The five particle theory of matter

PROPERTIES OF MATTER DEFINITION. Matter is anything that has weight and takes up space. Everything you can see and touch is made up of matter. Matter exists in three main forms: solids, liquids, and gases. It also has properties that we can describe through density, solubility, conductivity, magnetism, etc.

Some examples of physical properties are:

• physical state (solid, liquid or gas)
• color.
• odor.
• solubility in water (the ability of substance to dissolve in water)
• density.
• melting point 0 degrees for H20.
• boiling point 100 degrees for H20.
• freezing point 0 degrees for H20.

• All matter is made up of very small particles.
• All particles in a pure substance are the same. Different substances are made up of different particles.
• There is space between all particles.
• The particles are always moving.
• The particles in a substance are attracted to one another.

Assumptions. Molecules are in a state of continuous motion and hence they possess kinetic energy. The kinetic energy of molecules increases with an increase in temperature and decreases with a decrease in temperature.

The kinetic theory relates the independent motion of molecules to the mechanical and thermal properties of gases—namely, their pressure, volume, temperature, viscosity, and heat conductivity. Three men—Daniel Bernoulli in 1738, John Herapath in 1820, and John James Waterston in 1845—independently developed the theory.

Explains how particles in matter behave by making three assumptions: 1) All matter is made of small particles. 2) These particles are in constant, random motion. 3) These particles are colliding with each other and the walls of their container.

The kinetic theory makes three assumptions when applied to gases. Gases are composed of tiny particles with insignificant volume that are in rapid, random, and constant motion.

Terms in this set (5) Gas particles are continuous, rapid, random motion. They therefore possess kinetic energy, which is energy of motion. There are no forces of attraction between gas particles. The temperature of a gas depends on the average kinetic energy of the particles of the gas.

Assumptions of the kinetic-molecular theory include the following: Gas particles are in constant, random motion. There are no attractive forces between gas particles. Collisions of gas particles are elastic, so no energy is lost. The speed of a gas particle is directly proportional to the temperature of the system.

Kinetic Molecular Theory states that gas particles are in constant motion and exhibit perfectly elastic collisions. Kinetic Molecular Theory can be used to explain both Charles’ and Boyle’s Laws. The average kinetic energy of a collection of gas particles is directly proportional to absolute temperature only.