anonymous
  • anonymous
i need some help on understanding why the charges on these ionic compounds are balanced like they are... for example, tin (IV) dichromate is Sn(CrO7)2, but i'm not sure where the +4 of the tin goes, and why there are two dichromates... and mercury (I) nitrate, why are there two mercuries ( Hg2(NO3)2) )?
Chemistry
chestercat
  • chestercat
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anonymous
  • anonymous
Dichromate charge is -2 Charge of tin can vary but (IV) represents +4. All metals (the one in front) is positive, In order for the charges to balance out the dichromate must be multiplied by 2 in the subscript. For the second one, Hg usually have a +2. NO3 (nitrate) has a charge of -1 But this mercury has a +1 charge So it cannot be \[HgNO _{3}\] but \[Hg _{2}(NO3)_{2}\] since it is oxidized. +2 and -2 would cancel out.

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