Digital Scientific Notebook
Template:
Name:
Partner(s) Name:
Date (of Experiment):
Title:
Purpose:
Procedure:
Pre Lab Questions:
Data Table(s):
Data Tables and Observations:
Calculations and Graphs (on an “as needed” basis):
Conclusion:
- 1 to 3 sentances
Error Analysis:
Responses to Post Lab Questions & Challenge Extensions:
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Entry 1: Save Fred!
Name: Sol Manuel Garza
Partner(s) Name: Alaniz Enriquez
Date (of Experiment): 8/28/2014
Title: SAVE FRED!
Purpose: The purpose was to save Fred (a gummy worm) from the ocean (A blue sheet of paper), put him in his boat (a clear plastic cup) and put on his life vest (a gummy life saver) using the Fred handlers (paper clips). In addition, Fred cannot fall anywhere else: the table, the floor or on us.
Procedure:
- Partner 1 takes 2 of the paper clips and bends the outermost part to create two small handles.
- Partner 1 picks up Fred using the Fred handlers.
- Partner 2 takes 2 of the Fred handlers and bends one into a hook shape.
- Partner 2 flips the boat over.
- Partner 2 grabs the life preserver and, using the hooked Fred handler, picks up and stretches out the life preserver.
- Together, they fit Fred into his life preserver.
- Person 2 places Fred into his boat.
Pre Lab Questions:
1. Why is it important to follow an agreed upon procedure for a laboratory experiment?
Following the procedure prevents arguments between partners about how to do the experiment and stops partners from wasting materials. The procedure makes everything simpler, neater and easier to replicate.
2. Why is it important to document your procedure, errors you may have made, or differences in actual outcome vs. expected outcome?
It is important to document procedure so that the experiment can be duplicated by others. If we document an error that is made in the procedure, we can then fix it. It is important to document a different outcome than the expected outcome to disprove a theory or to realize that the procedure was wrong.
3. Why do we normally not have food in Chemistry class? (Be Specific)
We do not normally have food in the Chemistry classroom so that we do not accidentally mix food with the experiment and so we do not contaminate our food with chemicals.
Mixing food and chemicals can cause an unexpected chemical reaction that could be dangerous. Ingesting part of the experiment could cause us to be harmed or sick.
Data/Observations:
- Fred is slippery and will fall into the ocean if he is not held tightly by the Fred handlers.
- It requires team effort to get Fred into the life preserver. This is the most difficult part of the procedure.
Conclusion:
We developed an effective procedure that worked well the first time. Fred was successfully placed in his life preserver, and inside his boat the first attempt.
Error Analysis:
I dropped Fred into the ocean twice, on the second and third attempts. He was slipperier than I expected. Otherwise, everything worked.
Responses to Post Lab Questions & Challenge Extensions:
1. Was one of you more of a leader and the others followed, or did you share the responsibility equally? Why did it work that way?
Both of us contributed equally to the project. This was because both of us were enthusiastic and full of ideas. We were able to share our ideas in the designated time and cohesively devise a procedure. Simply because both of us too the lab seriously and were willing to work together, we both contributed equally.
2. What areas of expertise can you bring to a project? (What are you good at?)
I have done some labs in previous classes and am aware to some extent to how they usually work. I am enthusiastic and ready to work with my partner to do the lab. I am good at math and at recording data as well as enjoying being the person who puts on the gloves and handles the chemicals.
3. How do you feel about conducting laboratory experiments? (they won’t all be like saving Fred)
I am excited to see what experiments we will be conducting in class. I love the hands on aspect of chemistry.
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Entry 2: Flame Test Lab
Name: Sol Manuel Garza
Partner(s) Name: Alaniz Enriquez
Date (of Experiment): 9/25/2014
Title: Flame Test Lab
Purpose: To observe the characteristic colors produced by certain metallic ions when vaporized in a flame and to identify unknown metallic ions by means of this flame test.
Pre Lab Questions:
1. What color of light is the lowest in energy?
Red is the lowest visible color on the electromagnetic spectrum. It uses little energy and incidentally has big waves.
