Chlorine trifluoride, ClF3, is used in semiconductor processing because of its ability to clean metal surfaces without mechanical abrasion.
Respond to the prompts below regarding the structure and bonding of ClF3.
(a) Draw a complete Lewis diagram for ClF3 showing all lone pairs on the central chlorine atom.
(b) Determine the molecular geometry around the chlorine atom and state the ideal bond angles associated with that geometry.
(c) Experimentally, the Cl–F bonds that lie along the axis are longer than the Cl–F bonds in the plane perpendicular to the axis. Using your answer to part (b), provide a chemical rationale for this bond-length difference.
(d) Predict whether ClF3 is polar or nonpolar and justify your prediction using both geometric and electronegativity considerations.