Physical Science with Chemistry Exam Solutions - 3674 Verified Questions

Physical Science with Chemistry

Exam Solutions

Course Introduction

Physical Science with Chemistry is an introductory course designed to provide students with a foundational understanding of the core concepts in physical science, with a special focus on chemistry. The course explores the principles of matter and energy, atomic and molecular structure, chemical bonding, reactions, and the properties of elements and compounds. Students will investigate scientific phenomena through laboratory experiments, problem-solving exercises, and real-world applications, developing critical thinking and scientific literacy. By the end of the course, students will have a comprehensive overview of how chemistry fits into the broader field of physical science and its relevance to everyday life.

Recommended Textbook

Chemistry The Central Science 14th Edition by Theodore E. Brown

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24 Chapters

3674 Verified Questions

3674 Flashcards

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Chapter 1: Introduction: Matter, energy, and Measurement

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Sample Questions

Q1) The quantity 1.0 mg/cm²is the same as 1.0 × ________

kg/m².

A)10^-4

B)10²

C)10^-6

D)10^-2

E)10⁴

Answer: D

Q2) A separation process that depends on differing abilities of substances to form gases is called ________.

A)filtration

B)solvation

C)distillation

D)chromatography

E)All of the above are correct.

Answer: C

Q3) There are 6 significant figures in the number 0.003702.

A)True

B)False

Answer: False

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) The gold foil experiment performed in Rutherford's lab ________.

A)confirmed the plum-pudding model of the atom

B)led to the discovery of the atomic nucleus

C)was the basis for Thomson's model of the atom

D)utilized the deflection of beta particles by gold foil

E)proved the law of multiple proportions

Answer: B

Q2) The correct name for CCl₄ is ________.

A)carbon chloride

B)carbon tetrachlorate

C)carbon perchlorate

D)carbon tetrachloride

E)carbon chlorate

Answer: D

Q3) The formula for potassium sulfide is ________. Answer: K₂S

Q4) The formula for chromium (II)iodide is CrI₂.

A)True

B)False

Answer: True

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Chapter 3: Chemical Reactions and Reaction Stoichiometry

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Sample Questions

Q1) Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO₃ (s) PbO (s)+ CO₂ (g)

If the reaction yield is 92.4%,how many grams of lead (II)oxide will be produced by the decomposition of 1.30 g of lead (II)carbonate?

A)1.00

B)1.18

C)1.20

D)1.09

E)1.41

Answer: A

Q2) Combustion of a 0.9827-g sample of a compound containing only carbon,hydrogen,and oxygen produced 1.900 g of CO₂ and 1.070 g of H₂O.What is the empirical formula of the compound?

A)C₂H₅O

B)C₅H₇O₃

C)C₄H₁₁O₂

D)C₄H₁₀O

E)C₂H₅O₂

Answer: C

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Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) Zinc is more active than cobalt and iron but less active than aluminum.Cobalt is more active than nickel but less active than iron.Which of the following correctly lists the elements in order of increasing activity?

A)Co < Ni < Fe < Zn < Al

B)Ni < Fe < Co < Zn < Al

C)Ni < Co < Fe < Zn < Al

D)Fe < Ni < Co < Al < Zn

E)Zn < Al < Co < Ni < Fe

Q2) What are the respective concentrations (M)of K⁺ and CO₃^2- afforded by dissolving 0.530 mol K₂CO₃ in water and diluting to 1.50 L?

A)0.707 and 0.353

B)0.118 and 0.353

C)0.353 and 0.707

D)0.353 and 0.353

E)0.707 and 0.707

Q3) The compound HClO₄ is a weak acid.

A)True

B)False

Q4) The solvent in an aqueous solution is ________.

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Chapter 5: Thermochemistry

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Sample Questions

Q1) Hydrogen gas and bromine gas react to form hydrogen bromide gas.How much heat (kJ)is released when 155 grams of HBr is formed in this reaction? H° = -72 kJ.

A)137

B)69

C)-69

D)-137

E)1.12 × 10⁵

Q2) A slice of cake contains 29.0 grams of fat,9.0 grams of protein,and 77 grams of carbohydrate.If swimming burns 1000.0 kJ/hour,how many minutes would it take to completely burn off the slice of cake? The respective fuel values for protein,fat,and carbohydrate are 17,38,and 17 kJ/g,respectively.

A)154

B)2.56

C)23.4

D)117

E)262

Q3) The H_rxnfor the combustion of methane is -890.0 kJ.How much heat energy (kJ)is released if 82.1 grams of methane are burned in an excess amount of oxygen?

