Question

Give the Lewis structure of (a) an oxide of nitrogen in the +5 state. (b) the strongest oxoacid of nitrogen. (c) a tetrahedral oxoanion of sulfur.

Short answer

Question: Sketch the Lewis structures of (a) an oxide of nitrogen with a +5 oxidation state, (b) the strongest oxoacid of nitrogen, and (c) a tetrahedral oxoanion of sulfur. Answer: (a) The Lewis structure for dinitrogen pentoxide (N2O5) is: ``` O = N - O - N = O || O || ``` (b) The Lewis structure for nitric acid (HNO3) is: ``` O || H-O-N=O ``` (c) The Lewis structure for the sulfate ion (SO4^2-) shows resonance and is represented as: ``` O O || | S S | || O O ```

Step-by-step solution

Identification

The oxide of nitrogen in the +5 state is dinitrogen pentoxide (N2O5). For the strongest oxoacid of nitrogen ((b)):

Identification

The strongest oxoacid of nitrogen is nitric acid (HNO3). For a tetrahedral oxoanion of sulfur ((c)):

Identification

A tetrahedral oxoanion of sulfur is the sulfate ion (SO4^2-). Now, we will draw the Lewis structures for these species.

Lewis Structure for N2O5

To sketch N2O5: 1. Count the total number of valence electrons: N x 2 (5) + O x 5 (6) = 40 valence electrons. 2. Begin by drawing a skeleton structure by connecting N and O atoms and placing a double bond to satisfy the octet rule. 3. Calculate the formal charges and adjust the structure to minimize formal charges. The Lewis structure for N2O5 is: ``` O = N - O - N = O || O || ``` For the strongest oxoacid of nitrogen (HNO3):

Lewis Structure for HNO3

To sketch HNO3: 1. Count the total number of valence electrons: N (5) + O x 3 (6) + H (1) = 24 valence electrons. 2. Begin by connecting the N, O, and H atoms. 3. Calculate the formal charges and adjust the structure to minimize formal charges. The Lewis structure for HNO3 is: ``` O || H-O-N=O ``` For a tetrahedral oxoanion of sulfur (SO4^2-):

Lewis Structure for SO4^2-

To sketch SO4^2-: 1. Count the total number of valence electrons: S (6) + O x 4 (6) + 2 (extra electrons for 2- charge)= 32 valence electrons. 2. Place the central (S) atom and surround it with the O atoms. 3. Add bonding electrons and lone pairs to satisfy the octet rule. 4. Calculate the formal charges and adjust the structure to minimize formal charges. 5. Include resonance if possible. The Lewis structure for SO4^2- shows resonance and is represented as: ``` O O || | S S | || O O ```