101 498-510 F97 BOPS

Bonus Opportunity Problems
Fall 1997
Chemistry 101 - Sections 498-510

Bonus Opportunity Problems
Assignment
Answers to Some Problems

Bonus Opportunity Problems

A total of about 144 problems were carefully selected to complement the lectures. Additional practice problems, which are NOT to be handed in, are also provided. Answers to the even-numbered problems are in the textbook and worked out in the Solution Manual. The BOP's will be divided into five sets as we cover the material in class. The first four sets will be due on the Monday following each exam; the last set will be due on the last day of class. The BOP's may be turned in with a 10% penalty through Wednesday. After that time, the BOP's will absolutely not be accepted without a medical excuse. Please use regular notebook paper with your name, S.S. number, course and section number, date, my name and set number on the first page, and print your name and S.S. number on all additional pages. The problems submitted must be the "original" (not a photo- or carbon copy). The problem sets will NOT be returned to you. Please retain a copy of your work for future reference. You must show all work (messy is OK). You must hand in at least 70% to receive 1 BOP point, 80% to receive 2 BOP points and 90% to receive 3 BOP points. I encourage you to work the problems. You will find similar problems on the exams. I am available to answer any questions on BOP's during my office hours and review sessions.

Assignment

Set 1
Chapter 1: all
Chapter 2: all
Chapter 3: all

Set 2
Chapter 4: all
Chapter 5: all

Set 3
Chapter 6: all
Chapter 7: all
Chapter 8: all
Chapter 10: 6, 14, 20, 24, 26, 30

Set 4
Chapter 10: rest
Chapter 11: all
Chapter 12: 18, 28, 29, 34, 38, 41, 46, 52, 58, 64, 70

Chapter 1
(6 questions) 8, 18, 26, 29, 44, 52
[not for credit: 6, 14, 24, 28, 30, 46 and others]

Chapter 2
(14 questions) 12, 14, 19 (& explain), 20, 26, 30, 32, 37, 38, 46, 48, 58, 66, 80
[not for credit: 10, 22, 24, 28, 44, 56, 64, 94 and others]

Chapter 3
(17 questions) 4, 6, 14, 18, 26, 28, 34, 37, 50, 54, 56, 62, 66, 70, 78, 80, 90
[not for credit: 10, 12, 24, 30, 36, 38, 40, 52, 60, 64, 72, 76, 82 and others]

Chapter 4
(14 questions) 10, 15, 28, 38, 44 (Consider Ca(OH)₂ as soluble), 48, 52, 54, 58, 74, 82, 84, 90, 92 (& give the formula)
[not for credit: 12, 14, 26, 30, 40, 42, 50, 78, 80, 88 and others]

Chapter 5
(15 questions) 18, 22, 24, 30, 36, 50, 61 (& Define), 65, 66, 71, 76 (& (e) Cu, (f) Cr - tricky! Write the shorthand notation. Label diamagnetic or paramagnetic. Which one exhibits the highest degree of paramagnetism?), 80, 88, 90, 92
[not for credit: 14, 20, 26, 38, 48, 62, 64, 68, 70, 74, 78, 82, 84, 86 and others]

Chapter 6
(7 questions) 6, 8, 10, 34, 41,
100. Arrange the following atoms or ions in order of increasing diameter and explain why briefly.
(a) Ca, Mg, Sr (b) S^2-, Ar, Cl^- (c) P, Si, S, Al (d) Fe, Fe²⁺, Fe³⁺ (e) H, H⁺, H^- (f) F, Br, Te^2-, Se
101. Give examples and explain the following trends in the first ionization energy (a)across each period (include "dips" at IIIA and VIA elements for Periods 2 and 3 - see textbook), and (b) descending a periodic group.
[not for credit: 14, 16, 20, 22, 28, 36, 38, 42 and others]

