Chemistry for Life Sciences
Exam Materials
Course Introduction
Chemistry for Life Sciences introduces students to the fundamental principles of chemistry with a focus on their application in biological systems. The course covers essential topics such as atomic structure, chemical bonding, acids and bases, thermodynamics, and reaction kinetics, emphasizing how these chemical concepts underlie vital biological processes. Through lectures, laboratory experiments, and problem-solving exercises, students gain a comprehensive understanding of the molecular interactions that drive cellular functions, metabolism, and genetics, preparing them for further studies in life sciences, biochemistry, and related fields.
Recommended Textbook
Chemistry The Molecular Nature of Matter and Change 7th Edition by Silberberg
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24 Chapters
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Page 2
Chapter 1: Keys to the Study of Chemistry
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Sample Questions
Q1) Isopropyl alcohol, commonly known as rubbing alcohol, boils at 82.4°C. What is the boiling point in kelvins?
A) 387.6 K
B) 355.6 K
C) 323.6 K
D) 190.8 K
E) -190.8 K
Answer: B
Q2) The number 6.0448, rounded to 3 decimal places, becomes 6.045.
A)True
B)False
Answer: True
Q3) Acetic acid boils at 244.2°F. What is its boiling point in degrees Celsius?
A) 382.0°C
B) 167.7°C
C) 153.4°C
D) 117.9°C
E) 103.7°C
Answer: D
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Page 3
Chapter 2: The Components of Matter
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Sample Questions
Q1) Which one of the following groups does not contain any metals?
A) C, S, As, H
B) Cu, P, Se, Kr
C) N, Ne, Nd, Np
D) Xe, Hg, Ge, O
E) Cl, Al, Si, Ar
Answer: A
Q2) What are the approximate carbon:hydrogen mass ratios in methane (CH<sub>4</sub>) and ethyne (C<sub>2</sub>H<sub>2</sub>)?
A) 1:4 and 1:1
B) 3:2 and 6:1
C) 3:1 and 12:1
D) 3:2 and 12:1
E) 3:1 and 6:1
Answer: C
Q3) The molecular formula of a compound provides more information than its structural formula.
A)True
B)False
Answer: False
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Chapter 3: Stoichiometry of Formulas and Equations
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Sample Questions
Q1) How many molecules of molecular oxygen react with four molecules of NH<sub>3</sub> to form four molecules of nitrogen monoxide and six molecules of water?
A) 2
B) 10
C) 3
D) 4
E) 5
Answer: E
Q2) Balance the equation
B<sub>2</sub>O<sub>3</sub>(s) + NaOH(aq) \(\to\) Na<sub>3</sub>BO<sub>3</sub>(aq) + H<sub>2</sub>O(l)
Answer: B<sub>2</sub>O<sub>3</sub>(s) + 6NaOH(aq) \(\to\) 2Na<sub>3</sub>BO<sub>3</sub>(aq) + 3H<sub>2</sub>O(l)
Q3) One mole of O<sub>2</sub> has a mass of 16.0 g.
A)True
B)False
Answer: False
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Chapter 4: The Major Classes of Chemical Reactions
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Sample Questions
Q1) Select the classification for the following reaction. H<sub>2</sub>CO<sub>3</sub>(aq) \(\to\) H<sub>2</sub>O(l) + CO<sub>2</sub>(g)
A) combination
B) decomposition
C) displacement
D) acid-base
E) none of the above
Q2) For each of the following species, write down, next to the formula, the oxidation number of the indicated atom.
a. P in H<sub>2</sub>PO<sub>2</sub><sup>-</sup>
b. S in Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub>
c. C in CH<sub>2</sub>O
Q3) Some covalent compounds dissolve in water to produce conducting solutions.
A)True
B)False
Q4) An aqueous solution of lead nitrate, Pb(NO<sub>3</sub>)<sub>2</sub>, is mixed with one of sodium chromate, Na<sub>2</sub>CrO<sub>4</sub>, resulting in the formation of a precipitate of lead chromate. Write a balanced net ionic equation for this precipitation reaction, showing all phases.
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Chapter 5: Gases and the Kinetic-Molecular Theory
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Sample Questions
Q1) According to the postulates of kinetic-molecular theory, the molecules of all gases at a given temperature have the same average kinetic energy.
A)True
B)False
Q2) A gas consists of 85.7 % carbon and 14.3 % hydrogen, by weight. A sample of this gas weighing 0.673 g occupies 729 mL at a pressure of 720.0 mmHg and a temperature of 77°C. Calculate its empirical and molecular formulas.
