JEE MAIN - Chemistry (2021 - 16th March Evening Shift - No. 12)
Arrange the following metal complex/compounds in the increasing order of spin only magnetic moment. Presume all the three, high spin system.
(Atomic numbers Ce = 58, Gd = 64 and Eu = 63)
(a) (NH4)2[Ce(NO3)6]
(b) Gd(NO3)3 and
(c) Eu(NO3)3
(Atomic numbers Ce = 58, Gd = 64 and Eu = 63)
(a) (NH4)2[Ce(NO3)6]
(b) Gd(NO3)3 and
(c) Eu(NO3)3
(a) < (b) < (c)
(b) < (a) < (c)
(a) < (c) < (b)
(c) < (a) < (b)
Explanation
(A) $${}_{58}Ce \to [Xe]4{f^2}5{d^0}6{s^2}$$
In complex $$C{e^{ + 4}} \to [Xe]4{f^0}5{d^0}6{s^0}$$
There is no unpaired electron, so, $$\mu$$m = 0 BM
(B) $${}_{64}Gd \to [Xe]4{f^7}5{d^1}6{s^2}$$
In complex, $${}_{64}G{d^{2 + }} \to [Xe]4{f^7}5{d^1}$$
There are 8 unpaired electrons.
$$\therefore$$ $${\mu _m} = \sqrt {8(8 + 2)} = \sqrt {80} = 8.94BM$$
(C) $${}_{63}Eu \to [Xe]4{f^9}5{d^0}6{s^0}$$
In complex $${}_{63}E{u^{ + 3}} \to [Xe]4{f^6}5{d^0}6{s^0}$$
contain six unpaired electrons.
So, $${\mu _m} = \sqrt {6(6 + 2)} = \sqrt {48} BM = 6.93BM$$
Hence, order of spin only magnetic moment
$$B > C > A$$.
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