Chemistry for Health Sciences Final Test Solutions - 3504 Verified Questions by Quizplus

Chemistry for Health Sciences

Final Test Solutions

Course Introduction

Chemistry for Health Sciences provides an introduction to the fundamental concepts of chemistry with a focus on their applications in health and medical contexts. Topics include structure and properties of matter, chemical bonding, reactions, acids and bases, solutions, and the role of chemistry in biological systems. The course emphasizes the relevance of chemistry to human health, including drug interactions, metabolic pathways, and diagnostic techniques, preparing students for further study in health-related fields. Laboratory components reinforce theoretical knowledge through hands-on experiments and real-life scenarios encountered in healthcare professions.

Recommended Textbook

Chemistry The Central Science 12th Edition by Theodore E. Brown

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24 Chapters

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Page 2

Chapter 1: Introduction: Matter and Measurement

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Sample Questions

Q1) Which of the following is not an exact number?

A)The number of seconds in a year.

B)The number of millimeters in a kilometer.

C)The number of liters in a gallon.

D)The number of centimeters in an inch.

E)The number of grams in a kilogram.

Answer: C

Q2) Which one of the following has the element name and symbol correctly matched?

A)S, sodium

B)Tn, tin

C)Fe, iron

D)N, neon

E)B, bromine

Answer: C

Q3) Mass and volume are often referred to as __________ properties of substances. Answer: extensive

Q4) Gases do not have a fixed __________ as they are able to be __________.

Answer: volume, compressed

Q5) Sn is the symbol for the element __________.

Answer: Tin

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Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) The correct name for HNO2 is __________.

A)nitrous acid

B)nitric acid

C)hydrogen nitrate

D)hyponitrous acid

E)pernitric acid

Answer: A

Q2) Which one of the following basic forces is so small that it has no chemical significance?

A)weak nuclear force

B)strong nuclear force

C)electromagnetism

D)gravity

E)Coulomb's law

Answer: D

Q3) Which element in Group IA is the most electropositive?

Answer: francium

Q4) What is the name of an alcohol derived from hexane? Answer: hexanol

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Chapter 3: Stoichiometry: Calculations With Chemical

Formulas and Equations

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Sample Questions

Q1) When a hydrocarbon burns in air, a component produced is?

A)oxygen

B)nitrogen

C)carbon

D)water

E)argon

Answer: D

Q2) Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO3 (aq)+ AlCl3 (aq) Al(NO3)3 (aq)+ 3AgCl (s)

What mass in grams of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of AlCl3?

A)17.6

B)4.22

C)24.9

D)3.56

E)11.9

Answer: D

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Chapter 4: Aqueous Reactions and Solution Stoichiometry

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Sample Questions

Q1) What mass (g)of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?

A)1.44

B)1.23

C)53.6

D)34.5

E)188

Q2) Oxidation cannot occur without __________.

A)acid

B)oxygen

C)water

D)air

E)reduction

Q3) The compound HClO4 is a weak acid.

A)True

B)False

Q4) What is the concentration (M)of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Q5) The solvent in an aqueous solution is __________.

Page 6

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Chapter 5: Thermochemistry

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Sample Questions

Q1) H for the reaction IF5 (g) IF3 (g)+ F2 (g) Is __________ kJ, give the data below.

IF (g)+ F2 (g) IF3 (g) H = -390 kJ

IF (g)+ 2 F2 (g) IF5 (g) H = -745 kJ

A)+355

B)-1135

C)+1135

D)+35

E)-35

Q2) What is the enthalpy change (in kJ)of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 7.80 °C? (The specific heat of the solution is 3.74 joules/gram-K.)

A)-7.43

B)-12.51

C)8.20

D)-9.12

E)6.51

Q3) One joule equals 1 kg m2/s2.

A)True

B)False

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Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) The de Broglie wavelength of an electron is 8.7 × 10-11 m. The mass of an electron is 9.1 × 10-31 kg. The velocity of this electron is __________ m/s.

A)8.4 × 10-3

B)1.2 × 10-7

C)6.9 × 10-5

D)8.4 × 106

Q2) The 3p subshell in the ground state of atomic silicon contains __________ electrons.

