概要信息：

1 CLYau 2005.02.07 
Chemical Nomenclature: A Tutorial 
Rules & Drills with Answers 
 
Table of Contents 
 
Unit I: Chemical Symbols of Some Common Elements (Drill A)………………………2 
Unit II: Nomenclature of Pure Elements (Drill B)……………………………………… 4 
Unit III: Nomenclature of Monatomic Ions (Simple Ions) …………………………….. 5 
    Unit IIIA: Nomenclature of Monatomic Anions ……………………………………..5 
    Unit IIIB: Nomenclature of Monatomic Cations of Fixed Charges ………………….6 
    Unit IIIC: Nomenclature of Monatomic Cations of Variable Charges (Drill C)…….. 6 
Unit IV: Nomenclature of Ionic Compounds of Monatomic Ions ……………………... 7 
    Unit IVA: Writing Formulas from a Given Name (Drill D)…………………………. 8 
    Unit IVB: Writing Names from a Given Formula (Drills E thru H)………………….9 
Unit V: Nomenclature of Polyatomic Ions …………………………………………….11 
    Unit VA: The "Basic Eight" Polyatomic Ions (Drills I-1 thru I-4)…………………. 11 
    Unit VB: Polyatomic Ions with "- ite" Ending ……………………………………...14 
    Unit VC: Nomenclature of "- ate" and "- ite" Compounds (Drill I-5)……………… 14 
    Unit VD: Nomenclature of Oxohaloanions (Drills J & K)…………………………. 15 
Unit VI: Nomenclature of Acids (Drill L)……………………………………………...17 
Unit VII: Nomenclature of Acid Anions (Drill M)……………………………………. 20 
Unit VIII: Nomenclature of Other Common Polyatomic Ions (Drill N)……………….22 
Unit IX: Nomenclature of Molecular Binary Compounds (Drill O & P)……………... 23 
Unit X:  Nomenclature of Hydrates (Drill Q)…….…………………………………… 24 
 
Answers to Drill A…………………………………………………………………. 26 
Answers to Drill B…………………………………………………………………. 26 
Answers to Drill C…………………………………………………………………. 26 
Answers to Drill D………………………………………………………………… 27 
Answers to Drill E…………………………………………………………………. 27 
Answers to Drill F…………………………………………………………………. 27 
Answers to Drill G…………………………………………………………………. 28 
Answers to Drill H………………………………………………………………… 28 
Answers to Drill I-1, I-2, I-3………………………………………………………. 29 
Answers to Drill I-4, I-5…………………………………………………………… 30 
Answers to Drill J………………………………………………………………….. 31 
Answers to Drill K………………………………………………………………… 31 
Answers to Drill L………………………………………………………………..... 32 
Answers to Drill M………………………………………………………………… 33 
Answers to Drill N………………………………………………………………… 34 
Answers to Drill O………………………………………………………………… 34 
Answers to Drill P………………………………………………………………..... 34 
Answers to Drill Q……………………………………………………………..… 35 
 
 
 2 CLYau 2005.02.07 
Chemical Nomenclature: A Tutorial 
Rules & Drills with Answers 
 
For beginning students, the study of nomenclature (system of naming chemicals) can seem 
impossibly complex.  For that reason, the rules and drills presented here are broken down into 
Units, and it is not advisable to study all the units at one sitting, but you should take it one unit at 
a time.  If you are not able to spread out your work over several days, you should at least take a 
break in between units. 
 
Unit I: Chemical Symbols of Some Common Elements 
You must first learn the symbols of some common elements.  Your instructor may have 
different requirements on which elements you must learn.  The ones listed below are the one you 
have to know to make use of this tutorial, and most likely they are the only ones you will ever 
have to know even as you move on to more advanced courses.  You might want to put them on 
flash cards.  You should drill yourself one way or another before you proceed to the next unit. 
Notice that the elements below are boxed together in groups, some elements appearing in 
more than one group.  My suggestion is you learn them in groups, in this order: Elements #1 
through 18, Group IA, IIA, VIIA, VIIIA, Common Transition Elements, and finally, Other 
Common Elements.  If you have trouble with spelling, you’ll find it easier to learn correct 
spelling if you copy the names several times as you sound it out.  If you think this is too much 
work, then you are taking the wrong course.  Studying chemistry takes work, regardless of how 
smart you are. 
 
COMMON ELEMENTS: NAMES AND SYMBOLS 
Learn the names (with correct spelling) and symbols of the elements listed below (no need to 
memorize numbers).  Note that the symbols are capitalized.  If the symbol consists of two letters, 
only the first letter is capitalized. 
Elements # 1 - 18 Group IA Group VIIA 
   
H hydrogen H hydrogen H hydrogen 
He helium Li lithium F fluorine 
Li lithium Na sodium Cl chlorine 
Be beryllium K potassium Br bromine 
B boron Rb rubidium I iodine 
C carbon Cs cesium  
N nitrogen Fr francium  
O oxygen   
F fluorine Group IIA Group VIIIA 
Ne neon   
Na sodium Be beryllium He helium 
Mg magnesium Mg magnesium Ne neon 
Al aluminum Ca calcium Ar argon 
Si silicon Sr strontium Kr krypton 
P phosphorus Ba barium Xe xenon 
S sulfur Ra radium Rn radon 
Cl chlorine   
Ar argon   
 3 CLYau 2005.02.07 
 
Common Transition Other Common Elements 
   
Ti titanium  As arsenic Se selenium 
Cr chromium Sn tin Sb antimony Te tellurium 
Mn manganese Pb lead Bi bismuth  
Fe iron    
Co cobalt U uranium   
Ni nickel Pu plutonium   
Cu copper   
Zn zinc    
    
Pt platinum    
Ag silver    
Au gold    
Cd cadmium    
Hg mercury    
 
Drill A: Nomenclature of Elements 
This is a self-test, since you can easily look up answers yourself.  Take this as a practice test, 
after you have drilled yourself on the symbols and spelling of the elements listed above. 
 
Name Symbol  Symbol Name 
          
chlorine   S  
calcium   K  
arsenic   Fe  
mercury   Na  
copper   P  
  
Remember not to proceed to the next unit until you have studied Unit I.     
 
****************************************************************************** 
 4 CLYau 2005.02.07 
Unit II: Nomenclature of Pure Elements 
 
The term, “Pure Elements”, refers to elements when they are not combined with other 
elements such as in compounds.  Certain pure elements exist in clusters, joined by covalent 
bonds, called molecules.   For example, pure nitrogen exists as N2 rather than N.  When 
nitrogen is not part of a compound, it is also referred to as “free nitrogen” or “nitrogen in 
its elemental state”.   
 
