Formula # of atoms in formula If the following amounts of solute are dissolved in 100
mL of water: Is the solution SATURATED OR
KI K=1 UNSATURATED
Ce(SO4 ) 3 I=1
NH4 Cl 120 grams dissolved at 0º C
Ce = 1 Unsaturated
S=3
O = 12 7.2 grams dissolved at 70º C
Saturated
N=1
H=4 11 grams dissolved at 46.7º C
Cl = 1 Unsaturated
Name: Brenna Gillotti
Class: S7
QUIZ: Solubility and Naming Compounds
Part I. Charge
Directions: Write the symbol of the element with the charge.
Formula
1. Sodium Na +1
2. Neon Ne
3. Nitrate NO 3- 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
10. Calcium Ca +2
Part II.
Directions: Write the name for the compounds:
11. Na3 P O4 Sodium Phosphate
12. Li2 ( SO4) Lithium Sulfate
13. (NH4 ) 2C O3 Ammonium Carbonate
14. MgCl2 Magnesium Chloride
15. Ca(NO3 )2 Calcium Nitrate
16. BeF2 Beryllium Fluoride
Part III.
Directions: Write the chemical formula for the following compounds (Use your ions):
17. Calcium carbonate
Ca+2 CO3 -2
CaCO3
18. Ammonium phosphate
NH4 -1 PO4-3
(NH4) 3 P O4
19. Magnesium hydroxide
Mg+ 2 OH- 1
MgOH2
20. Potassium sulfate
K+ 1 S O4 -2
K2SO4
Part IV.
Directions: Determine the Mass % of Oxygen in Al2 ( SO4) 3 or AgNO3
Atomic Mass: A l (27) S (32) O (16) Ag (108) N (14)
Al2 ( 27) = 54/342 = 15.8%
S3 (32) = 96/342 = 28.1%
O1 2 (16) = 192/342 = 56.1%
The mass percent of oxygen is 56.1%
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 beaker shown in the graph is above the line of solubility, which makes the solvent
supersaturated. The beaker currently has a temperature of 15℃ and has 70 grams of solvent at
the bottom of the beaker. There are two ways for the solvent to become saturated. One way is
to take away 45 grams of the solvent so there will be 25 grams of the solvent. However, another
way to make the solvent saturated is to heat up by 23℃ which will bring the heat up to 38℃. To
conclude, the supersaturated solvent can become saturated using two simple methods.
Law Conservation
of Mass
Chemistry Test
3. Identify the Independent Variable in the attached experiment.
Your Answer: T emperature
Incorrect
0 / 1 point(s)
4. In an experiment to determine if the popping of popcorn is
affected by the temperature at which it is stored, counting the
popped kernels is an example of a(an)___________.
Your Answer: Control
Correct
+1 / 1 point(s)
5. When gasoline is burned in an engine, ___________.
Your Answer: new substances are formed
Correct
+1 / 1 point(s)
6. Matter that has a definite shape and volume is called a _________.
Your Answer: solid
Correct
+1 / 1 point(s)
7. Matter that has a definite volume but no definite shape is a
_______________.
Your Answer: l iquid
Correct
+1 / 1 point(s)
8. Matter in which the particles are free to move in all directions until
they have spread evenly throughout their container is a
_____________.
Your Answer: g as
Incorrect
0 / 1 point(s)
9. The amount of energy needed to change material from a liquid to a
gas is the Heat of ____________.
Your Answer: fusion
Incorrect
0 / 1 point(s)
10. When two or more substances are combined so that each
substance maintains its own properties, the result is a(n) ____.
Your Answer: compound
Incorrect
0 / 1 point(s)
11. A solution that contains all of the solute it can normally hold at a
given temperature and is graphed ON the line is ____.
Your Answer: supersaturated
Incorrect
0 / 1 point(s)
12. Increasing the surface area of a solid ____.
Your Answer: s lows speed of dissolving
Correct
+1 / 1 point(s)
13. The maximum amount of a solute that can be dissolved in a
given amount of solvent is its ____.
Your Answer: s olubility
Correct
+1 / 1 point(s)
14. Water is sometimes referred to as the universal solvent because
____.
Your Answer: m any substances can dissolve in it
Correct
+1 / 1 point(s)
15. A chemical reaction in which the energy released is primarily in
the form of HEAT is __________.
Your Answer: exothermic
Correct
+1 / 1 point(s)
16. Numbers that precede symbols and formulas in a chemical
equation are called
Your Answer: c oefficients
Correct
+1 / 1 point(s)
17. According to the law of conservation of mass, if two atoms of
hydrogen are used as a reactant, how many atoms of hydrogen must
be part of the product?
