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Hello students, in this question we have to draw the d -orbital diagram of hexa -cyano -cobaltate ion.
00:06
First of all we have to find out the oxidation state of the cobaltate ion in the given complex which is given by let the oxidation state of cobalt be x and the charge of cyanide ion is minus 1, 6 into minus 1 will be equal to minus 6, this will be equal to minus 4, then x will be equal to plus 2.
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Therefore, cobalt exists as cobalt 2 plus ion.
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So, the electronic configuration of cobalt 2 plus ion is argon 3d 7.
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So, let us start filling this orbital.
00:37
Since cyanide is a strong filled ligand, then the splitting of the d -orbital will consist of t2g will have a lower energy compared to the eg.
00:48
Therefore, this will be our eg orbital and this will be our t2g orbital and this will be our 3d orbitals.
00:55
Let us start filling the electron as there are 7 electrons in the d -orbital 1, 2, 3, 4, 5, 6 and 7.
01:05
Since cyanide is a strong filled ligand, the electron will exist as a pair.
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Therefore, 1, 2, 3, 4, 5, 6 and 7.
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So, this will be the d -orbital diagram of the given complex.
01:20
We have to predict whether the given complex is paramagnetic or diamagnetic...