March 16 and 17

This will be a double scribe post since I forgot to do it on Tuesday.

On Tuesday we read pages 14 to 18 in the Atomic Structure booklet together as a class. The pages described the development of the Quantum Mechanical Model of the Atom and how each scientist contributed to it.

We were assigned page 19 and corrected it together.

Answers:

G.P Thomson
Albert Einstein
Louis de Broglie
Erwin Schrodinger
Max Planck
C.J Davisson
L.H Germer
Wolfgang Pauli
Johannes Rydberg
Werner Heisenberg
Niels Bohr

On Wednesday we continued to read in the booklet through pages 20 to 27. We learned more in depth about the quantum mechanical model of the atom and also learned about atomic orbitals.

We were assigned page 24 to do and here are the answers:

1. Rutherford's model didn't explain why negatively charged electrons orbiting a positively charged nucleus don't collapse into the nucleus.

2. Bohr's model: ORBIT -> fixed circular path
Rutherford: Didn't mention fixed energy

3. Each line corresponds to a specific color.

4. Ground state: low energy Excited state: high energy

5. Major problem with Bohr's atomic model is that it didn't work with the line spectrum of other elements (only hydrogen).

6. Electrons emit light energy when dropping from a higher energy level to a lower energy level because it gives off the same amount of energy absorbed.

7. "Energy levels are quantized" means elections must posess specific amounts of energy at each level.

8. Each element possesses a characteristic spectrum because each element has a different number of electrons which results in a different line spectrum.

Important information:

* Bohr orbit: fixed circular path
Oribital -> likelihood of finding an electron
* The cloud is most dense where the probability of finding the electron is large. It is less dense where the probability of finding the electron is small. (page 20, paragraph 2)
* A spectroscope seperates light into it's component wavelengths, revealing a line spectrum that is unique to each element. (page 20, paragraph 2. The whole reason is important.)
* According to Bohr, the lines in the line spectrum for hydrogen are a result of the energy released when the hydrogen atom's electron fall from a higher energy level to a lower energy level. (page 23, paragraph 5)
* Orbitals related to energy sublevels within one principal energy level can overlap orbitals related to energy sublevels within another principal level. (page 25, paragraph 5)
* The Pauli exclusion principle states that a maximum of two electrons may occupy a single atomic orbital, but only if the election have opposite spins. (page 25, paragraph 6)

Ms. K mentioned there would be a test next week and that we should know this information (I think). Tomorrow we'll be learning more about electron configurations and doing practice problems.

The next scriber will be: jeck (?)