stream that sort of good stuff and then finally um go ahead and get out a periodic table preferably maybe not the one you got in ap chemistry because the ap chemistry formula or periodic table does not have element names so if you aren't comfortable with element names yet you should probably use a an alternative periodic table one that you can find online like using google images or some other online resource and then you'll also need a pencil and a periodic table because we are going to be doing practice problems along the way so um yeah and because there's gonna be a little bit of downtime while we're doing practice problems i have a list of really good chemistry jokes that i'm gonna say while we do those so let's go ahead and get started with part one which is ionic compounds so first we'll go ahead and define what an ionic compound is so an ionic compound is a compound made of believe it or not ions that are held together by electrostatic attraction and electrostatic forces are just uh describing the forces felt between different charges or felt between charges right so electrostatic attraction then is the attraction felt between a positive charge and a negative charge and the way that elements get these charges is through the transfer of electrons so let's look at the example of lithium chloride so you'll notice on your periodic table that lithium is in group one which means it has one valence electron and ultimately if the goal is to form a stable contour compound lithium needs to lose that electron to you know have the full octet and chlorine on the other hand is on the opposite side of the spectrum chlorine has seven valence electrons it needs another one to have a fold out or a filled outer shell which means this is a pretty good situation because then lithium can then transfer its uh valence electron to the chlorine and everybody's happy in doing this these atoms then gain charges they become ions and when lithium loses an electron that means it becomes less negative and it has a positive charge meanwhile on the other hand chlorine gains an electron so you know it has a negative charge and together these ions form a crystal lattice structure as shown below which is uh really you know structured which gives it some properties like having a high melting point because i ion ionic bonds are pretty difficult to break same with being hard and being brittle so with that being said let's move on to basic nomenclature rules for ionic compounds so for the cation and there are several ways to memorize what the cation is this is the ion that loses electrons and ends up gaining a positive charge and some mnemonics that you can use to remember what this is is plussy cat because of the cat and cat ion or you could think the t in cat looks like the positive sign or you could think you know positive charge as in cat pause anyways for the cation you just keep its name you don't do anything to the name of the element so look back to the example of lithium chloride again lithium is just lithium nothing happens to it and then for the anion then uh you add the eyed suffix you just cut off the end of the element name and add i'd instead so if you look at lithium chloride again instead of chlorine you take off the en part and add ide so the anion is the is the ion that gains electrons and has a negative charge and there aren't really great mnemonics to remember what this is you can think that the n in anion in the and part stands for negative so like a negative ion or you could just think well the anion has to be whatever the cation isn't so um go ahead and give me on a scale of like one to five in the chat one being i have no idea what's going on five being yeah i'm pretty good with this concept um you know how you're feeling about basic nomenclature rules if we could go ahead and do that um that's a good idea melanie you can think anion is kind of like onion if you don't like onions that can be negative all right so it looks like everyone's pretty good with this we're all pretty solid so we'll move on to some examples so um i'll go through the first example whenever we do practice problems and then i'll leave you to the next couple so for the first one sodium chloride so we know that n a is sodium and so you don't do anything to the element name you just keep it how it is and you don't always have to go through the process of thinking oh which one's the cation because the cation will always come first in the formula so if you just think oh na has to be the cation because it shows up first you can think of it that way instead and then chloride like in lithium chloride you cut off the ene in chlorine and add the eyed suffix so with that being said um go ahead and try the next one al2sc3 and type out the answer to that and while you're doing that i have a chemistry joke okay what do we do to chemists when they die we bury them um someone threw sodium chloride at me i yelled that's assault um okay so yeah those are the ions that are formed what we're asking is uh like what is the actual name of the compound so um yeah so melanie would be right here it's aluminum selenide and uh matthew you did get the ions right but we're looking for like the actual name of the compound so uh like before aluminum just keeps its name because that's the name of the element