For compound having the formula GaAlCl$$_4$$, the correct option from the following is

We need to identify the correct statement about the compound GaAlCl$$_4$$.

The compound GaAlCl$$_4$$ is an ionic salt with the formula Ga$$^+$$[AlCl$$_4$$]$$^-$$. Aluminum readily forms the stable tetrachloroaluminate anion [AlCl$$_4$$]$$^-$$, in which Al is tetrahedrally coordinated with four Cl atoms using $$sp^3$$ hybridization. Gallium exists as the monovalent cation Ga$$^+$$ due to the inert pair effect, where the 4s$$^2$$ electrons resist participation in bonding.

Now, the oxidation states are: Ga has +1 (not +3), and Al has +3 (since $$x + 4(-1) = -1$$, so $$x = +3$$). On the Pauling electronegativity scale, Ga (1.81) is more electronegative than Al (1.61). Despite being more electronegative, Ga forms the cation because Al has a very strong tendency to form the [AlCl$$_4$$]$$^-$$ complex anion.

Evaluating each option: Option 1 says Ga is coordinated with Cl, which is incorrect since Ga exists as a free cation. Option 2 says Ga is more electronegative than Al and forms the cationic part, which is correct. Option 3 says Cl bonds with both Al and Ga, which is incorrect. Option 4 says Ga has oxidation state +3, which is also incorrect.

Hence, the correct answer is Option 2.