Physical Science Exam Bank - 3504 Verified Questions

Course Introduction

Physical Science Exam Bank

Physical Science is an introductory course that explores the fundamental principles and concepts underlying the physical world, including topics from physics, chemistry, astronomy, and earth sciences. Students will examine the nature and properties of matter and energy, the laws of motion, the structure of atoms, chemical reactions, and the basics of the universe and our planet. Through experiments, observations, and problem-solving activities, learners will develop scientific reasoning skills and an appreciation for the role of physical science in everyday life and various technological advancements.

Recommended Textbook

Chemistry The Central Science 12th Edition by Theodore

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24 Chapters

3504 Verified Questions

3504 Flashcards

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Page 2

E. Brown

Chapter 1: Introduction: Matter and Measurement

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Sample Questions

Q1) In the following list, only __________ is not an example of a chemical reaction.

A)burning a plastic water bottle

B)the production of hydrogen gas from water

C)the tarnishing of a copper penny

D)chopping a log into sawdust

E)charging a cellular phone

Answer: C

Q2) Which one of the following is an intensive property?

A)mass

B)temperature

C)heat content

D)volume

E)amount

Answer: B

Q3) 38.325 lbs = __________ grams. (1 lb = 454 g)

Answer: 17400

Q4) Temperature is a physical property that determines the direction of heat flow.

A)True

B)False

Answer: True

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Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al₂X₃. Element X must be from Group __________ of the Periodic Table of Elements.

A)3A

B)4A

C)5A

D)6A

E)7A

Answer: D

Q2) Which element forms an ion with the same charge as the ammonium ion?

A)potassium

B)chlorine

C)calcium

D)oxygen

E)nitrogen

Answer: A

Q3) The correct name for Na₃N is sodium azide.

A)True

B)False

Answer: False

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Chapter 3: Stoichiometry: Calculations With Chemical

Formulas and Equations

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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 95.7%, how many grams of lead (II)oxide will be produced by the decomposition of 2.50 g of lead (II)carbonate?

A)1.04

B)1.55

C)2.09

D)4.00

E)5.55

Answer: C

Q2) Which one of the following substances is the product of this combination reaction? Al (s)+ I₂ (s) __________

A)AlI₂

B)AlI

C)AlI₃

D)Al₂I₃

E)Al₃I₂

Answer: C

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Chapter 4: Aqueous Reactions and Solution Stoichiometry

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Sample Questions

Q1) Of the reactions below, only __________ is not spontaneous.

A)Mg (s)+ 2HCl (aq) MgCl₂ (aq)+ H₂ (g)

B)2Ag (s)+ 2HNO₃ (aq) 2AgNO₃ (aq)+ H₂ (g)

C)2Ni (s)+ H₂SO₄ (aq) Ni₂SO₄ (aq)+

H₂ (g)

D)2Al (s)+ 6HBr (aq) 2AlBr₃ (aq)+ 3 H₂ (g)

E)Zn (s)+ 2HI (aq) ZnI₂ (aq)+ H₂ (g)

Q2) Calculate the concentration (M)of arsenic acid (H₃AsO₄)in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization.

Q3) What are the respective concentrations (M)of K⁺ and PO₄^3- afforded by dissolving 0.800 mol K₃PO₄in water and diluting to 1.63 L?

A)0.800 and 0.800

B)0.491 and 0.491

C)0.800 and 0.491

D)1.44 and 0.491

E)0.489 and 0.163

Q4) How many moles of Co²⁺ are present in 0.150 L of a 0.200 M solution of CoI₂?

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Chapter 5: Thermochemistry

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Sample Questions

Q1) When a system __________, E is always negative.

A)absorbs heat and does work

B)gives off heat and does work

C)absorbs heat and has work done on it

D)gives off heat and has work done on it

E)none of the above is always negative.

Q2) The value of E for a system that performs 168 kJ of work on its surroundings and loses 79 kJ of heat is __________ kJ.

A)+247

B)-247

C)+55

D)-55

E)-168

Q3) The primary component of natural gas is propane.

A)True

B)False

Q4) The standard enthalpy change of a reaction is the enthalpy change when all reactants and products are at ________ pressure and a specific temperature.

Q5) __________ is defined as the energy used to move an object against a force.

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Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) Elements in group __________ have a np⁵ electron configuration in the outer shell.

