Redox Reactions

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Oxidation is the addition of oxygen or an electronegative element to a substance, OR the removal of hydrogen or an electropositive element from a substance. Example: 2Mg + O₂ → 2MgO (addition of oxyge…

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Reduction is the removal of oxygen or an electronegative element from a substance, OR the addition of hydrogen or an electropositive element to a substance. Example: 2HgO → 2Hg + O₂ (removal of oxygen…

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Oxidation: Loss of electrons by any species. Reduction: Gain of electrons by any species. Example: Na → Na⁺ + e⁻ (oxidation), Cl₂ + 2e⁻ → 2Cl⁻ (reduction)…

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An oxidizing agent is a substance that accepts electrons from another substance, causing the other substance to be oxidized. The oxidizing agent itself gets reduced in the process. Example: In Zn + Cu…

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A reducing agent is a substance that donates electrons to another substance, causing the other substance to be reduced. The reducing agent itself gets oxidized in the process. Example: In Zn + Cu²⁺ → …

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Oxidation number is the oxidation state of an element in a compound, determined by a set of rules assuming complete electron transfer to the more electronegative atom. It helps in tracking electron tr…

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In elements in the free or uncombined state, each atom has an oxidation number of zero. Examples: H₂, O₂, Cl₂, Na, Mg, Al all have oxidation number 0.

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Oxygen has oxidation number -2 in most compounds. Exceptions: In peroxides (H₂O₂, Na₂O₂) it is -1, in superoxides (KO₂) it is -½, and when bonded to fluorine (OF₂) it is +2.