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प्रश्न
Magnetic moment of \[\ce{[MnCl4]^{2-}}\] is 5.92 BM. Explain giving reason.
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
Write the hybridization and shape of the following complexe : [Ni(CN)4]2–
(Atomic number : Co = 27, Ni = 28)
[Fe(H2O)6]3+ is strongly paramagnetic whereas [Fe(CN)6]3− is weakly paramagnetic. Explain.
Explain [Co(NH3)6]3+ is an inner orbital complex whereas [Ni(NH3)6]2+ is an outer orbital complex.
Write down the IUPAC name of the following complex and indicate the oxidation state, electronic configuration and coordination number. Also, give the stereochemistry and magnetic moment of the complex:
K[Cr(H2O)2(C2O4)2].3H2O
Amongst the following ions, which one has the highest magnetic moment value?
Why is [NiCl4]2− paramagnetic while [Ni(CN)4]2− is diamagnetic? (Atomic number of Ni = 28)
Write the hybridization type and magnetic behaviour of the complex [Ni(CN)4]2−. (Atomic number of Ni = 28)
Explain why \[\ce{[Fe(H2O)6]^{3+}}\] has magnetic moment value of 5.92 BM whereas \[\ce{[Fe(CN)6]^{3-}}\] – has a value of only 1.74 BM.
Why do compounds having similar geometry have different magnetic moment?
Assertion: \[\ce{[Fe(CN)6]^{3-}}\] ion shows magnetic moment corresponding to two unpaired electrons.
Reason: Because it has d2sp3 type hybridisation.
