Question

Determine the geometries and expected bond angles for the following molecules (i.e. indicate where possible and deviation from ideal angles).Give a brief explanation for your predictions. Also indicate where the lone pairs should be and why

i. NH3 ii. PF6- iii. NO2- iv. SeH2 v. XeOF2 vi. I3- vii. SOCl2

Answer 1

CI inverted v shape pyramidal structure Octahedral inverted v shape pyrammidal T-shape F-Xe-F-179 °c F-Xe-O-89 °C sp?d hybridization ideal angle is ideal angle is trigonalbipyramidal Linea structure structure 90 °c sp3d hybridization trigonalbipyramidal planar 114.5°C 92 °c 109.5°c 90°c 107°c sp' hybridization ideal angle is tetrahe sp'd'hybridization sp hybridization sp' hybridization ideal angle is tetrahedral ideal angle is trigonal deal angle is octahedral Ammonia has one lone pair electron thats why bond angle shifted from 109°C 28' to 107°C due to lone pair -bond pair repulsions NO, has one lone pair of electronsthats why bond angle shifted from 120°C to 114.5 °C due to lone pair -bond pair repulsions SeH2 has two lone pair of electrons thats why bond angle shifted from 109°C 28' to 92°C due to lone pair -lone pair repulsions XeOF2 hast wo lone pair of electrons thats why bond angle shifted from 180°C and 90°C to 179°C and 89°C due to lone pair -lone pair repulsions Ij has has three lone pair of electrons which are located at corners of trogonal bipyramidal thats why structure should be linear, repulsitions are less SOCl2 has one lone pair of electron thats why bond angle shifted from 120°C to 109.5°C due to lone pair -bond pair repulsions