Chapter 7 “Ionic Bonding” Chemistry Section 7.1 - Ions OBJECTIVES: OBJECTIVES: Determine the number of valence electrons in an atom of a representative

Chapter 7Chapter 7

“Ionic Bonding”“Ionic Bonding”

ChemistryChemistry

Section 7.1 - IonsSection 7.1 - Ions

OBJECTIVES:OBJECTIVES:

DetermineDetermine the number the number of of valence electronsvalence electrons in an atom of a in an atom of a representative element.representative element.



ExplainExplain how the octet how the octet rule applies to atoms of rule applies to atoms of metallic and metallic and nonmetallic elements.nonmetallic elements.



DescribeDescribe how how cationscations form.form.



ExplainExplain how how anionsanions form.form.

Valence Electrons are…?Valence Electrons are…?

The electrons responsible for the The electrons responsible for the chemical properties of atoms, and chemical properties of atoms, and are those in the are those in the outerouter energy energy level.level.

Valence electronsValence electrons - The - The ss and and pp electrons in the outer energy levelelectrons in the outer energy levelthe highest occupied energy levelthe highest occupied energy level

Core electronsCore electrons – are those in the – are those in the energy levels below.energy levels below.

Keeping Track of ElectronsKeeping Track of Electrons Atoms in the same column...Atoms in the same column...

1)1) Have the same outer electron Have the same outer electron configuration.configuration.

2)2) Have the same valence electrons.Have the same valence electrons. The number of valence electrons The number of valence electrons

are easily determined. It is the are easily determined. It is the group numbergroup number for a for a representative elementrepresentative element

Group 2: Be, Mg, Ca, etc.Group 2: Be, Mg, Ca, etc. have 2 valence electronshave 2 valence electrons

Electron Dot diagrams are…Electron Dot diagrams are…A way of showing & keeping A way of showing & keeping

track of valence electrons.track of valence electrons.How to write them?How to write them?Write the symbol - it Write the symbol - it

represents the nucleus and represents the nucleus and inner (core) electronsinner (core) electrons

Put one dot for each valence Put one dot for each valence electron (electron (8 maximum8 maximum))

They don’t pair up until they They don’t pair up until they have to (Hund’s rule)have to (Hund’s rule)

X

The Electron Dot diagram for Nitrogen

Nitrogen has 5 valence electrons to show.

First we write the symbol. NThen add 1 electron at a time to each side.Now they are forced to pair up.

We have now written the electron dot diagram for Nitrogen.

The Octet Rule In Chapter 6, we learned that noble gases

are unreactive in chemical reactions In 1916, Gilbert Lewis used this fact to

explain why atoms form certain kinds of ions and molecules

The Octet Rule: in forming compounds, atoms tend to achieve a noble gas configuration; 8 in the outer level is stableEach noble gas (except He, which has

2) has 8 electrons in the outer level

Formation of CationsFormation of CationsMetals Metals loselose electrons electrons to attain a noble to attain a noble

gas configuration.gas configuration.They make positive ions They make positive ions (cations)(cations)If we look at the electron configuration, If we look at the electron configuration,

it makes sense to lose electrons:it makes sense to lose electrons:Na Na 1s1s222s2s222p2p663s3s11 1 valence electron 1 valence electronNaNa1+1+ 1s1s222s2s222p2p66 This is a noble gas This is a noble gas

configuration with 8 electrons in the configuration with 8 electrons in the outer level.outer level.

Electron Dots For CationsElectron Dots For Cations

Metals will have few valence Metals will have few valence electrons (usually 3 or less); calcium electrons (usually 3 or less); calcium has only 2 valence electronshas only 2 valence electrons

Ca


Metals will have few valence electronsMetals will have few valence electronsMetals will Metals will lose the valence electronslose the valence electrons

Ca


Metals will have few valence electronsMetals will have few valence electronsMetals will Metals will lose the valence electronslose the valence electronsForming positive ionsForming positive ions

Ca2+NO DOTS are now shown for the cation.

This is named the “calcium ion”.


