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Published by mroberg, 2019-06-04 14:32:26

Final Product: Portfolio Martin Roberg

Final Product_ Portfolio - Google Docs

6/4/2019 Final Product: Portfolio - Google Docs

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Quarter 3

Blue Science Portfolio Part 3
Due: March 28, 2019

1. Atomic Structure Project 1/14
2. pHet Atomic Structure Simulation 1/16
3. Experiment: Families of Elements 1/18

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Atomic Structure Project
Portfolio

Due: Friday 1/25/19

Directions: Complete the requirements below that relate to atomic structure and the periodic
table.
Vocabulary - Define and make a Quizlet
https://quizlet.com/358811901/atomic-structure-flash-cards/

Atom: The smallest Neutron: Neutral Atomic Mass: Atomic Radius:
particle of an Particle, composed
element that still of quarks, inside Number of protons one-half the
retains the the nucleus of an and neutrons distance between
properties of the atom the nuclei of
element identical atoms that
are bonded
together

Nucleus: Electron: Isotope: Family (Group):

Positively charged particles Atoms of the same A vertical column in
center of an atom surrounding the element that have the periodic table
that contains center of an atom different numbers
protons and that has a charge of neutrons
neutrons and is of 1-
surrounded by a
cloud of electrons

Proton: Atomic number: Periodic Table: Period:

Particle, composed Number of protons Organized list of all The horizontal row
of quarks, inside in an atom's known elements in the periodic table
the nucleus of an nucleus that are arranged

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atom that has a by increasing
charge of 1+ atomic number and
by changes in
chemical and
physical properties

Alkali Metals: Alkaline Earth: Halogens: Noble Gases:

Group 1A, Any of the Contains the elements in
excluding elements Beryllium, nonmetals, 7 Group 8A of the
Hydrogen. Highly Magnesium, valence electrons in periodic table
reactive. Calcium, Strontium, its outermost
Barium, and energy level. Very
Radium, occupying reactive
Group IIA (2) of the
periodic table. They
are reactive,
electropositive,
divalent metals,
and form basic
oxides which react
with water to form
comparatively
insoluble
hydroxides.

Oxidation numbers Ionization Energy

Shows how many The amount of
electrons can be energy required to
shared, lost or remove an electron
gained to become from an atom
stable; you cancel
out the valence
numbers to make

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the compound

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Reading: https://www.livescience.com/37206-atom-definition.html 119/310
*Use this site for notes

1. Cover Page: Atomic Structure and Periodic Table

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● Comes from the Greek term for indivisible
○ Once thought to be the smallest things in the universe, couldn’t be divided

● Made of
○ Protons
○ Neutrons
○ Electrons
■ Quarks

● Took 380,000 years for the universe to cool down enough to slow down the electrons, for
nuclei could form atoms (CERN)

● Protons and Neutrons are heavier than electrons
● The electron cloud has a radius of 10,000 times the nucleus
● Protons and Neutrons have prominently the same mass
● One proton weighs more than 1,800 electrons
● Atoms normally have the same number of protons and neutrons
● Adding a proton makes a new element
● Adding a neutron makes an isotope, a heavier version of the atom
● The nucleus was discovered in 1911 by Ernest Rutherford
● Rutherford proposed the name of protons in 1920
● Virtually all the mass of the atom is in the nucleus

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● Held together by strong force, one of four basic forces in nature
● Overcomes rules of electricity that would normally push protons apart
● Some atomic nuclei are unstable because the binding force is different for each atom
● Can decay into other elements, e.x. Carbon-14 decaying into Nitrogen-14
● Protons have a relative mass of 0.9986
● The number of protons is the atomic number of the element
● The periodic table is arranged by atomic number
● Electrons have a relative mass of 0.0005439
● J.J. Thompson discovered the electron in 1897
● Electrons surround the nucleus in pathways called orbitals

○ Discovered by Erwin Schrödinger in the 1920s
● Only the outermost shell matters in chemistry
● By using the electrons configuration and principles of physics, chemists can predict

○ Stability
○ Boiling point
○ Conductivity
● Neutrons have a relative mass of 1
● Discovered by James Chadwick in 1932
○ Discovered when atoms were shot at a thin sheet of beryllium
● Found within all atomic nuclei besides Hydrogen-1
● The isotope is determined by the number of neutrons in an element
● The theory of the atom dates back to 440 BCE
● The theory was built by Democritus, a Greek scientist, and philosopher
● Believed the theory was contributed by his teacher Parmenides, who is known for
proposing the principle of identity
● The word atom comes from the Greek word for indivisible

