00:01
This question addresses the concept of electron configurations.
00:04
And we're asked to compare a few different species of oxygen first.
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And utilize, of course, our handy -dandy periodic table to do just that.
00:13
So oxygen in its ground state configuration.
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We follow the periodic table.
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We'll have a 1s subshell that's completely filled with two electrons.
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Then a 2s subshell that's also completely filled.
00:25
And then we start to utilize the three orbitals for the 2p subshell.
00:30
Oxygen being right here, where since it has four total 2p electrons, the first three we placed in their own space and their own orbital, but that fourth electron will have to be paired in one of the orbitals.
00:48
The question is how many unpaired electrons does oxygen have in its ground state configuration? well, it has two unpaired electrons we can see since these two electrons are unpaired in the remaining 2p orbitals.
01:06
We're also asked to take a look at what would happen into that 2p orbital if we were to have an oxygen canion.
01:14
Okay, so remove one of those electrons.
01:17
Which one would we remove then? well, we have an unfavorable pairing of electrons here in this first 2p orbital.
01:26
So it would be that one of those on the one of those paired electrons that would be removed to make the oxygen cat ion and then we would have we can see three unpaired electrons once that change takes place how about the oxygen anion well again go back to our original oxygen where we had two paired electrons and know that we need to find a space for one more electron that means we're going to have to pair up a second orbital and in this case we can see we will only have one unpaired electron in the oxygen anion.
02:10
Now the next example we're asked to take a look at is osmium in its ground state configuration.
02:16
So it's located here in the sixth row of the periodic table and we're going to just do a shorthand configuration.
02:25
All the core electrons are going to be contained in xenon and then we move to the sixth row of the periodic table where we contain the first two electrons in the 6s sub -shell.
02:37
Then we're going to completely fill that 4f sub -shell with all 14 electrons.
02:43
And then we move back to the 5d sub -shell, where we have 1, 2, 3, 4, 5, 6 d electrons that we need to find a home for.
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So remember that we have 5d orbitals.
02:57
The first 5 electrons are all going to be unpaired, but that 6th electron is going to have to share a home with one of the orbital.
03:04
Orbitals.
03:05
So that leaves four unpaired electrons in the osmium configuration.
03:18
Now the next example asks us to take a look at zirconium.
03:21
Again, a shorthand configuration shows the core electrons in krypton...