A) CH, C<sub>2</sub>H<sub>2</sub>
B) CH<sub>2</sub>, C<sub>2</sub>H<sub>4</sub>
C) CH<sub>2</sub>, C<sub>3</sub>H<sub>6</sub>
D) CH<sub>3</sub>, C<sub>2</sub>H<sub>6</sub>
E) CH<sub>4</sub>, CH<sub>4</sub>
Q3) What are the conditions of STP?
A) 0 K and l atm
B) 273.15 K and 760 torr
C) 0°C and 760 atm
D) 273.15°C and 760 torr
E) none of the above
Q4) State Avogadro's Law.
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Chapter 6: Thermochemistry: Energy Flow and Chemical Change
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Sample Questions
Q1) A Snickers<sup>®</sup> candy bar contains 280 Calories, of which the fat content accounts for 120 Calories. What is the energy of the fat content, in kJ?
A) 5.0 × 10<sup>-1 </sup>kJ
B) 29 kJ
C) 5.0 × 10<sup>2</sup> kJ
D) 1.2 × 10<sup>3</sup> kJ
E) 5.0 × 10<sup>5</sup> kJ
Q2) Standard heats (enthalpies) of formation of compounds, \(\Delta\)H°<sub>f</sub>, may be positive or negative.
A)True
B)False
Q3) a. Define, or explain fully what is meant by the standard enthalpy of formation of a substance, \(\Delta\)H°<sub>f.</sub>.
b. What is the standard state of the element oxygen?
c. Write down in full the formation reaction for liquid ethanol, C<sub>2</sub>H<sub>5</sub>OH(l). The equation should be balanced and should indicate the physical state of each substance.
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Chapter 7: Quantum Theory and Atomic Structure
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Sample Questions
Q1) Excited hydrogen atoms radiate energy in the
A) infrared region only.
B) visible region only.
C) ultraviolet region only.
D) visible and ultraviolet regions only.
E) infrared, visible, and ultraviolet regions.
Q2) Which of the following frequencies of electromagnetic radiation has the shortest wavelength?
A) 1 kilohertz
B) 1 terahertz
C) 1 dekahertz
D) 1 gigahertz
E) 1 megahertz
Q3) What type of spectrum, if any, would be produced if the light radiated by a heated atomic gas were to be dispersed through a prism?
A) a continuous band of color
B) a continuous band of color with some dark lines (missing wavelengths)
C) only blue light
D) only red light
E) discrete lines of different colors
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Chapter 8: Electron Configuration and Chemical Periodicity
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Sample Questions
Q1) In many-electron atoms, which quantum numbers specify the energy of an electron?
A) n and l
B) n and m<sub>l</sub>
C) l and m<sub>l</sub>
D) n and m<sub>s</sub>
E) n, l, and m<sub>l</sub>
Q2) Electron affinities of neutral atoms may be positive or negative.
A)True
B)False
Q3) Which of the following elements will form a cation with a +2 charge?
A) Si
B) Sr
C) Ga
D) Cs
E) S
Q4) Define what is meant by ionization energy, and write a balanced chemical equation to represent the relevant process for element X.
Q5) Define what is meant by electron affinity, and write a balanced chemical equation to represent the relevant process for element Y.
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Chapter 9: Models of Chemical Bonding
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Sample Questions
Q1) Select the compound with the lowest (i.e., least negative) lattice energy.
A) CsBr(s)
B) NaCl(s)
C) SrO(s)
D) CaO(s)
E) KBr(s)
Q2) In not more than three sentences, describe the electron arrangement responsible for bonding in Cl<sub>2</sub> molecules.
Q3) The melting points of metals are only moderately high because A) metallic bonding is weak.
B) metals have fewer bonding electrons than non-metals.
C) metals also have relatively low boiling points.
D) the melting process does not break the metallic bonds.
E) metals prefer to be bonded to non-metals.
Q4) In not more than three sentences, describe the electron arrangement responsible for bonding in solid SrCl<sub>2</sub>.
Q5) No real bonds are 100% ionic in character.
A)True
B)False
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Chapter 10: The Shapes of Molecules
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Sample Questions
Q1) Draw the Lewis structure of XeF<sub>4</sub>. Use this structure, in conjunction with VSEPR theory, to predict the shape of this molecule. Outline your reasoning.
Q2) In formaldehyde, CH<sub>2</sub>O, both the formal charge and the oxidation number of carbon are zero.
A)True
B)False
Q3) Considering all the bonds in a molecule with trigonal bipyramidal geometry, what are the bond angles present?
