Naming Compounds

Nomenclature is the system used in chemistry for the naming of different compounds and molecules. 

Ionic Compounds

Concept: Understanding how Ionic Compounds are formed

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Video Transcript

Hey, guys. Welcome back. In this new video, we're going to take a look at ionic compounds. Now, just realize in the advent of chemistry, in the beginnings of chemistry, there were common names that were given to tons of different compounds: morphine, quicklime, what have you.

But just realize, since the early stages of chemistry, hundreds if not thousands of compounds have been identified. It became more important to find a systematic way of naming each of these compounds. Instead of using a common name, chemists all around the world decided to use a new form of scientific naming structure in order to name these new compounds. They call this structure nomenclature. Chemists all around the world use nomenclature.

Now, our main focus here is to just identify the first type of compound we're going to learn how to name: ionic compounds. Remember, fundamentally, an ionic compound is just the connection between a positive ion, which is called a cation, and a negative ion, which is called an anion. Usually, this positive ion, or cation, will be a metal. We're going to say that the negative ion, which is our anion, will be our non-metal.

So if we take a look here, we're going to say metals will tend to lose electrons – because remember, if you're going to be a positive ion, you have to be losing your negative electrons. So they're going to become positively charged ions, which we just said were cations. Non-metals, on the other hand, non-metals tend to gain electrons, so you're gaining negative electrons, and as a result, you become negatively charged. These negative ions we said were anions.

So remember, fundamentally, all ionic compounds are a positive ion connecting with a negative ion. Usually this metal will be positive and the non-metal will be negative.

An example of us having a cation which is not a metal would be ammonium. Remember, ammonium is a polyatomic ion. It's NH4+. And we could have a negative ion, nitrate ion, which is NO3-. Since they're opposing charges, they're going to be attracted to one another, so they would form this compound. See, so it's not always true that an ionic compound is between a metal and a non-metal.

You most likely won't see things this complex initially, but just realize eventually you should be able to recognize this. So an ionic compound, again, is a connection between a positive ion and a negative ion. Usually that positive ion will be a metal. In some cases, it could be ammonium or other positive polyatomic ions.

Now, down here we have a periodic table. What we're going to do here is we're going to go through the different charges that we expect based on the groups of each of these elements. Remember, we already talked about this earlier on, but we're just going back to it again to refresh your memories.

Remember, Group 1A elements are +1, Group 2A are +2, Group 3A are +3. We're going to say Group 7A is -1, Group 6A -2, Group 5A -3. These are the things we already know. Remember, Group 4A is midway, so we don't really say that they're strictly positive or negative here.

Now remember, these are the charges associated with each of these groups. Our transition metals here in the pit, our transition metals have variable charges, meaning they have more than one charge. We're going to learn how to name them based on the type of transition metal we have later on when it comes to nomenclature.

But remember, we said that transition metals tend to have more than one charge, except for these common three. Remember, we said that silver is always +1, cadmium, which is Cd, is +2, and zinc is +2. So remember, these guys are transition metals, but unlike most other transition metals, they only have one charge.

And remember, we also said there's another weird thing that goes on. Remember that tin and lead here, both of them are not transition metals, but they act like it because they have more than one positive charge. Both of them could be either +2 or +4.

So those are the different charge distributions that you need to remember, and they're going to help us in naming a lot of different types of ionic compounds.

So guys, at this point just remember that an ionic compound is the connection between a cation and an anion, and just remember the different charge distributions associated with the different groups and associated with certain types of transition metals.

Metals lose electrons to be positive ions, whereas nonmetals gain electrons to become negative ions. 

Naming Binary Ionic Compounds

An ionic compound involves the bond between a cation (positive ion) and an anion (negative ion). 

Concept: Rules for Naming a Binary Ionic Compound

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Video Transcript

First, we're going to look at just regular ionic compounds, which we refer to as binary ionic compounds. What are the features? How do I know I have a binary ionic compound. Basically, a binary ionic compound is anytime we have a positive metal and a negative nonmetal connected together. Basically, we have a cation with an anion.
There's a system for naming. Remember, we said it's called nomenclature. For binary ionic compounds, the rules go as follows, we're going to say that the metal is named and written first. But, if that metal happens to be a transition metal – remember, transition metals have more than one charge. So it's important for us to determine, which one of the ions we're talking about.
For example, we could have cobalt plus one or cobalt plus two. But how do I know which one I have when I have my ionic compound? When we have the metal as a transition metal, we have to use a roman numeral to describe the positive charge. Cobalt plus one would be cobalt (I). We put it in brackets, the one. And Cl plus two would be cobalt (II).
The next part, remember our binary ionic compound is made up of a metal part which is positive and the negative, an anion, which is our nonmetal. The nonmetal will keep its base name. Here I give us a list of the most common types of nonmetals and with them, their base names. We're going to say that the nonmetal keeps its base name, but has its ending changed to -ide. 

