Lecture 08. Naming Compounds
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Chemical compoundChemistryChemistryChemical experimentLecture/Conference
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ChemistryChemical compoundInflammationChemical elementChemical compoundChemical elementPeriodateElementanalyseBoronThermoformingBranntweinPaste (rheology)Chemical experimentLecture/ConferenceComputer animation
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Alpha particleLecture/Conference
Transcript: English(auto-generated)
00:09
All right, dearest friends, welcome back. Chemistry lecture 8 is going pretty fast. Here it is. I'll say a few words about that on Wednesday, but there's already
00:27
a midterm kind of flavor coming along. So we will just get it in the right movement for that shortly. For now, we don't have to worry about it, but just to let you know, things are moving along. Today we're going to talk about
00:43
the naming of compounds. So we already talked about what compounds are, and now we have to know how to give them a proper name and how to recognize them. So let me turn back to
01:02
these notations. This is from the periodic table, right? and these are the elements. Elements in its single form is an atom. And this is boron. And boron actually, if you remember this from the previous lecture, is an element that is not present at very high
01:25
quantities on our planet. It's one of those elements that has a pretty big dip in the abundance graph that I showed. But I just bring up this issue for two reasons. The first reason is that boron, among its very first lectures, and I think it was the first lecture,
01:43
I was here at UCI doing things like this. I was trying to make a joke about boron, and boron, I thought was a funny word, I thought it was a very combination between somebody who is very boring and boron. So I was joking about that a little bit, and I had a
02:05
good time. Most of the people allowed it. After class, there was a person coming to my periodic table and he said, look, I didn't really like that joke at all. Because I happened to like boron, it's a great element, and I spent my entire summer working in a boron factory.
02:25
I did not believe him, but I looked up and he's right. He said, I work close by, he said, I work close by, in a boron factory. There is a boron factory, well, not a boron factory, it's more like a mine, if you want, boron. Okay? So this is Rio Tinto, it is north of Los Angeles, it's one of the locations of the boron factory, it's one of the most important places to work.
02:43
It depends on our planet where there's a very high concentration of boron in the soil, and people here have a set-up camp and are digging out that soil and filtering out boron. Here it is. A big chunk of boron, it looks a little metal-esque. Boron is an element, and as you can see,
03:03
it's a metalloid. So it has both metallically and metallically. So, for those of you interested in stories about borons, this is a nice book to read. So if you're interested in how elements got their names or peculiar properties of elements, this is actually excellent reading. It's really a lot of fun.
03:29
Here's boron once again, this is basically when you take a big clump of boron and you grind it up, it looks like this, like little metallic-looking petals. And again, that's elemental boron. But elemental boron is not a compound. It's an elemental boron.
03:47
It's not a compound made out of different kinds of elements. If I take this boron element and put it into something else, for instance, barium borate. You see here is boron. That is the element boron that sits in this particular compound.
04:04
This is an element, an elemental compound, this is not an elemental compound. This is a compound composed of multiple elements. This is very boring. It's a glassy type of material. It's transparent. And just to let you
04:20
know that these materials have nothing in common except for the fact that they contain boron elements. So this is not transparent whatsoever, this is. So completely different material properties if you put these atoms in different places and you give them different neighbors. I find it a fascinating aspect of matter.
04:43
You take the same elements and put them in slightly different surroundings, and you get something completely different. All right. So what kind of name do these compounds have? So barium borate, that's the word, that's the name for that compound. So how do we assign certain names to certain compounds?
05:05
Is there a set of rules? And the answer is yes. For the simplest compounds, there is a set of rules. And today we're going to talk about that. Okay. So let's talk with let's talk first about binary ions.
05:21
Binary ions that is a compound that contains two ions. Cation and anion. So the compound is a binary ionic compound. Sodium chloride is a binary ionic compound because it contains two ions, cation and anion.
05:43
Here they are. Sodium plus fluorine minus. The name is sodium chloride. Another example, cesium bromide also is a binary ionic compound. It contains two ions, a cation, cesium, and bromine minus, that's the anion. Its name is cesium bromide.
06:03
So you see already it's systematic here of the naming of these things. If you want to name binary ions, you have to look at the kind of metal that forms the cation. If the cation is a type one metal, then
06:23
this kind of naming is appropriate. But if the type sorry, if the metal is a type two metal, then we have to make sure that we give this name an additional bromide. So we have to make a distinction between type one
06:41
metals and type two metals in terms of the naming of compounds that follow from these cations. So let's first start with binary ionic compounds that contain a type one metal. Okay. So what is the set of rules? Everybody can do this because it's a set of rules, and if you follow it, you arrive at the right answer.
