3 questions

1. Recently I have completed 3 books in two days. I have no life.
2. I have learned a little more about spectroscopy and how to use a spectrophotometer, which I must say is pretty nifty. 
3. I am struggling with calculations, mostly because I can't seem to grasp the basics. I need to work on those by just going over the stoich and measurement rules.

Coulumb's Law Exploration

1. Coulumb's Law is a law describing the electrostatic attraction between two charged particles. The equation is E (energy) is equivalent to Q1 + Q2 over d (distance). The Q's are the different charges.
2. Distance and charge both effect the energy in  a different way. Distance is indirectly related to energy, the greater the distance, the less the energy to remove an electron from the atom. Charge and energy are directly related, so the greater the charge the greater the energy required to remove an electron from the atom.
3. Removing an electron is an endothermic process because it requires energy to be absorbed by the electron for it to overcome the attractive forces of the nucleus. Its not exothermic because it isn't letting go of energy. If it was, the electron would be moving closer to the nucleus, not away from it.
4. The amount of energy required to remove an electron is based on the distance from the electron and the charge of the nucleus, and also the net charge the nucleus has on the electron. The further from the nucleus, the less energy it takes to remove and electron. The closer to the nucleus, the harder it is to remove. The valence electron is the furthest electron from the nucleus, and the net charge on the valence electron is usually less than the net charge on the electron that are in closer orbitals.
5. The energy to remove an electron compared the energy to excite and electron are much different. If the electron is in a higher orbital, the energy to remove it is low. However, the energy to move an electron from a low orbital to a high orbital, or from ground state to an excited state, needs a lot of energy because its overcoming the attractive electrostatic forces. Now if the electron that you're removing is closer to the nucleus, it could potentially take around the same amount of energy to remove it as it would to move that electron to an excited state.

3 Questions

1. I have completed Allstate recently. It went really well, we even got an encore. That was definitely the best allstate year yet.
2. I am now extending my knowledge on light energy and electron transmission. I have to say, besides electrochemistry this is my favorite unit so far. 
3. I am still struggling with the thermodynamic unit, but hopefully with the help of unit 6 I will start putting two and two together.

Explore blog

The relationship between energy, wavelength and frequency of light is indirectly related. The higher the wavelength range, the lower the frequency and the lower the energy. This description fits with the color red. The wavelength is long, with a lot of space in between the crests and troughs. The photon energy is low, it ranges from 269 to 318 Joules. Light emission demonstrates electron transition by releasing the color the energy change corresponds to. If an electron moves from a high energy state to a lower energy state, it will likely give off a higher frequency color, like violet or blue, given the amount of energy it is releasing to move that electron closer to the nucleus.  Say an electron moved from energy level 6 to energy level 2. Since it would lose alot of energy because it moved much closer to the nucleus, it would give off a high frequency with a high photon energy, such as violet, which has a short wavelength of 380 to 440 nm. Say it was the other way around, and the electron was moving from a lower, or ground, state, to a higher, or excited, state. The electron would absorb the color light corresponding to its wavelength because the electron has to gain energy to overcome the forces of attraction with the protons in the nucleus. Light can be used to measure the electron transition of electrons simply by observing the color given off and relating it to its wavelength, frequency and energy.

 

sources: http://en.wikipedia.org/wiki/Light