Structure 3.1—The periodic table: Classification of elements: Practice Questions

Which group of the periodic table is correctly matched with its general name?

An element has a first ionization energy of \( 496 \text{ kJ mol}^{-1} \) and a second ionization energy of \( 4562 \text{ kJ mol}^{-1} \). In which block of the periodic table is this element found?

Which statement accurately describes the trend in the acid-base character of the highest oxides of Period 3 elements?

An element has the electron configuration $$[Ne] 3s^2 3p^4$$. In which block of the periodic table is this element found?

Periodic trends are based on the effective nuclear charge and the distance of valence electrons from the nucleus. Which equation correctly represents the first electron affinity of chlorine?

Describe the general trend in atomic radius as you move from left to right across a period in the periodic table.

Explain why magnesium has a higher first ionization energy than sodium.

Explain why the reactivity of non-metals generally increases across a period, while the reactivity of metals generally decreases across the same period.

Define atomic radius. Describe and explain the general trend in atomic radius for elements across Period 3 of the periodic table.

Consider the period 3 elements sodium (Na), magnesium (Mg), and phosphorus (P).
a) Define the term first ionization energy and write the chemical equation for the first ionization of phosphorus, including state symbols. (2)
b) Compare and explain the difference in atomic radius between sodium and magnesium. (2)
c) Explain why magnesium has a higher first ionization energy than sodium, despite sodium being in the same period. (1)