Step 1: Understand the structure.
The given structure is of ozone:
\[
\ce{O3}.
\]
In one resonance form of ozone, one terminal oxygen is double bonded to the central oxygen and the other terminal oxygen is single bonded to the central oxygen.
Step 2: Formal charge on double bonded oxygen.
The oxygen atom numbered \(2\) is double bonded.
For double bonded terminal oxygen:
\[
\text{Formal charge}=0.
\]
So:
\[
O_2=0.
\]
Step 3: Formal charge on central oxygen.
The central oxygen atom numbered \(1\) forms one double bond and one single bond.
It has one lone pair.
In ozone, the central oxygen carries:
\[
+1
\]
formal charge.
So:
\[
O_1=+1.
\]
Step 4: Formal charge on single bonded terminal oxygen.
The oxygen atom numbered \(3\) is single bonded to the central oxygen and has three lone pairs.
Such terminal oxygen carries:
\[
-1
\]
formal charge.
So:
\[
O_3=-1.
\]
Step 5: Final order.
The question asks charges on atoms \(2,1,3\), respectively.
Therefore:
\[
O_2=0,\quad O_1=+1,\quad O_3=-1.
\]
Hence, the correct answer is:
\[
0,+1,-1.
\]
