Post by sparkogre on May 13, 2009 15:58:12 GMT -5
This is basically what I do for my classes to study.
1. Take notes.
2. Type up notes.
3. Make question and answer things out of your notes.
4. Memorize the answers.
Here's an example:
Notes:
Quantum model – Bohr (1913)
-electrons orbiting around nucleus at fixed distances
-when electron moved between orbits was the explanation for why only certain λ light is emitted. When it goes to a different orbit, it can only emit certain values of energy.
Bohr’s model only works for hydrogen:
E = 2.178 x 10-18 * (Z2/n2)
Z = nuclear charge (ionic charge)
N = integer corresponding to which orbit the electron is in (when the electron is actually removed, n = ∞, so the equation value approaches 0 (limit).
∆E = Efinal orbit – Eoriginal orbit
Schrodinger – wave mechanical model
Questions:
10. Who invented the quantum model, and when? What is the only element that it works for?
11. What is the explanation of Bohr’s quantum model?
12. What is the equation for the energy an electron has in Hydrogen? What is the equation for when an electron moves to a different orbital? What is the energy required for removing an electron, and why?
13a What did Schrödinger’s quantum model thing say?
Answers:
10. Bohr invented the quantum model in 1913. It only works for hydrogen.
11. Electrons orbit around the nucleus at a fixed distance.
When the electron moves between orbits, only a specific wavelength of light can be emitted. When it goes to a different orbit, it can only emit certain values of energy.
12. E = 2.178 x 10-18 * (Z2/n2)
∆E = Efinal orbit – Eoriginal orbit
Removing an electron requires no energy, because actually removing the electron makes n approach ∞, and so the limit = 0.
13. Schrödinger created the wave mechanical model, and quantum mechanics. It gives wave properties to electrons that we previously thought behaved as particles. It visualized electron as a standing wave around the nucleus – and it can only exist in orbits corresponding to whole number wavelengths. (So it can never be between 2 different wavelengths.) So the electron has to be in orbitals in increments of wavelength, no decimals allowed.
Now, obviously, for a chemistry class, you're going to have to do problems too. But this is going to get most stuff out of the way.
1. Take notes.
2. Type up notes.
3. Make question and answer things out of your notes.
4. Memorize the answers.
Here's an example:
Notes:
Quantum model – Bohr (1913)
-electrons orbiting around nucleus at fixed distances
-when electron moved between orbits was the explanation for why only certain λ light is emitted. When it goes to a different orbit, it can only emit certain values of energy.
Bohr’s model only works for hydrogen:
E = 2.178 x 10-18 * (Z2/n2)
Z = nuclear charge (ionic charge)
N = integer corresponding to which orbit the electron is in (when the electron is actually removed, n = ∞, so the equation value approaches 0 (limit).
∆E = Efinal orbit – Eoriginal orbit
Schrodinger – wave mechanical model
Questions:
10. Who invented the quantum model, and when? What is the only element that it works for?
11. What is the explanation of Bohr’s quantum model?
12. What is the equation for the energy an electron has in Hydrogen? What is the equation for when an electron moves to a different orbital? What is the energy required for removing an electron, and why?
13a What did Schrödinger’s quantum model thing say?
Answers:
10. Bohr invented the quantum model in 1913. It only works for hydrogen.
11. Electrons orbit around the nucleus at a fixed distance.
When the electron moves between orbits, only a specific wavelength of light can be emitted. When it goes to a different orbit, it can only emit certain values of energy.
12. E = 2.178 x 10-18 * (Z2/n2)
∆E = Efinal orbit – Eoriginal orbit
Removing an electron requires no energy, because actually removing the electron makes n approach ∞, and so the limit = 0.
13. Schrödinger created the wave mechanical model, and quantum mechanics. It gives wave properties to electrons that we previously thought behaved as particles. It visualized electron as a standing wave around the nucleus – and it can only exist in orbits corresponding to whole number wavelengths. (So it can never be between 2 different wavelengths.) So the electron has to be in orbitals in increments of wavelength, no decimals allowed.
Now, obviously, for a chemistry class, you're going to have to do problems too. But this is going to get most stuff out of the way.