and then selenide you cut off the iam in selenium and you add the id suffix so it's aluminum selenide so the next one i want you guys to try is cabr4 while you're doing that i have another chemistry joke um did you hear the joke about cobalt radon and etrium it was corny um if h2o is water and h2o2 is hydrogen peroxide what is h2o4 drinking all right so yeah calcium bromide is the answer to the next one so yeah calcium don't do anything to the name of the element and then instead of bromine you have bromide and then finally the last one bai2 could you guys try that one and then i've got another chemistry joke in the meantime what should you do if no one laughs at your chemistry jokes keep telling them until you get a reaction um yeah riley barium iodide is right so barium just keeps its name and then iodide iodine you cut off the iron part and add the i'd suffix instead and then um matthew what i would suggest doing is get out like a periodic table if you aren't so comfortable with uh maybe the the like symbol for an element and its actual name and associating those so uh yeah so the reason why it's not like aluminum and boron is because it aluminum would have to have the capital letter right for the a to symbolize that it's another element so with these practice problems can you guys give me on a scale of one to five again how we're doing one being don't know what's going on five being yeah i know what's going on and then that helps me gauge where we're at and if you have like three or lower then please ask a question um yeah so it seems like all of us are in the four and five area so i'll move on to the next slide which is using the periodic table and charges so this is going to be the introduction to the other naming rules when it comes to ionic compounds because unfortunately there are some other things that you need to know about so when it comes to the left side of the periodic table in group 1 so that's your hydro hydrogen lithium sodium those those will usually have a plus one charge and the reason why i say usually is because hydrogen is a little bit different in that it can not only form a plus one charge um but it can also act as the anion like for example in lithium hydride and have a negative one charge and we don't have to go into all the details of why that happens right now especially because we haven't gone over like periodic trends yet um but other than that thus in the second group all of these will have a plus two charge when they form ions because they have two valence electrons you know so they uh want to lose two those two electrons so you have a philo octet and to become stable then when we get to the transition metals so scandium all the way over to zinc um these will are will act a little bit differently because they can form different ions based on the compound that they are in except for a certain few and that's what i have highlighted in the special cases part right above so uh silver for example will always have a plus one charge and then likewise zinc and cadmium will have a plus two charge and uh you should know about those because of something we'll get into a little bit later and then once you get to the right of the transition metals uh in that group with boron aluminum and those other elements uh the reason why i have plus three there even though not all of these will have a plus three charge when they form uh ions it's actually only a aluminum when it comes to elements like for example gallium or indium these ones will behave sort of like transition metals do where they can have different charges based on the compound that they are in aluminum is the only one i believe in this row or in this group that will actually form the plus three charge and then the reason why boron doesn't is because it is a metalloid it's more likely to form a covalent compound then in the group right next to that with carbon silicon germanium the reason why i don't have anything here is because either a they're non-metals or metalloids and are going to form probably a covalent compound instead or they're elements like tin or lead and these ones will also behave like transition metals do where they will have a different charge depending on the compound that they're in and we'll get into how to notate that a little bit later now to the right of that we start entering the nonmetals that will form ionic compounds and that would be your nitrogen and your phosphorus so these will have a minus three charge because they need to gain three electrons in order to have that full octet in order to gain that stability and then right next to that we have uh another group with a minus two charge which will include your oxygen sulfur selenium and then you have your halogens which will form a minus one charge and then over all the way on the right you'll have noble gases which are already stable so they're not going to they're probably not going to form ionic compounds okay so um so melanie arch okay are they everything else besides the halogens noble gases and metalloids um that's a good question i think that they're everything else besides the halogens noble gases and metalloids but i will probably search that up a little bit later when we get to the discussion period so yeah is it group 14 charge of negative four okay so group 14 is a