1. Chapter 17 Liquid and Solution

2. Intermolecular Forces Dipole-Dipole Forces Molecules with dipole moments can attract each other electrostatically by lining up so that the positive and negative ends are close to each other.

3. Dipole-Dipole Forces Dipole-dipole forces are typically only about 1% as strong as covalent or ionic bonds.

4. Hydrogen Bonding Particularly strong dipole-dipole forces are seen among molecules in which hydrogen is bound to a highly electronegative atom, such as nitrogen, oxygen, or fluorine. The hydrogen bond has only 5% or so of the strength of a covalent bond.

6. Relatively large electronegativity value of the lightest elements Nonpolar tetrahedral hydrides

7. Intermolecular Forces London Dispersion Forces Atoms can develop a momentary nonsymmetrical electron distribution that produces a temporary dipolar arrangement of charge. This instantaneous dipole can then induce a similar dipole in a neighboring atom, leading to an interatomic attraction.

10. The Effect of Molecular Size for London dispersion forces The electrons distribution around an atom or molecule can be distorted is called the polarizability ( 極化度 ). Larger and heavier atoms and molecules exhibit stronger dispersion forces than smaller and lighter ones. In a larger atom or molecule, the valence electrons are, on average, farther from the nuclei than in a smaller atom or molecule. They are less tightly held and can more easily form temporary dipoles.

11. The Effect of Molecular Shape for London dispersion forces At room temperature, neopentane (C 5 H 12 ) is a gas whereas n-pentane (C 5 H 12 ) is a liquid. London dispersion forces between n-pentane molecules are stronger than those between neopentane molecules. The cylindrical shape of n-pentane molecules allows them to come in contact with each other more effectively than the spherical neopentane molecules.

12. n-pentane neopentane

13. Temperature Dependence of Vapor Pressure

14. Vapor Pressure

15. Change of State

16. Normal melting point: the temperature at which the solid and liquid states have same vapor pressure under conditions where the total pressure is 1 atm. Normal boiling point: the temperature at which the vapor pressure of liquid is exactly 1 atm.

17. The supercooling of water

18. Supercooled and Superheated Supercooled: supercooling occurs because, as it is cooled, the water may not achieve the degree of organization necessary to form ice at 0 o C; thus it continues to exist as the liquid. Superheated: superheating can occur because bubble formation in the interior of the liquid requires that many high-energy molecules gather in the same vicinity.

19. Phase Diagram of Water P=218 atm T=374 o C Supercritical phase 超臨界態

20. Phase Diagram of Carbon Dioxide

21. The Thermodynamics of Solution Formation The cardinal rule of solubility is like dissolves like. Three distinct steps for the formation of solutions Step 1: Breaking up the solute into individual components. Step 2: Overcoming intermolecular forces in the solvent to make room for the solute. Step 3: Allowing the solute and solvent to interact to form the solution.

23. Step 1 and 2 require energy, are endothermic, since forces must be overcome to expand the solute and the solvent. Step 3 is usually exothermic. The overall enthalpy change associated with the formation of the solution, called the enthalpy of solution (∆H soln ). ∆H soln = ∆H 1 + ∆H 2 + ∆H 3

25. The Solubility of Sodium Chloride in Water ∆H 1 is large and positive because of the strong ionic forces in the crystal that must be overcome. ∆H 2 is expected to be large and positive because of the hydrogen bonds that must be broken in water. ∆H 3 is expected to be large and negative because of the strong interactions between the ions and the water molecules.

26. The dissolving process requires a small amount of energy.

27. Why is NaCl so Soluble in Water? Consider ∆G= ∆H-T∆S ∆H is positive and thus unfavorable. Therefore, ∆S must be positive and large enough to make ∆G negative. ∆S 1 and ∆S 2 are positive since the solute and solvent are expanded. ∆S 3 would be expected to be positive in general case.

28. Ionic Compounds in Water The assembling of a group of water molecules around the ion is an order producing phenomenon and would be expected to make a negative contribution to ∆S. The more charge density (Z/r) an ion possesses, the greater this hydration effect will be. The smaller ions presumably are able to bind the hydrating water molecules more firmly and thus show a more negative value to ∆S.

