Assign a set of four quantum numbers to each electron in oxygen.

Quantum numbers are a set of four numbers that describe the unique quantum state of an electron in an atom. They include the principal quantum number (n), which indicates the energy level; the azimuthal quantum number (l), which defines the shape of the orbital; the magnetic quantum number (m_l), which specifies the orientation of the orbital; and the spin quantum number (m_s), which describes the electron's spin direction.

Electron configuration refers to the distribution of electrons in an atom's orbitals. For oxygen, which has eight electrons, the electron configuration is 1s² 2s² 2p⁴. This configuration helps determine how electrons fill the available orbitals according to the Aufbau principle, Pauli exclusion principle, and Hund's rule, which are essential for assigning quantum numbers.

The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers. This principle is crucial when assigning quantum numbers to electrons, as it ensures that each electron occupies a unique state within an atom, leading to the correct identification of their quantum numbers in the context of oxygen's electron configuration.