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    i understand, for example, Fe (pure) has Fe positive ions, but do ALL the electrons on the outer shell move out?

    and do these electrons that move out (delocalised) attract to the positive Fe ions?

    thanks
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    (Original post by ilyking)
    i understand, for example, Fe (pure) has Fe positive ions, but do ALL the electrons on the outer shell move out?

    and do these electrons that move out (delocalised) attract to the positive Fe ions?

    thanks
    only the valence electrons...
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    To clarify, only the electrons in the outermost shell become delocalised. For example, with aluminium, which has the electron configuration [Ne] 3s2 3p1, the three electrons in the outer shell of each Al atom will become delocalised. There are electrostatic forces of attraction between the Al3+ ions and the 'sea' of delocalised electrons.

    Generally, the greater the ratio of electrons to ions, the stronger the attraction and thus the higher the boiling point for metals in the same period of the periodic table.

    If you have to draw out a diagram in an exam question, which you should always do if given the opportunity, make sure that the number of electrons you draw is correct for the number of metal ions you draw. For example, if you draw 6 aluminium ions, you will have to draw 3x6=18 electrons, as each aluminium ion gives 3 electrons.
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    (Original post by ilyking)
    i understand, for example, Fe (pure) has Fe positive ions, but do ALL the electrons on the outer shell move out?

    and do these electrons that move out (delocalised) attract to the positive Fe ions?

    thanks
    Not sure if this is what you're looking for, but the simplest definition of metallic bonding is:

    A (giant) lattice of positively charged ions, in a pool/sea of delocalised electrons!

    Sorry if this was not what you need
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    If you still don't understand there are a load of videos on youtube that are very useful i,e:

 
 
 
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