Q2) An NMR spectrum results from photon irradiation in which the nuclear spin alignment is flipped.

A)True

B)False

Q3) A spectrum containing radiation of specific wavelengths is called a __________.

Q4) Calculate the energy (J)change associated with an electron transition from n = 2 to n = 5 in a Bohr hydrogen atom.

A)6.5 × 10^-19

B)5.5 × 10^-19

C)8.7 × 10^-20

D)4.6 × 10^-1⁹

E)5.8 × 10^-53

Q5) Which one of the following configurations depicts an excited oxygen atom?

A)1s²2s²2p²

B)1s²2s²2p²3s²

C)1s²2s²2p¹

D)1s²2s²2p⁴

E)[He]2s²2p⁴

Page 8

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) All of the group VIA elements are solids except __________.

Q2) Sodium is much more apt to exist as a cation than is chlorine. This is because

A)chlorine is a gas and sodium is a solid

B)chlorine has a greater electron affinity than sodium does C)chlorine is bigger than sodium

D)chlorine has a greater ionization energy than sodium does E)chlorine is more metallic than sodium

Q3) Transition metals within a period differ mainly in the number of ________ electrons.

A)s

B)p

C)d

D)f

E)all of the above

Q4) A group of ions all containing the same number of electrons constitute an isoelectronic series.

A)True

B)False

Q5) Complete the following : P₄O₁₀ + 6 H₂O

Page 9

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) Given the electronegativities below, which covalent single bond is most polar?

Element: H C N O

Electronegativity: 2.1 2.5 3.0 3.5

A)C-H

B)N-H

C)O-H

D)O-C

E)O-N

Q2) The central atom in __________ violates the octet rule.

A)NH₃

B)SeF₂

C)BF₃

D)AsF₃

E)CF₄

Q3) Of the atoms below, __________ is the least electronegative. A)Ba B)Be C)Mg

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Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) The hybridization of orbitals on the central atom in a molecule is sp. The electron-domain geometry around this central atom is __________.

A)octahedral

B)linear

C)trigonal planar

D)trigonal bipyramidal

E)tetrahedral

Q2) According to MO theory, overlap of two p atomic orbitals produces __________.

A)one MO and one ^* MO

B)one MO and one MO

C)one MO and one ^* MO or one MO and one ^* MO

D)one ⁺ MO and one ^* MO

E)two MOs, two ⁺ MOs, one MO, and one ^*MO

Q3) Each molecular orbital can accommodate, at most, two electrons with their spins paired. This is called the __________.

Q4) XeF₄ is a polar molecule.

A)True

B)False

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Chapter 10: Gases

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Sample Questions

Q1) A sample of oxygen gas was found to effuse at a rate equal to two times that of an unknown gas. The molecular weight of the unknown gas is __________ g/mol.

A)64

B)128

C)8

D)16

E)8.0

Q2) SO₂ (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0°C. The total pressure in the container was __________ atm.

A)0.192

B)4.02

C)2.76

D)6.78

E)1.60

Q3) What is the density (in g/L)of oxygen gas at 77.0°C and 700.0 torr?

Q4) The effusion rate of a gas is proportional to the square root of its molar mass.

A)True

B)False

Q5) Abnormally high blood pressure is called __________.

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) The initial discovery of a liquid crystal resulted from studies on what compound?

Q2) Of the following substances, __________ has the highest boiling point.

A)H₂O

B)CO₂

C)CH₄

D)Kr

E)NH₃

Q3) Which type of liquid crystal is colored and changes color with temperature?

A)nematic

B)smectic A

C)cholesteric

D)smectic B

E)smectic C

Q4) Which of the following has dispersion forces as its only intermolecular force?

A)CH₄

B)HCl

C)C₆H₁₃NH₂

D)NaCl

E)CH₃Cl

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) Which of the following is not an alloy?

A)brass

B)steel

C)sterling silver

D)dental amalgam

E)ceramic

Q2) Silicon technology is based on the fact that silicon oxide is a chemically stable conductor.

A)True

B)False

Q3) Inorganic compounds that are semiconductors have an average of __________ valence electrons.

A)1

B)2

C)3

D)4

E)5

Q4) __________ are solid-state materials that can be made either semiconducting or metallic without any doping.

Q5) How many atoms are contained in a face-centered cubic unit cell?

Page 14

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) The ideal value of i (van't Hoff factor)for (NH₄)₃PO₄.