07:05
So if you want to name a compound like that, you name the cation first and the anion second. Remember, sodium chloride, sodium is the first element, you say sodium first, and then chloride, chloride is the chlorine anion. That one is second.
07:24
The monoatomic cation takes the name of the element. All right? Sodium chloride contains sodium. So that monoatomic cation is just called sodium. Sodium chloride. The monoatomic anion
07:40
takes the root name of the element plus the suffix "-i." Sodium chloride. The element is chlorine, but if you make a compound, you call it sodium chloride. That's the name of the anion. Okay, so here's a couple of other examples. This is a binary ionic compound. It contains two ions, cation and anion. The cation is cesium plus. Cesium is a type one metal.
08:07
So I just have to give it the name of the element, which is cesium, and then substitute that with the word fluoride. Because that's the n ion name. The anion is made of fluorine atoms and the suffix "-i." Cesium chloride.
08:25
Another one, aluminum chloride. Aluminum, that's the name of the metal. It's a type one metal. And then chlorine is becoming a type one metal. This is now called chloride, because it's an anion. Aluminum chloride.
08:44
Now note that I don't bother here about the number of chlorine ions in there. There's three, but that's not specified here. It's just called aluminum chloride. How about this? What's this called?
09:09
Calcium sulfide. Absolutely. Very good. Another one? magnesium oxide. All right. All right. Very good.
09:21
Now how about those type two binary ions? What's the difference? So if the compound contains a type two metal, then we have to do something extra. And that extra is, you follow exactly the same set of rules as before, but we supplement the name of the cation, the metal,
09:41
with a roman numeral indicating the charge of the ion. Or the oxidation state, as we will find out in subsequent lectures. So here is an ion this is manganese manganese 2+. It is an ion with a charge 2+.
10:01
If I make an oxide out of this, like this, okay, this is manganese oxide, I have to specify the charge of the manganese ion. In this case, 2. So the name for this is not manganese oxide, it's manganese 2 oxide. Like this. Because manganese is a type
10:22
2 metal that can exist in multiple oxidation states. Here's another one. It can exist in oxidation state, 3+. manganese 3+, the oxide that follows from it is a different formula. So there's multiple manganese oxides, and I can specify them
10:41
based on the oxidation state of the cation. This is called manganese 3-oxide. Which has a very different formula than manganese 2-oxide. manganese can yet exist in another oxidation state, where the charge of the cation is 4+, and in this case,
11:02
the oxide that follows from that cation is manganese O2. It is 2-oxide anion. The name of this compound is manganese 4-oxide. So here you see the necessity of specifying, with the Roman numeral, the oxidation state of the metal.
11:23
Yes. The question is, how do you differentiate between a type 1 and a type 2? So remember from the last lecture there was a periodic table with colors, and in that table there were metals, some of
11:42
these had only one option, some of them had multiple options. So those are the ones you have to know. But, the rule of thumb, actually, the first two columns of the periodic table are always type 1, okay? Those are the alkali and
12:02
alkali metals. Yes? No, no, no. You use the Roman numerals for every binary compound that has a type 2 metal in it. Okay? We'll see more examples of this. Yes? What you need to know is whether the metal is a type 1 or a type 2.
12:31
As you'll see, this is not completely arbitrary. The first two columns of the periodic table, right from the left, are type 1 metals. That's not hard to memorize. And aluminum is one of them, too.
12:45
All the metals in the middle, so to speak, are generally type 2. There are a couple of exceptions. Okay, so this is the same table from last time, and I'm showing it once again. These are common type 2 ions.
13:07
It would be good if you know them. You don't have to know them by far, necessarily, but be familiar with them enough that you may recognize them, or you know them.
13:27
You can work with this in the sense that you can find the names of these compounds. So here's an example. This is copper 1 chloride.
13:43
If I were to call this just copper chloride, I would be making a mistake. Because I have to specify what the oxidation state for copper is. Copper is a type 2 metal. It can exist in several oxidation states among which 2+, and plus. I need to specify which copper cation I'm talking about.
