Christopher Chong (Class of 2022) - Blue Science Portfolio #2 (2)

17. Calcium carbonate
Ca​+2C​ O​3-​ 2 ​CaCO3​

18. Ammonium phosphate
NH​4+​ 1P​ O4​ -​ 3 (​ NH4​ )​ ​3 ​PO4​

19. Magnesium hydroxide
Mg​+2​OH​- ​ MgOH2​

20. Potassium sulfate

K+​ 1​SO4​ -​ 2​ K2​ ​SO​4

Part IV.

Directions:​ Determine the Mass % of Oxygen in A​ l2​ ​(SO​4​)​3​ or AgNO​3
Atomic Mass: ​Al (27) S (32) O (16) Ag (108) N (14)

Al2​ ​(SO​4​)3​ ​ Al=27*2=54/342*100=15.8%
S=32*3=96/342*100=28.1%
O=16*12=192/342*100=56.1

56.1% is oxygen

Whole =342

Part V.
Directions:​ Write an essay about the graph below. U​ se data!
Vocabulary:​ Unsaturated, saturated, supersaturated, Ions, Heat, Temperature, grams,
solubility, chemical formula

The scientist put 70g of a solute inside a graduated cylinder with 100g cm3​ ​ of the solvent water.
They then heated it up to 15​o​c. The solvent is currently super saturated. This is due to the fact

that on the graph the point is above the line of solubility. There is 45g of the solute left in the
bottom of the cylinder that has not dissolved into positive and negative ions. I found this number
by subtracting the amount of the solute that was put inside the beaker by the amount that would
completely dissolve at 15​o​c. To completely dissolve 70g of this solute, the temperature would
have to be raised by 23​oc​ to the temperature 38o​ ​c. I found this by finding the point, (15,70) on
the graph and increasing the temperature on the X axis until I hit the line of solubility.

Atomic Structure Project 2018

By:Christopher Chong

The History of the Atom

Atoms, the structure of everything. Without atoms there would be nothing, and
without the discovery of atoms, we would have no deep understanding to what objects
and things are composed of and why different things have different densities,
solubilities, vaporization points, boiling points and melting points. Now let’s look at the
man 4 scientists that contributed the most with the development of our understanding of
the atom.

John Dalton

John Dalton was born September 6 1766 in Eaglesfield,
England. He inherited the hereditary feature of green color
blindness and revealed the concept of Dalton’s Law of Parietal
Features. After attending Quaker School in Cumberland, he
started to teach there at the young age of 12. He later left the
college to become a farm hand at 14 years old but later returned
to teaching. When he returned he became an assistant at one of
the boarding schools of Quaker in Kendall.Dalton was the
creator of the Atomic Theory. The theory included 4 parts, 1 All
matter is made of atoms. Atoms are indivisible and
indestructible.2 All atoms of a given element are identical in mass and properties. 3,
Compounds are formed by a combination by 2 or more different kinds of atoms.

J.J Thomson

Thomson - J.J Thomson was famous for his discovery of the electron. He was a Nobel
Prize winning physicist and he was born on December 18th, 1856. He went on to attend

Trinity College in Cambridge to start his groundbreaking career. Thomson’s father was
a bookseller who always had planned for his son to be an engineer.
However, when an apprenticeship couldn’t be found for Thomson, he
was sent to Owens college at the age of 14 to bide his time. He later got
a scholarship to Trinity College in 1876 to study mathematics. After he
graduated, Thomson worked in the Cavendish Laboratory under
another scientist named Lord Rayleigh. Due to his gifts in academics,
he was quickly inducted into the prestigious Royal Society where he
was appointed as Rayleigh’s successor as the Cavendish Professor of
Physics. In 1894, Thomson started his research on cathode rays.
Cathode rays are glowing beams of light that follow an electrical
discharge in a vacuumized tube. At this point in time, this was a hot
topic because the nature of cathode rays was very unclear. When he
passed the rays through the vacuum, Thomson was able to measure
the precise angle that they were deflected at to assist him in calculating
the ratio of the electrical charge to the mass of particles. Thomas
concluded that all mass was made up of tiny particles much smaller than atoms.
Originally, he called these particles corpuscles but now they are called electrons. He
conducted another famous experiment in 1912 where he channeled ionized neon
through a magnetic using deflection. As a result, he discovered that neon was
composed of two different kinds of atoms and proved the existence of isotopes in a
stable environment. The was the very first of mass spectrometry.

Ernest Rutherford

Ernest Rutherford was born on August 30, 1871, in Nelson, New
Zealand, the fourth child and second son in a family of seven sons
and five daughters. His father James Rutherford, a Scottish
wheelwright, immigrated to New Zealand with Ernest's grandfather
and the whole family in 1842. His mother, née Martha Thompson,
was an English schoolteacher, who, with her widowed mother, also
went to live there in 1855. Ernest got his education at an early age at
government schools. When he turned 16, he went to Nelson
Collegiate School. He was later awarded a university scholarship and
went to Trinity College.Rutherford's first researches, in New Zealand,
were concerned with the magnetic properties of iron exposed to
high-frequency oscillations. Later in Manchester, he discovered what
some say is his biggest contribution to science, the Nucleus.
According to Rutherford, practically the whole mass of the atom and at the same time all

positive charge of the atom is concentrated in a small space at the centre. ​ I​ n 1912 the
scientist Niels Bohr joined him at Manchester and he adapted Rutherford's nuclear
structure to Max Planck’s quantum theory and so obtained a theory of atomic structure
which, with later improvements, mainly as a result of Heisenberg's concepts, remains
valid to this day.

