None None 3. CIF 3 Chlorine Lewis Dot Structure Total Electron Pairs 4. 00 SF4 2001/bal Electron Geometry square pyramides of trifluoride AS : F :F: C:F: ü: Bonding Pairs trigonal bipyramidal Total Valence Electrons 28 27167 anil Molecular Geometry T-shaped ially Nonbonding Pairs Total Valence Electrons sulou 2
The Correct Answer and Explanation is :
Chlorine trifluoride (ClF₃) is a chemical compound with a T-shaped molecular geometry, as predicted by Valence Shell Electron Pair Repulsion (VSEPR) theory.
Lewis Structure and Valence Electrons:
The central chlorine (Cl) atom has seven valence electrons, and each fluorine (F) atom contributes seven valence electrons, totaling 28 valence electrons for ClF₃.
In the Lewis structure, chlorine forms single bonds with each of the three fluorine atoms, utilizing six electrons. The remaining 22 electrons are placed as lone pairs: two lone pairs on each fluorine atom and two lone pairs on the chlorine atom.
Electron Geometry and Molecular Geometry:
The electron geometry of ClF₃ is trigonal bipyramidal, with five positions: three equatorial and two axial. The two lone pairs on the chlorine atom occupy the two axial positions to minimize electron-electron repulsion. The three fluorine atoms occupy the three equatorial positions, resulting in a T-shaped molecular geometry.
Bond Angles:
In a perfect trigonal bipyramidal geometry, the bond angles are 90° and 120°. However, due to the presence of lone pairs, the bond angles in ClF₃ are slightly less than 90° and 180°, resulting in a T-shaped structure.
Hybridization:
The central chlorine atom undergoes sp³d hybridization, combining one 3s, three 3p, and one 3d orbital to form five sp³d hybrid orbitals. Three of these orbitals form bonds with the fluorine atoms, and the remaining two contain lone pairs.
Conclusion:
ClF₃ exhibits a T-shaped molecular geometry due to the arrangement of bonding and lone pairs around the central chlorine atom. This structure is consistent with the predictions of VSEPR theory and is supported by the compound’s chemical properties and reactivity.