ConceptConceptDocsDocuments

IB Chemistry HL 3.1.2 Electron configuration and periodic position Question Bank

Practise IB Chemistry HL 3.1.2 by analysing electron configurations and inferring periodic position and chemical behaviour.

Syllabus
First assessment 2025
Course
Chemistry HL
Level
HL

Exam points

  • Deduce group, period and block from a full or abbreviated electron configuration.
  • Analyse sublevel filling and valence electrons to compare elements in a period or group.
  • Evaluate a proposed configuration by checking electron count, orbital order and periodic location.

3.1.2—Electron configuration and position question 1

[Maximum number: 2]

Iron rusts in the presence of oxygen and water. Rusting is a redox process involving several steps that produces hydrated iron(III) oxide, Fe2O3∙nH2O\mathrm{Fe}_{2} \mathrm{O}_{3} \bullet \mathrm{nH}_{2} \mathrm{O}, as the final product. The half-equations involved for the first step of rusting are given below.

Half-equation 1: Fe(s)→Fe2+(aq)+2e−\quad \mathrm{Fe}(\mathrm{s}) \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-}

Half-equation 2: O2(aq)+4e−+2H2O(l)→4OH−(aq)\quad \mathrm{O}_{2}(\mathrm{aq})+4 \mathrm{e}^{-}+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow 4 \mathrm{OH}^{-}(\mathrm{aq})

State the relationship between the electron arrangement of an element and its group and period in the periodic table.

All question bank results loaded