In the following balanced reaction,
`4O_(2)^(x)+2H_(2)O rarr 4OH^(-)+3O_(2)`

Options

A. `x=-4` and species is oxide
B. `x=-2` and species is superoxide
C. `x=0` and species is oxygen
D. `x=-1` and species is superoxide

Explanation

To solve the problem, we need to determine the value of \( x \) in the balanced reaction:

\[ 4O_{2}^{(x)} + 2H_{2}O \rightarrow 4OH^{-} + 3O_{2} \]

### Step 1: Analyze the Charges on Both Sides

1. **Left Side Charges**:
- The charge of \( O_{2}^{(x)} \) is \( 4x \) (since there are 4 \( O_{2} \) molecules).
- The charge of \( H_{2}O \) is 0 (neutral molecule).
- Therefore, the total charge on the left side is:
\[ \text{Total charge (left)} = 4x + 0 = 4x \]

2. **Right Side Charges**:
- The charge of \( OH^{-} \) is -1, and there are 4 \( OH^{-} \) ions, so the total charge from \( OH^{-} \) is:
\[ \text{Charge from } OH^{-} = 4 \times (-1) = -4 \]
- The charge from \( O_{2} \) is 0 (neutral molecule).
- Therefore, the total charge on the right side is:
\[ \text{Total charge (right)} = -4 + 0 = -4 \]

### Step 2: Set Up the Equation

Now, we can set the total charge from the left side equal to the total charge from the right side:

\[ 4x = -4 \]

### Step 3: Solve for \( x \)

To find \( x \), we divide both sides of the equation by 4:

\[ x = \frac{-4}{4} = -1 \]

### Conclusion

The value of \( x \) is \( -1 \). This indicates that the species \( O_{2}^{(x)} \) is a superoxide ion.

### Final Answer
\[ x = -1 \]

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