRECT?

1)MO theory can describe molecular bonding in excited states.

2)Molecular orbitals are obtained from the combination of atomic orbitals.

3)MO theory predicts that electrons are delocalized over the molecule through molecular orbitals.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Q2) A molecular orbital that decreases the electron density between two nuclei is said to be ____.

A)hybridized

B)bonding

B)antibonding

D)pi-bonding

E)nonpolar

Q3) The hybridization of the carbon atom in CF₃⁺ is

Page 12

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Chapter 11: Gases and Their Properties

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Q1) Gaseous chlorine is held in two separate containers at identical temperature and pressure.The volume of container 1 is 1.30 L,and it contains 6.70 mol of the gas.The volume of container 2 is 2.33 L.How many moles of the gas are in container 2?

A) 12.0 mol

B) 20.3 mol

C) 0.452 mol

D) 3.74 mol

E) none of these

Q2) Real gases are those that

A) only behave ideally at high pressures or low temperatures

B) deviate from ideal behavior

C) are only available naturally in the earth's atmosphere

D) are called real gases because their behavior can easily be modeled

E) have an even number of protons

Q3) The pressure exerted by gas molecules inside a container is due to gas molecules colliding with the walls of the container.Why does one mole of oxygen molecules exert the same pressure inside a flask as one mole of hydrogen molecules,although the mass of an oxygen molecule is sixteen times greater than the mass of a hydrogen molecule?

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Chapter 12: Intermolecular Forces and Liquids

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Q1) For which of the following pure solids is it necessary to break covalent bonds to make a liquid or gas: C(graphite),CO₂(s),C₆₀(s),and C(diamond)?

A) C(graphite)only

B) CO₂(s)only

C) CO₂(s)and C₆₀(s)

D) C(graphite),C₆₀(s)and C(diamond)

E) C(graphite)and C(diamond)

Q2) Which of the following bonds can potentially contribute to the formation of a hydrogen bond in a solid or liquid?

A) Ge-H

B) P-H

C) N-H

D) Si-H

E) Cl-H

Q3) Which ion,K⁺ or Ca²⁺,is expected to have the more negative enthalpy of hydration? Why?

Q4) Above its critical temperature and pressure,a substance becomes a(n)________ fluid.

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Chapter 13: The Chemistry of Solids

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Q1) Cesium bromide crystallizes in a primitive cubic unit cell with bromide ions at the lattice points.The cesium ions occupy cubic holes.How many bromide ions surround each cesium ion in cesium bromide?

A) 1

B) 2

C) 4

D) 8

E) 12

Q2) Which of the following statements concerning the cubic unit cell is/are CORRECT?

1)For cubic unit cells,three cell symmetries occur: primitive cubic,face-centered cubic,and body-centered cubic.

2)The cell edges of a cubic unit cell are all equal in length.

3)The corner angles of a cubic cell are 90S1U1P1\(\circ\)S1S1P0.

A) 1 only

B) 2 only

C) 3 only

D) 2 and 3

E) 1,2,and 3

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15

Chapter 14: Solutions and Their Behavior

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Q1) What partial pressure of oxygen gas is required in order for 0.00392 g of the gas to dissolve in 23.7 mL of pure water? The Henry's law constant for oxygen gas is 1.3 \(\times\) 10^-3 M atm^-1.

A) 2.2 \(\times\) 10^-7 atm

B) 4.0 \(\times\) 10⁰ atm

C) 1.6 \(\times\) 10^-7 atm

D) 2.5 \(\times\) 10^-1 atm

E) 4.2 \(\times\) 10^-2 atm

Q2) A 12.0% sucrose solution by mass has a density of 1.05 g/cm³.What mass of sucrose is present in a 63.0-mL sample of this solution?

A) 7.94 g

B) 7.20 g

C) 0.126 g

D) 551 g

E) 7.56 g

Q3) If an egg's shell is carefully dissolved using an acid,the egg white and yolk will remain intact inside a membrane.If the egg is then placed in distilled water,it will slowly expand until it bursts.Why?

Q4) A surfactant used for cleaning is called a(n)________.

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Chapter 15: Chemical Kinetics: the Rates of Chemical Reactions

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Q1) For the first-order decomposition of N₂O₅ at a high temperature,determine the rate constant if the N₂O₅ concentration decreases from 1.04 M to 0.62 M in 375 seconds.

A) 5.99 \(\times\) 10^-4 s^-1

B) 1.59 \(\times\) 10^-3 s^-1

C) 1.74 \(\times\) 10^-3 s^-1

D) 1.38 \(\times\) 10^-3 s^-1

E) 1.94 \(\times\) 10² s^-1

Q2) Radioactive isotopes decay by ________-order kinetics.

