V.E.CHEM1 SP17 Exam III final PDF

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Solano College Chem 1 Spring 2017 - Exam III Instructor: Dr. V. Eskandari Detach and Use the last two pages as scratch papers. Scientific Calculators are allowed. No additional materials may be used such as iphones, ipads, ipods during the examination. Multiple Choice Questions: There is only one possible correct answer. Mark the correct answer on your scantron and double check your answers. (3 points each) Long Answer Questions: You must show your work to receive full credit. Show how you set up the problem, even if you are merely plugging numbers into your calculator.

Part I: Multiple Choice Questions: 1) Energy that is associated with the position or composition of an object is called A) potential energy B) thermal energy C) kinetic energy D) chemical energy 2) Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as losing heat to the surroundings? A) q = +, w = + B) q = -, w = + C) q = - , w = D) q = +, w = E) None of these represent the system referenced above. 3) Calculate the amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 K to 385.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. A) 28.4 kJ

B) 57.0 kJ

C) 16.6 kJ

D) 73.6 kJ

E) 12.9 kJ

4) Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 ĺ&22 + 18 H2O

A) 1.26 x 104 kJ

B) 4.82 x 103 kJ

ǻ+rxn = -11018 kJ

C) 9.64 x 103 kJ

D) 4.82 kJ

8VHWKHǻ+f LQIRUPDWLRQSURYLGHGWRFDOFXODWHǻ+rxn for the following: ǻ+°f (kJ/mol) SO2Cl2(g) -364 H2O(l) -286 HCl(g) -92 H2SO4(l) -814

A) -256 kJ

SO2Cl2 (g) + 2 H22Oĺ+&OJ+2SO4(l)

B) -62 kJ

C) +161 kJ

D) -422 kJ

ǻ+rxn = ?

E) +800. kJ

8VHWKHLQIRUPDWLRQSURYLGHGWRGHWHUPLQHǻ+rxn for the following reaction: ǻ+°f (kJ/mol) CH4(g) -75 CCl4(g) -96 HCl(g) -92 Cl2 0

A) -389 kJ

CH4(g) + 4 Cl2Jĺ&&O4(g) + 4 HCl(g)

B) -113 kJ

C) -71 kJ

D) +79 kJ

ǻ+rxn = ?

E) +113 kJ

7) The number of cycles that pass through a stationary point is called A) median

B) wavelength

C) frequency

D) amplitude

E) area

8) Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays

radio waves

A) radio waves < gamma rays < ultraviolet light B) gamma rays < radio waves < ultraviolet light C) ultraviolet light < gamma rays < radio waves D) gamma rays < ultraviolet light < radio waves E) radio waves < ultraviolet light < gamma rays 9) Place the following types of electromagnetic radiation in order of increasing frequency. visible light

microwaves

A) visible light < X-rays < microwaves B) X-rays < microwaves < visible light C) X-rays < visible light < microwaves D) microwaves < X-rays < visible light E) microwaves < visible light < X-rays

X-rays

10) Which of the following colors of electromagnetic radiation has the shortest wavelength? A) green B) blueC) violet D) orange E) yellow 11) Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm. A) 3.32 × 1014 s-1 B) 1.98 × 1014 s-1 C) 2.20 × 1014 s-1 D) 5.05 × 1014 s-1 E) 4.55 × 1014 s-1 12) For n = 3, what are the possible sublevels? A) 0, 1 B) 0, 1,2, 3 C) 0, 1, 2 D) 0 13) What are the possible orbitals for n = 3? A) s, p, d B) s, p, d, f C) s, p D) s 14) Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. A) n = 2, l = 2, ml =0 B) n = 4, l = 3, ml =-2 C) n = 3, l = 2, ml =-3 D) n = 2, l = 2, ml =-1 E) n = 4, l = 2, ml =+4 15) Identify the correct values for a 2p sublevel. A) n = 1, l = 0, ml = 0 B) n = 3, l = 1, ml = 0 C) n = 4, l = -1, ml = -2 D) n = 2, l = 1, ml = 0 E) n = 2, l = 1, ml = -2 16) Identify the correct values for a 4f sublevel. A) n = 3, l = 1, ml = 0 B) n = 4, l = 3, ml = -2 C) n = 1, l = 0, ml = 0 D) n = 2, l = 0, ml = 0 E) n = 2, l = 1, ml = -2

