Which of the following statements is incorrec | vedclass

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(B) Let us analyze the statements:$A$. The second ionization energy of $S$ $(3s^2 3p^4)$ is higher than $Cl$ $(3s^2 3p^5)$ because after removing one

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The third ionization energy of phosphorus is greater than that of aluminium

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(B) Let us analyze the statements:$A$. The second ionization energy of $S$ $(3s^2 3p^4)$ is higher than $Cl$ $(3s^2 3p^5)$ because after removing one electron,$S^+$ achieves a stable half-filled $p^3$ configuration.$B$. The third ionization energy of $P$ $(3s^2 3p^3)$ is actually lower than that of $Al$ $(3s^2 3p^1)$ because $Al^{2+}$ has a stable noble gas core configuration $([Ne] 3s^1)$,making the removal of the third electron very difficult. Thus,this statement is incorrect.$C$. The first ionization energy of $Al$ and $Ga$ are similar due to the poor shielding effect of $d$-electrons in $Ga$ (lanthanoid contraction effect).$D$. The second ionization energy of $B$ $(2s^2 2p^1)$ is greater than $C$ $(2s^2 2p^2)$ because the second electron in $B$ is removed from the stable $2s^2$ orbital.

Which of the following statements is incorrect?

Similar Questions

Assertion $(A)$: First ionisation enthalpy of oxygen is less than that of nitrogen.
Reason $(R)$: Atoms with half-filled or completely filled orbitals are less stable.
The correct option among the following is:

From the ground state electronic configuration of the elements given below,pick up the one with the highest value of second ionization energy.

Which is the correct order of the first ionization potential of $N$,$O$,and $C$?

Which of the following is the correct order of increasing second ionization energy?

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

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