29. Nonpolar Compounds in Water The dispersal of nonpolar solute particles in water can also produce negative value to ∆S. The polar water molecules will not strongly hydrate the nonpolar molecules. Water forms a cage to isolate the nonpolar solute from the water bulk.

30. Factors Affecting Solubility Structure Effects Fat soluble hydrophobic Water soluble hydrophilic

31. Factors Affecting Solubility Pressure Effect

32. Henry’s Law P=k H x P: the partial pressure of the gaseous solute x: the mole fraction of the dissolved gas. k H : constant The amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution.

34. Factors Affecting Solubility Temperature Effect

35. The Vapor Pressure of Solutions Nonvolatile Solute/Solvent Raoult’s Law

38. Raoult’s Law with Multiple Volatile compounds Ideal solution: A solution, obeys Raoult’s law, formed with no accompanying energy change, when the intermolecular attractive forces between the molecules of the solvent are the same as those between the molecules in the separate components.

39. Rauolt’s Law

40. 1.What is the total vapor pressure in a mixture of 50.0 g CH 3 OH (P° = 93.3 torr) and 25.0 g H 2 O (P° = 17.5 torr)? 2.In a mixture of 86.0 g C 6 H 6 (P° = 93.96 torr) and 90.0 g C 2 H 4 Cl 2 (P° = 224.9 torr), what is the total vapor pressure?

41. Nonideal Solution Solutions that do not obey Raoult’s Law are called nonideal solutions. Solute-solvent interactions are significantly different from solute-solute and solvent-solvent interactions, the solution is likely to be a nonideal solution. Intermolecular forces between components in a dissolved solution can cause deviations from the calculated vapor pressure.

42. Negative Deviation from Raoult’s Law Both components have a lower escaping tendency in the solution than in the pure liquids.    

43. Positive Deviation from Raoult’s Law If two liquids mix endothermically, this indicates that the solute-solvent interactions are weaker than the interactions among the molecules in the pure liquids. More energy is required to expand the liquid than is released when the liquids are mixed. The molecules in the solution have a higher tendency to escape than expected.

44. ideal systempositive deviationnegative deviation

45. Colligative Properties In the dilute solution, this change in solvent chemical potential leads to a change in the vapor pressure, the normal boiling point and the normal freezing point and causes the phenomenon of osmotic pressure. They depend only on the number of the solute particles in an ideal solution

46. Phase diagrams for water

47. Freezing Point Depression

48. Boiling Point Elevation

49. Molal Freezing Point Depression Constant Molal Boiling Point Elevation Constant

50. Osmotic Pressure  =MRT  : the osmotic pressure in atmospheres M: molarity of the solute R: gas law constant T: Kelvin temperature

53. Artificial Kidney

54. Reverse Osmosis

55. Colligative Properties of Electrolyte Solutions The relationship between the moles of solute dissolved and the moles of particles in solution is usually expressed by the van’t Hoff factor

56. Colloids A suspension of tiny particles in some medium. Colloidal suspensions exhibit light scattering. A beam of light or laser, invisible in clear air or pure water, will trace a visible path through a genuine colloidal suspension. Tyndall scattering is caused by reflection of the incident radiation from the surfaces of the particles, reflection from the interior walls of the particles, and refraction and diffraction of the radiation as it passes through the particles.

59. Liquid-Vapor Equilibrium at Fixed Pressure

60. X Lever Rule Tie Line Distillation

61. Vapor Liquid L+V D E

62. Dew-point( 露點 ): the temperature at which the saturated vapor starts to condense Bubble-point( 泡點 ): the temperature at which the liquid starts to boil

63. Azeotrope( 共沸 ) A mixture of two or more components which has a constant boiling point at a particular composition. ideal system negative deviation positive deviation

64. Component 1Component 2 ComponentWaterEthanol Component Boiling Point (K) 373.15351.65 Azeotrope Mol. Frac. 0.10530.8947 Azeotrope Temperature (K) 351.35