🤓 Based on our data, we think this question is relevant for Professor Ratliff's class at USF.
We’re being asked to show the electron configuration of vanadium and its 3+ ion to show why they are paramagnetic
Recall that for:
• diamagnetic: all of the electrons are paired
• paramagnetic: at least one electron is unpaired
To do so, we need to do the following steps:
Step 1: Determine the shorthand e– config. of the neutral element.
Step 2: Determine the e– config. of the ion.
Step 3: Draw the orbital diagram for the outermost sublevel and determine if the ion is diamagnetic or paramagnetic
Note that for a neutral element, Atomic Number = # of protons = # of electrons.
Both vanadium and its 3+ ion are paramagnetic.
Use electron configurations to explain why vanadium and its 3 + ion are 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 Ratliff's class at USF.