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Name:_________________
Chemistry Midterm Review 1999
1. A vapor is which state of matter?
2. All of the following are physical properties of a substance in the liquid state
EXCEPT_____.
3. A gas is a form of matter that ___________.
4. Which state of matter is characterized by having a definite shape and a definite
volume?
5. The chemical formula of a compound indicates the _______________.
6. What happens to the individual atoms in a chemical reaction?
7. Which of the following measurements contains two significant figures?
8. Express the sum of 7.68 m and 3.0 m using the correct number of significant digits.
9. Express the product of 4.0 X 10-2 m and 8.1 X 102 m using the correct number of
significant digits.
10. What is the SI unit of mass?
11. The density of a substance is found by dividing _______________.
12. What is the volume of 45.6 g of silver is the density of silver is 10.5 g/mL?
13. Which temperature scale has no negative temperatures?
14. Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees
Celsius?
15. How many joules are there in 115 calories? (1 cal = 4.18 J)
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16. Which of the following ratios is a correct conversion factor for changing kilometers
to meters?
17.A conversion factor factor __________________.
18.If the correct conversion factor is 1 L/ 1000 mL and the known measurement is 33
mL, what is the answer given by dimensional analysis?
19.What is the result of converting 67 mL to liters?
20.Five kilometers is equal to how many centimeters?
21.The number of seconds in an 8 hour day can be calculated as __________________.
22.The nucleus of an atom _____________________.
23.Which of these statements is FALSE?
24.The atomic number of an element is the total number of which particles in the
nucleus?
25.All atoms of the same element have the same _____________________.
26.The number of neutrons in the nucleus of an atoms can be calculated by __________.
27.Isotopes of the same element have different ____________________.
28. In which of the following is the number of neutrons correctly represented?
29. The number 84 in the name krypton-84 represents __________________.
30.Which of the following statements is true concerning molecular compounds?
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31.Which of the following formulas represents an ionic compound?
32. Molecular compounds are usually __________________.
33. Compounds that are composed of ions _________________.
34. Which of the following correctly represents an ion pair and the ionic compound the
ions form?
35. In which of the following are the names and formulas given correctly?
36. Which of the following compounds contains the lead (IV) ion?
37. The correct formula for barium chlorate is _________________.
38. Ternary ionic compounds contain three different _____________________.
39. When naming a transition metal that has more than one common ionic charge, the
numerical value of the charge is indicated by a ____________________.
40. What are the components of binary molecular compounds?
41. Which of the following is a binary molecular compound?
42. When naming acids, the prefix hydro- is used when the name of the acid anion ends
in _______________.
43. The SI unit that is used to measure the number of representative particles in a
substance is the ____________________.
44. How many moles of tungsten atoms are there in 4.8 x 1025 atoms of tungsten?
45. How many atoms are there in 5.20 mol of hafnium?
46. How many moles of helium atoms are there in 1.2 x 1024 helium atoms?
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47. How many atoms are there in 3.5 moles of arsenic atoms?
48. What is the gram formula mass of AuCl3?
49. How many grams are in 0.400 mol Pd?
50. The chemical formula of aspirin is C9H8O4. What is the mass of 0.40 mol of aspirin?
51. The volume of one mole of a substance is 22.4 L at STP for all ________________.
52. What is the volume, in liters, of 6.8 mol of Kr gas at STP?
53. What is the number of moles in 500 L of He gas at STP?
54. What is the volume, in liters, of 2.8 moles of NO2 gas at STP?
55. How many moles of Ar atoms are there in 202 L of Ar gas at STP?
56. The gram formula mass of a certain gas is 49 g. What is the density of the gas in g/L
at STP?
57. What is the mass of oxygen in 250 g of sulfuric acid, H2SO4?
58. If 20.0 grams of Ca combines completely with 16.0 grams of S to from a compound,
what is the percent composition of Ca in the compound?
59. What is the percent composition of carbon, in heptane, C7H16?
60. What is the chemical symbol for sodium?
61. What is the name of the element having to chemical symbol K?
62. What is the chemical symbol for copper?
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63. What is the chemical symbol for lead?
64. What is the name of the element having the chemical symbol Hg?
65. What is the chemical symbol for gold?
66. The nucleus of an atom is ___________________.
67. The element mercury has the atomic number 80. How many protons and electrons
are in a neutral mercury atom?
68. The atomic mass of an element ___________________.
69. Average relative atomic masses are are measured in ____________________.
70. Approximately how many elements exist?
71. Which of the following categories includes the majority of the elements?
72. Group A elements are known as the _____________________.
73. Which of the following is a nonmetal?
74. A column of elements in the periodic table is known as a ___________________.
75. What type of ions have names ending in –ide?
76. Ions form when atoms gain or lose _________________.
77. Which of the following formulas represents a molecular compound?
78. Ionic compounds are composed of ____________________.
79. The lowest whole-number ratio of ions in an ionic compound is called a (n)
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80. In which of the following are the symbol and name for the ion given correctly?
81. The charge on an ion of a Group 7A element is usually___________________.
82. Avogadro’s number of representative particles is equal to one_________________.
83. The names of all binary compounds, both ionic and molecular , end in ___________.
84. When naming acids, the prefix hydro- is used when the name of the acid anion ends
in _____________________.
85. The gram formula mass of a gas can be determined from ____________________.
86. All of the following are empirical formulas EXCEPT
87. The lowest whole-number ratio of the elements in a compound is called the
88. Which of the following is not an empirical formula?
89. What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by
weight?
90. Which of the following is an empirical formula?
91. A balanced chemical equation must have equal numbers of ________ on each side of
the arrow.
92. In the chemical equation:
H2O2  H2O + O2
Water is a __________.
93. The coefficients are missing from the skeleton equation below.
Cr (s) + Fe(NO3)2 (aq)
Fe(s) + Cr(NO3)3 (aq)
The correct order for the missing coefficients is_________.
94. The equation 2 C3H7OH + 9 O2  6 CO2 + 8 H2O is an example of which type of
reaction?
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95. The coefficients are missing from the following skeleton equation:
N2 + H2  NH3
The order of the missing coefficients is ______________.
96. Symbols used in chemical equations are shown below. Which set has the correct
symbol and explanation?
97. The activity series of metals tells us ____________.
98. When the following equation is balanced,
KClO3 (s)
KCl (s) + O2 (g)
The coefficient of KClO3 is __________.
99. The coefficients are missing from the following skeleton equation:
AlCl3 + NaOH
Al(OH)3 + NaCl
The order of the missing coefficients is ____________.
100. The coefficients are missing from the skeleton equation below.
Cr (s) + Fe(NO3)2 (aq)
Fe(s) + Cr(NO3)3 (aq)
The correct order for the missing coefficients is_________.