Paramagnetic & Diamagnetic Elements - Paired & Unpaired Electrons

TL;DR

Learn how to determine if an element is paramagnetic or diamagnetic based on its electron configuration.

Transcript

in this video we're going to talk about how to determine if an element is paramagnetic or diamagnetic so what you need to know is this a paramagnetic element has unpaired electrons a diamagnetic element does not have any unpaired electrons so in order to determine this we need to write the electron configuration for argon the atomic number of argon... Read More

Key Insights

• ❓ Paramagnetic elements have unpaired electrons, while diamagnetic elements have only paired electrons.
• #️⃣ The electron configuration of an element can be determined by writing out the orbitals and filling them with the correct number of electrons.
• ❓ Argon is an example of a diamagnetic substance because its electron configuration does not have any unpaired electrons.
• ❓ Aluminum is a paramagnetic substance because it has one unpaired electron in its 3p orbital.
• ❓ Manganese is highly paramagnetic due to its five unpaired electrons in the 3d orbital.
• ❓ Electrons prefer to occupy their own orbitals instead of sharing with other electrons.
• 🏑 Paramagnetic substances are weakly attracted to an external magnetic field, while diamagnetic substances are weakly repelled.

Summary & Key Takeaways

• Paramagnetic elements have unpaired electrons, while diamagnetic elements do not.

• The electron configuration of an element can be used to determine its paramagnetic or diamagnetic nature.

• Argon is an example of a diamagnetic substance, while aluminum and manganese are examples of paramagnetic substances.