Chapter 8 Redox reactions - CHAPTER 8 REDOX REACTIONS PN...

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CHAPTER 8: REDOX REACTIONS PN. NURUL IZZA TAIB
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LESSON OUTCOME Upon completion this lesson, you will be able to : 1. Determine the oxidation number of any element in a compound 2. Identify the oxidizing and reducing agents in a redox reactions 3. Balancing redox equations in acidic and basic medium 4. Identify characteristics and examples of redox reactions
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REDOX REACTION § Reduction and oxidation reactions occur simultaneously § A redox reaction involves the changes in oxidation number (or oxidation states) of elements in the reactants and products § Redox reaction can also be defined as reaction involving transfer of electron
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OXIDATION REDUCTION Loss of electrons by a substance Gain of electrons by a substance Increase in oxidation number Decrease in oxidation number
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Example 2Mg (s) + O 2(g) 2MgO (s) § MgO is an ionic compound made up of Mg 2+ and O 2- ions § This process involved two separate steps, loss and gain electrons
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2Mg 2Mg 2+ + 4e - O 2 + 4e - 2O 2- § The loss of four electrons by the two Mg atoms the other being the gain of four electrons by an O 2 molecule § Each of these steps is called a half- reaction, which explicitly shows the electrons involved in a redox reaction
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In the formation of MgO: § Magnesium is oxidized, act as a reducing agent = it donates electrons to oxygen and causes oxygen to be reduced § Oxygen is reduced, act as an oxidizing agent = it accepts electrons from Mg, causing Mg to be oxidized
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OXIDATION NUMBER (O.N) § Each atom in a molecule (or ionic compound) is assigned an oxidation number or oxidation states § Oxidation number, signifies the number of charges the atom would have in a molecule (ionic compound) if electrons were transferred completely.
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Exercise 1 Determine the O.N. of each element: 1. Cr in CrCl 3 2. Cr in Cr 2 O 7 2- 3. N in NO 3 - 4. Cl in HClO
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