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The Periodic Table: Classification of Elements · Paper 1 — Free Chemistry HL Practice Questions
1FoundationMCQPeriodic trends: Atomic radius, ionization energy, electronegativity1 markPaper 1~2 min
Across Period 2, atomic radius generally decreases from lithium to fluorine. Which of the following correctly explains why neon is excluded from this trend, and what is the smallest atomic radius among the elements Li to F?
Solutions
2FoundationMCQPeriodic trends: Atomic radius, ionization energy, electronegativity1 markPaper 1~2 min
Which statement correctly explains why chlorine has a higher first ionization energy than iodine?
Solutions
3FoundationMCQPeriodic trends: Atomic radius, ionization energy, electronegativity1 markPaper 1~2 min
Across Period 2, electronegativity generally increases from lithium to fluorine. Which of the following best explains why fluorine has a higher electronegativity than nitrogen?
Solutions
4MasteryMCQPeriodic trends: Atomic radius, ionization energy, electronegativity1 markPaper 1~2 min
The first ionization energies of successive elements in Period 3 are given below.
Element — Na — Mg — Al — Si — P — S — Cl — Ar
IE₁ / kJ mol⁻¹ — 496 — 738 — 578 — 786 — 1012 — 1000 — 1251 — 1520
Which statement best explains why the first ionization energy of Al is lower than that of Mg?
Solutions
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