Which of the following metals is expected to | vedclass

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(C) The electronic configurations of the given metals are:$Cr: [Ar] \, 3d^5 \, 4s^1$$V: [Ar] \, 3d^3 \, 4s^2$$Mn: [Ar] \, 3d^5 \, 4s^2$$Fe: [Ar] \, 3d

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$Mn$ $(Z=25)$

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(C) The electronic configurations of the given metals are:$Cr: [Ar] \, 3d^5 \, 4s^1$$V: [Ar] \, 3d^3 \, 4s^2$$Mn: [Ar] \, 3d^5 \, 4s^2$$Fe: [Ar] \, 3d^6 \, 4s^2$To find the third ionization enthalpy,we remove two electrons first:For $Mn$,the configuration after removing two electrons $(Mn^{2+})$ is $[Ar] \, 3d^5$. This is a half-filled stable $d$-orbital configuration.Removing the third electron from this stable $3d^5$ configuration requires a very high amount of energy.Therefore,$Mn$ has the highest third ionization enthalpy among the given options.

Which of the following metals is expected to have the highest third ionization enthalpy?

Similar Questions

Given below are two statements:
Statement $(I)$: The first ionisation enthalpy of the elements $Na$, $Mg$, $Cl$ and $Ar$ follows the order $Na > Mg > Cl > Ar$.
Statement $(II)$: Among $Ca$, $Al$, $Fe$ and $B$, the third ionisation enthalpy is very high for $Ca$.

The correct order of first ionization enthalpy values of the following elements is:
$A. O$,$B. N$,$C. Be$,$D. F$,$E. B$
Choose the correct answer from the options given below:

The correct trend in the first ionization enthalpies of the elements in the $3^{rd}$ period of periodic table is:

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

Among the following,which has the highest first ionization energy?

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