1. Intermolecular Forces

2. Gecko Feet
Gecko Feet

3. Gecko Feet Facts
These tiny setae are only as long as 2 diameters of a human hair. That’s 100 millionths of a meter long.

4. Gecko Feet Facts Each seta ends in up to 1000 even tinier tips.
The tips are only 200 billionths of a meter wide –below the wavelength of visible light.
setae

5. Gecko Feet Facts
A million setae could lift the weight of a child (20kg, 45lbs). A million setae could easily fit onto the area of a dime.

6. Gecko Feet Facts
Gecko-inspired adhesive

7. Intermolecular Forces
Van der Waal’s forces
Dipole/dipole
Ion/dipole
Dispersion (London forces)
Hydrogen bonds
These are all weaker than ionic or covalent bonds (intramolecular forces.)

8. Van der Waal’s Dipole-dipole forces occur between polar molecules.
Weaker forces may also be induced.

9. Van der Waal’s
Occur between nonpolar molecules
Transient

10. Van der Waal’s
Dispersion forces increase as the number of molecules increase, but are still the weakest force.

11. What does it matter?
Cl2 and Br2 have approximately the same shape and neither is polar.
Upon cooling, both Cl2 and Br2 form solids. Why?
At 25oC, chlorine (Cl2) is a gas whereas bromine (Br2) is a liquid. Why?

12. Ion-dipole attraction
This is what makes water a great solvent for ionic and polar substances.
Dissolving

13. Hydrogen Bonds
Occur between H bonded to a strong electronegative atom and another electronegative atom on a different molecule.
Strongest type of intermolecular forces.
Boiling point trend

14. Hydrogen bonds

15. Relative strength Dispersion < dipole/dipole < hydrogen
forces interactions bonds
Typical strengths for chemical bonds (ionic, covalent, metallic) are in the range of hundreds or thousands of kilojoules per mole. Intermolecular forces are usually less than 50 kJ/mol.

16. Examples

17. Examples