Tuesday, January 17, 2012

Activity 8 - Visualizing Chemistry

For activity 8, students have a choice to explore other topics of chemistry presented in the PhET simulations.



Let's Build Molecules! (created by Ashley Slinker)

You can find the simulation used for this activity at http://phet.colorado.edu/en/simulation/build-a-molecule.









































































Identify and meet three (3) science education standards.

A.4.1 When conducting science investigations, ask and answer questions that will help decide the general areas of science being addressed


B.4.1 Use encyclopedias, source books, texts, computers, teachers, parents, other adults, journals, popular press, and various other sources, to help answer science-related questions and plan investigations


C.4.8 Ask additional questions that might help focus or further an investigation

Monday, January 16, 2012

Activity 7 - Visualizing Chemistry

Complete the Teaching Idea “Concept Questions for Chemistry using PhET” posted by Trish Loeblein on the pH Scale simulation at PHET (http://phet.colorado.edu/en/simulation/ph-scale). On your blog post the answers with your scientific explanations from the “Clicker Questions pH Scale."


  1. b-false
  2. d-more than one
  3. c
  4. b
  5. d-more than one
  6. a-increase the pH
  7. b-decrease the pH
  8. a-ABC
  9. c-BAC
  10. a-something was added that made the equilibrium shift left


Complete the Teaching Idea “Intro to Strong and Weak Acids and Bases” posted by Chris Bires on the Acid-Base Solutions simulation.




















































Activity 6 - Visualizing Chemistry

Convert to Kelvin

0°F = 255.222 K
32°F = 273 K
70°F =  294.111 K
212°F = 373 K


Complete the Teaching Idea: States of Matter Simulation Lab by Kelly Vaughan. Complete the lab worksheet as if you were a student, and then post this on your blog. Take a picture of it.

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In the States of Matter simulation, choose the Solid, Liquid, and Gas Tab at the top of the screen. Choose the water molecule and cool the water to 0 K. Describe how the water molecules are aligned and attracted to each other. Which atoms are attracted to which other atoms?

Every water molecule in the simulation is touching another water molecule. The molecules stay connected to one another and move back and forth slowly. A water molecule is made up of two hydrogen atoms and one oxygen atom. The oxygen (negative charge) atoms are attracted to the hydrogen (positive charge) atoms of other molecules. The molecules arrange themselves when a positive charged hydrogen atom can attach to a negative charged oxygen atom. Therefore molecules arrange themselves based on their charges (opposites attract).

Switch to the Phase Changes Tab on the States of Matter simulation. Notice how on the bottom right there is a small red dot that indicates where the system is at as far as temperature, pressure and state of matter. Play with the simulation to notice changes, notice that when you push down the pressure can go way up and explode the box. On your blog, report a temperature and pressure required to make oxygen a liquid. This is sometimes how the oxygen exists in pressurized oxygen tanks, perhaps like ones you may use to go diving.

In order to make oxygen a liquid I increased the pressure to 51.18 ATM and this made the temperature of oxygen increase to 74 K.  I also (to make oxygen a liquid) increased the temperature of the oxygen to 385 K and this made the pressure increase to 12 ATM.


List and describe at least two Science Standards that this activity addresses.

A.4.3 When investigating a science-related problem, decide what data can be collected to determine the most useful explanations.


B.4.1 Use encyclopedias, source books, texts, computers, teachers, parents, other adults, journals, popular press, and various other sources, to help answer science-related questions and plan investigations.


D.4.3. Understand that substances can exist in different states - solid, liquid, gas.


D.4.4 Observe and describe changes in form, temperature, color, speed, and direction of objects and construct explanations for the changes.


D.4.5 Construct simple models of what is happening to materials and substances undergoing change, using simple instruments or tools to aid observations and collect data.

Wednesday, January 11, 2012

Activity 5 - Visualizing Chemistry

Run the Build an Atom simulation http://phet.colorado.edu/en/simulation/build-an-atom and build a neutral lithium atom and a neutral boron atom. List the number of protons, neutrons and electrons for each. Also look up and post the density for each of the elements on your blog.


