so I'm going to be teaching youtuber Melissa Lucy electron configuration today and it's gonna help her stress less and it's gonna help you stress less so breathe we're gonna get through this together so just starting off with like what orbitals are and what they represent this is like a fancy definition of saying like oh it's the probability of finding an electron at a point in space I just want you to think that electrons hang out there okay electrons like to be in orbitals that's probably the most likely place that we could find them it's I can't say that it's definite you know but we know that electrons exist within orbitals now there are different types of atomic orbitals that you're going to see specifically like different shapes so the first one you're going to talk about is known as s and that's like more of a sphere shape so s is gonna be our sublevel this is gonna be really important to understand like oh what's a sublevel what's an orbital and then how many electrons are in there because I've actually seen this question all the time just asking like oh how many orbitals are possible in a p subshell and like that little you know terminology if you don't know it it's going to be difficult to answer okay so just knowing okay it's it's at an s subshell and then there's only one orbital that can hold two electrons so by one orbital you're either gonna see it kind of represented like this with as an orbital diagram where it's kinda like boxes or you might just see it as a line so you might see it like either like this where it says 1s and then you might also see it as just like a line and it says 1s and then we would actually draw electrons just to note that electrons spin in opposite directions when they are actually in the same orbital so this should all kind of sound familiar yes okay cool so the next sub shell that we have is the P sub shell that has three orbitals and that can hold up to six electrons because there are two electrons for every orbital in since you know 3 times 2 gives a 6 that's where the six electrons come from so I did put the shapes I don't expect you to know the shapes you know all these like kind of funky shapes I don't expect you to know that but it's just a good visual this is actually what we kind of think it looks like and let's move on in the next one d subshell has five orbitals and can hold ten electrons and then lastly f subshell has seven orbitals and that can hold fourteen electrons this is probably the rarest one that you'll see typically they don't have you draw an orbital diagram for like an f subshell because it's so large but just in case we'll do one mm-hmm you never know and then something that also know is just how the orbitals are going to fill so it's gonna fill the lower energy orbitals like this one s and that out then it goes to to us 2 P 3 s and so on until it goes to like the higher energy orbitals so always fill the lower first and then it goes to the higher and how you know what's what's low what's high you know like you're not even looking at this chart is just based on the coefficient in front so like since this is one that's lower than two you know so that's how you know okay i'm gonna fill that first okay and the order is according to the letter also yes so we'll go over that I will definitely go over the order and then I'll teach you I don't want you to memorize the order because I think that is like one it's terrible to have to memorize and two it's gonna be a lot easier to just know where everything is positioned on your periodic table and then from there you'll be able to do it so it's gonna be a lot of counting like it's gonna seem kind of tedious but once you learn how to actually use the periodic table to find everything you don't have to remember the order okay or memorize the order I'll say so just knowing that these first two groups are our s subshell and then same thing here with helium this actually would have been helium and the next four are P sub shells that's going to be in that purple area and then D is going to be that transition metals and then lastly this last part is going to be F so we will do an example of every single type meaning like you know one in the S one in the P D and F before I move on something that's going to be really important specifically with D and F it's just the order of it so this is going to say you're probably going to either see this as n minus 1 or n minus 2 before I even get to that I just want you to know that n is talking about that coefficient in front so n is is talking about like the energy as we saw before you know we're like 1s is going to be lower energy than like 2's 2 so this is what's represented by n so and could be 1 to any sort of integer that we have so by n minus 1 that just means it's going to be 1 less than the row that it's in so like this would have been you know Row 1 Row 2 3 and 4 so this would have been like instead of like actually where it is iron actually let's say titanium so let's say if we're ending at titanium instead of this being 4d because it's in that level that because it's on D and that's always n minus 1 that's actually going to be 3d kind of making sense we'll go over a bunch but for now