This document discusses various types of intermolecular chemical bonding, including covalent bonds like disulfide bonds, and non-covalent bonds like ion-dipole bonds, dipole-dipole bonds, hydrogen bonds, van der Waals forces, pi-pi complexes, and hydrophobic interactions. It provides examples and diagrams to illustrate each type of bonding.

1. INTERMOLECULAR
CHEMICAL BONDING

2. Covalent Disulfide Bond
Ion-Dipole
Force of attraction between
INTERMOLECULAR molecules.
CHEMICAL BONDING Polar Dipole-Dipole
H-Bonding
Non-Covalent
Vander Waals
Non-Polar Pi-Pi Complex
Hydrophobic

3. Covalent:
Disulfide Bond

4. Covalent: Disulfide Bond
Attraction between cysteine residue.
Linkage is also called an SS-bond or
disulfide bridge.
Overall connectivity is therefore R-S-S-R.

5. Covalent: Disulfide Bond
Formal Depiction of Disulfide Bond
Formation as an Oxidation.

6. Covalent: Disulfide Bond
Cystine, which is Composed of Two
Cysteines Linked by a Disulfide Bond.

7. Non-Covalent:
Polar:
Ion-Dipole

8. Non-Covalent: Polar:
Ion-Dipole
 Attraction between ionic compound and
dipole molecule.
Cations are attracted to the negative end
of a dipole .
Anions are attracted to the positive end of
a dipole.
Ex. a salt in aqueous solvent

9. Non-Covalent: Polar:
Ion-Dipole
An Ion-Dipole Force Exist Between a
Charged Ion and a Polar Molecule.

10. Non-Covalent:
Polar:
Dipole-Dipole

11. Non-Covalent: Polar:
Dipole-Dipole
 Attraction between opposite charges of polar
molecule.
 Polar molecules attract one another when the
partial positive charge on one molecule is near the
partial negative charge on the other molecule
 The polar molecules must be in close proximity for
the dipole-dipole forces to be significant.
 Dipole-dipole forces are weaker than ion-dipole
forces.

12. Non-Covalent: Polar:
Dipole-Dipole
A Dipole-dipole Force Exists Between
Neutral Polar Molecules.

13. Non-Covalent: Polar:
Dipole-Dipole
HCL, With a Dipole-Dipole Force

14. Non-Covalent:
Polar:
Hydrogen Bond

15. Non-Covalent: Polar:
Hydrogen Bond
Force of attraction between H and more
electronegative atom of another molecule:
√ Hydrogen – 2.1 √ Nitrogen – 3.0
√ Oxygen – 3.5 √ Fluorine – 4.0
 considered to be dipole-dipole type
interactions, but are stronger than dipole-
dipole forces.

16. Non-Covalent: Polar:
Hydrogen Bond
 The hydrogen atom has no inner core of electrons, so
the side of the atom facing away from the bond
represents a virtually naked nucleus.
 This positive charge is attracted to the negative charge
of an electronegative atom in a nearby molecule.
 Because the hydrogen atom in a polar bond is electron-
deficient on one side, this side of the hydrogen atom can
get quite close to a neighboring electronegative atom.

17. Non-Covalent: Polar:
Hydrogen Bond
Water, Forming an Extensive Hydrogen Bonding
Network

18. Non-Covalent:
Non-Polar:
Vander Waals

19. Non-Covalent: Non-Polar:
Vander Waals
 Attraction between the proton and
valence electron of another non-polar
molecule.
 Strength of VDW:
SOLID>LIQUID>GAS

20. Non-Covalent:
Non-Polar:
Pi-Pi Complex

21. Non-Covalent: Non-Polar:
Pi-Pi Complex
 Interaction between aromatic molecules.
 Also called pi-pi interaction or plot
stocking.
 Ex. Attraction between benzene and
phenol.

22. Non-Covalent:
Non-Polar:
Hydrophobic

23. Non-Covalent: Non-Polar:
Hydrophobic
HYDROPHOBIC MOLECULES
 Are repelled by water (literally, hydrophobe
means fear of water).
 Includes alkanes, oils, fats, and other greasy
substances.
 Tend to be electrically neutral and non-polar
and work better with neutral and non-polar
solvents.
 Often cluster together when dropped in water.

24. Non-Covalent: Non-Polar:
Hydrophobic
 Interaction between Hydrocarbons or other non-
polar molecules.
 In a hydrophobic interaction, water is rejecting
the hydrophobic molecules in favor of bonding to
itself (intermolecular H-bond).
 Water bonds easily with polar molecules (likes
dissolve likes).
 Since water itself is polar, it will prefer water
molecules (polar) rather than oil molecules
(non-polar).

25. Non-Covalent: Non-Polar:
Hydrophobic
Hydrophobic molecules cluster together
though they're not attracted to each other,
because large numbers of like molecules
are energetically more favorable than
smaller numbers (thermodynamics).

26. Intermolecular Chemical
Bonding Group
Algaba, Beale
Corpuz, Blessy Jane
Damian, Sharmaine
Manlulu, Ivan Joseph
Soriano, Euniqa Dancille
Tiu, Lorraine
>Thank You<