okay it is time for the long ways AP chemistry review it's crazy I'm gonna be completely honest with you if you can is one of my most Gary ApS not gonna watch because I know physics I know math but chemistry come on hello everybody I'm Cara and today we're going to be doing unit one of the AP chem curriculum which as you can see on the screen is atomic structures and property then we're gonna cover all that nonsense so as you can probably tell we're gonna start with moles and molar mass nonsense now because a became an AP chem II only be at some level of proficiency it can when you're taking the test I'm not going to go over all the neutron proton electron nonsense there's no you got your protons for positive you got your electrons which are negative and you got your neutrons which is just boring and don't have charge and basically important on the periodic table we got our beautiful dynamic P table over you look at it change color beautiful but the point is like the numbers over here are obviously the protons and then you got your atomic masses over here so basically a time masses are the best way to introduce the point of a mole what type of the mole no it's not like they're beautifully cute walk even on lowly cubes have you seen the star-nosed mole or naked mole rat they look disgusting but the point is when a mole basically means is is a number of like atoms it's basically like if you have a dozen egg that's 12 right a mole means the most arbitrary number 6.02 times 10 to the 23 and you should probably know this club you do not want to be like checking your formula sheet every time you want to check what a mole is now like honestly the number itself it not super useful but basically what unless you do is it lets you convert from atomic mass unit which is basically like your a proton have one atomic mass unit neutron has one atomic Mathieu it converts that to grant that's literally all you got to know about mole it basically converts grams to atomic mass unit so basically we know that if you have one molecule of like nitrogen let's say one any boy over here basically it's gonna have only 14 and hugh's and you can't measure like 14 em use a nitrogen that does doesn't work a kiss but you can matter 14 grand but basically the point of the Avogadro's number would it take point Oh 10 to the 23 is that if you have 14 grams of nitrogen you could tell exactly how many molecules are in it we know that there's exactly one mole of nitrogen because we know that in order to get from one molecule which is 14 amu we in order to get to grant from 14 amu to 14 gram you have to multiply it by one mole now the reason why this is useful this concept of white walls is because it doesn't matter how many grams of something you have right if you have like let's say that one feather reacts with one Rock right make a rock feather sure why not so let's say you have five grams of better than five grams of raw obviously the more feathers in five grams then there are rocks in five grand so like you're gonna have wave extra feathers and like the five grams didn't tell us anything we have to know how many feather there are not how much they weigh so that's why I'm older nice but cuz I tell you how many there are okay so basically like this right now I was telling them to a mu of each atom but you can also think of it as grams per mole because we know that amu to get to grams we multiply that mole so mu times mole than equal to grant so if we want grams per mole which is basically our molar mass right mass over mole then that's that's equal to an emu so it's actually basically what I'm trying to say is that you could think of me numbers underneath all of these letters as molar mass right so the easiest way to think of stuff in a pecan business think of it as a ratio of units so in AMU is a gram over mole like if you want to get from remember mole it's a grand unit multiplied by moles and that way like it just makes your mother so much easier but they know exactly what you hadn't multiplied to get your answer your answer is in grams multiplied me mole if your entered the mole then you have to do grams over grams or moles and then you get more okay quick examples all right let's say you have like 25 grams of calcium okay then if you want to find out how many moles we had to do it over 40 point oh eight grams per mole you know why because if we cancel out the units mole gets into the numerator and we want moles so this makes so much sense and twenty-five over four forty point oh eight gives us zero point six two four we're am epic and if you want to convert from moles to molecules we just use our same conversion factor just think of everything that's converted packing 0.62 four times 6.02 times 10 is 23 molecules per mole and boom we have one at 6.0 2064 3.7 6 times 10 to the 23 molecule C like movie on mole here small cans about you doesn't molecule and that's what we wanted very cool okay that busy all you got to know about like a tonic mass and what it means and what moles are okay all right now we're gonna talk about isotope do you know that an isotope basically just an atom with the same number of protons but different number of neutrons right because it's the same element but it does have a different mass so just annoying right these elements just have to have different isotopes in nature right so like Brooke what are all these random decimal points doing well basically what this is is the average atomic mass of all the fluorine atoms in the world so clearly nature is not being attended to the Declaration of Independence or constituent or whatever I don't pay attention to me cuz I'm sorry but like you didn't pay attention to the fact that all men are created equal animate isotope unequal god Danny but basically the point