14:00
This is copper 1 chloride. Copper 2 chloride, we have a different formula. It would have looked like copper and then two chlorine anions, right? It's a different compound. This is iron 3 oxide. How do you know that? There's three, not two. Because there is
14:23
three of these oxides, oxide is always 2-, three of them means six. Six negative charges. That means if you have two of these, then the charge of the iron cation must be 3+. So this is what you should be able to figure out. If I give you this name
14:43
of the compound, you should be able to write this. You should be able to write it first. Okay. How about this? Now let's look at the chart here. I see here two types of mercury. It's a little funny. Mercury 2+, is here, and mercury 1 is also 2+, but it has two mercuries together. So this is basically two mercuries together, and the overall charge is 2+.
15:08
In this case, what I have is mercury and oxygen. This is 2-, this must be 2+, that is this guy right here. Mercury 2 oxide.
15:24
How about this? What is this? Is this lead? Is it lead 2 or lead 4? It's lead 2, right? Because Cl and Cl- that means two negative charges, that means this must be 2+.
15:42
Ooh, that goes fast. So this is, again, another chart I showed last time. And this is a table, once again, you should be able, I can ask you to memorize this, which is really more than is needed, you have to be able to work with this. Work with this. Recognize the names. That's the kind of idea.
16:05
You don't have to reproduce this table. You have to be able to work with the compounds that are on it. Again, there is systematic in this table especially in terms of those compounds that contain oxygen atoms.
16:22
For instance, the nitrate and nitrate. This guy, which has one oxygen less, is called nitrite and the one that has one oxygen more is called nitrate. And the same holds for sulfite and sulfate. I said it last time, I said it again. But note that sulfite is O3
16:42
and nitrite is O2 so the ite and the eight doesn't specify how many, it just specifies relative to the eight, and the ite is one less. That's the convention. You see, the same thing is reproduced on this side. This is chloride this is chloride, this is chlorate, which is one more,
17:03
and then hypochlorite is one less. So hypo, ite, eight, and then perchlorate is one more. So from one to four oxygens. Oxo anions have this kind of nomenclature. Okay. So again, we'll work with this and you'll see
17:22
in what way you have to be able to reproduce this information. All right. So now let's move on to another type of compound. Not ionic, but covalent. Binary covalent, meaning two types of elements make up this compound. And they are covalently bonded.
17:44
Here are two examples. This is nitrogen monoxide. It is a covalent compound, neither of these elements are metallic. Okay? So this is a covalent link between them. This is called nitrogen monoxide. This is also a covalent compound, sulfur dioxide.
18:06
None of these elements is metallic, so this is a covalent compound. The name is sulfur dioxide. How do you determine the name of these covalent compounds, these binary covalent compounds? Here's a little set of rules, if you follow these, you will be fine.
18:22
Okay. Again, the first element is named first. In this case, nitrogen, in this case, sulfur. The second element is named as if it were an anion. It's not an anion, it's covalently linked, but just pretend it is, because that's for the naming.
18:40
The naming follows the same kind of recipe. Then prefixes denote the number of atoms. If there's one, mono, two, di, tri, tetra for four, penta for five, hexa for six. But the prefix mono is never used for the first element.
19:03
Okay. So let's put it into practice and see what happens. Here's one. This is an element, sorry, a compound composed of two elements, phosphorous and chlorine. Both are not metals, it's a covalent compound. A binary covalent compound could have mattered. What I have to do is name the first element first, that is phosphorous,
19:23
the second one as if it were an anion. That means chloride. So, phosphorous, chloride. However, I have to specify the number of atoms. There's one phosphorous and three chlorines. That means, if I follow this rule over here, it should be called monophosphorous trichloride. However, the last rule says the
19:48
prefix mono is never used for the first element. So, I drop the mono for the first. Hence, phosphorous, trichloride. Phosphorous, trichloride.
20:04
Another one. This is nitrogen, two of it, and then one oxygen. This is nitrogen, two of it, and then one oxygen. Also a covalent compound. I see two nitrogen. So I call this di because definitely this is not one. Mono I can't really use for the first element, but di I can, so dinitrogen
20:24
and then one oxygen, monoxide. Dinitrogen, monoxide. So the naming is different than the naming for the binary anionic compound. To specify the number of atoms.
20:41
Okay. We'll practice a few later. Let's first move to another set of important compounds, namely acids. What is an acid? We'll talk about it extensively, close to a second different, not now, but very briefly, an acid is a substance that when you dissolve it in water, the cation is split off, forming a dissolved item in life.
21:09
Or a proton. Now, acids are typically written with an H as their first element. Like here. HCl.