Concept: Understanding the Base Name of the nonmetal

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Video Transcript

Nitrogen is in group 5A. We already said that group 5A has a charge of minus three. Nitrogen is neutral. But when it gets a negative three charge, it becomes an anion. Its name then changes. Nitrogen is going to keep the first part of its base name, nitr-, but then we have to put an -ide at the end. So N3- becomes nitride.
Sulfur is in group 6A. It's minus two because it's in group 6A. It's going to keep that first part of its name. And we're going to say that the ending is changed to -ide. So this becomes sulfide. Basically, that's the way you work it out. Remember, keep the base name for the nonmetal, put -ide at the end.
Now that we've seen the basic ways of naming binary ionic compounds, let's look at this example first. 

Example: Provide the molecular formula or name for each of the following compounds.

a) Calcium phosphide               b) CoO

 

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Problem: Provide the molecular formula or name for each of the following compounds.

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Naming Ionic Compounds with Polyatomics

Concept: Rules for naming Ionic Compounds with polyatomics

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Video Transcript

We're going to take a look at how do we name ionic compounds when they possess polyatomic ions. The features here will be we're going to have basically a cation and an anion once again, but, in this case, our cation or our anion may be a polyatomic ion. This could be a positive metal or a polyatomic ion. This anion could be a negative nonmetal or a polyatomic ion.
It follows the same basic rules that we learned for binary ionic compounds, so we're going to say the metal keeps its name and is named and written first. We say that if the metal happens to be a transition metal, remember transition metals have more than one charge, so it becomes important to distinguish which one am I talking about. Am I talking about tin 2 or tin 4? To do this we use a Roman numeral to describe the charge.
We're going to say that the polyatomic ion portion, whether it's positive or negative, is just named normally, so it keeps its name. It doesn't have anything changed to -ide, it doesn't use any type of Roman numerals. None of that happens. 

Example: Provide the formula or name for each of the following compounds. 

 a)  Iron (III) Acetate                                                                   b)  Copper (I) phosphate

           

c)  Strontium Carbonate                                                          d)  Ammonium Nitrite

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Example: Provide the formula or name for each of the following compounds.

a) Pb(CrO4)2                                                                             b)  Ga(ClO4)3

 

c) Mn(HSO4)2                                                                           d)   Ba(CN)2

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Naming Ionic Hydrates

Concept: Rules for Naming Ionic Hydrates

4m
Video Transcript

Basically, what are the features of a hydrate? We're just going to say it's an ionic compound, and we know how to identify those, and water. Right here we have a good example of an ionic hydrate. We have CUSO4 and then that little dot there, that little dot there means that those five water molecules are actually surrounding my ionic compound. What that really means is that I had my ionic compound and I decided to dunk it into water. Surrounding it are these five water molecules.
We're going to say the rules for naming the ionic part are the same rules we've been following. We're going to say that the metal is written and named first. If it's a transition metal, remember, transition metals have more than one charge, so we have to use Roman numerals to describe the particular positive charge that we see.
If that ionic compound happens to have just a regular nonmetal, remember that nonmetal keeps its base name and has its ending changed to -ide. If that nonmetal portion happens to be a polyatomic ion, we name that polyatomic as we normally would. The rules that we learned for ionic compounds stay the same.
Now we have to introduce rules when it comes to the water portion. We're going to say that the water portion will be called a hydrate. We're going to say to describe the number of water molecules around the ionic compound, we have to use these numerical prefixes that we have on our right. So mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, opta-, nona-, and deca-. This is the approach that we're going to take.
Let's go back up to that first compound that we saw. Remember that copper is a transition metal, so there's a possibility of it having more than one charge. Remember, what do we do when that happens. All we do is we just say that this is X. Then we're going to say SO4 is a polyatomic ion. Remember that is sulfate. Sulfate has a negative two charge. You have x minus two equals zero, so x equals plus two. So the charge of that copper is plus two, so its name would be copper (II) sulfate. That's how we name the ionic portion.
Now we have to name the water portion. Now we said that there were five waters, so the numerical prefix would be penta. The water portion we just say is called a hydrate. The name of the structure would be copper (II) sulfate pentahydrate. That's how we take the approach to naming ionic hydrates. 

An ionic hydrate is when an ionic compound is bonded to one or more molecules of water

Example: Write the formula for each of the following compounds.

a)  Calcium carbonate hexahydrate

            

b)  Lead (IV) sulfate pentahydrate

 

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Problem: Give the systematic name for each of the following compounds:

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Naming Molecular Compounds

Concept: Rules for Naming Molecular Compounds

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Video Transcript

Just so that you realize, when we say molecular compounds, another name for them are covalent compounds. Remember that covalent compounds are the connections between nonmetals. The features here are nonmetal and nonmetal together.
Because these nonmetals can arrange themselves in different proportions, we have to use a numerical prefix system in order to describe the numbers of each nonmetal combined in that covalent compound. These are the same numerical prefixes we had to use when we talked about the hydrides.
The rules we're going to say for our nonmetal connected to nonmetal is the first nonmetal is named normally, so we don't change its ending to -ide or anything like that. It's named normally. We're going to say it uses all of the numerical prefixes except mono. We never use mono to describe the first nonmetal in our covalent compound.
We're going to say the second nonmetal keeps its base name and has its ending changed to -ide. The second nonmetal will also use any of the numerical prefixes, including mono. 

A molecular compound represents a covalent compound, in which nonmetals are connected together. 

Example: Write the formula for each of the following compounds.

a)  Disulfur monobromide                                    b)  Iodine Tetrachloride

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Problem: Give the systematic name for each of the following compounds:

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Naming Acids

Concept: Rules for Naming Binary Acids

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Video Transcript

Before we begin, we should realize that acids come in two different forms. We have our binary acids and we have our oxy or oxoacids. Now let's take a look at the binary acids. What exactly are the features of a binary acid?
First of all, a binary acid has to have H+. That H+ will be connected to a negative ion, an anion. Now, remember this negative ion or anion comes in two different types for binary acids. It could either be a negative nonmetal. Example, we could have Cl-. Remember, chlorine is in group 7A, so its charge is -1. That H+ will combine with the Cl- to give us HCl. That will be an example of a binary acid.
Now, the anion could also be a negative polyatomic ion with no oxygens. A good example of polyatomic ion with no oxygens is CN-. The H+ and the CN- will combine to give us HCN, another type of binary acid.
So, what are we supposed to take from this? Well, we should realize that binary acids all have hydrogen involved. That hydrogen will be connected to non-metals that came from a negative ion. What we should also realize is that binary acids contain no oxygens at all. This is the difference between a binary acid and an oxy or oxo acid. Binary acids don't contain any oxygen, oxy or oxoacids do contain oxygen.
Now, we're going to say when it comes to naming binary acids, we follow these rules. We're going to say that prefix or the beginning of the name will be hydro. This hydro name comes from the H+ ion involved in creating our binary acid. We're going to say, we're going to use the base name of the nonmetal, the base name of the negative ion, the anion. We're going to say the suffix or ending of our binary acids will be -ic acid. 

A binary acid is a covalent compound that contains an H+ ion connected to negative ion

Example: Write the formula for each of the following compounds:

a) Hydroiodic acid                                  b)  Hydroselenic acid                              c)  Hydrofluoric acid

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Problem: Give the systematic name for each of the following compounds:

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Concept: Rules for Naming Oxyacids

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Video Transcript

Okay, guys, we're going to continue with the same page that we’ve been on, but now we're going to learn how to name oxo or oxyacids. First thing firsts, what are the features of an oxy or oxoacid? Well, we have to say that they contain H+ and now the second feature is that they possess a negative polyatomic ion with oxygen, with oxygen or oxygens. So, that’s the defining characteristic of oxo or oxyacids. Here we have a polyatomic ion connected to our H+. That polyatomic ion has one or more oxygens present.
Now, what are the rules for naming these types of acids? We're going to say, if the polyatomic ion that’s involved in the oxy or oxoacids has 'ate' as the ending then we’re going to change that ‘ate’ ending to 'ic' acid. If the polyatomic ion ends with -ite, then we're going to say we change the -ite ending to 'ous' acid. Again, remembering your polyatomic ion is going to be essential for naming oxo or oxyacids. Without that, it’s going to be really difficult.

An oxyacid is a covalent compound that contains an H+ ion connected to a polyatomic ion containing oxygen

Example: Give the systematic name or formula for each of the following compounds:

a)  H2CO3                                             b)  Nitric acid                                         c)  H2SO4

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Problem: Give the systematic name or formula for each of the following compounds:

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Naming Compounds Additional Practice Problems

An alkaline earth metal forms a compound with oxygen with the formula: 

(The symbol M represents any one of the alkaline earth metals.)

A) MO

B) M2O

C) MO2

D) M2O2

E) MO3

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What is the name of H2SO4(aq)?

a. hydrogen persulfate

b. sulfurous acid

c. dihydrogen sulfur tetraoxide

d. sulfuric acid

e. dihydrosulfate

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Gaseous HCl is known as

a. hydrogen chloride.

b. hydrochloric acid.

c. monohydrogen monochloride.

d. hydride (I) chloride.

e. hydrogen monochlorine.

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What is the molar mass of tetraphosphorus pentoxide?

(A) 100 g/mol

(B) 142 g/mol

(C) 173 g/mol

(D) 204 g/mol

(E) 220 g/mol

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Give formulas for the following compounds:

chlorine trifluoride

 

tetraphosphorus heptasulfide

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The formula of the compound formed in the reaction between lithium and sulfur is

A. LiS

B. LiS2

C. Li2S2

D. Li2S

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Which of the following compounds is incorrectly named?

