Hybridization and Orbitals

Overview

1. Adopt a bonding model in which each oxygen of 02 is sp hybridized. Draw a structure of dioxygen that of its sp-hybrid orbitals.
   shows only the sigma-type electrons. This picture should show what each oxygen is "doing" with each

1. What valence orbitals on each oxygen are don vecion the spyonsinate process? Draw a separate picture of O, that shows these orbitals, but don't include any electrons in the picture.
2. Propose how the leftover orbitals on the first oxygen could overlap with the leftover orbitals on the second oxygen to create new molecular orbitals. Draw the orbital interaction diagrams (note that it is diagrams--plural) below. [Hint: This will be very similar to how we handled the double- and triple-bond parts of an alkyne in class (we did ethyne, also known as acetylene).]

1. If you take the total number of valence electrons in dioxygen and subtract the number of electrons accounted for in part b, how many valence electrons do you have remaining to fill into the orbitals you created in part d?
2. Fill the number of electrons calculated in part e into the orbitals created in part d. Respect Pauli (as always) but also Hund.
3. Considering your answers from both part b and part f, calculate the O-O bond order in dioxygen.
4. Take a deep breath--Dioxygen! Comment on anything you find curious about the electronic structure picture that has emerged from the above analysis.