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IB Chemistry HL 1.3 Electron Configurations Questions

Practise IB Chemistry HL 1.3 with evidence-led questions on electron configurations, spectra, orbitals and ionisation energy.

Syllabus
First assessment 2025
Course
Chemistry HL
Level
HL

Exam points

  • Interpret emission spectra as evidence of quantized electron-energy transitions and compare photon energies.
  • Assign electrons to principal levels, sublevels and orbitals using capacities, filling order and spin rules.
  • Use orbital diagrams and configurations to compare paired and unpaired electrons in atoms and ions.
  • Interpret first and successive ionization-energy data using shell structure, shielding, sublevels and electron pairing.

Covered syllabus points

1.3.1—Emission spectra1.3.2—Hydrogen emission spectrum1.3.3—Main energy levels1.3.4—Sublevels1.3.5—Orbitals and electron spin1.3.6 (HL)—Ionization energy (IE)1.3.7 (HL)—Successive ionization energies

Learn this topic

Study 1.3 Electron configurations conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

Question 1

[Maximum number: 1]

Carbon is produced by fusion reactions in stars.

Outline how the spectra of light from stars can be used to detect the presence of carbon.

Question 2

[Maximum number: 3]

Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds.

Question (a)

(a)

Magnesium ions produce no emission or absorption lines in the visible region of the electromagnetic spectrum. Suggest why most magnesium compounds tested in a school laboratory show traces of yellow in the flame.

[ 1 ]

Question (b)

(b)

Explain the convergence of lines in a hydrogen emission spectrum.

[ 1 ]

Question (c)

(c)

State what can be determined from the frequency of the convergence limit.

[ 1 ]

Question 3

[Maximum number: 1]

What is the maximum number of electrons in energy level n = 4?

A

8

B

18

C

32

D

50

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