Ethene's Carbon Hybridization and Molecular Bonding Steps: - Identify structure: Ethene (C₂H₄) has a carbon-carbon double bond, with each carbon attached to two hydrogens. - Determine hybridization: Each carbon forms three sigma bonds (trigonal planar geometry), using sp² hybrid orbitals, leaving one p orbital per carbon. - Count sigma bonds: Four C-H sigma bonds (two per carbon) plus one C-C sigma bond, totaling five sigma bonds. - Count pi bonds: The two unhybridized p orbitals overlap sideways to form one pi bond. Why none match perfectly: - Standard description is sp² hybridization with 5 σ bonds and 1 π bond, but options misstate either hybridization or bond count. Why A is wrong: - sp² is correct, but lists only 4 σ bonds (ignores total molecular count). Why B is wrong: - 5 σ and 1 π is correct for bonds, but sp³ hybridization applies to tetrahedral geometry like ethane, not ethene's sp². Why C is wrong: - Identical to A; sp² correct, but 4 σ bonds incorrect for the molecule. Why D is wrong: - Same as B; wrong hybridization …