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Answer :
To find the formal charge of nitrogen in the nitrate ion [tex]\((NO_3^-)\)[/tex], where one of the oxygen atoms forms a double bond with the nitrogen atom, follow these steps:
1. Determine the Valence Electrons for Nitrogen:
- Nitrogen is in Group 15 of the periodic table, so it has 5 valence electrons.
2. Count the Bonding Electrons:
- In the nitrate ion, nitrogen forms a double bond with one oxygen atom and single bonds with the other two oxygen atoms.
- A double bond consists of 4 shared electrons, and each single bond consists of 2 shared electrons.
- So, the total number of bonding electrons shared by nitrogen is [tex]\(4 + 2 + 2 = 8\)[/tex] electrons.
3. Non-Bonding Electrons:
- Typically, in this structure, nitrogen does not have any lone pairs of electrons. Thus, it has 0 non-bonding electrons.
4. Calculate the Formal Charge:
- The formula for calculating formal charge is:
[tex]\[
\text{Formal Charge} = \text{Valence Electrons} - (\text{Non-bonding Electrons} + 0.5 \times \text{Bonding Electrons})
\][/tex]
- Plug in the values:
[tex]\[
\text{Formal Charge} = 5 - (0 + 0.5 \times 8)
\][/tex]
[tex]\[
\text{Formal Charge} = 5 - 4 = 1
\][/tex]
Therefore, the formal charge of nitrogen in the nitrate ion when one of the oxygen atoms forms a double bond with nitrogen is 1. The correct answer is B. 1.
1. Determine the Valence Electrons for Nitrogen:
- Nitrogen is in Group 15 of the periodic table, so it has 5 valence electrons.
2. Count the Bonding Electrons:
- In the nitrate ion, nitrogen forms a double bond with one oxygen atom and single bonds with the other two oxygen atoms.
- A double bond consists of 4 shared electrons, and each single bond consists of 2 shared electrons.
- So, the total number of bonding electrons shared by nitrogen is [tex]\(4 + 2 + 2 = 8\)[/tex] electrons.
3. Non-Bonding Electrons:
- Typically, in this structure, nitrogen does not have any lone pairs of electrons. Thus, it has 0 non-bonding electrons.
4. Calculate the Formal Charge:
- The formula for calculating formal charge is:
[tex]\[
\text{Formal Charge} = \text{Valence Electrons} - (\text{Non-bonding Electrons} + 0.5 \times \text{Bonding Electrons})
\][/tex]
- Plug in the values:
[tex]\[
\text{Formal Charge} = 5 - (0 + 0.5 \times 8)
\][/tex]
[tex]\[
\text{Formal Charge} = 5 - 4 = 1
\][/tex]
Therefore, the formal charge of nitrogen in the nitrate ion when one of the oxygen atoms forms a double bond with nitrogen is 1. The correct answer is B. 1.
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