2. What color of light is the highest in energy?
Violet (purple) is the color which is highest in energy.
3. What color of light is the lowest frequency?
Red has the biggest waves, causing it to have the lowest frequency of visible light.
4. What color of light is the highest frequency?
Violet has the shortest waves and the highest frequency of visible light.
5. Explain "ground state".
The state in which all of the electrons are at the lowest possible energy level. This is as close to the nucleus as possible.
6. How are electrons exited?
Electrons are exited when they absorb a photon of light at just the right amount of energy to make it have a quantum jump. Another way is to give the atom energy from heat. When either of these happen electrons in one shell jump out to another shell with a higher energy level, where they use more energy.
7. What does it mean when electrons are exited?
It means an electron has been elevated out of the ground state to a higher energy electron shell. Soon after an electron gets excited, it loses its energy and releases photons of light. The energy released is directly proportional to a specific frequency, or color, of light.
8. In your words, write a short explanation of how an electron absorbs energy and re-emits it as light and why different elements have different spectra.
Atoms absorb energy, causing an electron to move to a higher energy electron shell. Then the electron falls back to it's ground state and releases light while doing so. The frequency of light released, which is perceived as color by the observer, is caused by the amount of energy it took to move the electron to that shell.
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Entry 3: Geography is Density
Significance summary:
This chapter states several pieces of data that are important to understanding the structure of the Periodic Table as well as explaining elements and the bonds they form.
First, the article describes certain rows of the periodic table and how the elements in those rows interact. The eighteenth row of the Periodic Table, the Noble Gases, are unchanging and do not interact with the other elements. Elements from the alkali and halogen columns, such as Sodium and Chlorine, often bond as a result of the characteristics of elements in those columns.
Next, the article talks about different kinds of bonding and the bonds that form between different elements. Every element looks for a different element to form bonds with. As a result, elements are usually not found alone in nature but rather bonded together. Electrons are essential to form bonds. Bonds are formed by elements either taking or giving up valence electrons from each other (Ionic Bonds) or sharing valence electrons (Covalent Bonds). "Electron behavior drives the Periodic Table" (p. 27)
Finally, the article talks about the parts of an atom, protons, neutrons and electrons. It is explained that neutrons and protons compose the nucleus of an element. Nuclei can be stable or unstable. Their stability depends on having equal numbers of protons and neutrons. Helium is a perfect example of a stable nucleus with 8 protons and 8 neutrons. Electrons rapidly and imperfectly orbit the nucleus and are significantly smaller than protons and neutrons.
Evidence and connection summary:
This chapter is full of important historical, places and people related to the discovery of elements, compounds and the creation of the Periodic Table.
Thousands of years ago, great philosophers such as Plato believed that everything was an imperfect version of an ideal form. (i.e. The perfect tree, the perfect fish, etc.) This is the first stab at the idea of elements.
In the late 1800's and throughout all the 1900's many important discoveries/advances were made in discovering elements. In 1911, Dutch german scientist cooled mercury with liquid helium to create a perfect conductor. In 1937 a Russian-Canadian team created a superfluid with pure helium that could scale walls. In 1970, a superacid was created using the metalloid Antimony that could eat through glass.
This article also talked about some prominent Chemists such as Gilbert Lewis, Maria Goeppert and her husband Lewis Mayor and their contributions to Chemistry.
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Entry 4: Periodic Trends in Reactivity
Sol Manuel Garza
Nate Bogdan
9/10/2014
Title: Periodic Trends in Reactivity
Purpose
To explore the reactivity trends of metals in groups and periods of the periodic table.
Pre Lab Questions
1.
Groups are the vertical columns in the Periodic Table. Periods are the horizontal rows in the Periodic Table. Families are specific groups in the Periodic Table that have similar traits.
2.
Metals are located to the left of the metalloid boundary.
3.
The Alkali Metals are the first metal family. The Alkaline Earth Metals are the second metal family.
4.
Aluminum is found in Group 3 and Period 3.
Procedures
Part 1, step 1: Gather your supplies and label your test tubes.
step 2: Get your samples from Charlene and put them in your test tubes.
step 3: Using a disposable pipette, add enough water to cover the sample.
step 4: Record data and observations in the table below.
