Final answer:
Elements can be grouped by their ionization energies into periods by recognizing that noble gases have high ionization energies, marking the end of a period, while alkali metals with low ionization energies mark the beginning. For instance, Period 1 includes hydrogen and helium, Period 2 includes lithium to neon, Period 3 includes sodium to argon, and Period 4 includes potassium to krypton.
Step-by-step explanation:
The question asks about grouping elements by their ionization energies into four consecutive periods, with the range of atomic numbers in each group. Ionization energy generally increases across a period and decreases down a group in the periodic table. The peaks and troughs described correspond to the noble gases (high ionization energies) and alkali metals (low ionization energies), respectively.
To group the elements into periods based on ionization energies:
- Period 1: H (1) and He (2)
- Period 2: Li (3) to Ne (10)
- Period 3: Na (11) to Ar (18)
- Period 4: K (19) to Kr (36)
Period 5 would continue in this manner from Rb (37) to Xe (54), and so on for higher periods. By identifying the noble gases with high ionization energies, we can delineate the end of a period, while the alkali metals mark the beginning. Please note that Period 4 includes the first row of transition metals, which can slightly complicate the pattern due to their unique electron configurations.