Post on 30-Dec-2015
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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