Starter

1. Starter • What ions do Chlorine form? • Imagine you have 2 chlorine ions – how could they help EACH OTHER to reach a stable state? • It might help if you draw out the Lewis structures for 2 chlorine ions!

2. LET’S FIRST REVIEW IONIC BONDING

3. K F In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds.

4. K F

5. K F

6. K F

7. K F

8. K F

9. K F

10. _ + K F

11. _ + K F The compound potassium fluoride consists of potassium (K+) ions and fluoride (F-) ions

12. _ + K F The ionic bond is the attraction between the positive K+ ion and the negative F- ion

13. So what are covalent bonds?

14. In covalent bonding, atoms still want to achieve a noble gas configuration (8 valence electrons).

15. In covalent bonding, atoms still want to achieve a noble gas configuration. But rather than losing or gaining electrons, atoms now share an electron pair.

16. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair. The shared electron pair is called a bonding pair

17. Fluorine forms a covalent bond with itself F2

18. How will two fluorine atoms react? F F

19. F F Each fluorine atom wants to gain one electron to have 8 valence electrons.

20. F F Neither atom will give up an electron What’s the solution –what can they do to achieve 8 valence electrons?

21. F F

22. F F

23. F F

24. F F

25. F F 8 valence electrons

26. F F 8 valence electrons circle the electrons for each atom that completes their octets

27. F F Bysharing the electron pair in the middle, each fluorine atom feels like it has 8 valence electrons circle the electrons for each atom that completes their octets

28. F F The electron pair in the middle (the circled one) is shared by the two atoms of fluorine. circle the electrons for each atom that completes their octets

29. F F This is called the bonding pair circle the electrons for each atom that completes their octets

30. F F It is a single bonding pair circle the electrons for each atom that completes their octets

31. F F It is called aSINGLE BOND circle the electrons for each atom that completes their octets

32. F F Single bonds are shown with with a dash circle the electrons for each atom that completes their octets

33. F F This is the fluorine molecule, F2 circle the electrons for each atom that completes their octets

34. O2 How will this molecule form?

35. O O

36. O O Each atom has two unpaired electrons

37. O O

38. O O

39. O O

40. O O

41. O O

42. O O

43. O O Both atoms want to gain two electrons.

44. O O Oxygen atoms are highly electronegative. So both atoms want to gain two electrons.

45. O O

46. O O

47. O O

48. O O

49. O O Both electron pairs are shared.

50. O O 6 valence electrons plus 2 shared electrons = 8 valence electrons 