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Photoelectric Effect

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Question

Solve the following question which relates to the partial energy level diagram for the hydrogen electron:
$.54 e V$ ____________ $n_{5}$
$.85 e V$ ____________ $n_{4}$
$1.51 e V$ _________ $n_{3}$
$3.4 e V$ ____________ $n_{2}$
$13.6 e V$ ____________ $n_{1}$
The question relates to a hydrogen electron located at $E_{3}$ . What is the emission energy when the electron falls to $E_{2}$ from $E_{3}$ ?

A

\pm 66 e V

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B

\pm 966 e V

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C

\pm 1.89 e V

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D

\pm 10.2 e V

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E

\pm 12.09 e V

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Solution

The correct option is C $\pm 1.89 e V$
From the data given:
Energy of 3rd orbit, $E_{3} = 1.51$ $e V$
Also energy of 2nd orbit, $E_{2} = 3.4$ $e V$
Emission energy, $Δ E = \pm (1.51 - 3.4) = \pm 1.89$ $e V$

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Similar questions

Q. The following question relates to the partial energy level diagram for the hydrogen electron:

.54 e V

n_{5}

.85 e V

n_{4}

1.51 e V

n_{3}

3.4 e V

n_{2}

13.6 e V

n_{1}

The question relates to a hydrogen electron located at

E_{3}

.What is the emission energy when the electron falls to

E_{5}

E_{3}

?

Q. This question relates to the electron energy level diagram below. The questions are about a hydrogen electron located at

E_{3}

.38 e v

n = 6

-

.54 e v

n = 5

-

.85 e v

n = 4

-

1.52 e v

n = 3

-

3.39 e v

n = 2

-

13.6 e v

n = 1

what is the emission energy when it moves to

E_{2}

?

E_{4} = - 0.85 e V

E_{3} = - 1.5 e V

E_{2} = - 3.4 e V

E_{1} = - 13.6 e V

Consider the electron energy level diagram for hydrogen as shown above.
An electron in the ground state of hydrogen atom has an energy of -13.6eV. and 0 eV is the highest energy level present in a hydrogen atom. Identify which of the following energies not possible by photon emitted from hydrogen?

0.38 e v

n 6

0.54 e v

n 5

0.85 e v

n 4

1.52 e v

n 3

3.39 e v

n 2

13.6 e v

n 1

A hydrogen electron falls from the

n = 3

n = 1

energy level. Using the chart above, determine how much energy it must release:

Q. The ground state energy of hydrogen atom is -13.6 eV. If an electron makes a transition from an energy level -1.51 eV to -3.4 eV, calculate the wavelength of the spectral line emitted and name the series of hydrogen spectrum to which it belongs.

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