1. Ionic Compounds

2. Determine the number of subatomic particles in the following elements:  Cl has a mass of 35 and an atomic # of 17  p + = 17, n o = 18,e - = 17  K has a mass of 39 and an atomic # of 19  p + = 19, n o = 20,e - = 19

3. Write the formula of each of the following ionic compounds  Silver nitrate  Sodium oxalate  Magnesium hydroxide  Silver acetate

4. Forming Ionic Compounds w/ Variable Oxidation Numbers  Some elements (metals) can have more than one possible charge when they form ions  Use Roman Numerals to indicate their charge Example: Copper(II) Sulfate Chromium(III) Oxalate

5. Notes Naming Ionic Compounds  Left  Right  Left Side:  Name the metal (cation)  If it is variable, you must use a roman numeral to indicate its oxidation number/charge  Right Side  If polyatomic and on your reference chart, write the name  If monatomic, write the name of the element but change the ending to “-ide”

6. Practice  Write the name of each of the following compounds  AgBr  Ca 3 (PO 4 ) 2  LiH  RaCl 2

7. Notes Naming Ionic Compounds w/ Variable Oxidation Numbers  Start with what you know! (the anion)  Calculate the total anion charge  An ionic compound is neutral (no charge) so…. Total anion charge = Total cation charge  Calculate the charge of the individual cation  Name the compound by giving the cation a roman numeral to represent its oxidation number (charge)

8. Naming Ionic Compounds w/ Variable Oxidation Numbers Example: Cu 2 S Ni(OH) 2

9. Name the compound BiI 3 CoBr 2

10. Cu 2 S CuS

11. Ionic Compounds Lab  Review: signs of a chemical reaction

12. Ionic Compounds Lab  Goggle safety  Dropper safety  Silver Nitrate – Sodium hydroxide safety  Equation set-up  Double Displacement Reactions  Clean Up

13. Wrap Up  What does the roman numeral tell you in an ionic compound?  Assignment: Finish writing out all the reactions