• Like
  • Save
11.2 intermolecular forces
Upcoming SlideShare
Loading in...5

Thanks for flagging this SlideShare!

Oops! An error has occurred.

11.2 intermolecular forces



Published in Education
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Be the first to comment
No Downloads


Total Views
On SlideShare
From Embeds
Number of Embeds



Embeds 0

No embeds

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

    No notes for slide


  • 1. If you cannot draw lewis dot you need to review chapter 6 section 3. (pp. 208-213)
  • 2. Intermolecular Forces are forces between two or more molecules. 11.2 IMF
  • 3. Intermolecular Forces
          • Intermolecular attractions are weaker than ionic & covalent bonds. These attractions determine whether a molecular compound is a gas, a liquid, or a solid.
  • 4. Ionic vs Covalent
    • Ionic compounds have a larger force of attraction than covalent compounds.
    • The larger the charge the stronger the force of attraction.
    • Stronger force of attraction = harder to separate.
      • Higher boiling point
      • Higher melting point
  • 5. 3 Intermolecular Forces
    • Dipole-Dipole
    • Hydrogen Bonds
    • London-Dispersion Forces (LDF)
  • 6. Dipole-Dipole
    • Between polar molecules.
    • More polar = stronger forces.
    • Stronger force = higher boiling point.
  • 7. Hydrogen Bond
    • A form of dipole-dipole.
    • Extra strong.
    • A molecule can H-bond if it contains hydrogen bond to an atom with high electronegativity ( N, O, or F )
  • 8. No one in the corner grabs electrons like us! – N, O, & F N O F
  • 9. London Dispersion Forces (LDF)
    • Nonpolar
    • Weakest of all the IMF.
    • Occur between all molecules.
    • Only temporary.
    • Larger molecules have a larger LDF.
    Partial positive Partial negative
  • 10. These temporary partial charges can cause temporary partial charges on other molecules or atoms. London Dispersion Forces
  • 11. Stronger intermolecular force = a solid at room temperature. dipole-dipole or hydrogen bond usually means solid.
  • 12. Weak intermolecular forces = low boiling and low melting points. Strong intermolecular forces = high melting and high boiling points. Liquids with strong intermolecular forces will hold on to their molecules preventing them from escaping as a vapor.
  • 13.
    • Solid - Strong intermolecular forces hold molecules in a rigid & regular pattern (crystal).
    • Liquid - Some intermolecular forces are overcome and molecules can slip past each other.
    • Gas - Weak intermolecular forces can’t hold molecules together, so each molecule is free and independent.
    States of Matter
  • 14. Intermolecular forces Weakest lower melting point LDF Dipole-dipole H-bonds STRONGEST higher melting point Ionic compounds have even higher melting points because the ionic bond must be overcome to free the ions. Ionic bonds are much stronger than any intermolecular force. Intermolecular Forces