17) Calculate the energy change associated with the transition from n=4 to n=1 in the hydrogen atom. A) -6.12 × 10-18 J B) -2.04 × 10-18 J C) +3.55 × 10-18 J D) +1.64 × 10-18 J E) +4.89 × 10-18 J 18) Calculate the wavelength of a baseball (m = 0.155 kg) moving at 32.5 m/s.(hint: De Broglie) A) 2.68 × 10-34 m B) 1.32 × 10-34 m C) 7.60 × 10-36 m D) 3.57 × 10-32 m E) 2.15 × 10-32 m 19) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom. A) n = 3, l = 0, ml = 1, ms = B) n = 2, l = 1, ml = 1, ms = C) n = 3, l = 2, ml =1 , ms = + D) n = 3, l = 1, ml = 1, ms = + E) n = 3, l =2 , ml = 1, ms = 20) Give the number of core electrons for O. A) 2 B) 3 C) 1 D) 4 E) 0 21) The complete electron configuration of gallium, element 31, is __________. A) 3s 43p9 B)

3p 104s23d3

C)

3p 64s43d3 3p 84s3 3d104s24p1

D) E)

22) The condensed electron configuration of krypton, element 36, is __________. A) [Ar]4s4 B) [Ar]4s43d4 C) [Ar]3d104s24p6 D) [Kr]4s23d8 E) [Kr]4s43d8 23) Give the ground state electron configuration for Cd. A) [Kr]5s24d10 B) [Kr]5s25d10 C) [Kr]5s24d105p2 D) [Kr]5s24d8 E) [Kr]4d10 24) How many valence electrons does an atom of S have? A) 4 B) 1 C) 6 D) 3 E) 2 25) Place the following elements in order of increasing atomic radius. P A) P < Cl < Ba B) Ba < Cl < P C) Cl < P < Ba D) Cl < Ba < P E) Ba < P < Cl

Ba

Cl

Part II: Long Answer: Please show your work to receive full credit. Put your final answer in a box. 26. (3 pts) Complete the following statements; (no partial credit) a) When n =2, the value of l can be ______ and ________ b) Orbitals with l = 3 have max number of _________ electrons. c) When l = 2, the subshell is called a _________ subshell (orbital name) 27. (4 pts) Provide the trends of Zeff and Electronegativity across a row and down a group.

Zeff Increases or decreases across a row from left to right Zeff Increases or decreases down in a group from top to bottom Electronegativity Increases or decreases across a row from left to right Electronegativity Increases or decreases down in a group from top to bottom 28. (10 pts) Hess’s Law. Use the standard reaction enthalpies given below to determine ǻ+rxn for the following reaction: P4(g) + 10 Cl2(g) ĺ 4PCl5(s) ǻ+rxn = ? Given: PCl5(s) ĺ PCl3(g) + Cl2(g)

ǻ+rxn= +157 kJ

P4(g) + 6 Cl2(g) ĺ 4 PCl3(g)

ǻ+rxn

= -1207 kJ

29. (8 pts) Balance the following redox reaction if it occurs in acidic solution. Fe2+(aq) + MnO4ၱ(aq) ĺ Fe3+(aq) + Mn2+(aq)

Conversions: 1 atm = 14.7 psi = 101,325 Pa = 760 mmHg = 1.01325 bar = 760 Torr; 1in = 2.54 cm; 12 in = 1 ft °C + 273.15 = K Constants: c = 2.9979 x 108 m / s

h = 6.626 x 10-34 J.s

RH = 2.179 x 10-18 J

Equations and Various Tables: E= hC/ O 'x'p t

h 4S

C= QOq= mCp'T §1 1 · | 'E | RH ¨ 2  2 ¸ ¨ ni n f ¸ ¹ ©

O De Broglie wavelength

h mu

or

En= -2.18x10-18 j (1/nf2 – 1/ni2)

