1. Consider two hydrogen atoms A and B situated in the coordinate system shown below. Using similar axes draw: (a) the wave functions on individual H atoms 1 and i (b) the bonding combination of x and n (c) the antibonding combination of 1 and 11 (d) probability function 2 for the bonding combination (e) probability function 2 for the antibonding combination 2. Taking the inter-nuclear axis as the z axis, draw electron density sketches to illustrate the formation of bonding and antibonding molecular orbitals from the following atomic orbital combinations: (a) (s+s) (b) (pz+pz) (c) (px+px) Label each sketch with the signs of the underlying wavefunction. For each MO give its symmetry label, e.g., g 3. Define ,,,,, orbitals in terms of the nodal planes present (use diagrams where appropriate). Indicate whether each orbital is gerade or ungecade. 4. (a) Draw and label simple MO schemes to illustrate the bonding in the first row diatomic molecules B2 and O2. (b) Sketch the boundary surfaces of each MO. (c) Fxplain the differences between the MO schemes for B2 and O2. (d) Account for the magnetic properties and relative bend lengths in both B2 and O2 and the species generated by two-electron reduction of each. 5. (a) Draw and label MO energy level diagrams for HP,10O and CO. (b) Use the MO diagram for HF to describe the difference between non-bonding and anti-bonding molecular orbitals. (c) How is the MO scheme for carbon monoxide related to that for dinitrogen? 6. A main group element, A, reacts with hot concentrated sodium hydroxide solution to give two products, B and C, containing 33.31 and 60.66% A respectively. B(0.0958g) was reduced KMnOA solution. Identify A,B and C and write balanced equations for all reactions