Ionic CompoundsIonic Compounds

NomenclatureNomenclature

IntroductionIntroduction•We use the periodic table to tell us the most

commonly expected charges for the ions of elements.•We use the periodic table to tell us the most

commonly expected charges for the ions of elements.

•For example:•Group 1 (1A) elements have a 1+ charge.

•Na becomes Na+

•Group 2 (2A) elements have a 2+ charge.•Mg becomes Mg2+

•Group 13 (3A) elements have a 3+ charge.•Al becomes Al3+

•For example:•Group 1 (1A) elements have a 1+ charge.

•Na becomes Na+

•Group 2 (2A) elements have a 2+ charge.•Mg becomes Mg2+

•Group 13 (3A) elements have a 3+ charge.•Al becomes Al3+

IntroductionIntroduction•We use the periodic table to tell us the most

commonly expected charges for the ions of elements.•We use the periodic table to tell us the most

commonly expected charges for the ions of elements.

•For example:•Group 15 (5A) elements have a 3- charge.

•N becomes N3-

•Group 16 (6A) elements have a 2- charge.•O becomes O2-

•Group 17 (7A) elements have a 1- charge.•Cl becomes Cl-

•For example:•Group 15 (5A) elements have a 3- charge.

•N becomes N3-

•Group 16 (6A) elements have a 2- charge.•O becomes O2-

•Group 17 (7A) elements have a 1- charge.•Cl becomes Cl-

Forming Ionic Compounds

Forming Ionic Compounds

•We form ionic compounds by matching the charges of the ions to form a neutral compound.

•We form ionic compounds by matching the charges of the ions to form a neutral compound.

•For example:•Combining Na+ with Cl- gives NaCl.

•Combining Ca2+ with S2- gives CaS.

•Combining Ga3+ with N3- gives GaN.

•Each of these combinations gives a neutral compound.

•For example:•Combining Na+ with Cl- gives NaCl.

•Combining Ca2+ with S2- gives CaS.

•Combining Ga3+ with N3- gives GaN.

•Each of these combinations gives a neutral compound.

Forming Ionic Compounds

Forming Ionic Compounds

•More complex combinations of ions also need to be balanced to produce neutral compounds.

•More complex combinations of ions also need to be balanced to produce neutral compounds.

•For example:•Combining Na+ with O2- gives Na2O.

•Combining Ca2+ with Br- gives CaBr2.

•Combining Al3+ with F- gives AlF3.

•Each of these combinations gives a neutral compound.

•For example:•Combining Na+ with O2- gives Na2O.

•Combining Ca2+ with Br- gives CaBr2.

•Combining Al3+ with F- gives AlF3.

•Each of these combinations gives a neutral compound.

Forming Ionic Compounds

Forming Ionic Compounds

•For even more complex combinations of ions we use a trick to produce neutral compounds.

•For even more complex combinations of ions we use a trick to produce neutral compounds.

•For example:•Combining Ca2+ with N3-:

•For example:•Combining Ca2+ with N3-:CaCa2+2+ NN3-3-

•To find the proper number of Ca2+, we use the 3 of the N3-.

•To find the proper number of N3-, we use the 2 of the Ca2+.

•To find the proper number of Ca2+, we use the 3 of the N3-.

•To find the proper number of N3-, we use the 2 of the Ca2+.

3322CaCa NN

•We can use this “criss-cross” when ever we have a complex combination of ions.

•We can use this “criss-cross” when ever we have a complex combination of ions.

Binary Ion NomenclatureBinary Ion Nomenclature•When we name binary ionic compounds (ionic

compounds made from the ions of two elements), we name the cation first followed by the anion.

•When we name binary ionic compounds (ionic compounds made from the ions of two elements), we name the cation first followed by the anion.

•In general, cations that are metals are given the name of the elemental metal.

•NaCl is named sodium chloride.

•BaF2 is named barium fluoride.

•Ca3P2 is named calcium phosphide.

•In general, cations that are metals are given the name of the elemental metal.

•NaCl is named sodium chloride.

•BaF2 is named barium fluoride.

•Ca3P2 is named calcium phosphide.

Binary Ion NomenclatureBinary Ion Nomenclature•When we name binary ionic compounds (ionic

compounds made from the ions of two elements), we name the cation first followed by the anion.

•When we name binary ionic compounds (ionic compounds made from the ions of two elements), we name the cation first followed by the anion.

•In general, anions are given the name of the element followed by the suffix “-ide.”

•NaCl is named sodium chloride.

•BaF2 is named barium fluoride.

•Ca3P2 is named calcium phosphide.

•In general, anions are given the name of the element followed by the suffix “-ide.”

•NaCl is named sodium chloride.