Formulas of Pure Elements  
 
Diatomic molecules:   H2 
 N2 O2 F2 
   Cl2 
   Br2 
   I2 
 
Other molecular 
elements: P4 S8 
 
Monatomic elements: with a few exceptions, all others are monatomic (e.g. He, Ne, Fe, Al 
are monatomic). 
 
Exceptions:  Elemental oxygen also exists in a less stable form as O3 (ozone). 
 Although we usually write C for pure carbon, it usually exists as an extended 
network of various types.  Refer to your textbook if you are interested in these 
various allotropes of carbon.  We will simply write C as if it were monatomic. 
  
 
Physical States of Pure Elements 
 
gases:   H2 He 
 N2 O2 F2 Ne 
   Cl2 Ar 
    Kr 
    Xe 
    Rn 
 
liquids:  Br2  and  Hg 
 
solids:   with a few exceptions, all others are solids (e.g. K, Fe, Co, Sn, U are solids.) 
 
 5 CLYau 2005.02.07 
Drill B: Formulas and Physical States of Pure Elements 
 To make the best use of the drills in this tutorial, you should first study and memorize 
the above rules on the formulas and physical states of pure elements. Then write down the 
answers to the drill (rather than keeping them in your head).  Answers are provided in a later 
part of this exercise, but do not check your answers until you have written down your answers to 
the entire drill.  This takes discipline, but it would do you no good to flip to the answers without 
having put thought and time in working out the answers first. 
Using only a periodic table, give the formulas and physical states of the elements specified.  
Specify the physical states with (g), (l) or (s).  Example:  fluorine = F2 (g) 
chlorine   bromine   sulfur  
argon   phosphorus   lead  
nitrogen   krypton   element 
#112
 
chromiu
m
  mercury   gold  
strontium   iodine   hydrogen  
 
****************************************************************************** 
 
Unit III: Nomenclature of Monatomic Ions (Simple Ions) 
 
     “Simple Ions” refer to ions that are charged atoms, as opposed to charged molecules.  They 
are therefore also known as monatomic ions.   
 
Unit IIIA: Nomenclature of Monatomic Anions 
 
     A negatively charged ion is known as an “anion”.  Its name ends with –ide.  For example, the 
chlorine ion is named chloride, and the phosphorus ion is named phosphide.  The charge of a 
monatomic anion can be determined by its Group number in the periodic table.  An anion in 
Group VIIA has a charge of 1−.  An anion in Group VIA has a charge of 2−, etc.  See Table 
below. 
 
NAMES OF MONATOMIC ANIONS (SIMPLE ANIONS) 
IVA VA VIA VIIA
   H− hydride 
C4−    carbide N3− nitride O2− oxide F− fluoride 
 P3− phosphide S2− sulfide Cl− chloride 
 As3− arsenide Se2− selenide Br− bromide 
  Te2− telluride I− iodide 
 
 6 CLYau 2005.02.07 
 
Unit IIIB:  Nomenclature of Monatomic Cations of Fixed Charges 
 
     A positively charged ion is known as a cation.  Cations in Group IA, IIA and aluminum have 
fixed charges (i.e. nonvariable charges).  Those in Group IA always have a charge of 1+, and 
those in Group IIA, a charge of 2+.  The aluminum ion always has a charge of 3+.  The name of 
a monatomic cation of fixed charge is merely the name of the element followed by the word 
“ion”.  Thus Na+ is “sodium ion”.  It is not necessary to specify the charge since it is 
nonvariable.  There are a few other cations that also fall in this category, but we will keep it 
simple for now and stick with just Groups IA, IIA and aluminum. 
 
NAMES OF MONATOMIC CATIONS (SIMPLE CATIONS) 
IA IIA IIIA 
H+ hydrogen ion   
Li+ lithium ion Be2+ beryllium ion  
Na+ sodium ion Mg2+ magnesium ion Al3+ aluminum ion 
K+ potassium ion Ca2+ calcium ion  
Rb+ rubidium ion Sr2+ strontium ion  
Cs+ cesium ion Ba2+ barium ion  
Fr+ francium ion Ra2+ radium ion  
 
Unit IIIC: Nomenclature of Monatomic Cations of Variable Charges 
 
Cations not named above are assumed to be of variable charges.  For example iron can exist with 
various charges, the most common of which are in the form of Fe2+ and Fe3+.  Their names 
must therefore specify the charges.  This is done by following the name of the element with the 
charge in Roman numerals, within parentheses.  Fe2+ is named iron(II) ion, and Fe3+ is named 
iron(III) ion.  Tin(IV) ion refers to Sn4+.  Names based on this system of nomenclature are 
known as “Stock names”. 
 
Many of these ions have “common names”.  Of the two most common ions, the one with the 
lower charge has the ending –ous, and that with the higher charge has the ending −ic.  Thus Fe2+ 
has the common name, of ferrous ion.  Fe3+ has the common name of ferric ion.  Since some of 
these names are indeed quite commonly used (as in food labels), it would be wise to learn at least 
the four common names included in the table below. 
 
Formula Stock Name Common Name 
Fe2+ iron(II) ion ferrous ion 
Fe3+ iron(III) ion ferric ion 
Cu+ copper(I) ion cuprous ion 
Cu2+ copper(II) ion cupric ion 
 
 7 CLYau 2005.02.07 
Since the ending in the common name specifies the charge, it would be redundant (therefore 
wrong) to also include the Roman numeral.  Thus Cu+ should not be named as cuprous(I) ion.  
Incidentally, the ending –ous does not indicate the charge is 1+, nor 2+.  The –ous ending 
indicates the lower charge of the two most common charges.  In the case of iron, the two 
common charges are 2+ and 3+, so the lower charge would be 2+.  Thus ferrous refer to Fe2+ 
rather than Fe3+. 
 
Note:  Dr. Yau will not require you to learn the common names. (You do need to know that Fe2+ 
is iron(II), but you do not need to know whether it is ferrous or ferric.)  Check with your own 
instructor whether that is so in your class. 
 
Drill C: Nomenclature of Monatomic Ions 
Again, study the rules before taking this as a practice test.  Write down your answers and 
compare them with the answers provided only after you have finished the entire drill.  You may 
use only a periodic table. 
FORMULA NAME NAME FORMULA
Rb+  nitride
Ba2+  iodide
P3–  oxide
Br –  chromium(III) 
N3–  potassium ion
S2–  aluminum ion
V3+  magnesium
Cu2+  iron(II) ion
Ca  copper(I) ion
 
************************************************************************ 
Unit IV:  Nomenclature of Ionic Compounds of Monatomic Ions 
 
An ionic compound is generally made of one type of cation combined with one type of anion.  
The formula has no net charge even though the ions themselves are charged.  Thus, the number 
of cations and the number of anions present must reflect a net charge of zero.  These numbers 
appear as subscripts, immediately following each element. 
 