I just want you to understand the D is always one less okay then the row that it's in like it's in row four but that n is actually gonna be one less so three okay but the S section will always be just what it is correct same with the P okay I think I guess cool we'll go over it don't worry but okay the next one is also F that's actually two less so it's n minus two so that's two less than the row that it's in and then beware of this for the F let me see if I can I'll get to it but we'll cover that in a second but for now I just want you to know that little bit of okay D that's not going to be this as the roads in it's always gonna be one less and then f it's always gonna be two less than the road that it's actually in but s and P stay the same okay all right so just understanding what everything represents in our electron configuration knowing that they're basically just telling us how electrons are occupying our orbitals and specifically you know what energy level they're at or what type of sub shell they're at so sure this is the order and like I said I think it would just be a pain to have to remember all of this you know so it's gonna be a lot easier to just know where everything is on the periodic table and go from there so another thing they also know as we mentioned was just like what everything means for our electron configuration notation so like this is actually gonna mean that it's the orbital and then that superscript is going to be the number of electrons that are in that orbital so is the orbital the position of it so it's pretty much like we're here let me go back to the different types like let's say for like s like we can imagine that it looks like this like it's kind of like the sphere it's telling you what type of orbital it's going to be in so like whether it's gonna be an SPD or F like that's kind of what it's talking about okay and then and then typically you know based on like s P D and F it's also gonna help us understand you know either the shape of the orbital actually that's what that tells us that tells us the shape and then that coefficient in front tells us how how high that is on this like energy table so how much energy that orbital has or that atom at us I should say okay certain it kind of makes sense I know there's like little things that that you always have to know everything about me okay so I wanted to practice a bunch with this because it can get a little bit tricky so let's just start off with doing several different types of I'm gonna call this as like the full electron because there is the quality there an abbreviated noble gas method condensed shorthand so many words but typically they call it a condensed electron configuration and it's kind of like just a way that we can abbreviate it so instead of writing like the whole entire thing let's say if it was all the way at the bottom that would be way too long okay and you'll get what I mean in a second so if I were to start off with just writing the full electron configuration or let's say hydrogen so I'd see okay well this is this is the first row and I know that that's in the S location so that is one so I'm getting that one from the wrote in and then I know okay well this is s because it's telling me right here so s and then next is it's also going to let me know so you let me do a different color purple how many electrons hydrogen has and then we know okay everything's neutral right now so it's going to be the same amount of electrons as our our atomic number which is that one so one okay do we see that yes so that means that's the only one like for hydrogen yes but it's gonna change when we have more electrons so and it's also gonna be really important to just know well s can only have two electrons like that's it that's its max and then P its max is going to be six and then after that D is 10 and then F is 14 we can't go past that number so once you do then you go into the next group exactly yeah so I'll reset for now so let's say if I were to do beryllium then I'm gonna look again here and I'm gonna see okay I have to start in the very very beginning and then make my way all the way to beryllium so I'm going to start off with 1 so 1 and then this is s so I'm gonna say 1 s 1 1 s 2 because I'm literally going across and then I'm going to come back around to beryllium so then this is 1s2 good so far is that making sense um I can say it again so but I'm saying so you don't count like each individual one so you're not like saying like 1s 1 for hydrogen and then another 1s 1 yeah so you go all the way to the end of that group and then write it or yes and and the reason is because it's past its past that point so it's kind of like we have to go all the way until we get to the element that we're looking for and because this is this is one s one and this is another electron in the same row and in the same orbital for subshell sublevel sorry sublevel then I know that this is going to be a 2 so it's accounting for that because this is 1s to you guys this is 1 s 1 this is 1 s 2 ok then what about the lithium so then because we passed lithium like beryllium is is passed lithium then I know that this is going to be well 1 this is at 2 because it's