Given below are two statements:Statement-I: T | vedclass

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(B) The electronic configurations are:$Cr = [Ar] 3d^{5} 4s^{1}$$Mn = [Ar] 3d^{5} 4s^{2}$Statement-$I$: The first ionization enthalpy $(IE_{1})$ of $Cr

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Statement-$I$ is true but Statement-$II$ is false.

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(B) The electronic configurations are:$Cr = [Ar] 3d^{5} 4s^{1}$$Mn = [Ar] 3d^{5} 4s^{2}$Statement-$I$: The first ionization enthalpy $(IE_{1})$ of $Cr$ is lower than that of $Mn$ because $Mn$ has a stable half-filled $d$-subshell and a full $s$-subshell, making it harder to remove an electron. Thus, Statement-$I$ is true.Statement-$II$: For $IE_{2}$, $Cr$ loses its $4s^{1}$ electron to reach a stable $3d^{5}$ configuration, while $Mn$ loses its $4s^{1}$ electron from a $3d^{5} 4s^{2}$ configuration. However, $IE_{2}$ of $Cr$ is higher than $Mn$ because removing the second electron from $Cr$ disrupts the stable $d^{5}$ configuration. For $IE_{3}$, $Mn$ has a higher value because it involves removing an electron from the stable $d^{5}$ configuration of $Mn^{2+}$. Therefore, Statement-$II$ is false.

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