Which one of the following elements has the h | vedclass

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(C) The electronic configuration of the given elements corresponds to $Al$ $(3p^1)$,$Si$ $(3p^2)$,$P$ $(3p^3)$,and $Ge$ $(4p^2)$.Ionization energy gen

Vedclass · Accepted Answer

$[Ne] \, 3s^2 \, 3p^3$

Vedclass · Answer

(C) The electronic configuration of the given elements corresponds to $Al$ $(3p^1)$,$Si$ $(3p^2)$,$P$ $(3p^3)$,and $Ge$ $(4p^2)$.Ionization energy generally increases across a period.However,the $p^3$ configuration represents a half-filled stable subshell.Due to the extra stability of the half-filled $p$-orbital,the energy required to remove an electron from $[Ne] \, 3s^2 \, 3p^3$ is the highest among the given options.

Which one of the following elements has the highest ionisation energy?

Similar Questions

Given below are two statements:
Statement $I$: The second ionization enthalpy of $B$, $Al$ and $Ga$ is in the order of $B > Al > Ga$.
Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.

Element having highest $I.P.$ value is

The correct order of $C$, $N$, $O$ and $F$ in terms of second ionisation potential is

Which of the following electronic configurations will have the least $I.P.$ value?

Which of the following is not the correct increasing order of ionisation energy?

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