experiment 5 chemistry class 12

NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12

CBSE Class 12 Chemistry Lab Manual

Viva Questions with Answers.
Exp-2.1 : To prepare colloidal solution (sol) of starch.
Exp-2.2 : To prepare a colloidal solution of gum.
Exp-2.3 : To prepare colloidal solution (or sol) of egg albumin.
Exp-2.4 : To prepare ferric hydroxide, [Fe(OH) 3 ] sol.
Exp-2.5 : To prepare aluminium hydroxide, [Al(OH) 3 ] sol.
Exp-2.6 : To prepare colloidal solution of arsenious sulphide, [As 2 S 3 ].
Exp-2.7 :To study the dialysis of starch sol containing sodium chloride through a cellophane or parchment paper.
Exp-2.8 : Compare the precipitation values of sodium chloride, barium chloride and aluminium chloride for arsenious sulphide sol.
Exp-2.9 : To study the effectiveness of different common oils (castor oil, cotton seed oil, coconut oil, kerosene oil, mustard oil) in forming emulsions.
Exp-2.10 : To compare the effectiveness of a number of emulsifying agents in forming emulsions.
Surface Chemistry Viva Questions with Answers.
Exp-3.1 : To study the effect of concentration on the rate of reaction between sodium thiosulphate and hydrochloric acid.
Exp-3.2 : To study the effect of change in temperature on the rate of reaction between sodium thiosulphate and hydrochloric acid.
Exp-3.3 : To study the reaction rate of reaction of iodide ions with hydrogen peroxide at different concentrations of iodide ions.
Exp-3.4 : To study the reaction rate of the reaction between potassium iodate (KIO 3 ) and sodium sulphite (Na 2 S0 3 ) using starch solution as indicator.
Chemical Kinetics Viva Questions with Answers.
Exp-4.1 : Determine the calorimeter constant (W) of calorimeter (polythene bottle).
Exp-4.2 : Determine the enthalpy of dissolution of given solid copper sulphate (CuS0 4 .5H 2 0) in water at room temperature.
Exp-4.3 : Determine the enthalpy of neutralisation of hydrochloric acid with sodium hydroxide solution.
Exp-4.4 : Determine the enthalpy change during the interaction (hydrogen bond formation) between acetone and chloroform.
Thermochemistry Viva Questions with Answers.
Exp-5.1 : To set up simple Daniell cell and determine its emf .
Exp-5.2 : To set up simple Daniell cell using salt bridge and determine its emf .
Exp-5.3 : To study the variation of cell potential in Zn | Zn 2+ || Cu 2+ | Cu cell with change in concentration of electrolytes (CuS0 4 and ZnS0 4 ) at room temperature.
Electrochemistry Viva Questions with Answers.
Exp-6.1 : Separate the coloured components present in the mixture of red and blue inks by ascending paper chromatography and find their R f values .
Exp-6.2 : Separate the coloured components present in the given grass/flower by ascending paper chromatography and determine their R f values .
Exp-6.3 : Separate Co 2+ and Ni 2+ ions present in the given mixture by using ascending paper chromatography and determine their R f values .
Chromatography Viva Questions with Answers.
Exp-7.1 : To prepare a pure sample of ferrous ammonium sulphate (Mohr’s salt), [FeSO 4 . (NH 4 ) 2 SO 4 .6HO 2 0] .
Exp-7.2 : To prepare a pure sample of potash alum (Fitkari), [K 2 SO 4 .Al 2 (SO 4 ) 3 . 24H 2 0] .
Exp-7.3 : To prepare a pure sample of the complex potassium trioxalatoferrate(III), Kg[Fe(C 2 O 4 ) 3 l . 3H 2 0 .
Preparation of Inorganic Compounds Viva Questions with Answers.
Exp-8.1 : To prepare a sample of acetanilide from aniline.
Exp-8.2 : To prepare a sample of dibenzalacetone.
Exp-8.3 : To prepare a sample of p-nitroacetanilide from acetanilide .
Exp-8.4 : To prepare 2-naphthol aniline or phenyl-azo-β-naphtholdye .
Preparation of Organic Compounds Viva Questions with Answers.
Exp-9.1 : Identify the functional group present in the given organic compound.
Tests for the Functional Groups Present in Organic Compounds Viva Questions with Answers.
Exp-10.1 : To study some simple tests of carbohydrates .
Exp-10.2 : To study some simple tests of oils and fats .
Exp-10.3 : To study some simple tests of proteins .
Exp-10.4 : To detect the presence of carbohydrates, fats and proteins in the following food stuffs : Grapes, potatoes, rice, butter, biscuits, milk, groundnut, boiled egg .
Tests of Carbohydrates, Fats and Proteins in Pure Samples and Detection of Their Presence in Given Food Stuffs Viva Questions with Answers.
Exp-11.1 : Prepare 250 ml of M/10 solution of oxalic acid from crystalline oxalic acid .
Exp-11.2 : Prepare 250 ml of a N/10 solution of oxalic acid from crystalline oxalic acid .
Exp-11.3 : Preparation of 250 ml of M/20 solution of Mohr’s salt .
Exp-11.4 : Preparation of 250 ml of N/20 solution of Mohr’s salt .
Exp-11.5 : Prepare M/20 solution of ferrous ammonium sulphate (Mohr’s salt). Using this solution find out the molarity and strength of the given KMn04 solution.
Exp-11.6 : Prepare a solution of ferrous ammonium sulphate (Mohr’s salt) containing exactly 17.0 g of the salt in one litre. With the help of this solution, determine the molarity and the concentration of KMnO 4 in the given solution.
Exp-11.7 : Prepare M/20 ferrous ammonium sulphate (Mohr’s salt) solution. Find out the percentage purity of impure KMnO 4 sample 2.0 g of which have been dissolved per litre .
Exp-11.8 : Determine the equivalent mass and number of molecules of water of crystallisation in a sample of Mohr’s salt, FeSO 4 (NH 4 ) 2 SO 4 . nH 2 0. Provided KMnO 4 .
Exp-11.9 : Prepare M/50 solution of oxalic acid. With its help, determine 50 the molarity and strength of the given solution of potassium permanganate (KMnO 4 ).
Exp-11.10 : Find out the percentage purity of impure sample of oxalic acid. You are supplied M/100 KMnO 4 solution.
Exp-11.11 : The given solution has been prepared by dissolving 1.6 g of an alkali metal permanganate per litre of solution. Determine volumetrically the atomic mass of the alkali metal. Prepare M/20 Mohr’s salt solution for titration.

