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Intermolecular Forces Types Strengths Importance
- 1. What are Intermolecular Forces of Attraction? • We’ve discussed ionic and covalent bonds • involve attractions between atoms • involve the exchange or sharing of electrons between two or more atoms • The resulting molecules have different forces of attraction for one another • These are intermolecular forces
- 2. Why are Intermolecular Forces Important? • They often determine the phase a substance is more likely to be. • Solid, liquid, or gas • Life science applications: DNA
- 3. Types of Intermolecular Forces of Attraction • London (or van der Waals) Forces • Permanent Dipoles • Hydrogen Bonds
- 4. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 5. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 6. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 7. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 8. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 9. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 10. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 11. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 12. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 13. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 14. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 15. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 16. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 17. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 18. London Forces • Weakest force • Instantaneous Dipole • Electrons in constant motion • No permanent positive/ negative region • Strength of force depends on total # of electrons
- 19. Permanent Dipoles • More durable than London Force • Permanent imbalance of e- in molecule • Positive and Negative end • Example: Acetone Acetone
- 20. Hydrogen Bonds • Strongest of all of the intermolecular forces • Must have... • H-N; H-F; or H-O • N, F, O very high EN values • Higher than expected BP, MP Water
- 22. Are There Exceptions? • Yes, the total number of intermolecular forces present is very important • Some waxes (CH -CH -CH ....CH ) have 3 2 2 3 very high melting points despite having only London Forces • SbH has a higher BP than H O 3 2 • How can this be explained?
- 23. A Few Closing Questions... • Describe the bonding in CH3Cl? • CH3-CH2-CH2-OH • What about CH3-CH2-CH2-CH2-CH3? • What force holds the base pairs (C,G,A,T) together in DNA? • Covalent bonds? London forces? Hydrogen Bonds? • Why?
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