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Page 7

Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a one-electron system (such as hydrogen)?

A)n, l, and m_l

B)n and l only

C)l and m_l

D)m_l only

E)n only

Q2) The element that has a valence configuration of 5s²5p⁶ is

A)Xe

B)Rn

C)Ne

D)Ar

E)Kr

Q3) The energy of a photon that has a wavelength of 9.0 m is ________ J.

A)2.2 × 10^-26

B)4.5 × 10²⁵

C)6.0 × 10^-23

D)2.7 × 10⁹

E)4.5 × 10^-25

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) Ozone is a a(n)________ of oxygen.

A)isotope

B)allotrope

C)precursor

D)peroxide

E)free radical

Q2) Which group 6A element is a metal?

A)tellurium and polonium

B)sulfur

C)selenium

D)tellurium

E)polonium

Q3) Of the following elements,________ has the most negative electron affinity.

A)S

B)Cl

C)Se

D)Br

E)I

Q4) Which noble gas has the highest first ionization energy?

Q5) Write a balanced equation for the reaction of sodium metal with water.

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) For ________ forms of a molecule or ion,the observed structure is an average of the ________ forms.

A)resonance, covalent

B)resonance, resonance

C)ionic, resonance

D)resonance, ionic

E)resonance, metallic

Q2) Lattice energy is ________.

A)the energy required to convert a mole of ionic solid into its constituent ions in the gas phase

B)the energy given off when gaseous ions combine to form one mole of an ionic solid

C)the energy required to produce one mole of an ionic compound from its constituent elements in their standard states

D)the sum of ionization energies of the components in an ionic solid

E)the sum of electron affinities of the components in an ionic solid

Q3) The strength of a ________ bond is measured by its bond enthalpy.

Q4) An exothermic reaction should have ________ chemical bonds and decompose to a molecule with ________ bonds.

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Page 10

Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) Three monosulfur fluorides are observed: SF₂,SF₄,and SF₆.Of these,________ is/are polar.

A)SF₂ only

B)SF₂ and SF₄ only

C)SF₄only

D)SF₆ only

E)SF₂, SF₄, and SF₆

Q2) Which of the following molecules would be expected to be attracted to a magnetic field?

F₂ N₂ O₂

A)F₂and N₂

B)F₂and O₂

C)O₂only

D)N₂only

E)N₂ and O₂

Q3) A covalent bond in which overlap regions lie above and below an internuclear axis is called a(n)________.

Q4) Three molecules have similar electron domains,but different molecular shapes.Why?

Q5) The ________ hydrogen orbital overlaps with the ________ bromide orbital in HBr.

11

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Chapter 10: Gases

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Sample Questions

Q1) A real gas will behave most like an ideal gas under conditions of ________.

A)high temperature and high pressure

B)high temperature and low pressure

C)low temperature and high pressure

D)low temperature and low pressure

E)STP

Q2) Which of the following gases would have a similar rate of effusion to CO at 350 K?

A)H₂

B)He

C)CO₂

D)N₂

E)NO₂

Q3) The first person to investigate the relationship between the pressure of a gas and its volume was ________.

A)Amadeo Avogadro

B)Lord Kelvin

C)Jacques Charles

D)Robert Boyle

E)Joseph Louis Gay-Lussac

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Page 12

Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) The ease with which the charge distribution in a molecule can be distorted by an external electrical field is called the ________.

A)electronegativity

B)hydrogen bonding

C)polarizability

D)volatility

E)viscosity

Q2) Which molecule has hydrogen bonding as the predominant intermolecular force?

A)CH₄

B)C₆H₆

C)CH₃OH

D)CO₂

E)C₄H₁₀

Q3) Molecules containing many double bonds do not exhibit liquid-crystal behavior because free rotation can occur only around single bonds making these molecules rigid.

A)True

B)False

Q4) London Dispersion Forces tend to ________ in strength with increasing molecular weight.

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) All of the following can form a solid with a lattice structure similar to that of sodium chloride except ________.

A)NaF

B)CuBr₂

C)LiCl

D)KI

E)MgO

Q2) All of the following are polymers except ________.

A)nylon

B)cellulose

C)bronze

D)starch

E)protein

Q3) Define a face-centered cubic lattice.

Q4) Which of the following can be used as an elemental semiconductor?

A)Au

B)H

C)Ge

D)Li

E)Ne

Page 14

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) Which one of the following substances is more likely to dissolve in benzene (C₆H₆)?

A)CH₃CH₂OH

B)NH₃

C)NaCl

D)CCl₄

E)HBr

Q2) Of the concentration units below,only ________ uses kg of solvent in its calculation.

