To solve this problem, we need to determine the oxidation state of Cr in $$CrO$_5. \\$Let's analyze the structure of $$CrO$_5: \\$• CrO$_5$ is known to have two $(-O-O-)$ bonds, which are peroxo bonds.$\\$• The structure can be visualized as $$O$_2$Cr(O-O)_2$. \\$In this structure:$\\$• Each peroxo group $(-O-O-)$ contributes a total charge of $-2. \\$• There are two peroxo groups, contributing a total charge of $-4. \\$• The remaining oxygen (not part of the peroxo groups) is a typical oxide, contributing $-2. \\$Let's calculate the oxidation state of Cr:$\\$• Let the oxidation state of Cr be $x. \\$• The total charge of the compound is neutral (0).$\\$Setting up the equation:$\\ x + (-2) + 2(-2) = 0 \\$Simplify the equation:$\\ x - 2 - 4 = 0 \\ x - 6 = 0 \\ x = +6 \\$Therefore, the oxidation state of Cr in $$CrO$_5$ is $+6. \\$This corresponds to Option 3.