Part 1: Trends in Properties Within Groups.
Metal Observations
- Reactivity in Water
Magnesium
- No observable change
- floats a little
Calcium
- Mixes with the water a bit, turning the solution a milky white color
- The majority of the calcium stays at the bottom and turns into a wet paste
Part 2: Activity Series of some metal in HCL
step 1: Obtain samples from Charlene and place them in labeled test tubes.
step 2: Obtain dropper bottle of HCL from Charlene
step 3: Add enough HCL to completely cover each sample
step 4: Record all data and observations in the table below.
Metal Observation
- Reaction in HCL
Magnesium
- Solution bubbles and fizzes
- makes smoke
- The magnesium dissolves completely
- After the magnesium dissolves a white, foamy solution results
Zinc
- Bubbles and fizzes on contact
- makes smoke
- The sink turns black
- the solution feels warm
Tin - the tin is unaffected
Post Lab Questions
1) What might be the reason for difference is behavior between magnesium and calcium when placed in water?
Calcium is a non-metal (even though it is on the left of the metalloid boundary), as opposed to magnesium, which is a metal through and through. Calcium was more absorbent than magnesium, especially as a powder. As a result the calcium powder mixed with the water, turning it milky white and turning the bulk of calcium into a wet paste. The magnesium was a solid strip that was a harder, denser metal that did not mix or react with the water in any sort of visible way. This was because it was solid, not a powder and a stronger metal.
2) List four metals from most reactive to least reactive. Use data from your lab to support your answer.
Magnesium is the most reactive of the metals because, when it is placed in hydrochloric acid (HCL) it completely dissolves and causes the solution to smoke, bubble and fizz for about 30 seconds.
Zinc is the second most reactive metal because it also makes the solution smoke, bubble and fizz. However, the zinc does not dissolve. However, it does turn black. The tin does not react in any way with the HCL in any way.
3) In general, is there a relationship between the locations of metals on the periodic table and their relative activity? Explain why?
Metals to the far left of the Periodic Table such as the Alkali metals are much more reactive than metals in the middle of the Periodic Table. This is because the Alkali metals have only one extra electron, which makes it it easy for those elements to form bonds with many other elements. However as you go more toward the middle of the periodic table the elements have more full electron shells, making it harder for them to react.
4) Silicon(Si), Tin(Sn) and lead(Pb) are all in the same group. The density of Tin is about 7.28 g/cm3 and the density of
The difference between Pb and Sn is about 4, the difference between Sn and Ge (Ge is in the same column) is a little under 2. It seems that the difference in density is half of the difference of the two elements below it. So the difference between Ge and Si is going to be about 1. For this reason I think the density of Si will be about 4.1.
Analysis Questions
1. The elements are less reactive the farther down you go down in a group. For example, Magnesium, an element in Period 3 dissolved in HCL. Zinc, in Period 4 only turned black in the solution. And Tin, an element in Period 5, had no visible reaction to HCL. Given this data, I can reasonably come to the conclusion that the more reactive elements are on top of the column.
2. Elements on the edges go a period tend to be the most reactive. For example, in Period 4 Potassium is on the far left, Iron is in the middle and Bromine is on the far right. Potassium is so reactive it violently reacts with water. Iron is very stable, and Bromine is a Halogen.
3. metals Order of reactivity (Most reactive to least reactive)
Fr, Na, Cs Na, Cr, Fr
Rb, Ga, Fr Rb, Ga, Fr
4. The most reactive metal in the periodic table is lithium. This is because is is the highest metal on the farthest left column. I was confused at first about whether the far right or the far left would be more reactive but then I realized that the far right column was the Noble Gases, a very un-reactive column. Since the halogens are only the second to farthest column, the Alkali metals must be slightly more reactive. For this reason I chose Lithium as the most reactive metal.
5. Yes, because Calcium was affected by water; Magnesium and zinc reacted with hydrochloric acid (HCL). The only metal that does not seem to fit in the chart is Tin. Tin did not visibly react with HCL in any way. However, it is possible that there was a reaction too small to be seen.
