• 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) )?
  • chestercat
I got my questions answered at in under 10 minutes. Go to now for free help!
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.

Get this expert

answer on brainly


Get your free account and access expert answers to this
and thousands of other questions

  • 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.

Looking for something else?

Not the answer you are looking for? Search for more explanations.