An element has completely filled n = 1 and n = 2 shells and has six electrons in the n = 3 shell. Identify the element and its major group (i.e., main group, transition, etc.). Is it a metal or a nonmetal? Identify the orbital in which the last electron is found.

Electron configuration describes the distribution of electrons in an atom's orbitals. For the given element, the filled n = 1 and n = 2 shells indicate that these orbitals are fully occupied, while the presence of six electrons in the n = 3 shell suggests a configuration of 3s² 3p⁴, which corresponds to the element sulfur.

Elements are organized into groups on the periodic table based on their electron configurations and chemical properties. The element with six electrons in the n = 3 shell belongs to Group 16 (the chalcogens), which is classified as a main group element. This classification helps in predicting the element's reactivity and bonding behavior.

Metals and nonmetals are distinguished by their physical and chemical properties. Nonmetals, such as sulfur, typically have higher electronegativities and are poor conductors of heat and electricity. In this case, sulfur is a nonmetal, and the last electron is found in the 3p orbital, indicating its position in the p-block of the periodic table.