Two types of carbon -carbon covalent bond lengths are present in
Answers
Recall that resonance represents an average of the types of bonds that are present. To my knowledge, the idea of resonance is in sync with the calculations behind the Schrodinger's equation, (which represents that the observed particle is at the lowest possible energy level when it is at the "average" position relative to its neighbors) [Chem_Mod, please correct my explanation if I am wrong]. In the O3 Lewis structure you've drawn, there is a single bond (which is longer than a double bond), and a double bond. In the case of O2, there is a double bond in between the two oxygens to yield ::O::O::
Recall that single bonds are longer than double bonds, and double bonds are longer than triple bonds. This means that single bonds are relatively weak compared to double and triple bonds since the two atoms are further apart, and therefore, allow the atoms within the molecule to readily interact with other molecules more easily than double or triple bonded molecules. Back to the question, the average of the length of double bonds and single bonds is greater than that of a double bond, and less than that of a single bond. Thus, O3 will contain longer bond lengths as compared with O2.
The experimentally determined bond lengths of O2 and O3 are as follows:
Bond length of O2 is 0.121 nm.
Bond length of O3 is 0.128 nm.