Which of the following series of transition m | vedclass

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(B) The electronic configuration of the neutral atoms is as follows:$Ti (Z=22): [Ar] 3d^2 4s^2$$V (Z=23): [Ar] 3d^3 4s^2$$Cr (Z=24): [Ar] 3d^5 4s^1$$M

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$Ti^{2+}, V^{3+}, Cr^{4+}, Mn^{5+}$

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(B) The electronic configuration of the neutral atoms is as follows:$Ti (Z=22): [Ar] 3d^2 4s^2$$V (Z=23): [Ar] 3d^3 4s^2$$Cr (Z=24): [Ar] 3d^5 4s^1$$Mn (Z=25): [Ar] 3d^5 4s^2$Calculating the configurations for the ions in option $B$:$Ti^{2+}: [Ar] 3d^2$$V^{3+}: [Ar] 3d^2$$Cr^{4+}: [Ar] 3d^2$$Mn^{5+}: [Ar] 3d^2$All these ions possess a $3d^2$ electronic configuration.

Which of the following series of transition metal ions has a $3d^2$ electronic configuration?

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