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COORDINATION COMPOUNDS | Complete Chapter in 1 Shot | Class 12th Board - NCERT

NCERT Wallah・152 minutes read

Harsh Soni teaches a comprehensive lecture on D Coordination Compounds in the Winner Batch, covering topics like crystal field theory, isomerism, and the importance of understanding coordination compounds. The lecture aims to provide students with a deep understanding of coordination compounds, emphasizing the composition, naming of components, and complex stability through concepts like crystal field splitting and magnetic properties.

Insights

  • Understanding coordination compounds involves recognizing the composition and naming of components within a complex, stressing the interdependence of its parts.
  • The presence of ligands, their classification based on charge and dentility, and the coordination number around the central metal atom are crucial in determining the structure and properties of coordination compounds.
  • The Crystal Field Theory explains the interaction between ligands and metal ions, leading to the splitting of metal orbitals, which determines the stability and properties of complexes.
  • The importance of IUPAC nomenclature, hybridization, and Crystal Field Theory in understanding the structure, bonding, and properties of coordination compounds is emphasized, impacting their color, magnetic properties, and overall stability.

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Recent questions

  • What are coordination compounds?

    Coordination compounds are complexes that do not allow individual ions to exist independently. They involve a central metal atom coordinated with ligands, forming coordinate bonds. The number of ligands bound around the central metal atom is known as the coordination number, which can vary. These compounds play a crucial role in chemistry due to their unique structures and bonding characteristics.

  • How are ligands classified?

    Ligands are classified based on their charge and dentility. Positive, negative, or neutral ligands have specific naming conventions. Dentate ligands can be monodentate, bidentate, or polydentate, depending on the number of donor sites they possess. Examples like ethylene and ethylenediamine illustrate the concept of dentate ligands with varying numbers of donor sites, which can range from three to six.

  • What is the Crystal Field Theory?

    The Crystal Field Theory (CFT) explains the interaction between metal ions and ligands in coordination compounds. When ligands approach a metal ion, the metal orbitals degenerate and split, leading to crystal field stabilization energy. This theory helps distinguish between high spin and low spin complexes based on the extent of splitting and electron pairing. Understanding CFT is crucial for predicting the magnetic properties and color of coordination compounds.

  • How does the spectrochemical series impact complex stability?

    The spectrochemical series ranks ligands based on their strength, with ligands on the left being weak and those on the right being strong. Ligand strength affects the electron density and stability of the complex, influencing crystal field splitting. The type of metal, oxidation state, and number of ligands also play a role in determining complex stability, making the spectrochemical series a valuable tool in predicting ligand behavior.

  • Why is understanding isomerism important in coordination compounds?

    Isomerism is crucial in coordination compounds as it highlights the different ways in which molecules with the same chemical formula can be arranged. Structural isomerism, geometrical isomerism, and optical isomerism are common types found in coordination compounds. Understanding isomerism is essential for thorough exam preparation and a comprehensive grasp of the diverse properties exhibited by coordination compounds.

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Summary

00:00

Importance of D Coordination Compounds in Chemistry

  • Harsh Soni is teaching a lecture on D coordination compounds in the Winner Batch
  • The lecture emphasizes the importance of understanding D Coordination Compounds
  • Topics covered include Introduction to coordination compounds, Classification of D Ligands, IUPAC, Beta Varna Theory, Norman Clacher Theory, Near Balance bond theory, Crystal Field Theory, and Isomerism
  • Addition compounds are discussed, defined as the result of mixing two solutions in equal parts
  • Types of addition compounds include Double Salt and Coordination Compound
  • The individual existence of ions in a solution is highlighted through reactions with specific reagents
  • Coordination compounds are explained as complexes that do not allow individual ions to exist independently
  • The importance of understanding the composition and naming of components within a complex is stressed
  • The lecture aims to provide a comprehensive understanding of coordination compounds and their components
  • Students are encouraged to pay attention, take notes, and understand the concepts thoroughly

18:37

Understanding Coordination Complexes and Central Metal Atoms

  • Coordination complex involves square brackets, which represent the coordination phase.
  • The square brackets have their own name, known as coordination phase.
  • Anything outside the square brackets is called a counter ion, such as ionization fer.
  • The central metal atom is an essential part of the coordination complex.
  • Ligands are components connected to the central metal atom in a definite geometry.
  • Coordination number refers to the number of ligands bound around the central metal atom.
  • Central coordination compounds contain a central metal atom coordinated with ligands.
  • The bond between the metal and ligands is known as a coordinate bond.
  • Ligands can be ions or groups connected to the metal through coordinate bonds.
  • The coordination number is the number of dative bonds around the central metal atom in a coordination compound.

