Chemistry for Health Sciences Mock Exam - 3150 Verified Questions

Chemistry for Health Sciences

Mock Exam

Course Introduction

Chemistry for Health Sciences is designed to provide students with a foundational understanding of key chemical principles as they relate to the human body and healthcare. The course covers essential topics such as atomic structure, chemical bonding, solutions, acids and bases, chemical reactions, and the properties of biomolecules. Emphasis is placed on biochemical processes, drug action, and the chemical basis of physiological functions relevant to nursing, allied health, and pre-medical fields. Through lectures, laboratory experiments, and real-world examples, students will develop the skills necessary to apply chemical concepts to health-related scenarios and appreciate the vital role of chemistry in medical and health professions.

Recommended Textbook Chemistry 12th Edition by Raymond Chang

Available Study Resources on Quizplus

25 Chapters

3150 Verified Questions

3150 Flashcards

Source URL: https://quizplus.com/study-set/2995 Page 2

Chapter 1: Chemistry: The Study of Change

Available Study Resources on Quizplus for this Chatper

175 Verified Questions

175 Flashcards

Source URL: https://quizplus.com/quiz/59562

Sample Questions

Q1) How many square kilometers are equivalent to 28.5 cm²

A) 2.85 * 10^-9 km²

B) 2.85 * 10^-6 km²

C) 285 km²

D) 2.85 * 10^-4 km²

E) none of these

Answer: A

Q2) 16 megagrams (Mg) is equal to 1.6 * 10⁷ g.

A)True

B)False

Answer: True

Q3) The SI prefixes kilo and milli represent, respectively:

A) 10^-9 and 10^-6

B) 10⁶ and 10^-3

C) 10³ and 10^-3

D) 10⁹ and 10^-6

E) 10^-9 and 10^-1

Answer: C

To view all questions and flashcards with answers, click on the resource link above.

3

Chapter 2: Atoms Molecules and Ions

Available Study Resources on Quizplus for this Chatper

156 Verified Questions

156 Flashcards

Source URL: https://quizplus.com/quiz/59561

Sample Questions

Q1) Which of the following is the formula for hydroiodic acid

A) HIO₄

B) HIO₃

C) HIO₂

D) HIO

E) HI

Answer: E

Q2) What type of compound is HBrO₂

A) Ionic

B) Binary

C) Acid

D) Base

E) Hydrate

Answer: C

Q3) The correct name of the compound CH₃CH₂OH is ethanol.

A)True

B)False

Answer: True

Q4) What are the two different ions present in the compound FeCl₃

Answer: \(Fe^{2+}, Cl^-\)

Page 4

To view all questions and flashcards with answers, click on the resource link above.

Chapter 3: Mass Relationships in Chemical Reactions

Available Study Resources on Quizplus for this Chatper

194 Verified Questions

194 Flashcards

Source URL: https://quizplus.com/quiz/59560

Sample Questions

Q1) How many ICl₃ molecules are present in 1.75 kg of ICl₃

A) 4.22 x 10²³

B) 3.59 x 10²⁴

C) 4.12 x 10²⁴

D) 4.52 x 10²⁴

E) None of the above

Answer: D

Q2) What is the average mass, in grams, of one Rb atom

A) 6.02 x 10²³ g

B) 1.42 x 10^-22g

C) 5.15 x 10²⁵ g

D) 85.47 g

E) 85.47 amu

Answer: B

Q3) The definition of a mole is an Avogadro's number of a specific entity, such as an atom or molecule.

A)True

B)False

Answer: True

To view all questions and flashcards with answers, click on the resource link above.

Page 5

Chapter 4: Reactions in Aqueous Solutions

Available Study Resources on Quizplus for this Chatper

192 Verified Questions

192 Flashcards

Source URL: https://quizplus.com/quiz/59559

Sample Questions

Q1) Identify the oxidizing agent in the following chemical reaction. 2MnO₄^- + 5H₂SO₃ \(\rarr\) 2Mn²⁺ + 5SO₄^2- + 4H⁺ + 3H₂O

A) MnO₄^-

B) H₂SO₃

C) Mn²⁺

D) SO₄^2-

E) H⁺

Q2) The following net ionic equation correctly shows the result when a piece of zinc metal is added to an aqueous solution of lead(II) nitrate. After some time it was observed that the zinc metal appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel.

