Chemistry for Life Sciences
Mock Exam
Course Introduction
Chemistry for Life Sciences provides an introduction to the fundamental principles and concepts of chemistry as they apply to biological systems. The course covers essential topics such as atomic and molecular structure, chemical bonding, thermodynamics, kinetics, and equilibrium, with a particular focus on their relevance to living organisms. Students will also explore the chemical nature of biomolecules, the mechanisms of metabolic pathways, and the role of chemical reactions in physiological processes. Through a combination of lectures, laboratory experiments, and problem-solving exercises, this course equips students with the foundational chemical knowledge necessary for advanced studies in biology, medicine, and related fields.
Recommended Textbook
Chemical Principles 6th Edition by Professor Peter Atkins
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1986 Verified Questions
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Page 2
Chapter 1: The Quantum World
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Sample Questions
Q1) If a photon has an energy of 4.0 * 10<sup>-16</sup> J,what will its frequency be,in Hz?
A)6.0 * 10<sup>17 </sup>
B)6.0 * 10<sup>16 </sup>
C)3.9 * 10<sup>17 </sup>
D)1.8 * 10<sup>-</sup><sup>17 </sup>
E)1.3 * 10<sup>20 </sup>
Answer: A
Q2) Which of the following metals has the lowest work function?
A)Be
B)Sr
C)Li
D)Rb
Answer: D
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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3
Chapter 2: Quantum Mechanics in Action: Atoms
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Sample Questions
Q1) Which of the following pairs of elements has members with similar properties?
A)B and Si
B)Li and Be
C)Mg and Al
D)Na and Ca
E)Se and I
Answer: A
Q2) Write the ground-state electron configuration of In<sup>+</sup>.
A)[Kr]4d<sup>7</sup>5s<sup>2</sup>5p<sup>3 </sup>
B)[Kr]4d<sup>8</sup>5s<sup>1</sup>5p<sup>3 </sup>
C)[Kr]4d<sup>5</sup>5s<sup>1</sup>5p<sup>6 </sup>
D)[Kr]4d<sup>10</sup>5s<sup>2 </sup>
E)[Kr]4d<sup>10</sup>5s<sup>1</sup>5p<sup>1 </sup>
Answer: D
Q3) Which of the following atoms has the highest electron affinity?
A)Ar
B)P
C)Al
D)Si
Answer: D
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Chapter 3: Chemical Bonds
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Sample Questions
Q1) Which of the following has the highest melting point?
A)KF
B)KI
C)RbF
D)KBr
E)KCl
Answer: A
Q2) Which of the following compounds is the least stable?
A)CH<sub>4 </sub>
B)SnH<sub>4 </sub>
C)SiH<sub>4 </sub>
D)GeH<sub>4 </sub>
E)PbH<sub>4 </sub>
Answer: E
Q3) The Madelung constant is different for all crystals.
A)True
B)False
Answer: True
Q4) List the chalcogens in order of increasing electronegativity.
Answer: tellurium < selenium < sulfur < oxygen.
Page 5
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Chapter 4: Molecular Shape and Structure
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Sample Questions
Q1) What is the ground-state electron configuration of O<sub>2</sub><sup>-</sup>?
Q2) Identify the hybrid orbitals used by the underlined atom in acetone,CH<sub>3</sub>COCH<sub>3</sub>.
A)sp<sup>3</sup>d
B)sp<sup>2 </sup>
C)None; pure p<sub>z</sub>-orbitals are used in bonding.
D)sp<sup>3 </sup>
E)sp
Q3) All of the following are polar except
A)NO<sub>2</sub><sup> </sup>.<sub> </sub>
B)SO<sub>3</sub><sup>2 </sup>.<sub> </sub>
C)NO<sub>2</sub>Cl.
D)NO<sub>3</sub><sup> </sup>.<sup> </sup>
E)N<sub>2</sub>O (N is the central atom).<sub> </sub>
Q4) What is the shape of ICl<sub>4</sub><sup>-</sup>?
A)T-shaped
B)Trigonal bipyramidal
C)Seesaw
D)Tetrahedral
E)Square planar
Page 6
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Chapter 5: The Properties of Gases
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Sample Questions
Q1) At 80.0S1U1P1\(\circ\)S1S1P0C and 12.0 Torr,the density of camphor vapor is 0.0829 g.L<sup>-</sup><sup>1 </sup>.What is the molar mass of camphor?
