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Planck's Quantum Hypothesis

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Question

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 $E_{2}$ ?

A

+ 66 e V

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B

+ .98 e V

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C

+ 1.87 e V

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D

- 10.2 e V

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E

+ 12.08 e V

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Solution

The correct option is C $+ 1.87 e V$
The energy emitted is given by:
$Δ E = E_{3} - E_{2}$
$Δ E = - 1.52 - (- 3.39) = + 1.87 e V$

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Similar questions

Q. 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}

E_{3}

?

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}

?

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. Hydrogen atom emits blue light when an electron in it jumps from

n = 4

energy level to

n = 2

energy level. Which colour of light would the atom emit when an electron in it jumps from

n = 5

n = 2

Q. An excited electron in

n = 5

emits enough energy to fall to

n = 2

.
What is the wavelength associated with this energy emission?

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