Determine the hybridization of the central atom in BF3.

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Question: Determine the hybridization of the central atom in BF3.

Options:

Correct Answer: sp2

Solution:

Boron in BF3 is sp2 hybridized, forming three equivalent sp2 hybrid orbitals.

Determine the hybridization of the central atom in BF3.

Determine the hybridization of the central atom in BF3.

Step 1: Identify the central atom in BF3, which is boron (B).
Step 2: Count the number of bonds boron forms with surrounding atoms. In BF3, boron forms three bonds with three fluorine (F) atoms.
Step 3: Determine the number of electron groups around the central atom. Boron has three bonding pairs and no lone pairs.
Step 4: Use the VSEPR theory to determine the geometry. Three bonding pairs result in a trigonal planar shape.
Step 5: Identify the hybridization that corresponds to a trigonal planar shape. This is sp2 hybridization.
Step 6: Conclude that boron in BF3 is sp2 hybridized, forming three equivalent sp2 hybrid orbitals.

Hybridization – The concept of hybridization involves the mixing of atomic orbitals to form new hybrid orbitals that can accommodate bonding.
Molecular Geometry – Understanding the molecular geometry of BF3 helps in determining the hybridization of the central atom.
Valence Bond Theory – This theory explains how atomic orbitals combine to form bonds in molecules, which is essential for determining hybridization.