Lithium


Protons: 3
Neutrons: 4
Electrons: 3
Density: .53 g/cm3



Boron


Protons: 5
Neutrons: 6
Electrons: 5
Density: 2.34 g/cm3


Define density and the equation for density and post on your blog.

Definition: The state or quality of being dense; compactness; closely set or a crowded condition (dictionary.com).
Equation:  Density = mass/volume


Run the Density simulation http://phet.colorado.edu/en/simulation/density and complete one(your choice) of the prepared Teaching Ideas and post your results on your blog. The activity you choose should be one of the student intended activities.


Relative Density: Sink or Float using Density Simulation
Author: Jackie Esler
Pre-Lab for Density Simulation

Name: Ashley Slinker

1. Will cube A sink or float in water? I think it will float because it is bigger than block B.


 2. Will cube B sink or float in water? I think it will sink because it is bigger than cube A.



3. Will C (a plastic hockey puck) sink or float? C will sink because it is made of plastic.


4. Will D (a metal hockey puck) sink or float? D will sink because it is made of metal.


5. You are given two solid gold bricks (Au). Which properties change from brink #1 to brick #2? The volume and density of the bricks will change.

 6. I love silver (Ag)! I won a contest and the prizewas a life-sized statue of my dog! I pick up my prize worth $6,000! On the way out, I start thinking that it isn’t very heavy for an object of this size made of solid silver. I know it is only a “prize” that I won, but I think it might be made of something other than valuable silver.


How could I find out for sure if this statue is made of solid silver? Find out how much it weighs and find the dollar value for that unit of weight and if it adds up to $6000 then it is silver. Find out silver properties. See if it sinks or floats.

 Complete the Mystery Blocks activity on the Density simulation. Post on your blog the data you collected (mass, volume, and density) and the identification of the material and the known density.


Block A:
Mass: 65.14 kg
Volume: 3.38 L
Denisty (M/V): 19.272 kg/L

Block B:
Mass: .64 kg
Volume: .64 L
Denisty: 1 kilograms/L


Block C:
Mass: 4.08 kg
Volume: 4.08 L
Denisty: 1 kg/L


Block D:
Mass: 3.10 kg
Volume: 3.10 L
Denisty: 1 kg/L


Block E:
Mass: 3.53 kg
Volume: 1 L
Denisty: 3.53 kg/L



Identify and post on your blog the Science Standards that could be met through these activities completed in Activity 5


A.4.1 When conducting science investigations, ask and answer questions that will help decide the general areas of science being addressed.

A.4.3 When investigating a science-related problem, decide what data can be collected to determine the most useful explanations

B.4.1 Use encyclopedias, source books, texts, computers, teachers, parents, other adults, journals, popular press, and various other sources, to help answer science-related questions and plan investigations.

C.4.3 Select multiple sources of information to help answer questions selected for classroom investigations.

C.4.4 Use simple science equipment safely and effectively, including rulers, balances, graduated cylinders, hand lenses, thermometers, and computers, to collect data relevant to questions and investigations.

C.4.5 Use data they have collected to develop explanations and answer questions generated by investigations.

C.4.7 Support their conclusions with logical arguments.

Tuesday, January 10, 2012

Activity 4 - Visualizing Chemistry

Standard A

A.4.1 When conducting science investigations, ask and answer questions that will help decide the general areas of science being addressed.

I remember doing experiments in my ninth grade chemistry class. We had to come up with questions that we could answer after the experiments were completed. I can’t remember the exact experiments that we conducted but I remember learning about the scientific method. We had to prove and write down the steps we took to complete the entire experiment just like we did in this class (Visualizing Chemistry 105) for the freezing and boiling experiments.



Standard B

B.4.3 Show how the major developments of scientific knowledge in the earth and space, life and environmental, and physical sciences have changed over time.

I specifically remember learning about the Big Bang Theory in junior high. My teacher showed us a video about the Big Bang Theory. This would meet the WI standard for earth and space.

In my ninth grade science class we learned of the different theories that explain why humans and animals occupy the earth. We learned about evolution and how people, animals, and the environment have changed over time.


Standard C

C.4.4 Use simple science equipment safely and effectively, including rulers, balances, graduated cylinders, hand lenses, thermometers, and computers, to collect data relevant to questions and investigations.

