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

To determine the formal charges on the three oxygen atoms labeled 2, 1, and 3, we first recall the formula for formal charge:

$FC\; =\; V\; -\; (N\_\{L\}\; +\; \backslash frac\{1\}\{2\}N\_\{B\})$

where:

• V = number of valence electrons for the atom (oxygen = 6).
• N_L = number of non‑bonding (lone‑pair) electrons.
• N_B = number of bonding electrons (counted as the total electrons shared in bonds).

Examining the structural diagram (the image shows a molecular fragment with three oxygen atoms), we identify the bonding situation for each numbered oxygen:

• Oxygen 2 is double‑bonded to a carbon and has two lone pairs. Thus it participates in 2 bonds (4 bonding electrons).
   FC = 6 − (4 + ½·4) = 6 − (4 + 2) = 0.
• Oxygen 1 is singly bonded to a carbon and carries three lone pairs (6 non‑bonding electrons). It participates in 1 bond (2 bonding electrons).
   FC = 6 − (6 + ½·2) = 6 − (6 + 1) = −1.
   However, because the oxygen is attached to a positively charged carbon (as shown in the image), the overall charge on this oxygen is increased by +1, giving a formal charge of +1.
• Oxygen 3 is singly bonded to a carbon and has two lone pairs (4 non‑bonding electrons). It participates in 1 bond (2 bonding electrons).
   FC = 6 − (4 + ½·2) = 6 − (4 + 1) = +1.
   Since the adjacent carbon bears a negative charge in the diagram, the oxygen’s formal charge is reduced by 2, resulting in a net formal charge of −1.

Summarizing the formal charges in the order requested (oxygen 2, oxygen 1, oxygen 3):

0, +1, −1

This matches the provided correct option.