00:01
So for this question, we're trying to write the electron configuration for elements with these different number of electrons.
00:10
However, we're not allowed to use the periodic table.
00:16
So if you remember, electrons fill the orbitals in the specific pattern, which i've written down over here.
00:27
They go up quantum number, and so go 1s to 2s, then to 2p, then to 3s, then to 3p, and then 4s, et cetera, et cetera.
00:39
And so that is in the order they will fill.
00:41
The electrons will fill the orbitals.
00:45
And then if you remember an s orbital, an s has one orbital, and you can fit two electrons in one orbital.
00:57
So in the s orbital, we can have fit two electrons.
01:04
And then a d orbital, or the d, we have five orbitals.
01:12
And again, each orbital can have two electrons.
01:14
Two electrons.
01:14
So we have 10 total electrons for each d.
01:18
And then in the p block, a p has three orbitals, which each orbital has two electrons.
01:28
We'll have six electrons for every p.
01:31
So we just got to do a little bit of math.
01:34
So let's start with a, which has 10 electrons.
01:39
So we do one s.
01:40
S, we have two electrons, 2, 2s2.
01:45
We have four electrons, 2p6.
01:50
That gives us 10 electrons.
01:52
So that's going to be the electron configuration for a.
01:56
Let's go to 22...