little bit different because um so carbon silicon and germanium aren't going to form ionic compounds for the most part because it's very like difficult to do so they're probably going to form covalent compounds and then so the non-metals or the metalloids in that group aren't going to form ionic compounds um okay should you remember all of the charges for common elements uh you don't need to what i would do instead is memorize the names of common elements because then you can just use your periodic table on the test to you know figure out what the charges are that being said you do have to remember the charges for those special transition metals um like silver zinc and cadmium because those ones you just kind of have to know uh otherwise yeah you don't have to remember all the charges for the common elements that being said you probably ultimately will end up doing so because you're going to work with elements like hydrogen like lithium a lot throughout the year okay so with that being said let's go to the next part which is what we do those transition metals and those other metals that have you know multiple charges depending on the ion that are formed so that is formed so this is where we get roman numeral rules so depending on the uh ion produced these elements can have different charges so then we have to figure out how do we notate that so we determine the charge first of the actual metal and then add it after the name of the cation which you will write in roman numerals between parentheses that's kind of a lot of information to take in so i'll go through the first example again of cui 2. so this is copper 2 iodide and the reason why we know that is because by the way remember that copper is not co that is cobalt copper is cu and the reason why we know this is because of basically the anion so the charge on one iodine um ion would be negative one right so if we have two of that iodine atom it would be a total charge of negative two so because an ionic compound is going to be a neutral compound what we do with the copper then is it has to balance out that negative two charge right so it's going to have a charge of positive two which is how we get copper two iodide so is everyone good with that example scale of one to five again how are we feeling okay so it looks like we all have fives and we're doing good so let's try the next example i'll leave you guys to fecl3 in the meantime i've got another chemistry joke um what is a chemist's favorite type of dog a laboratory retriever um okay so yeah matthew you're pretty close iron iii chloride is right that is the charge on the iron that being said remember you do have to write it in roman numerals between the parentheses so yeah vanessa has it so iron three in parentheses and then chloride so yeah and then melanie we use the same naming rules as before so where we do iron the name of the element or the name of the cation and then chloride so you cut off the en and add the i'd suffix all we're doing now is just adding the charge in parentheses in roman numerals after the cation so like how vanessa has it iron iii chloride so with that being said i'll let you guys try the next one which is a little bit harder v2o5 in the meantime i have a really good chemistry joke um so we all know about the ideal gas law right pv equals nrt pivner if you don't um it just relates a bunch of properties of gases together um but what you might not know is this thing uh called cole's law but this one is actually usually served as a side um why did the bear dissolve in water because it was a polar bear um what happens to nitrogen when there's sunlight it becomes datrogen so how are you feeling about the last example v2o5 this one's a little bit more difficult um just remember to go through the same process find basically the total charge of the anion which in this case is the oxygen and then find out how many how uh the what the charge is on the vanadium based on that and because there are two vanadiums you'll have to like basically divide the total charge of the anion into two because there's two elements or two atoms of that element to find the charge on that um it looks like we'll need a little bit more time so i have more chemistry jokes don't worry did you hear about the date between oxygen and potassium it went okay okay yeah so vanessa has it again it's vanadium 5 oxide and this one is a little bit harder because you have to do an extra step where you find the total charge of the anion which would be 10 because the uh the charge of one oxygen ion would be negative two right and then negative two times five is negative ten so to balance that out we need a charge of positive 10 on the vanadium which because there are two atoms of that element you'd have to divide by two so then we have a charge of plus five on both of the vanadiums so you get vanadium five oxide so is everyone what's good with that example could you give me on a scale of one to five again how we're feeling okay looks like we're all at five again so we'll move on to the next subject which is polyatomic ions so i don't know how other classes do it but for me i did have to memorize a lot of the common polyatomic ions and by the way this is not a comprehensive list there are plenty more polyatomic ions these are just things that i thought were uh