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Determining the oxidation State of an element
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Determining the oxidation state of an element involves understanding the distribution of electrons in a compound. Here's a breakdown of the process:
1. Know the Rules:
The oxidation state of an element in its elemental form is always 0.
Alkali metals (Group 1) have a +1 oxidation state, and alkaline earth metals (Group 2) have a +2 oxidation state.
Halogens (Group 17) typically have a -1 oxidation state.
Oxygen usually has a -2 oxidation state (except in peroxides where it's -1).
2. Apply the Rules: The sum of the oxidation states in a neutral compound must be zero. In a polyatomic ion, the sum of the oxidation states must equal the charge of the ion.
3. Use Algebra: Assign known oxidation states to elements with predictable values. Use algebra to solve for the unknown oxidation state.
Example: Determine the oxidation state of sulfur in H2SO4.
H has a +1 oxidation state (rule 1).
O has a -2 oxidation state (rule 4).
Let x be the oxidation state of S.
The sum of the oxidation states must be zero: 2(+1) + x + 4(-2) = 0
Solving for x, we get x = +6.
Therefore, sulfur has an oxidation state of +6 in H2SO4.
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