Naming Acids - Video Tutorials & Practice Problems
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Acids, for the most part, are covalent compounds that begin with a hydrogen.
Naming Acids
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Naming Acids
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Before we start naming acids, let's first talk about what exactly is an acid. Now, an acid is usually a covalent compound beginning with a hydrogen ion. So hydrogen ion in this case is H+ And another name for this hydrogen ion is called the hydronium ion. Now going back to covalent, what exactly is meant by covalent compound? Well, a covalent compound is a compound that contains only nonmetals bonded together. Now if you don't remember who the nonmetals are, make sure you go back and take a look at my videos on the periodic table and the classifications of the elements that lie within it. If we take a look here, some common types of acids, all of them are covalent because all of them possess nonmetals together. And since they're all covalent, we also see next that they all begin with hydrogen. That tells us that they all represent acids. So HCl, Hn02, H2SO4, we see that some of them are pretty simple like HCl and some of them are pretty complicated like H3PO4. We'll talk about the different types of acids later on and the rules associated with naming them. Now, remember, we said that they usually begin with the hydrogen ion. Usually does not mean always. And with chemistry, you're gonna see that exceptions do pop up here and there. A good exception to this is acetic acid. Now acetic acid can be drawn 2 different ways. The first way goes along with the definition we have. It starts with the hydrogen and it's covalent because it only has nonmetals. But another way to write acetic acid is c h three c o o h. In this case, the hydrogen ion is actually written in the back. Okay. So this is an exception to our definition, where this is still an acid, but it doesn't begin with the hydrogen ion. Now that we know the basic structure of an acid, let's move on to some videos and let's tackle the different types of acids that exist and the ways of naming them.
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Naming Acids
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So here, let's take a look at binary acids. Now binary acids, since they're acid, they are also represented as covalent compounds and they're gonna contain the h+ ion, which is our hydrogen ion. But here they're going to be bonded to a non metal anion that is not oxygen. So binary acids are covalent compounds, usually beginning with hydrogen, that contain no oxygen. Here, how do we form them? Well, we know that they possess the h+ ion, and let's think of a nonmetal they can be connected to in the anion form, which means they have a negative charge. So let's say we're dealing with iodine. Iodine is in group 7 a, so its charge is minus 1. So here we have plus 1 from the hydrogen, minus 1 from the iodine. If you've seen our videos on writing ionic compounds, we apply the same principles here. Remember, if the numbers in the charges are the same, they simply cancel out and you combine together your elements. So here, this would be Hi. Hi would represent a typical binary acid. Alright. So here, rules for naming these binary acids. Well, step 1 is the prefix they're they're going to use. The prefix they use is hydro, and that basically represents the h+ion. And then we're gonna say step 2, use the base name of the nonmetal. Now here's the thing. Remember, the base name is usually the beginning part of the beginning name of the nonmetal that is being used and it's unchanged, except when we use sulfur or phosphorus. So in their acid forms, for sulfur, we actually use the entire name. We don't use the base name. We use the entire name for sulfur. And for phosphorus, we don't just use its base name, we use a little bit more. The base name of phosphorus is phospha, but in acid form, we actually use OR as well. So, again, the nonmetal part of the acid, that is not the h plus, we use its base name except for sulfur and and phosphorus. We use a little bit more than just their base names. Then finally, to end the name of the binary acid, we use ic acid for the end of the name. So we apply these principles and we'll be able to name any type of binary.
Binary Acids contain a hydrogen ion connected to a nonmetal that is not oxygen.
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example
Naming Acids Example 1
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So for this example question, it says write the formula for each of the following compounds. We have hydroiodic acid, hydrosalenic acid, and hydrofluoric acid. Alright. So we're going to say that hydro, we know that represents the H+ion involved, so we have H+ for all of these. Since they're all binary acids, we know they all end with -ic acid. What we look at is the base name. The base name tells us the nonmetal involved. So Iode means we're dealing with iodine. It's in group 7 a, so it's minus 1. Selenium. It's in group 6 a, so it's, 2 minus or minus 2. And then fluor means we're dealing with fluorine which is a group 7 a, so it is minus 1. Now for the first one, for a, remember, when the numbers and the charges are the same, they simply cancel out and you combine your elements together. So hydroiodic acid is just h I. And then also for c, plus 1, minus 1, the numbers are the same, so you just combine them together. So hydrofluoric acid is h f. For b, hydrosalinic acid, we have here different numbers in the charges. Remember, when the numbers are different, they crisscross. So one from here comes here, 2 from here comes here, so that means, hydrosalenic acid is h two s e. If you don't quite remember these rules, make sure you go back and take a look at our videos talking about writing ionic compounds. It's the same kind of principles behind this. We look at the ions, the charges, if the numbers are the same, they simply cancel out. If the numbers are different, then they crisscross. Using this helped us to determine each one of these 3 binary acids. Now that we've done this example, move on to the next video where we take a look at a practice problem.
