Problem: Identify whether the ions are diamagnetic or paramagnetic.a. Cd2+b. Au+c. Mo3+d. Zr2+

FREE Expert Solution

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



For Cd2+:


The shorthand e config. for Cd2+ is:


Cd2+: [Kr]4d10 



The orbital diagram for Cd2+ is:



Since there are no unpaired electrons, Cd2+ is diamagnetic.




For Au+:


The shorthand e config. for Au+ is:

Au+: [Ar]4s25d8


The orbital diagram for Au+ is:




Since there are 2 unpaired electrons, Au+ is paramagnetic.


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Problem Details

Identify whether the ions are diamagnetic or paramagnetic.
a. Cd2+
b. Au+
c. Mo3+
d. Zr2+

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