1051-2nd Chem Exam_1051207(A)
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) In which of the molecules below is the carbon-carbon distance the shortest?
A)H3C-CH2-CH3 B)H2C C CH2 C)H2C CH2 D)H3C-CH3
E) H-C C-H Answer: E
2)The Lewis structure of N2H2 shows ________.
A) a nitrogen-nitrogen triple bond
B) each nitrogen has one nonbonding electron pair C) each nitrogen has two nonbonding electron pairs D) a nitrogen-nitrogen single bond
E) each hydrogen has one nonbonding electron pair Answer: B
3) In the nitrite ion (NO2-), ________.
A) there are 20 valence electrons B) both bonds are single bonds
C) one bond is a double bond and the other is a single bond D) both bonds are double bonds
E) both bonds are the same Answer: E
4) Resonance structures differ by ________.
A) placement of electrons only B) number and placement of electrons C) number of electrons only
D) placement of atoms only E) number of atoms only Answer: A
For the questions that follow, consider the BEST Lewis structures of the following oxyanions:
(i) NO2- (ii) NO3- (iii) SO32- (iv) SO42- (v) BrO3- 5) There can be four equivalent best resonance structures of ________.
A) (i) B) (ii) C) (iii) D) (iv) E) (v)
Answer: D
6) In which of the ions do all X-O bonds (X indicates the central atom) have the same length?
A) none B) all C) (i) and (ii) D) (iii) and (v)
E) (iii), (iv), and (v) Answer: B
7) A valid Lewis structure of ________ cannot be drawn without violating the octet rule.
A)PF3 B) SO42- C)SbF3 D)IF3 E)NF3
Answer: B, D
8) Of the bonds C-C, C C, and C C, the C-C bond is ________.
A) strongest/shortest B) strongest/longest C) weakest/longest D) weakest/shortest
E) intermediate in both strength and length Answer: C
9) In the molecule below, which atom has the largest partial negative charge?
Cl F C Br
I
A) Br B) F C) Cl D) C E) I
Answer: B
10) Given the electronegativities below, which covalent single bond is most polar?
Element: H C N O
Electronegativity: 2.1 2.5 3.0 3.5
A) N H B) O C C) O N D) O H E) C H
Answer: D
11) ________ have the lowest first ionization energies of the groups listed.
A) Noble gases B) Halogens
C) Alkaline earth metals D) Transition elements
E) Alkali metals Answer: E
12) Of the following species, ________ has the largest radius.
A) Br- B) Sr2+ C) Rb+ D) Kr E) Ar
Consider the following electron configurations to answer the questions that follow:
(i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p6 3s2 (iii) 1s2 2s2 2p6 3s2 3p1 (iv) 1s2 2s2 2p6 3s2 3p4 (v) 1s2 2s2 2p6 3s2 3p5
13) The electron configuration belonging to the atom with the highest second ionization energy is ________.
A) (i) B) (ii) C) (iii) D) (iv) E) (v)
Answer: A
14) The electron configuration that belongs to the atom with the lowest second ionization energy is ________.
A) (i) B) (ii) C) (iii) D) (iv) E) (v)
Answer: B
15) The electron configuration of the atom with the most negative electron affinity is ________.
A) (i) B) (ii) C) (iii) D) (iv) E) (v)
Answer: E
16) The electron configuration of the atom that is expected to have a positive electron affinity is ________.
A) (i) B) (ii) C) (iii) D) (iv) E) (v)
Answer: B
17) The reaction of alkali metals with oxygen produce ________.
A) oxides B) superoxides C) peroxides D) all of the above
E) none of the above Answer: D
18) Of the hydrogen halides, only ________ is a weak acid.
A) HBr (aq) B) HF (aq) C) HI (aq) D) HCl (aq)
E) They are all weak acids.
Answer: B
19) Of the following transitions in the Bohr hydrogen atom, the ________ transition results in the emission of the lowest-energy photon.
A) n = 3 n = 6 B) n = 6 n = 1 C) n = 6 n = 3 D) n = 1 n = 4 E) n = 1 n = 6 Answer: C
20) Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number?
A) 2s B) 2d C) 2p
D) all of the above E) none of the above Answer: B
21)An electron cannot have the quantum numbers n = ________, l = ________, ml = ________.
A) 3, 2, 1 B) 2, 1, -1 C) 2, 0, 0 D) 3, 1, -1 E) 1, 1, 1
Answer: E
22) Which quantum number determines the energy of an electron in a hydrogen atom?
A) n B)ml C) l D) E E) n and l
Answer: A
23) Which one of the following orbitals can hold two electrons?
