Name: coordination complexes and chelation
Uploaded: 2020-09-24T15:06:53.000Z
Duration: 2 min 51 s
Channel: JoVE

K12 Standards

new-york-state-science-learning-standards

New York State Science Learning Standards

High School

Physical Science

HS. Structure and Properties of Matter

HS-PS2-6.

Metal-Ligand Bonds

En un ion complejo, el ion metálico está unido a moléculas aniónicas o neutras, conocidas como ligandos. Los ligandos tienen uno o más pares de electrones solitarios y actúan como donantes de pares de electrones o bases de Lewis. Donan el par de electrones al ion metálico, que actúa como un aceptor de un par de electrones o de un ácido de Lewis.Por lo tanto, un enlace covalente coordinado entre el ion metálico y el ligando forma un aducto ácido-base de Lewis. El átomo del ligando que dona un par de electrones se conoce como átomo donante. El número de átomos donantes que rodean al ion metálico se correlaciona con el número de coordinación del ion metálico.Dependiendo del número de átomos donantes presentes, los ligandos se clasifican además como ligandos monodentados, bidentados o polidentados, que pueden estar cargados o ser neutros. Los ligandos monodentados tienen un solo átomo donante. El oxígeno es un átomo donante en una molécula de agua neutra;el nitrógeno es un átomo donante en un ion cianuro cargado.Los ligandos bidentados tienen dos átomos donantes que están lo suficientemente separados para unirse simultáneamente a un ion metálico. Los átomos de nitrógeno de tres moléculas de bipiridina se unen a un ion de rutenio con el número de coordinación seis. Un ligando polidentado tiene dos o más átomos donantes presentes en su estructura.Aquí, seis nitrógenos de dos moléculas de dietilentriamina se unen a un ion cobalto. Como múltiples átomos donantes parecen contener el ion metálico central como una cuña, los ligandos bidentados y polidentados también se denominan agentes quelantes. Un agente quelante tiene más afinidad por el ion metálico central que un ligando monodentado, formando un complejo de coordinación más estable.Esto se conoce como efecto quelante. Los agentes quelantes son versátiles. Se utilizan para complejizar los iones metálicos que interfieren en una reacción, para aumentar la vida útil de los productos alimenticios al complejizar los iones metálicos traza involucrados en la catalización de reacciones de descomposición o en el tratamiento del envenenamiento por plomo usando etilendiaminotetraacetato o EDTA.La formación de iones complejos influye en las propiedades fisicoquímicas del ion metálico y los ligandos, como el cambio en los potenciales o colores de oxidación y reducción. Además, los ligandos pueden sufrir reacciones como la desprotonación de iones metálicos hidratados o el desplazamiento por otro ligando fuertemente atraído. Aquí, la molécula de agua es reemplazada por amoníaco, que se une de manera más fuerte al ion metálico.