21:21
This is called hyporic acid. This is another acid that starts with an H, this is sulfuric acid. So how do we find out the naming of these compounds? All right. Now, let's first distinguish two types of acids. One that contains an oxygen atom, and one that doesn't.
21:47
So let's start with the one that does not contain an oxygen atom, like this one here. How do you name that? All right? Here we go. You add the prefix hydro
22:00
to the anion name. And then the suffix "-ic-" is added to the anion name. So this is chlorine, I add hydro to it, hydrochlorine, but then I change the suffix into "-ic." So hydrochloric acid. I always add the word acid to the final name. Hydrochloric acid. You add
22:25
hydro as a suffix, and you add "-ic-" as a prefix, and suffix "-ic-" to the anion name. Here's one. This is a compound, it's an acid, it starts with an H
22:40
it has no oxygen, so I have to follow this set of rules. This is sulfur, and this hydro comes in front of it. Hydro sulfuric acid. Hydro sulfuric acid. Another one, what is this? Hydro bromic acid.
23:02
Hydro bromic acid. So keep that in mind, and then we'll stick over to acids that do have an oxygen present. And it's different.
23:21
Because if it has an oxygen, what I have to do is, I start with an anion name. Be it an elemental anion or a polyatomic anion. As you will see in a few seconds. And to this anion name, if this thing ends in "-ate," I add the suffix "-ic." But if it ends in "-ite," I replace it like this. Remember? Those polyatomic anions contain an oxygen, and it can end in "-ite," or "-ic."
23:51
And depending on whether they end in "-ate," or "-ite," I have to do different things. So let me give you a couple of examples.
24:01
This here is an acid, it starts with an H, it has an oxygen in it. In fact, this is a polyatomic anion. This is phosphate. Phosphate. So I take that word phosphate and then I substitute "-ate-" for "-ic." Phosphoric acid.
24:21
Here's another one. An acid. This is the polyatomic anion. Its name is sulfate. And I change the "-ate-" into "-ic." Sulfuric acid. I think the root name of the anion, sulfuric acid, is the name of this compound.
24:41
Here's another one. This is an acid it contains an oxygen this is nitrite and it ends in "-ite." So this should be nitrous acid. Oops, that was too fast. Nitrous acid. So whether the polyatomic anion, the anion oxygen, ends in "-ate-" or "-ite," we use the sulfate "-ate-" or "-ic."
25:15
Finally, the last set of substances or compounds we are looking at are the so-called hydrates. What are these?
25:24
Well, hydrates are compounds that have a specific number of water molecules incorporated in the structure. Here's an example. This is cobalt-2-chloride, but in the lattice structure are incorporated six water molecules per cobalt-chloride unit. So each cobalt-chloride unit has six water
25:50
molecules associated with it. That unit repeats itself throughout the system. The proper name of this compound is cobalt-2-chloride.
26:01
hexahydrate. The name is a spallox. Right in the middle of the root compound, which is cobalt-chloride, we add a prefix hydrate to the root. Prefix meaning the number of water molecules. In this case, six. So hexahydrate. Here's one. This is barium chloride dihydrate. Two water molecules added to the barium hydrate.
26:35
Barium chloride. How about this one? What is this?
26:50
Copper-2 copper-2-sulfate pentahydrate. It's copper-2 because the sulfate anion has a 2- charge. 2-. The aim of the copper must be 2+.
27:07
And I can specify because copper is a type 2 metal. So copper-2-sulfate pentahydrate. All right? All right. Well, those are the set of rules
27:20
for these kinds of compounds. So we talked about binary ionic, binary covalent, acids, both acids that contain an oxygen and acids that do not contain an oxygen, and hydrates. Those are the ones that we talked about. So we should be able to name these compounds properly.
27:41
This is just a small subset of the total number of compounds, of course, right? These are the simplest ones and we should be able to deal with them. Okay. So a few common stinkers. This is not iron chloride because iron is a type 2 metal, it is iron-3 chloride. Now, I can predict that on the midterm,
28:03
and the final, for that matter, there will be about 25% of the people that are forgetting about it. Every year. Just like that. Let it not be used. Just be mindful. Even in type 2, add this Roman numeral to it.
28:27
Another one. What is this? A very common problem with this one is that some people think it looks a lot like
28:41
SO3 2-, from the table of polyatomic anions. It's called sulfite. This is something that, again, about 30% of people call this sulfite. It's not sulfite. This is not an ion. This is a neutral molecule. This is sulfur trioxide.