(A) P2O5 is diphosphorus pentoxide

(B) N2O5 is dinitrogen pentoxide

(C) Si3N4 is trisilicon tetranitride

(D) CO2 is carbon dioxide

(E) S2Cl2 is disulfurous dichloride

Watch Solution

Which of the following compounds is incorrectly named?

(A) Mg(OH)2 is magnesium dihydroxide

(B) CaO is calcium oxide

(C) NH4NO3 is ammonium nitrate

(D) K3PO4 is potassium phosphate

(E) MgSO3 is magnesium sulfite

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The prefix “bi” is added to anion names to indicate an extra positive hydrogen, as for example, in bicarbonate compared to carbonate. Which of the following anions would be known as biphosphate?

(A) HP-

(B) (PO4)22-

(C) HPO32-

(D) HPO42-

(E) HPO43-

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Which of the following formulas represents gallium sulfide?

(A) GaS

(B) Ga3S3

(C) Ga3S2

(D) Ga2S2

(E) Ga2S3

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What is the chemical formula of magnesium phosphate?

(A) MgP

(B) MgPO

(C) MgPO4

(D) Mg2(PO4)3

(E) Mg3(PO4)2

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What is the name given to the compound whose formula is N 3S6 (be careful!!!!!)?

(A) nitrogen sulfur

(B) trinitrogen hexasulfur

(C) trinitrogen sexasulfide

(D) trinitrogen hexasulfide

(E) hexasulfur trinitride

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The naming of polyatomic anions, while seemingly random, actually does have some rules. Two in particular concern the use of the prefix “bi” , which is used to indicate an extra positive hydrogen, and the difference between the suffices "ite" and "ate," which is based on number of oxygen atoms ("ite" means one less than "ate"). These are exemplified by the differences between carbonate and bicarbonate and sulfite and sulfate, respectively! Given this, what is the formula of biphosphite?

(A) HP-

(B) (PO4)22-

(C) HPO32-

(D) HPO42-

(E) PO33-

Watch Solution

What is the molar mass of magnesium nitrate?

(A) 38.3 g/mol

(B) 43 g/mol

(C) 74 g/mol

(D) 86.3 g/mol

(E) 148.3 g/mol

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What is the formula of aluminum sulfite?

(A) AlS

(B) AlSO3

(C) Al2(SO4)3

(D) Al2(SO3)3

(E) Al2S3

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What is the name given to the compound whose formula is S 3F6?

(A) sulfur fluorine

(B) trisodium hexafluoride

(C) trisulfur sexafluoride

(D) sulfur fluoride

(E) trisulfur hexafluoride

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What is the formula of aluminum sulfide?

(A) AlS

(B) AlSO3

(C) Al3S2

(D) Al2(SO3)3

(E) Al2S3

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What is the chemical formula of magnesium phosphate?

(A) MgP

(B) MgPO

(C) MgPO4

(D) Mg2(PO4)3

(E) Mg3(PO4)2

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The IUPAC name for Cu2O is

  1. copper oxide
  2. copper (I) oxide
  3. copper (II) oxide
  4. copper (III) oxide
  5. none of these
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The chemical formula for ammonium hydrogen phosphate is

  1. (NH4)2HPO4
  2. NH4HPO4
  3. NH4(HPO4)2
  4. NH4H2PO4
  5. None of these
Watch Solution

Name the following compounds:

a) Ca(BrO2)2            

 

b) Sr3P2

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Name the following acids:

a) HI              

b) H2SO3       

c) HClO4       

d) HBrO3      

e) H2Te

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What is the name of N 2O?

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What is the name of PCl 5

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What is the name of PbCl 4?

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What is the name of FeSO 4

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Which is the correct formula of trisulfur monophosphide?

A. S3PO4

B. (SO4)3P

C. S3P

D. (SO3)3PO4

E. None of these choices are correct.

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Which is the correct name for Na 2SO3?

A. sodium sulfate

B. sodium sulfite

C. sodium sulfide

D. sodium hydrogen carbonate

E. ammonium sulfide

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Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.

A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2 NH4C2H3O2(aq)

B) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3C2H3O2(aq)

C) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3CO3(aq)

D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq)

E) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3 NH4CO2(aq)

Watch Solution

If a formula is given, provide the name. If a name is given, provide the formula.

a. LiOH

b. Perchloric acid

c. SeF6

d. potassium permanganate

e. chromium (III) nitrate

f. tetraphosphorous decasulfide

g. VCl5

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Name the compound SCl 6.