Q3) At a given temperature,a first-order reaction has a rate constant of 3.5 \(\times\) 10^-3 s^-1.How long will it take for the reaction to be 24% complete?

A) 410 s

B) 1200 s

C) 910 s

D) 34 s

E) 78 s

Q4) Termolecular elementary steps are rare.Why?

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Q5) The pre-exponential,A,in the Arrhenius equation is called the ________ factor.

Chapter 16: Principles of Reactivity: Chemical Equilibria

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Q1) If the reaction quotient,Q,is greater than 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) The K_a for the monoprotic acid hypochlorous acid is 3.5 \(\times\) 10^-8.What is K_b for the hypochlorite ion,the conjugate base of hypochlorous acid?

A) 2.9 \(\times\) 10^-7

B) 3.5 \(\times\) 10^-8

C) 2.9 \(\times\) 10⁷

D) 3.5 \(\times\) 10⁶

E) 3.5 \(\times\) 10^-22

Q2) What is the equilibrium concentration of H₂C₂O₄ in a 0.230 M oxalic acid,H₂C₂O₄,solution? For oxalic acid,K_a1 = 5.6 \(\times\) 10^-2 and K_a2 = 5.1 \(\times\) 10^-5.

A) 1.4 \(\times\) 10^-1 M

B) 1.1 \(\times\) 10^-1 M

C) 2.3 \(\times\) 10^-1 M

D) 5.1 \(\times\) 10^-5 M

E) 8.9 \(\times\) 10^-2 M

Q3) A molecule that can behave as either a Brønsted-Lowry acid or base is termed ________.

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

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Q1) What is the pH of a solution made by combining 175 mL of 0.33 M NaC₂H₃O₂ with 126 mL of 0.48 M HC₂H₃O₂? The K_a of acetic acid is 1.75 \(\times\) 10^-5.

A) 4.74

B) 4.78

C) 5.79

D) 4.69

E) 5.24

Q2) A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.143 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What was the original concentration of the propionic acid?

A) 0.295 M

B) 0.125 M

C) 0.082 M

D) 0.143 M

E) 0.250 M

Q3) If the ratio of acid to base in a buffer is increased by a factor of 10,the buffer pH decreases by ________.

Page 20

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Chapter 19: Entropy and Free Energy

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Q1) Does the formation of complex molecules such as proteins and nucleic acids from more simple molecules contradict the second law of thermodynamics?

Q2) What is \(\Delta\)G° at 298 K for the following reaction?

H₂(g)+

Br₂(g)\(\to\) 2HBr(g); \(\Delta\)_rHS1U1P1\(\circ\)S1S1P0 = -103.8 kJ/mol-rxn; \(\Delta\)_rSS1U1P1\(\circ\)S1S1P0 = 21.3 J/K.mol-rxn at 298 K

A) -97.45 kJ/mol-rxn

B) 110.1 kJ/mol-rxn

C) -110.1 kJ/mol-rxn

D) 6.451 \(\times\) 10³ kJ/mol-rxn

E) -6.451\(\times\) 10³ kJ/mol-rxn

Q3) The standard free energy change for a chemical reaction is +13.3 kJ/mol.What is the equilibrium constant for the reaction at 125 S1U1P1\(\circ\)S1S1P0C? (R = 8.314 J/K.mol)

A) 2.8 \(\times\) 10^-6

B) 2.0 \(\times\) 10^-5

C) 4.7 \(\times\) 10^-3

D) 1.8 \(\times\)10^-2

E) 2.1 \(\times\) 10²

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Chapter 20: Principles of Reactivity: Electron Transfer Reactions

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Q1) Explain the function of a salt bridge in a voltaic cell.

Q2) Which of the following statements is true concerning the electrochemical cell below, Ba(s)| Ba²⁺(aq,1.0 M)|| Mn²⁺(aq,1.0 M)| Mn(s)

And given the following standard reduction potentials?

Ba²⁺(aq)+ 2e^- \(\to\) Ba(s); \(~~~~~~~~\)\(~~~~~~~~\)E° = -2.91 V

Mn²⁺(aq)+ 2e^-\(\to\) Mn(s); \(~~~~~~~~\)\(~~~~~~~~\)E° = -1.19 V

A) The cell reaction is spontaneous with a standard cell potential of -4.10 V.

B) The cell reaction is spontaneous with a standard cell potential of 1.72 V.

C) The cell reaction is nonspontaneous with a standard cell potential of 1.72 V.

