ACADEMIC CHEMISTRY
FIRST SEMESTER EXAM REVIEW
2014-2015
Please bring with you to final exam:
Pencil and eraser (#2)
Calculator (if you have one – you may borrow one if needed) NO PHONES OR IPODS!!
You will be provided the following to take the test:
Periodic Table
The test is two parts - 35 multiple-choice questions completed on scantron and a 15 point free response
section. The percent grade you receive will be averaged with your second semester exam. This averaged
score will be your “Final Exam Score” as reported on your final report card and will count as 1/9 of your
course grade. This review sheet will give you an idea of what to study.
GOOD LUCK!!
1
Chapters 1-6:
Measurement and Numbers
Classification of Matter
Atomic Structure and Subatomic Particles
Electron Arrangements
The MOLE
The Periodic Table
Chemical Bonding
1. _______ The particles in a solid are
a. packed closely together
b. very far apart
c. constantly in motion
d. able to slide past each other
2.
Describe the gaseous state in terms of particles.
3. A horizontal row of blocks on the periodic table is called a(n) ___________________________
4. Complete the following matching section:
_____ Organic chemistry
A. Study of interrelationships between energy and matter
_____ Inorganic chemistry
B. Study of substances containing carbon
_____ Physical chemistry
C. Study of processes that occur in living things
_____ Analytical chemistry
D. Study of substances that do not contain carbon
_____ Biochemistry
E. Identification of substances and determination of the composition
5. Complete the following table with the proper names and symbols:
NAME
SYMBOL
aluminum
Ca
Mn
nickel
phosphorus
cobalt
Si
H
2
6.
Make the following conversions:
105 mL = _________ dL
1.6x103 m = _______ mm
0.37 g = _________kg
0.58 cm = ___________ mm
2.4 L = __________mL
.
7. 30 degrees Celsius = __________ Kelvin
8.
_______ Water freezes at
a. 273.15 K
b. 100 degrees C
c. 0 K
d. 373.15 K
9.
How many sig figs in each of the following numbers?
0.305 000 kg________
30.00dL _________
32.2 m _______
210 g _______
140. 020 km _______
10. Complete the following calculations. Use the proper number of sig figs in your answers.
1.27 * 1.3 * 2.5 =
214.53 + 32 =
666/3 =
4.5x103 x 3.9x10-2 =
11. Write each number in scientific notation:
0.000000035 =__________________
0.0930 = _______________
5900 = __________________
12. How many minutes are in two weeks? Show all work.
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13.
2 days = ? seconds
14. $222 = ? pennies
15. 5672 sec = ? days
16. Isotopes are atoms of the same element that have different ________________.
17. Fill in the following table about isotopes:
Name
Nuclear
Symbol
Atomic
Number
Mass
Number
6
12
Number of
Protons
Number of
Neutrons
Number of
Electrons
Uranium-235
18. _______ The atomic number of oxygen, 8, indicates that there are eight
a. protons in the nucleus of an oxygen atom
b. oxygen nuclides
c. neutrons outside the oxygen atom’s nucleus
d. energy levels moving about each nucleus
19. Convert the following:
a. 0.34mol H2O = ?g H2O
b. 4.56g NaCl = ?mol NaCl
c. 3.2x1023part HCl = ?mol HCl
d. 2.73g AgNO3 = ?part AgNO3
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20. The maximum number of electrons that can occupy the s orbitals at each energy level is _______.
21. At n= 1 the total number of electrons that could be found is ________.
22. The element with the electron configuration 1s22s22p63s23p2 is __________.
23. _______ In the correct electron dot notation for sulfur, the symbol S is surrounded by
a. three pairs of dots
b. two pairs of dots and two single dots
c. four single dots
d. two pairs of dots
24. The electron dot notation for an element in the third period is represented by a symbol surrounded by
a pair of dots and a single dot. Write the complete electron configuration for this element.
