Oxidation-Reduction Reactions Chemistry Worksheet Page 26
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Chapter 6
Oxidation-Reduction Reactions
Review
1.
For each of the following ionic formulas, write the formula for the cation and the
Questions
formula for the anion.
a. FeBr
c. AgCl
3
b. Co
(PO
)
d. (NH
)
SO
3
4
2
4
2
4
2.
Classify each of the following formulas as representing a binary ionic compound,
an ionic compound with polyatomic ions, or a molecular compound.
a. CF
e. H
S
4
2
b. Pb(C
H
O
)
f. ClF
2
3
2
2
c. CoCl
g. Cr(OH)
2
3
d. C
H
OH
h. H
PO
2
5
3
4
3.
Balance the following equations. (C
H
is a component of gasoline, and P
S
is
8
18
2
5
used to make the insecticides parathion and malathion.)
(l ) + O
( g) → CO
(g) + H
a. C
H
O(l )
8
18
2
2
2
(s) + S
(s) → P
b. P
S
(s)
4
8
2
5
Key Ideas
Complete the following statements by writing one of these words or phrases in each
blank.
carbon dioxide
oxidizing
change
oxidizing agent
decreases
partial
flow of electrons
pure element
gains
rarely
half‑reactions
reduced
heat
reducing
increases
reducing agent
light
reduction
loses
sulfur dioxide
one
transferred
oxidation
two or more
oxidized
water
4.
According to the modern convention, any chemical change in which an element
_____________ electrons is called an oxidation.
5. According to the modern definition, any chemical change in which an element
_____________ electrons is called a reduction.
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