1. You Will Need:
1. Pencil, Text Book- Periodic Table,
Colored Pencils
2. Pick up 2 manilla folders
3. Turn in STAR Cards 31-60 into the
box on the front table.
4. You will be assigned a computer
after your STAR test to continue
working on your Electrons and
Chemical Bonding Worksheet

2. You will have 15 minutes to complete your STAR
Quiz #2
When done:
1) Turn quiz into Turn-in Tray
2) Return Manilla folders to front bookshelf
3) Sign out a Computer w/Mrs. M.
4) Continue to work on completing pages 1-4 of your
Electrons and Chemical Bonding Worksheet
Please make sure:
1) You used your own words for the notes (except for
vocabulary words)
2) Highlighted important information
3) Review and Reflect on ALL pages.

3. Everything on this planet is made of atoms from
elements. Even though the number of elements
on the Periodic Table is limited, joining the
elements in different ways allows you to make a
huge number of combinations.
Chemical Bonding is the joining of atoms to form
new substances. The properties of these new
substances are different from the properties of
the original elements. When chemical bonds
form, electrons are shared, gained or lost.

4. Everything on this planet is made of atoms from elements.
Even though the number of elements on the Periodic
Table is limited, joining the elements in different ways
allows you to make a huge number of combinations.
Chemical Bonding is the joining of atoms to form new
substances. The properties of these new substances are
different from the properties of the original elements.
When chemical bonds form, electrons are shared,
gained or lost.
Understanding the electron configuration, (Electron Dot,)
for each atom will help you understand how different
elements will bond or not bond with other elements.
Need to Know!

5. Not all the electrons in an atom are used to
make chemical bonds. It is the electrons on
Outer-Most Level or VALENCE electrons,
(Electron-Dot) that determine how an atom
will react (bond). REMEMBER: You can use your
periodic table to determine valence values
for most elements.
Atoms want to be “happy” or stable….if they
have a full outer shell. Atoms that have fewer
than eight valence electrons usually form
bonds. The only time a full shell is equal to 2 if
for the element Helium.

6. Element Bohr Model Lewis Dot
(Symbol + Valence)
Lithium
Atomic #
Atomic Mass
– Atomic #
Neon
Atomic #
Atomic Mass
– Atomic #
Row =
Electrons=
Protons =
Neutrons =
2
3-
3+
7-3=
4
P = 3
N = 4
2
1
Li
Row =
Electrons=
Protons =
Neutrons =
P =10
N =10 Ne
2
10-
10+
20-10
10
2
8
valence
valence

7. Element Group Valence Bond or Not Bond
Hydrogen 1 1 Bond
Magnesium
Oxygen
Sulfur
Krypton
Lithium
Carbon

8. Compound Lewis Dot Bonding Config. Type of Bond and Why?
Sodium Fluoride
(NaF)
Diatomic Fluoride
(F2)
Hydrogen Fluoride
(HF)
Watch the video clip on Covalent & Ionic Bonding
(hyperlinked on Learning Point)

9. Question Answer
Ion • Charged atom
• Caused by a transfer (lose or gain)
or shared electron
What are the
characteristics of Ionic
Bonds?
• Usually between Metals and
Nonmetals
• Transfer of electrons – atoms
become IONS
• Form Crystal Lattices
• Brittle
• High melting and boiling points
• Dissolve easily in water
• Form compounds
• Specific shape

10. Crystal Lattice

11. Question Answer
What are the
characteristics of
Ionic Bonds?
• Usually between Metals and Nonmetals
• Transfer of electrons – atoms become
IONS
• Form Crystal Lattices
• Brittle
• High melting and boiling points
• Dissolve easily in water
• Form compounds
• Specific shape
Illustrate a
neutrally charged
Bohr Model of an
aluminum atom.
Before you move to the next slide….try
to draw this on your own and then
check to see how you did.
If you made a mistake….figure out what
you did incorrectly.

12. Question Answer
What are the characteristics
of Ionic Bonds?
• Usually between Metals and Nonmetals
• Transfer of electrons – atoms become
IONS
• Form Crystal Lattices
• Brittle
• High melting and boiling points
• Dissolve easily in water
• Form compounds
• Specific shape
Illustrate a neutrally
charged Bohr Model of
an aluminum atom. P=13
N=14
2 8
3

13. Question Answer
Illustrate a positively
charged Bohr Model
of an aluminum
atom. (3+)
Before you move onto the
next slide….try to draw this
on your own.

14. Question Answer
Illustrate a positively
charged Bohr Model of
an aluminum atom. (3+)
Why is Al3+
considered an ion?
(Look at all the subatomic particles before you
answer this question.)
P=13
N=14
2
8

15. Forming Sodium Chloride
http://www.youtube.com/watch?v=2mzDwgyk6QM
Before (pg. 233) After
Questions:
1) Why does Sodium become an Ion?
2) Is it Positive or Negative? Why?
3) Why does Chlorine become an Ion?
4) Is it Positive or Negative? Why?
Questions:
1) Why do Sodium and Chlorine bond?
2) What is the overall charge of the
compound?
3) Does NaCl have the same
characteristics as Na and Cl?
4) What are some unique
characteristics of NaCl?

16. Question Answer
Characteristics of
Covalent bonds
• Valance electrons are shared
• More often between nonmetal
• Low melting and boiling point
• Free flowing but can be brittle
• Form molecules
• Usually do not have a specific
shape - flexible
View Video – Covalent
Bonding – hyperlinked
on Learning Point.
http://www.youtube.com/
watch?v=1wpDicW_MQ
Q
How many types of covalent bonds
are shown in the video clip? ______

17. C6H10O5
C12H22O11

18. Molecule Illustration Explanation Electron Dot (Color Code each
element)
1. What kind of bond does
Hydrogen & Oxygen
make?
2. How do you know?
3. Why does one Oxygen
bond with two
Hydrogen atoms?
http://www.youtube.com/watch?v=ulyopnxjAZ8&feature=relmfu
Drawing Lewis Dot Diagram Bonds
P=8
N=8
P=1
N=0
P=1
N=0

19. P=8
N=8
P=1
N=0
P=1
N=0
How do we determine the type of
bond in a compound?
• Identify class of elements
• Same class usually covalent
• Opposite class usually ionic
• Calculate the electronegativity factor
What is ELECTRONEGATIVITY? A measure of how much an element
wants an electron
How do you know the
electronegativity factor of an
element?
Look it up (see next slide)
What are the determining values for
each type of bond?
0-0.4 = Non-polar covalent
.41-2.0 = Polar covalent
>2.0 = Ionic
http://www.youtube.com/watch?v=7DjsD7Hcd9U

20. http://www.tutor-homework.com/Chemistry_Help/electronegativity_table/electronegativity.html
ELECTRONEGATIVITY VALUES
0-0.4 = Non-polar covalent
.41-2.0 = Polar covalent
>2.0 = Ionic

21. Let’s try a couple:
P=8
N=8
P=1
N=0
P=1
N=0
H2O Calculate the electronegativity factor
H = 2.2
O = 3.44
3.44 – 2.2 = 1.24
NaCl
0-0.4 = Non-polar covalent
.41-2.0 = Polar covalent
>2.0 = Ionic
Polar Covalent
Ionic
Na = .93
Cl = 3.16
3.16 - .93 = 2.23

22. Homework:
1)Ionic and Covalent Bonding – Due
next Wed.
2)STAR Cards #31-30 – on 3x5
cards – Due Tomorrow at the
beginning of class