A) 120° only
B) 90° only
C) 180° only
D) 60° and 90° only
E) 90°, 120°, and 180°
Q4) When resonance occurs, the bond lengths in a molecule fluctuate rapidly.
A)True B)False
Q5) All possible resonance structures contribute equally to the resonance hybrid. A)True B)False
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Chapter 11: Theories of Covalent Bonding
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Sample Questions
Q1) A molecule with the formula AX<sub>3</sub> uses __________ to form its bonds.
A) sp hybrid orbitals
B) sp<sup>2 </sup>hybrid orbitals
C) sp<sup>3 </sup>hybrid orbitals
D) sp<sup>3</sup>d hybrid orbitals
E) sp<sup>3</sup>d<sup>2</sup> hybrid orbitals
Q2) a. In the context of valence bond theory, explain the difference in geometry between a \(\sigma\) and a \(\pi\) bond. Use a real molecule to illustrate your answer. b. What two important differences are there in the properties of \(\sigma\) and \(\pi\) bonds, in terms of how they affect the structure and reactivity of molecules?
Q3) Atoms of period 3 and beyond can undergo sp<sup>3</sup>d <sup>2</sup> hybridization, but atoms of period 2 cannot.
A)True
B)False
Q4) A carbon-carbon double bond in a molecule may give rise to the existence of cis and trans isomers.
A)True
B)False
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Chapter 12: Intermolecular Forces: Liquids, Solids, and Phase Changes
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Sample Questions
Q1) The vapor pressure of 1-butene is 1.268 atm at 273.15 K and its heat of vaporization is 22.9 kJ/mol. What is the normal boiling point of 1-butene?
Q2) Polonium crystallizes in the simple cubic lattice. What is the coordination number for Po?
A) 3
B) 4
C) 6
D) 8
E) 12
Q3) Which of the following should have the lowest boiling point?
A) C<sub>5</sub>H<sub>12</sub>
B) C<sub>6</sub>H<sub>14</sub>
C) C<sub>8</sub>H<sub>18</sub>
D) C<sub>10</sub>H<sub>22</sub>
E) C<sub>12</sub>H<sub>26</sub>
Q4) Assuming that atoms are spherical, calculate the fraction of space which is occupied by atoms (i.e., the packing efficiency) in a metal with a face-centered cubic unit cell.
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Q5) How do the electrical properties of semiconductors differ from those of metals?
Chapter 13: The Properties of Mixtures: Solutions and Colloids
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Sample Questions
Q1) Octane and nonane are liquids which are components of gasoline. Their vapor pressures at 25°C are 13.9 torr and 4.7 torr, respectively. What is the vapor pressure of a mixture consisting of 1 mole of each of these compounds?
Q2) In general, water is a good solvent for both polar and non-polar compounds.
A)True
B)False
Q3) Helical segments of protein molecules arise through hydrogen bonding between C=O and N-H groups.
A)True
B)False
Q4) Children under the age of six with more than 0.10 ppm of lead in their blood can suffer a reduction in I.Q. or have behavior problems. What is the molality of a solution which contains 0.10 ppm of lead?
A) 4.8 × 10<sup>-10</sup> m
B) 4.8 × 10<sup>-7</sup> m
C) 4.8 × 10<sup>-4</sup> m
D) 4.8 × 10<sup>-1</sup> m
E) none of the above
Page 15
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Chapter 14: Periodic Patterns in the Main Group Elements:
Bonding, Structure, and Reactivity
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Sample Questions
Q1) Which of the alkali metals has the highest melting point?
A) Li
B) Na
C) K
D) Rb
E) Cs
Q2) Predict the products for the reaction of the following set of reactants. Mg(s) + Cl<sub>2</sub>(g) \(\to\)
A) MgCl(s)
B) MgCl<sub>2</sub>(s)
C) MgCl(l)
D) MgCl<sub>2</sub>(l)
E) MgCl<sub>2</sub>(aq)
Q3) Predict the products for the following set of reactants. Cl<sub>2</sub>(g) + I<sup>-</sup>(aq) \(\to\)
A) ICl
B) ICl<sub>2</sub>
C) ICl<sub>3</sub>
D) I<sub>2</sub> + Cl<sup>-</sup>
E) I + Cl<sub>2</sub><sup>-</sup>
Page 16
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Chapter 15: Organic Compounds and the Atomic Properties of
Carbon
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Sample Questions
Q1) Given that each 3-base sequence in DNA is a "code word" for a particular amino acid, how many different code words are possible using a 3-base sequence and the bases available in DNA?
