Survey of Chemistry Exam Materials - 986 Verified Questions

Survey of Chemistry

Exam Materials

Course Introduction

Survey of Chemistry provides an overview of the fundamental principles and concepts of chemistry, with an emphasis on real-world applications and problem-solving. Topics typically include atomic structure, chemical bonding, stoichiometry, states of matter, solutions, acids and bases, and basic organic chemistry. The course is designed for students seeking a broad understanding of chemistry, particularly those in health-related or non-science majors, and it aims to develop scientific literacy and practical skills through laboratory experiments and classroom instruction.

Recommended Textbook

Introductory Chemistry An Active Learning Approach 6th Edition by Mark S. Cracolice

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Chapter 2: Matter and Energy

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Q1) Which of the following changes is/are endothermic for the underlined object?

i.baking a potato

ii.a person being burned by a pan

iii.a wood log burning

iv.a lit light bulb shining

v.a person digesting food

A)iii only

B)iii and iv

C)iii and iv.

D)i and iv

E)i and ii

Answer: E

Q2) Which of the following does not describe the gaseous state?

A)Same shape as a closed container

B)Same volume of a closed container

C)Random, independent particle movement

D)Easily compressed

E)All describe the gaseous state

Answer: E

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Page 3

Chapter 3: Measurement and Chemical Calculations

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Sample Questions

Q1) What is the volume of 22 g of gold,which has a density of 19.3 g/cm³?

A)21 cm³

B)3 cm³

C)1.1 cm³

D)0.88 cm³

E)4.2 × 10² cm³

Answer: C

Q2) Convert 3.77 × 10⁸ pL to mL,daL,and dL.1 pL = 10^-12 L,1 dL = 10^-1 L,1 daL = 10¹ L

A)3.77 × 10²³ mL, 3.77 × 10¹⁹ daL, 3.77 × 10²¹ dL

B)3.77 × 10¹⁷ mL, 3.77 × 10²¹ daL, 3.77 × 10¹⁹ dL

C)3.77 × 10^-1 mL, 3.77 × 10^-5 daL, 3.77 × 10^-3 dL

D)3.77 × 10^-4 mL, 3.77 × 10^-5 daL, 3.77 × 10^-3 dL

E)3.77 × 10^-7 mL, 3.77 × 10^-3 daL, 3.77 × 10^-5 dL

Answer: C

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4

Chapter 4: Introduction to Gases

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Sample Questions

Q1) Which of the following pressures is equal to 0.80 atm?

A)9.5 × 10² torr

B)1.3 bar

C)24 in. Hg

D)18 psi

E)1.0 kPa

Q2) A fixed quantity of a gas is maintained at a constant temperature.The gas has a volume of 0.847 m³ at 735 torr.What is the pressure of the gas when the volume is changed to 0.905 m³?

A)0.00145 torr

B)0.00127 torr

C)781 torr

D)563 torr

E)688 torr

Q3) Convert 1.47 atm to psi and in.Hg.

A)0.100 psi; 0.0491 in. Hg

B)1.12 × 10³ psi; 149 in. Hg

C)149 psi; 1.12 × 10³ in. Hg

D)1.49 × 10⁵ psi; 1.12 × 10³ in. Hg

E)21.6 psi; 44.0 in. Hg

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Chapter 5: Atomic Theory: The Nuclear Model of the Atom

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Sample Questions

Q1) Two natural isotopes exist for silver.51.83% of the atoms have a mass of 106.90509 u,and the remaining fraction has a mass of 108.9047 u.Calculate the atomic mass of silver.

A)52.46 u

B)55.41 u

C)106.90509 u

D)107.87 u

E)108.9047 u

Q2) Which of the following statements is false?