A)2

B)6

C)8

D)10

E)36

Q3) The uncertainty principle states that __________.

A)matter and energy are really the same thing

B)it is impossible to know anything with certainty

C)it is impossible to know the exact position and momentum of an electron

D)there can only be one uncertain digit in a reported number

E)it is impossible to know how many electrons there are in an atom

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Page 8

Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) Of the following metals, __________ exhibits multiple oxidation states.

A)Al

B)Cs

C)V

D)Ca

E)Na

Q2) Of the compounds below, __________ has the smallest ionic separation.

A)KF

B)K2S

C)RbCl

D)SrBr2

E)RbF

Q3) The ion with the largest diameter is __________.

A)Br-

B)Cl-

C)I-

D)F-

E)O2-

Q4) Of the alkaline earth metals, which two elements are the least reactive?

Q5) [Xe]6s2 is the electron configuration for __________.

Page 9

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) The ion NO- has __________ valence electrons.

A)15

B)14

C)16

D)10

E)12

Q2) Using the Born-Haber cycle, the Hf° of KBr is equal to __________.

A) Hf°[K (g)] + Hf°[Br (g)] + Il(K)+ E(Br)+ Hlattice

B) Hf°[K (g)] - Hf°[Br (g)] - Il(K)- E(Br)Hlattice

C) Hf°[K (g)] - Hf°[Br (g)] + Il(K)- E(Br)+ Hlattice

D) Hf°[K (g)] + Hf°[Br (g)] - Il - E(Br)+ Hlattice

E) Hf°[K (g)] + Hf°[Br (g)] + Il(K)+ E(Br)Hlattice

Q3) Write the balanced chemical equation for the reaction for which Hrxn is the lattice energy for potassium bromide.

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Page 10

Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) A typical double bond consists of __________.

A)three sigma bonds

B)three pi bonds

C)one sigma and two pi bonds

D)one sigma and one pi bond

E)three ionic bonds

Q2) Of the molecules below, only __________ is polar.

A)SbF5

B)AsH3

C)I2

D)SF6

E)CH4

Q3) The molecular geometry of the SiH2Cl2 molecule is

A)trigonal planar

B)tetrahedral

C)trigonal pyramidal

D)octahedral

E)T-shaped

Q4) The 1s hydrogen orbital overlaps with the __________ iodine orbital in HI.

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Chapter 10: Gases

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Sample Questions

Q1) The reaction of 25 mL of N2 gas with 75 mL of H2 gas to form ammonia via the equation: N2 (g)+ 3H2 (g) 2NH3 (g)

Will produce __________ mL of ammonia if pressure and temperature are kept constant.

A)250

B)50

C)200

D)150

E)100

Q2) The root-mean-square speed of H2S at 26.0°C is __________ m/sec.

A)334

B)62.4

C)468

D)751

E)214

Q3) The effusion rate of a gas is proportional to the square root of its molar mass.

A)True

B)False

Q4) What is the density (in g/L)of oxygen gas at 77.0°C and 700.0 torr?

Page 12

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol K. The conversion of 50.0 g of ice at 0.00°C to liquid water at 10.0°C requires __________ kJ of heat.

A)2110

B)18.8

C)2.11

D)16.7

E)Insufficient data are given.

Q2) Which compound has the strongest intermolecular forces?

A)CBr4

B)C12H26

C)CI4

D)N2

E)O2

Q3) Of the following, __________ is the most volatile.

A)CBr4

B)CCl4

C)CF4

D)CH4

E)C6H14

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) Polymers formed from two different monomers are called __________.

Q2) Write the chemical formulas for both polyethylene and the monomer from which it is formed.

Q3) The class of semiconductors, known as elemental, has special features. These are

A)band gap and individual element valence electrons

B)periodical table grouping and diamond crystal structure

C)tetrahedral coordination geometry and sp2 hybrid orbitals

D)overlapping hybrid orbitals and filed conduction bands

E)none of the above

Q4) What fraction of the volume of each corner atom is actually within the volume of a face-centered cubic unit cell?

