If an element is in its lowest oxidation state, under proper conditions it can act as :

Options

A. Reducing agent
B. An oxidising agent
C. Oxidising as well as reducing agent
D. Neither oxidising nor reducing agent

Answer

To solve the question, we need to analyze the behavior of elements in their lowest oxidation states. Here’s a step-by-step breakdown:

### Step 1: Understand Oxidation States
- The oxidation state of an element indicates the degree of oxidation (loss of electrons) of that element in a compound. The lowest oxidation state for metals is typically 0, while for non-metals, it can vary.

### Step 2: Identify the Lowest Oxidation State
- For metals, the lowest oxidation state is 0, meaning the metal is in its elemental form and is electron-rich.
- For non-metals, the lowest oxidation state can be negative, indicating that they can gain electrons.

### Step 3: Analyze the Behavior of Metals
- When a metal is in its lowest oxidation state (0), it has a tendency to lose electrons. This characteristic allows it to act as a reducing agent because it can donate electrons to other substances.

### Step 4: Analyze the Behavior of Non-Metals
- Non-metals in their lowest oxidation state (usually negative) can lose extra electrons to become neutral or to form bonds. This also allows them to act as reducing agents under certain conditions.

### Step 5: Conclusion
- Since both metals in their lowest oxidation state and non-metals in their lowest oxidation state can act as reducing agents, we conclude that the correct answer to the question is that an element in its lowest oxidation state can act as a reducing agent.

### Final Answer
- The correct option is: **Reducing Agent**