Niels Bohr

In the autumn of 1911 he made a stay at Cambridge, where he
profited by following the experimental work going on in the
Cavendish Laboratory under S​ ir J.J. Thomson's​ guidance, at the
same time as he pursued own theoretical studies. In the spring of
1912 he was at work in P​ rofessor Rutherford's​ laboratory in
Manchester, where just in those years such an intensive
scientific life and activity prevailed as a result of that
investigator's fundamental inquiries into the radioactive
phenomena. Having there carried out a theoretical piece of work
on the absorption of alpha rays which was published in the
Philosophical Magazine​, 1913, he passed on to a study of the
structure of atoms on the basis of Rutherford's discovery of the
atomic nucleus. By introducing conceptions borrowed from the Quantum Theory as
established by Planck, which had gradually come to occupy a prominent position in the
science of theoretical physics, he succeeded in working out and presenting a picture of
atomic structure that, with later improvements (mainly as a result of Heisenberg's ideas
in 1925), still fitly serves as an elucidation of the physical and chemical properties of the
elements.

In the autumn of 1911 he made a stay at Cambridge, where he profited by
following the experimental work going on in the Cavendish Laboratory under S​ ir J.J.
Thomson's​ guidance, at the same time as he pursued own theoretical studies. In the
spring of 1912 he was at work in P​ rofessor Rutherford's​ laboratory in Manchester,
where just in those years such an intensive scientific life and activity prevailed as a
consequence of that investigator's fundamental inquiries into the radioactive
phenomena. Having there carried out a theoretical piece of work on the absorption of
alpha rays which was published in the ​Philosophical Magazine,​ 1913, he passed on to a

study of the structure of atoms on the basis of Rutherford's discovery of the atomic
nucleus. By introducing conceptions borrowed from the Quantum Theory as established
by Planck, which had gradually come to occupy a prominent position in the science of
theoretical physics, he succeeded in working out and presenting a picture of atomic
structure that, with later improvements (mainly as a result of Heisenberg's ideas in
1925), still fitly serves as an elucidation of the physical and chemical properties of the
elements.

Structure of the Atom

Nucleus:
The nucleus is always in the center of all atoms.
The nucleus contains the protons and neutrons in
an atom. As you can see, the blue and red dots
are the protons and neutrons and they are located
nowhere else except inside the nucleus

Protons:

The protons in an atom are always located in the nucleus. Protons have a
+1 charge and have an atomic weight of 1. Their numbers vary based on
the element’s atomic number. For example, hydrogen would have 1 proton
since it’s atomic number is 1

Neutrons:
Like protons, neutrons are also only found in the
nucleus of atoms.Neutrons have a mass of 1 and their
numbers vary depending on the element’s atomic
weight and on the amount of protons that are found in
the element.For example, the element helium has an
atomic weight of 4 and since it’s atomic number is 2,
there is 2 neutrons.

Electrons:
Unlike protons or neutrons, electrons are
located on the outside rings of the atom.
Electrons have a negative charge meaning that
they cancel out the positive charge of the
protons. The amount of electrons varies based
on the elements ionic charge and the amount of
protons.

Atomic Mass:
Atomic mass is how much an element
weighs. This varies between different
elements since they all have a different

amount of protons and neutrons. For example, helium has an atomic mass
of 4 because it has 2 protons and 2 neutrons that make it up.

Valence Electrons:
Valence electrons are the electrons on the
outermost shell of the atom. These
electrons are later passed on to other
elements to create compounds. For
example, the valence electron in Sodium
is the one on the outside ring.This electron
will be passed on to chlorine if this sodium
is ever combined with it to make salt.

Helium 2 4 2 2 2

Lithium 3 7 3 4 2

Beryllium 4 9 4 5 2

Boron 5 11 5 6 2

Carbon 6 12 6 6 2

Nitrogen 7 14 7 7 11

Oxygen 8 16 8 8 10

Fluorine 9 19 9 10 10

Neon 10 20 10 10 10

Isotopes

Isotopes are essentially variations of elements. Isotopes are like different car models.
For example, Porsche sells a car called the 911. The 911 has many different variations such as
the base 911 with 370 horsepower and the 911 Carrera S with an engine that has 420
horsepower. Both of these cars are still 911s but the Carrera S just has more horsepower and
extra options included.Isotopes are very similar to this.

Take carbon for example, there are many different variations of carbon. These variations
include Carbon 12, Carbon 13 and Carbon 14. All of these isotopes are carbon and they all
have 6 protons. However, carbon 12 has 6 neutrons while carbon 13 has 7 neutrons and carbon
14 has 8 neutrons. All of these are still carbon but the one difference they share is the amount
of neutrons they have. Since neutrons have an atomic weight of 1, the different weights of the

carbon isotopes are affected by this. For example, Carbon 12 has an atomic weight of 12 while
Carbon 13 has a weight of 13 and Carbon 14 has a weight of 14. This is all due to the fact that
there is a change in the amount of neutrons in the atom but the protons still remain the same.

Another example of isotopes is the different
Iron isotopes. In the picture shown, there
are 4 different types of iron isotopes, Iron
54, Iron 56, Iron 57 and Iron 58. All of these
isotopes have the same amount of protons
since if we were to add or take away any
protons, the iron would become an entirely
different element. Just as with the Carbon
isotopes I explained earlier, the Iron
isotopes also all have different amounts of
neutrons which due to their weight of 1,
results in them having different atomic
weights.

You may be asking yourself, if their weights are the only thing that’s different about them,
then what good are they. The answer to this is radioactivity. Radioactivity gives the element
carbon the ability to perform an act called carbon dating. Carbon dating is a way of determining
an object’s age. For example, if someone says that they have a tree from when Jesus Christ
himself was living from over 2000 years ago, there would be no easy way to tell if it was actually
real without determining it’s age, This is where carbon dating comes in. The isotope Carbon 12
has 6 protons and 6 neutrons. This means that Carbon 12 is not radioactive. However, if you
add 2 more neutrons, to Carbon 12 and make it Carbon 14, this makes it radioactive giving it the
ability to perform carbon dating.

