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Describe the differences between the oxidation number of different elements in redox reactions.

The oxidation number of different elements in redox reactions can vary.

In redox reactions, oxidation numbers are used to track the transfer of electrons between atoms. The oxidation number of an element is the charge it would have if all its bonds were ionic. In a redox reaction, the oxidation number of the element being oxidised increases, while the oxidation number of the element being reduced decreases.

For example, in the reaction between magnesium and oxygen to form magnesium oxide, magnesium is oxidised and oxygen is reduced. The oxidation number of magnesium increases from 0 to +2, while the oxidation number of oxygen decreases from 0 to -2.

Some elements, such as oxygen and hydrogen, have predictable oxidation numbers in most compounds. Oxygen usually has an oxidation number of -2, while hydrogen usually has an oxidation number of +1. However, there are exceptions to these rules, such as in peroxides where oxygen has an oxidation number of -1.

Transition metals can have multiple oxidation states, which can make predicting their oxidation numbers more difficult. For example, iron can have an oxidation number of +2 or +3 in its compounds.

Overall, the oxidation number of different elements in redox reactions can vary depending on the specific reaction and the compounds involved.

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