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Balancing Redox Reactions (Balancing using oxidation number (Separate the…
Balancing Redox Reactions
Balancing using oxidation number
Write an unbalanced equation
Separate the process into half reactions
a) Assign oxidation numbers for each atom
b) Identify and write out all redox couples in reaction
c) Combine these redox couples into two half-reactions
Make electron gain equivalent to electron loss in the half-reactions
4.Add the half-reactions together
check if the chemical reaction is balance or not
Balancing using half reaction
Steps
1-The first step in balancing any redox reaction is determining oxidation-reduction reaction.
2-divide the oxidation and reduction equations in half
3-Balance elements in the equation other than O and H.
5- Balance the oxygen atoms by adding the appropriate number of water (H2O) molecules to the opposite side of the equation.
6- Balance the hydrogen atoms (including those added in step 2 to balance the oxygen atom) by adding H+ ions to the opposite side of the equation.
7- Add up the charges on each side. Make them equal by adding enough electrons (e-) to the more positive side. (Rule of thumb: e- and H+ are almost always on the same side.)
If basic solution
8-If the equation is being balanced in a basic solution, through the addition of one more step, the appropriate number of OH- must be added to turn the remaining H+ into water molecules.
Example
Example
Prepared by: Ghalia Altukhaifi
Redox Reaction
Oxidation
is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion.
Reduction
is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.
