Question

the hybridization of the carbon present in formaldehyde, ch₂o, is image: lewis structure of ch₂o (h-c(=o)-h with lone pairs on o) options: sp (green), sp³ (blue), sp² (orange)

Explanation:

Step1: Determine the structure of formaldehyde

Formaldehyde (\(CH_2O\)) has a carbon atom double - bonded to an oxygen atom (\(C = O\)) and single - bonded to two hydrogen atoms (\(C - H\)). The Lewis structure shows that the carbon atom is surrounded by three regions of electron density (the double bond to \(O\) and the two single bonds to \(H\) atoms).

Step2: Relate electron density to hybridization

The number of regions of electron density around a central atom determines its hybridization. For a central atom with three regions of electron density, the hybridization is \(sp^{2}\). This is because in \(sp^{2}\) hybridization, one \(s\) orbital and two \(p\) orbitals hybridize to form three equivalent \(sp^{2}\) hybrid orbitals, which can account for three regions of electron density (as in the case of the carbon in formaldehyde, where it forms three bonds: one double bond and two single bonds, and the double bond consists of one \(\sigma\) and one \(\pi\) bond, with the \(\sigma\) bonds and the lone - pair - free electron arrangement being accounted for by the \(sp^{2}\) hybrid orbitals).

Answer:

\(sp^{2}\)