Transcript 11 ATOMIC THEORY REVIEW_adj berg edit

ATOMIC THEORY
REVIEW
Where did the elements come from?
Hydrogen, a little helium and less lithium
were created in the big bang. The universe
is about 95% hydrogen. Clouds of
hydrogen gas and dust are compressed by
gravity into stars. When the star's core runs
out of hydrogen, the nuclear reaction
pauses, and gravity compresses the star,
heating it up enough to fuse helium.
Where did the elements come from?

If the star is big enough, like a supernova,
it can eventually create all the elements in
the periodic table up to iron. If a giant
star explodes as a supernova, it will
releases enough energy to make all the
elements heavier than iron. So stars
created the first elements!
The most common Elements in the
Earth’s CRUST
Element
Amount
Oxygen
46.1 %
Silicon
28.2 %
Aluminum
8.23 %
Iron
5.63 %
Calcium
4.15 %
The most common Elements in the
Earth’s OCEANS
Element
Amount
Oxygen
85.84 %
Hydrogen
10.82 %
Chlorine
1.94 %
Sodium
1.08 %
Magnesium
0.1292 %
The most common Elements in the
Earth’s ATMOSPHERE
Element
Amount
Nitrogen
78.1 %
Oxygen
20.9 %
Argon
0.96 %
What is ALL matter made of?
ATOMS !!!
What are the 3 subatomic particles?
Protons
Neutrons
Electrons
Subatomic Particle Charges
protons (+)
positive
We know that there are the same
number of p+ and e- in atoms on the
Periodic Table… So What is the overall
charge of any atom?
neutrons (0)
neutral
electrons (-)
negative
The overall charge of any atom is
NEUTRAL… the positive charge
cancels out the negative charge
= 0!!!
What are the masses (amu) of the subatomic
particles?
Atomic mass unit (AMU)
p+ = 1amu What is this AMU stuff?????
n = 1amu
2.2 lbs= 1 kg
e- = 0 amu 1.66 x 10-27 kg = 1 amu
What are the two areas of an atom?
Nucleus and electron cloud
e-
P+ & No
Where are the p+, n, and e- located in an
atom?
p+ in the nucleus
no in the nucleus
e- in the electron cloud
Where is most of the volume of an atom
Where is ALL the mass in an atom located?
located?
ElectronNucleus
Cloud
What does a Bohr model of the atom look like?
The nucleus contains the p+ and n… while the electrons
“orbit” the nucleus in the energy rings of the e- cloud.
So what are the charges of the
different areas?
1. So what is the overall charge
of the nucleus?
Positive
2. So what is the overall charge
of the electron cloud?
Negative
(opposite charges attract)
QUICK REVIEW- ATOMS
Sub-atomic particles:. protons, neutrons, and electrons
Parts of the atom: nucleus and electron cloud
particles
Protons
neutrons
Electrons
charge
+
Neutral
(0)
_
amu
location
abbrev.
1
nucleus
p+
1
nucleus
no
0
Electron
cloud
e-
Energy Levels of the Atom
Atoms can have several energy levels. Sometimes they are also
called energy rings, shells or orbits.
The
Nucleus
P+ N0
2e-
8 e- 8 e-
18 e- 18 e- 32e-
1st
2nd
3rd
4th
5th
6th
7th
shell
shell
shell
shell
shell
shell
shell
32e-
Lets take a look at the Periodic Table!
The periods equal the number of energy shells or rings in an atom.
Beginning with Bohr Models

Let’s try a few easy bohr models:
Li
Be
Bohr Model Practice
1. Ca
2. O
3. Ne
4. K
5. Rb
6. P
7. F
8. Cl
9. Br
10. I
More Bohr Model Practice
11. Fr
12. Te
13. Sn
14. Cs
15. Kr
16. At
17. Ga
18. Rn
19. Ag
20. W
Cs Fr
Sn Te
Kr At
Ga Rn W Ag
Bohr Model
Draw the bohr models
for the following atoms.
Explain why we use helium filled balloons
instead hydrogen filled balloons at Parties.
H
vs.
Energy
rings are
not filled
He
Energy
rings are
filled
Hydrogen is unstable and
flammable and helium is stable!
Burning Hindenburg
Complete the Bohr Models for the
following elements. Ne, Ar, Kr and Xe
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
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
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What 4 patterns or
trends did you notice
they have in common?
“Predict” what you
think Radon’s (Rn)
bohr model would look
like.
Six rings
Full shell
More massive




