Step 1: Identify the metal from its oxide formulas
The set of oxides M
2O
n with n = 3, 4, 5 corresponds to oxidation states +3, +4 and +5, respectively (since for M
2O
n, 2×Ox(M) − 2n = 0 ⇒ Ox(M) = n). Among first-row transition metals, vanadium forms precisely V
2O
3 (V(+3)), V
2O
4 (equivalently VO
2, V(+4)) and V
2O
5 (V(+5)). Vanadium is also noted for a very high enthalpy of atomisation in the first series, consistent with the prompt.
Step 2: Pick the amphoteric oxide from V2O3, V2O4, V2O5
Among these vanadium oxides, the one exhibiting amphoteric behaviour in many textbook treatments is V
2O
5. It can react with strong bases to give vanadates and participates in acid-vanadate equilibria (polyvanadates), reflecting amphoteric character.
Step 3: Determine the d-electron count in the amphoteric oxide
In V
2O
5, vanadium is in the +5 oxidation state. For vanadium (Z = 23), the neutral atom configuration is [Ar] 3d
3 4s
2. Therefore, V(+5) is 3d
0 (no d electrons).
Step 4: Compute the spin-only magnetic moment
The spin-only magnetic moment is given by
μ
so = √(n(n + 2)) BM, where n = number of unpaired electrons.
For V(+5) with 3d
0, n = 0 ⇒ μ
so = √(0 × 2) = 0 BM (near integer).
Final answer
0