2. Chapter 8 Ionic and Metallic Bonding

3. Keeping Track of Electrons l The electrons responsible for the chemical properties of atoms are those in the outer energy level. l Valence electrons - The s and p electrons in the outer energy level (d and f electrons are backfilled - never in valence shell). l Kernel (core) electrons -those in the energy levels below the valence shell.

4. Keeping Track of Electrons l Atoms in the same column l Have the same outer electron configuration. l Have the same valence electrons. l Easily found by looking up the group number on the periodic table. l Group 2 - Be, Mg, Ca,.- 2 valence electrons l The last digit in the representative group number gives the number of valence electrons

5. Electron Dot diagrams (Lewis Structure) l A way of keeping track of valence electrons. l How to write them l Write the symbol. l Put one dot for each valence electron l Don’t pair up until they have to X

6. The Electron Dot diagram for Nitrogen l Nitrogen has 5 valence electrons. l First we write the symbol. N l Then add 1 electron at a time to each side. l Until they are forced to pair up.

7. Write the electron dot diagram for Na Mg C O F Ne He Na Mg C O F Ne He

8. Electron Configurations for Cations l Metals lose electrons to attain noble gas configuration (Born losers). l They make cations (positive ions). l If we look at electron configuration it makes sense. l Na 1s 2 2s 2 2p 6 3s 1 - 1 valence electron l Na + 1s 2 2s 2 2p 6 -noble gas configuration

9. Electron Dots For Cations l Metals will have very few valence electrons Ca

10. Electron Dots For Cations l Metals will have very few valence electrons l These will come off Ca

11. Electron Dots For Cations l Metals will have very few valence electrons l These will come off l Forming cations (positive ions) Ca 2+

12. Electron Configurations for Anions l Nonmetals gain electrons to attain noble gas configuration. l They make anions (negative ions). l If we look at electron configuration it makes sense. l S 1s 2 2s 2 2p 6 3s 2 3p 4 - 6 valence electrons l S 2- 1s 2 2s 2 2p 6 3s 2 3p 6 -noble gas configuration.

13. Electron Dots For Anions l Nonmetals will have many valence electrons. l They will gain electrons to fill outer shell. P P 3-

14. Stable Electron Configurations l All atoms react to achieve noble gas configuration. l Noble gases have 2 s and 6 p electrons. l 8 valence electrons. l Also called the octet rule. Ar

15. Ionic Bonding l Anions and cations are held together by opposite charges. l Ionic compounds are called salts. l Simplest ratio is called the formula unit. l The bond is formed through the transfer of electrons. l Electrons are transferred to achieve noble gas configuration.

16. Ionic Bonding NaCl

17. Ionic Bonding Na + Cl -

18. Counting Electrons During the formation of an ionic compound the total number of electrons lost (by metals in forming cations) must equal the total number of electrons gained (by anions). Ca Group 2 loses 2 e - P Group 15 (5A) gains 3e - To keep totals equal a LCM of 6 is used. Therefore:3 x Ca = 3 x 2 + = 6 + 2 x P = 2 x 3 - = 6 - 6 lost (+6) = 6 gained (6-) Charges cancel.

19. Ionic Bonding l All the electrons must be accounted for, total lost = total gained! CaP

20. Ionic Bonding CaP

21. Ionic Bonding Ca 2+ P

22. Ionic Bonding Ca 2+ P Ca

23. Ionic Bonding Ca 2+ P 3- Ca

24. Ionic Bonding Ca 2+ P 3- Ca P

25. Ionic Bonding Ca 2+ P 3- Ca 2+ P

26. Ionic Bonding Ca 2+ P 3- Ca 2+ P Ca

27. Ionic Bonding Ca 2+ P 3- Ca 2+ P Ca

28. Ionic Bonding Ca 2+ P 3- Ca 2+ P 3- Ca 2+

29. Ionic Bonding Ca 3 P 2 Formula Unit

30. Properties of Ionic Compounds l Crystalline structure. l A regular repeating arrangement of ions in the solid. l Ions are strongly bonded. l Structure is rigid. l High melting points- because of strong forces between ions.

31. Crystalline structure

32. Crystal Lattice Crystal Lattice – a regular repeating pattern. The cations and anions are arranged to maximize the neutralization of electrostatic force fields. We se these patterns as crystals.

38. Do they Conduct? l Conducting electricity is allowing charges to move. l In a solid, the ions are locked in place. l Ionic solids are insulators. l When melted, the ions can move around. l Melted ionic compounds conduct. l First get them to 800ºC. l Dissolved in water they conduct.

39. Metallic Bonds l How atoms are held together in the solid. l Metals hold onto there valence electrons very weakly. l Think of them as positive ions floating in a sea of electrons.

40. Sea of Electrons ++++ ++++ ++++ l Electrons are free to move through the solid. l Metals conduct electricity.

41. Metals are Malleable l Hammered into shape (bend). l Ductile - drawn into wires.

42. Malleable ++++ ++++ ++++

43. ++++ ++++ ++++ l Electrons allow atoms to slide by.

44. Ionic solids are brittle +-+- + - +- +-+- + - +-

45. + - + - + - +- +-+- + - +- l Strong Repulsion breaks crystal apart.