Oxide

An oxide is a binary compound of oxygen and one other element, or an oxygen anion bonded to another element. Oxides include ionic salts, molecular compounds, and extended solids.

Oxygen: A chemical element with atomic number 8 that commonly forms two bonds in compounds. Its high electronegativity and usual −2 oxidation state shape the bonding in most oxides.
Oxidation: A chemical process in which a substance loses electrons or increases its oxidation state. Oxidation of an element by oxygen commonly produces its oxide.
Silicon dioxide: A silicon oxide with formula SiO₂, found in quartz and many silicate materials. Its glass-forming network makes it central to glassmaking and optical materials.
Peroxide: A compound or ion containing an oxygen–oxygen bond with each oxygen typically at oxidation state −1. Peroxides contain an O–O unit, unlike ordinary oxides with oxygen at −2.
Oxidation state: A formal charge assigned to an atom by treating its bonds as ionic. It provides a consistent way to describe oxygen’s charge and balance oxide formulas.
Combustion: A rapid exothermic reaction, commonly with oxygen, that releases heat and often light. Burning elements and fuels often generates characteristic oxides.
Aluminium oxide: An aluminium oxide with formula Al₂O₃, occurring naturally as corundum. Its hardness and thermal stability make it useful in abrasives and ceramics.
Superoxide: A compound or ion containing the O₂⁻ species, with oxygen atoms at average oxidation state −½. Its paired oxygen unit distinguishes superoxides from simple oxide compounds.
Chemical bond: An interaction that holds atoms or ions together in molecules and solids. Different bond types account for the varied structures and properties of oxides.
Acid–base reaction: A reaction involving proton transfer or, more broadly, electron-pair donation and acceptance. Acidic and basic oxides react with bases and acids, respectively.

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