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VanderWaalsForcesfor2B - Br Br Br Br Temporary attraction...

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Jim Hollister LSC/UCDavis Van der Waals Forces I. Ionic Interactions: strongest attractions II. Van der Waals Forces: intermolecular attractions A. Permanent dipole-dipole interactions: H C O H ! ! H C O H ! ! Permanent dipole-dipole interaction 1. H-Bonding: Special case of permanent dipole-dipole interactions: when H is bonded to the highly electronegative elements N, O, or F, H-bonding can occur. H 3 C H O C H 3 H O Hydrogen bonding ( H-bonding raises the boiling point higher than one would expect based on the molecular mass alone. See London Forces below.) B. London Forces: Instantaneous (temporary) dipole-dipole interactions.
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Unformatted text preview: Br Br Br Br ! ! ! ! Temporary attraction between molecules caused by a random electron excess at one Br which makes it a partial negative bromine. It causes one of the adjacent molecule's bromines to be partially positive because of electron repulsions. Boiling pt. α London Forces α number of electrons α molecular mass (or Melting pt. or Δ H of vaporization) α means “proportional to” The higher the molecular mass, the higher the number of electrons in a molecule, the higher the London Forces, the higher the boiling pt. (or Melting pt. or Δ H of vaporization)...
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