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    what does this mean, also when talking about transition metals how can iron be a 2+ ion or a 3+ ion because surely then it wont have an noble gas electronic configuration. Thanks, please answer in a way GCSE student would understand
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    (Original post by JackLeggett)
    what does this mean, also when talking about transition metals how can iron be a 2+ ion or a 3+ ion because surely then it wont have an noble gas electronic configuration. Thanks, please answer in a way GCSE student would understand
    Iron(II) means Fe2+ Iron (III) means Fe3+.

    All atoms try and have full outer shells to remain stable. This is why the undergo reactions with each other in nature. That's why iron ions are left with with no electrons in their outer most shell.
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    (Original post by GradeA*UnderA)
    Iron(II) means Fe2+ Iron (III) means Fe3+.

    All atoms try and have full outer shells to remain stable. This is why the undergo reactions with each other in nature. That's why iron ions are left with with no electrons in their outer most shell.
    Thanks I get the (II) is Fe2+ and (III) is Fe3+ but if Iron has 2 electrons in its outer shell how can it lose 3? then there would be no outer shell surly??
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    (Original post by JackLeggett)
    Thanks I get the (II) is Fe2+ and (III) is Fe3+ but if Iron has 2 electrons in its outer shell how can it lose 3? then there would be no outer shell surly??
    A2 content. You'll find out one day it's to do with orbitals and energy differences
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    (Original post by JackLeggett)
    Thanks I get the (II) is Fe2+ and (III) is Fe3+ but if Iron has 2 electrons in its outer shell how can it lose 3? then there would be no outer shell surly??
    The explanation is beyond GCSE, but as a very brief summary: Electron "shells" are split into three types fo orbitals: s, p and d. Iron's electro config is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d6. The 3d subshell is its outer subshell. In the subshell, electrons are placed in pairs, with opposite "spin". When iron forms ions, it promotes electron from its 4s subshell into its 3d subshell, to fill some pairs of electrons. Then, the remaining, unpaired electrons (either 2 or 3 of them) are lost.

    That was very condensed, but you certainly don't need to know that until A-level.
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    (Original post by GradeA*UnderA)
    A2 content. You'll find out one day it's to do with orbitals and energy differences
    Haha OK THanks
 
 
 
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