25. The electron configuration for the an atom is 1s22s22p2 . What is the atomic number of the element?
______
26. Write the electron configuration for the following: (long or short form)
a. N
b. Br
c. Ag
d. Ba
27. A(n) _________________ is a horizontal row of blocks on the periodic table.
28. _______ Elements in which the d-sublevel is being filled have the properties of
a. Metals
b. Nonmetals
c. Metalloids
d. Gases
29. _______ For Groups 13 through 18, the total number of electrons in the highest occupied level equals
the group number
a. plus 1
b. minus 1
c. plus 10
d. minus 10
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30. Aluminum has the electron configuration [Ne]3s23p1. Aluminum is in period _______.
31. The elements that border the zigzag line on the periodic table are called the
______________________.
32. The elements characterized by the electron configuration s2p5 in the highest occupied energy level
belong to group ______________.
33. Strontium’s highest occupied energy level is 5s2. Strontium belongs to group ________.
34. Oxygen must gain _________ electron(s) to form an ion with a charge of -2.
35. _______ A covalent bond consists of
a. a shared electron
b. a shared electron pair
c. two electrovalent ions
d. an octet of electrons
36. A covalent bond in which there is an unequal attraction for the shared electrons is _______________.
37. _______ A nonpolar covalent bond is likely to exist between
a. a metal and a nonmetal
b. two ions
c. two identical atoms
d. an atom and an ion
38. How many double bonds are in the Lewis structure for HF? ___________
39. How many double bonds are in the Lewis Structure of CO2? _________
40. _______ In metals, the valence electrons are considered to be
a. attached to particular positive ions
b. in an electron sea
c. Immobile
d. involved in covalent bonds
41. _______ The structure of the methane molecule (CH4) is described as
a. Square
b. pyramidal
c. pentagonal
d. tetrahedral
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42. Draw the ionic dot diagram for the combination of Al & O.
43. Draw the Lewis Structure for H2S.
a. What is the shape of a H2S molecule?
b. Is H2S a dipole, NPWPS, or nonpolar molecule?
44. Draw the Lewis Structure for CCl4.
a. What is the shape of a H2S molecule?
b. Is H2S a dipole, NPWPS, or nonpolar molecule?
7
ACADEMIC CHEMISTRY
SECOND SEMESTER EXAM REVIEW
2014-2015
Please bring with you to final exam:
Pencil and eraser (#2)
Calculator (if you have one – you may borrow one if needed) NO PHONES OR IPODS!!
You will be provided the following to take the test:
Periodic Table
Equation card
The test is two parts - 35 multiple-choice questions completed on scantron and a 15 point free
response section. The percent grade you receive will be averaged with your first semester exam.
This averaged score will be your “Final Exam Score” as reported on your final report card and will
count as 1/9 of your course grade. This review sheet will give you an idea of what to study.
GOOD LUCK!!
8
Chapter 7-9:
Formula Writing and Naming Chemical Compounds
Calculations involving Chemical Formulas (Molar Mass, Moles, % composition)
Empirical and Molecular Formulas
Chemical Reactions and Equations
Stoichiometry
1.
Name the following ions:
CO3-2
Ca+2
SO4-2
Mn+2
P-3
Au+3
Cl-1
Pb+2
+1
H
2.
Write the name for these IONIC compounds (criss-cross charges!!):
MgCl2
Na2SO4
HNO3
K2S
Ni3(PO4)2
3.
Write the name for these MOLECULAR compounds (use prefixes!!):
P3Cl5
C2H6
CBr4
4.
Write the formulas for these IONIC compounds:
Potassium hydroxide
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Calcium phosphate
Sodium bromate
Iron (II) sulfide
Iron (III) sulfate
5. Write the formulas for these MOLECULAR compounds:
Dicarbon dioxide
Dihydrogen monoxide
6.
Calculate the molar mass for:
MgCl2
Na2SO4
HNO3
K2S
Ni3(PO4)2
7.
