HCCS Brown/LeMay/Bursten CHEM 1411: PRACETICE EXAM III
Multiple Choices: Select ONE Best Answer. 40 questions
Chapter 7 (Q1 – Q17) , Chapter 8 (Q18 - Q26), Chapter 9 (Q27 – Q40 )
Page and sect provided are based on 13th edition.
1. In which set of elements would all members be expected to have very similar chemical
properties?
A) Os, Sr, Se
B) Ni, Os, Fr
C) Na, Ni, K
D) S, Se, Al
E) Ne, Ar, Kr
Sect 7.1 p. 256 or p. 55 Sample Exercise 2.5.
2. Which of the following explains that the atomic radius of main-group elements generally
decreases across a period?
A) effective nuclear charge increases across a period
B) effective nuclear charge decreases down a group
C) effective nuclear charge zigzags down a group
D) the principalcount quantum number of the valence orbitals increases
E) both effective nuclear charge increases down a group and the principal quantum number
of the valence orbitals increases
Sect 7.2: p.p. 261-262. Memorize the periodic trend.
3. Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ca?
A) Mg > Na > P > Si > Ca
B) Ca > Si > P > Na > Mg
C) Si > P > Ca > Na > Mg
D) Ca > Na > Mg > Si > P
E) P > Si > Mg > Na > Ca
Sect 7.3: Memorize periodic trend, Figure 7.7 (p. 263) or conclusion, p. 264 Sample Exercise 7.2.
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4. Which of the following is an isoelectronic series?
A) B5-, Si4-, As3-, Te2B) Be2+, Li+, He, HC) S, Cl, Ar, K
D) O2-, S2-, Se2-, Tl2E) O, F, Ne, Na
p. 266: Memorize the definition & know how to count electron number (chap 2).
5. Which isoelectronic series is incorrectly arranged in order of increasing radius?
A) K+ < Ca2+ < Ar < ClB) P3- > S2- > Cl- > Ar
C) Ne < F- < O-2 < N3D) Al3+ < Mg2+ < Na+ < Ne
E) Ca2+ < K+ < Ar < ClSect 7.3 p. 267 Sample Exercise 7.4.
6. Of the choices below, which gives the order for first ionization energies?
A) Kr > Se > Br > Ga > Ge
B) Kr > Br > Se > Ge > Ga
C) Ga > Br > Ge > Kr > Se
D) Ga > Ge > Se > Br > Kr
E) Br > Se > Ga > Kr > Ge
Sect 7.4: Memorize periodic trend in Figure 7. 10. Sample Exercise 7.6.
7. Which of the following have the first ionization energies closely related of the groups listed?
A) Alkali metals
B) Transition elements
C) Halogens
D) Alkaline earth metals
E) Noble gases
Sect 7.4: Periodic trend or see Figure 7.10.
8. Which of the following correctly represents the third ionization of aluminum?
A) Al+ (g) + e- → Al (g)
B) Al (g) → Al+ (g) + eC) Al+ (g) → Al2+ (g) + eD) Al2+ (g) → Al3+ (g) + eE) Al- (g) + e- → Al2- (g)
Sect 7.4: p. 269 Practice Exercise 1 of Sample Exercise 7.5.
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9. Which electron configuration/group of the atom has the most negative electron affinity?
A) (i)
B) (ii)
C) (iii)
D) (iv)
E. (vii)
Sect 7.5: Figure 7.12; periodic trend.
10. Which of the following elements has the most negative electron affinity?
A) S
B) Al
C) He
D) Sr
E) Ir
Sect 7.5: p. 272. Memorize periodic trend: which accepts electron(s) easily? Metal vs. nonmetal;
electron configuration that is filled or half-filled are less likely to accept electron(s).
11. Which is the correct order of metallic character?
A) B > N > C
B) F > Cl > S
C) Si > P > S
D) P > S > Se
E) Na > K > Rb
Sect 7.6. Memorize periodic trend in Figure 7.13; p. 274.
12. Which of the following metals exhibits multiple oxidation states?
A) Al
B) Br
C) Mn
D) N
E) Ca
Sect 7.6 and p. 275. Figure 7.15; p. 275 or Sect 2.8, p. 63.
13. Which of the following oxides is the most acidic?
A) MgO
B) CaO
C) SO3
D) Rb2O
E) Li2O
Sect 7.6 p. 275-276: conclusion or p. 277 Practice Exercise 1 of Sample Exercise 7.9.
