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E.1 Structure of the atom - IB Questionbank | RevisionDojo

Practice E.1 Structure of the atom with authentic IB Physics exam questions for both SL and HL students. This question bank mirrors Paper 1A, 1B, 2 structure, covering key topics like mechanics, thermodynamics, and waves. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of IB examiners.

Paper

Level

Question 1

SLPaper 2

The hydrogen atom can be modelled using the Bohr model.

Calculate the wavelength of light emitted when an electron transitions from the $n=5$ level to the $n=2$ level.

[3]

Sketch an energy level diagram showing this transition and label all levels from $n = 1$ to $n = 5$ .

[2]

Explain, using the Bohr model, why the energy levels become closer together at higher values of $n$ .

[2]

Question 2

SLPaper 1A

In the Bohr model, which of the following best describes the motion of electrons?

Question 3

SLPaper 1A

Which of the following is a feature of both the Rutherford model and the Bohr model?

Question 4

SLPaper 1A

Which of the following cannot be deduced from the results of the Geiger-Marsden-Rutherford experiment?

Question 5

SLPaper 1A

Electrons transition between energy states for $n=1,2,3,4,5$ in an atom. Some data regarding the photons emitted in the transitions is shown below.

Transition	Wavelength of Emitted Photon
5 → 1	$240\ \mathrm{nm}$
4 → 3	$710\ \mathrm{nm}$
3 → 1	$280\ \mathrm{nm}$
5 → 2	$310\ \mathrm{nm}$

What is the wavelength of the photon emitted in the transition between $n=3$ and $n=2$ ?

Question 6

HLPaper 1A

A hydrogen atom absorbs a photon of energy $12.1\ \mathrm{eV}$ . To which energy level is the electron most likely excited?

Question 7

HLPaper 2

The energy levels of hydrogen are given by $E_n = \dfrac{-13.6}{n^2}$ eV.

Calculate the energy of an electron in the $n = 4$ level.

[1]

Determine the energy of a photon emitted when the electron falls from $n = 4$ to $n = 2$ .

[2]

Determine the frequency of the emitted photon.

[2]

Outline why the hydrogen atom cannot emit photons of arbitrary energy.

[2]

Question 8

SLPaper 1A

Which of the following transitions in hydrogen will emit the photon with the greatest energy?

Question 9

HLPaper 2

The diagram shows the energy levels of an electron in a hydrogen atom. The energy values are given in kJ mol^-1 for different energy levels $n$ . The value at $n = \infty$ represents the ionization energy of the atom.

Calculate the energy difference, in kJ mol^-1, for the transition from $n = 4$ to $n = 2$ .

[1]

Determine the wavelength of the photon emitted during the $n = 4$ to $n = 2$ transition.

[3]

Identify the region of the electromagnetic spectrum this photon lies in.

[1]

Deduce whether the $n = 3 \rightarrow n = 2$ transition results in emission or absorption of radiation, and explain your answer.

[2]

Explain why the energy levels get closer together as $n$ increases.

[2]

Using the values on the diagram, determine the ionization energy of hydrogen in J per atom.

[2]

Question 10

HLPaper 2

Bohr’s model provided a framework to explain the hydrogen spectrum.

State two postulates of the Bohr model.

[2]

Explain why electrons in the Bohr model do not spiral into the nucleus.

[2]

Suggest why the Bohr model fails for atoms with more than one electron.

[2]

Topic A - Space, time and motion5 subtopics

Topic B - The particulate nature of matter5 subtopics

Topic C - Wave behaviour5 subtopics

Topic D - Fields4 subtopics

Topic E - Nuclear and quantum physics5 subtopics

E.1 Structure of the atom Questionbank