Question

Which of the following statements is correct for ${\text{NO}}_3^ -$ ion?
(A) Sum of all formal charges is +1.
(B) Formal charge on one of the oxygen atoms is -2.
(C) Formal charge on nitrogen atoms is +1.
(D) Average formal charge on oxygen atom is $- \dfrac{2}{3}$

Answer 1

${\text{NO}}_3^ -$ ion is nitrate ion. It is obtained when nitric acid ionizes and loses a proton.
Use the following expression to calculate the formal charge on each atom

{{\text{Formal charge}}} \\\ {{\text{on an atom}}} \end{array}} \right) = \left( {\begin{array}{*{20}{c}} {{\text{Number of}}} \\\ {{\text{valence electrons}}} \end{array}} \right) - \left( {\begin{array}{*{20}{c}} {{\text{Number of}}} \\\ {{\text{non bonding electrons}}} \end{array}} \right) - \left[ {\;\dfrac{{\text{1}}}{2}\left( {\begin{array}{*{20}{c}} {{\text{Number of}}} \\\ {{\text{bonding electrons}}} \end{array}} \right)} \right]$$ **Complete step by step answer:** Nitrogen atoms have 5 valence electrons. Oxygen atoms have 6 valence electrons. One oxygen atom has additional electrons due to negative charge on nitrate ions. This additional electron is transferred to oxygen when hydrogen-oxygen bond heterolytically breaks in nitric acid to provide an electron. Draw the Lewis dot structure for nitrate ion.  Nitrogen atoms have 5 valence electrons, 0 nonbonding electrons and 8 bonding electrons. Since nitrogen forms four bonds, it has eight electrons. Calculate the formal charge on nitrogen atom: $$\begin{array}{l} {\rm{Formal\;charge }} = {\rm{ 5 }} - {\rm{ 0 }} - \left[ {\dfrac{{\rm{1}}}{2}\left( {\rm{8}} \right)} \right]{\rm{ = 5 - 4 = + 1}}\\\ {\rm{on\;nitrogen \;atom}} \end{array}$$ Singly bonded atom has 6 valence electrons, 6 nonbonding electrons and 2 bonding electrons. Since oxygen forms one bond, it has two electrons. Calculate the formal charge on singly bonded atom: $$\begin{array}{l} {\rm{Formal\; charge }} = {\rm{ 6 }} - {\rm{ 6 }} - \left[ {\dfrac{{\rm{1}}}{2}\left( {\rm{2}} \right)} \right]{\rm{ = 0}} - {\rm{1 = }} - {\rm{1}}\\\ {\rm{on \;oxygen\; atom}} \end{array}$$ Doubly bonded atom has 6 valence electrons, 4 nonbonding electrons and 4 bonding electrons. Since oxygen forms two bonds, it has four electrons. Calculate the formal charge on doubly bonded atom: $$\begin{array}{l} {\rm{Formal\; charge }} = {\rm{ 6 }} - {\rm{ 4 }} - \left[ {\dfrac{{\rm{1}}}{2}\left( {\rm{4}} \right)} \right]{\rm{ = 2}} - 2{\rm{ = 0}}\\\ {\rm{on\; oxygen\; atom}} \end{array}$$ Let us consider all the options: (A) Sum of all formal charges is -1 not +1. It is equal to the charge on the nitrate ion. So this option is not correct. (B) Formal charge on one of the oxygen atoms is 0. For the remaining 2 oxygen atoms, the formal charge is -1 on each oxygen atom. So this option is also not correct. (C) Formal charge on nitrogen atoms is +1. So this option is correct. (D) Average formal charge on an oxygen atom is $$ - \dfrac{2}{3}$$. This is also correct. There are three oxygen atoms with a total of formal charges on three oxygen atoms being $$0 - 1 - 1 = - 2$$ . _**Hence, the correct options are the options (C) and (D).**_ **Note:** The formal charge on an atom in a compound represents the number of electrons gained, lost or shared by that atom to form a bond. When an oxygen atom forms two covalent bonds by sharing of electrons, it has formal charge of 0. When a nitrogen atom forms three covalent bonds and one coordinate bond, it has formal charge of +1. When an oxygen atom accepts an electron, it has formal charge of -1. When an oxygen atom accepts bond pairs of electrons due to heterolytic bond cleavage, it has a formal charge of -1.