37:22

Understanding Coordination Complexes and Ligands in Chemistry

  • Beta Copper was the first person to have the complex.
  • The charge above the square bracket determines the compound's name.
  • The coordination phase in the Time Coordination Complex of Beta Campus decides the charge for the premises.
  • The charge on the premises determines if the compound is cationized or anionized.
  • If there is no charge on the premises, it is considered neutral.
  • Different types of ligands present in the compound affect its classification.
  • Ligands attached to metal are called ligands, and different types of ligands result in heteroleptic or homoleptic compounds.
  • Ligands are classified based on their charge, with positive, negative, or neutral ligands having specific naming conventions.
  • Ligands are also classified based on their dentility, with monodentate, bidentate, and polydentate ligands having varying numbers of donor sites.
  • Examples like ethylene and ethylenediamine illustrate the concept of dentate ligands with different numbers of donor sites.

55:52

Ligands and EDTA: Bonding and Stability

  • Ligands can have three, four, five, or six donating sides.
  • Full form of EDTA is ethylenediaminetetraacetate.
  • The structure of EDTA should be remembered well.
  • The donating side of ligands should be noted, with nitrogen being a key donor.
  • Classification based on the bond formed between ligand and metal is discussed.
  • Synergic bonding is an important concept with few questions asked.
  • Stability order of complexes formed due to ligand-metal interactions is crucial.
  • Coordination number of complexes is significant, often being six.
  • Ring formation due to ligand donation is explained, with examples like ethylene.
  • Different ligands like cyanide, isocyanide, nitro, and nitrite have distinct donation patterns.

01:19:00

Ligands and Charges in Chemistry

  • Ligands play a crucial role in chemistry, with specific names and charges to remember.
  • Fluoro is a negative ligand with a charge of -1.
  • Sulphate is a ligand with a charge of -2, known as oxide.
  • Hydroxo is a ligand with a charge of -1.
  • NH2 is a ligand known as amide with a charge of -1.
  • Ammonia can become ammine with a positive charge by excluding one positive.
  • Neutral ligands have names like aqua, amine, carbonate, and nitrosyl, with charges of zero.
  • Polydentate ligands like ethylene and glyoxalate have specific structures and charges.
  • Coordination complexes involve primary and secondary valencies, oxidation states, and coordination numbers.
  • Determining oxidation states in coordination compounds involves breaking down the complex and calculating charges.

01:41:10

"Six Coordinate Bonds and Coordination Number"

  • Six ligands are forming, leading to the discovery of six coordinate bonds.
  • Coordination number is determined to be six.
  • Burner ji introduced the concept of coordination number.
  • The oxidation state of the son is emphasized.
  • The reaction of AGNO3 with AGCL results in AGCL's PPT.
  • The breakdown of the complex is explained, resulting in the formation of AGCL.
  • Molar conductance decreases from top to bottom due to the number of ions.
  • IUPAC nomenclature rules are detailed, emphasizing the order of naming ligands and metals.
  • The oxidation state is indicated in Roman numerals.
  • The presence of chloride ions is highlighted in the naming process.

01:58:40

Metal Complex Naming Conventions and Oxidation States

  • The name of the metal remains the same in a complex, not changing even with a complex time.
  • The metal's name should be clear and unchanged in a complex.
  • The next name in the complex is "Penta Amin."
  • The complex should be written alphabetically, with "Penta Amin Chloride" following "Cobalt Chloride."
  • The oxidation state in the complex is determined by the formula x + 5 * 0 + -1 = +2, resulting in an oxidation state of +3.
  • The charge on the metal in a complex affects the naming convention, with a positive charge keeping the metal's name unchanged.
  • The complex "K3FeCN6" should be written without spaces, with "Penta Amine Chloride" preceding "Cobalt Chloride" alphabetically.
  • In a complex, the positive part of the name is written before the negative part, with "Potassium" preceding "Chloride."
  • The number of ligands in a complex determines the naming convention, with "Hexacino" used for six ligands.
  • The oxidation state in a complex is calculated using the formula x + 3 * -2 = -3, resulting in an oxidation state of +3.

