Question

Question 4.4 Draw the Lewis structures for the following molecules and ions:

H2S, SiCl4, BeF2,, HCOOH

Class XI Chemical Bonding and Molecular Structure Page 129

Answer 1

steps To draw Lewis structure
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step 1 :- find the total number of valance electrons of the combining atoms .For anion , the total negative charge is added to and for cation, the total positive change is subtracted from the number of valance electrons .
$ex : \: \: \: in\:SO_4^2-$
total number of valance electrons = 6 + 6 × 4 +2 = 32

step 2 :- The least electronegative atom is placed at the centre, surrounded by highly electronegative atoms .
$ex : \: \: \: in\:SO_4^2-$
S occupies central atom surrounded by O - atoms. because
$E_O > E_S$

step 3 :- Draw single bond among each atom, and then complete octet of surrounding atoms followed by central atom by assigning lone pair, double bond or triple bond.

[ in question CO3^2- missing , I added it ]

Answer 2

Answer:

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