Double group

For mathematical details, see Finite subgroups of SU(2).

The concept of a double group was introduced by Hans Bethe for the quantitative treatment of magnetochemistry. Because the fermions' phase changes with 360-degree rotation, enhanced symmetry groups that describe band degeneracy and topological properties of magnonic systems are needed, which depend not only on geometric rotation, but on the corresponding fermionic phase factor in representations (for the related mathematical concept, see the formal definition). They were introduced for studying complexes of ions that have a single unpaired electron in the metal ion's valence electron shell, like Ti ³⁺, and complexes of ions that have a single "vacancy" in the valence shell, like Cu ²⁺. ^{[1] [2]}

In the specific instances of complexes of metal ions that have the electronic configurations 3d¹, 3d⁹, 4f¹ and 4f¹³, rotation by 360° must be treated as a symmetry operation R, in a separate class from the identity operation E. This arises from the nature of the wave function for electron spin. A double group is formed by combining a molecular point group with the group {E, R} that has two symmetry operations, identity and rotation by 360°. The double group has twice the number of symmetry operations compared to the molecular point group.

Background

In magnetochemistry, the need for a double group arises in a very particular circumstance, namely, in the treatment of the paramagnetism of complexes of a metal ion in whose electronic structure there is a single electron (or its equivalent, a single vacancy) in a metal ion's d- or f-shell. This occurs, for example, with the elements copper and silver in the +2 oxidation state, where there is a single vacancy in a d electron shell, with titanium(III), which has a single electron in the 3d shell, and with cerium(III), which has a single electron in the 4f shell.

In group theory, the character ${\displaystyle \chi }$, for rotation of a molecular wavefunction for angular momentum by an angle α is given by

${\displaystyle \chi ^{J}(\alpha )={\frac {\sin(J+{1 \over 2})\alpha }{\sin {1 \over 2}\alpha }}}$

where ${\displaystyle J=L+S}$; angular momentum is the vector sum of orbital and spin angular momentum. This formula applies with most paramagnetic chemical compounds of transition metals and lanthanides. However, in a complex containing an atom with a single electron in the valence shell, the character, ${\displaystyle \chi ^{J}}$, for a rotation through an angle of ${\displaystyle 2\pi +\alpha }$ about an axis through that atom is equal to minus the character for a rotation through an angle of ${\displaystyle \alpha }$ ^[3]

${\displaystyle \chi ^{J}(2\pi +\alpha )=-\chi ^{J}(\alpha )}$

The change of sign cannot be true for an identity operation in any point group. Therefore, a double group, in which rotation by ${\displaystyle 2\pi }$, is classified as being distinct from the identity operation, is used. A character table for the double group D′₄ is as follows. The new symmetry operations are shown in the second row of the table.

Character table: double group D′₄

D′4	E		C4	C43	C2	2C″2	2C″2
		R	C4R	C43R	C2R	2C′2R	2C″2R
A′1	1	1	1	1	1	1	1
A′2	1	1	1	1	1	−1	−1
B′1	1	1	−1	−1	1	1	−1
B′2	1	1	−1	−1	1	−1	1
E′1	2	−2	0	0	−2	0	0
E′2	2	−2	√2	−√2	0	0	0
E′3	2	−2	−√2	√2	0	0	0

The symmetry operations such as C₄ and C₄R belong to the same class but the column header is shown, for convenience, in two rows, rather than C₄, C₄R in a single row.

Character tables for the double groups T′, O′, T_d′, D_3h′, C_6v′, D₆′, D_2d′, C_4v′, D₄′, C_3v′, D₃′, C_2v′, D₂′ and R(3)′ are given in Salthouse and Ware. ^[4]

Applications

Sub-structure at the center of an octahedral complex

Structure of a square-planar complex ion such as [AgF₄]

An atom or ion (red) held in a C₆₀ fullerene cage

The need for a double group occurs, for example, in the treatment of magnetic properties of 6-coordinate complexes of copper(II). The electronic configuration of the central Cu²⁺ ion can be written as [Ar]3d⁹. It can be said that there is a single vacancy, or hole, in the copper 3d-electron shell, which can contain up to 10 electrons. The ion [Cu(H₂O)₆]²⁺ is a typical example of a compound with this characteristic.

