Questions: A student proposes the following Lewis structure for the nitrate (NO3-) ion. Assign a formal charge to each atom in the student's Lewis structure. atom formal charge central O N right O left O

A student proposes the following Lewis structure for the nitrate (NO3-) ion. Assign a formal charge to each atom in the student's Lewis structure. atom formal charge central O N right O left O
Transcript text: A student proposes the following Lewis structure for the nitrate $\left(\mathrm{NO}_{3}^{-}\right)$ion. Assign a formal charge to each atom in the student's Lewis structure. \begin{tabular}{|c|c|} \hline atom & formal charge \\ \hline central O & $\square$ \\ \hline N & $\square$ \\ \hline right O & $\square$ \\ \hline left O & $\square$ \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Understanding the Lewis Structure

The nitrate ion, \(\text{NO}_3^-\), consists of one nitrogen atom and three oxygen atoms. The total charge of the ion is \(-1\).

Step 2: Calculating Total Valence Electrons
  • Nitrogen (N) has 5 valence electrons.
  • Each oxygen (O) has 6 valence electrons.
  • The ion has an extra electron due to the \(-1\) charge.

Total valence electrons = \(5 + 3 \times 6 + 1 = 24\).

Step 3: Drawing the Lewis Structure

The typical Lewis structure for \(\text{NO}_3^-\) involves:

  • Nitrogen as the central atom.
  • One double bond with one oxygen and two single bonds with the other oxygens.
  • Each oxygen has a full octet.
Step 4: Assigning Formal Charges

The formal charge formula is: \[ \text{Formal charge} = \text{Valence electrons} - \text{Non-bonding electrons} - \frac{\text{Bonding electrons}}{2} \]

  • Central O (double-bonded):

    • Valence electrons = 6
    • Non-bonding electrons = 4
    • Bonding electrons = 4
    • Formal charge = \(6 - 4 - \frac{4}{2} = 0\)

  • N (central atom):

    • Valence electrons = 5
    • Non-bonding electrons = 0
    • Bonding electrons = 8
    • Formal charge = \(5 - 0 - \frac{8}{2} = +1\)

  • Right O (single-bonded):

    • Valence electrons = 6
    • Non-bonding electrons = 6
    • Bonding electrons = 2
    • Formal charge = \(6 - 6 - \frac{2}{2} = -1\)

  • Left O (single-bonded):

    • Valence electrons = 6
    • Non-bonding electrons = 6
    • Bonding electrons = 2
    • Formal charge = \(6 - 6 - \frac{2}{2} = -1\)

Final Answer

\[ \begin{array}{|c|c|} \hline \text{atom} & \text{formal charge} \\ \hline \text{central O} & \boxed{0} \\ \hline \text{N} & \boxed{+1} \\ \hline \text{right O} & \boxed{-1} \\ \hline \text{left O} & \boxed{-1} \\ \hline \end{array} \]

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