From a molecular viewpoint, explain the differences among gases, liquids, and solids.

When looking at matter from a molecular level, solids represent one of the most ordered and structured forms. Within a solid, the molecules are tightly bound to each other in a well-defined, often crystalline pattern. They are locked into place, which means they do not move from one position to another, but they can vibrate. These vibrations are more pronounced at higher temperatures yet are still very limited compared to other states of matter.

The strong intermolecular forces in solids result in unique properties. For instance, solids maintain a fixed volume and shape, and they are not easily compressible due to the close packing of their molecules. Materials like diamonds, metals, and ice illustrate the solid state and showcase attributes like rigidity and resistance to force – all rooted in their molecular arrangement.

In contrast to the rigidity of solids, liquids offer a more dynamic environment for their molecules. Here, molecules are close together but not in fixed positions, which allows them to move around and slide past one another – a process intimately connected with the concept of fluidity. This sliding motion enables liquids to take the shape of their containers while still maintaining their own unique volume, independent of the space they're in.

As temperature increases, the energy of these molecules also rises, leading to greater movement and a decrease in the forces holding them together. This phenomenon is readily observed in the form of droplets or when water takes the shape of a glass. The balance between attractive forces and motion defines this state, making liquids neither completely ordered like solids, nor completely disordered like gases.

Gases showcase the least amount of order in molecular arrangement. The molecules within a gas are spread apart and move rapidly in all directions, colliding with each other and the walls of their container. This high-speed, random movement leads to an even spread of the molecules throughout any available space, attributing to gases having neither a definite shape nor a fixed volume.

The ample space between gas molecules means they are easily compressible, a stark difference from solids and a factor in the workings of various technologies, such as engines and air compressors. Keeping a balloon inflated is a simple, everyday example of gas molecules pushing outwards equally in all directions, demonstrating both their kinetic energy and the power of their disordered arrangement.