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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 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 16
In some cases the removal of an electron from a species can result in a stronger net bonding \((e . g .\) an \(\mathrm{O}_{2}^{+}\) ion versus an \(\mathrm{O}_{2}\) molecule). Give an example in which the addition of an electron to a species produces a stronger net bonding.
Problem 19
How many valence electrons are there in a \(\mathrm{BH}_{3}\) molecule? Describe the bonding in a \(\mathrm{BH}_{3}\) molecule in terms of hybrid orbitals.
Problem 28
How many valence electrons are there in a chloroform molecule, \(\mathrm{HCCl}_{3}\) ? Describe the bonding in a chloroform molecule.
Problem 45
Draw the cis and trans isomers of 2-butene, \(\mathrm{CH}_{3} \mathrm{CHCHCH}_{3} .\) Label each isomer.
Problem 49
Naphthalene is a white, crystalline solid with an odor characteristic of mothballs. Write the complete Lewis formula for and describe the bonding in a naphthalene molecule, \(\mathrm{C}_{10} \mathrm{H}_{\mathrm{s}}\), How many \(\sigma\) bonds and \(\pi\) bonds are there in a naphthalene molecule? How many valence electrons occupy \sigma-bond orbitals and how many occupy \(\pi\) -bond orbitals?
Problem 57
What is meant by a "delocalized" electron? How are delocalized electrons described using Lewis formulas? How are they described using molecular orbital theory?
