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Basics of Chemical Bonding

Question

Write lewis structure of the following compounds and show formal charge on each atom $$ HNO_3 , NO_2 ,H_2SO_4$$

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Solution

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Formal charge on an atom in a Lewis structure = [total number of valence electrons in free atom] – [total number of non-bonding (lone pairs) electrons] —1/2 [total number of bonding or shared electrons]

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Q1

Write Lewis structure of the following compounds and show formal charge on each atom.

H N O_{3}, N O_{2}, H_{2} S O_{4}

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Q2

(i)

Write Lewis structure of the following compound and show formal charge on each atom.

$H N O_{3}$

(ii)

Write Lewis structure of the following compound and show formal charge on each atom.

$N O_{2}$

(iii)

Write Lewis structure of the following compound and show formal charge on each atom.

$H_{2} S O_{4}$

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Q3

Draw the Lewis dot structures of H2SO4 and HNO3 and hence show the formal charge on each of the atoms in both cases.

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Q4

48. Lewis dot structure of N2O. And formal charge on each atom.

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Q5

Consider the following Lewis Dot structure:

{[: ¨ N = N = ¨ N :]}^{-}

The formal charge on the central

N

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