Assign oxidation numbers to all the atoms in each of the...

Assign oxidation numbers to all the atoms in each of the following. a. $\mathrm{HNO}_{3}$ e. $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ i. $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ b. $\mathrm{CuCl}_{2}$ f. Ag j. $\mathrm{CO}_{2}$ c. $\mathrm{O}_{2}$ g. $\mathrm{PbSO}_{4}$ k. $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Ce}\left(\mathrm{SO}_{4}\right)_{3}$ d. $\mathrm{H}_{2} \mathrm{O}_{2}$ h. $\mathrm{PbO}_{2}$ 1. $\mathrm{Cr}_{2} \mathrm{O}_{3}$

Assign oxidation numbers to all the atoms in each of the following.
a. $\mathrm{HNO}_{3}$
e. $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
i. $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$
b. $\mathrm{CuCl}_{2}$
f. Ag
j. $\mathrm{CO}_{2}$
c. $\mathrm{O}_{2}$
g. $\mathrm{PbSO}_{4}$
k. $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Ce}\left(\mathrm{SO}_{4}\right)_{3}$
d. $\mathrm{H}_{2} \mathrm{O}_{2}$
h. $\mathrm{PbO}_{2}$
1. $\mathrm{Cr}_{2} \mathrm{O}_{3}$

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Key Concepts

Application to Polyatomic Species

When dealing with polyatomic ions or compounds, oxidation numbers must be assigned in such a way that the algebraic sum of all oxidation states equals the net charge of the molecule or ion. This systematic approach is essential for analyzing more complex species.

Special Cases and Exceptions

Certain compounds defy the usual rules; for example, oxygen in peroxides has an oxidation state of -1, and hydrogen can sometimes be -1 when bonded to less electronegative elements. Recognizing these exceptions is crucial for accurate oxidation state determination in a variety of chemical contexts.

Oxidation Numbers

Oxidation numbers (oxidation states) are assigned charges that atoms would have if all bonds were completely ionic. They provide a useful bookkeeping method for tracking electron transfer in redox reactions and help in balancing chemical equations.

General Rules for Assignment

There are several key rules: (1) An element in its pure form has an oxidation number of zero; (2) For a monoatomic ion, the oxidation state is equal to its ion charge; (3) In compounds, hydrogen is usually assigned +1 and oxygen is usually assigned -2 (with known exceptions such as peroxides); and (4) The sum of the oxidation numbers in a neutral compound is zero, or equals the overall charge in the case of an ion.

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