1. Ionic BONDING

3. Noble Gases

5. Have complete outer shells that cannot accept anymore electrons Unreactive Will not combine (form bonds) with any other element 2 2,8 2,8, 8 2,8, 8, 18

6. Metal atoms Metal atoms have incomplete outer shells Have 1, 2 or 3 electrons on their outer shell Metal atoms want to LOSE these extra electrons in order to have a full outer shell (like the noble gases)

7. Metal atoms Metal atoms lose electrons to form a CATION CATION: when a neutral metal atom loses one or more electrons to form a positively charged ion 2,8,1  2,8

9. Metal Cations Possible Metal Cations: Lose 1 electron = +1 eg. K + Lose 2 electrons = +2 eg. Ca 2+ Lose 3 electrons = +3 eg. Al 3+ Aluminum metal lost 3 electrons to become stable

10. Non-metal Atoms Non-metals have incomplete outer shells Have 5, 6, or 7 electrons on their outer shell Non-Metal atoms want to GAIN additional electrons in order to have a full outer shell (like the noble gases) 2, 8, 7 2, 6

11. Non-Metal atoms Non-Metal atoms gain electrons to form an ANION ANION: when a neutral non-metal atom gains one or more electrons to form a negatively charged ion 2,8,7  2,8,8

12. Non-Metal Anions Possible Non-Metal Anions: Gain 1 electron = -1 eg. F - Gain 2 electrons = -2 eg. O 2- Gain 3 electrons = -3 eg. N 3- Nitrogen non-metal atom gains 3 electrons to become stable

13. Ionic Bonds - results from the TRANSFER of electrons from a metal to a non-metal Lithium atom needs to lose 1e- where Fluorine atom needs to gain 1e- -What a perfect match! -They will form an ionic bond! -Cations Anions

14. Opposites Attract!!

15. Ions are held strongly by opposite charges in a 3D lattice

17. Properties 1. High melting points because of strong attractions between cations and anions 2. Soluble in water Soluble (lattice breaks apart into free ions)

18. 3. Conducts electricity because of the charged ions freely moving in water (but not in solid state)

19. 4. Brittle – similar ions can repel if they come into contact