Which of the following does not show the amomalous behaviour of lithium?

Options

A. Lithium reacts with nitrogen to form a nitride
B. Lithium carbonate decomposes on heating
C. Lithium nitrate gives `NO_(2)` on heating
D. lithium is the strongest reducing agent.

Explanation

To determine which of the following does not show the anomalous behavior of lithium, we first need to understand what is meant by "anomalous behavior" in the context of lithium compared to other alkali metals.

### Step-by-Step Solution:

1. **Understand Anomalous Behavior**:
- Lithium exhibits certain unique properties that differ from other alkali metals (like sodium, potassium, etc.) due to its small size and high charge density. This leads to a stronger polarizing power, greater covalent character in its compounds, and a tendency to form stable complexes.

2. **Identify Key Characteristics of Lithium**:
- Small atomic and ionic size.
- High ionization energy compared to other alkali metals.
- Strong reducing agent due to its ability to easily lose its outermost electron.

3. **Compare with Other Alkali Metals**:
- Other alkali metals do not exhibit the same degree of polarizing power or covalent character in their compounds as lithium does. For instance, sodium and potassium do not show these anomalous behaviors to the same extent.

4. **Identify the Options**:
- Without the specific options provided, we can infer that any property or behavior that aligns with the general characteristics of alkali metals (like being a strong reducing agent) would not be considered anomalous.

5. **Conclusion**:
- Since lithium is indeed a strong reducing agent, just like other alkali metals, this behavior does not qualify as anomalous. Therefore, if one of the options states that lithium is a strong reducing agent, that would be the correct answer.

### Final Answer:
- The option that states lithium is a strong reducing agent does not show the anomalous behavior of lithium.