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Magazine Problem 1
Use molecular orbital theory to explain why a diatomic beryllium molecule does not exist under normal conditions.
Problem 2
Use molecular orbital theory to calculate the bond order of a diatomic boron molecule.
Problem 3
Use molecular orbital theory to predict whether or not a diatomic carbon molecule is paramagnetic.
Problem 4
Use molecular orbital theory to predict whether or not a diatomic boron molecule is paramagnetic.
Problem 5
Use molecular orbital theory to explain why the bond energy of a \(\mathrm{N}_{2}\) molecule is greater than that of a \(\mathrm{N}_{2}^{+}\) ion.
Problem 6
Use molecular orbital theory to explain why the bond energy of an \(\mathrm{O}_{2}\) molecule is less than that of an \(\mathrm{O}_{2}^{+}\) ion.
Problem 7
Use molecular orbital theory to predict the relative bond energies and bond lengths of a \(\mathrm{F}_{2}\) molecule and a \(\mathrm{F}_{2}^{+}\) ion.
Problem 8
Use molecular orbital theory to predict the relative bond energies and bond lengths of a diatomic carbon molecule, \(\mathrm{C}_{2}\), and the acetylide ion, \(\mathrm{C}_{2}^{2-}\).
Problem 11
Write the ground state electron configurations and determine the bond orders of the following ions: (a) \(\mathrm{O}_{2}^{-}\) (b) \(\mathrm{C}_{2}^{+}\) (c) \(\mathrm{Be}_{2}^{+}\) (d) \(\mathrm{N}_{2}^{*}\)
Problem 12
Write the ground state electron configurations and determine the bond orders of the following ions: (a) \(\mathrm{C}_{-}\) (b) \(\mathrm{B}_{2}^{+}\) (c) \(\mathrm{He}_{2}^{+}\) (d) \(\mathrm{F}_{2}^{2-}\)
