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    I read somewhere on a website that melting points down group 2 decrease because:

    -Same charge on the metal (+2)
    -Same number of delocalised electrons
    -Increase in atomic radius
    -Therefore only thing affecting melting point in atomic radius. Increase in radius means less attraction so weaker bonds

    My question is, Why does the number of delocalised electrons stay the same down group 2, surely they should increase because the number of protons and therfore electrons are increasing.


    PS This is all in terms of melting points when the elements have metallic bonds, eg. Mg2+

    My other question is, do all metals such as sodium and magnesium naturally have mettalic bonds. If the answer is yes, then ignore the PS part.

    Thanks
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    Only the 2 outermost electrons delocalise, so there's more shielding between the positive nucleus and delocalised electrons.
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    (Original post by ThisIsOurDecision)
    Only the 2 outermost electrons delocalise, so there's more shielding between the positive nucleus and delocalised electrons.
    Ohhh, thanks so much mate.
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    My other question is, do all metals such as sodium and magnesium naturally have mettalic bonds, If yes, then does this mean all metals only exist as Ions
 
 
 
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