A)The atomic mass unit is exactly 1/12 of the mass of a carbon-12 atom

B)Both protons and neutrons have atomic masses very close to 1 u

C)A carbon-12 atom with six electrons has a mass of 12.6 u

D)The atomic mass of an element is the average mass of the atoms of an element compared to an atom of carbon-12 at exactly 12 u

E)To find the atomic mass of an element, you must know the atomic mass of each isotope and the fraction of each isotope in a sample

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Chapter 6: Chemical Nomenclature

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Sample Questions

Q1) For each of the following formulas,choose the correct name.

i.Pb²⁺

ii.S^2-

iii.Ni²⁺

I ii iii

A)lead ion sulfur ion nickel ion

B)lead ion sulfur ion nickelide ion

C)lead(II) ion sulfur ion nickel ion

D)lead(II) ion sulfide ion nickel ion

E)lead(II) ion sulfide ion nickel(II) ion

Q2) What are the names for the compounds H₂O and NH₃,in that order?

A)Dihydrogen oxide, nitrogen trihydride

B)Dihydrogen oxide, ammonia

C)Water, nitrogen trihydride

D)Water, ammonia

E)Hydrated oxygen, hydrated nitrogen

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Chapter 7: Chemical Formula Relationships

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Sample Questions

Q1) How many grams of oxygen are in 8.50 g of formaldehyde,CH₂O?

A)2.12 g

B)2.83 g

C)4.25 g

D)4.53 g

E)16.0 g

Q2) How many moles are in 6.27 × 10²⁴ formula units of sodium nitrate?

A)0.0960

B)10.4

C)85.0

D)3.77 × 10⁴⁸

E)2.65 × 10^-49

Q3) Which off the following provides the conversion factor to convert 10.7 g of sulfur dioxide to the corresponding number of moles of sulfur dioxide?

A)molar mass

B)molecular mass

C)formula mass

D)Avogadro's number

E)either a or c

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Page 8

Chapter 8: Chemical Reactions

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Sample Questions

Q1) Calcium nitrate and potassium fluoride solutions react to form a precipitate.How should this reaction be classified?

A)combination

B)decomposition

C)double-replacement

D)single-replacement

Q2) Calcium reacts with the oxygen in the air,forming calcium oxide.Write the balanced chemical equation for this reaction.What is the sum of the coefficients?

A)3 or less

B)4

C)5

D)6

E)7 or more

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Chapter 9: Chemical Change

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Sample Questions

Q1) What ions are present in an aqueous solution of hydrochloric acid?

A)H₂⁺(aq) + Cl₂^-(aq)

B)HCl(aq)

C)H⁺(aq) + Cl^-(aq)

D)H₃O⁺(aq) + ClO₃^-(aq)

E)H⁺(aq) + ClO₃^-(aq)

Q2) In the net ionic equation for the following,what are the spectator ions?

NH₄NO₃(aq)+ KCl(aq) KNO₃(aq)+ NH₄Cl(aq)

A)None of the ions are spectator ions

B)The cations are spectators; the anions are not

C)All the ions are spectators

D)The anions are spectators; the cations are not

E)The potassium ions are spectators

Q3) If a solution conducts electricity,it is positive evidence that...

A)molecules are dissolved in the solution.

B)the solution is pure water.

C)the solute must be a nonelectrolyte.

D)the solute is an strong electrolyte.

E)mobile ions are present.

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Chapter 10: Quantity Relationships in Chemical Reactions

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Sample Questions

Q1) A chemist combines hydrochloric acid with a sodium hydroxide solution,transferring 5.75 kJ of heat.Express this in calories.

A)2.41 × 10^-2 cal

B)2.41 × 10¹ cal

C)2.41 × 10⁴ cal

D)1.37 × 10^-3 cal

E)1.37 × 10³ cal

Q2) Ammonium sulfate can be made by the reaction H₂SO₄ + 2 NH₃ (NH₄)₂SO₄.What quantity of ammonium sulfate will result from the reaction of 5.00 kg of ammonia and 20.0 kg of sulfuric acid?

A)13.5 kg

B)19.4 kg

C)25.0 kg

D)26.9 kg

E)38.8 kg

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Chapter 11: Atomic Theory: The Quantum Model of the Atom

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Sample Questions

Q1) Which of the following provides the best explanation for the many chemical similarities between sodium and potassium?

