Electron Geometry
The electron geometry of CHCl3 is tetrahedral. This is because there are four regions of electron density around the central carbon atom: one for the carbon-hydrogen bond and three for the carbon-chlorine bonds.
Molecular Geometry
The molecular geometry of CHCl3 is also tetrahedral. Although the molecule has polar bonds, the overall shape does not create a dipole moment that would lead to a different molecular geometry.
Bond Angles
The bond angles in CHCl3 are approximately 109.5 degrees. This angle is consistent with the tetrahedral arrangement of electron pairs around the central carbon atom.
Polarity
CHCl3 is a polar molecule. The chlorine atoms are more electronegative than carbon, leading to dipole moments in the C-Cl bonds. Although the molecular geometry is symmetrical, the presence of three chlorine atoms results in an overall dipole moment due to their electronegativity.
Central Atom Hybridization
The central atom in CHCl3, which is carbon, is sp3 hybridized. This hybridization arises from one 2s and three 2p orbitals mixing to form four equivalent sp3 hybrid orbitals, which allow for the formation of four sigma bonds.