Which ion has the highest ionisation enthalpy | vedclass

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(C) The electronic configurations of the given ions are:$Ti^{+} (Z=22): [Ar] 3d^2 4s^1$$V^{+} (Z=23): [Ar] 3d^3 4s^1$$Cr^{+} (Z=24): [Ar] 3d^5 4s^0$$M

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$Cr^{+}$

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(C) The electronic configurations of the given ions are:$Ti^{+} (Z=22): [Ar] 3d^2 4s^1$$V^{+} (Z=23): [Ar] 3d^3 4s^1$$Cr^{+} (Z=24): [Ar] 3d^5 4s^0$$Mn^{+} (Z=25): [Ar] 3d^5 4s^1$Ionisation enthalpy is the energy required to remove an electron from the outermost shell.$Cr^{+}$ has a stable half-filled $3d^5$ configuration with no electrons in the $4s$ orbital.Removing an electron from a stable,half-filled $d$-subshell requires significantly more energy compared to removing an electron from the $4s$ orbital of the other ions.Therefore,$Cr^{+}$ has the highest ionisation enthalpy.

$E^{\Theta }$	$V$	$Cr$	$Mn$	$Fe$	$Co$	$Ni$	$Cu$
$(M^{2+}/M)$	$-1.18$	$-0.91$	$-1.18$	$-0.44$	$-0.28$	$-0.25$	$+0.35$

Which ion has the highest ionisation enthalpy?

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For the first row transition metals,the $E^{\Theta }$ values are:

$E^{\Theta }$ $V$ $Cr$ $Mn$ $Fe$ $Co$ $Ni$ $Cu$

$(M^{2+}/M)$ $-1.18$ $-0.91$ $-1.18$ $-0.44$ $-0.28$ $-0.25$ $+0.35$

Explain the irregularity in the above values.

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