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प्रश्न
Why is [NiCl4]2− paramagnetic while [Ni(CN)4]2− is diamagnetic? (Atomic number of Ni = 28)
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उत्तर
The compound, [NiCl4]2−, is paramagnetic since it contains two unpaired electrons.
The compound, [Ni(CN)4]2−, is diamagnetic as evident from the absence of unpaired electron
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संबंधित प्रश्न
For the complex [Fe(CN)6]3–, write the hybridization type, magnetic character and spin nature of the complex. (At. number : Fe = 26).
Write the hybridization and magnetic behaviour of the complex [Ni(CO)4].
(At.no. of Ni = 28)
[NiCl4]2− is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why?
Amongst the following ions, which one has the highest magnetic moment value?
Write the hybridisation and magnetic character of [Co(C2O4)3]3–.
(At. no. of Co = 27)
Write the hybridization and magnetic character of the following complexes:
[Fe(H2O)6]2+
(Atomic no. of Fe = 26)
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.
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
Given below are two statements:
Statement I: Ferromagnetism is considered as an extreme form of paramagnetism.
Statement II: The number of unpaired electrons in a Cr2+ ion (Z = 24) is the same as that of a Nd3+ ion (Z = 60).
In the light of the above statements, choose the correct answer from the options given below:
