SUMMARY
C2H4, or ethene, is definitively an example of sp2 hybridization due to the presence of a double bond between the two carbon atoms. Each carbon atom in ethene forms three sigma bonds: two with hydrogen atoms and one with the other carbon atom, resulting in a total of three bonding groups. In contrast, C2H2, or acetylene, exhibits sp hybridization because it contains a triple bond between the carbon atoms. The confusion arises from the interpretation of bonding groups in hybridization theory, which can vary based on the perspective of the chemist.
PREREQUISITES
- Understanding of hybridization concepts in chemistry
- Familiarity with molecular geometry and bonding theories
- Knowledge of sigma and pi bonds
- Basic principles of quantum mechanics as applied to atomic structure
NEXT STEPS
- Study the differences between sp, sp2, and sp3 hybridization
- Research the concept of bonding groups in molecular geometry
- Explore the implications of hybridization on molecular stability and reactivity
- Examine the role of double and triple bonds in determining hybridization states
USEFUL FOR
Chemistry students, educators, and professionals seeking to clarify concepts of hybridization and molecular geometry, particularly in organic chemistry.