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8)Consider the following graph:n-5n-4-52-82-146Brackettseriesn 3Paschenseriesorbitalenergieskj/mol328n-2BalmerSeries-1312Lyman seriesa)What is the minimum amount of energy to needed to completely eject an electron of ahydrogen atom from the first energy shell (which is a 1s orbital), to yield a free electron?b)What is the minimum amount of energy needed to promote an electron of an exitedhydrogen atom from the 3rd to the 4th energy level?If an electron in an excited hydrogen atom is occupying the 5th energy level and thenrelaxes back to the ground state, how much energy is released in the form ofelectromagnetic radiation?c)d)Consider the energy gaps between the energy levels in the graph above. Do the relativeenergies of the shells converge or diverge as n increases. Why might the observed trendoccur?e)Indicate which orbital transitions are associated with the 4 lines in the visible hydrogenline spectrum

Question
8)
Consider the following graph:
n-5
n-4
-52
-82
-146
Brackett
series
n 3
Paschen
series
orbital
energies
kj/mol
328
n-2
Balmer
Series
-1312
Lyman series
a)
What is the minimum amount of energy to needed to completely eject an electron of a
hydrogen atom from the first energy shell (which is a 1s orbital), to yield a free electron?
b)
What is the minimum amount of energy needed to promote an electron of an exited
hydrogen atom from the 3rd to the 4th energy level?
If an electron in an excited hydrogen atom is occupying the 5th energy level and then
relaxes back to the ground state, how much energy is released in the form of
electromagnetic radiation?
c)
d)
Consider the energy gaps between the energy levels in the graph above. Do the relative
energies of the shells converge or diverge as n increases. Why might the observed trend
occur?
e)
Indicate which orbital transitions are associated with the 4 lines in the visible hydrogen
line spectrum
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8) Consider the following graph: n-5 n-4 -52 -82 -146 Brackett series n 3 Paschen series orbital energies kj/mol 328 n-2 Balmer Series -1312 Lyman series a) What is the minimum amount of energy to needed to completely eject an electron of a hydrogen atom from the first energy shell (which is a 1s orbital), to yield a free electron? b) What is the minimum amount of energy needed to promote an electron of an exited hydrogen atom from the 3rd to the 4th energy level? If an electron in an excited hydrogen atom is occupying the 5th energy level and then relaxes back to the ground state, how much energy is released in the form of electromagnetic radiation? c) d) Consider the energy gaps between the energy levels in the graph above. Do the relative energies of the shells converge or diverge as n increases. Why might the observed trend occur? e) Indicate which orbital transitions are associated with the 4 lines in the visible hydrogen line spectrum

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Step 1

a)

The minimum amount of energy needed to completely eject an electron of a hydrogen atom from the first energy shell (1s or or n=1) can be calculated using the Bohr\'s equation to yield a free electron. The calculation of energy using the bohr equation is given in figure- 

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Step 2

b) 

The minimum amount of energy neede to promomt an electron of an excited hydrogen atom from...

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