Name:__________________ Date:__________ Block:_______ Honor Code:___________
This assignment is to be completed individually by students to prepare for the midterm exam.
Midterm Review
Unit 1 – Measurement and Matter
1. Underline the number of significant figures in the following measurements.
a.
905.0 m
c.
80 kPa
b.
2071000 kg
d.
0.001030 L
2. Round the following measurements to the requested number of significant figures and put the
numbers in scientific notation.
a.
34890 km 2
c.
1000.0 mm 3
b.
0.0087998 3
d.
0.0000932 J 2
3. Perform the following conversions. Put your answers in scientific notation.
a.
4.5 x 1013 ns s
e.
2.73 kg mg
b.
8.9 L mL
f.
4.5 mm cm
c.
3.56 x 10-3 kJ J
g.
800 cm3 m3
d.
198000 pL mL
h.
0.044 L cm3
4. Show ALL work for the following problems and remember, your UNITS and SIGNIFICANT FIGURES.
a. A chemical compound has a density of 9.25 g/mL. What is the volume of 7.29 kg of the
compound?
b. If I am traveling 5.00m/s, how many miles will I travel in 29.2 hours?
(Note: 2.54 cm = 1 in, 1 ft = 12 in, 5280 ft = 1 mile)
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5. Classify the following materials as heterogeneous mixtures (M), homogeneous mixtures/solutions (S),
compounds (C), or elements (E).
a.
d.
g.
gravel
sodium chloride
Kool-aid
b.
e.
h.
24 carat gold
carbon tetrafluoride
plutonium
c. 14 carat gold
f. air
i. oil and water
6. Classify the following properties as chemical (C) or physical (P). If it is physical, identify if it is intensive
(I) or extensive (E).
a.
d.
g.
color
odor
phase (solid, liquid, gas)
b.
e.
h.
malleability
ductility
rusting
c. flammability
f. solubility
i. reacts with air
7. Classify the following as chemical (C) or physical (P) changes.
a.
c.
e.
g.
dissolving salt
rusting iron
cutting paper
distilling water
b.
d.
f.
h.
melting ice
baking a cake
sublimation of CO2
oxidizing metal
8. You are given the following mixtures, give the physical separation method(s) you would used to
separate as well as the reasoning.
a. Food Color Mixture
b. Acetone and Water (They have different boiling points)
c. Gravel, Salt and Oregano
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Unit 2 – Atomic History, Isotopes, Average Atomic Mass, Nuclear Decay, and Half-lifes
9. Be able to give the contributions of the following scientists: Chadwick, Democritus, Rutherford,
Thomson, and Dalton.
10. The element lead consists of four naturally occurring isotopes with masses of 203.97302, 205.97444,
206.97587, and 207.97663 amu. The percent abundances of these four isotopes are 1.40, 24.10,
22.10, and 52.42% respectively. Calculate the average atomic mass of lead.
11. Calculate the average atomic mass of the unknown element. Identify this element.
Isotope
X
Y
Z
Atomic Mass (amu)
23.9850423
24.9858374
25.9825937
Write the balanced equation for the following nuclear decay.
12. Positron emission of Carbon-14
13. Alpha decay of Astatine-196
14. Electron capture of Aluminum-26
15. Alpha decay of Platinum-192
16. Beta decay of Phosphorus-32
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Percent Abundance (%)
78.99
10.00
11.01
Show ALL work!
17. After 4 half-lives, what mass of a 64.00 mg sample is remaining?
18. Iodine-126 has a half-life of 13.0 days. A sample of iodine-126 was originally 42.00 kg. How much
remains after 936 hours have passed?
19. What fraction of a radioactive isotope remains if its half-life is 35 seconds and 7 minutes have passed?
Unit 3 – Orbital Diagrams, Electron Configurations, Oxidation States, Quantum Numbers, and the Periodic
Table
Give the Orbital Diagram for the following elements:
20. Chromium
21. Nitrogen
22. Tungsten
23. Krypton
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Give the COMPLETE electron configuration for the following elements:
24. Argon
25. Phosphorus
26. Iron
Give the electron configuration for the following elements using the noble gas short cut:
27. Neodymium
28. Mercury
29. Cadmium
Complete the table.
Element
Total # of
electrons
Valence
Configuration
Gain or
Lose e-
How
many?
Ion
Symbol
Selenium
Sodium
Beryllium
Iodine
Give the 4 quantum numbers for the last electron of the following elements:
30. Phosphorus
31. Manganese
32. Zinc
33. Americium
34. Astatine
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New Valence
Configuration
Total # of
e-
Give the element with the LARGER radius, ionization energy and electronegativity.
ELEMENTS
Phosphorus
and Chlorine
Oxygen and
Sulfur
Calcium and
Beryllium
Rubidium and
Strontium
ATOMIC RADIUS
IONIZATION ENERGY
ELECTRONEGATIVITY
35. Circle the element / ion with the larger radius.
a. Mg or Mg2+
b. S or S2-
c. N3- or N
d. Sr2+ or Br-
e. Cl- or Mg2+
f. B or F
36. Be familiar with the following groups: Alkali Metals, Alkaline Earth Metals, Transition Metals,
Halogens, and Noble Gases.
Unit 4 – Bonding and Nomenclature
Determine the formula for the compound formed by the two atoms and indicate if it is an ionic or covalent
compound.
37. Potassium and Oxygen
38. Oxygen and Fluorine
39. Aluminum and Sulfur
40. Phosphorus and Bromine
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41. Complete the table below.
Formula
Electron Dot Diagram
Bonding
Orbitals
Shape
Structural Formula
BCl3
H2 O
CH4
NH3
CO2
SF2
Draw the dot diagram (Lewis Structure) for the IONIC compounds below.
42. MgBr2
43. Na2S
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Polar?
Write the formula for the following compounds.
44. Sulfurous Acid
45. Tin (II) Fluoride
46. Potassium Permangante
47. Aluminum Hyponitrite
48. Chromous Acid
49. Lead (IV) Oxide
50. Mercury(II) Sulfide
51. Sodium Sulfite
52. Ammonium Phosphate
53. Iron (II) Nitrate
54. Calcium Perchromate
55. Hyposulfurous Acid
56. Iron (III) Sulfide
57. Titanium (III) Chlorate
58. Nickel (II) Hydroxide
59. H2SO4
60. Ra(C2H3O2)2
61. Ni(ClO)2
62. HNO3
63. H3P
64. H3PO4
65. HNO2
66. Fe(ClO4)3
67. KH
68. Ba(ClO2)2
69. SnO
70. H2SO3
71. ZnSO2
72. Al(ClO)3
73. HI
Name the following compounds.
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Unit 5 – Balancing Equations, Reactions, and Predicting Products
Balance the and identify following reactions as a single replacement (SR), double replacement (DR),
decomposition (DC), synthesis (SY) or combustion (C).
74. Na + Cl2 ⟶
NaCl
75.
H2O ⟶
H2 +
76.
C2H4 +
O2 ⟶
CO2 +
77.
AgNO3 +
Zn⟶
Ag +
78.
Ca(C2H3O2)2 +
O2
NaCl ⟶
H2O
Zn(NO3)2
NaC2H3O2 +
CaCl2
Write the balanced chemical equation for the following chemical reactions AND give the type of reaction
that has occurred.
79. Sodium metal is added to sulfuric acid (H2SO4). Hydrogen gas is produced, along with sodium sulfate.
80. White phosphorus (P4) reacts with chlorine to make phosphorus trichloride.
81. Magnesium chlorate, Mg(ClO3)2, is heated strongly until it decomposes into magnesium chloride and
oxygen gas.
82. Ammonium carbonate decomposes when heated to give ammonia gas, water vapor, and carbon
dioxide.
83. Solid sulfur (S8) is burned in air to make sulfur dioxide.
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Write the balanced equation for the following chemical reactions (you must predict the products) AND give
the type of reaction that has occurred.
84. Butane gas (C4H10) is burned completely in air.
85. Iron metal is added to bromine. (Hint: It will make an Iron (III) product
86. Solutions of lead (II) nitrate and potassium chloride are mixed together.
87. Rubbing alcohol, (CH3)2CHOH, is burned completely in air.
Write the balanced equation AND the state of the reactants (solid, liquid, gas, or aqueous).
88. A solution of hydrochloric acid is poured into a solution of calcium hydroxide.
89. Aluminum metal is added to a solution of iron (III) chloride.
90. A piece of iron metal is exposed to oxygen gas (Fe3+ product would form).
91. A solution of nitric acid is poured on solid sodium carbonate.
92. Calcium metal is added to water.
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