
Among the following, which complex compound is diamagnetic?
(i)-
(ii)-
(iii)-
(iv)-
(a)- (i)
(b)- (ii)
(c)- (iii)
(d)- (iv)
Answer
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Hint: If the compound has unpaired electrons then the compound is paramagnetic and if it has all the electrons in pairs then it is diamagnetic. In a complex compound, the diamagnetic nature is calculated by finding the oxidation number of the central metal atom and then its configuration.
Complete answer:
Let us study all the complexes one by one:
(i)-
First, we have to calculate the oxidation number of cobalt ions.
The oxidation number of is zero because it is a neutral ligand and the oxidation number of is -1. So, the oxidation number of cobalt is:
So, the oxidation number of cobalt is +3.
The ground state electronic configuration of cobalt (27) is and in state
It has 6 electrons which are paired.
Hence, is diamagnetic.
(ii)-
First, we have to calculate the oxidation number of nickel ions.
The oxidation number of is zero because it is a neutral ligand and the oxidation number of is -1. So, the oxidation number of nickel is:
So, the oxidation number of nickel is +2.
The ground state electronic configuration of nickel (28) is and in state
It has 2 unpaired electrons.
Hence, is paramagnetic.
(iii)-
First, we have to calculate the oxidation number of chromium ion.
The oxidation number of is zero because it is a neutral ligand and the oxidation number of is -1. So, the oxidation number of chromium is:
So, the oxidation number of chromium is +3.
The ground state electronic configuration of chromium (24) is and in state
It has 3 unpaired electrons.
Hence, is paramagnetic.
(iv)-
First, we have to calculate the oxidation number of iron ions.
The oxidation number of is zero because it is a neutral ligand and the oxidation number of is -1. So, the oxidation number of iron is:
So, the oxidation number of iron is +2.
The ground state electronic configuration of iron (26) is and in state
It has 4 unpaired electrons.
Hence, is paramagnetic.
So, the correct option is (a)- (i)
Note:
If the complex compound has a strong field ligand like , etc they will pair up the unpaired electrons and if the compound has a weak field ligand , etc, they will not pair up the unpaired electrons.
Complete answer:
Let us study all the complexes one by one:
(i)-
First, we have to calculate the oxidation number of cobalt ions.
The oxidation number of
So, the oxidation number of cobalt is +3.
The ground state electronic configuration of cobalt (27) is
It has 6 electrons which are paired.
Hence,
(ii)-
First, we have to calculate the oxidation number of nickel ions.
The oxidation number of
So, the oxidation number of nickel is +2.
The ground state electronic configuration of nickel (28) is
It has 2 unpaired electrons.
Hence,
(iii)-
First, we have to calculate the oxidation number of chromium ion.
The oxidation number of
So, the oxidation number of chromium is +3.
The ground state electronic configuration of chromium (24) is
It has 3 unpaired electrons.
Hence,
(iv)-
First, we have to calculate the oxidation number of iron ions.
The oxidation number of
So, the oxidation number of iron is +2.
The ground state electronic configuration of iron (26) is
It has 4 unpaired electrons.
Hence,
So, the correct option is (a)- (i)
Note:
If the complex compound has a strong field ligand like
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