🤓 Based on our data, we think this question is relevant for Professor Gold's class at UTSA.
We are being asked if the species is paramagnetic or diamagnetic so we have to determine the electron configuration of Fe3+ ion.
Recall that paramagnetic species have 1 or more unpaired electrons while diamagnetic contains 0 unpaired electrons.
Write the electron configuration of a neutral (uncharged) Fe atom.
Ground-state means that Iron is in its lowest energy form (not in an excited state).
Neutral element: Atomic number = # protons = # of electrons
Neutral Iron (Fe):
• Atomic number = 26
• # of electrons = 26 e-
Is the following ion diamagnetic or paramagnetic?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Paramagnetic and Diamagnetic concept. You can view video lessons to learn Paramagnetic and Diamagnetic. Or if you need more Paramagnetic and Diamagnetic practice, you can also practice Paramagnetic and Diamagnetic practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Gold's class at UTSA.