NOMENCLATURENOMENCLATURE

Chapter 5Chapter 5

Charges on Common IonsCharges on Common Ions

+1

+2 +3

-4 -3 -2 -1

Table 5.1: Common Simple Cations and AnionsTable 5.1: Common Simple Cations and Anions

Chemical BondsChemical Bonds

- the forces that hold two or more atoms - the forces that hold two or more atoms together to form a compound.together to form a compound.

- the two types of chemical bonds are:- the two types of chemical bonds are:

1. Ionic bonds.1. Ionic bonds.

NaCl KINaCl KI

2. Covalent bonds.2. Covalent bonds.

HH22O CHO CH44

metal & nonmetal

two nonmetals

Chemical Bonds(continued)

Chemical Bonds(continued)

Ionic BondingIonic Bonding: : Force of attraction Force of attraction between oppositely charged ions.between oppositely charged ions.

- Chemical compounds must have a net - Chemical compounds must have a net charge of zero.charge of zero.

1. Both cations and anions must be present.1. Both cations and anions must be present.

2. The number of cations and anions must 2. The number of cations and anions must be such that the net charge is zero.be such that the net charge is zero.

Writing Formulas for Ionic Compounds

Writing Formulas for Ionic Compounds

-23

32

12

2

-11

SAl

FCa

ClNa

Charge must equal zero for each compound.

1+ & 1- = 0

2+ & 2- = 0

6+ & 6- = 0

COMPOUNDS FORMED COMPOUNDS FORMED FROM IONSFROM IONS

COMPOUNDS FORMED COMPOUNDS FORMED FROM IONSFROM IONS

CATION + CATION + ANION ---> ANION --->

COMPOUNDCOMPOUND

NaNa++ + Cl + Cl- - --> NaCl--> NaCl

A neutral compound A neutral compound requires equal requires equal number of (+) number of (+) and and (-) charges.(-) charges.

Chemical Bonds(continued)

Chemical Bonds(continued)

Covalent bonding:Covalent bonding: results from atoms results from atoms sharing electronssharing electrons..

MoleculeMolecule: a collection of covalently-: a collection of covalently-bonded atoms.bonded atoms.

HH22O CO C1212HH2222OO1111

Common NamesCommon Names

sugar of leadsugar of lead

blue vitriolblue vitriol

quicklimequicklime

Epsom saltsEpsom salts

milk of magnesiamilk of magnesia

gypsumgypsum

laughing gaslaughing gas

lead(II) acetatecopper(II) sulfatecalcium oxidemagnesium sulfate

magnesium

hydroxide

calcium sulfatedinitrogen monoxide

Common Names - Exceptions

HH22O = water, steam, iceO = water, steam, ice

NHNH33 = ammonia = ammonia

CHCH44 = methane = methane

NaCl = table saltNaCl = table salt

CC1212HH2222OO1111 = table sugar = table sugar

Types of CationsTypes of Cations

Type I Cations:Type I Cations: only one chargeonly one charge Group I ionsGroup I ions Group II ionsGroup II ions AluminumAluminum CadmiumCadmium SilverSilver ZincZinc Memorize Table 5.1, Memorize Table 5.1,

page 129page 129

Type II Cations:Type II Cations:•more than one chargemore than one charge•transition elementstransition elements•elements under the elements under the

stairstepstairstep•Memorize Table 5.2, Memorize Table 5.2,

page 133page 133

Metal CationsType I Type I

Metals that can only have one possible chargeMetals that can only have one possible charge Determine charge by position on the Periodic Determine charge by position on the Periodic

TableTable

Type IIType II Metals that can have more than one possible Metals that can have more than one possible

chargecharge Determine metal cation’s charge from the Determine metal cation’s charge from the

charge on anioncharge on anion

Naming CompoundsNaming Compounds

1. Cation first, then anion1. Cation first, then anion

2. Monatomic cation = name of the element2. Monatomic cation = name of the element

CaCa2+2+ = = calciumcalcium ionion

3. Monatomic anion = 3. Monatomic anion = rootroot + + -ide-ide

ClCl = = chlorchlorideide

CaClCaCl22 = = calcium chlorcalcium chlorideide

Binary Ionic Binary Ionic Compounds:Compounds:

Naming Compounds(continued)

Naming Compounds(continued)

-- metal forms more than one metal forms more than one cationcation

-- use use Roman numeral Roman numeral in namein name

CuClCuCl2 2 CuCu2+2+ is cationis cation

CuClCuCl22 = Copper ( = Copper (IIII) chloride) chloride

Cupric chlorideCupric chloride

Binary Ionic Compounds (Type Binary Ionic Compounds (Type II):II):

Naming Compounds(continued)

Naming Compounds(continued)

-- Compounds between two Compounds between two nonmetalsnonmetals-- First element First element in the formula is in the formula is named firstnamed first..-- Second element Second element is named as if it were an is named as if it were an anionanion..-- Use prefixes (Table 5.3 on page 137).Use prefixes (Table 5.3 on page 137).-- Never use Never use mono- mono- for the first element.for the first element.

