5 answers

Identify the species oxidized, the species reduced the oxidizing agent Ihe reducing agent in the following electron trunsfer reaction

Question:

Identify the species oxidized, the species reduced the oxidizing agent Ihe reducing agent in the following electron trunsfer reaction JCh; 2Ak 76cl" 2apt species orldized specles reduced oxidualg Hermt reducng #gent As Ihe reaction proccces electrs ure Iransfetexl Aamni Anator Ury Anotner Voteion Ito muliamm reinalnung


Answers

Identify the species that undergoes oxidation, the species that undergoes reduction, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem.

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Oxidation is lost off. Electron vile reduction is gain off. Electron oxidizing agent is the species that undergoes reduction. Violet oxidize the other species present in the reaction. The reducing agent is the species that undergoes oxidation, but it reduces the other species during the course off.

Reaction for option A The species that undergo oxidation is S 03 too negative. The species that undergoes reduction is see you. Which two for option B oxidation is undergone by Eman which two by reduction is gone by or do option C oxidation by EJ two on reduction by a notary negative optioned. The oxidation is undergone by aluminum by reduction by chromium..

For auction. E aluminum is losing electrons to form aluminum three. Positive it undergoes oxidation. Hence it will act as reducing Agent Vera's for sent our four positive it is gaining electrons to form said Are it undergoes reduction. Hence it will act as oxidizing agent What option? B in this reaction and always losing electrons to form and or too negative it undergoes oxidation.

Acting as reducing agent Bye for silver Eiji Positive is gaining electron to form Eiji, it undergoes reduction. Therefore, acting as oxidizing agent for option C In this mg is losing electrons to form mg which two it undergoes oxidation Hence act as reducing agent by S I 03 to negative is gaining electrons to form aside it undergoes reduction. Hence it is acting as oxidizing Agent for option d m n 02 is losing electron to form Eman or four Negative. It is an oxidizing agent while CNN or three negative is gaining electrons to form chlorine Negative, it undergoes reduction, hence acting as oxidizing Agent.

Okay, so for number seven, let me change the color here. F E, N B R two or an elemental form B R. Is a negative one in the compound, F E. Is a plus too. If you're going from zero to plus two, that means that's a loss of electrons.

So that means that this is oxidized. So this would be the reducing agent and then browning is going from a zero to a negative one, that's a gain of electrons. So this is reduced. So we would call it the oxidizing agent. Then on B, we've got a plus one on hydrogen and negative one on iodine, plus one on the H two, S.

H and H two. S. +04 negative two on the oxygen. To figure out the sulfur, we've got two hydrogen at a positive one plus sulfur plus negative eight on the oxygen adds up to the neutral compound, which is zero. So if we're going to end up being a plus six here, then here we've got plus one on the H and H two S, negative two on the sulfur, elemental iodine.

So that's zero. Oxygen is a negative two hydrogen as a plus one. Then you've got your id I'm going from a negative 1-0. So that's going to be a loss of electrons. So that means that this is oxidized.

We would call this the reducing agent and then you've got your sulfur going from a positive six to a negative two. That's a gain an electron. So that means it is reduced and we would call this the oxidizing agent, then in C you've got hydrogen peroxide. So it's a plus one on the hydrogen and minus one on oxygen mono atomic ion, which is the same as its charge, plus two oxygen. Here is a negative two hydrogen as a plus one mono atomic ion, same as its charge, which is plus three negative two on oxygen plus one on hydrogen.

If he goes from a plus two two plus three, that means this is a loss of electrons. So that means this is oxidized. We would call this the reducing agent and then you've got this oxygen going from a negative one to a negative two. That's a gain an electron. So this is reduced and we would call this the oxidizing agent..

Okay, so for six a aluminum chlorine or an elemental form. So their oxidation numbers are zero over here in aluminum chloride, we have a negative one on the chlorine and then you have a positive three on the aluminum. So this chlorine is going from zero to a negative one. So it's gaining electrons. So it is reduced.

That means that this is the oxidizing agent and then your aluminum is going from zero to a plus three. So that means it is losing electrons. So that means it is oxidized. And we would say that the aluminum is the reducing agent. Okay, and let her be, we've got a negative to oxidation state for the oxygen, which means hydrogen as a plus one in M N.

+04. We've got a negative two on the oxygen and then a positive seven on the Mn. Because mn plus a negative eight on the oxygen equals negative one. So, if you solve for M and that's how you get that plus seven. This is a mono atomic ion, which is plus two.

So is this, this is a plus three. Another mono atomic ion, plus two, oxygen is a negative two, hydrogen is a plus one here, you'll see that you're going from f plus two, two plus three. So we're losing electrons. So this is oxidized. That means that every plus two is the reducing agent.

And then you've got your Mn going from a plus seven, two plus two. So this is gaining electrons. So this is reduced. So that means that the and then is actually your oxidizing agent there. Okay, then, if you take a look at see, we've got a negative two on the sulfur plus two on the iron here, we have a negative two on the oxygen plus five on the nitrogen because nitrogen plus a negative six on the oxygen is a negative one, solve for the nitrogen, you're gonna get a plus five oxidation state, negative two on the oxygen here, plus one on the hydrogen, negative two on the oxygen plus two on the nitrogen, negative two on the oxygen plus six on the sulfur.

Because sulfur plus a negative eight on the oxygen is going to be a negative to sulfur sulfur, you're gonna end up with a plus six, then this is a mono atomic eye on it, plus three and then oxygen is a negative two hydrogen as a plus one. So here you'll see that the nitrogen is going from a plus five to plus two. So it's gaining electrons. So it's reduced. So that means that this is going to be the oxidizing agent.

And then you've got this F. E. Going from a plus two, two plus three and the sulfur, those both are. That's a loss of electrons. So that means that this is oxidized and this is going to be your reducing agent.

Okay,.

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