In the transformation of `Na(s) rarr Na^(o+) (g)`, the energies involved
are

Options

A. Ionisation energy
B. Sublimation energy
C. Ionisation energy and sublimation energy
D. Bond dissociation energy

Explanation

To solve the question regarding the transformation of sodium from solid to gaseous sodium ion, we need to analyze the energies involved in this process step by step.

### Step-by-Step Solution:

1. **Identify the Initial State**:
We start with sodium in its solid state, represented as Na(s).

2. **Sublimation Process**:
The first step in the transformation is the conversion of solid sodium (Na(s)) to gaseous sodium (Na(g)). This process requires energy to overcome the intermolecular forces holding the solid together. This energy is known as **sublimation energy**.

\[ \text{Na(s)} \rightarrow \text{Na(g)} \]
**Energy involved**: Sublimation energy (ΔH_sub)

3. **Ionization Process**:
Once we have sodium in the gaseous state, the next step is to convert gaseous sodium into a sodium ion (Na⁺). This involves removing one electron from the gaseous sodium atom, which requires energy. This energy is referred to as **ionization energy**.

\[ \text{Na(g)} \rightarrow \text{Na}^+(g) + e^- \]
**Energy involved**: Ionization energy (ΔH_ion)

4. **Total Energy Involved**:
The total energy required for the transformation from solid sodium to sodium ion in the gaseous state is the sum of the sublimation energy and the ionization energy.

\[ \text{Total Energy} = \Delta H_{sub} + \Delta H_{ion} \]

### Final Answer:
The energies involved in the transformation of `Na(s)` to `Na^(o+) (g)` are **sublimation energy** and **ionization energy**.

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