Your Answer: 2
Correct
+1 / 1 point(s)
18. Physical or Chemical Change: Breaking a pencil
Your Answer: P hysical
Incorrect
0 / 1 point(s)
19. Physical or Chemical Change: Boiling water
Your Answer: C hemical
Correct
+1 / 1 point(s)
20. Physical or Chemical Change: Rust forming on a bicycle
Your Answer: Chemical
Correct
+1 / 1 point(s)
21. Physical or Chemical Change: Silver Hydroxide + Sodium
Chloride --> Silver Chloride and Sodium Hydroxide
Your Answer: Chemical
Correct
+1 / 1 point(s)
22. Physical or Chemical Change: Blowing air into a balloon
Your Answer: P hysical
Correct
+1 / 1 point(s)
23. Heterogeneous or Homogeneous: Salad
Your Answer: Heterogeneous
Incorrect
0 / 1 point(s)
24. Heterogeneous or Homogeneous: Rocks and sand with iron
Your Answer: H omogeneous
Correct
+1 / 1 point(s)
25. Heterogeneous or Homogeneous: salt water
Your Answer: Homogeneous
Incorrect
0 / 1 point(s)
26. Heterogeneous or Homogeneous: Air
Your Answer: H eterogeneous
Incorrect
0 / 1 point(s)
27. Heterogeneous or Homogeneous: Sugar water
Your Answer: H eterogeneous
Correct
+1 / 1 point(s)
28. Heterogeneous or Homogeneous: Potassium Chlorate dissolved
in Water
Your Answer: H omogeneous
Correct
+1 / 1 point(s)
29. Heterogeneous or Homogeneous: Chicken noodle soup
Your Answer: H eterogeneous
Correct
+1 / 1 point(s)
30. A solution contained 57 grams of sodium nitrate at 20 C. What is
the Solute in the solution?
Your Answer: s odium nitrate
Correct
+1 / 1 point(s)
31. A solution contained 120 grams of Potassium nitrate at 85 C.
What is the solvent?
Your Answer: water
Correct
+1 / 1 point(s)
32. A scientist wanted to find out if he/she could dissolve 110 grams
of Sodium nitrate at 80 C. Would his solution be Supersaturated,
saturated or unsaturated?
Your Answer: u nsaturated
Correct
+1 / 1 point(s)
33. A scientist wanted to find out if he/she could dissolve 110 grams
of Sodium nitrate at 80 C. How many grams would be added to make
this a saturated solution?
Your Answer: 33
Correct
+1 / 1 point(s)
34. Mr. Kotulski tried to make a solution with 90 grams of Potassium
nitrate at 40 C. Describe this solution:
Your Answer: S upersaturated
Correct
+1 / 1 point(s)
35. Mr. Kotulski tried to make a solution with 90 grams of Potassium
nitrate at 40 C. How many grams of Potassium (KNO3) could be
taken away?
Your Answer: 30
Correct
+1 / 1 point(s)
36. Mr. Kotulski tried to make a solution with 90 grams of Potassium
nitrate (KNO3) at 40 C. What Temperature would Mr. Kotulski have to
heat the water to in order to make it dissolve?
Your Answer: 5 5
Correct
+1 / 1 point(s)
37. What is the Mass% of Oxygen in the following compound: NaNO3
Your Answer: 5 7
Incorrect
0 / 1 point(s)
38. What is the Mass% of Oxygen in the following compound:
Lithium sulfate
Your Answer: 47
Correct
+1 / 1 point(s)
39. How much Heat Energy would be required to completely
evaporate 35 grams of Ice from its Melting Pt. completely to steam?
Your Answer: 25200
Correct
+1 / 1 point(s)
40. How much Heat Energy would be required to completely
evaporate 25 grams of Silver from its melting point?
Your Answer: 61260
Correct
+1 / 1 point(s)
41. What type of chemical reaction is shown in the following link:
Your Answer: S ingle Displacement
Correct
+1 / 1 point(s)
42. What type of chemical reaction is shown in the following link:
Your Answer: S ynthesis
Incorrect
0 / 1 point(s)
43. What type of chemical reaction is shown in the following link:
Your Answer: Decomposition
Correct
+1 / 1 point(s)
44. Analyze the following Data: What is the % of Large rocks in the
following mixture?
Your Answer: 52
Correct
+1 / 1 point(s)
45. What is different about the 2 Pie Charts? (Mixture and
Compound)
Your Answer: H eterogeneous all have different %s of materials while Compounds
have the same
Incorrect
0 / 1 point(s)
46. Analyze the following Solubility Graph: A mass of 80 g of KNO3
is dissolved in 100 g of water at 50 ºC. The solution is heated to 70ºC.
How many more grams of potassium nitrate must be added to make
the solution saturated?
Your Answer: 40 g
Correct
+1 / 1 point(s)
47. Analyze the Solubility Graph: What is the solubility of NaNO3 at
25°C?