Dmitri Mendeleev

Dmitri Mendeleev was a Russian scientist who was born in Tobolsk Russia in the year
1834 on February 8th and died February 2nd 1907. Before Dmitri created the periodic table,
scientists used a variety of acronyms to represent different materials in substances, there was
no common language that they used, so their work would only make sense to them and not
other scientists. Mendeleev was the last of 14 children and as a child had a very hard life. His
father was Ivan Pavlovich and was a teacher in the local gymnasium. H​ is father went blind the

year of his birth and later died in 1847. In order to support his family, Dmitri’s mother, Mariya,
started to work at a small glass factory that her family owned. The factory later burned down in
December 1848 which made Dmitri’s mother bring him to St. Petersburg to enroll in the Main
Pedagogical Institute. Shortly before he graduated in 1855, his mother passed away.
Mendeleev’s first teaching position was in Simferopol in Crimea. He stayed for the short time of
2 months before deciding to return to St. Petersburg to complete his education. When he
returned, he received a masters degree in 1856 and started to conduct research in organic
chemistry. In order to go to the University of Heidelberg to study abroad, he received financial
aid from a government fellowship. When he attended the university, he ended up not working
with the fellow scientists in the labs the school provided and instead, set up his own lab in his
apartment. One day, Mendeleev couldn’t find a textbook that he could use for himself,
therefore, he would write one himself. This would later lead him to make his biggest contribution
to science, the foundation of the periodic law. In order to write his book, he had to study the
major groups of elements. He studied alkali metals, alkali earth metals and noble gases which
led him to organize all of them on a table. Mendeleev established that the order of atomic
weights could be used not only to arrange the elements within each group but also to arrange
the groups themselves. In his effort to make sense of the extensive knowledge that already
existed of the chemical and physical properties of the chemical elements and their compounds,
Mendeleev discovered the periodic law.

Trends In the Periodic Table

All of the elements in the first column all have an ionic charge of +1. This is due to the
fact that they all have a single positive charge left after the negative electrons cancel out the
positive protons. This is the same exact rule for all of the other elements. Let’s take some of the
elements in the second row for example. Some of these elements are Calcium, Beryllium and
Magnesium. All of these elements have ionic charges of +2. To prove this, we look at the
amount of Electrons each one has in its outermost shell. Let’s start with Beryllium. Beryllium has
2 electrons in its outermost shell giving it an ionic charge of +2. Next let’s move on to
Magnesium. Magnesium Also has 2 electrons in its outermost shell giving it an Ionic charge of
+2. Lastly, we have Calcium. Calcium also has 2 electrons in its outermost shell also giving it an
ionic charge of +2. You may ask what is the significance of this and this next part will answer
your question. When 2 elements are put together to make a compound, they must follow the
octet rule, meaning that there has to be 8 electrons in the outermost shell. Take the compound
Beryllium Chloride for example. Chlorine has 7 total electrons in its outermost shell. Since
Beryllium has an ionic charge of 2, that means that in the compound Beryllium Chloride, there is
2 Chlorine atoms and 1 Beryllium atom. Since there is 2 electrons in the Beryllium atom’s
outermost shell and 2 Chlorine atoms both with 1 missing electron, the Beryllium atom gives

away its two electrons to the Chlorine atoms. This goes for the same with all compounds and all
elements in the table.

1st Group
Hydrogen
Lithium
Sodium
Potassium

2nd Group
Beryllium
Magnesium
Calcium

3rd Group
Boron
Aluminum

4th Group
Carbon
Silicon

5th Group
Nitrogen
Phosphorous

6th Group
Oxygen
Sulfur

7th Group
Fluorine
Chlorine

8th Group
Helium
Neon
Argon

Alkali Metals

Alkali Metals are any of the elements that make up the first group of the periodic table.
These elements include, lithium, sodium, potassium, rubidium, cesium and francium. They are
called alkali metals because when they come in contact with water, a reaction occurs that forms
alkalies. Alkalies are strong bases capable of neutralizing acid. Sodium and potassium are the
6th and 7th most abundant elements on the periodic table constituting 2.6 and 2.4 percent of the
earth’s crust. The metals that are much more rare are ​rubidium, lithium, and cesium,
respectively, forming 0.03, 0.007, and 0.0007 percent of Earth’s crust. The last element of the
first group is Francium, a natural radioactive isotope and is extremely rare. It was only recently
discovered in 1939. All of the alkali metals have silver like lustre and are all excellent conductors
of electricity. By far, sodium is the most important metal in terms of industrial use. Sodium is
employed in the reduction of organic compounds and in the preparation of many commercial
compounds. As a free metal, it is used as a heat-transfer fluid in some nuclear reactors.

Alkaline Earth Metals

Alkaline earth metals are all of the elements in the second
column of the periodic table. These include The elements are
beryllium (Be), magnesium (Mg), calcium(Ca), strontium (Sr),
barium (Ba), and radium (Ra). They are classified as alkaline
earth metals because they all have 2 electrons in their outermost
shell of their atoms and because of basic nature of the
compounds the select elements are in when they’re bonded with
oxygen. Getting more into this, prior to the 19th century, things
that were metallic, insoluble in water and unaffected by fire were
called Earths. ​The atoms of the alkaline-earth metals easily lose
electrons to become positive ions.Most of their typical compounds
are therefore ionic: salts in which the metal occurs as the cation M2+, where M represents any
Group 2 atom. The salts are colourless unless they include a negative ion. With Radium as an
exception, the alkaline earth metals all find some kind of commercial purpose. For example,
magnesium and calcium are particularly abundant in nature and play important roles in
biological and geological purposes. Radium on the other hand is rare and all of its isotopes are

radioactive. Radium has never been mass produced and although it was largely used in the first
half of the 20th century for cancer treatment, it has been replaced by less expensive
alternatives.