2. History of the Atom
Link: https://www.youtube.com/watch?v=NSAgLvKOPLQ&t=490s
Link2:
What were the contributions of each of these scientists to the discovery of the atom?

a. Dalton

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● Came up with the first scientific experiment that showed that matter was made with
tiny particles

● Pictured atoms as tiny little balls that arranged in different variations to make
different things

● Imagined that the atoms were indivisible
b. Thomson - Video

● Discovered that electrons were much smaller than atoms
● Believed that they were divisible because they were made up of electrons, that

were much smaller than atoms
● Imagined that if you split an atom open, you would see tiny electrons stuck inside

(Plum pudding)
● Believed that the atom was positively charged, combined with electrons which

balanced each other out
c. Rutherford

● Discovered that atoms had a nucleus
● Believed that all of the positive charges in the atom was found in the nucleus

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D. Bohr

● Discovered that atoms had outer shells, like planets orbiting around the
sun

● Believed that they spun around in circular orbits around the nucleus
3. Structure of the Atom

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Video
Video2

a. Nucleus, protons, neutrons, electrons
● Electrons follow the octet rule, the rule of 8
○ Determines the layout of shells
○ Only applies to the first few rows of the periodic table
○ Applies to most of the important elements in biology

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b. Atomic Mass
● The combined number of protons and neutrons in the atom’s nucleus
● Neutrons weigh more than Protons
● Electrons have a very minor effect on weight (0.0005439)
○ Total of around 2000 electrons= 1 gram

c. Charge
● Determined by the number of electrons in the outermost shell
○ 1 Electron= +1
○ 2 Electrons= +2
○ 3 Electrons= +3
○ 4 Electrons= Can create unique compounds with itself
○ 5 Electrons= -3
○ 6 Electrons= -2
○ 7 Electrons= -1
○ 8 Electrons= 0

d. Valence Electrons
● How many shells the element has
○ Row one has 1 valence electron
○ Row two has 2 valence electrons etc.

***Use models to explain the difference between:
Sodium Chloride and Magnesium Chloride or Sodium sulfide and Calcium Sulfide or
Calcium phosphide and lithium phosphide

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4. Isotopes
Link: https://phet.colorado.edu/en/simulation/isotopes-and-atomic-mass

a. Provide Examples (screenshots from simulation)

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b. How are isotopes used to find the age of fossils? (Provide Research)
https://sciencing.com/radioactive-dating-used-date-fossils-5184705.html
● Many organisms contain radioactive isotopes, that decay at a predictable
time
● Most common isotope is U-235 (Uranium)
● C-14 (Carbon) is found in all living organisms
○ Often used in dating artifacts from humans

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5. Families of the Periodic Table
*Describe the life of Mendeleev and how he created the Periodic Table.
https://corrosion-doctors.org/Periodic/Periodic-Mendeleev.htm
● Arranged in order by the atomic mass
● Believed that gaps in the periodic table were undiscovered elements (turned out to
be right)
*What makes the elements similar in each family?
a. Alkali Metals

http://www.chem4kids.com/files/elem_alkalimetal.html
● All of the elements have one electron in its outermost shell besides
Hydrogen
○ Hydrogen is a unique element that doesn’t belong to any family
● They are all very reactive
● Are all metals
● Shiny and lightweight
● Bendable, sometimes soft enough to cut with a dull knife
● Elements
○ Hydrogen
○ Lithium
○ Sodium
○ Potassium
○ Rubidium
○ Cesium

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○ Francium
b. Alkaline Earth Metals
http://www.chem4kids.com/files/elem_alkalineearth.html

● Not very reactive, bond with other elements very easily
● Elements

○ Beryllium
○ Magnesium
○ Calcium
○ Strontium
○ Barium
○ Radium
c. Halogens
http://www.chemistryexplained.com/Ge-Hy/Halogens.html
● Relatively low melting and boiling points
● Span from all physical states
● Solid
○ Iodine
● Liquid
○ Bromine
● Gas
○ Fluorine
○ Chlorine
● Colorful, colors get more intense moving down
● As solid are brittle and crumbly
● Burn exposed flesh
● Are Toxic
● Have a variety of different oxidation numbers
● Variety of uses for the elements
● Elements
○ Floruine
○ Chlorine
○ Bromine
○ Iodine
○ Astatine
d. Noble Gases
http://www.chem4kids.com/files/elem_noblegas.html
● All of the elements have 8 electrons in the outermost shell
● Rarely combine with other elements
● Used to stabilize reactions
● As the atomic number increases the element becomes rarer
● Some have been used as compounds in explosives
● Elements
○ Helium