Your Answer: 91 g
Incorrect
0 / 1 point(s)
48. Which Phase of Matter would occupy the LEAST volume?
Your Answer: g as
Incorrect
0 / 1 point(s)
49. Which Phase of Matter would occupy the GREATEST volume?
Your Answer: solid
Correct
+1 / 1 point(s)
50. Which of the following equations follows the Law of
Conservation of Mass?
Your Answer: D
Incorrect
0 / 1 point(s)
51. What are the correct Coefficients for the following chemical
reaction?
Your Answer: 1, 2, 2, 1
Correct
+1 / 1 point(s)
52. Use the Solubility Rules Chart to determine if CaSO4 is the
Soluble or Insoluble
Your Answer: I nsoluble
Incorrect
0 / 1 point(s)
53. Use the Solubility Rules Chart to determine if PbCO3 is Soluble
or Insoluble
Your Answer: Soluble
Correct
+1 / 1 point(s)
54. Use the Solubility Rules Chart to determine if Ag3PO4 is Soluble
or Insoluble
Your Answer: I nsoluble
Correct
+1 / 1 point(s)
55. Use the Solubility Rules Chart to determine if Sodium Nitrate is
Soluble or Insoluble
Your Answer: Soluble
Correct
+1 / 1 point(s)
56. The ability of some solids to change directly from a solid to a gas
is called ___________.
Your Answer: s ublimation
Correct
+1 / 1 point(s)
57. Name the following compound: Na2SO4
Your Answer: Sodium Sulfate
Correct
+1 / 1 point(s)
58. Name the following compound: CaCO3
Your Answer: Calcium Carbonate
Correct
+1 / 1 point(s)
59. Name the following compound: NH4NO3
Your Answer: Ammonium Nitrate
Correct
+1 / 1 point(s)
60. Name the following compound: Li3PO4
Your Answer: Lithium Phosphate
Correct
+1 / 1 point(s)
61. Write the formula for the following compound: Magnesium
hydroxide
Your Answer: Mg(OH)2
Correct
+1 / 1 point(s)
62. Write the formula for the following compound: Calcium
phosphate
Your Answer: C a3(PO4)2
Correct
+1 / 1 point(s)
63. Write the formula for the following compound: Ammonium
sulfate
Your Answer: ( NH4)2SO4
Correct
+1 / 1 point(s)
64. Write the formula for the following compound: Lead (II) Nitrate
Your Answer: P b(NO3)2
Incorrect
0 / 1 point(s)
65. A scientist wanted to find out the % of Oxygen from the reaction
between Lithium carbonate and Ammonium bromide. Predict the
products and balance the chemical reaction. Determine the % of
Oxygen by mass in the compound that contains Oxygen found in the
product. DO NOT WRITE THE % SYMBOL!
Your Answer: 46
Correct
+1 / 1 point(s)
66. A second scientist wanted to find out the % of Oxygen from the
reaction between Magnesium sulfate and Sodium chloride. Predict
the products and balance the chemical reaction. Determine the % of
Oxygen by mass in the compound that contains Oxygen found in the
product. DO NOT WRITE THE % SYMBOL!
Your Answer: 4 5
Correct
+1 / 1 point(s)
67. Symbol for Gold
Your Answer: Au
Correct
+1 / 1 point(s)
68. Symbol for Mercury
Your Answer: H g
Correct
+1 / 1 point(s)
69. Name the following compound: (NH4)2CO3
Your Answer: Ammonium Carbonate
Correct
+1 / 1 point(s)
70. Write the Chemical Formula for: Potassium Carbonate
Your Answer: K 2CO3
Correct
+1 / 1 point(s)
71. Write the Chemical Formula for: Magnesium Phosphate
Your Answer: Mg3(PO4)2
Incorrect
0 / 1 point(s)
72. Write the Chemical Formula for: Aluminum hydroxide
Your Answer: AlOH3
Incorrect
0 / 1 point(s)
73. How many Oxygen atoms in the following compound: Mg(NO3)2
Your Answer: 3
Incorrect
0 / 1 point(s)
74. How many Oxygen atoms in the following compound: Calcium
Phosphate Hint: (Don't forget to criss-cross!)