Noble Gases

The elements that make up the category of noble gases are
helium (He), neon (Ne), argon (Ar), krypton(Kr), xenon (Xe),
radon(Rn), and oganesson (Og). These gases are colorless​,
odorless, tasteless and nonflammable T​ hey traditionally have
been labeled Group 0 in the periodic table because for decades
after their discovery it was believed that they could not bond to
other atoms; that is, that their atoms could not combine with those
of other elements to form chemical compounds. Most of the noble
gases at one point were thought to be exceedingly rare, however
later speculation found that they were quite abundant in nature and in the universe.The
abundances in noble gases decrease as their number increases. For example, radon (element
86), is much more rare than helium (element 2). Several important uses of the noble gases
depend on their inability to react chemically. Their incompatibility toward oxygen, for example,
results in non-flammability upon the noble gases. Although helium is not q as buoyant as
hydrogen is, its ability to not light on fire makes it a safer lifting gas for things lighter than
aircraft. Helium and Argon, the most inexpensive noble gases, are used to provide chemically
unreactive environments and are good with welding and refining of like aluminum (atmospheric
oxygen and, in some cases, nitrogen or carbon dioxide would react with the hot metal).

​Halogens

The halogen elements are fluorine (F), chlorine(Cl), bromine (Br), iodine (I), astatine (At),
and tennessine (Ts). They were given the name h​ alogen,​ from the Greek roots ​hal​ which means
alt and -​gen​ which means “to produce”. They were named this because they all produce sodium
salts with properties similar to their own, of which sodium chloride also known as salt , or halite
is best known.Because of their great reactivity, the free halogen elements are not found in
nature. In combined form, fluorine is the most abundant of the halogens in Earth’s crust. The
percentages of the halogens in the igneous rocks of Earth’s crust are 0.06 fluorine, 0.031
chlorine, 0.00016 bromine, and 0.00003 iodine. Astatine and tennessine are not in nature,
because they consist of only short lived radioactive isotopes.Chlorine is the most well known of
the halogens. The element is mostly used as a means of water purification most often in
swimming pools. It is employed in a number of chemical processes. Sodium chloride or salt, of
course, is one of the most familiar chemical compounds. Fluorides on the other hand are known

for helping stop tooth decay resulting in towns putting it inside the water supply. Organic
fluorides are also used as refrigerants and lubricants.The element iodine is most well known as
an antiseptic, and bromine is used chiefly to prepare bromine compounds that are used in flame
retardants and as general pesticides. In the past ethylene dibromide was extensively used as an
additive in leaded gasoline.

Atom Article

The article called “What is An Atom?” talks about the different parts of atoms as well as
isotopes and the history of the atom. First it talks about the bare basics of what atoms are. It
says that atoms are the basic building blocks of everything in the entire universe and were first
created over 13.7 billion years ago.. Next it talks about atom particles and says that the
neutrons and the protons of the atom reside in the nucleus and are heavier than the electrons
that reside awound the rings of the atom. It then goes in depth into the nucleus and explains
that it was first discovered by Ernest Rutherford in the year 1911. It also says that Rutherford
proposed the name proton for the positively charged molecules in the atoms. Next it talks about
isotopes. It explains that isotopes are essentially the same element but have different amounts
of neutrons. For example, carbon-12 has 6 neutrons and 6 protons while carbon 14 has 8
neutrons and 6 protons. Both of these elements are carbon however they differ in amounts of
neutrons. Next it goes in depth with the history of the atom and says that it goes as far back as
440 B.C t​ o ​Democritus, a Greek scientist and philosopher who first discovered the atom. It then
talks about John Dalton who created his atomic theory, Thomson who discovered the electron,
Rutherford who discovered the nucleus and Niels Bohr, who further built upon Rutherford’s
atom model .

A student finds a rock on the way to school. In the laboratory he determines that the volume of
the rock is 34.5 cm3, and the mass is 48.3 g. What is the density of the rock?

A scientist conducted an experiment to determine how the amount of salt in a body of water
affects the number of plants that can live in the water. In this experiment the dependent variable
is _____________.

In an experiment, the one variable that is changed by the experimenter is called the
_____________.

A scientist who wants to study the effects of fertilizer on plants sets up an experiment. Plant A
gets no fertilizer, Plant B gets 5 mg. of fertilizer each day, and Plant C gets 10mg. of fertilizer
each day. Which plant is the control group.

Homer notices that his shower is covered in a strange green slime. Homer decides to spray half
of the shower with coconut juice thinking this will kill the slime. He sprays the other half of the

shower with water. After 3 days of "treatment" the green slime on the coconut juice side of the
shower dies. The dependent variable in his experiment is _____________.

A scientist plants two rows of corn for experimentation. She puts fertilizer on row 1 but does not
put fertilizer on row 2. Both rows receive the same amount of water and light intensity. She
checks the growth of the corn over the course of 5 months. What is a constant in this
experiment.

A student hypothesized that the amount of sunlight a sunflower plant receives determines the
number of sunflower seeds the plant produces. In her experiment, the number of seeds
produces is the _____.

Sarah wanted to find out if temperature has an effect on the growth of bread mold. She grew the
mold in nine Petri dishes containing the same amount and type of nutrients. Three were kept at
0 C, three were kept at 90 C, and three were kept at room temperature, 27 C. The containers
were examined and the growth of the bread mold was recorded each Friday for five weeks.
Which of the following is her hypothesis?

5.9 km = _____________ m

756.0 cg = _____________ g

23,000 mm = _____________ m

Scientific Method Quiz

Correct

+1 / 1 point(s)

1. A scientist conducted an experiment to determine how the amount
of salt in a body of water affects the number of plants that can live in
the water. In this experiment the dependent variable is
_____________.

Your Answer: t​ he number of plants in the water

Correct

+1 / 1 point(s)

2. A scientist hypothesizes that the temperature at which an
alligator's egg is incubated will determine whether the alligator will
be male or female. The independent variable is ____________.