I took a botany course in college a couple of years ago and we looked at the cells of plants with a microscope. We looked a variety of plants cells and had to draw what we saw.

In my botany course we also conducted a “Leaf Disk Assay” experiment and in order to complete it, we used graduated cylinders, rulers, and computers to make charts and graphs.


Standard D

D.4.2 Group and/or classify objects and substances based on the properties of earth materials.

We met this standard in Visualizing Chemistry because we identified two elements that belonged to a different group of materials found on earth. We identified and explained how the periodic table is organized. I remember learning this in my high school chemistry class too, but I forgot exactly how the periodic table was organized. Once I reviewed it, the material became more familiar and what I learned in high school started to come back to me.


Standard E

E.4.1 Investigate that earth materials are composed of rocks and soils and correctly use the vocabulary for rocks, minerals, and soils during these investigations.

I took a geology course at UW-Eau Claire (fall 2011). During a lab activity, there were many different types of rocks set out on tables. We had had to identify the different properties of every rock, such as luster, hardness, and cleavage. By doing that, we could identify the name of each rock. I remember learning about the properties of rocks and minerals in my high school science class as well but it wasn’t as in depth as what I learned in my college geology course.


Standard F

F.4.2 Investigate* how organisms, especially plants, respond to both internal cues (the need for water) and external cues (changes in the environment).

In grade school (either 4th- 6th grade) we planted flowers in milk cartons. We measured the plants weekly and had the responsibility of watering and making the sure they received enough sun light. We learned the process of photosynthesis and the importance of different environments for different types of plants. I remember enjoying this activity. It was fun to watch the plant grow and see the progress of the growing stem, buds, and flowers.


Standard G

G.4.1 Identify* the technology used by someone employed in a job or position in Wisconsin and explain* how the technology helps.

I took the class Administration for Early Childhood Programs last fall and interviewed a manager of a child care facility in Green Bay, WI. One of the questions I asked was about the safety of children who attend the center. The manager said that technology has come a long way and has helped her center provide strong security for the children. The center uses security cameras that record 24 hours/7 days a week. Also, the center provides a security code system so only parents/guardians who know the code can enter or exit the building.


Standard H

H.4.1 Describe* how science and technology have helped, and in some cases hindered, progress in providing better food, more rapid information, quicker and safer transportation, and more effective health care.
Through my own observations and information learned in a variety of different courses I think that science and technology has helped improve health care by advancements in equipment used, such as lasers for eye surgeries.
Science has helped provide more efficient ways to produce foods. The FDA has created standards that must be met by all companies who sell food which allows consumers to feel safe about what they put into their bodies.
The internet has provided an abundance of information for people world wide.
Science and technology have truly made our lives easier but there seems to be a “dependence on technology” epidemic. Video games have decreased exercising amongst young children and teens and obesity rates have increased. Also, many young children, teens, and adults have more texting/phone conversations rather than real ones.
Science and technology do have negative results, but overall I believe that science and technology advancement has brought more positive results, especially within the health care industry.

Monday, January 9, 2012

Activity 3 - Visualizing Chemistry

Water: H20
IUPAC:Water Oxidane
















Carbon Monoxide
IUPAC: Carbon Monoxide





















Propane: C3H8
IUPAC: Propane





Post an image from the web, formula for 20 chemicals that you use or eat. Explore the ingredients of things like cosmetics and foods.







 IUPAC:  propane-1,2,3-triol
Common Name: Glycerol
Molecule Formula: C3H8O3








IUPAC: 1,2,3-Trinitroxypropane
Common Name: Nitroglycerin
Molecule Formula: C3H5N3O9








 IUPAC: Ethanol
Common Name: Ethanol
Molecule Formula: C2H6O












 IUPAC: 2-Hydroxybenzoic acid
Common Name: Salicylic acid
Molecule Formula: C7H6O3








IUPAC: Silicon dioxide
Common Name: Silica
Molecule Formula: O2Si










IUPAC: 4-chloro-N-(2,6-dimethylphenyl)-2-hydroxy-5-sulfamoylbenzamide
Common Name: Xipamide
Molecule Formula: C15H15CIN2O4S