All of the rings or
shell are full.
They are all in the
same group (18)
They gain an energy
ring as you go down
a period.
They gain more
subatomic particles
as you go down.
Patterns from the Bohr Models.
Ne
Ar
Kr
Radon Bohr Model
Xe
Even More Bohr Model Practice!
21. Os
22. Hf
23. Cm
24. Sr
25. Ho
26. Tc
27. Ac
28. Zr
29. Po
30. Np
“Life on the Edge”
with Valence Electrons
Valence electrons are electrons in the outermost
shell of an atom.
They determine whether the atom will bond with
another atom.
How many valence
electrons does
lithium have here?
1 valence electron
Circle the valence electrons
From your warm up.
Arrangement of the Periodic Table
1. What atom is this?
Oxygen
2. Which subatomic “particle” helped you to
determine that this Bohr model was of oxygen?
Protons
Arrangement of the Periodic Table
1. The periodic table is arranged according to what?
A. Atomic Symbol
B. Atomic mass
C. Atomic number
D. Number of Energy Shells
 Do the elements on the periodic table all increase
according to their masses?

No!! Can you find where they are not? There are a
few of them. Look carefully!
Periodic Table Card Sort Poster
Breaking the Code
Purpose: This lesson will help you identify many
of the patterns that are contained in the
periodic table of elements.
Use the card sort poster to answer the
following questions on your paper.
Do you notice any patterns here
as the elements move to the right?
Li
Na
Gaining more
p+, no, and e-.
K
Gaining
more mass
Rb
Gaining more
energy rings
Can you “predict” how many energy rings a bohr model of
Francium (Fr) would have?
Francium (Fr) Bohr Model
Seven
energy
rings
1
valence
electron
What Bohr model patterns are
you starting to see develop?





Periodic Table Patterns
The atomic number is the same number as the
number of protons and electrons.
Atoms get larger as you move down and two the
right on the periodic table.
As you move from left to right on the periodic table,
you gain protons and electrons and neutrons.
As you go down from the periodic table, the atom
gains another energy shell or orbit.
Element
Atomic
Number
Atomic
Mass
Zn
30
65
Xe
54
131
54
197
79
Au
79
Hg
80
I
53
201
127
# of
Protons
30
80
53
# of
Electrons
30
54
# of
Neutrons
35
77
79
118
80
121
53
30
Yttrium
2e
8e 8e
Manganese
18e 3e
2e
8e 8e
7e
P39
N50
P25
N30
Yttrium
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 18
Fifth Energy Level: 3
Manganese
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 7
Germanium
Krypton
2e
8e 8e
18e
2e
8e 8e
14e
P39
N50
P36
N48
Krypton
Germanium
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 18
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 14
Metals vs. Non-Metals
Stair steps
Non-metals
Metals
Man made elements and Rare Earth metals
Metalloids on the Periodic Table
FAMILIES/ GROUPS
Periods/ Rows
Metalloids
Properties of Metals
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
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
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Most elements are metals. 88 elements to the left of the
stairstep line are metals or metal-like elements.
Tend to have Luster (shininess)
High density (heavy for their size)
Ductile (most metals can be made into thin wires)
Malleable (most metals can be hammered into thin sheets)
Properties of Non-metals
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

Nonmetals are found to the right of the stairstep
line.
No luster (dull)
Brittle (breaks easily)
Not ductile
Not malleable
Properties of Metalloids





Metalloids are elements on both sides of the stair
step line. They have properties of both metals and
nonmetals.
Solids
Can be shiny or dull
Ductile
Malleable
Families on the Periodic Table
So where do the names come
from?
These abbreviations are for there LATIN names of the elements.
Iron (Fe)………….……Ferrum
Mercury (Hg) ……Hydragyrum
Sodium (Na)….. …….Natrium
Antimony (Sb)………… Stibium
Gold (Au)……………Aurum
Tin(Sn)….………… Stannum
Silver (Ag)………….Argentum
Potassium (K)………… Kalium
Copper (Cu) ………….Cuprum
Lead(Pb) ……………..Plumbum
Tungsten(W)………….Wolfran
Steps for creating a bohr model
1. Complete the particle
inventory for the atom
6. Put 2 electrons in the first
shell. If there are more
(protons, electrons and neutrons).
than 2, begin to fill the
2. Draw your nucleus.
next shell (maximum of 8).
3. Put the number of protons 7. You cannot begin to fill the
and neutrons in the
next shell until the previous
nucleus.
shell is filled.
4. Circle how many
8. Remember` how many
electrons you need to use
electrons each shell can
in the shells.
hold a maximum of.
5. Know how many electrons
(2, 8, 8, 18, 18, 32, 32,)
and shells you will need.