Name: __________________________________________________ Period:_____
2014
Chemistry I Level Final Exam Review
1. Review all your quizzes and “Story so far” sheets for every UNIT 1-12. 
2. Complete the Review Study Guide. The more practice, the better you will feel on
the day of your Chemistry final exam. Remember “Chem-is-try” Good luck!
The Atom and the Periodic Table
Locate and label the Alkali metals, Alkali-Earth metals, Transition elements, Metalloids, Halogens, and
Nobel Gases using this Periodic Table:
1. Identify the following elements:
(a) The most reactive nonmetal on the Periodic Table
(b) The least reactive Halogen.
(c) The least reactive member of the fifth period.
2. Explain why the atoms of the elements at the bottom of a given group (vertical column) are larger than
the atoms of the elements at the top of the same group.
3. Arrange the following sets of elements in order of increasing atomic size:
(a) Sn, Xe, Rb, Sr
4. Define ionization energy:
5. In the following set of elements, which element would be expected to have the highest ionization
energy?
(a) Cs, K, Li
Elements Aa and Cc are in the same group, Bb and Dd are in the same group, Aa and Bb are in the same
period, and Cc and Dd are in the same period. Which has the greatest ionization energy?
6. Which has the greatest ionization energy?
a. Aa
b. Bb
c. Cc
d. Dd
7. Which has the largest atomic radius?
a. Aa
b. Bb
c.
d.
Cc
Dd
8. Which has the most electrons?
a. Aa
b. Bb
c.
d.
Cc
Dd
9. Which will require the least amount of energy to remove an outer electron from?
a. Aa
c. Cc
b. Bb
d. Dd
10. How many valence electrons does each of the following atoms possess?
a. Sodium
c. Chlorine
b. Magnesium
d. Neon
11. How are the electron arrangements in a given group (vertical column) of the periodic table related?
12. Which of the following groups of atoms have the same outermost valence electron configurations
but with electrons in different energy levels?
a. N, O, F, Ne
b. S, Cl, Ar, K
c. O, S, Se, Te
13. The elements chlorine and iodine have similar chemical properties because they:
a. are both metals
b. are in the same chemical period
c. have the same number of electrons in their outer energy levels
d. have the same number of stable isotopes
14. Which three elements are likely to have similar chemical and physical properties?
a. sodium, lithium, and potassium
b. sodium, magnesium, and aluminum
c. nitrogen, oxygen, and neon
15. Locate Magnesium (#12), Calcium (#20), and Strontium (# 38). What do these elements have in
common?
Directions: Fill in the following information for chlorine:
35
16. The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an
atom contains a dense center of positive charge is:
a.
J. J. Thomson
b.
Ernest Rutherford
c.
Lord Kelvin
d.
James Chadwick
17. The identity of an element is determined by its:
a. mass number
b. atomic number
c. number of neutrons
d. atomic mass
18. Which atomic particle determines the chemical properties of the atom?
a. Proton
c. Electron
b. Neutron
d. Quark
19. What subatomic particle is never found in the atomic nucleus?
a. Proton
b. Neutron
c. Electron
20. How many protons, electrons, and neutrons does the following isotope of iodine contain? 12753 I
21. Give the isotopic notation for an atom containing 6 protons and 8 neutrons.
22.
If an atom of an element has a mass number of 201 and has 121 neutrons, what is the isotopic
notation of the element?
23.
An atom of an element has an atomic number of 24 and a mass number of 52. What is the isotopic
notation, the name, and the number of protons, neutrons, and electrons in this atom?
24.
Three isotopes of argon occur in nature: argon-36, argon-38, and argon-40. Calculate the average
atomic mass of argon, given the following relative atomic masses and abundances of each of the
isotopes: argon-36 (3.7%), argon-38 (6.3%), and argon-40 (90%).
Electrons and Ions
25. Metals tend to ___________________ elections; Non-metals tend to ___________________
electrons. (LOSE or GAIN)
26.
Which of the following is NOT a molecular compound? How do you know?
a. P2O5
c. H2O
b. NaF
d. PCl3
27.
How many protons, neutrons, and electrons are present in 42He?
Protons:
Neutrons:
Electrons:
28.
How many protons, neutrons, and electrons are present in 3717 Cl?
Protons:
Neutrons:
Electrons:
29.
How many protons, neutrons, and electrons are present in 4020 Ca?
Protons:
Neutrons:
Electrons:
30.
How many protons, neutrons, and electrons are present in the 2412 Mg+2 ion?
