University:
University of Arizona
Course:
CHEM 141 | General Chemistry Lecture I
Academic year:

2017
Views:

394

Pages:

1
Author:

CloudMaster

The following example will determine when an oxidation reaction can occur. Okay, so the example is the basic reaction in which an aqueous solution of iron (III) chloride oxidizes magnesium metal. X, so write the balanced molecular equation and net ionic equation for the reaction. So, the reactants are going to be iron chloride and magnesium. These are going to be the reactants. We are given two substances: iron chloride (FeCl2) and magnesium (Mg). Thank you! And, as if they react with each other in a way that will produce an oxidation. Redox reaction occurs when a reactant, which is a metal in its elemental form (in this case, magnesium), is located above another reactant, which is a metal in its oxidized form (iron), in the table of oxidation half-reactions. This means that magnesium is more easily oxidized than iron. It's at that table the magnesium is a boss of the metal. If this reactant is going to be iron, then that reaction could occur. Then, in that way, the iron chloride could oxidize magnesium. If the reaction occurs, the iron from iron chloride is reduced to iron and the magnesium will be oxidized to magnesium plus 2 because magnesium is above iron in the table. To write a formula for the salt produced in the reaction, we must remember the charges on iron. Iron commonly has a charge of plus 2, while magnesium has a charge of minus 1. Therefore, we will need 2 chloride ions (Cl-) to cancel out the positive charge of magnesium, resulting in a balanced formula for the salt. The salt is produced using this reaction, so the molecular equation will be R and chloride plus a metal, okay? Producing magnesium chloride plus the iron as a solid. Because remember, that desire was reduced in that way. When they reduced, you will produce that metal itself. So, both of them. Salts in the reactants and the products are soluble strong electrolytes, so we can write the ionic format of each to establish the net ionic equation. It will be like this:[blank line]And we can cancel the chloride because they are basically the spectator ions. Okay, so we cancel. This sentence seems to be a fragment and does not make sense. Could you please provide more information or clarify your statement? That the magnesium was oxidized while the iron went from plus two to zero. The oxidation number of iron, in the elemental state, is going to be zero. So, it went from plus two to zero. That's a reduction. Okay, so we can see here that we have the half reaction of the oxidation by magnesium and the half reaction of the reduction by iron.