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Oxidation
Process in which atoms or ions attain a more + oxidation stateEx.
Na → Na+ + eCl- → Cl + eCa+ → Ca2+ + e
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Reduction
Atoms or ions of elements attain a more negative oxidation stateEx. Cl + e → Cl-
Mnemonic: “OIL RIG”Oxidation involves loss, reduction involves gain
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Oxidation NumberUncombined elements have oxidation # of 0Monoatomic ions have oxidation # equal to their ion chargeF is always –1 in a compoundO is almost always –2 in a compoundH is +1 in all compounds except those with metals (then its –1)More electronegative element is assigned a number equal to its ion chargeAlgebraic sum of oxidation numbers in a compound is always zero
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Practice
Determine the oxidation numbers for each element in the compounds below
NaClH2SO4
NO3-
CO2
SF6
AgNO3
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Redox Reactions
Redox reactions are among the most common of all chemical processesCombustion, synthesis, decomposition, and single replacements are all redox reactions
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Definition
Reaction in which a change in oxidation number occursOxidation – becomes more positiveReduced – becomes more negativeOxidation and reduction always come in pairs Electrons are transferred from the substance being oxidized to the substance being reduced
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Example
In the reactions below, identify what is oxidized and what is reduced2PH3 + 4O2 P2O5 + 3H2O
2H2O + Al + MnO4- Al(OH)4
- + MnO2