IONIC COMPOUNDS

STABILITYRelates to nobilityEvery elements dreamTheyll do what they can to look like a noble gaspseudo-noble gas configurationDuet RuleOctet RulePotential Energy

Bond EnergyThe energy required to break a bondThe energy is absorbed when the bond is broken, thusreleased when formedStronger bonds are more stableRequire more energy to break themi.e. ionic bondsWeaker bonds are less stableRequire less energy to break themi.e. molecular or covalent bonds

Achieving StabilityIonic bonds made by transferring electronsMetals will do what?

Nonmetals will do what?

Once electrons are transferred, the atoms are converted to ions.lose electron(s)gain electron(s)

IonsPositively charged ions are called?

Negatively charged ions are called?

Bond to make an ionic compound or saltcationsanions

SaltsMade of metals and nonmetals or polyatomic ionsSolidOrdered arrangement called crystal latticeBrittleHigh melting pointElectrical conductors in aqueous and molten phases

More About IonsWritten as a symbol with superscript to the right indicating the chargeCharge is written as a number followed by a + or signMonatomic ionsone-atomed ionsPolyatomic ionsmany-atomed ions

Monatomic IonsUse periodic table to determine charges of representative elementsGroup 11+element name + ionGroup 22+element name + ionGroup 133+element name + ionGroup 14skipGroup 153-ide ending + ionGroup 162-ide ending + ionGroup 171-ide ending + ion

Monatomic IonsFor the transition metals, you must memorize the possible charges of the common ions

Cr2+Chromium (II) ionChromous ionCr3+Chromium (III) ionChromic ionMn2+Manganese (II) ionManganous ionMn3+Manganese (III) ionManganic ionFe2+Iron (II) ionFerrous ionFe3+Iron (III) ionFerric ion

Monatomic Ions

Co2+Cobalt (II) ionCobaltous ionCo3+Cobalt (III) ionCobaltic ionNi2+Nickel (II) ionNickelous ionNi3+Nickel (III) ionNickelic ionCu1+Copper (I) ionCuprous ionCu2+Copper (II) ionCupric ionHg22+Mercury (I) ionMercurous ionHg2+Mercury (II) ionMercuric ion

Monatomic Ions

Sn2+Tin (II) ionStannous ionSn4+Tin (IV) ionStannic ionPb2+Lead (II) ionPlumbous ionPb4+Lead (IV) ionPlumbic ionAg1+Silver ionZn2+Zinc ionCd2+Cadmium ion

Polyatomic IonsRefer to handoutKnow the formula (that means elements, subscripts, and charge) of each listed

Making Ionic CompoundsA cation and an anion will bond in order to bring the charge of the compound to zero.A criss-cross method is used to determine the number of each ion necessary to balance the chargesAlways reduce subscripts.

Making Ionic Compounds= NaCl= MgCl2= AlCl3

Making Ionic CompoundsNaClMgCl2AlCl3sodium chloridemagnesium chloridealuminum chloride

Making Ionic Compounds= Na2S= MgO= Ca3P2

Making Ionic CompoundsNa2SMgOCa3P2sodium sulfidemagnesium oxidecalcium phosphide

Making Ionic Compounds= PbO2= AgI= Fe2O3Fe3+O 2-23

Making Ionic CompoundsPbO2AgIFe2O3iron (III) oxide orferric oxidesilver iodideLead (IV) oxide orplumbic oxide

Making Ionic CompoundsPb4+ (OH)1-14= Pb(OH)4= MgSO4= Al2(C2O4)3Mg2+(SO4)2-22Al3+(C2O4)2-23

Making Ionic CompoundsPb(OH)4MgSO4Al2(C2O4)3lead (IV) hydroxide orplumbic hydroxidemagnesium sulfatealuminum oxalate