In the reaction shown below, which substance is oxidized? 2 Cr(s) + Fe 2 O 3 (aq) → Cr 2 O 3 (aq) + 2 Fe(s)

Hey everyone welcome back. So let's get started with this video here. They want us to identify the following for the reaction. So they want us to find the oxidized species to reduce species. The oxidizing agent and the reducing agent. Okay so here recall that the oxidizing agent gets reduced. So then the reducing agent gets oxidized and this will help us identify it later on. Okay. So then also recall leo so lost other electrons means oxygen oxidize again of electrons means reduce. Okay so with that being said let's go ahead and look at our reaction and assign oxidation values to the elements. So then we have B. R. Two which is in its normal state. So then it's charge is going to be zero. We have A. L. Which is also in its normal state and it's going to have a charge of zero. Then we have pr which has a negative charge. So it's Going to have a negative one and then A. L. It's going to have a positive three. Okay so then let's go ahead and write them down. So we have br And went from to -1. So it got more negative since I got more negative. That means again an electron. If you get an electron that means reduction. It was reduced. So B. R. Was reduced. So let's go ahead and write that in Reduced species was b. r. two. Okay let's look at A. O. And went from zero to positive three. So it got more positive. It got more positive because it lost electron you lose electron. That means it was oxidized. So oxidized species that is A. L. Okay oxidizing agent. That is the one that was reduced which was reduced. It was B. R. Reducing agent is the one that gets oxidized. Which one was oxidized. It was A. L. Okay. Identify where the electrons were transferred from and to where so brahman is being reduced. Therefore it gained electrons while aluminum is losing them. Therefore electrons transferred from aluminum two. B. R. Two. Okay thank you for watching. I hope this helped. And I'll see you in the next video.