Answer:
Any one structure in the image can used to show the Lewis structure for [tex]N_2O[/tex].
Explanation:
Lewis structure is used to represent the arrangement of the electrons around the atom in a molecule. The electrons are shown by dots and the bonding electrons are shown by line between the two atoms.
For [tex]N_2O[/tex],
The number of valence electrons = [tex](5\times 2)+6[/tex] = 16
The skeleton structure of the compound is in which one N molecule act as a central atom and is bonded to another N and O with one sigma bond each.
Number of valence electrons used in skeletal structure = 4
So,
Remaining valence electrons = 12
The central atom still needs 2 lone pairs and the nitrogen and oxygen attached to it, still needs 3 lone pairs each. So, total number of valence electrons needed to complete the octet of all the atoms = 16
But, we have 12 electrons and thus, 2 additional bonds are required in the structure which can be distributed in the 3 atoms in 3 ways.
[tex]\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}[/tex]
For Structure A:
Formal charge on central atom N:
[tex]\text{Formal charge}=\text{5}-\text{0}-\frac{\text{8}}{2}[/tex]
[tex]\text{Formal charge}= +1[/tex]
Formal charge on substituent atom N:
[tex]\text{Formal charge}=\text{5}-\text{4}-\frac{\text{4}}{2}[/tex]
[tex]\text{Formal charge}= -1[/tex]
Formal charge on substituent atom O:
[tex]\text{Formal charge}=\text{6}-\text{4}-\frac{\text{4}}{2}[/tex]
[tex]\text{Formal charge}= 0[/tex]
For Structure B:
Formal charge on central atom N:
[tex]\text{Formal charge}=\text{5}-\text{0}-\frac{\text{8}}{2}[/tex]
[tex]\text{Formal charge}= +1[/tex]
Formal charge on substituent atom N:
[tex]\text{Formal charge}=\text{5}-\text{6}-\frac{\text{2}}{2}[/tex]
[tex]\text{Formal charge}= -2[/tex]
Formal charge on substituent atom O:
[tex]\text{Formal charge}=\text{6}-\text{2}-\frac{\text{6}}{2}[/tex]
[tex]\text{Formal charge}= +1[/tex]
For Structure C:
Formal charge on central atom N:
[tex]\text{Formal charge}=\text{5}-\text{0}-\frac{\text{8}}{2}[/tex]
[tex]\text{Formal charge}= +1[/tex]
Formal charge on substituent atom N:
[tex]\text{Formal charge}=\text{5}-\text{4}-\frac{\text{2}}{2}[/tex]
[tex]\text{Formal charge}= 0[/tex]
Formal charge on substituent atom O:
[tex]\text{Formal charge}=\text{6}-\text{6}-\frac{\text{2}}{2}[/tex]
[tex]\text{Formal charge}= -1[/tex]
The Lewis structures in resonance of the compound is shown in the image.
