How covalent bonding occurs

1. PART II

2. Covalent
Bonds

3. LET’S
FIRST
REVIEW
IONIC
BONDING

4. In an IONIC bond,
electrons are lost or gained (transferred).
This resulting in the formation of IONS
in ionic compounds.
FK

5. FK

6. FK

7. FK

8. FK

9. FK

10. FK

11. FK
+
_

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

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

14. We can’t forget about Metallic Bonds either.
• A metallic bond forms when electrons are
shared between two metallic ions.
• Metallic bonds are formed from the attraction
between mobile electrons and fixed, positively
charged metallic ions.

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,
In a covalent bond 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. Cl2
Chlorine
forms
a
covalent
bond
with
itself

20. ClCl
How
will
two
chlorine
atoms
react?

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

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

23. ClCl

24. Cl Cl

25. Cl Cl

26. Cl Cl

27. Cl Cl
octet

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

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

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

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

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

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

36. O2
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. OO
Both electron pairs are shared.

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

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

54. two bonding pairs,
OO
making a double bond

55. OO=
For convenience, the double bond
can be shown as two dashes.
OO
Structural Formula for O2

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

58. Let’s Review - Please Flip over your note
outline and write this on the back!
• Ionic Bonds form when electrons are transferred
between metals and non-metals. Ionic Compounds are
brittle and have high melting points.
• Covalent bonds form when electrons are shared between
two non-metals. Covalent Compounds have lower
melting points, do not conduct electricity, and are softer.
• Metallic Bonds form when electrons move freely
between two metal ions. Metallic compounds are
malleable and good conductors of heat and electricity.