States of Matter
Solids have definite shape and definite volume Particles in a solid are packed very closely together and are in a fixed position. This is what causes solids to have a definite shape and volume.
Crystalline Solids: Particles of a crystalline solid are found in regular, repeating patterns. Melt at a specific temperature (melting point) Examples Salt, Sugar and Diamonds
Amorphous Solids Particles are not arranged in any regular pattern Do not melt at any specific temperature Examples Plastics, rubber and glass
Have a definite volume but no definite shape Liquids take on the shape of container Particles of a liquid are packed almost as tightly together as in a solid, but move around one another freely Because these particles are free to move liquids have no definite shape
Liquids are also called Fluids Fluids: a substance that flows *All liquids are fluid, but not all fluids are liquid
Properties of Liquids Surface Tension: is the result of inward pull among the molecules of a liquid. Viscosity: a liquids resistance to flow
Gas is a fluid Gas can change volume very easily As gas particles move they spread apart, filling the space available. Gases have neither definite shape nor definite volume.
Changes between Solid and Liquid How does the state of matter of a substance relate to its thermal energy? A substance changes state when its thermal energy increases or decreases sufficiently
Melting is the change of state from a solid to a liquid. Melting Point: is the specific temperature at which a substance melts. Melting point is a physical property that scientists can use to identify an unknown substance.
Change in state from a liquid to a solid At its freezing temperature, the particles of liquid are moving so slowly that they begin to form regular patterns.
Vaporization: change from a liquid to a gas Vaporization takes place when the particles in a liquid gain enough energy to form a gas. Evaporation: is vaporization that takes place only on the surface of a liquid
Boiling : vaporization that occurs below the liquids surface as well as on the surface. Boiling Point: temperature at which a liquid boils.
Boiling Point and Air Pressure The boiling point of a substance depends on the pressure of the air above it. The higher the pressure the more energy required for substance to boil; more energy equals higher boiling point
Condensation: is the opposite of vaporization -change of state from a gas to a liquid -occurs when a gas loses enough thermal energy to form a liquid
Sublimation: occurs when particles of a solid do not pass through the liquid state as they form a gas.
Measuring Gases Volume: the amount of space the gas fills. Units: cubic centimeters, milliliters, liters. Gas particles move and fill the space available in its container.
Measuring Gases Volume: the amount of space the gas fills. Units: cubic centimeters, milliliters, liters. Temperature : is the measure of …..? At room temperature particles of a gas travel about 500 m/s
Pressure: is the force of the outward push divided by the area of the walls of the container. Pressure = Force/Area The firmness of an object comes from the pressure of the gas.
Pressure and Volume What happens when you block the end of the tube on a bicycle pump and then push down on the plunger?
Boyle’s Law: relates the pressure of a gas and its volume. Boyle found that when the pressure of a gas, at constant temperature, is increased the volume of the gas decreases. When pressure is decreased, the volume increases.
Pressure and Temperature When the temperature of a gas, at constant volume, is increased, the pressure of the gas increases. When the temperature of a gas, at constant volume, is decreases, the pressure of the gas decreases.
Volume and Temperature Charles’s Law : Relates the volume with the temperature of a gas Charles found that when the temperature of a gas is increase, at constant pressure, the volume of the gas also increases. If the temperature of a gas, at constant pressure, is decreased, the volume of the gas also decreases.
Graph the data on pages 91 and 92 (figures 22 and 23)