It turns out that Ce has a ground-state electronic configuration of [Xe]4f15d16s2. The reason why this atom has 3+ and 4+ ions is now a little clearer: The 3+ ion probably has a [Xe]4f1 configuration while the 4+ ion has a simple [Xe] electronic configuration.
You can see from this example why I didn't make a big deal of the lanthanides and actinides in class: Their chemistry is really quite complex.
The
p1 and
p-1 orbitals are tori. If
we add two such orbitals (one from each atom), we get a
cylindrical molecular orbital with a nodal line (a region of
depressed electron density) along the bond
axis. These are
orbitals.
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transition |
24.32592 | 1.611852 | 2 |
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36.48882 | 2.417774 | 3 |
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48.65164 | 3.223691 | 4 |
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60.81408 | 4.029583 | 5 |
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