they don't.
Two equivalent Lewis structures are necessary to describe the bonding in O3. These structures involve adding a double bond between each pair of oxygen atoms in alternate arrangements.
They could be useful while determining the valency of atoms and the structures of chemical bonding in plausible ways.
Resonance effect: It is a way of describing delocalized electrons within certain molecules or polyatomic ions where the bonding cannot be expressed by one single Lewis formula.A molecule or ion with such delocalized electrons is represented by several contributing structures called as resonance structures or canonical forms. Inductive Effect: It is a permanent effect. When group attached to carbon atom attract electrons from them or push the electrons toward it is called as Inductive effect.
Ozone is not an example of resonance (by all possible meanings). It does have two bonding forms that it occasionally changes between. These two forms are called resonant states... but the bonding does not "resonate" per se.
Covalent Bonding
For SO3, two equivalent resonance structures are sufficient to describe the bonding.
In chemistry, resonance is a way of describing bonding in certain molecules or ions by the combination of several contributing structures (or forms, also variously known as resonance structures or canonical structures) into a resonance hybrid (or hybrid structure) in valence bond theory
Resonance structures refer to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure. The Lewis dot structures show valence electrons.
Two equivalent Lewis structures are necessary to describe the bonding in O3. These structures involve adding a double bond between each pair of oxygen atoms in alternate arrangements.
2
1
2
1
4
2
A single Lewis structure can be used to represent the bonding in SeF2O.
2