A)Both have atomic masses between 20 and 40 u

B)Both have an ns¹ electron configuration for their highest occupied energy level

C)Both are main group elements

D)Both are solids at room temperature and pressure

E)The atomic numbers of the two elements differ by less than ten

Q2) How many of the following elements belong to the chemical family known as the alkaline earths?

sodium,magnesium,chlorine,neon,calcium,bromine,argon,fluorine,helium,hydrogen

A)1

B)2

C)3

D)4

E)5

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Chapter 12: Chemical Bonding

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Sample Questions

Q1) Which bond is completely nonpolar?

A)F-F

B)H-F

C)C-N

D)H-O

E)C-H

Q2) Which of the following is the best description of metallic bonding?

A)Positively charged metal ions surrounded by freely moving electrons

B)Alternating positively charged metal ions and negatively charged metal ions

C)Pairs of metal atoms sharing electrons, plus weak intermolecular forces holding the pairs in place in the metal crystal

D)Groups of three metal atoms sharing electrons (three-center bonds), plus weak intermolecular forces holding the groups in place in the metal crystal

E)Metallic bonding is essentially the same as covalent bonding, except that in metallic bonding, protons are shared rather than electrons

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13

Chapter 13: Structure and Shape

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Sample Questions

Q1) Which of the following molecules is/are nonpolar?

i.CH₄

ii.CH₃Cl

iii.CH₂Cl₂

iv.CHCl₃

v.CCl₄

A)i only

B)iii only

C)i and v

D)ii and iv

E)i, iii, and v

Q2) Which of the following compounds is an alcohol?

A)CH₃CH₃

B)CH₃OCH₂CH₂CH₃ C)CH₃COOH

D)HOCH₂CH₂OH E)None is an alcohol.

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Page 14

Chapter 14: The Ideal Gas Law and Its Applications

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Sample Questions

Q1) How does the volume of 3 × 10²² hydrogen molecules compare with the volume of 3 × 10²² helium atoms,when both are measured at the same temperature and pressure?

A)The volume of hydrogen is twice the volume of helium

B)The volume of helium is twice the volume of hydrogen

C)The volume of hydrogen is four times the volume of helium

D)The volume of helium is four times the volume of hydrogen

E)Both volumes are the same

Q2) Which of the following statements is incorrect?

i.The molar volume of a gas is the number of moles in one liter

ii.The molar volume of a gas is variable depending on temperature and pressure

iii.All gases have the same molar volume at the same temperature and pressure

A)All are correct

B)i only

C)ii only

D)iii only

E)ii and iii

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15

Chapter 15: Gases, Liquids, and Solids

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Sample Questions

Q1) Calculate the specific heat of an unknown metal if a 123 gram sample requires 8.8 kJ of heat to change from 16°C to 97°C.

A)0.88 J/g °C

B)1.1 J/g °C

C)5.8 × 10³ J/g °C

D)1.3 × 10⁴ J/g °C

E)8.8 × 10⁷ J/g °C

Q2) Predict the order in which boiling points of the following hydrides decrease (highest boiling point first,lowest last): PH₃,AsH₃,SbH₃ (As is atomic number 33; Sb is atomic number 51).

A)PH₃, AsH₃, SbH₃ B)AsH₃, SbH₃, PH₃ C)SbH₃, AsH₃, PH₃ D)PH₃, SbH₃, AsH₃ E)SbH₃, PH₃, AsH₃

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16

Chapter 16: Solutions

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Q1) Silver nitrate is commonly used to determine the chloride ion concentration in an aqueous solution.37.0 mL of 0.174 N AgNO₃ is required to titrate the chloride ion in a 20.0 mL sample of zinc chloride solution.What is the normality of the zinc chloride? 2 AgNO₃(aq)+ ZnCl₂(aq) 2 AgCl(s)+ Zn(NO₃)₂(aq)

A)0.0470 N

B)0.0941 N

C)0.161 N

D)0.322 N

E)0.644 N

Q2) What volume of 0.142 N hydrochloric acid will react with 10.00 mL of 0.117 N barium hydroxide?

A)12.14 mL

B)6.07 mL

C)8.24 mL

D)16.48 mL

E)10.00 mL

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Chapter 17: Acidbase Proton Transferreactions

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Q1) A solution is made by dissolving 0.0010 mole KOH in enough water to make 1.00 liter of solution.What are the pH and the pOH of the solution?

