How would you explain the fact that first ionization enthalpy of na is lower than mg but its second enthalpy is higher than that of mg?
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electronic configuration of Na=1s2,2s2, 2p6, 3s1.
electronic configuration of Mg=1s2,2s2, 2p6, 3s2
s subshell of na is half filled whereas s subshell of mg is full filled.
full filled subshells are more stable than half filled subshells
hence it is easy to remove 1 electron from Na.
therefore its first ionisation enthalpy is low.
after losing 1 electron
electronic configuration of Na=1s2,2s2, 2p6
electronic configuration of Mg=1s2,2s2, 2p6, 3s1
as mentioned above full filled are more stable than half filled.
so it is easy to remove 1 electron from mg as compared to Na.
hence second ionisation enthalpy of Na is greater than Mg.
hope it helps you
electronic configuration of Mg=1s2,2s2, 2p6, 3s2
s subshell of na is half filled whereas s subshell of mg is full filled.
full filled subshells are more stable than half filled subshells
hence it is easy to remove 1 electron from Na.
therefore its first ionisation enthalpy is low.
after losing 1 electron
electronic configuration of Na=1s2,2s2, 2p6
electronic configuration of Mg=1s2,2s2, 2p6, 3s1
as mentioned above full filled are more stable than half filled.
so it is easy to remove 1 electron from mg as compared to Na.
hence second ionisation enthalpy of Na is greater than Mg.
hope it helps you
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