Chemistry for the Life Sciences Textbook Exam Questions - 1986 Verified Questions

Chemistry for the Life Sciences

Textbook Exam Questions

Course Introduction

Chemistry for the Life Sciences provides an introduction to the fundamental principles of chemistry with a focus on their application to biological systems. The course covers atomic and molecular structure, chemical bonding, properties of solutions, acids and bases, reaction kinetics, and thermodynamics, all through the lens of processes relevant to living organisms. Emphasis is placed on understanding the chemical basis of biological molecules and processes, including proteins, nucleic acids, metabolism, and cellular energetics, to equip students in life sciences with the foundational knowledge necessary for advanced study in fields such as biology, medicine, biochemistry, and allied health sciences.

Recommended Textbook

Chemical Principles 6th Edition by Professor Peter Atkins

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Chapter 1: The Quantum World

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Q1) Which of the following corresponds to an X-radiation wavelength?

A)0.0001 nm

B)0.001 nm

C)9 cm

D)9 nm

E)95 nm

Answer: D

Q2) What type of wavelength is characteristic of radio waves?

A)Very large.

B)Very small.

C)Large or small depending on frequency.

D)Close to that of visible light.

E)None of the above; radio waves are not a form of radiation.

Answer: A

Q3) The zero-point energy in 1,3-butadiene is larger than in 1,3,5,7-octatetraene.

A)True

B)False

Answer: True

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) The three quantum numbers for an electron in a hydrogen atom in a certain state are n = 4,l = 2,m_l = 1.The electron is located in what type of orbital?

A)4p

B)3p

C)4s

D)4d

E)3d

Answer: D

Q2) Consider the following ground-state electronic configurations.Which atom has both the highest first ionization energy and the highest electron affinity?

A)[Ne] 3s²3p⁵

B)[Ne] 3s²3p³

C)[Ne] 3s²3p¹

D)[Ne] 3s²3p⁴

Answer: A

Q3) What is the inert-pair effect?

Answer: The inert-pair effect is the tendency to form ions two units lower in charge than expected from the group number.

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Chapter 3: Chemical Bonds

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Q1) How many electrons are in the expanded valence in XeO₄?

Answer: 16

Q2) The electronegativity of an element can be expressed as ½(I + E_a)where I is the ionization energy and E_a is the electron affinity.

A)True

B)False

Answer: True

Q3) If dinitrogen oxide has a dipole moment,what is the arrangement of atoms?

Answer: N-N-O

Q4) Use the bond enthalpies given to estimate the heat released when 2-methyl-1-propene,(CH₃)₂C=CH₂,reacts with HBr to give (CH₃)₂CBrCH₃.Bond enthalpies (kJ.mol^-¹): C-H,412; C-C,348; C=C,612; C-Br,276; H-Br,366.

A)58 kJ.mol^-¹

B)507 kJ.mol^-¹

C)317 kJ.mol^-¹

D)288 kJ.mol^-¹

E)181 kJ.mol^-¹

Answer: A

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Chapter 4: Molecular Shape and Structure

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Q1) All of the following are polar except

A)SF₄.

B)ClO₂^-

C)IF₄⁺.

D)XeF₄

E)ClF_3.

Q2) What is the shape of ClF₃?

A)Tetrahedral

B)Seesaw

C)Trigonal bipyramidal

D)T-shaped

E)Square planar

Q3) Identify the hybrid orbitals used by the underlined atom in acetone,CH₃COCH₃.

A)sp³d

B)sp²

C)None; pure p_z-orbitals are used in bonding.

D)sp³

E)sp

Q4) Predict the electron arrangement in NO₂^-.

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Chapter 5: The Properties of Gases

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Q1) Consider the following reaction: 4KO₂(s)+ 2CO₂(g)\(\rightarrow\)2K₂CO₃(s)+ 3O₂(g)

How many liters of oxygen are produced at STP if 10.5 moles of carbon dioxide are used at STP?

A)15.8

B)0.703

C)706

D)353

E)235

Q2) What volume is occupied by 1,000.g of fluorine gas at 10.00°C at a pressure of 735 Torr?

A)22.3 L

B)44.6 L

C)621 L

D)632 L

E)4,690 L

Q3) The main composition of dry air at sea level is about 75.5% nitrogen,23.1% oxygen,and 1.3% argon.In a 1.00-g sample of dry air at 1.00 atm,calculate the partial pressure of argon gas.

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Chapter 6: Liquids and Solids

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Q1) How many atoms are there in a face-centered cubic unit cell?

Q2) If the ratio of the radius of the cation to the anion in a 1:1 compound is 0.800,

A)The compound adopts the rock-salt structure.