For example, Na+ combines with Cl− to form NaCl (net charge of zero, so no charges are 
shown).  When Na+ combines with O2−, however, you will need two Na+ to neutralize the 
charge of 2− on the oxygen, to give Na2O.  When Mg2+ combines with Cl−, you will similarly 
need two Cl– to neutralize the charge of 2+ on the magnesium, to give MgCl2.  Note that the 
subscript 2 refers only to the number of Cl, and not the number of Mg.  When no subscript 
shows, it is assumed to be one.  Thus, the formula MgCl2 tells us that there is one Mg ion for 
every two Cl ions.  The subscripts show us the simplest ratio of cation to anion.  (It would be 
wrong to write Mg2Cl4 because 2:4 can be reduced to 1:2.) 
 
 8 CLYau 2005.02.07 
When you combine Al3+ with O2−, in order to come up with a net charge of zero, you would 
need two Al3+ and three O2−, to give Al2O3.  You can arrive at this answer by simply thinking 
about how the charges must work out, or use the Cross Over Method. 
 Al   3+
 O       2− 
 
 
 
        Al  2    O    3 
 
The Cross Over Method is merely a fast way to figure out how to make the net charge come out 
zero.  It does not mean that Al now becomes 2− and oxygen now becomes 3+.  Note also that in 
the Cross Over Method, the signs (charges) do not cross over (i.e. charges do not appear in the 
subscript.)   Note also that in this method, you must always check that the subscripts are always 
reduced to the simplest ratio. 
 
 Mg   2+
 O       2− 
 
 
 
        Mg  2    O    2       = MgO, not Mg2O2 ! 
 
Even though there are ions (and charges) present in the compound, we do not show the charges 
in these formulas.  It would be improper to write Al3+
2O2−
3  or Mg2+O2−, unless you needed to 
stress the charges for a special reason. 
 
Unit IVA: Writing Formulas from a Given Name 
 
First figure out the charges of the cation and the anion by examining the name. Then combine the 
ions in a ratio that gives you a net charge of zero as described above.  If you have trouble 
deciding what the charges are on the ions, you need to review Unit III !  You should be able to do 
the drill without using anything but a periodic table. 
For example, given the name, tin(II) oxide, you know that the ions are Sn2+ and O2−. 
To write the formula for the compound with Sn2+ and O2−, you examine the charges and can see 
that it will take one Sn2+ and one O2− to form a neutral compound. 
Let’s look at another example.  Given the name, tin(IV) oxide, you know that the ions are Sn4+ 
and O2−.  In order to form a neutral compound, we must have one Sn4+ and two O2−.   The 
formula must therefore be SnO2. 
Now try out the Drill D. 
 9 CLYau 2005.02.07 
Drill D: Formulas of Ionic Compounds of Monatomic ions 
 
NAME FORMULA 
magnesium fluoride  
lithium sulfide  
calcium selenide  
nickel(II) fluoride  
copper(II) bromide  
chromium(III) sulfide  
tin(II) phosphide  
 
--------------------------------------------------------------------------------------------------------- 
Unit IVB: Writing Names from a Given Formula 
 Examine the formula.  If the cation belongs in the group that has fixed charges, then you just 
name the cation, followed by the anion, but drop the word “ion” that comes in between.  For 
example NaCl is sodium chloride, and not sodium ion chloride.  MgCl2 is magnesium chloride. 
 
Drill E: Writing Names of Compounds with Cations of Fixed Charges 
 
KBr  
Li2O  
Mg3As2  
Na3P  
   
 If the cation belongs in the group that has variable charges, you must figure out what that 
charge is from the charge of the anion (which is always fixed).  Do not use the Cross Over 
Method as it may lead to the wrong answer.  For example, the formula SnO tells us that Sn must 
have a charge of 2+ since the oxygen ion is always 2−.  If you used the Cross Over Method, you 
would have erroneously come up with Sn having 1+ charge.  The Cross Over Method may seem 
to work, but it works only in some and not all cases.  So, it would be wiser not to use it at all for 
going backwards (from formula to name). 
 
 Remember that the charge is per ion.  Thus Cu2S tells us that Cu had a charge of 1+, not 2+.  
Since the S ion is always 2− (Group VIA), the two Cu must have a total charge of 2+.  Thus 
each Cu must have 1+. 
 
 10 CLYau 2005.02.07 
Drill F: Determining the Charge and Name of the Cation First, Then Name of Compound 
 
Formula Charge of 
Cation Name of Cation Name of Compound 
MnO2    
PbS    
Cr2O3    
Rb2Se    
CuCl2    
CuO    
Cu2O    
 
Check your answers to the above drill before going on.  If you have made any mistakes be sure 
you find out why before you continue to the next drill.  If necessary you should review all the 
previous Units. 
 
Drill G: Nomenclature of Ionic Compounds of Monatomic Ions (Both Fixed & Variable 
Charges) 
 
FORMULA NAME  FORMULA NAME 
 sodium oxide  RbBr  
 magnesium nitride  FeBr2  
 copper(I) sulfide  PbS  
 manganese(II) iodide  BaO  
 iron(III) phosphide  K2O  
 copper(I) oxide  SbBr3  
 tin(II) nitride  Fe3P2  
 strontium oxide  Li2Se  
 tin(IV) oxide  CuCl2  
    
  
 11 CLYau 2005.02.07 
Check your answers to the above drill before going on.  If you have made any mistakes be sure 
you find out why before you continue to the next drill.  If necessary you should review all the 
previous Units. 
 
Extra Drill H: Nomenclature of Ionic Compounds of Monatomic Ions (Both Fixed & 
Variable Charges) 
 
FORMULA NAME 
RaCl2  
BiCl3  
Fe203  
CdBr2  
MnO  
MnO2  
 
 
Unit V: Nomenclature of Polyatomic Ions 
 
Unit VA: The “Basic Eight” Polyatomic Ions 
 
In this unit you are asked to memorize the names and formulas of 8 polyatomic ions, to start 
with.  You will be asked to learn more later on.  “Learning” means memorizing the correct 
spelling of the name, the correct subscript(s) and charge of each ion. 
 
1+ 1− 2− 3− 
NH4
+ 
ammonium 
C2H3O2
− 
acetate* 
CO3
2− 
carbonate 
PO4
3− 
phosphate 
 NO3
− 
nitrate 
SO4
2− 
sulfate 
 
 OH− 
hydroxide 
  
 ClO3
− 
chlorate 
  
    *acetate is also written as CH3CO2
− 
In memorization, it helps to look for patterns.  Note that all but two of the ions have the ending 
“−ate”.  For the ions with a charge of 1−, look up where the first element of each ion is located 
on the period table (C, N, O, Cl).  Study the formulas and names of this group of ions before 
 12 CLYau 2005.02.07 
moving on to ions with a charge of 2−.  Again look up the location of the first element of each 
ion in the periodic table (C and S).  Study these two names and formulas, and finally move to the 
ion with a charge of 3−.  Look up the position of P in the periodic table.  After you have studied 
each group based on charges, put them on flash cards and test yourself over and over. 
 
