Chemistry for Life Sciences
Exam Answer Key
Course Introduction
Chemistry for Life Sciences introduces fundamental chemical principles with an emphasis on their application to biological systems. The course covers atomic and molecular structure, chemical bonding, thermodynamics, solutions, acids and bases, and the properties of biomolecules such as proteins, nucleic acids, lipids, and carbohydrates. Through lectures, laboratory experiments, and problem-solving exercises, students will develop an understanding of how chemical processes underpin cellular structure and function, metabolism, genetic information flow, and the interaction between organisms and their environment. The course is designed to provide a solid chemical foundation for students pursuing studies in biology, medicine, pharmacy, and related fields.
Recommended Textbook
Chemical Principles 6th Edition by Professor Peter Atkins
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Page 2
Chapter 1: The Quantum World
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Sample Questions
Q1) Which of the following is a Lyman series UV band?
A)121.6 nm
B)221.6 nm
C)434.0 nm
D)121.6 cm
E)410.2 nm
Answer: A
Q2) A photon with energy of 3.9*10<sup>-17</sup> J has what frequency,in /sec?
A)6.6 * 10<sup>-34 </sup>
B)3.7 * 10<sup>15 </sup>
C)3.7 * 10<sup>-</sup><sup>15 </sup>
D)2.7 * 10<sup>14 </sup>
E)2.7 * 10<sup>-14 </sup>
Answer: D
Q3) Carotene,which is partly responsible for the color of carrots,has 22 \(\pi\) electrons in a conjugated system and a length of about 3 nm.The lowest energy transition in carotene is from n = ___ to n = ___.
Answer: 11; 12
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Chapter 2: Quantum Mechanics in Action: Atoms
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Sample Questions
Q1) A chloride ion contains how many unpaired electrons?
A)8
B)6
C)4
D)2
E)0
Answer: E
Q2) Which of the following is likely to form ions two units lower in charge than expected from the group number?
A)Hg
B)Cd
C)Sb
D)Ge
E)Zn
Answer: C
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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Sample Questions
Q1) What is the electronic configuration of Ag?
Answer: 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>2</sup> 3d<sup>10</sup> 4p<sup>6</sup> 5s<sup>1</sup> 4d<sup>10</sup>
Q2) Use the expression for the Coulomb potential energy to calculate the energy for formation of 1 mole of sodium chloride ion-pairs,that is,the energy change for the following reaction: Na<sup>+</sup>(g)+ Cl<sup>-</sup>(g)\(\rightarrow\)Na<sup>+</sup>Cl<sup>-</sup>(g)
Use r<sub>12</sub> = 283 pm.
Answer: -491 kJ.mol<sup>-</sup><sup>1 </sup>
Q3) How many electrons are in the expanded valence in XeOF<sub>2</sub>?
A)14
B)12
C)8
D)10
E)6
Answer: B
Q4) Which has the greater ionic character: H<sub>2</sub>S or H<sub>2</sub>O?
Answer: H<sub>2</sub>O
Page 5
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Chapter 4: Molecular Shape and Structure
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Sample Questions
Q1) Which of the following is polar?
A)SF<sub>6 </sub>
B)ICl<sub>4</sub><sup>-</sup><sup> </sup>
C)SF<sub>4 </sub>
D)AsF<sub>6</sub><sup>-</sup><sup> </sup>
E)XeF<sub>4 </sub>
Q2) Which of the following has bond angles slightly less than 109S1U1P1\(\circ\)S1S1P0?
A)CS<sub>3</sub><sup>2</sup><sup>-</sup><sup> </sup>
B)AsF<sub>3 </sub>
C)SO<sub>2 </sub>
D)COCl<sub>2 </sub>
E)COS
Q3) Which of the following species has two unpaired electrons?
A)OF<sup>+ </sup>
B)NO<sup>+ </sup>
C)CO<sup>+ </sup>
D)NF<sup>+ </sup>
E)CF<sup>+ </sup>
Q4) Predict the electron arrangement in ClF<sub>3</sub>.
