11.1

1.)

a) the wrapped penny was less corroded than the unwrapped penny

b) the protection cam from both the coating and sacrificial techniques because it was coated with steel wool and it was protected by the other penny.

c)  Copper isn't very reactive but iron can be oxidized but this prevents further oxidation because copper can't be oxidized.

2.)   These areas started to corrode because aluminum is higher on table J than iron

3.)    This could have been prevented if the spots were sealed with caulking because it uses the technique of "sacrifice"

4.)

a)  Corrosion is the breaking down of a metal and it is caused by the loss of valence electrons in an element over time.

b) A chemist can outsmart corrosion by coating the metal they need with another metal or the process of "sacrifice" 

11.2

1.)

a)  I think think this name is appropriate because it really doesn't do anything to help the reaction it just watches the other elements try to react.

b) Silver is oxidized and magnesium was reduced

2.)    They will react only if element y is higher on table j than table x

3.)

a.) An activity series is the ability of an element to lose electrons

b) This is able to predict that metals will be high on table j and non-metals will be low on table J

4.)

Gold and the other 4 elements were found pure because they aren't very reactive and if they don't react with anything they are found pure.

5.)   Copper and Tin were melted together to form bronze

10.2

Our graph was similar to the one on table G but, Our amount of solvent was 10% of the amount of solvent used in Table G. That affected or graph a lot because the values were totally different and there was less solute.

The temperature can have a huge impact on how quickly the KClO3 dissolved. Surface area can also affect how quickly something dissolves. When you raise the temperature the collisions of the molecules become a lot more effective. Surface area relates to how quick the KClO3 dissolves because the more space it takes up the longer it'll take to dissolve. Particle collisions make the KClO3 react which makes it dissolve and that's why it's important to the dissolving process.

Unsaturated:  When the KClO3 was undissovled at the bottom of the test tube

Saturated:      When the KClO3 is completely dissolved in the test tube

Supersaturated:  Never

10.1

In my experiment I discovered that sugar and salt were polar. The sample of vegetable oil was non-polar. From the data I collected I can say that ethanol's polarity was polar. Ethanol could dissolve in water since water is polar. Hexane would not dissolve in water because it is non-polar and water is polar. NH3 is a non-polar molecule and is would dissolve in hexane but not water. I2 is polar and it would dissolve in water but not hexane. HCl is polar and it would dissolve in water but not hexane. Ionic molecules dissolve in water because it is polar and their polarity is stronger compared to non-polar molecules.

9.2

  Station one:

When the HCl was added it shifted to the right because it added to the Cl-1 and that stressed the reaction on the products side of the equation 

1.) When the system was heated it shifted to the right and that means that the "heat energy" was on the products side of the equation

2.) If the potential energy of the products is more than the reactants then the heat of reaction will be positive and the reaction will be endothermic. If the potential energy of the products is less than the reactants that means that the heat of reaction will be negative and that means that the reaction is exothermic.


3.)
a)  Table F shows that the interaction between Ag 1+ and Cl 1- is insoluble

b) I know that when i added AgNO3 to the solution the reaction from table F occurred because the two elements mixed and there was no separation.

c) When AgNO3 was added the system shifted to the left because the reaction was trying to reach equilibrium by shifting back to the left when it was already shifted to the right.

Station 3 Processing Question

1.) When the bottle was opened the pressure shifts to the right side of the system and the system does that so that it can reach equilibrium.

9.1

My solution process was endothermic. I know this because the temperature of the solution was 14.4 degrees higher than the original temperature of the water. When the element was added to the water the heat transferred from the surroundings of the water into the water.

One thing that could cause different values is measurement. If you used too much or too little of a substance then it could have caused our values to vary. Another way would be that they used pure water in their calculations but the tap water has iron in it.

3.)  
a)  If the temperature of the room was 10 degrees colder there would be less moles of solute because the colder it is the slower the reaction happens

b) If you added less chemical but knew how much you added the moles of solute would be greater because there's less chemical but the reaction happens fast because there's less chemical to dissolve

c) If you added 40 mL of water but thought you added 50 mL you would have less moles of solute because there's less water for the chemical to be dissolved in

8.2

The higher the viscosity the stronger the intermolecular forces and the higher the boiling point the stronger the intermolecular forces. The smaller the molecule the stronger the intermolecular forces

8.1

During this experiment the results varied because groups chewed the gum for different amounts of time. I chewed mine for 15 minutes and the percent error was close to zero because of it. Errors in calculations and measurements were a problem for me too but those were easily corrected.

7.4

Elements in the same group are more similar in their properties than elements in the same period. This is because these elements have the same # of valence electrons and their oxidation states are similar.

Elements in the same group tend to have similar properties because they have similar electron configurations but they have the same # of valence electrons.

