00:01
Okay, so we need to figure out how many specific types of electrons are in different atoms.
00:10
So the first part they ask is how many p electrons are in nitrogen.
00:15
All right, so we need to write out its electron configuration first.
00:20
So for nitrogen, we know that its atomic number is 7.
00:23
So we can write that as z is equal to 7.
00:27
And since we know that nitrogen is in its neutral state that its atomic number of protons, the 7 will be equal to its number of electrons, which is 7 as well.
00:39
So we need to have 7 electrons in our electron configuration.
00:45
So we know we start with the lowest energy orbital.
00:49
So this is 1s.
00:51
All right.
00:52
We have 2 in there.
00:54
So we have 5 left.
00:55
Then we're going to go to the second lowest, which is.
00:58
2s.
01:00
We have two electrons in there because we know we can only hold two electrons in each s orbital.
01:06
Now we have to move on to the third lowest, which is going to be 2p.
01:12
All right.
01:12
Since we have we need seven, we have four already.
01:16
We're just going to go ahead and fill up three.
01:20
The p orbital, so each of these suborbital are going to have one electron in them.
01:26
So this would be, total would be three total p orbitals or electrons in p subshells or p orbitals.
01:36
So now we're looking for s electrons in silicon.
01:41
So silicon has an atomic number of 14.
01:47
And since we know that it's neutral, we know that there must be 14 electrons as well.
01:53
So we can go ahead and say 1s2.
01:59
2s2...