Zn(s) + Pb²⁺(aq) \(\rarr\)Zn²⁺(aq) + Pb(s)

A)True

B)False

Q3) H₂CO₃ is an example of a diproticacid.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above.

Page 6

Chapter 5: Gases

Available Study Resources on Quizplus for this Chatper

130 Verified Questions

130 Flashcards

Source URL: https://quizplus.com/quiz/59558

Sample Questions

Q1) The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

A) pressure.

B) temperature.

C) volume.

D) density.

Q2) Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100. cm³ at 95^\(\circ\)C, and 1,000. mmHg.

A) 0.19 g/mol

B) 35.3 g/mol

C) 70.9 g/mol

D) 137 g/mol

E) 384 g/mol

Q3) Dalton's Law states that the total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above. Page 7

Chapter 6: Thermochemistry

Available Study Resources on Quizplus for this Chatper

119 Verified Questions

119 Flashcards

Source URL: https://quizplus.com/quiz/59557

Sample Questions

Q1) Calculate the amount of heat necessary to raise the temperature of 135.0 g of water from 50.4^\(\circ\)F to 85.0^\(\circ\)F. The specific heat of water = 4.184 J/g·^\(\circ\)C.

A) 1.1 kJ

B) 10.9 kJ

C) 16.6 kJ

D) 19.5 kJ

E) 48.0 kJ

Q2) If 10.6 moles of water at 35^\(\circ\)C absorbs 12.30 kJ, what is the final temperature of the water The specific heat of water is 4.184 J/g·^\(\circ\)C.

A) 15^\(\circ\)C

B) 20^\(\circ\)C

C) 35^\(\circ\)C

D) 50.^\(\circ\)C

E) 312^\(\circ\)C

Q3) The heat capacity of 10.0 g of water is 83.7 J/^\(\circ\)C.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above. Page 8

Chapter 7: Quantum Theory and the Electronic Structure of Atoms

Available Study Resources on Quizplus for this Chatper

135 Verified Questions

135 Flashcards

Source URL: https://quizplus.com/quiz/59556

Sample Questions

Q1) The following set of quantum numbers is correct.n = 3, l = 3, m_l = 0, m_s = +1/2