A)1

B)1/2

C)1/4

D)1/8

E)1/16

Q5) Semiconductors are less conductive than metals because of __________ gap.

Q6) When lattice points occur only at the corners of a unit cell, the cell is called

Page 14

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) The concentration of urea (MW = 60.0 g/mol)in a solution prepared by dissolving 16 g of urea in 39g of H2O is __________ molal.

A)96

B)6.8

C)0.68

D)6.3

E)0.11

Q2) A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that __________.

A)there are 15 mg of benzene in 1.0 g of this solution

B)100 g of the solution contains 15 g of benzene

C)1.0 g of the solution contains 15 × 10-6 g of benzene

D)1.0 L of the solution contains 15 g of benzene

E)the solution is 15% by mass of benzene

Q3) What is the osmotic pressure (in atm)of a 0.040 M solution of a non-electrolyte at 30.0°C?

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

Q5) For a dilute aqueous solution, a concentration of 1 ppb also corresponds to a concentration of 1 __________ per liter of solution.

Page 15

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N2O5(g) 4NO2 (g)+ O2 (g)

When the rate of formation of O2 is 2.2 × 10-4 M/s, the rate of decomposition of N2O5 is __________ M/s.

A)1.1 × 10-4

B)2.2 × 10-4

C)2.8 × 10-4

D)4.4 × 10-4

E)5.5 × 10-4

Q2) The number of molecules that participate as reactants defines the __________ of the reaction.

Q3) How many moles of B are present at 10 s?

A)0.011

B)0.220

C)0.110

D)0.014

E)1.4 × 10-3

Q4) For the reaction aA + Bb cC + dD the rate law is __________.

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Page 16

Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) Pure __________ and pure __________ are excluded from equilibrium-constant expressions.

Q2) Which of the following statements is true?

A)Q does not change with temperature.

B)Keq does not change with temperature, whereas Q is temperature dependent.

C)K does not depend on the concentrations or partial pressures of reaction components. D)Q does not depend on the concentrations or partial pressures of reaction components.

E)Q is the same as Keq when a reaction is at equilibrium.

Q3) For an exothermic reaction, increasing the reaction temperature results in a(an)__________ in K.

Q4) If the reaction quotient Q for a reaction is greater 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.

Q5) If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture contains mostly __________.

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Page 17

Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) Ka for HX is 7.5 × 10-12. What is the pH of a 0.15 M aqueous solution of NaX?

A)7.97

B)1.96

C)6.00

D)8.04

E)12.10

Q2) Classify the following compounds as weak acids (W)or strong acids (S): benzoic acid nitric acid acetic acid

A)W W W

B)S S S

C)S W W

D)W S S

E)W S W

Q3) Of the following, which is the weakest acid?

A)HIO

B)HIO4

C)HIO2

D)HIO3

E)The acid strength of all of the above is the same.

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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) What change will be caused by addition of a small amount of HCl to a solution containing fluoride ions and hydrogen fluoride?

A)The concentration of hydronium ions will increase significantly.

B)The concentration of fluoride ions will increase as will the concentration of hydronium ions.

C)The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase.

D)The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase.

E)The fluoride ions will precipitate out of solution as its acid salt.

Q3) An assembly of a metal ion and the Lewis bases bonded to it is called a

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) The partial pressure of a component in a gas mixture is the product of its mole fraction and the total mixture pressure.

A)True

B)False

Q2) Approximately 90% of the earth's ozone is in the __________.

Q3) What is the final stage in municipal water treatment?

A)filtration through sand and gravel

B)aeration

C)settling

D)treatment with ozone or chlorine

E)removal of added fluoride

Q4) List two of the three major sources of nitrogen and phosphorus in water.

Q5) The lime-soda process is used for large-scale water-softening operations. CaO is added to __________.

A)oxidize Fe2+ to insoluble Fe2O3

B)cause precipitation of magnesium as Mg(OH)2

C)remove most Al3+ as solid Al(OH)3

D)cause precipitation of iron and magnesium as Fe2MgO4

E)reduce the pH to 3-4

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

Page 20

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Chapter 19: Chemical Thermodynamics

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Sample Questions

Q1) The entropy of a pure crystalline substance at 0°C is zero.

