VCE Chemistry Unit 2.1

1. VCE ChemistryUnit 2.1 Water as a solvent http://highered.mcgraw-hill.com/sites/0072410159/student_view0/chapter5/figures_alive_.html

2. Put sound on

3. Water • Is essential to life. • Covers 70% of earth’s crust, but only 1% is drinkable. • In ocean, atmosphere and on land. • Found naturally as gas, liquid or solid. • 67% of our body.

4. What do you know already about • Physical properties? • Structure and bonding?

5. Physical Properties • Colourless,odourless liquid at 25oC • Relativelyhigh melting(0oC) and boiling temperature(100oC) • High heat capacity-Requires a lot of energy to heat it up • High latent heat • Water expands when frozen • Density of ice less than water • Non-conductor • Good solvent for polar compounds

6. Bonding Polar molecule Discrete molecular compound covalent intramolecular bonding bent

7. Bonding Between Water Molecules • Most properties can be explained because of the hydrogen bondingbetween the molecules. (Intermolecular)

8. Bonding Between Water Molecules • Oxygen is much more electronegative than hydrogen. • Water forms polar molecules because electrons are more strongly attracted to the oxygen atom.

9. Hydrogen Bonding

10. Melting and Boiling Temperatures • Are higher than similar substances. • This is because of the relatively high hydrogen bonding forces.

11. Specific Heat Capacity • = energy needed to raise the temperature of 1g of the substance by 1oC. • It takes 4.19 J to raise the temperature of 1g water by 1oC. • Water requires a large amount of heat to increase its temperature because energy is needed to overcome the H-bonds.

12. Latent Heat • Amount of heat needed to change the state of a substance. • E.g. When heating ice the temperature remains constant until the ice is melted. • Water has a high latent heat because of the hydrogen bonding holding the molecules together.

13. Latent Heat Latent heat of fusion. Energy needed to melt a substance. Latent heat of vaporisation. Energy needed to vaporize a substance.

14. Expansion on Freezing • The regular arrangement of water molecules in ice takes up more space than the irregular arrangement in liquids. • Density of ice < density of water.

15. Water Molecules in Ice

16. Water As a Solvent • Water will dissolve many substances • Solutions in water are aqueous solutions (aq).

17. Solution Chemistry In order for substance to dissolve: • The particles of the solute are separated from each other. • The particles of the solvent are separated from each other. • The solvent and solute particles attract each other.

18. Substances That Dissolve 1. Molecular compounds that A) form hydrogen bonds B) ionise 2. Ionic compounds that dissociate

19. Molecular Substances 1 A.Those that can form hydrogen bonds with water.E.G. Ethanol • Both water and ethanol are polar molecules. They are able to mix freely forming hydrogen bonding between the molecules

20. water Animation (long): http://www.mpcfaculty.net/mark_bishop/ethanol_solution.htm hydrogen bonding ethanol

22. Molecular Substances 2 B.Those that ionise in water. E.g. hydrogen chloride • HCl has a highly polarised bond which breaks in water. • This is due to the force of attraction of the water molecules. • Two ions are formed

23. Ionisation • This process is known as IONISATION. • The ions are said to be hydrated. • HCl(g) + H20(l) H30+(aq) + Cl –(aq) Hydronium ion

24. Ionic Compounds • E.g. NaCl • The water molecules are attracted to the ions. They pull the sodium and chloride ions into the surrounding solution.

25. Sodium Chloride

26. Dissolving Salt • H2O is a polar molecule. • The charged regions are attracted to ions with the opposite charge. • Hence, the positively charged regions of water molecules are attracted to Cl- ions, and the negatively charged regions of water molecules are attracted to Na+ ions.

29. When several water molecules surround an ion in the crystal, the sum of the attractive forces between the water molecules and the ion may become strong enough to overcome the attractive forces between the cations and anions in the NaCl crystal.

30. Salt dissolving

31. http://ithacasciencezone.com/chemzone/lessons/03bonding/dissociate.htmhttp://ithacasciencezone.com/chemzone/lessons/03bonding/dissociate.htm Good animations of salt dissolving http://www.elmhurst.edu/~chm/vchembook/171solublesalts.html http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/thermochem/solutionSalt.html

32. Hydration of Ions • The ions are now hydrated. • This is ion-dipole attraction. • When positive and negative ions are separated from one another this called DISSOCIATION.

33. NaCl in Water

34. Hydration of Chloride ion

35. Hydration of Sodium Ion

36. Would you expect these molecules to be polar?

37. Solubility • The maximum amount of a solute that will dissolve in a given quantity of solvent at a particular temperature. • Usually measured as mass of solute in 100 g of water. • A solution in which no more solute will dissolve is called a saturated solution.

38. Solubility Curves • The relationship between solubility and temperature can be represented by a solubility curve. • Each point on the curve represents as saturated solution. No more solute can be dissolved at that temperature. • Saturated solution animation http://www.wwnorton.com/chemistry/tutorials/ch5.htm Demo http://genchem.chem.wisc.edu/demonstrations/Gen_Chem_Pages/11solutionspage/crystallization_from_super.htm

39. Solubility Curves

40. Solubility Rules

41. References • Solubility http://www.mhhe.com/physsci/chemistry/chang7/esp/folder_structure/cl/m2/s3/ Great site http://fc.hwcdsb.edu.on.ca/~shawr/solutions.htm