In its compounds, oxygen can show oxidation state `(s)` of

Options

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

Answer

To determine the oxidation states that oxygen can exhibit in its compounds, we will analyze the oxidation states based on different examples.

### Step 1: Understanding Oxidation States
Oxygen typically has an oxidation state of -2 in most of its compounds. However, it can exhibit other oxidation states under certain conditions.

### Step 2: Example of Hydrogen Peroxide (H₂O₂)
In hydrogen peroxide (H₂O₂):
- Let the oxidation state of oxygen be \( X \).
- The oxidation state of hydrogen is +1.
- The equation for the overall charge is:
\[ 2(+1) + 2X = 0 \]
Simplifying this:
\[ 2 + 2X = 0 \implies 2X = -2 \implies X = -1 \]
Thus, in H₂O₂, oxygen has an oxidation state of -1.

### Step 3: Example of Water (H₂O)
In water (H₂O):
- Let the oxidation state of oxygen be \( X \).
- The equation for the overall charge is:
\[ 2(+1) + X = 0 \]
Simplifying this:
\[ 2 + X = 0 \implies X = -2 \]
Thus, in H₂O, oxygen has an oxidation state of -2.

### Step 4: Example of Oxygen Difluoride (OF₂)
In oxygen difluoride (OF₂):
- Let the oxidation state of oxygen be \( X \).
- The oxidation state of fluorine is -1.
- The equation for the overall charge is:
\[ X + 2(-1) = 0 \]
Simplifying this:
\[ X - 2 = 0 \implies X = +2 \]
Thus, in OF₂, oxygen has an oxidation state of +2.

### Step 5: Summary of Oxidation States
From the examples analyzed:
- Oxygen can exhibit an oxidation state of -1 (in H₂O₂).
- Oxygen can exhibit an oxidation state of -2 (in H₂O).
- Oxygen can exhibit an oxidation state of +2 (in OF₂).

### Conclusion
The oxidation states that oxygen can show in its compounds are -1, -2, and +2. Therefore, the correct options are -1 and -2, and +2.