A)True

B)False

Q2) Which one of the following statements is true about the equilibrium constant for a reaction if G° for the reaction is negative?

A)K = 0

B)K = 1

C)K > 1

D)K < 1

E)More information is needed.

Q3) Find the temperature (in K)above which a reaction with a H of 123.0 kJ/mol and a S of 90.00 J/K mol becomes spontaneous.

Q4) The value of G° for a reaction conducted at 25°C is 3.05 kJ/mol. The equilibrium constant for a reaction is __________ at this temperature?

A)0.292

B)-4.20

C)0.320

D)-1.13

E)More information is needed.

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Chapter 20: Electrochemistry

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Sample Questions

Q1) What is the coefficient of the dichromate ion when the following equation is balanced? Fe2+ + Cr2O72- Fe3+ + Cr3+ (acidic solution)

A)1

B)2

C)3

D)5

E)6

Q2) The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a __________ process.

A)four-electron

B)one-electron

C)two-electron

D)three-electron

E)six-electron

Q3) The standard reduction potential of X is 1.23 V and that of Y is -0.44 V therefore X is oxidized by Y.

A)True

B)False

Q4) The major product of a hydrogen fuel cell is __________.

Page 22

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Chapter 21: Nuclear Chemistry

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Sample Questions

Q1) The three radioactive series that occur in nature end with what element?

A)Bi

B)U

C)Po

D)Pb

E)Hg

Q2) The largest number of stable nuclei have an __________ number of protons and an __________ number of neutrons.

A)even, even

B)odd, odd

C)even, odd

D)odd, even

E)even, equal

Q3) 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

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Chapter 22: Chemistry of the Nonmetals

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Sample Questions

Q1) A borane is a

A)compound containing only boron and oxygen.

B)compound containing only boron and aluminum.

C)compound containing only boron and hydrogen.

D)compound containing only boron and carbon.

E)three-dimensional covalent network of boron atoms.

Q2) Write the correctly balanced equation for the reaction between elemental fluorine and sodium iodide.

Q3) Ozone is a pale blue poisonous gas with an irritating odor.

A)True

B)False

Q4) The molecular shape of the SF6 molecule is __________.

A)tetrahedral

B)trigonal bipyramidal

C)octahedral

D)trigonal pyramidal

E)T-shaped

Q5) Why are nitric acid solutions sometimes yellowish?

Q6) The acid and salts of which halogen-oxyanion are the most stable?

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Q7) Explain why HF (aq)is a relatively weak acid compared to other hydrohalic acids.

Chapter 23: Transition Metals and Coordination Chemistry

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Sample Questions

Q1) Which one of the following complexes would most likely have tetrahedral geometry?

A)[NiCl4]2-

B)[Co(H2O)6]2+

C)[Cr(NH3)6]3+

D)[Fe(CN)6]3

E)[Pt(NH3)2Cl2]

Q2) What colors of light does chlorophyll-a absorb?

Q3) The attraction of a metal to a neutral ligand is due to __________ bonding.

A)ionic

B)covalent

C)ion-dipole

D)dipole-dipole

E)hydrophobic

Q4) The energy of a metal ligand complex is higher than the energy of the separated components.

A)True

B)False

Q5) 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.

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

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Sample Questions

Q1) Ethers can be made by condensation of two __________ molecules by splitting out a molecule of water.

A)alkyne

B)alcohol

C)ketone

D)aldehyde

E)olefin

Q2) Aromatic hydrocarbons __________.

A)readily undergo addition reactions like alkenes

B)contain a series of bonds on several consecutive carbon atoms

C)undergo substitution reactions more easily than saturated hydrocarbons

D)have sp3 hybridized carbon atoms

Q3) Gasoline and water do not mix because gasoline is __________.

A)less dense than water

B)less viscous than water

C)nonpolar and water is polar

D)volatile and water is not

E)polar and water is nonpolar

Q4) Lactose is a disaccharide of glucose and __________.

Q5) The primary ingredient in vinegar is __________

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