Electron Configuration of Vanadium (V)
What is the electron configuration of Vanadium?
The electron configuration of Vanadium (V, Z=23) is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d³ 4s². In noble gas shorthand: [Ar] 3d³ 4s². It has 3 unpaired electron(s) and is a d-block element.
| Symbol | V |
| Atomic Number | 23 |
| Full Electron Configuration | 1s² 2s² 2p⁶ 3s² 3p⁶ 3d³ 4s² |
| Noble Gas Shorthand | [Ar] 3d³ 4s² |
| Block | d |
| Period | 4 |
| Group | 5 |
| Unpaired Electrons | 3 |
| Exception? | No |
Orbital Filling Order
Following the aufbau principle, the 23 electrons in Vanadium fill orbitals in order of increasing energy: 1s (2 electrons), then 2s (2 electrons), then 2p (6 electrons), then 3s (2 electrons), then 3p (6 electrons), then 3d (3 electrons), then 4s (2 electrons).
Each orbital is filled according to the Pauli exclusion principle (at most 2 electrons per orbital) and Hund's rule (electrons occupy degenerate orbitals singly before pairing).
Noble Gas Shorthand
The inner electrons of Vanadium match the configuration of Ar. This allows us to abbreviate the configuration as [Ar] 3d³ 4s², where [Ar] represents the filled core and the remaining entries show the valence electrons.
Valence Electrons
The valence shell of Vanadium contains 3 electrons in the 3d subshell and 2 electrons in the 4s subshell. These outermost electrons determine Vanadium's chemical reactivity, bonding behavior, and position in the periodic table as a d-block element in period 4.
Visualize orbital filling with 3D orbital shapes, aufbau principle, and noble gas shorthand for 36 elements.
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Vanadium on the Periodic Table
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Orbital Hybridization
See how atomic orbitals mix to form sp, sp2, and sp3 hybrids