Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfer reaction.

2Fe3+ + Sn2Fe2+ + Sn2+
species oxidized species reduced


oxidizing agent reducing agent

As the reaction proceeds, electrons are transferred from
to
.

Ah, an electron transfer reaction! Let's break it down and have some fun with it!

In this reaction, the species that is losing electrons and being oxidized is Fe3+ (the iron ion with a +3 charge). Poor Fe3+ is losing its electrons, so it's the one getting oxidized. It's like Fe3+ is saying, "Hey, I'm feeling a bit rusty, time to let go of some electrons!"

On the other side, the species that is gaining those electrons and being reduced is Sn2+ (the tin ion with a +2 charge). Lucky Sn2+ gets to snatch those electrons and go from being Sn2+ to Sn, feeling all rejuvenated. Sn2+ is like, "I'm so glad I have my electron buddies now, taking me from Sn2+ to Sn!"

Now, let's talk about the agents in this gig. The oxidizing agent is the species that causes the oxidation to happen. In this case, Fe3+ is being oxidized, so the oxidizing agent is Sn2+. Sn2+ is the one saying, "Hey Fe3+, let me help you get rid of those electrons!"

Conversely, the reducing agent is the species that causes the reduction to happen. Sn2+ is being reduced, so the reducing agent is Fe3+. Fe3+ is the one saying, "Hey Sn2+, I have some extra electrons, want them? They'll give you a shiny new look!"

And as the reaction proceeds, electrons are transferred from Fe3+ to Sn2+. Fe3+ is like, "Here you go, Sn2+, have some electrons for a fresh start!" and Sn2+ is like, "Thank you, Fe3+, I'll put these electrons to good use, making me go from Sn2+ to Sn!"

Remember, in the world of electron transfer reactions, it's all about sharing electrons and making everyone feel balanced and cheerful! 🤡

In the given electron transfer reaction:

2Fe3+ + Sn2Fe2+ + Sn2+

The species that is oxidized is Fe2+ (it loses electrons and increases its oxidation state from +2 to +3), and the species that is reduced is Sn2+ (it gains electrons and decreases its oxidation state from +2 to 0).

So,

Species oxidized: Fe2+
Species reduced: Sn2+

The oxidizing agent is Sn2+ (it causes the oxidation of Fe2+ by accepting electrons), and the reducing agent is Fe2+ (it causes the reduction of Sn2+ by donating electrons).

As the reaction proceeds, electrons are transferred from Fe2+ to Sn2+.

To identify the species oxidized and reduced, as well as the oxidizing and reducing agents, we need to determine the changes in oxidation states for each element involved in the reaction.

In the given reaction: 2Fe3+ + Sn2 → 2Fe2+ + Sn2+

1. Start by assigning the oxidation states of each element in the reactants and products of the reaction.

Fe3+ has an oxidation state of +3 in this case, Sn2 has an oxidation state of +2, Fe2+ has an oxidation state of +2, and Sn2+ has an oxidation state of +2.

2. Next, compare the oxidation states of each element before and after the reaction.

In the reaction, the iron (Fe) goes from an oxidation state of +3 in Fe3+ to +2 in Fe2+. Its oxidation state decreases from +3 to +2, indicating that it has gained electrons. Therefore, Fe3+ is the species that is being reduced.

On the other hand, tin (Sn) goes from an oxidation state of +2 in Sn2 to +2 in Sn2+. Its oxidation state remains the same, indicating that there is no change in electrons for tin. Therefore, Sn2 is the species that is neither oxidized nor reduced.

3. Based on the previous observations, we can determine the oxidizing and reducing agents.

The species that causes oxidation is called the oxidizing agent, while the species that causes reduction is called the reducing agent.

In this reaction, Fe3+ is reduced, meaning it gains electrons. Therefore, Sn2 is the reducing agent since it loses electrons to Fe3+ and causes its reduction.

Conversely, Fe3+ causes the oxidation of Sn2. So Fe3+ is the oxidizing agent in this reaction.

To summarize:
- Species oxidized: Sn2
- Species reduced: Fe3+
- Oxidizing agent: Fe3+
- Reducing agent: Sn2

As the reaction proceeds, electrons are transferred from Sn2 to Fe3+.

Here are the definitions.

Loss of electrons is oxidation.
Gain of electrons is reduction.
The material oxidized is the reducing agent.
The material reduced is the oxidizing agent.

2Fe3+ + Sn ==> 2Fe2+ + Sn2+

You can see that 2Fe^3+ goes from 6+ to 4+ so that is a gain of electrons.

You can see Sn goes from 0 on the left to 2+ on the right which is a loss of electrons