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Understanding Intermolecular Forces: Polarity, Bonds, and Molecular Interactions

This article explores intermolecular forces that influence the behavior of molecules, focusing on polarity and bond types. We discuss polar bonds characterized by uneven electron sharing and defined by electronegativity differences, leading to polar and nonpolar molecules. The role of induced dipoles and the interactions between polar and nonpolar compounds are explained. Additionally, we highlight special dipole interactions like hydrogen bonding and the mechanics of London dispersion forces, the weakest intermolecular force that arises from electron motion.

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Understanding Intermolecular Forces: Polarity, Bonds, and Molecular Interactions

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Presentation Transcript

  1. Intermolecular Forces The forces in and around a molecule

  2. Polarity • Polar bonds - uneven sharing of electrons • Determined by difference in electronegativity • > 2 - ionic bond • 1-2 - polar • < 1 – nonpolar

  3. Polar Molecules • contain a dipole - one end slightly negative, one slightly positive • Not all polar bonds create polar molecules • Can cancel each other out • Induced Dipole- a polar molecule can ‘induce’ a dipole in a nonpolar compound by attracting its electrons

  4. Special Dipole Interactions • Hydrogen Bonding • hydrogen in a polar covalent bond can be attracted to an unshared electron pair in a nearby molecule • Strongest intermolecular force

  5. London Dispersion Forces • Exist in nonpolar molecules and even noble gas atoms because electrons are in continuous motion • ‘instantaneous’ dipoles form as polar molecules come close- called Van der Waals interactions • More electrons = stronger dispersion forces • Weakest intermolecular force

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