States of Matter

Kinetic Theory Definition: How particles in matter behave All Matter is composed of small particles. Particles are in constant random motion. Particles collide with each other and walls of their containers

Thermal Energy Kinetic Energy Definition: Total energy of a material’s particles; causes particles to vibrate in place. Kinetic Energy Definition: Temperature of the substance, or how fast the particles are moving. - Lower Temperature: Slower Motion

Four States of Matter Solid Liquid Gas Plasma Energy Level?

Solid Has a stable, definite shape Has a definite volume Particles are packed closely together Cannot move freely, can only vibrate Energy and temperature are very low Can only change their shape by force

Liquid Does not have a definite shape Shape is determined by the container in which it is held Volume is definite Particles are farther apart than in solids, and can slide past each other easily Energy and temperature, in comparison to a solid, are higher

Gas Has an indefinite, unstable shape Volume is determined by the container that is closely sealed Particles are far apart from each other, and can move around quickly Energy and temperature are the higher than those of both solids and liquids Gas

High Temperature gas with balanced positively and negatively charged particles. Made up the most state in the universe Examples: Fluorescent light, lightning, stars Plasma 8

How particles behave….

Changes of State/Phase

Phase Changes Original State New State Names of Change Solid Liquid Melting Freezing Gas Evaporation Condensation Sublimation

Physical Change Change that alters the substance without changing its chemical composition Breaking, Bending, Cutting Can be a reversible process Examples: Dissolving salt in water; Denting a car bumper; water to ice or vapor; Glass break Ice cream melts

Chemical Change Occurs when one or more substance change into one or more new substance Energy is released (exothermic) or absorbed (endothermic) Indicator: Change in color and odor Examples: Burning candle, Cooking Melting sugar Metal Rust Food Disgetion Photosynthesis

FLUID Definition: A substance that can flow and take the shape of the container in which it is held. Examples: Liquids and Gases.

Liquid vs Gas Example /Property Liquid Gas Water Air Shape No definite shape Volume No definite volume Particles Arrangement Close Far apart Energy binding particles Strong Weak

Properties of Fluid Density Pressure Buoyancy Viscosity

Density Mass (g or kg) Volume (liter, c.c. (cm3)) Definition: A measure of the mass of a substance per unit volume: Does not dependent on size. Density of a substance change as its phase change. Usually solid being denser. Mass (g or kg) Volume (liter, c.c. (cm3))

Pressure Force (N) Area (cm2, m2) Definition: Force exerted on a unit area of a substance. Pressure changes Gas density, but NOT Liquids. Thus, density can be used to identify a liquids (e.g. fancy drinks in layers) SI Unit: Pascal (Pa) Force (N) Area (cm2, m2)

Pressure Pascal’s principle – pressure applied to a fluid is transmitted throughout the fluid. Example: hydraulic machines.

Buoyancy Definition: the ability of a fluid to exert an upward force on an object that is immersed in it. Float - Weight of object < Buoyant Force - Density of object < Density of water Sink – Weight of object > Buoyant Force

Buoyancy How does an aircraft carrier made of steel (heavier than water) can stay afloat in the sea? Clues: Density and Pressure

Viscosity Definition: A liquid’s resistance to flow Determined by molecular structure Increased temperature will lower viscosity.

Behavior of Gases Pressure Boyle’s Law Charles’s Law Gay-Lussac’s Law

Pressure Measured in units called pascal (Pa) Collisions of particles in air result in atmospheric pressure.

Boyle’s Law Relates to pressure and volume Volume decreases as pressure increases. Pressure multiplied by volume is always equal to a constant if the temperature is constant.

Charles’s Law Relates to volume and temperature At a constant pressure, volume increases as temperature increases. At a constant pressure, volume decreases as temperature decreases.

Gay-Lussac’s Law Relates pressure and temperature; at a constant volume, as temperature increases, pressure increases.