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

في أيون معقّد،يكون الأيون الفلزي مرتبطًا بجزيئات سالبة أو محايدة الشحنة،تُعرف بالربيطات. تحتوي الربيطات على زوج وحيد أو أكثر من الإلكترونات،وتؤدي دور مانح الإلكترونات أو قواعد لويس. تمنح زوج الإلكترونات للأيون الفلزي،والذي يؤدي دور مستقبل الإلكترونات أو حمض لويس.وهكذا تنشأ رابطة تناسقية تساهمية بين الأيون الفلزي والربيطة،لتُكون ناتج إضافة حمض-قاعدة لويس. ذرة الربيطة المانحة لزوج الإلكترونات،تُعرف بالذرة المانحة. يرتبط عدد الذرات المانحة المحيطة بالأيون الفلزي،بالعدد التناسقي للأيون الفلزي.وفقًا لعدد الذرات المانحة الموجودة،تصنف الربيطات الى أحادية السن،ثنائية السن،أو متعددة السن،و التي يمكن أن تكون مشحونة أو محايدة. تحتوي الربيطات أحادية السن على ذرة مانحة واحدة. الأكسجين ذرة مانحة في جزيء ماء محايد،والنيتروجين ذرة مانحة في أيون سيانيد مشحون.تحتوي الربيطات ثنائية السن على ذرتين مانحتين متباعدتين بما يكفي،ليرتبطا بأيون فلزي في اللحظة ذاتها. ترتبط ذرات من ثلاثة جزيئات ثنائي البريدين مع أيون روثينيوم عدده التناسقي 6. أما الربيطات متعددة السن،فتحتوي على ذرتين مانحتين أو أكثر موجودة في تركيبتها.ترتبط،هنا،ست ذرات نيتروجين من جزيئين دايايثلين ترايامين مع أيون كوبالت. حيث يبدو أن عدة ذرات مانحة تمسك بالأيون الفلزي كالمخلب،تُسمى كذلك الربيطات ثنائية السن ومتعددة السن بعوامل التمخلب. عامل التمخلب أكثر تقاربًا مع الأيون المركزي من الربيطة أحادية السن،مما يشكل مركبًا تناسقيًا أكثر استقرارًا.يُعرف هذا بتأثير التمخلب. عوامل التمخلب متنوعة. تُستخدم لتعقيد الأيونات الفلزية المتداخلة في التفاعل—لإطالة صلاحية منتجات الطعام،عبر تعقيد أيونات الفلزات النادرة،المتورطة في تحفيز تفاعلات التفكك أو معالجة سمّية الرصاص،باستخدام ثنائي أمين الإيثيلين-رباعي حمض الأسيتيك أو EDTA.يؤثر تشكيل أيون المعقّد في الخواص الفيزيوكيميائية للأيون الفلزي والربيطات،كالتغير في التأكسد والاختزال أو في اللون. كما أن الربيطات قد تخضع لتفاعلات،مثل نزع البروتون من الأيونات الفلزية المميهة،أو الطرد بواسطة ربيطة أخرى قوية الانجذاب. هنا،يحل جزيء الأمونيا محل جزيء الماء،لأن جزيء الأمونيا يرتبط بقوة أكبر مع الأيون الفلزي.

