Second Nine Weks Study Guide
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
1. Magnesium bromide is an ionic compound with the chemical formula MgBr2. What does the “2” tell you?
a. Bromide has a 2 charge. b. There are two magnesium ions to every bromide ion. c. There are two
bromide ions for every magnesium ion. d. Bromide has a 2+ charge.
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2. Each family in the periodic table has its own characteristic properties based on the number of
a. neutrons. b. valence electrons. c. protons. d. ions.
____
3. When an atom loses an electron, it becomes a
a. positive ion. b. negative ion. c. neutral ion. d. neutral atom.
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4. An ionic bond is the attraction between
a. similarly charged ions. b. oppositely charged ions. c. neutral ions. d. neutral atoms.
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5. Ions that are made of more than one atom are examples of
a. polyatomic ions. b. negative ions. c. positive ions. d. neutral ions.
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6. What is the chemical name for the compound with the formula Na2S?
a. sodium fluoride b. magnesium sulfide c. lithium oxide d. sodium sulfide
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7. Which of the following is a characteristic property of ionic compounds?
a. They have low melting points. b. They have low boiling points. c. They form hard, brittle crystals with
characteristic shapes. d. They contain no charged particles.
____
8. A chemical bond formed when two atoms share electrons is called a(n)
a. ionic bond. b. covalent bond. c. polyatomic bond. d. crystal bond.
____
9. What is a double bond?
a. a bond between two atoms b. one pair of electrons shared between two atoms c. two pairs of electrons
shared between two atoms d. two pairs of electrons shared between four atoms
____ 10. A covalent bond in which electrons are shared unequally is
a. polar. b. a double bond. c. ionic. d. polyatomic.
____ 11. In the chemical formula for an ionic compound, which item is written first?
a. positive ion b. negative ion c. subscript d. charge
____ 12. Electrons involved in bonding between atoms are
a. valence electrons. b. inside the nucleus. c. closest to the nucleus. d. positively charged.
____ 13. What is the greatest number of valence electrons an atom can have?
a. 2 b. 3 c. 8 d. 12
____ 14. Water is polar and oil is nonpolar. What happens when the two liquids are poured into the same container?
a. Both liquids become nonpolar. b. A gas is produced. c. The liquids mix well. d. The liquids do not mix.
____ 15. If atoms of a halogen nonmetal (Group 17) gain one electron, the atoms then have
a. no valence electrons. b. 7 valence electrons. c. 8 valence electrons. d. 17 valence electrons.
____ 16. Ionic compounds are electrically
a. charged. b. positive. c. negative. d. neutral.
____ 17. Which of the following terms means that metals can be rolled into thin sheets, as in aluminum foil, or beaten
into complex shapes?
a. polar b. alloy c. ductile d. malleable
____ 18. A mixture that is made of two or more elements—one that is a metal—that has the properties of metal is a(n)
a. polymer. b. monomer. c. alloy. d. ceramic.
____ 19. What is an advantage that alloys might have over many pure metals?
a. Alloys occur naturally. b. Alloys resist rust. c. Alloys are weaker. d. Alloys can bend easily.
____ 20. Steel is an alloy of one or more elements combined with
a. copper. b. gold. c. iron. d. lead.
____ 21. Brass and steel are examples of
a. alloys. b. elements. c. pure metals. d. valence electrons.
____ 22. Which of the following terms means that metals can be pulled into thin strands or wires?
a. polar b. alloy c. ductile d. malleable
____ 23. The attraction between a positive metal ion and the electrons surrounding it is a(n)
a. chemical bond. b. covalent bond. c. ionic bond. d. metallic bond.
____ 24. Chemistry is
a. a characteristic of a substance that can be observed without changing the substance into another substance.
b. the study of matter and how matter changes. c. anything that has mass and takes up space. d. a rapid
reaction between oxygen and a substance called a fuel.
____ 25. What type of reaction is FeS + 2 HCl  FeCl2 + H2S?
a. a synthesis reaction b. a decomposition reaction c. a single replacement reaction d. a double
replacement reaction
____ 26. Which of the following is NOT a correct inference that you can make about the burning of gasoline?
a. Chemical bonds are broken and others are formed. b. The reaction is a physical change. c. New
substances are produced. d. Energy is released.
____ 27. A chemical equation that shows the same number of each kind of atom on both sides of the equation is said to
be
a. balanced. b. unbalanced. c. an incomplete reaction. d. a replacement reaction.
____ 28. Anything that has mass and takes up space is considered
a. matter. b. energy. c. chemistry. d. endothermic.
____ 29. What happens when chemical bonds break and new bonds form?
a. a physical change b. a chemical reaction c. matter is destroyed d. surface area increases
____ 30. CaCO3 represents a chemical
a. symbol. b. formula. c. subscript. d. reaction.
