Final answer:
Hybridization types sp and sp² allow for the formation of at least one pi bond, as they leave unhybridized p orbitals available, which can overlap laterally to form π bonds. The sp³ hybridization involves all s and p orbitals, leaving no p orbitals to form π bonds.
Step-by-step explanation:
The question asks which hybridization schemes allow the formation of at least one pi bond (π bond). In chemistry, hybridization is a concept that describes the bonding of atoms through the combination of their atomic orbitals. The hybridization types mentioned, sp, sp², and sp³, all relate to the different geometries and electron pair surroundings of a central atom in a molecule.
In sp hybridization, the carbon atom mixes one s orbital with one p orbital, resulting in two hybridized orbitals. The remaining two p orbitals are available for forming π bonds. An example is the triple bond in acetylene (C2H2), which has one sigma (o) bond and two π bonds.
The sp² hybridization occurs when one s orbital and two p orbitals mix, creating three hybridized orbitals. This setup leaves one p orbital unhybridized, which can participate in forming a π bond. Structures with double bonds, such as ethene (C2H4), are commonly associated with sp² hybridized carbon atoms, which have one o bond and one π bond in the double bond.
Finally, in sp³ hybridization, one s orbital and three p orbitals blend to form four hybridized orbitals, with no p orbitals remaining to form π bonds. Consequently, molecules with sp³ hybridized atoms, such as methane (CH4), only have single bonds (o bonds).
Taking all this into account, the MCQ answer to the question is hybridization schemes that allow the formation of at least one pi bond are sp and sp².