Protons:
Neutrons:
Electrons:
31.
How many protons, neutrons, and electrons are present in the 9140 Zr+4 ion?
Protons:
Neutrons:
Electrons:
32.
How many protons, neutrons, and electrons are present in the 7934 Se-2 ion?
Protons:
Neutrons:
Electrons:
Directions: Name and write chemical formulas for the following compounds. Circle all molecular
compounds.
Compound
33. NaOH
34.
MgBr2
35.
SiO2
36.
FeCl2
37.
Zn(OH)2
38.
Be2SO4
Name of Compound
Molar Mass of Compound
39.
P4O10
40.
N2O
Compound
41. sodium phosphide
42.
magnesium nitrate
43.
lead (II) sulfite
44.
calcium phosphate
45.
bromine monofluoride
46.
aluminum sulfide
47.
disulfur dichloride
48.
copper (I) arsenide
Formula of Compound
Molar Mass of Compound
Counting Atoms: Calculate the total number of atoms of each of the following elements
Na = 2
49. Na2CO3
C=1
52.
Be(OH)2
O=3
50. Al2(SO4)3
51. 4 Pb(OH)4
53. 3 C2H3O2
54. 3 Ca3(PO4)2
Types of Chemical Reactions
Identify each of the equations below as synthesis, decomposition, single displacement, combustion, or
double displacement reactions.
55.
KClO3 → KCl + O2
56.
Zn + CuSO4 → ZnSO4 + Cu
57.
Mg + O2 → MgO2
58.
C10H8 + O2 → CO2 + H2O
59.
Ca(OH)2 + HNO3 → Ca(NO3)2 + H2O
Directions: Balance the following chemical reactions and indicate the type of chemical reaction. Include
particle pictures of the reactants and products in each balanced chemical reaction.
60.
____ KClO3
→ ____ KCl + ____ O2
Reactants
61.
____ Fe + ____ H2O → ____ Fe2O4 + ____ H2
Reactants
62.
Products
____ H2SO4 + ____ NaCl  ____ HCl + ____ Na2SO4
Reactants
63.
Products
Products
____ SO2 + ____O2  ____SO3
Reactants
Products
Solubility Rules
1. All compounds containing an element from Group 1A are soluble
2. All compounds containing ammonium (NH4+) are soluble
3. All compounds containing a nitrate ion (NO3-) are soluble
Directions: Circle the precipitate (solid) that forms in each reaction. Use the solubility rules provided.
64. AgNO3 (aq) + BaCl2 (aq) 
AgCl
+ Ba(NO3)2
65. KOH (aq) + CuSO4 (aq) 
K2SO4 + Cu(OH)2
66. Na2S(aq) + AgNO3 (aq) 
NaNO3
+ Ag2S
67. Convert from g  moles or from moles  g. Use proportion.
a.
111.7 g Fe =
b.
35.45 g of chlorine gas =
mol of chlorine gas ****
c.
0.15 moles NaNO3 =
g NaNO3
d.
1.5 moles NO2
68. Empirical Formula
CH
NO2
mol of Fe
= __________________g NO2
Actual Molar Mass of
78 g/mol
Molecular Formula
92 g/mol
69. For each of the following solutions, calculate the Molarity (M).
a. 0.50 mol KBr; 250 mL
b. 0.50 mol KBr; 500 mL
c. 0.50 mol KBr; 1000 mL
70. For each of the following solutions, calculate the Molarity (M).
a.
26.89 g CuCl2; 250 mL
b. 42 g NaHCO3; 500 mL
c.
265 g Na2CO3; 1000 mL
71. In the Kool-Aid lab, the solute was considered the
and the solvent was the
.
72. Draw particle pictures for the following Kool-Aid (KA) solutions. Include the solute and solvent.
Include a total of 10 particles in each picture.
6 M Kool-Aid
2 M Kool-Aid
73. You have 1 L of a 0.5 M aqueous solution of Kool-Aid. You want to dilute the solution to 0.25
M. What do you do? Draw a particle picture before and after the dilution. Compare the solute to
solvent before and after the dilution.
0.5 M
0.25 M
74. Calculate the new concentration when 25 mL of a 5.0 M solution of CuSO4 is diuted to 125 mL. Draw a
particle picture before and after the dilution. Compare the solute to solvent before and after the
dilution.
25 mL of 5.0M CuSO4
75. Which of the following statements is true when diluting a solution?
a. The number of moles of solute particles remains constant
b. The number of moles of solute particles decreases upon dilution.
c. The number of moles of solvent particles decreases upon dilution.
