Chapter 14: Q52E (page 599)
Using an MO energy level diagram would you expect F2 to have lower or higher first ionization energy than atomic fluorine. Why?
According to the MO energy level diagram you will expect F2to have low ionization energy than atomic fluorine.
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Using the molecular orbital model to describe the bonding in predict the bond order and the relative bond length for these species. How many unpaired electrons are present in each species?
Bond energy has been defined in the text as the amount of energy required to break a chemical bond, so we have come to think of the addition of energy as breaking bonds. However, in some cases the addition of energy can cause the formation of bonds. For example, in a sample of helium gas subjected to a high-energy source, some He2 molecules exist momentarily and then dissociate. Use MO theory (and diagrams) to explain why He2molecules can come to exist and why they dissociate.
Use the MO model to explain the bonding in BeH2. When constructing the MO energy-level diagram, assume that the Be 1s electrons are not involved in bond formation.
Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. Its ability to bond to iron in haemoglobin is the reason that (CO) is so toxic. The bond carbon monoxide forms to metals is through the carbon atom:
a. On the basis of electronegativities, would you expect the carbon atom or the oxygen atom to form bonds to metals?
b. Assign formal charges to the atoms in CO. Which atom would you expect to bond to metal on this basis?
c. In the MO model, bonding MOs place more electron density near the more electronegative atom. (See the HF molecule, Figs.14.45 and 14.46.) Antibonding MOs place more electron density near the less electronegative atom in the diatomic molecule. Use the MO model to predict which atom of carbon monoxide should form bonds to metals.
Describe the bonding in the first excited state of N2 (the one closest in energy to the ground state) using the MO model. What differences do you expect in the properties of the molecule in the ground state and in the first excited state? (An excited state of a molecule corresponds to an electron arrangement other than that giving the lowest possible energy.)
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