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jcmartinez
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hello, i am studying chemistry. There are a lot of things i do not understand though. This is not homework, just studies of my own that i would like to reach a deeper understand of. I love the responses i have read, so decided to make an account and learn from all you geniuses!
Bohr model video i am using to learn.
1st question. classical electromagnetic theory predicts an orbiting e- should emit radiation. Why?
the frequency will change due to loss in energy, resulting in the electron crashing with the nucleus. If the e- looses its energy though, wouldn't it just stay floating?
2nd. some atoms glow, but do not change color, which indicate a frequency shift. I though frequency determined what type of wave was emitted. (e.g. uv, infrared, light) I also thought that wavelength determined color.
3rd. e- in smaller orbits posses less energy then those in bigger orbits (further away). The video says its due to the attraction with the nucleus. so more attraction equals smaller orbit number?
Bohr equated the allowed values of the angular momentum to the energy of the electron. He obtained the following equation. E= -R(little h)/n^2
R(little h) is known as Rydberg constant) 2.18 x 10^-18
So I am guessing to determine the energy of an e-, we use that formula. The smaller the "n" value is, the larger my "E" is. Since my result will be a negative number, it makes sense because -1000 is lower then -10. Since we cannot have a Negative orbital (or a -n) our "E" values will always be negative right? Cause if "E" was a positive value, 1000 to 10 would mean the smaller orbitals have more energy right? so does that explain the reason for the negative symbol in front of the equation? or did i just BS myself.
please shed light onto me ohh PF gurus!
-sincerely person trying to conquer chemistry
Bohr model video i am using to learn.
1st question. classical electromagnetic theory predicts an orbiting e- should emit radiation. Why?
the frequency will change due to loss in energy, resulting in the electron crashing with the nucleus. If the e- looses its energy though, wouldn't it just stay floating?
2nd. some atoms glow, but do not change color, which indicate a frequency shift. I though frequency determined what type of wave was emitted. (e.g. uv, infrared, light) I also thought that wavelength determined color.
3rd. e- in smaller orbits posses less energy then those in bigger orbits (further away). The video says its due to the attraction with the nucleus. so more attraction equals smaller orbit number?
Bohr equated the allowed values of the angular momentum to the energy of the electron. He obtained the following equation. E= -R(little h)/n^2
R(little h) is known as Rydberg constant) 2.18 x 10^-18
So I am guessing to determine the energy of an e-, we use that formula. The smaller the "n" value is, the larger my "E" is. Since my result will be a negative number, it makes sense because -1000 is lower then -10. Since we cannot have a Negative orbital (or a -n) our "E" values will always be negative right? Cause if "E" was a positive value, 1000 to 10 would mean the smaller orbitals have more energy right? so does that explain the reason for the negative symbol in front of the equation? or did i just BS myself.
please shed light onto me ohh PF gurus!
-sincerely person trying to conquer chemistry
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