enlaces metal-ligando

La hemoglobina en la sangre, la clorofila en las plantas verdes, la vitamina B-12, y el catalizador usado en la fabricación del polietileno contienen compuestos de coordinación. Es probable que los iones de los metales, especialmente los metales de transición, formen complejos.
 En estos complejos, los metales de transición forman enlaces covalentes coordinados, un tipo de interacción ácido-base de Lewis en la cual ambos electrones en el enlace son aportados por un donante (base de Lewis) a un aceptor de electrones (ácido de Lewis). El ácido de Lewis en los complejos de coordinación, a menudo llamado un ion de metal central (o átomo), es el metal de transición o el metal de transición interna. Los donantes de base de Lewis, llamados ligandos, pueden ser una amplia variedad de químicos—átomos, moléculas o iones. El único requisito es que tengan uno o más pares de electrones, que puedan ser donados al metal central. Más a menudo, esto implica un átomo donante con un par solitario de electrones que pueden formar un enlace de coordinación con el metal. La esfera de coordinación consiste en el ion o átomo del metal central más sus ligandos unidos. Los corchetes en una fórmula encierran la esfera de coordinación; las especies fuera de los corchetes no forman parte de la esfera de coordinación.
 Los ligandos son monodentados, del griego para “un diente”, cuando se conectan con el metal central a través de un solo átomo. Aquí, el número de ligandos y el número de coordinación son iguales. Los ligandos con un átomo donante, como NH3, Cl− y H2O, son ligandos monodentados. Muchos otros ligandos se coordinan con el metal en formas más complejas.
 Los ligandos bidentados son aquellos en los que dos átomos se coordinan con el centro de metal. Por ejemplo, la etilenodiamina (en, H2NCH2CH2NH2) contiene dos átomos de nitrógeno, cada uno de los cuales tiene un par solitario y puede servir como base de Lewis (Figura 1a). Ambos átomos pueden coordinarse a un único centro de metal. En el complejo [Co(en)3]3+, hay tres ligandos en bidentados, y el número de coordinación del ión cobalto (III) es seis (Figura 1b). Los números de coordinación más comunes son dos, cuatro y seis, pero se conocen ejemplos de todos los números de coordinación de 1 a 15.
 <img alt="Image1" src="/files/ftp_upload/11456/11456_Image_1.svg" style="text-align: center; height: 200px;" />
 Figura 1. (a) la etilenodiamina (en) contiene dos átomos de nitrógeno, con un par solitario cada uno, que pueden coordinarse con un ión metálico. (b) Tres ligandos bidentados se coordinan con un solo ión cobalto.
 Cualquier ligando que se une a un ion central de metal por más de un átomo donante es un ligando polidentato (o “muchos dientes”) porque puede morder el centro de metal con más de un enlace. El término quelato del griego para “garra” también se utiliza para describir este tipo de interacción. Muchos ligandos polidentatos son ligandos quelantes, y un complejo que consiste en uno o más de estos ligandos y un metal central es un quelato. Un ligando quelante también se conoce como un agente quelante. Un ligando quelante sostiene el ión de metal como una pinza de cangrejo sostendría un mármol. Los ligandos polidentados a veces se identifican con prefijos que indican el número de átomos donantes en el ligando. El complejo hemo en la hemoglobina es otro ejemplo importante (Figura 2). Contiene un ligando polidentado con cuatro átomos donantes que se coordinan con el hierro.
 <img alt="Image2" src="/files/ftp_upload/11456/11456_Image2.svg" style="text-align: center; height: 200px;" />
 Figura 2: El único heme ligando contiene cuatro átomos de nitrógeno que se coordinan con el hierro en la hemoglobina para formar un quelato.
 Este texto está adaptado de<a href="https://openstax.org/books/chemistry-2e/pages/19-2-coordination-chemistry-of-transition-metals"> Openstax, Química 2e, Capítulo 19.2 Química de Coordinación de los Metales de Transición</a>.

Enlaces Metal-Ligando

La hemoglobina en la sangre, la clorofila en las plantas verdes, la vitamina B-12 y el catalizador utilizado en la fabricación de polietileno contienen ...

Education

Educación

JoVE Core

Chemistry

Química

Transition Metals and Coordination Complexes

Metales de transición y complejos de coordinación

transition-metals-and-coordination-complexes

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

coordination complexes and chelation

Coordination complexes form when a metal ion bonds to ligands. These compounds appear in familiar examples such as hemoglobin in blood, chlorophyll in green plants, vitamin B-12, and the catalyst used to make polyethylene. Transition metal ions are especially likely to form these complexes.

In a coordination complex, the metal acts as a Lewis acid. The ligand acts as a Lewis base and donates both electrons in the coordinate covalent bond. A ligand can be an atom, molecule, or ion, as long as it has one or more electron pairs to share with the metal. The central metal ion or atom, along with its attached ligands, makes up the coordination sphere. Brackets in a formula show the coordination sphere, and anything outside the brackets is not part of it.

Ligands can bind in different ways. Monodentate ligands connect through only one atom, so the number of ligands equals the coordination number. Common examples are NH3, Cl−, and H2O. Bidentate ligands bind through two atoms. Ethylenediamine, or en, has two nitrogen atoms with lone pairs that can both bond to one metal center. In the complex [Co(en)3]3+, three bidentate ligands give cobalt(III) a coordination number of six.

Ligands that attach through more than one donor atom are called polydentate ligands. The word chelate comes from a Greek word meaning “claw,” and it describes how these ligands hold a metal ion. A complex with one or more chelating ligands is called a chelate, and a chelating ligand is also called a chelating agent. These ligands can be identified with prefixes that show the number of donor atoms they use.

The heme complex in hemoglobin is another key example. Heme is a single polydentate ligand with four donor atoms, and all four coordinate to iron. Coordination numbers in complexes are often 2, 4, or 6, but examples from 1 to 15 are known. These bonding patterns help explain the structure of many important metal-containing compounds.