Q2) All alcohols are capable of hydrogen bonding.
A)True
B)False
Q3) Name the three component parts of a nucleotide.
Q4) Both nylons and proteins are polyamides.
A)True
B)False
Q5) A characteristic reaction of haloalkanes is substitution.
A)True
B)False
Q6) All ketone molecules are capable of hydrogen bonding to other ketone molecules. A)True
B)False
Q7) A characteristic reaction of alkanes is addition.
A)True
B)False
Q8) Explain what is meant by "complementary" in the context of DNA strands. Page 17
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Page 18
Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions
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Sample Questions
Q1) What is the molecularity of the following elementary reaction? NH<sub>2</sub>Cl(aq) + OH<sup>-</sup>(aq) \(\to\) NHCl<sup>-</sup>(aq) + H<sub>2</sub>O(l)
A) unimolecular
B) bimolecular
C) termolecular
D) tetramolecular
E) Need to know the reaction order before molecularity can be determined.
Q2) For each of the following terms/concepts, give a brief explanation or definition. Where possible, use examples.
a. order of a reaction
b. elementary reaction
c. reaction intermediate
Q3) The units of the rate constant depend on the order of the reaction.
A)True
B)False
Q4) The greater the energy of activation, E<sub>a</sub>, the faster will be the reaction.
A)True
B)False
Page 19
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Chapter 17: Equilibrium: the Extent of Chemical Reactions
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Q1) Although a system may be at equilibrium, the rate constants of the forward and reverse reactions will in general be different.
A)True
B)False
Q2) If all the reactants and products in an equilibrium reaction are in the gas phase, then K<sub>p</sub> = K<sub>c</sub>.
A)True
B)False
Q3) If Q > K, more products need to be formed as the reaction proceeds to equilibrium.
A)True
B)False
Q4) Once a reaction system reaches equilibrium, the concentrations of reactions and products no longer change.
A)True
B)False
Q5) For some gas-phase reactions, K<sub>p</sub> = K<sub>c</sub>.
A)True B)False
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Chapter 18: Acid-Base Equilibria
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Sample Questions
Q1) Lactic acid has a pK<sub>a</sub> of 3.08. What is the approximate degree of dissociation of a 0.35 M solution of lactic acid?
A) 1.1%
B) 2.2%
C) 4.8%
D) 14%
E) none of the above
Q2) A solution is prepared by adding 0.10 mol of iron(III) nitrate, Fe(NO<sub>3</sub>)<sub>3</sub>, to 1.00 L of water. Which statement about the solution is correct?
A) The solution is basic.
B) The solution is neutral.
C) The solution is acidic.
D) The value of K<sub>a</sub> for the species in solution must be known before a prediction can be made.
E) The value of K<sub>b</sub> for the species in solution must be known before a prediction can be made.
Q3) Describe what is meant by the "leveling effect". Use a real acid as an example, and write an appropriate equation.
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Page 21
Chapter 19: Ionic Equilibria in Aqueous Systems
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Sample Questions
Q1) Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag<sup>+</sup> ion in the solution after equilibrium has been reestablished. For AgCl, K<sub>sp</sub> = 1.8 × 10<sup>- 10</sup>.
A) 1.8 × 10<sup>-10</sup> mol Ag<sup>+</sup>
B) 9.0 × 10<sup>-10 </sup>mol Ag<sup>+</sup>
C) 9.0 × 10<sup>-9 </sup>mol Ag<sup>+</sup>
D) 6.7 × 10<sup>-8</sup><sup> </sup>mol Ag<sup>+</sup>
E) 1.3 × 10<sup>-5 </sup>mol Ag<sup>+</sup>
Q2) A change in pH will significantly affect the solubility of which, if any, of the following compounds?
A) BaF<sub>2</sub>
B) CuCl
C) CuBr
D) AgI
E) None of the solubilities will be significantly affected.
Q3) What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA) and 0.250 mol of sodium propenoate (NaA)? (K<sub>a</sub> for propenoic acid is 5.52 × 10<sup>-5</sup>.)
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Chapter 20: Thermodynamics: Entropy, Free Energy, and the Direction
of Chemical Reactions
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Q1) Which relationship or statement best describes \(\Delta\)S° for the following reaction? BaCl<sub>2</sub>(aq) + Na<sub>2</sub>SO<sub>4</sub>(aq) \(\to\) BaSO<sub>4</sub>(s) + 2NaCl(aq)
A) .\(\Delta\)S°<sup> </sup>\(\approx\) 0
B) .\(\Delta\)S° < 0
C) .\(\Delta\)S° > 0
D) .\(\Delta\)S° = \(\Delta\)H°/T
E) More information is needed to make a reasonable prediction.
Q2) For what signs of \(\Delta\)H and \(\Delta\)S will a process
a. be spontaneous at high temperatures but not at low temperatures?
b. not be spontaneous at any temperatures?
Q3) For a chemical reaction to be non-spontaneous at any temperature, which of the following conditions must be met?
A) .\(\Delta\)S° > 0, \(\Delta\)H° > 0
B) .\(\Delta\)S° > 0, \(\Delta\)H° < 0
C) .\(\Delta\)S° < 0, \(\Delta\)H° < 0
D) .\(\Delta\)S° < 0, \(\Delta\)H° > 0
E) All reactions are spontaneous at some temperature.
Q4) State the second and third laws of thermodynamics.
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Chapter 21: Electrochemistry: Chemical Change and Electrical Work
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Q1) A voltaic cell consists of a Cd/Cd<sup>2+</sup> electrode (E° = -0.40 V) and a Fe/Fe<sup>2+</sup> electrode (E°<sup> </sup>= -0.44 V). If E<sub>cell</sub> = 0 and the temperature is 25°C, what is the ratio [Fe<sup>2+</sup>]/[Cd<sup>2+</sup>]?
A) 2 × 10<sup>1</sup>
B) 1 × 10<sup>1</sup>
C) 1
D) 1 × 10<sup>-1</sup>
E) 5 × 10<sup>-2</sup>
Q2) In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.
A) sodium and sulfur
B) hydrogen and sulfur
C) oxygen and sulfur
D) oxygen and sulfuric acid
E) hydrogen and oxygen
Q3) A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.
A)True
B)False
Page 24
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Chapter 22: The Elements in Nature and Industry
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Q1) In the commercial production of aluminum metal, the final stage involves the reaction 2Al<sub>2</sub>O<sub>3</sub>(in molten Na<sub>3</sub>AlF<sub>6</sub>) + 3C(graphite) \(\to\) 4Al(l) + 3CO<sub>2</sub>(g)
Briefly outline the method and equipment with which the reaction is accomplished.
Q2) In the industrial electrolysis of aqueous NaCl (the chlor-alkali process), the modern trend is toward the use of cells incorporating polymer membranes to separate the anode and cathode solutions.
A)True
B)False
Q3) The Earth's core consists mainly of A) Ni.
B) O.
C) Al.
D) Si.
E) Fe.
Q4) Give two important reasons why there is so much more Na<sup>+</sup> in the oceans than K<sup>+</sup>, despite their similar abundances in the earth's crust.
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Chapter 23: The Transition Elements and Their Coordination Compounds
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Q1) Give the systematic name for [CoCl<sub>3</sub>(H<sub>2</sub>O)]<sup>-</sup>.
A) cobalt(II) chloride monohydrate
B) aquatrichlorocobalt(II)
C) aquatrichlorocobaltate(II)
D) aquatrichlorocobaltite(I)
E) none of the above
Q2) If M represents a transition element, which of the following oxides should be the least basic?
A) MO
B) M<sub>2</sub>O
C) M<sub>2</sub>O<sub>3</sub>
D) MO<sub>2</sub>
E) MO<sub>3</sub>
Q3) Which of the following ligands is most likely to form a high spin octahedral complex with cobalt(II)?
A) CN<sup>-</sup>
B) en (ethylenediamine)
C) NO<sub>2</sub><sup>-</sup>
D) CO
E) I<sup>-</sup>
Page 26
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Chapter 24: Nuclear Reactions and Their Applications
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Q1) Gamma rays are not deflected by an electric field.
A)True
B)False
Q2) Write a complete, balanced equation to represent the beta decay of thallium-207.
Q3) Write a complete, balanced equation to represent the alpha decay of radon-210.
Q4) Carbon-14 will emit a \(\beta\) particle with an energy of 0.1565 MeV. What is this energy in joules?
A) 1.0 × 10<sup>-24</sup> J
B) 2.5 × 10<sup>-20</sup> J
C) 1.0 × 10<sup>-18</sup> J
D) 2.5 × 10<sup>-14</sup> J
E) none of the above
Q5) Which one of the following elements is formed largely in supernova explosions?
A) H
B) He
C) Mg
D) Fe
E) U
Q6) What is the mechanism by which control rods slow down the fission rate in a nuclear reactor?
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