125 mL of ? CuSO4
76. How many moles of water can be prepared from 2.5 moles of oxygen?
Equation:
_____ H2
+
_____ O2

_____ H2O
Before
Change
After
(a) How many moles of hydrogen (H2) reacted?
(b) How many moles of water (H2O) were produced?
77. How many grams of calcium hydroxide (Ca(OH)2) will be produced from 4.5 moles of calcium hydride
(CaH2) with excess water?
Equation:
___ CaH2
+
____ H2O

____ Ca(OH)2 +
_____H2
Before
Change
After
(a) How many moles of calcium hydroxide (Ca(OH)2) are produced?
(b) How many grams of calcium hydroxide (Ca(OH)2) are produced? (SHOW WORK)
(c) How many moles of water were consumed?
(d) How many grams of water were consumed? (SHOW WORK)
Directions: Use the following recipe to answer questions #86 and 87.
A cake recipe calls for:
2 cups water
4 cups flour
8 oz butter
4 eggs
4 cups sugar
8 squares chocolate
The following ingredients are in your kitchen cabinet:
Lots of water
4 eggs
5 cups flour
8 cups sugar
4 oz butter
12 squares of
chocolate
78. Which ingredient is the limiting reactant?
79. Which ingredients on hand were in excess of the quantities required for the recipe?
a) Water, chocolate, sugar, and butter
b) Water, flour, chocolate, and sugar
c) Water, flour, sugar, and butter
d) Water, flour, sugar, and butter
80. Sodium reacts with chlorine gas to produce sodium chloride. Balance the equation.
______
a.
Na + _____ Cl2  _____ NaCl
Sketch 10 atoms of sodium and 6 molecules of chlorine gas in the container on the left. In the
right container, sketch all the contents after the reaction is complete. Please note: Refer to the
chemical equation above to complete the particle pictures.
Before
After
After
b.
What is the limiting reactant?
c.
How many atoms of the excess reactant remain?
81. If 2.0 moles of ZnS are combined with 4.5 moles of O2, how many grams of ZnO can be produced?
If the limiting reactant is ________
Equation:
____ ZnS
_____ O2
+

___ ZnO
____ SO2
+
Before
Change
After
If the limiting reactant is ________
Equation:
____ ZnS
+
_____ O2

Before
Change
After
(a) Which reactant is in excess?
(b) Which of the reactants is the limiting reactant?
(c) How many moles of the limiting reactant remain?
(d) How many moles of ZnO were produced?
(e) How many grams of ZnO were produced? (SHOW WORK)
___ ZnO
+
____ SO2
82. What ion is present in the highest concentration in an acid?
83. What ion is present in the highest concentration in a base?
84. Draw a particle picture that compares an acid with a pH of 4 to an acid with a pH of 1. Explain the
meaning of your picture.
pH = 4
pH = 1
Directions: Match the following vocab words with their definitions.
_____ 85. Acid
A. Produces H+ ions in solution
_____ 86. Base
B. An acid that barely splits up in water like acetic acid
_____ 87. Weak acid
C An acid that completely splits up in water, such as HCl
_____ 88. Strong acid
D. Produces OH- ions in solution
Directions: Choose the one alternative that best completes the statement or answers the question.
89.
Which one of the following is an acid?
A) NaOH
C) Ca(OH)2
B) HCl
D) phenolphthalein
90.
Which one of the following is a base?
A) NaOH
B) H3PO4
91.
92.
C) HC2H3O2
D) universal indicator
Of the following pH values, which one is the most acidic?
A) 10
B) 3
C) 1
D) 8
E) 5
Of the following pH values, which one is the most basic?
A) 8
B) 5
C) 3.
D) 10
E) 1
93.
Which of these solutions has the lowest pH?
a. 10-2 M H+ concentration
b. 10-1 M OH - concentration
-3
+
c. 10 M H concentration
d. 10-12 M H+ concentration
Directions: Complete the pH table below.
[H+]
94.
[OH-]
pH
pOH
Acid or Base
1 x 10-3 M
1 x 10-5 M
95.
Directions: Complete the data table. Make sure you draw the electron pairs clearly 
Total # of
Valence
Electrons
96. PI3
97. H2O
98. COH2
99. CO2
100. CF2Cl2
101. NO3 -1
Lewis Dot Structure
Molecular
Shape Name
Polar or Nonpolar