Let’s do Let’s do ScandiumScandium, #21, #21The electron configuration is: The electron configuration is:

1s1s222s2s222p2p663s3s223p3p664s4s223d3d11

Thus, it can lose 2eThus, it can lose 2e-- (making (making it 2+), or lose 3eit 2+), or lose 3e-- (making (making 3+)3+)

ScSc = = ScSc2+ 2+ Scandium (II) ion Scandium (III) ion

Sc = Sc3+


Let’s do Let’s do SilverSilver, element #47, element #47PredictedPredicted configuration is: configuration is:

1s1s222s2s222p2p663s3s223p3p664s4s223d3d10104p4p665s5s224d4d99

ActualActual configuration is: configuration is: 1s1s222s2s222p2p663s3s223p3p664s4s223d3d10104p4p665s5s114d4d1010

Ag = AgAg = Ag++ (can’t lose any more, (can’t lose any more, charges of 3+ or greater are uncommon)charges of 3+ or greater are uncommon)


Silver did the best job it Silver did the best job it could, but it did not could, but it did not achieve a achieve a truetrue Noble Gas Noble Gas configurationconfiguration

Instead, it is called a Instead, it is called a “pseudo-noble gas “pseudo-noble gas configuration”configuration”

Electron Configurations: Electron Configurations: AnionsAnionsNonmetals Nonmetals gaingain electrons electrons to attain to attain

noble gas configuration.noble gas configuration.They make negative ions They make negative ions (anions)(anions)SS = = 1s1s222s2s222p2p663s3s223p3p44 = 6 valence = 6 valence

electronselectronsSS2-2- = = 1s1s222s2s222p2p663s3s223p3p66 = noble gas = noble gas

configuration. configuration. Halide ionsHalide ions are ions from chlorine are ions from chlorine

or other halogens that gain or other halogens that gain electronselectrons

Electron Dots For AnionsElectron Dots For Anions

Nonmetals will have many valence Nonmetals will have many valence electrons (usually 5 or more)electrons (usually 5 or more)

They will They will gaingain electrons to fill outer shell. electrons to fill outer shell.

P 3-(This is called the “phosphide ion”, and should show dots)

Stable Electron Stable Electron ConfigurationsConfigurations

All atoms react to try and achieve a All atoms react to try and achieve a noble gas configuration.noble gas configuration.

Noble gases have 2 s and 6 p electrons.Noble gases have 2 s and 6 p electrons.8 valence electrons = already stable!8 valence electrons = already stable!This is the This is the octet ruleoctet rule (8 in the outer (8 in the outer

level is particularly stable).level is particularly stable).

Ar

Section 7.2 Ionic Bonds and Section 7.2 Ionic Bonds and Ionic CompoundsIonic Compounds


ExplainExplain the electrical the electrical charge of an ionic charge of an ionic compound.compound.

Section 7.2 Ionic Bonds and Section 7.2 Ionic Bonds and Ionic CompoundsIonic Compounds


DescribeDescribe three three properties of ionic properties of ionic compounds.compounds.

Ionic BondingIonic BondingAnions and cations are held together Anions and cations are held together

by by opposite chargesopposite charges (+ and -) (+ and -)Ionic compounds are called Ionic compounds are called saltssalts..Simplest ratio of elements in an ionic Simplest ratio of elements in an ionic

compound is called the compound is called the formula unit.formula unit.The bond is formed through the The bond is formed through the

transfer of electrons (lose and gain)transfer of electrons (lose and gain)Electrons are transferred Electrons are transferred to achieve to achieve

noble gas configuration.noble gas configuration.

Ionic CompoundsIonic Compounds

1)1) Also called Also called SALTSSALTS

2)2) Made from: a Made from: a CATIONCATION with an with an ANIONANION (or (or literally from a literally from a metalmetal combining with a combining with a nonmetalnonmetal))

Ionic BondingIonic Bonding

Na ClThe metal (sodium) tends to lose its one electron from the outer level.

The nonmetal (chlorine) needs to gain one more to fill its outer level, and will accept the one electron that sodium is going to lose.


Na+ Cl -

Note: Remember that NO DOTS are now shown for the cation!

Negative charges are attracted to Negative charges are attracted to positive charges.positive charges.

Negative anions are attracted to Negative anions are attracted to positive cations.positive cations.

The result is an The result is an ionic bond.ionic bond.A three-dimensional A three-dimensional crystal crystal lattice lattice

of anions and cations is formed.of anions and cations is formed.

Ionic BondIonic Bond

Preserve ElectroneutralityPreserve Electroneutrality

When ions combine, When ions combine, electroneutrality must be electroneutrality must be preserved.preserved.

In the formation of magnesium In the formation of magnesium chloride,chloride,

2 Cl2 Cl-- ions must balance a Mg ions must balance a Mg2+2+ ion: ion:MgMg2+ 2+ + 2 Cl+ 2 Cl-- → MgCl → MgCl22


All the electrons must be accounted All the electrons must be accounted forfor, and , and eacheach atom will have a noble atom will have a noble gas configuration (which is stable).gas configuration (which is stable).

