States of Matter. Solids Liquids Gases

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1 States of Matter Solids Liquids Gases 1

2 Solid vs. Liquid vs. Gas Depends on only two things: What? Attractions Kinetic between particles vs Energy of particles 2

3 Intermolecular Forces (Molecular Attractions) Covalent molecules are attracted to each other by intermolecular forces. 3

4 Intermolecular Forces (Molecular Attractions) are what stick one molecule to other molecules (not the bonds within one molecule) are responsible for the solid and liquid states for molecules 4

5 3 Types: Intermolecular Forces (Molecular Attractions) Dipole-dipole force (dipole force) Dispersion force van der Waals forces Hydrogen bond force (a special dipole force) 5

6 1. Dipole-Dipole Force Electrostatic attraction of polar molecules For example: HF and H 2 O 6

7 Dipole-Dipole Buret with water charged rod (+) (-) (-) 7

8 Review: Polar Molecules A molecule with only two atoms is polar if the atoms have different electronegativities. H-Cl polar Br-Br nonpolar 8

9 Review: Polar Molecules If more than 2 atoms in molecule: Draw dot structure If outside atoms are the same and central atom has no nonbonding electrons, the molecule is nonpolar. 9

10 Are These Polar (do they have a dipole force)? CH 4 CH 3 Cl H 2 SO 2 NH 3 NaCl 10

11 2. Dispersion Force All molecules have instantaneous polarity due to the random motion of the e - around the nucleus

12 2. Dispersion Force Attractive force resulting from the temporary dipoles Responsible for condensation of nonpolar gases Is stronger the larger the molecule (molar mass) 12

13 The States of Halogens All are nonpolar and have only dispersion forces. At room temperature: F 2 and Cl 2 :gases Br 2 : liquid. I 2 : solid. Increased molar mass so larger dispersion force 13

14 3. Hydrogen Bond Force A strong dipole-dipole attraction between molecules when hydrogen is bonded to N, O, or F F H H-bond force F H Why? d- d+ strong d- d+ strong 14

15 Hydrogen Bond H H H O H O electronegative F, O, or N atom H-bond from H to lone pair on O H atom on different molecule 15

16 Strength of Molecular Attractions 1. Dispersion Force (weakest unless molecule is large) 2. Dipole Force 3. H-Bond Force (strongest) 16

17 Name the Type of Molecular Attractions N 2 NH 3 CH 4 H 2 O HCl SO 2 17

18 Gases (KE >> attractions) Kinetic Molecular Theory 18

19 Gases: KMT 1.Gas particles (atoms or molecules) are: Hard spheres Insignificant volume (compared to container) Far apart 19

20 Gases: KMT 2. Gas particles are in constant motion Random motion Straight line paths until collision Fill container 20

21 Gases: KMT 3. Gas particles have no attractive forces between them. (not 100% true!) 21

22 Gases: KMT 4. Collisions are perfectly elastic no energy lost during collisions 22

23 Gas Mostly Empty Space Compare volumes in liters of: 1 mole water vapor (gas) 22.4 L vs. 1 mole liquid water L Gas is >1000 times volume of liquid 23

24 Gas Speed Speed of O 2 at 20 o C is ~1660 km/hr. WOW!!! Why don t you smell perfume as soon as someone enters a room? 24

25 What keeps the walls of an inflated balloon pushed out? 25

26 Gas Pressure Pressure = force /area Gas molecules exert pressure on the walls of a container due to collisions. More molecules more pressure 26

27 Vacuum If there are no gas molecules, pressure is zero. 27

28 What Will Happen? water plastic sheet 28

29 Atmospheric Pressure Collision of air molecules with objects results in atm. pressure atm = ave. pressure at sea level 29

30 Atmospheric Pressure Is pressure higher or lower than 1 atm on top of Mt. Everest? 30

31 Measuring Pressure Vacuum 760 mm Hg atm P 31

32 Measuring Pressure 1 atm = 760 mm Hg = kpa What is pressure in atm. and kpa during a hurricane if P = 720 mm Hg? (Table A) 32

33 Gas Temperature What happens when a gas is heated? Molecules speed up Average kinetic energy (energy of motion) increases. Temperature (K) increases 33

34 % molecules Kinetic Energy Distribution 100% NO!!! low T (K) high T (K) kinetic energy 34

