Chem Blog Week 26

Chem Blog Week 25

Over the weekend we were given the task to make an electroscope. An electroscope is a device that is able to measure the amount of charge an object has.

How to Make it

An electroscope model closely replicated to my final product

After going through different prototypes of electroscopes this is the process I found to work best. Crumple a piece of foil into a ball. Roll the smaller piece of foil between your palms to form a long, thin rod shape. Now connect the foil ball to the end of the rod with a thin strip of foil. Make a hole in the middle of the jar lid with a hole punch. Be sure that the hole is large enough for the foil rod to fit through. Slide the rod through the hole in the lid, so the ball sits above the lid, outside the jar, when the top is screwed on. Bend the bottom of the rod so it makes a 90-degree angle. The angle should resemble an uppercase L. Make a narrow strip of foil and fold it in the middle. Fold up each end of the strip to make small flaps. Hang the folded strip of foil on the end of the rod where you formed the L shape. The strip should hang evenly on both sides. Screw the lid tightly on the jar, with the foil rod and flaps inside.

How it Works

When a charged body is brought near the metal knob, both strips acquire a like. As a result, they repel each other and spread apart to form an inverted V. Each dangling sheet of the foil will now have a charge, the two dangling halves of the foil will now seek to repel each other as they have the same charge. The electroscope is then charged. If an oppositely charged body is brought close to the knob, the charge on the strips is neutralized, and they again hang straight down. The strips of foil hang straight down when they are not charged. The charge will transfer to the metal foil. The degree to which the foil flattens itself out is a measure of the amount of charge on the foil which shows the amount of charge on the original object.

 The day of the testing went great. I thought my electroscope stopped working but it was just because the object I was using was harder to charge than something like vinyl. There were different types made but they were all mostly based off the same idea. I did have some trouble actually making the electroscope. My original idea using copper wire didn’t work out because I couldn’t find any copper wire, and even the substitute of a wire hanger for the antennae did not give any results. I did some more research and found the best model to get the best results. This week was fun with our project and I hope that we have another project soon!









Chem Blog Week 24

This week, we learned more about charges and how they work on a molecular basis. A positive charge is one with more positive ions than negative ions. A negative charge is the opposite. And now we know what a neutral charge is. A neutral charge is one with an equal number of positive and negative ions.

We were shown an experiment including a sweater and a balloon on the SMART Board. The sweater and the balloon initially didn't attract each other because they had neutral charges. But, that changed when the balloon was rubbed against the wall, it became more positive while the wall became negative. The negative ion moves. I then wondered why the negative ions were moved rather than the positive ions. Did it have to do with the greater electrostatic strength of positive ions than negative ions? Or was it because the opposite charges of positive ions and negative ions held each other in place? It seems as if though this is the case because I think that the positive ions are stronger than the negative ions. It seems as if though the negative ions have less strength because they have a greater number of electrons than the positive ions. The reason I think this is so is because I think that the less electrons there are, the less pressure is being put on the "electro-chain" that holds the electrons in place. So in summary the charge of positive ions is stronger than that of negative ions.   

This same principle also applies to ionic compounds, which form when ions transfer electrons to form neutral compounds. Through the exchange of electrons one of the elements become positive while the other one becomes negative. This is what happens when NaCl combine. The Na needed to lose an electron while the Cl needed to gain one. So, through this "electron exchange", the Na became positive and the Cl became negative. They then formed an ionic compound, which means a neutral compound.

In order to find element’s charge you look at the periodic table and based off what column that element is you will be able to know its charge. This brought back a memory freshmen year in honors biology when our teacher gave us a rhyme to help us remember the charge of elements: “+1, +2,+3,+4, (transitional metals) -3,-2,-1, no more!” With this, I am easily able to find charges for the elements.

This week went pretty well. I believe I understand the concepts we learned this week. I just need to practice with some of the equations with the elements. We were also given the assignment to make an electroscope for Monday. I’ve seen some videos on how to make one and it seems simple to make. But I need to further understand how it actually works.