D) The cell reaction is nonspontaneous with a standard cell potential of -4.10 V.

E) The cell reaction is spontaneous with a standard cell potential of -1.72 V.

Q3) In an electrolytic cell,reduction occurs at the ________ and oxidation occurs at the

Q4) 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.

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Chapter 21: Environmental Chemistry Earths

Environment,energy,and Sustainability

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Q1) What process is used to covert coal into coke?

A) steam reforming

B) liquefaction

C) fermentation

D) heating in the absence of air

E) heating in air

Q2) The largest \(\underline{\text{ renewable }}\) source of electricity production in the United States is from ___.

A) wind

B) hydroelectricity

C) solar

D) geothermal

E) biomass

Q3) The largest known source of tar sands is found in

A) the United States of America.

B) United Arab Emirates.

C) Venezuela.

D) Saudi Arabia.

E) Canada.

Q4) Explain why the melting of Arctic sea ice will not raise the sea level.

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Chapter 22: The Chemistry of the Main Group Elements

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Q1) Which of the following statements is INCORRECT?

A) Phosphoric acid gives a tart taste to carbonated beverages such as colas.

B) Sodium phosphate,Na₃PO₄,is a relatively strong base used in paint strippers.

C) Ca(H₂PO₄)₂.H₂O is used as an acid leavening agent in baking powder.

D) Ca₃(PO₄)₂ is a dark green compound used in latex paints.

E) Calcium monohydrogen phosphate is an abrasive and polishing agent in toothpaste.

Q2) Predict the formula of the product resulting from reaction of elemental forms of Sr and P.

A) SrP

B) SrP₂

C) Sr₂P

D) SrP₃

E) Sr₃P₂

Q3) The primary product of the reaction of potassium and oxygen is ________.This compound is used in oxygen generators.

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24

Chapter 23: The Chemistry of the Transition Elements

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Q1) What is the formula for potassium diamminetetrachlorovanadate(III)?

A) [KV(NH₃)₂Cl₄]

B) K₂[V(NH₃)₂Cl₄]

C) K[V(NH₃)₂Cl₄]

D) [KV(NH₃)₂]Cl₄

E) K[V(NH₃)₂]Cl₄

Q2) Determine the number of unpaired electrons in an octahedral,high-spin Cr(II)complex.

A) 1

B) 2

C) 3

D) 4

E) 5

Q3) 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) What is the product of the addition of HCl to ethylene?

A) chloroethane

B) chloroethylene

C) 1,2-dichloroethane

D) 1,1-dichloroethane

E) 1,1,2,2-tetrachloroethylene

Q2) How many structural isomers possessing the alcohol functional group have the molecular formula C₄H₁₀O?

A) 1

B) 2

C) 3

D) 4

E) 5

Q3) Low density polyethylene (LDPE)is most likely to be used in

A) sandwich bags.

B) bottle caps.

C) rigid pipes.

D) contact lenses.

E) fabrics and apparel.

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

Page 26

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Chapter 25: Biochemistry

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Q1) Saturated fats and oils have ___ melting points than unsaturated fats and oils because of greater ___ forces between molecules.

A) lower,hydrogen bonding

B) higher,London dispersion

C) higher,hydrogen bonding

D) higher,dipole-dipole

E) lower,London dispersion

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

1)Enzymes are biological catalysts.

2)A reaction occurs when substrate binds the enzyme active site.

3)Enzymes catalyze multiple types of reactions.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Q3) The oxygen that bridges two sugars in a disaccharide is known as a ___ bond.

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

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

Q6) A compound which contains both a positive and negative charge is called a ____.

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Chapter 26: Nuclear Chemistry

Available Study Resources on Quizplus for this Chatper

79 Verified Questions

79 Flashcards

Source URL: https://quizplus.com/quiz/72721

Sample Questions

Q1) If a nucleus decays by successive \(\alpha\),\(\beta\),\(\beta\) particle emissions,its atomic number will

A) decrease by four.

B) decrease by two.

C) increase by four.

D) increase by two.

E) be unchanged.

Q2) What is the percent activity of a radioactive sample (relative to its original activity)that has undergone two half-lives of decay?

A) 25.0%

B) 12.5%

C) 6.25%

D) 3.13%

E) 75.0%

Q3) At the high temperatures necessary for fusion,matter exists as a plasma,which is A) a liquid form of a radioactive element.

B) a gaseous cloud of electrons and positrons.

C) a mixture of unbound nuclei and electrons.

D) an equal mixture of matter and anti-matter.

E) a dense solid composed of neutrons.

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