Exp-11.13 : You are provided with a partially oxidised sample of ferrous sulphate (FeSO 4 .7H 2 0) crystals. Prepare a solution by dissolving 14.0 g of these crystals per litre and determine the percentage oxidation of the given sample. Given M/100 KMnO 4 solution.
Exp-11.14 : Calculate the percentage of Fe 2+ ions in a sample of ferrous sulphate. Prepare a solution of the given sample having strength exactly equal to 14.0 g/litre. Provided M/100 KMnO 4 .
Exp-11.15 : Prepare N/20 Mohr’s salt solution. Using this solution, determine the normality and strength of the given potassium permanganate solution.
Exp-11.16 : Prepare N/20 solution of oxalic acid. Using this solution, find out strength and normality of the given potassium permanganate solution .
Exp-11.17 : Determine the percentage purity of the given sample of oxalic acid. Ask for your requirement .
Exp-11.19 : Determine the equivalent mass and number of molecules of water of crystallisation in a sample of Mohr’s salt FeSO 4 (NH 4 ) 2 SO 4 .nH 2 0. Provided N/20 KMnO 4 .
Volumetric Analysis Viva Questions with Answers.
Exp-12.1 : To analyse the given salt for acidic and basic radicals .
Exp-12.2 : To analyse the given salt for acidic and basic radicals CO, Zn.
Qualitative Analysis Viva Questions with Answers.

Free Resources

NCERT Solutions

Quick Resources

[Updated] CBSE Class 12 Chemistry Lab Manual 2024-25 Session in PDF

CBSE Class 12 Chemistry Lab Manual is provided to the students to score well in the examinations. For a subject like Chemistry, it is important to remember the right reactions and what they result in is vital. Students must concentrate on Chemistry Practicals because it has been allocated 30 marks. They must try to get full marks in this section to increase their overall marks in the CBSE class 12 examination. Students should study the laws and theories before performing the experiments and are suggested to revise their practical notes before their examination. That’s why we are providing a Class 12 Chemistry Lab Manual for practice purposes to obtain a great score in the final examination.

Before we discuss the Class 12 Lab Manual, let us check the CBSE Class 12 Summary; Below, we have mentioned the complete CBSE Class 12 Summary. The student is advised to check out to complete the summary.


	12th
	Chemistry
	CBSE
	Lab Manual

Class 12 Chemistry Lab Manual

Below we have mentioned the CBSE Chemistry Lab Manual for Class 12. Students have checked the complete Class 12 Chemistry Lab Manual in pdf for a great score in the final examination.

Example of Lab Manual

NOTE : The links given below for downloading Class 12 Chemistry Lab Manual in pdf format


Unit 1	Colloids
Unit 2	Chemical Kinetics
Unit 3	Thermochemistry
Unit 4	Electrochemistry
Unit 5	Chromatography
Unit 6	Titrimetric Analysis (Redox Reactions)
Unit 7	Systematic Qualitative Analysis
Unit 8	Tests for Functional Groups in Organic Compounds
Unit 9	Preparation of Inorganic Compounds
Unit 10	Preparation of Organic Compounds

Class 12 Chemistry Lab Manual Projects


1

Class 12 Chemistry Syllabus

Check out the latest CBSE NCERT Class 12 Chemistry Syllabus. The syllabus is for the academic year 2024-25 sessions. First of all, check the CBSE Class 12 Chemistry Exam Pattern. Students should review the complete syllabus and exam pattern with the marking scheme.

Class 12 Chemistry Exam Pattern

In this section, we have mentioned the Class 12 Chemistry Exam Pattern. Students can check the Class 12 Chemistry Exam Pattern for the academic year 2024-25.


Unit I	Solid State	10	23
Unit II	Solutions	10	“
Unit III	Electrochemistry	12	“
Unit IV	Chemical Kinetics	10	“
Unit V	Surface Chemistry	08	“
Unit VI	General Principles and Processes of Isolation of Elements	08	19
Unit VII	p -Block Elements	12	“
Unit VIII	d -and f -Block Elements	12	“
Unit IX	Coordination Compounds	12	“
Unit X	Haloalkanes and Haloarenes	10	28
Unit XI	Alcohols, Phenols and Ethers	10	“
Unit XII	Aldehydes, Ketones and Carboxylic Acids	10	“
Unit XIII	Amines	10	“
Unit XIV	Biomolecules	12	“
Unit XV	Polymers	08	“
Unit XVI	Chemistry in Everyday Life	06	“
			70

NOTE:- To know more information about the Class 12 Chemistry Syllabus

Class 12 Chemistry Useful Resources

We have tried to bring CBSE Class 12 Chemistry NCERT Study Materials like Syllabus, Worksheet, Sample Paper, NCERT Solution, Important Books, Holiday Homework, Previous Year Question Paper, etc. You can visit all these important topics by clicking the links given.



ChemistryNCERT Solution

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NCERT Laboratory Manual for CBSE Class 12 Chemistry: Practicals & Projects

Ncert laboratory manual for cbse class 12 chemistry subject is available here for download in pdf format. here you will also get links to some other important articles for cbse 12th chemistry board exam preparation..

NCERT Chemistry lab manual for class 12 is available here for download in pdf format for free. It is published by NCERT (National Council of Educational Research and Training) itself. It contains complete details about practical and projects.

Download CBSE Class 12 Chemistry Syllabus 2020-21

As per the latest pattern, there will be a theory paper of 70 marks and a practical exam of 30 marks, at the end of the academic session. For complete detailed about weightage of topics and list of experiments, you can refer latest CBSE Class 12 Chemistry Syllabus 2020-21.

Links to download NCERT Laboratory Manual for CBSE Class 12 Chemistry: Practicals & Projects

- NCERT Laboratory Manual for CBSE Class 12: Unit-1 Introduction

- NCERT Laboratory Manual for CBSE Class 12: Unit-2 Basic Laboratory Techniques

- NCERT Laboratory Manual for CBSE Class 12: Unit-3 Purification and Criteria of Purity

- NCERT Laboratory Manual for CBSE Class 12: Unit-4 Chemical Equilibrium (Ionic Equilibrium in Solution)

- NCERT Laboratory Manual for CBSE Class 12: Unit-5 pH and pH Changes in Aqueous Solutions

- NCERT Laboratory Manual for CBSE Class 12: Unit-6 Titrimetric Analysis

- NCERT Laboratory Manual for CBSE Class 12: Unit-7 Systematic Qualitative Analysis

- NCERT Laboratory Manual for CBSE Class 12: Details of Projects

Other Important Articles for CBSE Class 12 Chemistry Exam Preparation:

NCERT Exemplar for Class 12 Chemistry: Download Now

NCERT Textbooks for Class 12 Chemistry: Download Now

Chapter-wise Notes for Class 12 Chemistry: Download Now

CBSE 12th Chemistry Board Exam 2020: Paper Analysis, Review, Feedback - Watch Video & Check Updates - Check Here

CBSE Syllabus 2020-21 for All Subjects of Class 12: Download PDF

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Last Modified 15-01-2024

Embibe Lab Experiments: Learn Simulations and Experiments

Embibe Lab Experiments: Embibe is an ed-tech platform providing students various educational resources and tools. One of these tools is the Embibe Lab Experiments. It is a simulated laboratory environment to help students learn and practice various scientific experiments. The Embibe Lab Experiments cover a wide array of experiments for concepts based on physics, chemistry, and biology, mapped to CBSE and NCERT topics and lab manuals.

The experiments are interactive and enable students to perform them virtually. Students can select and mix the chemicals, measure temperature, and observe chemical reaction changes in the comfort of their homes. The virtual lab also provides feedback to students on their performance and allows them to repeat experiments to improve their understanding. Overall, the Embibe Lab Experiments is a useful tool for students who may need access to physical laboratory equipment or who want to practice experiments in a safe and controlled environment.

Perform Virtual Lab Experiments on Embibe

While studying Science, memorising the theory is not enough. Students need to ensure that they are aware how the theory is proven. For this purpose, students can take to performing experiments. However, students always do not get an opportunity to experience a real-life like setting for performing the experiments, and more often than not, these experiments cannot be performed under certain conditions. In such cases, students turn to a digital setup for performing EMBIBE lab experiments .

Students can perform the virtual experiments with complete ease on Embibe. The AI-powered technology enables students of all classes to conduct experiments. With real-life-like examples, students get to understand why a particular theory comes into existence. Furthermore, it also enables the students to understand the concepts in a better way. All the experiments are explained to the students visually on Embibe.

Embibe Lab Experiments Modules

Embibe Lab Experiments is a useful tool for students to learn and practice laboratory experiments in a convenient, safe, and interactive environment. It contains three modules that act as the learning, practice and test features. The introduction module introduces students to what the experiment is about. The practice experiment module allows them to conduct it in a step-wise manner. The Evaluation module tests students’ understanding of the concept. Thus, students get 360-degree coverage of a topic. All three Embibe Lab Experiment modules are detailed below:

Introduction Videos: From the Introduction module, students can select the aim and apparatus for the experiment. Here, students get acquainted with the experimental setup. On starting the video, students can choose the objects and tools and choose the measurements. The ‘Theory’ part covers the concept associated with the experiment. It lists each experiment’s Aim, Apparatus, Theory, Procedure, and Precautions. Thus, students know exactly what, how and when to do it.
Practice Experiments: An interesting app feature, the Practice Experiments module, allows students to select the materials required to perform the sample experiment. Embibe also helps students pick the correct apparatus before they start the experiment. On clicking any apparatus, the information is displayed on the screen. Afterwards, students are guided with step-wise instructions to perform the experiment. They can also see the number of steps involved in completing the experiment. They can watch any experiment until they gain confidence in the concept.
Evaluation: The Evaluation module is a test based on the experiment. It includes a set of questions. Each question has 4 four options from which students must choose the correct one. On clicking the correct answer, students get a solution with an explanation. They can re-practice evaluation for the same questions.

Types of Embibe Lab Experiments: Overview

Embibe offers a range of interactive experiments covering topics such as physics, chemistry, and biology. These interactive experiments allow students to manipulate variables, measure and record data, and observe changes in reactions. The virtual lab also provides real-time feedback to students on their performance during the experiments. The Embibe virtual lab is a valuable resource for students to improve their understanding and skills in laboratory experiments.

Here are some examples of the experiments available on the Embibe platform:

Electrolysis of Water: This experiment allows students to explore the process of electrolysis by using a battery and electrodes to break water molecules into hydrogen and oxygen gases.
Acid-Base Titration: This experiment involves using a pH meter and various indicators to determine the concentration of an acid or base in a solution.
Photosynthesis: This experiment allows students to learn about the process of photosynthesis by observing changes in the color of leaves when exposed to different light sources.
Pendulum Motion: This experiment involves studying the motion of a pendulum by measuring the period and frequency of its oscillations.
DNA Extraction: This experiment involves extracting DNA from a sample of plant or animal tissue using household chemicals.

Embibe Lab Experiments for CBSE Class 12 Physics

There are 54 virtual experiments for CBSE Class 12 Physics in the Embibe Lab. Physics is fundamentally a practical subject. Thus, students must be well-versed in how the concepts can be executed through demonstration. Before starting an experiment, students can watch related Embibe Explainer videos to understand the concept. We have provided links to some Physics experiment topics for students’ ready reference in the table below:

Sr. No.	Topic	Embibe Lab Experiment Link
1	Convert Given Galvanometer Into a Voltmeter
2	Tracing the Path of a Light Ray through Glass Slab
3	Characteristic Curve of a Zener Diode
4	Image of an Object Beyond C by a Concave Mirror
5	Variation in Potential Drop With Length of a Wire
6	Image of Object Between C and F of Concave Mirror
7	Comparing EMF of Two Given Primary Cells
8	Image of an Object Beyond 2F by a Convex Lens
9	Focal Length of a Convex Lens by Plotting Graphs
10	Internal Resistance of a Cell Using Potentiometer

Click Here for more Embibe Lab Experiments for CBSE Class 12 Physics

Embibe Lab Experiments for CBSE Class 12 Chemistry

Embibe Lab Experiment has 67 virtual experiments for CBSE Class 12 Chemistry. It has demonstrations for organic, inorganic and physical chemistry topics. From the table below, students can access several experiments. Click on the link given after the table for all 67 CBSE Class 12 Chemistry experiments .

