The incorrect statement is:

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) . $Se$ $([Ar] 3d^{10} 4s^2 4p^4)$ and $As$ $([Ar] 3d^{10} 4s^2 4p^3)$. After removing one electron,$Se^+$ has $4p^3$ and $As^+$ has $4p^2$. Removi

Vedclass · Accepted Answer

Halogens have the highest $I.E.$ in their respective periods.

Vedclass · Answer

(D) . $Se$ $([Ar] 3d^{10} 4s^2 4p^4)$ and $As$ $([Ar] 3d^{10} 4s^2 4p^3)$. After removing one electron,$Se^+$ has $4p^3$ and $As^+$ has $4p^2$. Removing the second electron from $Se^+$ is harder due to the stable half-filled $p$-orbital,so this statement is correct.$B$. $C^{2+}$ has $1s^2 2s^2$ configuration,while $N^{2+}$ has $1s^2 2s^2 2p^1$. Removing an electron from the stable $2s^2$ shell of $C^{2+}$ requires more energy than from the $2p^1$ orbital of $N^{2+}$. This statement is correct.$C$. $F^{2+}$ has $1s^2 2s^2 2p^3$ and $O^{2+}$ has $1s^2 2s^2 2p^2$. Removing the third electron from $F^{2+}$ (half-filled $p$-orbital) is harder than from $O^{2+}$. This statement is correct.$D$. Noble gases have the highest $I.E.$ in their respective periods,not halogens. Therefore,this statement is incorrect.

Similar Questions

The correct values of ionization enthalpies (in $kJ \ mol^{-1}$) of $Si, P, Cl$ and $S$ respectively are

What will be the order of $1^{st}$ ionisation energy for the alkali metals $Li$,$Na$,and $K$?

With reference to the concept of ionisation potential,which one of the following sets is correct?

Which electrons are removed to determine the ionization enthalpy of beryllium and boron,respectively?

Which of the following electronic configurations will have the highest tendency to form a univalent gaseous cation?

Vedclass Test Series

Exam Paper Generator

Online Exam Module