 

Chem Blog Week 23

This week, I learned about atomic charges through a class demonstration. When a classmate rubbed the pen on his shirt, he then held it up to the match and the match moved–without any physical contact. I knew that the reason was because charge but I did not know how charges work a particle level. The first thing I learned was that a charge involves static electricity. We found that this from the flow of Electrons. Electrons are the smallest possible piece of an atom. This means that something is smaller than the atom. The exchange of electrons allowed the pen to have moved the paper clip without touching it. Because we now know that there is something smaller than the atom we have to change the way we draw particle diagrams to represent them at the smallest level. Particle diagrams in the past units could still be drawn the same using dots to represent particles.

Charges occur when the electrons transfer from one place to another. Depending on the charges, they could charge with other things. This is what I learned in the sticky tape lab. In this lab, we tested two pieces of tape: one tape taped onto another tape. The objective was to test the top tape and the bottom tape with other things to determine whether they would repel or attract. The top tape that was ripped off the bottom tape seemed to attract to the bottom tape. Next, the bottom tape was tested with the paper and the aluminum. The bottom tape attracted to the aluminum, but repelled the glass rod. Hence, the aluminum must be positive while the glass rod was negative. Through this example, I learned that opposite charges attract while the same charges repell

ed like a magnet would. This is because if the bottom tape and the top tape attracted together, they have opposite charges because when the top tape was ripped from the bottom tape, the top tape became positive while the bottom tape became negative. So, if the top tape is positive, then it would attract to something negative like the glass.

We also tested the conductivity of certain materials, like brass, silver, iron, zinc, copper, plastic, cardboard, and glass. The equipment we used included two battery sets, wire clips, and a light bulb. We found all the metal products were connected to the wires, the batteries, and the light bulb, the light bulb lit because the electrons flowed through the wires to the light bulb. The nonmetal products, however, did not conduct electricity because the light bulb did not light up.

Like I said in my last blog, this week was full of new things! I understand everything and it was easy to learn. We even had 3 experiments this week! I don’t know how next week will top it!

Chem Blog Week 22

This week, I learned more about the complexities of finding the number of moles. Also this week we had the MME/ACT testing so I was not in class for most of the week so this blog will be a short one. We practiced more with mole calculations and the concept and the mole but I am still a little shaky with how to find the number of particles or the number of moles or the mass.  It probably showed on the assessment we took online. I can describe what the mole represents and how it works in writing but the calculations mess me up. I am also able to find molar mass with the periodic table. This both connects with the electrolysis lab from last week and the things we learned earlier. Hopefully I will be ready before the reassessment because I tutor in chemistry and if I don’t have a grasp on the concept, neither will the person I tutor. I will ask my friends for some help about it.

Because this week was the ACT’s I will talk more about that than anything. I felt as if I was too calm compared to other people but I feel I did alright overall. I struggled on the science but I saw comfort that others also had some trouble with that subject as well. Even though my strongest subject is science. But it’s not really about your knowledge of science but your ability to understand graphs and charts and given information that was given. I’ll try to find something that would help me improve my test taking strategies. The other tests went well and the test went by quickly but when it was over I was exhausted!

Next week I am guessing that since we did not get to do much this week next week will be twice as busy. But I am okay it!

Chem Blog Week 21

This week in chemistry we learned the connection between molar mass and density that if you know molar mass you are able to determine the density of the the element. In the case of our electrolysis experiment, hydrogen and oxygen.

This week, my group and I did an electrolysis experiment. I was so excited because ever since we saw the process of electrolysis on the SMARTBoard I wanted to try it out for myself. We had to hook up two probes to two metals ends at the bottom of the trough. We had to fill the trough with sodium chloride water solution. But, why not water? This is the part I felt I wasn't so sure of, but I think it had to do with the fact that sodium chloride could conduct electricity in order for the hydrogen and oxygen particles to chemically split from each other.