pretty common that you'll see a lot and when it comes to polyatomic ions so first of all what are they they are basically covalently bonded elements that form a single unit that act as the anion in an ionic compound um so when it comes to naming compounds with polyatomic ions then you don't do the thing where you cut off the end and then add the eyed suffix rather you just keep the polyatomic ion how it is so for example in sodium nitrate you just call it sodium nitrate you don't do anything to the name of the polyatomic ion and then when it comes to actually memorizing these uh you there's not really very many rules that you can go by there are a couple that will cover but when it comes to polyatomic ions like ammonium or carbonate you just kind of have to know what these are and you do have to memorize the charges too um so with that being said i'll go to the next slide which is some naming patterns that you can find within these polyatomic ions so one of them is the ite thing so you'll notice that there was nitrite nitrate sulfite sulfite sulfate phosphite phosphate and uh yeah it does help you to memorize it according to a periodic table and so you'll notice that it is always one less oxygen than eight and the eighth suffix is given to the polyatomic ion that is most common you're probably not going to know that off the top of your head you're probably just gonna have to memorize that one uh but to find the other one the sulfite or the nitrite or the phosphite all you do is bring the oxygen down by one and then that's the formula for your new polyatomic ion with the ite suffix and the charge always stays the same between those two variations and then for halogens there is something different that you that might help you memorize these so when it comes to like chlorine bromine iodine there is a naming rule that goes a little bit past just the item eights and when you have one oxygen or one less oxygen than chlorite you have to add the hypo prefix so you get hypochlorite and then for uh when you have four oxygens or one more oxygen then the eight suffix you have to add the per prefix and you get perchlorate and this happens with other halogens too for example if you had bromine you would have hypobromite for one oxygen bromite for two bromate for three and then per bromate for four oxygens so that's kind of a lot of information to know uh we are going to use these polyatomic ions for some of the practice problems so if it helps i would click on the slides button down below to see the slides in case you need to go back and look at these naming rules are to look at the list of polyatomic ions and then otherwise how are we feeling with polyatomic ions on a scale of one to five again okay we got one five two five okay fives again so that being said we'll move on to some practice problems uh this time we're going to be talking about writing formulas so we aren't going to do any practice problems with just the polyatomic ions because you just use the name of it there's nothing really different and then i will learn how to actually write formulas for compounds when you're given the name so um okay is i'd always the least charged so i does the suffix that is given to when there's only like one element so this doesn't include polyatomic ions polyatomic ions won't have an eyed suffix uh that's given to like when a an ionic bom or an ionic compound has an anion that's only one element so like lithium chloride sodium chloride aluminum selenide all of those examples from before um if you're talking about it however it will have the least charge in some cases but um well yeah i will have the least charge now that i think about it but sometimes you will have to add that prefix in the case of halogens if that answers your question so uh with that being said we'll go through these like before so like when we had to name those transition metal compounds with the roman numerals you also have to do something similar here where you have to find out the charges of the or of the elements that would be able to balance each other out right so let's look at the first example of the aluminum sulfide so aluminum if you remember has a charge of plus three when it forms an ion sulfur on the other hand has a charge of minus two that's not going to work out to form a neutral compound so what we have to do instead is find the least common multiple between these charges so that would be six right because it's two and three so then you ask yourself how many aluminums do i need to have a total charge on the cations of plus six and the answer is two because if it has a charge of plus three then three times two is six and then you do the same thing with the sulfur where uh sulfur has a charge of minus two to get to a total charge of minus six on the sulfurs you need three of them right so then those become your subscripts for the formula you get al2s3 so is everybody good with that example one to five again okay looks like we're doing great so with that being said go ahead and try the lithium iodide and writing the formula for that compound yeah so that was pretty quick i didn't even have time to read a chemistry joke it's just li i because uh this one's a little simpler you don't have to do any of the least common multiple stuff because lithium just has a charge of plus