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)
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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 - 18Group 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
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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
S
chlorine
K
calcium
Fe
arsenic
Na
mercury
P
copper
I.
Remember not to proceed to the next unit until you have studied Unit
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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:H
2
N2O2F2
Cl2
Br2
I2
Other molecular
elements:P4S8
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:H
He
2
N2O2F2 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.)
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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 = F 2 (g )
chlorine bromine sulfur
argon phosphorus lead nitrogen krypton element
#112
chromiu m
mercury gold strontium iodine hydrogen
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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 C 4? carbide N 3? nitride O 2? oxide F ? fluoride P 3? phosphide S 2? sulfide Cl ? chloride As 3? arsenide Se 2? selenide Br ? bromide Te 2? telluride
I ? iodide
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
ion Ca2+ calcium ion
K+ potassium
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.
Name
Common
Formula Stock
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
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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
ion
S2–aluminum
V3+magnesium
Cu2+iron(II) ion
Ca copper(I) ion
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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.)
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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
.
2 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.
= 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?3or 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.
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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+.
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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
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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*
CO32?
carbonate
PO43?
phosphate NO3?
nitrate
SO42?
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
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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 SO42?
chlorate NH4+
ammonium NO3?
phosphate ClO3?
carbonate PO43?
hydroxide CO32?
C2H3O2?
nitrate
Drill I - 2: Nomenclature of Compounds of the "Basic Eight" Polyatomic Ions With
Cations of Fixed Charges:
FORMULA NAME
NAME FORMULA
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
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Drill I - 3: Nomenclature of Compounds of the "Basic Eight" Polyatomic Ions With
Cations of Variable Charges:
NAME
NAME FORMULA
FORMULA
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.)
FORMULA NAME
NAME FORMULA
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
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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, nitr ate is NO3? and nitr ite is NO2?. Below are the ones with which you should become familiar.
NO3?nitrate SO42?
sulfate
PO43?
phosphate
NO2?nitrite SO32?
sulfite
PO33?
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 SO42?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.
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Drill I-5: Nomenclature of “?ate” and “?ite” ions and compounds
FORMULA NAME
SO42?
SO32?
nitrite
phosphite
acetate
chlorite
Na3PO4
K2SO3
Pb(OH)2
CoClO2
Ca(NO3)2
iron(III)
carbonate
sulfite
copper(I)
nitrite
cesium
chlorate
aluminum
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
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Drill J: Nomenclature of Oxohalo Anions and Compounds:
FORMULA NAME
ClO?
ClO2?
ClO4?
hypochlorite
chlorate
perchlorate
chlorite
chloride
sodium
chlorite
chlorite
magnesium
perchlorate
ferrous
Note that once you have learned the above oxo chloro anions, you are just one step away from
learning the corresponding oxo bromo and oxo iodo 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?
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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
sulfite
potassium
aluminum
sulfide
sulfate
sodium
hydroxide
barium
carbonate
ammonium
hypochlorite
copper(I)
acetate
tin(IV)
phosphite
chromium(III)
magnesium
chlorate
phosphide
zinc(II)
nitrite
calcium
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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 SO42?), 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.
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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 sulfur ic acid ; sulfite becomes sulfur ous acid and sulfide becomes hydro sulfur ic acid.
Drill L: Nomenclature of Acids
ANIONS CORRESPONDING ACIDS Formula Name Formula Name ClO 4– _______________ __________ __________________ ClO 3– _______________ __________ __________________ ClO 2– _______________ __________ __________________ ClO – _______________ __________ __________________ Cl – _______________ __________ __________________ Br ?
_______________ __________ __________________
I ? _______________ __________ __________________ C 2H 3O 2? _______________ __________ __________________ NO 3? _______________ __________ __________________ NO 2?
_______________ __________ __________________
OH ? _______________
__________ __________________ ClO 3? _______________ __________ __________________ CO 32? _______________ __________ __________________ SO 42? _______________ __________ __________________ SO 32?
_______________ __________ __________________
PO 43? _______________
__________ __________________ PO 33? _______________ __________ __________________
Drill continues on following page
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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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 (SO42?), we would have the acid anion, HSO4?. If we add only one H+to the phosphite ion (PO33?), we would have the acid anion HPO32?. 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:
CO32?carbonate PO43?
phosphate
PO33?
phosphite
HCO3?
hydrogen carbonate or bicarbonate HPO42?
hydrogen phosphate
HPO32?
hydrogen phosphite
SO42?sulfate H2PO4?
dihydrogen phosphate
H2PO3?
dihydrogen phosphite
HSO4?
hydrogen sulfate
or bisulfate
SO32?
sulfite
HSO3?
hydrogen sulfite
or bisulfite
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