Your Answer: 4
Correct
+1 / 1 point(s)
75. How many Oxygen atoms in the following compound: Potassium
nitrate
Your Answer: 3
Atomic Structure/
Isotopes
Atomic Structure Project
Portfolio
Due: Friday 1/19/18
Directions: Construct a flipbook that covers the following categories related to Atomic Structure
and its relationship to the Periodic Table
Reading: https://www.livescience.com/37206-atom-definition.html
*Use this site for notes
1. Cover Page: Atomic Structure and Periodic Table
2. History of the Atom
● Atoms are the basic units of matter and the defining structure of elements
● Atoms were created 13.7 billion years ago
● Electrons were able to form once the extremely hot universe started to cool down
● Once the universe cooled, which took 380,000 years, conditions were suitable for quarks
to form as well
● Quarks are subatomic particles that come together to form neutrons and protons
● Hydrogen and helium were the earliest atoms to form
● John Dalton had discovered the idea of atoms while J.J Thomson discovered the
electron, Rutherford was the one who first thought that electrons orbit the nucleus and
Bohr discovered that the number of electrons orbiting the nucleus determines the
elements property
Link: https://www.youtube.com/watch?v=NSAgLvKOPLQ&t=490s
Link2:
a. Dalton- John Dalton came up with the theory of the atom in 1803. “John Dalton
was the first to recognize that the total pressure of a mixture of gases is the sum
of the contributions of the individual components of the mixture. By convention,
the part of the total pressure of a mixture that results from one component is
called the partial pressure of that component. Dalton's law of partial pressures
states that the total pressure of a mixture of gases is the sum of the partial
pressures of the various components.” Link to quote He discovered the basic
idea of the average atom.
b. Thomson - V ideo
● Thomson discovered the electron
● Found they were made of subatomic particles
● Used cathode ray tube (long glass like bottle) to pump air out and then have two pieces
of metal at one end
● Then connected a power source which created a ray to shoot through the metals and
created a glowing spot (electrons)
● He questioned if they had an electrical charge so put two plates, one positive and one
negative
● After doing so the ray was pulled towards the positive plate meaning it had a negative
charge
● Concludes: cathode rays must be made of stuff thats negatively charged; cathode rays
are 1,000 times smaller than a hydrogen atom; no matter the metal it’s always the same
= atoms have tiny negative particles in them (electrons)
c. Rutherford
● 1911 discovery of the nucleus during the gold foil experiment
● Started with a thin piece of gold foil which was shot at with alpha particles (which are
positive)
● Want to know what happens after they shoot the foil so they set up a material which
lights up after being hit with alpha particles
● Once they set up the foil in the circle of this material they see the flashes are mostly
behind the foil which suggest it goes through
● Then some are what it seems bouncing off the foil almost 180 degrees
● To conclude: most of the atom is empty space and that’s how it gets through; there is a
small center of these atoms which is making the particles bounce off; the center
(nucleus) is positively charged which could be for why the particles are bouncing off
because opposites don’t attract
D. Bohr
● Bohr knew that as it gives off radiation than the wavelength is going to vary and
are going to get this spectrum of electromagnetic radiations
● Rings which electrons are placed are energy level that grow the more electrons
and there are never any in the middle of these rings or energy levels
● Different types of wave series: lyman series - ultraviolet, paschen series - infrared,
balmer series - visible
3. Structure of the Atom
Video
Video2
● Nucleus - The Large membrane bounded organelle that contains the genetic material, in
the form of multiple linear DNA molecules organized into structures called chromosomes
● Protons - A positively charged elementary particle that is a fundamental constituent of all
atomic nuclei
● Neutrons - An atomic particle that has no electrical charge.
● Electrons - A stable subatomic particle with a charge of negative electricity, found in all
atoms and acting as the primary carrier of electricity in solids.
Atomic Mass
● The mass of an atom of a chemical element expressed in atomic mass units.
Charge
● A conserved property of certain subatomic particles that determines their
electromagnetic interaction
Valence Electrons
● An outer shell electron that is associated with an atom, and that can participate in
the formation of a chemical bond if the outer shell is not closed.
***Use models to explain the difference between:
● Sodium Chloride and M agnesium Chloride or S odium sulfide and C alcium Sulfide
Magnesium Chloride has two electrons to give away while Sodium Chloride only has one, So
Magnesium needs two Chlorides to get rid of the two unwanted electrons.
4. Isotopes
Definition: “Each of two or more forms of the same element that contain equal numbers of
protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic
mass but not in chemical properties; in particular, a radioactive form of an element.”
Link: https://phet.colorado.edu/en/simulation/isotopes-and-atomic-mass
a. Provide Example
b. How are they used by Scientists?
● Scientists use radioactive isotopes for purposes such as medicine as an
example. Cobalt-60 is often radiation source to arrest the development of cancer.
They also have the diagnostic purpose as being tracers for and as research
process of metabolism
● Isotopes in the nuclei have different stability levels, which measures in the speed
of decay that can help scientists with dating their archaeological findings.
Isotopes that are stable can be used to record a given climate change and are
also used for cancer treatment
5. Families of the Periodic Table
*Describe the life of Mendeleev and how he created the Periodic Table.