Your Answer: t​ he temperature

Correct

0 / 1 point(s)

3. In an experiment, the factor that we measure and is on the Y-axis
is called the ____________.

Your Answer: ​dependent variable

Correct

+1 / 1 point(s)

4. In an experiment, the one variable that is changed by the
experimenter is called the _____________.

Your Answer: ​independent variable

Correct

0 / 1 point(s)

5. If you were measuring the mass of a fly, you should use
____________.

Your Answer: ​milagrams

Correct

+1 / 1 point(s)

6. If you wanted to know the volume of water in a small can of soda,
you would use ______________.

Your Answer: ​milliliters

Correct

+1 / 1 point(s)

7. A scientist who wants to study the affects of fertilizer on plants
sets up an experiment. Plant A gets no fertilizer, Plant B gets 5 mg.
of fertilizer each day, and Plant C gets 10mg. of fertilizer each day.
Which plant is the control?

Your Answer: P​ lant A

Correct

+1 / 1 point(s)

8. Victoria grows the same bacteria in 20 petri dishes. She places 10
of the dishes in a container with a normal atmosphere. The
remaining dishes she places in a container in which the oxygen level
is double the normal level. She labels the first group "A" and the

second group "B". Which of the following best describes the
groups?

Your Answer: ​Group A is the control group; Group B is the experimental group

Correct

+1 / 1 point(s)

9. Homer notices that his shower is covered in a strange green
slime. Homer decides to spray half of the shower with coconut juice
thinking this will kill the slime. He sprays the other half of the shower
with water. After 3 days of "treatment" the green slime on the
coconut juice side of the shower dies. The dependent variable in his
experiment is _____________.

Your Answer: ​Whether or not the treatment worked

Correct

0 / 1 point(s)

10. For an experiment, a scientist put lime at the base of tomato
plant A and baking soda at the base of tomato plant B. She then
sealed the plants in plastic bags. Tomato plant A eventually died,
and tomato plant B stayed healthy. What is the Independent Variable
in this experiment?

Your Answer: W​ hat was put at the base of the plant

Correct

+1 / 1 point(s)

11. I am trying to clean my bathroom because it has mold on the
bottom. I was told to use oxy clean to get it up. I use oxy clean on
half of the bathroom and water on the other half. The control is:

Your Answer: ​water

Correct

+1 / 1 point(s)

12. A scientist plants two rows of corn for experimentation. She puts
fertilizer on row 1 but does not put fertilizer on row 2. Both rows
receive the same amount of water and light intensity. She checks the
growth of the corn over the course of 5 months. What is a constant
in this experiment.

Your Answer: A​ mount of water

Correct

+1 / 1 point(s)

13. A student wants to conduct an experiment to find out how pulse
rates changes as the length of time spent exercising increases. The
dependent variable will be _____.

Your Answer: ​pulse rate

Correct

0 / 1 point(s)

14. A student hypothesized that the amount of sunlight a sunflower
plant receives determines the number of sunflower seeds the plant
produces. In her experiment, the number of seeds produced is the
_____.

Your Answer: d​ ependent variable

Correct

+1 / 1 point(s)

15. In a controlled experiment, the independent variable is ____.

Your Answer: c​ hanged to test the hypothesis - it goes on the x-axis

Correct

+1 / 1 point(s)

16. Sarah wanted to find out if temperature has an effect on the
growth of bread mold. She grew the mold in nine Petri dishes
containing the same amount and type of nutrients. Three were kept
at 0 C, three were kept at 90 C, and three were kept at room
temperature, 27 C. The containers were examined and the growth of
the bread mold was recorded each Friday for five weeks. Which of
the following is her hypothesis?

Your Answer: ​If the temperature changes then the amount of bread mold will change.

Correct

+1 / 1 point(s)

17. Sarah wanted to find out if temperature has an effect on the
growth of bread mold. She grew the mold in nine Petri dishes
containing the same amount and type of nutrients. Three were kept
at 0 C, three were kept at 90 C, and three were kept at room
temperature, 27 C. The containers were examined and the growth of
the bread mold was recorded each Friday for five weeks. The
independent variable is:

Your Answer: ​temperature of the containers

Correct

+1 / 1 point(s)

18. What is the independent variable in the experiment found in the
link below?

Your Answer: ​color of the light

Correct

+1 / 1 point(s)

19. In the experiment found on the link, all of the following variables
must be held constant EXCEPT

Your Answer: c​ olor of the light

Correct

+1 / 1 point(s)

20. An unknown substance from planet X has a density of 10 g/mL. It
occupies a volume of 80 mL. What is the mass of this unknown
substance?

Your Answer: 8​ 00 g

Correct

+1 / 1 point(s)

21. A graduated cylinder has 22 mL of water placed in it. An
irregularly shaped rock is then placed in the graduated cylinder and
the volume of the rock and water in the graduated cylinder now
reads 30 mL . The mass of the rock is 24 g. What is the density of the
rock?

Your Answer: ​3 g/cm3

Correct

+1 / 1 point(s)

22. A rectangular solid of unknown density is 5 cm long, 2 cm high,
and 4 cm wide. The mass of this solid is 300 grams. Given this
information for this homogeneous material, calculate the density.

Your Answer: ​7.5 g/cm3

Correct

+1 / 1 point(s)

23. Silver has a density of 10.5 g/cm3 and gold has a density of 19.3
g/cm3 . Which would have a greater mass, 5 cm3 of silver or 5 cm3
of gold?

Your Answer: ​Gold

Correct

+1 / 1 point(s)

24. A 28.5 g of iron is added to a graduated cylinder containing 45.5
mL of water. The water level rises to the 49.1 mark. Calculate the
density.

