Since there are four groups encircling the sulphur atom, the electron geometry is tetrahedral ( 2 lone pairs and 2 hydrogens). Due to the lone pair repulsion of the S-H bonds, the hydrogen sulfide's molecular geometry is bent, something I hadn't encountered in university. As a result, the angle will be much less than 109.5 degrees, or roughly 92 degrees.
The difference between molecular and electronic geometry is that the latter is the geometry of the localised electron densities, whilst the former simply considers the bound substituents around the sulphur, such as the hydrogens ( bonds and lone pairs).
Four of the five geometries linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral are referred to as electron group geometries. The form of the molecule is changed but the electron geometry remains the same if one or more of the bonding pairs of electrons are swapped out for a lone pair.
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