is like some isotopes are more common than others so in order to do finding decimal things you gotta like take the weighted average of the components like the different isotopes so just like if you have more of a certain type of isotope its weight matters more so why don't we just search a relative abundance of carbon isotope Lana and then we will go to Wikipedia because Wikipedia is the most viable source of information all right so basically this gives us our abundance right here so essentially if we had 100 carbon atoms right 98.9 of them which doesn't make any sense but we're still gonna go with it not only when nine of them are going to be carbon 12 meaning they have six protons six neutrons okay and then 1.1 of them are going to be carbon 13 with one more Neutron okay so we have ninety eight point nine of them that way 12 amu then we basically have a total weight for all of those ones over there to be ninety eight point nine times twelve right and basically to find an average you have to take the total and item weight divided by the total molecule or atom so this is the total amount for carbon-12 then what is the total amount of weight for the carbon 13 there at one point one of them right and we have weight of 13 amu and then that's the total weight of over all of the carbon atoms in our 100 carbon sample and then we divided by the total number mark it was just 100 and what will this give us let us see already give the 12.011 wait a minute where did I see that before that's why you saw it in the periodic table let me show you this flex my epic skill look at that 12.1 hole on one we calculate it from scratch look at that flex okay I know how to calculate relative abundances no wait what is it having a talking about under the different location I'm just gonna stop there apparently the AP then does not want to stop there it's not gonna just stop and maybe you calculate the thing from scratch it's gonna actually show you in anagram so basically what we got to do is you got to explain the concept of mass spectrometry so basically let's say you got a little mix of like random isotope okay you got some carbon 13 spliced in there you got some carbon 12 there just hanging around here they're all normal carbon atoms so now the first thing that the mass spectrometer does it goes in here and it slams some electrons into these boys relentlessly okay it's like a massacre it's like the Boston Massacre except it's massacring them with electrons and it doesn't kill them see I did pay attention than a foot okay come on come on basically well the massacre actually does instead of killing them it turns them into ions so now that we have charges it doesn't even matter whether they're plus or minus charges but the reason we have some charge I'm not exactly sure what it is for carbon but anyway their charge that is the point and basically what these charge particles are done are they're fed up they're like slam through an electric field that goes super super speedy and then they enter a magnetic field Wow so now I have a magnetic field right we slam the electrons through basically and a magnetic field exerts a force proportional to your charm so anyway these arms pass me the electric fields the ones that are more charged get deflected even more however the more massive ones get deflected less because it's harder to move a more massive object so basically then they go like this right they get deflected so I'm get deflected more someday if I could last like that okay and then they all go into a certain detector that's over here boom it hits after they hit the detector boom to hit the detector and basically the ones that got deflected Leafs are going to hit at the top the one that gets deflected the most are gonna hit at the bottom and basically the ones with the highest charge to mass ratio are gonna get to them up okay so basically what you can take away from this without knowing that the entire working though a mass spectrometer is that it basically tells you the ratio of charge to map and basically what they do on the AP exam and they take it and put it in a chart and they basically give you the data there so they got your charge to mass ratio over here or I think that you're gonna do mass to charge and then they do your relative abundance abundance let's say some of the iZotope become plus one card right there's gonna be some from 12 they're gonna be some from carbon 13 so obviously if they both have a charge of +1 then like the carbon 13 ions are gonna have a higher mass to charge racism ratio because I have more mass however they'll be less of them detected so the only be like this menu this is like a number of carbon 13 atoms that hit the detector however at a lower mass Itard ratio which is your part of 12 there's gonna be way more of them essentially like need to leave this will be out of a hundred percent and then it'll give you ninety eight point nine percent and then one point one ampere so like absolutely mistake that a lot of people make is that they don't they send them to the after you make sure that this is mass or charge it matter yet it make sure you know what the charge is before you find out what the mass of the isotopes is but if you find out what the mass of each I picked up is we find that this one is 12 and this one is 13 then we could apply our same calculation to find the actual average atomic mass so know how to read mass spectrometry data is important the y-axis can also be relative abundance okay and basically what that does it it basically does everything relative to the highest peak so in this case I'm home of the highest peak and then this peak would be how much is one point one percent of 98.9% like how much is it relative to the carbon and then I'll give it here it's still