How to calculate the number of peroxide bond ? Easily.....
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An atom can only use its valence electrons for bonding.
How many valence electrons does an atom have in its neutral (0) state? For sulfur, it has 6 valence electrons. Its configuration is [Ne] 3s2 3p4 , and I've been told that 2+4 = 6.
A positive oxidation state means the atom has donated electrons to bonding.
If the calculated oxidation state on an atom in a compound exceeds the number of valence electrons, something funny must be going on. You can't donate more electrons than you have!
For sulfur, its oxidation state can't exceed +6, since it can donate no more than its 6 valence electrons to bonding.
So, on inspection of these chemical formulas, she assumed that oxygen was in the -2 state, as it generally is in non-peroxides. Her formulas came out to impossible oxidation states for sulfur based on that assumption, so it must be wrong.
In compounds with a lot of oxygen, it's likely that this implies that the oxidation state on oxygen must not be -2, as would be the case in a peroxide.
It's possible to solve these oxidation state discrepancies in other ways. For instance, you could have an azido group or something like that. In general, your assumptions of the oxidation state of the organic atoms must be wrong if the result of the oxidation calculation gives impossible oxidation states.
p.s. If you're having trouble with accents, I suggest watching a bunch of youtube! In science, very brilliant people come from all parts of the world and speak in all sorts of ways.
How many valence electrons does an atom have in its neutral (0) state? For sulfur, it has 6 valence electrons. Its configuration is [Ne] 3s2 3p4 , and I've been told that 2+4 = 6.
A positive oxidation state means the atom has donated electrons to bonding.
If the calculated oxidation state on an atom in a compound exceeds the number of valence electrons, something funny must be going on. You can't donate more electrons than you have!
For sulfur, its oxidation state can't exceed +6, since it can donate no more than its 6 valence electrons to bonding.
So, on inspection of these chemical formulas, she assumed that oxygen was in the -2 state, as it generally is in non-peroxides. Her formulas came out to impossible oxidation states for sulfur based on that assumption, so it must be wrong.
In compounds with a lot of oxygen, it's likely that this implies that the oxidation state on oxygen must not be -2, as would be the case in a peroxide.
It's possible to solve these oxidation state discrepancies in other ways. For instance, you could have an azido group or something like that. In general, your assumptions of the oxidation state of the organic atoms must be wrong if the result of the oxidation calculation gives impossible oxidation states.
p.s. If you're having trouble with accents, I suggest watching a bunch of youtube! In science, very brilliant people come from all parts of the world and speak in all sorts of ways.
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H2O2
Hydrogen peroxide/Formula
The most common peroxide is hydrogen peroxide (H2O2), colloquially known simply as "peroxide". It is marketed as a solution in water at various concentrations.
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