Naming Ionic

Compounds

Ionic Compounds

• Ionic Bond: A bond that results from the attraction between cations and anions.

• Cations: Positively charged ions– Metals or ammonium

• Anions: Negatively charged ions– Nonmetals and polyatomic ion (excluding ammonium)

Naming Ionic Compounds

• We will always be ignoring the Metalloids and the Inner Transition Metals

• For now we will be ignoring the Transition Metals

Charges!!!+1

+3 -4 -3 -2 -1+2 0

Naming Ionic Compounds

• NaCl

• You always name the cation first:– sodium

• You then name the anion:– If not a polyatomic ion change the ending to –ide• chlorine becomes chloride

• sodium chloride

Naming Ionic Compounds

• Ca3P2

• calcium phosphide• K2O• potassium oxide• BaS• barium sulfide• MgF2

• magnesium fluoride

Naming Ionic Compounds

• If it has a polyatomic ion name it as given• KClO3

• potassium chlorate• Ca(BrO4)2

• calcium perbromate• NH4Cl• ammonium chloride

Naming Ionic Compounds

• Practice– KCN– Ba(MnO4)2

– BaCl2

– Ca3(PO4)2

– Al2O3

– NH4OH

– potassium cyanide– barium permanganate– barium chloride– calcium phosphate– aluminum oxide– ammonium hydroxide

Naming Ionic Compounds

• If you have the name and you want to write the formula

• sodium sulfide• First write the symbols for each ion with the

charge• Na+ and S-2

Naming Ionic Compounds

• Determine how many of each ion you need to balance out the charge

• two Na+ to every one S-2

• Use subscripts to indicate how many you used and get rid of the charges

• Na2S

Naming Ionic Compounds

• calcium bromide• CaBr2

• sodium nitrate• NaNO3

• aluminum oxalate• Al2(C2O4)3

• ammonium oxide• (NH4)2O

Naming Ionic Compounds:

Using Transition Metals

Naming Ionic Compounds

• Transition Metals– Do not have a consistent charge

• Copper can have a +1 or a +2 charge• We use roman numerals to indicate the charge• Copper (I) is Cu+1

• Copper (II) is Cu+2

Naming Ionic Compounds

• copper (I) sulfate• Cu+1 and SO4

-2

• Cu2SO4

• copper (II) sulfate• Cu+2 and SO4

-2

• Cu2(SO4)2

• simplifies to CuSO4

Naming Ionic Compounds

• iron (III) oxide• Fe2O3

• molybdenum (II) thiocyanate• Mo(SCN)2

• chromium (I) nitride• Cr3N• tin (IV) silicate• Sn(SiO3)2

Naming Ionic Compounds

• Practice– titanium (I) nitrate

– chromium (II) cyanide

– manganese (II) bromide

– iron (III) silicate

– TiNO3

– Cr(CN)2

– MnBr2

– Fe2(SiO3)3

Naming Ionic Compounds

• NiCrO4

• nickel ___ chromate• chromate has a -2 charge• to balance it out nickel must have a +2 charge• nickel (II) chromate

Naming Ionic Compounds

• Mo(CN)3

• molybdenum ___ cyanide• cyanide has a -1 charge• to balance out three cyanides nickel must

have a +3 charge• molybdenum (III) cyanide

Naming Ionic Compounds

• Pb(SO3)2

• lead ___ sulfite• sulfite has a -2 charge• to balance out two sulfites lead must have a

+4 charge• lead (IV) sulfite

Naming Ionic Compounds

• VO2

• vanadium (IV) oxide• Co2CO3

• cobalt (I) oxalate

• SnCr2O7

• tin (II) dichromate

Naming Ionic Compounds

• Practice– Ti(MnO4)2

– CoCl2

– CrPO4

– Fe2O3

– NiOH

– titanium (II) permanganate

– cobalt (II) chloride

– chromium (III) phosphate

– iron (III) oxide

– nickel (I) hydroxide

Naming Ionic Compounds

• Three transition metals do NOT transition• Silver – Ag+1

• Zinc – Zn+2

• Cadmium – Cd+2

• AgNO3

• silver nitrate

Charges!!!+1

+3 -4 -3 -2 -1+2 0

+2+2

+1