Drill I - 1: Nomenclature of the "Basic Eight" Polyatomic Ions  
   
NAME FORMULA FORMULA NAME 
sulfate  OH−  
acetate  SO4
2−  
chlorate  NH4
+  
ammonium  NO3
−  
phosphate  ClO3
−  
carbonate  PO4
3−  
hydroxide  CO3
2−  
nitrate  C2H3O2
−  
 
Drill I - 2: Nomenclature of Compounds of the "Basic Eight" Polyatomic Ions With 
Cations of Fixed Charges:  
   
NAME FORMULA FORMULA NAME 
sodium carbonate  K3PO4  
strontium carbonate  Ca(NO3)2  
aluminum sulfate  (NH4)2SO4  
ammonium phosphate  Al(OH)3  
aluminum chlorate  LiC2H3O2  
potassium sulfate  MgCO3  
calcium acetate  Ba(ClO3)2  
 
 
 13 CLYau 2005.02.07 
Drill I - 3: Nomenclature of Compounds of the "Basic Eight" Polyatomic Ions With 
Cations of Variable Charges:    
 
NAME FORMULA FORMULA NAME 
iron(II) carbonate  Cu2CO3 
 
iron(III) carbonate  CuCO3 
 
copper(I) sulfate  SnSO4 
 
cobalt(II) phosphate  Fe3(PO4)2 
 
chromium(III) chlorate  Hg(C2H3O2)2  
tin(IV) sulfate  BiPO4  
antimony(III) acetate  Mn(ClO3)2  
 
 
Drill I - 4: Compounds of the "Basic Eight" Polyatomic Ions and –ide ions With Cations of 
Both Fixed and Variable Charges: (This helps you learn to distinguish between those that 
require Roman numerals and those that do not.)  
   
NAME FORMULA FORMULA NAME 
calcium phosphate  Na3N  
chromium(III) sulfide  NaNO3 
 
potassium carbonate  K2SO4 
 
magnesium acetate  CdCO3 
 
chromium(III) hydroxide  FeCl2 
 
aluminum chlorate  FeCl2 
 
lead(IV) selenide  NH4NO3 
 
copper(II) nitride  Mn(ClO3)2 
 
 
 14 CLYau 2005.02.07 
Unit VB: Polyatomic Ions with “−ite” Ending 
 
In the previous unit (Unit VA) you learned six polyatomic ions with the “−ate” ending.  Certain 
of these have counterparts with the “−ite” ending.  The only difference in formula for those with 
“−ite” endings is in having one less oxygen.  The charge is unchanged.  For example, nitrate is 
NO3
− and nitrite is NO2
−.  Below are the ones with which you should become familiar. 
 
NO3
− 
nitrate 
SO4
2− 
sulfate 
PO4
3− 
phosphate 
NO2
− 
nitrite 
SO3
2− 
sulfite 
PO3
3− 
phosphite 
 
ClO3
− 
chlorate 
ClO2
− 
chlorite 
 
Unit VC: Nomenclature of “−ate” and “−ite” Compounds 
 
The rules for naming and writing formulas for polyatomic ions are the same as for the 
monatomic ions (see Unit VI).  The only difference is if (and only if) there is more than one 
polyatomic ion, parenthesis must be used to avoid confusion. 
 
For example, magnesium nitrite is Mg(NO2)2.  Since Mg is in Group IIA, it has a charge of 2+ 
and nitrite has a charge of 1− (from memory), to obtain a net charge of zero, there must be two 
nitrite ions for every magnesium ion.  In the case of potassium acetate, since potassium is in 
Group IA, it must have a charge of 1+, and acetate has a charge of 1−, the formula is simply 
KC2H3O2.  No parenthesis is necessary. 
 
In naming compounds with cations of variable charges, the charge of the cation must be deduced 
from the charge of the anions.  It is therefore imperative that you have learned the charges of the 
ions presented in Units VA and VB.  For example, MnSO4 should be named manganese(II) 
sulfate.  Since you had previously memorized the fact that SO4
2−  has a charge of 2−, the 
manganese ion must have a charge of 2+.  In the case of Cu(NO3)2, since the nitrate ion has a 
charge of 1−, two nitrates would have a total charge of 2−.  Thus Cu must have a charge of 2+.  
The name for Cu(NO3)2 is therefore Cu(II) nitrate or cupric nitrate. 
 
 15 CLYau 2005.02.07 
Drill I-5: Nomenclature of “−ate” and “−ite” ions and compounds 
 
FORMULA NAME 
SO4
2−  
SO3
2−  
 nitrite 
 phosphite 
 acetate 
 chlorite 
Na3PO4  
K2SO3  
Pb(OH)2  
CoClO2  
Ca(NO3)2  
 iron(III) carbonate 
 copper(I) sulfite 
 cesium nitrite 
 aluminum chlorate 
 
Unit VD: Nomenclature of Oxohalo Anions 
 
These are the anions that contain a halogen and various number of oxygen atoms.  In this unit we 
will focus on the chlorine series.  Note that all have the charge of 1−.  Starting with chlorate 
which is one of our “Basic Eight” from Unit VA, when we lose one oxygen, we get the one with 
the −ite ending.  When we lose another oxygen, the name picks up the prefix hypo.  When we 
lose yet another oxygen, there is no oxygen left and we have the simple monatomic ion with the 
−ide ending (from Unit III).  Returning to chlorate as the base, if we add one extra oxygen, the 
name picks up the prefix per. 
 
