Name: _______________________________________
Date: _______________
Chemistry Midterm Exam Review Sheet
Significant Figures
1. Identify the number of significant figures in the following measurements:
a. 1.00 g
b. 0.0035 g
c. 0.004500 g
d. 101 g
2. Perform the following operations. Keep the correct number of significant figures.
a. 4.56 cm x 9.1 cm
b. 20.0 / 4
c. 7.1 + 6.00
d. 8.0 - 4
Metric System
3. List the appropriate SI unit for the following measurements
a. Length
b. mass
c. volume
d. temperature
4. Why is the metric system used in science?
5. Perform the following unit conversions: Use the factor label (dimensional analysis) method.
a. 44 mm = __________ km
b. 15 lbs = _________ mg (1lb = 454 g)
c. 5.0 x 106 sec = _________ days
d. 14,110 ft = _________ m (1m = 1.0936 yards)
6. Describe how mass is measured.
7. Read the following balance
Name: _______________________________________
Date: _______________
8. List the equipment that can be used to measure volume.
9. Read the following graduated cylinder.
10. Describe how you could determine the volume of an irregularly shaped object.
Density
11. What is the formula for density?
12. What is the density of an unknown substance if the mass is 100g and the volume is 100 ml?
13. What is the volume of an object if its density is 1.0 g/cm3 and the mass is 150 g?
14. What is the mass of an object if its density is 4.5 g/ml and the volume is 75 ml?
Matter
15. State the law of conservation of mass.
16. Distinguish between the following word pairs (terms):
a. homogeneous mixture and heterogeneous mixture
b. element and compound
17. Identify the following as a heterogeneous mixture, compound, element, or homogeneous mixture:
a. salt water
b. gold
c. water
d. Italian dressing
Name: _______________________________________
Date: _______________
18. Distinguish between a physical and a chemical change.
19. Identify the following changes as physical or chemical:
a. water freezing
b. paper burning
c. wax melting
d. metal rusting
20. Identify the following properties as physical or chemical:
a. density
b. flammability
c. reactivity
d. temperature
21. Distinguish between an endothermic and an exothermic reaction.
Atoms, Electron Configurations, Periodic Table
22. What is an atom?
23. List the 2 parts of an atom.
24. List the 3 subatomic particles, their charges, and their location in the atom.
25. Who discovered the nucleus in the famous “gold foil” experiment?
26. Who proposed the first atomic theory in the 1800’s?
27. Who discovered the electron?
28. The atomic number provides what information?
29. What is the mass number equal to?
30. How are the numbers of neutrons determined?
31. How are the numbers of electrons determined?
32. Complete the following chart:
Element
Atomic #
Mass #
# Protons
# Electrons
12
6
Uranium
# Neutrons
Name: _______________________________________
Date: _______________
33. How are isotopes of an element different from each other?
34. Calculate the average atomic mass for element Z, if it has the following isotopes:
Z-56
Z-57
25%
75%
55.98 amu
56.99 amu
35. Why do elements lose or gain electrons?
36. Why do ions have a + or – charge?
37. How many electrons are lost or gained if an ion has the following charge:
a. +1
b. +2
c. +3
d. +4
e. –4
f. –3
g. –2
h. –1
38. What elements are “Stable”?
39. How many valence electrons are needed for an element to be considered stable?
40. How is the periodic table arranged?
41. Distinguish between groups and periods.
42. Give the group/family name for the following elements:
a. helium
b. bromine
c. calcium
d. copper
43. List the 4 sublevels that can be present in energy levels. Give the maximum number of electrons for
each sublevel.
44. Write the electron configurations for the following elements:
a. Carbon
b. calcium
c. bromine
d. iron
45. Identify the number of valence electrons present in the following elements:
a. Radium
b. Iodine
c. Cesium
d. Aluminum
e. vanadium
46. For the following periodic trends describe how they change for groups and periods.
a. Electronegativity ______ as you go across a period (left to right) and _______ as you go down a group.
b. Atomic size ________ as you go across a period (left to right) and ________ as you go down a group.
c. Atomic mass ________ as you go across a period (left to right) and ________ as you go down a group.
Name: _______________________________________
Date: _______________
d. Ionic radius ______________ when you remove electrons (cations are ____ than the neutral atom of
the same element). Ionic radius ___________ when you add electrons. (Anions are _______ than the
uncharged atoms of the same element.)
Bonding
Fill in the blank: Choose the word from the word bank below that completes the sentences.
Molecule
e-dot structure
stable
double bond
single bond
Valence e-
electronegativity
triple bond
ionic bond
covalent bond
Metallic
Van der Waals force
polar
nonpolar
ionic
Covalent
Dipole Interaction
Dispersion Force
47. ______________________ is the ability of an atom to attract e- to itself when bonded.
48. A _____________________ is made up of atoms that have covalent bonds.
49. A (n) _____________________ ___________________ forms when e- are transferred from 1 atom to
another.
