Final answer:
The energy of an electron in a non-hydrogen atom is primarily determined by the principal (n) and angular momentum (l) quantum numbers, with n defining the shell and energy level, and l affecting the orbital shape.
Step-by-step explanation:
The energy of an electron in a non-hydrogen atom is largely determined by the principal quantum number (n) and the angular momentum quantum number (l). The principal quantum number defines the electron shell and generally corresponds to the energy level, with a larger n indicating a higher energy shell. In addition to n, the angular momentum quantum number l affects the shape of the electron's orbital, contributing to the energy state of the electron. Moreover, the orientation quantum number m (also known as magnetic quantum number) defines the orbital's orientation relative to the other orbitals within a subshell.
While the electron spin quantum number (ms) does affect the energy of the electron through interactions like spin-orbit coupling, it is the principal (n) and the angular momentum (l) quantum numbers that play a primary role in determining the energy states in an atom. For example, in a magnetic field, energy levels can split in a phenomenon known as the Zeeman effect, further illustrating the complexity of electron energy states beyond n and l.