PP22OO55 = = didiphosphorus phosphorus pentpentoxideoxide

Binary compounds (Type III):Binary compounds (Type III):

Prefixes

Drop last “a” in the prefix if the name begins with vowelDrop last “a” in the prefix if the name begins with vowel

octa-8

hepta-7

hexa-6

penta-5

tetra-4

tri-3

di-2

mono-

(not used on first nonmetal)

1

PrefixSubscript

Figure 5.1: A flow chart for naming binary compounds.

Figure 5.1: A flow chart for naming binary compounds.

Common Nomenclature Mistakes

Common Nomenclature Mistakes

Compounds: Compounds:

SOSO3 3 --Sulfur trioxide--Sulfur trioxide

NONO22 -- Nitrogen -- Nitrogen dioxide dioxide

NONO33 -- Nitrogen -- Nitrogen trioxide trioxide

NHNH33 -- Ammonia -- Ammonia

Polyatomic ions:Polyatomic ions:

SOSO332-2- -- Sulfite ion -- Sulfite ion

NONO221-1- -- Nitrite ion -- Nitrite ion

NONO331- 1- -- Nitrate ion-- Nitrate ion

NHNH441+1+ --Ammonium --Ammonium

ion ion

MOLECULAR FORMULASMOLECULAR FORMULAS

Formula for glycine is Formula for glycine is CC22HH55NONO22

In one molecule there areIn one molecule there are 2 C atoms2 C atoms 5 H atoms5 H atoms 1 N atom1 N atom 2 O atoms2 O atoms

Molecular ModelingMolecular Modeling

C

H

H C

H

H

O

O HN

Ball & stickBall & stick Space-fillingSpace-filling

Drawing of glycineDrawing of glycine

POLYATOMIC IONSPOLYATOMIC IONS

Groups of atoms with a charge.Groups of atoms with a charge.

MEMORIZEMEMORIZE the names and formulas the names and formulas

in Table 5.4, page 142.in Table 5.4, page 142.

Table 5.4: Names of Common Polyatomic IonsTable 5.4: Names of Common Polyatomic Ions

Patterns for Polyatomic Ions

-ate ion-ate ion chlorate = ClOchlorate = ClO33

--

-ate ion plus 1 O -ate ion plus 1 O same charge, same charge, per-per- prefix prefix perchlorate = ClOperchlorate = ClO44

--

-ate ion minus 1 O -ate ion minus 1 O same charge, - same charge, -iteite suffix suffix chlorite = ClOchlorite = ClO22

--

-ate ion minus 2 O -ate ion minus 2 O same charge, same charge, hypo-hypo- prefix, - prefix, -iteite suffixsuffix hypochlorite = ClOhypochlorite = ClO--

Some Common Some Common Polyatomic IonsPolyatomic Ions

NHNH44+ + ammonium ion One of the ammonium ion One of the

few common polyatomic few common polyatomic cationscations

Some Common Some Common Polyatomic IonsPolyatomic Ions

COCO332- 2- carbonate ion carbonate ion

HCOHCO33- - bicarbonate ionbicarbonate ion

- hydrogen carbonate ion- hydrogen carbonate ion

SOSO442- 2- sulfate ionsulfate ion

SOSO332- 2- sulfite ionsulfite ion

Some Common Polyatomic Some Common Polyatomic IonsIons

NONO33- - nitrate ionnitrate ion

NONO22- - nitrite ionnitrite ion

Some Common Some Common Polyatomic IonsPolyatomic Ions

Figure 5.2: Overall strategy for naming chemical compounds

Figure 5.2: Overall strategy for naming chemical compounds

NOMENCLATURE OF COMPOUNDS Binary -- 2 elements Ternary -- (3 elements) - Ionic

(metal ion + polyatomic ion)

Ca3(PO4)2 -- calcium phosphate FeSO4 -- iron (II) sulfate

-- ferrous sulfate

Type I - Ionic(Type I metal + nonmetal)Group I, II, Al+3, Ag1+,Cd2+, & Zn2+

NaCl -- Sodium Chloride

Type II - Ionic(Type II metal + nonmetal)All other metalsFe2S3 -- iron (III) sulfide -- ferric sulfide

Type III - covalent(2 nonmetals)CO2 -- carbon dioxide

Binary AcidsBinary Acids

• made up of made up of twotwo elements -- elements -- hydrogenhydrogen and a and a nonmetalnonmetal

• named by using:named by using:

prefix hydro + root of nonmetal + ic + acidprefix hydro + root of nonmetal + ic + acid

HCl -- hydrochloric acidHCl -- hydrochloric acid

HH22Se -- hydroselenic acidSe -- hydroselenic acid

Table 5.5: Names of Acids that Do Not Contain Oxygen

Table 5.5: Names of Acids that Do Not Contain Oxygen

Ternary Acids (oxyacids) Ternary Acids (oxyacids)

• contain contain threethree elements -- elements -- hydrogenhydrogen, , nonmetalnonmetal, , and and oxygenoxygen..

