what are solids, liquids, and gases? chapter 13 states of matter
TRANSCRIPT
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: