Name__________________________________________Date___________________Period____
PRE-AP CHEMISTRY FINAL REVIEW- Fall 2015
Measurement, Energy, and Matter (Units 1 & 2)

Orbital Diagrams

Lab Safety & MSDS (review your safety contract)

Valence Electrons/Dot Diagrams

Significant Figures

Frequency, wavelength, and energy calculations

Accuracy vs. precision

Types of Matter

Atomic size

Heat, including specific heat

Electronegativity

Law of Conservation of Mass/Matter

Ionization energy

Density

Metal and nonmetal reactivity

Ion size
Atomic Structure (Unit 3)
Periodic Table and Trends (Unit 5)

Atom

Ions

Covalent/Molecular Names and Formulas

Isotopes

Ionic Names and Formulas

Atomic Mass Calculations

Acid Names and Formulas

Nuclear Reactions and half-life

Properties of Ionic and Covalent compounds
Electrons (Unit 4)
Nomenclature (Unit 6)
Moles (Unit 7)
History of the atomic model (Bohr, Schrodinger,

Mole, Mass, Volume, and Particle conversions
etc!)

Percent composition

Orbitals, Sublevels, and Energy level basics

Empirical and Molecular Formulas

Electron Configurations

Reaction types and balancing (Unit 8)
*In order to use a 3x5 notecard (handwritten, notes on front side only, name on back) on the final exam,
you must have at least 90% of this review completed by the beginning of class on Monday, December 14.
**Make sure to SHOW WORK for any problems involving calculations in order to receive credit for your answers.
Measurement/Matter/Energy
1. Significant Figures Practice: How many significant figures are in the following?
a. 150 cm
_____
c. 728.0 mL
_____
b. 0.005740 g _____
d. 748.189 g _____
e.
0.00234 cm _____
e.
0.00234 cm
2.
Round the following values to only 2 sig figs. each.
a. 150 cm
c. 728.0 mL
b. 0.005740 g
d. 748.189 g
3.
Explain the difference between accuracy and precision.
4.
The correct value for the length of a metal rod is 22.6 cm. Which of the following sets of measurements of the rod
could be considered precise but not accurate?
a. 20.4 cm, 20.2 cm, 20.5 cm
c. 24.6 cm, 23.7 cm, 25.9 cm
b. 22.5 cm, 22.7 cm, 22.6 cm
d. 12.6 cm, 22.6 cm, 32.6 cm
5.
Classify each of the following as either physical (P) or chemical (C) properties.
a.
Blue color
c.
Flammability
b.
Density
d.
Solubility
6.
e.
Reacts with acid to form H2
j.
Hardness
f.
Combustion
k.
Boiling point
g.
Melting point
l.
Can neutralize an acid
h.
Reacts with water to form a gas
m. Luster
i.
Reacts with a base to form water
n.
Odor
Classify each of the following as either a physical (P) or chemical (C) change.
a.
Sodium hydroxide dissolves in water
g.
Milk sours.
b.
Chlorine and hydrogen react to produce
h.
Ice melting.
hydrochloric acid
i.
Sugar dissolves in water.
c.
A pellet of sodium is sliced in two.
j.
Wood rotting.
d.
Water vaporizes into steam.
k.
Mirror cracking.
e.
Iron rusts.
l.
Phase changes
f.
Evaporation.
7.
What are the four signs of a chemical change?
8.
What is the definition of a compound?
9.
Which of the following are pure substances: element, compound, homogeneous mixture, heterogeneous mixture?
10. Which of following can be separated by physical means: element, compound, or mixture?
11. The particle diagram to the right represents a sample of matter.
Which best describes the composition of the sample?
a. a mixture of compounds
b. a single compound
c. a single element
d. a mixture of elements and compounds
12. A student heats 35.0g of mercury (II) oxide. As it is heated, mercury (II) oxide decomposes and forms liquid mercury
and oxygen gas. If the student determines that the reaction yields 29.3g of mercury, how many grams of oxygen
should be produced?
mercury (II) oxide  mercury + oxygen
13. Calculate the density of an object with a mass of 45.0g and a volume of 25.0mL.
14. Calculate the mass of an object with a density of 2.0g/mL and a volume of 15.0mL.
15. What is specific heat?
16. How many joules are there in 245 calories? (1 cal = 4.18 J)
17. Your friend performed the Endothermic and Exothermic Reactions lab and
obtained the graph below for her first trial. Was her first experiment an
endothermic or exothermic reaction? Explain your answer.
18. Label the parts of this heating curve for
water.
19. Which phase changes are considered to be
exothermic? Endothermic? Why?
20. The specific heat of concrete is greater than that of soil. Given this fact, would you expect a major-league baseball field
or the parking lot that surrounds it to cool off more in the evening following a sunny day? Explain.
21. The specific heat of alcohol is about half that of water. Suppose you have 500 mL of alcohol at a temperature of 10°C in
one container, and 500 mL of water at a temperature of 80°C in a second container. When these fluids are poured into
the same container, and allowed to come to thermal equilibrium, is the final temperature closer to the alcohol or water?
Explain.
22. In an endothermic reaction, heat is ABSORBED / RELEASED by the system. As a result, the system will have
MORE / LESS energy than it did originally and the surroundings will have MORE / LESS energy. This will
cause an endothermic reaction to feel
HOT / COLD.
23. In an exothermic reaction, heat is
ABSORBED / RELEASED by the system. As a result, the system will have
MORE / LESS energy than it did originally and the surroundings will have MORE / LESS energy. This will
cause an exothermic reaction to feel
HOT / COLD.
Atomic Structure
24. What number identifies an element? _______________________________
25. What particle is represented by the atomic number? _______________________________
26. What particles are represented in the mass number? _______________________________
27. An ion is a charged particle that has lost or gained _____________________.
28. What is an isotope?
29. How many protons are present in carbon-12? __________ neutrons? __________
30. How many protons are present in carbon-13? __________ neutrons? __________
31. Chlorine-37 can be represented as
a.
b.
17
37
Cl
c.
37
17
Cl
35
20
Cl
37
35
Cl
d.
32. The diagram to the right represents the nucleus of an atom.
What are the atomic number and mass number of this atom?
a. The atomic number is 9 and the mass number is 19.
b. The atomic number is 9 and the mass number is 20.
c.
The atomic number is 11 and the mass number is 19.
d. The atomic number is 11 and the mass number is 20.
33. Which represents the most abundant isotope of sodium?
a. sodium-11
b. sodium-22
c. sodium-23
d. sodium-24
34. What is the total number of electrons in an Mg2+ ion? _________
35. What is the total number of neutrons in an atom of 26 Fe ? _________
57
36. Which phrase describes an atom?
A) a positively charged electron cloud surrounding a positively charged nucleus
B) a positively charged electron cloud surrounding a negatively charged nucleus
C) a negatively charged electron cloud surrounding a positively charged nucleus
D) a negatively charged electron cloud surrounding a negatively charged nucleus
37. Complete the following table.
Complete
Atomic
Mass
Symbol
Number
Number
Protons
Neutrons
Electrons
Charge
41
19
K
12
23
11
14
Na 
33
18
-3
38. What are the units for atomic mass? _________________
39. Showing all your work, calculate the atomic mass for the following element. Identify this element.
Isotope
Mass
Percent
(amu)
Abundance
Isotope #1
27.98
92.22%
Isotope #2
28.98
4.69%
Isotope #3
29.97
3.09%
40. What is half-life?
41. Which type of radiation is most difficult to shield (block)? ____________________________
42. What particle is needed to complete this nuclear reaction?
222
86
Rn
------->
218
84
Po
+ ?
43. Describe how α, β, and γ rays each behave when they pass
through an electric field.
a) α toward +, β toward -, γ straight
b) α toward -, β toward +, γ straight
c) α straight, β toward +, γ toward –
d) α toward -, β straight, γ toward +
Radioactive source
+
_
44. When the following nuclear reaction is complete, the missing numbers for U and for Th are:
?
92
231
4
?Th
2 He
------->
+
45. Which type of nuclear reaction results in a “splitting” of atoms? ______________________
U
46. Which type of nuclear reaction results in the “formation” of atoms? ______________________
47. Fill out the following table:
Type of particle
Alpha
Beta
Gamma
Symbol
Mass
Charge
Nomenclature
48. Classify the following compounds as ionic, covalent (molecular) or acid and then write the name or formula.
a.
Na2O
g.
phosphoric acid
b.
NO
h.
chromium(III) oxide
c.
PbSO4
i.
sulfur trioxide
d.
Al2(CO3)3
j.
pentaphosphorus decoxide
e.
N 2 O4
k.
ammonium cyanide
f.
HCl
l.
hydrosulfuric acid
Moles
49. What is the molar mass of BaCO3?
50. List all seven diatomics:
51. Determine the percent composition of oxygen in magnesium hydroxide.
52. If 60.2 grams of Hg combines completely with 24.0g of Br to form a compound, what is the percent composition of Br
in the compound?
53. Draw the Mole Road Map! 
54. If there are 3.45 mols of Ca in a container, how many particles would there be?
55. How many liters are there in 5.25g CO2 at STP?
56. There are 4.82X1025 formula units of Fe2O3, how many grams are there?
57. How many moles of Ne are there in 5.50g of the gas?
58. What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?
59. What is the empirical formula of a compound that is 50.7% antimony and 49.3% selenium by weight?
60. What is the molecular formula of the compound whose molar mass is 60.0g and empirical formula is CH 4N?
Electrons
61. What did Dalton’s Atomic Theory state?
62. What did J.J. Thomson discover and what did his model of the atom look like?
63. What did Rutherford discover and what did his model of the atom look like?
64. Who developed the quantum mechanical model? _________________________
65. Who developed the planetary model? _________________________
66. What was incorrect about Bohr’s model?
67. How many electrons can occupy each atomic orbital? ______ What do their spins look like? __________
68. What percent chance do you have of finding an electron in its orbital? ________
69. How many orbitals are found in a d-sublevel? ________
70. The letter, n, is used to represent the ________________. In other words, n =2 is the same thing as saying the
second energy level.
71. What types of atomic orbitals are in the third energy level? ____________________________________
72. How many electrons can occupy an f-sublevel? ______
73. Which sublevel has a spherical shape? ______ Dumb bell shape? ______
74. State Hund’s Rule.
75. State Pauli’s Exclusion Principle.
76. State the Aufbau Principle.
77. For the electron configuration, 1s22s22p1, how many electrons are in the second energy level? ______
78. For the electron configuration, 1s22s22p63s23p64s13d5, how many electrons are in p sublevels? ______
79. Write the electron configuration for each of the following elements.
a. Titanium (Ti)
b. Chlorine (Cl)
80. What element has an electron configuration that ends in 5p2? ______
81. What element has an electron configuration: [Kr]5s14d10? ______
82. What element has the electron configuration, 1s22s22p63s23p2? ______
83. How many energy levels are found in a potassium atom? ______
84. Draw the orbital diagram for phosphorus. How many electrons are in the p sublevel?
85. Draw the orbital diagram for carbon. How many unpaired electrons are found in carbon?
86. How many unpaired electrons are found in iron? ______
87. Write the shorthand electron configuration for radon. Which energy level is incomplete?
88. Write the electron configuration for magnesium ion.
89. What is the octet rule?
90. How does chlorine obey to octet rule when forming compounds?
c.
Copper (Cu)
91. Draw the Lewis dot diagram for the following elements:
a. Helium
b. Magnesium
c.
Sulfur
92. What is the energy of a photon of green light with a frequency of 5.80X1012 Hz?
93. A mercury lamp emits radiation with a frequency of 5.62 x1014 Hz. Calculate the wavelength of this radiation.
Periodic Trends
94. Who are the halogens? Alkali metals? Alkaline earth metal? Noble gases? Transition metals?
95. Define electronegativity:
96. Define ionization energy:
97. List the following elements in order of increasing atomic size. Rb, Mg, K, Na _________________________
98. List the following elements in order of increasing ionization energy. Fr, Cd, Rb, Te
_________________________
99. List the following elements in order of decreasing electronegativity. Al, Na, F, Cl
_________________________
100. List the following metals in order of increasing reactivity. Al, Mg, Cs, K
_________________________
101. List the following ions in order of increasing size. Mg2+, Ar, Na+, S2-, Cl-
_________________________
Chemical Reactions and Balancing
Write out the following reactions, balance them, and then classify the type of reaction.
102. Phosphorus and oxygen react to form solid phosphorus pentoxide.
103. Hydrochloric acid reacts with sodium to form hydrogen gas and sodium chloride.
104. Potassium chlorate decomposes into potassium chloride and oxygen.
105. Butane (C4H10) undergoes combustion.
106. Zinc sulfate and calcium acetate to yield a zinc acetate and calcium sulfate.