View source for Magnetochemistry

{{short description|Study of magnetic properties of chemical compounds}}
'''Magnetochemistry''' is concerned with the magnetic properties of [[chemical compound]]s and [[Chemical element|elements]]. Magnetic properties arise from the spin and orbital angular momentum of the electrons contained in a compound. Compounds are [[diamagnetic]] when they contain [[electron pair|no unpaired electrons]]. Molecular compounds that contain one or more [[unpaired electron]]s are [[paramagnetic]]. The magnitude of the paramagnetism is expressed as an effective magnetic moment, μ<sub>eff</sub>. For first-row [[transition metal]]s the magnitude of μ<sub>eff</sub> is, to a first approximation, a simple function of the number of unpaired electrons, the spin-only formula. In general, [[spin–orbit coupling]] causes μ<sub>eff</sub> to deviate from the spin-only formula. For the heavier transition metals, [[lanthanide]]s and [[actinide]]s, spin–orbit coupling cannot be ignored. [[Exchange interaction]] can occur in clusters and infinite lattices, resulting in [[ferromagnetism]], [[antiferromagnetism]] or [[ferrimagnetism]] depending on the relative orientations of the individual spins.

==Magnetic susceptibility==
{{main article|Magnetic susceptibility}}
The primary measurement in magnetochemistry is magnetic susceptibility. This measures the strength of interaction on placing the substance in a magnetic field. The '''volume magnetic susceptibility''', represented by the symbol <math>\chi_v</math> is defined by the relationship
:<math>\vec{M} = \chi_v \vec{H}</math>
where, <math>\vec{M}</math> is the [[magnetization]] of the material (the [[magnetic dipole moment]] per unit volume), measured in [[ampere]]s per meter ([[International System of Units|SI]] units), and <math>\vec{H}</math> is the [[magnetic field#B and H|magnetic field strength]], also measured in amperes per meter. Susceptibility is a [[dimensionless quantity]]. For chemical applications the '''molar magnetic susceptibility''' (χ<sub>mol</sub>) is the preferred quantity. It is measured in m<sup>3</sup>·mol<sup>−1</sup> (SI) or cm<sup>3</sup>·mol<sup>−1</sup> (CGS) and is defined as
:<math>\chi_\text{mol} = M\chi_v/\rho</math>
where ρ is the [[density]] in kg·m<sup>−3</sup> (SI) or g·cm<sup>−3</sup> (CGS) and ''M'' is [[molar mass]] in kg·mol<sup>−1</sup> (SI) or g·mol<sup>−1</sup> (CGS).
[[File:Gouy bal.png|thumb|150px|Schematic diagram of Gouy balance]]

A variety of methods are available for the measurement of magnetic susceptibility.

* With the [[Gouy balance]] the weight change of the sample is measured with an [[analytical balance]] when the sample is placed in a homogeneous magnetic field. The measurements are [[calibrated]] against a known standard, such as mercury cobalt thiocyanate, HgCo(NCS)<sub>4</sub>. Calibration removes the need to know the density of the sample. Variable temperature measurements can be made by placing the sample in a [[cryostat]] between the pole pieces of the magnet.<ref>Earnshaw, p. 89</ref>
* The [[Evans balance]].<ref>[http://www.sherwood-scientific.com/msb/msbindex.html Magnetic Susceptibility Balances]</ref> is a [[torsion balance]] which uses a sample in a fixed position and a variable secondary magnet to bring the magnets back to their initial position. It, too, is calibrated against HgCo(NCS)<sub>4</sub>.
* With a [[Faraday balance]] the sample is placed in a magnetic field of constant gradient, and weighed on a torsion balance. This method can yield information on [[magnetic anisotropy]].<ref>{{cite book|last=O'Connor|first=C.J.|editor=Lippard, S.J.|title=Magnetic susceptibility measurements|series=Progress in Inorganic Chemistry|volume=29|year=1982|publisher=Wiley|isbn= 978-0-470-16680-2|page=203}}</ref>
* [[SQUID]] is a very sensitive magnetometer.
* For substances in solution [[nuclear magnetic resonance|NMR]] may be used to measure susceptibility.<ref>{{cite journal|last=Evans|first=D.F.|year=1959|title=The determination of the paramagnetic susceptibility of substances in solution by nuclear magnetic resonance|journal=J. Chem. Soc.|pages=2003–2005|doi=10.1039/JR9590002003}}</ref><ref>Orchard, p. 15. Earnshshaw, p. 97</ref>

