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Solid metal crystals are composed of metal cations bound to delocalised electrons whereby the metal cations exhibit a full outer shell. So why do solid metals undergo oxidation when the metal cations are stable? Is it more energetically favourable for metal cations to form ionic bonds rather than metallic bonds?

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    $\begingroup$ You've stated the answer: It is more energetically favourable for metal cations to form ionic bonds rather than metallic bond. Otherwise, why would thew reaction proceed? $\endgroup$ – DrMoishe Pippik Jan 13 at 2:29

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