As you i just disputed in the Spectral lines page, electrons loss to lower energy levels and give off light in the form of a spectrum.
You are watching: Calculate the wavelength of light required to make a transition from n=1→n=2 and from n=2→n=3.
These spectral lines room actually certain amounts of energy for once an electron transitions to a lower energy level. If you assume the energy levels of an atom to it is in a staircase; if you role a round down the stairway the round only has a couple of "steps" the it have the right to stop on. This is the same situation an electron is in. Electrons can only occupy particular energy levels in an atom. It most be on an power level if the is in the atom. There is no in between. This is why you get lines and also not a "rainbow" that colors as soon as electrons fall.
Jahann Balmer in 1885 obtained an equation to calculate the clearly shows wavelengths that the hydrogen spectrum displayed. The present that show up at 410nm, 434nm, 486nm, and 656nm. These electrons are falling come the 2nd energy level from higher ones. This shift to the 2nd energy level is currently referred to as the "Balmer Series" that electron transitions.
Johan Rydberg usage Balmers job-related to derived an equation for every electron transitions in a hydrogen atom.
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Right here is the equation:
R= Rydberg consistent 1.0974x107m-1; λis the wavelength; nis same to the power level (initial and also final)
If we wanted to calculate energy we can change R by multipling by h (planks constant) and also c (speed the light)
Now we have actually Rydbergs equation to calculation energy.
RE= -2.178 x 10-18J (it is negative because power is gift emitted)
l = h c /E
l = ( 6.626 x 10- 34J s) (3.0 x 108m/s)/E
1nm= 1 x 10-9m
|Electron Transition||Energy (J)||Wavelength (Meters)||Wavelength (nm)||Electromagnetic region|
|Paschen collection (to n=3)|
|n=4 to n=3||1.06 x 10-19||1.875 x 10-6||1875||Infrared|
|n=5 to n=3||1.55 x 10-19||1.282 x 10-6||1282||Infrared|
|Balmer collection (to n=2)|
|n=3 come n=2||3.03 x 10-19||6.56 x 10-7||656||visible|
|n=4 come n=2||4.09 x 10-19||4.86 x 10-7||486||visible|
|n=5 to n=2||4.58 x 10-19||4.34 x 10-7||434||visible|
|n=6 come n=2||4.84 x 10-19||4.11 x 10-7||411||visible|
|Lyman series ( come n=1)|
|n=2 come n=1||1.632 x 10-18||1.22 x 10-7||122||Ultraviolet|
|n=3 to n=1||1.93 x 10-18||1.03 x 10-7||103||Ultraviolet|
|n=4 come n=1||2.04 x 10-18||9.73 x 10-8||97.3||Ultraviolet|
|n=5 to n=1||2.09 x 10-18||9.50 x 10-8||95.0||Ultraviolet|
|Wavelength (m)||Frequency (s-1)|
|1.875 x 10-6||1.6 x 1014|
|1.282 x 10-6||2.34 x 1014|
|6.56 x 10-7||4.57 x 1014|
|4.86 x 10-7||6.17 x 1014|
|4.34 x 10-7||6.91 x 1014|
|4.11 x 10-7||7.30 x 1014|
|1.22 x 10-7||2.45 x 1015|
|1.03 x 10-7||2.91 x 1015|
|9.73 x 10-8||3.08 x 1015|
|9.50 x 10-8||3.15 x 1015|