Consider
The central atom is dsp3 hybridized; it forms 1 sigma bond and 2 pi bonds by overlapping with 2p orbitals on F atoms, and the two sets of lone pairs reside in the remaining hybrid orbitals.
The central atom is sp2 hybridized; it forms 3 sigma bonds by overlapping with 2p orbitals on F atoms, and there are no lone pairs remaining on the central atom.
The central atom is sp2 hybridized; it forms 3 sigma bonds by overlapping with 2p orbitals on F atoms, and the two sets of lone pairs reside in the remaining unhybridized p orbitals.
The Correct Answer and Explanation is :
The given descriptions refer to the hybridization and bonding of the central atom in a molecule, likely involving fluorine (F) atoms, which typically form bonds with other elements. The explanations describe different hybridization states of the central atom and its bonding with fluorine. Let’s analyze each one:
- The central atom is dsp3 hybridized; it forms 1 sigma bond and 2 pi bonds by overlapping with 2p orbitals on F atoms, and the two sets of lone pairs reside in the remaining hybrid orbitals. This description is incorrect because dsp3 hybridization typically forms 5 hybrid orbitals, which are used to form 5 sigma bonds (or 4 sigma bonds and one lone pair, etc.), with no possibility of forming 2 pi bonds. In dsp3 hybridization, the central atom typically forms bonds using hybrid orbitals for sigma bonding, with lone pairs in the remaining orbitals. Therefore, the formation of pi bonds is not consistent with dsp3 hybridization.
- The central atom is sp2 hybridized; it forms 3 sigma bonds by overlapping with 2p orbitals on F atoms, and there are no lone pairs remaining on the central atom. This description is correct. Sp2 hybridization involves the mixing of one s orbital and two p orbitals, forming three sp2 hybrid orbitals that arrange themselves in a trigonal planar geometry. The central atom uses these hybrid orbitals to form 3 sigma bonds, typically with fluorine atoms, and there are no lone pairs remaining on the central atom. This type of hybridization and bonding is commonly seen in molecules such as BF₃.
- The central atom is sp2 hybridized; it forms 3 sigma bonds by overlapping with 2p orbitals on F atoms, and the two sets of lone pairs reside in the remaining unhybridized p orbitals. This description is correct. In sp2 hybridization, the central atom uses three sp2 hybrid orbitals to form sigma bonds with fluorine atoms, and the remaining unhybridized p orbitals hold the lone pairs. This bonding scenario is observed in molecules such as formaldehyde (CH₂O), where the central atom (C) is sp2 hybridized, with one set of lone pairs occupying the unhybridized p orbitals.
In conclusion, the second and third descriptions are correct, with the second describing a molecule like BF₃ and the third describing a molecule like formaldehyde.
Let me now generate an image to represent the hybridization states and bonding in these cases.

Here is the illustration showing the sp2 hybridization for the central atom with 3 sigma bonds formed with fluorine atoms. It includes both scenarios: one with no lone pairs on the central atom and one with lone pairs occupying unhybridized p orbitals. The bond angles and electron pairs are labeled for clarity.