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Intermolecular Forces

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Intermolecular Forces

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  1. Intermolecular Forces

  2. Intermolecular forces are weak, short-range attractive forces between atoms or molecules. Intermolecular forces ultimately derive from the electrostatic properties of molecules. Although intermolecular forces are weak, they result in significant effects on the physical properties of molecules because these forces are additive.

  3. Intramolecular bonds refer to the covalent bonds holding molecules together and are many-fold stronger than the weaker intermolecular forces of attraction between molecules. The strength of intermolecular forces between molecules is inversely proportional to the thermal energy of the system.

  4. Vibrational and Rotational Motion of Ethane

  5. Relative Motion of Water Molecules

  6. Summary of Intermolecular Forces Coulombic interactions Van der Waals interactions (London dispersion forces) Hydrogen bonds Hydrophobic effect

  7. Coulomb's Law o is the permittivity of the medium, also known as the dielectric constant

  8. Vacuum (o = 1) has little effect on Coulombic interactions Water (o = 80) significantly dampens Coulombic interactions Dielectric constants are related to the polarity and polarizability of the medium, that is the ability of the medium to diminish the force between two point charges at a constant distance d. Dielectric constants of common media Glass 5-10 Vacuum 1 Air (1 atm) 1.0006 Water 80 Air (102 atm)1.0548 Mylar 3 Benzene 4

  9. Van der Waals interactions arise from weak electrostatic forces that act over a short distance, generally near the point of physical contact. These forces ultimately rely on the inherent repulsive force of the outer electron clouds of molecules and its inherent polarizability.

  10. Attraction due to induced dipoles in outer electron shells - + - + Strong repulsion as outer electron shells begin to overlap Van der Waals radius Atomic radius The London-Jones Thought Experiment Infinite distance– no interaction

  11. Induced Dipole-Induced Dipole Interactions Induced Dipole-Dipole Interactions Dipole-Dipole Interactions

  12. Ion-Dipole Interaction

  13. The Structure of Water Conventional view Van der Waals representation Electron density (side view) Electron density (end view)

  14. Geometry of the Hydrogen Bond R = 2.976 (+0.000, -0.030) Å, α = 6 ± 20°, β = 57 ± 10°; α is the donor angle and β is the acceptor angle. The dimer (with slightly different geometry) dipole moment is 2.6 D. Although β is close to as expected if the lone pair electrons were tetrahedrallly placed (109.47°/2), the energy minimum (~21 kJ mol-1) is broad and extends towards β = 0°.

  15. Extended Hydrogen Bonding Structures

  16. Flicker Clusters Flicker clusters are short-lived local areas of order water within an otherwise disordered bulk solution.

  17. Relative Motion of Water Molecules

  18. Structure of Ice

  19. Space Filling Model of Liquid and Solid Water Liquid water Solid water

  20. Hydration Spheres Surrounding Ions

  21. Hydrophobic Effect The hydrophobic effect is an entropically-driven association of hydrophobic molecules that is a direct consequence of the polar nature of water and it propensity for hydrogen bonding.

  22. Bennion and Daggett (2003) Proc. Natl. Acad. Sci. USA100, 5142-5147.

  23. 1YPC rendered in PyMol

  24. Figure 1 Average Root Mean Square Deviation of the ca positions for the protein vs. time (a measure of overall protein structure) Nonpolar Surface Accessible Surface Area vs. time (a measure of protein “openness” Bennion and Daggett (2003) Proc. Natl. Acad. Sci. USA100, 5142-5147.

  25. Figure 3 water urea Bennion and Daggett (2003) Proc. Natl. Acad. Sci. USA100, 5142-5147.

  26. Figure 5 Bennion and Daggett (2003) Proc. Natl. Acad. Sci. USA100, 5142-5147.