Bonding & Lewis Dot Structures WS
The information below will help you better understand the behavior of the elements in the periodic table,
ionic bonding, covalent bonding, and Lewis dot structures.
Rules:
The elements of the periodic table can be classified into Losers, Takers, and Nobles.
1. Chemistry (like history) suggests that it is good to be Noble like kings! The Octet Rule says that all
elements would like to have 8 valence electrons, just like the noble gases in group 8A (except He)
because atoms want to have complete outer rings (valence shells).
2. The group (column) numbers of the periodic table indicate the number of valence electrons. The
only exception is Helium (He), which is complete with 2 electrons instead of 8 even though it is in
group 8A.
3. LOSERS = Metal elements in Groups 1-3A. Elements from these groups want to be like the noble
gases and happily lose their electrons. By losing their valence electrons, they expose complete
inner rings and become king-like. LOSERS of electrons are METALS, and they form IONIC BONDS
by transferring their electrons.
4. TAKERS = Nonmetal elements in Groups 4-7. These elements also want to be like the noble gases.
TAKERS of electrons are NONMETALS, and they can form IONIC or COVALENT BONDS depending
on who they’re paired with.
Nonmetal elements (TAKERS) can…
1) Steal (transfer) electrons from the metals to complete their valence shells to form IONIC bonds.
Draw the
Lewis dot
structures.
NaCl
→
→
→
Draw an arrow to show the
transfer (stealing) of
→
electrons from the metal
(Na) to the nonmetal (Cl).
Use charges to
→ distinguish between the
cation (+) and anion (-).
Write the
→ formula for the
ionic compound.
2) Share electrons with another nonmetal (including hydrogen) to complete valence shells and form
COVALENT bonds.
→
→
→
F2
Draw the
Lewis dot
structures.
→ Encircle the
electrons that
will be shared.
or
→ Draw to show the sharing of
electrons to complete the octet
for each element. Now each
element has 8 electrons.
→ Write the formula
for the molecular
(covalent)
compound.
Fill in the table below. Use an ARROW to show the transfer (stealing) of electrons in an ionic bond
or CIRCLE electrons that are shared in a covalent bond. Use the examples for help.
Element 1
(Label metal
or nonmetal)
Ca
metal
loses
Lewis Dot
Structure for
Element 1
Element 2
(Label metal
or nonmetal)
Cl
nonmetal
takes
Lewis Dot
Structure for
Element 2
Combined Dot Structures
with arrows (ionic) or
circles (covalent)
Formula of Compound
(Label ionic or
molecular)
CaCl2
Ionic
-
K
i
I
Na
Na
P
Ca
Ca
O
C
O
nonmetal
takes
nonmetal
takes
H
it
O
N
ii
H
S
is
F
p
O
Not Tia
Na
Nasp
ionic
i
Cao
ionic
CO2
Molecular
it
it
E
H2o
O
ii
molecular
Nits
i
molecular
É
SE
molecular
Use the name of each compound to determine the type of bond. Remember, in ionic compounds, metal
names stay the same and nonmetal endings change to -ide. In covalently bonded molecular compounds,
prefixes are used to tell the number of each atom since they can make more complex structures.
Name of
Compound
Sodium
chloride
Dot
Structure for
Element 1
Na
Carbon
tetrahydride
Magnesium
phosphide
Lead (IV)
oxide
Dot
Structure for
Element 2
ci
it
Nig
Pb
Combined Dot Structures with arrows
(ionic) or circles (covalent)
not.fi
t.M9
m.gg
O
ia
AI
N
ca
9.1
ci P
C
Bir
molecular
midiar
O
CI
F
c
c
B
gMgsPz
ionic
PDO
ionic
b
9.1
Phosphorous
trichloride
Nitrogen
tribromide
Pj
E
Carbon
tetrachloride
Aluminum
chloride
CH4
molecular
Diflouride
Calcium oxide
N
it
H
Formula of
Compound
(Label ionic or
molecular)
cao
ionic
ci
PCI
molecular
A
C
I
B.it
II
NBT
molecular