A)mass %

B)ppm

C)ppb

D)molarity

E)molality

Q3) Which produces the greatest number of ions when one mole dissolves in water?

A)Na₃PO₄

B)KBr

C)NaMnO₄

D)NH₄Cl

E)glucose

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) The reaction 2NOBr (g) 2 NO (g)+ Br₂ (g) Is a second-order reaction with a rate constant of 0.80 M^-1s^-1at 11 °C.If the initial concentration of NOBr is 0.0440 M,the concentration of NOBr after 6.0 seconds is ________.

A)0.0276 M

B)0.0324 M

C)0.0363 M

D)0.0348 M

E)0.0402 M

Q2) The half-life for a first order rate law depends on the starting concentration.

A)True

B)False

Q3) ________ are used in automotive catalytic converters.

A)Heterogeneous catalysts

B)Homogeneous catalysts

C)Enzymes

D)Noble gases

E)Nonmetal oxides

Q4) Define a homogeneous catalyst.

Q5) Define Beer's Law.

Page 16

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Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) In the coal-gasification process,carbon monoxide reacts with water to produce carbon dioxide and hydrogen gas.In an experiment,0.35 mol of CO and 0.40 mol of H₂O were placed in a 1.00-L reaction vessel.At equilibrium,there were 0.22 mol of CO remaining.K_eq at the temperature of the experiment is

A)5.5

B)0.28

C)0.75

D)3.5

E)1.0

Q2) If the reaction quotient Q for a reaction is equal to the value of the equilibrium constant K for that reaction at a given temperature,then the reaction is at ________.

Q3) Define the reaction quotient.

Q4) The equilibrium-constant expression depends on the ________ of the reaction.

A)stoichiometry

B)mechanism

C)stoichiometry and mechanism

D)the quantities of reactants and products initially present

E)temperature

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) Which solution will be the most basic?

A)0.10 M Ba(OH)₂

B)0.10 M KOH

C)0.10 M H₂O

D)0.10 M CH₃OH

E)All solutions have equal basicity.

Q2) A 0.14 M aqueous solution of the weak acid HA at 25.0 °C has a pH of 3.15.The value of K_a for HA is ________.

A)7.08 × 10^-4

B)3.58 × 10^-6

C)5.01 × 10^-7

D)7.02 × 10^-8

E)none of the above

Q3) What is the pOH of a sodium fluoride solution prepared by adding 0.4198 grams of sodium fluoride to 100.0 ml of water at 25.0 °C?

The K_a at 25.0 °C for HF is 7.2 × 10^-4.

Q4) The pOH of a 0.25 M aqueous solution of HA at 25.0 °C is 9.52.What is the value of K_a for HA?

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Chapter 17: Additional Aspects of Aqueous Equilibria

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Sample Questions

Q1) Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH.What is the final pH?

The K_a of HA is 1.77 × 10^-5.

Q2) What is the primary buffer system that controls the pH of the blood?

A)carbonate, bicarbonate

B)carbon dioxide, carbonate

C)carbonic acid, bicarbonate

D)carbonic acid, carbon dioxide

E)carbonate, carbonic acid

Q3) Suppose you have just added 100.0 ml of a solution containing 1.00 mole of acetic acid per liter to 500.0 ml of 0.100 M KOH.What is the final pH?

The K_a of acetic acid is 1.77 × 10^-5.

Q4) Which one of the following is not amphoteric?

A)Al(OH)₃

B)Ca(OH)₂

C)Cr(OH)₃

D)Zn(OH)₂

E)Sn(OH)₂

Q5) A complex ion is when a metal ion binds to a ________.

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) Of the noble gases,________ is present in highest concentration in dry air at sea level.

A)Ne

B)He

C)Xe

D)Kr

E)Ar

Q2) What are the primary chemical pollutants that create acid rain?

Q3) The principal component of smog is sulfur dioxide.

A)True

B)False

Q4) The amount of atomic O relative to O₂ ________.

A)is highest in the troposphere

B)is highest in the stratosphere

C)increases with altitude in the thermosphere

D)decreases with altitude in the thermosphere

E)is essentially independent of altitude in the thermosphere

Q5) In the equation below,what is the meaning of the asterisk?

O + O₂ O₃*

Q6) The three most concentrated ions in seawater are ________.

