Dipoleinteraction between polar molecules polar

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Unformatted text preview: pole-Dipole Attraction: 2. DipoleInteraction between polar molecules polar molecules A net result of attractive and repulsive dipoledipole forces Dipole-dipole forces → “preferred” orientations of molecules in the liquid or solid states. Intermolecular Intermolecular Forces I (van der Waals forces) If two molecules have about the same mass and size, then dipole-dipole forces increase with increasing polarity. increasing Intermolecular Forces I (van der Waals forces) 3. Induced Dipole Attraction 3. Weaker than dipoledipole-dipole forces • A nonpolar molecule or atom can be induced to be a nonpolar temporary temporary polar molecule. • Dipole-Induced Dipole Attraction The attraction between the polar molecules (permanent dipole) and the non-polar molecules (induced dipole). Intermolecular Forces I (van der Waals forces) 3. Induced Dipole Attraction 3. Can O2 or CO2 be dissolved in water ? Intermolecular Forces I (van der Waals forces) 4. London Dispersion Forces (Induced dipole-induced dipole Attraction) dipole• Interaction between two adjacent neutral molecules or atoms neutral atoms Electrons in the first molecule momentarily becomes unevenly unevenly distributed. The δ+ end of the 1st attracts the electrons in the 2nd and create a δ- end . London London Dispersion Forces and Polarizability Polarizability Polarizability: refers to the ease with which the charge charge distribution in a molecule can be distorted by an external distorted electric field. a. Higher Polarizability → easier to induce momentary dipoles→ stronger dispersion forces. Temporary distortion of He atoms Intermolecular Forces I (van der Waals forces) 4. London Dispersion Forces •Interaction between two adjacent neutral neutral molecules or atoms or Solid iodine Factors Affecting dispersion Forces • The strength of dispersion forces tends to increase with increased molecular weight. • Larger atoms have larger ele...
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This document was uploaded on 02/26/2014.

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