Russian chemist and inventor, Dmitri Ivanovich Mendeleev, had discovered the
classification of elements in 1869 and is known as the “father” of the periodic table. He
did have some empty gaps in the periodic table so he
was able to predict some of the elements that were
able to be filled within the spaces of the periodic table.
Mendeleev had made the periodic table in the order of
atomic and saw that some properties repeat
themselves but there aren’t any elements that have
noble gases so that left him with no empty slots to fill.
*What makes the elements the similar in each family?
c. Alkali Metals
● Aren’t free in nature
● Has 1 electron in its outer shell
● Malleable, ductile, good conductors of
heat and electricity
● Softer than most metals
d. Alkaline Earth Metals
● Second group on the periodic table
● +2 charge
● Very reactive
e. Halogens
● 7 electrons in its outer shell
● -1 charge
f. Noble Gases
● Stable
● Non-reactive
● 8 electrons in its outer shell
● 0 charge
*What are some trends in the Periodic Table?
One of some of the very common trends in the Periodic table is the ionization
energy. Ionization energy is the necessary quantity of energy to take away an electron
from the neutralized atom, which basically means its the necessary quantity of energy to
make a neutral atom into a positively charged ion. The amount of ionization energy
increases from left to right going across the Periodic Table. The first column has only 1
valence electron in each atom and because of that that electron can very easily be taken
away with a low ionization energy. However, the last column has the noble gases which
already have full valence shells and that means that they don’t need to lose any
electrons, giving it a high ionization energy amount. Ionization energy also decreases as
you go down the periodic table because each row adds one more orbital shell. The
electron cloud gets bigger as the rows go down. When there is less attraction to the
center, or the nucleus of the atom, less energy is needed to take away the electron,
which will give it a lower ionization energy amount.
Another common trend in the Periodic Table is the atomic radius. Atomic radius
is the length between the outermost ring of the electron cloud from the center of the
nucleus. Unlike the ionization energy, the atomic radius decreases from left to right
across the Periodic Table because as you go across the table, the amount of protons in
the nucleus increase. As the amount of protons in the nucleus increase, the amount of
electrons attracted to the nucleus increases. If the electrons are more attracted to the
nucleus, the closer they will get to it which will decrease the atomic radius. To add on,
the atomic radius increases as you go down the Periodic Table. Each level on the table
increases by one orbital shell. Each orbital shell will be farther away from the nucleus,
which increases the atomic radius.
6. Choose an article to read from site and summarize:
https://www.livescience.com/37206-atom-definition.html
While scientists have been working on fitting more protons into the nuclei to create
atoms with larger atomic numbers, some wonder if it’s possible to make an atom with no
protons? The chemist Andreas von Antropoff has done research with “Element Zero”, and has
been decided to be named as a neutronium. While there has not been a pure neutronium that
has been discovered or created yet, a similar substance has also been given the same name.
Neutronium is a gaseous substance found in
neutron stars, which are known as the densest
and smallest stars in existence. Neutron stars are
known for their density because they are almost
purely composed of neutrons clumped together
due to extreme gravity. Scientists are debating
about whether this neutronium truly fits the name
“Element Zero”.
Average Atomic Mass Worksheet
1. Rubidium has two common isotopes, 8 5Rb and 8 7Rb. If the abundance of 85R b is 72.2% and
the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?
85 * 0.722 = 61.37
87 * 0.278 = 24.186
61.37 + 24.186 = 85.556 amu
The average atomic mass of rubidium is about 85.556 amu.
2. Uranium has three common isotopes. If the abundance of 2 34U is 0.01%, the abundance of
235U is 0.71%, and the abundance of 238U is 99.28%, what is the average atomic mass of
uranium?
234 * 0.0001 = 0.0234
235 * 0.0071 = 1.6685
238 * 0.9928 = 236.2864
0.0234 + 1.6685 + 236.2864 = 237.9783 amu
The average atomic mass of uranium is about 237.9783 amu.
3. Titanium has five common isotopes: 46T i (8.0%), 4 7Ti (7.8%), 48Ti (73.4%), 4 9Ti (5.5%), 50Ti
(5.3%). What is the average atomic mass of titanium?
46 * 0.08 = 3.68
47 * 0.078 = 3.666
48 * 0.734 = 35.232
49 * 0.055 = 2.695
50 * 0.053 = 2.65
3.68 + 3.666 + 35.232 + 2.695 + 2.65 = 47.923 amu
The average atomic mass of titanium is about 47.923 amu.
4. Explain why atoms have different isotopes. In other words, how is it that helium can exist in
three different forms?
Atoms have different isotopes because there can be a different amount of neutrons in an
atom; the mass varies. Although the number of protons and electrons can’t necessarily
be changed in order for an atom to be considered an isotope, neutrons, for example, can.
