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| Names | |||
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| Other names
Lutetium bisphthalocyanine | |||
| Identifiers | |||
3D model (JSmol) |
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| Properties | |||
| LuC64H32N16 | |||
| Molar mass | 1200.04 g/mol | ||
| Appearance | green solid; red when oxidized; blue when reduced | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lutetium phthalocyanine (LuPc2) is a coordination compound derived from lutetium and two phthalocyanines. It was the first known example of a molecule that is an intrinsic semiconductor.[1][2] It exhibits electrochromism, changing color when subject to a voltage.
LuPc2 is a double-decker sandwich compound consisting of a Lu3+ ion coordinated to two the conjugate base of two phthalocyanines. The rings are arranged in a staggered conformation. The extremities of the two ligands are slightly distorted outwards.[3] The complex features a non-innocent ligand, in the sense that the macrocycles carry an extra electron.[4] It is a free radical[1] with the unpaired electron sitting in a half-filled molecular orbital between the highest occupied and lowest unoccupied orbitals, allowing its electronic properties to be finely tuned.[3]
LuPc2, along with many substituted derivatives like the alkoxy-methyl derivative Lu[(C8H17OCH2)8Pc]2, can be deposited as a thin film with intrinsic semiconductor properties;[4] said properties arise due to its radical nature[1] and its low reduction potential compared to other metal phthalocyanines.[2] This initially green film exhibits electrochromism; the oxidized form LuPc+
2 is red, whereas the reduced form LuPc−
2 is blue and the next two reduced forms are dark blue and violet, respectively.[4] The green/red oxidation cycle can be repeated over 10,000 times in aqueous solution with dissolved alkali metal halides, before it is degraded by hydroxide ions; the green/blue redox degrades faster in water.[4]
LuPc2 and other lanthanide phthalocyanines are of interest in the development of organic thin-film field-effect transistors.[3][5]
LuPc2 derivatives can be selected to change color in the presence of certain molecules, such as in gas detectors;[2] for example, the thioether derivative Lu[(C6H13S)8Pc]2 changes from green to brownish-purple in the presence of NADH.[6]
