1 / 56

Unit 10 - Gases, Liquids and Solids

Unit 10 - Gases, Liquids and Solids. General Properties : I. Gases: 1. Expansion 2. Compressible 3. Fluid 4. Low density 5. Diffusion 6. Effusion. 7. Condense to liquid 8. No definite shape 9. No definite volume 10. Change volume with Temperature

ursula
Télécharger la présentation

Unit 10 - Gases, Liquids and Solids

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Unit 10 - Gases, Liquids and Solids General Properties: I. Gases: 1. Expansion 2. Compressible 3. Fluid 4. Low density 5. Diffusion 6. Effusion

  2. 7. Condense to liquid 8. No definite shape 9. No definite volume 10. Change volume with Temperature 11. Change volume with Pressure 12. Deposition (to solid) Fluid: Substance that can flow and take shape of container

  3. II. Liquids: 1. Definite volume 2. Fluid 3. High density 4. Diffuse 5. Incompressible 6. Dissolve solids 7. Surface tension 8. Boil / evaporate 9. Solidify

  4. III. Solids: 1. Definite shape 2. Definite volume 3. Not fluid 4. Melt 5. High density 6. Incompressible 7. Slow diffusion 8. Sublimation (solid to gas) 9. Rigid form

  5. Diffusion: move from area of high concentration to low concentration

  6. Kinetic Properties (KMT): (Movement) I. Gases: 1. Tiny particles 2. Constant straight line motion 3. Elastic collisions 4. Little or no attraction forces 5. Average kinetic energy KE = ½ mv2

  7. II. Liquids: 1. Tiny particles 2. Constant motion (limited) 3. Elastic collisions 4. Some intermolecular attractions 5. Closely fit together

  8. III. Solids: 1. Tiny particles 2. Constant vibratory motion 3. Strong intermolecular forces 4. Rarely move position 5. Closely packed (fixed position)

  9. Examples of Gases, Liquids, and Solids Gases: elements and compounds Elements: a) monatomic gases – He, Ne, Ar, Kr, Xe, Rn b) diatomic gases – H2, N2, O2, F2, Cl2 Compounds: CO, CO2, NO, NO2, N2O, N2O3, NH3, C2H6, C3H8, SO2, SO3, AsH3 …..

  10. Liquids: elements and compounds Elements: Hg, Br Compounds: HOH, C3H2OH, C3H5(OH)3, C2H5OH, C8H18 …

  11. Solids: elements and compounds Elements: most metals (Except Hg) nonmetals P, S, I, C Compounds: NaCl, NaHCO3, CuSO4, MgSO4, AlNa(SO4)2, C6H12O6, C12H22O11…

  12. Types of Solids 1) Crystalline: crystal lattice (3-D) Shapes: unit cells – cubic, body center or face center Basic crystal systems: a) isomeric cubic d) orthorhombic b) tetragonal e) monoclinic c) trigonal f) triclinic g) hexagonal

  13. Types of Crystals • Ionic – Hard, Brittle, High melting pt. examples: NaCl, CuSO4, AgNO3 • Covalent – Soft, Low melting pt. examples: NH3, HOH, CH4 • Network - hardness vary, High MP examples: diamond, graphite, quartz • Metallic – MP range, hardness range examples: Cu, Fe, Al,…

  14. Forming Crystals: evaporation or from magma SLOW cooling: large perfect crystal Defect: flaws (mistake in crystals) a) foreign atom /ion (changes color ) b) internal misalignment (fuzzy) c) dislocation - edge - screwed Edge dislocation: extra layer of atoms extends part of the way into a crystal Screwed dislocation: unequal growth while the crystal form

  15. 2) Microcrystalline Fullerines / Buckyballs contain carbon (graphite)16–128atoms sulfur 4 – 8 atoms phosphorus 30 +/- atoms Properties: strong, durable, hollow, fluffy shapes are spheres or tubes network bonding Examples: tennis racket frames golf club shafts airplanes frame / outer covering

  16. Types of Solids: 3) Amorphous: is also called meta-stable liquids or super -cooled liquids Properties: -melting pt range -weak intermolecular forces -temperature sensitive -random molecular arrangement Examples: Glass, Rubber, Plastics, Waxes

  17. Phases

  18. Below 0oC

  19. Phase Changes I. Chart- G Evaporate/ Condense boil Deposition L Sublimation Solidify Melt S

  20. II. Graph- release energy T E M P G condense boil L solidify add energy melt S E N E R G Y

  21. III. Diagram- 4 • Melting Pt • Boiling Pt • Triple pt • 4. Critical pt P S L 1 2 1 atm G 3 Temp

  22. Terms Melting: solid to liquid (add heat) Evaporation: liquid to gas without boiling Boiling: change of liquid to bubbles of vapor that appear throughout the liquid Condensation: gas to liquid (release heat) Solidification/Freezing: liquids to solids Sublimation: solid to gas without becoming a liquid Ex: I2, CO2, paradichlorobenzene Deposition: gas to solid without passing liq.

