# Transition metals chem (redox)

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#1
Hey can someone pls explain the half equation of O2???? Is O2 always oxidised to H2O or what?
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4 years ago
#2
O2 is reduced. Oxygen is a much more electronegative atom so would 'steal' the electrons from the hydrogen.
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4 years ago
#3
(Original post by pondsteps)
Hey can someone pls explain the half equation of O2???? Is O2 always oxidised to H2O or what?
O2 is being reduced not oxidised.

What do you need explaining?
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#4
Yeah I meant reduced sorry .. But when I did the equation I wrote it as O2 +2e- --> 2O- , isn't this the reduction equation!😭
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4 years ago
#5
(Original post by pondsteps)
Yeah I meant reduced sorry .. But when I did the equation I wrote it as O2 +2e- --> 2O- , isn't this the reduction equation!😭
There are no oxide ions in the products.

The "rules" for balancing redox half-equations are that you can only use:

In acid medium: H+ and H2O
In basic medium: OH- and H2O
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#6
(Original post by charco)
There are no oxide ions in the products.

The "rules" for balancing redox half-equations are that you can only use:

In acid medium: H+ and H2O
In basic medium: OH- and H2O
How do we know which kind of balancing to do???? Like if there were oxide ions in the products would mine have been correct???
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4 years ago
#7
(Original post by pondsteps)
How do we know which kind of balancing to do???? Like if there were oxide ions in the products would mine have been correct???
You can see from the given equation for reaction that there are no oxide ions in the products.

Your second question probably, as you will only get oxide ions formed in things like the combustion of metals.

2Mg + O2 --> 2MgO

IMHO rather too trivial for a redox question.
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