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Intermolecular Forces

Intermolecular Forces. Bonding. Ionic Covalent Polar covalent. Intermolecular Forces. O. H. H. O. H. H. inter. molecular forces. Intermolecular Vs. Intramolecular Forces. intra molecular forces (  “bonds”). H. O. H.

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Intermolecular Forces

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  1. Intermolecular Forces

  2. Bonding • Ionic • Covalent • Polar covalent

  3. Intermolecular Forces

  4. O H H O H H inter molecular forces Intermolecular Vs. Intramolecular Forces intramolecular forces (“bonds”) H O H

  5. Figure 10.1 The Schematic Representations of the Three States of Matter

  6. Intermolecular Forces Vaporize: 40.7 kJ Break O-H Bonds: 467 kJ

  7. Table 10.6 Comparison of Atomic Separations Within Molecules (Covalent Bonds) and Between Molecules (Intermolecular Interactions)

  8. Intermolecular Forces • Covalent and Ionic bonds are intramolecular forces • Attractions between molecules are intermolecular forces • Intermolecular forces are weaker than intramolecular forces (vaporizing H2O vs. breaking OH bonds) • 3 Possible Different Types of IM forces: - Dipole-Dipole -Hydrogen bonding - London Dispersion forces • Properties of pure substances (in liquid or solid form) that depend on the strength of intermolecular forces: Melting point, boiling point, ΔHvap, ΔHfus, Vapor pressure, surface tension * ALL molecular substances’ molecules will be attracted by London Dispersion forces, but not of equal strength. * NOT all molecular substances’ molecules will be attracted by Dipole-Dipole or Hydrogen bonding “forces”

  9. Dipole-Dipole Forces

  10. If a molecule is polar, it has a positive and negative end • If a molecule is polar, the positive end of one molecule will be attracted to the negative end of another • That’s basically dipole-dipole forces! • If a molecule is nonpolar then it will not have “dipole-dipole” forces of attraction between its molecules

  11. Figure 10.2 a-b (a) The Electrostatic Interaction of Two Polar Molecules (b) The Interaction of Many Dipoles in a Condensed State

  12. Okay, so how do you know if a substance is polar? • See separate handout….later. • One example now: If substance has only one bond, and that bond is polar, then the whole molecule is polar • HCl is polar; ClF is polar • H2 (H-H) is nonpolar; Cl2 (Cl-Cl) is nonpolar; • Just remember that you need to first “figure out” if a substance is polar before you conclude it “has” dipole-dipole forces acting between its molecules!

  13. Polarity of Substances HCl, CO2, NaCl **Polarity only applies to molecular substances. Ionic compounds are at the “extreme”—the bonding is not considered “polar (covalent)”, but simply “ionic”! **Ion-ion forces are comparable to intra-molecular forces. VERY STRONG

  14. Figure 10.3 a-b (a) The Polar Water Molecule (b) Hydrogen Bonding Among Water Molecules

  15. Hydrogen Bonding is a Special Case Version of Dipole-Dipole Hydrogen Bonding - Strong dipole-dipole forces - Found in substances in which H is bound to highly electronegative atom (N, O, F) Why? - Very polar bond - H atom is really small

  16. Example Which substance has the strongest dipole-dipole forces (between its molecules)? HF, HCl, HBr

  17. Figure 10.4 The Boiling Points of the Covalent Hydrides of the Elements in Groups 4A, 5A, 6A, and 7A

  18. Hydrogen Bonding

  19. London Dispersion Forces

  20. Figure 10.5 (a) An Instantaneous Polarization can Occur on Atom A (b) Nonpolar Molecules Such as H2 also can Develop Instantaneous and Induced Dipoles

  21. Figure 10.4 The Boiling Points of the Covalent Hydrides of the Elements in Groups 4A, 5A, 6A, and 7A

  22. Table 10.2 The Freezing Points of the Group 8A Elements

  23. London Dispersion Forces • Present between any two molecules • The only forces present between Nonpolar molecules (& between Noble Gas Atoms) • London dispersion forces increase as size of atom or molecule increases

  24. London Dispersion Forces • Which substance has the strongest London dispersion forces? CH4 , CH3CH3, CH3CH2CH3

  25. Properties • Boiling Point • Melting Point (same as Freezing Point) • Δ Hvap • Δ Hmelting • Vapor Pressure

  26. Boiling Points Explain the difference in boiling points: • n-pentane, C5H12 MW: 72.15 B.P.= 36.2 C Vs. Neopentane, C5H12 MW: 72.15 B.P.= 9.5 C • dimethyl ether, CH3OCH3MW: 46.07 B.P.= -25 C Vs. ethanol, CH3CH2OH MW: 46.07 B.P. = 79 C • Napthalene, C10H8 MW: 128.16 B.P.= 218 C Vs. Acetic Acid, CH3CO2H MW: 60.05 B.P.= 118  C

  27. Examples What type of interparticle forces are present in these substances? Ar, HCl, CaCl2 What is the most important interparticle force in teflon, CF3(CF2CF2)nCF3? Which substance has stronger intermolecular forces? SeO2 Vs. SO2 Which has the highest boiling point? NaCl or HCl Which substance has the highest freezing point? H2O, NaCl, or HF

  28. Summary of IM Forces • All substances have London Dispersion Forces - London Dispersion Forces Increase w/ MW • Dipole-Dipole Interactions - Stronger when molecules are more polar - Special Case: Hydrogen Bonding (N, O, F) Take into account all forces as well as the size and shape of molecule when deciding which substance has the strongest IM forces

  29. Intermolecular Force Trends As IM Forces Increase: • Boiling Point Increases • Melting/Freezing Point Increases • Δ Hvap Increases • Δ Hmelting Increases • Vapor Pressure Decreases

  30. Next Lecture • Vapor Pressure • Phase Diagrams

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