What type of hybridization does a BCl3 molecule undergo?a)spb)sp2c)sp3d)sp3dCorrect answer is option 'B'. Can you explain this answer?

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Answer

Answer

In the BCl³ molecule, one s-orbital and two p-orbitals intermix and form three equivalent hybrid orbits. Therefore it undergoes sp² hybridization and forms trigonal planar shape, like B in the center and Cl in the 3 corners.

Answer

Answer:

To determine the hybridization of a molecule, we need to look at the central atom and the number of regions of electron density around it. In the case of BCl3, boron (B) is the central atom.

Regions of Electron Density:
1. The boron atom is bonded to three chlorine (Cl) atoms, resulting in three sigma bonds.
2. There are no lone pairs of electrons on the boron atom.

Therefore, the total number of regions of electron density around the boron atom is 3.

Hybridization:
The hybridization of an atom is determined by the number of regions of electron density around it.

In BCl3, since there are 3 regions of electron density, the boron atom undergoes sp2 hybridization.

Explanation:
1. The atomic orbitals of the boron atom mix to form three sp2 hybrid orbitals.
2. These three hybrid orbitals are oriented in a trigonal planar arrangement around the boron atom, with an angle of 120 degrees between them.
3. Each of these sp2 hybrid orbitals overlaps with a 2p orbital of a chlorine atom to form a sigma bond.
4. The remaining 2p orbital on each chlorine atom contains a lone pair of electrons.

Summary:
The BCl3 molecule undergoes sp2 hybridization, where the boron atom forms three sp2 hybrid orbitals that overlap with the 2p orbitals of three chlorine atoms, resulting in three sigma bonds in a trigonal planar arrangement.

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