PF3: Phosphorus trifluoride consists of a phosphorus atom bonded to three fluorine atoms. The central phosphorus atom has one lone pair of electrons, leading to a trigonal pyramidal shape due to electron pair repulsion. The bond angles are approximately 107 degrees, similar to ammonia (NH3).
COCl2: In carbon dichloride, the carbon atom is bonded to two chlorine atoms and has no lone pairs. The molecular geometry is trigonal planar, resulting in bond angles of approximately 120 degrees.
CS2: Carbon disulfide features a carbon atom double-bonded to two sulfur atoms. The molecule is linear because there are no lone pairs on the central carbon, leading to bond angles of 180 degrees.
PbCl2: Lead(II) chloride has a lead atom which is surrounded by two chlorine atoms and a lone pair. This results in a bent or angular shape with a bond angle slightly less than 120 degrees due to the presence of the lone pair.
CBr4: Carbon tetrabromide has a carbon atom bonded to four bromine atoms and no lone pairs. It adopts a tetrahedral shape with bond angles of approximately 109.5 degrees.
SF2: In sulfur difluoride, the sulfur atom is bonded to two fluorine atoms and has two lone pairs of electrons, resulting in a bent molecular shape. The bond angle is about 104.5 degrees, which is influenced by the repulsion from the lone pairs.