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Name: ________________________ Class: ___________________ Date: __________
ID: A
Chapter 4 Atomic Structure Explains the formation of Compounds
Modified True/False
Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement tr ue.
____
1. All the noble gases have a stable octet of eight valence electrons.
____
2. The charge on each tin ion in the compounds Sn(Cr2O7)2 and Sn3(PO4)4 is the same.
____
3. When the following unbalanced formula equation is balanced, the coefficient 21 will be placed in
front of the oxygen molecule on the reactant side.
C10H22 + O2 → CO2 + H2O
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
4. Atoms of each element are positively identified by their:
a. neutron number
c. atomic number
b. mass number
d. valence electron number
____
5. Which of the following elements will be represented by a Lewis diagram containing three unpaired
electrons?
a. sodium
b. fluorine
c.
d.
phosphorus
sulfur
Use the following Lewis diagram to answer the next two questions.
____
6. Element L in the diagram shown above could be:
a. nitrogen
c. hydrogen
b. oxygen
d. fluorine
____
7. An acceptable formula for the compound formed from the reaction of the two elements shown above
would be:
a. KL2
b. K2L
c.
d.
1
KL
K2L2
Name: ________________________
____
8. A Lewis diagram for an atom differs from a Bohr diagram because the:
a. Bohr diagram shows only the valence electrons and a Lewis diagram shows all the
b.
c.
d.
____
ID: A
electrons
Lewis diagram shows only the valence electrons and a Bohr diagram shows all the
electrons
Lewis diagram shows the nuclear contents and a Bohr diagram does not
Lewis diagram shows inner energy level electrons and a Bohr diagram does not
9. The Lewis structure for an atom of carbon will show which of the following combinations of
electrons?
Pairs of Electrons
2
1
4
0
a.
b.
c.
d.
a.
a
b.
Unpaired Electrons
0
2
0
4
b
c.
c
d.
d
____ 10. The Lewis diagram for a molecule of water (H2O) will have which of the following combinations of
electron pairs associated with the central oxygen atom?
Lone Pairs
2
3
1
2
a.
b.
c.
d.
a.
a
Bonding Pairs
2
2
3
3
b.
b
c.
c
d.
d
____ 11. Which of the following compounds would require the use of parentheses (brackets) in its chemical
formula?
a. ammonium chlorate
b. iron(III) phosphate
c.
d.
aluminum nitrate
tin(II) dichromate
____ 12. Which of the following chemical formulas contains the greatest number of oxygen atoms?
a. aluminum dichromate
c. chromium(III) phosphate
b. tin(IV) permanganate
d. silver nitrate
____ 13. Which of the following compounds will require the use of the largest Roman numeral in its chemical
name?
a. SnCr2O4
b. CCl4
c.
d.
2
MnO2
Cr(ClO3)3
Name: ________________________
ID: A
____ 14. What is the total amount of each type of charge (positive and negative) existing in the chemical
formula for lead(IV) phosphate?
a. +16 and -16
b. +12 and -12
c.
d.
+10 and -10
+8 and -8
____ 15. In which of the following compounds will the bonding involve the sharing of electrons between
atoms?
a. Na2O
b. N2O4
c.
d.
Nb2O3
NiO
____ 16. Which of the following compounds will not require the use of either a prefix or a Roman numeral in
its chemical name?
a. Cl2O7
b. CO
c.
d.
Sn(SO4)2
Mg3(PO4)2
____ 17. Which of the following will never appear as a reactant in a chemical equation?
a. He
c. Ce
b. Fe
d. Be
____ 18. Which of the following, when appearing as elements in a chemical equation, would not exist as a
diatomic molecule?
a. hydrogen
b. carbon
c.
d.
nitrogen
oxygen
____ 19. Consider the following balanced formula equation, representing the combustion of pentane, a
component of lighter fluid:
C5H12 + 11 O2 → 5 CO2 + 6 H2O
How many molecules of carbon dioxide can be produced if 3 molecules of pentane are burned?
a. 5
c. 15
b. 10
d. 20
Use the following chemical equations to answer the next two questions.
I.
II.
III.
Na + 2 H2O → NaOH + 2 H2
3 Sr(OH)2 + 2 H3PO4 → Sr3(PO4)2 + 3 H2O
NaHCO3 → Na2CO3 + CO2 + H2O
____ 20. Which of the equations shown above is/are not balanced?
a. II. and III. only
c. II. only
b. I. and II. only
d. all are not balanced
3
Name: ________________________
ID: A
____ 21. One of the components of gasoline is octane (C8H18), which burns in oxygen according to the
following equation:
2 C8H18 + ? O2 → 16 CO2 + 18 H2O
The missing coefficient necessary to balance the equation is:
a. 16
c. 25
b. 17
d. 50
____ 22. Potassium iodide reacts with lead(II) nitrate to produce potassium nitrate and lead(II) iodide. In the
balanced formula equation representing this reaction, the coefficient for potassium iodide and
potassium nitrate is the same and would be:
a. 4
c. 2
b. 3
d. 1
Matching
Match the type of compound (ionic or covalent) with the appropriate description. Each type of
compound may be used more than once.
a. ionic compound
b. covalent compound
____ 23. this compound forms when metals react with non-metals
____ 24. molecules exist in this compound
____ 25. the name of this compound may include Roman numerals
____ 26. electrons are transferred when this compound forms
Short Answer
27. An element is a member of group 1 and also of period 2 in the periodic table. Without referring to
the periodic table, describe what this information tells you about this element’s electron arrangement.
28. Write a balanced formula equation for the reaction of solid sodium metal with liquid water to
produce an aqueous solution of sodium hydroxide and hydrogen gas.
