For the following reaction

KClO2->KCl+O2

assign oxidation states to each element on each side of the equation.

KClO2->KCl+O2

assign oxidation states to each element on each side of the equation.

Reactants

K=?

Cl=?

O=?

Which element is reduced?

I got K=5, Cl=-1, and O=-4 . The element that reduced is K, but its says its wrong. Help, Please!

1 Answers

If you intended KClO2 (and not KClO3), here is he scoop.

K is +1. It’s ALWAYS +1 because it’s in group I of the periodic table. Cl is +3 on the left (remember all compounds are 0 so K + Cl + 2O = 0; therefore, 1 + ? + 2*-2 = 0. That makes Cl +3) and O is -2 for EACH oxygen and as you have it as -4 for the total. USUALLY, you want oxidation states for EACH atom. On the right K is +1, Cl is -1 and O2 is 0.

What is reduced? Reduction is the gain of electrons.

So Cl goes from +3 on the left to -1 on the right or gain of 4 e for each Cl.

O goes from -4 total on the left to 0 on the right or loss of 4e.

So Cl is reduced and O is oxidized.

It is important that you know the rules. Here they are.

http://www.chemteam.info/Redox/Redox-Rules.html

K is +1. It’s ALWAYS +1 because it’s in group I of the periodic table. Cl is +3 on the left (remember all compounds are 0 so K + Cl + 2O = 0; therefore, 1 + ? + 2*-2 = 0. That makes Cl +3) and O is -2 for EACH oxygen and as you have it as -4 for the total. USUALLY, you want oxidation states for EACH atom. On the right K is +1, Cl is -1 and O2 is 0.

What is reduced? Reduction is the gain of electrons.

So Cl goes from +3 on the left to -1 on the right or gain of 4 e for each Cl.

O goes from -4 total on the left to 0 on the right or loss of 4e.

So Cl is reduced and O is oxidized.

It is important that you know the rules. Here they are.

http://www.chemteam.info/Redox/Redox-Rules.html

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