Final answer:
The correct electron configuration for fluorine (F) is 1s² 2s² 2p⁵. A p orbital can hold a maximum of six electrons. The arrow notation for nitrogen shows one electron in each of the three 2p orbitals, following Hund's rule.
Step-by-step explanation:
The correct electron configuration for the element fluorine (F) is 1s² 2s² 2p⁵. Fluorine has nine electrons, and according to quantum theory, these electrons are distributed over different energy levels and sublevels. The first two electrons fill the 1s sublevel, the next two occupy the 2s sublevel, and the remaining five electrons are assigned to the 2p sublevel.
Regarding the maximum number of electrons that a p orbital can hold, the answer is six. Each p sublevel consists of three orbitals, and since each orbital can hold two electrons with opposite spins, the p sublevel can accommodate a total of six electrons.
For nitrogen (atomic number 7), the arrow notation that depicts its electron configuration would be as follows: 1s (††) 2s (††) 2p (†)(†)(†). This reflects that nitrogen has a fully filled 1s and 2s subshells, with one electron in each of the three 2p orbitals, adhering to Hund's rule of maximum multiplicity.