Basic Civil Engineering first year Notes- Chapter 4 Building.pptx
Bohr Model vs. Wave Model + Lewis Dot Diagrams - Day 2
1. You Will Need:
1. Pencil, Text Book- Periodic Table,
Colored Pencils
2. Get out Bohr Model vs. Wave Model &
Lewis Dot
3. Textbook open to Periodic Table (196-
197)
3. Electrons & Chemical Bonding 2
pages-4 sides (Pick-up from bookshelf-
Please Staple to the back of yesterdays
papers)
YOU SHOULD NOW HAVE 4 pages 7 sides
to your packet.
2. Please SCHEDULE:
1. To take Part 2 for the 1st time
OR to
2. Retake Test #3
• Part 2 – 101/145 or lower
3. Parent Signature and
Corrections – due
Tomorrow.
3. 1. What is one similarity between the
Bohr Model and Wave Model?
2. Why do scientists use models to study
the atom?
3. Which scientist believed the atomic
structure to be like Plum Pudding?
4. What is an electron configuration?
5. Where do you find the valence
electrons?
6. What is the valence of Silicon? How do
you know?
7. How many more bonds does Silicon
need to be full?
4. 8. What are the names of the two main
types of bonds?
9. Which type of bond are made when
oppositely charged atoms are
attracted to each other?
10.If I find an element on Row 2, how
many shells will the atomic structure
have?
11.What is the valence of Helium?
12. What does the Lewis Dot Diagram
show??
5. Question Answer
How do you determine the • Rows the element is on = # of shells
electron configuration of the around nucleus
atom? (This works for only the 1st • To load electrons on each shell – count
3 rows) the number of elements in each row….this
is the maximum number of electrons that
can fit on that shell
• YOU MUST load the inner shell FULL
before moving on to the next shell.
If the element is found in:
Row #1 = 1 shell Maximum # of
electrons = 2
Row #2 = 2 shells Maximum # of
electrons = 8
Row #3 = 3 shells Maximum # of
electrons = 8
YOU MUST ALWAYS fill the inner most shell FULL before moving on to
the next shell.
6. Row # = # of shells in diagram
# of elements in each row = Max
electrons on that shell
7. Question Answer
How do you determine the • Rows the element is on = # of shells
electron configuration of the around nucleus
atom? (This works for only the 1st • To load electrons on each shell – count
3 rows) the number of elements in each row….this
is the maximum number of electrons that
can fit on that shell
• YOU MUST load the inner shell FULL
before moving on to the next shell.
If the element is found in:
Row #1 = 1 shell Maximum # of
electrons = 2
Row #2 = 2 shells Maximum # of
electrons = 8
Row #3 = 3 shells Maximum # of
electrons = 8
YOU MUST ALWAYS fill the inner most shell FULL before moving on to
the next shell.
8. Question Answer
What about elements on • These Bohr models include subshells,
rows 4,5,6 and 7? s, p,d & f
(Do not need to know this for 8th
grade)
• http://www.chem4kids.com/files/element
s/006_shells.html
• http://education.jlab.org/qa/electron_con
fig.html
What is the Lewis Dot • Shows how an element will bond
Diagram? • Use the element symbol + the number
http://www.youtube.com/watch?v= of valence electrons
ulyopnxjAZ8&feature=relmfu
Example: Beryllium = Family 2 = Valence of 2
Please correct your
worksheet.
Be
9. Let’s try a couple: Follow these directions to complete the next
page
1. Locate the element on the P.T.
2. Record the information about the element in column 1 of the
chart
3. Draw the nucleus and write the # of each type of subatomic
particle
4. Draw the correct amount of shells outside the nucleus based
on the row the element is found
5. Start loading electrons on the specific shells from the inside out
(closest to the nucleus)
6. Load each level (shell) FULL before going to the next.
(Remember: each shell has a “maximum FULL” amount.)
10. Element Bohr Model Lewis Dot (Symbol +
Valence)
Lithium
Row =
Before moving to the next slide…..try
Electrons=
Atomic #
Protons =
to do this on your own and then check
Atomic Mass
your answer
– Atomic # Neutrons =
11. Element Bohr Model Lewis Dot
(Symbol + Valence)
Lithium
Row = 2
1
Atomic # Electrons= 3-
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
12. Oral Presenters: In charge of today’s
lesson on the computer
Everything on this planet is made of atoms from
elements.
Even though the number of letters on the Periodic Table
is limited, joining the letters in different ways allows
you to make a huge number of combinations.
13. Question Answer
What is chemical bonding? • The joining of two or more atoms
to form a compound
Do the compounds have the same • NO
characteristics as the elements that • Compounds have very different
make them up? characteristics
What happens when elements • They can share valence electrons
bond? (COVALENT)
http://www.mhhe.com/physsci/che • They can transfer valence
mistry/animations/chang_7e_esp/b electrons (donate or accept electrons
om1s2_11.swf (View the animation on becoming ions)
LearningPoint) (IONIC)
Do all the electrons in the atom • NO
make a chemical bond? • Only the valence electrons are
involved in most cases
When will atoms bond? • When their outermost shell is not
complete
14. Element Group Valence Bond or Not Bond
Hydrogen 1 1 Bond
Magnesium
Oxygen
Sulfur
Krypton
Lithium
Carbon
15. Question Answer
What are the characteristics • Usually between Metals and Nonmetals
of Ionic Bonds? • Transfer of electrons – atoms become
IONS
• Form Crystal Lattices
• Brittle
• High melting and boiling points
• Dissolve easigly in water
• Form compounds
• Specific shape
17. Question Answer
What are the characteristics • Usually between Metals and Nonmetals
of 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
Model of an aluminum atom.
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.
18. Question Answer
What are the characteristics • Usually between Metals and Nonmetals
of 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
19. Question Answer
Illustrate a positively charged Bohr Before you move onto the next
Model of an aluminum atom. (3+)
slide….try to draw this on your own.
20. Question Answer
Illustrate a positively charged Bohr
Model of an aluminum atom. (3+)
8
2
P=13
N=14
Why is Al3+ considered an ion? (Look at all the subatomic particles before
you answer this question.)
21. Forming Sodium Chloride
http://www.youtube.com/watch?v=upg-FUHp6ys
http://www.youtube.com/watch?v=7DjsD7Hcd9U
Before (pg. 233) After
Questions: Questions:
1) Why does Sodium become an 1) Why do Sodium and Chlorine
Ion? bond?
2) Is it Positive or Negative? Why? 2) What is the overall charge of
3) Why does Chlorine become an the compound?
Ion? 3) Does NaCl have the same
4) Is it Positive or Negative? Why? characteristics as Na and Cl?
4) What are some unique
characteristics of NaCl?
22. Question Answer
What is a covalent bond? • 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
24. http://www.youtube.com/watch?v=ulyopnxjAZ8&feature=relmfu
Drawing Lewis Dot Diagram Bonds
Molecule Explanation Electron Dot (Color Code
Illustration each element)
1. What kind of bond
does Hydrogen &
Oxygen make? How
P=8 do you know?
2. Why does one
N=8
P=1
Oxygen bond with
two Hydrogen
P=1
N=0 N=0
atoms?
25. 1. Schedule Test #3 retake
2. Signed & Corrected Test #3-
Due Tomorrow
3. Bohr Model vs. Wave Model &
Lewis Dot + Electrons and
Chemical Bonding– Pgs. 1-7 –
due Thursday
