Honors General Chemistry
Exam Questions
Course Introduction
Honors General Chemistry is an intensive introductory course designed for students with strong backgrounds in science who seek a deeper and more rigorous exploration of chemical principles. The course covers fundamental topics including atomic and molecular structure, stoichiometry, chemical bonding, thermodynamics, kinetics, equilibrium, and electrochemistry. Laboratory sessions emphasize advanced experimental techniques, data analysis, and scientific communication, fostering critical thinking and problem-solving skills. Through in-depth lectures, discussions, and laboratory work, students are challenged to apply quantitative reasoning and conceptual understanding to complex chemical systems, preparing them for further study in science and related fields.
Recommended Textbook
Chemical Principles The Quest for Insight 7th Edition by Peter Atkins
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Page 2
Chapter 1: Atoms
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Sample Questions
Q1) Which of the following atoms or ions is isoelectronic with Be<sup>2+</sup>?
A) Na<sup>+ </sup>
B) Br<sup>-</sup>
C) He
D) Xe
E) He<sup>+ </sup>
Answer: C
Q2) Which of the following subshells cannot exist in an atom?
A) 4d
B) 5g
C) 5f
D) 4f
E) 3f
Answer: E
Q3) A node is a point at which the wavefunction becomes zero.
A)True
B)False
Answer: False
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Chapter 2: Molecules
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Q1) Which of the following species has the shortest bond length?
A) NO<sup>2</sup><sup>-</sup>
B) NO<sup>2+ </sup>
C) NO<sup>-</sup>
D) NO
E) NO<sup>+ </sup>
Answer: E
Q2) Consider the following equilibrium: S<sub>2</sub>O<sub>4</sub><sup>2</sup><sup>-</sup>(aq)\(\Leftrightarrow\)2SO<s ub>2</sub><sup>-</sup>(aq)
K ~ 10<sup>-</sup><sup>9</sup>Write a Lewis structure for each species.
Answer: The arrangement of atoms in S<sub>2</sub>O<sub>4</sub><sup>2</sup><sup>-</sup> is O<sub>2</sub>S-SO<sub>2</sub>.
The latter has a Lewis structure that obeys the octet rule, but SO<sub>2</sub><sup>-</sup> is a radical.
Q3) Predict the electron arrangement in NO<sub>2</sub><sup>-</sup>.
Answer: trigonal planar
Q4) How many valence electrons are present in W<sup>4+</sup>?
Answer: 2
Page 4
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Chapter 3: States of Matter
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Sample Questions
Q1) If the interaction between two species is proportional to 1/r<sup>2</sup>, which of the following is likely involved?
A) Chloromethane molecules in the liquid phase
B) Na<sup>+</sup> and H<sub>2</sub>O
C) Bromine molecules in the liquid phase
D) Chloromethane molecules in the gas phase
E) Ions in an ionic solid
Answer: B
Q2) What properties are usually associated with high carbon steel?
A) Hardness and brittleness.
B) Ductility and low hardness.
C) Ductility and high hardness.
D) Low hardness and high brittleness.
E) Corrosion resistance and high malleability.
Answer: A
Q3) The doping of a solid is the spreading of small amounts of impurities through it.
A)True
B)False
Answer: True
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Chapter 4: Thermodynamics
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Sample Questions
Q1) Why is the entropy of vaporization of a material always smaller than its entropy of fusion?
A) Because it involves a less disordered product.
B) Because it involves a less disordered starting material.
C) Because gases are always smaller in density than their corresponding liquids or solids.
D) It is not; it is always larger.
Q2) For any isothermal process, \(\Delta\)U > 0 for an ideal gas.
A)True
B)False
Q3) An isothermal change is one that occurs at a constant temperature.
A)True
B)False
Q4) Which of the following would probably have a positive \(\Delta\)S value?
A) He(g, 2 atm) \(\rarr\) He(g, 10 atm)
B) H<sub>2</sub>(g) + I<sub>2</sub>(s) \(\rarr\) 2HI(g)
C) 2Ag(s) + Br<sub>2</sub>(l) \(\rarr\) 2AgBr(s)
D) O<sub>2</sub>(g) \(\rarr\) O<sub>2</sub>(aq)
E) 2NO<sub>2</sub>(g) \(\rarr\) N<sub>2</sub>O<sub>4</sub>(g)
Q5) Work is reported in joules; and 1 joule = ____________
Page 6
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Chapter 5: Equilibrium
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Sample Questions
Q1) For the reaction
2CaSO<sub>4</sub>(s) \(f\)
2CaO(s)+ 2SO<sub>2</sub>(g)+ O<sub>2</sub>(g)
K = 0.032 at 700 K.What is the total pressure starting from pure CaSO<sub>4</sub>(s)?
A) 0.22 bar
B) 0.011 bar
C) 0.60 bar
D) 0.20 bar
E) 0.40 bar
Q2) The normal boiling point of ethanol is 78<sup>\(\omicron\)</sup>C.If the vapor pressure of ethanol is 13.3 kPa at 34.9<sup>\(\omicron\)</sup>C,calculate the enthalpy of vaporization of ethanol.
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
Q4) What is the vapor pressure of carbon disulfide at its normal boiling point?
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Chapter 6: Reactions
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Sample Questions
Q1) Consider the following reaction: 2Cu<sup>+</sup>(aq)\(\rightarrow\) Cu(s)+ Cu<sup>2+</sup>(aq)If the standard potentials of Cu<sup>2+</sup> and Cu<sup>+</sup> are +0.34 and +0.52 V,Respectively,Calculate the value of E<sup>\(\omicron\) </sup>for the given reaction.
