Kinetic Theory
Gas particles are very far apart compared with this.
Their size
An ideal gas follows these, while a real gas follows real-world constraints.
The assumptions of kinetic molecular theory
A fluid is a substance that can do this in its container.
Take the shape
Particles in this kind of solid sit in an orderly, repeating pattern.
Crystalline
A system of atoms with uniform composition and properties is called this
Phase
Collisions of gas particles with each other and with the walls are this kind of collision.
Elastic
Gases can expand and be compressed because they lack this.
A definite volume
Both liquids and gases are classed as these.
Fluids
Particles in this kind of solid are arranged randomly
Amorphous
Liquid to gas is boiling; gas to liquid is this.
Condensation
Kinetic molecular theory says there are no this between gas particles.
Forces of attraction
This is the spontaneous mixing of two substances by random motion.
Diffusion
Liquids are denser than gases and resist this, but they can still diffuse.
Compression
Amorphous solids are sometimes called these, and they lack a definite melting point.
Supercooled liquids
The transition from gas to solid is this.
Deposition
The temperature of a gas is the average amount of this of its particles.
Kinetic energy
This is the movement of a gas through a small opening.
Effusion
This force pulls adjacent liquid particles together and shrinks the surface.
Surface tension
This is the smallest piece of a crystal that still shows the whole three-dimensional pattern.
A unit cell
This is the energy needed to vaporize one mole of liquid at constant pressure
Molar enthalpy of vaporization
Gas particles carry kinetic energy and are in continuous this
Motion
Attractive forces ignored by the ideal-gas picture are present in this kind of gas.
A real gas
The curve of the liquid in a tube is this.
Meniscus
This crystal type is held by intermolecular forces.
Covalent molecular
All three phases meet at this point
Triple point