Download MIDTERM EXAM – JANUARY, 2003

CHEMISTRY Study Guide – JANUARY, 2014
Significant Figures, Metric System and Density
1. How many significant figures does 0.0530 have?
2. 2.61 x 10-3 written in the long form…
3. List the prefixes of metric units from largest to smallest?
4. Calculate the following (the answer must be in correct notation, round to 2 significant
figures):
2.1 x1024 x 6.3 x10-8
5. The fundamental unit of length in the metric system is the
6. 1.245633501 x 108 rounded to three significant figures is…
7. Write an example of a number in which the zero is NOT significant.
8. Write an example of a number in which the zero IS significant.
9. Using the rules for significant figures, the sum of 0.027 and 0.0023 should be expressed as…
10. What is the answer to the multiplication problem below, expressed with the proper
number of significant figures?
12 X 402 = ?
11. Place the following into correct scientific notation: 0.005060
12. How many grams are in 35 kilograms?
13. 3.2 mg is equal to how many grams?
14. The SI prefix that corresponds to a factor of 10-3 is
15. The density of silver is 10.5 g/cm3. What is the volume of a piece of silver having a mass
of 31.5 grams? (Express your answer with the correct significant figures)
16. The correct mass of an object with a density of 4.50 g/cm3 and a volume of 12.0 cm3
is…(Express your answer with the correct significant figures)
Classification of Matter and Atomic Structure
17. What is an example of a pure substance?
18. Which group of elements would be unlikely to form any compounds? Name one.
19. Write an example of a formula of a compound?
20. Which subatomic particle has the smallest mass?
21. Which atomic particle determines the chemical behavior of an atom?
22. The mass number of an atom is always equal to the:
23. What is the total number of neutrons in an atom with an atomic number of 16 and
a mass number of 35?
24. The first person to devise something similar to the modern periodic table was
25. The ______________________ uncertainty principle states that it is impossible to
simultaneously know both the position and velocity of an electron.
26. Write a symbol for an isotope of strontium?
27. Write a symbol for an isotope of calcium?
28. What are three clues that a chemical reaction has taken place?
29. The symbol for sodium is
30. The atomic number of manganese is
31. What happens when a chemical change takes place?
32. An electrically neutral atom of mercury, with atomic number 80, has how many electrons?
33. sulfur-35 has more ______ than sulfur-32.
34. The atomic number for iron is
35. A neutral atom of magnesium contains ____ electrons.
36. What is the total number of electrons in a fluoride ion?
37. What are the characteristics of an element with 26 protons, 24 electrons, and a mass
number of 56?
38. What happens to the number of protons, neutrons and electrons as an Mg2+ ion becomes an
Mg0 atom?
39. How many protons, electrons, and neutrons, respectively, does 35S have?
40. What is an example of a binary compound?
Electron Configurations and Average Atomic Mass
41.
42.
43.
44.
The shape of a p orbital is
The maximum number of electrons allowed in each of the d orbitals is
Write an example of an incorrect designation for an atomic orbital?
A nitrogen atom needs to gain ______________ electrons to achieve a noble gas
configuration.
45. A calcium atom needs to lose ______________ electrons to achieve a noble gas
configuration.
46. The energy levels of the hydrogen atom (and all atoms) are _____________, meaning that
only certain discrete energy levels are allowed.
47. When electrons are shared unequally, chemists characterize the bond to be...
48. Which is the electron configuration of a neutral atom in the ground state with a total of
five valence electrons?
49. How many valence electrons does aluminum have?
50. How many valence electrons does fluorine have?
51. How many valence electrons does chlorine have?
52. How many valence electrons does every element in group 1 have?
53. Which atom in the ground state has three unpaired electrons in its outermost principal
energy level?
54. What is the total number of electrons found in the valence shell of a Group VI (or Group
16) element in the ground state?
55. Which sublevel has a total of 5 orbitals?
56. Which sublevel has a total of 3 orbitals?
57. Which sublevel has just 1 orbital?
58. Write an example of two atoms/ions with identical electron configurations?
59. Identify the following element based on its electron configuration: [Kr] 5s2
60. Identify the following element based on its electron configuration: [Ne] 3s23p5
61. Identify the following element based on its electron configuration: [Rn] 7s2
62. How many valence electrons does Boron have?
63. Write three examples of a correctly written noble gas shortcut electron configuration?
64. Boron has two naturally occurring isotopes: B-10 (abundance = 19.8%, atomic mass = 10.0
amu); B-11 (abundance = 80.2%, atomic mass = 11.0 amu). Calculate the average atomic
mass of boron.