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Chapter 5: The Properties of Gases
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Sample Questions
Q1) A sample of a gas weighing 15.1 g occupies 2.25 L at 1.75 atm and 20.0S1U1P1\(\circ\)S1S1P0C.If the empirical formula of the gas is NO<sub>2</sub>,what is the molecular formula?
A)N<sub>5</sub>O<sub>10 </sub>
B)N<sub>3</sub>O<sub>6 </sub>
C)NO<sub>2 </sub>
D)N<sub>4</sub>O<sub>8 </sub>
E)N<sub>2</sub>O<sub>4 </sub>
Q2) The value of the gas law constant,R,in units of m<sup>3</sup>.Pa.mol<sup>-</sup><sup>1</sup>.K<sup>-</sup><sup>1</sup> is A)8.31
B)0.0821
C)7.62
D)0.0752
E)62.4
Q3) If it takes 15 s for a certain sample of neon to effuse through a porous barrier,it will take ________________________________ (15 s,greater than 15 s,less than 15 s)for the same amount of nitrogen gas to effuse through the barrier under the same conditions.
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Chapter 6: Liquids and Solids
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Sample Questions
Q1) In the rock-salt structure (NaCl),the cations occupy all the octahedral holes.True or false?
A)True
B)False
Q2) Sodium has a body-centered cubic unit cell.If the atomic radius of sodium is 190 pm,what is the density of sodium?
Q3) 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
Q4) Which of the following ions forms only anhydrous salts?
A)Ba<sup>2+</sup>
B)Na<sup>+</sup>
C)Li<sup>+</sup>
D)La<sup>3+</sup>
E)K<sup>+</sup>
Q5) Which has the higher boiling point,HCl or HI?
Q6) How many atoms are there in a face-centered cubic unit cell?
Page 8
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Chapter 7: Inorganic Materials
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Sample Questions
Q1) 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.
Q2) What is a magnetic domain?
A)A magnetic field.
B)A region of temporary aligned spins.
C)A region of permanent aligned spins.
D)An induced magnetic field.
E)A randomly applied magnetic field.
Q3) Resistance in a material is defined as:
A)R = \(\kappa\).A<sup>2</sup> / l<sup> </sup>
B)R = \(\kappa\).A / l
C)R = \(\kappa\).l / A
D)R = \(\kappa\).A / l<sup>2</sup>
E)R = \(\kappa\)<sup>2</sup>.A / l
Q4) A metal sample can be considered a sea of
(protons,electrons,neutrons)in an array of cations.
Page 9
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Chapter 8: Thermodynamics: The First Law
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Q1) The lattice enthalpy of calcium bromide is the energy change for the reaction
A)CaBr<sub>2</sub>(s)\(\rightarrow\) Ca(g)+ 2Br(g)
B)CaBr<sub>2</sub>(s)\(\rightarrow\) Ca<sup>2+</sup>(g)+ 2Br<sup>-</sup>(g)
C)Ca(s)+ Br<sub>2</sub>(l)\(\rightarrow\) CaBr<sub>2</sub>(s)
D)CaBr<sub>2</sub>(s)\(\rightarrow\) Ca(g)+ Br<sub>2</sub>(g)
E)Ca(g)+ 2Br(g)\(\rightarrow\) CaBr<sub>2</sub>(g)
Q2) For Br<sub>2</sub>(l),the standard enthalpy of formation is ______________________ (positive/ negative/ zero).
Q3) In the combustion of coal,C(s),the C=O bonds are stronger than the O=O bond.
A)True
B)False
Q4) For gaseous hydrogen atoms at 298 K is +217.kJ.mol<sup>-1 </sup>,the standard enthalpy of formation can be best written as:
A)2 H(g)\(\rightarrow\) H<sub>2</sub>(g)
B)½H<sub>2</sub>(g)\(\rightarrow\) H(g)
C)H<sub>2</sub>(g)\(\rightarrow\) 2 H(g)
D)2 H<sub>2</sub>(g)\(\rightarrow\) 4 H(g)
E)H(g)\(\rightarrow\) ½H<sub>2</sub>(g)
Q5) Work is reported in joules; and 1 joule = ____________
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Chapter 9: Thermodynamics: The Second and Third Laws
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Q1) The experimental value of the molar entropy of 1 mol NO at 0 K is about 5 JK<sup>-1</sup>.We can conclude that in the crystal the molecules of NO are arranged randomly.