ClO4
− perchlorate 
ClO3
− chlorate 
ClO2
− chlorite 
ClO− hypochlorite 
Cl− chloride 
 
 
 16 CLYau 2005.02.07 
Drill J: Nomenclature of Oxohalo Anions and Compounds: 
 
FORMULA NAME 
ClO−  
ClO2
−  
ClO4
−  
 hypochlorite 
 chlorate 
 perchlorate 
 chlorite 
 chloride 
 sodium chlorite 
 magnesium chlorite 
 ferrous perchlorate 
 
Note that once you have learned the above oxochloro anions, you are just one step away from 
learning the corresponding oxobromo and oxoiodo anions.  Your instructor may require you to 
learn these as well: 
 
perbromate, bromate, bromite, hypobromite, bromide 
BrO4
− BrO3
− BrO2
− BrO− Br− 
 
periodate,  iodate, iodite, hypoiodite, iodide 
IO4
− IO3
− IO2
− ΙΟ− Ι− 
 
 17 CLYau 2005.02.07 
Drill K: Nomenclature of “−ate”, “−ite”, oxohaloanions & Their Compounds 
 
FORMULA NAME 
ClO4
−  
ClO3
−  
ClO2
−  
ClO−  
Cl−  
 nitrite 
 nitrate 
 nitride 
 hydroxide 
Ca(ClO)2  
Ca3(PO3)2  
Sc(OH)2  
Ti(NO3)3  
Hg(ClO)2  
K3N  
 potassium perchlorate 
 potassium sulfite 
 aluminum sulfide 
 sodium sulfate 
 barium hydroxide 
 ammonium carbonate 
 copper(I) hypochlorite 
 tin(IV) acetate 
 chromium(III) phosphite 
 magnesium chlorate 
 zinc(II) phosphide 
 calcium nitrite 
************************************************************************ 
 
Unit VI: Nomenclature of Acids 
 
The system of naming acids presented in this unit relies on how well  you know the formulas of 
the polyatomic ions.  If necessary review all of the above units. 
 
Starting with a polyatomic ion (such as SO4
2−), add as many H+ as necessary to neutralize the 
charge.  For sulfate, with a charge of 2−, you would have to add two H+.  Generally the 
hydrogen is placed at the front of the formula (H2SO4).  For phosphate, you would have to add 
three H+, and the acid has the formula of H3PO4. 
 18 CLYau 2005.02.07 
The name of the acid depends on the ending of the anion.  If the ending is −ate, the 
corresponding acid has the ending −ic acid.  If the ending is −ite, the corresponding acid has the 
ending –ous acid.  If the ending is −ide, the acid has the prefix of hydro− and an ending of −ic 
acid. 
Ending of Anion Name of Corresponding Acid  
−ate −ic acid 
−ite −ous acid 
−ide hydro−….−ic acid 
Thus, sulfate becomes sulfuric acid; sulfite becomes sulfurous acid and sulfide becomes 
hydrosulfuric acid. 
 
Drill L: Nomenclature of Acids 
 
 ANIONS CORRESPONDING ACIDS   
Formula Name Formula Name 
ClO4
– _______________ __________ __________________ 
ClO3
– _______________ __________ __________________ 
ClO2
– _______________ __________ __________________ 
ClO– _______________ __________ __________________ 
Cl– _______________ __________ __________________ 
Br− _______________ __________ __________________ 
I− _______________ __________ __________________ 
C2H3O2
− _______________ __________ __________________ 
NO3
− _______________ __________ __________________ 
NO2
− _______________ __________ __________________ 
OH− _______________ __________ __________________ 
ClO3
− _______________ __________ __________________ 
CO3
2− _______________ __________ __________________ 
SO4
2− _______________ __________ __________________ 
SO3
2− _______________ __________ __________________ 
PO4
3− _______________ __________ __________________ 
PO3
3− _______________ __________ __________________ 
 Drill continues on following page 
 19 CLYau 2005.02.07 
         
Name Formula Formula Name 
sulfuric acid  HNO3  
nitrous acid  H2CO3  
hydrochloric acid  H3PO3  
carbonic acid  HClO  
phosphorous acid  H2SO4  
chlorous acid  HC2H3O2  
sulfurous acid  HNO2  
hypochlorous acid  HClO4  
chloric acid  HBr  
phosphoric acid  H2SO3  
nitric acid  H2Se  
acetic acid  H3PO4  
hydrotelluric acid  HOH  
 
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 20 CLYau 2005.02.07 
Unit VII: Nomenclature of Acid Anions 
 
In Unit VI you learned that acids generally have one or more H at the front of the formula.  It 
does not have a charge because we have added as many H+ as necessary to keep it neutral.  An 
“acid anion”, however, by definition must have a H in front (to be called an acid), as well as a 
negative charge (to be called an anion).  It is derived from having added less than the necessary 
number of H+. 
 
For example, if we add only one H+ to the sulfate ion (SO4
2−), we would have the acid anion, 
HSO4
−.  If we add only one H+ to the phosphite ion (PO3
3−), we would have the acid anion 
HPO3
2−.  If we added two, we would have the acid anion H2PO3
−.  Note that the negative charge 
of the anion is reduced by each additional H+. 
 
Study the following names and formulas and then test yourself using flash cards: 
 
CO3
2− 
carbonate 
 PO4
3− 
phosphate 
PO3
3− 
phosphite 
HCO3
− 
hydrogen carbonate 
or bicarbonate 
 HPO4
2− 
hydrogen phosphate 
HPO3
2− 
hydrogen phosphite 
SO4
2− 
sulfate 
 H2PO4
− 
dihydrogen phosphate 
H2PO3
− 
dihydrogen phosphite 
HSO4
− 
hydrogen sulfate 
or bisulfate 
   
SO3
2− 
sulfite 
   
HSO3
− 
hydrogen sulfite 
or bisulfite 
   
 
 21 CLYau 2005.02.07 
Drill M: Nomenclature of Acid Anions 
 
 Formula Stock Name Common Name  
(when appropriate) 
1 Ca(HCO3)2   
2 Fe(HCO3)2   
3 Pb(HPO4)2                 xxxxxxxxxxxxxxxxx 
4 AgHSO3   
5 Bi(H2PO3)3                 xxxxxxxxxxxxxxxxx 
6  barium hydrogen phosphate                xxxxxxxxxxxxxxxxx 
7  magnesium hydrogen sulfite  
8  aluminum hydrogen phosphate                xxxxxxxxxxxxxxxxx 
9  mercury(II) dihydrogen 
phosphite                xxxxxxxxxxxxxxxxx 
10  zinc(II) hydrogen carbonate  
11   barium bisulfite 
12   iron(III) bicarbonate 
13   copper(I) bisulfate 
14   copper(II) dihydrogen phosphite 
15 
  tin(IV) hydrogen phosphate xxxxxxxxxxxxxxxxx 
16 
  antimony(III) hydrogen 
phosphite xxxxxxxxxxxxxxxxx 
 
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 22 CLYau 2005.02.07 
Unit VIII: Nomenclature of Other Common Polyatomic Ions 
 
We began with a small set of polyatomic ions, the “Basic Eight” (see Unit V).  All the 
subsequent units were based on solely those eight.  Now it is time to expand our base to a few 
more ions that we often come across.  The nomenclature rules you have learned will apply to 
these as well. 
 
