1. Naming Binary Compounds ****CRISS-CROSS METHOD!!!!!***  Take the oxidation state of each element and/or polyatomic ion and criss-cross them to get your formula!! (Do not include charge in formula)  Always reduce ionic compounds so that atoms are in their smallest whole # ratio! Mg +2 and Cl -1 MgCl 2 (magnesium chloride)

2. Table E—Selected Polyatomic Ions

3. Variations for Type 1 Compounds Metal & Non-metal (NaF= sodium fluoride) Metal & - polyatomic ion (NaOH = sodium hydroxide) +Polyatomic ion & Non-metal +Polyatomic ion & Non-metal (NH 4 F = ammonium fluoride) 2 polyatomic ions (NH 4 OH = ammonium hydroxide)

4. If metal has more than one + oxidation number use roman numerals to show which one FeCl 3 = Iron (III) chloride FeCl 2 = Iron (II) chloride

5. Naming Binary Compounds Type 3 Rules for Naming Binary Covalent/Molecular Compounds (non-metal & non-metal) 1.The first element in the formula is named first, using the full element name. 2.Drop the ending of the 2 nd element in the compound and add the ending –ide. 3.Prefixes (shown below) denote the # of atoms present Also consider that: A)The prefix mono is never used with the first element, only from -di on. B)The second non-metal always gets a prefix

6. Names and Formulas of Ionic Compounds (Type 1 & 2) Putting It All Together: PRACTICE!! Name the following compounds given the formula: 1)Na 2 SO 4 9) Al(NO 3 ) 3 10) Cu(ClO 4 ) 2 10) Cu(ClO 4 ) 2 3)Fe(NO 3 ) 3 11) NH 4 Br 4)Mn(OH) 2 12) Cr 2 O 3 5)Na 2 SO 3 13) Co(NO 3 ) 2 6)Na 2 CO 3 14) K 2 SO 4 7)CaCl 2 15) Ba(OH) 2 8)FeCl 3

7. Names and Formulas of Ionic Compounds Putting It All Together: PRACTICE!! Write the formula for each compound, given the name: 1)Sodium hydrogen carbonate7) Nickel (II) perchlorate 2)Cesium perchlorate8) Iron (II) phosphate 3)Sodium hypochlorite9) Titanium (IV) oxide 4)Sodium selenate10) Magnesium sulfate 5)Potassium bromate11) Silver sulfide 6)Potassium sulfide12) Lead (II) nitrate

8. Names and Formulas of Binary Covalent/Molecular Compounds Name the following compounds: 1)Cl 2 O 5) SO 2 2)N 2 O 4 6) PCl 5 3)NF 3 7) N 2 O 3 4)P 4 S 10

9. Classifying Chemical Reactions  Synthesis: H 2 O + CO 2  H 2 CO 3  Decomposition: NaCl  Na + Cl  Single Replacement: Fe + CuSO 4  FeSO 4 + Cu  Double Replacement: NaCl + AgNO 3  NaNO 3 + AgCl

10. Balancing Chemical Reactions LAW OF CONSERVATION OF MASS, ENERGY, & CHARGE:  In all chemical reactions there is conservation of mass, energy and charge.  The amount of matter stays the same (one side equals the other).  The total amount of energy stays the same (one side equals the other).  The number of positive (or negative) charges stays the same (one side equals the other).  In a chemical reaction, all of the elements or compounds found to the left of the equation are known as the reactant(s), and resulting elements or compounds are known as the product(s). 2H 2 + O 2  2H 2 O (reactants) (product) (reactants) (product)

11. IUPAC International Union of Pure and Applied Chemistry  When a question states “Write the IUPAC name” they are talking about the organization above. All chemical and “common” names must be approved by them. Basically it means “JUST NAME IT!!”  When a question states “Write the IUPAC name” they are talking about the organization above. All chemical and “common” names must be approved by them. Basically it means “JUST NAME IT!!”