Determine the electron geometry (eg),molecular geometry (mg),and polarity of PCl₃. A) eg = tetrahedral, mg = trigonal planar, nonpolar B) eg = trigonal planar, mg = tetrahedral, polar C) eg = linear, mg = linear, polar D) eg = tetrahedral, mg = trigonal pyramidal, polar E) eg = trigonal pyramidal, mg = trigonal pyramidal, nonpolar

Question

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The central atom (P) in PCl₃ has 5 valence electrons and forms covalent bonds with 4 other atoms (3Cl and 1S). Thus, the electron geometry is tetrahedral. However, one of the bonded atoms is a lone pair on the S atom, which causes the molecular geometry to be trigonal pyramidal. The molecule is therefore polar due to the asymmetric shape and the presence of polar bonds between P and Cl atoms. Option D correctly identifies the electron geometry as tetrahedral and the molecular geometry as trigonal pyramidal, with the correct polarity as polar. The other options do not correctly match the shape and polarity of the molecule.

Determine the Electron Geometry (Eg),molecular Geometry (Mg),and Polarity of PCl3

Determine the Electron Geometry (Eg),molecular Geometry (Mg),and Polarity of PCl₃