When `H_(2)O_(2)` is oxidesed, the product is

Options

A. `OH^(-)`
B. `O_(2)`
C. `O^(2-)`
D. `HO_(2)^(-)`

Answer

To determine the product when hydrogen peroxide (H₂O₂) is oxidized, we can follow these steps:

### Step 1: Identify the oxidation state of oxygen in H₂O₂
In hydrogen peroxide (H₂O₂), the oxidation state of oxygen is -1. This is important because it tells us how the oxygen atoms are behaving in this compound.

**Hint:** Remember that in peroxides, oxygen has an oxidation state of -1.

### Step 2: Understand the oxidation process
When H₂O₂ is oxidized, it can lose electrons and increase the oxidation state of its oxygen atoms. The oxidation reaction involves the conversion of H₂O₂ to molecular oxygen (O₂).

**Hint:** Oxidation involves an increase in oxidation state.

### Step 3: Write the balanced oxidation reaction
The oxidation of H₂O₂ can be represented by the following reaction:
\[ 2 H_2O_2 + 2 OH^- \rightarrow O_2 + 2 H_2O \]
In this reaction, H₂O₂ reacts with hydroxide ions (OH⁻) to produce molecular oxygen (O₂) and water (H₂O).

**Hint:** Look for the reactants and products that involve the transfer of electrons and changes in oxidation states.

### Step 4: Analyze the change in oxidation states
In the reaction, the oxidation state of oxygen changes from -1 in H₂O₂ to 0 in O₂. This increase in oxidation state indicates that oxidation has occurred.

**Hint:** Check the oxidation states before and after the reaction to confirm oxidation.

### Conclusion
The product of the oxidation of hydrogen peroxide (H₂O₂) is molecular oxygen (O₂) and water (H₂O).

**Final Answer:** The product when H₂O₂ is oxidized is O₂ (molecular oxygen) and H₂O (water).