Ca P

Let’s do an example by combining calcium and phosphorus:


Ca P


Ca2+ P

Ionic Bonding

Ca2+ P

Ca

Ionic Bonding

Ca2+ P 3-

Ca

Ionic Bonding

Ca2+ P 3-

Ca P

Ionic Bonding

Ca2+ P 3-

Ca2+ P

Ionic Bonding

Ca2+ P 3-

Ca2+ P

Ca

Ionic Bonding

Ca2+ P 3-

Ca2+ P

Ca

Ionic Bonding

Ca2+ P 3-

Ca2+P

3-

Ca2+

Ionic Bonding

= Ca3P2Formula Unit

This is a chemical formula, which shows the kinds and numbers of atoms in the smallest representative particle of the substance.

For an ionic compound, the smallest representative particle is called a: Formula Unit

Properties of Ionic CompoundsProperties of Ionic Compounds

1.1. CrystallineCrystalline solids - a regular solids - a regular repeating arrangement of ions in repeating arrangement of ions in the solid: Fig. 7.9, page 197the solid: Fig. 7.9, page 197

Ions are Ions are stronglystrongly bonded together. bonded together. Structure is rigid.Structure is rigid.

2.2. High melting pointsHigh melting points Coordination numberCoordination number- number of - number of

ions of opposite charge ions of opposite charge surrounding itsurrounding it

- Page 198

Coordination Numbers:

Both the sodium and chlorine have 6

Both the cesium and chlorine have 8

Each titanium has 6, and each oxygen has 3

NaCl

CsCl

TiO2

Do they Conduct?Do they Conduct?

Conducting electricity means Conducting electricity means allowing charges to move.allowing charges to move.

In a solid, the ions are locked in In a solid, the ions are locked in place.place.

Ionic solids are insulators.Ionic solids are insulators. When When meltedmelted, the ions can move , the ions can move

around.around.3.3. Melted ionic compounds conduct.Melted ionic compounds conduct.

NaCl: must get to about 800 ºC.NaCl: must get to about 800 ºC. Dissolved in waterDissolved in water,, they also conduct they also conduct

(free to move in aqueous solutions)(free to move in aqueous solutions)

- Page 198

The ions are free to move when they are molten (or in aqueous solution), and thus they are able to conduct the electric current.

Section 9.1Section 9.1Naming IonsNaming Ions

OBJECTIVES:OBJECTIVES:ModelModel the valence the valence electrons of metal electrons of metal atoms.atoms.



IdentifyIdentify the charges on the charges on monatomic ions by using monatomic ions by using the periodic table, and the periodic table, and namename the ions. the ions.


OBJECTIVES:OBJECTIVES:DefineDefine a polyatomic ion and a polyatomic ion and

writewrite the names and formulas the names and formulas of the most common of the most common polyatomic ions.polyatomic ions.



IdentifyIdentify the two common the two common endingsendings for the names of for the names of most polyatomic ions.most polyatomic ions.

Atoms and IonsAtoms and IonsAtomsAtoms are electrically neutral. are electrically neutral.

Because there is the same number of Because there is the same number of protons (+) and electrons (-).protons (+) and electrons (-).

IonsIons are atoms, or groups of are atoms, or groups of atoms, with a charge (positive or atoms, with a charge (positive or negative)negative)They have They have differentdifferent numbers of numbers of

protons and electrons.protons and electrons.Only Only electronselectrons can move, and can move, and ionsions are are

made by made by gaining or losing electrons.gaining or losing electrons.

An Anion is…An Anion is…

A negative ion.A negative ion.Has Has gainedgained electrons. electrons.Nonmetals can gainNonmetals can gain electrons. electrons.Charge is written as a superscript on Charge is written as a superscript on

the right.the right.