A)243 g.mol<sup>-</sup><sup>1 </sup>
B)34.5 g.mol<sup>-</sup><sup>1 </sup>
C)152 g.mol<sup>-</sup><sup>1 </sup>
D)3490 g.mol<sup>-</sup><sup>1 </sup>
E)20.3 g.mol<sup>-</sup><sup>1 </sup>
Q2) How many liters of nitrogen gas measured at 25.0S1U1P1\(\circ\)S1S1P0C and 745 Torr are produced by detonation of 90.8 g of TNT,trinitrotoluene,C<sub>7</sub>H<sub>5</sub>(NO<sub>2</sub>)<sub>3</sub>?
A)0.839 L
B)1.26 L
C)9.98 L
D)15.0 L
Q3) If the compression factor,Z,is less than one for a given gas,the van der Waals coefficient "a" is dominant for real gases.True or false?
A)True
B)False
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Chapter 6: Liquids and Solids
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Sample Questions
Q1) BN 2.I<sub>2</sub> 3.ice 4.SiO<sub>2</sub> 5.Ba 6.C 7.BeCl<sub>2</sub> 8.B
A)2,3,7,and 1,4,6,8
B)1,2,3,and 6,8
C)1,2,4,7,and 5,6,8
D)1,2,4,7,and 6,8
E)2,4,7,and 6,8
Q2) The atomic radius of magnesium is 160 pm.Estimate its density,given that the metal has a close-packed structure.
A)1.74 g.cm<sup>-3 </sup>
B)0.435 g.cm<sup>-3 </sup>
C)10.5 g.cm<sup>-3 </sup>
D)4.45 g.cm<sup>-3 </sup>
E)2.78 g.cm<sup>-3 </sup>
Q3) Glycerol,C<sub>3</sub>H<sub>8</sub>O<sub>3</sub>,has a higher viscosity than propanol,C<sub>3</sub>H<sub>8</sub>O.True or false?
A)True
B)False
Q4) Which has the higher boiling point,1,1-dichloroethene or cis-dichloroethene?
Q5) How many atoms are there in a face-centered cubic unit cell?
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Chapter 7: Inorganic Materials
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Q1) delocalized pi-bonds are the reason carbon nano-tubes conduct electricity.
A)True
B)False
Q2) A metal sample can be considered a sea of __________________ (protons,electrons,neutrons)in an array of cations.
Q3) Why is gravel often used as a filler in concrete?
A)Because it is hard.
B)Because it is inexpensive.
C)It is easily deformable.
D)Because it is a granite.
E)Gravel is not a filler in concrete.
Q4) How can quantum dots be made?
A)In solution.
B)By depositing atoms on a surface.
C)At high temperature.
D)Both A and B.
E)Both A and C.
Q5) Ceramics are not brittle.
A)True
B)False
9
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Chapter 8: Thermodynamics: The First Law
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Sample Questions
Q1) A piece of a newly synthesized material of mass 25.0 g at 80.0S1U1P1\(\circ\)S1S1P0C is placed in a calorimeter containing 100.0 g of water at 20.0S1U1P1\(\circ\)S1S1P0C.If the final temperature of the system is 24.0S1U1P1\(\circ\)S1S1P0C,what is the specific heat capacity of this material?
A)0.30 J.g<sup>-1</sup>.(S1U1P1\(\circ\)S1S1P0C)<sup>-1 </sup>
B)7.46 J.g<sup>-1</sup>.(S1U1P1\(\circ\)S1S1P0C)<sup>-1 </sup>
C)1.19 J.g<sup>-1</sup>.(S1U1P1\(\circ\)S1S1P0C)<sup>-1 </sup>
D)4.76 J.g<sup>-1</sup>.(S1U1P1\(\circ\)S1S1P0C)<sup>-1 </sup>
E)0.84 J.g<sup>-1</sup>.(S1U1P1\(\circ\)S1S1P0C)<sup>-1 </sup>
Q2) A system had 150 kJ of work done on it and its internal energy increased by 60 kJ.How much energy did the system gain or lose as heat?
A)The system lost 90 kJ of energy as heat.
B)The system lost 210 kJ of energy as heat.
C)The system gained 60 kJ of energy as heat.
D)The system gained 90 kJ of energy as heat.
E)The system gained 210 kJ of energy as heat.
Q3) A closed system can exchange energy with the surroundings.
A)True
B)False
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Page 10
Chapter 9: Thermodynamics: The Second and Third Laws
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Q1) For He(g,10 atm)\(\rightarrow\) He(g,1 atm),is the entropy change positive or negative?
Q2) Which of the following statements is true?
A)The molar entropy does not depend on the structure of the compound.
B)The molar entropy of H<sub>2</sub>O(l)is about the same as the molar entropy of ice.
C)An isothermal process that leads to a decrease in free energy is spontaneous.
D)If \(\Delta\)G<sub>r</sub>S1U1P1\(\circ\)S1S1P0> 0,then the reaction is spontaneous.
E)All processes that give positive changes in energy are spontaneous.
Q3) Calculate the standard entropy of fusion of ethanol at its melting point,159 K.The standard molar enthalpy of fusion of ethanol at its melting point is 5.02
J.K<sup>-1</sup>.mol<sup>-1 </sup>
A)(-5.02 J.K<sup>-1</sup>.mol<sup>-1 </sup>)
B)(-31.6 J.K<sup>-1</sup>.mol<sup>-1 </sup>)
C)+5.02 J.K<sup>-1</sup>.mol<sup>-1 </sup>
D)+31.6 J.K<sup>-1</sup>.mol<sup>-1 </sup>
E)(-44.0 J.K<sup>-1</sup>.mol<sup>-1 </sup>)
Q4) For CO<sub>2</sub>(g)\(\rightarrow\) CO<sub>2</sub>(aq),is the entropy change positive or negative?
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Chapter 10: Physical Equilibria
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Sample Questions
Q1) Benzene would likely dissolve which of the following substances?
A)Cl<sub>2</sub>CCCl<sub>2</sub>
B)NaCl<sub> </sub>
C)Na<sub>2</sub>CO<sub>3 </sub>
D)Ca(HCO<sub>3</sub>)<sub>2 </sub>
E)C<sub>6</sub>H<sub>12</sub>O<sub>6 </sub>
Q2) The increase in entropy of the system is responsible for the solubilities of substances that dissolve endothermically.
A)True
B)False
Q3) Estimate the enthalpy of vaporization of CCl<sub>4</sub> 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<sup>-1 </sup>
B)48.6 kJ.mol<sup>-1 </sup>
C)142 kJ.mol<sup>-1 </sup>
D)3.98 kJ.mol<sup>-1 </sup>
E)33.1 kJ.mol<sup>-1 </sup>
Q4) What is the vapor pressure of carbon disulfide at its normal boiling point?
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Chapter 11: Chemical Equilibria
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Sample Questions
Q1) Consider the reaction
4NH<sub>3</sub>(g)+ 7O<sub>2</sub>(g) 2N<sub>2</sub>O<sub>4</sub>(g)+ 6H<sub>2</sub>O(g)
If,initially,[NH<sub>3</sub>(g)] = [O<sub>2</sub>(g)] = 3.60 M,at equilibrium,[N<sub>2</sub>O<sub>4</sub>(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.
Q2) What is the relationship between K and K<sub>c</sub> for the reaction below? 2HgO(s) 2Hg(l)+ O<sub>2</sub>(g)
A)K<sub>c</sub> = (RT)<sup>2</sup>K
B)K = K<sub>c </sub>
C)K<sub>c</sub> = RTK
D)K = RTK<sub>c </sub>
E)K = (RT)<sup>2</sup>K<sub>c </sub>
Q3) The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.
A)True
B)False
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13
Chapter 12: Acids and Bases
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Sample Questions
Q1) Write the autoprotolysis reaction for liquid ammonia.
Q2) Which of the following is not a Lewis acid?
A)H<sub>3</sub>O<sup>+</sup>
B)SO<sub>3</sub>
C)NO<sub>2</sub><sup>-</sup>
D)BF<sub>3 </sub>
E)BCl<sub>3</sub>
Q3) Calculate the equilibrium constant for the reaction HSS1U1P1-S1S1P0(aq)+ H<sub>2</sub>O(l) H<sub>2</sub>S(aq)+ OH<sup>-</sup>(aq),
Given K<sub>a1</sub> = 1.3 * 10<sup>-7</sup> and K<sub>a2</sub> = 7.1 * 10<sup>-15</sup> for H<sub>2</sub>S.
A)1.3 * 10<sup>-7 </sup>
B)7.7 *10<sup>-8 </sup>
C)9.2 *10<sup>-22 </sup>
D)7.1 * 10<sup>-15 </sup>
E)1.4
Q4) the pH of 0.10 M and 0.40 M NaHCO<sub>3</sub>(aq)solutions is 8.31 for both?
A)True
B)False
Q5) What is the conjugate acid of O<sup>2-</sup>?
Page 14
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Chapter 13: Aqueous Equilibria
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Sample Questions
Q1) Consider the titration of 10.0 mL of 0.100 M (CH<sub>3</sub>)<sub>3</sub>N(aq)with 0.100 M HClO<sub>4</sub>(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?