2+ 1– 2− 
Hg2
2+    
mercury(I) ion 
CN–           
cyanide 
C2O4
2−     
oxalate 
 MnO4
–     
permanganate 
O2
2−        
peroxide 
  CrO4
2−     
chromate 
  Cr2O7
2−  
dichromate 
  
Drill N:  Nomenclature of Other Polyatomic Ions and Compounds 
 
FORMULA NAME 
FeCr2O7  
Na2O2  
HgO  
 calcium cyanide 
 ammonium oxalate 
 silver(I) permanganate 
 mercury(I) chloride 
 mercury(II) chloride 
 
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 23 CLYau 2005.02.07 
Unit IX: Nomenclature of Molecular Binary Compounds 
 
Units III through VIII dealt with ions and ionic compounds.  In this unit we will deal with 
molecular compounds.  In particular, the molecular binary compounds, compounds containing 
only two nonmetals.  They involve a completely different set of rules.  Since there are no ions, 
there are no charges and no Roman numerals.  
 
The number of atoms of each element is specified by a Greek prefix (see table below).  The 
second element has the ending “−ide”.  For example, N2F4 is named dinitrogen tetrafluoride.   
 
When two vowels are adjacent to each other, one is dropped. For example P2O5 is named 
diphosphorus pentoxide rather than pentaoxide. 
 
When the first element has only one atom, the prefix mono is often omitted.  For example, NO2 
is often referred to as nitrogen dioxide rather than mononitrogen dioxide. 
 
When the second element has only one atom, the prefix mono is retained.  For example, CO is 
carbon monoxide rather than monocarbon monoxide. 
 
Number Prefix  Number Prefix 
1 mono  6 hexa 
2 di  7 hepta 
3 tri  8 octa 
4 tetra  9 nona 
5 penta  10 deca 
 
Drill O: Nomenclature of Molecular Binary Compounds 
 
FORMULA NAME 
CBr4  
PCl5  
S2Br2  
N2O4  
 sulfur dioxide 
 diiodine trioxide 
 dibromine monoxide 
 
Remember that the rules stated here for using prefixes (mono, di, tri, etc.) are for molecular 
binary compounds.  That excludes ionic compounds!  For ionic compounds you follow the rules 
 24 CLYau 2005.02.07 
you have learned from Units III through VIII earlier in this tutorial.  Thus PCl3 is phosphorus 
trichloride, but AlCl3 is aluminum chloride and MnCl3 is manganese(III) chloride. You have 
already learned all the rules (when to use prefixes, when to use Roman numerals and when not to 
use either).  The drill below is to help you practise choosing the appropriate rules to follow. 
 
The key is to first determine whether a compound is molecular or ionic.  That is easily done by 
seeing whether the first element shown is a metal or nonmetal.  There are exceptions to this rule, 
but for now, let us consider only the usual cases.  If the compound is molecular, you use prefixes.  
If it is ionic, you must decide whether the cation has fixed or variable charges in order to 
determine whether or not to use Roman numerals (Unit III). 
 
Drill P: Drill in Determining When to Use Prefixes and Roman Numerals 
 
FORMULA NAME 
PbCl2  
SCl2  
MgCl2  
Co2S3  
Al2O3  
N2Br4  
K3P  
 
 
*********************************************************************** 
 
Unit X: Nomenclature of Hydrates 
 
A hydrate is a compound with a fixed number of water molecules as an integral part of its 
structure.  An example is CuSO4⋅5H2O, a blue crystalline material.  As the formula 
indicates, it has five water molecules for each unit of CuSO4.  Although it contains water 
molecules, it is a solid. 
 
Note that a hydrate is not simply a sample that is wet!  A wet sample would have a variable 
amount of water and would not have the fixed ratio of water attached. 
 
In naming hydrates, you would name the compound with the rules that you have learned 
previously, followed by specifying how many water molecules are attached with a prefix.  
 25 CLYau 2005.02.07 
Thus, CuSO4⋅5H2O is named copper(II) sulfate pentahydrate, and cobalt(II) chloride 
tetrahydrate has the formula CoCl2⋅4H2O. 
 
Note that the dot in front of the formula H2O does not represent a multiplication sign!  It 
merely separates out the H2O from the rest of the formula and the coefficient in front of the 
H2O tells you how many water molecules are present.  CoCl2⋅4H2O, therefore, contains one 
Co2+ ion, two Cl− ions and four water molecules.  It has a total of one cobalt, two chlorine, 
eight hydrogen and four oxygen atoms. 
 
Drill Q:  Drill on Naming Hydrates 
 
Formula Name Name Formula 
Ca(ClO3)2⋅2H2O  cobalt(II) fluoride tetrahydrate  
Sn(SO4)2⋅2H2O  zinc(II) acetate dihydrate  
NiSO4⋅7H2O  copper(II) nitrate trihydrate  
Co(C2H3O2)2⋅4H2O  iron(III) bromide hexahydrate  
 
************************************************************************ 
 
End of Nomenclature Tutorial 
(See the following pages for the answers to the drills.) 
 
If you have questions or comments you may contact me at cyau@ccbcmd.edu 
 
 
 26 CLYau 2005.02.07 
Answers to “Nomenclature: A Tutorial” 
 
Drill A: Nomenclature of Elements 
 
Name Symbol  Symbol Name 
          
chlorine Cl  S sulfur 
calcium Ca  K potassium 
arsenic As  Fe iron 
mercury Hg  Na sodium 
copper Cu  P phosphorus 
 
Drill B: Formulas and Physical States of Pure Elements 
  
chlorine Cl2 (g)  bromine Br2 (l)  sulfur S8 (s) 
argon Ar (g)  phosphorus P4 (s)  lead Pb (s) 
nitrogen N2 (g)  krypton Kr (g)  element #112 Uub (s) 
chromiu
m
Cr (s)  mercury Hg (l)  gold Au (s) 
strontiu
m
Sr (s)  iodine I2 (s)  hydrogen H2 (g) 
 
Drill C: Nomenclature of Monatomic Ions 
 
FORMULA NAME  NAME FORMULA 
Rb+ rubidium ion  nitride N3– 
Ba2+ barium ion  iodide I – 
P3– phosphide  oxide O2– 
Br – bromide  chromium(III) Cr3+ 
N3– nitride  potassium ion K+ 
S2– sulfide  aluminum ion Al3+ 
V3+ vanadium(III)  magnesium Mg 
Cu2+ copper(II) ion  ferrous ion Fe2+ 
Ca calcium  cuprous ion Cu+ 
 
 27 CLYau 2005.02.07 
Drill D: Formulas of Ionic Compounds of Monatomic ions 
 
NAME FORMULA 
magnesium fluoride MgF2 
lithium sulfide Li2S 
calcium selenide CaSe 
nickel(II) fluoride NiF2 
cupric bromide CuBr2 
chromium(III) sulfide Cr2S3 
tin(II) phosphide Sn3P2 
 
