Chem Final Exam

Oxidation

Loss of Electrons

Reduction

Gain of Electrons

Oxidizing Agent

Something that takes the electrons from something else (reducing itself)

Reducing Agent

Something that gives electrons to something else (oxidizing itself)

Steps to balancing complex redox reactions

1) Write the skeletal equation for oxidation and reduction half-reactions

2) Balance each half-reaction for all elements except H and O

3) Balance each half-reaction for O by adding H₂O

4) Balance each half-reaction for H by adding H+

5) Balance each half reaction for charge by adding electrons

6) If necessary, multiply one or both half-reactions so that the number of electrons consumed one is equal to the number produced in the other

7) Add the two half-reactions and simplify both sides

8) If the reaction takes place in basic conditions, add OH- ions to the equation from Step 7 to neutralize the H+ ions (add in equal numbers to both sides of the equation) and simplify

What needs to balance out on either side of a reaction equation?

1) Molecular formulas (atoms!)

2) Charges and electrons

What are the units to the Standard Reduction Potential, or E⁰?

V (volts)

Anode: Ox or Red?

Oxidation rxn

Cathode: Ox or Red?

Reduction rxn

Oxidation rxn: Cathode or Anode?

Anode

Reduction rxn: Cathode or Anode?

Cathode