## Assign oxidation states to each element on each side of the equation.

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### Question:

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

For the following reaction KClO2 -> KCl + O2 assign oxidation states to each element on each side of the equation.
BOTH Reactants AND Products
Reactants
K

Cl

O

WHICH ELEMENT IS OXIDIZED
Products- K

Cl

O

WHICH ELEMENT IS REDUCED?
Oxidation States and Reduction/Oxidation:
The oxidation state of an atom can be determined by following certain rules as shown below:

1. Alkali metals usually have an oxidation state of +1

2. Oxygen usually has an oxidation state of -2, unless it is bonded to itself

In a reaction, we say that if an atom lost electrons, it became oxidized. Conversely, if it gained electrons, it became reduced.

Using the rules above, we can determine the oxidation states of the reactants and products. First, we do the reactants below:
KClO2

K = +1
O = -2
Then, we find the oxidation state of Cl by noting that the overall molecule has a net charge of 0 so the oxidation number of Cl must cancel out the oxidation numbers of the rest of the molecule:

Cl = -(+1 + 2*-2) = +3

Now we can do the same for the products.
KCl

K = +1

Cl = -1

O2

O = 0

Since K started with an oxidation number of +1 and ended with an oxidation of +1, it was neither reduced nor oxidized. However, Cl went from +3 to -1 which means it gained electrons and was reduced. O, on the other hand, went from -2 to 0 which means it lost electrons and was oxidized.

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