1. Intermolecular Forces: relationships between molecules

2. Polarity and Shape
Polar bonds do not necessarily always create a polar molecule.
The shape of the molecule and the polarity of each bond is considered before stating if a molecule is considered POLAR or NON-POLAR
We will watch a 5 minute explanation to help us understand this difficult concept
major intermolecular forces

4. Intramolecular forces intra = inside
Intramolecular forces: forces that bond the atoms to each other within the molecule.
COVALENT BONDS!!!

5. Intermolecular Forces inter = between
Forces affecting the relationships between molecules
London Forces (Dispersion Forces) AKA van der Waals forces
Dipole-Dipole Interactions
Ion-dipole forces
Hydrogen Bonding

6. London (dispersion) Forces aka van Der Waals forces
weakest intermolecular force
occurs between all types of molecules
It is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles

7. London Dispersion forces in a molecule
These instantaneous dipoles may be induced and stabilized as an ion or a polar molecule approaches the non-polar molecule.

8. Dipole-Dipole Forces Dipole = polar molecule
Molecules with dipoles will change their direction so that their oppositely charged ends are near to one another.
The electrostatic attraction between the ends is dipole-dipole force

9. Orientation of Polar Molecules in a Solid
Dipole-Dipole Forces
Attractive forces between polar molecules
Orientation of Polar Molecules in a Solid
11.2

10. Dipole - Dipole Interactions

11. Ion Dipole Forces (the reason why ionic compounds dissolve in water)
The force of attraction between an ion and a polar molecule.
NaCl breaks up because the ion dipole with water is stronger than the attraction of Na+ to Cl-

12. Polar molecules can interact with ions:
Ion - Dipole Interactions

13. The Hydrogen Bond

14. A hydrogen bond is the strongest form of dipole-dipole interaction.
A hydrogen bond is formed between polar molecules that contain hydrogen covalently bonded to the small, highly electronegative atoms, F, O, or N.
F—H
O—H
N—H

15. A molecule containing this combination of atoms, will be attracted to another molecule with the same atom combination.
A strong attractive force between the two molecules which is called a hydrogen bond is formed.
hydrogen bond
covalent bond
covalent bond

16. water has the lowest molar mass water has the highest heat of fusion
water has the highest melting point
water has the highest boiling point
water has the highest heat of vaporization
The melting point, boiling point, heat of fusion and heat of vaporization of water are extremely high and do not fit the trend of properties relative to molar mass within Group 17.

17. Hydrogen bonding in water animation
hydrogen bonding animation
Water exhibits these unusual properties because of hydrogen bonding between water molecules.

18. Why do we care about intermolecular forces?
The forces that act on molecules determine their physical properties
Strong intermolecular forces between molecules increase melting and boiling points because it is these forces that are broken when substances change state.

19. Polarity and Boiling Point:
The polarity of the molecules determines the forces of attraction between the molecules in the liquid state.
Polar molecules are attracted by the opposite charge effect (the positive end of one molecule is attracted to the negative end of another molecule).
Molecules have different degrees of polarity as determined by the functional group present.
The greater the forces of attraction the higher the boiling point or the greater the polarity the higher the boiling point.

20. What is boiling point?
Boiling point is the temperature at which a liquid turns into a gas (or vapour).
For a liquid to turn into a gas, intermolecular forces must be broken.
The stronger the intermolecular forces, the higher the boiling point of a substance.

21. The evidence for hydrogen bonding
Many elements form compounds with hydrogen - referred to as "hydrides".
If you plot the boiling points of the hydrides of the Group 4 elements, you find that the boiling points increase as you go down the group.
The increase in boiling point happens because the molecules are getting larger with more electrons, and so van der Waals dispersion forces become greater.

22. The evidence for hydrogen bonding
If you repeat this exercise with the hydrides of elements in Groups 5, 6 and 7, something odd happens.

23. Solubility and Intermolecular Forces
Like dissolves like
Polar solutes dissolve in polar solvents
Nonpolar solutes dissolve in nonpolar solvents
Molecules with similar intermolecular forces will mix freely

24. Ionic Solute with Polar Solvent

25. Ionic Solute with Nonpolar Solvent

26. Nonpolar Solute with Nonpolar Solvent

27. Nonpolar Solute with Polar Solvent

30. Comparison of the Properties of Substances with Ionic, Covalent, Metallic or Intermolecular Bonds
Bond strength
Strong
Very strong
Variable strength, generallymoderate
Weak
Hardness
Moderate to high
Insulators in solids and liquid states
Low to moderate; ductile, malleable
Crystal soft and somewhat plastic
Electrical conductivity
Conducts by ion transport, but only when liquid or dissociated
Low
Good conductors; conducts by electron transport
Insulators in both solid and liquid states
Melting point
Very high
Generally high
Solubility
Soluble in polar solvents
Very low solubility
Insoluble except in acids or alkalis by chemical reaction
Soluble in organic solvents
Examples
Most minerals
Diamond, oxygen, hydrogen, organic molecules
Cu, Ag, Au, other metals
Organic compounds

31. Boiling Point of Various Material (˚C)
Noble gas
Helium neon argon
He Ne Ar
Nonpolar covalent
hydrogen oxygen methane chlorine
H2 O2 CH4 Cl2
polar covalent
ammonia hydrogen fluoride water
NH3 HF
H2O
100
ionic
potassium chloride sodium chloride magnesium oxide
KCl
NaCl
MgO
771
1413
2826
metallic
copper iron tungsten
Cu Fe W