The correct formal charges on oxygen atoms numbered 2, 1 and 3 respectively are :

(B) The formal charge (FC) on an atom in a Lewis structure is given by the formula:
\(F C=V-L-\frac{S}{2}\)
where \(V\) is the number of valence electrons, \(L\) is the number of non-bonding electrons, and \(S\) is the number of shared (bonding) electrons.
For oxygen, the number of valence electrons is \(V = 6\).
For oxygen atom \(1\) (central atom):
It has \(1\) lone pair ( \(2\) non-bonding electrons) and 3 bonds ( \(6\) shared electrons).
\(F C_1=6-2-\frac{6}{2}=+1\)
For oxygen atom 2 (left atom):
It has 2 lone pairs ( \(4\) non-bonding electrons) and 2 bonds ( 4 shared electrons).
\(F C_2=6-4-\frac{4}{2}=0\)
For oxygen atom 3 (right atom):
It has \(3\) lone pairs ( \(6\) non-bonding electrons) and 1 bond ( 2 shared electrons).
\(F C_3=6-6-\frac{2}{2}=-1\)
The formal charges on oxygen atoms numbered \(2 , 1\), and 3 respectively are \(0 ,+ 1 ,- 1\).