Paramagnetism and Diamagnetism - Video Tutorials & Practice Problems

Paramagnetism and Diamagnetism

Now recall that an orbital can hold a maximum of two electrons that pair up with opposite spins. Remember the opposite spins is part of the poly exclusion principle. Now, we have two terms paramagnetic versus diamagnetic with paramagnetic. This is when at least one electron in given orbitals is unpaired. And diamagnetic is when all electrons and given orbitals are paired, we're gonna realize that paramagnetic substances are also magnetic, meaning that they're influenced by a magnetic field. So if we take a look here, paramagnetic, if we look, we have an S orbital, all the electrons within that one orbital are paired up. But if we look at the p orbitals, we have this electron by itself in an orbital. So it's unpaired. And this one too, as long as you have one electron in an orbital by itself unpaired, it's paramagnetic for diamagnetic. If we look all the electrons in the S orbital are paired up, and then all the electrons in the P orbitals are paired up, there's not one electron by itself within a given orbital. So this is what is meant by diamagnetic. So just keep this in mind when doing the electron configurations of either elements or ions paramagnetic elements. And ions have at least one electron by itself in an orbital somewhere diamagnetic. Every single orbital has two electrons in it. All of the electrons are therefore paired up.

Paramagnetism and Diamagnetism Example

Here, it says to determine if the vanadium atom is paramagnetic or diamagnetic. So atom means that it's in its neutral form, vanadium is represented by the, if you look at the periodic table, its atomic number is 23. Here, its electron configuration would be argo 42 3d 1. If we look, we know that in S orbitals, there's only one orbital and they can hold a maximum of two electrons. So the four S orbital is already filled in with two electrons. RD sublevel has five orbitals. And here there's only one electron there. So vanadium has one electron by itself within or in orbital. So it's unpaired, meaning that the vanadium atom is paramagnetic. So just remember if you have at least one electron by itself in any given orbital, it's a paramagnetic species.

Which of the following atoms has the most unpaired electrons? 

• A. Co
• B. Mn
• C. Ti
• D. Zn
• E. Fe

Write the condensed electron configuration for the nickel (III) ion and state if it is paramagnetic or diamagnetic.

• A. [Ar]3d⁷; Paramagnetic
• B. [Ar]3d⁷; Diamagnetic
• C. [Ar]4s²3d⁵; Paramagnetic
• D. [Ar]4s²3d⁵; Diamagnetic

Write the condensed electron configuration for the copper (I) ion and is it magnetic?

• A. $\left[ Ar\right]4s^23d^9$ ; Diamagnetic
• B. $\left[Ar\right]3d^{10}$ ; Diamagnetic
• C. $\left[ Ar\right]4s^23d^9$ ; Paramagnetic
• D. $\left[ Ar\right]3d^{10}$ ; Paramagnetic