A)True

B)False

Q2) How many unpaired electrons does an atom of carbon have in its ground state

A) 0

B) 1

C) 2

D) 3

E) 4

Q3) Which one of the following sets of quantum numbers is not possible \(\begin{array}{lrrr}

~~~~~\text { n } & \text { l } & \mathrm{m}_{l} & \mathrm{~m}_{\mathrm{s}} \\

\text { A. } 4 & 3 & -2 & +1 / 2 \\

\text { B. } 3 & 0 & 1 & -1 / 2 \\

\text { C. } 3 & 0 & 0 & +1 / 2 \\

\text { D. } 2 & 1 & 1 & -1 / 2 \\

\text { E. } 2 & 0 & 0 & +1 / 2 \end{array}\)

Page 9

To view all questions and flashcards with answers, click on the resource link above.

Chapter 8: Periodic Relationships Among the Elements

Available Study Resources on Quizplus for this Chatper

144 Verified Questions

144 Flashcards

Source URL: https://quizplus.com/quiz/59555

Sample Questions

Q1) Consider the following reaction: 3Li + Z \(\rarr\)Li₃Z. What is the formula for the compound if we substitute sodium for lithium

A) NaZ

B) Na₂Z

C) NaZ₂

D) Na₃Z

E) NaZ₃

Q2) An element with the general electron configuration for its outermost electrons of ns²np¹ would be in which element group

A) 2A

B) 3A

C) 4A

D) 5A

E) 8A

Q3) The radii of ions are always smaller than the radii of the corresponding atoms of the same element.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above.

10

Chapter 9: Chemical Bonding I: Basic Concepts

Available Study Resources on Quizplus for this Chatper

136 Verified Questions

136 Flashcards

Source URL: https://quizplus.com/quiz/59554

Sample Questions

Q1) BeF₄^2- is called the fluoberyllate ion. The formal charge on the beryllium atom in this ion is

A) -2

B) -1

C) 0

D) +1

E) +2

Q2) The number of lone electron pairs in the N₂ molecule is ___.

A) 1

B) 2

C) 3

D) 4

E) 5

Q3) What is the formal charge on the singly bonded oxygens in the Lewis structure for the carbonate ion

A) -2

B) -1

C) 0

D) +1

E) +2

To view all questions and flashcards with answers, click on the resource link above. Page 11

Chapter 10: Chemical Bonding II: Molecular Geometry and Hybridization

of Atomic

Available Study Resources on Quizplus for this Chatper

146 Verified Questions

146 Flashcards

Source URL: https://quizplus.com/quiz/59553

Sample Questions

Q1) The geometrical structure of PF₅ and IF₅ are both square pyramidal.

A)True

B)False

Q2) Which one of the following molecules is polar

A) PBr₅

B) CCl₄

C) BrF₅

D) XeF₂

E) XeF₄

Q3) The geometry of the ClF₃ molecule is best described as:

A) distorted tetrahedron

B) trigonal planar

C) tetrahedral

D) T-shaped

E) trigonal pyramidal

Q4) In VSEPR theory the molecular geometry of SF₄ (sulfur tetrafluoride) is distorted tetrahedron (seesaw).

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above. Page 12

Chapter 11: Intermolecular Forces and Liquids and Solids

Available Study Resources on Quizplus for this Chatper

149 Verified Questions

149 Flashcards

Source URL: https://quizplus.com/quiz/59552

Sample Questions

Q1) Which of the following properties is not influenced by hydrogen bonding

A) melting point

B) boiling point

C) vapor pressure

D) viscosity

E) flammability

Q2) Which of the following would be expected to have the lowest vapor pressure at room temperature

A) ethanol, bp = 78^\(\circ\)C

B) methanol, bp = 65^\(\circ\)C

C) water, bp = 100^\(\circ\)C

D) acetone, bp = 56^\(\circ\)C

Q3) Indicate all the types of intermolecular forces of attraction in He(l).

A) Dispersion and Dipole-dipole

B) Dipole-dipole and Ionic

C) Ion-dipole and Hydrogen bonding

D) Hydrogen bonding and Dispersion

E) Dispersion

To view all questions and flashcards with answers, click on the resource link above. Page 13

Chapter 12: Physical Properties of Solutions

Available Study Resources on Quizplus for this Chatper

122 Verified Questions

122 Flashcards

Source URL: https://quizplus.com/quiz/59551