  23. Phase Changes “ 2 phases Substance • Chart Graph depositoin Gas sublimation Solid

  24. Diagram L solid 1 atm Gas

  25. Get your thinking caps on this will be FUN!!!!!!

  26. Holy Moley!!!!!

  27. Le Chatelier & Stress I’ll start will an easy concept!

  28. Equilibrium (Le Chatelier & Stress):equilibrium will shift to ease stress Open System: evaporation and condensation hot cool

  29. Closed System: Stress Heat or Cool: HEAT COOL Explosion Implode

  30. Dynamic Equilibrium: evaporation = condensation at one specific temperature Equilibrium: Two Opposing changes occur at equal rate

  31. Boiling Point Boil at same temperature until all liquid has vaporized Vapor pressure=atmospheric pressure Boiling Point changes with Pressure and / or Altitude changes: Increase pressure, BP (pressure cooker) Decrease pressure, BP (high Mt range)

  32. BOILING and ELEVATION • DEATH VALLEY CA 100.3C • HAZLET NJ 100.0C • BOULDER CO 94.0C • LEADVILLE CO 89.0C • MT WHITNEY CA 85.0C • MT McKINLEY CA 79.0C • MT EVEREST TIBET 70.0C

  33. Water: occurance - freshwater, salt water, glaciers, groundwater • Solid: (Physical Properties) 1. Strong Hydrogen bonds 2. Rigid form 3. expands when froze 4. MP/FP is 0 oC at STP 5. D= 0.917 g/ml 6. Hf = 334 J/l

  34. Liquid: 1. colorless, odorless, tasteless, transparent 2. Universal solvent 3. most dense at 4 oC 4. D = 1 g/ml 5. FP O oC and BP 100 oC at STP 6. Csp = 4.18 J/g oC

  35. Gas: 1. separate molecules 2. low density D = 0.000148 g/L 3. BP = 100 oC 4. Hv= 2260 J/g 5. Csp = 2.02 J/g oC

  36. Water: Chemical Properties • Solid: 1. Stable at STP 2. Hydrogen bonds 3. 3 –D hexagon shape 4. angle = 105 degree

  37. Liquid 1. Stable/ wet 2. Reaction with - Active metals - metal oxide metal hydroxide (base) - Nmetal oxide Hnmetal oxide (acid) 3. promotes chemical reactions 4. group of 4 – 8 molecules 5. angle 105 degrees

  38. Vapor 1. Decomposes at very high temperatures to form hydrogen and oxygen 2. Independent molecules 3. angle 105 degrees

  39. Uses of water • Solid Cooling food preservations Ice sports Sculpting medical

  40. Liquid: Drink/ medical Bath/ wash sanitation agriculture aqua culture heating/ cooling cooking extinguish transportation

  41. Vapor: cooking/ heating ironing/ cleaning sanitizing power humidifier/ vaporizer transportation whistles

  42. Heavy Water: D2O (deuterium oxide) a) 2400 liters HOH 83 ml D2O b) more dense d= 1.2 g/cm3 c) BP 101.4 oC / MP 3.8 oC d) used as “tracer” in chem RXNs chemical and biological

  43. Used as a Standard for: 1. Temperature at sea level(thermometer) 2. Pressure (Barometer) 3. Volume (Liter) 4. Mass (Gram) 5. Density (specific gravity) 6. Heat (calorie/joule)

  44. Terms: 1. Water of crystallization: homogeneous particles bounded by surface making definite angles. The slower the crystals form, the more perfect they are. 2. Hydrated crystal: a crystallized substance containing HOH 3. Anhydrate: substance without water

  45. 4. Effervescence: rapid evolution of small gas bubbles 5. Efflorescence: hydrated crystals lose HOH when expose to the air Ex: Na2CO3.10HOH fast process CuSO4.5HOH slow process 6. Deliquence: take up water from the air Ex: NaOH fast / CaCl2 slow 7. Hydroscope: insoluble material take up water vapor from the air Ex: hair, wool, silk

  46. 8. Miscible: two liquids can dissolve freely in one another in any portion. Ex: water + isopropanol 9. Immiscible: two liquids are not soluble in each other. Ex: water + oil

  47. 10. Effuse: gas particles pass through a tiny opening 11. Viscosity: the resistance of a liquid to flow. Ex: syrup 12. Lattice: 3-D arrangement of particles of a crystal 13. Unit cell: 3-D pattern of the entire lattice (repeating pattern)

More Related