14. Which of the following is the electron configuration of the Aluminum ion (Al3+)?
A) [He]2s2
B) [He]2s22p1
C) [He]2s22p4
D) [He]2p2
E) [He]2s22p6
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Sect 7.4: p. 271 Sample Exercise 7.7 & Practice Exercises 1 & 2.
15. What species has the electron configuration [Ar]3d5?
A) Mn3+
B) Cr2+
C) V3+
D) Fe3+
E) K+
Sect 7.4: p. 271 Sample Exercise 7.7 & Practice Exercises 1 & 2.
16. Which of the following would have to gain three electrons in order to achieve a
noble gas electron configuration?
N Mg Al
Cl
P
A) Si
B) Al
C) N, P
D) Cl
E) Mg, Al, P
Sect 7.4: p. 271 Sample Exercise 7.7 & Practice Exercises 1 & 2.
17. Which of the following has eight valence electrons?
A) Ti4+
B) K+
C) ClD) S2E) all of the above
Sect 8.1 or Sect 7.4: p. 271. Know how to count electrons (chap 2) and what the valance electrons
(chap 7: p. 239) are.
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18. Which of the following is correct concerning the lattice energy?
A) NaBr > NaCl > NaF
B) CaO > SrO > BaO
C) KF > MgO > Al2O3
D) NaI > BaO > NaF
E) Al2O3 > NaBr > MgO
Sect 8.2 p. 303 Sample Exercise 8.1 & Practice Exercises 1 & 2.
19. In which of the molecules below is the carbon-carbon distance the shortest?
A) H2C CH2
B) H—C≡C—H
C) H3C—CH3
D) H2C C CH2
E) H3C—CH2—CH3
Sect 8.4 p. 309 & Sect 8.8 p. 329. Memorize conclusion in p. 303.
20. Which of the following bonds/molecules is the most polar?
A) HBr
B) HI
C) HCl
D) HF
E) H2
Sect 8.4 p. 310. Sample Exercise 8.4 & Practice Exercises 1 & 2.
21. The Lewis structure of N2H2 shows
.
A) a nitrogen-nitrogen triple bond
B) a nitrogen-nitrogen single bond
C) each nitrogen has one bonding electron pair
D) each nitrogen has two nonbonding electron pairs
E) each nitrogen has one nonbonding electron pair
Sect 8.5: p.p. 315-317. First, draw the Lewis Structure and second, answer the question.
22. In the nitrite ion (NO2-),
.
A) both bonds are single bonds
B) both bonds are double bonds
C) one bond is a double bond and the other is a single bond
D) both bonds are the same
E) there are 20 valence electrons
Sect 8.5: p.p. 315-317. First, draw the Lewis Structure and second, answer the question.
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23. Which of the following violates the octet rule?
A) NO2
B) SF2
C) PF3
D) SbF3
E) BF4Sect 8.7: p.p. 323-324. Draw Lewis structures & know three types of violations.
Focus on the central atom.
24. Which of the following central atom does not violate the octet rule?
A) SF4
B) KrF2
C) CF4
D) XeF4
E) ICl3
Sect 8.7: p.p. 323-324. Draw Lewis structures & know three types of violations.
Focus on the central atom.
25. Of the bonds N-N, N N, and N≡N, the N N bond is
A) strongest/shortest
B) strongest/longest
C) weakest/longest
D) weakest/shortest
E) intermediate in both strength and length
Sect 8.4 p. 309 & Sect 8.8 p. 329. Memorize conclusion in p. 303.
.
26. Using the table of average bond energies below, the ΔH for the reaction is
Bond:
D (kJ/mol):
C≡C
839
C-C
348
H-I
299
C-I
240
C-H
413
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A) +160
B) -160
C) -217
D) -63
E) +63
Sect 8.8. Sample Exercise 8.12 & Practice Exercises 1 & 2.
27. Which of the following is not included when counting the electron domains around
the central atom in VSEPR theory?
A) nonbonding pair of electrons
B) single covalent bond
C) core level electron pair
D) double covalent bond
E) triple covalent bond
Sect 9.2: one of the rules.
kJ.
28. Which of the following has molecular geometry as square planar?
A) CCl4
B) XeF4
C) PH3
D) XeF2
E) ICl3
Sect 9.2:First Draw Lewis structure and then apply Table 9.3 in p. 353. Memorize the table.
Sample Exercise 9.1 and Practice Exercises 1 & 2; Sample Exercise 9.2.
