Regent’s Warm-Up What is the electron configuration of a sulfur atom in the ground state?



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Regent’s Warm-Up

  • What is the electron configuration of a sulfur atom in the ground state?

  • (1) 2–4 (3) 2–8–4

  • (2) 2–6 (4) 2–8–6


Regent’s Warm-Up

  • What is the electron configuration of a sulfur atom in the ground state?

  • (1) 2–4 (3) 2–8–4

  • (2) 2–6 (4) 2–8–6



Oxidation Reduction Reactions

  • s



Oxidation Reduction Reactions

  • Purifying metals (e.g. Al, Na, Li)

  • Producing gases (e.g. Cl2, O2, H2)

  • Electroplating metals

  • Electrical production (batteries, fuel cells)



Oxidation Reduction Reactions



Oxidation Reduction Reactions

  • Classical Definitions

  • Reduction – the removal of O2 from a substance

  • Example:

  • CuO(aq) + H2(g)  Cu(s) + H2O(l)

  • H2 is the REDUCING AGENT

  • CuO loses oxygen and is reduced



Oxidation Reduction Reactions

  • Current Definitions

  • Take into account the charge of the ions and atoms involved in the reaction

  • Oxidation – the Loss of Electrons

  • Example: 2Mg0 + O20  2Mg+2O-2

  • The oxidation # of Mg goes from 0 to +2

  • Since Mg0 lost 2e-s, Mg0 is OXIDIZED

    • 2Mg0  2Mg+2 + 4e-


Oxidation Reduction Reactions

  • Current Definitions

  • Reductionthe Gain of Electrons

  • Example: Cu+2O-2 + H20  Cu0 + H2+1O-2

  • If you look closely oxygen is not reacting, its oxidation # stays the same (-2)

  • Copper goes from Cu+2 to Cu0

  • Copper gains 2e-s & is REDUCED

  • Cu+2 + 2e-s  Cu0



Oxidation Reduction Reactions

  • What is the MAIN

  • difference between the

  • classical and current

  • definitions?

  • *Oxygen is NOT

  • required in the current

  • definition*



Oxidation Reduction Reactions

  • Oxidation and Reduction reactions are opposite processes that occur simultaneously

  • For something to lose an electron there must be something else that wants to gain that electron





Oxidation Reduction Reactions

  • Loss of Electrons is Oxidation

  • Gain of Electrons is Reduction



Oxidation Reduction Reactions

  • The substance that loses electrons is OXIDIZED and is the REDUCING AGENT

  • The substance that gains electrons is REDUCED and is the OXIDIZING AGENT



Oxidation Reduction Reactions

  • Which half-reaction

  • correctly represents

  • reduction?

  • 1. Ag --> Ag+ + e-

  • 2. Au3+ + 3e- --> Au

  • 3. F2 --> 2 F- + 2e-

  • 4. Fe2+ + e- --> Fe3+



Oxidation Reduction Reactions

  • Given the balanced equation representing a redox reaction: 2Al + 3Cu2+ --> 2Al3+ + 3Cu

  • Which statement is true about this reaction?

  • 1. Each Al loses 2e- and each Cu2+ gains 3e-.

  • 2. Each Al3+ gains 2e- and each Cu loses 3e-.

  • 3. Each Al loses 3e- and each Cu2+ gains 2e-.

  • 4. Each Al3+ gains 3e- and each Cu loses 2e-.



Oxidation Reduction Reactions

  • Given the reaction shown: Which species undergoes oxidation?

  • 1. Mg(s)

  • 2. Cl-(aq)

  • 3. H+(aq)

  • 4. H2(g)



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