B)The coordination number of the cation and anion are 6 and 6.

C)The compound adopts the same structure as calcium fluorite.

D)Each cation occupies one-half of the tetrahedral holes of each anion cube.

E)Each cation occupies all the cubic holes in the center of each anion cube.

Q3) All the following hydrated compounds are commonly available except

A)BaCl₂·2H₂O.

B)NH₄NO₃·2H₂O.

C)NaClO₄·H₂O.

D)Cr(ClO₄)₃·6H₂O.

E)La₂(SO₄)₃·9H₂O.

Q4) Which of the following is the strongest intermolecular force between molecules?

A)Dipole-dipole (stationary)

B)Hydrogen bonding

C)Dipole-dipole (rotating)

D)London

E)Ion-dipole

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Chapter 7: Inorganic Materials

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Q1) What is the diameter range of a nano-tube?

A)A few angstroms.

B)A few nanometers.

C)A few microns.

D)No more than 5 angstroms.

E)No more than 5 microns.

Q2) At what general temperature are interstitial carbides formed?

A)00^oC

B)200^oC

C)1,000^oC 

D)2,000^oC

E)20,000^oC

Q3) Portland cement is made from what materials?

A)Oxides.

B)Sand and clay.

C)Crushed limestone

D)Only B and C,above.

E)A,B,and C,above.

Q4) Atom arrangements that move relative to one another along set two-dimensional surfaces are called what?

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Chapter 8: Thermodynamics: The First Law

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Q1) A CD player and its battery together do 500 kJ of work.The battery also releases 250 kJ of energy as heat and the CD player releases 50 kJ as heat due to friction from spinning.What is the change in internal energy of the system,with the system regarded as the battery and CD player together?

A)+200 kJ

B)(-700 kJ)

C)(-800 kJ)

D)(-200 kJ)

E)(-750 kJ)

Q2) If 2.00 mol of an ideal gas at 300 K and 3.00 atm expands from 6.00 L to 18.00 L and a final pressure of 1.20 atm in two steps: (1)the gas is cooled at constant volume until its pressure has fallen to 1.20 atm,and (2)it is heated and allowed to expand against a constant pressure of 1.20 atm until its volume reaches 18.00 L,which of the following is correct?

A)w = 0 for step (1)and w = -1.46 kJ for step (2)

B)w = -4.57 kJ for the overall process

C)w = -6.03 kJ for the overall process

D)w = -4.57 kJ for step (1)and w = -1.46 kJ for step (2)

E)w = 0 for the overall process

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Chapter 9: Thermodynamics: The Second and Third Laws

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Q1) For the reaction

2SO₃(g)\(\rightarrow\)2SO₂(g)+ O₂(g)

\(\Delta\)H_r° = +198 kJ.mol^-1 and \(\Delta\)S_r° = 190 J.K^-1.mol^-1 at 298 K.The equilibrium constant for this reaction will be greater than 1 at

A)all temperatures.

B)temperatures above 1315 K.

C)temperatures below 1042 K.

D)no temperature.

E)temperatures above 1042 K.

Q2) Calculate \(\Delta\)S_surr° at 298 K for the reaction H₂(g)+ F₂(g)\(\rightarrow\) 2HF(g)

\(\Delta\)H_r° = -546 kJ.mol^-1,\(\Delta\)S_r° =

+14.1 J.K^-1.mol^-1

A)+14.1 J.K^-1.mol^-1

B)+1820 J.K^-1.mol^-1

C)+1830 J.K^-1.mol^-1

D)(-1830 J.K^-1.mol^-1)

E)(-14.1 J.K^-1.mol^-1)

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Chapter 10: Physical Equilibria

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Q1) Estimate the enthalpy of vaporization of CCl₄ given that at 25S1U1P1\(\circ\)S1S1P0C and 58S1U1P1\(\circ\)S1S1P0C its vapor pressure is 107 and 405 Torr,respectively.Assume that the enthalpy of vaporization is independent of the temperature.

A)486 J.mol^-1

B)48.6 kJ.mol^-1

C)142 kJ.mol^-1

D)3.98 kJ.mol^-1

E)33.1 kJ.mol^-1

Q2) Calculate the vapor pressure at 25S1U1P1\(\circ\)S1S1P0C of a mixture of benzene and toluene in which the mole fraction of benzene is 0.650.The vapor pressure at 25S1U1P1\(\circ\)S1S1P0C of benzene is 94.6 Torr and that of toluene is 29.1 Torr.

A)84.4 Torr

B)124 Torr

C)51.3 Torr

D)71.7 Torr

E)61.5 Torr

Q3) Which liquid would you expect to be the more volatile,CH₃CHO or CH₃OCH₃?