50. Elements form bonds to become ______________________.
51. A (n) _________________ ___________________ forms when e- are shared between
52. An __________________ __________________ ________________ shows the number of valence e- in
an atom.
53. __________________ _____________________ are electron in the outer energy level of an atom.
54. A __________________ bond forms between 2 or more metals.
55. A ___________________ ________________ forms when 2 pairs of e- are shared.
56. A ___________________ ________________ forms when 1 pair of e- are shared.
57. A ___________________ ________________ forms when 3 pairs of e- are shared.
58. A ___________________ ________________ is an attraction between polar molecules.
59. A ___________________ ________________ is an attraction between nonpolar molecules.
60. A _______________________ bond results when e- are equally shared between atoms.
61. A _______________________ bonds when e- are unequally shared between atoms.
Name: _______________________________________
Date: _______________
62. Weak forces that hold molecules together are called intermolecular attractions or ____________
___________
_______________ ________________.
63. If the electronegativity difference between 2 atoms is greater than 1.70, a __________________ bond
will form.
64. If the electronegativity difference between 2 atoms is less than 1.70, a ____________________ bond
will form.
Short Answer
65. Draw an electron dot structure for the following then predict the oxidation number or charge:
a. Nitrogen
b. argon
c. magnesium
d. sodium
e. aluminum
f. sulfur
g. silicon
h. fluorine
66. Use the electronegativity to determine what type of bond will form for the following atoms. (ionic, Polar
Covalent, or Nonpolar Covalent).
a.
Br & Br
b. Zn & Cl
c. H & F
d. N & H
e. C & H
67. Determine the type of bond that will form between the following elements and then draw the electron
dot structure to show either ionic bonding or covalent bonding.
a. Sodium and chlorine
c. nitrogen and hydrogen
b. carbon and hydrogen
d. calcium and nitrogen
68. Using e- dot structures, predict the 3-D shapes of the following molecules.
a.
H2S
b. CCl4
c. H2
d. NH3
69. Determine if the following molecules are polar or nonpolar:
a.
Cl2
b. HBr
c. CHI3
d. H2O
e. CH4
Name: _______________________________________
Date: _______________
Naming Compounds / Writing Formulas
Ionic Compounds –
Name the following ionic compounds
70. CaBr2
__________________________
74. SnBr4 __________________________
71. KF
__________________________
75. Na2CO3 ________________________
72. Mn(OH)2 __________________________
76. Cu2O __________________________
73. BeS
77. PbCl2 __________________________
__________________________
Write the formulas for the following ionic compounds. (Make sure the charges add up to zero.)
78. Sodium fluoride
____________________
81. Iron (III) sulfate _____________________
79. Calcium nitrate
_____________________
82. Sodium bicarbonate __________________
80. Magnesium nitride _____________________
83. Lead (IV) Phosphate __________________
Molecular Compounds
Write the prefixes used for the following numbers:
84. 1 __________
87. 3 __________
90. 5 __________
85. 2 __________
88. 10 __________
91. 8 __________
86. 4 __________
89. 6 __________
92. 7 __________
Name the following molecular compounds:
93. CO2 _________________
95. N2O5 _________________
94. CCl4 _________________
96. NO2 _________________
Write the formulas for the following molecular compounds:
97. phosphorus trichloride _______
99. Tetraoxygen hexafluoride ________
98. silicon dioxide ________
100. Heptasulfur octaphosphide ______
Acids: Name the following acids
Write the formula for the following acids:
101. HCl _________________
104. nitrous acid _________________
102. H2SO4 _________________
105. phosphoric acid _________________
103. HNO3 _________________
106. hydrosulfuric acid _________________
Complete the following nuclear equations. Identify the type of radiation or identify the type of reaction.
107. 146C  0-1e + _________ Alpha
Beta
Gamma
108. 24294Pu 
109.
226
88Ra
238
92U
+ ______ Alpha
 ______ +
110. 4420Ca +
1
1H
→
44
0
21Sc
-1e
+ 00γ
Beta
Alpha
+ ________
111. 23592U + 10 n → 14455Cs + ______ + 2 10n
Gamma
Beta
Fission
Gamma
Fusion
Fission
Fusion
Other Important Concepts
112. Chapter 2 “Data Analysis”
a. Define percent error
b. Solve the following problem. Show all calculations. Express your answer with the correct number of significant figures.
A student measured a piece of steel pipe and found its length to be 5.4 m. The accepted length of the
steel pipe is 5.1m. Calculate the percent error.
113. Chapter 5: “Electrons in Atoms”
a. Define each of the following terms:
spectroscopy
quantum
photon
atomic emission spectrum
b. What is the difference between an atom’s ground state and an excited state?
c. Compare frequency and wavelength in electromagnetic energy.
114. Chapter 8: “Ionic Compounds”
Define each of the following terms:
Electron sea model
Delocalized electrons
Metallic bond
115. Know your safety rules
116. Scientific method
117. You are responsible for all vocabulary discussed from Chapters1-6 & 8-9