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$\text{Hint: Maximum oxidation state of Cr is } +6\text{.}$ $\text{Explanation:}$ $\text{Step 1: Initial calculation of oxidation state}$ $\text{Assume the typical oxidation state of oxygen is } -2\text{.}$ $\text{Let the oxidation state of Cr be } x\text{.}$ $x + 6 \times (-2) = 0$ $x - 12 = 0$ $x = +12$ $\text{Step 2: Check for abnormality and presence of peroxide linkage.}$ $\text{The maximum oxidation number shown by Chromium (Cr) is } +6\text{. Since the calculated oxidation number of Cr in } \text{CrO}_6 \text{ is } +12\text{, which is greater than its maximum possible oxidation state, this indicates that } \text{CrO}_6 \text{ contains peroxide linkages.}$ $\text{Step 3: Calculate the number of peroxide bonds.}$ $\text{Number of peroxide bonds} = \frac{\text{Calculated oxidation number} - \text{Maximum oxidation number}}{2}$ $\text{Number of peroxide bonds} = \frac{+12 - +6}{2} = \frac{6}{2} = 3$ $\text{This means there are three peroxide linkages in } \text{CrO}_6\text{.}$ $\text{The structure of } \text{CrO}_6 \text{ is as follows:}$ $\text{It has a structure where the central Cr atom is bonded to three } \text{O}_2 \text{ units (peroxide groups) and two single oxygen atoms forming a ring, or more commonly described as having three peroxide bridges.}$ $\text{In this structure, there are three peroxide linkages (-O-O-) and no oxygen atoms with an oxidation state of } -2\text{. Each oxygen atom in a peroxide linkage has an oxidation state of } -1\text{.}$ $\text{Recalculate the oxidation state of Cr based on the peroxide structure:}$ $\text{Let the oxidation state of Cr be } X\text{.}$ $\text{There are } 6 \text{ oxygen atoms in } \text{CrO}_6\text{. If there are three peroxide linkages, all } 6 \text{ oxygen atoms are involved in these linkages, meaning their oxidation state is } -1\text{.}$ $X + 6 \times (-1) = 0$ $X - 6 = 0$ $X = +6$ $\text{Hence, the oxidation number of Cr in } \text{CrO}_6 \text{ is } +6\text{.}$