no guessing.
2006-06-27 10:36:44 · 5 answers · asked by Richardicus 3 in Science & Mathematics ➔ Chemistry
from Br2
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2006-06-27 10:37:01 · update #1
There is an absorption at 265 nm and 234 nm according to the literature.
If you look up "Constants of Diatomic Molecules" by Huber and Herzberg, you can find the first predissociative state for the bromine molecule. This is where an electron is excited into an anti-bonding molecular orbital, and the molecule then dissociates.
I have Herzberg's "Spectra of Diatomic Molecules" and he cites dissociative states at 47000cm-1. That would be 212 nm.
BTW UV light is not at 5x10-8 m. That's considered Deep UV or Extreme UV...really close to soft x-rays.
2006-06-27 13:59:19 · answer #1 · answered by Iridium190 5 · 0⤊ 0⤋
Radical bromination occurs in the presence of UV light.
The wavelength of UV light is 5 x 10^ -8 m
2006-06-27 11:17:14 · answer #2 · answered by BeC 4 · 0⤊ 0⤋
radical formation is usually occurs when you subject the necessry amount of energy to expel a radical from the molecule.
what wavelength of light? well, it seems UV does the trick. sometimes, high energy is required too.
2006-06-27 15:26:12 · answer #3 · answered by zwanzig 1 · 0⤊ 0⤋
UV, I guess (380–200 nm wavelength), I probably would check the lower end.
2006-06-27 10:59:17 · answer #4 · answered by nickyTheKnight 3 · 0⤊ 0⤋
most of those radiated from household appliances , etc !
2006-06-27 10:53:22 · answer #5 · answered by love 3 · 0⤊ 0⤋