==Types of magnetic behaviour==
{{Main article|Magnetism}}
When an isolated atom is placed in a [[magnetic field]] there is an interaction because each [[electron]] in the atom behaves like a magnet, that is, the electron has a [[magnetic moment]]. There are two types of interaction.
# Diamagnetism. When placed in a magnetic field the atom becomes magnetically polarized, that is, it develops an induced magnetic moment. The force of the interaction tends to push the atom out of the magnetic field. By convention diamagnetic susceptibility is given a negative sign. Very frequently diamagnetic atoms have no unpaired electrons ''ie'' each electron is paired with another electron in the same [[atomic orbital]]. The moments of the two electrons cancel each other out, so the atom has no net magnetic moment. However, for the ion Eu<sup>3+</sup> which has six unpaired electrons, the orbital angular momentum cancels out the electron angular momentum, and this ion is diamagnetic at zero Kelvin. 
# Paramagnetism. At least one electron is not paired with another. The atom has a permanent magnetic moment. When placed into a magnetic field, the atom is attracted into the field. By convention paramagnetic susceptibility is given a positive sign.

When the atom is present in a [[chemical compound]] its magnetic behaviour is modified by its chemical environment. Measurement of the magnetic moment can give useful chemical information.

In certain crystalline materials individual magnetic moments may be aligned with each other (magnetic moment has both magnitude and direction). This gives rise to [[ferromagnetism]], [[antiferromagnetism]] or [[ferrimagnetism]]. These are properties of the crystal as a whole, of little bearing on chemical properties.

==Diamagnetism==
{{Main article|Diamagnetism}}
Diamagnetism is a universal property of chemical compounds, because all chemical compounds contain electron pairs. A compound in which there are no unpaired electrons is said to be diamagnetic. The effect is weak because it depends on the magnitude of the induced magnetic moment. It depends on the number of electron pairs and the chemical nature of the atoms to which they belong. This means that the effects are additive, and a table of "diamagnetic contributions", or [[Pascal's constants]], can be put together.<ref>Figgis&Lewis, p. 403</ref><ref>Carlin, p. 3</ref><ref>{{cite journal|last=Bain|first=Gordon A.|author2=Berry , John F.|year=2008|title=Diamagnetic Corrections and Pascal's Constants|journal=J. Chem. Educ.|volume=85|page=532|doi=10.1021/ed085p532|issue=4|bibcode = 2008JChEd..85..532B }}</ref> With paramagnetic compounds the observed susceptibility can be adjusted by adding to it the so-called diamagnetic correction, which is the diamagnetic susceptibility calculated with the values from the table.<ref>Figgis&Lewis, p.&nbsp;417</ref>

==Paramagnetism==
{{Main article|Paramagnetism}}

===Mechanism and temperature dependence===
[[File:Susceptibility.png|thumb|200px| Variation of magnetic susceptibility with temperature]]
A metal ion with a single unpaired electron, such as Cu<sup>2+</sup>, in a coordination complex provides the simplest illustration of the mechanism of paramagnetism. The individual metal ions are kept far apart by the ligands, so that there is no magnetic interaction between them. The system is said to be magnetically dilute. The magnetic dipoles of the atoms point in random directions. When a magnetic field is applied, first-order [[Zeeman splitting]] occurs. Atoms with spins aligned to the field slightly outnumber the atoms with non-aligned spins. In the first-order Zeeman effect the energy difference between the two states is proportional to the applied field strength. Denoting the energy difference as Δ''E'', the [[Boltzmann distribution]] gives the ratio of the two populations as <math>e^{-\Delta E/kT}</math>, where ''k'' is the [[Boltzmann constant]] and ''T'' is the temperature in [[kelvin]]s. In most cases Δ''E'' is much smaller than ''kT'' and the exponential can be expanded as 1 – Δ''E/kT''. It follows from the presence of 1/''T'' in this expression that the susceptibility is inversely proportional to temperature.<ref>Figgis&Lewis, p. 419</ref>
:<math>\chi={C \over T}</math>
This is known as the [[Curie law]] and the proportionality constant, ''C'', is known as the [[Curie constant]], whose value, for molar susceptibility, is calculated as<ref>Orchard, p. 48</ref>
:<math>C=\frac{N g^2S(S+1)\mu_B^2}{3k}</math>
where ''N'' is the [[Avogadro constant]], ''g'' is the [[Landé g-factor]], and μ<sub>B</sub> is the [[Bohr magneton]]. In this treatment it has been assumed that the electronic [[ground state]] is not degenerate, that the magnetic susceptibility is due only to electron spin and that only the ground state is thermally populated.

