9-25-08[lecture8]jr

9-25-08[lecture8]jr - anyway) cancel out since the molecule...

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Chem 116 Lecture #8 Notes 9/25/08 (JR) Summarizing Intermolecular Forces London Dispersion forces are weakest, but depend on size of molecules so these kind of forces dominate for large molecules Dipole-Dipole forces are the next strongest under the London Dispersion, although sometimes Dipole-Dipole forces sometimes can be stronger. Hydrogen bonding is a type is a type of Dipole-Dipole force that is next on the line. The strongest attractive force is Ion-Ion forces. The strength of force holding the molecules together is proportional to the charge magnitude of the individual parts as well as the separation between them. Comparing Substances (Number the Substances from lowest boiling point to highest with 1 being the lowest) - Boiling point depends on the strength of forces (amount of energy needed to break apart the bonds) and also the size of the molecule. 1. CH 4 2. CH 3 OCH 3 3. CH 3 OH 4. CCl 4 CH 4 is a non-polar molecule because its bond dipoles (which are nearly zero
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Unformatted text preview: anyway) cancel out since the molecule is symmetrical. CH 3 OCH 3 is a dipole because the C-O bonds are polar and are not symmetrical around the O atom, but this molecule does not have any hydrogen bonds like CH 3 OH, which makes CH 3 OH a stronger dipole than CH 3 OCH 3 . CCl 4 is a non-polar molecule because it is also is symmetrical, so even though the C-Cl bonds are very polar, the bond polarities cancel out due to symmetry, BUT it is a larger molecule than CH 4 (which has similar properties), and therefore CCl 4 would have a higher boiling point than CH 4 . I-Clicker Questions H 2 O: London Dispersion forces and Hydrogen bonding CO 2 : London Dispersion forces NH 3 : London Dispersion forces and Hydrogen bonding CaCl 2 : Ion-Ion forces and London dispersion forces C 8 H 18 : London Dispersion forces...
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