Sample Questions

Q1) What is the percent by mass of a Na₂SO₄ solution in water with a mole fraction of Na₂SO₄, X = 0.350

A) 2.76%

B) 4.25%

C) 19.1%

D) 73.4 %

E) 80.9%

Q2) To interconvert the concentration units of molarity (M) and mass percent, you must also know the density of the solution.

A)True

B)False

Q3) Which of the following aqueous solutions has the highest osmotic pressure at 25^\(\circ\)C (assume 100% dissociation for all soluble ionic compounds)

A) 0.15m K₃PO₄

B) 0.20m KI

C) 0.25m K₂CO₃

D) 0.30m NH₄NO₃

E) 0.45m C₁₂H₂₂O₁₁

To view all questions and flashcards with answers, click on the resource link above. Page 14

Chapter 13: Chemical Kinetics

Available Study Resources on Quizplus for this Chatper

131 Verified Questions

131 Flashcards

Source URL: https://quizplus.com/quiz/59550

Sample Questions

Q1) When the concentrations of reactant molecules are increased, the rate of reaction increases. The best explanation for this phenomenon is that as the reactant concentration increases,

A) the average kinetic energy of molecules increases.

B) the frequency of molecular collisions increases.

C) the rate constant increases.

D) the activation energy increases.

E) the order of reaction increases.

Q2) Given the rate law for a reaction, rate = k[A][B]², where rate is measured in units of M s^-1, what are the units for the rate constant k

A) M^-2s^-2

B) M^-1s

C) M^-2s

D) M²s

E) None of the above

Q3) In the reaction, 2N₂O \(\rarr\) 2N₂ + O₂, oxygen and nitrogen gases are formed at the same rate (mol/L·s).

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above.

Page 15

Chapter 14: Chemical Equilibrium

Available Study Resources on Quizplus for this Chatper

119 Verified Questions

119 Flashcards

Source URL: https://quizplus.com/quiz/59549

Sample Questions

Q1) When the following reaction is at equilibrium, which of these relationships is always true

2NOCl(g) \(\rightleftharpoons\) 2NO(g) + Cl₂(g)

A) [NO] [Cl₂] = [NOCl]

B) [NO]² [Cl₂] = [NOCl]²

C) [NOCl] = [NO]

D) 2[NO] = [Cl₂]

E) [NO]² [Cl₂] = K_c[NOCl]²

Q2) For the following reaction at equilibrium in a reaction vessel, which change will cause the Br₂ concentration to decrease 2NOBr(g) 2NO(g) + Br₂(g), \(\Delta\)Hº_rxn= 30 kJ/mol

A) Increase the temperature.

B) Remove some NO.

C) Add more NOBr.

D) Compress the gas mixture into a smaller volume.

E) Add a catalyst

Q3) For the reaction H₂(g) + I₂(g) 2HI(g), K_P = K_c.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above. Page 16

Chapter 15: Acids and Bases

Available Study Resources on Quizplus for this Chatper

178 Verified Questions

178 Flashcards

Source URL: https://quizplus.com/quiz/59548

Sample Questions

Q1) What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [K_a(HCN) = 4.9 * 10^-10]

A) 240 g

B) 0.032 g

C) 0.059 g

D) 0.94 g

E) 0.24 g

Q2) The hydrolysis of NH₄NO₂ will result in which of the following types of solutions given: (K_a(NH₄⁺) = 5.6 x 10^-10, K_b(NO₂^-) = 2.2 x 10^-11)

A) acidic, pH < 7

B) basic, pH > 7

C) neutral, pH = 7

Q3) In aqueous solutions at 25^\(\circ\)C, the sum of the ion concentrations ([H⁺] + [OH ^-]) equals 1 * 10 ^{- 14}.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above.

Page 17

Chapter 16: Acid-Base Equilibria and Solubility Equilibria

Available Study Resources on Quizplus for this Chatper

145 Verified Questions

145 Flashcards

Source URL: https://quizplus.com/quiz/59547

Sample Questions

Q1) At 25 ^\(\circ\)C, the base ionization constant for NH₃ is 1.8 * 10^-5. Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100. mL of 0.150 M ammonia.

A) 3.47

B) 8.73

C) 10.4

D) 12.3

E) None of the above

Q2) Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF₃ , K_sp = 6.6 * 10^-11.)

A) 0.023 M

B) 0.032 M

C) 7.7 * 10^-8 M

D) 2.9 * 10^-9 M

E) 6.9 * 10^-10 M