one iodine would have a charge of minus one when they form ion so that just works out um now for the next one this includes the roman numeral rules now uh try out cobalt ii chloride uh yeah so melanie and sarah have it and then matthew you got a little mixed up there with the c-u-n-c-o remember that cu is copper and cobalt is co that's a little bit tricky to get straight and that's something that you should know by the time of the ap test because you won't get element names on your periodic table okay and then the final one calcium calcium hypo iodide this is one where you're going to have to know those halogen naming rules with the polyatomic ions so if you don't remember exactly what those are uh maybe pull up the slides again and then uh oh one thing that you might need to know is that iodide or any forms of iodine will always have a charge of minus one that's probably helpful so with that being said try out this example and then i have some more chemistry jokes where do you put dirty dishes in the zinc um did you hear about the man who got cooled to absolute zero he's okay now okay so matthew the reason why it's not cai2 is because hypoidite would be the name of a polyatomic ion so if you remember uh so yeah sarah has it and uh if you remember from before iodide would have or sorry chlorite had the clo2 formula and then hypochlorite had the clo formula where there was just one oxygen so that happens with other halogens too like iodide hypoiodi and hypobromite would be similar like hypo iodide is just io with a negative one charge and then hypobromite is bro with a negative one charge and then melanie very close you just need the parentheses to indicate that the io is like a group of things and so that would have the two subscript and not just the oxygen so are we all good with those examples can you give me on a scale of one to five again how we're feeling um so uh if you mean like the subscript on the oxygens melanie then yeah or no then the subscript for one oxygen is uh hypo eight and then two oxygens is just ite and but you're if you're look asking about the charge the charge is always the same for any variation of those like halogen polyatomic ions so it's always just negative one so seems like we're all good with that so we'll move on to part two which is molecular compounds and acids so first we'll go ahead and define what a molecular compound is so a molecular compound is made up of covalent bonds which uh as opposed to ionic bonds involves the sharing of electrons instead of transferring transferring right so we don't form any ions and molecular compounds and then covalent bonds are usually between two nonmetals or they can be between metalloids so with that being said let's go to the nomenclature rule so these ones i think are a little bit easier than ionic compound naming because there aren't so many different ways to name them so the first thing you do is ask yourself what is the subscript on the elements right and then that is the number of atoms of an element so then you have to add a prefix so let's look at the example of i don't know n3o8 i just made that up so if there are three nitrogens you add the tri suffix using the little table on the left so you'd have tri nitrogen and because there are eight oxygens you'd have the octa suffix so it would become trinitrogen octoxide and then like before with the ionic compound naming rules you add the i'd suffix to the end of the second element so instead of oxygen it became oxide and then if there's only one element of the first atom you don't need the mono prefix it's just kind of implied that there's only one of that element when uh you don't have the mono prefix so for example in co that would just be carbon monoxide you don't need to say monocarbon monoxide and then the last little stipulation is that if the element starts with and the prefix ends with a or o you will usually drop the last vowel of the prefix and what this means is that for example in oxygen if you had oct or eight oxygens in a compound like before you don't say octa oxide you'd just say octoxide or like when we said carbon monoxide it's carbon monoxide not carbon mono oxide uh so that's the last thing you need to know about naming molecular compounds do we all feel good with that give me a scale of one to five again how we're feeling okay looks like we're all doing great so now we'll move on to some examples so again i'll go through the first one which is a compound you've probably seen before carbon dioxide so uh the first element there's only one carbon so you don't need the mono prefix on the first element so it's just carbon and then you add the id suffix to the second element so you'd get oxide and then because there's two of that element you'd add the dye prefix so it would become dioxide carbon dioxide so with that being said i'll let you guys try the next example of the n2o5 and go ahead and see what that one's named yeah so that's pretty fast dinitrogen pentoxide would be right oops there we go and then we can try the next one too which is sf6 and go ahead and try to name that compound um yeah so chi is right sulfur hexa fluoride and then it's not hex oxide because i think it just got a little mixed up it's sf6 um and then so6 would be sulfur hex oxide and then let's try the final example with