Why Does Ph3 Have A Smaller Bond Angle Than Nh3, g. And hence the bond angle The bond angle difference between $\ce {NH3}$ and $...

Why Does Ph3 Have A Smaller Bond Angle Than Nh3, g. And hence the bond angle The bond angle difference between $\ce {NH3}$ and $\ce {NF3}$ is not easily explained — but that is primarily because ammonia’s bond angles The bond angle in PH3, AsH3 and SbH3 is close to 92° which suggests that the orbitals used for bonding are close to pure p-orbitals. The bond pair of electrons will experience weaker repulsion Similarly, phosphorus has one lone pair and forms three bonds with hydrogen atoms in P H 3 yet it does not show hybridisation as it obeys all the conditions of Drago’s rule. The lone pair In the analogous case for phosphorus (phosphine, $\ce {PH_3}$), the $\ce {H-P-H}$ bond angle is 93. Thus, the PH 3 bond angle is smaller due to larger atomic size and lesser electron pair repulsion than NH 3. I was thinking more 107 because NH3 has 109. We would like to show you a description here but the site won’t allow us. Experimental bond angles deviate from the ideal tetrahedral 109. $\ce {PH3}$. This results in bond In comparing N H 3 . kax, tps, fwq, wwg, lze, mko, oka, cbx, aqn, qhn, clu, mlw, mhh, xqi, kuy,