The spin-only magnetic moment value of the most basic oxide of vanadium among $$V_2O_3$$, $$V_2O_4$$ and $$V_2O_5$$ is ______ B.M. (Nearest integer)

We need to find the spin-only magnetic moment of the most basic oxide of vanadium.

Identify the most basic oxide.

The oxides given are $$V_2O_3$$, $$V_2O_4$$ (i.e., $$VO_2$$), and $$V_2O_5$$.

The oxidation states of vanadium are +3, +4, and +5 respectively.

Lower oxidation state oxides are more basic. Therefore, $$V_2O_3$$ (with V in +3 state) is the most basic oxide.

Find the electronic configuration of $$V^{3+}$$.

V: [Ar] 3d$$^3$$ 4s$$^2$$

$$V^{3+}$$: [Ar] 3d$$^2$$ (2 unpaired electrons)

Calculate the spin-only magnetic moment.

$$\mu = \sqrt{n(n+2)} \text{ B.M.}$$

where $$n$$ = number of unpaired electrons = 2

$$\mu = \sqrt{2(2+2)} = \sqrt{8} = 2\sqrt{2} \approx 2.83 \text{ B.M.}$$

Rounding to the nearest integer: $$\mu \approx \textbf{3}$$ B.M.