Final answer:
The hybridization of an oxygen atom depends on its bonding and lone pairs; it can be sp for a linear molecule with pi bonds, sp3 for a molecule like water with two lone pairs, and less commonly, sp2 for an atom with one bond and three lone pairs.
Step-by-step explanation:
To predict the hybridization of the oxygen atom in a molecule, we must first understand its steric number or the number of electron pairs (bonding and lone pairs) around it. Since the question code 10-82a doesn't provide specific molecular context, we'll refer to common scenarios for an oxygen atom in organic compounds. Typically, an oxygen atom with two bonds (one sigma bond and one pi bond) and no lone pairs is sp hybridized, resultant in a linear geometry. This can be seen for example in carbon dioxide (CO2). If the oxygen has two bonds (both sigma) and two lone pairs, it is sp3 hybridized, which is common in water (H2O) and results in a bent geometry. Lastly, if the oxygen has one sigma bond and three lone pairs, which is less common, the hybridization can be described as sp2, leading to a bent geometry as well.