What are the sublevels in a period that contains 32 elements?

The sublevels in a period that contains 32 elements are 6s, 4f, 5d, and 6p. This particular arrangement of sublevels defines the sixth period of the periodic table, which is notably longer than earlier periods due to the inclusion of the f-block elements.

Understanding Periods and Sublevels

Periods in the periodic table represent the principal energy levels (n) of an atom's electrons. As you move down the periodic table from one period to the next, electrons fill higher energy shells and their associated sublevels. The number of elements in a period is determined by the maximum number of electrons that can occupy the sublevels available in that principal energy level, following the Aufbau principle.

For a period containing 32 elements, the electron filling order involves specific sublevels, which dictate the types of elements found within that period:

• s-sublevel (e.g., 6s): These orbitals can hold up to 2 electrons, corresponding to the two elements in the s-block (alkali metals and alkaline earth metals).
• f-sublevel (e.g., 4f): These orbitals can hold up to 14 electrons, corresponding to the 14 elements of the f-block (lanthanides or actinides). The 4f sublevel is filled in the sixth period.
• d-sublevel (e.g., 5d): These orbitals can hold up to 10 electrons, corresponding to the 10 elements of the d-block (transition metals). The 5d sublevel starts filling after the 4f sublevel in the sixth period.
• p-sublevel (e.g., 6p): These orbitals can hold up to 6 electrons, corresponding to the six elements in the p-block.

The Sixth Period: A Detailed Look

The period with 32 elements is the sixth period. Its unique length and composition are directly attributed to the sequence in which its sublevels are filled. This includes the introduction of the f-block elements (lanthanides), which adds 14 elements to the period's total count.

Below is a summary of periods, their element counts, and the sublevels involved:

As illustrated in the table, the sixth period clearly distinguishes itself with its comprehensive set of sublevels: 6s, followed by the deep 4f, then 5d, and finally 6p. This full complement of sublevels allows for the accommodation of 32 electrons, resulting in 32 unique elements within this period.