Consider the elements Mg,Al,S,P and Si. The c | vedclass

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(B) In general,from left to right in a period,the first ionization enthalpy increases due to an increase in effective nuclear charge. However,due to t

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$Al < Mg < Si < S < P$

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(B) In general,from left to right in a period,the first ionization enthalpy increases due to an increase in effective nuclear charge. However,due to the extra stability of half-filled $(p^3)$ and fully-filled $(s^2)$ electronic configurations,the ionization enthalpy of certain elements is higher than their neighbors. The electronic configurations are: $Mg$ $([Ne] 3s^2)$,$Al$ $([Ne] 3s^2 3p^1)$,$Si$ $([Ne] 3s^2 3p^2)$,$P$ $([Ne] 3s^2 3p^3)$,and $S$ $([Ne] 3s^2 3p^4)$. Due to the stable $s^2$ configuration of $Mg$,its ionization enthalpy is higher than $Al$. Due to the stable half-filled $p^3$ configuration of $P$,its ionization enthalpy is higher than $S$. Thus,the correct increasing order is $Al < Mg < Si < S < P$.

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

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