Why is Br a weaker field ligand than CO?

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Solution

Ligands
Ligands are electron donors to metal atoms.
Strong field ligands and weak field ligands are the two kinds of ligands.
Strong field ligands cause a large splitting, whereas weak field ligands produce a small splitting.
$Br$ is a weak field ligand than $CO$
Carbonyl ligands $(CO)$ are composed of carbon and oxygen atoms, with the oxygen atom acting as a donor and forming pi-bonds.
These pi-bonds are held loosely and are readily ready for donation.
$CO$ is a stronger field ligand than $Br$ because of pi-bonds.
Bromine $(Br)$ is a negatively charged ligand that is found in the form of ${Br}^{-}$ .
Bromine is a weak field ligand because of its electronegativity, which makes it difficult to donate electrons.

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On the basis of crystal field theory explain why Co(III) forms paramagnetic octahedral complex with weak field ligands whereas it forms diamagnetic octahedral complex with strong field ligands.

H_{2} O

is a weaker field ligand than

N H_{3}

and

Δ_{o c t}

([C r (N H_{3})_{6}]^{3 +}) < Δ_{o c t} ([C r (H_{2} O)_{6}]^{3 +})

H_{2} O

is a weaker field ligand than

N H_{3}

and

Δ_{o c t}

([C r (N H_{3})_{6}]^{3 +}) < Δ_{o c t} ([C r (H_{2} O)_{6}]^{3 +})

If true 1 else 0.

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Q. Why is CO a stronger ligand than Cl-?

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