The first ionization enthalpy of the followin | vedclass

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(A) The first ionization enthalpy $(\Delta H_{IE})$ generally increases across a period from left to right and decreases down a group.
Comparing the

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$Si < P < C < N$

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(A) The first ionization enthalpy $(\Delta H_{IE})$ generally increases across a period from left to right and decreases down a group.
Comparing the elements $C$ (Group $14$,Period $2$),$N$ (Group $15$,Period $2$),$Si$ (Group $14$,Period $3$),and $P$ (Group $15$,Period $3$):
$1$. Elements in Period $2$ $(C, N)$ have higher ionization enthalpy than those in Period $3$ $(Si, P)$ due to smaller atomic size.
$2$. Within the same period,Group $15$ elements have higher ionization enthalpy than Group $14$ elements due to the stable half-filled $p$-orbital configuration $(ns^2 np^3)$.
$3$. Combining these trends,the order is $Si < P < C < N$.

The first ionization enthalpy of the following elements are in the order:

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