1. III. Writing & Naming Ionic Formulas

2. A. Ionic Compound Basics Always composed of a metal and a nonmetal Metal donates an electron to the nonmetal Metal becomes positively charged Nonmetal becomes negatively charged Opposite charges is what causes the atoms to bond to one another (electrostatic force)

3. B. Ionic Formula Basics BaCl 2 Cation (Metal) ALWAYS COMES FIRST Anion (Nonmetal) ALWAYS COMES SECOND Subscript tells how many atoms are present

4. B. Ionic Formula Basics NaCl Cation (Metal) ALWAYS COMES FIRST Anion (Nonmetal) ALWAYS COMES SECOND No subscript = assume only 1 atom

5. C. Writing Ionic Formulas cations and anions combine to form NEUTRAL compounds Positive and negative charges must cancel out when forming compounds RULES 1. Write the symbols and charges for both the cation and anion involved 2. If both charges cancel out, simply combine to form compound 3. If charges DO NOT cancel out, add subscripts so that charges cancel 4. Simplify to smallest whole number ratio

6. Writing Ionic Formulas Example Write the formula for the compound made when sodium and fluorine combine Write the formula for the compound made when magnesium and oxygen combine

7. Writing Ionic Formulas Example Write the formula for the compound made when calcium and bromine combine Write the formula for the compound made when manganese (III) and chlorine combine

8. D. Criss-Cross Method To simplify balancing charges, make the charge of one atom the subscript of the other. Aluminum &Oxygen AlO 3+ 2– Al 2 O 3

9. Writing Ionic Formulas Example Write the formula for the compound made when lead (II) and nitrogen combine Write the formula for the compound made when lead (IV) and oxygen combine

10. E. Naming Ionic Compounds (For cations with only one oxidation number) (For non-transition metals) Always name the cation (metal) first, then the anion (nonmetal) Ignore subscripts when naming Cation = just the name of the element Ca = Calcium Na = Sodium Al = Aluminum Anion = root + -ide F = Fluoride Cl = Chloride P = Phosphide Example: NaCl Sodium chloride MgO Magnesium oxide BaCl 2 Barium chloride Al 2 S 3 Aluminum sulfide

11. Practice Write the names for the following ionic compounds 1. CaBr 2 2. K 3 P 3. BeO 4. LiF 5. SrI 2

12. F. Naming Ionic Compounds (For cations with multiple oxidation number) Same rules apply as before, but must determine the charge of the transition metal Cation = name of element Anion = root + –ide Subscripts become important to determine charge of transition metal Remember, we want charges to cancel to make NEUTRAL COMPOUNDS

13. 1. Recognize that iron is located in the d-block (transition metal) Therefore, does not have a “set in stone” charge Oxygen, however, does 2. Determine the charge of oxygen –2 Since there are 3 oxygen atoms, total charge from oxygen = –6 3. Determine charge of iron needed to cancel charge of oxygen There are 2 iron atoms, therefore, each must have a +3 charge 4. Iron (III) oxide Example: Fe 2 O 3

14. Example: Fe 2 O 3

15. Practice Name the following ionic compounds 1. SnO 2 2. Mn 2 O 7 3. FeN 4. CuBr 5. TiF 3

16. Ionic Bonds HW #3 Write name/formula for the following (representative elements) Write name/formula for the following (transition metals) 1. Aluminum oxide 2. Ca 3 N 2 3. Lithium bromide 4. KCl 5. Barium fluoride 6. MgS 1. Copper (I) nitride 2. CoF 2 3. Iron (III) chloride 4. Fe 3 N 2 5. Titanium (IV) oxide 6. Mn 2 O 7