UNIT 3 States of Matter

1. UNIT 3States of Matter Solids Liquids Gases

2. C4.3 B Describing three states of matter... Solid - definite shape and volume Liquid - definite volume, changes shape Gas - changes shape and volume

4. Kinetic Molecular Theory • All matter is made up of small particles. • Which are . . . . • All of the particles are in constant motion. • Kinetic Energy = KE = ½ mv2 • Collision between particles are perfectly elastic (no energy is lost to the surroundings).

5. C2.2B Three types of particle motion • Vibrational - moves around fixed point • solids, liquids, gases • Translational - particles freely move past one another • liquids, gases • Rotational- rotates around fixed axis • gases

6. Solids • Amorphous • a random arrangement of the particles with no repeating pattern. • No set melting point • Example: Glass, rubber, chocolate

7. Crystalline • Crystalline • a regular arrangement of the particles with some kind of repeating pattern producing a crystal. • Known melting point • Crystal shapes are classified according to their shapes into 7 systems

8. Crystal Structures (pg 281) • Cubic • Tetragonal • Orthorhombic • Monoclinic • Triclinic • Hexagonal • Rhombohedral

9. Diamonds • Cubic Crystal Structure • The hardest of all known minerals, can only be scratched by another diamond.

10. The 4 C’s of Diamonds • Cut • Color • Clarity • Carat • NOTICE – COST IS NOT A “C”

11. Cut • The brilliance is dependent on the proportions and symmetry of the cut. • Round, princess, etc… • Rated with - Excellent, Very Good, …

12. Color • Usually colorless, but can occur in all colors. • DEF (Colorless) • All the way to Z (yellow)

13. Carat (not karat) • One carat equal 0.2 grams • Measured to 0.001 carat and rounded to 0.01 carats

14. Clarity • Fl (Flawless, no blemish under 10x) • V V S1 and V V S2 • VS1 and VS2 • SI1 and SI2 • I1,I2, I3 (obvious blemishes)

15. History of Engagement Ring • Became popular in 1477 • Archduke Maximillian of Hamburg and Mary of Burgandy • De Beers Consolidate Mines, Ltd 1888 was created to protect the investment of diamond mine investors from new mine found in S. Africa 1870. • This flooded the market and by 1919 sales declined by 50% • Ad campaign of 1939 made diamond ring of choice

16. World’s Largest/ Famous Diamonds • Cullinan I – known as the Star of Africa • Largest cut diamond at 530 carats, found in Tower of London as part of the crown jewels

18. The Blue Hope Diamond • owned by Louis XIV • Stolen in French revolution and reappeared in 1830 • Bought by Henry Phillip Hope of London • Cursed- two of the owner had their entire families die just one year apart • Found in Smithsonian

19. Colored Diamonds • Colored Diamonds are a result of impurities

20. Life Gems • Making diamonds from loved ones • Your loved one’s ashes under extreme temperature and pressure can be changed into a colored diamonds pendant or ring

21. Carbon… • Allotropes (draw or describe each) • graphite • diamonds • buckeyball

22. Graphite

23. Diamonds

24. Buckyballs

25. Conduction • Transfer of heat between substances that are in direct contact with each other.

26. Good conductors? • Poor conductors?

27. Convection • Up and downward movement of gases and liquid caused by heat transfer

28. Radiation • Electromagnetic waves come in contact with an object and the waves transfer heat

29. Pressure • The ratio of force per unit area. • Standard Pressure is defined as air pressure at sea level. • As altitude increases, pressure decreases

30. Barometer

31. Standard Pressures • Pressure at Sea Level in 7 different units • 14.7 Psi • 30.00 inches Hg • 760 mm Hg • 760 torr • 1.00 atmospheres (atm) • 1013 Millibars • 101.3 kilopascals (kPa)

32. Standard Pressure Uses • psi – tire pressure/ paint ball • inches Hg – US weather reports • mm Hg- same as torr - medical • Normal blood pressure is 110 to 150 mmHg when heart beats and 60 to 80 mmHg when heart relaxes • Torr – another name for mmHg (named after scientists Torricelli)

33. More pressures • mb – meteorologist • kPa– pascals is SI unit • atm – pressure at earth’s surface (1 atm)

34. Temperature • The hotness or coldness of an object corresponding to its molecular activity • A measure of the average kinetic energy of the particles in an object.

35. Temperature Effects • As temp increases, average KE (kinetic energy) increases • As temp decrease, average KE decreases

36. How low can you go? • Absolute Zero • Particles have zero KE • All particle motion stops • 0 Kelvin = -273.15 Celsius

37. Record Low Temperatures • Prospect Creek, Alaska • Jan. 23, 1971 -80ºF • Rogers Pass, Montana • Jan. 20, 1954, -70 F • Michigan • Feb 9, 1934, -51 F What is the only state to never have a below zero temperature? (Hawaii, 12 F is lowest)

38. Record High Temperatures • Death Valley, California • July 10, 1913, 134 F • Michigan • July 13, 1936, 112 F

39. Temperature scales • K F C • 0 K • -40 °C/ -40 °F

40. Converting Temperature • K = C + 273 • F = (1.80*C) + 32 • Solve this equation for C.

41. Try these... • 3 °C to F • 432 K to °C • 212 F to K • 25.7 psi to mmHg • 1.5 atm to kPa • 2000 mbar to torr

43. C4.3A

44. C5.4A Changes of State involving Solids • Solid  Liquid • Melting • Examples- other than water • Solid  Vapor (gas) • Sublimation • Example: dry ice, air fresheners, freeze dried food

47. Behavior of Liquids • Viscosity : the measure of a liquid’s resistance to flow • Surface Tension: Inward forces that must be overcome in order to expand the surface area Cohesion: molecules sticking to each other Adhesion: forces that bind liquid to surface • Capillary Action: rise of liquid up very narrow tubes

48. Changes of State w/ Liquids • Liquid --> solid • freezing • Liquid --> gas • Vaporization • Evaporation: occurs are the surface of the liquid only • Vapor --> liquid • Condensation • Gas - - > solid ? • Deposition

49. GAS LIQUID SOLID

50. Equilibrium • equilibrium - no net change in a system (usually closed) • static - no net change because nothing is happening • dynamic - no net change because two opposite processes are occurring at the same rate