____ 31. The only sure evidence for a chemical reaction is
a. the formation of a gas. b. a color change. c. the production of one or more new substances. d. changes in
properties.
____ 32. A shorter, easier way to show chemical reactions, using symbols instead of words, is called a
a. chemical equation. b. chemical formula. c. symbol. d. subscript.
____ 33. The substances listed on the left side of a chemical equation are the
a. products. b. coefficients. c. precipitates. d. reactants.
____ 34. In chemical reactions, what does the principle of conservation of mass mean?
a. Matter is not created or destroyed. b. The total mass of the reactants is greater than the total mass of the
products. c. The total mass of the reactants is less than the total mass of the products. d. Matter is not
changed.
____ 35. Which of the following is a balanced chemical equation?
a. H2O2  H2O + O2 b. 2 Fe2O3 + 3 C  4 Fe + 3 CO2 c. SO2 + O2 + 2 H2O  4 H2SO4 d. 2 Mg + HC1 
MgCl2 + H2
____ 36. A bottle of hydrogen peroxide that eventually turns into a bottle of water and oxygen gas is an example of a
a. synthesis reaction. b. decomposition reaction. c. replacement reaction. d. precipitate reaction.
____ 37. A chemical reaction that absorbs energy in the form of heat is described as
a. endothermic. b. exothermic. c. combustion. d. unbalanced.
____ 38. A rapid reaction between oxygen and a fuel is known as
a. combustion. b. heat. c. activation. d. decomposition.
____ 39. In a chemical equation, numbers often appear in front of a chemical formula. These numbers tell you the
a. number of atoms in each molecule in the reaction. b. number of elements in the reaction. c. number of
molecules or atoms of each substance in the reaction. d. number of molecules in each atom in the reaction.
____ 40. The number placed below an element’s symbol in a chemical formula is called a
a. subscript. b. coefficient. c. reactant. d. product.
Short Answer
Use the diagram to answer each question.
41. List three elements from the group containing the most reactive nonmetals. Fluorine Chlorine Bromine,
42. In an electron dot diagram of aluminum (Al), how many dots should be drawn around the element’s symbol?
3
43. Which group of elements loses electrons most easily? Group I
44. Which group contains elements with two valence electrons? Group 2
Second Nine Weks Study Guide
Answer Section
MULTIPLE CHOICE
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C
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PS.6.2.3
B
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L3
L2
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L1
L1
L2
L1
L2
L2
L3
L1
L1
L3
L1
L1
L1
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L2
L3
L1
L1
L2
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L2
L1
L2
L1
L3
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p. PS-161
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p. PS-152
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p. PS-159
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p. PS-160
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p. PS-159
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p. PS-161
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p. PS-162
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p. PS-167
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p. PS-168
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p. PS-170
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p. PS-161
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p. PS-150
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p. PS-151
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p. PS-171
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p. PS-153
OBJ:
p. PS-161
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p. PS-175
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p. PS-173
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p. PS-173
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p. PS-173
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p. PS-173
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p. PS-175
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p. PS-174
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p. PS-184
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p. PS-201
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p. PS-186
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p. PS-198
OBJ:
p. PS-184
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p. PS-187
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p. PS-195
OBJ:
p. PS-188
OBJ:
p. PS-195
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p. PS-195
OBJ:
p. PS-196
OBJ:
p. PS-198, p. PS-199
PS.5.2.2
PS.5.1.2
PS.5.2.1
PS.5.2.1
PS.5.2.1
PS.5.2.2
PS.5.2.3
PS.5.3.1
PS.5.3.1
PS.5.3.3
PS.5.2.2
PS.5.1.1
PS.5.1.2
PS.5.3.3
PS.5.1.2
PS.5.2.1
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PS.5.4.1
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PS.6.1.1
PS.6.2.4
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PS.6.1.1
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PS.6.1.2
PS.6.2.1
PS.6.2.1
PS.6.2.2
DIF:
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L2
L2
L1
L2
L1
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p. PS-200
p. PS-190
p. PS-213
p. PS-199
p. PS-199
PS.6.2.4
PS.6.1.2
PS.6.4.1
PS.6.2.3
PS.6.2.3
OBJ:
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SHORT ANSWER
41. ANS:
Accept any three elements from Group 17: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At).
DIF: L3
REF: p. PS-153
OBJ: PS.5.1.2
42. ANS:
Three. Elements in Group 13 have 3 valence electrons.
DIF: L2
43. ANS:
Group 1
REF: p. PS-152
OBJ: PS.5.1.2
DIF: L2
44. ANS:
Group 2
REF: p. PS-153
OBJ: PS.5.1.2
DIF: L2
REF: p. PS-152
OBJ: PS.5.1.2