1. Ionic Bonding: Ms. McKeever 8 th Grade Science

2. Electron (Lewis) dot diagrams for elements of the periodic table.

3. Categories for notes: 1.What is ionic bonding? 2.What is the overall charge of an ionic bond? 3.Examples of ionic bonds 4.What are polyatomic ions?

4. Categories for notes: 5. Why do ionic bonds form? 6. Naming ionic compounds 7. Properties of ionic compounds

5. Categories for notes: 1.What is ionic bonding?

6. Bonding: Ionic Atoms with 1, 2 or 3 electrons can lose electrons to other elements. Atoms with 5, 6, or 7 electrons can gain electrons from other elements. Atoms or groups of atoms that gain or lose electrons are called Ions. When an ion bonds with another ion, it forms a chemical bond called an ‘Ionic’ bond.

7. Electron (Lewis) dot diagrams for elements of the periodic table. Groups 1 and 17 bond ionically with one another.

8. Categories for notes: 2. What is the overall charge of an ionic bond?

9. Bonding: Ionic Ionic bonds are neutral because the negative and positive charges cancel each other out.

10. Categories for notes: 3. Examples of ionic bonds

11. Bonding: Ionic Atoms located in families/groups 1 and 17 always form ionic bonds with each other. Atoms in these families/groups do not generally form ionic bonds with elements from the center of the periodic table.

12. Bonding: How Ions Bond: Chlorine takes an electron from sodium

13. Bonding: How Ions Bond: Iodine takes an electron from potassium

14. Two atoms are walking down the street one day, and one of them says to the other: "Hey, wait up a second. I think I lost an electron" The first atom replied, "Are you sure?" The second atom exclaimed, "Yes, I'm positive!"

15. Categories for notes: 4. What are polyatomic ions?

16. Polyatomic Ions Bonding: Ionic: Polyatomic Ions Some ions are made from more than one different atom. Poly = many, atomic = atoms Polyatomic ions react like a single ion. They have an overall charge.

17. Polyatomic Ions Bonding: Ionic: Polyatomic Ions O H x C O A bicarbonate ion O [HCO 3 ] - or [HCO 3 ] -1 Atomic bond between two atoms Electron from carbon x Electron from hydrogen Electron from oxygen Extra Electron

18. Polyatomic Ions Phosphate: P0 4 -3 or P0 4 3- Bonding: Ionic: Polyatomic Ions Phosphate: P0 4 -3 or P0 4 3-

19. A proton, neutron, and electron went out to dinner one night. After a luxurious meal, the waiter brought the check to the proton and the electron. The neutron was perplexed as to why the waiter didn't bring him his check. So, he summoned the waiter to the table and asked him about it. "For you, there's no charge!" The waiter explained to the neutron, "For you, there's no charge!"

20. What do you do with a dead chemist? Barium!

21. Why do chemists like nitrates so much? They're cheaper than day rates!

22. Why does hamburger have lower energy than steak? Because it's in the ground state!

24. Ionic Bonds:  Ionic bonds form as a result of the attraction between a positive and a negative ion.  How do you know how many of each one will form? Because they want to form a perfect octet with 8 electrons on the outside!

25. Ionic Bonds: When ionic compounds form, the ions come together in order to balance out the charges to zero (if possible). Example: Barium ion (Ba +2 ) combines with Chlorine (Cl -1 ) form barium chloride (BaCl 2 ) Ba x x Cl x x x

26. Ionic Bonds: Example: Barium ion (Ba +2 ) combines with Chlorine (Cl -1 ) form barium chloride (BaCl 2 ). The subscript ‘2’ tells you that there are two chlorine ions in the formula.

27. Categories for notes: 6. Naming ionic compounds

28. Naming Ionic compounds: When naming ionic compounds you name the positive ion (usually a metal) first and then the negative ion (usually a nonmetal), changing the ending to – ide. Examples: Sodium chloride Barium bromide Note: Polyatomic ions do not always follow this rule.

29. Categories for notes: 7. Properties of ionic compounds

30. Properties of Ionic compounds:  They form crystals (groups 1 + 17 form salts)  They have very high melting points  They conduct electricity in solution See page 195 in textbook Neo K-12 http://www.neok12.com/Chemical-Reactions.htm

31. Practice page:  Li +1 + F -  LiF(also for Na +, K +,  Li 1+ + Cl -  LiCl and NH 4 + )  Li + + I -  LiI  Li + + HCO 3 -  LiHCO 3  Li + + NO 3 -  LiNO 3  Li + + S -2  Li 2 S  Li + + PO 4 -3  Li 3 PO 4

32. Interactive page:  Ca +2 + F -  CaF 2  Ca +2 + Cl -  CaCl 2  Ca +2 + I -  CaI 2  Ca +2 + HCO 3 -  Ca(HCO 3 ) 2  Ca +2 + NO 3 -  Ca(NO 3 ) 2

33. Interactive page:  Al +3 + F -  AlF 3  Al +3 + Cl -  AlCl 3  Al +3 + I -  AlI 3  Al +3 + HCO 3 -  Al(HCO 3 ) 3  Al +3 + NO 3 -  Al(NO 3 ) 3  Al +3 + SO 4 -2  Al 2 (SO 4 ) 3 (same as CO 3 -2 )  Al +3 + PO 4 -3  Al(PO 4 )