F1-Has gained one electron (-ide is new ending = fluoride)

O2- Gained two electrons (oxide)

A Cation is… A positive ion. Formed by losing electrons. More protons than electrons. Metals can lose electrons

K+ Has lost one electron (no name change for positive ions)

Ca2+ Has lost two electrons

Predicting Ionic ChargesPredicting Ionic ChargesGroup 1AGroup 1A:: Lose 1 electron to form Lose 1 electron to form 1+1+ ions ions

HH++ LiLi++ NaNa++ KK++ RbRb++

Predicting Ionic ChargesPredicting Ionic ChargesGroup 2Group 2:: Loses 2 electrons to form Loses 2 electrons to form 2+2+ ions ions

BeBe2+2+ MgMg2+2+ CaCa2+2+ SrSr2+2+ BaBa2+2+

Predicting Ionic ChargesPredicting Ionic ChargesGroup 13Group 13:: Loses 3 Loses 3

electrons to form electrons to form 3+3+ ions ions

BB3+3+ AlAl3+3+ GaGa3+3+

Predicting Ionic ChargesPredicting Ionic ChargesGroup 14Group 14:: Do they Do they loselose 4 electrons or 4 electrons or gaingain 4 electrons? 4 electrons?

Neither! Neither! Group 14 Group 14 elements rarely form elements rarely form ions ions (they tend to share)(they tend to share)

Predicting Ionic ChargesPredicting Ionic ChargesGroup 15Group 15:: Gains 3 Gains 3 electrons to form electrons to form 3-3- ions ions

NN3-3-

PP3-3-

AsAs3-3-

Nitride

Phosphide

Arsenide

Predicting Ionic ChargesPredicting Ionic ChargesGroup 16Group 16:: Gains 2 Gains 2 electrons to form electrons to form 2-2- ions ions

OO2-2-

SS2-2-

SeSe2-2-

Oxide

Sulfide

Selenide

Predicting Ionic ChargesPredicting Ionic ChargesGroup 17Group 17:: Gains 1 Gains 1 electron to form electron to form 1-1- ions ions

FF--

ClCl--

BrBr--Fluoride

Chloride

Bromide

II-- Iodide

Predicting Ionic ChargesPredicting Ionic ChargesGroup 18Group 18:: Stable Stable

noble gases noble gases do notdo not form ions!form ions!

Predicting Ionic ChargesPredicting Ionic Charges Many Many transitiontransition elements elements have have more than onemore than one possible oxidation state. possible oxidation state.

Iron (II) = Fe2+

Iron (III) = Fe3+

Note the use of Roman numerals to show charges

Naming cationsNaming cations Two methodsTwo methods can clarify when can clarify when

more than one charge is possible:more than one charge is possible:1)1) Stock systemStock system – uses – uses roman roman

numeralsnumerals in parenthesis to indicate in parenthesis to indicate the numerical valuethe numerical value

2)2) Classical methodClassical method – uses root word – uses root word with with suffixessuffixes (-ous, -ic) (-ous, -ic) Does not give true valueDoes not give true value

Naming cationsNaming cationsWe will use the We will use the Stock systemStock system..Cation - if the charge is always the Cation - if the charge is always the

same (like in the main group of same (like in the main group of metals) just write the name of the metals) just write the name of the metal.metal.

Transition metals can have more Transition metals can have more than one type of charge.than one type of charge.Indicate their charge as a Indicate their charge as a roman roman

numeralnumeral in parenthesis after the name in parenthesis after the name of the metal (Table 9.2, p.255)of the metal (Table 9.2, p.255)

Predicting Ionic ChargesPredicting Ionic Charges Some of the Some of the post-transitionpost-transition elements also elements also have have more than onemore than one possible oxidation state. possible oxidation state.Tin (II) = Sn2+ Lead (II) = Pb2+

Tin (IV) = Sn4+ Lead (IV) = Pb 4+

Predicting Ionic ChargesPredicting Ionic Charges Some Some transitiontransition elements have elements have only oneonly one possible oxidation state, such as these three:possible oxidation state, such as these three:

Zinc = Zn2+Silver = Ag+ Cadmium = Cd2+

Exceptions:Exceptions:Some of the transition metals Some of the transition metals

have have only oneonly one ionic charge: ionic charge:Do notDo not need to use need to use roman numerals for these:roman numerals for these:

SilverSilver is is alwaysalways 1+ ( 1+ (AgAg++))CadmiumCadmium and and ZincZinc are are alwaysalways 2+ ( 2+ (CdCd2+2+ and and ZnZn2+2+))

Practice by naming these:Practice by naming these:NaNa++ CaCa2+2+ AlAl3+3+ FeFe3+3+ FeFe2+2+ PbPb2+2+ LiLi++

Write symbols for these:Write symbols for these:

Potassium ionPotassium ionMagnesium ion Magnesium ion Copper (II) ionCopper (II) ionChromium (VI) ionChromium (VI) ionBarium ionBarium ionMercury (II) ionMercury (II) ion

Naming AnionsNaming Anions

Anions are Anions are alwaysalways the the same chargesame charge

Change the monatomic Change the monatomic element ending to – element ending to – ideide

FF-- a Fluor a Fluorineine atom will atom will become a Fluorbecome a Fluorideide ion. ion.

