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Kinetic Molecular Theory (KMT) is a framework used to describe the behavior of gases and explains a range of phenomena, including compressibility. According to KMT, gas particles are tiny compared to the distances between them and are in relentless, chaotic motion. This incessant motion contributes to gas pressure, which arises from collisions of particles with the walls of a container. The significant gaps between gas particles mean there is a substantial amount of empty space that can be reduced when pressure is applied, thus allowing gases to compress.

The arrangement of particles in matter varies drastically among the three states: solids, liquids, and gases. In solids, particles are tightly packed in a rigid, structured pattern which restricts movement. Liquids have a looser arrangement; particles are still close but can flow around each other. Gases, on the other hand, have a very dispersed arrangement. Gas particles are separated by relatively large distances, which is why they can be easily pushed closer together, making gases highly compressible. The understanding of particle arrangement in these states is essential for grasping why different states of matter react differently to pressure.

Intermolecular forces are the forces of attraction or repulsion which act between neighboring particles: atoms, molecules, or ions. These forces are particularly strong in solids, where particles are locked in place, and somewhat less in liquids, which allows for flow and fluidity. In gases, these intermolecular attractions are weak due to the large distances between the particles. When external pressure is applied to a gas, its particles, which are initially not held tightly together, can move closer without much resistance, facilitating compression. It's the relative strength of these forces in different states of matter that influences how much they resist compression.

The three primary states of matter—solid, liquid, and gas—can be distinguished by their unique characteristics in terms of shape, volume, and particle arrangement. Solids have a fixed shape and volume due to their organized particle formation. Liquids have a fixed volume but adopt the shape of their container because of the intermediate level of particle mobility. Gases have neither a fixed volume nor shape, as their particles can spread out indefinitely. The tendency of a substance to resist compression is deeply connected to its state; solids resist compression significantly, liquids less so, and gases are easily compressible due to the freedom of particle motion and space between them.