Different isotopes are based off of the number of neutrons found. Helium can exist in
three different forms because of this. The only thing that’s different between each variety
is the number of neutrons found in the atom. Neutrons exist to stabilize the nucleus –
without them, the nucleus would consist of nothing but positively-charged protons in
close proximity to one another. Because there are different ways of stabilizing the
protons, there are different isotopes.
1. The term “average atomic mass” is a w eighted a verage, and so is calculated differently from
a “normal” average.
2. The element copper has naturally occurring isotopes with mass numbers of 63 and 65. The
relative abundance and atomic masses are 69.2% and 30.8% respectively. Calculate the
average atomic mass of copper.
63 * 0.692 = 43.596
65 * 0.308 = 20.02
43.596 + 20.02 = 63.616 amu
The average atomic mass of copper is about 63.616 amu.
3. Calculate the average atomic mass of sulfur if 95.00% of all sulfur isotopes are Sulfur-32,
0.76% are Sulfur-33 and 4.22% are Sulfur-34.
32 * 0.95 = 30.4
33 * 0.076 = 2.508
34 * 0.0422 = 1.4348
30.4 + 2.508 + 1.4348 = 34.3428 amu
The average atomic mass of sulfur is about 34.3428 amu.
4. The four isotopes of lead are shown below, each with its percent by mass abundance and the
composition of its nucleus. Using the following data, first calculate the approximate atomic mass
of each isotope. Then calculate the average atomic mass of lead.
82p 82p 82p 82p
122n 124n 125n 126n
1.37% 26.26% 20.82% 51.55%
Pb-204 Pb-206 Pb-207 Pb-208
204 * 0.0137 = 206 * 0.2626 = 207 * 0.2082 = 208 * 0.5155 =
2.7948 amu 54.0956 amu 43.0974 amu 107.224 amu
2 .7948 + 54.0956 + 43.0974 + 107.224 = 207.2118 amu
The average atomic mass of lead is about 207.2118 amu.
5. There are three isotopes of silicon. They have mass numbers of 28, 29 and 30. The average
atomic mass of silicon is 28.086amu. What does this say about the relative abundances of the
three isotopes?
Silicon-28 is the most abundant of the three isotopes because its weighted average is
closest to the atomic mass, 28.086 amu.
6. Calculate the average atomic mass of bromine. One isotope of bromine has an atomic mass
of 78.92amu and a relative abundance of 50.69%. The other major isotope of bromine has an
atomic mass of 80.92amu and a relative abundance of 49.31%.
Isotope #1:
78.92 * 0.5069 = 40.004548
Isotope #2:
80.92 * 0.4931 = 39.901652
40.004548 + 39.901652 = 79.9062 amu
The average atomic mass of bromine is about 79.9062 amu.
Activity: Determine which fossil is older
Directions: Watch videos, take notes and construct the graphs below using
your spreadsheet.
Film:
https://www.bing.com/videos/search?q=radiometric+dating&&view=detail&mid=0913F60FB719
BC591269 0913F60FB719BC591269&&FORM=VDRVRV
Film #2:
https://www.bing.com/videos/search?q=radiometric+dating&&view=detail&mid=33AAFAE1F005
C0E7E25833AAFAE1F005C0E7E258&&FORM=VDRVRV
Take notes:
● Fossils form when organisms are buried in sand and mud
● As layers of deposits build up, sediments are compressed into rock → organisms form
fossils within the rock
● The younger the rock, the higher it is in the rock layers
● The fossils in the rock layer are the same age as the rock itself
● The gradual breakdown of a radioactive substance in rocks is the “clock” that scientists
uses to measure geological time
○ Cenozoic Era
○ Mesozoic Era
○ Paleozoic Era
● Radioactive isotopes decay into different elements as they emit radiation (ex: Uranium
-238 → Lead-206
● “Half-life”: the time it takes for half of a given quantity of a radioactive isotope to decay
into another isotope
● An isotope with a shorter half-life would be better for calculating the age of a younger
rock
● Isotope with a shorter half life → decays more significantly in a shorter time
● “Radiometric Dating”: a method of determining the ages of fossils using radioactive
isotopes
Isotope #1 100
0 50
25
2300 12.5
4600 6.25
6900 3.125
9200 1.06
11,500 .5
13,800 .25
16,100 .125
18,400
20,700
23,000 0
Isotope #2 100
0 50
25
1500 12.5
3000 6.25
4500 3.125
6000 1.06
7500 .5
9000 .25
10,500 .125
12,000 0
13,500
15,000
Graphs:
Write an Essay that explains which fossil is older: (use your graphs)
Fossil A
18% of Fusarus remaining
6,000 years old.
Fossil B
35% of Montanosaurus remaining
2,200 years old.
