Question

Draw an energy-level diagram for the valence molecular orbitals of CO. Include the relevant atomic orbitals in your diagram. Clearly label each molecular orbital (e.gs2s, p2p, etc.) and fill in the appropriate number of electrons. Use the same energy order as the neutral O2 molecule.

b) Is CO paramagnetic or diamagnetic? What is the bond order of CO? c) Draw a Lewis structure for CO. Does this match the predicted bond order? d) CO can react withOH– to form the formate ion, HCO2–. Draw the best possible Lewis structurefor the formate ion. Include any non-zero formal charges and resonance if appropriate.Describe the bonding in terms of sigma (s) and/or pi (p) bonds, discussing the orbitals involved in bond formation, and describing any delocalization if appropriate.(Note: In the formate ion, C is the only central atom; the H is bonded to C.)

The polyatomic ion [HCNXeF]+ has all the atoms bonded in the listed order, and its molecular geometry is entirely linear. Provide a Lewis structure that is consistentwith this molecular geometry.
b) Is CO paramagnetic or diamagnetic? What is the bond order of CO? c) Draw a Lewis structure for CO. Does this match the predicted bond order? d) CO can react withOH– to form the formate ion, HCO2–. Draw the best possible Lewis structure
b) In the molecule XeO2F2, the Xe–O bonding electrons take up slightly more space around the xenon atom than the Xe–F bonding electrons do. Given this information,predict the geometry of the XeO2F2 molecule. Draw a sketch of how this would appear, including the lone pair, and explain your reasoning.

Answer 1

diamagnetic

bond order = 2.5

Lewis Structure
http://upload.wikimedia.org/wikipedia/commons/1/14/Carbon-monoxide-2D-dimensions.png