Chapter 7
(15 questions) 2, 6, 8, 16, 22, 46, 52, 64, 66, 74
100. Draw Lewis dot formulae for the following. Which violate the octet rule? (worth 5 points) Use the solution manual wisely, esp. the solutions to 34, 38, 40, 48, and 52 to help you.
(a) H₂O (b) H₃O⁺ (c) HCN (d) NH₃ (e) AsF₃ (f) BeCl₂ (g) BCl₃ (h) PH₄⁺ (i) BrCl₂^- (j) SeF₄ (k) AsCl₄^- (l) ClF₃ (m) SeF₆ (n) IO₄^- (o) XeF₄
[not for credit: 8, 12, 16, 44, 50, 54, 62 and others]

Chapter 8
(6 questions) 50 (& Give the total number of sigma and pi bonds)
100. Consider the species listed in Exercise 100 in Ch. 7. For the central atom, give the number of regions of high electron density, the number of lone pairs, hybridization, electronic geometry and ideal bond angle(s). Determine the molecular or ionic geometry and polarity of the species. Use the Solution Manual wisely for help.. (worth 5 points)
[not for credit: 2, 4, 14, 18, 20, 22, 24, 34, 44, 52, 54 and other problems]

Chapter 9
(1 question) 18 (& Are they diamagnetic or paramagnetic?)
[not for credit: 12, 20, 22, 24, 26 and others]

Chapter 10
(11 questions) 6, 14, 20, 24, 26, 30, 44, 50, 58, 80, 86
[not for credit: 8, 18, 28, 44, 48, 54, 78, 84 and others]

Chapter 11
(14 questions) 4, 8, 24, 34, 36 (& normality), 42, 44, 46, 48, 52 (Hint: use normality), 56, 66, 70,
100. Consider the reaction: Cr + H⁺ Cr³⁺ + H₂ (unbalanced). How many grams of chromium will react with 75.0 mL of 0.100 N H₂SO₄. Note: in this example, H₂SO₄ is an oxidizing agent.
[not for credit: 12, 32, 38, 54, 68 and others]

Chapter 12
(15 questions) 18, 28, 29 (& explain briefly), 34, 38, 41, 46, 52, 58, 64, 70, 76, 80, 88, 96
[not for credit: other relevant even problems]

Chapter 13
(9 questions) 10, 12, 20, 44, 46, 56, 60, 66, 68
[not for credit: 14, 18, 22, 26, 28, 34, 70 and others]

Chapter 14 [not for credit: 12, 34, 38, 40, 44, 52, 54, 68, 70, 80, 84]

Answers to Some Problems

(Answers to even-numbered problems are in the textbook, solutions are given in the Solution Manual.)

Chapter 1 29. (a) 4.541 x 10⁴ cm³ (b) 5676 mL (c) 2.53 x 10⁵ in³ (d) 1.54 x 10⁵ mL

Chapter 2 19. (a) no (b) yes (c) no (d) no 37. (a) 2.02 mol P₄ (b) 1.21 x 10²⁴ molecules P₄ (c) 4.86 x 10²⁴ atoms P

Chapter 3 37. 27.8 % 53. 80.3 g NH₄Cl 65. 14.7 M H₃PO₄

Chapter 4 38. (a) occurs since CuS is insoluble salt
molecular: Cu(NO₃)₂(aq) + Na₂S(aq) CuS(s) + 2NaNO₃(aq)
total ionic:
Cu²⁺(aq) + 2NO₃^-(aq) + 2Na⁺(aq) + S²^-(aq) CuS(s) + 2Na⁺(aq) + 2NO₃^-(aq)
net ionic: Cu²⁺(aq) + S^2-(aq) CuS(s) since Na⁺ and NO₃- are spectator ions

Chapter 5 65. (a) n=1, l=0 (b) n=4, l=2, etc. 66. n=3 energy level has n²=9 orbitals and 2n²=18 electrons. E.g. the lowest energy level is n=3,l=0, m_l=0, an s orbital since l=0. 71. (a) m_s must be ą1/2 since 2 electrons in the same orbital cannot have the same spin (b) l must be 1, not 2 76. (a) paramagnetic (3 unpaired e-) (b) paramagnetic (2 unpaired e-) (c) diamagnetic (d) paramagnetic (2 unpaired e-) (e) paramagnetic (1 unpaired e-) (f) paramagnetic (6 unpaired e-)

Chapter 6 100. for example, (a) Mg > Ca> Sr

Chapter 7 17. (a) CaF₂ (b) SrCl₂ (c) K₂Se 100. Octet rule violaters: (f), (g), (i), (j), (k), (l), (m), and (o).

