Draw a labelled diagram showing the atomic orbitals for C and O on each side and the molecular orbitals for CO in the middle. The diagram should clearly show: /) which atomic orbitals combine to form each molecular orbital, ii) the relative position (increasing energy going up the page) of the molecular orbitals and the locations of electrons in the atomic orbitals and the molecular orbitals. Use your diagram to determine the following: • What is the bond order? Explain how you obtained this number from your MO diagram. The calculation must be presented. • Is the molecule diamagnetic or paramagnetic? Explain how you deduced this from your MO diagram. • From the following three possibilities, CO+, CO, CO-, determine which has the strongest bond? Explain with reference to your MO diagram.

How can we drsw the Lewis structures for the 4 boxes? And how many charges are in Oxime?

Which of the following statements about molecular orbital theory is incorrect? a) Bonding molecular orbitals result from the constructive interference of atomic orbitals. b) Antibonding molecular orbitals have higher energy than the corresponding bonding orbitals. c) Electrons in antibonding orbitals stabilize the molecule. d) The number of molecular orbitals formed equals the number of atomic orbitals combined.

how does molecular orbital theory make it possible to explain both ionic and covalent bonding? The degree of ionic characters in bonding is related to electronegativity in topic 2D. How does electronegativity affect the molecular orbital diagram so that bonds become ionic?