Final answer:
The 6p sublevel contains three orbitals, the same as all p sublevels. Each of these orbitals can hold up to 2 electrons, allowing for a total capacity of 6 electrons when fully filled. These orbitals are filled in accordance with Hund's rule.
Step-by-step explanation:
The 6p sublevel, like all p sublevels irrespective of the principal quantum number (n), consists of three orbitals. This is defined by the quantum number l (azimuthal quantum number) which equals 1 for p orbitals. As such, for any n-value (where n is the shell number), when l = 1, it signifies that the sublevel is a p sublevel with three distinct orbitals
These orbitals can each hold two electrons, according to Pauli's exclusion principle, resulting in a total capacity of six electrons in a fully filled 6p sublevel. These three 6p orbitals are often denoted as 6px, 6py, and 6pz, each representing an orientation in three-dimensional space. The distinguishing feature among them is their spatial orientation, but their energy levels are usually the same.
Electrons populate these orbitals following Hund's rule, which suggests that each orbital must be singly occupied before any orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. As a result, when discussing the sixth electron in a p sublevel, it will enter the second p orbital maintaining the same spin as the fifth electron as per Hund's rule.