We’re being asked to classify each ion as diamagnetic or paramagnetic.
Recall that for:
• diamagnetic: all of the electrons are paired
• paramagnetic: at least one electron is unpaired
When filling up the orbitals, take note of:
• Aufbau Principle: totally fill in the lowest energy orbital first
• Hund’s Rule: electron orbitals that are degenerate (same energy orbital) are first half-filled before they are totally filled
The shorthand e– config. for Cd2+ is:
The orbital diagram for Cd2+ is:
Since there are no unpaired electrons, Cd2+ is diamagnetic.
The shorthand e– config. for Au+ is:
The orbital diagram for Au+ is:
Since there are 2 unpaired electrons, Au+ is paramagnetic.
Identify whether the ions are diamagnetic or paramagnetic.
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