1. INTERMOLECULAR FORCES
What Holds Molecules to Each Other

2. Types of Bonds
Recall that there are three fundamental types of bonding.
Ionic bonding
Covalent bonding
Metallic bonding

3. Types of Bonds
Because ionic and covalent bonding uses electrostatic attractions between areas of full charge, the resulting force of attraction is strong.
Ionic bonds are held together by attractions between cations and anions.

4. Types of Bonds
Covalent bonds are held together by attractions between positive nuclei and the negative electron clouds that reside between them.

5. Types of Bonds
The results of these bonding processes are the strongest, commonly used, mechanisms for attaching atoms to one another.

6. Intermolecular Forces
Intermolecular forces are a secondary method of holding a structure together.
As the name implies, these are forces that exist BETWEEN molecules. Bonds exist WITHIN molecules.

7. Intermolecular Forces
Intermolecular forces are only associated with systems that use covalent bonding within the molecules.
Intermolecular forces are not encountered in systems that employ ionic bonding.

8. Intermolecular Forces
Some elements, such as the Noble Gases, exist with intermolecular forces and no bonding at all.
Intermolecular forces are what make solid and liquid molecular compounds possible.

9. Intermolecular Forces
Intermolecular forces exist in three different levels of strength.
The three intermolecular forces (from strongest to weakest) are hydrogen bonding, dipole–dipole forces and London dispersion forces.

10. Intermolecular Forces
Polar molecules will have a partially positive side and a partially negative side, or a dipole.
The partial positive on one molecule will be attracted to the partial negative on a second molecule.
This attraction is an intermolecular force.

11. Intermolecular Forces
Because the molecules are polar, the force is either a dipole-dipole attraction or a Hydrogen bond.

12. Intermolecular Forces
Because these attractions are between areas of partial charge, they will produce weak forces of attraction.
A system that has this mechanism holding the structure together will break up relatively easily.

13. Intermolecular Forces
It will always break at the weak links – the dipole-dipole forces or Hydrogen bonds.
The covalent bonds will remain intact.

14. Hydrogen Bonding
The difference between dipole-dipole forces and Hydrogen bonding is subtle.
When hydrogen is directly bonded to nitrogen, oxygen or fluorine, then the system will be capable of Hydrogen bonding.

15. Hydrogen Bonding
In these systems, the difference between the electronegativity values of the bonded atoms will produce fairly large partial charges.
As a result, the resulting intermolecular forces will be strong. They will still not be as strong as a true bond, however.

16. Hydrogen Bonding

18. Dipole-Dipole Forces
Attractions between oppositely charged regions of polar molecules are called dipole–dipole forces.

19. Dipole-Dipole Forces
Dipole-dipole forces exclude those molecules covered by Hydrogen bonding.
Hydrogen bonding intermolecular forces are about 10 times stronger than dipole-dipole forces because they involve large differences in electronegativity, thus creating a large electric dipole.

20. Dipole-Dipole Forces
Dipole-dipole forces depend on the number of electrons.
Bigger molecules result in more electrons, and more electrons mean stronger forces.

21. London Dispersion Forces
Dispersion forces are weak forces that result from temporary shifts in the density of electrons in electron clouds.

22. London Dispersion Forces
The electron density around each nucleus is, for a moment, greater in one region of each cloud.

23. London Dispersion Forces
As a result each molecule forms a temporary dipole.

24. London Dispersion Forces
When temporary dipoles are close together, a weak dispersion force exists between oppositely charged regions of the dipoles.
Due to the temporary nature of the dipoles, dispersion forces are the weakest intermolecular force.

25. London Dispersion Forces
Dispersion forces exist between noble gases and compounds that are nonpolar.

26. London Dispersion Forces
Dispersion forces increase as the mass of the molecule increases.
C2H6 (MW = 30.0 g/mol) has stronger dispersion forces than CH4
(MW = 16.0 g/mol).

27. Intermolecular Forces
To determine what type of intermolecular force a compound has, ask yourself the following questions.
1) Does the compound contain hydrogen attached to N, O, or F?
If yes, the force is hydrogen bonding.

28. Intermolecular Forces
Determine the number of bonds from the Wetter Way and draw the dash-dot diagram.

29. Intermolecular Forces
2) Does the central element of the compound contain any lone pairs of electrons or are different elements attached to the central atom?
If yes, the force is dipole-dipole.
If no, the force is London dispersion.

30. Problem
1) Determine the type of intermolecular force in each of the following compounds.
a) BCl3
dispersion
b) Xe
dispersion

31. Problem
Determine the type of intermolecular force in each of the following compounds.
c) NH3
hydrogen bonding
d) CH4
dispersion

32. Problem
Determine the type of intermolecular force in each of the following compounds.
e) SO2
dipole-dipole
f) H2
dispersion

33. Problem
Determine the type of intermolecular force in each of the following compounds.
g) SO3
dispersion
h) CH3Cl
dipole-dipole

34. Problem
Determine the type of intermolecular force in each of the following compounds.
i) HF
hydrogen bonding
j) HBr
dipole-dipole