What element is being oxidized in the following redox reaction?

zn2+(aq) + nh4+(aq) → zn(s) + no3(aq)

The element that is being oxidized in the given redox reaction is Nitrogen (N)

From the question,

We are to determine the element that is being oxidized in the given redox reaction equation

First and foremost, we will write the redox reaction properly.

The given redox reaction equation is

Zn²⁺(aq) + NH₄⁺(aq) → Zn(s) + NO₃⁻(aq)

Now, to determine the element that is being oxidized

First, we will define the term oxidation

Oxidation can be defined as gain of oxygen. It can also be defined as an increase in oxidation state.

In the given redox reaction, the oxidation state of Nitrogen increased from -3 to +5. That means, Nitrogen is the element being oxidized.

NOTE:

Oxidation state of N in NH₄⁺ is -3

and Oxidation state of N in NO₃⁻ is +5

Hence, the element that is being oxidized in the given redox reaction is Nitrogen (N)

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The element that has been oxidized is the N

Explanation:

Zn²⁺(aq) + NH₄⁺(aq) → Zn(s) + NO₃⁻(aq)

See all the oxidation states:

Zn²⁺  → acts with +2

In ammonia, H acts with +1 and N with -3

Zn(s), acts with 0. In all the elements in ground state, the oxidation state is 0.

Zn changed from 2+ to 0. The oxidation number, has decreased.

This element has been reduced.

NO₃⁻ (aq) it's a ion, from nitric acid.

N acts with +5

O acts with -2

The global charge is -1

The N, has increased the oxidation state, so this element is the one oxidized.

2b2t

explanation:

2b2t