Consider the elements Mg. Al, S, P and Si, the correct increasing order of their first ionization enthalpy is.

Question:

Consider the elements $\mathrm{Mg} . \mathrm{Al}, \mathrm{S}, \mathrm{P}$ and $\mathrm{Si}$, the correct increasing order of their first ionization enthalpy is.

$\mathrm{Al}<\mathrm{Mg}<\mathrm{Si}<\mathrm{S}<\mathrm{P}$

  1. (1) $\mathrm{Mg}<\mathrm{Al}<\mathrm{Si}<\mathrm{S}<\mathrm{P}$

  2. (2) $\mathrm{Al}<\mathrm{Mg}<\mathrm{Si}<\mathrm{S}<\mathrm{P}$

  3. (3) $\mathrm{Mg}<\mathrm{Al}<\mathrm{Si}<\mathrm{P}<\mathrm{S}$

  4. (4) $\mathrm{Al}<\mathrm{Mg}<\mathrm{S}<\mathrm{Si}<\mathrm{P}$

Correct Option: , 2

Solution:

In general from left to right in a period, ionistion enthalpy increases due to effective nuclear charge increases. but due to extra stability of half filled and full filled electronic configuration, required ionisation enthalpy is more from neighbouring elements. i.e. first ionisation enthalpy order is 

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