What element is being oxidized in the following redox reaction? fe 2+(aq) + nh4 +(aq) → fe(s) + no3 -(aq)

Explanation:

When there occurs a decrease in oxidation state of an element then it means the element has been reduced.

Whereas when there occurs an increase in oxidation state of an element then it means the element has been oxidized.

As the given reaction is as follows.

Oxidation state of iron is changing from +2 to 0. It means iron is getting reduced.

On the other hand, oxidation state of N in is as follows.

                                  x + 4(1) = +1

                                    x = 1 - 4

                                        = -3

Hence, oxidation state of N in is -3.

Oxidation state of N in is as follows.

                              x + 3(-2) = -1

                              x - 6 = -1

                               x = +5

Hence, oxidation state of N in is +5. It means nitrogen is being oxidized.

Thus, we can conclude that nitrogen is the element which is being oxidized in the given reaction.

it is to be noted that an alpha particle is an helium nucleus. so it contains 2 protons 2 neutrons and has a mass number of 4. when alpha decay particles are ejected from the nucleus it gets transformed into an atom which has atomic number less than 2 and a mass number less than 4.

an equation that could represent alpha decay is radium 226 decay of alpha particle forms radon 222.

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