29. Which one of the following species has bond angles of 90°, 120° and 180°?
A) PH3
B) ClF3
C) NH3
D) AlCl3
E) PF5
Sect 9.2:First Draw Lewis structure and then apply Table 9.1 in p. 348. Memorize the table.
p. 355 Sample Exercises 9.3 and Practice Exercises 1 & 2.
30. The molecular geometry of the CS2 molecule is
.
A) linear
B) bent
C) tetrahedral
D) trigonal planar
E) T-shaped
Sect 9.2:First Draw Lewis structure and then apply Table 9.3 in p. 353. Memorize the table.
31. The hybridization of the oxygen atom labeled y in the structure below is
bond angle is
.
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A) sp, 180°
B) sp2, 109.5°
C) sp3, 109.5°
D) sp3d2, 90°
E) sp, 90°
. The C-O-H
Sect 9.2: p. 355 Sample Exercises 9.3 and Practice Exercises 1 & 2.
Apply Table 9.1 in p. 348. Memorize the table.
32. The bond angles marked a, b, and c in the molecule below are about
, respectively.
,
A) 109.5°, 109.5°, 109.5°
B) 120°, 109.5°, 120°
C) 109.5°, 109.5°, 120°
D) 90°, 180°, 90°
E) 109.5°, 109.5°, 90°
Sect 9.2: p. 355 Sample Exercises 9.3 and Practice Exercises 1 & 2.
Apply Table 9.1 in p. 348. Memorize the table.
33. The central S atom in the SF4 molecule has
unbonded electron pair(s)
and
bonded electron pair(s) in its valence shell.
A) 1, 4
B) 2, 4
C) 4, 0
D) 4, 1
E) 4, 2
Sect 9.2:First Draw Lewis structure and then answer the question.
Unbounded = nondonding (p. 347)
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34. Which of the following is polar?
A) H2
B) O3
C) SF4
D) SF6
E) PF5
Sect 9.3. Draw Lewis structure, determine molecular geometry, and then apply symmetry
(or dipole moment analysis) to determine polarity of the molecule. From symmetry viewpoint,
if the molecule is symmetric, it is nonpolar; if the molecular is asymmetric, it is polar.
, and
35. The molecular geometry of the PF3 molecule is
, and this molecule is
.
A) trigonal planar, polar
B) trigonal planar, nonpolar
C) trigonal pyramidal, polar
D) trigonal pyramidal, nonpolar
E) tetrahedral, unipolar
Sect 9.3. Draw Lewis structure, determine molecular geometry, and then apply symmetry
(or dipole moment analysis) to determine polarity of the molecule. From symmetry viewpoint,
if the molecule is symmetric, it is nonpolar; if the molecular is asymmetric, it is polar.
36. Which of the following has the hybridization of the central atom as sp?
A) PCl5
B) XeF4
C) PH3
D) Br3E) BeF2
Sect 9.5 Memorize Table 9.4. Focus on the total electron pairs on the central atom.
Sample Exercise 9.5 and Practice Exercises 1 & 2.
37. The hybridizations of bromine in BrF5 and of arsenic in AsF5 are
respectively.
A) sp3, sp3d
B) sp3d, sp3d2
and
C) sp3d, sp3
D) sp3d2, sp3d
E) sp3d2, sp3d2
Sect 9.5 Memorize Table 9.4. Focus on the total electron pairs on the central atom.
Sample Exercise 9.5 and Practice Exercises 1 & 2.
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38. How many σ bonds and π bonds are there in H3C–CH CH–C CH
respectively?
A) 14, 2
B) 10, 2
C) 12, 2
D) 13, 2
E) 10, 3
Sect 9.6 Know the definitions of σ bond and π bond in p. 365.
Learn how to count them in p.p. 366-367.
,
39. Which of the following molecules or ions will exhibit delocalized bonding?
C6H6
O3
NO3-
A) C6H6
B) NO3- only
C) C6H6, O3, and NO3D) O3 and NO3E) None of the above will exhibit delocalized bonding.
Sect 9.6 p.p. 368-371. Pay attention to the resonance structures. Sample Exercise 9.7 & Practice
Exercises 1 & 2.
40. The C-C bond in HCCH consists of
.
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A) one σ bond and one π bond
B) one σ bond and two π bonds
C) two σ bonds and one π bond
D) two σ bonds and two π bonds
E) three σ bonds and two π bonds
Comprehensive. Draw Lewis structure and then answer the question. The C-C bond in HCCH is a triple bond
(i.e. one σ bonds and two π bonds). There are total 3 σ bonds and two π bonds in HCCH.