IUPAC: 1,4-diaminobenzene
Common Name: p-Phenylenediamine (PPD)
Molecule Formula: C6H8N2














IUPAC: trihydroxidooxidophosphorus
phosphoric acid
Common Name: Phosphoric acid
Molecule Formula: H3PO4










IUPAC: 2-hydroxypropane-1,2,3-tricarboxylic acid
Common Name: Citric acid
Molecule Formula: C6H8O7












IUPAC: Sodium benzoate
Common Name: Sodium benzoate
Molecule Formula: NaC6H5CO2














IUPAC: Cyclohexanamine
Common Name: Cyclohexanamine
Molecule Formula: C6H13N








IUPAC: 1,3,7-trimethyl-1H-purine-2,6(3H,7H)-dione 3,7-dihydro-1,3,7-trimethyl-1H-purine-2,6-dione
Common Name: Caffeine
Molecule Formula: C8H10N4O2






IUPAC: Potassium (2E,4E)-hexa-2,4-dienoate
Common Name: Potassium sorbate
Molecule Formula: C6H7KO2






IUPAC: Nicotinic acid
Common Name: Niacin
Molecule Formula: C6NH5O2




IUPAC: 2-[3-[(4-Amino-2-methyl-pyrimidin-5-yl)methyl]-4-methyl-thiazol-5-yl] ethanol
Common Name: Thiamine
Molecule Formula: C12H17ClN4OS


 
 
 
 
 
 
IUPAC: Decamethyl-1,3,5,7,9,2,4,6,8,10-pentaoxapentasilecne
Common Name: Decamethylcyclopentasiloxane (D5)
Molecule Formula: C10H30O5Si5







IUPAC: poly(dimethylsiloxane)
Common Name: Polydimethylsiloxane (PDMS)
Molecule Formula: (C2H6OSi)n





IUPAC:(−)-(6aR,10aR)-6,6,9-trimethyl-
3-pentyl-6a,7,8,10a-tetrahydro-
6H-benzo[c]chromen-1-ol
Common Name: Tetrahydrocannabinol (THC)
Molecule Formula: C21H30O2






IUPAC: Hexane
Common Name: Hexane
Molecule Formula: C6H14



 
IUPAC: 4,4'-(propane-2,2-diyl)diphenol
Common Name: Bisphenol A (BPA)
Molecule Formula: C15H16O2





 

Look over your molecules and the bonding characteristics, how many bonds does each of the following elements typically have? Carbon? Hydrogen? Oxygen?

The lowest amount of bonds for carbon is 2 bonds and the highest amount of bonds for carbon is 21. However, most of the carbon bonds in my molecules are 3's and 6's.

The lowest amount of bonds for oxygen is 1 bond and the highest amount of bonds for oxygen is 7. However, most of the molecules contained 2 oxygen bonds.

The lowest amount of bonds for hydrogen is 3 bonds and the highest amount of bonds for hydrogen is 30. Hydrogen has the most irregular number of bonds compared to carbon and oxygen.


What does IUPAC stand for?
International Union of Pure and Applied Chemistry

As you explore ingredients, notice how everything around us is made up of chemicals consisting of atoms bound together into molecules. But what about companies that claim their products are chemical free! How can this be?
Of course there are going to be chemicals in the products that claim "chemical free." Companies use "chemical free" as a marketing tool. It is a way to sell the product. However, I believe when companies claim "chemical free" products it means that the products are safer for the enviroment, children, and pets. So if I were to buy "chemical free" products I would do it because I would like to have a more safe product rather than something harsh (like bleach). 

        

Saturday, January 7, 2012

Activity 2 - Visualizing Chemistry

Helium (He)


Atomic #: 2
Atomic mass: 4.002602 amu
Subatomic particles equal in number: 2 neutrons, 2 electrons, 2 protons

Hydrogen (H)

Atomic #: 1
Atomic mass: 1.00794 amu
Subatomic particles equal in number: 1 proton, 1 electron


Lithium

Atomic #: 3
Atomic mass: 6.941 amu
Subatomic particles equal in number: 3 protons, 3 electrons, 3 neutrons

How would you make an isotope for one of your models? What would change with the model?
Deuterium is a hydrogen isotope. A normal hydrogen atom has 1 electron and 1 proton. In order to make the deuterium isotope for hydrogen a neutron must be added. So the deuterium isotope would contain 1 neutron, 1 proton and 1 electron.