Q3) The solubility of a salt increases as its K_sp increases.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above.

Page 18

Chapter 17: Entropy Free Energy and Equilibrium

Available Study Resources on Quizplus for this Chatper

128 Verified Questions

128 Flashcards

Source URL: https://quizplus.com/quiz/59546

Sample Questions

Q1) The reaction SiO₂(s) + Pb(s) \(\rarr\) PbO₂(s) + Si(s) is spontaneous.

\(\Delta\)G^\(\circ\)_f (PbO₂) = -217 kJ/mol

\(\Delta\)G^\(\circ\)_f (SiO₂) = -856 kJ/mol

A)True

B)False

Q2) For a certain reaction, \(\Delta\)G^\(\circ\) = 87 kJ/mol, \(\Delta\)H^\(\circ\) = 100 kJ/mol at STP. At what temperature, in K, is the reaction at equilibrium, assuming that \(\Delta\)S^\(\circ\)and \(\Delta\)H^\(\circ\) are temperature-independent

A) 1,700 K

B) 1,900 K

C) 2,100 K

D) 2,300 K

E) None of the above

Q3) The entropy of a perfectly ordered crystalline substance at 0 K is 0 J/mol.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above.

19

Chapter 18: Electrochemistry

Available Study Resources on Quizplus for this Chatper

154 Verified Questions

154 Flashcards

Source URL: https://quizplus.com/quiz/59545

Sample Questions

Q1) Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge.

- a Fe electrode in 1.0 M FeCl₂ solution

- a Ni electrode in 1.0 M Ni(NO₃)₂ solution

When the cell is running spontaneously, which choice includes only true statements and no false ones

A) The nickel electrode loses mass and the nickel electrode is the cathode.

B) The nickel electrode gains mass and the nickel electrode is the cathode.

C) The iron electrode gains mass and the iron electrode is the anode.

D) The iron electrode loses mass and the iron electrode is the cathode.

Q2) Calculate \(\Delta\)G^\(\circ\) for the electrochemical cell Fe(s) | Fe²⁺(aq) || Sn⁴⁺(aq) | Sn²⁺(aq) | Pt(s).

A) -5.5 x 10¹ kJ/mol

B) -1.1 x 10² kJ/mol

C) 6.0 x 10¹ kJ/mol

D) 1.1 x 10⁵ kJ/mol

E) 1.2 x 10² kJ/mol

To view all questions and flashcards with answers, click on the resource link above. Page 20

Chapter 19: Nuclear Chemistry

Available Study Resources on Quizplus for this Chatper

128 Verified Questions

128 Flashcards

Source URL: https://quizplus.com/quiz/59544

Sample Questions

Q1) List the number of protons, neutrons, and nucleons (protons + neutrons), in that order, for an isotope with the symbol: \(^{137}_{~~55}\)Cs

A) 137, 55, 192

B) 55, 137, 192

C) 55, 82, 137

D) 82, 55, 137

E) 82, 137, 219

Q2) What fraction of radioactive atoms remains in a sample after five half-lives

A) zero

B) 1/6

C) 1/16

D) 1/32

E) 1/64

Q3) A typical radius of an atomic nucleus is about

A) 100 µm

B) 5000 mm

C) 100 nm

D) 5 * 10^-3 pm

E) 500 pm

To view all questions and flashcards with answers, click on the resource link above.

Page 21

Chapter 20: Chemistry in the Atmosphere

Available Study Resources on Quizplus for this Chatper

50 Verified Questions

50 Flashcards

Source URL: https://quizplus.com/quiz/59543

Sample Questions

Q1) The following balanced equation shows what happens to nitrogen dioxide in sunlight.NO₂(g) + hn \(\rarr\) NO(g) + O(g)

A)True

B)False

Q2) The steps in the reaction scheme for nitrogen fixation by lightening are as follow: N₂(g) + O₂(g) \(\underrightarrow{~~~~\text { lightening }~~~~}\) 2NO(g)

2NO(g) + O₂(g) \(\rarr\) 2NO₂(g)

2NO₂(g) + H₂O(l) \(\rarr\) HNO₂(aq) + HNO₃(aq)

A)True

B)False

Q3) Which one of the following reactions is an example of nitrogen fixation

A)N₂O₅(g) \(\rarr\)NO₃(g) + NO₂(g)

B)N₂(g) + O₂(g) \(\rarr\) 2NO(g)

C)3NO₂(g) + H₂O(l) \(\rarr\)2HNO₃(aq) + NO(g)

D)2NO(g) + O₂(g) \(\rarr\) 2NO₂(g)

E)2NH₃(g) \(\rarr\)3H₂(aq) + N₂(g)

To view all questions and flashcards with answers, click on the resource link above. Page 22

Chapter 21: Metallurgy and the Chemistry of Metals

Available Study Resources on Quizplus for this Chatper