Perform the following calculations:
6.8 g MgCl2 = ? mol MgCl2
2.1 mol MgCl2 = ? g MgCl2
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MATCHING (#47-54)
47. _____ Nitrate
A. SO4-2
48. _____ Ammonium ion
B. Fe+3
49. _____ Hydroxide
C. Cl-1
50. _____ Calcium ion
D. OH-1
51. _____ Sulfate
E. NH4+1
52. _____ Iron (II) ion
F. Fe+2
53. _____ Chloride
G. NO3-1
54. _____ Iron (III) ion
H. Ca+2
For 55-58, identify the name or the formula for the following chemical compounds:
55. _______ Calcium hydroxide
a. CaOH
b. CaOH2
c. Ca(OH)2
56. _______ Magnesium oxide
a. MgO
b. MgO2
c. Mg2O
57. _______ Iodine Gas
a. I
b. I2
c. I3
58. _______ HF
a. hydrofluoric acid
b. monohydrogen monofluoride
c. dihydrogen difluoride
For #59-64, write the balanced equation and state which type of reaction it is.
59. Aluminum metal + Copper(II) nitrate  Copper metal + Aluminum nitrate
60. Magnesium oxide  Magnesium metal + Oxygen gas
61. Iron (II) sulfide + Hydrogen chloride  Hydrogen sulfide + Iron (II) chloride
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64. Hydrogen gas + Oxygen gas  Water
65. Predict the products and balance the following double displacement equation:
CuSO4 + AgNO3 
Chapter 10-19:
Properties of Gases and the Gas Laws
Gas Stoichiometry
Properties of Solids and Liquids
Solutions
Acids and Bases
Thermochemistry (Calculate ΔH)
Redox Reactions
66. Balance the following equation and fill in the blanks.

Hg (s) +
O2 (g)
HgO(s)
27.8 g
______mol
______mol
_____g
68.5 g
_______g
_____g
32.6 L at STP
_______g
_____g
32.6 L at 20 oC
& 754 mmHg
_______g
67. Use arrows to explain the following relationships:
V_____ , P _____
T _____, V _____
moles _____, V _____
68. 1.1 atm = _________mmHg
69. 777 mmHg = _____atm
70. 104.1 kPa = _____atm
71. 101.5 kPa = _____mmHg
72. A gas occupies 300 mL at 25oC and 1.1 atm. What volume would it have at STP?
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73. A gas occupies 1.1 L at 18oC and 774 mmHg. What temperature would be required to yield 1.5 L and 780
mmHg?
74. What temperature is necessary for 1.5 mol of a gas to occupy 300 mL at 1.2 atm?
75. 18.8 g Oxygen gas occupies what volume at 780 mmHg and 25oC?
76. Explain the effect of increasing atmospheric pressure on boiling point.
77. Define:
Solute=
Solvent=
Solution=
Soluble=
78. Calculate the molarity of 3.5 L of solution containing 2.5 moles NaOH.
79. How many grams of NaOH are needed for 2.0 L of a 4.0 M solution?
80. Calculate the molality of a solution made from 3.6 g NaCl and 200 g H2O.
81. How many grams of NaCl would you need to make a 4.8 m solution with 600 g H2O?
82. T or F: Acids have a high pH and a high [H+].
83. What is the pH, pOH, and [OH-] of a solution containing 1.3 x10-7 M H3O+?
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84. Define thermochemistry.
85. What is the sign (+ or -) of the ∆H value of an exothermic reaction?
86. Calculate the ∆H of the following reaction using the given ∆H of formations.
2 B5H9 + 12 O2  5 B2O3 + 9 H2O
∆Hf B5H9 = 73.2 kJ/mol
∆Hf O2 = 0 kJ/mol
∆Hf B2O3 = -1263.6 kJ/mol
∆Hf H2O = -285.8 kJ/mol
87. Assign oxidation numbers to all of the atoms / ions in:
6 Li(s) + N2(g)
2 Li3N(s)
88. Which element from the previous question was oxidized?
89. Assign oxidation numbers to all of the atoms in:
a.
Sodium ion
b.
NaNO3
c.
HCl
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