1. sulfur(VI) chloride

2. sulfur hexachloride

3. silicon hexachloride

4. silicon chloride

5. sulfur chloride

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The correct name for CuSO4·5H2O is

A) cuprous sulfate pentahydrate

B) copper(I) sulfate pentahydrate

C) cuprous sulfate tetrahydrate

D) copper(II) sulfate tetrahydrate

E) copper(II) sulfate pentahydrate

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The name for the two compounds HBrO and Fe2(SeO3)3 are, respectively:

A) hypobromic acid, iron (III) selenite

B) hypobromous acid, iron (III) selenite

C) bromic acid, iron (II) selenite 

D) perbromic acid, iron (II) selenate

E) hypobromous acid, iron (III) selenate

Watch Solution

Give the name for PBr3.

A) phosphorus tribromide

B) potassium tribromide

C) phosphorus (III) bromide

D) phosphorus (II) bromide

E) phosphorus bromide

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Rb2S is named

A) rubidium disulfide.

B) rubidium sulfide.

C) rubidium(II) sulfide.

D) rubidium sulfur.

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Give the structure for sodium perchlorate.

A) NaClO

B) NaClO2

C) NaClO3

D) NaClO4

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Write a sentence describing this reaction using correct chemical names. Do not worry about states:

Pb(NO3)2 + Ca(OH)2 → Pb(OH)2 + Ca(NO3)2

 

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Give the formulas for the following compounds

a)  dihydrogen oxide                           _________________

b)  nickel(II) nitrate hexahydrate         ­­­­­­­­_________________

c)  sodium nitride                                _________________

d)  calcium perchlorate                       _________________

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Name the following compounds

a)  Co3(PO4)2 · 4H2O         _____________

b)  NH4Cl                          _____________

c)  Mn(OH)2                      _____________

d)  SO3                              ­­­­­­­­­­­­­­­­­­­­­­­­­­­­_____________

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What are the formulas of tetraphosphorous heptasulfide and copper(II) sulfate pentahydrate?

A. K4S7 and CuSO4 . 7 H2O

B. K4S5 and CuSO4 . 7 H2O

C. P4S7 and CuSO4 . 5 H2O

D. P4S5 and CuSO4 . 5 H2O

E. none of these

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Which set of the statements below includes only the correct names and formulas?

i) Barium oxide has the formula BaO2

ii) CrCO3 is chromium(II) carbonate

iii) Magnesium sulfite has the formula MnSO3

A. ii) only

B. i) only

C. i) and ii) only

D. iii) only

E. i) and iii) only

Watch Solution

Give the formulas or names for the following compounds:

sodium nitrate          ___________  CaSO 4    ___________________________
sulfur hexaflouride   ___________  NH4NO3  ___________________________
sodium chlorate       ___________  K2HPO4  ___________________________

Watch Solution

How many hydrogen atoms appear in the formula of ammonium sulfate?

1. 6 atoms

2. 10 atoms

3. 4 atoms

4. 2 atoms

5. 8 atoms 

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What is the correct name for SO2?

1. sodium dioxide

2. sulfur dioxide 

3. sulfur oxide

4. sodium oxide

5. silicon oxide

6. silicon dioxide

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Write the formula for Cadmium sulfide (yellow paint)  

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Write the formula of ammonium chloride.

 

Write the formula of iron (II) perchlorate.

 

What is the name of Sn(SO 4)2?

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Write a  balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.

a. H2SO4 (aq) + LiOH (aq) → H2O (l) + Li 2SO4 (aq)

b. H2SO3 (aq) + 2 LiOH (aq) → 2 H 2O (l) + Li2SO3 (aq)

c. HSO3 (aq) + LiOH (aq) → H 2O (l) + LiSO3 (aq)

d. HSO4 (aq) + LiOH (aq) → H 2O (l) + LiSO4 (aq)

e. H2S (aq) + 2 LiOH (aq) → 2 H 2O (l) + Li 2S (aq)

 

Watch Solution

Write the formula for barium nitrite.

a. Ba3N2

b. BaNO3

c. BN

d. Ba(NO2)2

e. B(NO2)3

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Which acid/name pair is NOT correct?

a. HBr, hydrobromic acid

b. H2CrO4, chromic acid

c. H3PO4, hydrophosphoric acid

d. HCl, hydrochloric acid

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Determine the name for P4O10.

a. phosphorus (IV) oxide

b. diphosphorus pentoxide

c. phosphorus oxide

d. phosphorus (II) oxide

e. tetraphosphorus decoxide

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What is the chemical formula for a compound containing strontium ions and perchlorate?

a. SrClO4

b. SrCl2

c. Sr(ClO3)2

d. Sr(ClO4)2

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Which of the following is the best representation of the compound magnesium nitride?

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Which of the following is the correct formula for sodium hypochlorite?

1. NaClO2

2. NaClO3

3. NaCl

4. NaClO

5. NaClO4

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What is the correct name for (NH 4)2CO3?

1. ammonium carboxide

2. ammonium bicarbonate

3. ammonium carbonate 

4. biammonium carbonate

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Give the formula for aluminum hydroxide.

