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Liquids

Liquids. Forces Between Liquid Molecules and their Effect on the Properties of Liquids. Types of Forces. Intramolecular-forces within a molecule-bonding types examples: ionic and covalent Intermolecular-forces between molecules examples: ionic, dispersion, dipole-dipole,

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Liquids

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  1. Liquids Forces Between Liquid Molecules and their Effect on the Properties of Liquids

  2. Types of Forces • Intramolecular-forces within a molecule-bonding types examples: ionic and covalent • Intermolecular-forces between molecules examples: ionic, dispersion, dipole-dipole, and hydrogen bonding

  3. Ionic Forces • Exist between “molecules” that contain ionic bonds. • Result from the electrostatic charges within the compound. • Opposite charges attract. • Strongest type of intermolecular force.

  4. London Dispersion Forces • Exist between noble gas atoms and nonpolar molecules • Weakest • Temporary-as electrons move around the nucleus, a momentary asymmetrical distribution of electrons can occur (provides a temporary dipole) • The instantaneous dipole can induce a similar dipole in a neighboring atom

  5. London Dispersion Forces (continued) • Large atoms with many electrons have stronger London Dispersion Forces • Larger nonpolar molecules have stronger LD forces

  6. Which has the stronger LD force? • Cl2 • Br2 0

  7. Which has the stronger LD force? • CH4 • C2H6 • C4H10 0

  8. Which has the stronger LD force • He • Ne • Ar • Xe 0

  9. Dipole-Dipole Forces • Exist between polar molecules • Permanent • Stronger than London Dispersion Forces (1% as strong as ionic/covalent bonds) • Created through an unequal sharing of electrons which results in a partial negative and positive charge • Positive end of one molecule attracts the negative end of another molecule

  10. Which of the following molecules have dipole-dipole forces present? • NH3 • CH4 • Both 0

  11. Which of the following molecules have dipole-dipole forces? • CO2 • H20 • Both 0

  12. Which of the following molecules have dipole-dipole forces present? • SF4 • SF6 • Both 0

  13. Hydrogen Bonding • A specific type of dipole-dipole force • Occurs when hydrogen atoms are bonded to highly electronegative atoms such as N, O, or F. • Created because of high levels of polarity and small size of hydrogen atoms (especially strong dipole-dipole attraction occurs)

  14. Which of the following compounds has hydrogen bonding present? • CH4 • CH3OH • Both 0

  15. Which of the following compounds has hydrogen bonding present? • H2S • H2O • Both 0

  16. Which of the following compounds has hydrogen bonding present? • HCl • HF • Both 0

  17. Review of Intermolecular Forces • Identify the most important type of interparticle forces present in each of the following substances. Ar HCl HF CaCl2 CH4 CO NaNO3

  18. What is the most importance type of interparticle force present in Ar? 10 • Ionic • London Dispersion • Dipole-Dipole • Hydrogen Bonding

  19. What is the most important type of interparticle force present in HCl? 10 • Ionic • London Dispersion • Dipole-Dipole • Hydrogen Bonding

  20. What is the most important type of interparticle force present in HF? 10 • Ionic • London Dispersion • Dipole-Dipole • Hydrogen Bonding

  21. What is the most important type of interparticle force present in CaCl2? 10 • Ionic • London Dispersion • Dipole-Dipole • Hydrogen Bonding

  22. What is the most important type of interparticle force present in CH4? 10 • Ionic • London Dispersion • Dipole-Dipole • Hydrogen Bonding

  23. What is the most important type of interparticle force present in CO? 10 • Ionic • London Dispersion • Dipole-Dipole • Hydrogen Bonding

  24. What is the most important type of interparticle force present in NaNO3? 10 • Ionic • London Dispersion • Dipole-Dipole • Hydrogen Bonding

  25. Arrange the following molecules in order of decreasing intermolecular interaction:SO2, Cl2, CH3OH, CH3NH2 10 • CH3OH > CH3NH2>SO2>Cl2 • Cl2>SO2>CH3OH>CH3NH2 • SO2>CH3NH2>CH3OH>Cl2 • CH3NH2>CH3OH>SO2>Cl2

  26. Properties of Liquids

  27. Surface Tension • Resistance of a liquid to increase in surface area • Measure of the inward forces • Liquids with high intermolecular forces have high surface tensions

  28. Capillary Action • Spontaneous rising of a liquid in a narrow tube • Caused by cohesive and adhesive forces cohesive forces-intermolecular forces among liquid molecules adhesive forces- force between the liquid molecules and the container; occur when the container is made of a polar substance

  29. Example of Capillary Action • When water is placed in a glass graduated cylinder, the meniscus is concave adhesive forces > cohesive forces (glass is polar) • When mercury is placed in the same graduated cylinder, the meniscus is convex cohesive forces > adhesive forces (mercury contains only dispersion forces-nonpolar)

  30. Viscosity • A resistance to flow • Strong intermolecular forces result in high viscosity • Large molecules also have high viscosity due to greater LD forces • As temperature increases, viscosity decreases

  31. Vapor Pressure • Pressure of vapor above the surface of a liquid • Caused when the molecules on the surface break away and go into the gas phase • In order to break away, the molecules must possess a minimum amount of kinetic energy • High intermolecular forces result in low vapor pressures • Volatile liquids are liquids that evaporate rapidly resulting in high vapor pressures

  32. Vapor Pressure (continued) • Substances with weak intermolecular forces tend to be volatile • As temperature increases, vapor pressure increases (more molecules possess the minimum kinetic energy and the rate of evaporation increases) • See the diagram on page 487.

  33. Calculating Vapor Pressure • The equation used to calculate the vapor pressure is: ln(PvapT1) = ∆Hvap(1 - 1) (PvapT2) = R (T2 - T1) ∆H is the heat of vaporization in J/mol, T is Kelvin temperature, R is 8.314 J/Kmol, and Pvap is vapor pressure

  34. Practice Problem • In Breckenridge , Colorado, the typical atmospheric pressure is 520. torr. What is the boiling point of water (∆Hvap= 40.7 kJ/mol) in Breckenridge?

  35. Melting Point and Boiling Points • Melting point- temperature at which the solid and liquid have the same vapor pressure • Boiling point-temperature at which the vapor pressure is equal to 1 atm (atmospheric pressure) • Melting and boiling points are higher when the intermolecular forces are stronger

  36. Which of the following has the highest boiling point? • H2O • HF • HI • HBr 0

  37. Which of the following liquids will be the most viscous? • C3H8 • C6H6 • CH4 • C2H6 0

  38. Arrange the following liquids, A, B, C, with vapor pressures at room temperature of 88, 680, and 155, respectively, in order of decreasing boiling points. • B>C>A • A>B>C • A>C>B • C>A>B 0

  39. Knowing that solutes with a certain polarity are best dissolved in solutions with similar polarity, which of the following solvents would be optimal for the solvation of CH3COOH? • CH4 • CH3OH • C2H6 • C6H6 0

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