Write formulas for the compounds that form from In and each of the following polyatomic ion: NO−3, SO2−4, PO3−4.
(Assume In charge is 3+.)
InNo9, InSO6, AND InP4 is wrong
NO-3 ? , SO2-4 ?, PO3 -4
Where did you get these strange charges for the ions?
eg PO3 normally -3
ASSUMING your strange valences:
In +3
NO -3
then to be neutral
InNO
In+3 * 4 = +12
SO2-4 * 3 = -12
so
In4(SO2)3
similarly
In4 (PO3)4
But I suspect you have the original statement messed up
I'm sure you mean [NO3]^-, [SO4]^2- etc.
Then In(NO3)3, In2(SO4)3, etc.
If we could write subscripts very well on this forum the nitrate would be [NO3]-
there copied straight from the question page, this is making sense
To write the correct formulas for the compounds that form from In and each of the polyatomic ions NO3-, SO42-, and PO34-, we need to use the correct charges for both In (3+) and the polyatomic ions.
First, let's determine the charge of each polyatomic ion:
1. The nitrate ion, NO3-, has a charge of 1-. To balance the charge, we need three NO3- ions for every In ion. Therefore, the formula for the compound will be In(NO3)3.
2. The sulfate ion, SO42-, has a charge of 2-. To balance the charges, we need two SO42- ions for every In ion. Therefore, the formula for the compound will be In2(SO4)3.
3. The phosphate ion, PO34-, has a charge of 3-. To balance the charges, we need one PO34- ion for every In ion. Therefore, the formula for the compound will be InPO4.
In summary, the correct formulas are:
- In(NO3)3 (for the compound formed with NO3- ion)
- In2(SO4)3 (for the compound formed with SO42- ion)
- InPO4 (for the compound formed with PO34- ion)