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प्रश्न
Magnetic moment of \[\ce{[MnCl4]^{2-}}\] is 5.92 BM. Explain giving reason.
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उत्तर
The magnetic moment of 5.92 BM corresponds to the presence of five unpaired electrons in the d-orbitals of \[\ce{Mn^2+}\] ion. As a result the hybridisation involved is sp3 rather than dsp2. Thus tetrahedral structure of \[\ce{[MnCl4 ]^{2-}}\] complex will show 5.92 BM magnetic moment value.
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संबंधित प्रश्न
For the complex [Fe(H2O)6]+3, write the hybridisation, magnetic character and spin of the complex. (At, number : Fe = 26)
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(At.no. of Ni = 28)
Write the hybridization and shape of the following complexe : [CoF6]3–
(Atomic number : Co = 27, Ni = 28)
[NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why?
[Fe(H2O)6]3+ is strongly paramagnetic whereas [Fe(CN)6]3− is weakly paramagnetic. Explain.
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[At. No.: Co = 27, Ni = 28]
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K[Cr(H2O)2(C2O4)2].3H2O
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(At. no. of Co = 27)
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Which of the following options are correct for \[\ce{[Fe(CN)6]^{3-}}\] complex?
(i) d2sp3 hybridisation
(ii) sp3d2 hybridisation
(iii) paramagnetic
(iv) diamagnetic
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Assertion: \[\ce{[Fe(CN)6]^{3-}}\] ion shows magnetic moment corresponding to two unpaired electrons.
Reason: Because it has d2sp3 type hybridisation.
[Ti(H2O6]3+ T is paramagnetic is nature due to
Low oxidation state of metals in their complexes are common when ligands ______.
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[Atomic number: Fe = 26]