Then we use two graduated cylinders (one for hydrogen and the other for oxygen) and put them on top of the metal ends making sure that they are still full. This was a little hard but we were able to do so in a few attempts .This reminded me of the experiment a while ago with the trough but I think this was a bit simpler because instead we had to scoop the tubes with the solution and slowly tilt them to the bottom of the trough, then tilt it again toward the metal end and cover it with the tube without going over the top of the tube. It felt like doing brain surgery with the amount of caution to flip over a test tube!

Then, after that ordeal was over with, we then cranked the machine and repeatedly turned the handle clockwise. We then kept track of the volumes for each of the tubes filled with the hydrogen and oxygen. Every time we recorded the data, there was twice as much volume of the hydrogen as there was oxygen.

We ended up finding out that compared to hydrogen oxygen is much denser even though hydrogen has twice as much volume. This adds up because we now know that the molar mass of oxygen is 16 g/mol and that hydrogen is only 1 g/mol.

This week was very fun because we did a group lab and that is one of my favorite aspects of chemistry and science in general: the experiments! With this experiment I was able to get a greater grasp of molar mass and of the fixed ratio of compounds. Feel confident with the concepts of this week hopefully I do this well next week. I am not sure what is to come next week but I trust that I won’t be disappointed with what I learn next!

Chem Blog Week 20

This week, we learned about the mole and it’s used in chemistry. In class, I did an experiment with my group. The goal was to compare the mass of 1 item to all the rest. The items were an empty bottle, small brown nails, hexnuts, pennies, screws, washers, bolts, and panel nails. To do the experiment, the first item we measured the mass of was the empty bottle. We found out it was 9.5g, and since all the elements had to stay in bottles, we subtracted 9.5g from all the rest of the total masses to find the masses of the small brown nails, hexnuts, pennies, screws, washers, bolts, and panel nails.

We had to choose one item to compare to all the other objects. Since the small brown nails had the least mass, we decided to compare it to the other items, and we found the ratios of their masses to the small brown nails. The picture above shows the data. The small brown nails had a mass of 1.3g, the hexnuts 18.9g, the pennies 11g, the screws 10g the washers 23.6g, the bolts 7.1g, and the panel nails 4g. The small nails to hexnuts were 1 to 14.5, small nails to panel nails were 1 to 5.46, the small nails to pennies were 1 to 8.3, the small nails to washers were 1 to 18.15, the small nails to screws were 1 to 7.69, and the small nails to bolts were 1 to 5.46. Therefore, I have concluded that small nails were the smallest, and the washers have the largest mass since the ratio between small nails and washers was the greatest.

I still felt unsure, though, on particles and how to count them. How can I represent them in a group? This question was then answered as I learned in class that for every mole, there are 6*10^23 particles. Thus, the word mole is the collective group of particles.

We found out that like this lab, this was how scientists found the atomic masses of the elements. They compared it to hydrogen, which has the smallest atomic mass, to all the rest. Also, the overall concept I learned from this was that there can be some way of calling 6 pieces of hardware to 1 collective group (e.g. 1 dozen=12 items). 1 dozen would be the collective group. So, we came up with a collective group name for the 6 hardware pieces: the Quinn. Therefore, proportionally speaking, for every Quinn, there are 6 hardware pieces and vice versa.

With this information we are able to plug in information like an algebraic equation and easily find an answer!

Overall this week feel okay with what I learned. I understand the concept, however, I am having a little trouble with the calculating of moles. I should be able to understand it with some practice.

Chem Blog Week 19

This week, our studies were mostly based off the following experiment of chemically mixing zinc and hydrogen chloride and finding its product and its volume so I wanted to describe the process of what we did thoroughly for full understanding.

