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 LawRatea = √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 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: