1. ATOMS
ATOMIC STRUCTURE
We began Honors Chemistry class by learning about Atomic Structure, which included ions, protons, neutrons, electrons, energy levels, the nucleus, excited states, and the ground level.
Ions - In Phase 1, we viewed a video on material that can be burnt or added to a burning fire, causing the flame to change to different colors. After viewing this video, we considered what might be causing the color emission. To further study this concept, we performed an experiment. The goal of this lab was to determine what colors ions generate when each is exposed to a flame. The materials we used were ion samples, toothpicks, and a torch. In this experiment, we were instructed to use a toothpick to take take samples of each ion individually, place over a torch, and observe the color that was emitted. From our observation, we found that each ion generated a different color. We observed the following ions and colors: Sodium (Na+) = Orange, Potassium (K+) = Purple, Lithium (Li+) = Deep Red, Strontium (Sr+) = Red, Barium ( Ba2+) = Yellow, Copper (Cu2+) = Green, Calcium (Ca2+) = Light Orange. (Examples are below)
*An ion is a charged atom or molecule. It acquires a charge because its number of electrons does not equal its number of protons.
The reason why the ions emit color: Electrons of an atom like to relax in orbitals that leave the atom with the lowest possible energy (ground state). Exposing atoms to a flame excites its electrons which causes them to jump to higher energy levels. When the electrons return to lower energy levels, they emit energy in the form of light. When these excited electrons drop back to where they are supposed to be, they release the energy that they stored up as particles of light which are the colors that are seen.
Magic Flame - Ions - After determining which ions generated what colors, we performed another experiment using the flame test. The goal of this lab was to determine what ions composed "Magic Flames" and to replicate it by making a mixture with those ions. The materials we used were the Magic Flame mixture, ion samples, toothpicks, and a torch. In this experiment, we were instructed to use a toothpick to take take samples of the Magic Flame mixture, place it above a flame, observe the color, and determine which ions were present by the color of the flame. Since we knew what colors the specific ions generated, we were able to determine what ions were in the Magic Flames in petri dish. Once we determined which ions composed the mixture, we replicated it.
subATOMIC Particles
Periodic Table - In the phase 2 of our Journey of atoms, we studied subatomic particles. We learned about the Periodic Table - elements, the atomic number of an element (its number of protons and electrons), its atomic mass, and the concept of molar mass.
Oxidation - In the next part of this phase, we learned that when Steel Wool is rapidly burned using the current from a battery, oxygen bonds with the iron in the alloy. The goal of this lab was to determine the total number of moles that bond when an entire roll of Steel Wool is oxidized. The materials we used were steel wool, scale, 9V battery, and a flame. In this experiment, we were instructed to weigh the steel wool, burn it, and weigh the steel wool again. After the steel wool was burned, we used the original weight and the weight after burning and determined that the steel wool had actually increased in weight. We found that this is because when burned, the steel wool oxidizes and as a result gains mass.
Magnesium Sulfate Hydrate - We concluded this phase with learning about the function of the Mars Rover. Its main objective is to search for water in the form of hydrated salts, an ionic compound that has proportional amounts of water bonded to its crystal lattice. When heated, the water is removed and a dehydrated sample remains. By recording the weight of a sample before and after heating, we can determine the moles of water in the sample.
To study this concept, we performed an experiment. The goal of this lab was to determine the moles of water in a sample of magnesium sulfate hydrate (MgSO4xH2O). The materials we used were a sample of magnesium sulfate hydrate (MgSO4xH2O), bowl, Bunsen burner, stand, and a scale. In this experiment, we were instructed to take a small amount of MgSO4xH2O, place in a bowl, weigh it (83.08g), place on stand over a flame, and wait until all water evaporates. We completed this, and after all water had evaporated, we weighed the bowl with MgSO4xH2O again (66.81g). We then used the original weight and the weight after water was evaporated to determined the amount of water by converting into moles. From our calculation, we found that there were 0.90 moles of water in our sample.
reflection
Overall, I really enjoyed this portion of honors chemistry class. It is my first exposure to chemistry, and I find it extremely interesting. I learned all new concepts and a lot of information during Journey 1 of Honors Chemistry. I feel that Ramsey is an amazing teacher, and I grasped all concepts he taught.
As the final phase of our class concluded, I prepared for the test. I did this by reviewing class notes, my labs, and the homework. I felt that I was totally prepared for the test.
Overall, I learned a lot of information and I love everything about the class so far.