To determine which species has bond angles of $120^\circ,$ we need to consider the molecular geometry of each option.$\\$• Option 1: $$ClF$_3 \\$ClF$_3$ has a $$T-shaped$$ molecular geometry due to the presence of two lone pairs on the central chlorine atom.$\\$The bond angles are less than $90^\circ$ and $180^\circ,$ not $120^\circ. \\$• Option 2: $$NCl$_3 \\$NCl$_3$ has a $$trigonal pyramidal$$ geometry due to one lone pair on the nitrogen atom.$\\$The bond angles are approximately $107^\circ,$ not $120^\circ. \\$• Option 3: $$BCl$_3 \\$BCl$_3$ has a $$trigonal planar$$ geometry with no lone pairs on the boron atom.$\\$The bond angles are exactly $120^\circ. \\$• Option 4: $$PH$_3 \\$PH$_3$ has a $$trigonal pyramidal$$ geometry due to one lone pair on the phosphorus atom.$\\$The bond angles are approximately $93.5^\circ,$ not $120^\circ. \\$Therefore, the species with bond angles of $120^\circ$ is $$BCl$_3. \\$This corresponds to Option 3.