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Problem
Problem
Give the systematic name for the following compound:H2S
A
sulfuric acid
B
hydrosulfuric acid
C
sulfic acid
D
hydrosulfic acid
E
hyposulfuric acid
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Problem
Problem
Give the systematic name for the following compound:HCN
A
cyanate acid
B
cyanous acid
C
hydrocyanous acid
D
cyanic acid
E
hydrocyanic acid
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concept
Naming Acids
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When it comes to oxyacids, oxyacids represent our second type of acid. Now we're gonna say they represent covalent compounds because they're acids, they contain hydrogen ion as well, but now they're bonded to a polyatomic ion containing oxygen. And it's pretty clear why that is because the name is oxy, highlighting the fact that we have oxygen present now. So how could we form an oxyacid? Well, here we have our h+ion, so h plus 1, and let's just think of a polyatomic ion that possesses oxygen. Here, we could have n o three minus. N o three minus is our nitrate ion, and remember, when the numbers in the charges are the same, they just simply cancel out and you combine together your elements. So HNO 3 would represent an oxyacid. It is covalent because it possess only nonmetals. It has your hydrogen ion at the beginning of the compound structure and altogether we have our oxyacid. Now that we know how they're formed and what they represent, click on to the next video and let's go over the rules for naming them.
Oxyacids contain a hydrogen ion connected to a polyatomic ion with oxygen.
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Naming Acids
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When it comes to naming oxyacids, it's first important to remember your polyatomic ions. Now if you don't remember your polyatomic ions or you haven't watched my videos on them, I suggest you pause this video and go back and take a look at those videos first. Then come back and we can tackle naming oxyacids together. Alright. So for those of you who are ready, let's go. We're going to say here rules for naming oxyacids. Rule 1, if the polyatomic ion ends with 8, then change the ending when it's in its acid form to ic acid. Here, we have a memory tool that'll help us. So here we're gonna say I 8 in acid, and it was icky. Now, don't go biting into acids or eating them in any way, but just remember that 8 goes with icky. Okay? So in its polyatomic ion form, it's 8, but in its acid form, we change the ending to ic acid. So here we have H plus with n o three minus. Remember, n o three minus is your nitrate ion. When I combine them together to give me H n o three, that is our oxyacid form. Here, the 8 ending changes to ic, acid. So nitrate becomes nitric acid. But remember, we also have polyatomic ions that end with ite. What do we do in those situations? Well, we're gonna say if the polyatomic ion ends with -ite, then in its acid form, we'll change the ending to oce acid. And, again, we have a great memory tool, so I only bite into delicious into things that are delicious. So So this will help us remember, if we have a polyatomic ion that ends with ite, in its acid form it becomes ose ending, ose acid. So here we have H+ with NO2 minuteus. N o two minus is our nitrite ion. When it combines with h plus, we get HNO 2, which is our oxyacid form. The ite ending changes to oce acid. So nitrite becomes nitrous acid. So again, unless you know your polyatomic ions, it gets pretty tricky in terms of naming the oxyacid Now that we've seen the rules for this, let's continue on with some questions and test what we've learned.
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example
Naming Acids Example 2
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In this example question it says write the formula for each of the following compounds. Alright. So for a we have h 2 c o 3. Alright. So think about what is making up this oxyacid. Well, we know that this is h plus, and we know here this c o three is altogether, c o 3. The 2 that comes here originated from the c o 3 because here, this is carbonate ion. Remember, the ending is ate. Remember, I ate an acid and it was icky. So that means that ate will become ich acid. So that means that this represents carbonic acid. So h 2 c03 is carbonic acid. Next, h 3p0 3. What makes it up? We know we have h plus here and we know that p o 3 here, polyatomic ion wise it was 3 minus. We also know based on what we've seen in the polyatomic ion videos, that this would be called phosphite, phosphite, ending ends with -ite. So remember, if it ends with -ite, we're gonna say here that I bite into things that are delicious. Right? So ite becomes ose acid. Also, remember that phosphorus, we use more than just the base base name. We also include or, and then it would be oseacid. So this is phosphorous acid. Finally, we have h 2 s o four, which is composed of h+ and s o four, which is a polyatomic ion that is two minus. It's one of our common types of tetraoxides. Alright. So this is called sulfate. It ends with 8, so that means that our acid form would be ic acid. Just like phosphorus, sulfur uses more than just the base name. So we actually use the whole name sulfur, and remember, it becomes ic acid. So this is sulfuric acid as the name for our oxyacid. So, again, you have to remember your polyatomic ions because they go hand in hand with learning and recognizing the oxyacid forms that exist. Now that we've done this example, let's continue onward with more practice on naming oxyacids.
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Problem
Problem
Write the formula for the following compound:Hypobromous acid
A
HBrO
B
H2BrO
C
HBrO2
D
HBrO3
E
H2BrO4
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Problem
Problem
Write the formula for the following compound:Cyanic acid