Question

The number of species from the following in which the central atom uses sp3 hybrid orbitals in its bonding is ______. $NH_3​, SO_2​, SiO_2​, BeCl_2​, CO_2​, H_2​O, CH_4​, BF_3$​

Answer 1

• $NH_3$: The nitrogen atom is surrounded by three bonded atoms and one lone pair, resulting in an sp3 hybridization due to the tetrahedral arrangement.
• $SO_2$: Sulfur in $SO_2$ is sp2 hybridized because it forms two sigma bonds and has one lone pair, giving a bent structure.
•** ** $SiO_2$: Each silicon atom forms four sigma bonds with oxygen atoms. However, due to its extended lattice structure, we consider the local bonding, indicating sp3 hybridization for the central Si atom.
• $BeCl_2$: The beryllium atom is sp hybridized as it forms two sigma bonds with chlorine atoms, leading to a linear geometry.
• $CO_2$: Carbon in $CO_2$ is sp hybridized since it forms two sigma bonds with oxygen atoms, resulting in a linear structure.
• $H_2O$: The oxygen atom has two sigma bonds and two lone pairs, leading to sp3 hybridization, resulting in a bent structure.
• $CH_4$: Carbon in $CH_4$ is sp3 hybridized as it forms four sigma bonds, resulting in a tetrahedral geometry.
• $BF_3$: Boron in $BF_3$ is sp2 hybridized, as it forms three sigma bonds with fluorine atoms, resulting in a planar triangular structure.