Name _____________________________________________________________________ Period _______
Chemistry Mid-Term Review
The midterm will consist of 50 multiple choice questions. Each question is worth one point. You will have
one period to complete the exam – it will be curved back to the highest score out of 50.
Match the following branches with their area of emphasis.
_____ 1. Analytical chemistry
a) Most carbon-containing chemicals
_____ 2. Biochemistry
b) Matter that does not contain carbon
_____ 3. Environmental chemistry
c) Behavior & changes of matter and related energy changes
_____ 4. Industrial chemistry
d) Components and composition of substances
_____ 5. Inorganic chemistry
e) Matter and processes of living organisms
_____ 6. Organic chemistry
f) Matter and the environment
_____ 7. Physical chemistry
g) Chemical processes in industry
_____ 8. Polymer chemistry
h) Polymers and plastics
_____ 9. Theoretical chemistry
i) Chemical interactions
_____ 10. Thermochemistry
j) Heat involved in chemical processes
Identify the components of scientific investigations in the following scenario
A student wants to investigate whether the time of day affects student performance in academic classes. She
thinks that students will get better grades in classes held in the afternoon. She collects the following data:
Average Grades
Time
Chemistry
World Cultures
CP English
Trig
nd
82%
86%
88%
81%
2 period
80%
86%
85%
80%
7th period
11. What is the hypothesis?
12. What is the independent variable?
13. What is the dependent variable?
14. What would need to be held constant in this experiment?
15. Is there a control?
16. What conclusion can be drawn from the data?
17. What type of graph would best represent this data?
18. Would this be an example of pure or applied research?
19. Name 3 pieces each of qualitative and quantitative data you could observe about a person.
Perform the following conversions:
20. 785 cg = _____________ kg
28. 678 cm3 = _____________ ft3
21. 9879 mm = _____________ nm
29. 98.4 lb/in2 = _____________ g/mm2
22. 5 g = _____________ pg
30. 30oC = _____________ K
23. 0.897 L = _____________ fL
31. 9 K = _____________ oC
24. 0.7809 Ms = _____________ ms
32. 50oC = _____________ oF
25. 78 m = _____________ inches
33. 80oF = _____________ oC
26. 9,789,000 mg = _____________ lb.
34. 560K = _____________ oF
27. 500.00 cm3 = _____________ gallons
35. 50oF = _____________ K
Put the following into correct scientific notation, keeping the number of sig figs the same.
36. 34,567,200 = _____________
37. 0.005600 = _____________
38. 6780.23 x 10-3 = _____________
39. 0.000087 x 10-9 = _____________
How many significant digits are in the following numbers?
40. 0.0000005 = _____________
41. 0.0000570 = _____________
42. 100000.0 = _____________
43. 30,000 = _____________
44. 400. = _____________
45. 3.0000 = _____________
Perform the following operations and report the answers to the correct number of significant digits.
46. 56.789 + 23.5 + 56.908765 + 32 = _____________
47. (56.878)(3.1)(3.0000) = _____________
48. (56.78 – 32) / 6.789 = _____________
Solve the following problems. Answers should be reported to the correct number of significant digits.
49. A gas has a density of 7.56 mg/L. If you have 5.4L of the gas, what is the mass of the gas you have?
50. An object has a mass of 67.8 kg and a density of 9.4 kg/m3. What is its volume?
51. An object has a mass of 679.09g and has a volume of 320 cm3. What is its density? If the accepted
value for the density of the substance is 2.25 g/cm3, what is the percent error of the experimental
density?
Measure the following objects.
52. _________________
53. _____________
54. _____________
55. Graph the following data and determine the slope of the best fit line, including a unit for your slope.
Mass (g)
Volume (mL)
0.0
0.0
6.3
3.0
10.8
5.0
21.5
10.0
Choose the properties that apply to each of the states of matter
56. Solid
Shape: definite
indefinite
Volume: definite
indefinite
57. Liquid
Shape: definite
indefinite
Volume: definite
indefinite
58. Gas
Shape: definite
indefinite
Volume: definite
indefinite
59. What is the difference between a gas and a vapor?
Label the following as elements, compounds, solutions, or heterogeneous mixtures.
60. chocolate chip cookie
61. oxygen gas
62. salt water
63. taco
64. gold
65. carbon dioxide
66. water
67. kool aid
E
E
E
E
E
E
E
E
C
C
C
C
C
C
C
C
S
S
S
S
S
S
S
S
HM
HM
HM
HM
HM
HM
HM
HM
68. table salt
69. muddy water
70. potassium
71. brass
72. graphite
73. glass
74. air
E
E
E
E
E
E
E
C
C
C
C
C
C
C
S
S
S
S
S
S
S
HM
HM
HM
HM
HM
HM
HM
Label the following as either intensive or extensive and as physical or chemical properties/changes.
75. mass
76. color
77. density
78. malleability
79. reactivity
80. luster
I
I
I
I
I
I
E
E
E
E
E
E
P
P
P
P
P
P
C
C
C
C
C
C
81. length
82. volume
83. solubility
84. boiling point
85. brittleness
86. flammability
I
I
I
I
I
I
E
E
E
E
E
E
P
P
P
P
P
P
C
C
C
C
C
C
Solve:
87. In a catalytic converter, found in a car exhaust systems, carbon monoxide (CO) reacts with oxygen
gas (O2) to form carbon dioxide gas (CO2). If CO reacts with 16g of O2 to form 44 g of CO2, what is
the mass of CO in the catalytic converter?
