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Oxidation of iron(ii) ions by air

Why is iron very easily oxidized under alkaline conditions?
Reply 1
Avatar for RMNDK
RMNDK
3
Original post by mystreet091234
Why is iron very easily oxidized under alkaline conditions?


If you surround an iron metal with an alkali, you're going to surround it with hydroxide ions.

This makes the complex negative, i.e. [Fe(OH)6]4-

Oxidation is loss of electrons, i.e. loss of a cloud of negative charge.

It's easier to lose this negative charge from a negatively charged species due to the electrostatic repulsion.
Original post by RMNDK
If you surround an iron metal with an alkali, you're going to surround it with hydroxide ions.

This makes the complex negative, i.e. [Fe(OH)6]4-

Oxidation is loss of electrons, i.e. loss of a cloud of negative charge.

It's easier to lose this negative charge from a negatively charged species due to the electrostatic repulsion.


What do you mean by electrostatic repulsion in terms of it's easier the lose the negative charge ?
Reply 3
Avatar for RMNDK
RMNDK
3
Original post by PlayerBB
What do you mean by electrostatic repulsion in terms of it's easier the lose the negative charge ?


Yeah exactly.
The electrons (or negative charge) repel each other reducing the energy taken to remove one electron/cloud of charge.

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