basically one point one percent because like ninety eight point nine so big so this would still be one point one over here about a little bit bigger though if you're given relative abundances to get their original abundance you basically just do like one point one over the total who did 1.1 plus a 5 okay well you can really do that regardless this is just a good rule to know you basically do my percentage over the percent the sum of all the consent is of all the other one okay that's all you gotta know from mass spectrometry and isotope moving on Dalton's logs okay what are Dalton's all basically what Dalton says is this epic God Allison okay he looks kind of like this basically what he said is he says the first thing is that like atoms are the smallest unit of stuff same he also said that mass is conserved all right this stuff is pretty common sense may not for him because it was like ancient but yeah to know this stuff okay and then another thing he said is that compounds have a characteristic ratio of like atoms so basically if you have pure h2o every single molecule in the app in that like substance is going to have the same ratio of hydrogen to oxygen no matter which part of that something you think is gonna have the same ratio and maybe that's called a law of constant composition alright now that we know that the law of constant composition exists what we could basically do is start writing out formulas to represent compound so basically it doesn't go over really quick like what makes up different types of materials you've even got your elements which are individual pure substances that are made up of only one element right then you got compounds which are pure substances of course but they're made up of multiple elements then you got your mixtures which are not made up of multiple compounds and not bonded to each other like covalently but they are together in the same mixture and then with a mixture and you got like solutions you got your suspensions blow water we're not talking about that now we're only focused on caliphal right now so yeah the point is you doing other stuff but Bisby right now we're kind of a compound so basically to represent compounds the first thing you gotta know is there a chemical formula which is basically exactly what their molecule is the vending the pretty good example right you got Ben being this boy over here lately this is all the structural form law of benzene and it basically shows you the bomb then doesn't a great structural form oh because the struggle for my should show you the 3d representation like whether it come out of your pumped in at you but I'm too lazy for that nonsense but that's not the point who cares only the I am we got to do the important stuff so Ken big weed you write out the number of each element to the molecule so maybe we got six carbons epic so we're gonna write C which is the symbol for carbon to the sick and then we got six hydrogen each stick nice you got a chemical formula now we've got to convert this to an empirical formula which basically reduces everything to the so that like the smallest lemon fonville puts it in not fraction there so in this case literally you could divide everything by 6 and we got CH you got to make sure that your proportions are the same like if you want to check with your empirical formula right that make sure that you don't have any practice and you multiplied by some number it gets to the actual formula okay there's some nonsense about dealing with empirical formulas but we will wait until we get it Stokey on between to talk about that I'm pretty sure we'll talk about that in the next unit so that should be yeah let's label our diagram so this is called structural right this over here is called chemical and the most reduced one is called empirical all right now that we got that down we got to talk about ions so basically your atom looks like this right you've got nice little nucleus that's positively charged then you gotta put your electron swirling around like cool kids over here okay so electrons kind of look like shells they're turning on a challenge because there's orbitals because other probability nonsense but you can basically think of it a shot doesn't like it increases in energy so basically your outermost energy level is called your valence energy level or your valence shell of electrons and basically the only thing that's really important about an atom is valence electron like no one cares about the guys on the inside okay those got informed so in this particular atom you got six electrons okay so oh I don't want to make eight electrons so this island is going to get to electron that in order to make eight so I'm gonna have a two plus charge just kidding I know that L are kinda negative two minus charge there we go so this boy is gonna make it to - char similarly if you have seven then it would be one - if ya like only two oh I probably want to lose those two electrons to get to empty sub shell instead and it would be two plus so basically that what two things gonna remember is the negative ion there an ion and then two clusters a cation because positive and the way to remember this is cap our you guessed it the epoca spot of the century positive wow that's some beautiful stuff not gonna lock you I could have thought of that myself and I am the best pie maker in the universe all right so some atoms are cool and they like giving away their electrons or maybe well they're kind of selfish honestly because they didn't want to get to that beautiful eight-pack electron but they do give away their electrons sometimes or sometimes it snatching from others but tonight I was cool though likes dip so in the case of sodium right let us look at sodium sodium is over here right and basically if