Principles of Chemistry
Exam Answer Key
Course Introduction
Principles of Chemistry introduces students to the foundational concepts of chemical science, emphasizing the structure of atoms and molecules, chemical bonding, stoichiometry, states of matter, and thermodynamics. The course covers the periodic table, chemical reactions, equilibrium, acids and bases, and solutions, providing a thorough grounding in both theoretical concepts and problem-solving techniques.
Designed for students in science and related disciplines, this course lays the groundwork for advanced studies in chemistry and related fields, fostering an understanding of how chemical principles apply to processes in everyday life and industry.
Recommended Textbook
Chemical Principles The Quest for Insight 7th Edition by Peter Atkins
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11 Chapters
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Page 2
Chapter 1: Atoms
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Sample Questions
Q1) Consider the following ground-state electronic configurations .Which atom has both the highest first ionization energy and the highest electron affinity?
A) [Ne] 3s<sup>2</sup>3p<sup>5</sup>
B) [Ne] 3s<sup>2</sup>3p<sup>3</sup>
C) [Ne] 3s<sup>2</sup>3p<sup>1</sup>
D) [Ne] 3s<sup>2</sup>3p<sup>4</sup>
Answer: A
Q2) A node is a point at which the wavefunction becomes zero.
A)True
B)False
Answer: False
Q3) Which set of orbitals encompass two shapes?
A) The s orbitals.
B) The p orbitals.
C) The d orbitals.
D) Both B and C, above.
E) Both A and C, above.
Answer: C
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3
Chapter 2: Molecules
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Sample Questions
Q1) Which of the following species has bonds with the most ionic character?
A) CO<sub>2 </sub>
B) NO<sub>2 </sub>
C) SnO<sub>2 </sub>
D) P<sub>4</sub>O<sub>10 </sub>
E) PCl<sub>3 </sub>
Answer: C
Q2) What hybrid orbitals are used by the N atoms in urea, H<sub>2</sub>NCONH<sub>2</sub>?
A) sp
B) sp<sup>2</sup>
C) sp<sup>3</sup>
D) dsp<sup>3</sup>
Answer: C
Q3) There are three resonance structures of the sulfate ion.A resonance structure can be written where the formal charge on sulfur is 0.
A)True
B)False
Answer: True
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Chapter 3: States of Matter
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Sample Questions
Q1) Resistance in a material is defined as:
A) R = \(\kappa\)S1U1P1.S1S1P0AS1U1P12S1S1P0 / lS1U1P1 S1S1P0
B) R = \(\kappa\)S1U1P1.S1S1P0A / l
C) R = \(\kappa\)S1U1P1.S1S1P0l / A
D) R = \(\kappa\)S1U1P1.S1S1P0A / lS1U1P12S1S1P0
E) R = \(\kappa\)S1U1P12S1S1P0S1U1P1.S1S1P0A / l
Answer: B
Q2) How many octahedral holes are there in a face-centered cubic unit cell?
A) 6
B) 13
C) 12
D) 4
E) 8
Answer: D
Q3) The ability of water to "wet" paper is due to hydrogen bonding between water molecules and surface molecules in the paper.
A)True
B)False
Answer: True
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Page 5
Chapter 4: Thermodynamics
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Sample Questions
Q1) Calculate the lattice enthalpy of potassium chloride given the following enthalpy data.
