Question

Oxidation and reduction Lewis​

Answer 1

Oxidation involves an increase in the oxidation number of an atom. Reduction occurs when the oxidation number of an atom decreases. According to this model, CO2 is reduced when it reacts with hydrogen because the oxidation number of the carbon decreases from +4 to +2.

So to identify an oxidizing agent, simply look at the oxidation number of an atom before and after the reaction. If the oxidation number is greater in the product, then it lost electrons and the substance was oxidized. If the oxidation number is less, then it gained electrons and was reduced.

Answer 2

Draw the Lewis structure.

Assign each atom all of its lone pair electrons. For bonding electrons assign all of the electrons to the more electronegative element.

For each atom perform the following calculation: number of electrons in the atom in its elemental state - assigned electrons = oxidation state.

In your example, the oxidation number of each HH is +1 and of FF is -1. The oxidation number of CC is -2 and of OO is 0.

.............***××××××××××××××***...............

A Lewis acid is defined as an electron acceptor. An oxidizing agent is also defined as an electron acceptor (in the electronic theory of oxidation).

So then what is the basic difference between an Lewis acid and an oxidizing agent?

Similarly;

A Lewis base is defined as an electron donor (Lewis theory). A reducing agent is also defined as an electron donor (electronic theory).