1. Chemical Reactions Ch 5.1, 5.2, 5.3 starting at page 141
Chemical Reactions wiki
Questions 1-14 page 147
Chemical Equations - Part A Youtube 10 mins
Chemical equations – Part B Youtube 9 mins

2. Ch 5.1 page 142 – What is a Chemical Equation?
Chemical equation: a short-hand notation that scientists use to communicate what happens during a chemical reaction
Word equation: involves replacing the reactants and products with their chemical names.

3. Formula equation – uses the chemical formulas for the reactants and products.
Copy the formula

5. Showing states of matter

6. Balanced chemical equations pg 143
Copy this section including the definition and description below

7. Read the instructions but copy the equations and working. P 143

8. Read the instructions but copy the equations and working. P 143

9. Draw simple stick models. P 144

10. Read the instructions but copy the equations and working. P 144

11. Chemical equations – Part B
Youtube 9 mins
Read each instruction/thinking process, then write the equation as directed on page 145. Then do the interactive – Balancing Equations
Review Q’s 1-14 page 147

12. 5.2 page 149 Classifying chemical reactions
Decomposition reactions
Combination reactions
Precipitation reactions
Oxidation and Reduction reactions
Extraction of Metals
As you finish the notes – go on with the Unit Review questions on page 158 – answer in full sentences where appropriate. Q 1-21 (leave out Q 16)

13. Copy all of the above + the reaction to the right

14. Copy the definition above + the blue reactions to the right

15. Copy the definition above.

16. Copy these notes in total.

17. Page 152

18. We are not doing the section on predicting precipitates on page 152

19. Naming Ionic Compounds page152
To name Ionic compounds simply place the cation first and the anion second
Ammonium, hydrogen carbonate, carbonate, nitrate and phosphate are poly-atomic ions – they are treated as a single entity with a set of brackets around the ion.

20. Crossover rule – Balanced ionic compounds
Cross-over rule youtube - 5 mins
The superscript eg 3+ represents the ionic charge.
The subscript number represents the number of atoms of each ion in the neutral compound.
A number in front is call a coefficient that multiplies all atoms in the molecule.

21. Write balanced ionic formulae for the following ion compounds (page 152 or your notes)
Hydrogen fluoride Sodium hydrogen carbonate Calcium nitride
Potassium oxide Magnesium sulfate Potassium iodide
Ammonium bromide Iron (III) oxide Barium hydroxide

22. Oxidation and reduction reactions page 153
Oxidation: when a substance gains oxygen atoms or loses electrons
Reduction: when a substance loses oxygen atoms or gains electrons
Redox: an abbreviation for oxidation and reduction pairs of reactions

23. Oxidation – combustion page 153
Combustion reaction: any chemical reaction where a substance burns in oxygen to produce heat and light.
Read the explanation below and copy the equations.

24. Oxidation – Corrosion page 154
Corrosion is a natural process, which converts refined metal to their more stable oxide. It is the gradual destruction of materials (usually metals) by chemical reaction with their environment. In the most common use of the word, this means electrochemical oxidation of metal (rusting) in reaction with an oxidant such as oxygen.

25. Read the explanation and copy the equations.

26. Reduction reactions page 154
Copy the definition, then read the explanation and copy the equations.

27. Read the explanation and copy the blue definitions.

28. Metal displacement (redox) reactions page 154
Read the explanation and copy the equations.

29. For replacement reactions to occur, the solid metal (Zn) must be higher on the reactivity scale than the ionic solution ion (Cu) for this REDOX reaction to occur.
Zn transfers electrons to Cu++ ions, therefore Zn has been oxidized to Zn+ (OILRIG).
Cu++ ions have been reduced as it has gained electrons to become Copper metal crystals (OILRIG).

30. Extraction of metals
Activity series plays a large role in the extraction of metals.
Highly reactive metals such as K, Na and Mg are usually found in compounds or as ions – therefore must be extracted by electrolysis – electrons are forced into the ions, reducing them to their pure element.
The least reactive metals such as Ag and Au rarely form compounds and are regularly found as pure elements in nature – froth floatation can be used for these P 156.
Zn, Fe, Pb, Sn, Cu can all be extracted by carbon reduction (heat and carbon)

31. Copy the definition below, then read the explanation and copy the equations.

32. Electrolysis page 157
Reduction
Oxidation
REDOX

33. Ch 5.3 Rates of Chemical reactions
Reaction rates can be affected by the following factors. Increasing the following will increase reaction rates by increasing the likelihood of particles interacting with one another.
Temperature
Concentration
Surface area
Agitation
Catalysts such as enzymes increase the rate but are not consumed by the reaction.