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○ Neon
○ Argon
○ Krypton
○ Xenon
○ Radon

6. Choose an article to read from site and summarize:
https://www.livescience.com/37206-atom-definition.html
Atoms have been around since the beginning of time 13.7 billion years ago. These atoms contain
three things that are all very different, protons, neutrons, and electrons. Protons and Neutrons are
in the nucleus, while electrons are attracted on the outside. The nucleus was discovered in 1911
by Ernest Rutherford, who also discovered protons in experiments conducted between 1911 and
1919. The number of protons defines what the element is. Electrons were first discovered in 1897
by J.J. Thompson and the idea of the outer shells was first put forth by Erwin Schrödinger in the
1920s. The idea of the atom dates back to 440 BCE, from the Greek philosopher Democritus.
Throughout the last few thousand years, the idea has been expanded and modified to what
scientists know today as the formation of the element.

7. What are some trends in the periodic table as you move from left to right and top to bottom?
Use evidence (graphs) from the graphing activity.

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Periodic Table Trends

Skill: Analyzing data
Due: Wednesday Part 7 on Atom Project

Directions: Construct 2 graphs related to trends found on the Periodic Table. Use the data from
the graph and the vocabulary below to explain a relationship between Atomic Structure and the
Periodic Table.

*Use at least 3 transition words (However, Therefore, …)Highlight the words
*Use Diagrams of the elements and their atomic structure
*Use the following vocabulary: (highlight some of the vocabulary words)

● Atomic Radius
● Ionization Energy
● Opposite charges attract
● Valence Electrons (1-8) Na has 1 valence electron
● Nucleus
● Charge (+1, +2, +3, -3, -2, -1)
● Proton, Neutron, Electron
● Alkali, Alkaline Earth, Halogens, Noble Gases
● Energy levels (1 ring, 2 rings, 3 rings)

USE the Following Outline

Conclusion: (You should have 8-10 sentences in each body paragraph)

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I. Topic Sentence (Atomic Radius and Ionization Energy)
A. Topic Sentence for Body Paragraph - Left to Right on Periodic Table
B. Topic Sentence for Body paragraph - Top to Bottom on Periodic Table
C. Transition sentence

II. Topic Sentence - Left to right on Periodic Table
A. Explain Atomic Radius and Ionization Energy
B. Trend for Atomic Radius (Lithium and Fluorine) Left to Right
● The radius decreases because it adds protons and electrons as spots on the rings are
being taken up by more electrons
● Fluorine gains 6 electrons, lowering its radius
● Protons and electrons make atom smaller
● Atoms gain a new ring in each period
● Atoms get bigger due to having more rings
C. Trend for Atomic Radius (Sodium and Argon) Left to Right
D. Use data from the table
E. How does the radius relate to the Ionization Energy?

III. Topic Sentence - Top to Bottom on Periodic Table
A. Trend for Atomic Radius (Lithium and Sodium) Top to Bottom
B. Trend for Atomic Radius (Magnesium and Calcium) Top to Bottom
C. How does the radius relate to the Ionization Energy as you move down the Periodic
Table?
D. Use data from Table
E. Conclusion Sentence

Atoms are molecules that are made up of the nucleus, of which is filled with protons and neutrons,
and the surrounding electrons. On the periodic table, there is a clear correlation between the
atomic radius and the periodic table. This correlation can be found within the periods and the
families on the periodic table. Both left to right and top to bottom show clear correlations,
correlations that are very different from each other.

By increasing its number of electrons, the size of the atom going left to right shrinks,
lowering the atomic radius of the atom as well. The two main contributing factors to the atomic
radius are the total amount of rings that the atom has, and the number of electrons that occupy
them. Both of these numbers can be found directly within the periodic table quickly and easily. For
example, Lithium is in the first element in the Alkali Family, which gives it an atomic number of
three on the periodic table. Because it’s the first in its family, it also lies in the first period which all
only have a total of two rings. Like every element besides Hydrogen, it’s the first ring is completely
filled with electrons. With the number of electrons that can go into the first ring being two, this
leaves one electron to go into the second ring. The second ring can hold 8 electrons, but with
Lithium is only holding 1. This leaves it with a high atomic radius because, with just a single