•BaF2 is named barium fluoride.

•Ca3P2 is named calcium phosphide.

Binary Ion NomenclatureBinary Ion Nomenclature•The single element anions are:•The single element anions are:

CC NN OO FF

PP SS ClCl

SeSe BrBr

II

AsAs

fluoridefluoride

chloridechloride

bromidebromide

iodideiodide

sulfidesulfide

oxideoxide

selenideselenide

nitridenitride

phosphidephosphide

arsenidearsenide

1-1-2-2-3-3-

Binary Ion NomenclatureBinary Ion Nomenclature•Transition (d-block) metals most commonly

have a 2+ charge.•Transition (d-block) metals most commonly

have a 2+ charge.

ScSc TiTi VV CrCr MnMn FeFe CoCo NiNi CuCu ZnZn

YY ZrZr NbNb MoMo TcTc RuRu RhRh PdPd AgAg CdCd

LuLu HfHf TaTa WW ReRe OsOs IrIr PtPt AuAu HgHg

LrLr RfRf DbDb SgSg BhBh HsHs MtMt DsDs RgRgUubUub

TiTi2+2+ScSc2+2+

MoMo2+2+

• There are exceptions to this rule.There are exceptions to this rule.• Some transition and main group metals Some transition and main group metals have two orhave two or

more common charges.more common charges.

VV2+2+, V, V3+3+, V, V4+4+CrCr2+2+, Cr, Cr3+3+MnMn2+2+, Mn, Mn3+3+FeFe2+2+, Fe, Fe3+3+CoCo2+2+, Co, Co3+3+CuCu++, Cu, Cu2+2+

GaGa

InIn

TlTl

SnSn

PbPb BiBi PoPo

PbPb2+2+, Pb, Pb4+4+

SnSn2+2+, Sn, Sn4+4+ZnZn2+2+

AgAg++

AuAu++, Au, Au3+3+

Binary Ion NomenclatureBinary Ion Nomenclature•Since these cations can have different

charges, we need a nomenclature that will distinguish between the different cations.

•The Stock system is used to identify different ions.

•We use the element name followed by the charge of the ion in parenthesis.

•For example:•Cu+ is written as copper(I)•Cu2+ is written as copper(II)•Pb2+ is written as lead(II)•Pb4+ is written as lead(IV)

•Since these cations can have different charges, we need a nomenclature that will distinguish between the different cations.

•The Stock system is used to identify different ions.

•We use the element name followed by the charge of the ion in parenthesis.

•For example:•Cu+ is written as copper(I)•Cu2+ is written as copper(II)•Pb2+ is written as lead(II)•Pb4+ is written as lead(IV)

Binary Ion NomenclatureBinary Ion Nomenclature•Examples of Stock nomenclature:

•CuCl = copper(I) chloride•CuCl2 = copper(II) chloride

•FeO = iron(II) oxide•Fe2O3 = iron(III) oxide

•PbS = lead(II) sulfide•PbS2 = lead(IV) sulfide

•VO = vanadium(II) oxide•V2O3 = vanadium(III) oxide•VO2 = vanadium(IV) oxide

•Examples of Stock nomenclature:

•CuCl = copper(I) chloride•CuCl2 = copper(II) chloride

•FeO = iron(II) oxide•Fe2O3 = iron(III) oxide

•PbS = lead(II) sulfide•PbS2 = lead(IV) sulfide

•VO = vanadium(II) oxide•V2O3 = vanadium(III) oxide•VO2 = vanadium(IV) oxide

Polyatomic Ion NomenclaturePolyatomic Ion Nomenclature

•Polyatomic ions are single ions that are made up of several atoms.

•Examples of polyatomic ions include:•nitrate: NO3

-

•sulfate: SO42-

•phosphate: PO43-

•ammonium: NH4+

•nitrite: NO2-

•hydroxide: OH-

•dimercury: Hg22+

•acetate: CH3COO-

•Polyatomic ions are single ions that are made up of several atoms.

•Examples of polyatomic ions include:•nitrate: NO3

-

•sulfate: SO42-

•phosphate: PO43-

•ammonium: NH4+

•nitrite: NO2-

•hydroxide: OH-

•dimercury: Hg22+

•acetate: CH3COO-

Polyatomic Ion NomenclaturePolyatomic Ion Nomenclature•Each of these units acts as a single ion.

•Nitrate (1-)acts in the same manner as chloride.•Sodium nitrate is NaNO3.•Calcium nitrate is Ca(NO3)2.•Aluminum nitrate is Al(NO3)3.

•Sulfate (2-) acts in the same manner as oxide.•Sodium sulfate is Na2SO4.•Calcium sulfate is CaSO4.•Aluminum sulfate is Al2(SO4)3.

