Ionisation of energy `F^(ɵ)` is `320 kJ mol^(-1)`. The electronic gain enthalpy of fluorine would be

Options

A. `-320 kJ mol^(-1)`
B. `-160 kJ mol^(-1)`
C. `+320 kJ mol^(-1)`
D. `+160 kJ mol^(-1)`

Explanation

To find the electronic gain enthalpy of fluorine given its ionization energy, we can follow these steps:

### Step-by-Step Solution:

1. **Understand Ionization Energy and Electron Gain Enthalpy**:
- Ionization energy (IE) is the energy required to remove an electron from a neutral gaseous atom.
- Electron gain enthalpy (EGE) is the energy change when an electron is added to a neutral gaseous atom.

2. **Relationship Between Ionization Energy and Electron Gain Enthalpy**:
- Ionization energy and electron gain enthalpy have the same magnitude but opposite signs. This means:
\[ \text{Ionization Energy} = -\text{Electron Gain Enthalpy} \]

3. **Given Data**:
- The ionization energy of fluorine is given as \( F^{\circ} = 320 \, \text{kJ mol}^{-1} \).

4. **Calculate Electron Gain Enthalpy**:
- Using the relationship from step 2, we can express the electron gain enthalpy as follows:
\[ \text{Electron Gain Enthalpy} = -\text{Ionization Energy} \]
- Substituting the given value:
\[ \text{Electron Gain Enthalpy} = -320 \, \text{kJ mol}^{-1} \]

5. **Final Answer**:
- Therefore, the electronic gain enthalpy of fluorine is:
\[ \text{Electron Gain Enthalpy} = -320 \, \text{kJ mol}^{-1} \]