As shown in the graphs, Fossil A seemed to be older than Fossil B. Representing Fossil
A was the “Fusarus” isotope, with 18% remaining. On the other hand, Fossil B represented the
“Montanosaurus” isotope, with 35% remaining. To begin with, the data shows that when
Fusarus was 18% decayed, it was approximately 6,000 years old. Different from the first
isotope, Fossil B, the Montanosaurus, would be about 2,200 years old considering that it was
35% decayed. Generally, the graphs show the rate of decay for both fossils. Likewise, as seen
in the data, it takes about 23,000 years for the Fusarus to be fully decayed (0% remaining),
whereas it takes only 15,000 years for Montanosaurus to reach its endpoint (0% remaining).
Clearly, this shows that Fossil A is older, due to the fact that it takes longer for it to decay
compared to Fossil B. Furthermore, after decaying 50%, the Fusarus would be approximately
2,300 years old. In contrast to the Fusarus, the Montanosaurus would be approximately 1,500
years old after decaying 50%. Therefore, as seen in the graphs and data tables, the Fusarus is
much older than the Montanosaurus, with an 800-year difference after both fossils have
decayed at least 50%.
QUIZ: Isotopes
Name: Brenna Gillotti Date: 2/6/18
Directions construct a graph that will help you determine the age of fossils.
Isotope A Percent Isotope
Years
0 100
5730 50
11,460 25
17,190 12.5
22,920 6.25
28,650 3.125
34,380 1.06
40,110 .5
45,840 .25
51,570 .125
57,300 0
Hint: Remember to add gridlines
Graph: ( place graph here:
Questions: (Use your graph above to answer the questions below)
1. How old is the following fossil?
Fossil A - 73% of Isotope A remaining
Fossil A is 5,730 years old.
2. How old is the following fossil?
Fossil B - 15% of Isotope A remaining
Fossil B is 17,190 years old.
3. What percentage of Isotope A is remaining if the fossil is 1200 years old?
(Use your graph)
The fossil that is 1200 years old has 95% left of decaying.
Average Atomic Mass Calculations
1. Naturally occurring chlorine that is put in pools is 75.53 percent 35Cl (mass = 34.969
amu) and 24.47 percent 37Cl (mass = 36.966 amu). Calculate the average atomic mass
of chlorine.
34.969 * 0.7553= 26.41
36.966 * 0.2447= 9.05
9.05 + 26.41 = 35.46 amu
2. Calculate the atomic mass of silicon. The three silicon isotopes have atomic masses and
relative abundances of 27.9769 amu (92.2297%), 28.9765 amu (4.6832%) and 29.9738
amu (3.0872%).
27.9769 * 0.922297= 25.80
28.9765 * 0.046832= 13.57
29.9730 * 0.030872= 0.925
25.80 + 13.57 +0.925 = 40.295 amu
‘
Writing:
Use one of the examples above to discuss how you determine the number of neutrons for each
isotope. You also need to discuss how the %abundance contributed to the Average Atomic
Mass of the element. (HINT: Think of the M&M Lab!)
The number of neutrons and protons in an isotope can be determined by the mass. The
atomic mass for the most common isotope of silicon is 28.0855. When finding out the number of
protons needed in the nucleus, the atomic number for silicon (14) is the number of protons
needed. The protons always stay the same in an isotope. However, the number of neutrons
change depending on the mass of the isotope. The number of neutrons is determined by the
mass of the atom subtracted by the number of protons. Also, the percent abundance contributes
to the atomic mass of the element because the percent abundance times the isotopes atomic
mass gives the overall average atomic mass. In the data shown above, the average atomic
mass has an atomic number and an atomic mass percent. The M&M lab is also like what has
been discussed because each M&M has a different mass and mass %, much like an isotope.
Isotopes also have different appearances, purposes, and masses from each other, like an M&M
has different appearances, flavors, and mass. In conclusion, the mass of an isotope contributes
to many different ways of what was discussed in the paragraph.
Velocity/
Acceleration
Velocity Story
Name: Brenna Gillotti Date: 2/12/18
Directions: Work in a group to tell a story of a classmate in motion. You must include 3 turns
(change in direction) and 3 different velocities. Your story must also have an amount of time
where the classmate does not move. What did the person do when they stopped? Where were
they going?
Data Table:
Example: Velocity = Distance/Time
V = 12 m/3 sec
V = 4 m/sec.
Description Distance (m) Time (sec.) Velocity (m/s)
4
Walked from Mr. Lopez’s room to 12 3
Leighas locker 0
4
Stopped 02
0
Walked from Leighas locker to my 40 10 4
locker
0
Stopped 02
Walked from my locker to Hidas 20 5
locker
Stopped 02
Graph: (X-axis is Time; y axis is Distance)
Story:
So after science class, Brenna decided to say hi to her acquaintance, Leigha! It
took her about 3 seconds to get from her science teachers classroom to Leigha’s locker
at a velocity of 4 m/s. She stopped at her locker for about 2 seconds at 0 m/s. After we
both said hi to each other, Brenna had to go to her locker to get her materials for the next
class and also chose to get some mint flavored chewing gum and it took her about 10
seconds to get from Leigha’s locker to Brenna’s locker at a velocity of 4 m/s. She
stopped to get her stuff which took her about 2 seconds at a velocity of 0 m/s.
