Chapter 4.2 Naming Compounds. Naming Ionic Compounds Before you name it, you have to know when you see it! What is an Ionic Compound? How to identify

Chapter 4.2Naming Compounds

Naming Ionic Compounds

Before you name it, you have to know when you see it! What is an Ionic Compound? How to identify an Ionic Compound?


What is an Ionic Compound?How to identify an Ionic Compound? Metal and non-metal bonded togetherPositive and negative ionsIONs and IONic compound

Ionic or Covalent Compound?

1. NaCl 2. CH4 3. S5Br18 4. MgO 5. NO

Naming Ionic Compounds (copy)

Metal ion = name stays the sameNon-metal ion = change the ending to "-ide" Example: NaCl = Sodium ChlorideNa = SodiumCl = Chlorine >>> change ending to chloride


Examples: 1. Li3N 2. CaO 3. ZnS 4. AlP


Examples: 1. Li3N = Lithium Nitride 2. CaO = Calcium Oxide 3. ZnS = Zinc Sulphide 4. AlP = Aluminum Phosphide

Chemical Names to Formulas

Write the chemical formula of Potassium Iodide. Find the charge of each ionPotassium ion = K+1Iodine ion = I-1 The ratio is 1 to 1, so the formula is KI

Chemical Names to FormulasWrite the chemical formula of Potassium Oxide. Find the charge of each ionPotassium ion = K+1

Oxygen ion = O-2

The ratio is 1 to 2, so there must be 2 K for each O = K2OOR cross the charges down

Chemical Names to Formulas

Write the chemical formula for Aluminum Nitride. Find the charge of each ion.Aluminum ion = Al+3 Nitrogen ion = N-3

Ratio is 3 to 3, or Al3N3 Reduce like a fraction.AlN

Practice Problems

TextbookPage 187 - formula to namesPage 188 - names to formula

Multivalent Metal Ionic Compounds

Multivalent- Multi means more than one- Valent refers to the valence electrons So multivalent metals are metals with more than one charge. Example: Copper, Cu (#29)It can be Cu+1 or Cu +2 . Need to know which one!


Write the chemical formula for: 1. Copper (I) fluoride 2. Copper (II) fluoride 3. Copper (II) nitride 4. Copper (II) oxide


Write the chemical formula for: 1. Copper (I) fluoride = CuF 2. Copper (II) fluoride = CuF2 3. Copper (II) nitride = Cu3N2 4. Copper (II) oxide = CuO


Use brackets ( ) and Roman numerals (I, II, III, IV, V, VI, ...)in the chemical name. Examples:Write the chemical name of:1. CuF2. CuCl23. PbO4. PbO2


Use brackets ( ) and Roman numerals (I, II, III, IV, V, VI, ...)in the chemical name. Examples:Write the chemical name of:1. CuF = Copper (I) Fluoride2. CuCl2 = Copper (II) Chloride3. PbO = Lead (II) Oxide4. PbO2 = Lead (IV) Oxide

Polyatomic Ions

Poly = manyatomic = atomsPolyatomic Ions = ions with many different atoms. They stick together, treat them as one thing.Look in the table for the name and formula. Example: Sodium Nitrate = NaNO3 Sodium ion = Na+ Nitrate ion = NO3-

Polyatomic Ions

Use brackets to show how many polyatomic ions. Example: Zinc HydroxideZinc ion = Zn+2 Hydroxide ion = OH-1

Zn(OH)2

Polyatomic Ions

ExamplesWrite the name of:1. LiCH3COO2. Mg3(PO3)2

3. CrSO4

Write the formula of:4. Calcium Perchlorate5. Lead (IV) Chromate6. Ammonium Sulfite

Polyatomic Ions

ExamplesWrite the name of:1. LiCH3COO = Lithium Acetate2. Mg3(PO3)2 = Magnesium Phosphite3. CrSO4 = Chromium (II) SulfateWrite the formula of:4. Calcium Perchlorate = Ca(ClO4)2 5. Lead (IV) Chromate = Pb(CrO4)2 6. Ammonium Sulfite = (NH4)2SO3

Polyatomic Ions

Practice ProblemsTextbookPage 193

Naming Covalent Compounds

Check that it IS a covalent compound first!Two non-metals Recall: Ionic or Covalent Compound?1. NaCl2. CH4 3. S5Br18 4. MgO5. NO


Use a prefix to show how many of each element First element - name stays the same. Only add a prefix if there is more than one. Second element - change the ending to "-ide" Example: CO2 = Carbon dioxide


Prefixes1 mono2 di3 tri4 tetra5 penta6 hexa7 hepta8 octa9 nona 10 deca


ExamplesWrite the name of:1. P2Br3

2. SO4

3. F5O10 Write the formula of:1. dicarbon trinitride2. hexaoxygen heptaiodide3. octabromine monohydride


Write the name of:1. P2Br3 = diphosphorous tribromide2. SO4 = sulfur tetraoxide3. F5O10 = pentafluorine decaoxideWrite the formula of:1. dicarbon trinitride = C2N3 2. hexaoxygen heptaiodide = O6I7

3. octabromine monohydride = Br8H


Practice ProblemsTextbook Pg 195

Diatomic Elements

H2 = hydrogenN2 = nitrogenO2 = oxygenF2 = fluorineCl2 = chlorineBr2 = bromineI2 = iodine

Common Mistakes

Be careful:Sulfide = S-2 Sulfate = SO4

-2 Sulfite = SO3-2

Sulfur tetraoxide = SO4 Sulfur trioxide = SO3 Nitride = N-3 Nitrate = NO3

-2 Nitrite = NO2-1

Nitrogen dioxide = NO2 Nitrogen trioxide = NO3

Naming Everything

Ionic, Covalent, Multivalent, Polyatomic will all be mixed together. You need to tell them apart to name them. Practice ProblemsTextbook Page 197, 201

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Chapter 4.2 Naming Compounds. Naming Ionic Compounds Before you name it, you have to know when you see it! What is an Ionic Compound? How to identify