For elements 1-36, there are two exceptions to the filling...

For elements $1-36$, there are two exceptions to the filling order as predicted from the periodic table. Draw the atomic orbital diagrams for the two exceptions and indicate how many unpaired electrons are present.

Key Concepts

Electron Configuration

Electron configuration is the arrangement of electrons in an atom's orbitals and shells. It follows a set of rules that predicts how electrons fill orbitals based on their energy levels and distinguishes between different elements by this unique arrangement.

Aufbau Principle

The Aufbau principle is a rule that electrons occupy the lowest energy orbitals available before filling higher ones. This principle is used to build an atom’s electron configuration sequentially, although there are notable exceptions where the energetics of electron-electron interactions lead to deviations.

Hund's Rule

Hund's rule states that when electrons occupy degenerate orbitals (orbitals of equal energy), they will fill each orbital singly before any orbital is doubly occupied. This minimizes electron repulsion and maximizes total electron spin, influencing the number of unpaired electrons in an atom.

Pauli Exclusion Principle

The Pauli exclusion principle notes that no two electrons in an atom can have the same set of quantum numbers, meaning each orbital can hold a maximum of two electrons with opposite spins. This principle is fundamental in determining the structure of electron configurations and orbital diagrams.

Orbital Diagram

An orbital diagram is a visual representation of an atom's electron configuration where each orbital is drawn as a box and electrons are depicted by arrows indicating their spins. This diagram shows how electrons fill the various energy levels and orbitals, and it highlights the presence of unpaired electrons.

Unpaired Electrons

Unpaired electrons refer to electrons that reside alone in an orbital rather than as a paired spin with another. The count of unpaired electrons in orbital diagrams is important for understanding an element's magnetic properties and its behavior in chemical reactions.

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