Sr. No.	Topic	Embibe Lab Experiment Link
1	Identify the Alcohol Group in Organic Compounds
2	Chromatography: Separation of Cations
3	Amino Group in Organic Compounds
4	Electrolysis of Water
5	Iodoform Test for Alcohol
6	Effect of Temparature on the Rate of a Reaction
7	Paper Chromatography and Calculation of R, Value
8	Detection of Aromatic Amino Group
9	Schiff’s Test and Benedict’s Test
10	Tests for the Phenolic Group

Click Here for more Embibe Lab Experiments for CBSE Class 12 Chemistry

Embibe Lab Experiments for CBSE Class 12 Biology

Embibe Lab Experiments has 32 experiments for CBSE Class 12 Biology. Biology is mainly theoretical, but several topics require practical understanding and knowledge. Students can also build a strong foundation in the concepts by watching topics demonstrations.

Sr. No.	Topic	Embibe Lab Experiment Link
1	Nucleic Acid Staining
2	Importance of Pedigree Analysis
3	Activity on Controlled Pollination
4	Test the pH of Different Solid Samples
5	Embryonic Development in Mammals: Blastula
6	Stages of Female Gametophyte Development
7	Texture of Soil Samples
8	Ecological Adaptation is Hydric Plants
9	Androecium of Flowering Plants
10	Law of Independent Assortment

Click Here for more Embibe Lab Experiments for CBSE Class 12 Biology

Embibe Lab Experiments for CBSE Class 11 Physics

There are 35 virtual experiments for CBSE Class 11 Physics in the Embibe Lab.

Sr. No.	Topic	Embibe Lab Experiment Link
1	Units and Measurements
2	Systems of Particles and Rotational Motion
3	Kinetic Theory
4	Waves
5	Work, Energy and Power
6	Mechanical Properties of Solids
7	Laws of Motion
8	Thermal Properties of Matter
9	Oscillations
10	Motion in a Plane

Click Here for Embibe Lab Experiments for CBSE Class 11 Physics

Embibe Lab Experiments for CBSE Class 11 Chemistry

There are 44 virtual experiments for CBSE Class 11 Chemistry in the Embibe Lab.

Sr. No.	Topic	Embibe Lab Experiment Link
1	Cutting a Glass Tube and a Glass Rod
2	Measuring the Volume of Liquids in the Lab
3	Crystallisation: Purification of an Impure Sample
4	Shift in Equilibrium: Fe3+ and SCN–
5	Variation in pH With Dilution
6	Acid-Base Titration: Strength of Hydrochloric Acid
7	Charcoal Cavity Test
8	Preparation of Lassaigne’s Extract
9	Detecting Halogens in Organic Compounds
10	Detection of Sulphur and Nitrogen

Click Here for Embibe Lab Experiments for CBSE Class 11 Chemistry

Embibe Lab Experiments for CBSE Class 11 Biology

There are 59 virtual experiments for CBSE Class 11 Biology in the Embibe Lab.

Sr. No.	Topic	Embibe Lab Experiment Link
1	Cell : The Unit of Life
2	Biological Classification
3	Plant Kingdom
4	Animal Kingdom
5	Anatomy of Flowering Plants
6	Structural Organisation in Animals
7	Cell Cycle and Cell Division
8	Morphology of Flowering Plants
9	The Living World
10	Transport in Plants

Click Here for Embibe Lab Experiments for CBSE Class 11 Biology

Embibe Lab Experiments for CBSE Class 10 Science

Embibe Lab has 85 virtual experiments for CBSE Class 10 Science. Students can either look for a topic from the search bar or scroll through the options on the screen. On selecting a topic, students get a brief overview of the concept. We have provided links to a few CBSE Class 10 Science experiments in the table below:

Sr. No.	Topic	Embibe Lab Experiment Link
1	Complete Combustion of Alcohol
2	Tracing the Path of a Light Ray Through Glass Slab
3	Study of Redox Reactions
4	Image of an Object Beyond C by a Concave Mirror
5	How Can We Prepare Soap in the Lab?
6	Carbon Dioxide is Essential for Photosynthesis
7	Force and Motion of a Current-carrying Conductor
8	Process of Aerobic Respiration
9	Fehling’s and Tollens’ Tests
10	How Do Metals React With Dilute Acids?

Click Here for Embibe Lab Experiments for CBSE Class 10 Science

Embibe Lab Experiments for CBSE Class 9 Science

Embibe Lab has 47 virtual experiments for CBSE Class 9 Science.

Sr. No.	Topic	Embibe Lab Experiment Link
1	The Fundamental Unit of Life
2	Gravitation
3	Matter in our Surroundings
4	Is Matter around Us Pure?
5	Atoms and Molecules
6	The Fundamental Unit of Life
7	Tissues
8	Improvement in Food Resources
9	Diversity in Living Organisms
10	Motion

Click Here for Embibe Lab Experiments for CBSE Class 9 Science.

Steps to Access Embibe Lab Experiments

For students who wish to improve their understanding and skills in laboratory experiments, trying the Embibe Lab Experiments is the best way to go about it.

Step 1: Download the Embibe Lab Experiments app for IOS and for Android .
Step 2: Sign up for an account. Once students create an account, they can access the virtual lab and start performing interactive experiments.
Step 3: Select the board from the ‘Select your goal’ option and click ‘Next’.
Step 4: Select the class from the ‘Select your exam’ option and click ‘Next’.
Step 5: Choose the Subject and experiment students want to conduct from the list of options.
Step 6: Click on ‘Start Experiment’.
Step 7: Select a module to continue.

Benefits of Embibe Lab Experiments: Easy and Efficient

The Embibe Lab Experiments app has several features to benefit students’ learning and practice of laboratory experiments. Most experiments are done at schools under the supervision of teachers with the required safeguards. Thus, if students have not understood the concept or missed a practical, they can watch, perform and learn it in the Embibe lab. This independence in learning allows students to carve their own study journey and prepare according to their personal requirements and study plan.

