How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
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first ionization enthalpy of sodium is lower than magnesium because atomic size of sodium is greater than magnesium. After removal of one electron sodium acquire neon's configuration which is highly stable as it is inert gas. Therefore energy requirement will more to remove second electron in sodium. while in magnesium after removing one electron it acquires sodium's configuration which can easily loose second electron therefore energy required will be less. hence
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Answer:
Explanation:
since, Mg has full filled 3s orbital it is in a very stable state and it does not want to lose any electron because it will make it unstable. while Na has only one electron in 3s and to attain the nearest noble gas configuration it only requires to lose one electron which is not so expensive because altogether it will make it more stable. And this is why Na always forms ionic compounds.
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