While some substances obey the Curie law, others obey the [[Curie-Weiss]] law.
:<math>\chi = \frac{C}{T - T_{c}}</math>
''T<sub>c</sub>'' is the [[Curie temperature]]. The Curie-Weiss law will apply only when the temperature is well above the Curie temperature. At temperatures below the Curie temperature the substance may become [[ferromagnetic]]. More complicated behaviour is observed with the heavier transition elements.

===Effective magnetic moment===
When the Curie law is obeyed, the product of molar susceptibility and temperature is a constant. The '''effective magnetic moment''', μ<sub>eff</sub> is then defined<ref name=HoppeJI>{{cite journal|last=Hoppe|first=J.I.|year=1972|title=Effective magnetic moment|journal=J. Chem. Educ.|volume=49|issue=7|pages=505|doi=10.1021/ed049p505|bibcode = 1972JChEd..49..505H }}</ref> as
:<math>\mu_{\text{eff}} = \mathrm{constant}\sqrt{T \chi}</math>
Where C has CGS units cm<sup>3</sup> mol<sup>−1</sup> K, μ<sub>eff</sub> is 
:<math>\mu_{\text{eff}} = \sqrt{3 k \over N \mu_B^2} \sqrt{T \chi} \approx 2.82787 \sqrt{T \chi}</math>

Where C has SI units m<sup>3</sup> mol<sup>−1</sup> K,  μ<sub>eff</sub> is
:<math>\mu_{\text{eff}} = \sqrt{3 k \over N \mu_0 \mu_B^2} \sqrt{T \chi} \approx 797.727 \sqrt{T \chi}</math>
The quantity μ<sub>eff</sub> is effectively dimensionless, but is often stated as in units of [[Bohr magneton]] (μ<sub>B</sub>).<ref name=HoppeJI />

For substances that obey the Curie law, the effective magnetic moment is independent of temperature. For other substances μ<sub>eff</sub> is temperature dependent, but the dependence is small if the Curie-Weiss law holds and the Curie temperature is low.

===Temperature independent paramagnetism===
Compounds which are expected to be diamagnetic may exhibit this kind of weak paramagnetism. It arises from a second-order Zeeman effect in which additional splitting, proportional to the square of the field strength, occurs. It is difficult to observe as the compound inevitably also interacts with the magnetic field in the diamagnetic sense. Nevertheless, data are available for the [[permanganate]] ion.<ref>Orchard, p. 53</ref> It is easier to observe in compounds of the heavier elements, such as [[uranyl]] compounds.

===Exchange interactions===
{{main article|Exchange interaction}}
[[File:Copper(II)-acetate-3D-balls2.png|thumb|left|160px|Copper(II) acetate dihydrate<ref name=b1/>]]
[[File:Ferrimagnetic ordering.svg|thumb|130px|Ferrimagnetic ordering in 2 dimensions]]
[[File:Antiferromagnetic ordering.svg|thumb|130px|Antiferromagnetic ordering in 2 dimensions]]

