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Intermolecular Forces and Liquids and Solids Chapter 10
A  phase  is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases Solid phase - ice Liquid phase - water 11.1
Intermolecular Forces 11.2 Intermolecular forces  are attractive forces  between  molecules. Intramolecular forces  hold atoms together in a molecule. ,[object Object],[object Object],[object Object],“ Measure” of intermolecular force boiling point melting point  H vap  H fus  H sub Generally,  inter molecular forces are much weaker than  intra molecular forces.
Types of Intermolecular Forces 1. Hydrogen Bond (strongest) 11.2 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.  IT IS NOT A BOND. A & B are N, O, or F A H … B A H … A or
Hydrogen Bond 11.2
Why is the hydrogen bond considered a “special” dipole-dipole interaction? 11.2 Decreasing molar mass Decreasing boiling point
Types of Intermolecular Forces 2. Ion-Dipole Forces Attractive forces between an  ion  and a  polar molecule 11.2 Ion-Dipole Interaction
11.2
Types of Intermolecular Forces 3. Dipole-Dipole Forces Attractive forces between  polar molecules 11.2 Orientation of Polar Molecules in a Solid
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 11.2 ion-induced dipole interaction dipole-induced dipole interaction
Intermolecular Forces 4. Dispersion Forces Continued 11.2 Polarizability  is the ease with which the electron distribution in the atom or molecule can be distorted. ,[object Object],[object Object],[object Object],Dispersion forces usually increase with molar mass.
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. CH 4 CH 4  is nonpolar: dispersion forces. SO 2 SO 2  is a polar molecule: dipole-dipole forces.  There are also dispersion forces between SO 2  molecules. 11.2 S O O
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
Properties of Liquids Cohesion  is the intermolecular attraction between like molecules 11.3 Adhesion  is an attraction between unlike molecules Adhesion Cohesion
Properties of Liquids Viscosity  is a measure of a fluid’s resistance to flow. 11.3 Strong intermolecular forces High viscosity
Density of Water 11.3 Water is a Unique Substance Maximum Density 4 0 C Ice is less dense than water
A  crystalline solid  possesses rigid and long-range order.  In a crystalline solid, atoms, molecules or ions occupy specific (predictable) positions. An  amorphous   solid  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. Unit Cell Unit cells in 3 dimensions 11.4 ,[object Object],[object Object],[object Object],[object Object],lattice point
11.4
11.4
Types of Crystals ,[object Object],[object Object],[object Object],[object Object],[object Object],CsCl ZnS CaF 2 11.6
Types of Crystals ,[object Object],[object Object],[object Object],[object Object],[object Object],11.6 diamond graphite carbon atoms
Types of Crystals ,[object Object],[object Object],[object Object],[object Object],[object Object],11.6
Types of Crystals ,[object Object],[object Object],[object Object],[object Object],[object Object],11.6 Cross Section of a Metallic Crystal nucleus & inner shell e - mobile “sea” of e -
Types of Crystals 11.6
An  amorphous   solid  does not possess a well-defined arrangement and long-range molecular order. A  glass  is an optically transparent fusion product of inorganic materials that has cooled to a rigid state  without crystallizing Crystalline quartz (SiO 2 ) Non-crystalline quartz glass 11.7
Chemistry In Action:  High-Temperature Superconductors
Evaporation 11.8 Condensation Greatest Order Least Order T 2  > T 1
The  equilibrium vapor pressure  is the vapor pressure measured when a dynamic equilibrium exists between condensation and evaporation 11.8 H 2 O  ( l )   H 2 O  ( g ) Rate of condensation Rate of evaporation = Dynamic Equilibrium
Molar heat of vaporization  (  H vap ) 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 ln  P  = -  H vap RT +  C Clausius-Clapeyron Equation
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
The  critical temperature  ( T c ) is the temperature above which the gas cannot be made to liquefy, no matter how great the applied pressure. The  critical pressure  ( P c ) is the minimum pressure that must be applied to bring about liquefaction at the critical temperature. 11.8
Melting 11.8 Freezing 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 H 2 O  ( s )   H 2 O  ( l )
Molar heat of fusion  (  H fus ) is the energy required to melt 1 mole of a solid substance. 11.8
11.8
Sublimation 11.8 Deposition Molar heat of sublimation  (  H sub ) is the energy required to sublime 1 mole of a solid.  H sub =   H fus  +   H vap ( Hess’s Law) H 2 O  ( s )   H 2 O  ( g )
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
11.9
Where’s Waldo? 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)? Carbon Dioxide
11.9
Colligative Properties ,[object Object],[object Object]

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Power Point Solids & Liquids

  • 1. Intermolecular Forces and Liquids and Solids Chapter 10
  • 2. A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases Solid phase - ice Liquid phase - water 11.1
  • 3.
