1. You Will Need:
1. Pencil, Text Book- Periodic Table,
Colored Pencils
2. Ionic & Covalent Bonding 2 pages-4
sides (Pick-up from bookshelf)
4. Log #3 Update
5. Building Blocks of Matter –
Counting Atoms– Due tomorrow

2. Please SCHEDULE:
1. To take Retake Test #2
• 129/185 or lower
2. Starts Thursday of this week
3. Parent Signature and
Corrections – due Wed.

3. You will need 100 3 x 5 cards
1. Print out Questions & Answers hyperlinked
on Learning Point
• Glue, Staple or Tape Questions on
the Front and Answers on the back
OR
• You can write out the questions &
answers
2. Due at the beginning of class on
Friday
3. Quiz on Friday

4. • Please Pick up your belongings
1. Move to the back of the room
2. Take your new seat when your
name is called
• Decide on your new job
• Manager, Materials
Manager, Timer Designer,
Oral Presenter

5. 1. The substances on the left side of a
periodic table are most likely this class
of elements….
2. Which subatomic particle determines
the charge of the atom?
3. The scientist who believed the atomic
structure resembled the solar system?
4. The least reactive elements on the
Periodic Table are the ______________.
5. The type of electrons that determine
how an atom will bond to another
atom are the ___________________.

6. 6. The subatomic particle responsible for
determining the atom you are looking
at are the ____________.
7. Why are elements’ atoms on the
periodic table neutral?
8. When an element’s atomic structure
has more or less neutrons we call this
an ______.
9. What is the valence of Nitrogen? How
do you know?
10. How many more electron bonds
would Nitrogen need to have a full
outer shell?

7. Timer Designers: In charge of today’s lesson
on the computer (R & R Required)
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.

8. 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.
Need to Know!
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.

9. 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.

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

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

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

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

14. Crystal Lattice
uth
Bi s m

15. Question Answer
What are the characteristics of • Usually between Metals and Nonmetals
Ionic Bonds? • 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 Before you move to the next slide….try to draw
Model of an aluminum atom. this on your own and then check to see how
you did.
If you made a mistake….figure out what you
did incorrectly.

16. Question Answer
What are the characteristics of • Usually between Metals and Nonmetals
Ionic Bonds? • 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.
3
2 8
P=13
N=14

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

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

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

20. 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
• Do not have a specific shape - flexible
View Video – Covalent Bonding –
hyperlinked on Learning Point. How many types of covalent bonds are shown in the
http://www.youtube.com/watch?v=1wpDicW_MQQ
video clip? ______

21. C 12 H 22 O 11
C 6 H 10 O 5

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

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

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

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

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

27. Homework:
1) Building Blocks of Matter –
Counting Atoms – Due Tomorrow
2) Test #2 Corrections and Signature
– Due Wednesday
3) Ionic and Covalent Bonding – Due
Thursday
4) STAR Cards #1-30 – on 3x5 cards
– Due Friday at the beginning of
class