02:18:38

Chemical Bonding and Magnetic Properties Explained

  • The value of X plus three determines the oxidation state, crucial for understanding chemical structures.
  • Understanding IUPAC naming is essential for creating chemical structures accurately.
  • Coordination compounds and hybridization play a significant role in chemical bonding.
  • Coordination numbers four and six are common in chemical compounds, affecting their hybridization.
  • The concept of Valence Bond Theory is crucial for understanding chemical bonding.
  • Hybridization determines the shape and structure of chemical compounds.
  • The presence of unpaired electrons affects the magnetism of chemical compounds.
  • The formula for calculating magnetic moment involves the number of unpaired electrons.
  • The magnetic moment value indicates the presence of unpaired electrons in a compound.
  • Diamagnetic and paramagnetic properties are determined by the presence of unpaired electrons in a compound.

02:37:29

Key Concepts in Transition Metal Chemistry

  • The presence of 4 unpaired electrons indicates a magnetic moment of 4.90.
  • Questions regarding balance calculation and Bond Theory are crucial and must be taken seriously.
  • Hybridization, outer and inner electrons, and paramagnetic properties are key topics to address.
  • Coordination number four and the electronic configuration of nickel are significant considerations.
  • Accommodating four relatives is essential, requiring four boxes.
  • The importance of unpaid electrons and magnetic moment being zero is emphasized.
  • The electronic configuration of copper and the hybridization of a complex are essential to understand.
  • The exception in the crystal field theory regarding hybridization is discussed.
  • The distinction between ionic bonding and the interaction between metal and ligand is explained.
  • Forces of attraction and repulsion between ligand and metal are crucial in understanding bonding.

03:07:32

Metal-Ligand Interactions: Electron Density and Stability

  • Metal with electron density attracts ligands, causing repulsion between ligands and metal electrons.
  • Force of attraction and repulsion between ligands and metal electrons is crucial.
  • Metal orbitals, like DX² and DX² - Y², are affected by ligand approach, leading to repulsion.
  • Electron density is significant in determining repulsion and attraction forces.
  • Metal orbitals degenerate when ligands are at a distance, but split when close.
  • Splitting of metal orbitals leads to crystal field stabilization energy.
  • Isolated and spherically symmetrical fields are observed when ligands are at varying distances.
  • Crystal field stabilization energy is influenced by the distance between ligands and metal.
  • High spin and low spin complexes are distinguished by the extent of splitting and stability.
  • Electron pairing in complexes is determined by the extent of splitting, affecting stability.

03:27:47

"Electron movement and complex stability factors"

  • To understand electron movement, it's crucial to consider the gap's size and the electron's position.
  • Low spin complexes require filling the bottom box first, while high spin complexes involve filling the top half initially.
  • Electronic configuration calculation involves specific formulas like -0.4 * 5 and -0.4 * P + 0.6 * K.
  • Factors affecting CFMS include the oxidation state of the metal, where higher states lead to more splitting.
  • The type of metal, such as 4D or 5D, impacts complex stability and splitting.
  • The number of ligands influences repulsion forces, with more ligands leading to increased splitting.
  • Splitting varies in square planar, tetrahedral, and octahedral complexes, with the most significant in square planar.
  • Crystal field theory and the spectrochemical series are essential for understanding ligand strength and complex stability.

03:53:40

Ligand Strength and Color in Coordination Compounds

  • The strength of a ligand increases from left to right, affecting the electron density and stability of the complex.
  • Ligands can be weak or strong depending on their position in the series and the electron density they possess.
  • Creating a crystal field splitting diagram involves determining the electronic configuration, oxidation state, and ligand strength.
  • High spin complexes with strong ligands have a significant impact on metal bonding and stability.
  • The Crystal Field Theory (CFT) helps in understanding the magnetic properties and color of coordination compounds.
  • Color in coordination compounds is determined by the presence of unpaired electrons and DD transitions.
  • Metal charge transfer between ligands and metals influences the color of the complex.
  • Isomerism is the final topic to be covered in the lecture series on coordination compounds, emphasizing the importance of thorough preparation for exams.
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