• most oxygenmost oxygen per + root of nonmetal + ic + per + root of nonmetal + ic + acidacid

• less oxygenless oxygen root of nonmetal + ic + acidroot of nonmetal + ic + acid

• less oxygenless oxygen root of nonmetal + ous + acidroot of nonmetal + ous + acid

• least oxygenleast oxygen hypo + root of nonmetal + hypo + root of nonmetal + ous + acidous + acid

Ternary Acids(continued)

Ternary Acids(continued)

HBrOHBrO44 perbromic acid perbromic acid

HBrOHBrO3 3 bromic acidbromic acid

HBrOHBrO22 bromous acid bromous acid

HBrOHBrO hypobromous acidhypobromous acid

HH33POPO44 phosphoric acid phosphoric acid

HH33POPO3 3 phosphorous acidphosphorous acid

HH33POPO22 hypophosphorus acid hypophosphorus acid

Figure 5.3: A flow chart for naming

acids

Figure 5.3: A flow chart for naming

acids

Salt Nomenclature (continued)Salt Nomenclature (continued)Ternary salts ( metal and polyatomic ion)Ternary salts ( metal and polyatomic ion)

name of positive ion + root of nonmetal + ate or itename of positive ion + root of nonmetal + ate or ite

If the salt comes from anIf the salt comes from an ic ic acid, changeacid, change ic ic toto ate.ate.

HH22COCO33 carboncarbonicic acidacid NaNa22COCO33 sodium sodium carboncarbonateate

HH33POPO44 phosphorphosphoricic acid acid KK33POPO44 potassiumpotassium phosphphosphateate

If the salt comes from anIf the salt comes from an ousous acid, changeacid, change ousous toto ite.ite.

HH22SOSO33 sulfursulfurousous acid acid LiLi22SOSO33 lithium lithium sulfsulfiteite

HClOHClO hypohypochlorchlorousous acid acid NaClONaClO sodium sodium hypohypochlorchloriteite

Chemical NomenclatureChemical Nomenclature

Name each of the following:Name each of the following:

CuCl CuCl

HgOHgO

FeFe22OO33

MnOMnO22

PbClPbCl22

CrClCrCl33

copper(I) chloride cuprous chloridemercury(II) oxide mercuric oxide

iron(III) oxide ferric oxide

manganese(IV) oxide manganic oxide

lead(II) chloride plumbous chloride

chromium(III) chloride chromic chloride

Chemical NomenclatureChemical Nomenclature

Name each of the following:Name each of the following:

PP44OO1010

NN22OO55

LiLi22OO22

Ti(NOTi(NO33))44

SOSO33

SFSF66

OO22FF22

tetraphosphorus decoxidedinitrogen pentoxide

lithium peroxide

titanium(IV) nitrate

sulfur trioxide

sulfur hexafluoride

dioxygen difluoride

Writing the Formulas from the Names

For Type III compounds, use the prefixes to For Type III compounds, use the prefixes to determine the subscripts determine the subscripts

For Type I, Type II, polyatomic Compounds For Type I, Type II, polyatomic Compounds and Acidsand Acids Determine the ions presentDetermine the ions present Determine the charges on the cation and anionDetermine the charges on the cation and anion Balance the charges to get the subscriptsBalance the charges to get the subscripts

Determining the Charge on a Cation – Au2S3

Determine the charge on the anionDetermine the charge on the anion

AuAu22SS33 - the anion is S, since it is in Group 6A, its charge is -2 - the anion is S, since it is in Group 6A, its charge is -2

Determine the total negative chargeDetermine the total negative chargesince there are 3 S in the formula, the total negative charge is -since there are 3 S in the formula, the total negative charge is -66

Determine the total positive chargeDetermine the total positive chargesince the total negative charge is -6, the total positive charge is since the total negative charge is -6, the total positive charge is +6+6

Divide by the number of cationsDivide by the number of cationssince there are 2 Au in the formula & the total positive charge since there are 2 Au in the formula & the total positive charge is +6, each Au has a +3 chargeis +6, each Au has a +3 charge