4
ID: A
Chapter 4 Atomic Structure Explains the formation of Compounds
Answer Section
MODIFIED TRUE/FALSE
1. ANS: F
Most noble gases have a stable octet of eight valence electrons. Helium has only two valence
electrons.
PTS:
KEY:
2. ANS:
LOC:
KEY:
3. ANS:
1
DIF: Average
LOC: C1-3
TOP: Atomic Theory and Bonding
noble gases MSC: K
T
PTS: 1
DIF: Average
C2-6
TOP: Names and Formulas of Compounds
ionic formulas | ionic names
MSC: U
F
When the unbalanced formula equation is balanced, the coefficient 31 will be placed in front of the
oxygen molecule on the reactant side.
PTS: 1
DIF: Average
KEY: balanced chemical equations
LOC: C4-3
MSC: U
TOP: Chemical Equations
MULTIPLE CHOICE
4. ANS:
TOP:
MSC:
5. ANS:
TOP:
MSC:
6. ANS:
TOP:
MSC:
7. ANS:
TOP:
MSC:
8. ANS:
TOP:
MSC:
9. ANS:
TOP:
MSC:
10. ANS:
TOP:
MSC:
C
PTS: 1
Atomic Theory and Bonding
K
C
PTS: 1
Atomic Theory and Bonding
U
D
PTS: 1
Atomic Theory and Bonding
U
C
PTS: 1
Atomic Theory and Bonding
H
B
PTS: 1
Atomic Theory and Bonding
K
D
PTS: 1
Atomic Theory and Bonding
U
A
PTS: 1
Atomic Theory and Bonding
H
DIF: Easy
LOC: C1-3
KEY: atomic theory
DIF: Difficult
LOC: C1-6
KEY: Lewis structures/diagram
DIF: Average
LOC: C1-6
KEY: covalent bonding
DIF: Difficult
LOC: C1-6
KEY: covalent bonding | Lewis structures/diagrams
DIF: Easy
LOC: C1-3, 6
KEY: Lewis structures/diagrams | Bohr diagrams
DIF: Average
LOC: C1-5
KEY: Lewis structures/diagrams
DIF: Difficult
LOC: C1-6, 7
KEY: Lewis structures/diagrams
1
ID: A
11. ANS:
TOP:
MSC:
12. ANS:
TOP:
MSC:
13. ANS:
TOP:
MSC:
14. ANS:
TOP:
MSC:
15. ANS:
TOP:
MSC:
16. ANS:
TOP:
MSC:
17. ANS:
TOP:
18. ANS:
TOP:
MSC:
19. ANS:
TOP:
MSC:
20. ANS:
TOP:
MSC:
21. ANS:
TOP:
MSC:
22. ANS:
TOP:
MSC:
C
PTS: 1
DIF:
Names and Formulas of Compounds
U
A
PTS: 1
DIF:
Names and Formulas of Compounds
U
C
PTS: 1
DIF:
Names and Formulas of Compounds
U
B
PTS: 1
DIF:
Names and Formulas of Compounds
H
B
PTS: 1
DIF:
Names and Formulas of Compounds
K
D
PTS: 1
DIF:
Names and Formulas of Compounds
U
A
PTS: 1
DIF:
Chemical Equations
KEY:
B
PTS: 1
DIF:
Chemical Equations
KEY:
K
C
PTS: 1
DIF:
Chemical Equations
KEY:
U
D
PTS: 1
DIF:
Chemical Equations
KEY:
U
C
PTS: 1
DIF:
Chemical Equations
KEY:
U
C
PTS: 1
DIF:
Chemical Equations
KEY:
H
Average
LOC: C2-6
KEY: ionic formulas | ionic names
Average
LOC: C2-6
KEY: ionic formulas | ionic names
Average
LOC: C2-6
KEY: ionic formulas | ionic names
Difficult
LOC: C2-6
KEY: ionic formulas | ionic names
Easy
LOC: C2-7
KEY: covalent formulas
Average
LOC: C2-6, 7
KEY: ionic names | covalent names
Easy
LOC: C1-4, C4-3
noble gases MSC: K
Easy
LOC: C4-3
chemical equations
Average
LOC: C4-3
chemical equations
Average
LOC: C4-3
balanced chemical equations
Easy
LOC: C4-3
balanced chemical equations
Difficult
LOC: C4-2, 3
balanced chemical equations
MATCHING
23. ANS:
TOP:
MSC:
24. ANS:
TOP:
MSC:
25. ANS:
TOP:
MSC:
A
PTS: 1
Atomic Theory and Bonding
K
B
PTS: 1
Atomic Theory and Bonding
K
A
PTS: 1
Atomic Theory and Bonding
K
DIF: Average
LOC: C1-2
KEY: ionic compounds | covalent compounds
DIF: Average
LOC: C1-2
KEY: ionic compounds | covalent compounds
DIF: Average
LOC: C1-2, C2-6
KEY: ionic compounds | covalent compounds
2
ID: A
26. ANS: A
PTS: 1
TOP: Atomic Theory and Bonding
MSC: K
DIF: Average
LOC: C1-2
KEY: ionic compounds | covalent compounds
SHORT ANSWER
27. ANS:
Being a member of group 1, this element must have one electron in its valence shell. Being a
member of period 2, the valence electron shell of the atom must be the second energy level.
PTS: 2
DIF: Average
KEY: periodic table
28. ANS:
LOC: C1-4
MSC: U
TOP: Atomic Theory and Bonding
2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g)
PTS: 4
DIF: Average
LOC: C2-6, C4-3
KEY: chemical formulas | balanced chemical equations
3
TOP: Chemical Equations
MSC: U