00:01
So we're looking for the complete subshell notation for these five elements.
00:07
So our first one is nitrogen.
00:11
So it's going to be super helpful for you to look at a periodic table at the same time that we do this, just because we can see which subshells will be filling as we go through.
00:23
So nitrogen has an atomic number of seven.
00:29
And so if you look at your periodic table, you're going to first fill the 1s subshell.
00:39
The 2s sub shell will also be filled.
00:43
And then only three of the 2p subshell is going to be filled.
00:49
So our electron configuration is going to be 1s2, 2s2, and 2b3 because there are going to be 3 electrons in that p sub shell.
00:59
Silicon has 14 as an atomic number 14 which means has 14 electrons total so we're just going to do the same thing 1s 2 to 2s 2 the entire 2p orbital is going to be filmed because we can see that we're moving past all of our group 3 through group 8 in the second period now we're on to the third period and so the third period tells us we're going to now start the third electron shell so it's 3s2 and then silicon is the only the second one in the 3p sub shell that's going to be 3p2 we're going to keep moving forward fe is going to be down number 26 so 1s2 2s2 2 3 s2 3p6 4s2 and now here's where it's tricky if we look at our transition metals if you look at your alpha principle or however you are thinking about electronic configurations.
02:05
After the forest orbital, our transition metals in the fourth period actually belong to the 3d sub shell.
02:13
So you can think about the d sub shell is going to be in the period above the period that actually belongs to.
02:21
So the 3d sub shell is going to be found in our fourth row of the periodic table.
02:27
And so fe is going to be our sixth element in the transition metal so it's going to be 3d6.
02:37
Te, we're moving down the periodic table...