1. Count the Valence Electrons:
* Chlorine (Cl) has 7 valence electrons.
* Fluorine (F) has 7 valence electrons.
* Total valence electrons: 7 + 7 = 14
2. Determine the Central Atom:
* Chlorine is less electronegative than fluorine, making it the central atom.
3. Connect the Atoms with Single Bonds:
* Place a single bond (two electrons) between the chlorine and fluorine atoms: Cl-F
4. Distribute Remaining Electrons:
* Chlorine now has 6 electrons around it (2 in the bond and 4 non-bonding).
* Fluorine also has 6 electrons around it (2 in the bond and 4 non-bonding).
5. Check Octet Rule:
* Both chlorine and fluorine now have 8 electrons around them, satisfying the octet rule.
The Lewis Structure:
```
..
:Cl:
|
F:
..
```
Key Points:
* The chlorine atom has three lone pairs of electrons.
* The fluorine atom has three lone pairs of electrons.
* The single bond between the chlorine and fluorine atoms is a polar covalent bond, with the fluorine atom being slightly more electronegative.
