The magnetic moments of a complex ion is 2.83 BM. The complex ions is:

[V (H_{2} O)_{6}]^{3 +}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

[C r (H_{2} O)_{6}]^{3 +}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

[C u (C N)_{4}]^{2 -}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

[M n C l_{4}]^{2 -}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $[V (H_{2} O)_{6}]^{3 +}$
$\sqrt{n (n + 2)}$ = 2.83. Hence n=2 i.e. The number of unpaired electron =2.The compound $[V (H_{2} O)_{6}]^{3 +}$ have $3 d^{2}$ configuration and 2 unpaired electron. Hence the correct option is A.

Suggest Corrections

Similar questions

P, Q,

R

P = [F e F_{6}]^{3 -}, Q = [V (H_{2} O)_{6}]^{2 +}

R = [F e (H_{2} O)_{6}]^{2 +}

2.83 B M

2.83 B M

P = [F e F_{6}]^{3 -}, Q = [V (H_{2} O)_{6}]^{2 +} and R = [F e (H_{2} O)_{6}]^{2 +}

{[C r {(H_{2} O)}_{6}]}^{3 +}

Join BYJU'S Learning Program