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Chapter 11: Chemical Equilibria

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Q1) What is the relationship between K and K_c for the reaction below?

NH₄(NH₂CO₂)(s) 2NH₃(g)+ CO₂(g)

A)K_c = (RT)²K

B)K = RTK_c

C)K = (RT)²K_c

D)K = (RT)³K_c

E)K_c = (RT)³K

Q2) Consider the reaction 2Fe₂O₃(s)+ 3C(s)\(\rightarrow\) 4Fe(s)+ 3CO₂(g),\(\Delta\)HS1U1P1\(\circ\)S1S1P0= 462 kJ,\(\Delta\)SS1U1P1\(\circ\)S1S1P0= 558 J.K^-1

Calculate the equilibrium constant for this reaction at 525S1U1P1\(\circ\)S1S1P0C.

A)3.04 * 10^-3

B)8.07 * 10^-2

C)5.20 * 10^-7

D)1.9 * 10⁶

E)2.18 * 10^-2

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Chapter 12: Acids and Bases

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Q1) The pH of 0.010 M H₃PO₄(aq)is 2.24; estimate the concentration of PO₄³^- in the solution.For H₃PO₄,the values of K_a1,K_a2,and K_a3 are 7.6 *10^-³,6.2 * 10^-⁸,and 2.1 * 10<sup>-</sup¹³,respectively.

A)5.8 * 10^-3 M

B)2.1 * 10^-13 M

C)7.6 * 10^-3 M

D)6.2 * 10^-8 M

E)2.3 * 10^-18 M

Q2) All of the following are strong bases in water except

A)NaHCO₃

B)CaO

C)Na₂O

D)Na₂SO₄

Q3) All of the following are Lewis bases except

A)OH^-

B)H₂O

C)SO₃

D)Br^-

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Chapter 13: Aqueous Equilibria

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Q1) What is the pH of an aqueous solution that is 0.018 M C₆H₅NH₂ (K_b = 4.3 * 10^-10)and 0.12 M C₆H₅NH₃Cl?

A)5.46

B)4.63

C)3.81

D)10.19

E)8.54

Q2) For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq),calculate the pH after the addition of 55.0 mL of KOH(aq).For salycylic acid,pK_a = 2.97.

A)10.98

B)7.00

C)11.26

D)12.02

E)12.30

Q3) Consider the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq),with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

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Chapter 14: Electrochemistry

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Q1) The products of the electrolysis of CuSO₄(aq)are

A)H₂(g)and H₂SO₃(aq).

B)H₂SO₃(aq)and O₂(g).

C)Cu(s)and H₂SO₃(aq).

D)Cu(s)and O₂(g).

E)H₂(g)and O₂(g).

Q2) If ES1U1P1\(\circ\)S1S1P0 for the following cell is 0.36 V at 25S1U1P1\(\circ\)S1S1P0C

Pb(s)|PbSO₄(s)|SO₄²^-(aq,0.60 M)m H⁺(aq,0.70 M)|H₂(g,192.5 kPa)|Pt

How is the Nernst equation for the cell properly expressed at this temperature?

A)E = 0.36 - 0.01285ln[1.90/{(0.70)²(0.60)}]

B)E = 0.36 - 0.02569ln[192.5/{(0.70)²(0.60)}]

C)E = 0.36 + 0.01285ln[192.5/{(0.70)²(0.60)}]

D)E = 0.36 + 0.01285ln[1.90/{(0.70)²(0.60)}]

E)E = 0.36 - 0.01285ln[1.90/{(0.70)(0.60)}]

Q3) A cell that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K has a negative potential?

A)True

B)False

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Chapter 15: Chemical Kinetics

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Q1) Consider the following mechanism for the destruction of ozone. O₃ + NO \(\rightarrow\) NO₂ + O₂ NO₂ + O \(\rightarrow\) NO + O₂

What is the catalyst in this reaction?

Q2) Given:

CH₄(g)+ Cl₂(g)\(\rightarrow\) CH₃Cl(g)+ HCl(g)

The rate law for this elementary process is

A)rate = k[Cl₂].

B)k[CH₃Cl][HCl].

C)rate = k[CH₄][Cl₂].

D)rate = k[CH₄].

E)rate = k[CH₄]².

Q3) Consider the reaction

A + B\(\rightarrow\)C + D rate = k[A]²

The time it takes for [A] to decrease from 1.0 to 0.50 M is the same as the time it takes for [A] to decrease from0.50 to 0.25 M.

A)True

B)False

Q4) What is the half-life of a second order reaction?