Exchange interactions occur when the substance is not magnetically dilute and there are interactions between individual magnetic centres. One of the simplest systems to exhibit the result of exchange interactions is crystalline [[copper(II) acetate]], Cu<sub>2</sub>(OAc)<sub>4</sub>(H<sub>2</sub>O)<sub>2</sub>. As the formula indicates, it contains two copper(II) ions. The Cu<sup>2+</sup> ions are held together by four acetate ligands, each of which binds to both copper ions. Each Cu<sup>2+</sup> ion has a d<sup>9</sup> electronic configuration, and so should have one unpaired electron. If there were a covalent bond between the copper ions, the electrons would pair up and the compound would be diamagnetic. Instead, there is an exchange interaction in which the spins of the unpaired electrons become partially aligned to each other. In fact two states are created, one with spins parallel and the other with spins opposed. The energy difference between the two states is so small their populations vary significantly with temperature. In consequence the magnetic moment varies with temperature in a [[sigmoid function|sigmoidal]] pattern. The state with spins opposed has lower energy, so the interaction can be classed as antiferromagnetic in this case.<ref name=b1>{{cite book|author=Lawrence Que|title=Physical methods in bioinorganic chemistry: spectroscopy and magnetism|url=https://books.google.com/books?id=KYZ6EXIdjYwC&pg=PA347|access-date=22 February 2011|date=March 2000|publisher=University Science Books|isbn=978-1-891389-02-3|pages=345–348}}</ref> It is believed that this is an example of [[superexchange]], mediated by the oxygen and carbon atoms of the acetate ligands.<ref>Figgis&Lewis, p. 435. Orchard, p. 67</ref> Other dimers and clusters exhibit exchange behaviour.<ref>Carlin, sections 5.5–5.7</ref>

Exchange interactions can act over infinite chains in one dimension, planes in two dimensions or over a whole crystal in three dimensions. These are examples of long-range magnetic ordering. They give rise to [[ferromagnetism]], [[antiferromagnetism]] or [[ferrimagnetism]], depending on the nature and relative orientations of the individual spins.<ref>Carlin, chapters 6 and 7, pp. 112–225</ref>

Compounds at temperatures below the Curie temperature exhibit long-range magnetic order in the form of ferromagnetism. Another critical temperature is the [[Néel temperature]], below which antiferromagnetism occurs. The hexahydrate of nickel chloride, NiCl<sub>2</sub>·6H<sub>2</sub>O, has a Néel temperature of 8.3 K. The susceptibility is a maximum at this temperature. Below the Néel temperature the susceptibility decreases and the substance becomes antiferromagnetic.<ref>Carin, p. 264</ref>

==Complexes of transition metal ions==
The effective magnetic moment for a compound containing a transition metal ion with one or more unpaired electrons depends on the total orbital and spin [[angular momentum]] of the unpaired electrons, <math>\vec{L}</math> and <math>\vec{S}</math>, respectively. "Total" in this context means "[[vector sum]]". In the approximation that the electronic states of the metal ions are determined by [[Angular momentum coupling|Russell-Saunders]] coupling and that [[spin–orbit coupling]] is negligible, the magnetic moment is given by<ref>Figgis&Lewis, p. 420</ref>
:<math>\mu_{\text{eff}} = \sqrt{\vec{L}(\vec{L}+1)+ 4\vec{S}(\vec{S}+1)} \mu_B</math>

===Spin-only formula===
Orbital angular momentum is generated when an electron in an orbital of a degenerate set of orbitals is moved to another orbital in the set by rotation. In complexes of [[molecular symmetry|low symmetry]] certain rotations are not possible. In that case the orbital angular momentum is said to be "quenched" and <math>\vec{L}</math> is smaller than might be expected (partial quenching), or zero (complete quenching). There is complete quenching in the following cases. Note that an electron in a degenerate pair of d<sub>x<sup>2</sup>–y<sup>2</sup></sub> or d<sub>z<sup>2</sup></sub> orbitals cannot rotate into the other orbital because of symmetry.<ref>Figgis&Lewis, pp. 424, 432</ref> 
:{|class="wikitable" style="text-align:center"
|+Quenched orbital angular momentum
!rowspan=2|d<sup>n</sup>||colspan=3|Octahedral||Tetrahedral 
|-
! ||high-spin||low-spin ||
|-
|d<sup>1</sup>|| || || ||e<sup>1</sup>
|-
|d<sup>2</sup>|| || || ||e<sup>2</sup>
|-
|d<sup>3</sup>||t<sub>2g</sub><sup>3</sup>|| || ||
|-
|d<sup>4</sup>|| ||t<sub>2g</sub><sup>3</sup>e<sub>g</sub><sup>1</sup>|| ||
|-
|d<sup>5</sup>|| ||t<sub>2g</sub><sup>3</sup>e<sub>g</sub><sup>2</sup>|| ||
|-
|d<sup>6</sup>|| || ||t<sub>2g</sub><sup>6</sup> ||e<sup>3</sup>t<sub>2</sub><sup>3</sup>
|-
|d<sup>7</sup>|| || ||t<sub>2g</sub><sup>6</sup>e<sub>g</sub><sup>1</sup> ||e<sup>4</sup>t<sub>2</sub><sup>3</sup>
|-
|d<sup>8</sup>||t<sub>2g</sub><sup>6</sup>e<sub>g</sub><sup>2</sup>|| || ||
|-
|d<sup>9</sup>||t<sub>2g</sub><sup>6</sup>e<sub>g</sub><sup>3</sup>|| || ||
|}
:legend: t<sub>2g</sub>, t<sub>2</sub> = (d<sub>xy</sub>, d<sub>xz</sub>, d<sub>yz</sub>). e<sub>g</sub>, e = (d<sub>x<sup>2</sup>–y<sup>2</sup></sub>, d<sub>z<sup>2</sup></sub>).
 
