Atomic orbitals are regions of space around an atomic nucleus where electrons are likely to be found. There are several types of atomic orbitals, each designated by a specific letter and shape:

S orbitals (spherical shape): S orbitals are spherically symmetric and have no directional orientation. They are the simplest type of atomic orbitals and can hold up to 2 electrons.

P orbitals (dumbbell shape): P orbitals have a dumbbell or peanut shape and come in three orientations: px, py, and pz. They are oriented along the x, y, and z axes, respectively, and can hold up to 6 electrons (2 electrons in each orientation).

D orbitals (complex shapes): D orbitals have more complex shapes and come in five orientations: dxy, dyz, dzx, dx^2-y^2, and dz^2. They have two lobes with a doughnut-like shape and can hold up to 10 electrons (2 electrons in each orientation).

F orbitals (complex shapes): F orbitals have even more complex shapes and come in seven orientations: fxyz, fx(x^2-y^2), fy(3x^2-y^2), fz(x^2-y^2), f(x^2-3y^2)z, fxyz^2, and fz^3. They have multiple lobes and can hold up to 14 electrons (2 electrons in each orientation).

These atomic orbitals combine to form the electron cloud or electron density distribution around an atom, defining the electron's probable location in three-dimensional space according to the quantum mechanical model of the atom.
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