Your Answer: ​7.92 g/cm3

Correct

+1 / 1 point(s)

25. 43.2 m = __________ mm

Your Answer: ​43200

Correct

+1 / 1 point(s)

26. 8700 mL = ________ L

Your Answer: 8​ .7

Correct

+1 / 1 point(s)

27. 5.9 km = _____________ m

Your Answer: ​5900

Correct

+1 / 1 point(s)

28. 756.0 cg = _____________ g

Your Answer: 7​ .56

Correct

+1 / 1 point(s)

29. 23,000 mm = _____________ m

Your Answer: ​23

Correct

+1 / 1 point(s)

30. Metric Unit for Mass

Your Answer: ​GRAMS

Correct

+1 / 1 point(s)

31. Metric Unit for Density of a Solid

Your Answer: g​ /cm3

Correct

+1 / 1 point(s)

32. Metric Unit for Density of a Liquid

Your Answer: ​g/mL

Correct

+1 / 1 point(s)

33. Which appliance is used twice as many hours on the weekends
as it is on weekdays?

Your Answer: T​ V

Correct

+1 / 1 point(s)

34.On average, how many hours is the computer used on a
weekday?

Your Answer: ​2

Correct

+1 / 1 point(s)

35. Which 2 objects are the same substance?

Your Answer: 1​ and 4

Correct

+1 / 1 point(s)

36. What would the mass of the gold in B if the volume is 50% of A?

Your Answer: ​500 g

Correct

+1 / 1 point(s)

37. Why does the Oceanic Plate sink below the Continental Plate in
the picture?

Your Answer: ​The Oceanic Plate made of Basalt is MORE DENSE than the
Continental Plate made of Granite.

Correct

+1 / 1 point(s)

38. Why are mountains such as the Himalayans formed? Study the
picture.

Your Answer: C​ ontinental plates collide with equal density Continental Plates and are
forced upwards.

Correct

+1 / 1 point(s)

39. What volume of silver metal will have a mass of exactly 300.0 g.
The density of silver is 10.5 g/cm3.

Your Answer: ​28.6 cm3

Correct

+1 / 1 point(s)

40. The density of lead is 11.342 g/cm3. What would be the volume of
a 400.0 g sample of this metal?

Your Answer: ​35.3 cm3

Correct

+1 / 1 point(s)

41. If two objects have the same volume but one has a greater mass,
the one with greater mass

Your Answer: h​ as a higher density

Correct

+1 / 1 point(s)

42. If the density of water is 1 gram/cm3, this means that the mass of
100 cm3 of water should be

Your Answer: 1​ 00 grams

Correct

+1 / 1 point(s)

43. The density of hot an cold water are different mainly because

Your Answer: t​ he molecules in hot water move faster and are slightly further apart

Phase Changes of Water

3. Activity: Phase Change of Water

Directions:
● Melt the ice water and record the temperatures every 30 seconds until you reach the
boiling point of water.
● Record the temperatures on the following data table:
​ C​ onstruct a graph of your results. *​Use Link on Classroom
● Respond to the Critical Thinking Questions

Graph:

Critical Thinking Questions:

1. When did the temperatures stay the same on the graph? Why did the
temperatures stay the same at 2 points during the lab?

The temperatures stayed the same because a phase change was occurring.

2. How would the graph be different if we tried this experiment with Gold?
Explain:T​ he graph would have had much higher temperatures and much
higher times since gold has a much higher heat of fusion and heat of
vaporization than water does. It takes much more energy to melt gold, get it to
it’s boiling point and turn it into vapor than it does with water.

3. What is the role of energy during the phase changes?
For every solid object, a certain amount of energy is required to get that solid
object to its melting point or it’s heat of fusion. Next it will have a physical
change and turn into a liquid. It’s temperature will continue to rise until it gets
to it’s heat of vaporization which will turn it into a gas form. Each time the
object changed physically and gained temperature, it required more and more
energy.

4. Describe the motion of the molecules throughout the experiment. Find
diagrams that show the motion.

In the beginning, the molecules in the water will barely be moving. The molecules
with partial negative charges will be attracted to the molecules with partial
positive charges and vice versa. As heat is added, the molecules will start to
move around more and become a lot more spread out than when the object was
in a solid form. In a liquid form, the molecules are less lined up than in a solid and
moving around more. Finally in a gas, the molecules are moving around
everywhere and are all over the place.
5. How does the Average Kinetic Energy change throughout the experiment?

(Be specific)

6. Suppose you had 200 mL of ice in one beaker and 400 mL of ice in another
beaker. Compare and explain the following in the beakers after they have
reached the boiling point:

A. Heat Energy
B. Temperature
C. Average Kinetic Energy
D. Specific Heat
E. Latent Heat (Define it)
Latent heat is the amount of heat that is required to turn a solid into a liquid or
vapor without changing its temperature

The higher the amount of water the more amount of energy is required to get it to
its melting point and its point of vaporization. With 200 mL of water,it would take
it 66720 joules of energy to get it to it’s melting point. With 400 mL of water it
would take exactly double the amount of joules it takes to melt 200 mL of water.
So it would take 133440 joules of energy to melt 400 mL of ice since it has double
the mass of 200 mL of ice. The exact temperature of when the ice starts melting
for both 200mL and 400mL would be 0 degrees celsius. The boiling point of both
the amounts of water is 100 degrees celsius. In the graph, when the temperature
is going up so is the kinetic energy of the water since the molecules inside the
water will start to shake more the more amount of energy that is added.

7. Why do we put water in a car’s engine? Explain:
We add a mixture of coolant and water in order to keep the engine from

overheating. This excessive heat it made by the energy that is being put into
the engine in order to power the car. Since the cylinders in the car’s engine
are moving so fast, they create a lot of kinetic energy which means that they
will also create a high amount of heat.

This is a graph showing the phase changes of slowly melting Moth Crystals. The temperature
started at 62​o​ Celsius and gradually started to go down until it hit its melting point at 53o​ ..​ We
recorded the temperature of the crystals once every half a minute.We recorded 53​o​ 21 times in
10 minutes since the crystals were undergoing a phase change at that temperature. After that,
the temperature of the crystals decreased rapidly until we ended the experiment at 21.5
minutes.

