Phases of Matter Overview Solid, liquid, gas (vapor) properties Molecular motion vs. phase Gases and pressure Liquids, evaporation, boiling Solids, melting

Properties of the different phases 1-1. In your group, list the different physical properties of Solids Liquids Gases or vapors

Solids Fixed volume and shape Heating  melting Powders vs. chunk of something Crystals

Liquids Fixed volume, but adopt shape of container “Wet”, pourable Heating  vaporization (boiling) Cooling  freezing

Gases or Vapors No fixed volume or shape, assume shape and volume of container Cooling  condensation

What is the difference at the molecular level? Molecules are always in motion: kinetic energy Molecules are attracted to each other (intermolecular forces) Amount of motion related to substance and temperature Solid Atoms/molecules very close to each other in crystal lattice Fixed positions relative to each other Molecular motion: vibrational only

Crystal Lattice—NaCl

Crystal Lattice

Crystal lattice of molecular solid

Water crystal lattice

Energy and Molecules Energy and phases of matter Molecules are always in motion: kinetic energy Amount of motion related to temperature Solid: crystal lattice, molecular motion is predominantly vibrational Liquid: molecules in close proximity, molecular motion is vibrational, rotational, translational

Liquids Rotational motion: molecules can rotate in space (spinning) Translational motion: molecules move relative to each other

Liquids Molecules are close together (attractive forces) but have a lot of freedom of movement. Gives rise to macroscopic properties associated with liquids: Can pour a liquid, Adopts shape of container Viscosity: resistance to flow

Energy and Molecules Energy and phases of matter Molecules are always in motion: kinetic energy Amount of motion related to temperature Solid: crystal lattice, molecular motion is predominantly vibrational Liquid: molecules in close proximity, molecular motion is vibrational, rotational, translational Gas: molecules widely separated, translational motion predominates

Gas or Vapor Phase Molecules are far apart; no intermolecular forces Molecules move independently of each other, shape and volume of container Translational motion predominates Elastic collisions w/ other gas molecules and with container walls Collisions with container walls gives rise to “pressure”

Phase Changes Molecular motion (Kinetic Energy, KE) increases with temperature: KE  Tabs (Kelvin scale) KE = ½ mv2 m = mass, v = velocity (Kinetic Molecular Theory)

Phase Changes: Solid  Liquid Solid: vibrational motion increases with temperature until energy overcomes intermolecular forces to some extent. Lattice collapses but molecules still in close proximity. More molecular motion possible (rotational, translational) Liquid ensues MELTING

Phase Changes: Liquid  Gas Liquid: motion (vibrational, rotational, translational) increases with temperature. Molecules eventually have enough kinetic energy to completely overcome intermolecular forces. Molecule escape into gas phase. VAPORIZATION

Phase Changes: Gas  Liquid Vapor: motion (translational) decreases with decreasing temperature. Molecules eventually do not have enough kinetic energy to overcome intermolecular forces; stick together on collisions. Molecules cluster and form droplets of liquid. CONDENSATION (precipitation)

Phase Changes: Liquid  Solid Liquid: motion (vibrational, rotational, translational) decreases with decreasing temperature. Molecules stick together more and more as substance is cooled. Eventually form small crystal lattices (seed crystals, nucleation) which grow. FREEZING

Other Phase Changes Solid  Vapor: sublimation (low temperature, low pressure) “dry” ice, frozen CO2 snow disappearing below freezing temps Vapor  Solid: deposition (low temperature, low pressure) frost

Phase Changes gas liquid solid vaporization condensation sublimation deposition Energy of system liquid freezing melting solid

Heating Curve Water vapor Liquid water & vapor (vaporization) 100 Temperature, ºC Liquid water 75 50 25 Ice & liquid water melting –25 ice Heat added (kJ)

Properties of Gases (Gas Laws) Pressure and Temperature are directly proportional Pressure and volume are inversely proportional Volume and temperature are directly proportional (video) Volume and amount of a gas are directly proportional What is happening at the molecular level?

Pressure (P) and Temperature (T) Pressure results from collisions of molecules w/ container walls. As temperature (T) , molecules move faster (more KE), more collisions, P  T  then P  T  then P  Directly proportional Assumes constant volume

Pressure (P) and Volume (V) Pressure results from collisions of molecules w/ container walls. As Volume (V) , number of collisions decreases, P  V  then P  V  then P  Inversely proportional Assumes constant temperature

Volume (V) and Temperature (T) As T increases, molecules move faster. To maintain same pressure, number of collisions must remain the same, thus V increases T  then V  T  then V  Directly proportional Assumes constant pressure

Volume (V) and Number of molecules Two samples of gas at the same P, T, and V: same number of collisions same number of molecules

Properties of Gases Explain each of the following: Balloons hung outside in the sunshine pop. A hot air balloon rises up in the air. Collapsing can. Balloon in liquid nitrogen (video). Your water bottle shrinks when you fly to Dallas. How you pull liquid up in a straw. How a siphon works.

Gas Laws—Quantitative Pressure and Temperature are directly proportional: P = C1 x T Pressure and volume are inversely proportional: Volume and Temperature are directly proportional: V = C3 x T Volume and amount are directly proportional: V = C4 x n

Gas Laws—Quantitative V = C3 x T V = C4 x n P = C1 x T P x V = n x R x T Ideal Gas Equation (Law)

Molecular Effusion and Diffusion ACTIVITY: smelly balloons perfume

Molecular Effusion and Diffusion perfume

Molecular Effusion and Diffusion perfume

Molecular Effusion and Diffusion perfume

Molecular Effusion and Diffusion Effusion & Diffusion are dependent upon: Temperature (hotter = faster) Molecular Size (bigger = slower)

Properties of Liquids Intermolecular attractive forces (IMAF) Forces between molecules “Like dissolves like.”  similar IMAF Stronger forces Larger molecules Polar molecules (like water)

Properties of Liquids Viscosity: resistance to flow Surface Tension As IMAF  viscosity  Viscosity  as T  Surface Tension Surface effect of stronger IMAF As IMAF  surface tension  Surface tension  as T  Surfactants

Vapor Pressure Vapor pressure: the pressure exerted by the vapor above a liquid when the liquid and the vapor are in dynamic equilibrium VERY difficult conceptually for students

Vapor Pressure Pvap Dynamic equilibrium: molecules  vapor = molecules  liquid Molecules escape into vapor phase

Vapor Pressure Pvap  as T  When Pvap = Patm: “boiling” Bubbles of gas in liquid

Explain the following… How a pressure cooker works. Why it takes longer to cook rice or pasta at high altitude. How we were able to boil water with ice.

Heating Curve Water vapor Liquid water & vapor (vaporization) 100 Temperature, ºC Liquid water 75 50 25 Ice & liquid water melting –25 ice Heat added (kJ)

Phase Diagrams Melting Freezing solid Critical point liquid Pressure Vaporization Condensation Pressure Sublimation Deposition gas Triple point Temperature

Phase Diagrams solid liquid 1 atm Pressure gas Temperature Normal melting point Normal boiling point

Phase Diagrams solid liquid Pressure CO2 1 atm gas Temperature

Phase Diagrams H2O solid liquid 1 atm gas Pressure Temperature