Electron configurations of transition element ions

Write electron configurations of first-row transition element ions, removing 4s electrons before 3d, and explain variable oxidation states by the closeness of the successive ionization energies of the 4s and 3d electrons.

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What is the electron configuration of the $\ce{Co^2+}$ ion? A. $\ce{[Ar] 3d^7}$ B. $\ce{[Ar] 4s^2 3d^5}$ C. $\ce{[Ar] 4s^1 3d^6}$ D. $\ce{[Ar] 4s^2 3d^7}$

Vanadium forms compounds in the +2, +3, +4 and +5 oxidation states. Which statement explains why vanadium shows a range of oxidation states? A. The 3d sublevel splits into two sets of orbitals of different energy in its complexes B. The 3d and 4s electrons…

Which element forms a stable compound in which its oxidation state is +6? A. Ti B. V C. Cr D. Zn

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