A)True
B)False
Q2) Calculate \(\Delta\)G for the process
He(g,1 atm,298 K)\(\rightarrow\) He(g,10 atm,298 K)
Q3) Which of the following reactions has the smallest value of \(\Delta\)SS1U1P1\(\circ\)S1S1P0?
A)NH<sub>3</sub>(g)+ HCl(g)\(\rightarrow\) NH<sub>4</sub>Cl(s)
B)2H<sub>2</sub>(l)+ O<sub>2</sub>(l)\(\rightarrow\) 2H<sub>2</sub>O(g)
C)N<sub>2</sub>(g)+ 3H<sub>2</sub>(g)\(\rightarrow\) 2NH<sub>3</sub>(g)
D)K(s)+ O<sub>2</sub>(g)\(\rightarrow\) KO<sub>2</sub>(s)
E)BaCl<sub>2</sub>.2H<sub>2</sub>O(s)\(\rightarrow\) BaCl<sub>2</sub>(s)+ 2H<sub>2</sub>O(g)
Q4) Reactions with positive values of \(\Delta\)S<sub>r</sub><sup>o</sup> always become spontaneous at low temperatures.
A)True
B)False
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Chapter 10: Physical Equilibria
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Sample Questions
Q1) The vapor pressures of pure carbon disulfide and carbon tetrachloride are 360 and 99.8 Torr,respectively,at 296 K.What is the vapor pressure of a solution containing 50.0 g of each compound?
A)260 Torr
B)274 Torr
C)241 Torr
D)33.0 Torr
E)460 Torr
Q2) The vapor pressure of benzene at 25S1U1P1\(\circ\)S1S1P0C is 94.6 Torr and its enthalpy of vaporization is 30.8 kJ.mol<sup>-1 </sup>.Estimate the normal boiling point of benzene.Assume the enthalpy of vaporization is independent of temperature.
A)640 K
B)358 K
C)470 K
D)624 K
E)Not enough information given.
Q3) Consider the phase diagrams for water and carbon dioxide given in the text on page 315.Explain the significance of the slopes of the solid-liquid lines.
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Chapter 11: Chemical Equilibria
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Sample Questions
Q1) Consider the reaction Na<sup>+</sup>(g)+ Cl<sup>-</sup>(g) NaCl(s) If the temperature is lowered,the products/reactants are favored.
Q2) For the reaction NH<sub>3</sub>(g)+ H<sub>2</sub>S(g) NH<sub>4</sub>HS(s) K<sub>c</sub> = 9.7 at 900 K.If the initial concentrations of NH<sub>3</sub>(g)and H<sub>2</sub>S(g)are 2.0 M,what is the equilibrium concentration of NH<sub>3</sub>(g)?
A)1.9 M
B)1.7 M
C)0.20 M
D)0.10 M
E)0.32 M
Q3) Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) Ni(CO)<sub>4</sub>(g)
Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)<sub>4</sub>(g)are 1.25 and 6.65 atm over 1.00 kg of nickel.
Q4) Calculate the standard free energy of formation of chloroform,CHCl<sub>3</sub>(l),at 25°C.The standard free energy of formation of CHCl<sub>3</sub>(g)is -70.12 kJ.mol<sup>-1</sup> and the vapor pressure of chloroform at 25°C is 0.499 atm.
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Chapter 12: Acids and Bases
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Sample Questions
Q1) Calculate the hydroxide ion concentration for an aqueous solution that has a pH of 3.45.
