Write formulas for the compounds that form from {\rm Rb} and each of the following polyatomic ion: {\rm NO}_{3}^{-}, {\rm SO}_{4}^{2-}, {\rm PO}_{4}^{3-}.
You really need to look at your posts. They don't make sense to me because of the various symbols used. Using {\rm and_ along with } is confusing unless we know what those symbols mean.
Apparently you want the formula for rubidium nitrate. RbNO3.
rubidium sulfate. Rb2SO4. We CAN write subscripts and superscripts on the board but it is too much trouble to do; therefore, we understand that Rb2SO4 means the 2 and 4 are subscripts.
rubidium phosphate is Rb3PO4.
hell no
Write the name of \({\rm CrPO}_{4}\)
ddfr
To find the formulas for the compounds that form from Rb and each of the given polyatomic ions (NO3-, SO4^2-, PO4^3-), we need to consider the charges of the elements involved.
Rb (Rubidium) is a group 1 element with a charge of +1.
Let's go one by one:
1. Compound formed with NO3- (nitrate):
The formula will be RbNO3.
To determine this, we cross the charges of Rb and NO3- ions. Since Rb has a +1 charge and NO3- has a -1 charge, we do not need to use subscripts to balance the charges.
2. Compound formed with SO4^2- (sulfate):
The formula will be Rb2SO4.
To determine this, we cross the charges of Rb and SO4^2- ions. Rb has a +1 charge, and SO4^2- has a -2 charge. In this case, we need two Rb ions to balance the charge of SO4^2-.
3. Compound formed with PO4^3- (phosphate):
The formula will be Rb3PO4.
To determine this, we again cross the charges of Rb and PO4^3- ions. Rb has a +1 charge, and PO4^3- has a -3 charge. In this case, we need three Rb ions to balance the charge of PO4^3-.
So, the formulas for the compounds formed between Rb and the given polyatomic ions are:
- RbNO3 (Rubidium nitrate)
- Rb2SO4 (Rubidium sulfate)
- Rb3PO4 (Rubidium phosphate)