Slam a revolving door

Chuck Norris can slam a revolving door
Besides from the obvious... today in class, first thing we did was review the forces. We reviewed the dispersion forces, dipole forces, and hydrogen bonding. for more information you can look below at Elim's post.
After our review, we started our lab.
This lab has 7 stations to observe trends and patterns in several properties of liquids and to use a model of intermolecular forces to explain the findings.

Station 1: Evaporation Rates
This station measured the rate at which the liquid evaporated. the rate that the liquid evaporates depends on the strength of the intermolecular forces between liquid molecules. liquids with the lowest evaporation rates have the strongest intermolecular forces.
Insert Photo here that I could not find

Station 2: Capillary Action
A liquid tends to climb up the walls of narrow columns, this is known as capillary action. This is based upon two forces: adhesive forces, and cohesive forces. The greater the cohesive strength, the more the liquid climbs the column. The greater the adhesive strength, the lesser the liquid climbs the column.

Station 3: Vortex Formation and Relaxation
If you swirl water, you get a water tornado. That's what this is, just making vortex's by swirling the liquids. The time it takes for a liquid to settle down from a swirl is different for all liquids depending on the intermolecular forces. the longer it takes to relax, the stronger the intermolecular forces are. We did this with three liquids: Water, Hexane, and Heavy oil.

Station 4: Viscosity or Resistance to Flow
Not every liquid flows at the same rate (compare water to waffle syrup). Viscosity is the property of a liquid which provides a measure of that liquids tendency to resist flow. Liquids with stronger intermolecular forces have a greater resistance to flow, a higher viscosity. We took the same three substances as station 3, and put them in test tubes. After that we timed the seconds of a marble falling to the bottom of the test tube. The faster it is, the lower the liquids tendency to resist flow, or the lower the Viscosity. The lower the viscosity, the weaker the intermolecular forces.

Station 5: Surface Tension
Molecules on the very surface of a liquid can form strong enough intermolecular forces between them to make their surface impenetrable. It's this surface tension (along with other factors) that make leaves floar on water. For this expirement, we had to lower a paperclip using a tray to try to make it float on the liquid. The liquid that the paperclip can most easily float has the greatest surface tension.

Station 6: Beading
Many liquids have a tendency to bead. For example water droplets that look circular, that is actually the water beading. This is cause by liquid molecules to form a strong intermolecular attraction with itself and curl into a spherical bead or droplet. The greater the strength of the intermolecular forces, the greater the tendency of the liquid to bead. If placed on a surface the liquid is attracted to, the liquids beads less. For this expirement we dropped droplets of liquids onto wax paper and our lab benches. We then made observations according to what beaded and what didnt.

Station 7: Freezing point and Boiling Point
unlike the other stations, this one was all on our packet. all liquids have a freezing and boiling point. These points depend on the strength of the intermolecular forces. Liquids with stronger intermolecular forces have higher boiling points. The graph on our paper is pretty straightforward if you just remember that.


Don't forget we have a ton of webassigns due on Friday as well as this lab.
This lab must also have a conclusion on a seperate piece of paper (though the data can all be in the packet).
The next scribe will be Emilio.

Sharing is Caring

Today, Mr. Lieberman had a pack of sour patch kids. He shared them with Zoe by giving her 1 of them and eating the rest. With a second pack of candy, he gave half to Zoe and the rest he ate. With a third, he gave the whole pack to Katie, taking none for herself. We learned that Mr. Lieberman was sharing his candy as molecules share electrons.
First, we learned about polar and non-polar. These are only between 2 nonmetals.
Polar covalent bonds are where electrons are not shared equally between molecules, and the electronegativity difference is between 0.4 and 1.7.
Non-polar covalent bonds are where electrons are shared equally between molecules, and the electronegativity different is between 0 and 0.4.
An example of a non-polar covalent bond is C-C. It is said to be like "tug of war with your twin". No one would win and the forces trying to win, or gain the electrons are equal, so the electrons would be shared equally. The electronegativity for the two atoms are the same, so they are equally pulling for the electrons. This is the scenario where Mr. Lieberman gave half his candy to Zoe and kept half for himself.
An example for a polar covalent bond would be C-F. The electronegativity for fluorine is strong than that of carbon, and therefore, there is an unequal share of electrons, because flourine would be winning the game of tug of war with carbon. Fluorine becomes more negative because the electrons are closer to fluorine than carbon, even though they are still shared with carbon, so that would mean fluorine is partially negative. Carbon has less of a pulling force on the electrons so it is partially positive. The opposite ends (+ and -) create a dipole. This is the scenario where Mr. Lieberman gave one piece of candy to Zoe and ate the rest.
Ionic bonds are where one molecule gets all the electrons, having a complete transfer, even though this is considered sharing. The electronegativity of one nonmetal atom is so much greater than the other metal atom that it pulls the electrons away. This is the scenario where Mr. Lieberman gave all his candy away to Katie.
We also had a pop quiz at the end of class.
Have a great rest of the weekend everyone!
~Kaitlyn Y.
The next scribe will be Elim.

Continuation on Electron Pairs and Start of Hybridization

To start off class today, we first discussed the types and names of the electron pairs we learned yesterday (In Ethan's Post). Next, we moved into looking at 4,5, and 6 areas of concentration. These are the highest levels of concentration that can ever happen in an atom.

The first molecule that we looked at for the day was PF5. PF5 has 40 valence electrons and using this, we constructed the Lewis structure. Phosphorus can break the octet rule, which is the only reason why this Lewis Structure works. Then we used that to help us form the angles at which the balloons in the demonstration were forming(90,120,180). PF5 is an example of a trigonal bipyramid molecule. We then did the same steps for the Octahedron molecule of SF6. Sulfur can also break the octet rule.

During the demonstrations of the shapes of how these molecules would look like if they were much bigger, we also saw how the non-bonding pairs of atoms continuously took away an equatorial angle, instead of a linear angle. This happens because this is the most stable configuration.

The Last thing we learned about for the day was hybridization. Hybridization is the mixing of one s orbital and one p orbital in order to produce two sp orbitals. We looked at a video that explained the different formations as well as the actual action of what it would look like. . That is all we learned.

The next scribe is...Deena M.