2. Covalent bonding Grade 9 Chemistry

3. 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!

4. LET’S FIRST REVIEW IONIC BONDING

5. In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds. FK

6. FK

7. FK

8. FK

9. FK

10. FK

11. FK

12. FK + _

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

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

15. So what are covalent bonds?

16. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule).

17. 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.

18. 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

19. Cl 2 Chlorine forms a covalent bond with itself

20. Cl How will two chlorine atoms react?

21. Cl Each chlorine atom wants to gain one electron to achieve an octet

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

23. Cl

27. octet

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

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

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

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

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

33. Cl circle the electrons for each atom that completes their octets It is called a SINGLE BOND

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

35. Cl circle the electrons for each atom that completes their octets This is the chlorine molecule, Cl 2

36. O2O2 Oxygen is also one of the diatomic molecules

37. How will two oxygen atoms bond? OO

38. OO Each atom has two unpaired electrons

39. OO

40. OO

41. OO

42. OO

43. OO

44. OO

45. Oxygen atoms are highly electronegative. So both atoms want to gain two electrons. OO

46. Oxygen atoms are highly electronegative. So both atoms want to gain two electrons. OO

47. OO

48. OO

49. OO

50. OO

51. O O Both electron pairs are shared.

52. 6 valence electrons plus 2 shared electrons = full octet O O

53. 6 valence electrons plus 2 shared electrons = full octet O O

54. two bonding pairs, O O making a double bond

55. O O = For convenience, the double bond can be shown as two dashes. O O

56. O O = This is the oxygen molecule, O 2 this is so cool! !

57. COVALENT BOND bond formed by the sharing of electrons

58. What is a covalent bond? Atoms ___________ one or more electrons with each other to form the bond. Each atom is left with a ________________ outer shell. A covalent bond forms between two _________________. Example 1: Hydrogen + HydrogenExample 2: Hydrogen + Oxygen SHARE COMPLETE NONMETALS 1.Dot and cross diagram 2.Formula

59. Covalent Bond Between nonmetallic elements of similar electronegativity. Formed by sharing electron pairs They are not conductors at any state Examples; O 2, CO 2, C 2 H 6, H 2 O, SiC

60. Now try the covalent bonding practice sheet