Types of Bonding and Lewis
Structures
Quiz on Monday
Describe the structure of metallic
bonding.
•Positive
metallic ions surrounded by electrons.
Example of Metallic
Bonding
What type of bonding must exist if a
substance can conduct electricity dry?
Why?

Metallic; the delocalized electrons are able to
flow freely around the positive metal ions
Potassium bromide forms a crystal
lattice structure. What type of bonding
would you expect it have?

Ionic
If a substance dissolves in water
and makes a solution that
conducts electricity, what types of
bonds do you expect hold it
together?
•Ionic; forms
ions in solution to make it an electrolyte
If a substance melts in your hands, what
type of bonds do you expect to hold it
together?

Covalent (polar and non-polar); covalently
bonded substances have low melting points
Which of these elements would
make a covalent bond with
nitrogen?
Al
Mg
•C; non-metal
Ba
C
with non-metal bonding (also similar
electronegativity)
Which of these elements would
make an ionic bond with
potassium?
Mg
N
•N, Cl; metal
Sr
Cl
with non-metal bond (also difference in
electronegativities is relatively large)
Which of these elements would
make an ionic bond with chlorine?
O
•Li; metal
F
Li
Xe
with non-metal bond (also difference in
electronegativities is relatively large)
What type of bond exists
between chlorine (EN = 3.0) and
bromine (EN = 2.8)
•Non-polar
covalent; both elements are non-metals with
their difference in electronegativity being less than 0.5
What type of bond exists between
nitrogen (EN = 3.0) and hydrogen
(EN = 2.1)
•Polar
covalent; both elements are non-metals with their
difference in electronegativity being between 0.5 and 1.7
Draw the correct Lewis dot
structure for CH2O
Draw the correct Lewis dot
structure for CH2O
Draw the correct Lewis dot
structure for SCl2
Draw the correct Lewis dot
structure for SCl2
Draw the correct Lewis Dot Structure
for O2
Draw the correct Lewis Dot Structure
for O2
Electron Configuration
Review Questions
Write the electron configuration
for the element fluorine
•1s22s22p5
Write the electron configuration
for the element potassium
•1s22s22p63s23p64s1
Write the electron configuration
for the element silicon
•1s22s22p63s23p2
Write the electron configuration
for the element titanium
•1s22s22p63s23p64s23d2
Write the noble gas configuration
for the element rubidium
•[Kr]5s1
Write the noble gas configuration
for the element chlorine
•[Ne]3s2 3p5
Which element has the following
electron configuration:
2
2
6
2
6
2
6
1s 2s 2p 3s 3p 4s 3d
•Iron, Fe
Which element has the following
electron configuration:
2
2
6
2
6
2
10
3
1s 2s 2p 3s 3p 4s 3d 4p
•Arsenic, As
Write the orbital notation for the
element carbon
•↑↓
1s
↑↓
↑
2s
↑
.
2p
Write the orbital notation for the
element sulfur
•↑↓
1s
•↑↓
3s
↑↓
2s
↑↓ ↑
↑↓ ↑↓ ↑↓.
2p
↑.
3p
Write the orbital notation for the
•↑↓ element
↑↓
↑↓ ↑↓ ↑↓selenium
↑↓
1s
2s
2p
3s
3p
3d
4p
4s
Write the Lewis Dot structure for
the following atoms and their ions
Aluminum

Al (group 13; 3 valence electrons)

Al+3 (aluminum loses its 3 valence electrons to
satisfy the octet rule)
Phosphorus


P (group 15; 5 valence electrons)
P -3 (phosphorus gains 3 electrons to satisfy
the octet rule)
Helium

He (group 18 but it has 2 valence electrons)

No ionic form of helium. It already has a full
valence shell so it already satisfies the octet rule
Strontium

Sr (group 2; 2 valence electrons)

Sr+2 (strontium loses its 2 valence electrons to
satisfy the octet rule)