Gases have the most kinetic energy

Evaporation occurs at the surface of liquid that is not boiling

Average kinetic energy of particles

Calculate Heat Energy: * SH

Apply the following Equations: Boiling Heat of
Heat = Mass * Heat of Fusion Pt. ​(C) Vaporization
Heat = Mass * Change in Temperature
Heat = Mass * Heat of Vaporization (cal/g)
Data Table:

Metal Mass Heat of Melting Specific Heat
Fusion Pt.​ (C) Heat Energy
(cal/g) (cal/gC) (cal)

Water 65 g 80 0 100 540 1

Aluminum 65 g 95 660 2467 2500 0.21

Gold 65 g 15 1063 2800 377 0.03

Copper 65 g 49 1085 2562 4730 .385

*SHOW ALL MATH STEPS
Math Steps (____ out of 4)
A. Aluminum
Heat=m*hf​ usion

Heat = 65g*95 cal/g

Heat= 6175 joules
Melted the aluminum and made it liquid

Heat=m*change in temperature*SH
Heat=65*1807​0​*0.21cal/gC
Heat=24665.5 calories

I got the liquid aluminum to its boiling point

Heat=m*hv​ aporization

Heat =65g*2500cal/g

Heat= 162500 Cal

213340.5 calories

B. Gold
Heat = m*H​fusion
Heat=65g*15cal/g
heat = 975calories
Heat= 65*17370​ *​ 0.03cal/gC
3387.15Calories

Heat=M*H​Vaporization
Heat=65g*377 cal/g
Heat=24505 calories

Heat=28867.615 calories

C. Water
Heat=M*H​fusion
Heat=65*80c
5200 calories
Heat=M*change in temperature*1
Heat=65g*100c*1
Heat=6500 Calories
Heat=M*Hv​ aporization
Heat=65g*540cal/g

Heat=35100 calories

Heat=46800

Graph your Results:

Questions:
1. How are the substances different?

The substances all require different amounts of energy for their heat of vaporization, their heat
of fusion, and their melting point. A substance with a higher heat of fusion will also have a
higher heat of vaporization.

2. What is the difference between Heat and Temperature?
Heat is the amount of energy put into an object to raise itś temperature. Temperature is

3. Place your Heat Energy results in Scientific Notation.
4. Why do metals have such low specific heats? How does this relate to Conductors?

5. How are Heat and Temperature different for the following pictures of​ ​boiling

water? Explain:​ (Hint: Use the Heat equation)

QUIZ: Phase Changes

Calculate Heat Energy: * SH

Apply the following Equations: Boiling Heat of
Heat = Mass * Heat of Fusion Pt. ​(C) Vaporization
Heat = Mass * Change in Temperature
Heat = Mass * Heat of Vaporization (cal/g)
Data Table:

Metal Mass Heat of Melting Specific Heat
Fusion Pt.​ (C) Heat Energy
(cal/g) (cal/gC) (cal)

Water 37 g 80 0 100 540 1 26640

Silver 37 g 26 961 2212 2356 0.057 90772.4

Directions: ​Determine the Heat Energy required to completely evaporate the substances in the
data table.

*SHOW ALL MATH STEPS
Math Steps (____ out of 4)
A. Water
Heat=M*H/F​ usion
Heat=37g*80cal/g
Heat=2960 calories

Heat=M*Change In temperature*SH

Heat=37g*100o​ ​C*1 cal/gC

Heat=3700 Calories

Heat= M*H/V​ aporization

Heat=37g*540 cal/g

19980 Calories

Heat energy= 19980 calories+2960 calories+3700 Calories
Heat energy= 26640 Calories

Scientific Notation:
2.664*104​
B. Silver
Heat=M*H/​Fusion
Heat=37g*26 cal/g
Heat=962 Calories

Heat=M*Change In temperature*SH
Heat=37g*1251​oC​ *0.057 Cal/gC
Heat=2638.4 Calories
Heat= M*H/​Vaporization
Heat=37g*2356o​ C​
Heat=87172 calories

Heat Energy= 2638 cal*962 cal*87172 cal
Heat energy

Scientific Notation:
9.07724 × 10​4

Graph your Results:

Writing (_____ out of 4)
Questions:

1. How are Heat and Temperature different for the following pictures of​ ​boiling​ ​water?

Explain:​ (Hint: Use the Heat equation)
The heat and temperature are different because the picture on the left has much more

mass than the picture on the right. To get the picture of water on the left to its boiling point
would take an enormous amount of heat energy due to the amount of mass it has. To get the
picture of water on the right to its boiling point would take much less heat energy since it has so
much less mass than the water on the left. Both of the water in the picture are required to get to
100o​ ​ in order to boil but since the picture on the left has more mass, it will take much more
energy to get all of its water to boil.

2. How can you use the unit (cal/gC) to explain the difference between Water and Silver?

Cal/gC represents is the unit used for the specific heat of an object with water and
silver, water has a much higher specific heat at 1 cal/gC than silver at 0.057 cal/gC. This
means that wate​r will melt much faster than silver since it has a higher specific he​ at. It
also means that silver is a better conductor of heat than water is since it takes more heat
to get it to its melting point.

3. Would it be possible for there to be solid oxygen on another planet? Explain:

It would be possible for there to be solid oxygen on another planet. This is
because our planet's temperature will never go or even get close to -218o​ ​C. On other
planets though, the temperature may go down to 218o​ C​ and cause the oxygen, if there is
any, to reach it´s freezing point and become solid.
Oxygen Melting Point: -218 C
Oxygen Boiling Point: -183 C

In this experiment

Mixture Project

Textbook: Chapter 15 (448-473)

Due:
Vocabulary
Directions: ​Write the definition and master the words on Vocab.com.
Include a screenshot on google drive showing your mastery of the words.
Include a picture that represents each word.