A) 3s B)2px C)4dxy
D) all of the above E) none of the above Answer: D
24) Which one of the following is the correct electron configuration for a ground-state nitrogen atom?
A)
B)
C)
D)
E) None of the above is correct.
Answer: B
25) Which one of the following configurations depicts an excited oxygen atom?
A) [He]2s22p4 B) 1s22s22p1 C) 1s22s22p4 D) 1s22s22p23s2
E) 1s22s22p2 Answer: D
26) Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
A)
B)
C)
D)
E)
Answer: C
27) The n = 8 to n = 4 transition in the Bohr hydrogen atom occurs in the ________ region of the electromagnetic spectrum.
A) microwave B) ultraviolet C) infrared D) visible E) X-ray
Answer: C
28) The n = 1 shell contains ________ p orbitals. All the other shells contain ________ p orbitals.
A) 6, 2 B) 0, 3 C) 3, 6 D) 0, 6 E) 3, 3
Answer: B
29) How many quantum numbers are necessary to designate a particular electron in an atom?
A) 4 B) 1 C) 3 D) 2 E) 5
Answer: A
30)Which one of the following represents an impossible set of quantum numbers for an electron in an atom?
(arranged as n, l, ml, and ms)
A) 4, 3, -3, 1/2 B) 4, 3, 0, 0 C) 4, 3, 0, +1/2 D) 4, 3, 3, -1/2 E) 4, 2, -2, -1/2 Answer: B
31) Of the following, which one is a state function?
A) H C) wB) q D) heat
E) none of the above Answer: A
32) Which of the following is a statement of the first law of thermodynamics?
A) A negative H corresponds to an exothermic process.
B) Energy lost by the system must be gained by the surroundings.
C) Ek = 1 2mv2
D) 1 cal = 4.184 J (exactly) E) E = Efinal - Einitial Answer: B
33) When a system ________, E is always negative.
A) absorbs heat and has work done on it B) gives off heat and has work done on it C) gives off heat and does work
D) absorbs heat and does work
E) None of the above is always negative.
Answer: C 34) The reaction
4Al (s) + 3O2 (g) 2 Al2O3 (s) H° = -3351 kJ is ________, and therefore heat is ________ by the reaction.
A) endothermic, released B) endothermic, absorbed C) exothermic, absorbed D) exothermic, released
E) thermoneutral, neither released nor absorbed Answer: D
35)For which one of the following reactions is H°rxn equal to the heat of formation of the product?
A)N2 (g) + 3H2 (g) 2NH3 (g) B)P (g) + 4H (g) + Br (g) PH4Br (l)
C)12C (g) + 11H2 (g) + 11O (g) C6H22O11 (g) D)6C (s) + 6H (g) C6H6 (l)
E)(1/2)N2 (g) + O2 (g) NO2(g)
36) Consider the following two reactions:
A 2B H°rxn = 456.7 kJ/mol A C H°rxn = -22.1 kJ/mol
Determine the enthalpy change for the process:
2B C A) -478.8 kJ/mol
B) -434.6 kJ/mol C) 434.6 kJ/mol D) 478.8 kJ/mol
E) More information is needed to solve the problem.
Answer: A
37)For which one of the following reactions is the value of H°rxn equal to H°f for the product?
A)3Mg (s) + N2 (g) Mg3N2 (s) B)C2H2 (g) + H2 (g) C2H4 (g) C)C (diamond) + O2 (g) CO2 (g) D)2C (graphite) + O2 (g) 2CO (g)
E)2Ca (s) + O2 (g) 2CaO (s) Answer: A
38) The value of H° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ________ kJ.
2S (s) + 3O2 (g) 2SO3 (g)
A) -790 B) -12 C) 23 D) 12 E) -23
Answer: B
39) The enthalpy change for the following reaction is -483.6 kJ:
2H2 (g) + O2 (g) 2H2O (g)
Therefore, the enthalpy change for the following reaction is ________ kJ.
4H2 (g) + 2O2 (g) 4H2O (g)
A) -967.2 B) 483.6 C) 2.34 × 105 D) -483.6 E) 967.2
Answer: A
40) Given the following reactions
Fe2O3 (s) + 3CO (s) 2Fe (s) + 3CO2 (g) H = -28.0 kJ 3Fe (s) + 4CO2(s) 4CO (g) + Fe3O4(s) H = +12.5 kJ the enthalpy of the reaction of Fe2O3 with CO
3Fe2O3 (s) + CO (g) CO2 (g) + 2Fe3O4 (s) is ________ kJ.
A) +109 B) -59.0 C) -109 D) 40.5 E) -15.5
Answer: B