the second row 2s and it's like I'm counting to s 1 - okay ok well and then if I were to do let's say if I let's look at carbon my not-so would do the same thing for carbon so I'll start off in the very beginning so this is 1 s 1 s 1 1 s 2 now typically so anything cast helium we're always going to start with 1 s - yes correct ok and it's like like anything passed kind of like the next point you're gonna fill the orbitals entirely so the same thing here because we're going to carbon I'm passing this point right this is 2 s 2 s 1 and 2 and then I'm going to keep going straight across until I get to carbon so this is still in the second row but now we've changed the sub level two P so now it's P and then I'm going to count again one and two so two P 2 is P still like N equals like you know degree or that it is yes ok yeah it's still going to be the same number as the roads in it's only D and F that change Scott okay so another thing also know is just if we were to count the electrons like the the superscript here which is the electrons that would give us the same amount of electrons as beryllium or whatever element we're looking for so like here this is you know two plus two gives us four beryllium has four electrons and then same thing here for carbon so two four six carbon has six electrons so you might get a question where they actually give you the electron configuration and they ask you to say you know to figure out what element it is and that's a trick just add everything up and that'll give you the correct amount of electrons okay God and then you would just find it on the periodic table yes okay yeah all right that's okay I can do it I'm gonna do another one yeah this is good this is good practice I am was very confused so it's nice to know that there's a system and I don't have to remember all of those because that's yeah like there's no need to memorize it once you understand it it's that's all that matters um I'll do maybe one more because I do want to talk about something else let's see okay let's do phosphorus alright so you want to try oh sure no but I'm sure okay so one s two for sure so passive feeling cool and then to s2 correct okay good going straight across and this I just want you to count so what row are we in currently we're going to P nu right and then what what row like now we just need to pee yeah okay and then count so we're going all the way to like this is what we're trying to get phosphorus okay gonna have to keep going all the way through so we can literally just count so one two three four five six which tells us I know that four for the p subshell only six electrons can be there like that's the maximum good keep going I'm going to turn around okay so now it's gonna be three s - mm-hmm go straight across this is so weird that's every kind of a peg like this okay it's like okay so now we are gonna do 3 P 3 yes ok cool ok good so that's the general idea of this it's gonna be it's gonna change a little bit of course there will be exceptions but knowing like having a good foundation of this understanding what it should be it's gonna help a lot so the other thing I wanted to talk about like this is the full electric configuration now we're gonna do the condensed electron configuration so the condensed electron configuration is going to look something like this so let's do this for phosphorus here what you're going to always do like the notation of this is you're always going to put whatever noble gas is in the row right above it right above the element that you're looking for so that noble gas is going to go into in brackets and then the remaining electron configuration or like you know sub shells are gonna go at the end so if I were to look at phosphorus right here what's the noble gas that is right before it like in the row right before it I don't know what is this row okay oh this girl oh okay so these are the noble gases got it all of these yeah something Andy I just don't know what that one means neon yeah oh that's me on okay got it still working so neon would basically take the place of all of this like all of this gets replaced with just the noble gas and we know that because if I were to do the electric configuration of neon I would start with okay well 1s to know make my way I'm here now I'm at 2's to go straight on across and then I'd end that one two three four five and six at 2p 6 so do we see how that literally replaces this chunk like this beginning portion of our full lecture configuration and like now it's like neon telling us oh this is kind of like a bookmark like kind of like a placeholder to tell you where to start and then where do you continue yeah and it adds up to 10 - right so right okay so so then from there I can just put the remaining part of it so the remaining portion of this would have been 3s2 3p3 so this is the elect the condensed electron configuration okay that top part is the full electron configuration yeah that's nice ok cool we'll do more so let's do nitrogen together why don't you start it off okay just a regular one just the regular one okay so nitrogen is right there yeah um so we do 1s - good you're 2s2 good goin straight across to p3 perfect so now let's try doing