The formal charges on the atoms marked as (1) to (4) in the Lew is representation
of $$HNO_{3}$$ molecule respectively are

We need to determine the formal charge on each of the atoms marked (1) to (4) in the Lewis structure of the nitric acid ($$HNO_3$$) molecule.

Key Formula: The formal charge of an atom in a Lewis structure is calculated using the following equation:

$$\text{Formal Charge} = \text{Valence electrons} - \text{Non-bonding electrons} - \frac{1}{2}(\text{Bonding electrons})$$

Alternatively, this can be written as:

$$\text{Formal Charge} = \text{Valence electrons} - L - B$$

Where $$L$$ is the number of lone pair electrons (individual dots) and $$B$$ is the number of bonds (lines connected to the atom).

Step-by-Step Calculation for Each Atom:

• Atom (1) — Oxygen atom bonded to Hydrogen and Nitrogen ($$\text{-OH}$$ group):

  • Valence electrons for Oxygen = $$6$$
  • Number of non-bonding electrons (dots) = $$4$$ (two lone pairs)
  • Number of shared bonds (lines) = $$2$$
  • $$\text{Formal Charge} = 6 - 4 - 2 = 0$$

• Atom (2) — Central Nitrogen atom ($$\text{-N-}$$):

  • Valence electrons for Nitrogen = $$5$$
  • Number of non-bonding electrons (dots) = $$0$$
  • Number of shared bonds (lines) = $$4$$ (one double bond, two single bonds)
  • $$\text{Formal Charge} = 5 - 0 - 4 = +1$$

• Atom (3) — Oxygen atom double-bonded to Nitrogen ($$\text{=O}$$):

  • Valence electrons for Oxygen = $$6$$
  • Number of non-bonding electrons (dots) = $$4$$ (two lone pairs)
  • Number of shared bonds (lines) = $$2$$
  • $$\text{Formal Charge} = 6 - 4 - 2 = 0$$

• Atom (4) — Oxygen atom single-bonded to Nitrogen ($$\text{-O}^-$$):

  • Valence electrons for Oxygen = $$6$$
  • Number of non-bonding electrons (dots) = $$6$$ (three lone pairs)
  • Number of shared bonds (lines) = $$1$$
  • $$\text{Formal Charge} = 6 - 6 - 1 = -1$$

Summarizing the calculated values in order from (1) to (4), we get: 0, +1, 0, -1.

Answer: Option A — 0, +1, 0, -1