Why are oxides generally insoluble?
Oxides are generally insoluble in water because of the following factors:

* **Lattice energy:** The lattice energy of an oxide is the energy required to separate the ions in the solid and bring them to an infinite distance apart. The lattice energy of an oxide is typically high, which means that a lot of energy is required to dissolve the oxide in water.
* **Hydration energy:** The hydration energy is the energy released when an ion is surrounded by water molecules. The hydration energy of an oxide ion is typically low, which means that there is not a lot of energy released when the oxide dissolves in water.
* **Steric effects:** The steric effects of an oxide refer to the way in which the water molecules are able to interact with the oxide ions. If the oxide ions are small and tightly packed, then the water molecules will have a hard time interacting with them. This will make the oxide more insoluble in water.

There are some exceptions to this rule, however. For example, the oxides of some alkali metals, such as sodium oxide and potassium oxide, are soluble in water. This is because the hydration energy of the oxide ions in these cases is high enough to overcome the lattice energy.

In general, however, oxides are insoluble in water. This is why you will not find oxides dissolved in water solutions, such as tap water or seawater.
Are those all the possible exceptions or are there more possible exceptions than the ones you detailed?