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.

List-$I$	List-$II$
$(1)$ $Ti^+$	$(A)$ $(n-1)d^4ns^2$
$(2)$ $_{30}Zn$	$(B)$ $(n-1)d^{10}ns^1$
$(3)$ $_{24}Cr$	$(C)$ $(n-1)d^2ns^0$
$(4)$ $_{29}Cu$	$(D)$ $(n-1)d^5ns^1$
	$(E)$ $(n-1)d^0ns^2$
	$(F)$ $(n-1)d^{10}ns^2$

Which ion has the highest ionisation enthalpy?

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Match the elements in List-$I$ with their electronic configurations in List-$II$.

List-$I$ List-$II$

$(1)$ $Ti^+$ $(A)$ $(n-1)d^4ns^2$

$(2)$ $_{30}Zn$ $(B)$ $(n-1)d^{10}ns^1$

$(3)$ $_{24}Cr$ $(C)$ $(n-1)d^2ns^0$

$(4)$ $_{29}Cu$ $(D)$ $(n-1)d^5ns^1$

$(E)$ $(n-1)d^0ns^2$

$(F)$ $(n-1)d^{10}ns^2$

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