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The magnetic moment (spin only) of [NiCl...

The magnetic moment (spin only) of `[NiCl_(4)]^(2-)` is

A

1.82 B.M.

B

5.46 B.M.

C

2.82 B.M.

D

1.41 B.M.

Text Solution

Verified by Experts

The correct Answer is:
C
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Deduce the structure of [Nicl_(4)]^(2) and [Ni(Cl_(4)]^(2-) considering the hybridization of the metal. Calculate the magnetic moment (spin only) of the species.

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Knowledge Check

  • Valence bond theory successfully explains the magnetic behaviour of complexes. The substances which contains unpaired electrons. and paramagnetic character increases as the mumber of unpaired electrons increases. Magnetic moment of a complex can be determined experimentally and by using formula sqrt(n(n+2)) and we can determine the number of unpaired electrons in it. This information is important in writing the electronic structure of complex which in turm is also useful in deciding the geometry of complex. The magnetic moments (spin only) of [NiCl_(4)]^(2-) and [Ni(CN)_(4)]^(2-) are:

    A
    0,0
    B
    2.82 B.M., 2.82 B.M.
    C
    0,2.82 B.M.
    D
    2.82 B.M., 0

  • The magnitude of magnetic moment of [NiCl_(4)]^(2-) will be:

    A
    2.82 B.M
    B
    3.25 B.M
    C
    1.23 B.M
    D
    5.64 B.M

  • The spin only magnetic moment of [MnBr_(4)]^(2-) is 5.9 B.M. Geometry of the complex ion is

    A
    Tetrahedral
    B
    Octahedral
    C
    Square planar
    D
    Pentagonal pyramidal

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    Deduce the structure of [Nicl_(4)]^(2) and [Ni (Cl_ (4)] ^ (2-) considering the hybridization of the metal. Calculate the magnetic moment (spin only) of the species.

    The spin only magnetic moment of [MnBr_(4)]^(2-) is 5.9 BM. Predict the geometry of the complex ion.

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    Ion(s) having non zero magnetic moment (spin only) is/are

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