NomenclatureNomenclature

- the method of assigning - the method of assigning names to chemical names to chemical

compoundscompounds

We will be using the IUPAC We will be using the IUPAC (International Union of Pure and (International Union of Pure and Applied Chemistry) to name Applied Chemistry) to name compoundscompounds

The old system is the Stock system; The old system is the Stock system; you may see this used in some older you may see this used in some older textbooks.textbooks.

You You mustmust know the normal charges know the normal charges each element takes (this is based on each element takes (this is based on their position in the periodic table)their position in the periodic table)

Many elements are capable of more than Many elements are capable of more than one charge the ones you must know are:one charge the ones you must know are:

copper:copper: CuCu1+1+ or Cu or Cu2+2+

iron: iron: FeFe2+2+ or Fe or Fe3+3+

tin:tin: SnSn2+2+ or Sn or Sn4+4+

lead:lead: PbPb2+2+ or Pb or Pb4+4+

nickel:nickel: NiNi2+2+ or Ni or Ni3+3+

gold:gold: AuAu++ or Au or Au3+3+

You must also know the charge on You must also know the charge on silver: Agsilver: Ag1+1+ zinc: Zn zinc: Zn2+2+ cadmium: cadmium:

CdCd2+2+

(Do not use Roman Numerals for these (Do not use Roman Numerals for these metals!)metals!)

Multivalent MetalsMultivalent Metals

Binary Ionic Compounds Binary Ionic Compounds These are made up of a metal and non-These are made up of a metal and non-

metalmetal To name binary ionic compounds we use To name binary ionic compounds we use

the following procedure:the following procedure:

metal non-metalidemetal non-metalide

THE METAL ALWAYS COMES FIRST, BOTH IN THE METAL ALWAYS COMES FIRST, BOTH IN NAMING AND IN THE FORMULA.NAMING AND IN THE FORMULA.

e.g.e.g. LiClLiCl

CaCa33PP22

MgOMgO

lithium chloride

calcium phosphide

magnesium oxide

Binary Ionic Compounds Cont’dBinary Ionic Compounds Cont’d To write the formula use “To write the formula use “cross and cross and

dropdrop””e.g. e.g. 2+2+ 3- 3-

Sr NSr N becomes Srbecomes Sr33NN22

2+2+ 2- 2-

Ca OCa O becomes Cabecomes Ca22OO22

REDUCE to CaOREDUCE to CaO

Only ever reduce ionic compounds not Only ever reduce ionic compounds not covalent.covalent.

potassium bromide KBrpotassium bromide KBr calcium oxidecalcium oxideCaOCaO

lithium nitridelithium nitride Li Li33NN potassium phosphide potassium phosphide KK33PP

sodium bromidesodium bromide NaBr NaBr beryllium sulfideberyllium sulfide BeSBeS

zinc chloridezinc chloride ZnCl ZnCl2 2 copper (II) oxidecopper (II) oxideCuOCuO

iron (III) bromideiron (III) bromide FeBr FeBr33 silver oxidesilver oxide AgAg22OO

BeOBeO beryllium oxideberyllium oxide CaBrCaBr33 calcium bromide calcium bromide

LiLi22NN lithium nitridelithium nitride SrISrI22 strontium iodidestrontium iodide

NaClNaCl sodium chloridesodium chloride CsCs22SeSe cesium selenidecesium selenide

AuAu22OO gold (I) oxidegold (I) oxide ZnSZnS zinc sulfidezinc sulfide

PbOPbO22 lead (IV) oxidelead (IV) oxide CdFCdF22 cadmium fluoride cadmium fluoride

Name the Following:Name the Following:

Ionic Compounds with Polyatomic Ionic Compounds with Polyatomic IonsIons

Polyatomic ions are a cluster of non-Polyatomic ions are a cluster of non-metal atoms held together by metal atoms held together by covalent bonding yet they have a covalent bonding yet they have a charge.charge.

Most polyatomics are negatively Most polyatomics are negatively charged and therefore combine with charged and therefore combine with a positively charged metal a positively charged metal

Most of the polyatomics contain Most of the polyatomics contain oxygen and are therefore known as oxygen and are therefore known as oxyanionsoxyanions

You MUST memorize the following polyatomics:

All the rules for ionic compounds apply; except that if the polyatomic ion is the anion, its ending does not change.

The polyatomic ion must be placed in brackets if the formula requires more than one; never use brackets if only one is needed!

