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    Hi

    Can someone explain to me why the second IE of sodium is greater than the 2nd IE of Magnesium.

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    This is because after one electron has been removed there will be less electrons and the nuclear charge will remain the same so there will be a greater attraction between the nucleus and the outer shell electrons. (hope this helps)
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    (Original post by chronicl3)
    Hi

    Can someone explain to me why the second IE of sodium is greater than the 2nd IE of Magnesium.

    Thanks
    Na is in Gp 1, Mg is in Gp 2. After 1st IE, the next electron to be removed from in Na is in 2p that is a fully filled 2p. As E is inversely proportional to n square, lower n mean bigger E(empirically).

    This is due to greater effective nuclear charge in Na+ if removing from 2p compared to removing the second electron from a 3s(ie Mg+). Greater Zeff = greater IE
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    (Original post by chronicl3)
    Hi

    Can someone explain to me why the second IE of sodium is greater than the 2nd IE of Magnesium.

    Thanks

    heyy well the electron being removed from Na is in the 2nd energy level, whilst the electron being removed from Mg is still in the 3rd energy level, so for Na there is less shielding, and the electron is closer to the nucelus so the attraction is stronger for Na,
    i think i know which paper ur doing, would you like the markscheme ?
 
 
 
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