Here are some key features of Embibe lab experiments:

Simulated Laboratory Environment: The Embibe Virtual Lab provides a simulated laboratory environment that allows students to perform experiments without needing external guidance, safety precautions, and physical laboratory equipment.
Interactive Experiments: The virtual lab offers over 500 interactive experiments for concepts based on biology, physics, and chemistry. The Class 10 and 12 board students can strengthen their conceptual base in the topics and ace practical and theory exams. Students can modify the variables, measure and record the data, and observe reaction changes.
Learn Perquisites on Each Topic: Students can watch the topics required for each experiment to obtain conceptual understanding. They can watch Embibe Explainer videos, DIY on the topic, Fun on the Topic, Related Topics. What better way to ace each concept?
Real-time Feedback: The virtual lab provides real-time feedback to students on their performance during experiments. All the steps a student takes are recorded, and a performance report is generated. This feedback helps students and teachers to identify mistakes and rectify them. The reports also assist teachers in understanding a student’s shortcomings and take measures to overcome them.
Real-time Feedback: The virtual lab provides real-time feedback to students on their performance during experiments. All the steps taken by a student are recorded and a performance report is generated. This feedback helps students and teachers to identify mistakes and rectify them. The reports also assist teachers in understanding a student’s shortcomings and take measures to overcome them.
Repeat Experiments: Students can repeat the experiments multiple times. It helps them to improve their understanding and master the concepts. Students can align the practical topics with the theory part and prepare for both the exams simultaneously. Thus, if they understand a concept by way of Embibe lab experiment, they can produce succinct information in their theoretical answers as well.
Safe and Controlled Conditions: The Embibe lab is a safe and controlled environment for students to perform the virtual experiments without being in a hazardous situation, risk of injury or damage to equipment. Thus, students can take more risks and do trials to satisfy their curiosity and find answers to ‘what if’ questions.
Accessible Anywhere, Anytime: The Embibe Virtual Lab can be accessed anytime, anywhere as long as the student has a good internet connection and a smartphone.

FAQs on Embibe Lab Experiments

Below we have provided some of the most frequently asked questions on Embibe Lab Experiments:

Ans : Embibe Lab Experiments is a platform to to perform Science experiments in a virtual setting. Students get to learn about these experiments via videos.

Ans : Yes, students can perform virtual lab experiments online with Embibe. They need to create an account on the app to undertake these experiments.

Ans : The Embibe lab experiments for different subjects will help students get a more in-depth idea about the topic.

Ans : Students can perform the virtual lab experiments on Embibe for Physics, Chemistry, and Biology.

Ans : The virtual labs create simulations for performing experiments. Students can choose the topic from the given options to perform experiment.

The Embibe virtual lab is a valuable resource that offers a range of features, including a simulated laboratory environment, real-time feedback, and a safe and controlled environment for practice. It is also accessible at students’ convenience, making it easy for students who may not have access to actual laboratory equipment. So, if they want to enhance their learning and skills in laboratory experiments, download and try the Embibe Virtual Lab today!

We hope that the article above on embibe lab experiments has helped you. If you want to learn more about simulations and experiments, subscribe to Download the Embibe Lab Experiments app for IOS and for Android . .

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Laboratory Manuals

Class I to VIII
Class I to V
Class VI to VIII

Mathematics

Activities for I to V(1 - 16)
Activities for I to V(17 - 27) and Projects
Activities for VI to VIII(1 - 27)
Activities for VI to VIII(28 - 51)
Activities for VI to VIII(52 - 74)
Activities for VI to VIII(75 - 93) and Projects
कक्षा (I-V) के लिए क्रियाकलाप(1 - 16)
कक्षा (I-V) के लिए क्रियाकलाप (17 - 27) और परियोजना
कक्षा (VI-VIII) के लिए क्रियाकलाप(1 - 27)
कक्षा (VI-VIII) के लिए क्रियाकलाप(28 - 51)
कक्षा (VI-VIII) के लिए क्रियाकलाप(52 - 74)
कक्षा (VI-VIII) के लिए क्रियाकलाप(75 - 93) और परियोजना
About this Manual
Theme 1- Food
Theme 2- Materials
Theme 3- The world of the living
Theme 4- Moving things, people and ideas
Theme 5- How things work
Theme 6- Natural phenomena
Theme 7- Natural Resources
Project Work
Exemplar projects
Exemplar Educational games
Activities for Class IX (1 to 10)
Activities for Class IX (11 to 20)
Activities for Class IX (21 to 34)
कक्षा 9 के लिए क्रियाकलाप (1 to 10)
कक्षा 9 के लिए क्रियाकलाप (11 to 20)
कक्षा 9 के लिए क्रियाकलाप (21 to 34)
Introduction
The World of Living
Moving things, People and ideas
पदार्थ - प्रयोग पर आधारित विडियो कार्यक्रम

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प्रयोग -2
प्रयोग -3
प्रयोग -4
प्रयोग -5
प्रयोग -6
प्रयोग -7
प्रयोग -8
प्रयोग -9
प्रयोग -10
प्रयोग -11
प्रयोग -12
प्रयोग -13
प्रयोग -14
प्रयोग -15
प्रयोग -16
प्रयोग -17
प्रयोग

गतिमान वस्तुएं, व्यक्ति एवं विचार
गतिमान वस्तुएं व्यक्ति एवं विचार - प्रयोग पर आधारित विडियो कार्यक्रम

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प्रयोग -1
प्रयोग -2
प्रयोग -3

प्रयोग -5
प्रयोग -6
प्रयोग -7

Activities for Class X (1 to 10)
Activities for Class X (11 to 20)
Activities for Class X (21 to 32)
कक्षा 10 के लिए क्रियाकलाप (1 to 10)
कक्षा 10 के लिए क्रियाकलाप (11 to 20)
कक्षा 10 के लिए क्रियाकलाप (21 to 32)
The Natural Phenomenon
How Things Work


प्रयोग -1
प्रयोग -2
प्रयोग -3
प्रयोग -4
प्रयोग -5
प्रयोग -6
प्रयोग -7
प्रयोग -8
प्रयोग -9
प्रयोग -10
प्रयोग -11
प्रयोग -12
प्रयोग -13
प्रयोग -14
प्रयोग -15
प्रयोग -16
प्रयोग -17
प्रयोग -18
प्रयोग -19
प्रयोग -20
प्रयोग -21
प्रयोग -22
प्रयोग

