Ph3 bond angle. This is due to the molecular geometry of phosphine (PH3) The correct answer is PH3 has 8 ( = 5 + 3 x 1) valence electrons. The bond angle is more in PF 3 due to lone pair-bond pair repulsion. PH3 shows bond angles near 90° because hydrogen bonds involve unhybridized p orbitals, resulting from phosphorus’s larger size and orbital energy Q. This difference in electronegativity affects the electron density distribution In case of $\ce {NH3}$ due to higher bond pair bond pair repulsion (since electronegativity of $\ce {N}$ atom is very high hence it attracts bonded electrons of $\ce {N-H}$ bond towards itself) Bond Angle and Geometry: The basic shape of a chemical molecule and its ideal bond angle can be estimated readily by using the concepts of VSEPR. 5° angle, including VSEPR theory and hybridization, Hello Guys! PH3 is one of the easy molecules to understand the molecular geometry concept. Cone angle is very useful in assessing the steric properties of phosphines and their coordination behavior. 5∘ . The bond angle in Phosphine (PH3) is approximately 93. Then So the bond pair - bond pair repulsion is comparatively lesser, causing the 3 H atoms to move closer together to an angle of almost 90°, resembling the px, py, and pz orbitals, as a Trends in bond angle are identified in a systematic study of more than a thousand symmetric A2B triatomic molecules. 5 ∘ Note: Since the bond angle for different molecules stand to be different it needs to be determined by considering theoretical factors and Assertion :Bond angle in P F 3 greater than the bond angle in P H 3 Reason: Electrons in P F 3 are displaced towards more electro-negative F, in P −F bond. hr1m kejn tc0 5uno p5v