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Label each reaction as Oxidation or Reduction

Co 0 → Co +2 + 2 e N 0 + 3 e → N -3 Br 0 + 1 e → Br -1 Ni 0 → Ni +3 + 3 e Ag 0 → Ag +1 + 1 e. Sr 0 → Sr +2 + 2 e Se 0 + 2 e → Se -2 Sb 0 + 3 e → Sb -3 Fe 0 → Fe +2 + 2 e W 0 → W +6 + 6 e. Label each reaction as Oxidation or Reduction.

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Label each reaction as Oxidation or Reduction

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  1. Co0 → Co+2 + 2 e N0 + 3 e → N-3 Br0 + 1 e → Br-1 Ni0 → Ni+3 + 3 e Ag0 → Ag+1 + 1 e Sr0 → Sr+2 + 2 e Se0 + 2 e → Se-2 Sb0 + 3 e → Sb-3 Fe0 → Fe+2 + 2 e W0 → W+6 + 6 e Label each reaction as Oxidation or Reduction Do metals or nonmetals tend to gain e and be reduced? Nonmetals Do metals or nonmetals tend to lose e and be oxidized? Metals

  2. Co0 → Co+2 + 2 e N0 + 3 e → N-3 Br0 + 1 e → Br-1 Ni0 → Ni+3 + 3 e Ag0 → Ag+1 + 1 e Sr0 → Sr+2 + 2 e Se0 + 2 e → Se-2 Sb0 + 3 e → Sb-3 Fe0 → Fe+2 + 2 e W0 → W+6 + 6 e Label the element in the reactions as an oxidizing agent or a reducing agent: Do metals tend to be oxidizers or reducing agents? Metals Do non-metals tend to be oxidizers or reducing agents? Nonmetals

  3. Extra one for practice Done in class

  4. Galvanic / Voltaic A galvanic cell is one in which a redox reaction takes place spontaneously to produce electricity. Chemical energy is changed to electrical energy.  

  5. Electrolytic Cell An electrolytic cell is one in which electrolysis occurs, a compound is decomposed by passing electricity through it. The reaction occurring is not spontaneous, it is forced by applying a voltage (electricity). Electrical energy is converted to chemical energy

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