How do you determine oxidation states of elements?

Answer 1

The oxidation state of an element is generally #0#

Oxidation/reduction reactions are characterized by the formal loss or gain of electrons. An element is zerovalent, and electron transfer is presumed to occur after reaction. The reactants in the following redox process certainly are oxidation state #0#:

#C(s) + O_2(g) rarr CO_2(g)#

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Answer 2

Ellie Andrews

Oxidation states of elements are determined by several rules, including:

For elements in their natural state, the oxidation state is 0.
In compounds, assign hydrogen an oxidation state of +1 and oxygen an oxidation state of -2, unless in peroxides or compounds with fluorine, where hydrogen is -1 and oxygen is -1.
In compounds, alkali metals (Group 1) have an oxidation state of +1, alkaline earth metals (Group 2) have an oxidation state of +2.
Fluorine always has an oxidation state of -1.
In binary compounds, the more electronegative element takes on its typical oxidation state, while the less electronegative element takes on the difference.
The sum of oxidation states in a compound equals its overall charge.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.