2. Intermolecular Forces of Attraction Attractive forces that cause atoms or molecules to stick together

3. Mixtures  Elements or compounds blended together but not chemically combined

4. Mixtures  Can be solid, liquid, or gaseous mixtures  Solid mixture examples:  Jewelry gold, most rocks, steel, alloys  Liquid mixture examples  Beverages, sea water, solutions  Gaseous mixture examples  Air, car exhaust

5. Mixtures  Why do they form? What allows the parts to stay mixed? Why do they stay together?  The components of a mixture are held together by IMF’s – intermolecular forces of attraction

6. Intermolecular Forces All intermolecular forces are: attractive forces attractive forces between molecules between molecules do not make new compounds do not make new compounds Makes the molecules “sticky” Makes the molecules “sticky” weaker than true “bonds” weaker than true “bonds”

7. Types of IMF’s  London (dispersion) forces  all molecules  weakest interaction  dipole-dipole forces  polar molecules  ion-dipole forces  Between polar molecules and ions  hydrogen bonding  H atoms w/ O, N, F not covalently bonded to it  strongest interaction

8. Polar forces “Dipole - Dipole” interactions “Dipole - Dipole” interactions positive ends attract negative ends of other molecules positive ends attract negative ends of other molecules about 1% as strong as a covalent bond about 1% as strong as a covalent bond

9. Dipole - Dipole interactions

10. London forces Momentary dipole-dipole interaction Momentary dipole-dipole interaction “instantaneous” dipole “induces” a dipole in a neighboring molecule “instantaneous” dipole “induces” a dipole in a neighboring molecule brief attractive force results brief attractive force results

11. Step 1

12. Step 2

13. Result...

14. London forces Strength depends on:Strength depends on: size of electron cloudsize of electron cloud –bigger = stronger number of atoms in moleculenumber of atoms in molecule –more atoms = more electrons = stronger

15. Ion – dipole forces Between polar molecules and ions Between polar molecules and ions Aqueous solutions of ionsAqueous solutions of ions Positive ends of polar molecules attract negative ions Positive ends of polar molecules attract negative ions Negative ends attract positive ions Negative ends attract positive ions Only important in aqueous solutions Only important in aqueous solutions

17. Hydrogen Bonds Special case of polar attraction Special case of polar attraction H atom is H atom is 1)bonded to high EN atom and1)bonded to high EN atom and 2)attracted to a high EN atom it is not bonded to (N, O, F)2)attracted to a high EN atom it is not bonded to (N, O, F) 5 times stronger than regular polar attractions 5 times stronger than regular polar attractions

18. Hydrogen Bonds

19. Physical property effects of Intermolecular Forces of Attraction …all come down to how sticky the molecules are toward each other…

20. The Key Idea… The stronger the IMF’s, the tighter the molecules cling to each other, the harder it is to separate them. The stronger the IMF’s, the tighter the molecules cling to each other, the harder it is to separate them.

21. The Key Idea… In other words, the harder it is to separate molecules, the stronger their IMF’s In other words, the harder it is to separate molecules, the stronger their IMF’s

22. What does that mean…”separate the molecules”? Pull them apart: Melting Melting Boiling Boiling Physically move them apart Physically move them apart Peel them away. Wipe them off, etc… Peel them away. Wipe them off, etc…

23. Boiling Point Effects

26. Intermolecular Forces of Attraction Attractive forces that cause atoms or molecules to stick together

27. Types of IMF’s  London (dispersion) forces  all molecules  weakest interaction  dipole-dipole forces  polar molecules  ion-dipole forces  Between polar molecules and ions  hydrogen bonding  H atoms w/ O, N, F not covalently bonded to it  strongest interaction

28. The Key Idea… The stronger the IMF’s, the tighter the molecules cling to each other, the harder it is to separate them. The stronger the IMF’s, the tighter the molecules cling to each other, the harder it is to separate them.

29. Solubility of a solid in liquid General rule: Like dissolves Like Polar solutes dissolve in polar solventsPolar solutes dissolve in polar solvents Sugar (polar solute) in H 2 O (polar solvent) Sugar (polar solute) in H 2 O (polar solvent) Ionic solids dissolve in polar solventsIonic solids dissolve in polar solvents NaCl (ionic solid) in H 2 O (polar solvent) NaCl (ionic solid) in H 2 O (polar solvent) Nonpolar solutes dissolve in nonpolar solventsNonpolar solutes dissolve in nonpolar solvents Dried paint (nonpolar solute) in paint stripper – turpentine, etc. (nonpolar solvent) Dried paint (nonpolar solute) in paint stripper – turpentine, etc. (nonpolar solvent)

30. Colligative properties of Solutions -Properties of solutions that are affected by the number of dissolved particles, not the identity of the particles Example: vapor pressure lowering The more particles (with little tendency to vaporize) that are added to a solvent, the lower the vapor pressure of the solution becomes

