Question

Phosphorus trichloride, PCl3, is commonly used in the chemical industry as a source of phosphorus in various reactions. Indicate the electron pair geometry and the molecular geometry of the PCl3 molecule. Electron pair geometry: T-shaped tetrahedral trigonal planar trigonal pyramidal trigonal bipyramidal Molecular geometry: tetrahedral trigonal pyramidal trigonal bipyramidal trigonal planar T-shaped

Answer 1

Answer:

Electron pair geometry - tetrahedral

molecular geometry- trigonal pyramidal

Explanation:

According to Valence Shell Electron Pair Repulsion Theory, the shape of a molecule is determined by the number of electron pairs around the central atom in the molecule. Lone pairs distort a molecule away from its expected geometry based on VSEPR. This is why the electron pair geometry differs from the actual molecular geometry.

PCl3 has four regions of electron density, three substituents and one lone pair hence its electron pair geometry is tetrahedral. However, the three substituents are arranged in a trigonal pyramidal geometry(its molecular geometry).