The intergalogen which does not exist is:

Options

A. `IF_(5)`
B. `ClF_(3)`
C. `BrCl`
D. `IC l_(4)`

Answer

To determine which interhalogen does not exist, we need to analyze the given options based on the electronic configurations of the halogens involved. The halogens include fluorine (F), chlorine (Cl), bromine (Br), and iodine (I), all of which have seven electrons in their valence shell.

### Step-by-Step Solution:

1. **Understanding Interhalogens**: Interhalogens are compounds formed between two different halogens. The stability of these compounds depends on the electronic configurations and the ability to form stable bonds.

2. **Analyzing the Options**:
- **Option 1: IF5**
- Iodine (I) has 7 valence electrons. In IF5, iodine forms bonds with 5 fluorine atoms.
- This means 5 electrons from iodine will pair with 5 electrons from fluorine, leaving 2 electrons as a lone pair on iodine.
- The structure is stable, so IF5 exists.

- **Option 2: ClF3**
- Chlorine (Cl) also has 7 valence electrons. In ClF3, chlorine bonds with 3 fluorine atoms.
- This results in 3 electrons pairing with 3 fluorine, leaving 4 electrons. These 4 electrons can form 2 lone pairs.
- The structure is stable, so ClF3 exists.

- **Option 3: BrCl**
- Bromine (Br) has 7 valence electrons. In BrCl, bromine bonds with one chlorine atom.
- This means 1 electron pairs with chlorine, leaving 6 electrons. These can form 3 lone pairs.
- The structure is stable, so BrCl exists.

- **Option 4: ICl4**
- Iodine (I) has 7 valence electrons. In ICl4, iodine bonds with 4 chlorine atoms.
- This means 4 electrons pair with 4 chlorine, leaving 3 electrons.
- This results in 1 lone pair and 1 unpaired electron, which makes the structure unstable.
- Therefore, ICl4 does not exist.

3. **Conclusion**: The interhalogen that does not exist is **ICl4**.