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electron, the proton isn’t pulling it too close. As you go down the column, the number of electrons
increases and at the same time the atomic radius decreases. At the end of the first period, is the
element Fluorine, which has an atomic number of ten. With one ring that holds two electrons and
a second ring that holds 8 electrons, this takes up all 10 of the available electrons for fluorines two
rings. Because of this, the atom is far smaller than lithium, as the protons are trying to keep the
electrons, which shrinks the atom in on itself. This is the case in all periods. In the second period,
Sodium is the first element. To compensate with the number of electrons in the atom being
greater than ten, the limit for a two ring atom, every element in this period has three rings. Like
Lithium, the charge of Sodium only takes up one of the spots for the electrons, meaning that it has
the highest atomic radius of the entire second period. In addition, despite also being in the Alkali
family, Sodium has a greater atomic radius than Lithium, with Sodium having an atomic radius of
186 and Lithium having an atomic radius of 152. This is due to Sodium having one more ring than
Lithium, meaning that it can attract more electrons without shrinking as much as the first period.
However, even with fewer rings than the second period, only Sodium and Beryllium have larger
atomic radius than Lithium. Just like flouride, due to it having all of the possible slots for electrons,
18, it is the smallest element in its period, but still bigger than a few elements in the first column
such as flourine. These elements get bigger due to the ionization energy, the amount of energy
required to remove an electron. The electrons are kept in place because of the nucleus of the
atom. With the protons being positive and the electrons being negative, they attract to each other.
As you go further and further to the right, the amount of energy needed to remove an electron
from the atom increases. An example of this is with Lithium and Neon. Lithium has 3 electrons, 2
in its innermost shell and one in its outer. Due to their only being one electron in the outer shell,
it's pull to the nucleus is weak, therefore causing the large atomic radius. With the weak pull, it is
easier to take away the electron. In the graph, you can see how the ionization energy gained
actually lowers as you go to the right on the periodic table. Lithium’s ionization energy is 520, with
the next element in its family, Beryllium having ionization energy of 899. The difference between
the two is +379. The gain from the first two elements in the next group, however, is only 242, with
Sodium having an ionization energy of 496, and Magnesium having an ionization energy of 738.
As you continue going further and further down the periodic table, the gain between the two
elements will continue to drop. This is because as the amount of electrons increases and the
atomic radius decreases, the nucleus becomes more effective at holding the electrons in place.
Unlike going left to right, as you go up to down the atom’s get bigger and bigger, with its ionization
energy getting smaller and smaller.

When you go down the column’s, the atoms gain more and more rings, and by increasing
the total amount of rings, the size of the atoms increases. When going down the columns, the
charge is constant which means that the total amount of electrons occupying the final ring is the
same, no matter how many rings it has. With more rings, the atomic radius logically increases.
With the protons and electrons shrinking down the atom with a greater total of atoms in the final
ring making it smaller, but when more rings are added the size increases. With the Alkali family,
every element in the column from Lithium, to Sodium, have a charge of +1. Lithium has a total of
two rings, which makes it the smallest of its family despite being the largest of its period. This isn’t
a constant trend due to Lithium being the only element that follows this rule. With the most rings

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and the least electrons occupying its outer ring, Sodium ends up having the largest atom size, as
well as the largest atomic radius out of all of the atoms. Similarly, Magnesium is the second
largest atom in its period but is the smallest in its family while the element below it, calcium, ends
up being larger. Another difference from left to right, to up and down is the ionization energy. As
you go down the family, the amount of ionization energy decreases. This is due to the number of
shells increasing. With the number of shells increasing, the nucleus becomes less and less
effective at keeping electrons, due to them being farther and farther away. This trend shows the
correlation that the larger the atom is, the lower the ionization energy is. For example, the Alkali
family all have one valence electron. As the number of rings increases the nucleus is less
effective at keeping the electron. Overall, going left to right versus up and down shows different
trends from each other.

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1.
a. Identify The Element: Chlorine
b. Number of Neutrons: 18
c. Charge: -1

d. Draw Element

2. 136/310
a. Identify the Two Elements: Nitrogen (A) Phosphorous (B)
b. Identify the Family: Halogen
c. Charge: -3
d. Write a compound with sodium and one of these elements
Na+1P-3

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3.
a. Identify the Element: Sodium
b. Charge: +1
c. Family: Alkali
d. 2 other Elements in Family: Hydrogen, Lithium

4.
a. Identify the Element: Boron
b. Neutrons: 6
c. Charge: +3
d. Atomic Number: 5

5.
a. Identify the Elements: Neon (A) Argon (Ar)
b. Family: Noble Gases
c. Why it doesn’t make compounds: Due to both of the elements having a charge of
zero, this being due to their outer shell being filled with all 8 electrons, they cannot
become a compound

