Housekeeping: Chapter 9 will take at least two weeks. There's a minimum of 8 lessons and because redox is so difficult, we will take our time. The good news is that I create the mocks, so I won't include anything we haven't officially covered.
I still have not received your IA drafts. The final IA is due December 15, 2016; both hard copy and soft copy to be sent to IB. So IDK what y'all are doing, but if you want feedback, I need those papers this week.
Content Review:
Textbook: Chapter 9
Links: ChemGuide Redox For Dummies Half-Equations
Agenda:
1. Housekeeping
2. Intro to Redox Reactions
3. Half-Equations
Mission 1:
Mission Objectives. You should be able to:
1. Describe redox reaction in terms of electrons lost and gained.
2. Explain oxidation number and know the rules for determining oxidation numbers.
3. Contrast oxidizing agent and reducing agent.
4. Deduce the oxidation state of an atom or ion in a compound.
5. Identify species that are oxidized, species that are reduced, and spectator ions.
The definitions of oxidation and reduction have evolved over the years. They used to mean loss of oxygen/gain of oxygen. However, the definitions have become broader and we now refer to them as loss or gain of electrons. The reason for this is because many chemical processes do not include oxygen, but do undergo oxidation and reduction.
Handy little reference chart can be found HERE.
Oxidation and reduction are complementary processes. Oxidation refers specifically to the loss of electrons. Reduction refers to the gain of electrons. Transferring electrons from one substance to another leads to a flow of electrons, which is nothing but an electric current. Reversing the process (using electricity to drive redox reactions) allows for stable compounds to decompose into their component ions and elements. This process is called electrolysis. Applications of redox reactions are significant because this is the foundation for electrochemistry. Think: batteries. What would happen if there were no batteries?
I still have not received your IA drafts. The final IA is due December 15, 2016; both hard copy and soft copy to be sent to IB. So IDK what y'all are doing, but if you want feedback, I need those papers this week.
Content Review:
Textbook: Chapter 9
Links: ChemGuide Redox For Dummies Half-Equations
Agenda:
1. Housekeeping
2. Intro to Redox Reactions
3. Half-Equations
Mission 1:
Mission Objectives. You should be able to:
1. Describe redox reaction in terms of electrons lost and gained.
2. Explain oxidation number and know the rules for determining oxidation numbers.
3. Contrast oxidizing agent and reducing agent.
4. Deduce the oxidation state of an atom or ion in a compound.
5. Identify species that are oxidized, species that are reduced, and spectator ions.
The definitions of oxidation and reduction have evolved over the years. They used to mean loss of oxygen/gain of oxygen. However, the definitions have become broader and we now refer to them as loss or gain of electrons. The reason for this is because many chemical processes do not include oxygen, but do undergo oxidation and reduction.
Handy little reference chart can be found HERE.
Oxidation and reduction are complementary processes. Oxidation refers specifically to the loss of electrons. Reduction refers to the gain of electrons. Transferring electrons from one substance to another leads to a flow of electrons, which is nothing but an electric current. Reversing the process (using electricity to drive redox reactions) allows for stable compounds to decompose into their component ions and elements. This process is called electrolysis. Applications of redox reactions are significant because this is the foundation for electrochemistry. Think: batteries. What would happen if there were no batteries?
Mission 2:
Mission Objectives. You should be able to:
1. Write redox half-equations.
Mission Objectives. You should be able to:
1. Write redox half-equations.
Sometimes it is necessary to write half equations first if you know the species. You'll have to write the oxidation and reduction parts separately and make sure they're balanced before adding them together to form the full equation. Many of these reactions are aqueous, so water and H+ ions are used to balance the half-equations.
Homework: We will follow the steps on pages 274-275 and work the problems on page 275-276.
Homework: We will follow the steps on pages 274-275 and work the problems on page 275-276.
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