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LIQUIDS, SOLIDS, & SOLUTIONS

LIQUIDS, SOLIDS, & SOLUTIONS. Chemical bonds (strong connections) Metallic Covalent Ionic. What sticks atoms together?. What sticks molecules together?. Intermolecular forces (IMFs) relatively weak Dispersion Dipole-dipole Hydrogen bonding. Chemical Bonds can be….

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LIQUIDS, SOLIDS, & SOLUTIONS

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  1. LIQUIDS, SOLIDS, & SOLUTIONS

  2. Chemical bonds (strong connections) • Metallic • Covalent • Ionic What sticks atoms together? What sticks molecules together? • Intermolecular forces (IMFs) relativelyweak • Dispersion • Dipole-dipole • Hydrogen bonding

  3. Chemical Bonds can be… Dependent upon: Molecules can be… Dependent upon:

  4. Shapes refresher: Trigonal- Trigonal- Tetrahedral Bipyramidal Octahedral Planar Linear Example: BF3 Example: CH3 Example: PF5 Example: SF6 Example: CO2

  5. Polar or Nonpolar

  6. IMFs

  7. Dispersion Forces/Induced Dipoles

  8. Dipole-Dipole Forces

  9. Hydrogen Bonding Forces

  10. LIQUIDS & THEIR PROPERTIES

  11. Strength of IMFs and properties

  12. Surface tension

  13. Viscosity

  14. Capillary Action

  15. Boiling Point

  16. Vapor Pressure

  17. Vapor Pressure

  18. SOLIDS & THEIR PROPERTIES

  19. Nature of solids • Solids tend to contain particles that are vibrating, but are restricted in their ability to move • High Density • Definite Volume • Definite Shape • Definite Melting Point • Incompressible • Low Rate Of Diffusion

  20. Nature of solids • Solids differ in their arrangements and in the forces that are holding them in place. • Properties that they all share are melting point, hardness, and density • Types of arrangements • Crystalline • Can be metallic/molecular/ionic or covalent-network • Amorphous

  21. Crystalline solids • Overall structure of a crystalline solid is a highly ordered, repeating pattern called unit cells • A unit cell is a representative unit of a larger crystal • It’s the smallest representation of the crystal

  22. Unit cells

  23. Crystalline: covalent/molecular • Held together by combinations of different intermolecular forces • Melting pt is dependent on IMF • Relatively soft • Poor conductors • Sugar, ice, dry ice

  24. Crystalline solids: ionic • Tightly packed solid composed of cations & anions • Intra-molecular forces • Form strongest crystal possible • Pack to minimize repulsive forces • Are hard and brittle • Have high melting points • Produce a crystal with a shape dependent on ions present

  25. Crystalline: metallic solids • Solid formed by the attraction between metal atoms and the surrounding sea of e-s • Electrons flow • Good conductors • Ductile and malleable • Can create mixtures called Alloys

  26. Covalent-network • Strong covalent bonds involved without a particular molecule being formed • Form a network of connections • They have extremely high melting points • Tend to be very hard, but brittle

  27. COVALENT NETWORK Graphite Diamond Vs. Dispersion Forces

  28. Crystalline solids:

  29. Amorphous solids • A solid in which the particles are arranged randomly • No crystal structure • Rigid appear solid-like • Glass, rubber, plastics • Sometimes called extremely viscous liquids

  30. Phase Diagrams

  31. Phase Diagrams

  32. SOLUTIONS & THEIR PROPERTIES

  33. Solutions Parts of:

  34. Solutions: Formation

  35. Solution Properties: Electrolytes

  36. Solution Properties: Concentrations

  37. What is the molarity of NaOH in a solution which contains 24.0 g NaOH dissolved in 300 ml of solution? Concentration Calculations: A soln contains 116 g acetone (CH3COCH3), 138 g of ethyl alcohol (C2H5OH) and 126 g of water. Determine the mole fraction of water. Calculate the molality of acetic acid in a solution prepared by dissolving 120 g acetic acid in 100 g of water. 17.5 g of sugar is dissolved in 200.0 g of water. What is the percent by mass concentration of the sugar solution?

  38. Solution Properties: Dilutions

  39. C1V1=C2V2 Dilution Calculations: You have 200 ml of 2.00 M stock solution. If we want to make 50 ml of 0.50 M solution, how much stock solution would we need? If we were then to take 10.0 ml of the new solution and add 10.0 ml of water, what concentration would the new solution be?

  40. 1 2 3 4 5 6

  41. Solution Properties: Making a Soln

  42. Solution Properties: Making a Soln

  43. Solution Properties: Saturation

  44. Solution Properties: Solubility Like Dissolves Like

  45. Solubility: Making the incompatible-compatible

  46. Increasing Solubility: Temperature

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