Paramagnetism and Diamagnetism: Videos & Practice Problems
Write the condensed electron configuration for the nickel (III) ion and state if it is paramagnetic or diamagnetic.
Write the condensed electron configuration for the copper (I) ion and is it magnetic?
; Diamagnetic
; Diamagnetic
; Paramagnetic
; Paramagnetic
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Paramagnetism and diamagnetism are distinguished by the presence or absence of unpaired electrons in an atom or ion's electron configuration. According to the Pauli exclusion principle, each orbital can hold a maximum of two electrons with opposite spins. Paramagnetic substances have at least one unpaired electron in their orbitals, which causes them to be attracted to magnetic fields. In contrast, diamagnetic substances have all their electrons paired, meaning every orbital contains two electrons with opposite spins, resulting in no net magnetic moment. Understanding whether an element or ion is paramagnetic or diamagnetic requires analyzing its electron configuration to identify unpaired electrons.
The Pauli exclusion principle states that an orbital can hold a maximum of two electrons, and these electrons must have opposite spins. This principle is fundamental in determining whether a substance is paramagnetic or diamagnetic. If all electrons in an atom or ion are paired with opposite spins in their orbitals, the substance is diamagnetic and not attracted to magnetic fields. However, if there is at least one electron that is unpaired (not paired with an electron of opposite spin in the same orbital), the substance is paramagnetic and will be attracted to magnetic fields. Thus, the Pauli exclusion principle helps explain the electron pairing that influences magnetic properties.
Paramagnetic substances have at least one unpaired electron in their orbitals, which creates a net magnetic moment because unpaired electrons have magnetic spins that do not cancel out. When placed in an external magnetic field, these unpaired electrons align with the field, causing the substance to be attracted to it. On the other hand, diamagnetic substances have all electrons paired, meaning their magnetic moments cancel each other out. As a result, diamagnetic substances do not have a net magnetic moment and are not attracted to magnetic fields; in fact, they are slightly repelled. This difference in electron pairing explains the contrasting magnetic behaviors.
To determine if an element or ion is paramagnetic or diamagnetic, first write out its electron configuration. Then, examine the orbitals to see if there are any unpaired electrons. If at least one electron is unpaired in any orbital, the species is paramagnetic. If all electrons are paired, meaning each orbital contains two electrons with opposite spins, the species is diamagnetic. For example, oxygen (O) has the electron configuration 1s2 2s2 2p4, where the 2p orbitals contain unpaired electrons, making oxygen paramagnetic. This method applies to both neutral atoms and ions.
Unpaired electrons are crucial in determining the magnetic properties of substances. Each unpaired electron has a magnetic moment due to its spin, which contributes to the overall magnetism of the atom or ion. When unpaired electrons are present, their magnetic moments do not cancel out, resulting in a net magnetic moment that causes the substance to be attracted to magnetic fields, a property known as paramagnetism. Conversely, if all electrons are paired, their magnetic moments cancel each other, and the substance exhibits diamagnetism, meaning it is not attracted to magnetic fields. Therefore, the presence or absence of unpaired electrons directly influences whether a substance is paramagnetic or diamagnetic.
