To calculate the formal charge on the nitrogen atom in the compound NO nitrate ion , we will use the formula:Formal charge = Valence electrons of the atom - Non-bonding electrons - 0.5 * Bonding electrons First, let's determine the number of valence electrons, non-bonding electrons, and bonding electrons for the nitrogen atom in NO.1. Valence electrons: Nitrogen belongs to Group 15 or Group 5A in the periodic table, so it has 5 valence electrons.2. Non-bonding electrons: In the nitrate ion, nitrogen is bonded to three oxygen atoms, and there are no lone pairs of electrons on the nitrogen atom. Therefore, there are 0 non-bonding electrons.3. Bonding electrons: Nitrogen forms one double bond with an oxygen atom and two single bonds with the other two oxygen atoms. A double bond consists of 4 electrons 2 pairs , and a single bond consists of 2 electrons 1 pair . So, there are a total of 4 from the double bond + 2 from the first single bond + 2 from the second single bond = 8 bonding electrons.Now, we can plug these values into the formula:Formal charge = 5 - 0 - 0.5 * 8 Formal charge = 5 - 0 - 4Formal charge = 1However, we must consider that the nitrate ion has a -1 overall charge. This means that the formal charge on the nitrogen atom should be adjusted by -1:Formal charge = 1 - 1Formal charge = 0So, the formal charge on the nitrogen atom in the compound NO is 0.