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coordination compounds one shot revision class 12th chemistry, coordination compounds one shot

Munil Sir・70 minutes read

Coordination Compounds are complex structures that involve the central metal atom, ligands, and coordination numbers. Understanding IUPAC naming, isomerism, bonding theories, and spectrochemical series is crucial for comprehending the formation and properties of coordination compounds.

Insights

Coordination compounds involve a central metal atom bonded to ligands, defining the coordination number based on ligand arrangement.
IUPAC naming for coordination compounds follows specific rules, focusing on ligands, metal names, oxidation numbers, and charges within the coordination sphere.
Understanding isomerism in coordination compounds, including optical isomerism and various types like geometrical and facial isomerism, is crucial for comprehensive knowledge.

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Recent questions

What is Coordination Compound?
Coordination Compound is a complex chemical topic.
How are Coordination Compounds named?
Coordination Compounds are named using IUPAC conventions.
What is Chelation in Coordination Compounds?
Chelation involves ligands forming ring-like structures around central metal atoms.
What is the significance of isomerism in Coordination Compounds?
Isomerism in Coordination Compounds involves different structural arrangements.
How does Crystal Field Theory explain Coordination Compounds?
Crystal Field Theory describes the splitting of orbitals in Coordination Compounds.

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Summary

00:00

Essential Concepts in Coordination Compound Formation

Coordination Compound is a comprehensive topic that requires thorough understanding and honesty in studying.
Chapter One and a Half hours is crucial for grasping the concepts of Coordination Compound.
The chapter involves hard work and dedication, focusing on the central metal atom and ligands.
Coordination Compound is also known as Complexion Compound, emphasizing the importance of understanding its structure.
Pouring water into the compound showcases its unique properties of not breaking, highlighting its complexity.
The compound formation is stabilized by bonding between the central metal atom and ligands, creating a Coordination Compound.
The arrangement of ligands around the central metal atom defines the coordination number, indicating the number of ligands binding to it.
Different types of ligands, such as Uni-dented and Di-dented, play a crucial role in forming Coordination Compounds.
Poly-dented ligands consist of multiple donor atoms within the same molecule, enhancing the complexity of the compound.
Understanding the various types of ligands, such as Glycinate and Oxalato, is essential for comprehending the formation of Coordination Compounds.

13:09

IUPAC Naming for Coordination Compounds

Monotech Ligands are special ligands that can coordinate through more than one side, such as NO2, which can coordinate through O and N.
Chelation is a process where a ligand forms a ring-like structure around a central metal atom, stabilizing it by donating electrons from multiple sides.
Chelation occurs when a ligand can donate electrons in multiple ways to a central metal atom, increasing stability.
Coordination number represents the number of places from which electrons are obtained, with examples like Cobalt having a coordination number of 6.
IUPAC naming for ligands includes terms like Chlorido for Cl, Cyano for CN, and Nitro for NO2, while metal names like Cobalt are used in coordination compounds.
The IUPAC naming process involves determining the oxidation number of the central metal atom, naming ligands and metals, and considering charges within the coordination sphere.
In IUPAC naming, ligands are named first, followed by the metal name and its oxidation number, with attention to charges and the presence of ligands on the side.
The trick for IUPAC naming involves focusing on ligands and metals inside the coordination sphere, with specific naming conventions for ligands like Nitrito and metals like Iron.
Understanding the charge distribution and naming conventions is crucial for accurately naming coordination compounds using the IUPAC system.
Practical examples and step-by-step explanations are provided to guide the process of IUPAC naming for coordination compounds, emphasizing clarity and precision in the naming conventions.

22:39

Determining Oxidation Numbers and Isomerism in Coordination Compounds

The text discusses the process of determining oxidation numbers in coordination compounds.
It emphasizes the importance of understanding the charges and coordination spheres of ions.
The text mentions the significance of identifying ligands and their coordination numbers.
It explains the rules for assigning oxidation numbers to different elements in coordination compounds.
The text delves into the concept of isomerism in coordination compounds, including ionization, solvate, hydrate, linkage, and coordination isomerism.
It details the differences between various types of isomerism, such as facial and geometrical isomerism.
The text also covers optical isomerism, highlighting the need to consider mirror images of compounds to determine if they are optically active.
It provides examples of compounds and their mirror images to illustrate optical isomerism.
The text underscores the importance of understanding the coordination number of elements in coordination compounds.
It concludes by mentioning the relevance of optical isomerism in organic chemistry and the necessity of analyzing mirror images for isomeric compounds.

32:26

Understanding Coordination Compounds: Valence Bond Theory Essentials

Coordination number four is represented in a diagram as 1 2 3 4, while coordination number six is shown as 1 2 3 4 5 6.
When dealing with coordination number six, cobalt is used, and six lines are drawn to represent the coordination.
If there are three 'no's, one 'no' is placed in the diagram to show bonding.
The process of bonding is explained, emphasizing how certain elements bond with each other.
Mirror images are taken to show optical isomerism, with a focus on rotating and adjusting the diagram.
Werner's theory is discussed, highlighting the primary and secondary valencies in coordination compounds.
Practical examples are given to illustrate the application of primary and secondary valencies in coordination compounds.
The process of creating coordination compounds is detailed, including the placement of ligands and the formation of bonds.
Specific examples are provided, such as the reaction between cocl3 6 nh3 and agno3, to demonstrate the formation of coordination compounds.
The importance of understanding Valence Bond Theory and the Spectro Chemical Series in creating coordination compounds is emphasized.

42:01

"Chemistry: Coordination Compounds and Orbital Splitting"

Atomic number 27 corresponds to cobalt.
Questions on coordination compounds may involve hybridization, spin, and magnetic behavior.
Diagrams need to be created for d, s, and p orbitals.
Electron filling involves one doti f pa, six electrons in a, and one or two electrons in p.
Cobalt's P3 configuration results from two electrons moving from s to d.
Ammonia is filled in empty boxes, resulting in sp3 d2 configuration.
Hybridization leads to low spin behavior due to pairing of electrons.
Paramagnetic behavior occurs when electrons are unpaired, while diamagnetic behavior results from pairing.
Crystal field theory explains the splitting of orbitals in octahedral coordination compounds.
Energy gap and splitting occur due to repulsion between approaching ligands.

53:29

Transition Metal Bonding and Coordination Compounds

Energy increases in a free ion, with a shift in proportions from 3/5 to 2/5, leading to no change in overall energy.
Coordination compounds absorb light from the visible range, causing electron transitions from low to high energy levels, known as DD transitions.
Organometallic compounds contain at least one metal-carbon bond, crucial for understanding metal carbonyl bonding.
Metal carbonyl bonding involves the formation of sigma and pi bonds between metal and carbon, creating a synergic effect by electron transfer.
The limitations of valence bond theory (VBT) include the inability to distinguish weak and strong field ligands and insufficient information on color in coordination compounds.

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