Q2) A buffer contains equal concentrations of NH<sub>3</sub>(aq)and NH<sub>4</sub>Cl(aq).What is the pH of the buffer? (K<sub>b</sub> (NH<sub>3</sub>)= 1.8 * 10<sup>-5</sup>)
A)9.26
B)4.74
C)7.00
D)13.00
Q3) Consider the titration of 50.0 mL of 0.0200 M C<sub>6</sub>H<sub>5</sub>COOH(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.
Q4) A certain weak acid has a K<sub>a</sub> of 2.0 * 10<sup>-</sup><sup>5</sup>.What is the equilibrium constant for the reaction of this acid with a strong base?
Q5) What is the main factor that determines the pH of any buffer?
Q6) What is the main factor that directly determines the pH of any buffer?
Page 15
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Chapter 14: Electrochemistry
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Q1) In order to convert hydrazine,N<sub>2</sub>H<sub>4</sub>,to nitric acid,
A)an oxidizing agent is required.
B)a reducing agent is required.
Q2) If the standard potentials for the couples Cu<sup>2+</sup>/Cu,Ag<sup>+</sup>/Ag,and Fe<sup>2+</sup>/Fe are +0.34,+0.80,and -0.44 V,respectively,which is the strongest reducing agent?
A)Fe
B)Ag
C)Ag<sup>+ </sup>
D)Cu
E)Fe<sup>2+ </sup>
Q3) The galvanic cell shown above uses the half-cells Pb<sup>2+</sup>/Pb and Zn<sup>2+</sup>/Zn,and a salt bridge containing KCl(aq).The voltmeter gives a positive voltage reading.The electrode B could be inert platinum metal or lead.
A)True
B)False
Q4) Consider the following cell: Zn(s)|Zn<sup>2+</sup>(aq,0.10 M)m Cu<sup>2+</sup>(aq,0.10 M)|Cu(s)
At equilibrium,what is the concentration of Cu<sup>2+</sup>(aq)?
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Chapter 15: Chemical Kinetics
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Q1) A given first-order reaction has a rate constant of 0.00300 s<sup>-1</sup>.The time required for 85% reaction is
A)632 s.
B)23.5 s.
C)275 s.
D)316 s.
E)54.2 s.
Q2) Given: 2O<sub>3</sub>(g)\(\rightarrow\)3O<sub>2</sub>(g) Rate = k[O<sub>3</sub>]<sup>2</sup>[O<sub>2</sub>]<sup>-1</sup>
The overall order of the reaction and the order with respect to [O<sub>3</sub>] are A)-1 and 3.
B)1 and 2.
C)0 and 1.
D)2 and 2.
E)3 and 2.
Q3) For a zero-order reaction,the rate constant has the same units as the rate of reaction.
A)True
B)False
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Page 17
Chapter 16: The Elements: the Main Group Elements
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Q1) The products of the reaction of Al<sub>4</sub>C<sub>3</sub>(s)with water are
A)Al<sub>2</sub>O<sub>3</sub>(s)and CH<sub>4</sub>(g).
B)Al(OH)<sub>3</sub>(s)and C<sub>2</sub>H<sub>2</sub>(g).
C)Al(OH)<sub>3</sub>(s)and C<sub>2</sub>H<sub>4</sub>(g).
D)Al<sub>2</sub>O<sub>3</sub>(s)and C<sub>2</sub>H<sub>2</sub>(g).
E)Al(OH)<sub>3</sub>(s)and CH<sub>4</sub>(g).
Q2) The sublimation of "dry ice" is spontaneous at 25S1U1P1\(\circ\)S1S1P0C and 1 atm.What are the signs of \(\Delta\)HS1U1P1\(\circ\)S1S1P0and \(\Delta\)SS1U1P1\(\circ\)S1S1P0,respectively?
A)0,+
B)+,-
C)-,+
D)+,+
E)-,-
Q3) Sodium borohydride is an oxidizing agent.
A)True
B)False
Q4) Sulfur dioxide can act as both an oxidizing agent and a reducing agent; explain.
Q5) When aluminum sulfate is dissolved in water,is the resulting solution acidic or basic? Explain.
Page 18
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Chapter 17: The Elements: The D Block
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Q1) Which of the following would be the strongest acid in aqueous solution?