Drill E: Writing Names of Compounds with Cations of Fixed Charges 
 
KBr potassium bromide 
Li2O lithium oxide 
Mg3As2 magnesium arsenide 
Na3P sodium phosphide 
 
Drill F: Determining the Charge and Name of the Cation First, Then Name of Compound 
 
Formula Charge of 
Cation Name of Cation Name of Compound 
MnO2 4+ manganese(IV) ion manganese(IV) oxide 
PbS 2+ lead(II) ion lead(II) sulfide 
Cr2O3 3+ chromium(III) ion chromium(III) oxide 
Rb2Se 1+ rubidium ion rubidium selenide 
CuCl2 2+ copper(II) ion copper(II) chloride 
CuO 2+ copper(II) ion copper(II) oxide 
Cu2O 1+ copper(I) ion copper(I) oxide 
 
 28 CLYau 2005.02.07 
Drill G: Nomenclature of Ionic Compounds of Monatomic Ions  
 (Both Fixed & Variable Charges) 
 
FORMULA NAME  FORMULA NAME 
Na2O sodium oxide  RbBr rubidium bromide 
Mg3N2 magnesium nitride  FeBr2 iron(II) bromide 
Cu2S cuprous sulfide  PbS lead(II) sulfide 
MnI2 manganese(II) iodide  BaO barium oxide 
FeP ferric phosphide  K2O potassium oxide 
CuO cupric oxide  SbBr3 antimony(III) bromide 
Sn3N2 tin(II) nitride  Fe3P2 iron(II) phosphide 
SrO strontium oxide  Li2Se lithium selenide 
SnO2 tin(IV) oxide  CuCl2 copper(II) chloride 
 
Extra Drill H: Nomenclature of Ionic Compounds of Monatomic Ions  
 (Both Fixed & Variable Charges) 
 
FORMULA NAME 
RaCl2 radium chloride 
BiCl3 bismuth(III) chloride 
Fe2O3 iron(III) oxide or ferric oxide 
CdBr2 cadmium(II) bromide 
MnO manganese(II) oxide 
MnO2 manganese(IV) oxide 
 
 29 CLYau 2005.02.07 
Drill I - 1: Nomenclature of the "Basic Eight" Polyatomic Ions  
   
NAME FORMULA FORMULA NAME 
sulfate SO4
2− OH− hydroxide 
acetate C2H3O2
− SO4
2− sulfate 
chlorate ClO3
− NH4
+ ammonium 
ammonium NH4
+ NO3
− nitrate 
phosphate PO4
3− ClO3
− chlorate 
carbonate CO3
2− PO4
3− phosphate 
hydroxide OH−      CO3
2− carbonate 
nitrate NO3
− C2H3O2
− acetate 
 
 
Drill I - 2: Nomenclature of Compounds of the "Basic Eight" Polyatomic Ions With 
Cations of Fixed Charges:  
   
NAME FORMULA FORMULA NAME 
sodium carbonate Na2CO3 K3PO4 potassium phosphate 
strontium carbonate SrCO3     Ca(NO3)2 calcium nitrate 
aluminum sulfate Al2(SO4)3     (NH4)2SO4 ammonium sulfate 
ammonium 
phosphate 
(NH4)3PO4 Al(OH)3 aluminum hydroxide 
aluminum chlorate Al(ClO3)3 LiC2H3O2 lithium acetate 
potassium sulfate K2SO4     MgCO3 magnesium carbonate 
calcium acetate            Ca(C2H3O2)2 Ba(ClO3)2 barium chlorate 
                               
 
Drill I - 3: Nomenclature of Compounds of the "Basic Eight" Polyatomic Ions With 
Cations of Variable Charges:    
 
NAME FORMULA NAME FORMULA 
ferrous carbonate FeCO3     
CuCO3 (stock name) 
copper(II) carbonate 
ferric carbonate Fe2(CO3)3     
CuCO3 (common name) 
cupric carbonate 
cuprous sulfate Cu2SO4 SnSO4 tin(II) sulfate 
cobalt(II) phosphate Co3(PO4)2     
Fe3(PO4)2 (stock name) 
iron(II) phosphate 
chromium(III) 
chlorate Cr(ClO3)3     
Hg(C2H3O2)2 mercury(II) acetate 
tin(IV) sulfate Sn(SO4)2 BiPO4 bismuth(III) phosphate 
antimony(III) acetate 
Sb(C2H3O2)3  
or 
Sb(CH3CO2)3 
Mn(ClO3)2 manganese(II) chlorate 
 30 CLYau 2005.02.07 
 
 
                                                            
 
        
Drill I - 4: Compounds of the "Basic Eight" Polyatomic Ions and –ide ions With Cations of 
Both Fixed and Variable Charges: (learning to distinguish between those that require 
Roman numerals and those that do not)    
NAME FORMULA FORMULA NAME 
calcium phosphate Ca3(PO4)2 Na3N sodium nitride 
chromium(III) sulfide Cr2S3 NaNO3 sodium nitrate 
potassium carbonate K2CO3 K2SO4 potassium sulfate 
magnesium acetate Mg(CH3CO2)2 CdCO3 cadmium(II) carbonate 
chromium(III) hydroxide Cr(OH)3 FeCl2 
(stock name) 
iron(II) chloride 
aluminum chlorate Al(ClO3)3 FeCl2 
(common name) 
ferrous chloride 
lead(IV) selenide PbSe2 NH4NO3 ammonium nitrate 
cupric nitride Cu3N2 Mn(ClO3)2 manganese(II) chlorate 
ferrous nitrate Fe(NO3)2 Cu3PO4 
(common name) 
cuprous phosphate 
 
 
Drill I-5: Nomenclature of “−ate” and “−ite” ions and compounds 
 
FORMULA NAME 
SO4
2− sulfate 
SO3
2− sulfite 
NO2
– nitrite 
PO3
3− phosphite 
C2H3O2
− acetate 
ClO2
− chlorite 
Na3PO4 sodium phosphate 
K2SO3 potassium sulfite 
Pb(OH)2 lead(II) hydroxide 
CoClO2 cobalt(I) chlorite 
Ca(NO3)2 calcium nitrate 
Fe2(CO3)3 iron(III) carbonate 
Cu2SO3 copper(I) sulfite 
CsNO2 cesium nitrite 
Al(ClO3)3 aluminum chlorate 
 
 31 CLYau 2005.02.07 
Drill J: Nomenclature of Oxohalo Ions and Compounds: 
FORMULA NAME 
ClO− hypochlorite 
ClO2
− chlorite 
ClO4
− perchlorate 
ClO− hypochlorite 
ClO3
− chlorate 
ClO4
− perchlorate 
ClO2
− chlorite 
Cl– chloride 
NaClO2 sodium chlorite 
Mg(ClO2)2 magnesium chlorite 
Fe(ClO4)2 ferrous perchlorate 
 