Practice by naming these:Practice by naming these:

ClCl-- NN3-3- BrBr-- OO2-2-

GaGa3+3+

Write symbols for these:Write symbols for these:

Sulfide ionSulfide ionIodide ionIodide ionPhosphide ionPhosphide ionStrontium ionStrontium ion

Polyatomic ions are…Polyatomic ions are…Groups of atoms that stay together Groups of atoms that stay together

and have an overall charge, and one and have an overall charge, and one name.name.

Usually end in Usually end in –ate–ate or or -ite-ite

AcetAcetateate: : CC22HH33OO22--

NitrNitrateate: : NONO33--

NitrNitriteite: : NONO22--

PermanganPermanganateate: : MnOMnO44--

HydroxHydroxideide: : OHOH-- and Cyan and Cyanideide: : CNCN--? ?

SulfSulfateate: : SOSO442-2-

SulfSulfiteite: : SOSO332-2-

CarbonCarbonateate: : COCO332-2-

ChromChromateate: : CrOCrO442-2-

DichromDichromateate: : CrCr22OO772-2-

PhosphPhosphateate: : POPO443-3-

PhosphPhosphiteite: : POPO333-3-

Ammonium: Ammonium: NHNH44++

Know Table 9.3 on page 257

If the polyatomic ion begins with H, then combine the word hydrogen with the other polyatomic ion present:

H+ + CO32- → HCO3

-

hydrogen + carbonate → hydrogen carbonate ion

(One of the few positive polyatomic ions)

Section 9.2 Naming and Section 9.2 Naming and Writing Formulas for Ionic Writing Formulas for Ionic

CompoundsCompoundsOBJECTIVES:OBJECTIVES:

Apply the rulesApply the rules for for naming and writing naming and writing formulasformulas for for binary ionic binary ionic compounds.compounds.

Section 9.2 Naming and Section 9.2 Naming and Writing Formulas for Ionic Writing Formulas for Ionic

CompoundsCompoundsOBJECTIVES:OBJECTIVES:

Apply the rulesApply the rules for for naming and naming and writing formulaswriting formulas for compounds for compounds containing containing polyatomicpolyatomic ions. ions.

Writing Ionic Compound Writing Ionic Compound FormulasFormulas

Example: Barium nitrate (note the 2 word name)

1. Write the formulas for the cation and anion, including CHARGES! BaBa2+2+ NONO33

--

2. Check to see if charges are balanced.

3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Use the criss-cross method to balance subscripts.

Not balanced!

( )( ) 22Now balanced.

= Ba(NO3)2


Example: Ammonium sulfate (note the 2 word name)

1. Write the formulas for the cation and anion, including CHARGES!

NHNH44++ SOSO44

2-2-


3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Use the criss-cross method to balance the subscripts.

Not balanced!

( )( )22

Now balanced.

= (NH4)2SO4


Example: Iron (III) chloride (note the 2 word name)


FeFe3+3+ClCl--



Not balanced!

33

Now balanced.

= FeCl3


Example: Aluminum sulfide (note the 2 word name)


AlAl3+3+ SS2-2-



Not balanced!

22 33

Now balanced.

= Al2S3


Example: Magnesium carbonate (note the 2 word name)


MgMg2+2+ COCO332-2-


They are balanced!

= MgCO3


Example: Zinc hydroxide (note the 2 word name)


ZnZn2+2+ OHOH--



Not balanced!

( )( )22

Now balanced.

= Zn(OH)2


Example: Aluminum phosphate (note the 2 word name)

1. Write the formulas for the cation and anion, including CHARGES! AlAl3+3+ POPO44

3-3-

2. Check to see if charges are balanced. They ARE

balanced!= AlPO4

Naming Ionic CompoundsNaming Ionic CompoundsNaming Ionic CompoundsNaming Ionic Compounds1. Name the cation first, then anion1. Name the cation first, then anion

