Weakest reducing agent:

Options

A. Atomic hydrogen
B. Nascent hydrogen
C. Molecular hydrogen
D. Occluded hydrogen

Explanation

To determine the weakest reducing agent among the given options, we can follow these steps:

### Step 1: Understand the concept of reducing agents
A reducing agent is a substance that donates electrons to another substance, thereby reducing it. The strength of a reducing agent depends on its ability to lose electrons.

**Hint:** Remember that the more stable a substance is, the less likely it is to donate electrons.

### Step 2: Analyze the given options
The options provided are likely different forms of hydrogen:
- Molecular hydrogen (H₂)
- Atomic hydrogen (H)
- Nascent hydrogen (H)
- Ocular hydrogen (H)

**Hint:** Identify the stability of each form of hydrogen.

### Step 3: Compare the stability of the hydrogen forms
- **Molecular hydrogen (H₂)** is a stable diatomic molecule with a full electron shell.
- **Atomic hydrogen (H)** is less stable because it has a single electron, making it more reactive.
- **Nascent hydrogen** refers to hydrogen in its atomic form that is generated during chemical reactions, which is also unstable and reactive.
- **Ocular hydrogen** (if referring to a specific form) is generally considered to be a reactive form of hydrogen.

**Hint:** The more unstable forms of hydrogen will be better reducing agents.

### Step 4: Determine the weakest reducing agent
Since molecular hydrogen (H₂) is the most stable form and does not readily donate electrons, it is the weakest reducing agent among the options provided.

**Hint:** Recall that stability correlates with reducing ability; the more stable the substance, the weaker it is as a reducing agent.

### Conclusion
Based on the analysis, the weakest reducing agent among the options is **molecular hydrogen (H₂)**.

**Final Answer:** Option C (Molecular Hydrogen) is the correct answer.