Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. a. Cd²⁺ b. Au⁺ c. Mo³⁺ d. Zr²⁺

Orbital diagrams visually represent the distribution of electrons in an atom's orbitals. Each orbital can hold a maximum of two electrons with opposite spins, and the diagram helps illustrate how electrons fill these orbitals according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Understanding how to construct these diagrams is essential for determining the electron configuration of ions.

Diamagnetism and paramagnetism are properties that describe how materials respond to magnetic fields. Diamagnetic substances have all their electrons paired, resulting in no net magnetic moment and a weak repulsion from magnetic fields. In contrast, paramagnetic substances have unpaired electrons, leading to a net magnetic moment and a weak attraction to magnetic fields, which is crucial for identifying the magnetic properties of ions.

The electron configuration of ions is derived from the neutral atom's configuration, adjusted for the loss or gain of electrons. For cations, electrons are removed from the outermost orbitals first, which can affect the overall electron arrangement. Understanding how to write the electron configuration for ions is vital for constructing their orbital diagrams and determining their magnetic properties.