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    Why is iron very easily oxidized under alkaline conditions?
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    (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.
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    (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 ?
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    (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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