(a) Using only the valence atomic orbitals of a hydrogen
atom and a fluorine atom, and following the model of
Figure 9.46, how many MOs would you expect for the HF
molecule? (b) How many of the MOs from part (a) would be
occupied by electrons? (c) It turns out that the difference in
energies between the valence atomic orbitals of H and F are
sufficiently different that we can neglect the interaction of
the 1s orbital of hydrogen with the 2s orbital of fluorine.
The 1s orbital of hydrogen will mix only with one 2p orbital
of fluorine. Draw pictures showing the proper orientation
of all three 2p orbitals on F interacting with a 1s orbital
on H. Which of the 2p orbitals can actually make a bond
with a 1s orbital, assuming that the atoms lie on the z-axis?
(d) In the most accepted picture of HF, all the other atomic
orbitals on fluorine move over at the same energy into the
molecular orbital energy-level diagram for HF. These are
called “nonbonding orbitals.” Sketch the energy-level diagram
for HF using this information and calculate the bond
order. (Nonbonding electrons do not contribute to bond
order.) (e) Look at the Lewis structure for HF. Where are the
nonbonding electrons?
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