I am having problems with this redox question.
3 Ag2S + 2Al ---6 Ag + Al2S3
What are the charges on each;
To determine the charges on each element in the given redox reaction, we need to identify their oxidation states.
Here's a step-by-step guide on how to determine the oxidation states:
1. Start by assuming that the oxidation state of each element in a compound is equal to zero.
2. In the case of elemental forms like Ag and Al, their oxidation states are always zero.
3. For compounds, some general rules can help determine the oxidation states:
- The oxidation state of an atom in a monoatomic ion is equal to the charge of that ion. For example, in Ag+, the oxidation state of Ag is +1.
- In a compound, the sum of the oxidation states must equal zero. For example, in Al2S3, the total oxidation state should be zero.
Now let's apply these rules to the given redox reaction:
3 Ag2S + 2Al --- 6 Ag + Al2S3
- The oxidation state of Ag is always +1, so each Ag in the reaction has an oxidation state of +1.
- The oxidation state of S is usually -2, so in Ag2S, each Ag must have an oxidation state of +1 to balance the overall charge. Therefore, the oxidation state of S in Ag2S is -2.
- The oxidation state of Al is always +3.
- The oxidation state of S in Al2S3 can be determined by considering the overall charge. Since Al has an oxidation state of +3, each S should have an oxidation state of -2 to balance the overall charge. Therefore, the oxidation state of S in Al2S3 is -2.
So, the charges for each element in the redox reaction are as follows:
- Ag: +1
- S in Ag2S: -2
- Al: +3
- S in Al2S3: -2