Name:
Partner(s) Name:
Date (of Experiment):
Title:
Purpose:
Procedure:
Pre Lab Questions:
Data Table(s):
Data Tables and Observations:
Calculations and Graphs (on an “as needed” basis):
Conclusion:
- 1 to 3 sentances
Error Analysis:
Responses to Post Lab Questions & Challenge Extensions:
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Entry 1: Save Fred!
Name: Sol Manuel Garza
Partner(s) Name: Alaniz Enriquez
Date (of Experiment): 8/28/2014
Title: SAVE FRED!
Purpose: The purpose was to save Fred (a gummy worm) from the ocean (A blue sheet of paper), put him in his boat (a clear plastic cup) and put on his life vest (a gummy life saver) using the Fred handlers (paper clips). In addition, Fred cannot fall anywhere else: the table, the floor or on us.
Procedure:
- Partner 1 takes 2 of the paper clips and bends the outermost part to create two small handles.
- Partner 1 picks up Fred using the Fred handlers.
- Partner 2 takes 2 of the Fred handlers and bends one into a hook shape.
- Partner 2 flips the boat over.
- Partner 2 grabs the life preserver and, using the hooked Fred handler, picks up and stretches out the life preserver.
- Together, they fit Fred into his life preserver.
- Person 2 places Fred into his boat.
Pre Lab Questions:
1. Why is it important to follow an agreed upon procedure for a laboratory experiment?
Following the procedure prevents arguments between partners about how to do the experiment and stops partners from wasting materials. The procedure makes everything simpler, neater and easier to replicate.
2. Why is it important to document your procedure, errors you may have made, or differences in actual outcome vs. expected outcome?
It is important to document procedure so that the experiment can be duplicated by others. If we document an error that is made in the procedure, we can then fix it. It is important to document a different outcome than the expected outcome to disprove a theory or to realize that the procedure was wrong.
3. Why do we normally not have food in Chemistry class? (Be Specific)
We do not normally have food in the Chemistry classroom so that we do not accidentally mix food with the experiment and so we do not contaminate our food with chemicals.
Mixing food and chemicals can cause an unexpected chemical reaction that could be dangerous. Ingesting part of the experiment could cause us to be harmed or sick.
Data/Observations:
- Fred is slippery and will fall into the ocean if he is not held tightly by the Fred handlers.
- It requires team effort to get Fred into the life preserver. This is the most difficult part of the procedure.
Conclusion:
We developed an effective procedure that worked well the first time. Fred was successfully placed in his life preserver, and inside his boat the first attempt.
Error Analysis:
I dropped Fred into the ocean twice, on the second and third attempts. He was slipperier than I expected. Otherwise, everything worked.
Responses to Post Lab Questions & Challenge Extensions:
1. Was one of you more of a leader and the others followed, or did you share the responsibility equally? Why did it work that way?
Both of us contributed equally to the project. This was because both of us were enthusiastic and full of ideas. We were able to share our ideas in the designated time and cohesively devise a procedure. Simply because both of us too the lab seriously and were willing to work together, we both contributed equally.
2. What areas of expertise can you bring to a project? (What are you good at?)
I have done some labs in previous classes and am aware to some extent to how they usually work. I am enthusiastic and ready to work with my partner to do the lab. I am good at math and at recording data as well as enjoying being the person who puts on the gloves and handles the chemicals.
3. How do you feel about conducting laboratory experiments? (they won’t all be like saving Fred)
I am excited to see what experiments we will be conducting in class. I love the hands on aspect of chemistry.
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Entry 2: Flame Test Lab
Name: Sol Manuel Garza
Partner(s) Name: Alaniz Enriquez
Date (of Experiment): 9/25/2014
Title: Flame Test Lab
Purpose: To observe the characteristic colors produced by certain metallic ions when vaporized in a flame and to identify unknown metallic ions by means of this flame test.
Pre Lab Questions:
1. What color of light is the lowest in energy?
Red is the lowest visible color on the electromagnetic spectrum. It uses little energy and incidentally has big waves.
2. What color of light is the highest in energy?
Violet (purple) is the color which is highest in energy.
