Below are some resources that I think are helpful for CHE 132 students . If you have any questions come to an SI session or leave a comment below. You can also upload any of your helpful resources in the comment section!
My Session Schedule, Winter 2016
[box]Monday 1:30-2:30pm, Richardson Library 111
Friday 11:30am-12:30pm, Richardson Library 111
Office Hour – Thursday 3-4pm, Richardson Library 111 [/box]
Can’t attend any of my sessions? Check out other CHE 132 SI leaders’ schedules here.
I am a junior majoring in Chemistry with a Medical/Biochemistry concentration. I enjoy the sciences because it allows me to have a deeper understanding to how and why the world works the way it does. As part of my passion for chemistry, I research with Dr. Grice in McGowan South during the school year. Outside of academics I enjoy eating food, listening to music, drinking coffee/tea, and exploring new places in Chicago when I have the time. If you have suggestions, absolutely let me know!
- Remember Sig Fig Rules and Unit Conversions. For a quick refresher, look no further then [ilink url=”https://www.youtube.com/watch?v=hQpQ0hxVNTg”]here[/ilink] !
- Always be one with your calculator and periodic table. [ilink url=”https://www.youtube.com/watch?v=UL1jmJaUkaQ”]Stoichiometry[/ilink] will never go away!
- When in doubt, always double check the list of equations you have. Something will work or get you on the road there!
- Review fundamental concepts. Chemistry is a little like poetry, you see the same phenomena here and there.
- For those of you who have taken, are taking, or will take physics, take note! A lot of what you see in chemistry is tied to important physics concepts!
- The first thing you need to do is observe the useful data that they provide you as the sign of the enthalpy will likely tell you the direction of the arrow in your diagram. For your reference, a positive sign indicates an increase in enthalpy while a negative sign indicates a decrease in enthalpy. Certain types of energy tend to strictly follow either a positive value or a negative value but always pay attention to the sign just in case it doesn’t follow normal trends.
- There are pros and cons to doing either the diagram or math portion first. However, the diagram helps you keep track of all reagent quantities.
- In my review session, there was a student who described the order in which the diagram energies are listed. Generally, you list the heat of formation for the product first. The next thing you do is make sure everything is in the gas phase by using sublimation energy if provided. As you can expect, sublimation energy is usually positive. For the next step, you want to focus on making any cations by using ionization energies. Removing electrons always requires a positive input of energy. Lastly, focus on bond dissociation energies keeping in mind how many atoms you need in the final product. You focus on the above before proceeding to electron affinity and lattice energy.
- Electron affinity can be positive or negative depending on the circumstances. As you might imagine, an electronegative atom like oxygen will likely want electrons and eagerly take up the first electron. In this process, we release heat in forming a new attachment to oxygen. However, the second electron is more difficult to attach to oxygen as there is a net negative charge on the oxygen opposing the new electron. As a result, the addition of the second electron to oxygen is an energy intensive process. You wouldn’t need to explain this on a test, but it is helpful to be wary of this phenomenon. In addition, keep in mind how many atoms you need to add electrons to.
- Lattice energy is the release of heat in forming a very stable bond. This will likely be the largest arrow in your diagram.
- Always double check your math and diagram. A mock diagram is shown below.
- A helpful way to remember gas laws. The three big ones change volume. Key think is, think alphabetically. Gay-Lussac’s Law can be remembered as the odd one out and keeps volume constant while changing P and T.
- Avogadro’s Law = n, V
- Boyle’s Law = P, V
- Charle’s Law = T, V
Van der Waals Equation
Molarity vs. Molality
Boiling Point Elevation and Freezing Point Depression