I am having problems with this redox question.

3 Ag2S + 2Al ---6 Ag + Al2S3

What are the charges on each;

Ag + S 2- Al0 Ag0 Al 3+ S2-

To determine the charges on each element in the redox equation, we need to assign oxidation numbers to each element.

In Ag2S, the oxidation number of Ag is +1 (since it is in a compound) and the oxidation number of S is -2.

In Al2S3, the oxidation number of Al is +3 (since it is in a compound) and the oxidation number of S is -2.

In Al, the oxidation number of Al is 0 (since it is in its elemental form).

We can use the changes in oxidation numbers to assign the charges on each element in the equation:

In Ag2S, Ag has a charge of +1, and S has a charge of -2.
In Al2S3, Al has a charge of +3, and S has a charge of -2.
In Al, Al has a charge of 0.

Therefore, the charges on each element are as follows:
Ag: +1
S: -2
Al: +3

To determine the charges on each element in a redox reaction, you need to consider their oxidation states. The oxidation state of each element can be determined by assigning electrons to each atom in a compound or ion based on a set of rules.

In this reaction, you have silver sulfide (Ag2S) and aluminum (Al) reacting to form silver (Ag) and aluminum sulfide (Al2S3). Let's determine the oxidation state for each element:

1. Silver (Ag):
Since silver (Ag) is a metal, its oxidation state is typically +1. However, in this reaction, silver is being reduced, so its oxidation state will be 0. Therefore, the charges on Ag in this reaction are 0.

2. Sulfur (S):
In silver sulfide (Ag2S), each silver atom has an oxidation state of +1 (since Ag typically has a +1 oxidation state). The overall charge of Ag2S is 0, so the oxidation state of sulfur (S) will be -2 to balance out the positive charges of the silver atoms.

3. Aluminum (Al):
The oxidation state of aluminum (Al) can be determined by comparing it to the known oxidation state of sulfur in the compound Al2S3. The overall charge of Al2S3 is 0, and there are three sulfur atoms with an oxidation state of -2 each. Therefore, each aluminum atom must have an oxidation state of +3 to balance out the negative charges. So, the charge on the aluminum (Al) atoms in this reaction is +3.

To summarize:
- The charge on each silver (Ag) atom is 0.
- The charge on each sulfur (S) atom is -2.
- The charge on each aluminum (Al) atom is +3.

Note: These charges represent the oxidation states of each element in this specific reaction. It's important to note that oxidation states can vary in different compounds and reactions.