you're on the leftmost column of the periodic table you basically have one valence electron so sodium got one valence electron hanging out over here and then on the other side is one from the right side of the periodic table so it has one valence or it's like seven valence electrons all right now neither of these guys have a full outer shell dude like Lauren's missing one so do you have an extra one God dang it but they want to help each other out so so I didn't give it an electron and boom that I can go there chlorine becomes negative sodium becomes positive and now that are attracted to each other come on to the chair well I guess they would look hotter now that they have their full outer shells but that's not the point so this is big be called an ionic bond of course the other type of bond is basically a covalent bond which basically we're like if hydrogen had one of extra electrons and chlorine had one missing electrons they basically share their electrons so that they both are happy and that is what a covalent bond is but we are talking about ions okay so basically if abundant things come together and make ionic bonds with each other they're called an ionic compound right and these guys aren't the easiest to name so we'll just go around and name there really quick so if you have any CL that's basically gonna be you take the cation which is sodium and then you put the anion on the back and you take klore except you end with an ID okay pull it doesn't matter if it's like ba which have two valence electrons and co2 you know that it's a co2 because very much two extra so you only have one of the thoughts so in order to give away all this electrons that have to by the two chlorine atoms so barium chloride you don't even care how many there it doesn't matter the only thing that matters is the actual identity of them except except when they are metal its transition metal so they're in here they don't have a necessary one type of charge that they can have so in this case I'll give you FB co2 Ironton not always too close okay so that is why you have to say iron ii chloride okay don't forget the - oh you're gonna get it roasted alright can also be three so it was fecl3 IV iron three chloride but I don't economize hard evening the name so that's what we all do really gone note but you do have a know the names of polyatomic on okay boo-boo I'm sorry but you do have to know it I'm sorry I can't I can't tell it to you at any other way all right here basically all them but like I unfortunately don't have a good way of remembering them I just smashed it into my head before the nomenclature test on mine so I don't know how to help you here like the only like pattern you could draw here is like yeah your normal chlorate is feel of three - right so that means that your core right is gonna have one less because and I instead of eight and then if you even have less often it's gonna be high coat will come hypo meat less than it / is like like hikers I think it's cut off the hi4 no reason and it has one wrong okay because this is a review and doesn't not a well find out syllabus or any nonsense like that we're gonna talk about electron configurations after talking about valence electrons he's not affordable shift in perspective well ok who cares we're talking about electron configurations now so basically what atoms have or they have orbitals surrounding them right and electrons fall into orbitals but orbitals only have two electrons per orbital okay that's what Pauli exclusion principle says then how the heck do you get a shell with each electron but doesn't make any sense well my friend she'll cut out multiple electrons in there so maybe we gotta know that there's three subdivisions for orbital okay you got your n which is your energy level and this is the one you guys like a call show so definitely if you want eight valence electrons you want to have eight in your X energy level okay then you go up L which is big wheat whether or not it's SPD or X and basically there's different shapes of orbitals like a spherical orbital and it's the lowest energy orbital then you got p orbital which are like dumbbell shape and they are fighting more energetic than da the different orbital the more D orbitals and P orbitals that there's less energetic and so on and so forth if you wanna be fancy this is called the principle of quantum number and second one is called like the absolute look on a not mistaken yes sir the next one is called M the basically am telling you the orientation of the orbital right because the S orbital you have one Sol per energy level right so there's only one possible orientation so at the end for each s orbital is this going to be zero so that's the only possible orientation for it however if you have all equal to one which means the corresponds to P orbitals there are multiple P orbitals in each sub level or higher if your L is equal to one which means that the p orbital there could be multiple P orbitals in each energy level so that's why M could either be 1 0 or negative 1 so like this is corresponds to 0 1 2 3 and then basically M goes from 0 plus or minus 1 dot all the way to plus or minus oh so that's how you remember quickly how many orbitals are in each energy level or sub low so Allen basically your sub level right so if the question is like how many orbitals are in the D sub show you can literally just say and go from 0 to plus or minus 2 so you go from negative 2 to 2 there's five orbitals there and then this is just called a magnetic core and then last but not least you got your spin okay and this could just be plus or minus 1/2 that's the Eevee's one remember because of basically things that there's two electrons per orbital very cool and it's basically why the Pauli exclusion principle