First ionisation enthalpy of ({Al}) is lower than that of ({... | Chemistry | SolveeIt

Question

First ionisation enthalpy of ${Al}$ is lower than that of ${Mg}$ . This is because

the size of Al is bigger than $\({Mg}$ )

ionisation enthalpy decreases in a period from left to right

it is easier to remove electron from unpaired $3p^1$ than from paired $3s^2$

aluminium is a passive metal while magnesium is active.

Answer

it is easier to remove electron from unpaired $3p^1$ than from paired $3s^2$

Explanation

Solution

Electronic configuration of $\({Al} - 1s^2 2s^2 2p^6 3s^2 3p^1$ ) Electronic configuration of $\({Mg} - 1s^22s^22p^63s^2$ ) It is difficult to remove electron from paired $\(3s^2$ )-orbital than unpaired $\(3p^1$ ). Hence, $\(I.E.$ ) of $\({Al}$ ) is lower than $\({Mg}$ ).

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