प्राकृतिक परिघटनाएंं विचार
वस्तुएं कैसे कार्य करती है?
प्रोजेक्ट कार्य
Activities (1 to 10)
Activities (11 to 20)
Activities (21 to 33)
क्रियाकलाप (1 - 10)
क्रियाकलाप (11 - 20)
क्रियाकलाप (21 - 33)
Major Skills in Physics Practical work
Experiments (1 to 5)
Experiments (6 & 7)
Experiment 8
Experiments 10
Experiments (11 to 13)
Experiments (14 to 17)
Activities (1 to 5)
Activities (6 to 13)
Projects (1 to 8)
Projects 10 & 11
Natural sines/cosines/tangents
Demonstrations
भौतिकी के प्रायोगिक कार्य कि प्रमुख कुशलताएँ
प्रयोग (1 - 5)
प्रयोग (6 & 7)
प्रयोग (8 & 9)
प्रयोग (10)
प्रयोग (11 - 13)
प्रयोग (14)
प्रयोग (15 - 17)
क्रियाकलाप (1 - 5)
क्रियाकलाप (6 - 13)
परियोजना (1 - 8)
परियोजना (9)
परियोजना (10 & 11)
Unit-1 Introduction
Unit-2 Basic Laboratory Techniques
Unit-3 Purification and Criteria of Purity
Unit-4 Chemical Equilibrium (Ionic Equilibrium in Solution)
Unit-5 pH and pH Changes in Aqueous Solutions
Unit-6 Titrimetric Analysis
Unit-7 Systematic Qualitative Analysis
प्रारंभिक परिचय
प्रयोगशाला कि मूलभूत तकनीक
शुद्धिकरण एवं शुद्धता की कसौटी
रसायनिक साम्य
pH और जलीय में pH परिवर्तन
अनुमापंमितीय विश्लेषण
क्रमबद्ध गुणात्मक विश्लेषण
Exercise 7 & 8
Exercise 9 & 10
Exercise 11 & 12
Exercise 13
Exercise 14
Exercise 15 to 20
Exercise 21 to 24
Exercise 25 to 27
Exercise 28 to 30
Exercise 31 to 34
Activities(1 - 10)
Activities(11 - 20)
Activities(21 - 27)
क्रियाकलाप (21 - 27)
Unit 1(Colloids)
Unit 2(Chemical Kinetics)
Unit 3(Thermochemical Measurement)
Unit 4(Electrochemistry)
Unit 5(Chromatography)
Unit 6(Titrimetric Analysis (Redox Reaction))
Unit 7(Systematic Qualitative Analysis)
Unit 8(Tests for Functional Groups in Organic Compounds)
Unit 9(Preparation of Inorganic Compounds)
Unit 10(Preparation of organic Compounds)
Unit 11(Tests for Carbohydrates, Fats and Proteins)
एकक 1(कोलाइड)
एकक 2(रसायनिक बलगातिकी)
एकक 3(ऊष्मा रसायनिक मापन)
एकक 4(वैद्युत रसायन)
एकक 5(क्रोमैटोग्रैफी (वर्णलेखिकी))
एकक 6(अनुमापनमितीय विश्लेषण (रेडाक्स अभिक्रियाएं)
एकक 7(क्रमबद्ध गुणात्मक विश्लेषण)
एकक 8(कार्बनिक यौगिक में प्रकार्यात्मक समूहों का परिक्षण)
एकक 9(आकार्बनिक यौगिक का विरचन)
एकक 10(कार्बनिक यौगिक का विरचन)
एकक 11(कार्बोहाइड्रेट, प्रोटीन और वसा का परिक्षण )
Exercise 2 & 3
Exercise 4 & 5
Exercise 8 & 9
Exercise 10
Exercise 11
Exercise 12 & 13
Exercise 15
Exercise 16 to 20
Exercise 21
Exercise 22 to 24
Exercise 25
Investigatory Project Work
Introduction to Major skills in Physics practical work
Experiment 1 & 2
Experiment 3
Experiment 4
Experiment 5
Experiment 6 & 7
Experiment 8 & 9
Experiment 10
Experiment 11 to 13
Experiment 14 to 18
Activities 1 to 6
Activities 7 to 11
Activities 12 to 14
Project 1 to 7
Demonstration 1 to 14
Data section
प्रयोग (1 & 2)
प्रयोग (14 - 18)
क्रियाकलाप (1 - 6)
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CBSE Class 12 Chemistry Investigatory Project Topics

Author : Akash Kumar Singh

August 6, 2024

Summary: Discover the amazing world of CBSE Class 12 Chemistry Investigatory Projects! Dive into exciting chemical experiments, insightful analysis, and unexpected discoveries. Explore a variety of fascinating topics that ignite your scientific curiosity.

Chemistry is one of the most fascinating science subjects. Chemistry is engaged in practically every aspect of our daily lives. It's always fascinating to discover how chemical reactions affect our lives.

A chemical investigational project is a scientific investigation aimed at investigating a specific topic or question. It usually entails performing research in the discipline of chemistry as part of a scientific fair or an individual study.

Examining the qualities of a novel material, analysing the chemical composition of a specific item, or evaluating the efficiency of a newly established technique for synthesising a chemical molecule are all examples of CBSE class 12 chemistry investigatory projects.

Designing and executing experiments, systematically analysing the collected results, and finally presenting the findings through a detailed report or a well-structured presentation are all part of the process of completing a CBSE class 12 chemistry investigatory project.

We give an extensive list of popular CBSE class 12 chemistry investigatory project topics that students might explore in their studies in the sections that follow.

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CBSE Class 12 Chemistry Investigatory Project Topics: Overview

Before we get into the CBSE Class 12 chemistry investigative project topics, let's have a look at the CBSE Class 12 exams in general.


Commonly Known As	CBSE Class 12 Board Exams
Conducting Body	Central Board of Secondary Education (CBSE)
Level of Examination	National level mode
Mode of Registration	Offline via the school for regular students Online for private students registration
Registration Fees	INR 1500/- for five subjects and INR 300/- per additional subject
Mode of Exam	Offline
Class 12 Language Subjects	English, Hindi, Telugu, Kannada, Sanskrit, Tamil, Malayalam, Urdu, Bengali, Marathi, Gujarati, Punjabi, etc.
Class 12 Academic Subjects	Mathematics, Biology, Physics, Chemistry, Computer Studies, Social Studies, Economics, Accountancy, Political Science, etc.
Frequency of Exam	Once a year

Read more: CBSE Class 12 Chemistry Syllabus

10 Most Popular CBSE Class 12 Chemistry Investigatory Project Topics

Because you have less time to study for your board examinations, it is best to prepare your chemistry project so that it is easy to explain. The most common chemistry project for class 12 is described here.