31. Colligative properties of Solutions Density of a solution The presence of dissolved particles (whose mass is greater than the mass of the solvent particles) in a solution causes the density of a solution to increase Sugar water is more dense than pure water Sugar water is more dense than pure water Sugary sodas are more dense than diet sodas Sugary sodas are more dense than diet sodas it takes more sugar molecules than artificial sweetener moleculesit takes more sugar molecules than artificial sweetener molecules

32. Swimming in the Dead Sea

33. Colligative properties of Solutions Boiling point elevation: The presence of dissolved particles tends to increase the boiling point of a liquid Salt added to water before boiling to prepare food increases the temperature the water boils at, and thus cooks the food faster, as the water is hotter

34. Colligative properties of Solutions Freezing point depression The presence of dissolved particles tends to lower the freezing point of a liquid Salt or other substances are used to melt ice, because as they dissolve into the ice, they lower the freezing point of the ice, and thus even more of the ice melts

35. Compressibility gases are compressiblegases are compressible –empty space between molecules –Weak IMF’s won’t keep molecules together liquids, solids aren’tliquids, solids aren’t –closely packed

36. Diffusion The intermingling of molecules with each other The intermingling of molecules with each other gases = rapid  much empty space gases = rapid  much empty space liquids = slowly  more closely packed liquids = slowly  more closely packed solids = negligible  locked in place solids = negligible  locked in place

37. Cohesion/Adhesion Cohesion = molecules sticking together Cohesion = molecules sticking together Adhesion = molecules sticking to a substrate Adhesion = molecules sticking to a substrate

38. Viscosity The resistance of a fluid to flow. The resistance of a fluid to flow. The stronger the IMF’s, the higher the viscosity The stronger the IMF’s, the higher the viscosity

39. Surface Tension Intermolecular attractions at the surface are only inward towards the substance Intermolecular attractions at the surface are only inward towards the substance

40. Surface Tension, continued Molecules at the surface of a liquid act as a “skin” Molecules at the surface of a liquid act as a “skin” the greater the IMF’s, the more pronounced the effect the greater the IMF’s, the more pronounced the effect liquids seek to lower their surface tension liquids seek to lower their surface tension water drops are spherical water drops are spherical

41. Surface Tension, continued

42. Surface Wetting The spreading of a liquid across a surface The spreading of a liquid across a surface must have adhesion  cohesion must have adhesion  cohesion

43. Gasoline – a nonpolar hydrocarbon Low surface tensionLow surface tension –only London forces low cohesionlow cohesion –spreads easily across most surfaces does not effectively “wet” glassdoes not effectively “wet” glass

44. H 2 O – a polar molecule that H- bonds High surface tensionHigh surface tension –hydrogen bonding High cohesive forcesHigh cohesive forces High adhesive forcesHigh adhesive forces –will H-bond with O’s in glass Good wetting agent for glassGood wetting agent for glass

45. Water beads on greasy glassWater beads on greasy glass –eliminates H-bonding to glass –low adhesion

46. Surfactants, used in soaps and detergents, drastically lower the surface tension of water Surfactants, used in soaps and detergents, drastically lower the surface tension of water –soapy water spreads more easily over dirty surfaces

47. Vaporization The change of a liquid → gas is called vaporizationThe change of a liquid → gas is called vaporization an example of separating moleculesan example of separating molecules Evaporation: happens at the exposed surface of a liquidEvaporation: happens at the exposed surface of a liquid Boiling: happens within the liquid itselfBoiling: happens within the liquid itself

48. Evaporation Liquids exert vapor pressure due to the evaporated liquid Liquids exert vapor pressure due to the evaporated liquid The stronger the IMF’s, the slower the evaporation rate, the lower the vapor pressure for a given temperature The stronger the IMF’s, the slower the evaporation rate, the lower the vapor pressure for a given temperature

49. Evaporation The higher the T of a substance, the more molecules with enough energy to overcome cohesive forces/surface tension and evaporate The higher the T of a substance, the more molecules with enough energy to overcome cohesive forces/surface tension and evaporate As liquid T , vapor P  As liquid T , vapor P 

50. Minimum E to evaporate AbundanceAbundance coolest warmest Energy Temperature is ~ the average KE of a sample

51. What happens... To the evaporation rateTo the evaporation rate –if the temperature = the boiling point ? All the molecules, on average, have enough energy to vaporizeAll the molecules, on average, have enough energy to vaporize –the liquid boils

52. What happens... If the vapor pressure equals the atmospheric pressure ?If the vapor pressure equals the atmospheric pressure ? All the molecules, on average, have enough energy to vaporizeAll the molecules, on average, have enough energy to vaporize –the liquid boils

53. T vs Vapor Pressure Temperature Vap PressureVap Pressure 1.00 atm 100 o C

54. How can you boil a liquid? 1)Heat it to its boiling point vapor P = air P 2)Reduce the air P above it to equal the vapor P of the liquid at that temperature air P = vapor Pair P = vapor P all done! all done! all done! all done!

55. Intermolecular Forces of Attraction Forces of attraction between molecules