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Intermolecular Forces and Intramolecular Forces

Intermolecular Forces and Intramolecular Forces. Chapter 6.2. Definitions. Intermolecular: T he forces that bond molecules to each other. Intramolecular: T he forces that bond atoms to each other within a molecule. Intramolecular Vs. Intermolecular Forces.

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Intermolecular Forces and Intramolecular Forces

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  1. Intermolecular Forces and Intramolecular Forces Chapter 6.2

  2. Definitions • Intermolecular: • The forces that bond molecules to each other. • Intramolecular: • The forces that bond atoms to each other within a molecule.

  3. Intramolecular Vs. Intermolecular Forces The bonds made by Intramolecular forces are much stronger than the bonds made by Intermolecular forces.

  4. Intramolecular Forces • Three main types listed in order of strength: • Ionic • Sodium Chloride (salt, Na+Cl-) • Covalent • Hydrogen (H-H), Methane (CH4) • Metallic • Na+, Mg2+ Page 209 of your book has a table with all forces listed in order of strength.

  5. Intermolecular Forces • Listed from weakest to strongest • Dispersion (London) • Dipole-Induced Dipole • Ion-Induced Dipole • Dipole-Dipole • Hydrogen Bonding • Ion-Dipole

  6. Dispersion (London) Forces Fritz London 1900 - 1954 • A weak intermolecular force of attraction that is present between all molecules due to temporary dipoles. • Increases as molecular weight increases. • More electrons present • Outermost electrons not as tightly held to the nucleus. • The bigger the molecule, less prominent and accessible polar regions are.

  7. Dipole-Induced Dipole The charge on a polar molecule is responsible for inducing the charge on the non-polar molecule.

  8. Ion-Induced Dipole • This results when an ion in close proximity to a non-polar molecule distorts the electron density of the non-polar molecule. • Ex. Fe2+ and O2

  9. Dipole-Dipole Forces HCl interacting with another HCl Is the electrostatic attractions between oppositely charged ends of a polar molecule.

  10. Hydrogen Bonding • the strong intermolecular attraction between the nucleus of a hydrogen atom, bonded to an atom of a highly electronegative element such as oxygen (as in water), and the negative end of a dipole nearby. • Only happens with H’s bonded to Oxygen, Fluorine and Nitrogen. • Solid water floats in liquid water. How come this is important?

  11. Ion Dipole The force of attraction between an ion and a polar molecule.

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