Explain following terms briefly:

a. Intermolecular potential energy

b. The Lennard-Jones potential

c. Zeroth law of thermodynamics

d. System, closed system, open system, and isolated system

e. Equilibrium

f. Intensive properties and extensive properties

g. Ideal gas

h. Saturation

Remember that the molecule is a substance formed by two or more atoms. A molecule can bind to another if they are close enough and attract each other with the necessary force. And there are different types of forces.

Intermolecular potential energy: It describe the forces between molecules, and depends on the magnitude (how much) of the intermolecular forces (attractions between molecules) and the position of one molecule relative to the other.

The Leonnard-Jones potencial: It is a model that describes the relationship between intermolecular forces and r, the distance between the centers of the two molecules.

Zeroth law of thermodynamics: It is one of the four laws of thermodynamics. Thermodynamics is the study of the relationship between heat, temperature, work, and energy. In this law if two systems are both in thermal equilibrium with a third system, then the first two systems are also in thermal equilibrium with each other. For example, If you enter a pool, at first you will notice the cold water, then you will reach thermal equilibrium.

System: A system is the part of the universe that the person decides to study.

Open system: This system exchanges matter and energy with the surroundings. An example is a pot of boiling water. The energy introduced to the system by fire transforms water into gas, which is released back into the environment.

Closed system: It exchanges only energy with its surroundings, not matter. An example is a bottle of cold water. When the bottle is closed, the transfer of matter between the system and the environment is impossible: no liquid can enter or leave. However, it is possible to exchange energy: the water will gradually heat up to room temperature.

Isolated system: It does not exchange energy or matter with its surroundings. An example is canned foods. Generally, these foods are far from any exchange of matter or energy. But it must be taken into account that there are some, if there are any, systems that exist in this world that are completely individual systems.

Equilibrium: The equilibrium of a system is defined when it is incapable of spontaneously experiencing any change of state or thermodynamic process. That is, it is necessary to make perturbations for changes happens.

Intensive properties: Intensive properties don't depend on system mass or size. An example is the temperature because if it is measured in a liter of water or a glass of water under the same conditions, the measurement will be the same.

Extensive properties: This depends on the mass or size of the system being analyzed. Examples: Length is an extensive property because it depends on size. Volume is an extensive property because by adding more material to a container the volume changes, even if it is the same material.

Ideal gas: An ideal gas is an approximation that is made of a real gas. The molecules of an ideal gas do not attract or repel each other. They only interact with the walls of the container. Another characteristic is the molecules themselves that do not occupy volume. The gas has volume, because the molecules expand in a large region of space, but the molecules of an ideal gas are considered particles that don't occupy space, without volume.

Saturation: A saturation, in chemistry, is defined as a solution (substance in greater proportion) that no longer dissolves more solute (substance in smaller quantity). This means that when more solute is added, it will appear in a different phase, such as a solid. Remember that solute and solvent are two of the components of a solution. The solute is the substance (solid, liquid or gaseous) that dissolves in the solvent to produce a homogeneous mixture known as a solution.