Which of the following readily forms nitride ?

Options

A. K
B. Mg
C. Ba
D. Ca

Answer

To determine which of the given options readily forms nitride, we need to analyze the properties of the elements in question, particularly focusing on their ability to form nitrides based on their group in the periodic table and the associated lattice energies.

### Step-by-Step Solution:

1. **Identify the Elements**:
- Let's assume the options provided are: Lithium (Li), Sodium (Na), Magnesium (Mg), and Barium (Ba).

2. **Understand the Group Characteristics**:
- Lithium is in Group 1 (Alkali metals), Sodium is also in Group 1, while Magnesium and Barium are in Group 2 (Alkaline earth metals).
- Group 1 elements typically do not form nitrides readily due to their tendency to form oxides and hydroxides instead.

3. **Examine the Formation of Nitrides**:
- Nitrides are formed when an element reacts with nitrogen. The ability to form nitrides generally increases as we move from Group 1 to Group 2.
- Among the alkaline earth metals, the ability to form nitrides decreases down the group (from Be to Ba).

4. **Lattice Energy Consideration**:
- The formation of nitrides is influenced by the lattice energy of the resulting nitride compound.
- Smaller cations (like Mg²⁺) can stabilize the nitride ion (N³⁻) better due to higher lattice energy compared to larger cations (like Ba²⁺).

5. **Conclusion**:
- Magnesium (Mg) is the smallest cation among the options and can effectively stabilize the nitride ion due to its higher lattice energy.
- Therefore, Magnesium readily forms nitride compared to the other elements listed.

### Final Answer:
**Magnesium (Mg) readily forms nitride.**

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