A)Mg(OH<sub>2</sub>)<sub>6</sub><sup>2+</sup>(aq)
B)V(OH<sub>2</sub>)<sub>6</sub><sup>2+</sup>(aq)
C)Ni(OH<sub>2</sub>)<sub>6</sub><sup>2+</sup>(aq)
D)Sc(OH<sub>2</sub>)<sub>6</sub><sup>3+</sup>(aq)
E)Fe(OH<sub>2</sub>)<sub>6</sub><sup>2+</sup>(aq)
Q2) How many unpaired electrons are predicted for a tetrahedral iron (II)complex?
A)5 or 1,depending on the ligands.
B)0 or 4,depending on the ligands.
C)1
D)4
E)5
Q3) The lanthanide contraction results because
A)the shielding effect of the d-electrons is less than that of the f-electrons.
B)the shielding effect of the d-electrons is greater than that of the f-electrons.
C)of the poor shielding effect of the f-electrons and the higher nuclear charge.
D)the d-electrons shield the f-electrons from the nucleus.
E)f-electrons interact more strongly with each other than d-electrons.
Q4) What do all rhodium complexes have in common?
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Chapter 18: Nuclear Chemistry
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Q1) All of the following are stable except A)<sup>15</sup>O.
B)<sup>20</sup>Ne.
C)<sup>14</sup>N.
D)<sup>12</sup>C.
E)<sup>16</sup>O.
Q2) What nuclide is formed when <sup>24</sup>Na undergoes \(\beta\) decay?
A)<sup>28</sup>S
B)<sup>24</sup>Ne
C)<sup>28</sup>P
D)<sup>24</sup>Mg
Q3) What is the element produced when <sup>44</sup>Ti undergoes electron capture?
A)Ar
B)K
C)Sc
D)V
E)Ca
Q4) Boron neutron capture therapy is used to destroy tumors.In this reaction,<sup>10</sup>B absorbs a slow neutron to produce <sup>11</sup>B<sup>*</sup>,which produces \(\alpha\) particles and __________ plus high-energy photons.
Page 20
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Chapter 19: Organic Chemistry I
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Q1) Consider the reaction of ethene with bromine water to produce 1,2-dibromoethane.Which of the following statements is correct regarding this reaction?
A)This reaction is a nucleophilic reaction.
B)This reaction is a substitution reaction.
C)A negatively charged intermediate is involved in this reaction.
D)A cyclic bromonium ion is an intermediate in this reaction.
Q2) Name the compound CH<sub>3</sub>CH=CHCH=CH<sub>2</sub>.
Q3) Treating benzoic acid with both nitric acid and concentrated sulfuric acid results in what product?
A)ortho-nitrobenzoic acid
B)meta-nitrobenzoic acid
C)para-nitrobenzoic acid
D)meta- and para-nitrobenzoic acids
Q4) When 2-methyl-1-butene reacts with HBr,the reaction occurs in two steps.What is the major product? (Hint: Intermediate carbocations are most stable when formed at tertiary carbons.)
Q5) Name the compound (CH<sub>3</sub>)<sub>2</sub>CHCCCH<sub>3</sub>.
Q6) Name the compound CH<sub>2</sub>=CHC(CH<sub>3</sub>)CH(CH<sub>3</sub>)<sub>2</sub>.
Page 21
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Chapter 20: Organic Chemistry II
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Q1) If 2-bromobutane reacts with OH<sup>-</sup> by an S<sub>N</sub>1 mechanism,the product is optically active and has the reverse chirality compared to the reactant.
A)True
B)False
Q2) All the following produce a silver mirror with Tollens reagent except A)HCHO.
B)CH<sub>3</sub>CH<sub>2</sub>CH(CHO)CH<sub>3</sub>.<sub> </sub>
C)CH<sub>3</sub>CH<sub>2</sub>COCH<sub>3</sub>.<sub> </sub>
D)CH<sub>3</sub>(CH<sub>2</sub>)<sub>3</sub>CHO.
E)CH<sub>3</sub>CH<sub>2</sub>CHO.
Q3) What is the product of the reaction
C<sub>5</sub>H<sub>9</sub>CH<sub>2</sub>CH<sub>2</sub>Br + NaCN \(\rightarrow\)
Q4) Predict the product of the reaction of acetic acid with trimethylamine.
A)CH<sub>3</sub>CON(CH<sub>3</sub>)<sub>3</sub><sup>+ </sup>
B)CH<sub>3</sub>CONHCH<sub>3 </sub>
C)CH<sub>3</sub>CON(CH<sub>3</sub>)<sub>2 </sub>
D)CH<sub>3</sub>CONH<sub>2 </sub>
E)No reaction occurs.
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Q5) Which atom of formaldehyde,H<sub>2</sub>CO,is a Lewis acid site?
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