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The angular shape of ozone molecule ($O_3$) consists of -
A
1 sigma and 1 pi bonds
B
2 sigma and 1 pi bonds
C
1 sigma and 2 pi bonds
D
2 sigma and 2 pi bonds
Detailed Solution
In ozone the central oxygen atom is $sp^2$ hybridised and the molecule is angular (bent) with a bond angle of about $117^\circ$.
Each resonance structure is written as $O=O^+-O^-$: the central oxygen forms one double bond and one single bond.
The single bond is one sigma bond.
The double bond consists of one sigma bond and one pi bond.
The central oxygen also carries one lone pair.
Total: 2 sigma bonds and 1 pi bond.
The two resonance structures make both O-O bonds equal in length (about 128 pm), but the count of bonds remains 2 sigma and 1 pi.
Each resonance structure is written as $O=O^+-O^-$: the central oxygen forms one double bond and one single bond.
The single bond is one sigma bond.
The double bond consists of one sigma bond and one pi bond.
The central oxygen also carries one lone pair.
Total: 2 sigma bonds and 1 pi bond.
The two resonance structures make both O-O bonds equal in length (about 128 pm), but the count of bonds remains 2 sigma and 1 pi.