A)1

B)2

C)3

D)4

E)5

Q2) A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl^- in this solution is __________ M.

A)0.214

B)0.562

C)1.12

D)1.20

E)6.64 × 10^-2

Q3) A solution with a solute concentration greater than the solubility is called a supercritical solution.

A)True

B)False

Q4) The formula weight of FeCl₃^.6H₂O is

Page 15

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) The relationship of absorbed light to the concentration of the substance absorbing the light is governed by __________.

Q2) Of the following, all are valid units for a reaction rate except __________.

A)mol/L

B)M/s

C)mol/hr

D)g/s

E)mol/L-hr

Q3) The rate law for a reaction is rate = k [A][B]²

Which one of the following statements is false?

A)The reaction is first order in A.

B)The reaction is second order in B.

C)The reaction is second order overall.

D)k is the reaction rate constant

E)If [B] is doubled, the reaction rate will increase by a factor of 4.

Q4) Rates of reaction can be positive or negative.

A)True

B)False

Q5) A catalyst that is present in a different phase from the reacting molecules is called a __________ catalyst.

Page 16

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Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) The effect of a catalyst on an equilibrium is to __________.

A)increase the rate of the forward reaction only

B)increase the equilibrium constant so that products are favored

C)slow the reverse reaction only

D)increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture

E)shift the equilibrium to the right

Q2) If the reaction quotient Q for a reaction is less than the value of the equilibrium constant K for that reaction at a given temperature, __________ must be converted to __________ for the system to reach equilibrium.

Q3) If a reaction is endothermic, __________ the reaction temperature results in an increase in K.

Q4) The number obtained by substituting starting reactant and product concentrations into an equilibrium-constant expression is known as the __________.

Q5) For an exothermic reaction, increasing the reaction temperature results in a(an)__________ in K.

Q6) Pure __________ and pure __________ are excluded from equilibrium-constant expressions.

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) According to the Arrhenius concept, an acid is a substance that __________.

A)is capable of donating one or more H⁺

B)causes an increase in the concentration of H⁺ in aqueous solutions

C)can accept a pair of electrons to form a coordinate covalent bond

D)reacts with the solvent to form the cation formed by autoionization of that solvent

E)tastes bitter

Q2) The pH of a 0.30 M solution of a weak acid is 2.67. What is the K_a for this acid?

A)2.1 × 10^-⁴

B)4.4 × 10^-⁴

C)1.5 × 10^-⁴

D)6.6 × 10^-⁴

E)none of the above

Q3) Which of the following ions will act as a weak base in water?

A)OH^-

B)Cl^-

C)NO₃^-

D)ClO^-

E)None of the above will act as a weak base in water.

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Chapter 17: Additional Aspects of Aqueous Equilibria

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Sample Questions

Q1) A solution containing which one of the following pairs of substances will be a buffer solution?

A)KI, HI

B)AgBr, HBr

C)CuCl, HCl

D)CsI, HI

E)none of the above

Q2) Human blood is __________.

A)neutral

B)very basic

C)slightly acidic

D)very acidic

E)slightly basic

Q3) Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The K_a of acetic acid is 1.77 × 10^-5.

Q4) Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) The C-Cl and C-F bond dissociation energies in CF₃Cl are 339 kJ/mol and 482 kJ/mol, respectively. The maximum wavelengths of electromagnetic radiation required to rupture these bonds are __________ and __________, respectively.

A)45.0 nm, 307 nm

B)742 nm, 654 nm

C)482 nm, 248 nm

D)353 nm, 248 nm

E)979 nm, 953 nm

Q2) The fourth most abundant component of dry air is __________.

Q3) Nitrogen oxides catalytically destroy ozone.

A)True

B)False

Q4) The pressure of the atmosphere __________.

A)increases with altitude

B)follows the same trend as temperature

C)decreases with altitude

D)follows the reverse trend as temperature

E)stays the same

Q5) The contribution of sulfur to acid rain is via the production of __________.

Page 20

Q6) Describe the process of reverse osmosis that is used to desalinate seawater.

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Chapter 19: Chemical Thermodynamics

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Sample Questions

Q1) The more negative G° is for a given reaction, the larger the value of the corresponding equilibrium constant, K.

A)True

B)False

Q2) S is positive for the reaction __________.