good you can't have two of the same s in each orbital so if there's only two possible value for s you only have two lifetime per orbital so if asked on the electron they're in the D orbital we take the number of orbitals is at five and you multiply by 2 and you get 10 orbital ok epic now that we've got down all the quantum numbers we can basically start talking about electron configurations ok all right so the easy way to like find electron configurations and do let me get to look at the periodic table like there's a bunch of random stupid rules for it but like doing from the periodic table that's a fast way to do it but before we get into that let us just explain the different rules because why not so you got tons but basically says if you have this D orbitals over here like either all P orbitals let's say then your electrons will first try to fill up spaces without the to each other could they're like not very good at social stuff like me do they even look like what the heck but anyway the point is they like don't sit next to each other and then if you have to add more electrons then they start sitting next to each other when they absolutely have to so that's the order in which they fill the books mainly they like the people sitting in the bus room then you got outbound but basically tells you the order in which the energy levels are filled and basically you want to fill the lowest energy levels the highest energy levels and basically the actual way to do that is called made Lanka rule that tells you the exact order I'll cause that's lowest to highest energy level and this one tells me which ones are the actual low energy level but you don't really better this one and he became not very useful but anyways alcohol you clearly don't need not to worry about it come periodic table Tony everything okay so let's figure it out so these are the energy levels correspond to rows in the periodic table basically and then as you go from each element to the next guy to add one more electron each time so your first hydrogen is just gonna have one electron and that goes in the lowest energy sublevel which has the lowest quantum numbers career and lmms and that's mainly gonna be zero for all of them and that's just the 1s orbital so you're gonna have one electron in the 1s orbital then helium adds another one but this one could take another or boat or electron in it so we add one of two there we go to lithium but when ice can't hold anymore but now we are also on the second row so we have to add another orbital so our next orbital Lowenthal looks to X and then lithium has one but then when we go to beryllium it becomes two and then you go on to borrow now boron we can't put anything into it ass anymore but we're still on the two level so we can't do it to us again that doesn't make sense so we haven't move up a different quantum number which is busy PR L and now we go from F we go to the next level which is going to be P so we got to pee and then we only have one we've only added one so far then to get to carbon we have another one then a Nigerian 3 and so on and so forth until you get to neon which lump six wait a minute there's only six in the last one how is neon a noble gas and have a full valence electron what the heck so basically you're being shale in all this entire part so no like all them that have the highest number over here today the Sun tip of 6 and Wow has eat doesn't be expected and then you do three s to four so form a medium then to p6 for argon okay and now we do another boy well that's three p6 and then we go to for us too but now we have a pretty different thing that's not the P area well let me just break it down for you okay so we have this part of the s okay we already got that we get there's a P but then one second - what's this boys over here basically these fill the D sub level but the detail level is weird because it reason we shift everything up one because the D level is actually not that energetic so even though this is wrote before we put it into 3d level so scandium we're gonna add another electron from calcium we're gonna add another electron so it's gonna become 3d instead of 43 new one and then if we go to think we have 10 electrons added from calcium so I cook on 3d 10 for then alright so now let me know how to deal with the D block I'll teach you how to deal with F block later but let us first learn noble gas the hidden so I know how to write down the whole silly electron configuration every time okay basically if you want to put calcium you can literally take the earliest noble gas port put it in braces argon and then start the electron configuration from there so after our Monyetta ad to us or for s2 and you get counting all right happy so now let us figure out how to do lanthanum okay that I'm basically going to be what's the first one is a xenon then we have to add in our 6s 2 over here and now we're on the apps law so it gets shifted up 2 so we're at 6 but we shift up to now our four up and it's only one that's big there's some weird stuff with the f-block I wouldn't worry too much about it cuz it's probably not gonna be on the AP exam but yeah it's pretty cool you don't have to worry about the exact workings of the f-block but you can know a little basics all right and lastly the exception okay basically it's just half shells and full shells for the d-block right so if you have like 3d 2 3 4 right d subshell could have 10 electrons and doesn't get a spew back to the ik for electrons and just one off from half a subshell come on man so basically what has for the electrons chromium does right so basically chromium's like I don't like this half so we're gonna snack from F because if I take one firm ass right then I become one in my F orbital and that's hackle that's