Hybrid orbitals in ozone. A. Construct the normalized hybrid bonding orbitals on

Question

Hybrid orbitals in ozone. A. Construct the normalized hybrid bonding orbitals on the central oxygen atom in O3 that are derived from the oxygen 2s and 2p orbitals. The bond angle 0 in ozone is 116.8 degree. Hint Assume a single resonance structure in which the 0-0 bonds are identical. Start with the following expression for the bonding hybrid orbitals. (The molecule is in they z plane.) B. Next, show that these two orbitals are orthogonal (to within round-off error). C. Next, derive the coefficients for the hybrid orbital for the for the lone pair electrons on the central atom. (This orbital is orthogonal to the bonding hybrid orbitals). Use the following expression for the orbital to determine the magnitude of the coefficients. Then, choose the signs of the coefficients such that the orbital has the correct orientation. D. With all of this done, calculate the percent s and p character of each of the three orbitals; (The squares of the coefficients of the orbitals gives the fractional composition of that orbital; thus for the bonding orbitals, N^2 (c2^2 c3^2) is the fraction of p character in each bonding orbital.) How do these percentages compare for those in the 'standard' hybrid orbitals used in general chemistry for ozone?

Explanation / Answer

In the above 3 structures, structure 3 is called resonance structure in which the bond angle is same both the sides there will be one lone pair of electron on the central oxygen atom. The molecule is of the type AB2E, where AB2 is three oxygen atoms & E is electron.

Therefore in ozone we have 2 bond pair & 1 lone pair giving it a bent structure with bond angle 116.80       

            .|.

             A

         /       

B    B

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