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Title: Wave length / Bohr model full lab report
Description: I got a 100 on this lab
Description: I got a 100 on this lab
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Bohr Model Lab
Title:
Table depicting the Wave Length, Light Frequency, Energy, Balmer Transitions, Upper
Energy Level, Percent Error for Upper Energy Level, and Change in Energy For Hydrogen
Wavelength Wavelength
(nm)
(m)
Light
Frequency
Energy
N upper
ΔE
Percent
Error
397
...
97007E07
7
...
01E19 6
...
99E19
0
...
174 4
...
31E+14 4
...
94E+00
4
...
39%
434
...
34047E07
6
...
58E19 4
...
56E19
0
...
133 4
...
17E+14 4
...
98E+00
4
...
39%
656
...
56272E07
4
...
03E19 3
...
02E19
0
...
285 6
...
57E+14 3
...
00E+00
3
...
39%
1
...
0 × 108m/s = 3
...
56 x 10
E = vh
E = 7
...
36 s × 10−34) J × s
E = 5
...
1 = R((2)2 − n2 )
λ
1
3
...
1 × 107((2)2 − n2 )
n = 6
...
178 × 10−18((2)2 − (6
...
0005 × 10−19
ΔE = 5
...
% error = |theoretical −experimental | × 100
theoretical
% error =
5
...
99×10−19 × 100
5
...
39%
18
2
2
1
1
4
...
178 x 10(1/1
1/∞
) >=
E
18
2
...
I calculated how much energy it would take to move hydrogen's valence electron, which is
found in the first energy level, to the infinite energy level, or out of the atom
...
Next I
plugged infinity into n upper in Bohr’s equation because that is the energy level the electron got
excited too, to be ejected from the atom
...
6
...
178 x 10 ( 1/3
1/5
) >
1
...
548 x 10 = (6
...
548 x 10 / 6
...
435 x 10
m/s > avelength ( C = λv )
W
= (3
...
435 x 10
x λ > λ = 3
...
435 x 10
>
1
...
Lyman series calculation,
energy from electron falling from the 3rd energy level to the
18
2
2
18
1
1
1st energy level: ( ΔE = R′(n2lower − n2upper ) ) = 2
...
452 x 10 J
18
34)
18
34
> Frequency ( E = vh )
1
...
36 x 10 x
V > V = 1
...
36 x 10
15
8
15
> V = 2
...
0 x 10
W
:
(
) = 2
...
0 x 10
/ 2
...
3 x 10
M: this light is on the ultraviolet radiation region
of the electromagnetic spectrum
...
Energy from energy level 5 4: E = R′(n2lower − n2upper ) >
Δ
E = 2
...
9 x 10
18
2
2
1
1
Energy from energy level 2 1: E = R′(n2lower − n2upper >
Δ
E = 2
...
63 x 10
More energy is given off when an electron is transferred from the 2nd to the 1st energy level,
than when an electron is transferred from the 5th to the 4th energy level
...
9
...
This unique emission spectra is unique do to the
fact that each element has a different number of electrons, and therefore absorb and emit
energy differently
...
Scientists can use the emission spectra to determine the composition of stars by looking at
them through spectrometers, to the determine their emission spectra, and then matching the
emission spectra of the star with the emission spectras of known elements, thus telling scientists
exactly what stars are made of
...
Emission:
A spectrum that shows only the wavelengths of the photons released by certain
electrons as they fall back to their ground energy state
...
Continuous spectra
: Virtually impossible to achieve, a spectrum is which all the wavelengths of
the selected region have intensities ( for example: perfectly white light is a continuous visible
light spectra)
Sources:
http://hyperphysics
...
gsu
...
html
http://education
...
com/spectroscopyidentifyelements3503
Title: Wave length / Bohr model full lab report
Description: I got a 100 on this lab
Description: I got a 100 on this lab