1. SOLID
1.1. Have a definite shape and volume.
1.2. The atoms are closely arranged and in fixed positions.
1.3. Crystalline solids - Atoms/molecules that are arranged in a repeating, orderly, geometric pattern.
1.3.1. Include diamonds, rubies, emeralds, quartz, and salts.
1.3.2. The type of crystal is based on geometric patterns (crystal lattices).
1.3.2.1. The types of crystal systems: Cubic, Hexagonal, Orthorhombic, Monoclinic, Tetragonal, Triclinic, and Trigonal.
1.4. Amorphous solids - atoms/molecules that are randomly arranged. Can be melted and cooled in a mold to make a specific shape.
1.4.1. AMORPHOUS- (“a” means “without”; “Morph” means “shape”.)
1.4.2. Amorphous Solids include glass, lava, and plastics, molten steel.
1.5. Characteristics include definite melting point, high density & incompressibility, and low rate of diffusion.
1.6. Categories of solids based on Intermolecular Forces: Ionic crystals, Covalent Network crystals, Metallic crystals, and Covalent molecular crystals.
2. LIQUID
2.1. Definite volume but no definite shape.
2.2. Least common of all states of matter.
2.3. Narrow range of temperatures and pressures at which they can exist.
2.4. Can flow and take the shape of its container.
2.5. Relatively high density.
2.6. Relative incompressibility.
2.6.1. Ex. Under 1000 atm of pressure, water compresses 4%
2.7. Ability to diffuse: particles are in constant, random motion; much slower than gases
2.8. Surface tension: caused by the pull of water molecules to each other (intermolecular forces) resulting in a decrease in surface area; produces a “film-like” effect on the surface, as well as making drops of liquid round.
2.9. Capillary action is also caused by surface tension: When liquids are attracted to each other AND the container they are in, which causes liquids to move against gravity.
2.9.1. Ex. Water up a tree Xylem
3. KMT
3.1. The “states” of matter are defined by the kinetic (moving) ability of the composing atoms. All atoms/molecules move to some degree at the molecular level.
3.2. Colder or heavier atoms/molecules move slower.
3.3. Warmer or lighter atoms/molecules move faster.
3.4. All movement (Kinetic Energy) is directly related to temperature and mass.
3.5. When applying KMT to a state of matter, use expansion, fluidity, density, compressibility, diffusion, and effusion.
3.5.1. Expansion- Can the atoms/molecules “expand” their given “space”.
3.5.2. Fluidity- The attractive forces between atoms/molecules and the ease of movement past one another.
3.5.3. Density- How close are the atoms/molecules to each other?
3.5.4. Compressibility- Can the atoms/molecules be moved closer to each other?
3.5.5. Diffusion- The ability of atoms/molecules to ‘mix’ together over time.
3.5.6. Effusion- The ability of a gas to move through a tiny pore/hole in another substance.
4. PHASE CHANGES
4.1. Sublimation (solid to gas): Absorbs heat
4.2. Melting (solid to liquid): Absorbs heat
4.3. Vaporization (liquid to gas): Absorbs heat
4.4. Deposition (gas to solid): Releases heat
4.5. Freezing (liquid to solid): Releases heat
4.6. Condensation (gas to liquid): Releases heat
4.7. Boiling and Evaporation require different levels of heat
4.8. Phase Diagram – a graph of Pressure vs. Temperature that shows the conditions under which that state of matter can exist.
4.8.1. X-axis: Independent Variable
4.8.2. Y-axis: Dependant Variable
4.9. If two (or three) states of matter are at an equilibrium of 1 ATM, that means Each state has equal amounts of heat within its atoms/molecules.
5. GASES
5.1. Composed of individual, free-moving atoms/molecules, with each one possessing large amounts of Kinetic Energy(KE).
5.2. Has no defined shape or volume.
5.3. The particles are in constant random motion.
5.4. Gases fill the container they are in (expansion), taking the shape of the container.
5.5. Most of the space in a container of gas is empty space.
5.6. Ideal Gases - hypothetical; Do not exist
5.6.1. An ideal gas is a hypothetical gas that perfectly fits all the assumptions of the Kinetic Molecular Theory.