1. 3D structure  2. Hybridization and underlined atom geometry  3. bond angles around the underlined atom 4. overlapping orbitals for two of the (different) bonds around the central atom

Consider a heteronuclear diatomic molecule, AB, where A and B are period 2 elements. Using the following pieces of information, provide details on the molecular orbital diagram of AB: Clue 1: The MO diagram of AB does not contain non- bonding electrons. Clue 2: The s and p orbital energies of both atoms are quite close to one another that interactions between different orbital types occur. Clue 3: AB" is more stable than AB, but AB2 is less stable than AB". Clue 4: The potential energies of the atomic orbitals of A are higher than the potential energies of the atomic orbitals of B. Table 1. Atomic orbital energies of period 2 elements. Atom Orbital energy Orbital energy (2s) (2p) Li -5.45 Ве -9.30 B -14.0 -8.30 C -19.5 -10.7 -25.5 -13.1 -32.3 -15.9 F -46.4 -18.7 Ne -48.5 -21.5

A bond arises from "sideways" overlap of two parallel p orbitals. The electron density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals. orbital on C+ References Use the References to access important values if needed for this question. orbital on O What atomic or hybrid orbitals make up the bond between C and O in carbon dioxide, CO2? How many o bonds does C have in CO2? How many bonds does C have? + p-orbital p-orbital atom ₁ atom 2 T bond