In the experiment we used a known procedure to find the volume and type of the reactant. We were told to fill a bottle all the way with water while filling the trough with water. Then, mix the zinc and the hydrogen chloride together. But, we had to seal the beaker quickly so that the gas wouldn't escape. The gas goes through an opening inside the trough by a tube connecting the two. So, to collect the product, you should fill a bottle with water and tip it over right side using a lens to prevent spilling while removing the lens afterward. (I have become a pro at this art!) Then, combine the zinc and hydrogen chloride to react. When the glass bottle once filled with water is now full with gas we used the lens again to remove the bottle.

Now, with the gas in the bottle, my group and I can test its chemical properties to determine what the gas is. We previously learned that Hydrogen is flammable and oxygen is combustible. To determine if the gas had these properties, we lit a match to test for combustibility and flammability. Once we put the match in the container, the flame got brighter. Therefore, the gas was flammable. When the match got in contact with the gas, a popping sound was made. Therefore, the gas was combustible. We also had to find the density of the gas to help determine what it is. Subtract the mass of the beaker from the total mass. Then, find the volume of the gas by looking at the bottle. If there is any water in the bottle, this shows the amount of space it takes up. Then, you divide the mass of the reactant by the volume in which it took up the bottle to find the density.

To measure the zinc, we just put it on a measuring scale to calculate its mass. Then, to find out the mass of hydrogen chloride, I figured that in order to do so, we must find out the change in mass when comparing the beaker's mass to the mass of the beaker and the hydrogen chloride in it. Then, I subtracted the mass of the beaker with the total mass, therefore, to find the mass of hydrogen chloride.

By finding the masses of all these variables, we figured this would be the best way to find out the total mass after the zinc and the hydrogen chloride are chemically combined together is by adding the masses of hydrogen chloride and zinc before they were combined. I assumed that since hydrogen or chlorine would escape from the system, the mass would have to decrease. With these results, we concluded that since the gas was combustible and flammable, it had both oxygen and hydrogen. But we asked the question “Where did the zinc and the chloride go?” And how did the oxygen get into the bottle? We conclude that since the air has oxygen, and since it is diatomic, it combined with hydrogen to form water. It makes sense because the bottle had condensation in it.

With this experiment it should be easy to understand the lessons ahead and I am very excited about it!

Chem Blog Week 18

This week, We learned about the concepts of Dalton's theory.

 

On Monday, our class did a simulation on Dalton's theory in the computer game. The first part of the game (Priestley)  consisted of burning calx. As 7.39g of the 100g calx was burned, only 92.61g remained. We then had to use 200g of calx. With conservation of mass it would be understandable that the mass would be two times as much than the product from the first trial. The change in mass was 14.78g from the 200g calx. Therefore, depending on the mass of a substance burning, it loses mass at a proportional rate. We also had to find the volume of gas produced after burning the calx. I noticed that more mass was burned, the more volume the calx would be surrounded in. Using the 100g, the volume of gas came out to be 5.171L, and then using the 200g, the volume of gas came out to be 10.34L. So since there is only half of the mass of calx left, the volume doubled. Also, the volume of gas changed at a proportional rate to the rate at which the mass of calx changed. With this simulation, we learn that all chemical reactions occur in a fixed ratio.

The next experiment was the Lavoisier portion. This is where the phlogiston and the oxygen were tested at burned at different rates to see how they would change in mass or volume. First, 1/3 of the phlogiston was burned. To begin with, both started out with volumes of 6L and they were both in separate beakers , which had tubes connecting to a center beaker, which is where the gas would go. As the oxygen and phlogiston burned, 5L for both were left. Next, as 2/3 of the phlogiston were burned, 4 L for both oxygen and phlogiston were left. But then, when all the phlogiston was burned, only half of the phlogiston was used up so that 3L of oxygen were left. This would mean that the phlogiston burned quicker, two times to be exact. We were then later told that they renamed phlogiston to hydrogen simply meaning “water maker”.

