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
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