When orbital angular momentum is completely quenched, <math>\vec{L}=0</math> and the paramagnetism can be attributed to electron spin alone. The total spin angular momentum is simply half the number of unpaired electrons and the spin-only formula results.
:<math>\mu_{\text{eff}}= \sqrt{n(n+2)} \mu_B</math>
where ''n'' is the number of unpaired electrons. The spin-only formula is a good first approximation for high-spin complexes of first-row [[transition metal]]s.<ref>Figgis&Lewis, p. 406</ref>
:{|class="wikitable" style="text-align:center"
!Ion!!Number of <br/>unpaired<br/>electrons!!Spin-only<br/> moment /μ<sub>B</sub>!!observed<br/>moment /μ<sub>B</sub>
|-
|Ti<sup>3+</sup> ||1||1.73||1.73
|-
|V<sup>4+</sup>||1 ||1.73||1.68–1.78
|-
|Cu<sup>2+</sup> ||1 ||1.73||1.70–2.20
|-
|V<sup>3+</sup>||2||2.83||2.75–2.85
|-
|Ni<sup>2+</sup>||2||2.83||2.8–3.5
|-
|V<sup>2+</sup> ||3||3.87||3.80–3.90
|-
|Cr<sup>3+</sup> ||3||3.87||3.70–3.90
|-
|Co<sup>2+</sup> ||3||3.87||4.3–5.0
|-
|Mn<sup>4+</sup> ||3||3.87||3.80–4.0
|-
|Cr<sup>2+</sup> ||4||4.90 ||4.75–4.90
|-
|Fe<sup>2+</sup> ||4 ||4.90||5.1–5.7
|-
|Mn<sup>2+</sup> ||5||5.92 ||5.65–6.10
|-
|Fe<sup>3+</sup> ||5||5.92||5.7–6.0
|}
The small deviations from the spin-only formula may result from the neglect of orbital angular momentum or of spin–orbit coupling. For example, tetrahedral d<sup>3</sup>, d<sup>4</sup>, d<sup>8</sup> and d<sup>9</sup> complexes tend to show larger deviations from the spin-only formula than octahedral complexes of the same ion, because "quenching" of the orbital contribution is less effective in the tetrahedral case.<ref>Figgis&Lewis, Section 3, "Orbital contribution"</ref>

===Low-spin complexes===
{{main article|crystal field theory}}
[[File:CFT-Low Spin Splitting Diagram-Vector.svg|thumb|200px|Crystal field diagram for octahedral low-spin d<sup>5</sup>]]
[[File:CFT-High Spin Splitting Diagram-Vector.svg|thumb|200px|Crystal field diagram for octahedral high-spin d<sup>5</sup>]]

According to crystal field theory, the ''d'' orbitals of a transition metal ion in an octahedal complex are split into two groups in a crystal field. If the splitting is large enough to overcome the energy needed to place electrons in the same orbital, with opposite spin, a low-spin complex will result. 
 
