Question

which diagram shows how the covalent bonds most likely form in a phosphorous trichloride molecule?

Explanation:

Step1: Determine valence electrons

Phosphorus has 5 valence electrons, chlorine has 7 valence electrons. In \(PCl_3\), phosphorus forms single bonds with three chlorine atoms.

Step2: Analyze bond types

Each single bond (\(-\)) represents a pair of shared electrons. Double bonds (\(=\)) are not formed here as phosphorus only needs to share three pairs of electrons (one with each \(Cl\)) to achieve a more stable electron configuration (it has a lone pair left after forming three single bonds).

Answer:

The diagram with only single bonds (\(Cl - P - Cl\) with appropriate lone - pair dots) is the correct one. (Since the options are not labeled, but based on the bond - type analysis, the structure with three single \(P - Cl\) bonds is correct).