The Electron Configuration: Exceptions (Simplified)

So when it comes to electron orbital stability, you just need to remember that D sub shells orbital's are most stable when they are half filled or totally filled with electrons because of symmetry. So what we mean by half field, remember, we're gonna follow huns rule which says that orbital's that have the same energy that are the generate our first half filled. So we're dealing with. But up up up up here, we have a set of D orbital's electrons that are all facing up. So this set of orbital's are half filled. Now totally fill, we go up up, up, up, up, then come back around, down, down, down, down down. So here we have an example of a half filled set of D orbital's in here, a set of totally filled in D orbital's.

Now, when looking at exceptions to the electron configurations, we're going to say starting from chromium, which is CR as the atomic number Z increases exceptions to electron configurations can be observed. A memory tool here we can have is that chromium has an atomic number off 24. So think about that two and four. We're going to say that the exceptions happen with these two elements and with these four elements, so two and four we're going to say here we're gonna start out with chromium. We know that's where it starts, and we're gonna skip the next four columns, right? So we start out with chromium and you skip next four. So skip, manganese, skip iron, skip cobalt, skip nickel, and then you land on copper, where the next group of exceptions can exist. So just remember, these are the six major types of elements where we were going to see exceptions to the electron configuration. So keep this in mind when we're looking at their electron configurations. Now that we know that these are the 60 that we have to deal with, let's see how these exceptions arise. So click on the next video and let's see what happens

So remember exceptions start with chromium. So let's look at chromium if we're to determine its electron configuration. Initially, we would see that it would look like are gone for us to three d four. Now here. What do we have here? We have three D with four electrons within it. But remember earlier we said that s N d sub shells or sub levels have this urge to try to be half filled or totally filled. Now we're gonna say an s orbital electron can be promoted to create half filled orbital's with D four electrons. So what we're saying here is if you're doing the electron configuration of chromium, you're gonna end with a D four. That's a key to tell you that O d four. We have only four electrons within these d orbital's. But if I could somehow get one more electron in there, those deorbit will be half filled. So what's gonna happen here is we're gonna take one electron from the forests and donated over here, so our three d four is going to become a D five and our for us to just gave up on electrons. It becomes for us one. So it now looks like this. This would be the correct electron configuration of chromium. So again, remember, chromium has this type of exception, and the driving force is trying to get a half filled set of d orbital's. Okay, so here we're not gonna land. We're not going to stay as D four when it's neutral. It's gonna become a D five. Now that we've seen this with the first column, let's see what happens with the second column. So click on the next video and let's see what happens with them.

So if we look at the second column, let's look at copper now, Copper, If we look at the periodic table, we'd initially think it's are gone for us to three d nine. But if we look at the three d nine Orbital's, what we should notice is we just need one more electron here and it will be completely filled. Remember, there is this need this drive by your P and D sub levels or some shells to be either half filled or totally filled. So we're gonna say here in electron and s orbital electron can be promoted to create completely filled orbital's with D nine elements. Here, copper is a D nine element. It ends with D nine. If you could just get one more electron, it could become the 10. And that's what's gonna happen. We take one from the S orbital before s orbital on. We donated over to the deep doing this. Now, we only have one electron here within for us, and this now becomes totally filled in and therefore more stable. So now this is for us. 13 d 10. So just remember, we have these six elements we discussed previously um in the videos, they have this drive where we're going to take one electron from an s orbital and promoted to one of the D orbital's so that we can create either a half filled D orbital's or totally filled, completely filled the orbital's remember this driving force that causes the exceptions within these neutral elements?

here in this example question it says, based on the exceptions, provide the condensed electron configuration for the silver atom. So we're gonna say here that silver is a G. It has an atomic number of 47. Since we're dealing with an atom, it's the neutral form of it. So it has 47 electrons now, looking at the periodic table. What we would see initially is we would see crypt on five s to four d nine. Remember, Silver is one of the elements within the second column we discussed. And remember, it's a D nine element. If it could become D 10, those orbital's will be completely filled. In order to do this, we're gonna take one electron from the S orbital and promoted up to the D set of Orbital's doing. This gives us now the correct exception to silver, which is crypt on five s, one four d 10. So this would be the correct electron configuration for silver. So just keep in mind the six elements we discussed earlier, all of them to do this where we take one electron from the S orbital and promoted up so that we either have half filled the orbital's or completely filled in D. Orbital's like silver here