:{|class="wikitable" style="text-align:center"
|+ High and low -spin octahedral complexes
!rowspan=2|d-count ||colspan=2|Number of unpaired electrons||rowspan=2|examples
|-
!high-spin!!low-spin
|-
|d<sup>4</sup>||4||2||Cr<sup>2+</sup>, Mn<sup>3+</sup>
|-
|d<sup>5</sup>||5 ||1 ||Mn<sup>2+</sup>, Fe<sup>3+</sup> 
|-
|d<sup>6</sup>||4 ||0 ||Fe<sup>2+</sup>, Co<sup>3+</sup>
|-
|d<sup>7</sup>|| 3||1 ||Co<sup>2+</sup>
|}
With one unpaired electron μ<sub>eff</sub> values range from 1.8 to 2.5 μ<sub>B</sub> and with two unpaired electrons the range is 3.18 to 3.3 μ<sub>B</sub>. Note that low-spin complexes of Fe<sup>2+</sup> and Co<sup>3+</sup> are diamagnetic. Another group of complexes that are diamagnetic are [[square-planar]] complexes of d<sup>8</sup> ions such as Ni<sup>2+</sup> and Rh<sup>+</sup> and Au<sup>3+</sup>.

===Spin cross-over===
When the energy difference between the high-spin and low-spin states is comparable to ''kT'' (''k'' is the [[Boltzmann constant]] and ''T'' the temperature) an equilibrium is established between the spin states, involving what have been called "electronic isomers". Tris-[[dithiocarbamate|dithiocarbamato]] iron(III), Fe(S<sub>2</sub>CNR<sub>2</sub>)<sub>3</sub>, is a well-documented example. The effective moment varies from a typical d<sup>5</sup> low-spin value of 2.25 μ<sub>B</sub> at 80 K to more than 4 μ<sub>B</sub> above 300 K.<ref>Orchard, p. 125. Carlin, p. 270</ref>

===2nd and 3rd row transition metals===
Crystal field splitting is larger for complexes of the heavier transition metals than for the transition metals discussed above. A consequence of this is that low-spin complexes are much more common. Spin–orbit coupling constants, ζ, are also larger and cannot be ignored, even in elementary treatments. The magnetic behaviour has been summarized, as below, together with an extensive table of data.<ref>Figgis&Lewis, pp. 443–451</ref>
:{| class=wikitable
!d-count!!kT/ζ=0.1<br/>μ<sub>eff</sub>!!kT/ζ=0<br/>μ<sub>eff</sub>!!Behaviour with large spin–orbit coupling constant, ζ<sub>nd</sub> 
|-
|d<sup>1</sup>||0.63||0||μ<sub>eff</sub> varies with T<sup>1/2</sup>
|-
|d<sup>2</sup>||1.55||1.22||μ<sub>eff</sub> varies with T, approximately
|-
|d<sup>3</sup>||3.88||3.88||Independent of temperature
|-
|d<sup>4</sup>||2.64||0||μ<sub>eff</sub> varies with T<sup>1/2</sup>
|-
|d<sup>5</sup>||1.95||1.73||μ<sub>eff</sub> varies with T, approximately
|}

===Lanthanides and actinides===
[[Russell-Saunders coupling]], LS coupling, applies to the lanthanide ions, crystal field effects can be ignored, but spin–orbit coupling is not negligible. Consequently, spin and orbital angular momenta have to be combined
:<math>\vec{L} = \sum_i \vec{l}_i</math>
:<math> \vec{S} = \sum_i \vec{s}_i</math>
:<math>\vec{J} = \vec{L} + \vec{S}</math>
and the calculated magnetic moment is given by
:<math>\mu_{\text{eff}}=g \sqrt{\vec{J}(\vec{J}+1)}; g={3 \over 2} +\frac{\vec{S}(\vec{S}+1)-\vec{L}(\vec{L}+1)}{2 \vec{J}(\vec{J}+1)}</math>
:{|class="wikitable" style="text-align:center"
|+Magnetic properties of trivalent lanthanide compounds<ref>Greenwood&Earnshaw p. 1243</ref>
!lanthanide!!Ce!!Pr!!Nd!!Pm!!Sm!!Eu!!Gd!!Tb!!Dy!!Ho!!Er!!Tm!!Yb!!Lu
|-
|Number of unpaired électrons||1||2||3||4||5||6||7||6||5||4||3||2||1||0
|-
|calculated moment /μ<sub>B</sub>||2.54||3.58||3.62||2.68||0.85||0||7.94||9.72||10.65||10.6||9.58||7.56||4.54||0
|-
|observed moment /μ<sub>B</sub>||2.3–2.5||3.4–3.6||3.5–3.6|| ||1.4–1.7|| 3.3–3.5||7.9–8.0||9.5–9.8||10.4–10.6||10.4–10.7||9.4–9.6||7.1–7.5||4.3–4.9||0
|}
In actinides spin–orbit coupling is strong and the coupling approximates to ''j'' ''j'' coupling.
:<math>\vec{J} = \sum_i \vec{j}_i 
= \sum_i(\vec{l}_i + \vec{s}_i)</math>
This means that it is difficult to calculate the effective moment. For example, uranium(IV), f<sup>2</sup>, in the complex [UCl<sub>6</sub>]<sup>2−</sup> has a measured effective moment of 2.2 μ<sub>B</sub>, which includes a contribution from temperature-independent paramagnetism.<ref>Orchard, p. 106</ref>

