SUMMARY
The molecular geometry of ClF3 is T-shaped, as determined by VSEPR theory. Chlorine trifluoride (ClF3) has a total of five electron pairs around the chlorine atom, consisting of three bonding pairs and two lone pairs, designated as AB3E2. The presence of these lone pairs influences the molecular shape, resulting in the T-shaped configuration rather than a trigonal bipyramidal structure.
PREREQUISITES
- Understanding of VSEPR theory
- Knowledge of molecular geometry terminology
- Familiarity with electron pair geometry
- Basic chemistry concepts related to bonding and lone pairs
NEXT STEPS
- Study VSEPR theory in detail
- Learn about different molecular geometries and their classifications
- Explore the properties and applications of chlorine trifluoride (ClF3)
- Investigate the impact of lone pairs on molecular shapes
USEFUL FOR
Chemistry students, educators, and professionals interested in molecular geometry and VSEPR theory applications.