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Emission and Absorption Spectra

The energy of...

Question

The energy of hydrogen atom in its ground state is $- 13.6 e V$ . The energy of the level corresponding to $n = 5$ is:

A

- 0.54 e V

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B

- 5.40 e V

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C

- 0.85 e V

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D

- 2.72 e V

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Solution

The correct option is A $- 0.54 e V$
For a hydrogen atom, the energies that an electron can have are given by the expression, $E = - \frac{13.6}{n^{2}} e V$ , where n is an integer.
For fifth energy level, $n = 5$
$E_{5} = - \frac{13.6}{5^{2}} e V = - 0.54 e V$ .

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Similar questions

Q. The energy of a hydrogen atom in its ground state is

- 13.6 e V

. The energy of the level corresponding to the quantum number

n = 5

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

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

what is the emission energy when it moves to

E_{5}

?

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?

Q. The ground state energy of hydrogen atom is

- 13.6 e V

. If an electron make a transition from an energy level

- 0.85 e V

- 1.51 e V

, calculate the wavelength of the spectral line emitted. To which series of hydrogen spectrum does this wavelength belong?

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