Compounds that exhibit reduced solubility as temperature rises are typically gases. This phenomenon can be explained by Le Chatelier's principle and the nature of gas solubility in liquids. As temperature increases, the kinetic energy of the gas molecules increases, which leads to a higher tendency for gas molecules to escape from the liquid phase into the vapor phase, thereby reducing solubility.
In contrast, many solids and ionic compounds generally show increased solubility with rising temperature due to the endothermic nature of their dissolution process, which can absorb heat and drive the dissolving reaction forward. However, when it comes to gases, their solubility usually decreases with temperature.
In summary, the compounds that exhibit reduced solubility as temperature rises are primarily gases, due to their increased tendency to escape from the solvent as thermal energy increases.