1. 2.2.1
Ionic Bonding

2. Protons
Electrons
Overall Charge
18 18+
18 18 0
40
Ar
18
ATOM
•Noble Gas •Also Ne, He, Xe, Kr, Rn
•Stable or Unreactive
18+
•Full outer shell
•All atoms want to be like
this i.e. have a full outer
shell - Octet Rule

3. Protons 11 11+
Electrons 11 11Overall
0
23
Na
11
•One electron in outer shell
ATOM
11+
•Wants to get a full
outer shell
•To have the same
pattern as a Noble Gas
•Loses electron from
outer shell

4. Protons 11 11+
Electrons 11 11Overall
0
11+
23
Na
11

5. Protons
11 11+
+
Na
Electrons 10 101+
Overall
ION
Full outer shell
Same pattern as neon
11+
Stable
Now has a + charge
Called an ION

6. Where has the electron gone?

7. Protons
Electrons
17 = 17+
17 = 17 =0
Overall
ATOM
35
Cl
17
7 electrons in outer shell
17+
Wants to get a full
outer shell
Takes an electron into
its outer shell

8. Protons
Electrons
17 17+
18 18 -
Overall
1-
ION
Cl
Full outer shell
Same pattern as Argon
17+
Stable
Now has a - charge
Called an ION

9. Unlike charges attract
Na+
Na+
Cl-
Cl-

10. Sodium atoms lose an electron to become
sodium ions
 Sodium ions have a +ve charge
 Chlorine atoms gain an electron to become
Chloride ions
 Chloride ions have a − ve charge
 Opposite charges attract so the Na+ and Clcome together and stick to each other
 This is called an ionic bond


12. Ionic Bonding involves a transfer of electrons
It happens when the difference in
electronegativity between atoms > 1.7
 Metals lose electrons to form positive ions
 They gain one plus charge for each electron lost
 Non-metals gain electrons to form negative
ions
 They gain one minus charge for each electron
gained
 Total electron loss must equal electron gain



13.  Atoms in the same group [column]
 Have the same outer electron
configuration.
 Have the same valence electrons.
 Easily found by looking up the group
number on the periodic table.
 Group 2A - Be, Mg, Ca, etc. 2 valence electrons

14. +
M
Group I lose 1 e- to become
2+
Group II lose 2 e- to become M
3+
Group III lose 3 e- to become M
3Group V gain 3 e- to become X
Group VI gain 2 e- to become X2Group ViI gain 1 e- to become X+
There are exceptions

15. Group I with Group VII
M +1
Formula MX
X-1

16. Group II with Group VI
Be
Mg
Ca
Sr
Ba
Ra
M 2+
Formula MX
X2-
O
S
Se
Te
Po

17. Group III with Group V
B
Al
Ga
In
Tl
M 3+
Formula MX
X3-
N
P
As
Sb
Bi

18. Group II with Group VII
Be
Mg
Ca
Sr
Ba
Ra
M 2+
Formula MX2
X1-
X1-
F
Cl
Br
I
At

19. Group III with Group VII
B
Al
Ga
In
Tl
X1M 3+
Formula MX3
X1-
X1-
F
Cl
Br
I
At

20. Group II with Group VI
Be
Mg
Ca
Sr
Ba
Ra
M+
X2M+
Formula M2X
O
S
Se
Te
Po

21. Group I with Group V
Li
Na
K
Rb
Cs
Fr
M+
X3M+
Formula M3X
M+
N
P
As
Sb
Bi

22. Group III with Group VII
M 3+
B
Al
Ga
M 3+
In
Tl
X2-
X2-
Formula M2X3
F
Cl
Br
X2I
At

23. Group II with Group V
M 2+
Be
Mg 2+
M
Ca
Sr
M 2+
Ba
Ra
Formula M3X2
X3-
X3-
N
P
As
Sb
Bi

24. 






Aluminium :oxygen •
Magnesium :nitrogen
Barium: Arsenic
•
Aluminium :Iodine
Gallium :Sulphur
•
Barium :Oxygen
Sodium :Fluorine
•
Draw diagrams – outer
shell only required
Show electron movement
with arrows
Show atoms with charge
and number
Write formula [without
charges] and name