•Phosphate (3-) acts in the same manner as nitride.•Sodium phosphate is Na3PO4.•Calcium phosphate is Ca3(PO4)2

•Aluminum phosphate is AlPO4.

•Each of these units acts as a single ion.•Nitrate (1-)acts in the same manner as chloride.

•Sodium nitrate is NaNO3.•Calcium nitrate is Ca(NO3)2.•Aluminum nitrate is Al(NO3)3.

•Sulfate (2-) acts in the same manner as oxide.•Sodium sulfate is Na2SO4.•Calcium sulfate is CaSO4.•Aluminum sulfate is Al2(SO4)3.

•Phosphate (3-) acts in the same manner as nitride.•Sodium phosphate is Na3PO4.•Calcium phosphate is Ca3(PO4)2

•Aluminum phosphate is AlPO4.

Polyatomic Ion NomenclaturePolyatomic Ion Nomenclature•Cations:Cations:

ammonium: NHammonium: NH44++ dimercury: Hgdimercury: Hg22

2+2+

•Anions:Anions:nitrate: NOnitrate: NO33

--

nitrite: NOnitrite: NO22--

cyanide: CNcyanide: CN--

hydroxide: OHhydroxide: OH--

perchlorate: ClOperchlorate: ClO44--

chlorate: ClOchlorate: ClO33--

chlorite: ClOchlorite: ClO22--

hypochlorite: ClOhypochlorite: ClO--

acetate: CH3COOacetate: CH3COO--

hydrogen carbonate: hydrogen carbonate: HCOHCO33

--

sulfate: SOsulfate: SO442-2-

sulfite: SOsulfite: SO332-2-

carbonate: COcarbonate: CO332-2-

chromate: CrOchromate: CrO442-2-

dichromate: Crdichromate: Cr22OO772-2-

silicate: SiOsilicate: SiO332-2-

oxalate: Coxalate: C22OO442-2-

phosphate: POphosphate: PO443-3-

phosphite: POphosphite: PO333-3-

Polyatomic Ion NomenclaturePolyatomic Ion Nomenclature•When we form ionic compounds from When we form ionic compounds from

polyatomic ions, we treat the polyatomic polyatomic ions, we treat the polyatomic ions as individual units of charge.ions as individual units of charge.

BaBa2+2+ (NO(NO33))--

We use the criss-cross trick to find the formula We use the criss-cross trick to find the formula of the compound.of the compound.

Ba(NOBa(NO33))22

•For example:For example:

•barium 2+ and nitrate 1-barium 2+ and nitrate 1-

barium barium nitratenitrate

Polyatomic Ion NomenclaturePolyatomic Ion Nomenclature•When we form ionic compounds from When we form ionic compounds from

polyatomic ions, we treat the polyatomic polyatomic ions, we treat the polyatomic ions as individual units of charge.ions as individual units of charge.

(NH(NH44))++ (SO(SO44))2-2-

We use the criss-cross trick to find the formula We use the criss-cross trick to find the formula of the compound.of the compound.

(NH(NH44))22SOSO44

•For example:For example:

•ammonium 1+ and sulfate 2-ammonium 1+ and sulfate 2-

ammonium ammonium sulfatesulfate

Knowledge CheckKnowledge Check

•Determine the formulas of the following compounds:

1.sodium carbonate

2.copper(II) sulfate

3.lead(IV) phosphate

4.aluminum nitrite

5.ammonium sulfide

•Determine the formulas of the following compounds:

1.sodium carbonate

2.copper(II) sulfate

3.lead(IV) phosphate

4.aluminum nitrite

5.ammonium sulfide

NaNa22COCO33

CuSOCuSO44

PbPb33(PO(PO44))44

Al(NOAl(NO22))33

(NH(NH44))22SS

NaNa++ (CO(CO33))2-2-

CuCu2+2+ (SO(SO44))2-2-

PbPb4+4+ (PO(PO44))3-3-

AlAl3+3+ (NO(NO22))--

(NH(NH44))++ SS2-2-

Knowledge CheckKnowledge Check

•Determine the names of the following compounds:

1.Fe2(CrO4)3

2.VO2

•Cr(CH3COO)2

1.AuPO4

2.NaClO

•Determine the names of the following compounds:

1.Fe2(CrO4)3

2.VO2

•Cr(CH3COO)2

1.AuPO4

2.NaClO

iron(III) chromateiron(III) chromate

vanadium(IV) oxidevanadium(IV) oxide

chromium(II) acetatechromium(II) acetate

gold(III) phosphategold(III) phosphate

sodium hypochloritesodium hypochlorite