Atomic Orbitals and Quantum States

This page delves deeper into atomic orbitals and quantum states of electrons.

The concept of wave functions is introduced, explaining that an electron's state is fully described by five quantum numbers. The difference between atomic orbitals (described by three quantum numbers) and spin orbitals (described by all five) is clarified.

Definition: An atomic orbital is a wave function described by the set of three quantum numbers n, l, and ml.

The page also explains orbital regions and introduces orbital notation, showing how quantum numbers correspond to specific orbital symbols.

Highlight: The notation 3d-2 represents an electron in the d orbital of the third shell with a magnetic quantum number of -2.

A formula for calculating the number of electrons in a shell or subshell is provided: 2(2l+1) = 4l+2.

Orbital Shapes and the Pauli Exclusion Principle

The final page visualizes the shapes of different types of orbitals, including s, p, and d orbitals.

Definition: An orbital contour is the surface of the smallest geometric shape outside of which the probability of finding an electron is negligible.

Diagrams illustrate the three-dimensional shapes of s, px, py, and pz orbitals, helping students visualize the spatial distribution of electrons in atoms.

The page concludes with an explanation of the Pauli exclusion principle, a fundamental concept in quantum mechanics:

Highlight: The Pauli exclusion principle states that no two electrons in an atom can have identical sets of all five quantum numbers.

This principle is crucial for understanding electron configuration and the structure of the periodic table.