# of consonants# of consonants # of vowels# of vowels

= # of oxygens= # of oxygens = = chargecharge

nitrate nitrate NONO33-- Nick Nick 33 11

carbonate COcarbonate CO332-2- CamelCamel 33 22

chlorate chlorate ClOClO33-- ClamClam 33 11

sulfate sulfate SOSO442-2- SupperSupper 44 22

phosphate POphosphate PO443-3- PhoenixPhoenix 44 33

hydroxide OHhydroxide OH--

ammonium NHammonium NH44++

AcetateAcetate C C22HH33OO22--

the

ate a

for

in

Name the followingName the followingAlAl22OO33

FeSFeSSr(NOSr(NO33))22

CuCu33(PO(PO44))

Write the formulasWrite the formulasMagnesium nitrideMagnesium nitrideBarium chlorateBarium chlorateLead (IV) sulfideLead (IV) sulfideSilver carbonateSilver carbonate

aluminum oxide

iron (II) sulfide

strontium nitrate

copper (I) phosphate

Mg3N2

Ba(ClO3)2

PbS2

Ag2CO3

Different Forms of Different Forms of OxyanionsOxyanions

The usual suffix for an oxyanion is “ate”The usual suffix for an oxyanion is “ate”

One more oxygen One more oxygen perperchloratechlorate ClOClO44--

NormalNormal chlorate chlorate ClOClO33--

One less oxygenOne less oxygen chlorite chlorite ClOClO22--

Two less oxygensTwo less oxygens hypohypochlorchloriteite ClOClO--

e.g. LiNOe.g. LiNO22

KK22SOSO33

NaClONaClO44

lithium nitritepotassium sulfite

sodium perchlorate

Name Formula hypochlorite ion ClO-

 phosphite ion PO33-

perchromate ion CrO52- 

phosphate ion PO43- 

 sulfate ion SO42-

nitrite ion NO2- 

carbonate ion CO32- 

 carbonite ion CO22-

hyposulfite ion SO22- 

chlorate ion ClO3- 

 nitrate ion NO3-

percarbonate ion CO42- 

chromate ion  CrO42-

 perchlorate ion ClO4-

perphosphate ion PO53- 

 sulfite ion SO32-

hypophosphite ion PO23- 

Name the Following:Name the Following:

Li2SO3 lithium sulfite KMnO4 potassium permanganateNaCrO5 sodium perchromateCu(NO2)2 copper (II) nitrite CdCO2 cadium carboniteFePO5 iron (III) perphosphatelead (IV) sulfite Pb(SO3)2

molybdenum (VI) persulfate Mo(SO5)3

vanadium (V) nitrite V(NO2)5

ammonium hypophosphite (NH4)3PO2

Binary Covalent CompoundsBinary Covalent Compounds

These are composed of two or more These are composed of two or more nonmetalsnonmetals

Electrons are shared not transferredElectrons are shared not transferred

Ions are not formedIons are not formed

For these compounds the more For these compounds the more electronegative element is written first both electronegative element is written first both in the formula and the name. (Exception in the formula and the name. (Exception however with C-H and N-H compounds, eg. however with C-H and N-H compounds, eg. CHCH44 – methane, NH – methane, NH33 – ammonia) – ammonia)

Many covalent compounds have common names – water (H2O); ammonia (NH3); methane (CH4); ozone (O3); hydrogen peroxide (H2O2)

Several elements do not exist as single atoms; they occur as “diatomic molecules” (2 atoms in a covalent bond) – hydrogen (H2), nitrogen (N2), oxygen (O2), fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2)

They are referred to by their element names and do not end in “ide” (hockey stick and puck on periodic table)

Binary Covalent Binary Covalent CompoundsCompounds

Binary Covalent CompoundsBinary Covalent Compounds Do not reduce covalent compounds (SDo not reduce covalent compounds (S22ClCl22

does not become SCl)does not become SCl) Greek prefixes are used in naming, the Greek prefixes are used in naming, the

second element ends in “ide”second element ends in “ide” ““mono” need not be used with the first mono” need not be used with the first

element but usually is with the secondelement but usually is with the second For element names that begin with a For element names that begin with a

vowel (oxygen, iodine), the “o” or “a” of vowel (oxygen, iodine), the “o” or “a” of the prefix is dropped (e.g. monoxide); the the prefix is dropped (e.g. monoxide); the “i” in di and tri is “i” in di and tri is nevernever dropped dropped

Name the followingName the following

antimony tribromideantimony tribromide SbBrSbBr33 P P44SS5 5 tetraphosphorus pentasulfide tetraphosphorus pentasulfide

chlorine dioxidechlorine dioxide ClOClO22 SeF SeF66 selenium hexafluoride selenium hexafluoride

iodine pentafluorideiodine pentafluoride IFIF55 SCl SCl44 sulfur tetrachloride sulfur tetrachloride

ammoniaammonia NHNH33 B B22SiSi diboron monosilicide diboron monosilicide

hexaboron monosilicidehexaboron monosilicide BB66Si Si O O22 oxygen oxygen

hydrogen moniodidehydrogen moniodide HI HI Si Si22BrBr66 disilicon hexabromide disilicon hexabromide

dinitrogen trioxidedinitrogen trioxide NN22OO33 CH CH44 methane methane

phosphorus triiodidephosphorus triiodide PIPI33 NF NF33 nitrogen trifluoride nitrogen trifluoride