good and then Mikey over it'll also get tackle so it's a win-win situation so like you might expect chromium to be argon 4s 2 3 D four but know it snatches an S electron it becomes 3e pop and it's similarly for copper it doesn't want to be almost do a full d subshell become a full D sub level that would be amazing so what copper does is it takes instead of being a our 4s 2 3 D 9 take 1 and becomes a 10 wow you don't forget the exceptions that told me so hard on the a protest you have 6 points in my 85 if you can tell so bad all right that was kind of big brain oh alright now that we understand electron configurations basically if we only look at the valence shell and often ask you how many unpaired electrons are there right so let's do the example of sulfur right so you have neon and then you have 3 X 2 and 4 P 3 P 6 ok so your hybrid orbitals 3s over here and that's what's gonna be up down down EMP 3p and it's three of them so basically Oviatt 4 rom : okay so beyond four electrons ok so we've heard that it for as long the next one to the long 6 and that's it next and because the first guy the troll then it goes to the next one and then the fourth guy finally half the next two it's the boom so there are 2 unpaired electrons very cool and basically if a condition I don't have unpaired electron it makes colors ok so that's another cool thing no but what does the mean to have unpaired electron basically there's two types of magnetism um you know whether they're on the AP exam but you might well no it's paramagnetism basically unpaired and just like it's a pair all right so it's like almost with something like parallel it's basically going to go attracted into magnetic field and then diamagnetism means pair all the electrons are paired and then repelled magnetic field we're almost done guys Ron's done he's got to talk about photoelectron spectroscopy and we gotta talk about periodic trends which shouldn't take too long alright so photo electron spectroscopy so you shine a light on an atom right in excite two electrons and eventually if you excite the electron another look it yanked off dad however if it was really hard to excite the atoms that I'm gonna move a lot slower because you had a little less extra energy to make it to our movies you had to spend all the energy on getting it out of the atom not actually making it move so basically what photon electron spectroscopy does is or photoelectron spectroscopy if the basically shines a bunch of photons on an electron it snatches all electrons off the atoms and basically the ones that are eating this natural are moving super fast and the ones that are harder to take off and move super slow and then ultimately you could have a graph of how many of each energy or how many of these speeds were hitting the actual print so let's find a photoelectron spectroscopy data somewhere all right so this is a pretty good example know why some small rill there we go so basically you can notice that the like potential energy is decreasing as you go here so the one with the highest potential energy over here and basically like you can think of it as the one they're closest to the atom or how the most highly right so they're it's so hard to pull them out so they have the highest potential energy so the ones close it to the atom electrons that are closer to the atom are here and the ones that are farther here and we also know that things within the same orbital have the same energy and things within the same sub shell like SRP although the same energy so this one the closest to the atom so obviously they're just going to be your first sub show so one app so this one on the netbook is there going to be to us then you got your 2p then you got your 3x and you can tell like the height is the number of electrons but sometimes they don't give you this but you can tell the relative height is the number of electron so this is going to be 2 s 1 s 2 then the 2 O 2 then 2p 6 and this is 3 s 2 so that's how you find your electron configuration from photoelectron spectroscopy there really not much else to photoelectron spectroscopy except knowing how it works but yeah this is all right carry on trans let's do it all right let us go quickly what they're called alkali metal ER on the left they make one plus ions only have one valence electron you got a called alkaline earth smell if you can see over here and basically they lose two electrons to become two plus then you got your transition metals over here which have after we've used their electrons so I have no idea they could be 2 plus 2 4 plus 3 plus I don't know then you got all your nonmetals over here this over here it's called metalloids you've got a technically metals but they're called post transition metals then you got your nonmetals and you got your noble gases cuz they don't react with anything it should be reviewed ok now we're going to talk about trends so first thing first atomic radio this thing was like pretty confusing to me because I like if you add electrons why is it not getting bigger cuz it doesn't get here lithium is the biggest one in this row over here what the heck well the reason is as you're adding electrons they're all in the same energy stumbo right like if you're adding electron they're all in the second level the whole in a second show so they're not really getting farther away they're just like hanging out in that same show however you are adding more protons and if you have more positive charge in the nucleus they're gonna attract the electrons more so just pull them in like spider-man and boom they get closer which is why how'd you go from lobster right you're getting more protons so it's bringing in the charges closer so you got smaller atomic reading power as you go down you do get another pull