atomic spectrum hydrogen experiment

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D. The Balmer Series

1. When Balmer found his famous series for hydrogen in 1886, he was limited experimentally to wavelengths in the visible and near ultraviolet regions from 250 nm to 700 nm, so all the lines in his series lie in that region.

Based on the entries in Table 2 and the transitions on your energy level diagram, what common characteristic do the lines in the Balmer series have?



What would be the longest possible wavelength for a line in the Balmer series?
λ = ___________nm



What would be the shortest possible wavelength that a line in the Balmer series could have? Hint: What is the largest possible value of ΔE to be associated with a line in the Balmer series?



λ = ___________nm

The Ionization Energy of Hydrogen

1. In the normal hydrogen atom the electron is in its lowest energy state, which is called the ground state of the atom. The maximum electronic energy that an electron in a hydrogen atom can have is 0 kJ/mole, at which point it would essentially be removed from the atom and it would become a H+ ion. How much energy in kilojoules per mole does it take to ionize a hydrogen atom?

______________ kJ/mole

The ionization energy of hydrogen is often expressed in units other than kJ/mole. What would it be in joules per atom? in electron volts per atom? (1 ev = 1.602 x 10-19 J)

______________J/atom; _____________ ev/atom

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Explanation & Answer

Here is my answer :)

atomic spectrum hydrogen
experiment
Data & Calculations
A. Calculation of the Energy Levels of the Hydrogen Atom.
For this part, we have to use the next equation for the 10 lowest energy states:
𝐸𝑛 =

−1312.04
𝑘𝑗/𝑚𝑜𝑙
𝑛2
Table 1

Quantum Number (n)
1
2
3
4
5
6
7
8
9
10

Energy En in kJ/mol
-1312.04
-328.01
-145.78
-82.002
-52.482
-36.446
-26.776
-20.501
-16.198
-13.120

B. Calculation of Wavelengths in the Spectrum of the Hydrogen Atom:
For this part, we have to use the next equations:
∆𝐸 = 𝐸𝑛ℎ𝑖 − 𝐸𝑛𝑙𝑜
𝜆=

1.19627 ∗ 105
∆𝐸
Table 2

1
2
3
4
5

n higher
n lower
∆E
λ
∆E
λ
∆E
λ
∆E
λ
∆E
λ

6

5

4

3

2

1276
93.75
291.6
410.2
109.3
1094
45.56
2626
16.04
7458

1260
94.94
275.5
434.2
93.3
1282
29.52
4052

1230
97.26
246
486.3
63.78
1876

1166
102.6
182.2
656.5

984
121.6

1

C. Assigment of Wavelenghts
As directed in the procedure, assing nhi and nlo for each wavelength in Table 3 which corresponds to a
wavelength calculated in Table 2.
Table 3
Wavelenght
97.25
102.57
121.57
398.02
397.12

Assignment
4->1
3->1
2->1
-

Wavelenght
410.29
434.17
486.27
656.47
954.86

Assigment
6->2
5->2
4->2
3->2
-

Wavelenght
1005.2
1094.1
1282.2
1857.6
4052.3

Assigment
6->3
5->3
4->3
5->4

List below any remaining wavelengts you cannot yet assing
Wavelenght

∆𝐸𝑇𝑟𝑎𝑛𝑠𝑖𝑡𝑖𝑜𝑛

398.02
397.12
954.86
1005.2

307.5
301.2
125.3
119.0

Probable
Transition
8->2
7->2
8->3
7->3

D. The Balmer Series

1. When Balmer found his famous series for hydrogen in 1886, he was limited experimentally to
...


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