Name: coordination complexes and chelation
Uploaded: 2020-09-24T15:06:53.000Z
Duration: 2 min 51 s
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K12 Standards

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New York State Science Learning Standards

High School

Physical Science

HS. Structure and Properties of Matter

HS-PS2-6.

Metal-Ligand Bonds

Karmaşık bir iyonda metal iyon, ligandlar olarak bilinen anyonik veya nötr moleküllere bağlanır. Ligandlar bir veya daha fazla yalnız elektron çiftine sahiptir ve elektron çifti vericileri veya Lewis bazları olarak işlev görürler. Elektron çiftini, bir elektron çifti alıcısı veya bir Lewis asidi görevi gören metal iyonuna bağışlarlar.Bu nedenle, metal iyonu ve ligand arasındaki koordinat kovalent bir bağ, bir Lewis asit-baz eklentisi oluşturur. Bir elektron çifti veren ligand atomu, verici atom olarak bilinir. Metal iyonunu çevreleyen verici atomların sayısı, metal iyonunun koordinasyon sayısı ile ilişkilidir.Mevcut verici atomların sayısına bağlı olarak ligandlar ayrıca yüklü veya nötr olabilen monodentat, bidentat veya polidentat ligandlar olarak sınıflandırılır. Tek dişli ligandlar yalnızca bir verici atom içerir. Oksijen, nötr bir su molekülündeki bir verici atomdur;nitrojen, yüklü bir siyanür iyonunda bir verici atomdur.Çift dişli ligandlar, aynı anda bir metal iyonuna bağlanmak için yeterince uzak olan iki verici atomuna sahiptir. Üç bipiridin molekülünün nitrojen atomları, altı koordinasyon ile bir rutenyum iyonuna bağlanır. Bir polidentat ligand, yapısında bulunan iki veya daha fazla verici atoma sahiptir.Burada, iki dietilentriamin molekülünden altı nitrojen, bir kobalt iyonuna bağlanır. Birden fazla verici atomun merkezi metal iyonunu bir pençe gibi tuttuğu görüldüğünden, iki dişli ve çok dişli ligandlara şelatlama maddeleri de denir. Bir kenetleme maddesi, merkezi metal iyonu için tek dişli bir liganddan daha fazla afiniteye sahiptir ve daha kararlı bir koordinasyon kompleksi oluşturur.Bu şelatlama etkisi olarak bilinir. Şelat ajanları çok yönlüdür. Bozunma reaksiyonlarını katalize eden eser metal iyonlarını kompleksleştirerek veya etilendiamintetraasetat veya EDTA kullanarak kurşun zehirlenmesini tedavi ederek gıda ürünlerinin raf ömrünü uzatmak için bir reaksiyonda karışan metal iyonlarını karmaşık hale getirmek için kullanılırlar.Karmaşık iyon oluşumu, metal iyonunun ve ligandların, oksidasyondaki değişim ve indirgeme potansiyelleri veya renkler gibi fizikokimyasal özelliklerini etkiler. Ayrıca ligandlar, hidratlanmış metal iyonlarının deprotonasyonu veya kuvvetli bir şekilde çekilen başka bir ligand tarafından yer değiştirmesi gibi reaksiyonlara girebilir. Burada su molekülü, metal iyonuna daha güçlü bağlanan amonyak ile değiştirilir.

metal-ligand bağları

Kandaki hemoglobin, yeşil bitkilerdeki klorofil, B-12 vitamini ve polietilen üretiminde kullanılan katalizörün hepsi koordinasyon bileşikleri içerir. Metallerin iyonları, özellikle geçiş metalleri, kompleksler oluşturma olasılığı daha yüksektir.
 
