This document discusses ionic bonding, which involves the transfer of electrons between atoms to form ions. Metals form cations by losing electrons to achieve a full outer shell like a noble gas. Nonmetals form anions by gaining electrons to also achieve a full outer shell. Oppositely charged ions then attract through ionic bonding. The number of electrons lost or gained can be predicted based on the group of elements in the periodic table. Examples of ionic compounds formed between different groups are given along with their formulas and electron arrangements.

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