Chapter 11 100. 0.130 g

Chapter 12 29. (a) false (b) true (c) true (d) false (e) true 41. 2.69 x 10²² molecules

Set 1	Chapter 1: all Chapter 2: all Chapter 3: all
Set 2	Chapter 4: all Chapter 5: all
Set 3	Chapter 6: all Chapter 7: all Chapter 8: all Chapter 10: 6, 14, 20, 24, 26, 30
Set 4	Chapter 10: rest Chapter 11: all Chapter 12: 18, 28, 29, 34, 38, 41, 46, 52, 58, 64, 70

Chapter 1 (6 questions)	8, 18, 26, 29, 44, 52 [not for credit: 6, 14, 24, 28, 30, 46 and others]
Chapter 2 (14 questions)	12, 14, 19 (& explain), 20, 26, 30, 32, 37, 38, 46, 48, 58, 66, 80 [not for credit: 10, 22, 24, 28, 44, 56, 64, 94 and others]
Chapter 3 (17 questions)	4, 6, 14, 18, 26, 28, 34, 37, 50, 54, 56, 62, 66, 70, 78, 80, 90 [not for credit: 10, 12, 24, 30, 36, 38, 40, 52, 60, 64, 72, 76, 82 and others]
Chapter 4 (14 questions)	10, 15, 28, 38, 44 (Consider Ca(OH)₂ as soluble), 48, 52, 54, 58, 74, 82, 84, 90, 92 (& give the formula) [not for credit: 12, 14, 26, 30, 40, 42, 50, 78, 80, 88 and others]
Chapter 5 (15 questions)	18, 22, 24, 30, 36, 50, 61 (& Define), 65, 66, 71, 76 (& (e) Cu, (f) Cr - tricky! Write the shorthand notation. Label diamagnetic or paramagnetic. Which one exhibits the highest degree of paramagnetism?), 80, 88, 90, 92 [not for credit: 14, 20, 26, 38, 48, 62, 64, 68, 70, 74, 78, 82, 84, 86 and others]
Chapter 6 (7 questions)	6, 8, 10, 34, 41, 100. Arrange the following atoms or ions in order of increasing diameter and explain why briefly. (a) Ca, Mg, Sr (b) S^2-, Ar, Cl^- (c) P, Si, S, Al (d) Fe, Fe²⁺, Fe³⁺ (e) H, H⁺, H^- (f) F, Br, Te^2-, Se 101. Give examples and explain the following trends in the first ionization energy (a)across each period (include "dips" at IIIA and VIA elements for Periods 2 and 3 - see textbook), and (b) descending a periodic group. [not for credit: 14, 16, 20, 22, 28, 36, 38, 42 and others]
Chapter 7 (15 questions)	2, 6, 8, 16, 22, 46, 52, 64, 66, 74 100. Draw Lewis dot formulae for the following. Which violate the octet rule? (worth 5 points) Use the solution manual wisely, esp. the solutions to 34, 38, 40, 48, and 52 to help you. (a) H₂O (b) H₃O⁺ (c) HCN (d) NH₃ (e) AsF₃ (f) BeCl₂ (g) BCl₃ (h) PH₄⁺ (i) BrCl₂^- (j) SeF₄ (k) AsCl₄^- (l) ClF₃ (m) SeF₆ (n) IO₄^- (o) XeF₄ [not for credit: 8, 12, 16, 44, 50, 54, 62 and others]
Chapter 8 (6 questions)	50 (& Give the total number of sigma and pi bonds) 100. Consider the species listed in Exercise 100 in Ch. 7. For the central atom, give the number of regions of high electron density, the number of lone pairs, hybridization, electronic geometry and ideal bond angle(s). Determine the molecular or ionic geometry and polarity of the species. Use the Solution Manual wisely for help.. (worth 5 points) [not for credit: 2, 4, 14, 18, 20, 22, 24, 34, 44, 52, 54 and other problems]
Chapter 9 (1 question)	18 (& Are they diamagnetic or paramagnetic?) [not for credit: 12, 20, 22, 24, 26 and others]
Chapter 10 (11 questions)	6, 14, 20, 24, 26, 30, 44, 50, 58, 80, 86 [not for credit: 8, 18, 28, 44, 48, 54, 78, 84 and others]
Chapter 11 (14 questions)	4, 8, 24, 34, 36 (& normality), 42, 44, 46, 48, 52 (Hint: use normality), 56, 66, 70, 100. Consider the reaction: Cr + H⁺ Cr³⁺ + H₂ (unbalanced). How many grams of chromium will react with 75.0 mL of 0.100 N H₂SO₄. Note: in this example, H₂SO₄ is an oxidizing agent. [not for credit: 12, 32, 38, 54, 68 and others]
Chapter 12 (15 questions)	18, 28, 29 (& explain briefly), 34, 38, 41, 46, 52, 58, 64, 70, 76, 80, 88, 96 [not for credit: other relevant even problems]
Chapter 13 (9 questions)	10, 12, 20, 44, 46, 56, 60, 66, 68 [not for credit: 14, 18, 22, 26, 28, 34, 70 and others]
Chapter 14	[not for credit: 12, 34, 38, 40, 44, 52, 54, 68, 70, 80, 84]

