Vanadium (V)

Atomic Model Details

Vanadium (V) is a d-block transition element with atomic number 23.

Atomic Number (Z): 23
- Indicates 23 protons in the nucleus.
- In a neutral Vanadium atom, there are 23 electrons.
Atomic Mass (Average): 50.9415 u
Most Common Isotope: $^{51}$V
- Number of Protons: 23
- Number of Neutrons: (Mass Number - Atomic Number) = 51 - 23 = 28
- Number of Electrons: 23 (in a neutral atom)
Atomic Radius:
- Metallic Radius: 134 pm
- Covalent Radius: 122 pm (approx.)

Ground State Electronic Configuration: $[Ar] 3d^3 4s^2$
- This configuration indicates that the outermost electrons are in the 3d and 4s subshells, characteristic of a d-block element. The 4s electrons are filled before the 3d electrons, but in writing, the d-subshell is often grouped with the principal quantum number ‘3’ shells.
Shell-wise Electron Distribution:
- K-shell (n=1): 2 electrons ($1s^2$)
- L-shell (n=2): 8 electrons ($2s^2 2p^6$)
- M-shell (n=3): 11 electrons ($3s^2 3p^6 3d^3$)
- N-shell (n=4): 2 electrons ($4s^2$)
- Thus, the electron distribution can be represented as: 2, 8, 11, 2.

Ionization Enthalpy:
- First Ionization Enthalpy ($IE_1$): 650.9 kJ/mol (Energy required to remove the first electron)
- Second Ionization Enthalpy ($IE_2$): 1414 kJ/mol (Energy required to remove the second electron)
- Third Ionization Enthalpy ($IE_3$): 2830 kJ/mol (Energy required to remove the third electron)
- Trend: Ionization enthalpies generally increase across a period due to increasing effective nuclear charge. For transition metals, the removal of 4s electrons typically precedes 3d electrons for the formation of ions.
Electronegativity (Pauling Scale): 1.63
- Trend: Electronegativity generally increases across a period. Vanadium’s value is typical for a transition metal, indicating moderate electron-attracting power.
Electron Gain Enthalpy: -50 kJ/mol
- This value indicates that energy is released when a neutral Vanadium atom gains an electron, though it is not strongly exothermic compared to p-block elements.
Atomic Radius: (See Atomic Model Details above)
- Trend: Atomic radius generally decreases across a period due to increasing effective nuclear charge pulling the electron cloud closer to the nucleus. However, for transition metals, this decrease is less pronounced due to the screening effect of the d-electrons.