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# The angular shape of ozone molecule ${O_3}$ consists of:A. 1 sigma and 1 pi bondsB. 2 sigma and 1 pi bondsC. 1 sigma and 2 pi bondsD. 2 sigma and 2 pi bonds

Last updated date: 23rd May 2024
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Hint: Oxygen molecule has valency of -2. That is why it can form two sigma bonds with the other atoms. It has three lone pairs to form pi bonds with other atoms. Ozone has all three oxygen atoms and it’s a dihedral molecule with $s{p^2}$ hybridisation.

The Lewis structure for ozone ${O_3}$ consists of a central oxygen atom that has a double bond to one of the outer oxygen atoms and a single bond to the other oxygen atom. Lewis structure is based on the octet rule which states that there should be eight electrons in the outermost shell or orbit of an atom for the molecule to be stable.
Here, the lone pair on the central atom repels the electrons in the two side bonds present, forcing the atom to adopt a bent molecular geometry. Expected geometry is the trigonal planar, where O-O-O bond angle to be ${120^o}$. However, as per the context of the VSEPR model, lone pairs of electrons are considered slightly more repulsive than bonding pairs of electrons due to their closer proximity to the central atom. Therefore, the O-O-O angle is slightly less than ${120^o}$ i.e. ${116.8^o}$.
There are six valence electrons for each molecule of Oxygen in ozone and thus the total number of valence electrons is $6 \times 3 = 18$. As the octet rule applies, the central atom should have eight electrons in its outer shell. So, one molecule of the Oxygen is in the centre with the other two on the opposite sides of it.