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

🤓 Based on our data, we think this question is relevant for Professor Demoin's class at UARK.

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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Based on our data, we think this problem is relevant for Professor Demoin's class at UARK.