Adsorption

A process that leads to the transfer of a substance from fluid bulk to a solid surface, because of the forces of chemical bonds is called Adsorption. In this, the gaseous or liquid particles bind to a solid surface called adsorbate and form a molecular or atomic adsorbate film. Adsorption is usually a reversible process and in most cases, it is described at equilibrium which quantifies the amount which is equal to the amount of substance attached to the surface given and the concentration in the fluid. This is a popular concept among students for the chemistry project for class 12.

Synthesis of Aspirin

One of the choicest Chemistry projects for class 12 students is the making of Aspirin which is a common name for a compound named acetylsalicylic acid, majorly used as a pain killer in our day-to-day use. It is derived from salicylic acid, which is a natural product originating from the bark extracts of the willow family of plants, and was earlier used as a home remedy for curing headaches and fever. As the salicylic acid is bitter and irritating for the stomach, it is administered in the form of aspirin which proves to be less irritating.

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Chemistry investigatory projects for class 12, topics and samples.

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Safalta Expert Published by: Noor Fatima Updated Fri, 14 Jun 2024 01:11 PM IST

Here is important and relevant information regarding Chemistry Investigatory Projects for Class 12. Read the article to know about these projects and around 100 ideas for Chemistry Investigatory Projects for Class 12.

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Popular Chemistry Investigatory Projects for Class 12

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Synthesis of Aspirin

Adsorption

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Sterilization of water using bleaching powder

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Quality of Presence of Casein in Different Samples of Milk

Paper chromatography .

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Effect of potassium bisulfate as a food preservative

Surface chemistry colloidal solutions.

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Top 50 Chemistry investigatory projects for class 12

Common food adulterants in fat, butter, oil, turmeric powder, pepper, chili powder, sugar, etc.
Measuring solubility of saturated solutions
Measure the amount of acetic acid in vinegar
Determination of contents in cold drinks
Removal of alcohol from the body through Esterification
Study of diffusion of solids in liquids
Analysis of fertilizer
Chemistry in black and white photography
Presence of oxalate ions in guava fruit and different stages of ripening
Compare the rate of evaporation of water
Check the ions present in toothpaste
Preparation of Toilet Soaps
Study of Constituents of an Alloy
Study of Diffusion of Solids in Liquids
To Analyze a Sample of Brass Qualitatively
To Prepare a Smoke Bomb
Acidity In Tea
Aldol Condensation
Analysis Of Honey
Water concentration and texture
Study the effects of metal coupling on the rate of corrosion
Effects of voltage and concentration
Variation of conductance with temperature in electrolytes
Measurement of the diffusion coefficient in liquids
Preparation of soya bean milk
Determining caffeine in tea samples
Catalytic decomposition
Presence of pesticides and insecticides in fruits and vegetables
Properties of alpha, beta, and gamma rays
Digestion of starch by salivary amylase
Invisible Ink: Modeling A Molecular Switch
Green Chemistry: Bio-Diesel and Bio-Petrol
Rate of Evaporation of Different Liquids
Red Cabbage pH paper
Effect of heat on vitamin C in tomatoes
Removal of natural pigments by the interaction of oxygen and UV lights
Uses of exothermic reactions
Production of Hydrogen
Reversible sunglasses
Biodiesel formation
Determining the amount of phosphate in detergents
Preparation of Potash Alum
DNAs Secret Code
To Determine the Ignition Property of Potassium Nitrate
Setting Of Mixture of Cement with Sand, Time, and Fly Ash
Formation Of Biodiesel
Electrochemical Cell
The Neutralizing Ability of Antacid Tablets

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Can we use a whitener on the Project file?

What are the passing marks for class 12 chemistry, what is some important chemistry in with investigatory projects for class 12, is it significant to get passing marks for the class 12 chemistry practical.

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अपनी वेबसाइट पर हम डाटा संग्रह टूल्स, जैसे की कुकीज के माध्यम से आपकी जानकारी एकत्र करते हैं ताकि आपको बेहतर अनुभव प्रदान कर सकें, वेबसाइट के ट्रैफिक का विश्लेषण कर सकें, कॉन्टेंट व्यक्तिगत तरीके से पेश कर सकें और हमारे पार्टनर्स, जैसे की Google, और सोशल मीडिया साइट्स, जैसे की Facebook, के साथ लक्षित विज्ञापन पेश करने के लिए उपयोग कर सकें। साथ ही, अगर आप साइन-अप करते हैं, तो हम आपका ईमेल पता, फोन नंबर और अन्य विवरण पूरी तरह सुरक्षित तरीके से स्टोर करते हैं। आप कुकीज नीति पृष्ठ से अपनी कुकीज हटा सकते है और रजिस्टर्ड यूजर अपने प्रोफाइल पेज से अपना व्यक्तिगत डाटा हटा या एक्सपोर्ट कर सकते हैं। हमारी Cookies Policy , Privacy Policy और Terms & Conditions के बारे में पढ़ें और अपनी सहमति देने के लिए Agree पर क्लिक करें।

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Practical Chemistry with Experiments

Chemistry is the science of experiments. Scientific concepts can be easily understood by performing experiments. Laboratory experiments are being influenced by modern technique and electronic devices and there is adequate blending of information and communication technology and practical laboratory experiments.

A chemistry laboratory is a place where experiments in chemistry are performed. A student needs to understand the proper way of working in a chemistry laboratory. A student must know the proper use of each equipment and the precautions to be observed while working in the laboratory.

Students can access the chemistry chapter-wise experiments on this page from the links provided below.

Class 12 Chemistry Practicals

Class 11 chemistry practicals, class 10 chemistry practicals, class 9 chemistry practicals, chemistry viva questions with answers.

The fundamental ideas of each experiment have been discussed for a better understanding. The topic is presented in a clear and lucid manner under key headings and subheadings. Students will have a better comprehension of the idea by participating in the experiments since they will be able to observe the changes unfold right before their eyes.

As students learn by doing, their fundamentals will solidify. As a result of this practice, they will acquire an interest in the subject. Students will learn how to ask probing questions and how to study in a scientific manner.