==Main group elements and organic compounds==
[[File:EPR methyl.png|thumb|left|Simulated [[electron paramagnetic resonance|EPR]] spectrum of the CH<sub>3</sub>• radical]]

[[File:MTSL chemical structure.png|thumb|100px|MSTL spin-label]]
Very few compounds of [[main group]] elements are paramagnetic. Notable examples include: [[oxygen]], O<sub>2</sub>; [[nitric oxide]], NO; [[nitrogen dioxide]], NO<sub>2</sub> and [[chlorine dioxide]], ClO<sub>2</sub>. In [[organic chemistry]], compounds with an unpaired electron are said to be [[free radical]]s. Free radicals, with some exceptions, are short-lived because one free radical will react rapidly with another, so their magnetic properties are difficult to study. However, if the radicals are well separated from each other in a dilute solution in a solid matrix, at low temperature, they can be studied by [[electron paramagnetic resonance]] (EPR). Such radicals are generated by irradiation. Extensive EPR studies have revealed much about electron delocalization in free radicals. The simulated spectrum of the CH<sub>3</sub>• radical shows [[hyperfine splitting]] due to the interaction of the electron with the 3 equivalent hydrogen nuclei, each of which has a spin of 1/2.<ref>{{cite book|last1=Weil|first1=John A.|last2= Bolton |first2=James R.|last3=Wertz|first3=John E. |title=Electron paramagnetic resonance : elementary theory and practical applications |year=1994|publisher=Wiley|isbn=0-471-57234-9}}</ref><ref>{{cite book|last1=Atkins|first1=P. W. |last2=Symons |first2=M. C. R.|title=The structure of inorganic radicals; an application of electron spin resonance to the study of molecular structure|year=1967|publisher=Elsevier}}</ref>

[[Spin label]]s are long-lived free radicals which can be inserted into organic molecules so that they can be studied by EPR.
<ref>{{cite book|last=Berliner|first=L.J.|title=Spin labeling : theory and applications I|year=1976|publisher=Academic Press|isbn=0-12-092350-5}}{{cite book|last=Berliner|first=L.J.|title=Spin labeling II : theory and applications |year=1979|publisher=Academic Press|isbn=0-12-092352-1}}</ref> For example, the nitroxide [[MTSL]], a functionalized derivative of TEtra Methyl Piperidine Oxide, [[TEMPO]], is used in [[site-directed spin labeling]].

==Applications==
The [[gadolinium]] ion, Gd<sup>3+</sup>, has the f<sup>7</sup> electronic configuration, with all spins parallel. Compounds of the Gd<sup>3+</sup> ion are the most suitable for use as a [[MRI contrast agent|contrast agent]] for [[MRI scan]]s.<ref>{{cite book|last=Krause|first=W.|title=Contrast Agents I: Magnetic Resonance Imaging: Pt. 1|year=2002|publisher=Springer|isbn=3540422471}}</ref> The magnetic moments of gadolinium compounds are larger than those of any transition metal ion. Gadolinium is
preferred to other lanthanide ions, some of which have larger effective moments, due to its having a [[Degenerate energy level|non-degenerate]] electronic [[ground state]].<ref>{{cite journal| last1 = Caravan| first1 = Peter| last2 = Ellison, Jeffrey J.; McMurry, Thomas J. ; Lauffer, Randall B.| year = 1999| title = Gadolinium(III) Chelates as MRI Contrast Agents: Structure, Dynamics, and Applications| journal = Chem. Rev.| volume = 99| pages = 2293–2352| doi = 10.1021/cr980440x| first2 = Jeffrey J.| last3 = McMurry| first3 = Thomas J.| last4 = Lauffer| first4 = Randall B.| issue = 9| pmid = 11749483}}</ref>
 
