Question

Help please, assign oxidation numbers to each element on both sides of the reaction, the write half-reactions showing the transfer of electrons for the redox pair, identify the oxidizing agent and the reducing agent.

Mg(s)+Fe(No3)2(aq)=Mg(No3)2(aq)+Fe(s)

Answer 1

There are rules when assigning oxidation numbers. All elements by themselves have the oxidation number as their charge if they are ions or zero if they are not.

0 +2 +5 -2 +2 +5 -2 0
Mg(s) + Fe (No3)2(aq) = Mg(No3)2(aq) + Fe(s)

As you can see, magnesium is being oxidized by losing 2 electrons since it's oxidation number is being increased from 0 to +2. Remember that electrons have a negative charge, so losing electrons increase the oxidation number.

Iron is being reduced by gaining 2 electrons since it's oxidation number is being reduced from +2 to 0.

The element that is being oxidized is itself the reducing agent (causing another element to become reduced). In this reaction it is Mg.

The element that is being reduced is itself the oxidizing agent (causing another element to become oxidized). In this reaction it is Fe(NO3)2.

Answer 2

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