Why h2 and o2 are ideal gases at room temperature but SO 2 is real gas?

H₂ and O₂ are considered ideal gases at room temperature because they are simple diatomic molecules with negligible intermolecular forces and occupy a large volume compared to their size, allowing them to behave according to the ideal gas law. In contrast, SO₂ is a larger, polar molecule that exhibits significant intermolecular forces, such as dipole-dipole interactions and potential van der Waals forces, leading to deviations from ideal gas behavior. These interactions become more pronounced at room temperature, making SO₂ behave more like a real gas.