For many years the nature of [[oxyhemoglobin]], Hb-O<sub>2</sub>, was highly controversial. It was found experimentally to be diamagnetic. Deoxy-hemoglobin is generally accepted to be a complex of iron in the +2 [[oxidation state]], that is a d<sup>6</sup> system with a high-spin magnetic moment near to the spin-only value of 4.9 μ<sub>B</sub>. It was proposed that the iron is oxidized and the oxygen reduced to superoxide.
:Fe(II)Hb (high-spin) + O<sub>2</sub> {{eqm}} [Fe(III)Hb]O<sub>2</sub><sup>−</sup>
Pairing up of electrons from Fe<sup>3+</sup> and O<sub>2</sub><sup>−</sup> was then proposed to occur via an exchange mechanism. It has now been shown that in fact the iron(II) changes from high-spin to low-spin when an oxygen molecule donates a pair of electrons to the iron. Whereas in deoxy-hemoglobin the iron atom lies above the plane of the heme, in the low-spin complex the effective [[ionic radius]] is reduced and the iron atom lies in the heme plane.<ref>Greenwood&Earnshaw, pp. 1099–1011</ref> 
:Fe(II)Hb + O<sub>2</sub> {{eqm}} [Fe(II)Hb]O<sub>2</sub> (low-spin)
This information has an important bearing on research to find artificial [[oxygen carrier]]s.

Compounds of gallium(II) were unknown until quite recently. As the atomic number of gallium is an odd number (31), Ga<sup>2+</sup> should have an unpaired electron. It was assumed that it would act as a [[free radical]] and have a very short lifetime. The non-existence of Ga(II) compounds was part of the so-called [[inert-pair effect]]. When salts of the anion with [[empirical formula]] such as [GaCl<sub>3</sub>]<sup>−</sup> were synthesized they were found to be diamagnetic. This implied the formation of a Ga-Ga bond and a dimeric formula, [Ga<sub>2</sub>Cl<sub>6</sub>]<sup>2−</sup>.<ref>Greenwood&Earnshaw, p. 240</ref>

==See also==
*[[Magnetic mineralogy]]
*[[Magnetoelectrochemistry]]
*[[Magnetic ionic liquid]]
*[[Spin ice]]
*[[Spin glass]]
*[[Superdiamagnetism]], [[Superparamagnetism]], [[Superferromagnetism]]
*[[Single-molecule magnet|Single-molecule magnetism]]

==References==
{{reflist|30em}}

==Bibliography==
*{{cite book|last=Carlin|first=R.L.|title=Magnetochemistry|year=1986|publisher=[[Springer Science+Business Media|Springer]]|isbn=978-3-540-15816-5}}
*{{cite book|last=Earnshaw|first=Alan|title=Introduction to Magnetochemistry|year=1968|publisher=[[Academic Press]]}}
*{{cite book|last1=Figgis|first1=B.N.|last2=Lewis|first2=J.|editor=Lewis. J. and Wilkins. R.G.|title=Modern Coordination Chemistry|year=1960|publisher=[[John Wiley & Sons|Wiley]]|location=New York|chapter=The Magnetochemistry of Complex Compounds}}
*{{Greenwood&Earnshaw2nd}}
*{{cite book|last=Orchard|first=A.F.|author-link=Tony Orchard|title=Magnetochemistry|series=Oxford Chemistry Primers|year=2003|publisher=[[Oxford University Press]]|isbn=0-19-879278-6}}
*{{cite book|last=Selwood|first=P.W.|title=Magnetochemistry|year=1943|publisher=[[Interscience Publishers]] Inc.|url=https://archive.org/details/magnetochemistry032763mbp}}
*{{cite book|last=Vulfson |first=Sergey |title=Molecular Magnetochemistry |year=1998|publisher=[[Taylor & Francis]]|isbn=90-5699-535-9}}

==External links==
* [https://web.archive.org/web/20100728014337/http://www.internetchemie.info/chemistry/magnetochemistry.htm Online available information resources on magnetochemistry]
*[http://www.jce.divched.org/JCEDLib/ChemInfo/Inorganic/pascal.html Tables of Diamagnetic Corrections and Pascal's Constants]

{{Magnetic states}}
{{Branches of chemistry}}
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[[Category:Magnetism]]
[[Category:Chemistry]]