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Match List - I with List - II.
| Column I | Column II |
|---|
(a)[Fe(CN)6]3− | (i) 5.92 BM |
(b)[Fe(H2O)6]3+ | (ii) 0 BM |
(c)[Fe(CN)6]4− | (iii) 4.90 BM |
(d)[Fe(H2O)6]2+ | (iv) 1.73 BM |
hard
Coordination Compounds
2021
chemistry
Explanation
To solve this problem, we need to determine the magnetic moments of the given complexes.The magnetic moment is given by the formula:μ=n(n+2)
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Sign up / Login BM, where
is the number of unpaired electrons.
Let's analyze each complex:
(a)
[Fe(CN)6]3−: • Iron is in the +3 oxidation state, so
has 5 d-electrons.
• CN
is a strong field ligand, causing pairing of electrons.
• All 5 electrons are paired, so
n=0. • Magnetic moment
μ=0(0+2)=0 BM.
(b)
[Fe(H2O)6]3+: • Iron is in the +3 oxidation state, so
has 5 d-electrons.
• H
is a weak field ligand, so electrons remain unpaired.
• There are 5 unpaired electrons, so
n=5. • Magnetic moment
μ=5(5+2)=35≈5.92 BM.
(c)
[Fe(CN)6]4−: • Iron is in the +2 oxidation state, so
has 6 d-electrons.
• CN
is a strong field ligand, causing pairing of electrons.
• There are no unpaired electrons, so
n=0. • Magnetic moment
μ=0(0+2)=0 BM.
(d)
[Fe(H2O)6]2+: • Iron is in the +2 oxidation state, so
has 6 d-electrons.
• H
is a weak field ligand, so electrons remain unpaired.
• There are 4 unpaired electrons, so
n=4. • Magnetic moment
μ=4(4+2)=24≈4.90 BM.
Matching the calculated magnetic moments with the given options:
• (a)
[Fe(CN)6]3−→ (ii) 0 BM
• (b)
[Fe(H2O)6]3+→ (i) 5.92 BM
• (c)
[Fe(CN)6]4−→ (ii) 0 BM
• (d)
[Fe(H2O)6]2+→ (iii) 4.90 BM
Therefore, the correct option is Option 4:
(a) -> (ii), (b) -> (i), (c) -> (ii), (d) -> (iii).