\[\begin{array} { l l }
\mathrm { K } ( \mathrm { s } ) \rightarrow \mathrm { K } ( \mathrm { g } ) & + 89 \mathrm {~kJ} \cdot \mathrm { mol } ^ { - 1 } \\
\mathrm {~K} ( \mathrm {~g} ) \rightarrow \mathrm { K } ^ { + } ( \mathrm { g } ) + \mathrm { e } ^ { - } & + 418 \mathrm {~kJ} \cdot \mathrm { mol } ^ { - 1 } \\
1 / 2 \mathrm { Cl } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { Cl } ( \mathrm { g } ) & + 122 \mathrm {~kJ} \cdot \mathrm { mol } ^ { - 1 } \\ \mathrm { Cl } ( \mathrm { g } ) \mathrm { e } ^ { - } \rightarrow \mathrm { Cl } ^ { - } ( \mathrm { g } ) & - 349 \mathrm {~kJ} \cdot \mathrm { mol } ^ { - 1 } \\ \mathrm {~K} ( \mathrm {~s} ) + 1 / 2 \mathrm { Cl } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { KCl } ( \mathrm { s } ) & - 437 \mathrm {~kJ} \cdot \mathrm { mol } ^ { - 1 }
\end{array}\]
Q2) For He(g,10 atm)\(\rightarrow\) He(g,1 atm),is the entropy change positive or negative?
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Chapter 5: Equilibrium
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Sample Questions
Q1) Consider the reaction
2CuBr<sub>2</sub>(s)\(\rightarrow\) 2CuBr(s)+ Br<sub>2</sub>(g)If the equilibrium vapor pressure of Br<sub>2</sub>(g)
Is 1.43 F1F1F1S1*F1F1F10 10F1F1F1S1<sup>-</sup>F1F1F10<sup>5</sup> Torr at 298 K, What is \(\Delta\)G at this temperature when Br<sub>2</sub>(g) Is produced at a pressure of 7.50 F1F1F1S1*F1F1F10 10F1F1F1S1<sup>-</sup>F1F1F10<sup>8</sup> Torr.
A) F1F1F1S1-F1F1F105.65 kJ
B) 13.0 kJ
C) 5.65 kJ
D) F1F1F1S1-F1F1F103.42 kJ
E) F1F1F1S1-F1F1F1013.0 kJ
Q2) At 600F1F1F1S1?F1F1F10C, K<sub>c</sub> = 2.8 for the reaction
2HgO(s)\(f\)2Hg(l)+ O<sub>2</sub>(g)
Calculate K at 600F1F1F1S1?F1F1F10C for this reaction.
A) 6800
B) 200
C) 1.4 F1F1F1S1*F1F1F10 10<sup>4 </sup>
D) 2.8
E) 138
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Page 7
Chapter 6: Reactions
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Sample Questions
Q1) In the cell shown above, A is a standard Ag<sup>+</sup>/Ag electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is +0.80 V, What is the equation for the cell reaction?
A) Ag(s) + H<sup>+</sup>(aq) \(\rightarrow\) Ag<sup>+</sup>(aq) + ½H<sub>2</sub>(g)
B) Ag<sup>+</sup>(aq) + ½H<sub>2</sub>(g) \(\rightarrow\)Ag(s) + H<sup>+</sup>(aq)
Q2) Given: S<sub>2</sub>O<sub>4</sub><sup>2</sup><sup>-</sup>(aq) \(\rightarrow\)SO<sub>3</sub><sup>2</sup><sup>-</sup>(aq),Basic solution. How many electrons appear in the balanced half-reaction?
A) 3
B) 6
C) 1
D) 4
E) 2
Q3) When a lead-acid battery discharges,sulfuric acid is produced.
A)True
B)False
Q4) Write the autoprotolysis reaction for liquid ammonia.
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Chapter 7: Kinetics
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Q1) An elementary process has an activation energy of 92 kJ/mol .If the enthalpy change for the reaction is -62 kJ/mol, What is the activation energy for the reverse reaction?
A) 154 kJ/mol
B) 62 kJ/mol
C) 92 kJ/mol
D) 30 kJ/mol
Q2) The fraction of molecules that collide with a kinetic energy equal to the activation energy for a reaction decreases rapidly with an increase in temperature.
A)True
B)False
Q3) For the reaction cyclopropane(g)\(\rightarrow\) propene(g)at 500<sup>\(\omicron\)</sup>C,a plot of ln[cyclopropane] vs t gives a straight line with a slope of -0.00067 s<sup>-</sup><sup>1</sup>.What is the order of this reaction and what is the rate constant?
