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Lesson: Energy Levels in the Bohr Model

Worksheet • 11 Questions

Q1:

Using the Bohr model, calculate the energy of an electron in the 𝑛 = 8 energy level of the hydrogen atom.

  • A βˆ’ 3 . 4 0 6 Γ— 1 0 βˆ’ 2 0 J
  • B βˆ’ 2 . 1 4 6 Γ— 1 0 βˆ’ 1 8 J
  • C βˆ’ 2 . 7 2 4 Γ— 1 0 βˆ’ 1 9 J
  • D βˆ’ 6 . 8 1 2 Γ— 1 0 βˆ’ 2 0 J
  • E βˆ’ 1 . 3 6 2 Γ— 1 0 βˆ’ 1 9 J

Q2:

The electron in a hydrogen atom occupies the energy level with 𝑛 = 3. Calculate the ionisation energy of this atom.

  • A 2 . 4 2 2 Γ— 1 0 βˆ’ 1 9 J
  • B 1 . 4 5 3 Γ— 1 0 βˆ’ 1 9 J
  • C 1 . 9 3 8 Γ— 1 0 βˆ’ 1 8 J
  • D 7 . 2 6 6 Γ— 1 0 βˆ’ 1 9 J
  • E 8 . 0 7 9 Γ— 1 0 βˆ’ 1 9 J

Q3:

The electron in a H e + ion occupies the energy level with 𝑛 = 7. Calculate the ionisation energy of this atom.

  • A 1 . 7 7 9 Γ— 1 0 βˆ’ 1 9 J
  • B 2 . 6 7 0 Γ— 1 0 βˆ’ 1 7 J
  • C 4 . 4 4 9 Γ— 1 0 βˆ’ 2 0 J
  • D 1 . 2 4 6 Γ— 1 0 βˆ’ 1 8 J
  • E 8 . 8 9 7 Γ— 1 0 βˆ’ 2 0 J

Q4:

Which of the following ions would have the same ionization energy as a hydrogen atom with an electron in the 𝑛 = 4 energy level?

  • AA L i 2 + ion with an electron in the 𝑛 = 1 2 energy level.
  • BA L i 2 + ion with an electron in the 𝑛 = 1 8 energy level.
  • CA H e + ion with an electron in the 𝑛 = 6 energy level.
  • DA H e + ion with an electron in the 𝑛 = 1 2 energy level.
  • EA B e 3 + ion with an electron in the 𝑛 = 1 8 energy level.

Q5:

Using the Bohr model, calculate the energy of an electron in the 𝑛 = 4 energy level of the L i 2 + ion.

  • A βˆ’ 1 . 2 2 6 Γ— 1 0 βˆ’ 1 8 J
  • B βˆ’ 4 . 9 0 5 Γ— 1 0 βˆ’ 1 8 J
  • C βˆ’ 5 . 4 5 0 Γ— 1 0 βˆ’ 1 9 J
  • D βˆ’ 3 . 8 7 5 Γ— 1 0 βˆ’ 1 8 J
  • E βˆ’ 1 . 6 3 5 Γ— 1 0 βˆ’ 1 8 J

Q6:

Using the Bohr model, calculate to 4 significant figures the lowest possible energy of an electron in the H e + ion.

  • A βˆ’ 8 . 7 1 9 Γ— 1 0 βˆ’ 1 8 J
  • B βˆ’ 5 . 4 5 0 Γ— 1 0 βˆ’ 1 9 J
  • C βˆ’ 4 . 3 6 0 Γ— 1 0 βˆ’ 1 8 J
  • D βˆ’ 1 . 0 9 0 Γ— 1 0 βˆ’ 1 8 J
  • E βˆ’ 2 . 1 8 0 Γ— 1 0 βˆ’ 1 8 J

Q7:

The electron in the 𝑛 = 3 energy level of a L i 2 + ion absorbs a photon and is promoted to the energy level with 𝑛 = 6 . In which of the following transitions would an electron absorb a photon of the same energy?

  • APromotion of an electron from 𝑛 = 2 to 𝑛 = 4 in the H e + ion.
  • BPromotion of an electron from 𝑛 = 2 to 𝑛 = 8 in the H e + ion.
  • CPromotion of an electron from 𝑛 = 2 to 𝑛 = 4 in the hydrogen atom.
  • DPromotion of an electron from 𝑛 = 2 to 𝑛 = 8 in the hydrogen atom.
  • EPromotion of an electron from 𝑛 = 1 to 𝑛 = 2 in the H e + ion.

Q8:

An electron in a hydrogen atom moves from the 𝑛 = 5 energy level to the 𝑛 = 2 energy level. Using the Bohr model, calculate the energy of the photon produced by this transition.

Q9:

The electron in the 𝑛 = 3 energy level of a H e + ion absorbs a photon and is promoted to the energy level with 𝑛 = 5 . Calculate the wavelength of the absorbed photon to 3 significant figures.

  • A 3 . 2 0 Γ— 1 0 βˆ’ 7 m
  • B 1 . 8 2 Γ— 1 0 βˆ’ 7 m
  • C 1 . 7 1 Γ— 1 0 βˆ’ 7 m
  • D 6 . 4 1 Γ— 1 0 βˆ’ 7 m
  • E 3 . 4 2 Γ— 1 0 βˆ’ 7 m

Q10:

The electron in the 𝑛 = 4 energy level of a hydrogen atom absorbs a photon and is promoted to the energy level with 𝑛 = 6. Calculate to 3 significant figures the wavelength of the absorbed photon.

  • A 2 . 6 2 Γ— 1 0 βˆ’ 6 m
  • B 9 . 3 7 Γ— 1 0 βˆ’ 8 m
  • C 1 . 0 9 Γ— 1 0 βˆ’ 6 m
  • D 4 . 5 6 Γ— 1 0 βˆ’ 8 m
  • E 4 . 5 6 Γ— 1 0 βˆ’ 9 m

Q11:

An electron in an excited hydrogen atom occupies the 𝑛 = 2 energy level. Using the Bohr model, calculate the ionization energy for the excited hydrogen atom.

  • A 5 . 4 5 0 Γ— 1 0 βˆ’ 1 9 J
  • B 2 . 4 2 2 Γ— 1 0 βˆ’ 1 9 J
  • C 2 . 7 2 5 Γ— 1 0 βˆ’ 1 9 J
  • D 7 . 2 6 6 Γ— 1 0 βˆ’ 1 9 J
  • E 1 . 0 9 0 Γ— 1 0 βˆ’ 1 8 J
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