 Bu komplekslerde, geçiş metalleri, bağdaki elektronların her ikisinin de bir donör (Lewis bazı) tarafından bir elektron alıcısına (Lewis asidi) katkıda bulunduğu bir tür Lewis asit-baz etkileşimi olan koordinat kovalent bağları oluşturur. Genellikle merkezi bir metal iyonu (veya atomu) olarak adlandırılan koordinasyon komplekslerindeki Lewis asidi, geçiş metali veya iç geçiş metalidir. Ligandlar olarak adlandırılan Lewis baz donörleri, çok çeşitli kimyasallar -atomlar, moleküller veya iyonlar- olabilir. Tek gereklilik, merkezi metale bağlanabilen bir veya daha fazla elektron çiftine sahip olmalarıdır. Çoğu zaman, bu, metale koordinat bağı oluşturabilen yalnız bir elektron çiftine sahip bir donör atomunu içerir. Koordinasyon küresi, merkezi metal iyonu veya atomunun yanı sıra bağlı ligandlarından oluşur. Bir formüldeki parantezler koordinasyon küresini içine alır; parantezlerin dışındaki türler koordinasyon küresinin bir parçası değildir.
 
 Ligandlar, merkezi metalle sadece bir atomla bağlandıklarında, Yunanca’da 'tek dişli' anlamına gelen monodentattır. Burada ligand sayısı ve koordinasyon sayısı eşittir. NH3, Cl− ve H2O gibi bir donör atomuna sahip ligandlar monodentat ligandlardır. Diğer birçok ligand, metali daha karmaşık şekillerde koordine eder.
 
 Bidentat ligandları, iki atomun metal merkezine koordine ettiği ligandlardır. Örneğin, etilendiamin (en, H2NCH2CH2NH2), her biri yalnız bir çifte sahip olan ve bir Lewis bazı olarak hizmet edebilen iki azot atomu içerir (Şekil 1a). Her iki atom da tek bir metal merkezine koordine olabilir. [Co(en)3]+3 kompleksinde üç bidentat en ligand vardır ve kobalt(III) iyonunun koordinasyon numarası altıdır (Şekil 1b). En yaygın koordinasyon numaraları iki, dört ve altıdır, ancak 1'den 15'e kadar olan tüm koordinasyon numaralarının örnekleri bilinmektedir.
 
 <img alt="Image1" src="/files/ftp_upload/11456/11456_Image_1.svg" style="text-align: center; height: 200px;" />
 
 Şekil 1. (a) etilendiamin (en), her biri bir metal iyonu ile koordine olabilen yalın bir çift olan iki azot atomu içerir. (b) Üç bidentat en ligandları tek bir kobalt iyonu ile koordine olur.
 
 Birden fazla donör atomu ile merkezi bir metal iyonuna bağlanan herhangi bir ligand, bir polidentat liganddır (veya 'birçok diş'), çünkü birden fazla bağ ile metal merkezini ısırılabilir. Yunancadan 'pençe' anlamına gelen şelat terimi de bu tür bir etkileşimi tanımlamak için kullanılır. Birçok polidentat ligand şelat ligandlarıdır ve bu ligandlardan bir veya daha fazlasından oluşan bir kompleks ve merkezi metal, bir şelattır. Bir şelatlama ligand da bir şelatlama maddesi olarak bilinir. Şelatlı bir ligand, bir yengeç pençesinin bir mermeri tuttuğu gibi metal iyonunu tutar. Polidentat ligandları bazen liganddaki donör atomlarının sayısını gösteren öneklerle tanımlanır. Hemoglobindeki heme kompleksi bir başka önemli örnektir (Şekil 2). Demir ile koordine olan dört donör atomuna sahip bir polidentat ligand içerir.
 
 <img alt="Image2" src="/files/ftp_upload/11456/11456_Image2.svg" style="text-align: center; height: 200px;" />
 
 Şekil 2::  Tek ligand heme, bir şelat oluşturmak için hemoglobin içindeki demire koordine olan dört azot atomu içerir.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/19-2-coordination-chemistry-of-transition-metals">Openstax, Chemistry 2e, Chapter 19.2 Coordination Chemistry of Transition Metals</a>.

Metal-Ligand Bağları

Kandaki hemoglobin, yeşil bitkilerdeki klorofil, B-12 vitamini ve polietilen üretiminde kullanılan katalizörün tümü ...

Education

JoVE Core

Chemistry

Kimya

Transition Metals and Coordination Complexes

Geçiş Metalleri ve Koordinasyon Kompleksleri

transition-metals-and-coordination-complexes

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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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