Drill K: Nomenclature of “−ate”, “−ite”, oxohaloanions & Their Compounds: 
FORMULA NAME 
ClO4
− perchlorate 
ClO3
− chlorate 
ClO2
− chlorite 
ClO− hypochlorite 
Cl− chloride 
NO2
− nitrite 
NO3
− nitrate 
N3− nitride 
OH− hydroxide 
Ca(ClO)2 calcium hypochlorite 
Ca3(PO3)2 calcium phosphite 
Sc(OH)2 scandium(II) hydroxide 
Ti(NO3)3 titanium(III) nitrate 
Hg(ClO)2 mercury(II) hypochlorite 
K3N potassium nitride 
KClO4 potassium perchlorate 
K2SO3 potassium sulfite 
Al2S3 aluminum sulfide 
Na2SO4 sodium sulfate 
Ba(OH)2 barium hydroxide 
(NH4)2CO3 ammonium carbonate 
CuClO cuprous hypochlorite 
Sn(C2H3O2)4 tin(IV) acetate 
CrPO3 chromium(III) phosphite 
Mg(ClO3)2 magnesium chlorate 
Zn3P2 zinc(II) phosphide 
Ca(NO2)2 calcium nitrite 
 
 32 CLYau 2005.02.07 
Drill L: Nomenclature of Acids  
 
 ANIONS CORRESPONDING ACIDS 
  
Formula Name Formula Name 
ClO4
– perchlorate HClO4 perchloric acid 
ClO3
– chlorate HClO3 chloric acid 
ClO2
– chlorite HClO2 chlorous acid 
ClO– hypochlorite HClO hypochlorous acid 
Cl– chloride HCl hydrochloric acid 
Br− bromide HBr hydrobromic acid 
I− iodide HI hydroiodic acid 
C2H3O2
− acetate HC2H3O2 acetic acid 
NO3
− nitrate HNO3 nitric acid 
NO2
− nitrite HNO2 nitrous acid 
OH− hydroxide HOH water 
ClO3
− chlorate HClO3 chloric acid 
CO3
2− carbonate H2CO3 carbonic acid 
SO4
2− sulfate H2SO4 sulfuric acid 
SO3
2− sulfite H2SO3 sulfurous acid 
PO4
3− phosphate H3PO4 phosphoric acid 
PO3
3− phosphite H3PO3 phosphorous acid 
 33 CLYau 2005.02.07 
 
Name Formula Formula Name 
sulfuric acid H2SO4 HNO3 nitric acid 
nitrous acid HNO2 H2CO3 carbonic acid 
hydrochloric acid HCl H3PO3 phosphorous acid 
carbonic acid H2CO3 HClO hypochlorous acid 
phosphorous acid H3PO3 H2SO4 sulfuric acid 
chlorous acid HClO2 HC2H3O2 acetic acid 
sulfurous acid H2SO3 HNO2 nitrous acid 
hypochlorous acid HClO HClO4 perchloric acid 
chloric acid HClO3 HBr hydrobromic acid 
phosphoric acid H3PO4 H2SO3 sulfurous acid 
nitric acid HNO3 H2Se hydroselenic acid 
acetic acid HC2H3O2 H3PO4 phosphoric acid 
hydrotelluric acid H2Te HOH water 
 
Drill M: Nomenclature of Acid Anions 
 
1.  calcium hydrogen carbonate, 
 calcium bicarbonate 
2.  iron(II) hydrogen carbonate, 
 ferrous bicarbonate 
3.  lead(IV) hydrogen phosphate 
4.  silver(I) hydrogen sulfite,       
  silver(I) bisulfite 
5.  bismuth(III) dihydrogen phosphite 
6.  BaHPO4 
7.  Mg(HSO3)2 ,     magnesium bisulfite 
8.  Al2(HPO4)3 
9.   Hg(H2PO3)2  
10. Zn(HCO3)2 ,  zinc(II) bicarbonate 
11. Ba(HSO3)2 ,  barium hydrogen sulfite 
12. Fe(HCO3)3 ,  
 iron(III) hydrogen carbonate 
13. CuHSO4 ,      copper(I) hydrogen sulfate 
14. Cu(H2PO3)2 ,  
 copper(II) dihydrogen phosphite 
15. Sn(HPO4)2 
16. Sb2(HPO3)3 
 
 34 CLYau 2005.02.07 
Drill N: Nomenclature of Other Polyatomic Ions and Compounds 
 
 
Drill O: Nomenclature of Molecular Binary Compounds 
FORMULA NAME 
CBr4 carbon tetrabromide 
PCl5 phosphorus pentachloride 
S2Br2 disulfur dibromide 
N2O4 dinitrogen tetroxide 
SO2 sulfur dioxide 
I2O3 diiodine trioxide 
Br2O dibromine monoxide 
 
Drill P: Drill in Determining When to Use Prefixes and Roman Numerals 
FORMULA NAME 
PbCl2 lead(II) chloride (ionic, cation with variable charges) 
SCl2 sulfur dichloride (molecular) 
MgCl2 magnesium chloride (ionic, cation with fixed charges) 
Co2S3 cobalt(III) sulfide (ionic, cation with variable charges) 
Al2O3 aluminum oxide (ionic, cation with fixed charges) 
N2Br4 dinitrogen tetrabromide (molecular) 
K3P potassium phosphide (ionic, cation with fixed charges) 
 
 
FORMULA NAME 
FeCr2O7 iron(II) dichromate 
Na2O2 sodium peroxide 
HgO mercury(II) oxide 
Ca(CN)2 calcium cyanide 
(NH4)2C2O4 ammonium oxalate 
AgMnO4 silver(I) permanganate 
Hg2Cl2 mercury(I) chloride 
HgCl2 mercury(II) chloride 
 35 CLYau 2005.02.07 
Drill Q:  Drill on Naming Hydrates 
 
 
Formula Name Name Formula 
Ca(ClO3)2⋅2H2O calcium chlorate 
dihydrate 
cobalt(II) fluoride 
tetrahydrate CoF2⋅4H2O 
Sn(SO4)2⋅2H2O tin(IV) sulfate dihydrate zinc(II) acetate dihydrate Zn(C2H3O2)2⋅2H2O 
NiSO4⋅7H2O nickel(II) sulfate 
heptahydrate 
copper(II) nitrate 
trihydrate Cu(NO3)2⋅3H2O 
Co(C2H3O2)2⋅4H
2O 
cobalt(II) acetate 
tetrahydrate 
iron(III) bromide 
hexahydrate FeBr3⋅6H2O 
 
 
End of Answers to the Nomenclature Tutorial Drills 
 
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