= Oxidation
An <oxidation> increases an <oxidation state>, recording loss from the formal <electron> assignment. For $\mathrm{Zn}\to\mathrm{Zn}^{2+}+2e^-$, the increase is $0\to+2$. <Oxidation> need not involve <oxygen>.<Chemistry 2e by Paul Flowers and others>[§4.2, “Oxidation-Reduction Reactions”: oxidation as increasing oxidation number]{ref}
In the <electrochemistry> examples here, <oxidation> is loss of <electrons> by a <chemical species>; it occurs at the <anode>. That <electrode> definition holds in both a <galvanic cell> and an <electrolytic cell>; it does not fix terminal polarity. The oxidized <chemical species> serves as the <reducing agent> in the coupled <redox>.
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