Key Atomic Number Symbol Atomic Mass Electronegativity

1

H 1.008 2.20

2

He 4.003 -

3

4

5

6

7

8

9

10

Li

Be

B

C

N

O

F

Ne

6.941 0.98

9.012 1.57

10.81 2.04

12.01 2.55

14.01 3.04

16.00 3.44

19.00 3.98

20.18 -

11

12

13

14

15

16

17

18

Na

Mg

Al

Si

P

S

Cl

Ar

22.99 0.93

24.31 1.31

26.98 1.61

28.09 1.90

30.97 2.19

32.06 2.58

35.45 3.16

39.95 36

19

20

21

22

23

24

25

26

27

28

29

30

31

32

33

34

35

K

Ca

Sc

Ti

V

Cr

Mn

Fe

Co

Ni

Cu

Zn

Ga

Ge

As

Se

Br

Kr

39.10 0.82

40.08 1.00

44.96 1.36

47.90 1.54

50.94 1.63

52.00 1.66

54.94 1.55

55.85 1.83

58.93 1.88

58.70 1.91

63.55 1.90

65.38 1.65

69.72 1.81

72.59 2.01

74.92 2.18

78.96 2.55

79.90 2.96

83.80 -

37

38

39

40

41

42

43

44

45

46

47

48

49

50

51

52

53

54

Rb

Sr

Y

Zr

Nb

Mo

Tc

Ru

Rh

Pd

Ag

Cd

In

Sn

Sb

Te

I

Xe

85.47 0.82

87.62 0.95

88.91 1.22

91.22 1.33

92.91 1.6

95.94 2.16

(98) 1.9

101.1 2.2

102.9 2.28

106.4 2.20

107.9 1.93

112.4 1.69

114.8 1.78

118.7 1.96

121.8 2.05

127.6 2.1

126.9 2.66

131.3 -

55

56

71

72

73

74

75

76

77

78

79

80

81

82

83

84

85

86

Cs

Ba

Lu

Hf

Ta

W

Re

Os

Ir

Pt

Au

Hg

Tl

Pb

Bi

Po

At

Rn

132.9 0.79

137.3 0.89

175.0 1.27

178.5 1.3

180.9 1.5

183.9 2.36

186.2 1.9

190.2 2.2

192.2 2.20

195.1 2.28

197.0 2.54

200.6 2.00

204.4 2.04

207.2 2.33

209.0 2.02

(209) 2.0

(210) 2.2

(222) -

87

88

103

104

105

106

107

Fr

Ra

Lr

Unq

Unp

Unh

Uns

Une

(223) 0.7

(226) 0.9

(260) -

-

-

-

-

-

57

58

59

60

61

62

63

64

65

66

67

68

69

70

La

Ce

Pr

Nd

Pm

Sm

Eu

Gd

Tb

Dy

Ho

Er

Tm

Yb

138.9 1.10

140.1 1.12

140.9 1.13

144.2 1.14

(145) 1.13

150.4 1.17

152.0 1.2

157.3 1.20

158.9 1.2

162.5 1.22

164.9 1.23

167.3 1.24

168.9 1.25

173.0 1.1 102

109 -

89

90

91

92

93

94

95

96

97

98

99

100

101

Ac

Th

Pa

U

Np

Pu

Am

Cm

Bk

Cf

Es

Fm

Md

No

(227) 1.1

232.0 1.3

(231) 1.5

238.0 1.38

(237) 1.36

(244) 1.28

(243) 1.3

(247) 1.3

(247) 1.3

(251) 1.3

(252) 1.3

(257) 1.3

(258) 1.3

(259) 1.3...