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I think sp3 was so common just because of the molecules we were dealing with (I noticed the pattern too). I believe we will be encountering molecules that have other hybridizations because in a workshop I went to, as well as textbook problems, there were hybridizations other than sp3 that was present, so I think it will just depend on what we're given!
I think sp3 was so common because it means that the central atom has 4 regions of electron density, and tetrahedral is a common arrangement of electron density. The fact that sp3 was the hybridization for the majority of the Sapling homework may just be a coincidence though.
It seems to be common considering that when you use the octet rule to complete a lewis structure, there are always four bonds between the central atom and the surrounding atom. In this way, if we consider the electron arrangement of the molecule in terms of the central atom, we will always get four regions of electron density most of the time and therefore a tetrahedral arrangement and an sp3 hybridization.
Most simple molecules are molecules that have carbon, nitrogen, or oxygen as a central atom. This tends to make the electron geometries tetrahedral, therefore implying an sp3 hybridization, just based on how many lone pairs and bonding sites there are on the central atoms.
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