Intermolecular Forces Practice Answers

Intermolecular Forces Practice Answers - ozone is still a...

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Molecules Types of Forces CO2 Dispersion forces BCl3 Dispersion forces O3 Dispersion forces Dipole-dipole *see note CH4 Dispersion forces NH3 Dispersion forces, Dipole-dipole, H-bonding H20 Dispersion forces, dipole-dipole, H-bonding CCl2F2 Dispersion forces Dipole-dipole PF 5 Dispersion forces SF4 Dispersion forces, Dipole-dipole I3- Dispersion forces SF6 Dispersion forces BrF5 Dispersion forces, Dipole-dipole XeF4 Dispersion forces CH2CHCHC H2 Dispersion forces CH2CCHCH CH2 Dispersion forces NH2CN Dispersion forces, Dipole-dipole, H-bonding For the chart shown at the right, the strongest force present in the molecule is *An O-O bond would be considered non-polar, but
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Unformatted text preview: ozone is still a polar molecule. How? This is because of the bent geometry of the molecule and the fact that the central O has a different electron density than the side oxygen atoms. (This is due to the different number of bonds and lone pairs on this central oxygen atom as compared to the side atoms.) That said, I will not expect you to figure out the polarity of molecules such as this that consist of just one type of atom bonded together. Hence, I would not expect you to predict that ozone has dipole-dipole interactions. You should be able to predict the dispersion interactions....
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This note was uploaded on 09/19/2011 for the course CH 301 taught by Professor Fakhreddine/lyon during the Fall '07 term at University of Texas at Austin.

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