Posted by Moi on Sunday, October 17, 2010 at 1:01pm.
You are absolutely correct on one count and not quite right on the second. Hg occurs both as Hg(I) and Hg(II) but nitrate is -1, not -2 We NORMALLY use the smallest set of subscripts but in the case of Hg(I) compounds, most of them are dimeric. Hg2Cl2, Hg2(NO3)2, etc. Note that there also is a mercury(II) nitrate; i.e., Hg(NO3)2. Therefore, although the empirical formula for mercury(I) nitrate is HgNO3, the molecular formula is Hg2(NO3)2 anf I was always encouraged to write the molecular formula instead of the empirical formula.
YOUR RIGHT,the charge of nitrate is -1, my mistake. But I still don't understand how to figure out the formula for Mercury(I) nitrate. Given that the charge for mercury in this case is -1 and nitrate is -1 also then where do the subscripts "2" come from, [given that the correct formula is Hg2(NO3)2]
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