Covalent Bonds

1. Covalent Bonds

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 tend to achieve a noble gas configuration (the octet rule).

15. In covalent bonding, atoms still tend to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair.

16. In covalent bonding, atoms still tend 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. Chlorine forms a covalent bond with itself Cl2

18. How will two chlorine atoms react? Cl Cl

19. Cl Cl Each chlorine atom gains one electron to achieve an octet

20. Cl Cl Neither atom will lose an electron – chlorine is highly electronegative. What’s the solution –what can they do to achieve an octet?

21. Cl Cl

22. Cl Cl

23. Cl Cl

24. Cl Cl

25. Cl Cl octet

26. Cl Cl octet circle the electrons for each atom that completes their octets

27. Cl Cl The octet is achieved by each atom sharing the electron pair in the middle circle the electrons for each atom that completes their octets

28. Cl Cl The octet is achieved by each atom sharing the electron pair in the middle circle the electrons for each atom that completes their octets

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

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

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

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

33. Cl Cl This is the chlorine molecule, Cl2 circle the electrons for each atom that completes their octets

34. O2 Oxygen is also one of the diatomic molecules

35. O O How will two oxygen atoms bond?

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 Oxygen atoms are highly electronegative. So 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 = full octet