Chemical Nomenclature: A Tutorial for Prep Chem

Chemical Nomenclature for an Introductory Chemistry Course

A Tutorial with Rules & Drills and Answers

* The format used here is designed for working online, with links to answers etc. and not suitable for converting into a hard copy.
If you prefer to work from a printed copy, click here to download a printable version of this tutorial (Adobe Acrobat Reader required). There is a total of 33 pages, including the answers to the drills.

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.

OUTLINE:
Unit I: Chemical Symbols of Some Common Elements (Drill A)
Unit II: Nomenclature of Pure Elements (Drill B)
Unit III: Nomenclature of Monatomic Ions (Simple Ions)
    Unit IIIA: Nomenclature of Monatomic Anions
    Unit IIIB: Nomenclature of Monatomic Cations of Fixed Charges
    Unit IIIC: Nomenclature of Monatomic Cations of Variable Charges (Drill C)
Unit IV: Nomenclature of Ionic Compounds of Monatomic Ions
    Unit IVA: Writing Formulas from a Given Name (Drill D)
    Unit IVB: Writing Names from a Given Formula (Drills E thru H)
Unit V: Nomenclature of Polyatomic Ions
    Unit VA: The "Basic Eight" Polyatomic Ions (Drills I-1 thru I-4)
    Unit VB: Polyatomic Ions with "- ite" Ending
    Unit VC: Nomenclature of "- ate" and "- ite" Compounds (Drill I-5)
    Unit VD: Nomenclature of Oxohaloanions (Drills J & K)
Unit VI: Nomenclature of Acids (Drill L)
Unit VII: Nomenclature of Acid Anions (Drill M)
Unit VIII: Nomenclature of Molecular Binary Compounds (Drill N & O)
Unit IX: Nomenclature of Hydrates (Drill P)

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 ones you are expected to know in an introductory chemistry course. 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.

Study the elements listed in the table. You must be able to give the name (with correct spelling) when given the symbol, and to give the symbol when given the name. Use flash cards to test yourself. Study them in small groups in this order. Do not proceed until you know each group well:

1) Elements #1 through 18. Test yourself with flash cards.

2) Elements in Group IA. (Except for hydrogen, these are the alkali metals.)

3) Elements in Group IIA. (These are the alkaline earth metals.)

4) Elements in Group VIIA. (Except for hydrogen, these are the halogens.)

5) Elements in Group VIIIA. (These are the halogens.)

6) Elements listed as “common transition metals.” Locate these on your periodic table. They are in the first row of the elements known as transition metals.

7) Elements listed as “other common elements.” Locate these on your periodic table.

Learn the elements learn all the elements listed below in Group IA. Except for hydrogen, these are the alkali metals.

Then learn all the elements listed below in Group VIIA. Except for hydrogen, these are the halogens.

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		I iodine
C carbon
N nitrogen
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

Common Transition Metals	Other Common Elements
Cr chromium	As arsenic	U uranium
Mn manganese	Sn tin	Pu plutonium
Fe iron	Pb lead
Co cobalt	Ag silver
Ni nickel	Hg mercury
Cu copper
Zn zinc

Elements that you should be able to provide names or symbols are highlighted in RED.

The ones in BLUE you will learn a little later in the semester.

VIIA

VIIIA

IIA

III A

IV A

V A

VI A

III B

IV B

V B

VI B

VIIB

VIIIB

I B

II B

104

105

106

107

108

109

110

111

112

Uub

113

Uut

114

Uuq

115

Uup

116

Uuh

117

118

Uuo

Lanthanides:

*Ce

Actinides:

**Th

100

101

102

103

Name all the elements listed above that are marked in red, and then the ones in blue.

Drill A: Nomenclature of Elements

This is a self-test, since you can easily look up answers yourself. After you have drilled yourself on the symbols and spelling of the elements listed above, take this as a practice test.

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.
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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 N₂rather 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 (Note where these elements are located on the Periodic Table.)

*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.)