 

Lastly, we worked on the Diamond and Charcoal lab. We started out with 0.20g of charcoal and diamond and kept the mass of oxygen at 1.06g and volume at 0.74L constant (charcoal and diamond were tested individually). The mass of the oxygen decreased from 1.06g to 0.73g as the subtracted amount went to the 0.20g of charcoal, thus increasing the mass of charcoal to 0.53g. Next, 0.40g of charcoal was tested with the same volume of gas (0.74L). Then, the mass of gas decreased from 1.06g to 0g and the volume dropped from 0.74L to 0L. Therefore, with twice the mass, the rate at which volume dropped doubled, hence the rate at which charcoal's mass increased. It was interesting to see that while charcoal and diamond look so different, they do still share chemical properties. I learned that they were related because of Jimmy Neutron! In conclusion, when something is taken away it is always somewhere else due to it being in a closed system and that chemical reactions occur at a fixed ratio.

We later on in the week focused on the things we learned in class on Monday and we had an assessment on Friday. I am not sure how I did, but I know I struggled in some areas that I missed that week.

Chem Blog Week 16/17

When I came back to school the class was talking about mixtures, compounds, and elements, how they were different and how they relate to each other. While I was behind a week I had some understanding of the concepts. When I was sick, I checked up on Google Drive an experiment the rest of the class did last week. It involved having to separate different materials from each other using different tactics of removal. The mixture of these materials is just that a mixture:  a group of matter that is physically combined. While a compound is chemically combined. I also found a worksheet that they did in class. It had particle diagrams that had different looking figures in each box. One showed one element combined to a different element and then another one with a different element but not combined. The top picture showed two elements in a substance not chemically bonded. I found out this is a mixture because the elements have still retained their physical properties, and as a result, they haven't changed. The bottom picture showed two different elements chemically combined together. Therefore, this is a compound because their properties have changed as they have formed a new substance. This week we did another separation but it was the separation of a compound: Pepsi. Mr. Abud told us to break up into teams so we could plan out and find information that would contribute to the process of separation. My table along with another tables did research on the ingredients of Pepsi which include high fructose corn syrup, sugar, dyes, and of course water. When we found out the ingredients the other groups were working on the distillation of the compound. When this was done we were asked to find the volume of the water.  Because we distilled the water all we had to do was measure it.  But I still questioned if we got all of the water because ingredients left still looked watery because I would think that what was left behind would have been a darker and thicker substance. But we ran out of time in class to find out if I was right.   While I was gone a week I was able to catch up with the class pretty quickly. I felt like I was talking and answering questions more than a lot of  the kids in class were.  When I came back I was also able to help my friends on past subjects and then they helped me on what I missed. However , I am still slightly behind on some of the things they studied while I was gone. Hopefully this does effect on how I do on the midterm. But thanks to Google drive I am not too behind.

Chem Blog Week 15

This week I along with my group formed a soap company with our self- made soap!

For this project, we were told that we were going to make soap and would have to present it as an actual company with company name, packaging, and a business card. We also had to make an Evernote presentation on our process in creating our soap along with information pertaining to the questions asked in the rubric. There are two ways of making soap that we talked about, mixing a fat base like coco butter or olive oil with lye or the melt and pour ,method using a soap base and melting it along with adding essential oils, dye, and a scent. Mr. Abud said that we will be using the melt and pour method because when using lye it is necessary to have more ventilation. He also recommended that we buy additional supplies like molds, packaging, special ingredients and soap bases.

A few days later we were ready to make our soap. I brought my group Chinese takeout boxes which were all decorated for the holidays to create a type of theme. I also brought plastic wrap for the soap so the bars could stay neat in the boxes. Everyone came into class excited and ready to work on their soaps. It was pretty entertaining see the entire class go into attack mode to get the best supplies Mr. Abud brought with him! When we all had our supplies we began to work. We started by dividing our soap base up into four parts for each person. We then melted ¼ of the base but I noticed that it was going very slowly so  conjured up the idea of cutting the base into smaller pieces to quicken the melting process. We then cut the cubes smaller and that really helped the base melt faster. We found that the melting point of our base was about 80 degrees and it took it a few minutes for it to completely dissolve into its liquid form. We were told that when melting the soap that we should be careful  of not boiling the soap base because it would mess up the following processes. When it melted we then added the essential oils and he the dyes and the poured the mixture into the molds.