For one of your models, show with another image what happens when energy excites an electron.







Once the electron is excited, what do we typically observe when the electron returns to the ground-state?

When an electron is excited it goes to a higher energy levels state and when it returns to a lower energy state it emits a photon of energy. The photon may be observes as light.

Why are some elements different colors when they are excited?

Different elements emit different colors. The color of the excited elements depends on what the element is and what it is made up of. Different elements are used in fireworks to make them different colors.

Do a little research to list which elements are used to make the different colors of fireworks.

Aluminum is used to make silver and white flames and sparks. It is commonly found in sparklers.

Barium is used to create green colors. This element also helps stabilize other volatile elements found in fireworks.

Calcium salts are used to make orange fireworks. It also deepens other firework colors.

Antimony is used to create glitter effects.

Carbon is used to fuel fireworks.


Copper is used to produce blue colors.

Lithium is used to make a red color. Lithium is commonly used as a colorant in many fireworks.

Magnesium creates a very bright white color in fireworks.


 
Explain the overall organizational structure of the periodic table.

The periodic table is arranged so elements with similar properties are grouped near each other. The far left side of the periodic table is the alkali metals group (the top left is where the first atomic number starts) and the far right side of the periodic table is the noble gas group (the bottom right is where the last atomic number is located). Each element within the table has its own atomic number (number of protons in the nucleus) and its own mass number (the sum of protons and neutrons within the nucleus). The atomic number is listed across (horizontally-left to right) the table.


List two example elements for each of these groups or classes:

Alkali Metals: Potassium & Sodium

Alkaline Earth: Magnesium & Calcium

Halogens: Chlorine & Iodine

Noble Gases: Neon & Argon


Transition Metals: Nickel & Copper

Non-Metals: Sulfur & Carbon

Metalloids: Silicone & Arsenic


Considering the overall volume of your element models, what makes up most of the volume of an atom?

It seems as though empty space takes up the most volume. However, if I must name a subatomic particle that takes up the most volume it would be electrons. Electrons spread out while the protons and neutrons are closer to each other.

Thursday, January 5, 2012

Activity 1 - Visualizing Chemistry

My Hypothesis

1. Does hot water or cold water freeze faster?


I think that cold water will freeze faster because it is colder than hot water which means that is closer to the freezing point. The hot water will need to cool before it can start to freeze which would make it freeze slower.

2. Does hot water or cold water boil faster?


I think that hot water will boil faster because it is closer to the boiling point than cold water. The cold water would need to warm up first before it can boil which would make it boil slower.

3. Does salt water freeze faster or slower than regular water?


I think that salt water will freeze slower than regular water. I think this will happen because salt is used to melt snow so (to me) it makes sense that salt water would freeze slower than regular water. 

Pictures of My Experimental Materials and Setup



















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The ice tray labeled “cold” has formed ice on top of the cubes (at 70 minutes). The cold water freezes first. The hot water began to form ice on the top of the cubes but there was still open water on the top of the cubes.
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The glass labeled “regular” has formed ice on top of the water (at 90 minutes). The “regular” water freezes first. The salt water has formed a tiny bit of crystals on the side of the glass.

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The hot water boiled in 2.10 minutes. 



















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The cold water boiled in 3.09 minutes.

Data in the Form of a Table


Hot Water (1 ½ cups) Freeze Time
Cold Water (1/2 cups) Freeze Time
95 minutes (layer of ice on top cubes)70 minutes (layer of ice on cubes)



Salt Water (1/2 cup of room temperature) Freeze Time
Regular Water (1/2 cup room temperature) Freeze Time
At 90 minutes ice/salt crystals began to form on the sides of glass90 minutes (layer of ice on cubes)



Cold Water (2 cups) Boil TimeHot Water (2 cups) Boil Time
3 minutes and .09 seconds2 minutes and 10 seconds



Data of Experiment Repeated


Hot Water (1 ½ cups) Freeze Time
Cold Water (1/2 cups) Freeze Time
100 minutes (layer of ice on top of cubes)70 minutes (layer of ice on top of cubes)



