VSEPR Theory - lone electron pair influence

The video tutorial explains the influence of lone pairs on molecular geometry, using water, sulphur dioxide, and ammonia as examples. It discusses how lone pairs occupy more space and cause greater repulsions than bonded pairs, affecting molecular shapes. The VSEPR theory is used to predict molecular geometry, considering lone pair and bond pair repulsions. Sulphur dioxide is shown to have a bent shape due to lone pair repulsions, while ammonia's geometry is affected by its lone pair, resulting in a bond angle less than the typical tetrahedral angle.

Discuss the differences in repulsion strength between lone pairs and bond pairs.

How does VSEPR theory help in predicting the geometry of molecules with lone pairs?

What is the bond angle in ammonia, and how does the presence of a lone pair influence this angle?