1. BONDING
PART II

2. Covalent
Bonds

3. LET’S
FIRST
REVIEW
IONIC
BONDING

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

5. K F

6. K F

7. K F

8. K F

9. K F

10. K F

11. + _ K F

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

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

14. So
what
are
covalent
bonds?

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

16. But rather than losing or gaining electrons,
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.

17. The shared electron pair is called a bonding pair
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

18. Chlorine
forms a
covalent
bond
with
itself
Cl2

19. How
will
two
chlorine
atoms
react? Cl Cl

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

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

22. Cl Cl

23. Cl Cl

24. Cl Cl

25. Cl Cl

26. Cl Cl
octet

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

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

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

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

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

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

35. O2
Oxygen is also one of the diatomic molecules

36. O
How will two oxygen atoms bond?

37. O
Each atom has two unpaired electrons

38. O

39. O

40. O

41. O

42. O

43. O

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

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

46. O

47. O O

48. O O

49. O O

50. Both electron pairs are shared.

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

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

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

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

55. This is the oxygen molecule,=
this is so cool!!
This is the oxygen molecule, O2