1. Hydrogen Bonding Learning intention
Learn about this strong type of intermolecular forces which exists between molecules containing N-H, O-H or F-H bonds.

2. Relating physical properties to intermolecular forces
Learning intention
Learn how to explain differences in physical properties such as viscosity, melting point and boiling point in terms of differences in strength of intermolecular forces.

3. Intermolecular - Hydrogen Bonding
Consider the compounds formed between elements in group 4 of the Periodic table and hydrogen
The group 4 hydrides are CH4, SiH4, GeH4, SnH4
They are all covalent molecular so have low melting points and boiling points.

4. The boiling point increases as you go down the group.

5. As you go down the group the central atom gets bigger.
There are more electrons so a greater chance of an uneven distribution of electrons within the atom.
The London’s forces between the molecules gets stronger as you go down the group.
More energy is needed to separate the molecules from each other.

6. Intermolecular – Hydrogen Bonding
A similar pattern would be expected in the other covalent molecular hydrides
The group 5 hydrides NH3, PH3, AsH3 and SbH3
The group 6 hydrides H2O, H2S, H2Se and H2Te
The group 7 hydrides HF, HCl, HBr and HI

7. NH3, has a higher boiling point than expected.

8. H2O has a higher boiling point than expected.

9. HF has a higher boiling point than expected.

10. Intermolecular - Hydrogen Bonding
H2O HF
NH3
It is more difficult to separate NH3, H2O and HF molecules from each other than expected.

11. Intermolecular - Hydrogen Bonding
These compounds all have H atoms directly bonded to very electronegative atoms.
In HF the H-F bond is polar covalent.
The F has a much higher electronegativity than H.
The pair of shared electrons in the covalent bond spend more time closer to the fluorine than the hydrogen.
The H-F bond is polar. Hδ+ - Fδ-

12. Intermolecular - Hydrogen Bonding
The HF molecules can attract each other
Hδ+ - Fδ-
Hδ+ - Fδ-
Hδ+ - Fδ-
This is called hydrogen bonding.
Hydrogen bonding is weak but is stronger than very weak London’s forces.

13. Intermolecular - Hydrogen Bonding
NH3 has H atoms directly bonded to very electronegative N atoms.
There are Hydrogen bonds as well as London’s forces between the ammonia molecules.
N-
H+ H+ H+
H+
N- H+
N H+
H+ H+

14. Intermolecular - Hydrogen Bonding
H2O has H atoms directly bonded to very electronegative O atoms.
There are Hydrogen bonds as well as London’s forces between the water molecules.
O-
H+ H+
H+O-
H+
O H+
H+

15. Proteins consist of long chain atoms containing polar C=O and H-N bonds. Hydrogen bonds help give enzymes their shape.

16. Water O H Oxygen has 2 lone pairs of electrons which can form- O H + +
Oxygen has 2 lone pairs of electrons which can form
a hydrogen bonds with two hydrogen atoms.
Each water molecule, in theory, could be surrounded
by 4 hydrogen bonds

17. Hydrogen bonding in water

18. Water
Density of water
Water has its greatest density at a temperature of 4oC. When, as water cools further, the molecules start to move further apart, due to the hydrogen bonding, until a more open structure is formed at its freezing point. So ice floats!!
New Higher Chemistry E Allan J Harris

19. Video trends\3dwater.wmv
Water 3D model

20. Hydrogen bonding in ice
Hydrogen bonding in solid water gives rise to an open structure. This is why ice is less dense than liquid water.

22. Hydrogen bonding is also responsible for holding the two strands of nucleic acids together in DNA

23. Viscosity
Viscosity is related to the molecular mass and the number of –OH present.
Hydrogen bonding between the molecules will increase its viscosity.
Density of water
New Higher Chemistry E Allan J Harris

24. Water
Surface tension
Water has a high surface tension. The molecules on the surface
have in effect, hydrogen bonds. This has the effect of pulling
the surface molecules closer together.

25. Bond Strengths Bond Type Strength (kJ mol –1) Metallic 80 to 600 Ionic
Covalent
Hydrogen 40
Dipole-Dipole 30
London’s forces
1 to 20

26. Behaviour in electrical fields
Video clip
New Higher Chemistry E Allan J Harris

27. Nappies
Cloth nappies cost between £100-£400 as opposed to disposable at £800-£1,200 for the 2.5 years of normal nappy use.
3 billion nappies are thrown away in the UK each year with 90% going to landfill. They can take up to 500 years to decompose.
Disposables make up 4% of total household waste and up to 50% of that of families with one baby
Disposable nappies use up to 5 times more energy to produce than cotton ones – that's including the washing process .
Seven million trees are felled every year in Canada and Scandinavia to supply the pulp for disposables sold in the UK. 27

28. Disposable nappy

29. Sodium polyacrylate is a polymer with a molecular weight of over one million!
sodium carboxylate
Chemical Background
Groups called sodium carboxylate are attached along the backbone. 29

30. - Sodium poly(acrylate) absorbs 500 times its own mass of water. water+ +
Na+ -

31. - Sodium poly(acrylate) absorbs 500 times its own mass of water. + + +

32. Sodium poly(acrylate) absorbs 500 times its own mass of water.- - - - - -

33. Predicting solubility from solute and solvent polarities
Learning intention
Learn how the polarity of both the solute and solvent molecules influences solubility.

34. Solvent Action

35. Solvent Action
A liquid that a substance dissolves in is called a SOLVENT.
Solvents can be either polar or non-polar molecules.
Immiscible liquids do not mix, e.g. oil and water, however,
non-polar liquids are miscible with each other.
Polar solvents will usually dissolve polar molecules.
Non-polar solvents will usually dissolve non-polar molecules.
Water is a polar molecule so it is a polar solvent.
Water has a polar covalent bonding
between O and H. + + - H O - H +

36. Dissolving in Water Ionic Compound dissolving in water - + - +- + - + - - + + - +
Hydrated
ions

37. Dissolving in Water

38. Dissolving in Water
Pure Hydrogen chloride is polar covalent. When water is added it breaks to produce ions - + + -
H Cl - +
Cl- - + + - H+
Hydrated
ions

39. Dissolving in Water
Generally, covalent molecules are insoluble in water. However, small molecules
like ethanol (C2H5OH), with a polar O-H functional group, will dissolve,
Ethanol - +
H2O + O H C -

40. Dissolving salt
solubility KMnO4 and I2(upper layer is water solvent lower layer is hexane)