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Hey there!
A ) PO₄³⁻
The element exhibits resonance (4 times) as there is a double bondwith 1 oxygen and a single with the other 3 oxygen. This switchesin each resonance structure. (I know its weird b/c I leaves Phosphorus with 10 electrons surrounding it)
b) SO₄²⁻
Sulfur is the central atom ,double bond 2 oxygens so that they can only have 4 valence electrons ( the little dots around the oxygen ) ,single bond 2 oxygens ( So that they have 6 valence electrons )
Formal charges are 0 for the two double bonded oxygens [ 6-6 = 0 ]and 0 for the sulfur [ 6-6=0 ]
But the oxygens are -1 [ 6-7 = -1 ]
Since there are two of them, there is a negative charge of -2
Bracket the whole structure and on the top right of the outside ofthe brackets write 2- and include a - (negative sign) next to eachof the single bonded oxygens
Don't forget there are resonance structures. The double bonds canbe placed around any of the oxygens
Hope that helps!
The polyatomic oxyanion have 4 bonded oxygen atoms.
(A) Polyatomic oxyanion are the molecules consisting of nonmetal bonded woth more than one oxygen atom.
Thus the central atom in the structure is a nonmetal from period 3.
Based on the valence electrons in the structure i.e. 32.
The charge for -1, -2, and -3 is calculated.
The n = -3 has 5A group belongs to Phosphorus.
The n = -1 has Chlorine
n = -2 is Sulfur.
(B) Formal charge = Valence electrons - nonbonding electrons - [tex]\rm \frac{bonding\;electrons}{2}[/tex]
For n = -1,
Formal charge = 32 - 24 - [tex]\rm \frac{8}{2}[/tex]
Formal charge = 4
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