A)2NO (g)+ O₂ (g) 2NO₂ (g)

B)2N₂ (g)+ 3H₂ (g) 2 NH₃ (g)

C)C₃H₈ (g)+ 5 O₂ (g) 3CO₂ (g)+ 4 H₂O (g)

D)Mg (s)+ Cl₂ (g) MgCl₂ (s) E)C₂H₄ (g)+ H₂ (g) C₂H₆ (g)

Q3) Calculate G°(in kJ/mol)for the following reaction at 1 atm and 25°C: C₂H₆ (g)+ O₂ (g) CO₂ (g)+ H₂O (l)(unbalanced)

G_f° C₂H₆ (g)= -32.89 kJ/mol; G_f°CO₂ (g)= -394.4 kJ/mol; G_f° H₂O (l)= -237.13 kJ/mol

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Page 21

Chapter 20: Electrochemistry

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Sample Questions

Q1) Which substance is the reducing agent in the reaction below? Pb + PbO₂ + 2H₂SO₄ 2PbSO₄ + 2H₂O

A)Pb

B)H₂SO₄

C)PbO₂

D)PbSO₄

E)H₂O

Q2) Which of the following reactions will occur spontaneously as written?

A)Sn⁴⁺ (aq)+

Fe²⁺ (aq)

Fe³⁺ (aq)

Sn²⁺ (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)

Q3) What is the oxidation number of potassium in KMnO₄?

A)0

B)+1

C)+2

D)-1

E)+3

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Chapter 21: Nuclear Chemistry

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Sample Questions

Q1) The half-life of cobalt-60 is 5.20 yr. How many milligrams of a 2.000-mg sample remains after 6.55 years?

A)0.837

B)3.23 × 10^-15

C)4.779

D)1.588

E)1.163

Q2) The relative biological effectiveness (RBE)values of beta rays, gamma rays, and alpha rays are, respectively

Q3) On average, __________ neutrons are produced by every fission of a uranium-235 nucleus.

A)4

B)3.5

C)1

D)2.4

E)2

Q4) Carbon-11, fluorine-18, oxygen-15 and nitrogen-13 are all used in the clinical diagnostic technique known as __________.

Q5) What isotope of what element is produced if krypton-81 undergoes beta decay?

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Chapter 22: Chemistry of the Nonmetals

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Sample Questions

Q1) In the following chemical equation Na₃P + 3H₂O

The products (when the equation is balanced)are

A)H₂PO₃ + 3NaH

B)NaOH + 3PH

C)3NaH + POH₃

D)3NaO + PH₆

E)3NaOH + PH₃

Q2) Which pair of formula/name is incorrect?

A)NO / nitric oxide

B)N₂O / nitrous oxide

C)NO₂ / nitrogen dioxide

D)N₂O₄ / dinitrogen trioxide

E)N₂O₅ / dinitrogen pentoxide

Q3) The least electronegative of the elements below is __________.

A)I

B)Cl

C)H

D)F

E)Br

Q4) Compounds containing only boron and hydrogen are called __________.

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Chapter 23: Transition Metals and Coordination Chemistry

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Sample Questions

Q1) What is the most common geometry found in four-coordinate complexes?

A)square planar

B)octahedral

C)tetrahedral

D)icosahedral

E)trigonal bipyramidal

Q2) What is the oxidation number of chromium in [Cr(NH₃)₄Cl₂]Cl?

A)-3

B)+3

C)+2

D)-2

E)0

Q3) How can high-spin and low-spin transition metal complexes be distinguished from each other?

Q4) In the leaves of plants, visible light is absorbed by a compound known as __________, and is aided by a __________ ion bonded to a porphyrin ring.

Q5) Define the chelate effect.

Q6) A compound that can occupy two coordination sites is a (an)__________.

Page 25

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

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Q1) The compound below is an __________. H-C=CH-CH₃

A)alkyne

B)alkene

C)alkane

D)aromatic compound

E)olefin

Q2) What forces hold the strands of DNA together?

A)covalent bonds

B)hydrogen bonding

C)ion-dipole attraction

D)coordinate covalent bonds

Q3) __________ is a monosaccharide.

A)Sucrose

B)Maltose

C)Glucose

D)Lactose

Q4) The anaerobic conversion of carbohydrates to ethanol is driven by the presence of

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Q5) In the reaction of nitric acid with benzene, which isomer is formed when a second nitro group is substituted?