lewis structure of CIF3
The Correct Answer and Explanation is:
Correct Lewis Structure of ClF₃ (Chlorine Trifluoride):
The Lewis structure of ClF₃ consists of:
- Chlorine (Cl) as the central atom
- Three fluorine (F) atoms bonded to chlorine with single bonds
- Two lone pairs on chlorine
- Each fluorine atom has three lone pairs
Step-by-step Construction and Explanation
To draw the Lewis structure for ClF₃, start by counting the total number of valence electrons available. Chlorine has 7 valence electrons, and each fluorine atom also has 7. Since there are three fluorine atoms, the total number of valence electrons is:
7 (from Cl) + 3 × 7 (from F) = 28 valence electrons.
Step 1: Central Atom Selection
Chlorine is less electronegative than fluorine, so it goes at the center.
Step 2: Draw Single Bonds
Connect each fluorine to the chlorine atom with a single bond. This uses up 6 electrons (3 bonds × 2 electrons = 6 electrons).
Step 3: Distribute Remaining Electrons
After using 6 electrons for bonding, 22 electrons remain. Assign 6 electrons (3 lone pairs) to each fluorine atom, which uses 18 electrons. Now 4 electrons are left.
Step 4: Place Remaining Electrons on Central Atom
Place the remaining 4 electrons as 2 lone pairs on the chlorine atom.
At this point, chlorine is surrounded by 10 electrons (3 bonding pairs + 2 lone pairs). This is more than the octet rule but acceptable because chlorine is in Period 3 and can expand its octet.
Final Structure Summary:
- Chlorine at the center
- Three single bonds connecting to three fluorine atoms
- Each fluorine has 3 lone pairs
- Chlorine has 2 lone pairs
The molecular geometry of ClF₃ is T-shaped, as predicted by the VSEPR theory, because there are five regions of electron density around chlorine (three bonding pairs and two lone pairs).
ClF₃ is a reactive, interhalogen compound with polar characteristics due to the asymmetrical arrangement of bonds and lone pairs.
