Kinetic Particle Model of Matter

Vocabulary flashcards covering the Kinetic Particle Model of Matter, including states of matter, gas laws, and thermal properties.

Solid (Particle Arrangement)

Particles are tightly packaged, usually in a regular pattern, and vibrate in fixed positions.

Liquid (Particle Arrangement)

Particles are close together with no regular pattern and can slide past one another.

Gas (Particle Arrangement)

Particles are well separated with no regular pattern and move freely at high speeds.

Solids (Macroscopic Properties)

Maintain a fixed shape and fixed volume because they are not fluid and have no compressibility.

Liquids (Macroscopic Properties)

Take the shape of their container but maintain a fixed volume with almost negligible compressibility.

Gases (Macroscopic Properties)

Take the shape of their container and expand to fill it, being highly compressible.

Changes of State

A reversible physical change where the number of molecules and mass remain the same, but the energy of the substance changes.

Intermolecular Forces

Forces between particles that determine the state of matter by affecting the relative distances and motion of particles.

Intermolecular Forces in Solids

Very strong forces that hold molecules in place, resulting in a rigid shape and fixed volume.

Intermolecular Forces in Liquids

Moderately strong forces that keep molecules close together while allowing them enough energy to slide past each other.

Intermolecular Forces in Gases

Very weak or negligible forces that molecules have overcome, allowing them to move randomly at high speeds.

Types of Particles in Matter

The small units that make up matter, including atoms, molecules, ions, and electrons.

Brownian Motion

The random, erratic movement of microscopic particles (like pollen or smoke) caused by collisions with smaller, unseen atoms or molecules.

Temperature

A measure of the average kinetic energy of the individual particles in an object.

Absolute Zero

The lowest possible temperature, $-273\,^{\circ}\text{C}$ or $0\,\text{K}$, where particles have the least amount of kinetic energy.

Kelvin Scale

An absolute temperature scale starting at $0\,\text{K}$ where temperatures are calculated using the formula $T\,\text{K} = \theta\,^{\circ}\text{C} + 273$.

Gas Pressure

The force per unit area caused by gas molecules colliding with the walls of their container.

Pressure Law

States that for a fixed mass of gas at constant volume, the pressure and temperature are directly proportional.

Boyle's Law

States that for a fixed mass of gas at constant temperature, pressure and volume are inversely proportional ($p \propto \frac{1}{V}$).

Boyle's Law Equation (Extended)

The mathematical relationship for a gas at constant temperature: $p_1V_1 = p_2V_2$ or $pV = \text{constant}$.