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:

Similar Questions

What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?

Which of the following electronic configurations represents a sudden large gap between the values of second and third ionisation energies of an element?

Which of the following has the least ionization potential?

Which one of the following statements is incorrect in relation to ionisation enthalpy?

The correct order of the first ionization enthalpies of the following elements is:

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