Oxidation state of oxygen in `CrO_(5)` is

Options

A. -1
B. -2
C. Both (1) & (2)
D. `-1/2`

Answer

To determine the oxidation state of oxygen in CrO₅, we will follow these steps:

### Step 1: Understand the Compound
CrO₅ consists of chromium (Cr) and oxygen (O). We need to find the oxidation state of oxygen in this compound.

### Step 2: Assign Oxidation States
Typically, the oxidation state of oxygen is -2. However, in some compounds, particularly peroxides and superoxides, it can be different. In CrO₅, we need to consider the structure of the compound.

### Step 3: Analyze the Structure
CrO₅ contains a peroxy linkage. In this case, we have two types of oxygen:
1. Oxygen that is part of a peroxide bond (O-O) which has an oxidation state of -1.
2. Oxygen that is double-bonded to chromium, which has an oxidation state of -2.

### Step 4: Set Up the Equation
Let the oxidation state of chromium be \( x \). In CrO₅, there are 5 oxygen atoms:
- 4 of these oxygen atoms are in the form of two peroxy linkages (2 O-O bonds), contributing a total of -2 (since each O in the O-O bond has -1).
- 1 oxygen atom is double-bonded to chromium, contributing -2.

The equation can be set up as follows:
\[ x + 4(-1) + (-2) = 0 \]

### Step 5: Solve for x
Now, substituting the values:
\[ x - 4 - 2 = 0 \]
\[ x - 6 = 0 \]
\[ x = +6 \]

### Step 6: Conclusion
The oxidation state of chromium in CrO₅ is +6. Since we have determined that there are two types of oxygen, we conclude that:
- The oxidation state of the four oxygen atoms in the peroxy linkages is -1 each.
- The oxidation state of the one oxygen atom that is double-bonded to chromium is -2.

### Final Answer
Thus, in CrO₅, the oxidation state of oxygen can be -1 for the peroxy oxygen and -2 for the double-bonded oxygen.

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