Why is an O - Oxygen with 3 lone pairs (6 lone oxygens) and a negitive sign, Sp2 hybridized, and not Sp3?

Why is an O - Oxygen with 3 lone pairs (6 lone oxygens- and a single bond to a c) and a negitive sign, Sp2 hybridized, and not Sp3?
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Answer:
Hybridization can be due to the number of bonds as well, not just the charge.

The Oxygen with 3 lone pairs is negatively charged due to its electron orbitals not being bonded. The reason is is sp2 and not sp3 is because there is a missing pi bond compared to the sp3, and the ratio to sigma bond is lower.
oxides arent sp2, they are sp3

edit, wait, it depends on what else its connected to...

enolates are sp2, so are phenoxides, all due to resonance. if you have the ability to donate one of those lone pairs to the carbon through resonance, even though you show the oxygen as negative, its really partially bonding with the carbon, making a pseudo-double bond, which is sp2

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