What is v2+ electron configuration?

Vanadium(II) (V²⁺) has an electron configuration that is derived from its neutral atom vanadium (V).

• Neutral Vanadium (V): The electron configuration of neutral vanadium (atomic number 23) is [Ar] 3d³4s².

• Vanadium(II) (V²⁺): When vanadium forms a 2+ ion, it loses two electrons. These electrons are removed from the outermost shell first, which are the 4s electrons. Therefore, the electron configuration of V²⁺ becomes [Ar] 3d³.

• Important Aspects:

  • [Argon Core]: The "[Ar]" represents the filled electron configuration of argon, which is 1s²2s²2p⁶3s²3p⁶.

  • d-Orbital Configuration: The 3d³ configuration indicates that there are three electrons in the 3d orbitals. These electrons will typically occupy the d-orbitals individually according to Hund's%20Rule to minimize electron-electron repulsion.

  • Paramagnetism: Because V²⁺ has unpaired electrons (three of them), it is paramagnetic. This means it is attracted to magnetic fields.

  • Color: Aqueous solutions of V²⁺ are typically violet in color due to d-d transitions.