1. Br2(l) ΔHf◦ = ?
zero

2. 2A  2C ∆H=+40 C  A ∆H=?
-20

3. Al(s)  Al(l) ∆S = ? +, 0, or - +

4. Ln[A]
time
Rate = k[A]x What is x? 1

5. a.Ag(s) b.C3H8O(aq) c.Ca(NO3)2(s) Conducts electricity?

6. KNO3(aq) Strong, weak, or non-electrolyte?

7. F S F
Bond angle?
104

8. Carbonate Shape?
Trigonal planar

9. SF4 and TeCl4 Shape?
seesaw

10. N2 vs. O2 Longer bond?
Oxygen

11. N2 vs. O2 Greater bond energy?
nitrogen

12. HBr vs. HI Stronger acid? HI

13. H2SeO4 vs. H2TeO4 Stronger acid?

14. 3A + C  2B ΔH=+8kJ If heat is added, K will a. increase b. decrease c
3A + C  2B ΔH=+8kJ If heat is added, K will a. increase b. decrease c. stay the same A

15. HF(aq) Strong, weak, or non-electrolyte?

16. A ↔ B Q = 6.0 K = 2.2 Direction of Shift?
reverse

17. A ↔ B K = 4.2x1017 Which is there more of at equilibrium?

18. H2S or PF3 Which is polar?
both

19. Li+ + e-  Li E=-3. 05V Sn2+ + 2e-  Sn E=-
Li+ + e-  Li E=-3.05V Sn2+ + 2e-  Sn E=-.136V Which will be oxidized? Li

20. E- E- E-
KNO3(aq) A B
Cathode? A

21. A  2B If a catalyst is added, will reaction shift left or right?
Neither

22. 2A + B  2C + D If D is added at equilibrium, what happens to K?
nothing

23. 2A + B  2C + D If D is added at equilibrium, which way will reaction shift?
reverse

24. Al  Al+ + e- Ga Ga+ + e- Greater Ionization Energy?

25. O2-, F- and Ne These are all ____________.
isoelectronic

26. PbI2(s) ↔ Pb2+ + 2I- Ksp expression?

27. O or F Higher effective nuclear charge?

28. K or Ca Greater nuclear shielding?
equal

29. AX5 Shape?
Trigonal bipyramidal

30. C – C, C=C, C=C Longest bond?

31. ΔH=+ and ΔS=+ When is it spontaneous?
Only at high temps

32. rate=k[A]2[B] Reaction order?3

33. Ln[A]
time
Is this 1st order? no

34. H
H C O H
Type of IMF?
Hydrogen bonds

35. Bond angle between Br atoms?Cl Br S
Bond angle between Br atoms?
<120, <180

36. Cl Br S
Polar or nonpolar?
polar

37. CsI or LiCl Higher melting point?

38. 1 2
Which is catalyzed? 2

39. A + B  C + E slow E + A  C + D fast rate law?
Rate = k[A][B]

40. A + B  C + E slow E + A  C + D fast overall reaction?

41. A + B  C + E fast E + A  C + D slow rate law?
Rate = k[A]2[B]

42. Rate = k[A]2 What’s on the y-axis?
time
Rate = k[A]2 What’s on the y-axis?
1/[A]

43. Larger specific heat capacity?
30 g A
10 g A
Larger specific heat capacity?
Same

44. Si or Ge less electronegative?

45. Mg or Na Higher 2nd Ionization Energy?

46. N2O5 + H2O  ?
HNO3

47. a.Zn(NO3)2(s) b.CCl4(g) c.MgF2(l) Conducts electricity?
none

48. C2O5 + H2O  ? Acidic or Basic
acidic

49. H C N
Number of pi bonds? 2

50. Temp. X
time
Solid, liquid, or gas?
Both liquid and solid

51. Temp Pressure a. High High b. Low High c. High Low d
Temp Pressure a. High High b. Low High c. High Low d. Low Low Largest deviation from ideal gas behavior? b

52. Ksp = 3.1 x 10-7 Q = 4.8 x 10-10 Unsaturated, saturated, or supersaturated?

53. 2Al + 3Cu2+  2Al3+ + 3Cu n = ? 6

54. [Kr]5s24d105p1 Number of valence electrons?3

55. X D X C pH B X X A
time
Buffer region?
A-C

56. Ag+(aq) + Cl-(aq) AgCl(s) ∆S = + or -?

57. I2(g) I2(s) ∆H = +, 0, or -? -

58. CO CO2 O3 Which has a coordinate covalent bond?

59. CCl4 PBr5 H2S Which one is polar?

60. Cu(s) Metallic, ionic, molecular covalent, or network covalent bonds?

61. K2CO3(s) Metallic, ionic, molecular covalent, or network covalent bonds?

62. e-
Light will be _______.
emitted

63. rate = k[A]2 units on k?
M-1s-1

64. H + H  H H ΔH = + or -? -

65. N2O4(g)  2NO2(g) ΔS = + or -? +

66. Rate = k[NO] What’s on the y-axis?
time
Rate = k[NO] What’s on the y-axis?
Ln[NO]

67. Energy
Is ∆H + or -?
Time +

68. Na(s) ΔH˚f = ?

69. H2O + CO2  ?
H2CO3

70. H2O or CO2 Which contains POLAR bonds?
Both

71. SO2 Oxidation number of sulfur?+4

72. 2Al + 3CuCl2  2AlCl3 + 3Cu What is reduced?

