Oxidation Number Exercise

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Oxidation Number Exercise
Oxidation Number Exercise
Do not hand in this work sheet. When you are ready, you will be given an examination
over this material. Complete the examination by yourself and hand it in to receive
credit.
Purpose: This exercise is designed to teach the student how to assign oxidation
numbers. Oxidation numbers are very important and are used for 1) naming
compounds, 2) balancing oxidation-reduction reactions, 3) calculations in
electrochemistry and other areas of chemistry.
Rule 0
The following rules are in the form of a hierarchy; that is, the first stated rule
takes precedence over subsequent rules if a conflict arises.
Rule 1
The oxidation numbers for all the atoms in a neutral molecule must add up
to 0. Similarly, the oxidation numbers for all the atoms of an ion must add
up to the charge of the ion. (You are expected to recognize polyions. For
the common polyions, know their charges and their names. A summary of
the common polyions appears on page xiv. The first step is, always, to
determine what polyions are present.)
Rule 1a
The oxidation number of elements in the elemental form is 0. (Note - this
rule is a direct consequence of rule 1. How so?)
Rule 1b
The oxidation number of any monatomic ion is the same as its charge.
(See comment in 1a.)
Exercises - Give the oxidation number for the following atoms:
O
O =
F
F =
2
2
S
S =
Cl
Cl =
8
2
N
N =
Al
Al =
_
2
2+
2+
Co
Co =
Mn
Mn =
-
3+
Cl
Cl =
Cr
Cr =
-
2+
I
I =
Hg
Hg =
3
2

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