1. AlH3

2. AlOH3

3. Al(OH)3

4. AlOH 

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Provide the missing information.

Formula                       Name

CuCl2                           _________________________

 

______                        nitrous acid

 

NF3                                 _________________________

 

Watch Solution

The correct name for the ClO3- ion is

a) perchlorate ion

b) hypochlorite ion

c) chlorite ion

d) chlorate ion

e) chlorine trioxide ion

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What are the names of acids HNO 3 and HI?
A. nitric acid and hydroiodic acid
B. hydronitric acid and hydroiodic acid
C. hydrogen nitrate and hydrogen iodide
D. nitric acid and hdrogen iodide

Watch Solution

Give the systematic name for Cr3P2 and the chemical formula for calcium nitrate.

A. chromium phosphide and CaN  2
B. chromium (II) phosphide and Ca(NO 32
C. chromous disphosphide and CaNO 3
D. chromium (II) phosphide and Ca 23

Watch Solution

What is the formula for the ionic compound formed between sodium and nitrogen?

A) NaN               

B) NaN2             

C) Na3N         

D) Na3N2          

E) NaN3

 

Watch Solution

What is the chemical formula of sodium perchlorate?

A) NaClO          

B) NaClO2         

C) NaClO3         

D) NaClO4          

E) NaMnO4

Watch Solution

What is the name for SnO?

A) tin (I) oxide    

B) tin (II) oxide    

C) tin oxide          

D) tin (IV) oxide  

E) tin monoxide

Watch Solution

What is the name for SO3?

A) sulfite

B) sulfur (VI) oxide

C) sulfur trioxide

D) sulfur (III) oxide

E) sulfur oxide

Watch Solution

Determine the name for TiCO3.

A) titanium carbonite

B) titanium (II) carbonite

C) titanium (I) carbonate

D) titanium carbide

E) titanium (II) carbonate

Watch Solution

Write the formula for barium nitrite.

A) Ba3N2

B) B(NO2)3

C) BaNO3

D) Ba(NO2)2

E) BN

Watch Solution

Write the formula for strontium nitride.

A) Sr(NO3)2

B) SrN

C) Sr2N3

D) Sr(NO2)2

E) Sr3N2

Watch Solution

Determine the name for P4O10.

A) phophorus oxide

B) tetraphophorus decaoxide

C) diphosphorus pentaoxide

D) phosphorus (IV) oxide

E) phosphorus (II) oxide

Watch Solution

Write the name for Sn(SO 4)2.

A) tin (II) sulfite

B) tin (I) sulfite

C) tin (I) sulfate

D) tin (IV) sulfate

E) tin sulfide

Watch Solution

Write the name for Ca 3(PO4)2.

A) tricalcium phosphorustetraoxide

B) calcium (II) phosphite

C) calcium phosphite

D) calcium (III) phosphite

E) calcium phosphate

Watch Solution

Write the formula for the compound formed between potassium and sulfur.

A) KS

B) K3S2

C) K2SO3

D) KS2

E) K2S

Watch Solution

Which of the following formula/name pairs is incorrect?               

A)  FeO  iron(II) oxide

B)  K2SO4   potassium sulfide

C)  MnO2  manganese(IV) oxide

D)  LiOH  lithium hydroxide

E)  MgO  magnesium oxide

Watch Solution

Write the balanced chemical equations.

Nitric acid forms when gaseous nitrogen dioxide reacts with gaseous oxygen and liquid water.

Watch Solution

Name the Ionic Compounds

1. KMnO4
2. Sn(SO4)2
3. CuSO4 • 5H2O
4. CH3COONa

Watch Solution

Write the name for Sr 3(PO4)2.
A) strontium (III) phosphite
B) strontium (II) phosphite
C) strontium phosphate
D) tristrontium phosphorustetraoxide
E) strontium phosphite

Watch Solution

Which name for the corresponding chemical formula is  INCORRECT?   

A) BBr3:  boron tribromide

B) FeCl3: iron (III) chloride

C) MgS: magnesium sulfide

D) Li2O: lithium oxide

E) PCl5:  phosphorus(V) pentachloride

Watch Solution

Determine the name for Cl2O.

a. chlorine oxide

b. dichlorine monoxide

c. chlorine (I) oxide

d. chlorine (II) oxide

e. chlorate

Watch Solution

Which of the following statements is/are correct?

i. Ca(CIO2)2 is the symbol for calcium chlorite
ii. VF5 would be called vanadium pentaflouride
iii. Sodium phosphide would be symbolized as Na3PO3

A. i only
B. iii only
C. i and iii
D. ii and iii
E. i, ii and iii

Watch Solution

Which of the following statements is correct.