A)3.2 * 10<sup>-2</sup> M
B)0.54 M
C)3.5 * 10<sup>-4</sup> M
D)2.8 * 10<sup>-11</sup> M
E)2.6 * 10<sup>-5</sup> M
Q2) The pH of a 0.0050 M aqueous solution of calcium hydroxide is A)11.40
B)2.00
C)12.00
D)12.70
E)11.70
Q3) Write the charge balance equation for a dilute aqueous solution of HI.
A)[I<sup>-</sup>] = [OH<sup>-</sup>] + [H<sub>3</sub>O<sup>+</sup>]
B)[H<sub>3</sub>O<sup>+</sup>] = [OH<sup>-</sup>]
C)[H<sub>3</sub>O<sup>+</sup>] = [I<sup>-</sup>]
D)[H<sub>3</sub>O<sup>+</sup>] = [I<sup>-</sup>] + [OH<sup>-</sup>]
E)[HI]<sub>initial</sub> = [I<sup>-</sup>]
Q4) What is the conjugate acid of O<sup>2-</sup>?
Page 14
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Chapter 13: Aqueous Equilibria
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Q1) If a small amount of a strong base is added to buffer made up of a weak acid,HA,and the sodium salt of its conjugate base,NaA,the pH of the buffer solution does not change appreciably because
A)the K<sub>a</sub> of HA is changed.
B)No reaction occurs.
C)the strong base reacts with A<sup>-</sup> to give HA,which is a weak acid.
D)the strong base reacts with HA to give AOH and H<sup>+</sup>.
E)the strong base reacts with HA to give A<sup>-</sup> which is a weak base.
Q2) If the molar solubility of the compound M<sub>2</sub>A<sub>3</sub> is 7.0 * 10<sup>-</sup><sup>6</sup> M,what is the K<sub>sp</sub> for this compound?
A)1.7 * 10<sup>-</sup><sup>26</sup>
B)1.8 * 10<sup>-</sup><sup>24</sup>
C)2.9 * 10<sup>-</sup><sup>10</sup>
D)3.5 * 10<sup>-</sup><sup>5</sup>
Q3) 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?
Q4) What is the main factor that directly determines the pH of any buffer?
Q5) What is the main factor that determines the pH of any buffer?
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Chapter 14: Electrochemistry
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Q1) Which of the following occurs when HCl(aq),Cu(s),and Fe(s)are mixed under standard conditions?
A)O<sub>2</sub>(g)is formed.
B)Cu(s)dissolves.
C)Cl<sub>2</sub>(g)is formed.
D)No reaction takes place.
E)Fe(s)dissolves.
Q2) A cell that uses bromine to oxidize chloride ion under standard conditions at 298 K has a positive potential.True or false?
A)True
B)False
Q3) Which of the following is the strongest reducing agent?
A)F<sup>-</sup>
B)Co<sup>2+ </sup>
C)Fe<sup>2+ </sup>
D)H<sub>2 </sub>
E)Cr<sup>2+</sup>
Q4) What reaction occurs at the cathode in the following cell diagram?
Cd(s)|CdSO<sub>4</sub>(aq)|Hg<sub>2</sub>SO<sub>4</sub>|Hg(l)
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Chapter 15: Chemical Kinetics
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Q1) Consider the mechanism
NO<sub>2</sub>(g)+ F<sub>2</sub>(g)\(\rightarrow\) NO<sub>2</sub>F(g)+ F(g)k<sub>1</sub> (slow)
F(g)+ NO<sub>2</sub>(g)\(\rightarrow\) NO<sub>2</sub>F(g)k<sub>2</sub> (fast)
Give the molecularity of the first step and any intermediates in the mechanism.
A)2,and F(g)
B)2,and NO<sub>2</sub>F(g)
C)2,and NO<sub>2</sub>(g)
D)1,and no intermediate
E)2,and no intermediate
Q2) The reaction
3C + D \(\rightarrow\) products
Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?
A)0.21
B)0.12
C)0.56
D)0.28
E)0.41
Q3) 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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Sample Questions
Q1) Consider the unbalanced reactions
Na(s)+ P<sub>4</sub>(s)\(\rightarrow\) A
A + H<sub>2</sub>O(l)\(\rightarrow\) B + C
Write the formulas of A,B,and C.