Salt Water (1/2 cup of room temperature) Freeze Time
Regular Water (1/2 cup room temperature) Freeze Time
At 90 minutes ice/salt crystals began to form on the sides of glass 90 minutes (layer of ice on top)



Cold Water (2 cups) Boil TimeHot Water (2 cups) Boil Time
3 minutes and 5 seconds2 minutes and 18 seconds




List Of My Controlled Variables from My Experiment


·     2 ice cube trays (same kind)
·    Same amount of water for hot water and cold water (1 ½ cups poured in each ice cube tray)
·    Recorded the freeze time for salt, hot, and cold water when a layer of ice formed on the top of the cubes and in the glasses (cubes and glasses were not entirely solid when recorded)
·    2 of the same glasses
·    Same amount of water for salt water and regular water (1/2 cup of room temperature water for each glass)
·    Same pot for water to boil in (room temperature water) (waited for pot to cool again before testing the next 2 cups of water)
·    Temperature of stove was the same for both cold and hot water (set on high heat)
·    Same amount of water for the hot and cold water that was to be boiled (2 cups of hot water and 2 cups of water for cold water)
·    Recorded the boil point time when both the cold and hot water started to bubble


My theory that Answers the Questions Posed


After conducting the three experiments twice, I have come to three conclusions.


First, I have found that cold water freezes faster than hot water. The cold water is at a colder temperature than the hot water therefore it is able to freeze faster. Hot water must cool down first before it can start the freezing process.


Second, I found that regular water freezes faster salt water. In fact salt water takes a very long time to freeze because it slows down the process. The salt interferes with the freezing process because salt makes the water more dense than regular water.
Third, I found that hot water boils faster than cold water. This is similar to my first conclusion, except the opposite. Since hot water is closer to the boiling point it boils faster. The cold water must heat up first therefore it takes longer for cold water to boil.


***In my apartment, I don’t think that my water heater is regulated. My tap water gets unbelievably hot which is why I believe my hot water boiled so fast. So my hot water may be hotter than the average person’s tap water. I have burned my hands many times and if I had children I would be calling my landlord!


Image of the Atoms that Make up Water Molecules


















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A water molecule is made up of 2 hydrogen (H) atoms and 1 oxygen (O) atom that are bonded together.
















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Water molecules are attracted to other water molecules like shown in the picture above.

Video of how Water Molecules are Arranged (3 States of Matter)

·         Click on the link below (or copy and paste link) to view video:



Scientific Method/Process and how Each Step Correlates to My Experiments

1.     Ask a Question
The questions I asked were as follows:
                    1. Does hot water or cold water freeze faster?
2. Does hot water or cold water boil faster?
3. Does salt water freeze faster or slower than regular water?

When coming up with questions it is important that the questions are measureable so a conclusion can be made.

2.    Conduct Background Research
I looked up the questions on the internet before conduction the experiment myself and found that most of the websites believe that cold water freezes faster, hot water boils faster, and regular water freezes faster. However, there were a few websites that explained these conclusions can be controversial. For example, there is a possibility that hot water can freeze faster than cold water depending on the variables within the experiment.
It is important to do research so you know what to expect and do not conduct an experiment that will not work.
3.    Conduct a Hypothesis
I predicted that hot water would boil faster than cold water, cold water would freeze faster than hot water, and regular water would freeze faster than salt water. After conducting the experiments I found that my hypothesis was correct.
It is important to state a hypothesis in a way that can be measured. The hypothesis should be constructed in a way that will answer the original question.

4.    Experiment to Find Answers
By experimenting you can test whether your hypothesis if false or true. You want to be sure that there are controlled variables like the ones I have posted above.
It is important to repeat an experiment at least twice in order to be sure you made no mistakes in the first experiment. When I conducted my experiment a second time, I found that the freezing times and boiling times were pretty much the same which assures me that I made no major mistakes while experimenting.
5.    Come to a Conclusion
After you have completed the experiment you want to review all of your data and develop a theory.  I developed three theories after conducting my experiments.
First, I have found that cold water freezes faster than hot water.

Second, I found that regular water freezes faster salt water.

Third, I found that hot water boils faster than cold water.