The next day they were ready to take the soaps out of their molds and put them into their packages. We then later on had to show our presentations to the class. Our presentation had a good layout, great explanation, and an awesome logo edited by yours truly! We were able to answer all of the questions given by Mr. Abud thoroughly.  

I had a lot of fun with this project because I was able to practice my team work skills. I am the type of person who likes to work alone because I have had experiences with people not doing their part in the assignment. But also working by myself I do not have debate with decisions that need to be made. However, this project went fine teamwork wise but I wish we were more prepared and connected but overall it was great!

Chem Blog Week 14

This week, we learned more about energy, particle arrangement and particle motion.

I also learned about Heat of Vaporization and Heat of Fusion. Heat of Vaporization is the amount of energy that is required to convert a unit mass of a liquid into the vapor without a change in temperature. Heat of Vaporization occurs in state changes of liquid to gas and vice versa: (Vaporization) or (Condensation). Heat of Fusion is the amount of energy that is required to convert a unit mass of a solid into the liquid without a change in temperature. Heat of Fusion occurs in state changes of solid to liquid and vice versa: (Melting) or (Freezing).

We spoke more about solid, liquid and gas. We used water the most as an example. The states of water are very different not only because of their physical states but because of the attraction of their particles. Solid has stronger attraction between particles because the particles in a solid have the least amount of energy so the particles are closer together. It’s like a spring being pulled apart. It takes more energy to hold on to the ends of the spring when the spring is stretched. The same thing applies with the movement of particles. In a solid,  particles have strong attractions and move the least because there isn't enough energy to change the arrangement of particles. In a gas, the particles barely bump into each because they are farthest apart. The particles in a gas have the most amount of energy because it takes a higher amount of energy to separate the particles and make them move faster.

When physical states of substances change, this is because the attractions between the particles must be overcome in a solid to change to a liquid or gas (Eph). Just because the arrangement of particles changes, it doesn't mean that the motion of particles has changed. They could still move at the same rate (Eth). This is what Mr. Abud was saying about water  on the T-shirt if it evaporated. The state of the water changed from liquid to gas, but the temperature of the water couldn't have change because if it were at the boiling point (100ºC), it would be pretty noticeable to the person wearing the shirt! While the Eth did not increase the Eph did because the water turned from a liquid to a gas.

Therefore, a solid has the most orderly arrangement of particles and the lowest amount of energy as well as motion of particles. The liquid has the second most fluid arrangement of particles, meaning they move freely about but not as rapidly as gas particles. Thus, liquid is more structured than a gas and has less energy. Gas has the most amount of energy with the particles being the farthest apart with the least attraction. Thus, the distance between the particles and the attraction between them has an inverse relationship much like volume and density.

This week was pretty great because I got all 4’s and one 3 on my assessment! I was so excited and proud of myself and I was able to tutor some people this week for the reassessment next week. I’m glad that Christmas break is almost here so I can somewhat relax but I don’t think that will happen…

Chem Blog Week 13

This week, I learned about energy transfer through the three states of matter, and I learned about ETh and EPh.

 Eph is the energy transferred when a state of matter is changed. When a substance changes state from liquid to gas, the particles of gas are arranged even more freely and are spread out the most. So, if a solid changed to a liquid, there would be more phase energy because the arrangement of the particles is farther apart than that of a solid. So when you think about state changes think about phase energy.Eth is associated with temperature changes and the movement of particles. The increase of Eth means that the speed of the particles is more fluid and that the temperature is higher . To change the motion and speed of the particles, the amount of energy changes the attraction between the particles. If the particles have a weak attraction, then the particles will move faster, and if they have a strong attraction, then they will move slower. Thus, in a liquid, the particles of a liquid have a weak attraction since they are not closely together. In contrast, a solid has the strongest attraction between the particles since they are the closest together. A gas has the weakest attraction because the particles are the farthest together.