K, Li, and Na have similar properties because they all react with air fast, they react with water fast as well.

When an atom of sodium reacts with a non-metal it tends to:

• Lose electrons
• Become a positive ion
• The electrical charge of the ion becomes +1
• Have an electron configuration of the element Neon
• Be more stable because the valence electrons are closer to the nucleus

  

7.3

The Heaviest elements have the smallest radii because as protons increase it brings the shells tighter.

Electronegativity decreases as you move down a group because there are more shells and the electrons are further away from the nucleus so it weakens the attraction.

It's easier to strip an electron from a non metal than from a metal because non metals like to gain electrons and metals like to lose electrons so it make sense that it would be harder to strip an electron from a non metal than a metal.

I think these trends are referred to as periodic because they are ongoing

7.1

Conclusion

1.) & 2.)  An element's spectrum is just like a fingerprint because each element's spectrum is unique. Each element has a unique elctron configuration which makes each spectrum different. When electrons enter the excited state they absorb energy which gives off light and that produces the spectrum. When the electrons return to the ground state energy is released. The spectrum goes away because there's no more energy left

Lab 4.1

1. A decrease in pressure causes the volume of a balloon to           Increase

                                                                                                  (increase, decrease or stay the same?)

As pressure decreases the volume rises. Such as the syringe example, when you put more pressure on it the volume decreases and when there's less pressure the volume increases

2. Adding more gas to a bottle ___________Increases_________ the pressure in that bottle.

                                                       (increases or decreases?)

As you add more gas that leaves less space for the particles to move around so there are more collisions which create more pressure. Inside the bottle.

3. As the volume of a cylinder is increased the pressure will ____________Decrease______________.

                                                                                               (increase, decrease or stay the same?)

The pressure will decrease because there's more volume. If you have more space that gives you less pressure. The syringe example again, when you put less pressure you have more air or volume on the inside. 

4. Increasing the pressure in a tire by adding more gas will cause the volume to ______Decrease_________ .

                                                           (increase, decrease or stay the same?)

When the pressure is increased there's less room for gas particles to move and there's less space so that decreases the volume inside the tires.

5. As the temperature of a closed container of water is increased the amount of water vapor  above the water causes a(n) __________Increase_______________ in vapor pressure.

                                          (increase, decrease or no change?)

The vapor pressure will increase because there is more limited space for the particle to move

6. As the air pressure above a liquid is increased by adding more air, the boiling point of the liquid will _________Decrease____________.  (increase, decrease, or remain the same?)

The boiling point of the liquid will decrease because it has more pressure on it.

7. If a balloon filled with air is taken under water to a depth of 10 feet, it’s volume will ___________Decrease___________ . (increase, decrease, or remain the same?)

it's volume will decrease because there's more pressure and that make there more room to move

8. The temperature of a beaker of boiling water will _______Increase___________ as more heat is  added.                                                                                  (increase, decrease, or remain the same?)

The temperature of a beaker of boiling water will increase because heat it constantly added

  

9. Hot air rises because it is _____Less________ dense the cold air around it.  

                                                  (less or more?)

Hot air is less dense than cold air because gases aren't as compact as a solid and that makes them rise

10.  When heated, the volume occupied by air in a balloon  will ____________decrease_______________ .

                       (increase, decrease or stay the same?)

When heated a balloon is compressed which decreases the volume because there's less space

Lab 3.1 Properties of Ionic and Covalent Compounds

Ionic compounds are hard, they don't have any conductivity and They have high boiling pionts. Covalent bonds on the other hand are brittle or easily broken and have low boiling points but they also don't have conductivity.

Ionic bonding is between metals and nonmetals. Ionic bonding transfers electrons. Non metals gain electrons and the metals lose them. Which means that instead of the electrons going to waste they are added to the nonmetal's electrons.

Covalent bonding is nonmetals only. This means that instead of the electrons being transferred they are shared between the elements. Since they're all nonmetals they have to feed off of eachother's electrons to be stable.

Covalent bonds lack conductivity as a solid or in a solution because they don't have any positive elements which means that they can't conduct electricity.

Ionic bonds can only conduct electricity in a solution because the elctrons can freely move and there can be positive elements because the electrons can be transferred to another molecule. In solids there is very little movement possible.

Lab 2.2 Bag of Ions & Periodic Table Chem Crunch

In the periodic table there are several ways to organize it but when you look at it it's organized by groups  ( Metals, Metalloids, nonmetals). It's also organized by atomic mass and number. If an atom is in the same group then they will have the same number of valence electrons.

Atoms and ions are two totally different things.

Atom- The object or element is neutral

Ion- The object or element has a positive or negative charge.

