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

Correct Answer: 4

• \(NH_3\): 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.