21. Consider the following balanced chemical reaction between a metal "M" in its elemental form (uncombined state), and oxygen gas (O,) to produce a metal oxide with a formula M,0: 4M(5) + Ozig) → 2M20[s) Use the space below to work out how many electrons are either lost or gained by each of the reactants. For full credit, make sure to clearly show the oxidation numbers of each atom and the number of electrons involved in the transfer.

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21. Consider the following balanced chemical reaction between a metal “M" in its elemental form
(uncombined state), and oxygen gas (O,) to produce a metal oxide with a formula M,O:
4M(s) + Ozig) → 2M20[s)
Use the space below to work out how many electrons are either lost or gained by each of the
reactants. For full credit, make sure to clearly show the oxidation numbers of each atom and the
number of electrons involved in the transfer.
Transcribed Image Text:21. Consider the following balanced chemical reaction between a metal “M" in its elemental form (uncombined state), and oxygen gas (O,) to produce a metal oxide with a formula M,O: 4M(s) + Ozig) → 2M20[s) Use the space below to work out how many electrons are either lost or gained by each of the reactants. For full credit, make sure to clearly show the oxidation numbers of each atom and the number of electrons involved in the transfer.
a) The balanced oxidation half-reaction is:
b) The balanced reduction half-reaction is:
Transcribed Image Text:a) The balanced oxidation half-reaction is: b) The balanced reduction half-reaction is:
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