In an atom, the atomic number represents the number of protons in the nucleus, which also determines the number of electrons in a neutral atom. When considering the p-subshell, it refers to the set of orbitals within the p sublevel.
Each orbital in the p-subshell can hold a maximum of 2 electrons. There are three p orbitals labeled as px, py, and pz, which correspond to different spatial orientations.
The number of unpaired electrons in a p-subshell depends on the specific electron configuration of the atom. If we know the atomic number of the element, we can determine the electron configuration and, subsequently, the number of unpaired electrons.
For example, in the case of nitrogen (atomic number 7), its electron configuration is 1s² 2s² 2p³. This means that in the 2p subshell of nitrogen, there are three electrons. Since each p orbital can hold two electrons, there are two paired electrons in two of the orbitals (px and py), and one unpaired electron in the remaining orbital (pz).
In general, for any element, the number of unpaired electrons in a p-subshell can range from zero to a maximum of six, depending on the specific electron configuration and the filling of the orbitals within the p-subshell.