29:04
Okay. How about this? Well, I put this in here because some people call this hydrogen carbonate. This is a carbonate anion, this is hydrogen, so this is not wrong, necessarily. But we do consider this wrong in this particular context, because it says aqueous. That means this thing is dissolved in water.
29:27
Once it's dissolved in water, it is an acid. And we don't call this hydrogen carbonate anymore. It's called carbonic acid. Why is it called carbonic acid? Because this is carbonate, it is an acid, it ends in 8, it becomes 8. Carbonic acid.
29:43
Carbonic acid. Here's another one this is a compound that contains selenium and fluorine it is a covalent compound a lot of folks call this selenium fluoride it's not correct, because it is selenium hexafluoride. The hexafluoride has to be in there, because this is a covalent compound. So
30:07
the hexafluoride indicates what kind of compound it is. If you say selenium fluoride, you consider this to be a binary ionic compound. How about this one?
30:23
Covalent compound containing nitrogen and oxygen some people call this nitrogen trioxide it's almost right, but not quite, because it is dinitrogen trioxide why do people drop the dye? Because they tend to drop the mono, and then they drop everything.
30:44
Only the mono prefix is dropped from the first element. That's it. Nothing else. Okay. another example selected cases in which the compound name correctly matches the formula
31:05
okay, so here I have a series of compounds, let's see if the name is correct or not rubidium selenide yes, says the person now in this particular case, and this is maybe a little bit early for you
31:21
to completely know this, but I have to check whether or not the charges are correct rubidium is always 1+. Okay? Rubidium is actually the first code on the pair of tables. Those ions always have 1+. The second code has always 2+. Rubidium must be 1+.
31:42
selenium is 2-. So this is not neutral. Okay? This is not correct, for that matter. Another example. Rubidium iodide. Is that good? Yeah, this one is good because iodide always has negative 1.
32:03
Rubidium is 1+, like we just saw. Okay. How about this one? No! It's wrong! Good answer. Tell you right, it's 2-, this is 1+, it's not correct. How about the fourth?
32:21
Sodium bromide. Is that correct? No, it's not correct. Sodium is a first column, okay, Macaulay metal and it's 1+, bromine, 1-, so this should be just NaBr. Then it will be sodium bromide, in this case it's not. This compound does not exist. How about this?
32:44
Rubidium sulfide. Sulfide is 2-, rubidium 1+, incorrect. And finally this one here. Complete nonsense. Rubidium is 1-, 3 of them is 3-. Rubidium is only 1+. Doesn't work.
33:03
All right? So this is kind of the kind of exercise you have to be able to do. And things like this. Enter the formula for each compound. So we'll start with cesium iodate. This is kind of a tricky situation because iodate we haven't talked about. So let's see what it is.
33:22
Iodate is an iodine atom with three oxygens. Just like carbonate is a carbon with three oxygens. cesium iodate is a combination of these two guys, both have charged 1-, sorry, 1- here, 1- for the cesium. Put them together, they're from a different compound. So this is the formula for cesium iodate.
33:47
Iodate is a compound I'm showing to you so you know it exists. It's not part of the table, you have to be able to work with it. But this is just to indicate that there's more beyond that table. And the chemistry is not just summarizing as small as the table. It's much more than that, and it's giving you a flavor. Don't be afraid.
34:06
Iron 2 carbonate is composed of iron 2+, and the carbonate anion, which happens to be 2-. Okay? So when you put them together, they form a nice neutral compound. Iron CO3.
34:26
How about this? Cesium sulfate. cesium 1+, sulfate SO4 2-. There it is. This is 2, this is 1, so I need two cesiums. cesium 2, SO4.
34:46
Chromium 3-chloride okay, there's a 3 here, that means that chromium is in its oxygenated state, 3, that means 3+, for the charge of the cation, chlorine is always 1-. I need three chlorines to make a neutral compound, so it's
35:01
chromium Cl3. That is chromium 3-chloride, a beautiful purple compound. Very nice.
35:27
Before you guys go, let me make it one o'clock, one o'clock, I sent a post in email, and on the left side, the whole professor. We have a forum called the alpha forum, some people have tried it. It is actually a great means to discuss things with your peers.
35:45
If you don't, if you're unable to solve a question on the homework basis, you can just ask questions online, and hopefully somebody will answer it, including myself. So try to use it, it's a great tool, we'll see you again at the midterm, we'll be happy to answer that.