Page 20

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Chapter 19: Chemical Thermodynamics

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Sample Questions

Q1) The value of H° for the formation of phosphorous trichloride from its constituent elements, P₂ (g)+ 3Cl₂ (g) 2PCl₃(g)

Is ________ kJ/mol

A)-288.1

B)+432.4

C)-720.5

D)+720.5

E)-432.4

Q2) The value of S° for the decomposition of gaseous sulfur trioxide to solid elemental sulfur and gaseous oxygen, 2SO₃ (g) 2S (s,rhombic)+ 3O₂ (g) Is ________ J/K mol.

A)+19.3

B)-19.3

C)+493.1

D)+166.4

E)-493.1

Q3) A reversible change produces the maximum amount of ________ that can be achieved by the system on the surroundings.

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Page 21

Chapter 20: Electrochemistry

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Sample Questions

Q1) Which of the following reactions will occur spontaneously as written?

A)Sn⁴⁺ (aq)+ Fe³⁺ (aq) Sn²⁺ (aq)+ Fe²⁺ (aq)

B)3Fe (s)+ 2Cr³⁺ (aq) 2Cr (s)+ 3Fe²⁺ (aq)

C)Sn⁴⁺ (aq)+ Fe²⁺ (aq) Sn²⁺ (aq)+ Fe (s)

D)3Sn⁴⁺ (aq)+ 2Cr (s) 2Cr³⁺ (aq)+ 3Sn²⁺ (aq)

E)3Fe²⁺ (aq) Fe (s)+ 2Fe³⁺ (aq)

Q2) Which element is oxidized in the reaction below?

I^- + MnO₄^- + H⁺ I₂ + MnO₂ + H₂O

A)H

B)I

C)O

D)Mn

Q3) The amount of a substance that is reduced or oxidized is inversely proportional to the number of electrons produced in a cells half reaction.

A)True

B)False

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Page 22

Chapter 21: Nuclear Chemistry

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Sample Questions

Q1) Charged particles are accelerated because the faster they move there is a greater chance of producing a nuclear reaction.

A)True

B)False

Q2) Cesium-131 has a half-life of 9.7 days.What percent of a cesium-131 sample remains after 60 days?

A)100

B)0

C)1.4

D)98.6

E)more information is needed to solve the problem

Q3) At approximately what number of protons,or neutrons,does the 1:1 ratio of protons to neutrons start to produce unstable nuclei?

A)10

B)20

C)30

D)50

E)80

Q4) The use of radioisotopes in tracing metabolism is possible because ________.

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Chapter 22: Chemistry of the Nonmetals

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Q1) Oxides can react with water to form acids or bases.

A)True

B)False

Q2) How many oxygen atoms are bonded to each silicon atom in SiO₂?

A)1

B)2

C)3

D)4

E)none

Q3) The molecular shape of the PF₃ molecule is ________.

A)trigonal pyramidal

B)trigonal bipyramidal

C)see-saw

D)T-shaped

E)octahedral

Q4) Explain why silicon does not form any allotropes with structures analogous to that of graphite or buckminsterfullerenes,even though it is in the same group as carbon.

Q5) What process replenishes O₂?

Q6) What are the three steps in the Ostwald process of nitric acid synthesis?

Page 24

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Chapter 23: Transition Metals and Coordination Chemistry

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Sample Questions

Q1) Which one of the following is the correct formula for pentaamminechlorocobalt (III)chloride?

A)[Co(NH₃)₅Cl]Cl₂ B)[Co(NH₃)₄Cl]Cl₂ C)[Co(NH₃)₆Cl]Cl₂ D)[Co(NH₃)₅]Cl₄ E)[Cl(NH₃)₅Co]Co₂

Q2) Which of the following is not a chelating agent?

A)water

B)ethylenediamine

C)ortho-phenanthroline

D)carbonate ion

E)triphosphate ion

Q3) How many d electrons are associated with the metal ion in [Cr(NH₃)₃⁺?

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Chapter 24: The Chemistry of Life: Organic and Biological Chemistry

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Q1) Alcohols are hydrocarbon derivatives in which one or more hydrogens have been replaced by a hydroxyl functional group.________ is the general formula of an alcohol.

A)R-O-R

B)R-CO-R

C)R-CO-OH

D)R-OH

E)R-CO-H

Q2) Isooctane is assigned an octane number of 100,whereas ________ is assigned an octane number of 0.

A)methane

B)propane

C)benzene

D)heptane

E)nitrous oxide

Q3) The hydrolysis of an ester in the presence of a base is called ________.

Q4) The condensation reaction of a carboxyl group of one amino acid and the amino group of a second amino acid results in the formation of a(n)________.

Q5) Large protein molecules that act as catalysts are called ________.

Page 26

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