Match the following separation techniques with their description.
_____ 88. Chromatography
a) Uses a porous barrier to separate a solid from a liquid
_____ 89. Crystallization
b) Uses differences in boiling points to separate substances
_____ 90. Distillation
c) Results in pure solid particles of a substance from a solution of that substance
_____ 91. Filtration
d) Separates a mixture by allowing one solid to turn to a gas
_____ 92. Sublimation
e) Separates the components by their ability to travel or be drawn along a surface
Calculate:
93. Complete the table.
94. Are the compounds the same compound? If they are different, use the law of multiple proportions to
show the relationship between them.
What did each scientist do?
_____ 95.
Antoine Lavoisier
a) First modern atomic theory; definite proportions;
multiple proportions
_____ 96.
Aristotle
_____ 97.
Democritus
_____ 98.
Dmitri Mendeleev
_____ 99.
Enrico Fermi
_____ 100.
Ernest Rutherford
_____ 101.
Erwin Schrodinger
_____ 102.
Henry Mosely
_____ 103.
J.J. Thompson
_____ 104.
James Chadwick
_____ 105.
John Dalton
_____ 106.
John Newlands
_____ 107.
Lothar Meyer
j) Discovered the electron, cathode ray tube experiment;
Plum Pudding model
_____ 108.
Marie Curie
k) Discovered the nucleus; gold foil experiment
_____ 109.
Murray Gell-Mann
l) Studied the spectrum of hydrogen; solar system model
_____ 110.
Niels Bohr
m) Wave equation; Quantum Mechanical model
_____ 111.
Werner Heisenberg
n) Discovered the neutron
b) Atomic numbers
c) Everything is made of fire, air, earth, and water
d) All matter is made up of atomos
e) Law of octaves; properties repeat every 8 elements
f) Composed a list of all of the elements and grouped
them into 4 categories
g) Published a periodic table; did not predict
undiscovered elements
h) Published a periodic table; predicted undiscovered
elements
i) Discovered radium; studied radiation
o) The Uncertainty Principle; you cannot know the
energy and position of an electron at the same time
p) Nuclear fission
q) Discovered quarks
Complete the following table.
Element/Ion
Atomic
Number
Atomic
Mass
113.
85
207
85
114.
27
59
27
72
112.
Neutrons
Electrons
Ge
32
115.
7
133
116.
Calculate:
117.
Protons
8
10
Cs +
55
Three magnesium isotopes have atomic masses and relative abundances of 23.985 (78.99%),
24.986 (10.00%), and 25.982 (11.01%). Calculate the atomic mass of magnesium.
Write equations for the following nuclear reactions:
118.
Thorium undergoes beta decay.
119.
Uranium undergoes alpha decay while emitting 2 gamma rays.
What does each of the following stand for? Define each term and show what unit each has.




122.
c
123.
E
124.
h
Calculate:
125.
What is the wavelength of radiation with frequency of 4.5 x 1017 Hz?
126.
What is the energy of a photon of light that has a wavelength of 602 nm?
Draw an orbital diagram (arrows!) for each of the following elements.
127.
oxygen
128.
bromine
Write an electron configuration for each of the following elements.
129.
silicon
130.
tungsten
Write a condensed electron configuration for each of the following elements.
131.
arsenic
132.
uranium
Draw Electron Dot Symbols for the following:
133.
Li
134.
Si
135.
Cu
136.
O
137.
Ar
Name 2 elements in each of the following:
138.
139.
140.
141.
142.
143.
155.
Group 6
Period 4
Alkali metals
Alkaline Earths
Halogens
Metalloids
144.
145.
146.
Lanthanides
Actinides
Noble Gases
147.
Transition Metals
148.
149.
p-block
s-block
150.
151.
152.
153.
154.
d-block
f-block
diatomics
gases
liquids
Explain how the periodic table is arranged.
For each of the following, circle the atom that has the higher value for the given property.
Size
Ionization Energy
Electronegativity
156.
Mg or Ca
161.
Li or Be
166.
F or Cl
157.
C or O
162.
O or S
167.
Li or Be
158.
F or Ne
163.
K or Ca
168.
C or N
159.
Ne or Ar
164.
Ca or Mg
169.
N or P
160.
Ar or F
165.
Mg or K
170.
C or P
Write formulas for each of the following compounds.
171.
nickel (III) selenide
175. vanadium (III) thiocyanate
179.
cuprous iodide
172.
potassium hydroxide
176.
vanadium (II) peroxide
180.
magnesium oxide
173.
barium sulfite
177.
ammonium phosphate
174.
cobalt (II) phosphate
178.
chromium (II) thiosulfate
Write names for each of the following compounds.
181.
(NH4)2Se
185.
SnO
189.
Cu2O2
182.
Y2(Cr2O7)3
186.
Pb3P2
190.
Cr(H2PO4)3
183.
Sr(CN)2
187.
Pb(SO3)2
184.
K3PO4
188.
Au2Cr2O7
In each pair, circle the compound that has the strongest ionic bond.
191. Li2O or LiCl
194.
192. NaCl or CsI
193. BaS or CsCl
Describe metallic bonding and two properties of metals that rely on metallic bonding.