identify the oxidation state for each atom in the following reaction:

4fe + 3o2 → 2fe2o3

a. elemental iron (fe)
b. elemental oxygen (o2)
c. one iron atom in fe2o3
d. one oxygen atom in fe2o3

  a. Elemental iron (Fe) : 0

b. Elemental oxygen : 0

c. One iron atom in : +3

d. One oxygen atom in : -2

Explanation:

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

In neutral ionic compound , the oxidation states are exchanged to give the molecular formula. Thus in iron has oxidation state of +3 and oxygen has oxidation state of -2.

For the reaction :

On reactant side:

Oxidation state of iron in elemental state = 0

Oxidation state of oxygen = 0

On product side:

Oxidation state of iron = +3

Oxidation state of oxygen = -2

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.