2. 12 Weeks to TAKS Week 11 Part II

3. 12 Weeks to TAKS – Week 10 Objective 4: IPC 7D: The student is expected to relate the chemical behavior of an element including bonding, to its placement on the periodic table.

4. IonsIons Cation: A positive ionCation: A positive ion Mg 2+, NH 4 +Mg 2+, NH 4 + Anion: A negative ionAnion: A negative ion Cl , SO 4 2 Cl , SO 4 2  Ionic Bonding: Force of attraction between oppositely charged ions.Ionic Bonding: Force of attraction between oppositely charged ions.

5. Predicting Ionic Charges Group (IA) 1: Lose 1 electron to form 1+ ions H+H+H+H+ Li + Na + K+K+K+K+

6. Predicting Ionic Charges Group (IIA) 2: Loses 2 electrons to form 2+ ions Be 2+ Mg 2 + Ca 2+ Sr 2 + Ba 2+

7. Predicting Ionic Charges Group (IIIA) 13: Loses 3 electrons to form 3+ ions B 3+ Al 3+ Ga 3+

8. Predicting Ionic Charges Group (IVA) 14: Lose 4 electrons or gain 4 electrons? Many Group IVA (14) elements rarely form ions. Many Group IVA (14) elements rarely form ions.

9. Predicting Ionic Charges Group (VA) 15: Gains 3 electrons to form 3- ions N 3- P 3- As 3- Nitride Phosphide Arsenide

10. Predicting Ionic Charges Group (VIA) 16: Gains 2 electrons to form 2- ions O 2- S 2- Se 2- Oxide Sulfide Selenide

11. Predicting Ionic Charges Group (VIIA) 17: Gains 1 electron to form 1- ions F 1- Cl 1- Br 1- Fluoride Chloride Bromide I 1- Iodide

12. Predicting Ionic Charges Group (VIIIA) 18: Stable Noble gases do not form ions!

13. Predicting Ionic Charges Groups 3 - 12: Many transition elements Many transition elements have more than one possible oxidation state. Roman numerals are used to indicate the oxidation state Iron(II) = Fe 2+ Iron(III) = Fe 3+

14. Predicting Ionic Charges Groups 3 - 12: Some transition elements Some transition elements have only one possible oxidation state. have only one possible oxidation state. Zinc = Zn 2+ Silver = Ag +

15. Writing Ionic Compound Formulas Example: Iron(III) with chloride 1. Write the formulas for the cation and anion, including CHARGES! Fe 3+ Cl - 2. Check to see if charges are balanced. 3. Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced! 3 Fe 3+ Cl - Balanced! Iron(III) chloride 4. Name the ions

16. Example: Barium with nitrate 1. Write the formulas for the cation and anion, including CHARGES! Ba 2+ NO 3 - 2. Check to see if charges are balanced. 3. Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced! ( ) 2 Ba 2+ NO 3 - Balanced! Barium nitrate 4. Name the ions

17. Example: Ammonium with sulfate 1. Write the formulas for the cation and anion, including CHARGES! NH 4 + SO 4 2- 2. Check to see if charges are balanced. 3. Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced! ( ) 2 NH 4 + SO 4 2- Your Turn! Ammonium sulfate 4. Name the ions

18. Example: Aluminum with sulfide 1. Write the formulas for the cation and anion, including CHARGES! Al 3+ S 2- 2. Check to see if charges are balanced. 3. Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced! 2 3 Al 3+ S 2- Aluminum sulfide 4. Name the ions

19. Example: Magnesium with carbonate 1. Write the formulas for the cation and anion, including CHARGES! Mg 2+ CO 3 2- 2. Check to see if charges are balanced. They are balanced! Magnesium carbonate 4. Name the ions

20. Example: Zinc with hydroxide 1. Write the formulas for the cation and anion, including CHARGES! Zn 2+ OH - 2. Check to see if charges are balanced. 3. Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced! ( ) 2 Zn 2+ OH - Zinc hydroxide 4. Name the ions

21. Example: Calcium with phosphate 1. Write the formulas for the cation and anion, including CHARGES! Ca 2+ PO 4 3- 2. Check to see if charges are balanced. Not balanced! Calcium phosphate Ca 2+ PO 4 3- 23 ( ) 4. Name the ions 3. Balance charges, if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion.