Question
Explain redox reaction in terms of electron transfer.
✓
Answer
$i.$ Redox reaction can be described in terms of electron transfer as shown below:
$2Mg_{(s)} + O_{2(g)} \rightarrow Mg^{2+} + 2O^{2-}$
$ii.$ Charge development suggests that each magnesium atom loses two electrons to form $Mg^{2+}$ and each oxygen atom gains two electrons to form $O^{2-}.$ This can be represented as follows:
$iii.$ When $Mg$ is oxidised to $MgO,$ the neutral $Mg$ atom loses electrons to form $Mg^{2+} \ in \ MgO$ while the elemental oxygen gains electrons and forms $O^{2-} \ in \ MgO.$
$iv.$ Each of the above steps represents a half reaction which involves electron transfer $($loss or gain$).$
$v.$ Sum of these two half reactions or the overall reaction is a redox reaction.
$2Mg_{(s)} + O_{2(g)} \rightarrow Mg^{2+} + 2O^{2-}$
$ii.$ Charge development suggests that each magnesium atom loses two electrons to form $Mg^{2+}$ and each oxygen atom gains two electrons to form $O^{2-}.$ This can be represented as follows:
$iii.$ When $Mg$ is oxidised to $MgO,$ the neutral $Mg$ atom loses electrons to form $Mg^{2+} \ in \ MgO$ while the elemental oxygen gains electrons and forms $O^{2-} \ in \ MgO.$
$iv.$ Each of the above steps represents a half reaction which involves electron transfer $($loss or gain$).$
$v.$ Sum of these two half reactions or the overall reaction is a redox reaction.
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