When one mole of F atoms are ionised to `F^(-)` , the energy released is X Joules. Then :-

Options

A. X Joules is sufficient to ionise 1 mole of gaseous Cl into `Cl^(+)`
B. X Joules is sufficient to ionise 1 mole of gaseous F into `F^(+)`
C. X Joules is sufficient to ionise 1 mole of gaseous F into `F^(+)` as well as 1 mole of gaseous Cl into `Cl^(+)`
D. Less than 1 mole of gaseous F or Cl atom will be ionised to `F^(+) or Cl^(+)`

Answer

To solve the question, we need to analyze the energy changes involved in the ionization of fluorine and chlorine atoms. Here’s a step-by-step breakdown:

### Step 1: Understand the Ionization Process
When one mole of fluorine (F) atoms is ionized to form fluorine anions (F⁻), energy is released. This process can be represented as:
\[ \text{F} \rightarrow \text{F}^- + \text{Energy} \]

### Step 2: Energy Released
The amount of energy released during the ionization of one mole of fluorine atoms is given as \( X \) Joules. This means that when one mole of F atoms is converted to F⁻, \( X \) Joules of energy is released.

### Step 3: Compare with Chlorine
The question asks whether this energy \( X \) Joules is sufficient to ionize one mole of gaseous chlorine (Cl) into Cl⁺. The ionization of chlorine can be represented as:
\[ \text{Cl} \rightarrow \text{Cl}^+ + \text{Energy} \]

### Step 4: Analyze the Energy Requirements
Since both fluorine and chlorine belong to the same group in the periodic table (Group 17 - Halogens), they exhibit similar chemical properties, including ionization energies. However, the ionization energy of chlorine is generally lower than that of fluorine because chlorine is larger and has a lower effective nuclear charge compared to fluorine.

### Step 5: Conclusion
Given that \( X \) Joules is the energy released when one mole of fluorine is ionized, this amount of energy is sufficient to ionize one mole of gaseous chlorine into Cl⁺. Thus, we can conclude that:

**The correct option is that \( X \) Joules is sufficient to ionize 1 mole of gaseous chlorine into Cl⁺.**

### Final Answer
The answer to the question is:
**X Joules is sufficient to ionize 1 mole of gaseous chlorine into Cl⁺.**

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