p4s7 and try to name that compound um i don't know if i have many chemistry jokes left oh why did the hipster chemist get burned he touched the beaker before it was cool okay um so matthew you're pretty close tetra potassium is right just remember that you or no that's not right wow i got a little mixed up so potassium is k uh phosphorus would be p so remember that potassium for some reason the kemp the the symbol for it is k and then p would stand for phosphorus so yeah tetraphosphorus would be right sorry and then um it is hepta sulfide if we remember the um prefixes and if you need to pull up those prefixes uh that would be helpful too and then the reason why it's not sept sulfide honestly i have no idea it's hepta not septa uh when it comes to naming molecular compounds so you just need to memorize all these pre all these prefixes to get that straight in your head so it would be tetraphosphorus hepta sulfide okay so how are you feeling with naming molecular compounds are we good one to five okay and then if you put anything lower than five uh feel free to ask a question if you need to um otherwise like the advice i would say is to just make sure you get the common elements element names straight in your head because you won't have those on the test unfortunately and uh that's usually just the top of the periodic table and more so the metals and the nonmetals more than the transition metals and just knowing what those are names so like sodium is n a potassium is k that sort of stuff and yeah so now we'll go on to acids so we're going to briefly define what acids are and in ap chemistry even though there are different definitions of acids for example in your introductory chemistry class you might have learned about lewis acids we don't care about those here instead the definition that we're going to use in ap chemistry is the bronsted-lowry definition and this is also the definition that is uh that the college board course and exam description tells you you're going to use right so a bronsted-lowry acid is a species that can donate a proton or h plus so this is usually going to be one of the or this is going to be one of the reactants right because it has to do donate the proton to the um other compound in the reaction so which molecule is the bronsted-lowry acid one two three or four and i just said it was one of the reactants so you can probably eliminate three and four already so yeah so one is correct uh because if you'll notice on the product side you have a chlorine uh ion which means that the hcl must have lost and donated its hydrogen proton to the water so are we all good with what a bronsted-lowry acid is if we're not that's fine too because acids and bases is its own entire unit so we just need to know like basically here's what an acid is by the bronsted-lowry definition okay so now we'll go on to the nomenclature rules and when we go to the practice problems it would probably be very helpful to have this slide up because there are kind of a lot of rules to know when it comes to acid naming and this is probably going to be the new material for people who have taken an introductory chemistry class so acids are named by their anion and the reason why is because the cation is going to be hydrogen so there's not really a point in using that so uh for an element with the i'd suffix so that means when there's only one element right it will change to an ick suffix instead and it will have the prefix hydro so for so for an example hcl is hydrochloric acid and then for a polyatomic with the eight suffix that will change to ick likewise but that's all that happened so for hno3 where no3 is nitrate you will have nitric acid and then finally for a polyatomic with the ite suffix this will change to us so for sulfite for example which is so3 and in the compound h2so3 that acid would be called sulfurous acid is everyone good with those ideas i know i went a little bit fast so on a scale of one to five again how are we feeling okay so we got a five and another five so it looks like we're doing pretty good and then if you need to have the slide up when we're doing practice problems uh just click on the button for the slides again and then yeah so we'll move on to the practice problems and i'll go with through the first one again so hf is hydrofluoric acid so remember that when the uh anion ends with the i'd suffix usually so when it's just a single element you add the ick suffix instead and you add hydro to the beginning of the word so it would become hydrofluoric acid so let's go ahead and try the next one h3po4 and it might be helpful also to have the list of polyatomic ions up too in case you forgot what po4 is and then i'm using the naming rules we just uh went over try naming this acid i'll try to see if i have any oh just kidding i guess we went fast enough that i couldn't even tell a chemistry joke so phosphoric acid is correct because it is phosphate and then eight corresponds with the ick suffix so yeah phosphoric acid so now let's try the next one which is hclo and remember that cielo is one of those polyatomic ions with a halogen that has um those special naming rules so remember what is clo and if you need to go back to that slide feel free to do that too and then go ahead and try to name this acid okay um have i already said the