Three resonance structures possible for N 2 O is to be drawn and also on the basis of formal charges relative importance of each structure is to be determined. Concept introduction: When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonances structure have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted into another by moving lone pairs to bonding positions, and vice versa. More important resonance structure selected as follows: 1. Always prefer smaller formal charge over the larger formal charge. 2. Always prefer the different non zero formal charge on adjacent atoms instead of the same non zero formal charge. 3. A more negative formal charge must be located on the most electronegative atom. Formula to calculate the formal charge of the atom is as follows: Formal charge = ( number of valence electrons ) − ( ( number of non-bonding electrons ) + ( 1 2 ) ( number of bonding electrons ) ) (1)

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Chapter 10, Problem 10.85P

Interpretation Introduction

Interpretation:

Three resonance structures possible for N2O is to be drawn and also on the basis of formal charges relative importance of each structure is to be determined.

Concept introduction:

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonances structure have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted into another by moving lone pairs to bonding positions, and vice versa.

More important resonance structure selected as follows:

1. Always prefer smaller formal charge over the larger formal charge.

2. Always prefer the different non zero formal charge on adjacent atoms instead of the same non zero formal charge.

3. A more negative formal charge must be located on the most electronegative atom.

Formula to calculate the formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of non-bonding electrons )+(12) (number of bonding electrons)) (1)

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