@disha9876 There are oxygen atoms in this molecule that have two different oxidation states (-1 and -2). The two oxygen atoms that are bonded to each other have an oxidation state like that of a peroxide (-1). The rest are as expected (-2). As a result, the sulfur atoms are each +6.
@wruckie If you mean SO4 (polyatomic), then it is not necessary to find the individual atom charges. You can just know the overall charge of the polyatomic species. In this case, it is -2.
@Phalanx93 This is a freshman level (first quarter) question. It's a difficult question using the concepts already learned because students haven't seen this type of molecule yet. The application of the concepts is the same. Students won't see this type of molecule described in class until they cover transition metal complexes, which is usually at the end of the first year.
I like how this goes straight to the tougher oxidation state problems students may have, as one would have to be a pretty big chemistry n00b not to be able to figure simple ones out with the 3 basic rules. This is the sort of examples that end up on first-year university chem. assessment.
Many, many species would fall in the same category. For example, NaCl is neutral. Na is +1 and Cl is -1. The charge of the species turns out to be the sum of the individual oxidation states.
CAN I ASK WHAT IT WILL BE FOR H2S2O8?
THROUGH THE FORMULA I GET +7 BUT sulphur can exhibit a maximum of 6 right?
disha9876 1 month ago
@disha9876 There are oxygen atoms in this molecule that have two different oxidation states (-1 and -2). The two oxygen atoms that are bonded to each other have an oxidation state like that of a peroxide (-1). The rest are as expected (-2). As a result, the sulfur atoms are each +6.
EnderlePhD 1 month ago
This really helped! Thanks!
kmody32 5 months ago
can i ask why you didnt include the charge for O4? wouldnt that be -8??
wruckie 5 months ago
@wruckie If you mean SO4 (polyatomic), then it is not necessary to find the individual atom charges. You can just know the overall charge of the polyatomic species. In this case, it is -2.
EnderlePhD 5 months ago
at my high school we learned this in grade 10...
thecowthatgoesmoo 1 year ago
@thecowthatgoesmoo That's awesome!
EnderlePhD 1 year ago 4
I'm sorry but I'm really curious ... what grade do they learn this kind of chemistry ?
Phalanx93 1 year ago
@Phalanx93 This is a freshman level (first quarter) question. It's a difficult question using the concepts already learned because students haven't seen this type of molecule yet. The application of the concepts is the same. Students won't see this type of molecule described in class until they cover transition metal complexes, which is usually at the end of the first year.
EnderlePhD 1 year ago
@EnderlePhD So this kind of chemistry we learn when we're in college ? It's easier than it looks ..
Phalanx93 1 year ago
@Phalanx93 That's good. Maybe you should be a chemistry major. And don't worry, there will be hard stuff.
EnderlePhD 1 year ago
@EnderlePhD Yea.I know it and I have to face it . Thanks ..
Phalanx93 1 year ago
I like how this goes straight to the tougher oxidation state problems students may have, as one would have to be a pretty big chemistry n00b not to be able to figure simple ones out with the 3 basic rules. This is the sort of examples that end up on first-year university chem. assessment.
=)
karlkarlkarl1234 2 years ago
sir ...can u plz tell me y the compound az a whole haz an oxidation state zero but an element in a compound not.....good tutorial thanks alot...
zelunika 2 years ago
Many, many species would fall in the same category. For example, NaCl is neutral. Na is +1 and Cl is -1. The charge of the species turns out to be the sum of the individual oxidation states.
EnderlePhD 2 years ago