1. Six-coordinate complexes of the Cu(II) ion, with the generic formula [CuL₆]²⁺, are subject to the Jahn-Teller effect so that the symmetry is reduced from octahedral (point group O_h) to tetragonal (point group D_4h). Since d orbitals are centrosymmetric the related atomic term symbols can be classified in the subgroup D₄.
2. To a first approximation spin–orbit coupling can be ignored and the magnetic moment is then predicted to be 1.73 Bohr magnetons, the so-called spin-only value. However, for a more accurate prediction spin–orbit coupling must be taken into consideration. This means that the relevant quantum number is J, where J = L + S.
3. When J is half-integer, the character for a rotation by an angle of α + 2π radians is equal to minus the character for rotation by an angle α. This cannot be true for an identity in a point group. Consequently, a group must be used in which rotations by α + 2π are classed as symmetry operations distinct from rotations by an angle α. This group is known as the double group, D₄′.

With species such as the square-planar complex of the silver(II) ion [AgF₄]²⁻ the relevant double group is also D₄′; deviations from the spin-only value are greater as the magnitude of spin–orbit coupling is greater for silver(II) than for copper(II). ^[5]

A double group is also used for some compounds of titanium in the +3 oxidation state. Titanium(III) has a single electron in the 3d shell; the magnetic moments of its complexes have been found to lie in the range 1.63–1.81 B.M. at room temperature. ^[6] The double group O′ is used to classify their electronic states.

The cerium(III) ion, Ce³⁺, has a single electron in the 4f shell. The magnetic properties of octahedral complexes of this ion are treated using the double group O′.

When a cerium(III) ion is encapsulated in a C₆₀ cage, the formula of the endohedral fullerene is written as {Ce³⁺@C₆₀³⁻}. ^[7] The magnetic properties of the compound are treated using the icosahedral double group I²_h. ^[8]

Free radicals

Double groups may be used in connection with free radicals. This has been illustrated for the species CH₃F⁺ and CH₃BF₂⁺, each of which contain a single unpaired electron. ^[9]

See also

• Molecular symmetry
• Point group
• Magnetochemistry

References

1. Cotton, F. Albert (1971). Chemical Applications of Group Theory. New York: Wiley. pp. 289–294, 376. ISBN   0-471-17570-6.
2. Tsukerblat, Boris S. (2006). Group Theory in Chemistry and Spectroscopy. Mineola, New York: Dover Publications Inc. pp. 245–253. ISBN   0-486-45035-X.
3. Lipson, R.H. "Spin-orbit coupling and double groups" (PDF).
4. Salthouse, J.A.; Ware, M.J. (1972). Point group character tables and related data. Cambridge: Cambridge University Press. pp. 55–57. ISBN   0-521-081394.
5. Foëx, D.; Gorter, C. J.; Smits, L.J. (1957). Constantes Sélectionées Diamagnetism et Paramagnetism. Paris: Masson et Cie.
6. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 971. ISBN   978-0-08-037941-8.
7. Chai, Yan; Guo, Ting; Jin, Changming; Haufler, Robert E.; Chibante, L. P. Felipe; Fure, Jan; Wang, Lihong; Alford, J. Michael; Smalley, Richard E. (1991). "Fullerenes with metals inside". The Journal of Physical Chemistry. 95 (20): 7564–7568. doi:10.1021/j100173a002.
8. Balasubramanian, K. (1996). "Double group of the icosahedral group (I_h) and its application to fullerenes". Chemical Physics Letters. 260 (3): 476–484. Bibcode:1996CPL...260..476B. doi:10.1016/0009-2614(96)00849-4.
9. Bunker, P.R. (1979), "The Spin Double Groups of Molecular Symmetry Groups", in Hinze, J. (ed.), The Permutation Group in Physics and Chemistry, Lecture Notes in Chemistry, vol. 12, Springer, pp. 38–56, doi:10.1007/978-3-642-93124-6_4, ISBN   978-3-540-09707-5

Further reading

• Earnshaw, Alan (1968). Introduction to Magnetochemistry. Academic Press.
• Figgis, Brian N.; Lewis, Jack (1960). "The magnetochemistry of complex compounds". In Lewis, J.; Wilkins, R.G. (eds.). Modern Coordination Chemistry. New York: Interscience. pp. 400–451.
• Orchard, Anthony F. (2003). Magnetochemistry. Oxford Chemistry Primers. Oxford University Press. ISBN   0-19-879278-6.
• Vulfson, Sergey G.; Arshinova, Rose P. (1998). Molecular Magnetochemistry. Taylor & Francis. ISBN   90-5699-535-9.