Question

Which one of the following cyano complexes would exhibit
the lowest value of paramagnetic behaviour ?
(a) Co(CN)₆]³⁻ (b) [Fe(CN)₆]³⁻
(c) [Mn(CN)₆]³⁻ (d) [Cr(CN)₆]³⁻
(At. Nos : Cr = 24, Mn = 25, Fe = 26, Co = 27)

Answer 1

Which one of the following cyano complexes would exhibit

the lowest value of paramagnetic behaviour ?

(a) Co(CN)₆]³⁻

(b) [Fe(CN)₆]³⁻

(c) [Mn(CN)₆]³⁻

(d) [Cr(CN)₆]³⁻

(At. Nos : Cr = 24, Mn = 25, Fe = 26, Co = 27)

Answer 2

[Co(CN)₆]³⁻ is the complex having least paramagnetic behaviour.

Explanation:

• Paramagnetism is a phenomenon where the ion or radicle responds to the magnetic field.

• Paramagnetism is seen because of the presence of unpaired electrons.

• In case of the complex hexacyanocobalt 3+,

• The atomic number of Cobalt is 27.

• So the electronic configuration of Co is [Ar] 4s2 3d7.

• So the electronic configuration of Co3+ is [Ar] 4s0 3d6.

• Cyanide is a strong field chelate.

• So in presence of cyanide the electrons pair up.

• So there remains zero unpaired electrons to exhibit paramagnetism.

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