Hydrated SaltsHydrated Salts Hydrated salts are salts that contain Hydrated salts are salts that contain

molecules of water within the crystal molecules of water within the crystal structure. (Remember the word salt structure. (Remember the word salt simply means an ionic compound)simply means an ionic compound)

The formula of a hydrate includes a “dot” The formula of a hydrate includes a “dot” and the number of water molecules:and the number of water molecules:

CuSOCuSO44•5H•5H22OO

We add the word “hydrate” to the name We add the word “hydrate” to the name with the proper Greek prefix to indicate with the proper Greek prefix to indicate the number of water moleculesthe number of water molecules

Hydrated Salts Cont’dHydrated Salts Cont’d

CuSOCuSO44•5H•5H22OO is calledis called

Copper (II) sulfate pentahydrateCopper (II) sulfate pentahydrate

Practice:Practice:

FeClFeCl22•6H•6H22O O

magnesium sulfite heptahydrate magnesium sulfite heptahydrate

iron (II) chloride hexahydrate iron (II) chloride hexahydrate

MgSOMgSO33•7H•7H22

OO

Binary AcidsBinary Acids Binary acids contain H and one other Binary acids contain H and one other

non-metallic elementnon-metallic element

They are named as “They are named as “hydrohydroelementelementicic acidacid””

The bonds are covalent; but when The bonds are covalent; but when naming acids, the rules for ionic naming acids, the rules for ionic compounds apply, because acids form compounds apply, because acids form ions in solutionions in solution

They are aqueous substances and They are aqueous substances and MUST have (aq) written after themMUST have (aq) written after them

Binary Acids Cont’dBinary Acids Cont’d

For Example:For Example:

HCl(aq) is HCl(aq) is hydrochloric hydrochloric acid acid BUTBUT HCl(g) is HCl(g) is hydrogen hydrogen chloridechloride

Name: Name: HF(aq) HF(aq)

HH22S(aq)S(aq)

hydrofluoric acidhydrosulfuric acid

Ternary Acids (aka Ternary Acids (aka Oxyacids)Oxyacids)

These occur in the form: HThese occur in the form: HaaXXbbOOc c where X where X is any element.is any element.

““ate”ate” changes to “ic acid”changes to “ic acid”

““ite” changes to “ous acid”ite” changes to “ous acid”HNOHNO33 (aq) nitric acid (aq) nitric acid HNO HNO22 (aq) nitrous acid (aq) nitrous acid

HH22SOSO4 4 (aq) (aq) H H22SOSO33 (aq) (aq)

HClOHClO44 (aq) (aq) HClO HClO22 (aq) (aq)

phosphoric acidphosphoric acid

sulfuric acid sulfurous acid

perchloric acid chlorous acidH3PO4 (aq)

Acid SaltsAcid Salts

Acids salts are salts whose anion have an Acids salts are salts whose anion have an added H atom covalently bonded.added H atom covalently bonded.

They combine with cations just as anions They combine with cations just as anions dodo

These salts form when a diprotic or These salts form when a diprotic or triprotic acid is partially neutralizedtriprotic acid is partially neutralized

Acid salts can act as an acid or a base, Acid salts can act as an acid or a base, depending on the conditions in the solutiondepending on the conditions in the solution

Examples:Examples:

COCO332-2- carbonate carbonate HCOHCO33

-- hydrogen hydrogen carbonate carbonate (bicarbonate)(bicarbonate)

SOSO442-2- sulfate sulfate HSOHSO44

-- hydrogen sulfate hydrogen sulfate (bisulfate)(bisulfate)

SOSO332-2- sulfite sulfite HSOHSO33

-- hydrogen sulfite hydrogen sulfite

(bisulfite)(bisulfite)

POPO443-3- phosphate phosphate HPOHPO44

2-2- hydrogen hydrogen phosphatephosphate

HH22POPO44-- dihydrogen dihydrogen

phosphatephosphate

Acid Salts Cont’dAcid Salts Cont’d

Name the followingName the followingsodium hydrogen carbonatesodium hydrogen carbonate

or or sodium bicarbonatesodium bicarbonate

potassium hydrogen phosphatepotassium hydrogen phosphate

magnesium hydrogen sulfitemagnesium hydrogen sulfite

or or magnesium bisulfitemagnesium bisulfite

aluminum dihydrogen phosphatealuminum dihydrogen phosphate

NaHCONaHCO33

KK22HPOHPO44

Mg(HSOMg(HSO33))22

Al(HAl(H22POPO44))33