What are Solids, Liquids, and Gases? Chapter 13 States of Matter

Kinetic Molecular Theory (KMT) “all matter is in constant, random motion” Gases- particles move freely and independently of one another Liquids- particles are attracted to one another, but are still able to slide past each other Solids- particles are strongly attracted to each other and shake in place

Gases and KMT Individual gas particles are super tiny and hold no actual volume Particles move in straight lines until they collide Collisions are elastic- no kinetic energy is lost

Gas Behavior Compression- gases can be compressed because they have very LOW DENSITY Expansion- gases will fill any size container because the particles are not held together

Graham’s Law Diffusion- movement of one material through another Effusion- gas particles escaping through tiny holes in the container Graham’s Law Ratea = √molar massb Rateb √molar massa

Gases and Pressure Pressure- force per unit area Gases cause pressure by colliding with the walls of their container Barometer-measures atmospheric pressure Manometer-measures vapor pressure Dalton’s Law: Ptotal=P1+ P2+P3+...

Units of Pressure 1 atmosphere= normal atmospheric pressure 1atm = 760 mmHg = 14.7 psi = 101,325 Pascals = 101.325 KPa 1.5 atm = ? mmHg 804 mmHg = ? psi

Assignment P. 388-392 # 1-12 Show all mathematical work Answer in full sentences

Intermolecular Forces Intermolecular Forces- the forces that exist between particles of a substance 3 Types (in order of INCREASING strength) Dispersion- caused by electron movement Dipole- caused by polar attractions Hydrogen Bonds- caused by hydrogen and N,O,F

Particle Spacing How do solids, liquids, and gases compare?

Liquid Behavior Density- much denser than gases, not compressible Fluidity- diffuse slower than gases, still “flow” Viscosity- measure of resistance to flow Effect of temperature- higher temp, lower viscosity

Liquid Behavior Surface Tension Capillary Action Causes drops and meniscus Capillary Action Water can climb narrow tubes

Solid Behavior Density- more dense than gases and liquids and incompressible Crystalline Solids Unit Cells Crystal Structure

Solid Behavior Molecular Solids-dispersion, dipole, or H-bonds (ex: sugar) Covalent Network Solids- covalent bonds with self (ex: diamond) Ionic Solids- ionic attraction (ex: salt) Metallic Solids- mobile electrons (ex: copper) Amorphous Solids- irregular pattern (ex: glass)

Assignment P. 395 # 13-16 P. 403 # 17-23 Full sentences

Phase Changes

Heating Curve

Endothermic Phase Changes Melting- solid absorbs energy until particles have enough speed to break free of IM forces holding them in place Vaporization-liquid absorbs energy until particles have enough speed to break free of IM forces holding them close together

Liquid to Gas Evaporation- occurs at surface Boiling- occurs throughout when vapor pressure equals atmospheric pressure

Sublimation-solid to gas

Exothermic Phase Changes Condensation Deposition Freezing

Phase Diagrams

Assignment P. 409 # 24-28 Yes, sentences please P. 4 in packet

Test Review Assignment due the day before the test Test: