Download Unit 3 The History of the ATOM

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BUFF Time CHAMPS
1.
No talking during announcements/silent reading
2.
Raise hand if you need help/question
3.
Follow directives and participate
4.
Stay in your assigned seats
5.
Actively engage
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
Haltom Fight Song
Haltom fight, Haltom fight
And it's goodbye to...
Haltom fight, Haltom fight
Let's put over one more win!
Haltom fight, Haltom fight!
For it's Haltom that we love best.
Hail, Hail, the gangs all here
And it's goodbye to all the rest!
Yea Orange! Yea Black! Yea Buffs!
Fight! Fight! Fight!
Go Orange! Go Black! Go Buffs!
Fight! Fight! Fight!
H-A-L-T-O-M, Haltom High Buffalos!
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Get PREPed!!
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DO RIGHT NOW:
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Materials:

Find your group’s poster and
get ready to present.

Interactive Notebook

Pen

Ruler

Scissors
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I will start as soon as the bell
rings!!!
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Democritus 460-370 B.C.

Greek Philosopher

He called nature’s basic particle an
atomos, based on the Greek word
“indivisible.”
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Had no evidence so people didn’t
take him seriously.

He considers education to be the
noblest of pursuits, but cautioned that
learning without sense leads to error.
(THERE MUST BE A POINT!!!)
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Aristotle said empty space did not
exist & rejected Democritus; said
matter was EARTH, WATER, AIR &
FIRE
+ John Dalton 1803
Dalton’s Atomic Theory
1.
All elements are composed
of tiny indivisible particles
called atoms.
Element
A
2. Atoms of the same element
are identical. The atoms of
any one element are different
from those of any other
elements.
+ Dalton’s Atomic Theory
3. Atoms of different elements can
physically mix together or can chemically
combine with one another in simple wholenumber ratios to form compounds.
+ Dalton’s Atomic Theory
4. Chemical reactions occur when atoms
are separated, joined, or rearranged.
Atoms of one element, however, are
never changed into atoms of another
element as a result of a chemical
reaction.
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Stop and think:

What was the key difference between what Democritus said
and Dalton’s Atomic Theory?

Record this discussion on your time line.
+ J.J. Thomson 1897 (with
Crookes & Millikan)
 discovery of the electron (e-)
disproved
Dalton’s theory; atoms DID have
smaller parts after all
Used
a cathode ray tube to prove that
there were charged particles (stream of (-)
particles) within the atom
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Thomson Model
Plum pudding model
aka chocolate chip
cookie model
Millikan found out
that electrons
were negatively
charged and had a
mass of 1/1840 of
a hydrogen atom
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Stop and think:

Let’s watch this video on the cathode ray tube experimenttake notes!! You need to understand how this experiment
worked!
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How does it work?
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What part of Dalton’s atomic theory was disproved by JJ
Thomson? How do you know it was disproved?
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Do right now:

Get your materials ready for class.
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Materials:

Write down the HW in your planner.
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Interactive Notebook

On your index card, describe the
difference between Dalton’s model of
the atom and Thomson’s model of the
atom. You may use your notes
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Planner
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Pen
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Glue Stick
HW: Complete the Scientist magic square.
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Ernest Rutherford 1911
 Used
alpha particles to shoot
at gold foil. Got unexpected
results. Something was
deflecting particles back to
the source. Hmmm….
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Buried next to Sir Issac
Newton and Lord Kelvin in
Westminster Abbey. (way
cool!)
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Empty Space
Nucleus
Electrons
Rutherford
said,
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“Atoms have a nucleus!”
Dense
& positively charged
Contains
most of the mass of the atom
Contains
the protons (positive charge; heavy
Electrons
are around the outside of the
nucleus flying around the empty space
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Stop and think:
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Let’s look at his experiment:
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What did he do?
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Let’s model his experiment.
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What was the key difference between Rutherford’s model
and Thomson’s? How did this change the perception of the
atom?
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James Chadwick
 Discovered
 Has
the neutron in 1932
a neutral charge
 Found
in the nucleus
 About
½ of the mass of the nucleus
 Wanted
to know where the extra mass was
coming from in an atom; shot particles @
beryllium
 Eventually
led to experiments to bombard
atoms with neutrons –> uranium  bombs!
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Niels Bohr - 1913
Created
the Bohr model
Electrons
travel in definite orbits/
energy levels around the nucleus
aka “Planetary
Model” – orbit the nucleus
like planets around the sun
Electrons
have fixed amounts of energy
“quanta”
 Low
energy  closer to nucleus
 High energy  further from nucleus
+ Bohr Model
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Werner Heisenberg, 1927
It’s
impossible to know
both the location and the motion
of an electron at the same time
Heisenberg
Uncertainty Principle
+ Quantum Mechanical Model
(aka wave mechanical model)
Erwin
Schrodinger – 1926
Electrons
Electrons
DO NOT orbit the nucleus
DO have quanta of energy that
determine placement in an atom
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Electron Cloud
Area
where there is a high probability
that the electron will reside there 90%
of the time
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Schrodinger’s Cat
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Do right now:
Mark on your
scantron the
questions you
got wrong:
1)
2)
3)
4)
5)
6)
7)
8)
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Materials:
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Your test
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Homework
(magic
square)
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Your scantron
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2 pieces of
notebook
paper
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Planner
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Calculator
9)
A
20)
D
10)
A
21)
B
11)
C
12)
B
13)
A
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Pen
14)
D
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Marker
15)
B
16)
56.7
17)
8.31
18)
B
19)
A
D
A
C
D
C
B
B
B
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Homework
tracker
Interactive
Notebook
For each question you missed:
1. Write the original answer and explain why this is
wrong.
2. Write the correct answer and explain why this is
correct (for math problems this means SHOW
YOUR WORK)
3. You may use a book, your notes, you may ask me
for help, but you may not discuss with one another
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HW: Watch the video: Atomic
Structure and take Cornell notes
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1.
2.
Materials:
DO RIGHT NOW:
1.
Interactive Notebook
Put everything at back of room if it
is not on the materials list.
2.
Homework Tracker
3.
Planner
4.
Colored pencils: red, blue,
green
Write your homework in your
planner.
3.
Glue:
A. Atomic Structure worksheet
(back of magic square)- pg 46
4.
Set up pg 42 with the title: Atom
Basics
HW: Complete the bottom of pg
46: Atomic Structure Worksheet
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Atom Boards
EQ: Can I build a model to
accurately represent various
atoms?
Protons
Electrons
Neutrons
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DO
RIGHT
NOW:
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Write down the HW in your planner
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Make pg 49 look like this:
Protons
Neutrons
Electrons
A
17
18
17
B
17
20
17
C
3
3
3
D
3
4
3
E
15
15
15
F
15
16
15
G
1
0
1
H
1
2
1
I
8
7
8
J
8
9
8
K
12
12
12
L
12
14
12
Materials:
1.
Interactive
Notebook
2.
Pen
Atomic
Numbers
3.
Planner
4.
Homework
Tracker
Mass
Nuclear
Number Notation
Hyphen
Notation
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Isotope Notes: pg 53
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Isotope Notes
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Gallery Walk Questions pg 48:
1.
What is an isotope?
2.
What is the same in an isotope?
3.
What is different in an isotope?
4.
How do you determine the mass number?
5.
What are the two ways we designate isotopes?
6.
According to Dalton’s theory, atoms of the same element are identical.
Explain how your work today disproves this idea. Your explanation must
include the following words (protons, neutrons, atom, atomic mass,
element, atomic number)
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Materials:
DO RIGHT NOW:
1. Glue
in:
1. Isotopes Worksheet-51
2. Isotopes(bonus)-pg 50
2. You
have a HW quiz
today! It is over
scientists, atomic
structure, and isotopes.
Please take an extra 3
minutes to study!!
1.
Interactive Notebook
2.
Pen
3.
Calculator
4.
Homework tracker
5.
Homework (and bonus)
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What element do you have?
How many total cards do you have?
How many cards are in this group?
How many cards are in this group?
How many protons does this atom have?
How many protons does this atom have?
How many electrons does this atom have?
How many electrons does this atom have?
How many neutrons does this atom have?
How many neutrons does this atom have?
What is the atomic mass of this atom?
What is the atomic mass of this atom?
Calculations:
1. # of cards in group/total # of cards
2. Multiply this by the atomic mass
Calculations:
1. # of cards in group/total # of cards
2. Multiply this by the atomic mass
Which of the two isotopes is more abundant? How do you know?
Add the values from both sets together and calculate the average atomic mass:
_______________________
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For each baggie:

Protons-black dots

Neutrons-white dots
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Electrons-grey dots
1.
Count and record the total number of cards from the baggie.
2.
Count the protons on one card to determine the element.
3.
Count the neutrons on each card and sort into 2 piles based on
the number of neutrons.
4.
Fill in the chart for each isotope
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Materials:
DO RIGHT NOW:
Write your homework in your planner: Finish
average atomic mass worksheet.
Get out your average atomic mass worksheet
from Friday.
Get out the cards and re-separate them into the
two piles of isotopes.
Today I will be stamping your prep-make sure
you have ALL your materials and everything else
is put away at the back of the room by the time
the tardy bell rings!
1.
Worksheet from Friday
2.
Interactive Notebook
3.
Planner
4.
Pen
5.
Calculator
6.
Homework Tracker
+ Example: Calculate the average atomic
mass for Lithium if 7.5% of Li atoms have
a mass of 6.0151 amu and 92.5% of Li
atoms have a mass of 7.0160 amu.
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Example:
Calculate the average atomic
mass for Gallium if Ga-69 is 60.11 %
abundant and Ga-71 is 39.89 %
abundant.
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Materials:
DO RIGHT NOW:
Write down HW in Planner: finish mole
calculations worksheet.
Cut out a pink periodic table, put your
name on it with sharpie, and hole punch it.
THIS IS TO BE KEPT IN YOUR BUFF BINDER
FOREVER!
Glue:
-Average Atomic Mass (the activity)-pg 55
-Average Atomic Mass Worksheet (HW)-pg
54
1.
Interactive Notebook
2.
Pen
3.
Calculator
4.
Planner
5.
Pink Periodic Table
6.
Homework
7.
Homework Tracker
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On pg 57: Calculations with the Mole
 Helpful
equalities with the mole:
 1 mole = 6.022 x 1023 atoms/molecules/formula
units
1
mole = average atomic mass (g) for an element
 Except
the HOFBrINCls-these form diatomic
molecules (H2, O2, N2, Cl2 etc) so you multiply the
average atomic mass by two.
1
mole = 22.4 liters of gas.
https://www.youtube.com/watch?v=TEl4jeETVmg
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How many atoms of carbon in 2.6
grams of carbon?
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How many moles on 36.2 g of
chlorine (Cl2)?
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How many liters of gas are
produced from 5.0 moles of
helium?
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How many grams in 4.3 x 1023
atoms of boron?
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DO RIGHT NOW:
Glue:
Mole Calculations
Worksheet-page 56
Review Worksheet-pg
59
I’m
coming around to
stamp homework and
gluing!
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Materials:
1.
Interactive notebook
2.
Calculator
3.
Pen
4.
Planner
5.
Pink periodic table
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Unit 3 test and notebook check
tomorrow!
Notebook
reminders:
Word wall-pick any 6 vocabulary
word-word, definition, picture
Cornell notes-3 questions and a
summary that answers the essential
question
Pages complete and glued in (do
not fold)
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