Q4) Consider the following mechanism for the destruction of ozone. O<sub>3</sub> + NO \(\rarr\) NO<sub>2</sub> + O<sub>2</sub> NO<sub>2</sub> + O\(\rarr\) NO + O<sub>2</sub> What is the catalyst in this reaction?
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Page 9
Chapter 8: The Main-Group Elements
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Sample Questions
Q1) What is the shape of ClF<sub>4</sub><sup>+</sup>?
A) Seesaw
B) T-shaped
C) Trigonal bipyramidal
D) Tetrahedral
E) Square planar
Q2) What reaction produces diborane?
A) BH<sub>3</sub>(g) and B(s).
B) BF<sub>3</sub>(g) and NaBH<sub>4</sub>(s).
C) B(s) and H<sub>2</sub>(g).
D) B(s) and NH<sub>3</sub>(g).
E) BCl<sub>3</sub>(g) and NaH(s).
Q3) Dinitrogen pentoxide is the anhydride of
A) nitrous acid.
B) nitric acid.
C) dinitrogen tetroxide.
D) hydrazine.
E) hydrazoic acid.
Q4) Write an equation for the first ionization energy of sodium.
Q5) What happens to the saline hydrides when they are dissolved in water?
Page 10
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Chapter 9: The D-Block Elements
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Sample Questions
Q1) A ligand is
A) a Lewis base.
B) necessary in a complex to balance the charge on the metal ion.
C) used to force octahedral geometry on a metal ion.
D) a Lewis acid.
E) used to precipitate metal ions from aqueous solution.
Q2) The d-metals can be mixed together to form a wide range of alloys because
A) the d-electrons interact strongly with each other.
B) the d-metals have a wide range of metal radii.
C) the nucleus is well shielded by the d-electrons.
D) the range of d-metal radii is not very great.
E) the d-metals have low melting points.
Q3) The ligand 4-cyanopyridine can form _____ complex(es)with penataamminecobalt(III).
Q4) Which of the following has the largest atomic radius?
A) Ru
B) Pt
C) Mo
D) Cd
E) Zn
Page 11
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Chapter 10: Nuclear Chemistry
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Sample Questions
Q1) How many nucleons does boron-11 contain?
A) 6
B) 10
C) 5
D) 11
E) 16
Q2) A nuclide undergoes positron emission to form <sup>22</sup>Ne .What is the nuclide?
A) <sup>23</sup>Mg
B) <sup>18</sup>O
C) <sup>22</sup>Na
D) <sup>22</sup>F
E) <sup>23</sup>Na
Q3) A nuclide undergoes \(\alpha\) decay and forms <sup>231</sup>Th .What is the nuclide?
A) <sup>235</sup>Pu
B) <sup>235</sup>U
C) <sup>235</sup>Th
D) <sup>237</sup>U
E) <sup>231</sup>Pa
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Chapter 11: Organic Chemistry
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Q1) When 2-methyl-1-butene reacts with HBr,the reaction occurs in two steps.The attacking agent in the first step is __________.
Q2) The formula of the polymer methyl methacrylate (Plexiglass) is -(CH<sub>3</sub>OC(O)C(CH<sub>3</sub>)CH<sub>2</sub>)-.What is the monomer used to produce this polymer?
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) What is the missing compound in the reaction below? ethanol, 70<sup>\(\omicron\)</sup>C
CH<sub>3</sub>CH<sub>2</sub>CHBrCH<sub>3</sub> +____ \(\rightarrow\)CH<sub>3</sub>CH=CHCH<sub>3</sub> + Br<sup>-</sup> + CH<sub>3</sub>CH<sub>2</sub>OH
Q5) Where is the electrophilic site in the compound 2-bromo-2-methylbutane?
Q6) Which atom of formaldehyde, H<sub>2</sub>CO,Is a Lewis acid site?
Page 13
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