The oxidation numbers for each element in the compound Ag2SO3 are: (Enter numbers ONLY in the format +1 or -1; no spaces.)
Ag
S
O
for Ag i got +4
for S i got -2 and same for O
The oxidation numbers for each element in the compound NaClO4 are: (Enter numbers ONLY in the format +1 or -1; no spaces.)
Na
Cl
O
for Na i got +1 for Cl +7 and for O -2
Can any one verify these.
S is +4 and not -2
O is -2, correct.
BUT Ag is +1. Remember a compound is zero; therefore, 3 O at -2 each is -6, S is +4, which makes 2Ag +2 or +1 each.
You are on the money for NaClO4.
Na is +1
Cl is +7
Each O is -2.
Here is a good site if you need the rules.
http://www.chemteam.info/Redox/Redox-Rules.html
To determine the oxidation numbers for each element in a compound, there are some guidelines you can follow.
For the compound Ag2SO3:
- Start by assuming that all the elements have their most common oxidation numbers. In this case, the most common oxidation number for Ag is +1, for S is +6, and for O is -2.
- Then, analyze the overall charge of the compound and distribute it to the different elements.
- Since Ag is a transition metal, it can exhibit multiple oxidation states. In Ag2SO3, the compound has no overall charge, so the sum of the oxidation numbers of all the elements must be zero.
- Therefore, you need to adjust the oxidation numbers of Ag, S, and O to satisfy this condition.
Here's how you can calculate the oxidation numbers for each element in Ag2SO3:
Since there are two Ag atoms, let's assume each Ag atom has an oxidation number of x.
So, the contribution from Ag is +2x.
The oxidation number of S is -2.
There are three oxygen atoms, so let's assume each oxygen atom has an oxidation number of y.
So, the contribution from O is 3y.
The compound is neutral, so the sum of oxidation numbers is zero.
Therefore, 2x - 2 + 3y = 0.
Simplifying the equation, we get:
2x + 3y = 2.
Since the actual values of x and y will satisfy this equation, we can solve it:
If we let x = +1, then y = -2/3.
If we let x = +2, then y = +2/3.
So, one possible set of oxidation numbers for Ag2SO3 is:
Ag: +1
S: -2
O: +2/3.
However, it is important to note that oxidation numbers are not always whole numbers, and they can sometimes represent fractional charges when necessary.
Now, let's move on to the compound NaClO4:
The oxidation number of Na is +1 (most common oxidation state for alkali metals).
The oxidation number of Cl is -1 (most common oxidation state for halogens always in binary compounds).
The oxidation number of O is -2 (most common oxidation state for oxygen).
Therefore, the oxidation numbers for each element in NaClO4 are:
Na: +1
Cl: -1
O: -2.
So, your answer is correct.