Answer:
Oxidation state is a number assigned to an element in a compound according to some rules. This number enable us to describe oxidation-reduction reactions, and balancing redox chemical reactions. When a covalent bond forms between two atoms with different electronegativities the shared electrons in the bond lie closer to the more electronegative atom:
The oxidation number of an atom is the charge that results when the electrons in a covalent bond are assigned to the more electronegative atom
It is the charge an atom would possess if the bonding were ionic
In HCl (above) the oxidation number for the hydrogen would be +1 and that of the Cl would be -1
Explanation:
EXAMPLE:
Determine which element is oxidized and which element is reduced in the following reactions (be sure to include the OS of each):
Zn + 2H+ → Zn2+ + H2
2Al + 3Cu2+→2Al3+ +3Cu
CO32- + 2H+→ CO2 + H2O
SolutionS
SOLUTIONS:
a. Zn is oxidized (Oxidation number: 0 → +2); H+ is reduced (Oxidation number: +1 → 0)
b. Al is oxidized (Oxidation number: 0 → +3); Cu2+ is reduced (+2 → 0)
c. This is not a redox reaction because each element has the same oxidation number in both reactants and products: O= -2, H= +1, C= +4.
(For further discussion, see the article on oxidation numbers).
An atom is oxidized if its oxidation number increases, the reducing agent, and an atom is reduced if its oxidation number decreases, the oxidizing agent. The atom that is oxidized is the reducing agent, and the atom that is reduced is the oxidizing agent. (Note: the oxidizing and reducing agents can be the same element or compound).
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