00:01
So for this question, you're asked to find several different things about the element germanium.
00:07
So first, we're asked to find the full electron configuration and then the noble gas configuration.
00:16
So first, let's do the full electron configuration.
00:19
So first, if you look at your periodic table, the symbol for germanium is ge.
00:24
So if you look, and it's number 32 on the periodic table.
00:28
So when we start filling out our electron configuration, right, we start with one and we go all the way through.
00:40
So i have the rows labeled one, two, three, four, five, right, which those are going to be our principal quantum number.
00:48
And then remember with the periodic table, these first two columns are in the s block.
00:57
The transition metals or these 10 in the middle are in the d block.
01:02
And then these six columns on the right are in the p block.
01:08
So let's start.
01:12
So in the first row, we have 1s2, and then the second row we go 2s2 and then 2p6.
01:31
Then we start in a row 3, 3s2, then 3p6, then we go into row 4, so we have 4s2, then we go completely through the d block.
01:49
So remember with the d block, the principal number is one less than the row it's in.
01:55
So we're in one row four.
01:56
So the principal quantum number is going to be three.
02:00
And then we're going to 3d10, right, because we have 10 electrons in the d block.
02:05
And then we go two until we hit germanium.
02:08
So this will be 4p2.
02:13
And that's going to be your full electron configuration.
02:17
So next, let's go.
02:18
To the noble gas configuration.
02:22
And so this is just kind of a shortcut way to write the full electron configuration.
02:28
So basically we start where germanium is on the periodic table.
02:31
We go back to the nearest noble gas, so which would be argon, right? because germanium doesn't have enough electrons to make it to krypton.
02:46
So we have to go to the row three noble gas, which is argon.
02:50
So we'll write argon as our.
02:53
Noble gas core, and then we start counting electrons from argon forward.
02:58
So we're starting at row four.
03:02
So then we go 4s2.
03:05
Again, we hit that d block, which the number is one less.
03:09
The principal quantum number is one less than the row it's in.
03:13
So 3d10, so we have 10 electrons in the d block.
03:17
And then over two till we get to germanium.
03:20
So it'll be 4p2 because we only have two.
03:24
Electrons in the p block.
03:29
So this will be your noble gas electron configuration.
03:35
Now, which ones are the valence electrons? so the valence electrons are going to be in your outermost shell.
03:46
And so those electrons are going to be in the shells with the highest principal quantum number.
03:52
So it's going to be of the electrons with the principal quantum number four, right? because that's the highest.
04:00
So we're not going to include the 3d.
04:02
So our valence electrons, here i'll put ve for valence electrons, are going to be in the 4s2 and 4p2.
04:14
And if you count them up, we have the two electrons in the s block and the two electrons on the p block.
04:19
So germanium actually has four valence electrons.
04:25
So now, now we're asked to find the quantum numbers for each of those four valence electrons.
04:33
So let's start with the quantum numbers for the two electrons in the 4s block.
04:42
So remember quantum number? it starts first with n, the principal quantum number, which we have given to us already.
04:50
So four is our principal quantum number, so that's going to be n, that first number.
04:55
Then l is always going to be at least one less than the principal quantum number.
05:05
So if you remember l, if the n is 4, then l can be 3, 2, 1, or 0.
05:17
And these numbers actually correspond to which orbital it is in...