Worksheet: Electron Energy Level Transitions

In this worksheet, we will practice calculating the energy of the photon that is absorbed or released when an electron transitions from one atomic energy level to another.

Q1:

The diagram shows the binding energy of each energy level of a hydrogen atom. If an electron is in the ground state, what frequency of photon must it absorb in order to move to the energy level 𝑛 = 3 ? Use a value of 4 . 1 4 × 1 0    eV⋅s for the value of the Planck constant. Give your answer to 3 significant figures.

  • A 3 . 2 9 × 1 0   Hz
  • B 2 . 9 2 × 1 0   Hz
  • C 8 . 2 1 × 1 0   Hz
  • D 3 . 6 5 × 1 0   Hz
  • E 4 . 5 7 × 1 0   Hz

Q2:

The diagram shows the emission spectrum of hydrogen for the visible part of the electromagnetic spectrum. The table shows the binding energies for the different energy levels of a hydrogen atom.

Energy Level 1 2 3 4 5
Binding Energy (eV) − 1 3 . 6 − 3 . 4 0 − 1 . 5 1 − 0 . 8 5 0 − 0 . 5 4 4

Between which two energy levels must an electron transition in order to produce the emission line marked 𝐷 on the diagram?

  • A 4 → 3
  • B 4 → 1
  • C 4 → 2
  • D 3 → 2
  • E 3 → 1

Between which two energy levels must an electron transition in order to produce the emission line marked 𝐵 on the diagram?

  • A 4 → 2
  • B 5 → 2
  • C 4 → 3
  • D 5 → 4
  • E 5 → 3

Q3:

The diagram shows four possible transitions that an electron can make between the energy levels of a hydrogen atom. What name is given to this series of transitions?

  • AThe Brackett series
  • BThe Balmer series
  • CThe Lyman series
  • DThe Paschen series
  • EThe Pfund series

Q4:

The diagram shows the binding energy of each energy level of a hydrogen atom. If an electron is in the ground state, what energy level would it transition to if it absorbed a photon with a wavelength of 97.4 nm? Use a value of 4 . 1 4 × 1 0    eV⋅s for the value of the Planck constant.

Q5:

The diagram shows four possible transitions that an electron can make between the energy levels of a hydrogen atom. What name is given to this series of transitions?

  • AThe Paschen series
  • BThe Lyman series
  • CThe Pfund series
  • DThe Balmer series
  • EThe Brackett series

Q6:

The diagram shows the transition of an electron in a hydrogen atom from 𝑛 = 3 to 𝑛 = 2 , emitting a photon as it does so.

What is the energy of the photon?

What is the wavelength of the photon? Use a value of 4 . 1 4 × 1 0    eV⋅s for the value of the Planck constant. Give your answer to 3 significant figures.

Q7:

The diagram shows the binding energy of each energy level of a hydrogen atom. If an electron is in the ground state, what wavelength of photon must it absorb in order for the hydrogen atom to become completely ionized? Use a value of 4 . 1 4 × 1 0    eV⋅s for the value of the Planck constant. Give your answer to 3 significant figures.

Q8:

The diagram shows four possible transitions that an electron can make between the energy levels of a hydrogen atom. What name is given to this series of transitions?

  • AThe Pfund series
  • BThe Brackett series
  • CThe Paschen series
  • DThe Balmer series
  • EThe Lyman series

Q9:

The diagram shows the transition of an electron in a hydrogen atom from 𝑛 = 2 to 𝑛 = 1 , emitting a photon as it does so.

What is the energy of the photon in electron volts?

What is the energy of the photon in joules? Give your answer to 3 significant figures.

  • A 2 . 1 8 × 1 0    J
  • B 1 . 6 3 × 1 0    J
  • C 5 . 4 4 × 1 0    J
  • D 1 . 3 6 × 1 0    J
  • E 2 . 7 2 × 1 0    J

Q10:

The diagram shows the transition of an electron in a hydrogen atom from 𝑛 = 4 to 𝑛 = 2 , emitting a photon as it does so.

What is the energy of the photon in electron volts?

What is the energy of the photon in joules? Use a value of − 1 . 6 0 × 1 0    C for the charge of an electron. Give your answer to 3 significant figures.

  • A 1 . 3 6 × 1 0    J
  • B 5 . 4 4 × 1 0    J
  • C 4 . 0 8 × 1 0    J
  • D 1 . 0 6 × 1 0    J
  • E 3 . 0 2 × 1 0    J

Q11:

The diagram shows the transition of an electron in a hydrogen atom from 𝑛 = 3 to 𝑛 = 1 , emitting a photon as it does so.

What is the energy of the photon? Give your answer to 3 significant figures.

  • A 12.1 eV
  • B 3.40 eV
  • C 10.2 eV
  • D 1.51 eV
  • E 2.55 eV

What is the frequency of the photon? Use a value of 4 . 1 4 × 1 0    eV⋅s for the value of the Planck constant. Give your answer to 3 significant figures.

  • A 3 . 6 5 × 1 0   Hz
  • B 8 . 1 2 × 1 0   Hz
  • C 6 . 1 6 × 1 0   Hz
  • D 2 . 9 2 × 1 0   Hz
  • E 2 . 4 6 × 1 0   Hz

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