3. What color of light is the lowest frequency?
Red has the biggest waves, causing it to have the lowest frequency of visible light.
4. What color of light is the highest frequency?
Violet has the shortest waves and the highest frequency of visible light.
5. Explain "ground state".
The state in which all of the electrons are at the lowest possible energy level. This is as close to the nucleus as possible.
6. How are electrons exited?
Electrons are exited when they absorb a photon of light at just the right amount of energy to make it have a quantum jump. Another way is to give the atom energy from heat. When either of these happen electrons in one shell jump out to another shell with a higher energy level, where they use more energy.
7. What does it mean when electrons are exited?
It means an electron has been elevated out of the ground state to a higher energy electron shell. Soon after an electron gets excited, it loses its energy and releases photons of light. The energy released is directly proportional to a specific frequency, or color, of light.
8. In your words, write a short explanation of how an electron absorbs energy and re-emits it as light and why different elements have different spectra.
Atoms absorb energy, causing an electron to move to a higher energy electron shell. Then the electron falls back to it's ground state and releases light while doing so. The frequency of light released, which is perceived as color by the observer, is caused by the amount of energy it took to move the electron to that shell.
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Entry 3: Geography is Density
Significance summary:
This chapter states several pieces of data that are important to understanding the structure of the Periodic Table as well as explaining elements and the bonds they form.
First, the article describes certain rows of the periodic table and how the elements in those rows interact. The eighteenth row of the Periodic Table, the Noble Gases, are unchanging and do not interact with the other elements. Elements from the alkali and halogen columns, such as Sodium and Chlorine, often bond as a result of the characteristics of elements in those columns.
Next, the article talks about different kinds of bonding and the bonds that form between different elements. Every element looks for a different element to form bonds with. As a result, elements are usually not found alone in nature but rather bonded together. Electrons are essential to form bonds. Bonds are formed by elements either taking or giving up valence electrons from each other (Ionic Bonds) or sharing valence electrons (Covalent Bonds). "Electron behavior drives the Periodic Table" (p. 27)
Finally, the article talks about the parts of an atom, protons, neutrons and electrons. It is explained that neutrons and protons compose the nucleus of an element. Nuclei can be stable or unstable. Their stability depends on having equal numbers of protons and neutrons. Helium is a perfect example of a stable nucleus with 8 protons and 8 neutrons. Electrons rapidly and imperfectly orbit the nucleus and are significantly smaller than protons and neutrons.
Evidence and connection summary:
This chapter is full of important historical, places and people related to the discovery of elements, compounds and the creation of the Periodic Table.
Thousands of years ago, great philosophers such as Plato believed that everything was an imperfect version of an ideal form. (i.e. The perfect tree, the perfect fish, etc.) This is the first stab at the idea of elements.
In the late 1800's and throughout all the 1900's many important discoveries/advances were made in discovering elements. In 1911, Dutch german scientist cooled mercury with liquid helium to create a perfect conductor. In 1937 a Russian-Canadian team created a superfluid with pure helium that could scale walls. In 1970, a superacid was created using the metalloid Antimony that could eat through glass.
This article also talked about some prominent Chemists such as Gilbert Lewis, Maria Goeppert and her husband Lewis Mayor and their contributions to Chemistry.
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Entry 4: Periodic Trends in Reactivity
Sol Manuel Garza
Nate Bogdan
9/10/2014
Title: Periodic Trends in Reactivity
Purpose
To explore the reactivity trends of metals in groups and periods of the periodic table.
Pre Lab Questions
1.
Groups are the vertical columns in the Periodic Table. Periods are the horizontal rows in the Periodic Table. Families are specific groups in the Periodic Table that have similar traits.
2.
Metals are located to the left of the metalloid boundary.
3.
The Alkali Metals are the first metal family. The Alkaline Earth Metals are the second metal family.
4.
Aluminum is found in Group 3 and Period 3.
Procedures
Part 1, step 1: Gather your supplies and label your test tubes.
step 2: Get your samples from Charlene and put them in your test tubes.
step 3: Using a disposable pipette, add enough water to cover the sample.
step 4: Record data and observations in the table below.