روابط الربيطات المعدنيّة

تحتوي كل من الهيموغلوبين في الدم، والكلوروفيل في النباتات الخضراء، وفيتامين بي-12، والمحفز المستخدم في تصنيع البولي إيثيلين، على مركبات التنسيق. ومن المحتمل أن تشكل أيونات المعادن، وخاصة المعادن الانتقالية، معقدات . في هذه المجمعات، تشكل المعادن الانتقالية روابط تساهمية منسقة، وهو نوع من تفاعل حمض لويس حيث يساهم متبرع (قاعدة لويس) في مستقبل الإلكترون (حمض لويس). حمض لويس في معقدات التنسيق، غالباً ما يطلق عليه أيون معدني مركزي (أو ذرة)، هو معدن انتقالي أو معدن انتقالي داخلي. يمكن أن تكون الجهات المانحة لقاعدة لويس، والتي تسمى الروابط، مجموعة متنوعة من المواد الكيميائية— الذرات أو الجزيئات أو الأيونات. الشرط الوحيد هو أن يكون لديهم واحد أو أكثر من أزواج الإلكترونات، والتي يمكن التبرع بها للمعدن المركزي. في أغلب الأحيان، يتضمن ذلك ذرة مانحة بزوج وحيد من الإلكترونات يمكن أن يشكل رابطة إحداثيّة مع المعدن. يتكون مجال التنسيق من أيون معدني مركزي أو ذرة بالإضافة إلى الروابط المرتبطة به. تضم الأقواس في الصيغة مجال التنسيق ؛ الأنواع الموجودة خارج الأقواس ليست جزءًا من مجال التنسيق. الربيطات هي روابط أحادية، من اليونانية لـ “ذات سن واحد,” عندما يتصلون بالمعدن المركزي من خلال ذرة واحدة فقط. هنا، عدد الروابط ورقم التنسيق متساويان. الروابط التي تحتوي على ذرة مانحة واحدة، مثل NH3, Cl−, و H2O، هي روابط أحادية. العديد من الروابط الأخرى تنسق مع المعدن بأشكال أكثر تعقيداً. الروابط الثنائية هي تلك التي تتناسق فيها ذرتان مع مركز المعدن. على سبيل المثال، يحتوي إيثيلين ديامين (إن)(H2NCH2CH2NH2) على ذرتين من النيتروجين، كل منهما التي لها زوج وحيد ويمكن أن تكون بمثابة قاعدة لويس (الشكل 1 أ). يمكن لكل من الذرات التنسيق في مركز معدني واحد. في المركب [Co(en)3]3+، هناك ثلاثة ربيطات en ثنائية، ورقم تنسيق الكوبالت (III ) أيون ستة (الشكل 1 ب). أرقام التنسيق الأكثر شيوعًا هي رقمان وأربعة وستة، ولكن من المعروف أن جميع أرقام التنسيق من 1 إلى 15 معروفة. <img alt="Image1" src="/files/ftp_upload/11456/11456_Image_1.svg" style="text-align: center; height: 200px;" /> الشكل 1 . (أ) يحتوي إيثيلين ديامين (إن) على ذرتين من النيتروجين، مع زوج واحد لكل منهما، يمكن أن ينسق مع أيون معدني. (ب) تنسق ثلاث روابط en ثنائية مع أيون كوبالت واحد. أي ربيطة مرتبطة بأيون معدني مركزي بأكثر من ذرة مانحة هو يجند متعدد الأرجل (أو “متعدد الأسنان”) لأنه يمكن أن يعض في المركز المعدني بأكثر من رابطة واحدة. مصطلح شيلات من اليونانية لـ “مخالب” يستخدم أيضاً لوصف هذا النوع من التفاعل. العديد من الترابطات المتعددة هي بروابط مخلبية، والمركب يتكون من واحد أو أكثر من هذه الروابط والمعدن المركزي هو مخلّب. يُعرف الارتباط المخلب أيضًا باسم عامل مخلب. يجند مخلب يحمل الأيونات المعدنية إلى حد ما مثل مخلب’ السلطعون الذي يحمل قطعة رخامية. يتم التعرف أحيانًا على الروابط المتعددة البادئات مع البادئات التي تشير إلى عدد الذرات المانحة في الترابط. يعتبر مركب الهيم في الهيموجلوبين مثالًا مهمًا آخر (الشكل 2). يحتوي على يجند متعدد الأسطح مع أربع ذرات مانحة تنسق مع الحديد. <img alt="Image2" src="/files/ftp_upload/11456/11456_Image2.svg" style="text-align: center; height: 200px;" />الشكل2:&#160؛ يحتوي الهيم الترابطي المنفرد على أربع ذرات نيتروجين تنسق مع الحديد في الهيموغلوبين لتكوين مخلّب. هذا النص مقتبس من <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>.

يحتوي الهيموجلوبين الموجود في الدم ، والكلوروفيل في النباتات الخضراء ، وفيتامين ب 12 ، والمحفز المستخدم في تصنيع البولي إيثيلين ، على ...

Education

JoVE Core

Chemistry

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واحد

Transition Metals and Coordination Complexes

الفلزات الانتقالية والمعقدات التناسقية

transition-metals-and-coordination-complexes

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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

chemistry

JoVE Core Chemistry brings general chemistry concepts to life using concise and easy-to-understand animated video lessons. Plus, in the scientist-in-action videos, we demonstrate classical and original research experiments performed in today's laboratories worldwide.

Periodic Classification of the Elements

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definition-measurement-pressure-atmospheric-pressure-barometer

Definition and Measurement of Pressure: Atmospheric Pressure, Barometer, and Manometer

Gas pressure is caused by force exerted by gas molecules colliding with the surfaces of objects. Although the force of each collision is very small, any ...

gas-laws-boyle-s-gay-lussac-charles-avogadro-s-and-ideal-gas-law

Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and ...

applications-of-the-ideal-gas-law-molar-mass-density-and-volume

Applications of the Ideal Gas Law: Molar Mass, Density, and Volume

The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT, &nbsp;suggests that the volume of a given quantity of gas ...

mixtures-of-gases-dalton-s-law-of-partial-pressures-and-mole-fractions

Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other&rsquo;s pressure. Each gas ...

chemical-stoichiometry-gases-using-ideal-gas-law-to-determine

Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.

In addition to measuring quantities ...

Analyze data to support the claim that the combined gas law describes the relationships among volume, pressure, and temperature for a sample of an ideal gas.

HS-PS1-9.

Coordination Complexes and Chelation

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