IB Chemistry SL 3.1.2 Electron Configuration and Periodic Position

Practise translating between an element's electron configuration and its place in the periodic table. Use the highest occupied principal level for period, valence and subshell…

Syllabus
First assessment 2025
Objective
3.1.2
Level
SL

Exam points

  • use the highest occupied principal level to determine an element's period
  • deduce group and block from valence-electron count and the highest occupied sublevel
  • construct a full or condensed configuration from atomic number and periodic position

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.

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