2. Monoatomic cation = name of the 2. Monoatomic cation = name of the elementelement

CaCa2+2+ = calcium = calcium ionion

3. Monoatomic anion = 3. Monoatomic anion = rootroot + - + -ideide

ClCl = chlor = chlorideide

CaClCaCl22 = calcium chloride = calcium chloride

Naming Ionic CompoundsNaming Ionic CompoundsNaming Ionic CompoundsNaming Ionic Compounds

some some metals can form more than one metals can form more than one charge (usually the transition metals)charge (usually the transition metals)

use a use a Roman numeralRoman numeral in their name:in their name:PbClPbCl22 – use the – use the anionanion to find the charge to find the charge

on the cation (chloride is always 1-)on the cation (chloride is always 1-)

PbPb2+2+ is the lead (II) cationis the lead (II) cation

PbClPbCl22 = lead ( = lead (IIII) chloride) chloride

(Metals with multiple oxidation states)(Metals with multiple oxidation states)

Things to look for:Things to look for:

1)1) If cations have ( ), the If cations have ( ), the number in parenthesis is number in parenthesis is their charge.their charge.

2)2) If anions end in If anions end in -ide-ide they are they are probably off the periodic probably off the periodic table (Monoatomic)table (Monoatomic)

3)3) If anion ends in If anion ends in -ate-ate or or –ite–ite, , then it is polyatomicthen it is polyatomic

Practice by writing the Practice by writing the formula or name as formula or name as

required…required…Iron (II) PhosphateIron (II) PhosphateStannous FluorideStannous FluoridePotassium SulfidePotassium SulfideAmmonium ChromateAmmonium ChromateMgSOMgSO44

FeClFeCl33

Practice by writing the Practice by writing the formula for the following:formula for the following:

Magnesium hydroxideMagnesium hydroxideIron (III) hydroxideIron (III) hydroxideZinc hydroxideZinc hydroxide

Some compounds contain HSome compounds contain H22O in their struc-O in their struc-

ture. These compounds are called hydrates.ture. These compounds are called hydrates.The HThe H22O can usually be removed if heated.O can usually be removed if heated.A dot separates water: e.g. CuSOA dot separates water: e.g. CuSO44•5H•5H22O is O is

copper(II) sulfate pentahydrate.copper(II) sulfate pentahydrate.A greek prefix indicates the # of HA greek prefix indicates the # of H22O groups.O groups.

HydratesHydrates

sodium sulfate decahydratesodium sulfate decahydrate nickel(II) sulfatenickel(II) sulfate hexahydratehexahydrate

NaNa22COCO33•H•H22O O

BaClBaCl22•2H•2H22O O

NaNa22SOSO44•10H•10H22O O

NiSONiSO44•6H•6H22O O

sodium carbonate monohydratesodium carbonate monohydratebarium chloride dihydratebarium chloride dihydrate

Prefixes

11 monomono2 di2 di33 tritri

44 tetratetra55 pentapenta66 hexahexa77 heptahepta88 octaocta99 nonanona10 deca10 deca

HydratesHydratesExamples: I. Give the name of the following: I. Give the name of the following:

1. CuSO1. CuSO44 5H 5H22O O

2. MgCl2. MgCl22 6H 6H22O O

3. Na3. Na22SOSO44 10H 10H22OO II. Write the formula for:II. Write the formula for:

1. zinc chloride hexahydrate 1. zinc chloride hexahydrate 2. calcium phosphate dihydrate 2. calcium phosphate dihydrate 3. copper (I) chloride pentahydrate3. copper (I) chloride pentahydrate

Summary of Naming and Summary of Naming and Formula WritingFormula Writing

For naming, follow the For naming, follow the flowchart- Figure 9.20, page flowchart- Figure 9.20, page 277277

For writing formulas, follow For writing formulas, follow the flowchart from Figure the flowchart from Figure 9.22, page 2789.22, page 278

Helpful to remember...Helpful to remember...1. In an ionic compound, the net ionic 1. In an ionic compound, the net ionic

charge is charge is zero zero (criss-cross method)(criss-cross method)

2. An 2. An -ide-ide ending generally indicates a ending generally indicates a binary compoundbinary compound

3. An 3. An -ite-ite or or -ate-ate ending means there ending means there is a polyatomic ion that has oxygenis a polyatomic ion that has oxygen

4. 4. PrefixesPrefixes generally mean molecular; generally mean molecular; they show the number of each atomthey show the number of each atom

Helpful to remember...Helpful to remember...

5. A 5. A Roman numeralRoman numeral after the after the name of a cation is the name of a cation is the ionic ionic chargecharge of the cation of the cation

Documents

Chapter 7 “Ionic Bonding” Chemistry Section 7.1 - Ions OBJECTIVES: OBJECTIVES: Determine the number of valence electrons in an atom of a representative