States of Matter Glue the following table in your science notebooks Complete the table as the slides progress. Solid Liquid Gas Plasma

Definite Shape

Definite Volume

Structure

Particle Kinetic Energy

Other Info Four States (Phases) of Matter Solid State

• The particles of a solid are packed closely together and constantly vibrating in place.

• The attractions between particles are strong, and solids have a fixed volume and shape. Liquid State

• The attractive forces are strong enough to cause particles to cling together.

• Liquids have a definite volume, but not a definite shape. Gas State

• In a gas, the forces between particles are so weak that the particles no longer cling together.

• Gases do not have a definite shape or volume. Plasma State

• The most common state of matter in the universe is the plasma state.

• Plasma is matter consisting of positively and negatively charged particles and does not have a definite shape or volume. Changing States

Melting

• The temperature at which a solid begins to melt is its melting point.

• The amount of energy required to change 1 kg of a substance from a solid to a liquid at its melting point is known as the heat of fusion. Freezing

• The heat of fusion is also the energy released when a liquid freezes.

• The attractive forces are strong enough that the particles form an ordered arrangement. Vaporization

• Vaporization occurs as a liquid changes into a gas. • Vaporization that occurs at the surface of a liquid is called evaporation.

• Evaporation causes the temperature of the liquid to decrease. Boiling

• The boiling point of a liquid is the temperature at which the pressure of the vapor in the liquid is equal to the external pressure acting on its surface.

• The heat of vaporization is the amount of energy required for 1 kg of the liquid, at its boiling point, to become a gas. Condensation • The heat of vaporization is also the amount of energy released during condensation.

Heating Curve for Water • This graph E 3500 n e 3000 shows the r g 2500 temperature y Heat of Vaporization --- J 2000 change of water o u 1500 l as thermal e 1000 s energy is added. 500 <---Heat of Fusion 0 -50 0 50 100 150

Temperature (° C ) Condensation • The average kinetic energy of the water molecules doesn’t change.

Heating Curve for Water

E 3500 n e 3000 r g • The temperature 2500 y Heat of Vaporization --- J remains constant 2000 o u during melting. l 1500 e s 1000

500 <---Heat of Fusion 0 -50 0 50 100 150

Temperature (° C ) Condensation

• After the liquid water Heating Curve for Water

E 3500 has changed n e 3000 completely into a gas, r g 2500 the temperature of y Heat of Vaporization --- J 2000 o the gas increases as u l 1500 energy is added. e (Does this graph s 1000 500 <---Heat of Fusion remind you of 0 anything?) -50 0 50 100 150 Temperature (° C ) Thermal Expansion The Thermal Expansion of Matter

• The increased separation between the particles results in the expansion of the object, and the size of the object increases.

• When a material cools, the particles in the material move more slowly and become closer together. Thermal Expansion of Liquids

• The forces between the particles in liquids are weaker than the forces between the particles in a solid.

• The same temperature increase usually causes liquids to expand much more than solids. Thermal Expansion of Gases

• In a gas, the forces between particles are much weaker than they are in liquids.

• Gases expand even more than liquids for the same increase in temperature.