A)pH = 3, pOH = 11

B)pH = 3, pOH = 3

C)pH = -11, pOH = -3

D)pH = 11, pOH = 3

E)pH = 10^-11, pOH = 10^-3

Q2) Which of the following is a Lewis acid but not a Brønsted-Lowry acid?

A)OH^-

B)HPO₄^2-

C)HCl

D)NH₄⁺

E)Fe³⁺

Q3) What is the conjugate base of H₃C₆H₅O₇?

A)C₆H₅O₇^3-

B)H₂C₆H₅O₇^-

C)H₃C₆H₅O₇^-

D)H₄C₆H₅O₇⁺

E)H₃C₆H₅O₇(OH)^-

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Chapter 18: Chemical Equilibrium

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Q1) Which of the following statements does not correctly describe the character of a chemical equilibrium?

A)As a system comes to equilibrium, the chemical reactions come to a stop

B)In a liquid-gas equilibrium, the number of moles of the gas does not necessarily equal the number of moles of the liquid

C)In a solution equilibrium, the number of moles of the solvent does not necessarily equal the number of moles of the liquid

D)All of the statements above correctly describe a chemical equilibrium

E)None of the statements above correctly describes a chemical equilibrium

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

i.An object hanging motionless on a spring is in a static equilibrium

ii.In a dynamic equilibrium,the reversible changes occur continuously,even though there is no appearance of change

iii.The amounts of substances present in a system at equilibrium are equal

A)i only

B)ii only

C)iii only

D)i and ii

E)ii and iii

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Chapter 19: Oxidationreduction Electron Transferreactions

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Q1) Which of the following statements is incorrect?

A)Acid-base reactions involve a transfer of protons; redox reactions, a transfer of electrons

B)In both redox and acid-base reactions, the reactants are given special names to indicate their roles in the transfer process

C)Just as certain species can either donate or accept protons and thereby behave as an acid in one reaction and a base in another, certain species can either accept or donate electrons, acting as an oxidizing agent in one reaction and a reducing agent in another

D)Just as acids and bases may be classified as "strong" or "weak" depending on how readily they donate or accept protons, the strengths of oxidizing and reducing agents may be compared according to their tendencies to attract or release electrons

E)Unlike most acid-base reactions in aqueous solution, which reach a state of equilibrium, most aqueous redox reactions do not reach a state of equilibrium and proceed entirely in either the forward or reverse direction

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Chapter 20: Nuclear Chemistry

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Q1) Which of the following statements is/are correct?

i.A chain reaction is a reaction that has as a product one of its own reactants

ii.The critical mass of an element is the minimum mass necessary to react with a transuranium element

iii.A breeder reactor is a device whose purpose is to produce fissionable fuel from nonfissionable isotopes

A)i and iii

B)ii and iii

C)i and ii

D)All are correct

E)None is correct

Q2) Which of the following is the best description of a positron?

A)Positively charged electromagnetic radiation

B)A proton

C)A positive electron

D)A particle accelerator

E)An artificial element

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Chapter 21: Organic Chemistry

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Q1) What are the IUPAC and common names for the alkene with the molecular formula C₂H₄?

IUPAC name Common name

A)acetylene ethyne

B)ethyne acetylene

C)ethylene ethene

D)ethene ethylene

E)ethyne ethene

Q2) A certain compound is a gas at room temperature and undergoes only substitution reactions.Which of the following is most likely to be this compound?

A)C₄H₁₀

B)C₆H₁₀

C)C₇H₁₄

D)C₉H₁₈

E)Any of is a possibility

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22

Chapter 22: Biochemistry

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Q1) Which of the following correctly lists the three parts of a nucleotide found in DNA?

A)ribose, phosphate, uracil

B)ribose, phosphate, thymine

C)deoxyribose, phosphate, adenine

D)deoxyribose, phosphate, uracil

Q2) Which of the following monosaccharides combine to make the disaccharide sucrose?

i.Glucose

ii.Fructose

iii.Ribose

iv.Galactose

A)i and ii

B)i and iii

C)i and iv

D)ii and iii

E)ii and iv

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