The oxidation states exhibited by hydrogen in its compounds are:

Options

A. `-1` only
B. Zero only
C. `+1,-1` and zero
D. `+1` only

Explanation

To determine the oxidation states exhibited by hydrogen in its compounds, we can analyze the different scenarios in which hydrogen can bond with other elements. Here’s a step-by-step breakdown of the oxidation states of hydrogen:

### Step 1: Identify the Oxidation State in Diatomic Hydrogen (H₂)
- When hydrogen is in its diatomic form (H₂), it is not combined with any other element. In this case, the oxidation state of hydrogen is **0**.

### Step 2: Analyze Hydrogen in Compounds with Non-metals
- When hydrogen forms a bond with a non-metal (e.g., HCl with chlorine), it typically has an oxidation state of **+1**. This is because hydrogen is less electronegative than non-metals, leading to a positive charge on hydrogen.

### Step 3: Analyze Hydrogen in Compounds with Metals
- When hydrogen forms a bond with a metal (e.g., LiH with lithium), the oxidation state of hydrogen can be **-1**. In this case, the metal (lithium) is more electropositive than hydrogen, resulting in hydrogen carrying a negative charge.

### Conclusion
From the analysis above, we can conclude that hydrogen can exhibit the following oxidation states in its compounds:
- **0** (in H₂)
- **+1** (in compounds with non-metals, e.g., HCl)
- **-1** (in compounds with metals, e.g., LiH)

Thus, the oxidation states exhibited by hydrogen in its compounds are **0, +1, and -1**.

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