Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R). Assertion (A) : The total number of geometrical isomers shown by $$[Co(en)_2Cl_2]^+$$ complex ion is three. Reason (R) : $$[Co(en)_2Cl_2]^+$$ complex ion has an octahedral geometry. In the light of the above statements, choose the most appropriate answer from the options given below :

We need to evaluate the Assertion (A) and Reason (R) about the complex $$[Co(en)_2Cl_2]^+$$.

Analysis of Assertion (A):

"The total number of geometrical isomers shown by $$[Co(en)_2Cl_2]^+$$ is three."

To determine geometrical isomers, we need to understand the structure:

- Co$$^{3+}$$ is the central metal ion (cobalt in +3 oxidation state: $$d^6$$ configuration)

- $$en$$ (ethylenediamine) is a bidentate ligand that occupies 2 coordination positions

- Two en ligands occupy $$2 \times 2 = 4$$ positions, and two Cl$$^-$$ ligands occupy 2 positions, totaling 6 positions (octahedral)

For an octahedral complex of the type $$[M(AA)_2X_2]$$ (where AA is a bidentate ligand and X is a monodentate ligand), the possible geometrical isomers are:

1. cis isomer: The two Cl ligands are adjacent to each other (at 90 degrees)

2. trans isomer: The two Cl ligands are opposite to each other (at 180 degrees)

There are only 2 geometrical isomers (cis and trans), NOT 3. The assertion that there are three geometrical isomers is incorrect.

Analysis of Reason (R):

"$$[Co(en)_2Cl_2]^+$$ has an octahedral geometry."

Co$$^{3+}$$ has a coordination number of 6 in this complex (2 bidentate en ligands providing 4 donor atoms + 2 Cl atoms = 6 donor atoms). With 6 donor atoms, the geometry is indeed octahedral. This is consistent with the $$d^2sp^3$$ hybridization of Co$$^{3+}$$ (or inner orbital complex with strong field en ligands).

The reason is correct.

Conclusion: Assertion (A) is incorrect (there are only 2 geometrical isomers, not 3), but Reason (R) is correct (the complex does have octahedral geometry).

The correct answer is Option (2): (A) is not correct but (R) is correct.