The oxidation number of `Cl` in `CaOCl_(2)` is

Options

A. `-1 and +1`
B. `+2`
C. `-2`
D. None

Explanation

To determine the oxidation number of chlorine (Cl) in calcium oxychloride (CaOCl₂), we can follow these steps:

### Step 1: Identify the components of the compound
The compound CaOCl₂ consists of calcium (Ca), oxygen (O), and chlorine (Cl). We need to find the oxidation states of each element.

### Step 2: Assign oxidation states based on known values
- Calcium (Ca) is an alkaline earth metal and typically has an oxidation state of +2.
- Oxygen (O) usually has an oxidation state of -2.

### Step 3: Set up the equation for the overall charge
The overall charge of the compound CaOCl₂ is neutral (0). We can express this as:
\[ \text{Oxidation state of Ca} + \text{Oxidation state of O} + \text{Oxidation state of Cl (1)} + \text{Oxidation state of Cl (2)} = 0 \]

### Step 4: Substitute known oxidation states into the equation
Substituting the known oxidation states into the equation gives us:
\[ +2 + (-2) + x + y = 0 \]
Where x is the oxidation state of one Cl and y is the oxidation state of the other Cl.

### Step 5: Identify the oxidation states of Cl
In CaOCl₂, there are two different oxidation states for chlorine:
1. In the OCl⁻ ion, the oxidation state of Cl is +1.
2. In the Cl⁻ ion, the oxidation state of Cl is -1.

### Step 6: Summarize the oxidation states
Thus, in CaOCl₂:
- One chlorine atom has an oxidation state of +1 (from OCl⁻).
- The other chlorine atom has an oxidation state of -1 (from Cl⁻).

### Conclusion
The oxidation numbers of chlorine in CaOCl₂ are +1 and -1.

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