A) +0.86 V
B) +0.70 V
C) +0.18 V
D) -0.18 V
E) -0.70 V
Q2) In a working electrochemical cell (+ cell voltage),the electrons flow from the anode through the external circuit to the cathode.
A)True
B)False
Q3) Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH<sub>3</sub>(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.
Q4) What is the conjugate acid of O<sup>2</sup><sup>-</sup>?
Q5) What is the main factor that determines the pH of any buffer?
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Chapter 7: Kinetics
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Sample Questions
Q1) Given:
CH<sub>4</sub>(g)+ Cl<sub>2</sub>(g)\(\rightarrow\)CH<sub>3</sub>Cl(g)+ HCl(g)
The rate law for this elementary process is
A) rate = k[Cl<sub>2</sub>].
B) k[CH<sub>3</sub>Cl][HCl].
C) rate = k[CH<sub>4</sub>][Cl<sub>2</sub>].
D) rate = k[CH<sub>4</sub>].
E) rate = k[CH<sub>4</sub>]<sup>2</sup>.<sup> </sup>
Q2) Consider the reaction
2N<sub>2</sub>O(g)\(\rightarrow\)2N<sub>2</sub>(g)+ O<sub>2</sub>(g)
Rate = k[N<sub>2</sub>O]For an initial concentration of N<sub>2</sub>O of 0.50 M,What is the concentration of N<sub>2</sub>O remaining after 2.0 min if k = 3.4 * 10<sup>-</sup><sup>3</sup> s<sup>-</sup><sup>1</sup>?
A) 0.50 M
B) 0.55 M
C) 0.66 M
D) 0.33 M
E) 0.17 M
Q3) What is the half-life of a second order reaction?
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Chapter 8: The Main-Group Elements
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Sample Questions
Q1) The lattice enthalpies of ionic compounds of fluoride tend to be very high because
A) fluorine has a high electronegativity.
B) fluoride ion has an oxidation state of -1.
C) fluorine gas is very reactive.
D) the fluoride ion is small.
E) fluorine is a strong oxidant.
Q2) Which of the following reactions does not occur?
A) 2Br<sup>-</sup>(aq) + Cl<sub>2</sub>(g) \(\rarr\) Br<sub>2</sub>(l) + 2Cl<sup>-</sup>(aq)
B) 2I<sup>-</sup>(aq) + Cl<sub>2</sub>(g) \(\rarr\) I<sub>2</sub>(aq) + 2Cl<sup>-</sup>(aq)
C) Cl<sub>2</sub>(g) + H<sub>2</sub>O(aq) \(\rarr\) HClO(aq) + HCl(aq)
D) KI(s) + H<sub>3</sub>PO<sub>4</sub>(aq) \(\rarr\) KH<sub>2</sub>PO<sub>4</sub>(AQ) + hi(G)
E) 2F<sup>-</sup>(aq) + Cl<sub>2</sub>(g) \(\rarr\) F<sub>2</sub>(g) + 2Cl<sup>-</sup>(aq)
Q3) Write the equation for the production of sulfur by the Claus process,identify the reducing agent,and state the total number of electrons transferred in the reaction.
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Chapter 9: The D-Block Elements
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Sample Questions
Q1) Which complex,[CoBr<sub>4</sub>]<sup>2</sup>1<sup>-</sup> or [Co(NH<sub>3</sub>)<sub>5</sub>]<sup>3+</sup>,is the more highly colored?
Q2) How many oxidation states do most d-block elements have?
A) 0
B) 1
C) More than one
D) It depends on the ligands to which it is bound.
E) It depends on the number of unpaired d-electrons in the element.
Q3) There are two geometric isomers of tris(glycinato)cobalt(III).Neither of these isomers is chiral.
A)True
B)False
Q4) Which of the following has the largest atomic radius?
A) Ru
B) Pt
C) Mo
D) Cd
E) Zn
Q5) The ligand 4-cyanopyridine can form _____ complex(es)with penataamminecobalt(III).
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Chapter 10: Nuclear Chemistry
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Sample Questions
Q1) The rate of nuclear decay does not depend on temperature.
A)True
B)False
Q2) 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.
Q3) Calculate the time required for the activity of a 9.0-mCi sodium-25 source to decay to 7.0-mCi (the half-life of sodium-25 is 60.0 s).
A) 22 s
B) 44 s
C) 0.029 s
D) 19 s
E) 9.4 s
Q4) For the fusion of two deuterium atoms to produce helium-4,the difference in mass between products and reactants is -0.0256 u.What is E per mole of helium?
Q5) Why does the band of stability curve upward at high atomic number?
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Chapter 11: Organic Chemistry
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Sample Questions
Q1) What reactants would be used to synthesize diethyl ether?
Q2) Name the compound CH<sub>3</sub>CH(CH<sub>3</sub>)CH(CH<sub>2</sub>CH<sub>3</sub>)C(CH<sub> 3</sub>)<sub>3</sub>.
A) 2,4,4-trimethyl-3-ethylpentane
B) 2,2,4-trimethyl-3-ethylpentane
C) Decane
D) 1,2-tetramethylpentane
E) 2,2-dimethyl-3-ethyl-4-methylpentane
Q3) 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
Q4) 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
Q5) Name the compound CH<sub>3</sub>CH=CHCH=CH<sub>2</sub>.
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