The document discusses the formation of covalent bonds between non-metallic elements using dot-and-cross diagrams. It explains that in covalent bonding, atoms share electron pairs rather than gaining or losing electrons in order to achieve a noble gas configuration. Chlorine atoms form a single covalent bond by each sharing one electron pair between them to fill their octets. Similarly, oxygen atoms form a double covalent bond by each sharing two electron pairs to fill their octets.

1. DONE BY :GRACE MELLISA ARIFIN
CLASS :3I

2. Using ‘dot-and-cross’
diagrams:
The formation of
covalent bonds
between non- metallic
elements

3. what
are
covalent
bonds?

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

5. 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.

6. 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

7. Chlorine
forms
covalent
a Cl2
bond
with
itself

8. How
will
Cl Cl two
chlorine
atoms
react?

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

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

11. Cl Cl

12. Cl Cl

13. Cl Cl

14. Cl Cl

15. Cl Cl
octet

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

17. 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

18. 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

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

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

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

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

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

24. O2
Oxygen is also one of the diatomic molecules

25. O O
How will two oxygen atoms bond?

26. O O
Each atom has two unpaired electrons

27. O O

28. O O

29. O O

30. O O

31. O O

32. O O

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

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

35. O O

36. O O

37. O O

38. O O

39. O O
Both electron pairs are shared.

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

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

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

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

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

46. CRED