The sum of oxidation states of all atoms in `ClO_(4)^(-)` ion is

Options

A. zero
B. `-4`
C. `-1`
D. `+2`

Answer

To find the sum of oxidation states of all atoms in the \( \text{ClO}_4^{-} \) ion, we can follow these steps:

### Step 1: Identify the oxidation states of the known elements.
- In the \( \text{ClO}_4^{-} \) ion, we have chlorine (Cl) and oxygen (O).
- The oxidation state of oxygen is typically \(-2\).

### Step 2: Set up the equation for the oxidation states.
- Let the oxidation state of chlorine be \( x \).
- Since there are four oxygen atoms, their total contribution to the oxidation state will be \( 4 \times (-2) = -8 \).

### Step 3: Write the equation based on the charge of the ion.
- The overall charge of the \( \text{ClO}_4^{-} \) ion is \(-1\).
- Therefore, we can set up the equation:
\[ x + (-8) = -1 \]

### Step 4: Solve for \( x \).
- Rearranging the equation gives:
\[ x - 8 = -1 \]
\[ x = -1 + 8 \]
\[ x = +7 \]

### Step 5: Calculate the sum of oxidation states.
- Now we know the oxidation state of chlorine is \( +7 \) and that of each oxygen is \( -2 \).
- The total sum of oxidation states in \( \text{ClO}_4^{-} \) is:
\[ +7 + 4 \times (-2) = +7 - 8 = -1 \]

### Conclusion:
- The sum of oxidation states of all atoms in the \( \text{ClO}_4^{-} \) ion is \(-1\).