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
chromium	mercury	arsenic
strontium	iodine	hydrogen

Remember not to proceed to the next unit until you have studied Unit II.
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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
C⁴^- carbide	N³^- nitride	O²^- oxide	F^- fluoride
	P³^- phosphide	S²^- sulfide	Cl^- chloride
	As³^- arsenide		Br^- bromide
			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
K⁺ potassium ion	Ca²⁺ calcium ion
	Sr²⁺ strontium ion
	Ba²⁺ barium ion
	Ra²⁺ radium ion

*Other common cations that have fixed charges include the following: Ag⁺, Ni²⁺, Zn²⁺, Cd²⁺

These do not require Roman numerals, although including Roman numerals would not be incorrect.

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 be at least familiar with 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

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 the iron(II) ion, 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
P^3–		oxide
Br^–		chromium(III) ion
N^3–		potassium ion
S^2–		aluminum ion
Hg²⁺		magnesium
Cu²⁺		iron(II) ion
Ca		copper(I) ion
Ni²⁺		zinc ion

Remember not to proceed to the next unit until you have studied Unit III A through III C.
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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.)

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.

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 Image.jpg

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.

Drill D: Formulas of Ionic Compounds of Monatomic ions

NAME	FORMULA
magnesium fluoride
lithium sulfide
calcium nitride
nickel fluoride
copper(II) bromide
chromium(III) sulfide
tin(II) phosphide

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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

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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+.

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
K₂S
CuCl₂
CuO
Cu₂O
ZnO

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.

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Drill G: Nomenclature of Ionic Compounds of Monatomic Ions (Both Fixed & Variable Charges)

FORMULA	NAME	FORMULA	NAME
	sodium oxide	KBr
	magnesium nitride	FeBr₂
	copper(I) sulfide	PbS
	manganese(II) iodide	BaO
	iron(III) phosphide	K₂O
	copper(I) oxide	CrBr₃
	tin(II) nitride	Fe₃P₂
	strontium oxide	Li₂S
	tin(IV) oxide	CuCl₂
	nickel chloride	AgF

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Extra Drill H: Nomenclature of Ionic Compounds of Monatomic Ions (Both Fixed & Variable Charges)

FORMULA	NAME
RaCl₂
CrCl₃
Fe₂0₃
MgBr₂
MnO
MnO₂

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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 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. You MUST know these 8 polyatomic ions backwards and forwards before you proceed to the next unit.

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^-
nitrate		C₂H₃O₂^-

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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

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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		FePO₄
chromium(II) acetate		Mn(ClO₃)₂

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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		HgCO₃
chromium(III) hydroxide		FeCl₂
aluminum chlorate		FeCl₂
lead(IV) selenide		NH₄NO₃
copper(II) nitride		Mn(ClO₃)₂
silver oxide		Zn(C₂H₃O₂)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, nitrate is NO₃^- and nitrite 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.

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
	copper(I) sulfite
	lithium nitrite
	aluminum chlorate

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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

Drill J: Nomenclature of Oxohalo Anions and Compounds:

FORMULA	NAME
ClO^-
ClO₂^-
ClO₄^-
	hypochlorite
	chlorate
	perchlorate
	chlorite
	chloride
	sodium chlorite
	magnesium chlorite
	iron(II) perchlorate
	nickel hypochlorite

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Note that once you have learned the above oxochloro anions, you are just one step away from learning the corresponding oxobromo and oxoiodo anions. Dr. Yau does not expect you to learn the following, but please note bromine and iodine follow the same rules as Cl. You will learn these for General Chemistry.

perbromate, bromate, bromite, hypobromite, bromide

BrO₄^-BrO₃^-BrO₂^-BrO^-Br^-

periodate, iodate, iodite, hypoiodite, iodide

IO₄^- IO₃^-IO₂^-IO^- I^-

Drill K: Nomenclature of “-ate”, “-ite”, oxohaloanions & Their Compounds

FORMULA	NAME
ClO₄^-
ClO₃^-
ClO₂^-
ClO^-
Cl^-