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First draw the lewis structure. You see that BeCl2 only has two regions of electron density around it. Thus, its hybrid orbital will be sp. If it had three regions of electron density around it, the hybrid orbital would be sp2. Regions of electron density is equal to the number of hybrid orbitals.
Aside from looking at the regions of electron density in the Lewis dot structure, when you find Be on the periodic table, you see that has 2 valence electrons. When looking at its hybridization, this would give it an s2 denotation. However, we need to have two sites of bonding and through hybridization, that s2 moves an electron to the p orbital so that there can be two possible bonds for the 2 chlorine. This, in turn, makes the hybridization an sp rather than an s2.
Why does BeCl2 even have a lewis structure with bonds in the first place? I thought it was an ionic compound but then I just figured we could draw it with bonds because no ionic compound is 100% ionic... is that the reason?
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