1. I can define oxidation and reduction. (A)

2. I can identify which half of a reaction is oxidation and reduction. (A)

3. I can explain how I identified oxidation and reduction by linking it back to observations. (M)

4. I can balance half equations. (M)

5. I can explain oxidation and reduction linking back to the specific gain/loss of electrons. (M)

7. I can balance full redox equations. (E)

1. Do Now (Day 1) - Collect your beaker from yesterday.

2. Copy down Ms Garlick's iron and copper sulfuric exemplar write up.

3. Practice filling in the Assessment Template for each of the following reactions that you do below. 

   • • Adding magnesium to sulfuric acid 

     • Burning hydrogen gas with oxygen - You will do the experiment for this today, but we'll do the write up in the next lesson (Lesson 3: Extension Redox) because Ms Garlick needs to teach you oxidation numbers to do this one. 

4. Do Now (Day 2) - Week 6 Check-In. Random Question: What was the best gift you ever received?

5. Work on writing up redox answers on the Assessment Template. Remember, you're not expected to complete all of these questions, just do what you need to feel confident for the assessment. 

   • • Magnesium, a grey shiny metal, is burned in oxygen, a colourless gas. A white powder forms. (Note we did this as a practical in class.)

     • Aluminum, a grey shiny metal, is placed in a solution of zinc chloride, a colourless solution. A new type of grey shiny metal forms, replacing the other one and the solution stays colourless. 

     • Magnesium, a grey shiny metal, is placed in a solution of copper sulfate, a blue solution. A pink-brown metal forms, and the solution goes from blue to colourless. 

     • Zinc, a grey shiny metal, is added to a solution of hydrochloric acid, a colourless solution. The grey shiny metal disappears and colourless bubbles form, which are flammable. 

     • Fluorine, a pale yellow gas, is burnt with sodium, a grey shiny metal. A white powder is formed. 

     • Magnesium, a grey shiny metal, is added to a solution of iron (ii) nitrate, a pale green solution. A new type of grey shiny metal forms, replacing the other one and the solution turns colourless.

     • Sulfur, a yellow solid, is burn with zinc, a shiny grey metal, forming a white powder. 

     • Iron, a grey shiny metal, is added to sulfuric acid. The solution turns a pale green colour and colourless bubbles that are flammable form. 

Continue to do practice write ups on the assessment template