what is the oxidation number on each of these ions - Ag2S + 2Al - 6Ag + Al2S3
Can you show your work? Thanks a bunch:)
To determine the oxidation numbers of the elements in a compound, you need to understand the rules for assigning oxidation numbers.
1. For uncombined elements, the oxidation number is always zero. Consequently, Ag and Al, when not combined with any other element, would have an oxidation number of zero.
2. The sum of oxidation numbers in a neutral compound is zero. In Ag2S, the compound is neutral, so the sum of the oxidation numbers must be zero. Let's assume that the oxidation number of Ag is x. Since Ag2S contains two Ag atoms, the total oxidation number of Ag would be 2x. The oxidation number of S is -2 because it's in Group 16 and typically has a -2 charge. Therefore, we can write the equation: 2x + (-2) = 0. Solving for x, we get x = +1. Therefore, the oxidation number of Ag in Ag2S is +1.
3. In ionic compounds, the sum of the oxidation numbers is equal to the charge of the compound. In 2Al, aluminum has an unknown oxidation number, let's assume it to be y. In order for the compound to be neutral, the sum of the oxidation numbers must be zero. So y + y = 0, which means y = 0. Therefore, the oxidation number of Al in 2Al is also zero.
4. Using the same concept, let's analyze 6Ag. Since the compound is neutral, the sum of oxidation numbers must be zero. Let's assume the oxidation number of Ag is z. Thus, 6z = 0, which leads to z = 0. Therefore, the oxidation number of Ag in 6Ag is also zero.
5. Lastly, for Al2S3, let's apply the same logic. The two Al atoms would have an oxidation number of zero each. The oxidation number of S is -2, as mentioned earlier. So, we have 2(0) + 3(-2) = 0, which simplifies to -6 = 0. This equation is not balanced, but that's expected because Al2S3 is an ionic compound and carries a net charge. So, the compound Al2S3 doesn't have an oxidation number.
To summarize:
- In Ag2S, the oxidation number of Ag is +1, and the oxidation number of S is -2.
- In 2Al, the oxidation number of Al is 0.
- In 6Ag, the oxidation number of Ag is 0.
- Al2S3 doesn't have an oxidation number since it's an ionic compound.
I hope this explanation helps! Let me know if you have any more questions.
Sure! Here's a step-by-step breakdown of how to determine the oxidation numbers for each ion:
1. Ag2S:
- The overall compound is neutral, so the sum of the oxidation numbers of each element should be zero.
- Since sulfur is a nonmetal, we assume its oxidation number to be -2.
- Let the oxidation number of silver be x. Since there are 2 silver atoms, the total oxidation number of silver would be 2x.
- Setting up the equation: 2x + (-2) = 0
- Solving for x gives x = +1.
- Therefore, the oxidation number of silver in Ag2S is +1, and the oxidation number of sulfur is -2.
2. 2Al:
- Aluminum is a metal, so its oxidation number is typically +3.
3. 6Ag:
- The 6Ag represents 6 atoms of silver, so we need to determine the oxidation number for each atom.
- Since there is no charge specified for the compound, we assume it is neutral.
- Therefore, the sum of the oxidation numbers of each silver atom should be zero.
- Let the oxidation number of each silver atom be x.
- Setting up the equation: 6x = 0
- Solving for x gives x = 0.
- Therefore, the oxidation number of each silver atom in 6Ag is 0.
4. Al2S3:
- The overall compound is neutral, so the sum of the oxidation numbers of each element should be zero.
- Aluminum is a metal, so its oxidation number is typically +3.
- Let the oxidation number of sulfur be y. Since there are 3 sulfur atoms, the total oxidation number of sulfur would be 3y.
- Setting up the equation: 2(+3) + 3y = 0
- Solving for y gives y = -2.
- Therefore, the oxidation number of aluminum in Al2S3 is +3, and the oxidation number of sulfur is -2.
Hope this helps!
Here are the rules. Let me know if you need clarification or post your results and I'll be glad to check them.
http://www.chemteam.info/Redox/Redox.html