i. The formula for hydrosulfurous acid is H2SO3
ii. The correct name for HBrO3 is bromic acid
iii. The symbol for hypobromous acid is HBrO

a. i only
b. ii only
c. iii only
d. i and ii
e. ii and iii

Watch Solution

Sulfurous acid is:

a. H2S

b. H2SO2

c. H2SO4

d. H2SO3

e. HSO3

Watch Solution

SeO42- is the  selenate ion, so the correct nomenclature for H 2SeO3 is

a. hydroselenic acid

b. selenic acid

c. selenous acid

d. hydroselenous acid

e. hyposelenous acid

Watch Solution

Which of the following statements is/are true?

i. The correct name for Cl2O6 is chlorine hexoxide

ii. The correct formula for tetraboron decahyride is B4H10.

iii. The correct name for CF4  is monocarbon tetrafluoride.

a. i only

b. ii only

c. iii only

d. i and ii

e. i and iii

Watch Solution

Determine the names for I2F7 and HNO2

a. iodine heptoxide and nitrous acid

b. iodine fluoride and nitric acid

c. diiodine heptafluoride and nitrous acid

d. heptafluoroidic acid and hydrogen (I) nitrite.

e. diiodoheptafluorodine and nitric acid

Watch Solution

Give the systematic  name for Co3N2 and the chemical formula for potassium carbonate.

a. cobalt (III) nitrade and K(CO3)2

b. cobalt (II) nitride and K2CO3

c. cobaltic dinitride and KCO3

d. cobalt (II) nitrogide and K2C3

Watch Solution

The most commercially important form of vanadium is the compound of vanadium (V) oxide, which is used as a catalyst in the production of sulfuric acid. What is the chemical formula for this compound?

a. VO5

b. 5VO

c.V5O2

d. V2O5

Watch Solution

Consider the chemical reaction: 2 SO2 (g) → SO(g) + SO3 (g)

Determine if the sentence below is true or false

The name of SO is sulfur oxide.

Watch Solution

Which of the following diagrams is the most accurate representation of MgCl(aq)?

Watch Solution

The formula for dinitrogen trioxide is

a) (NO3)2.

b) N(OH)3.

c) N2O3.

d) N3O2.

Watch Solution

The name for KHCO3 is

a) calcium carbonate.

b) potassium hydrogen carbonate.

c) calcium hydrogen carbon trioxide.

d) potassium carbonate.

e) calcium bicarbonate.

Watch Solution

Name the following compounds:

1. CaF2 ______________________________

2. CoF2 ______________________________

3. BF3 ______________________________

Watch Solution

Neodymium chromate is Nd2(CrO4)3. What are the formulas of neodymium nitrate and neodymium phosphate?

A. Nd(NO3)3, Nd3(PO4)2

B. Nd(NO3)3, Nd3PO4

C. Nd3(NO3)2, NdPO4

D. Nd2(NO3)3, Nd2(PO4)3

E. Nd(NO3)3, NdPO4

Watch Solution

Write the formulas for the following compounds

a) ammonium sulfate:

 

b) calcium hypobromite:

 

c) magnesium hydroxide:

 

d) aluminum phosphate:

 

e) hydroiodic acid:

 

Watch Solution

For each of the following equations, write the chemical formulas and balance the equation. Try to indicate all the physical states (solid, liquid, gas) as well.

a) potassium + water → potassium hydroxide + hydrogen

 

 

b) potassium hydride + water → potassium hydroxide + hydrogen

 

 

c) silicon dioxide + carbon → silicon carbide + carbon monoxide

 

 

d) silicon dioxide + hydrogen fluoride → silicon tetrafluoride + water

 

 

e) phosphorus + chlorine → phosphorous tetrachloride

Watch Solution

Name the following compounds: 

Cl2O7 _______________________________________________________________

Co(NO2)3 • 4H2O _______________________________________________________________

Mg(HCO3)2 _______________________________________________________________

 

Write formulas for the following compounds:

chromium(III) hypobromite ________________________________________________________

sulfurous acid ________________________________________________________ 

 

Watch Solution

For each of the items written below, state why it is wrong and write a version that is correct. 

Iron Chloride

What’s wrong? 

Write a correct version

 

Watch Solution

Write the formula for the compound expected to form between barium and nitrogen.

Watch Solution

Provide the name for this given compound :

Mg3(PO4)2

(a) mercury(III) diphosphate

(b) magnesium phosphate

(c) magnesium(II) perphosphate

(d) manganese phosphide

(e) manganese(II) phosphate

Watch Solution

Name the compound K2SO3

a) potassium sulfate

b) dipotassium sulfate

c) dipotassium sulfite

d) potassium sulfite

e) potassium persulfate

Watch Solution

What would be the correct formula for an ionic compound that combines calcium and sulfate?

A. CaS            B. Ca 2S2            C. Ca(SO 4)2            D. CaSO 4            E. CaSO 8

Watch Solution

All but one of the following compounds is named incorrectly. Which of the following statements is correctly named?

