Oxidation-Reduction Reactions Chemistry Worksheet Page 12
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Chapter 6
Oxidation-Reduction Reactions
e
6.1 - Oxidation Numbers
xerCise
In one part of the steel manufacturing process, carbon is combined with iron to form
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3
bjeCtive
pig iron. Pig iron is easier to work with than pure iron because it has a lower melting
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point (about 1130 °C compared to 1539 °C for pure iron) and is more pliable. The
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following equations describe its formation. Determine the oxidation number for each
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atom in the formulas. Decide whether each reaction is a redox reaction, and if it is,
identify what is oxidized, what is reduced, what the oxidizing agent is, and what the
reducing agent is.
2C(s) + O
(g) → 2CO(g)
2
(s) + CO(g) → 2Fe(l ) + 3CO
Fe
O
(g)
2
3
2
2CO(g) → C(in iron) + CO
(g)
2
Equations for redox reactions can be difficult to balance, but your ability to
determine oxidation numbers can help. You can find a description of the process
for balancing redox equations at the textbook’s Web site.
6.3
Types of Chemical Reactions
Chemists often group reactions into general categories, rather than treating each
chemical change as unique. For example, you saw in Chapter 4 that many chemical
changes can be assigned to the category of precipitation reactions. Understanding
the general characteristics of this type of reaction helped you to learn how to predict
products and write equations for specific precipitation reactions. You developed similar
skills in Chapter 5 for neutralization reactions. Because several types of chemical
reactions can also be redox reactions, we continue the discussion of types of chemical
reactions here.
Combination Reactions
In combination reactions, two or more elements or compounds combine to form one
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compound. Combination reactions are also called synthesis reactions. The following
are examples of combination reactions.
2Na(s) + Cl
(g) → 2NaCl(s)
2
C(s) + O
(g) → CO
(g)
2
2
MgO(s) + H
O(l ) → Mg(OH)
(s)
2
2
Two of the above combination reactions are also redox reactions. Can you tell which
one is not?
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