73. X D X C pH B X X A
time
Where is [HA] greatest? A

74. X D X C pH B X X A
time
Equivalence Point? C

75. _________ acid titrated with strong base?X D
8.9 X C pH B X X A
time
_________ acid titrated with strong base?
weak

76. Strong acid titrated with strong base. pH at equivalence point = ?X D X C pH B X X A
time
Strong acid titrated with strong base. pH at equivalence point = ? 7

77. pH is 3.0 What is [HNO3]?
1x10-3M

78. pH is 3.0 What is [NaOH]?
1x10-11M

79. pH is 3.0 Ka = 1x10-4 What is [HA]?
1x10-2M

80. [HA] = 3.0 M [HX] = 3.0 M How do pH values compare?
pH of HX is greater than pH of HA

81. Na or Mg Which is has a larger radius?

82. F or O Which is has a larger radius?

83. Exothermic Sign on ΔH?
negative

84. Breaking Bonds Endothermic or Exothermic?

85. 1 mol H2
1 mol N2
at STP
Total Volume?
44.8 L

86. C4H10 Empirical Formula?
C2H5

87. 1 mol H2
1 mol N2
at 25˚C
Which is faster? H2

88. 1 mol H2
1 mol N2
at 25˚C
Which has more energy?
Equal energy

89. 1 mol H2
1 mol N2
2 Liters at 27˚C
Total Pressure?
About 30 atm

90. a.Zn(NO3)2 b.NH4Br c.MgF2 Dissolves in water?
All of them

91. 2CH4  2C +4H2 ΔH = ? Bond Bond Dissociation Energy (kJ/mol) C-H 400
450
2CH4  2C +4H2 ΔH = ?
1400 kJ

92. C2H2 Oxidation number of Carbon?-1

93. CaH2 Oxidation number of Hydrogen?-1

94. 3 moles in 6 liters Molarity?

95. Na2S + Li  Li2S + Na Sum of coefficients?6

96. Na2S + 2Li  Li2S + 2Na Limiting Reactant?
2 mol 3 mol
Na2S + 2Li  Li2S + 2Na Limiting Reactant? Li

97. Na2S + 2Li  Li2S + 2Na Moles of Na that form?
2 mol 3 mol
Na2S + 2Li  Li2S + 2Na Moles of Na that form? 3

98. Na2S + 2Li  Li2S + 2Na Moles of Li2S that form?
2 mol 3 mol
Na2S + 2Li  Li2S + 2Na Moles of Li2S that form?
1.5

99. Na2S + 2Li  Li2S + 2Na Excess moles of Na2S?
2 mol 3 mol
Na2S + 2Li  Li2S + 2Na Excess moles of Na2S?
0.5 moles

100. C2O42- Oxidation number of carbon?+3

101. HNO3 Oxidation number of nitrogen?+5

102. a.HNO3 b.H2SO3 c.H2CO3 d.NH4OH Forms a gas?
All except a

103. a.HClO4 b.H2SO3 c.H2CO3 d.HF Strong Acid?

104. Ca3PO Name?
Calcium phosphate

105. NaOH(aq) Spectator Ion?

106. NaOH(aq) + HF(aq)  H2O(l) + NaF(aq) Color of spectator ion(s)?
green

107. CsOH(aq) + Ca(NO3)2(aq)  Identify products?
Ca(OH)2 + CsNO3

108. CsOH(aq) + Ca(NO3)2(aq)  Ca(OH)2 + CsNO3 Identify precipitate?

109. pH = pOH?
10.16

110. 6 x 10-3/2 x Answer?
3 x 10-2

111. (3 x 10-3)(2 x 10-1) Answer?
6 x 10-4

112. 0.004/ Answer?
2 x 10-1

113. -log (1x10-6) Answer? 6

114. Ka = 1 x pKa? 4

115. Total pressure? PN2 = 3 atm O2(g) PO2 = 5 atm N2O4(g) PN2O4 = 4 atm
N2(g)
O2(g)
N2O4(g)
PN2 = 3 atm
PO2 = 5 atm
PN2O4 = 4 atm
Total pressure?
12 atm

116. Mole Fraction for N2? PN2 = 3 atm O2(g) PO2 = 5 atm N2O4(g)
N2(g)
O2(g)
N2O4(g)
PN2 = 3 atm
PO2 = 5 atm
PN2O4 = 4 atm
Mole Fraction for N2?
0.25

117. True or False: There are more moles of O2.
N2(g)
O2(g)
N2O4(g)
PN2 = 3 atm
PO2 = 5 atm
PN2O4 = 4 atm
True or False: There are more moles of O2.
True

118. If there is 1.0 mole of N2O4, how many moles of O2?
N2(g)
O2(g)
N2O4(g)
PN2 = 3 atm
PO2 = 5 atm
PN2O4 = 4 atm
If there is 1.0 mole of N2O4, how many moles of O2?
1.25 moles

119. Double the volume. What’s the total pressure?
N2(g)
O2(g)
N2O4(g)
PN2 = 3 atm
PO2 = 5 atm
PN2O4 = 4 atm
Double the volume. What’s the total pressure?
6 atm