  • 4. Types of Intermolecular Forces 1. Hydrogen Bond (strongest) 11.2 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. IT IS NOT A BOND. A & B are N, O, or F A H … B A H … A or
  • 6. Why is the hydrogen bond considered a “special” dipole-dipole interaction? 11.2 Decreasing molar mass Decreasing boiling point
  • 7. Types of Intermolecular Forces 2. Ion-Dipole Forces Attractive forces between an ion and a polar molecule 11.2 Ion-Dipole Interaction
  • 9. Types of Intermolecular Forces 3. Dipole-Dipole Forces Attractive forces between polar molecules 11.2 Orientation of Polar Molecules in a Solid
  • 10. 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 11.2 ion-induced dipole interaction dipole-induced dipole interaction
  • 11.
  • 12. 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. CH 4 CH 4 is nonpolar: dispersion forces. SO 2 SO 2 is a polar molecule: dipole-dipole forces. There are also dispersion forces between SO 2 molecules. 11.2 S O O
  • 13. 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
  • 14. Properties of Liquids Cohesion is the intermolecular attraction between like molecules 11.3 Adhesion is an attraction between unlike molecules Adhesion Cohesion
  • 15. Properties of Liquids Viscosity is a measure of a fluid’s resistance to flow. 11.3 Strong intermolecular forces High viscosity
  • 16. Density of Water 11.3 Water is a Unique Substance Maximum Density 4 0 C Ice is less dense than water
  • 17.
  • 18. 11.4
  • 19. 11.4
  • 20.
  • 21.
  • 22.
  • 23.
  • 25. An amorphous solid does not possess a well-defined arrangement and long-range molecular order. A glass is an optically transparent fusion product of inorganic materials that has cooled to a rigid state without crystallizing Crystalline quartz (SiO 2 ) Non-crystalline quartz glass 11.7
  • 26. Chemistry In Action: High-Temperature Superconductors
  • 27. Evaporation 11.8 Condensation Greatest Order Least Order T 2 > T 1
  • 28. The equilibrium vapor pressure is the vapor pressure measured when a dynamic equilibrium exists between condensation and evaporation 11.8 H 2 O ( l ) H 2 O ( g ) Rate of condensation Rate of evaporation = Dynamic Equilibrium
  • 29. Molar heat of vaporization (  H vap ) 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 ln P = -  H vap RT + C Clausius-Clapeyron Equation
  • 30. 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
  • 31. The critical temperature ( T c ) is the temperature above which the gas cannot be made to liquefy, no matter how great the applied pressure. The critical pressure ( P c ) is the minimum pressure that must be applied to bring about liquefaction at the critical temperature. 11.8
  • 32. Melting 11.8 Freezing 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 H 2 O ( s ) H 2 O ( l )
  • 33. Molar heat of fusion (  H fus ) is the energy required to melt 1 mole of a solid substance. 11.8
  • 34. 11.8
  • 35. Sublimation 11.8 Deposition Molar heat of sublimation (  H sub ) is the energy required to sublime 1 mole of a solid.  H sub =  H fus +  H vap ( Hess’s Law) H 2 O ( s ) H 2 O ( g )
  • 36. 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
  • 37. 11.9
  • 38. Where’s Waldo? 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)? Carbon Dioxide
  • 39. 11.9
  • 40.