63 Verified Questions

63 Flashcards

Source URL: https://quizplus.com/quiz/59542

Sample Questions

Q1) The naturally occurring form of a metal that is concentrated enough to allow economical recovery of the metal is known as

A) an element.

B) a mineral.

C) gangue.

D) an ore.

E) an amalgam.

Q2) Which of these elements when doped into silicon would give an n-type semiconductor

A) C

B) Ga

C) P

D) Ge

E) B

Q3) The following depicts a correctly balanced chemical equation illustrating roasting.2ZnS + 3O₂ \(\rarr\) 2ZnO + 2SO₂

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above. Page 23

Chapter 22: Nonmetallic Elements and Their Compounds

Available Study Resources on Quizplus for this Chatper

52 Verified Questions

52 Flashcards

Source URL: https://quizplus.com/quiz/59541

Sample Questions

Q1) When liquid phosphorus trichloride reacts with water, the products are

A) PCl₅ and H₃PO₄.

B) H₃PO₃ and Cl₂.

C) H₃PO₄ and HCl.

D) H₃PO₄ and Cl₂.

E) H₃PO₃ and HCl.

Q2) The bond energy of F₂ is unusually low, in comparison with the other halogens, due to the small size of the fluorine atom. Which of the following periodic properties is also unusually low in the case of fluorine

A) first ionization energy

B) electron affinity

C) electronegativity

D) diatomic bond length

E) ionic radius

Q3) What element is the most abundant by mass in Earth's crust

A) Fe

B) H

C) K

D) P

E) O

To view all questions and flashcards with answers, click on the resource link above. Page 24

Chapter 23: Transition Metals Chemistry and Coordination Compounds

Available Study Resources on Quizplus for this Chatper

92 Verified Questions

92 Flashcards

Source URL: https://quizplus.com/quiz/59540

Sample Questions

Q1) In the complex ion [Fe(CN)₆]^4-, the oxidation number of Fe is

A) +1.

B) +2.

C) +3.

D) -4.

E) +6.

Q2) In the complex ion [ML₆]ⁿ⁺, Mⁿ⁺ has seven d electrons and L is a weak field ligand. According to crystal field theory, the magnetic properties of the complex ion correspond to how many unpaired electrons

A) 0

B) 1

C) 2

D) 3

E) 5

Q3) The chemical formula of the dibromobis(oxalato)cobaltate(III) ion is:

[CoBr₂(C₂O₄)₂]^3-

A)True

B)False

Page 25

To view all questions and flashcards with answers, click on the resource link above.

Chapter 24: Organic Chemistry

Available Study Resources on Quizplus for this Chatper

66 Verified Questions

66 Flashcards

Source URL: https://quizplus.com/quiz/59539

Sample Questions

Q1) The alkane with six carbon atoms is called

A) butane.

B) hexane.

C) heptane.

D) butene.

E) none of these.

Q2) What is the name of the molecule

CH₃-(CH₂)₈-CH₃

A) hexane

B) heptane

C) octane

D) nonane

E) decane

Q3) Alkenes have the general formula

A) C_nH_2n-4.

B) C_nH_2n-2.

C) C_nH_2n.

D) C_nH_2n+2.

E) C_nH_2n+4.

To view all questions and flashcards with answers, click on the resource link above.

Page 26

Chapter 25: Synthetic and Natural Organic Polymers

Available Study Resources on Quizplus for this Chatper

46 Verified Questions

46 Flashcards

Source URL: https://quizplus.com/quiz/59538

Sample Questions

Q1) The intermolecular force between bases on the opposite strands of DNA responsible for its double-helical structure is

A) hydrogen bonding..

B) dispersion force..

C) covalent bonding.

D) ionic force

E) dipole-dipole force

Q2) The primary structure of a protein refers to the unique amino acid sequence of the polypeptide chain.

A)True

B)False

Q3) Proteins occurring in the b-pleated sheet structure

A) are relatively inelastic.

B) never occur in nature.

C) produce structurally weak materials.

D) contain no peptide bonds.

E) are not involved in hydrogen bonds.

Q4) Both DNA and RNA have double-helical structures.

A)True

B)False

Page 27

To view all questions and flashcards with answers, click on the resource link above.