Chapter 13.3 The Nature of Solids

Particles of a Solid are…. 1.orderly arranged 2.attracted to each other 3.tightly packed 4.The densest state 5.in a fixed location 6.melting at the Melting Point solids to liquids

The Melting Point is a Temperature…. where a solid has enough kinetic energy for particles to break out of their organization where solid melts, called Fusion that stays constant until the last piece of solid is melted That is very specific for each substance Ex: Ice: 0 o C, gold: 1060 o C

Freezing Point Same temperature as melting point Reverse process than melting Loss of temperature Loss of kinetic energy substances solidify many form a crystal lattice

Phases of substances Ammonia (NH3) MP = o C BP = o C Draw a temperature scale indicating when ammonia is present as a solid, liquid, gas

Crystals Most solids are arranged in a crystal lattice Precise geometrical shapes with defined angles

Allotropes Solids that can exist in more than one crystal form Example: Carbon atoms can be arranged to form either a diamond or graphite

Non crystalline solids Amorphous solids are mixtures of compounds like rubber, asphalt, glass that don’t have a defined melting/boiling point Glass: Softens gradually has different stages of viscosity