Substance Heterogeneous Solubility Solvent
Mixture
Element Atom Saturated
Homogeneous
Compound Mixture Solute Unsaturated
Mixture Suspension Supersaturated
Solution

Concentration

2. Classification of Matter
*Provide Examples of each form of matter. Include a picture.

Heterogeneous Homogeneous Element Compound
Mixture can see Mixture Cant see

Sand Mayonaise Oxygen Water

Hamburger Vinegar Hydrogen Salt

Soil Laundry Mercury Oxide

detergent

Fruit Loops Soda Calcium Alcohol

Citric Acid Coffee Carbon Sulfide

Critical Thinking:
● How are the examples for Heterogeneous and Homogeneous
MIxtures different?
● How are Elements and Compounds similar and different?

Elements and compounds are different based on the atoms they are made

up of. Elements are made of the same kind of atoms while compounds are

made up of different kind of atoms such as H2O.

In heterogeneous mixtures, the parts that make up the mixture are visible
while in homogeneous mixtures, the parts are not visible.

Tray=​ 2 grams

Whole=​ 51 grams-2g=49 grams

M&Ms=​ 11 grams

Crunchy M&Ms​=9 grams

Marshmallows=​ 13 grams

Skittles=​ 16 grams

M&Ms P=11g/49g*100
P=22%

Crunchy M&Ms P=9g/49g*100
P=18%

Marshmallows P=13g/49g*100
P=27%

Skittles P=16g/49g*100
P=33%

PIE CHART BELOW

QUIZ: Classifying Matter

I. Directions: I​ dentify the following as either a Heterogeneous Mixture, Homogeneous Mixture,

Element or Compound. Write the following letters in Column B for your choices:

A. Heterogeneous

B. Homogeneous

C. Element

D. Compound

Column A Column B

Salad A

Copper C

Lemonade B

Rocks, sand, gravel A

Salt Water B

Gold C

Sodium Chloride (​ NaCl) D

Air (Oxygen, nitrogen, carbon monoxide…) B

K​2​SO4​ D
Twix, snickers, pretzels, popcorn in a bag A

II. Directions:​ Determine the Mass % of each mixture and construct the appropriate graphs.

Mixture A Mass (g) %

Large Rocks 125 52%

Small Rocks 75 31%

Coarse Sand 32 13%

Iron 9 4%

Mixture B Mass (g) %
Large Rocks 205 53%
Small Rocks 58 15%
Coarse Sand 97 25%
Iron 29 7%

Calculation Examples ​(Provide 2 Examples showing how you determined the Mass %)
Large Rocks= 205g/241g*100=85%
Small Rocks=75g/241g*100g=31%

Graphs:
Mixture A

Mixture B

Part III.​ Determine the Mass % of Elements in each Compound:

K​2​SO​4​ - Potassium Sulfate
(Show Math Here)
K=(2)*39=78/174*100=45%
S=(1)32=32/174*100=18%
O(4)16=64/174*100=37%
32=78=64=174

Na3​ P​ O​4​ - Sodium Phosphate
(Show Math Here)

Na(3)23=69/164*100=42%
P=(1)31=31/164*100=19%
O=(4)16=64/164*100=39%
69=31=64=164

Graphs:

IV. Conclusion:
1. Explain the difference between Mixtures and Compounds using data. Compare the pie

charts.
The difference between mixtures and compounds is compounds contain one or more element
that are combined chemically while mixtures are made up of 2 or more different substances that
are mixed but not combined chemically. Based on the information from the pie charts, it shows
that mixtures can have the same materials, however, the quantities are completely random.
With compounds like salt, the things they consist of,(elements) will always be the same with the
same quantities. For example, you will never have 2 bags of mixed candy with the same
amounts of candy and the same kinds of candy. However, to get the compound of salt, you
must always have the same elements and quantities. This shows with mixture A and mixture B.
Mixture A was made up of, 4% iron, 31% small rocks, 52% big rocks and 13% coarse sand. In
Mixture B, the materials it consisted of were the same, however their quantities were completely
different. In mixture B, instead of 4% iron there was 7%. Instead of 31% small rocks it had 15%
small rocks. Comparing these two mixtures to the compounds sodium phosphate and potassium
sulfate, we can see that the mixture quantities are completely random while compound
quantities are always one certain number. For example, in sodium phosphate, it is made up of
39% oxygen, 19% phosphorus and 42% sodium. Sodium phosphate will always consist of the
same elements as well have the same quantities of the elements. Also, in potassium sulfate, it

consisted of 37% oxygen, 18% sulfur and 45% potassium. Just like with the compound sodium
phosphate, it will always consist of these same elements as well as the same quantities of these
elements.

2. ​Explain how you separated the Salt from the Sand. Use as much new vocabulary as you
can.
First, we got a ring stand, coffee filters, 2 beakers, 1 small 1 large, a funnel, a hot plate and a
tray of fine sand. Next, we stuck the funnel inside the ring on the ring stand and put the coffee
filter inside of it. After this, we poured the fine sand inside of the coffee filter and added the
solvent onto it which was water.After we did this, we put the other beaker underneath the funnel
to catch the homogenous mixture we created. We then put it on the hot plate and heated it up
until it was boiling. After we let it boil for a few minutes, eventually all the water evaporated and
left us with just sodium chloride also known as salt at the bottom of the beaker..

Name: ____________________________ Class: _________
QUIZ:​ Solubility and Naming Compounds

Part I. Charge
Directions:​ Write the symbol of the element with the charge.

Formula

1. Sodium Na +2

2. Neon Ne +0

3. Nitrate No3 -1

4. Chlorine Cl -1

5. Magnesium Mg +2

6. Silver Ag +1

7. Sulfur S -2

8. Phosphorus P -3

9. Aluminum Al +3