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Chapter 16: The Elements: the Main Group Elements

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Q1) Which of the following metals,Ag,Zn,Cu,Ni,Au,Pt,Sn,cannot be extracted by hydrometallurgical reduction of their ions with hydrogen?

A)Au,Pt

B)Ag,Au,Pt

C)Zn,Ni,Au

D)Zn,Ni,Sn

E)Ag,Cu,Au,Pt

Q2) The phase diagram for helium

A)indicates that helium exists as He(g)and He(l)at about 2 K.

B)indicates that helium exists only as a gas.

C)has two triple points.

D)indicates that helium can be liquefied at ordinary pressures.

E)indicates that helium has three phases.

Q3) Which of the following are all allotropes?

A)Graphite,diamond,and C₆₀

B)Silicon,carbon,and C₆₀

C)Boron carbide and carbon

D)Carbon monoxide and carbon dioxide

E)Silicon carbide,diamond,and C₆₀

Q4) Sulfur dioxide can act as both an oxidizing agent and a reducing agent; explain.

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Chapter 17: The Elements: The D Block

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Q1) Which of the following is likely to be a good oxidizing agent?

A)Fe²⁺

B)Cr²⁺

C)V²⁺

D)Mn²⁺

E)MnO₄^-

Q2) One mole of cis-tetraamminedichlororhodium(III)chloride dissolves in water to give

A)3 moles of ions.

B)2 moles of ions.

C)1 mole of ions.

D)6 moles of ions.

Q3) What is the name of the complex

[Cr(en)₂(OH₂)Cl]Cl₂?

A)diethylenediaminebis(aquachloro)chromium(III)chloride

B)Aquachlorobis(ethylenediamine)chromium(III)chloride

C)Chloroaquabis(ethylenediamine)chromate(III)chloride

D)Aquachlorobis(ethylenediamine)chromium(II)dichloride

E)Aquachloridebis(ethylenediamine)chromium(III)chloride

Q4) What do all rhodium complexes have in common?

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Chapter 18: Nuclear Chemistry

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Q1) Nuclides that lie above the band of stability are proton rich.

A)True

B)False

Q2) When ¹³¹I emits a \(\beta\) particle,what nuclide is produced?

A)¹³⁰I

B)¹²⁷Sb

C)¹³¹Xe

D)¹³¹Te

E)¹³⁰Te

Q3) The nuclide ²⁹P decays by ejecting a \(\beta\) particle.

A)True

B)False

Q4) The nuclear binding energy for calcium-40 is the energy released when

A)calcium-39 and 1 neutron form calcium-40.

B)20 protons and 20 neutrons form calcium-40.

C)20 protons and 20 electrons form calcium-20.

D)40 neutrons form calcium-40.

E)40 protons form calcium-40.

Q5) Why does the band of stability curve upward at high atomic number?

Q6) What is the product of the emission of a \(\beta\) particle from K-40?

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Chapter 19: Organic Chemistry I

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Q1) Which of the following species is likely to attack benzene and result in substitution?

A)NH₃

B)FeBr₄^-

C)OH^-

D)HCl

E)NO₂⁺

Q2) Why do alkanes not react with boiling nitric acid?

Q3) A dichlorobenzene reacts with HNO₃/H₂SO₄ and produces three mononitrated products.Identify the initial dichlorobenzene.

Q4) A dichlorobenzene reacts with HNO₃/H₂SO₄ and produces one mononitrated product.Identify the initial dichlorobenzene.

Q5) Name the compound

CH₃C(CH₃)₂CH₂CH₃.

A)2-isopropylpropane

B)1-methyl-2-propylethane

C)2,2-dimethylbutane

D)1,1-dimethylbutane

E)Hexane

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Chapter 20: Organic Chemistry II

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Q1) Oxidation of secondary alcohols produces A)acids.

B)aldehydes. C)ketones.

D)Secondary alcohols cannot be oxidized. E)ethers.

Q2) What is the product of the reaction

CH₃CH(NH₂)CH₃ + CH₃CH₂C(O)OCH₃ \(\rightarrow\)

Q3) Which of the following is a peptide bond?

A)(-C(O)O-)

B)(-CONH-)

C)(-C-NH-)

D)(-C=N-)

E)(-C(O)-)

Q4) When amines condense with carboxylic acids,what molecule is eliminated?

Q5) What is the product of the reaction

C₅H₉CH₂CH₂Br + NaCN \(\rightarrow\)

Q6) What reactants could be used to synthesize CH₃CONH₂?

Page 22

Q7) Which atom of formaldehyde,H₂CO,is a Lewis acid site?

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