the condensed electric configuration okay so helium is right there so we just put an AGM in the brackets perfect and then it's gonna be oh I still have to do okay so what's the remaining part now um 2s2 2p3 that's it okay yeah not too bad yeah perfect now let's do something that is in that d subshell so we'll do this one together I'll look for wherever iron is which is right here so I'll start off with just the typical one the full electric configuration so starting off with actually I'll have I'll have you start off and then once we get to the D level I'll explain what to do okay so um 1s2 2s2 2p6 you're right okay 3 s 2 correct and then went across three p6 perfect gone around again and 4s - good and then once we're we get to that D sublevel we know it's always going to be 1 less than the row it's actually in so instead of 4d it's going to be 3 D and then you count to wherever your element is so from here it would have been 1 2 3 4 5 and 6 so 3 D 6 ok yeah yeah so always one less the D is always like n minus 1 1 less than the row that it's actually in so instead of 4 it's three got it what would the condensed electron configuration be here um it would be is that are gone yes okay so a are for us too good and then three these six perfect okay yeah that's it awesome well we'll do some more alright so this one's gonna be a little bit longer we're gonna go to PR which is all the way down here oh I'm gonna have you walk me through it until we get to until we get to here and then I'll explain cheese are we gonna have space we'll have space I'll have to write a little bit smaller the love space so let's just start off with the first one good okay umm 1s2 2s2 good mm 2p6 3s2 3p6 great 4s2 oh now it's this next place since we're not stopping anywhere do I still have to do the whole thing where it's less you do and it's because you have to go through the entire periodic table until you get the element that you're looking for and that's all the way down here so we're gonna still be in the threes then yes okay so I don't know how many's in this one ten oh yes the DA always has ten d sub levels and then f has 14 okay so three D 10 okay um for p6 you're right and then five or yeah five mmm that's two and then we're gonna do before this time okay so for T 10 this is like a puzzle it's like a trick question to me okay um so now we're on five so five piece makes good and then 6s too cool and I'm gonna say let's stop and the reason we're gonna stop here is because um this group like this is actually meant to be like right here and why did we do it this way and it has to do with properties but unfortunately that's how the periodic table is designed so a clue here is just looking at the atomic numbers so like seeing that this went from 56 to 71 that's not all right there right counting you know so from 56 to 57 that should make more sense so then that's why we have to like stop here so we're stopping like right here and then we're actually going go through this entire like level and then go back since this is 71 okay so then this is our F block so we know okay well this is F and this is always 2 less than the row that's in so we previously said we were in row 6 so what should that be now so it's gonna be for F 3 so yes perfect that's it okay so you're just like so I need to remember that point on the periodic table to know when the other ones come in correct okay yeah and we'll do several examples but what would be condensed electrical figuration be here do I still go based on where it would be like right there right oh okay so then X a good Xenon okay so so we start with 6 s 2 and then 5 D 10 hold on but still we had that little break oh just kidding okay oh no we're going to - so for after oh and I'd say hey that's it all right that's it I prefer that one thank you same-same so once again remember that xenon is taking the place of all of this okay and then that's why we can just say oh okay just left the last little portion cool let's do another one so it's to mercury which is I mean but that's in a different color which is here all right so I'll have you started off again I am in an even more room let me delete this okay go for it okay so um 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5 s 2 4 d 10 dead 5 P 6 good success - good and breaking point right because we're trying to get to mercury which is 80 but we have to go through this entire oh my gosh okay so um so now we're gonna be at 4 again so we do oh wait there's 14 in this one right yes okay so it's gonna be for f-14 good and then 5 f-14 and then haunt then then we go back so this is 71 we go back to 70 sorry 270 and then we go back to 71 so now we're back in the D sub level oh okay okay wow that's so you gotta pay attention okay yeah yeah definitely so now we're gonna be 5d oh okay okay and then I think I think we're good with that any questions so far no no this is like finally making a little bit of sense which is nice [Music] if you're enjoying studying along with us so far make sure you give this video a like and turn on your notification bell because we're going to keep studying all semester long all right if you're ready to learn something new click on that next video [Music]