In the following complex ions order of paramagnetism is :

P: [FeF₆]^3-

Q: [CoF₆]^3-

R: [V(H₂O)₆]³⁺

S: [Ti(H₂O)₆]³⁺

P > Q > R > S

The answer is (1) P > Q > R > S.

Here is the explanation for the order of Paramagnetism:

\([FeF_6]^{3-}\): The oxidation state of iron is +3, so it has 5 electrons in the 3d orbital. The fluoride ligand is a weak field ligand, so it does not cause the electrons to pair up. Therefore, \([FeF_6]^{3-}\) has 5 unpaired electrons and is the most paramagnetic complex ion.

\([CoF_6]^{3-}\): The oxidation state of cobalt is +3, so it has 6 electrons in the 3d orbital. The fluoride ligand is a weak field ligand, so it does not cause the electrons to pair up. Therefore, \([CoF_6]^{3-}\) has 3 unpaired electrons.

\([V(H_2O)_6]^{3+}\): The oxidation state of vanadium is +3, so it has 2 electrons in the 3d orbital. The water ligand is a weak field ligand, so it does not cause the electrons to pair up. Therefore, \([V(H_2O)_6]^{3+}\) has 2 unpaired electrons.

\([Ti(H_2O)_6]^{3+}\): The oxidation state of titanium is +3, so it has 1 electron in the 3d orbital. The water ligand is a weak field ligand, so it does not cause the electrons to pair up. Therefore, \([Ti(H_2O)_6]^{3+}\) has 1 unpaired electron.