Chemical Bonds – Ionic Bonds
1. Identify the Number of Valance Electrons and Draw the Lewis Dot Structure
Notes: Scientists use Lewis Dot Structures to show the valance electrons of an element as dots.
Since bonding involves the valance shell electrons only, it is only necessary to illustrate those outer
electrons.
Element
Calcium
Carbon
Hydrogen
Helium
Oxygen
Fluorine
Neon
Sodium
Aluminum
Group Number
(PT)
# of Valance
Electrons
Lewis Dot Structure
Notes: Remember that Metals tend to lose their electrons, falling back to their inner octet,
becoming smaller, forming positive “cations”. Nonmetals tend to gain electrons, filling up their
current energy levels, becoming larger, forming negative “anions”. Complete the chart below.
Element
Na
Be
Cl
S
Al
Ne
K
N
O
Ca
P
B
Mg
Lewis Dot
# of Valance e-
Gain/Lose ___ e-
Valance Charge
1
L1
+1
Chemical Bonds – Ionic Bonds KEY
2. Identify the Number of Valance Electrons and Draw the Lewis Dot Structure
Notes: Scientists use Lewis Dot Structures to show the valance electrons of an element as dots.
Since bonding involves the valance shell electrons only, it is only necessary to illustrate those outer
electrons.
Element
Calcium
Carbon
Group Number
(PT)
IIA 2
IVA 14
Hydrogen
IA 1
Helium
VIIIA 18
# of Valance
Electrons
2
4
2
●●
He
6
Fluorine
VIIA 17
7
Sodium
IA 1
Aluminum
IIIA 13
●
●C●
●
1
VIA 16
VIIIA 18
●
Ca●
●
H
Oxygen
Neon
Lewis Dot Structure
●●
●O●
●●
●●
:F:
●
●●
8
:Ne:
1
●●
●
Na
3
●
●Al●
Notes: Remember that Metals tend to lose their electrons, falling back to their inner octet,
becoming smaller, forming positive “cations”. Nonmetals tend to gain electrons, filling up their
current energy levels, becoming larger, forming negative “anions”. Complete the chart below.
Element
Lewis Dot
# of Valance e-
Gain/Lose ___ e-
Valance Charge
Na
●
Na
1
L1
+1
Be
●
Be●
2
L2
+2
7
G1
-1
●●
Cl
:Cl:
●
●
S
: S:
6
G2
-2
Al
●
●
Al●
●
●●
3
L3
+3
Ne
:Ne:
8
0
0
●●
●
K
1
L1
+1
5
G3
-3
:O:
6
G2
-2
●
●
Ca●
2
L2
+2
K
N
O
Ca
●●
●N●
●
●
P
B
Mg
●●
●P●
●
●
●B
●
●
Mg
●
5
G3
-3
3
L3
+3
2
L2
+2