What is the oxidation number of oxygen in each of the...

What is the oxidation number of oxygen in each of the following compounds? Tell whether the compound is an oxide, a peroxide, or a superoxide.
(a) $\mathrm{Rb}_{2} \mathrm{O}_{2}$
(b) $\mathrm{CaO}$
(c) $\mathrm{CsO}_{2}$
(d) $\mathrm{SrO}_{2}$
(e) $\mathrm{CO}_{2}$

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Key Concepts

Oxide

An oxide is a compound where oxygen typically has an oxidation state of -2. In these compounds, oxygen acts as a typical anion and is combined with a metal or nonmetal that donates electrons, forming a stable ionic or covalent compound.

Peroxide

A peroxide is a compound that contains an oxygen-oxygen single bond, with each oxygen atom exhibiting an oxidation state of -1. The peroxide ion (O2^2-) reflects a different bonding situation compared to standard oxides, and these compounds often participate in unique chemical reactions, including decomposition into reactive oxygen species.

Oxidation Number

The oxidation number (or oxidation state) is a formalism used to assign a numerical value to the degree of oxidation of an atom in a chemical compound. It represents the hypothetical charge an atom would have if all bonds were completely ionic, allowing for the systematic analysis of electron transfer in chemical reactions.

Superoxide

A superoxide is a compound that contains the superoxide ion, O2^-, in which the oxygen atoms share a bond that results in an overall oxidation state of approximately -1/2 per oxygen atom. This unusual oxidation state arises because the extra electron is delocalized over the O2 unit, giving superoxides distinct chemical properties from both oxides and peroxides.

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