Rust (fe2o3) forms on abandoned cars such as the one in this photo through a series of reactions between iron in the car and oxygen in the atmosphere. the unbalanced chemical equation is given below. fe(s)+o2→fe2o3which element is oxidized and which is reduced during the formation of rust? a. is oxidized b. is reduced

Fe has been oxidized

O₂ has been reduced

Explanation:

Here we are going to determine the change in oxidation states and answer the question, remembering that oxidation is the loss of electrons and reduction is the gaining of electrons from the equation:

                                       4Fe     +         3O2→         2Fe2O3

oxidation states                 0                    0               3⁺     2⁻

so we see that oxygen goes from 0 to 2⁻ so it has been reduced, iron goes from 0 to 3⁺ so it has been oxidized.

We could also  answer this question  by noticing that iron has been combined with oxigen therefore it has been oxidized and oxigen has been reduced. I solved the question by determining the change in oxidation states because is more general and applie to any oxidation-reduction reaction

6.4 cm (max) - 25 cm (min)

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8