Work through the list without notes. If you cannot do a statement, follow its link, then come back. Guide = study guide; Practice = practice questions.
Understanding
- I can explain why elements in the same group have similar properties, using their valence electron configurations. (Guide: “Why the periodic table repeats”)
- I can explain shielding and effective nuclear charge, and make a simple Z_eff estimate for a main-group atom. (Guide: “The model behind every trend”)
- I can use Coulomb’s law to say how nuclear charge and distance change the attraction for an outer electron. (Guide: “The model behind every trend”; Practice Q6)
- I can tell electron affinity apart from electronegativity. (Guide: “Electron affinity” and “Electronegativity”)
Skills
- I can put atoms in order of atomic radius from their positions on the periodic table. (Practice Q1)
- I can compare an atom with its ion, and order an isoelectronic series of ions by size. (Guide: Worked example 1; Practice Q7)
- I can predict the more electronegative of two elements, including diagonal pairs such as O and Cl. (Practice Q3)
- I can use successive ionization energies to find the number of valence electrons and the likely ion. (Practice Q4)
- I can estimate a missing value from neighbouring elements in a group or period. (Guide: Worked example 3; Practice Q6)
Reasoning
- I can explain the general rise in first ionization energy across a period and the fall down a group. (Practice Q5, Q6)
- I can explain the dips at groups 13 and 16 by naming the subshell or the electron pairing involved. (Guide: Worked example 2; Practice Q2, Q5)
- I can explain a trend with a cause (charge, distance, shielding, repulsion), not just describe its direction. (Practice Q5–Q7)
- I can evaluate a claim about atomic or ionic size and correct it with evidence. (Practice Q7)
All ticked? Move on to Topic 1.8, Valence Electrons and Ionic Compounds, or return to the course roadmap.