Coordination Complexes and Chelation

properties of transition metals

Transition Metals in the Periodic Table

Transition metals are the d-block elements and the inner transition metals in the f-block. They are defined by partially filled d orbitals. In the periodic table, the transition elements are in groups 3 through 11, and the inner transition metals appear in the two rows below the main body of the table. The d-block is often grouped into transition series. The first transition series runs from Sc through Cu. The second series runs from Y through Ag. The third series includes La and Hf through...

coordination compounds and nomenclature

How Transition Metal Complexes Are Named

Transition metal complexes are named by following rules for ligands, metal ions, and oxidation state. These compounds form when a central metal ion or atom, often a transition metal or inner transition metal, accepts electron pairs from ligands. A ligand is a Lewis base that can be an atom, molecule, or ion with one or more lone pairs to donate. In these complexes, the bond is a coordinate covalent bond. That means both electrons in the bond come from the donor, such as ammonia, and are...

metal-ligand bonds

Coordination complexes form when a metal ion bonds to ligands. These compounds appear in familiar examples such as hemoglobin in blood, chlorophyll in green plants, vitamin B-12, and the catalyst used to make polyethylene. Transition metal ions are especially likely to form these complexes. In a coordination complex, the metal acts as a Lewis acid. The ligand acts as a Lewis base and donates both electrons in the coordinate covalent bond. A ligand can be an atom, molecule, or ion, as long as...

coordination number and geometry

Transition Metal Shapes from Coordination Number

Transition metal complexes are often identified by their coordination number and the shape around the metal ion. The coordination number is the number of donor atoms bonded to the central metal. In many complexes, the most common shapes are octahedral, tetrahedral, and square planar. Coordination number and molecular geometry are linked in a clear pattern. A coordination number of 2 gives a linear shape, as in [Ag(NH3)2]+. A coordination number of 3 gives a trigonal planar shape, as in...

structural isomerism

Linkage and Ionization Isomers

Isomers are different chemical species that share the same chemical formula. In coordination compounds, structural isomerism includes linkage isomers and coordination-sphere isomers. These two forms show how the same atoms can be arranged in different ways around a metal center. Linkage isomers form when a ligand can attach to a transition metal through two different atoms. The cyanide ligand, CN−, can bind through carbon or nitrogen. The thiocyanate ligand, SCN−, can bind through sulfur or...

stereoisomerism

Isomer Shapes in Coordination Complexes

Isomer shapes in coordination complexes can change a compound’s properties even when the chemical formula stays the same. Isomers are different chemical species with the same formula. In transition metal complexes, the atoms stay connected through the same types of bonds, but their arrangement in space can differ. One common form is geometric isomerism. In these complexes, ligands (the ions or molecules attached to the metal) can sit in cis or trans positions. The octahedral [Co(NH3)4Cl2]+ ion...

valence bond theory

Metal Ligand Bonds in Coordination Complexes

Coordination complexes form metal-ligand bonds through valence bond theory. In this model, Linus Pauling explained bonding with hybridization and overlap of atomic orbitals. The central metal atom or ion acts as a Lewis acid. It uses empty orbitals of suitable energy to accept electron pairs from ligands, which act as Lewis bases. These coordinate covalent bonds help explain the color, geometry, and magnetic behavior seen in coordination compounds. The type of hybridization helps determine the...

crystal field theory - octahedral complexes

crystal-field-theory-octahedral-complexes

Octahedral d-Orbital Splitting in Crystal Fields

Crystal field theory explains how ligands affect the d orbitals in transition metal complexes. This electrostatic model helps predict the colors, magnetic behavior, and some structures of coordination compounds. It focuses on the nonbonding electrons on the central metal ion, not on the metal-ligand bonds. In crystal field theory, the metal ion and ligands are treated as very small point charges. Because electrons are negative, electrons donated by the ligands repel the electrons in the...

crystal field theory - tetrahedral and square planar complexes

crystal-field-theory-tetrahedral-and-square-planar-complexes

Crystal Field Splitting in Non-Octahedral Shapes

Crystal field theory also explains d orbital splitting in tetrahedral and square planar complexes. These shapes do not follow the same pattern as an octahedral complex, so the d orbitals respond to ligand placement in different ways. In tetrahedral complexes, the four ligands sit between the axes. None of the d orbitals points directly at the ligands, but the d x2−y2 and d z2 orbitals lie along the Cartesian axes and overlap less with the ligands than the d xy, d xz, and d yz orbitals. The d...

colors and magnetism

Color and Spin in Coordination Complexes

Color in coordination complexes comes from how metal electrons absorb light. When atoms or molecules absorb light at the right frequency, electrons move to higher-energy orbitals. For many main-group atoms and molecules, the absorbed light is ultraviolet and cannot be seen. In coordination compounds, the energy gap between d orbitals often matches visible light, so the compound can absorb and emit colors that the human eye detects. Small changes in orbital energy can cause large shifts in the...

key terms and concepts

Explore coordination complexes, ligand types, coordination numbers, and chelation using examples like hemoglobin, chlorophyll, and heme for high school chemistry.

Coordination Complexes and Chelation | JoVE K12

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Coordination Complexes and Chelation

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