Final answer:
The highest occupied energy level of a neutral iodine atom is the fifth level, which includes the 5s and 5p sublevels, holding a total of 4 orbitals.
Step-by-step explanation:
To determine how many orbitals are in the highest occupied energy level of a neutral iodine atom, one must consider the electron configuration of iodine. Iodine has an atomic number of 53, meaning it has 53 protons and, in a neutral atom, 53 electrons. Its electron configuration up to the fourth energy level is [Kr]4d105s25p5.
The highest occupied energy level is therefore the fifth level (n=5), which includes the 5s and 5p sublevels. The 5s sublevel has 1 orbital, and the 5p sublevel has 3 orbitals, totaling 4 orbitals at the fifth energy level. Each orbital can hold a maximum of two electrons, meaning that the 5p sublevel, which is partially filled, contributes significantly to the chemical properties of iodine.