In the reaction `2H_(2)O_(2)rarr2H_(2)O+O_(2)` oxidation state of oxygen change as :

Options

A. Only - 1 to -2
B. Only - 1 to zero
C. Both of the above
D. `-1`to` -3`

Explanation

To determine the change in oxidation states of oxygen in the reaction \(2H_2O_2 \rightarrow 2H_2O + O_2\), we will follow these steps:

### Step 1: Identify the oxidation states of oxygen in hydrogen peroxide (\(H_2O_2\)).
- In \(H_2O_2\), let the oxidation state of oxygen be \(x\).
- The formula for hydrogen peroxide is \(H_2O_2\), which contains 2 hydrogen atoms and 2 oxygen atoms.
- The total charge of the molecule is neutral (0), so we can set up the equation:
\[ 2(+1) + 2x = 0 \]
\[ 2 + 2x = 0 \]
\[ 2x = -2 \implies x = -1 \]
- Therefore, the oxidation state of oxygen in \(H_2O_2\) is \(-1\).

### Step 2: Identify the oxidation states of oxygen in water (\(H_2O\)).
- In \(H_2O\), let the oxidation state of oxygen be \(y\).
- The formula for water is \(H_2O\), which contains 2 hydrogen atoms and 1 oxygen atom.
- Again, the total charge of the molecule is neutral (0), so we can set up the equation:
\[ 2(+1) + y = 0 \]
\[ 2 + y = 0 \]
\[ y = -2 \]
- Therefore, the oxidation state of oxygen in \(H_2O\) is \(-2\).

### Step 3: Identify the oxidation state of oxygen in molecular oxygen (\(O_2\)).
- In \(O_2\), the oxidation state of oxygen is \(0\) because it is in its elemental form.

### Step 4: Summarize the changes in oxidation states.
- In \(H_2O_2\), the oxidation state of oxygen changes from \(-1\) to \(-2\) when it is converted to \(H_2O\).
- In \(H_2O\), the oxidation state of oxygen changes from \(-1\) to \(0\) when it is converted to \(O_2\).

### Conclusion
- The oxidation state of oxygen in the reaction changes as follows:
- From \(-1\) in \(H_2O_2\) to \(-2\) in \(H_2O\) (reduction).
- From \(-1\) in \(H_2O\) to \(0\) in \(O_2\) (oxidation).

Thus, the correct answer is that the oxidation state of oxygen changes as described above.