An atomic orbital is a region in an atom where there is a high probability of finding electrons. Atomic orbitals are defined by quantum numbers and have specific shapes and orientations.
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Atomic orbitals are characterized by the principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m_l), and spin quantum number (m_s).
The shape of an atomic orbital is determined by the azimuthal quantum number (l): s-orbitals are spherical, p-orbitals are dumbbell-shaped, d-orbitals have more complex shapes.
Each type of orbital can hold a maximum of two electrons with opposite spins, according to the Pauli exclusion principle.
Orbitals within a subshell are degenerate, meaning they have the same energy level.
Electron configurations follow the Aufbau principle, Hund's rule, and Pauli exclusion principle to fill orbitals in increasing order of energy.
Review Questions
What determines the shape of an atomic orbital?
How many electrons can an atomic orbital hold?
Explain what it means for orbitals within a subshell to be degenerate.