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NomenclatureTutorialAnswersPRINTABLE2005.02.07

NomenclatureTutorialAnswersPRINTABLE2005.02.07
NomenclatureTutorialAnswersPRINTABLE2005.02.07

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

******************************************************************************

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

************************************************************************

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

************************************************************************

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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