The molecular geometry of PF3 (phosphorus trifluoride) is trigonal pyramidal. This geometry arises because phosphorus has five valence electrons, three of which are used to form bonds with three fluorine atoms. The remaining two electrons form a lone pair on the phosphorus atom.
In a trigonal pyramidal geometry, the three fluorine atoms are positioned at the corners of a triangular base, while the lone pair occupies the apex of the pyramid. This arrangement results in bond angles that are slightly less than 109.5 degrees due to the repulsion between the lone pair and the bonding pairs of electrons.
Understanding the molecular geometry of PF3 is crucial for predicting its chemical behavior and interactions with other molecules.