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) The first reaction in the Ostwald process for the synthesis of nitric acid is the
A)oxidation of ammonia to nitrogen dioxide.
B)reduction of ammonia with copper.
C)decomposition of ammonia to nitrogen and hydrogen.
D)production of NH<sub>3</sub>(l).
E)oxidation of ammonia to nitrogen oxide.
Q4) The complex (NH<sub>3</sub>)<sub>5</sub>RuN<sub>2</sub><sup>2+</sup> can be synthesized by the reaction of hydrazine with RuCl<sub>3</sub>.In this reaction,the reducing agent is ____________ and the oxidizing agent is ____________.
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Chapter 17: The Elements: The D Block
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Q1) Which of the following complex ions is colorless?
A)[Cr(OH<sub>2</sub>)<sub>6</sub>]<sup>3+ </sup>
B)[Ti(OH<sub>2</sub>)<sub>6</sub>]<sup>3+ </sup>
C)[Ni(OH<sub>2</sub>)<sub>6</sub>]<sup>2+ </sup>
D)[V(OH<sub>2</sub>)<sub>6</sub>]<sup>2+ </sup>
E)[Zn(OH<sub>2</sub>)<sub>6</sub>]<sup>2+ </sup>
Q2) rhodium complexes are high spin?
A)True
B)False
Q3) Except for scandium and titanium,all the 3d transition metals form divalent ions in aqueous solution.
A)True
B)False
Q4) The complex CoCl<sub>4</sub><sup>2-</sup> absorbs light at approximately ____________ nm and its color is ____________.
Q5) Why is \(\Delta\)<sub>T</sub> is always greater than \(\Delta\)<sub>O</sub>?
Q6) If AgNO<sub>3</sub>(aq)is added to a 1 M aqueous solution of pentaamminechlorocobalt(III)chloride,how many moles of silver chloride are precipitated?
Q7) 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) A 9.9-g sample of iodine-131 is stored for exactly 3 weeks.If the decay constant is 0.0861 day<sup>-1</sup>,what mass of the isotope remains?
A)0.15 g
B)7.6 g
C)1.6 g
D)2.6 g
E)5.5 g
Q3) What is the product of the emission of a \(\beta\) particle from K-40?
Q4) What nuclide is formed when <sup>234</sup>Th undergoes \(\beta\) decay?
A)<sup>232</sup>Pu
B)<sup>234</sup>Pa
C)<sup>234</sup>U
D)<sup>233</sup>Th
E)<sup>230</sup>Rn
Q5) The nuclide <sup>7</sup>Be decays by electron capture.
A)True
B)False
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) Consider a molecule of molecular formula C<sub>10</sub>H<sub>18</sub>.What total number of rings plus \(\pi\) bonds are present in the molecule?
A)3
B)1 C)4
D)0
E)2
Q3) The product of the reaction of 2-butene with HBr is A)1-bromobutane.
B)2-bromo-2-butene. C)butane.
D)2-bromo-1-butene. E)2-bromobutane.
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Chapter 20: Organic Chemistry II
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Q1) The polymer that is formed from acrylonitrile is A)teflon.
B)orlon. C)cucite.
D)polystyrene.
E)PVC.
Q2) Which atom of formaldehyde,H<sub>2</sub>CO,is susceptible to attack by a nucleophilic reagent?
Q3) Which of the following compounds is most likely to undergo nucleophilic substitution by an S<sub>N</sub>2 reaction?
A)CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>Br
B)(CH<sub>3</sub>CH<sub>2</sub>)<sub>3</sub>CBr
C)CH<sub>3</sub>CH<sub>2</sub>CBr(CH<sub>3</sub>)CH<sub>3</sub> D)(CH<sub>3</sub>)<sub>3</sub>CBr
Q4) In the S<sub>N</sub>1 mechanism for nucleophilic substitution,the carbocation produced is a Lewis acid and the nucleophile is a Lewis base.
A)True
B)False
Q5) Where is the electrophilic site in the compound 2-bromo-2-methylbutane?
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