We also did an experiment to find the specific heat of copper. This week, my group and I had to come up with a procedure before we started. First, we had to measure the mass of the copper, then the water's mass, then, the temperature change of copper after putting it in water and the temperature change of water . This also included us to find the original temperature by looking at a graph of different metal colors depending on their temperature.  Then, I set the specific heat formula of water to the specific heat formula of copper equal to each other to figure out the specific heat (c) with E=mcΔT formula for both. Since the volume of water was 150 ml, and the density of water is 1g/ml, its mass was 150 g, the temperature change was 12.5ºC, and the specific heat is 4.18J/gºC. With the copper, the mass was 39.5 g, and its temperature change was around 480ºC. When we found our specific heat , all the other groups  compared and averaged them all out. However we found the actual measurement of specific heat wasn’t really close to our results!

This week was pretty easy. I understood all of the concepts and I really enjoyed doing the experiment with the copper. I learned that when doing an experiment like this one it is essential to pay attention to the directions and not to rush, if not it could skew the results and someone could be injured due to carelessness. While I still don’t have a computer these weekly blogs still help me remember the things I learned. Hopefully I will have it back soon, but writing them down still does the job!

 

Chem Blog Week 11

In this blog I will be talking about my experience of making my thermos!

We were assigned by Mr. Abud to make a thermos that would be able to hold a Styrofoam cup and to maintain the same temperature of water (or at least as close to the original temperature) as possible.

The Design

 

When planning out my thermos design I knew that it needed 1 thing: insulation. I then looked up materials that would be the best to insulate liquids. The main material was foam. I then looked up the construction methods of different types of thermoses. The ideal design was a vacuumed container with a reflective inside. I knew that I would have to make a vacuum but I didn’t know what to use. I needed something that would be able to take out as much air form in between the two containers as much as possible then my dad told me about expanding foam. With expanding foam you are able to spray the substance where you want it and then it will expand taking up all of the space in between. I then used aluminum foil for the inside container. While it is metal, the aluminum reflects not allowing energy escape the thermos. The containers I started were tin cans but found out that metal was a conductor and would make the water become cooler. I then found a different inner container but I wasn’t able to find a big enough outer container so I used the can I already had. But what I changed was that I “painted” the inside of the can with the spray foam to make it better insulated. I also found shiny house insulation with bubble wrap inside to wrap the inner and outer containers in before spraying the inside. I made a cap for the thermos with a Styrofoam circle and aluminum foil putting a hole for the thermometer. I then made a “hat” for my thermos for more lining with the same insulation putting a small cut at the top for the thermometer.  My motto was “when in doubt, spray foam” during that time and it worked wonders!

                                       The Test    

        The day of the testing was a day to remember. Everyone came to class with their thermoses and no one's looked the same. But most to all of the thermoses had styrofoam and aluminum foil included in their designs. For testing, everyone had to heat up their water to 80 degrees celsius and then we poured in our styrofoam cups then place it in our thermoses. We checked the temperature of the water every minute writing down its changes in temperature. When I began, I made the mistake of not having a hole for the thermometer. This lead to me to putting a hole in the bottome of the cup and having to continually take te top on and off to check the temperature making the water lose more energy than it should. Thankfully Mr. Abud counted that day as a practice day so we could improve our thermos designs. What I changed is that the top of my thermos had a slit at the top to insert the thermos. The next day we tested out thermoses and my new designed while being a simple change worked out perfectly. I only lost about 3 degrees from my water and I got the highest percentage in my class! 
It was fun creating the thermos and I can't wait for our next project.