Frequently Asked Question

Here's a breakdown of the orbital structures for Ethanone (Acetone), Ethylene, and Acetylene:
Ethanone (Acetone)
Hybridization: The carbon atom in the carbonyl group (C=O) is sp2 hybridized, meaning it forms three sigma bonds (two with carbons and one with oxygen) and has one unhybridized p orbital.
Structure: The molecule has a planar geometry around the carbonyl carbon. The three sp2 orbitals form a trigonal planar structure with bond angles of approximately 120°. The remaining unhybridized p orbital on the carbonyl carbon overlaps with the p orbital of the oxygen to form a pi bond.
Ethylene (Ethene)
Hybridization: Each carbon atom is sp2 hybridized, forming three sigma bonds (two with hydrogen atoms and one with the other carbon) and one unhybridized p orbital.
Structure: The molecule has a planar geometry. The three sp2 orbitals of each carbon atom form a trigonal planar structure with bond angles of approximately 120°. The unhybridized p orbitals on each carbon atom overlap to form a pi bond, resulting in a double bond between the carbon atoms.
Acetylene (Ethyne)
Hybridization: Each carbon atom is sp hybridized, forming two sigma bonds (one with hydrogen and one with the other carbon) and two unhybridized p orbitals.
Structure: The molecule has a linear geometry. The two sp orbitals of each carbon atom form a linear structure with bond angles of 180°. The two unhybridized p orbitals on each carbon atom overlap to form two pi bonds, resulting in a triple bond between the carbon atoms.