1. Chemical Bonds (general), Ionic, Covalent, & Metallic Bonds
BONDING
Chemical Bonds (general),
Ionic, Covalent, & Metallic Bonds

2. Discuss with your elbow partners
CHEMICAL BONDS: GENERAL
What type of electron configuration (# valence electrons) do atoms need to be stable?
What group of elements is naturally stable?
What do elements do to become stable if they don’t have a full valence shell?
What is a chemical bond?
What is a compound?
Discuss with your elbow partners

3. IONIC
BONDS

4. 1. What is an ionic bond?
Atoms GAIN or LOSE electrons (which gives them positive or negative charges and makes them ions).
Always between a METAL and NONMETAL

5. 2. Properties of Ionic Compounds
When ions bond together, they form ionic compounds.
Ionic compounds are:
Brittle
Have high melting points (usually solids)
Dissolve in water/conduct electricity

6. 3. Example/additional notesF K

7. K F

8. K F

9. K F

10. K F

11. K F

12. K F

13. + _ K F
Cation
Anion

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

15. K F _ Potassium Fluoride + NOW CALLED The ionic bond is the attraction
between the positive K+ ion
and the negative F- ion
NOW CALLED
Potassium Fluoride

17. Review - Work with your elbow partner to complete the Review at the top of page 2.

18. Review Ionic bonds form between a METAL and a NONMETAL.
Metals will LOSE electrons while nonmetals will GAIN electrons.
This makes the metal have a + charge (CATION) and the nonmetal have a - charge (ANION).
These opposite charges cause the atoms to be attracted to each other.

19. Review
Group 1 will form ionic bonds with group 17. Group 2 will form ionic bonds with group 16.
To name the new compound, name the metal first and change the nonmetal’s ending to -ide.

20. Element
Atomic Symbol
Total electrons
# of Valence electrons
Electron Dot Diagram (EDD)
# of Electrons lost or gained
Charge on Atom
(oxidation #)
Bromine
Lithium
Calcium
Sulfur
Chlorine
Carbon and
Silicon
Explain why these won’t form ionic bonds.

21. Sodium + Chlorine Magnesium + Iodine Potassium + Iodine Sodium + Oxygen
EDD
EDD for ions formed (include correct charge and # of atoms for each)
Formula of new compound:
Name of new compound:
EDD for ions formed (include correct charge and # of atoms for each)
EDD for ions formed (include correct charge and # of atoms for each)
EDD for ions formed (include correct charge and # of atoms for each)

22. COVALENT
BONDS

23. So what are covalent bonds?

24. In covalent bonding,
atoms still want to achieve
a full outer electron shell.
(the octet rule).

25. But rather than losing or gaining electrons,
In covalent bonding,
atoms still want to achieve
a full outer electron shell
(the octet rule).
But rather than losing or gaining
electrons,
atoms share an electron pair.

26. 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.

27. Covalent bonds occur between TWO nonmetals.
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.
Covalent bonds occur between
TWO nonmetals.

28. Chlorine
forms a
covalent
bond
with
itself
Cl2

29. How
will
two
chlorine
atoms
react? Cl Cl

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

31. Cl Cl do to achieve an octet? What’s the solution – what can they
Neither atom will give up an electron –
What’s the solution – what can they
do to achieve an octet?

32. Cl Cl

33. Cl Cl

34. Cl Cl

35. Cl Cl

36. Cl Cl
octet

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

38. 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

39. 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

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

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

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

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

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

45. O2
Oxygen in the air is composed of two covalently
bonded molecules

46. O
How will two oxygen atoms bond?

47. O
Each atom has two unpaired electrons

48. O

49. O

50. O

51. O

52. O

53. O

54. O
both atoms want to gain two electrons.

55. O .
both atoms want to gain two electrons.

56. O

57. O O

58. O O

59. O O

60. Both electron pairs are shared.

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

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

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

64. can be shown as two dashes.=
The double bond
can be shown as two dashes.

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

67. Video showing
Na + Cl  NaCL (ionic Bond)
2H + O  H20
Another video showing ionic and covalent bonds

71. METALLIC
BONDS

72. Metallic Bonding
Metallic bonds = attraction between metal ions and delocalized electrons
Electrons are far from the nucleus and free to travel around “sea of electrons”
Valence shells of nearby atoms overlap
Electrons can flow between atoms (electricity)
when an atom’s electrons “leave” it becomes a positive ion which attracts nearby electrons
Free electrons can slide over each other, nuclei follow  metals are malleable and ductile

74. Metallic Bonds: Mellow dogs with plenty of bones to go around These bonds are best imagined as a room full of puppies who have plenty of bones to go around and are not possessive of any one particular bone. This allows the electrons to move through the substance with little restriction.
(for other bond type analogies)