My basic knowledge about nomenclature is: A mineral acid is called hypo when it has one less oxygen than the original one,
- a pyro acid when 2 molecules of acid add up with release of $\ce{H2O}$
- a meta acid when one molecule releases $\ce{H2O}$ and
- a per acid when it has one extra $\ce{O}$ in the structure connected with a peroxide bond.
Question 1
I was taught in my class that this structure:
is correct because when we are drawing structures of a hypo-,per-,meta- or pyro- oxyacid, one must try to maximise the covalency.
Why is that so?
Also, usually in pyro- acid we find a $\ce{M-O-M}$ bond where $\ce{M}$ is the central atom(s). Like $\ce{P-O-P}$ in pyrophosphoric acid as show below:
Then shouldn't the structure of pyrosulfurous acid be like this:
Why is the structure not similar to pyrophosphoric acid?
Question 2
We know that in hypo-acids, there is one less $\ce{O}$ in the empirical formula of the acid i.e. Hypophosphoric acid should have one less $\ce{O}$ than in $\ce{H3PO4}$ i.e. it should be something like $\ce{(H3PO3)_$n$}$. If we put $n=2$ we have $\ce{H6P2O6}$.
But why is its formula $\ce{H4P2O6}$?
I might lack some information about it or maybe I've understood the concept wrong. Please help.
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