Part 1: Trends in Properties Within Groups.
Metal Observations
- Reactivity in Water
Magnesium
- No observable change
- floats a little
Calcium
- Mixes with the water a bit, turning the solution a milky white color
- The majority of the calcium stays at the bottom and turns into a wet paste
Part 2: Activity Series of some metal in HCL
step 1: Obtain samples from Charlene and place them in labeled test tubes.
step 2: Obtain dropper bottle of HCL from Charlene
step 3: Add enough HCL to completely cover each sample
step 4: Record all data and observations in the table below.
Metal Observation
- Reaction in HCL
Magnesium
- Solution bubbles and fizzes
- makes smoke
- The magnesium dissolves completely
- After the magnesium dissolves a white, foamy solution results
Zinc
- Bubbles and fizzes on contact
- makes smoke
- The sink turns black
- the solution feels warm
Tin - the tin is unaffected
Post Lab Questions
1) What might be the reason for difference is behavior between magnesium and calcium when placed in water?
Calcium is a non-metal (even though it is on the left of the metalloid boundary), as opposed to magnesium, which is a metal through and through. Calcium was more absorbent than magnesium, especially as a powder. As a result the calcium powder mixed with the water, turning it milky white and turning the bulk of calcium into a wet paste. The magnesium was a solid strip that was a harder, denser metal that did not mix or react with the water in any sort of visible way. This was because it was solid, not a powder and a stronger metal.
2) List four metals from most reactive to least reactive. Use data from your lab to support your answer.
Magnesium is the most reactive of the metals because, when it is placed in hydrochloric acid (HCL) it completely dissolves and causes the solution to smoke, bubble and fizz for about 30 seconds.
Zinc is the second most reactive metal because it also makes the solution smoke, bubble and fizz. However, the zinc does not dissolve. However, it does turn black. The tin does not react in any way with the HCL in any way.
3) In general, is there a relationship between the locations of metals on the periodic table and their relative activity? Explain why?
Metals to the far left of the Periodic Table such as the Alkali metals are much more reactive than metals in the middle of the Periodic Table. This is because the Alkali metals have only one extra electron, which makes it it easy for those elements to form bonds with many other elements. However as you go more toward the middle of the periodic table the elements have more full electron shells, making it harder for them to react.
4) Silicon(Si), Tin(Sn) and lead(Pb) are all in the same group. The density of Tin is about 7.28 g/cm3 and the density of
The difference between Pb and Sn is about 4, the difference between Sn and Ge (Ge is in the same column) is a little under 2. It seems that the difference in density is half of the difference of the two elements below it. So the difference between Ge and Si is going to be about 1. For this reason I think the density of Si will be about 4.1.
Analysis Questions
1. The elements are less reactive the farther down you go down in a group. For example, Magnesium, an element in Period 3 dissolved in HCL. Zinc, in Period 4 only turned black in the solution. And Tin, an element in Period 5, had no visible reaction to HCL. Given this data, I can reasonably come to the conclusion that the more reactive elements are on top of the column.
2. Elements on the edges go a period tend to be the most reactive. For example, in Period 4 Potassium is on the far left, Iron is in the middle and Bromine is on the far right. Potassium is so reactive it violently reacts with water. Iron is very stable, and Bromine is a Halogen.
3. metals Order of reactivity (Most reactive to least reactive)
Fr, Na, Cs Na, Cr, Fr
Rb, Ga, Fr Rb, Ga, Fr
4. The most reactive metal in the periodic table is lithium. This is because is is the highest metal on the farthest left column. I was confused at first about whether the far right or the far left would be more reactive but then I realized that the far right column was the Noble Gases, a very un-reactive column. Since the halogens are only the second to farthest column, the Alkali metals must be slightly more reactive. For this reason I chose Lithium as the most reactive metal.
5. Yes, because Calcium was affected by water; Magnesium and zinc reacted with hydrochloric acid (HCL). The only metal that does not seem to fit in the chart is Tin. Tin did not visibly react with HCL in any way. However, it is possible that there was a reaction too small to be seen.