Atoms and ions of the same element have the same atomic number or number of protons. But the ions will have different numbers of valence electrons. When an element is a metal it losses electrons so it will have a positive charge. When an element is a nonmetal it will gain electrons so it will have a negative charge. That's exactly how ions are formed, whenever ions are gained or lost because then the atom will have a charge.

That's how ions and atoms are different.

Lab1-4 Physial & Chemical Change

Physical and chemical change can be easily mixed up. For instance, when a substance changes colors after something is added. Some people would think that it's a chemical change but it's only physical because it just changed the color it didn't change the chemical compositon of the substance

Physical Change-   Any process involving a substance's change from one state (gas, liquid, solid) to another without alteration of the chemical composition. ( Dictionay.com)

Ex.)  Freezing water is a physical change because both water and ice are H2O.

Chemical Change-    Any change from one state (gas, liquid, solid) which is accompanied by alteration of the chemical composition; any process in which one or more substances are changed into one or more different substances. ( Dictonary.com)

Ex.)  Making water out of hydrogen and oxygen

One thing that would convince methat a physical change has occurred is color change.

One thing that would convince me that a chemicalchange has occurrred is the bubbling or boiling of a substance.

When you're unsure you could use your reference tables or th internet to see if the two substances ar reactant to eachother.

Or

You could try to seperate the ixture and then see if it's different tan before.

Lab 1-3 Separation of a mixture

In this lab mainly we mixed iron, sand and salt together. Then one by one we separated the mixture with different substances such as water and heat. We also recorded the percentages of the substances in the mixture.


Afterwards, we recorded the experimental percentages of the substances. These values didn't match the original. The reason for this is because some substances were absorbed and some were dissolved into other substances.


To make the separation better we could've used more water or heat to make the iron turn to a gas.


To find the decimal to round to use the crapiest mesurment or the lowest decimal and round to that place.


In class we are talking about elements, compounds and mixtures. We're also working on particle diagrams for those elements, compounds and mixtures. What we're doing in class also helps with this lab because the practice with math and calculations and visual representation gives us an idea of what's going on. Great lessons = Great results.

Lab 1-2 Indirect Measurment

The Lab had numerous steps into getting your results. You had to compare many numbers. This lab was all about thickness of the objects and how to get that thickness. For example, the foils, HD foil was much thicker than regular foil but they looked similar. So you had to take the mass of the foils then get the volume by dividing that mass by the density of aluminum, which gave you the thickness. My group then compared the two and they were very different in size but similar in appearance. For The copper it was the same pretty much because you had to get the same measurments. But on the end of the calculations you used the diameter formula.

1.) With the water displacement method it's not very accurate because even though the HD foil and the regular foil had differtent masses they might get the same volume which is incorrect. To get an accurate measurment you have to find the mass of the foil then divide the mass of the foil by the density of aluminum. that will give you the volume which is the thickness.

When you measure with a ruler it's the same as water displacement it's inaccurate. in order to get the correct thickness you have to measure the legth with a ruler but not the width. Next, you have to perform the diameter formula which will give you the thickness.These are some methods to get accurate measurments.

2.)When calculating the actual thickness you can be confident if the answer has lots of decimals because normally if it's a precise measurment it won't be a whole number. For instance the thickness of someone's arm. for sure that won't be a whole number. That's why you should be confident if your answer has a lot of decimals.

3.) Some sources of error would be your reference table or your calculator because the numbers are rounded. The scale could be a source oferror as well because it could be a tenth off it there is any extra pressure on the scale.

I believe I could measure the thickness of a pen in a future experiment because it's cylindrical just like copper wire but it has different measurments. The pen might not have an exact measurment but if you try you'll find out.

Green Stuff Lab

First, I put 25ml of water in a beaker. Next, I poured the green stuff into a separate beaker. After that, I poured the green stuff into the water. Next, I put a few drops of the solution on aluminum foil. Lastly, I put the remains of the aluminum foil in the solution.

Something I observed during the lab was that the color changed when the green stuff was added to the water. This answers the question about the properties of the green stuff. Something else I observed was that the water bubbled when the green stuff was poured in. This answers the question about physical and chemical properties, that occurrence was a chemical change. I learned that the solution that water and copper chloride made was acidic because it burned through the aluminum foil. I also learned that when aluminum foil is added to that solution it can make copper.

Some practical use of what i learned today is to make large amounts of this solution and burn through certain items for fun or entertainment of others. Another practical use of what i learned today was to burn used aluminum foil to make copper.

A further experiment that i would conduct would be to use the same solution but use it on a variety of items not just aluminum foil. Plus you could separate the solution and use just water and just copper chloride in two different beakers and then the solution in a third beaker. This experiment could broaden the results.This lab taught me a lot about the physical and chemical properties of copper chloride.