Periodic Trends
65. The charge on an oxide ion would be
66. The charge on a magnesium ion would be
67. The charge on an iodide ion would be
68. The charge on an aluminum ion would be
69. Why do noble gases have low reactivity?
70. Name three elements that often form an anion?
71. Describe how atomic radius changes as you move down a group.
72. Describe how atomic radius changes as you move across a period from left to right.
73. Describe how ionization energy changes as you move across the periodic table.
74. Describe how electronegativity changes as you move across the periodic table.
75. The transition metals occupy the ______________ block of the periodic table
76. The alkali metals and alkaline earth metals occupy the ______________ block of the
periodic table
77. The name of the group which contains fluorine, chlorine, bromine, iodine, and astatine is
78. When they react chemically, the halogens (Group VII or 17) change in what way?
Naming, Bonding and Writing Chemical Formulas
79. Describe what happens to the electrons in each element when the compound, NaF is formed.
80. Atoms with almost identical electronegativity values are expected to form
81. Write an example of a compound thatcontains one or more covalent bonds?
82. Which elements are found as diatomic molecules?
83. The correct name for an aqueous solution of H2S would be
84. If an element from group 1 reacts with an element from group VII (or group 17), the bonds
would be characterized as…
85. Write an example of the formula for an ionic compound?
86. The charge on the hydroxide ion is
87. Sodium and phosphate would form which compound?
88. Write the correct formula for aluminum phosphate.
89. The name of the compound NH4Cl is
90. Draw a correct Lewis structure for a molecule of nitrogen gas (N2).
91. The binary compound CCl4 is called
92. The name of CuCl is
93. The name of Fe2O3 is
94. The name of CaSO4 is
95. The name of HCl (aq) is
96. What is true of a polar covalent bond?
97. The correct name for FeO is
98. Magnesium reacts with sulfur to form
99. The correct name for LiCl is
100. The correct name for P2O5 is
101. CO is the formula for
102. Describe the bonds, bond angles, polarity and shape for the compound, NH3?
103. The correct name for an aqueous solution of HBr is
104. The correct formula and charge for the permanganate ion would be
105. The formula (and charge) for the ammonium ion is
106. The name for the acid HNO3 is ______________.
Lewis Structures and VSEPR
107. Draw a correct Lewis dot diagram for each of the following elements.
(a)
F
(c)
S
(b)
Mg
(d)
Ca
What is the correct molecular structure for the given molecules below?
108.
109.
110.
111.
112.
113.
CO
NH3
CH4
H2S
H2O
SO42-
114. Write the correct Lewis dot structure for hydrosulfuric acid?
Classifying Reactions, Predicting Products and Balancing Equations
115. Write an equation that represents a decomposition reaction.
116. Write an equation that represents a cationic single replacement
117. Calcium carbide, CaC2, reacts with water to produce calcium hydroxide and
acetylene, C2H2. Write the balanced equation for this reaction.
118. Choose the correct products to complete the following equation.
Barium chloride + sodium sulfate 
?
119. An equation is balanced by
120. The unbalanced chemical equation for the reaction in which propane (C3H8)
burns in oxygen to form carbon dioxide is
121. A reaction that has two compounds as reactants and one compound as a
product might be described as a
122. A reaction that has one compound as a reactant and two compounds as
products might be described as a
123. When the equation NH3 + O2  N2 + H2O is completely balanced using the
smallest whole numbers, the coefficient of the N2 will be
124. When the following equation is completed and balanced, what is the sum of the
coefficients (include the unwritten coefficient 1 if any are present)?
Na + MgCl2 
125. Given the balanced equation:
2Na + 2H2O  2X + H2
What is the correct formula for the product represented by the letter X?
When the following equations are balanced using the smallest possible integers, what is the
number in front of the underlined substance in each case?
126. C3H8(g) +
127. Mg(s) +
O2(g)  CO2(g) + H2O(g)
HCl(aq)  MgCl2(aq) + H2(g)
128. Write a compound that would have a linear shape.
129. Write a compound thatwould have a trigonal pyramidal shape?
130. Write a compound that would have a bent shape?