Which formula represents strontium phosphate?
(1) SrPO4 (3) Sr2(PO4)3
(2) Sr3PO8 (4) Sr3(PO4)2
Strontium has a charge of 2+ as an ion, and \(PO_{4}\) a charge of -3. So to get an equal charge, the least common multiple is 6, so you would need 3 Strontium ions and you would need 2 phosphate ions. Keep in mind that you have to multiply the entire ion, so you would need to have \((PO_{4})_{2}\), NOT \(PO_{8}\) because then you would only have 1 phosphorous, and that would not be phosphate anymore.
So the correct one is #4
Answer: The correct answer is Option 3.
Explanation:
Strontium is the 38th element of the periodic table having electronic configuration of \([Kr]5s^2\)
This element will loose 2 electrons to form \(Sr^{2+}\) ion.
Phosphate ion is the polyatomic ion having formula of \(PO_4^{3-}\)
By criss-cross method, the oxidation state of the ions form the subscript of the other atom which represents the number of atoms.
Hence, the chemical formula of strontium phosphate becomes \(Sr_3(PO_4)_2\)
Thus, the correct answer is Option 3.