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Liquids and Solids and Intermolecular Forces

Liquids and Solids and Intermolecular Forces. Chapter 11. Generally, inter molecular forces are much weaker than intra molecular forces. Intermolecular Forces. Intermolecular forces are attractive forces between molecules. Intramolecular forces hold atoms together in a molecule.

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Liquids and Solids and Intermolecular Forces

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  1. Liquids and Solids and Intermolecular Forces Chapter 11

  2. Generally, intermolecular forces are much weaker than intramolecular forces. Intermolecular Forces Intermolecular forces are attractive forces between molecules. Intramolecular forces hold atoms together in a molecule. • Intermolecular vs Intramolecular • 41 kJ to vaporize 1 mole of water (inter) • 930 kJ to break all O-H bonds in 1 mole of water (intra) “Measure” of intermolecular force boiling point melting point DHvap DHfus DHsub 11.2

  3. Orientation of Polar Molecules in a Solid Intermolecular Forces Dipole-Dipole Forces Attractive forces between polar molecules 11.2

  4. Ion-Dipole Interaction Intermolecular Forces Ion-Dipole Forces Attractive forces between an ion and a polar molecule Example: Complex ions, Al(H20)63+ 11.2

  5. Intermolecular Forces Ion-Induced Dipole and Dipole-Induced Dipole Attractive forces that arise as a result of temporary dipoles induced in non-polar atoms or molecules Non-polar atom or molecule ion-induced dipole interaction dipole-induced dipole interaction Polarizability and Dispersion Force @ KSU - YouTube 11.2

  6. Dispersion forces usually increase with molar mass. Intermolecular Forces Dispersion (London) Forces Occurs in all substances Polarizability is the ease with which the electron distribution in the atom or molecule can be distorted. • Polarizability increases with: • greater number of electrons • more diffuse electron cloud van der Waals force are dispersion and Dipole forces combined 11.2

  7. O O S What type(s) of intermolecular forces exist between each of the following molecules? HBr HBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules. CH4 CH4 is nonpolar: dispersion forces only. SO2 SO2 is a polar molecule: dipole-dipole forces. There are also dispersion forces between SO2 molecules. 11.2

  8. or … … H H B A A A Intermolecular Forces Hydrogen Bond The hydrogen bond is a special dipole-dipole interaction between they hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom. A & B are N, O, or F 11.2

  9. Decreasing molar mass Decreasing boiling point Why is the hydrogen bond considered a “special” dipole-dipole interaction? 11.2

  10. Properties of Liquids Surface tension is the amount of energy required to stretch or increase the surface of a liquid by a unit area. Strong intermolecular forces High surface tension 11.3

  11. Adhesion Cohesion Properties of Liquids Cohesion is the intermolecular attraction between like molecules Adhesion is an attraction between unlike molecules Meniscus Inverted meniscus 11.3

  12. Properties of Liquids Viscosity is a measure of a fluid’s resistance to flow. Strong intermolecular forces High viscosity 11.3

  13. Maximum Density 40C Ice is less dense than water Water is a Unique Substance Density of Water 11.3

  14. Properties of Solids

  15. lattice point A crystalline solid possesses rigid and long-range order. In a crystalline solid, atoms, molecules or ions occupy specific (predictable) positions. An amorphoussolid does not possess a well-defined arrangement and long-range molecular order. A unit cell is the basic repeating structural unit of a crystalline solid. • At lattice points: • Atoms • Molecules • Ions Unit cells in 3 dimensions Unit Cell 11.4

  16. 11.4

  17. 11.4

  18. Types of Crystals • Ionic Crystals • Lattice points occupied by cations and anions • Held together by electrostatic attraction • Hard, brittle, high melting point • Poor conductor of heat and electricity CsCl ZnS CaF2 11.6

  19. carbon atoms Types of Crystals • Covalent Crystals • Lattice points occupied by atoms • Held together by covalent bonds • Hard, high melting point • Poor conductor of heat and electricity graphite diamond 11.6

  20. Types of Crystals • Molecular Crystals • Lattice points occupied by molecules • Held together by intermolecular forces • Soft, low melting point • Poor conductor of heat and electricity 11.6

  21. nucleus & inner shell e- mobile “sea” of e- Types of Crystals • Metallic Crystals • Lattice points occupied by metal atoms • Held together by metallic bonds • Soft to hard, low to high melting point • Good conductors of heat and electricity Cross Section of a Metallic Crystal 11.6

  22. Types of Crystals 11.6

  23. Least Order Greatest Order T2 > T1 Condensation Evaporation 11.8

  24. H2O (l) H2O (g) Dynamic Equilibrium Rate of evaporation Rate of condensation = The equilibrium vapor pressure is the vapor pressure measured when a dynamic equilibrium exists between condensation and evaporation 11.8

  25. (manometer) At Equilibrium Before Evaporation 11.8

  26. Clausius-Clapeyron Equation ln P = - DHvap + C RT Molar heat of vaporization (DHvap) is the energy required to vaporize 1 mole of a liquid. P = (equilibrium) vapor pressure T = temperature (K) R = gas constant (8.314 J/K•mol) 11.8

  27. The boiling point is the temperature at which the (equilibrium) vapor pressure of a liquid is equal to the external pressure. The normal boiling point is the temperature at which a liquid boils when the external pressure is 1 atm. 11.8

  28. H2O (s) H2O (l) The melting point of a solid or the freezing point of a liquid is the temperature at which the solid and liquid phases coexist in equilibrium Freezing Melting 11.8

  29. Molar heat of fusion (DHfus) is the energy required to melt 1 mole of a solid substance. 11.8

  30. 11.8

  31. H2O (s) H2O (g) Molar heat of sublimation (DHsub) is the energy required to sublime 1 mole of a solid. Sublimation Deposition DHsub = DHfus + DHvap ( Hess’s Law) 11.8

  32. A phase diagram summarizes the conditions at which a substance exists as a solid, liquid, or gas. Phase Diagram of Water 11.8

  33. The critical temperature (Tc) is the temperature above which the gas cannot be made to liquefy, no matter how great the applied pressure. The critical pressure (Pc) is the minimum pressure that must be applied to bring about liquefaction at the critical temperature. 11.8

  34. What is a supercritical fluid? • A supercritical fluid is a material which can be either liquid or gas. • It shows unique properties that are different from those of either gases or liquids under standard conditions. • A supercritical fluid has both the gaseous property of being able to penetrate anything, and the liquid property of being able to dissolve materials into their components.

  35. Supercritical Fluid Applications • It offers the advantage of being able to change density to a great extent in a continuous manner. • The use of carbon dioxide or water in the form of a supercritical fluid offers a substitute for an organic solvent in the fields of the food industry and medical supplies. • YouTube - Supercritical fluidsRelated Videos

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