Chapter 1	29. (a) 4.541 x 10⁴ cm³ (b) 5676 mL (c) 2.53 x 10⁵ in³ (d) 1.54 x 10⁵ mL
Chapter 2	19. (a) no (b) yes (c) no (d) no 37. (a) 2.02 mol P₄ (b) 1.21 x 10²⁴ molecules P₄ (c) 4.86 x 10²⁴ atoms P
Chapter 3	37. 27.8 % 53. 80.3 g NH₄Cl 65. 14.7 M H₃PO₄
Chapter 4	38. (a) occurs since CuS is insoluble salt molecular: Cu(NO₃)₂(aq) + Na₂S(aq) CuS(s) + 2NaNO₃(aq) total ionic: Cu²⁺(aq) + 2NO₃^-(aq) + 2Na⁺(aq) + S²^-(aq) CuS(s) + 2Na⁺(aq) + 2NO₃^-(aq) net ionic: Cu²⁺(aq) + S^2-(aq) CuS(s) since Na⁺ and NO₃- are spectator ions
Chapter 5	65. (a) n=1, l=0 (b) n=4, l=2, etc. 66. n=3 energy level has n²=9 orbitals and 2n²=18 electrons. E.g. the lowest energy level is n=3,l=0, m_l=0, an s orbital since l=0. 71. (a) m_s must be ą1/2 since 2 electrons in the same orbital cannot have the same spin (b) l must be 1, not 2 76. (a) paramagnetic (3 unpaired e-) (b) paramagnetic (2 unpaired e-) (c) diamagnetic (d) paramagnetic (2 unpaired e-) (e) paramagnetic (1 unpaired e-) (f) paramagnetic (6 unpaired e-)
Chapter 6	100. for example, (a) Mg > Ca> Sr
Chapter 7	17. (a) CaF₂ (b) SrCl₂ (c) K₂Se 100. Octet rule violaters: (f), (g), (i), (j), (k), (l), (m), and (o).
Chapter 11	100. 0.130 g
Chapter 12	29. (a) false (b) true (c) true (d) false (e) true 41. 2.69 x 10²² molecules