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Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids. Chapter 11. A phase is a ___________ part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases. __________ phase - ice. __________ - water. 11.1.

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Intermolecular Forces and Liquids and Solids

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  1. Intermolecular Forces and Liquids and Solids Chapter 11

  2. A phase is a ___________ part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases __________ phase - ice __________ - water 11.1

  3. Generally, ____molecular forces are much weaker than ____molecular forces. Intermolecular Forces I_____________ forces are attractive forces ________molecules. I_____________ hold atoms ____________ 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

  4. or … … H H B A A A Types of Intermolecular Forces 1. __________ (strongest) The _________ is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom. IT IS NOT A BOND. A & B are N, O, or F 11.2

  5. Hydrogen Bond 11.2

  6. Ion-Dipole Interaction Types of Intermolecular Forces 2. Ion-Dipole Forces Attractive forces between an ion and a polar molecule 11.2

  7. 11.2

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

  9. Types of Intermolecular Forces 4. Dispersion Forces – van der Walls forces/London forces (weakest) Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules ion-induced dipole interaction dipole-induced dipole interaction 11.2

  10. Dispersion forces usually increase with molar mass. Intermolecular Forces 4. Dispersion Forces Continued 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 11.2

  11. 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. SO2 SO2 is a polar molecule: dipole-dipole forces. There are also dispersion forces between SO2 molecules. 11.2

  12. 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

  13. Adhesion Properties of Liquids Cohesion is the intermolecular attraction between like molecules Adhesion is an attraction between unlike molecules attracted to glass Cohesion attracted to each other 11.3

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

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

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

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

  18. 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

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

  20. 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

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

  22. 11.8

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

  24. A phase diagram summarizes the conditions at which a substance exists as a solid, liquid, or gas. The triple point is where all 3 phases meet. Phase Diagram of Water 11.9

  25. 11.9

  26. Can you find… The Triple Point? Critical pressure? Critical temperature? Where fusion occurs? Where vaporization occurs? Melting point (at 1 atm)? Boiling point(at 6 atm)? Where’s Waldo? Carbon Dioxide

  27. 11.9

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