35 Liquids A condensed state of matter. 35

36 Liquids similar Kinetic Energy of particles vs Attractions between particles 36

37 Molecules in Liquid in constant motion not much affected by pressure touching held together by intermolecular forces can glide past each other (flow) 37

38 Evaporation What happens to a glass of water left overnight? Not magic! 38

39 % molecules Evaporation Energy to break intermolecular forces kinetic energy 39

40 Evaporation After some liquid evaporates, the remaining liquid is cooler. Why? The liquid warms again. Why? Then more evaporates. 40

41 Evaporation in Closed Container Vapor pressure: Pressure due to evap. gas in closed container. open closed Depends on 2 things Attractions between particles vs Kinetic Energy of particles 41

42 Dynamic Equilibrium (closed container) evaporation Liquid Vapor (gas) condensation At equilibrium: rate evap. = rate cond. 42

43 Vapor Pressure As T increases, vapor pressure increases (more KE) 43

44 Table H: Vapor Pressure VP depends only on: substance temperature 44

45 Vapor Pressure Using Regents Table H: What is VP of ethanol at 60 o C? At what T does VP of water equal 50 kpa? Which substance has greater molecular attractions: ethanol or water? 45

46 Boiling Point (BP) normal boiling point (BP at 1 atm.) The temperature at which vapor pressure equals external pressure. 46

47 Boiling Add heat energy to overcome molecular attractions (T doesn t change!) How do you know when something is boiling? What s in the bubble? What s P in bubble? 47

48 Table H is also BP vs. Pressure! What is Boiling Point of H 2 O: in Endwell where P = 1.0 atm? in Denver where P = 86 kpa? on Mt. Everest where P = 35 kpa? 48

49 Boiling Point Would it take longer or shorter time to boil at egg in Denver than in Endwell? 49

50 50

51 Solids Particles arranged in regular, repeating pattern called crystal lattice. 51

52 Comparison of K.E. to Molecular Attractions Gas: KE >> I.M. forces Liquid: KE ~ I.M. forces Solids: KE << I.M. forces (only vibrations are possible) 52

53 Solid Melting melting freezing Liquid Ionic compounds: high M.P. NaCl: 801 o C Break ionic bond Na + Cl - Molecular compounds: low M.P. HCl: -112 o C Break IM force HCl HCl 53

54 Allotropes Different forms of the same state of an element or compound. Example: carbon diamond graphite bucky-ball 54

55 Other examples: Allotropes O 2 and O 3 Sulfur Red & white phosphorous 55

56 Amorphous Solids Solids with no crystal structure Examples: plastic & rubber asphalt glass 56

57 Pressure (atm) Phase Diagram for H 2 O Normal M.P. Normal B.P. 1 solid liquid vapor Triple point Temperature ( o C) 57

58 Sublimation Substance passes from solid directly to vapor. See phase diagram below Triple Point. examples: dry ice (CO 2 ) iodine (I 2 ) (demo) 58

59 59

60 Lab 12 Analysis CuCl 2 + Fe Cu + FeCl 2 vs. 3CuCl 2 + 2Fe 3Cu + 2FeCl 3 DATA TABLE Mass empty dry beaker Mass iron nails (before rxn) Mass iron nails (after rxn) Mass beaker & dry product 60

61 Warm-up What is an intermolecular force? List the three types of IM forces 61

62 Warm-up List the three types of molecular attractions. What causes the dispersion force? Which molecules have this force? 62

63 Warm-up Predict the shape of PCl 3. Is it polar? What forces hold molecules of PCl 3 together? What are the 4 assumptions of KMT? 63

64 Warm-up Predict the shape of SCl 2. Is it polar? What forces hold molecules of SCl 2 together in the liquid state? What is meant by kinetic energy distribution? What is pressure? What is vapor pressure? What is VP of H 2 O at 80 o C? At 100 o C? 64

65 Warm-up Predict the shape of SCl 2.Is it polar? What forces hold molecules of SCl 2 together in the liquid state? What is pressure? Use KMT to explain why a balloon gets smaller when cold. 65

66 Warm-up What is STP? What molecular attractions hold ammonia molecules (NH 3 ) together? What temp. will water boil at if P = 620 mm Hg? How can liquid water in underground geysers be hotter than 100 o C? What is meant by kinetic energy distribution? 66

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