Name ___________________________________________________________________ Date _________
CHAPTER TEST: CHEMICAL BONDS AND EQUATIONS
Multiple Choice
Choose the answer that best completes each statement.
____ 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.
____ 2. When an atom loses an electron, it becomes a _____.
a. positive ion
b. negative ion
c. neutral ion
d. neutral atom
____ 3. An ionic bond is the attraction between _____.
a. similarly charged ions
b. oppositely charged ions
c. neutral ions
d. neutral atoms
____ 4. Ions that are made of more than one atom are examples of _____.
a. polyatomic ions
b. negative ions
c. positive ions
d. neutral ions
____ 5. What is the chemical name for the compound with the formula Na2S?
a. sodium fluoride
b. magnesium sulfide
c. lithium oxide
d. sodium sulfide
____ 6. A chemical bond formed when two atoms share electrons is called a (an) _____.
a. ionic bond
b. covalent bond
c. polyatomic bond
d. crystal bond
____ 7. 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
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____ 8. A covalent bond in which electrons are shared unequally is _____.
a. polar
b. a double bond
c. ionic
d. polyatomic
____ 9. Electrons involved in bonding between atoms are _____.
a. valence electrons
b. inside the nucleus
c. closest to the nucleus
d. positively charged
____ 10. What is the greatest number of valence electrons an atom can have?
a. 2
b. 3
c. 8
d. 12
____ 11. 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
____ 12. CaCO3 represents a chemical _____.
a. symbol
b. formula
c. subscript
d. reaction
____ 13. 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
____ 14. 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
____ 15. The substances listed on the left side of a chemical equation are the _____.
a. products
b. coefficients
c. precipitates
d. Reactants
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____ 16. 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
____ 17. A chemical reaction that absorbs energy in the form of heat is described as
a. endothermic
b. exothermic
c. combustion
d. unbalanced
Fill-in-the-blank
Complete each statement with the correct vocabulary term.
18. When an atom gains an electron it becomes a ____________________ ion.
19. The attraction between a positive ion and a negative ion results in
____________________ bond.
20. When electrons are ____________________ between two atoms, a covalent bond is
formed.
21. Nitrate (NO3–), ammonium (NH4+), and carbonate (CO32–) are examples of
____________________ ions.
22. Bonds that form between two nonmetal atoms usually are ____________________
bonds.
23. Elements in Group 1 lose one electron to form ions with a (an)
____________________ charge.
24. In a chemical equation, a (an) ____________________ tells you how many atoms or
molecules of a reactant or a product take part in a reaction.
25. The principle of _________________________ states that during a chemical
reaction, matter is not created or destroyed.
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Interpreting Diagrams
Use the diagram to answer each question.
Equation A
Cu(s)+ 2AgNO3(aq)
Equation B
Cu(NO3)2(aq)+2Ag(s)
2Al2O3(I)
4Al (I)+ 3O2(g)
26. What are the reactants in:
Equation A: __________________________ Equation B: ____________________________
27. What are the products in:
Equation A: __________________________ Equation B: ____________________________
28. What do the coefficients tell you about the ratio of the reactants in:
Equation A: __________________________ Equation B: ____________________________
29. What is the physical state of the products in:
Equation A: __________________________ Equation B: ____________________________
30. Write Equation A as a sentence:
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Use the diagram to answer each question.
31. Which letter represents decomposition?
32. Which letter represents single displacement?
33. Which letter represents synthesis?
34. Which letter represents double displacement?
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Essay
Choose TWO essays and answer using the space provided.
35. Compare a covalent bond and an ionic bond.
36. For each situation described below, tell whether the reaction is endothermic or
exothermic. Explain your reasoning in terms of the energy of the reactants and
products. A) A log burns in a fireplace, giving off gases and leaving behind ash.
B) When vinegar and baking soda are mixed, new substances form and the
solution becomes cooler.
37. Describe the difference between a synthesis reaction and a decomposition
reaction.
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Essay 1
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Essay 2
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ANSWER KEY
CHAPTER TEST: Chemical Bonds and Equations
MULTIPLE CHOICE
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
C
A
B
A
D
B
C
A
A
C
B
B
C
A
D
B
A
FILL-IN-THE-BLANK
18.
19.
20.
21.
22.
23.
negative
an ionic
shared
polyatomic
covalent
1+
1 positive
24. coefficient
25. conservation of mass
INTERPRETING DIAGRAMS
26.
27.
28.
29.
30.
31.
32.
33.
34.
copper, silver nitrate: aluminum oxide
copper nitrate, silver; aluminum, oxygen
1 molecule copper: 2 molecules silver nitrate; 2 molecules silver oxide
solid, aqueous; liquid
Solid copper plus two molecules of silver nitrate dissolved in water yields
dissolved copper nitrate plus two molecules of solid aluminum
C
A
B
D
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ESSAY
35. A covalent bond is formed when two atoms share valence electrons. Neither
atom loses electrons or takes electrons from the other. No charged particles
form. In an ionic bond, one or more electrons are transferred from one atom to
another. Atoms that lose electrons become positively charged ions, and atoms
that gain electrons become negatively charged ions. These oppositely charged
particles then attract each other.
36. A) The reaction is exothermic because heat and light are given off. The energy
of the products is less than the energy of the reactants. B) The reaction is
endothermic. Energy is absorbed by the reaction, making the solution feel
cooler. The energy of the products is greater than the energy of the reactants.
37. A synthesis reaction produces a more complex substance from simpler
substances. A decomposition reaction produces simpler substances from a more
complex substance. These two reactions are opposite processes.
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