1. Iron (III) nitrate is Fe(NO3)3

2. Manganese sulfate is MnSO3

3. Bromic acid is HBrO

4. Lithium phosphide is Li3PO4

Watch Solution

Which of the following compounds is incorrectly named?

1. Iron (III) carbonate       Fe 2(CO3)3

2. Sodium sulfite             Na  2SO4

3. Dinitrogen tetroxide       N 2O4

4. Aluminum phosphide         AlP

Watch Solution

What is the formula of titanium (II) phosphate?

1. Ti2PO4            2. Ti 3(PO4)2            3. TiPO3            4. Ti2(PO4)3

Watch Solution

The formula of sodium vanadate is Na 3VO4. What is the formula of calcium vanadate?

A. CaVO4            

B. Ca(VO4)2            

C. Ca(VO4)3

D. Ca3(VO4)2            

E. Ca 2VO4

Watch Solution

What is the formula of lead (II) nitrite?

A. Pb3N2

B. Pb(NO3)2

C. Pb2NO3

D. Pb(NO2)2

E. Pb2N3

Watch Solution

Which of the following formulas is incorrect?

1. K2O            

2. Al 2S3            

3. MgO            

4. BaF

Watch Solution

The formula for arsenous acid is:

a) H2AsO3

b) H3AsO2

c) H2AsO4

d) H3AsO4

e) H3AsO3

Watch Solution

Which of the following formulas is incorrect?

A. Ba3P2          

B. SrCO 3          

C. Cs 3N

D. CaBr            

E. Li  2SO3

Watch Solution

What is the name of the following polyatomic ion, BrO 3 ?

a) Bromate

b) Bromide

c) Perbromate

d) Hypobromite

 

Based on the previous question, the compound HBrO 3 is correctly named as:

a) Hydrobromic acid

b) Bromous acid

c) Bromic acid

d) Perbromic acid

Watch Solution

What is the name of the following polyatomic ion, ClO ?

a) Chloride           b) Perchlorate           c) Chlorate           d) Hypochlorite

 

 

Based on the previous question, the compound HClO is correctly named as:

 

a) Hydrochloric acid           b) Chloro-oxyacid           c) Hypochlorous acid           d) Chloric acid

Watch Solution

Determine the names for N2O5 and HNO3

A. nitrogen pentoxide and nitrous acid

B. nitrogen oxide and nitric acid

C. nitrogen (IV) oxide and hydronitrous acid

D. nitrogen (II) oxide and hydrogen (I) nitrate

E. dinitrogen pentoxide and nitric acid

Watch Solution

Give the systematic name for Fe3P2 and the chemical formula for calcium nitrate.

A. iron (II) phosphide and CaN2

B. iron (II) phosphide and Ca(NO3)2

C. ferrous diphosphide and CaNO3

D. iron (II) phosphide and Ca2N3

Watch Solution

Give the systematic name for Fe3P2 and the chemical formula for calcium nitrate.

A. iron (II) phosphide and CaN2

B. iron (II) phosphide and Ca(NO3)2

C. ferrous diphosphide and CaNO3

D. iron (II) phosphide and Ca2N3

Watch Solution

As a transition metal, osmium can exhibit many different charges, but one of the most highly charged is found in osmium (VIII) oxide. What is the chemical formula for this compound?

A. Os8O

b. OsO4

c. OsO8

D. OsO2

Watch Solution

Name the compound K2SO3

 

a. potassium sulfate

b. dipotassium sulfate

c. dipotassium sulfite

d. potassium sulfite

e. potassium persulfate

Watch Solution

In K2O2, the oxygen is called a

a. dioxide

b. oxide

c. peroxide

d. peroxite

e. superoxide

Watch Solution

Name the compound N2O5

a. nitrogen oxide

b. nitrogen pentoxide

c. dinitrogen pentoxide

d. nitrogen (5) oxide

e. nitrogen (V) pentoxide

Watch Solution

Name the following compounds:

1. Cr(BrO)3

 

2. Ba(IO4)2

 

3. NH4C2H3O2

Watch Solution

Give formulas for the following compounds:

 

1. nickel(II) nitrite tetrahydrate:

 

2. barium hydrogen sulfate:

 

3. arsenic pentafluoride:

Watch Solution

Given that the ion is named sulfate, we can infer that the ion would be named selenate.

 

Name the following compounds containing the selenate ion:

Cr2(SeO4)3:

MgSeO4 • 4H2O:

 

Name the following ions:

SeO32-:  

HSeO4- :

Watch Solution

What is the correct name for FeCl3?

a) iron(III) chloride

b) iron trichloride

c) ferrum trichloride

d) ferric trichloride

e) iron chloride

Watch Solution

Which one of the formula-name combinations is not correct?

a) sulfur monoxide: SO

b) sulfur dioxide: SO2

c) sulfur trioxide: SO3

d) disulfur monoxide: S2O

e) heptasulfur oxide: S6O

Watch Solution