6. 137/310
a. Identify the Element: Oxygen
b. Protons: 8
c. Neutrons: 8

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d. Draw atom

7.
a. Identify the Element: Phosphorous
b. Atomic Number: 15
c. Family Name: Halogens
d. Draw atom

8. 138/310
a. Identify Element: Neon
b. Number of Neutrons: 10
c. Draw Atom

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9.
a. Identify the Element: Boron
b. Charge: +3
c. Make a compound with Sulfur: B+3S-2 B2S3

10.
a. Identify the Element: Magnesium
b. Neutrons: 12
c. Draw the Atom

11. 139/310

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a. Identify the Elements: Sodium (A) Nitrogen (B)
b. Charge For Both Atoms Sodium +1 Nitrogen -3
c. Write a Compound for these two elements

Na+1 N-3
Na3N

12.
a. Identify the Elements: Chlorine (A) Fluorine (B)
b. Family: Halogens
c. Why are they similar: Due to both being in the same family, they have the same
amount of electrons occupying the outer shell. Due to being in different periods,
however, they have a different amount of shells.
d. Which one has the larger atomic radius: Due to having more shells, Chlorine has a
larger atomic radius than Fluorine

13.
a. Identify the Element: Sulfur
b. Neutrons: 16
c. Charge: -2
d. Draw the Atom

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14.
a. Hydrogen (A) Lithium (B)
b. Family: Alakai
c. Why are they Similar: They are both in the same family, which means that they
have the same amount of electrons in their outer shell
d. Make a compound with one of these two elements
Li+1 O-2
Li2O

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Age of Fossil % of Isotope

0 100
50
413 25
12.5
826 6.25
3.125
1239 1.06
0.5
1652 0.25
0.125
2065 0

2478

2891

3304

3717

4130

Fossil #1: Age
Description
13% Remaining
Fossil #2: 87% Decayed

Description Trilobites (One of the Earliest Known groups of arthropods)

Fossil #3: 8% Remaining
Description 92% Decayed

Fossil #4: Dinosaur: Archaeopteryx (Transitional bird between dinosaurs and
Description birds)

Fossil #5: 18% Remaining
82% Decayed

Snail

90% Remaining
10% Decayed

Green River Diplomystus Fish (Fish From The Green River Formation)

27% Remaining
73% Decayed

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Description Triceratops
Fossil #6: 17% Remaining
Description 83% Decayed
Fossil #7: Starfish
Description 21% Remaining
Fossil #8: 79% Decayed
Description Spine
Fossil #9: 83% Remaining
Description 17% Decayed
Fossil #10 Dragonfly
Description 32% Decayed
68% Remaining
Leaf
65% Remaining
35% Decayed
Fly

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Chemistry II Test Review 2019

Balance and draw the Electron Dot Structure for the following Chemical
Reaction: Use your notebook

*Include: Ions, Products, Compound names, Balanced equation, Correct valence electrons,

charges

Example #1

→Sodium chloride+
Lithium phosphide Sodium Phosphide

+ Lithium Chloride

Na+1 Cl-2 Li+1 P-3 Na+1 P-3
Li+1 Cl-2 Li3P Na3P

Na2Cl
Li2Cl

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Determine the Number of Neutrons for the following Elements:

Element Neutrons

1. Lead 207-82
125

2. Uranium 238-92
146

3.Phosphorus 31-15
16

4. Copper 64-29
35

5. Plutonium 244-94
150

Determine the Valence Electrons and Charge for the Following Elements:

Element Valence Electrons Charge (+1, -1, +2…)

6. Sodium 1/8 +1

7. Iodine 7/8 -1

8. Sulfur 6/8 -2

9. Boron 3/8 +3

10. Oxygen 6/8 -2

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Isotopes

1. Suppose you discovered a new element with an Atomic number of 129. It

has two different isotopes: one with 134 neutrons and one with 137

neutrons. 65% have 134 neutrons and 35% have 137 neutrons. What is the

atomic mass of the new element? (show math work)

129 129

+134 +137

--------- ----------

263 266

A. 263(0.65)=170.95
B. 266(0.35)=93.1

=264.05
The atomic mass of the new element is 264.05 grams

Atomic Radius/Ionization Energy - Review your essay and try to look at

examples.

Atomic Radius Ionization Energy

Li > N Mg > Ca

C < Ge Mg < Cl

K > Ca

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More Reactive
Li < Cs

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M&M Lab

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Chemistry Test:

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