we barium joke what do we do to chemists when they die we bury them um if you're struggling in ap chemistry just keep your eye on the prize helium walks into a bar the bartender says we don't serve noble gases here he does not react okay so the reason why we don't have uh the hydro prefix is because it's not a single element right it doesn't have the eyed suffix it has the ite suffix however which would correspond to the us suffix when it comes to naming the acid so instead of hydra we don't need the hydro part hypochlorite is the name of the anion though is the name of the polyatomic ion we just have to uh like transfer that into naming the acid so that would be hypochlorous acid so remember that the ice suffix corresponds with is and i haven't thought of a very good mnemonic the way i remembered it in ap chemistry is oh if it ends with ick it can't or if it ends with ite it can't have the ick suffix because they both start with i not a great naming like mnemonic but that's what i used um so it would be hypochlorous acid how do you feel about that example that one was a little bit more difficult so on a scale of one to five do we understand that one okay we got a couple of fives so yeah looks like we're pretty good and then let's try the last example hbro4 and this is another one of those where you're going to need to know that halogen polyatomic ion naming rule like what is bro4 to be able to name the acid um i think i'm almost out of chemistry jokes oh two electrons were arguing they were sick of each other's negativity um what do you call a clown who is in jail a silly con okay so bromic acid would be if the polyatomic ion was bromate bromate however is bro3 so you'll just have to remember what is bro4 then if bromate is bro3 you're just missing a little prefix that you need to name this acid okay a neutron walks into a bar and asks how much for a drink the bartender replies for you no charge did i already say that one i don't remember anyways so yeah you do need the per prefix when it comes to naming this acid so it would just be per bromic acid you just had to know oh those uh halogen polyatomic ion naming rules so bromic would be if it were hbro3 when it's hbr04 you need the per prefix to make it per bromate and then that becomes per bromic acid so how are we feeling about all of those acid naming rules on a scale of one to five again okay so a little bit more iffy on this one but the good news is that this is all the information we're gonna cover so the next part is a discussion period if you don't feel comfortable with anything feel free to ask a question and uh you can also ask questions about the class or the exam that a student would be able to answer if you're wondering about that or ask questions about the material we just covered so melanie asked um hypo goes along with is right so yeah that would be right because i goes along with this so hypo would also have the ite suffix which means it would also go along with this so do we have any questions about what we just covered are we feeling or are we feeling good okay so we got one person who's feeling good um okay so it looks like we're doing pretty good with all the material that we just covered the main thing is just to like practice these rules so you're more comfortable with them and memorizing you know what are the prefixes for molecular compounds what uh like how do i name compounds with transition metals and you know just go doing more practice problems maybe because it's honestly just gonna come down to how you're able to apply these rules i don't think the rules are very hard to like use but just memorizing them i think is the more difficult part um so melanie asked do i have any study tips um the way i studied for ap chemistry was not the greatest i would say you should probably be studying throughout the year most of my studying came at the end of the year so what i did was i took um a practice exam like a full-length practice exam multiple choice and free response and i gauged based on my score and where i was struggling you know what i needed to work on because obviously if i didn't get like several questions right about maybe titrations maybe i should have studied titration so that's what i did i just tried to find my problem areas and study those instead of you know studying everything in chronological order because uh i think that would be a little bit better because if you already know something there's not really a point in spending a lot of time studying it like you should be spending most of your time studying concepts you struggle with um that being said i would also suggest studying like throughout the year to make sure that you know every concept that you're coming across um so you don't have to like cram everything at the end sort of like how i did but um this study method did work out pretty well for me so yeah that's what i would suggest okay so when naming nomenclature do you have to note functional groups okay so that's more of an organic chemistry thing you do not need to know about functional groups for the purpose of ap chemistry so you don't need to know about those suffixes so if that is all the questions we have then it looks like we're doing pretty well on these naming rules so thank you for coming to the stream and goodbye and good night