electron shell and like the electrons inside that are shielding it so like basically the valence electron of sodium right this is hanging out there and then all the other shells are on the inside so all the other shells are gonna block the charge of the nucleus from affecting this hey guys it hanging out here so it's actually the nuclear charge gets canceled out by the all the other electrons and basically the blowing one positive charge left it gets to the final charge so essentially the effective nuclear charge is called is exactly the same however that one charge out here and on a whole another energy level so it's farther from the nucleus so it has a bigger atomic grease so basically if you go down an increasing radius and you go right at deeper than radius and okay the best way to memorize trends is just to memorize the one has the most extreme on them okay so which one had the biggest atomic radius its francium so then if you didn't remember it you literally like as it gets farther from fancier it gets smaller and radius and they get closer to France you look I'm figuring Ruiz that's how I like to think of it if you just memorize the corners at which things increased and you know how to remember like separate four rows and column you just get close to it Francie but another thing you got to consider ions right so let's say you have Li and Li one which one is bigger well Li Li one plus one the same number of protons right so they both have the same attractive board however if you take out electron like it's for sure going to get smaller right because you're just taking out electrons but the attractive force do sing so you have what stuff that hanging out on the outside and then of course like there's no electron-electron repulsions that are putting them outward right if you take out one electrons at the rest of them or not pushed out by that electron so essentially if you take out electrons but remain the same amount of protons you actually decrease your atomic radius so li looks like this here Li one plus actually looks like this so it's actually a lot smaller than this so essentially whenever you're dealing with the more electron the word like the more like on the bigger let's like on the smaller that's all you gotta remember alright ionization energy basically it's like how easy it is to remove the first valence electron so it's really easy for lithium sodium whatever these guys because they want to lose that electron these guys kind of don't want to lose it but they're they're okay with it right because then they get an apple 1s orbital that'd be kind of epic so these guys have the next highest now these guys are kind of sketched you don't really have to worry about them but these guys have higher because they're not getting anything special by losing an electron it's kind of late for them to do that electron so basically fluorine has some highest ionization energy first ionization energy because it does not want to lose an electron wants a gain in electron but then have you go down the thing like the final electron is farther and farther away from the nucleus right so it becomes even easier to take it away so once again francium have the lowest ionization take the least amount of energy you could get rid of that one electron and then everything does be pizzas that way second eyes the night vision energy you may be shifted over on because basically lithium got the same as although no gases brilliant up click on the lithium when you take off an electron well not exactly a no Billy they become similar in electron configuration so essentially your highest second ionization energy that's going to be radium and then we got electron affinity which is basically the energy release when you take in an electron and for this one I just really don't like thinking about it too much but basically chlorine releases the most amount of energy when you take in an electron because it just really wants to do it so it just takes it in and boom it's happy and releases so much energy so chlorine is the most I don't know why it's not boring it has something to do with like it being at the right distance from the nucleus of some stuff on a glass here but chlorine doesn't know it's Corinne of the most electron affinity and as you get farther permanent if decrease electronegativity basically how much is snatches electrons from other guys in a covalent bond so fluorine in this case and the most because it wants out electrons so badly it has a very small atomic radius so it's like closer to the electron so it's gonna snatch it very much and then in DP so that you get away from floor and then just know how electronegativity affects bonds right so if you have one really electronegative element with a less electronegative element it's going to be cooler Camille if it's really really big that difference then it's gonna be ionic but one just kind of completes natural electrons if they're approximately equal there's going to be a normal covalent bond epoch and last but not least metallicity basically the ones that like this have to get closer to francium because francium is like very willing to give up its electrons so francium has a - metallicity and i've to get away from it deep pieces in metallicity that one's like the most boring boring but it exists so there you go alrighty thank you guys for watching if you guys ever need suggestions please let me know because this is new for me I think it's working I know you guys tell me a lot of you guys wanted a view cam but if there's a specific way in which you wanted to cover please let me know please please I beg but anyways as always thank you guys for watching if you enjoyed the video leave a like and subscribe for more things I'm for watching again see you god next time