Kinetic Molecular Theory and States of Matter

Vocabulary practice flashcards covering kinetic molecular theory, states of matter, physical and chemical changes, phase transitions, and Boyle's Law.

Kinetic molecular theory

A scientific model stating that all matter is made of tiny particles in continuous motion, which is useful for explaining observations and state changes.

Atoms

The extremely tiny particles that make up all matter according to kinetic molecular theory.

Constant motion

The state of continuous, unending movement exhibited by all particles of matter.

Empty spaces

The gaps between particles of matter that, along with the particles themselves, are too small to be seen.

Solid

A state of matter in which particles are so close together and move so slowly that they can only vibrate.

Liquid

A state of matter in which particles are slightly further apart and move slightly faster than those of a solid.

Gas

A state of matter in which particles are further apart and move very quickly.

Thermal energy (heat)

A form of energy that, when supplied to matter, makes its particles move faster.

Chemical change

Changes in which new substances are produced with properties that are different from those of the starting material(s).

Physical change

Changes in which no new substance is produced, and the properties of the starting substances remain the same in the end product.

Naturally occurring change

A state change in matter that takes place on its own in nature.

Artificially induced change

A change in matter brought about through intentional human or external intervention.

Definite shape of ice

The rigid shape maintained by ice due to bonding and close packing between its particles.

Vibration

The restricted movement of particles held tightly in place by close packing and bonds within a solid.

Melting point

The point at which supplied energy causes solid particles to break away from one another and their bonds to be broken, becoming a liquid.

Liquid particle arrangement

The particle configuration where particles are not closely packed as in a solid and move further apart as energy is supplied.

Boiling

The transition process where heated liquid particles become energized enough to break their weak bonds and form a gas.

Water vapour

The gas formed when heated liquid water reaches its boiling point and particle bonds are broken.

Weak bonds in liquids

The characteristic intermolecular attractions holding a liquid together, which are broken when particles become energized by heating.

Boyle’s Law

The law stating that the volume of a gas is inversely proportional to the pressure, provided that temperature and the number of particles remain constant.

Conditions of Boyle’s Law

The requirement that both temperature and the number of gas particles must remain constant for Boyle's Law to hold true.

Inverse gas pressure-volume relationship

The principle stating that as pressure increases, gas volume decreases, and as pressure decreases, gas volume increases.

Application of force to gases

An action that alters the pressure acting on a gas and leads to a change in its volume.

Melting

The physical change of state from a solid to a liquid.

Freezing

The physical change of state from a liquid to a solid.

Condensation

The physical change of state from a gas to a liquid.

Sublimation

The direct physical change of state from a solid into a gas without passing through the liquid phase.

Deposition

The direct physical change of state from a gas into a solid without passing through the liquid phase.

Energy-vibration correlation

The principle that little energy causes little vibration, whereas as energy increases, particle vibrations also increase.

States of matter transition diagram

A visual representation showing the phase transitions between solid, liquid, and gas: melting, freezing, boiling, condensation, sublimation, and deposition.