Afterwards, she saw her friend, Hida, and decided to say hi to her as well. It was about a
5 second walk from Brenna’s locker to Hida’s locker at a velocity of 4 m/s. Brenna
stopped and talked to her for about 2 seconds at a velocity of 0 m/s, but Hida had to
leave after that, so Brenna had to go to her next class, realizing she forgot her pencil
somewhere. Looking at the ground, Brenna found her pencil on the floor in front of
Hida’s locker and went through the rest of her school day.
Velocity Project 2018
Due: Wednesday night February 21,2018
1. Define the following terms and include pictures if possible:
Motion Speed Position
“the action or process of “the rate at which someone “a place where someone or
moving or being moved.” or something is able to move something is located or has
or operate.” been put.”
Distance Acceleration Terminal Velocity
“an amount of space between “increase in the rate or speed “the constant speed that a
freely falling object eventually
two things or people.” of something.” reaches when the resistance
of the medium through which
it is falling prevents further
acceleration.”
Time Initial Velocity Displacement
“the indefinite continued “The initial velocity, is the “the moving of something
progress of existence and
events in the past, present, velocity of the object before from its place or position.”
and future regarded as a
whole.” acceleration causes a
change. After accelerating for
some amount of time, the
new velocity is the final
velocity”
Velocity Final Velocity Key Metric units
“the speed of something in a “The vector quantity velocity “A system of measurement in
given direction.” is the change in speed with which the basic units are the
respect to time. The meter, the second, and the
kinematic equations describe kilogram. In this system, the
the motion of object in terms ratios between units of
of constant velocity or a measurement are multiples
constant acceleration. ... The of ten.”
initial velocity is the velocity
at the starting point while the
final velocity is the velocity at
the final point of time.”
2. What is the difference between Speed and Velocity? Explain using an example
in your own words.
The difference between speed and velocity is that speed doesn’t have a direction, is
measured in distance divided by the time to get velocity. However, velocity is the speed
that is going in a specific direction and the velocity can be found from distance divided
by time.
3. Pick 2 cities (minimum 500 miles apart) in the United States or world and
construct a data table and graph showing the amount of hours that it would take
to travel between the 2 cities with the following modes of transportation: New
York to Paris
A. Fastest Runner
T= D/V
T=3625 mi/ 0.16 min
T= 22656.25 hours
B. Model T Ford
T= D/V
T= 3625 mi/45 mph
T= 81 hours
C. Hindenburg
T= D/V
T= 3625 mi/84 mph
T= 43 hours
D. Tesla top speed (155 mph)
T= D/V
T= 3625 mi/155 mph
T= 23 hours
E. Fastest train (267 mph)
T= D/V
T= 3625 mi/267 mph
T= 14 hours
F. F35 Fighter Jet (1200 mph)
T= D/V
T= 3625 mi/1200 mph
T= 3 hours
G. Vehicle of your choice (Toyota 86, 136 mph)
T= D/V
T= 3625 mi/136 mph
T= 27 hours
*Provide a map showing your cities
4. What would like to see in this city when you arrive? What tourist attraction?
What restaurant would you like to visit in this city? Provide pictures
What is the basic history of this city?
When I get to Paris there are many attractions I would like to see the many
beautiful attractions such as the Eiffel Tower,
Notre Dame Cathedral, and Disneyland Paris. I
would also like to visit many of the cafes and
shops that are there.
5. Determine and graph an 18% increase in
Velocity for each vehicle - Show how the
Times would be affected by the increase in
speed. Show a double bar graph with the 2
different times for each vehicle.
*Include pictures and brief description of each mode of transportation
H. Fastest Runner
T= D/V
T=3625 mi/ 0.16 min + 18%
T=3625 mi/ 0.1888 min
T= 1 9200.2 hours
I. Model T Ford
T= D/V
T= 3625 mi/45 mph + 18%
T= 3625 mi/ 53.1 mph
T= 68.26 hours
J. Hindenberg
T= D/V
T= 3625 mi/84 mph + 18%
T= 3625 mi/ 99.12 mph
T= 3 6.6 hours
K. Tesla top speed (155 mph)
T= D/V
T= 3625 mi/155 mph + 18%
T= 3625/ 182.9 mph
T= 19.8 hours
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Brenna Gillotti (Class of 2022) Blue Team Science Portfolio 2018
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