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CBSE Class 12 Lab Manual Chapter Experiment No 5 Download here in pdf format. These Lab Manual may be freely downloadable and used as a reference book. Learning does not mean only gaining knowledge about facts and principles rather it is a path which is informed by scientific truths, verified experimentally. Keeping these facts in mind, CBSE Class 12 Lab Manual for Chapter Experiment No 5 have been planned, evaluated under subject Improvement Activities. Check our CBSE Class 12 Lab Manual for Chapter Experiment No 5. We are grateful to the teachers for their constant support provided in the preparation of this CBSE Class 12 Lab Manual.

CBSE Class 12 Lab Manual for Chapter Experiment No 5

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Coordination Compounds Class 12 Notes CBSE Chemistry Chapter 5 (Free PDF Download)

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CBSE class 12 chemistry notes for class 12 chapter 5 coordination compounds in PDF are available in Vedantu mobile app and web version for free download. The best platform for CBSE students now provides the latest coordination compounds revision notes for the quick and smooth preparation of board exams of CBSE and other school-based annual exams. The notes on coordination compounds for class 12 are also available to download in their respective official website as well.

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Chapter 9 - Coordination Compounds

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Coordination Compounds Class 12 Notes Chemistry - Basic Subjective Questions

Section – a (1 mark questions).

1. What is the IUPAC name of K 2 [Ni(CN) 4 ] ?

Ans. IUPAC name: potassium tetracyanonickelate (II)

2. Write down the formula of: Tetraamineaquachloridocobalt (III) chloride.

Ans. [Co(NH 3 ) 4 (H 2 O)Cl]Cl 2

3. What is linkage isomerism.

Ans. Linkage isomerism: When more than one atom in an ambidentate ligand is linked with central metal ion to form two types of complexes, then the formed isomers are called linkage isomers and the phenomenon is called linkage isomerism.

For example, a thiocyanato group could be connected to the metal atom by either the S atom or the N atom.

4. Write IUPAC name of the complex: [CoCl 2 (en) 2 ] +

Ans. Dichloridobis(ethane-1,2-diamine)cobalt(III) ion.

5. What is the Denticity of the ligand N(CH 2 CH 2 NH 2 ) 3

Ans. Denticity of the ligand N(CH 2 CH 2 NH 2 ) 3 is 4

6. Specify the oxidation numbers of the metal in [Co(H 2 O) 3 Cl 3 ]

Ans. [Co(H 2 O) 3 Cl 3 ]

x + 3(0) + 3 (–1) = 0 x – 3 = 0 x = 3

7. How many geometrical isomers are possible in the following coordination entities?

[Co(C 2 O 4 ) 3 ] 3–

Ans. In [Co(C 2 O 4 ) 3 ] 3− no geometric isomers are present because it is a bidentate ligand.

8. How many ions are produced from the complex Co(NH 3 ) 6 Cl 2 in solution?

Ans. The given complex [Co(NH 3 ) 6 ]Cl 2 ionizes to give three ions, i.e. one [Co( NH 3 ) 6 ] + and two Cl – ions.

9. The oxidation number of Cobalt in K[Co(CO) 4 ] is

Ans. K[Co( CO ) 4 ] = K + [Co( CO ) 4 ] – We know,

$\therefore$ x + 0 = – 1 [Where x is the oxidation number.] x = -1

10. Give IUPAC name of [Cr(H 2 O) 5 Cl]Cl 2 .

Ans. IUPAC name: Pentaaquachlorochromium (III) chloride

Section – B (2 Marks Questions)

11. Define ambidentate ligand with a suitable example.

Ans. Ambidentate ligand: The monodentate ligands with more than one coordinating atoms is known as ambidentate ligand. For example, the nitrate ion NO 2 – can bind to the central metal atom/ion at either the nitrogen atom or one of the oxygen atoms.

Example: - SCN thiocyanate, – NCS isothiocyanate.

12. On the basis of crystal field theory explain why Co(III) forms paramagnetic octahedral complex with weak field ligands whereas it forms diamagnetic octahedral complex with strong field ligands.

Ans. With weak field ligands; Δ O < p, the electronic configuration of Co (III) will be t 4 2g e 2 g and it has 4 unpaired electrons and is paramagnetic. With strong field ligands, Δ 0 > p, the electronic configuration will be t 6 2g e 0 g . It has no unpaired electrons hence diamagnetic.

13. Explain why [Fe(H 2 O) 6 ] 3+ has magnetic moment value of 5.92 BM whereas [Fe(CN) 6 ] 3- has a value of only 1.74 BM.

Ans. [Fe(CN) 6 ] 3- involves d 2 sp 3 hybridization with one unpaired electron (as shown by its magnetic moment 1.74 BM) and [Fe(H 2 O) 6 ] 3+ involves sp 3 d 2 hybridisation with five unpaired electrons (because magnetic moment equal to 5.92 BM).

14. Using valence bond theory, explain the following in relation to the complex given below: [Co(NH 3 ) 6 ] 3+

(i) Type of hybridization.

(ii) Inner or outer orbital complex.

(iii) Magnetic behavior.

(iv) Spin Only magnetic moment

Ans. [Co(NH3)6]3+ Co3+ = 3d6

(ii) Inner orbital complex

(iii) Diamagnetic

15. Why does a tetrahedral complex of the type [Ma 2 B 2 ] not show geometrical isomerism?

Ans. Because the relative position of ligand A and B are same with respect to each other in the tetrahedral complex [Ma 2 b 2 ], so it does not show geometrical isomerism.

16. Why do compounds having similar geometry have different magnetic moment?

Ans. The compounds having similar geometry may have different number of unpaired electrons due to the presence of weak and strong field ligands in complexes. If CFSE is high, the complex will show low value of magnetic moment. For example, the [CoF 6 ] 3+ is paramagnetic moment but [Co(NH 3 ) 6 ] 3+ is diamagnetic.

17. The complexes [Co(NH 3 ) 6 ] [Cr(CN) 6 ] and [Cr(NH 3 ) 6 ] [Co(CN) 6 ] are the examples of which type of isomerism?

Ans. Coordination isomerism occurs in compounds containing complex anionic and cationic parts and can be viewed as the interchange of one or more ligands between the cationic complex ion and the anionic complex ion. e.g.,

[Co(NH 3 ) 6 ] [Cr(CN) 6 ] is an coordination isomer of [Co(CN) 6 ] [Cr(NH 3 ) 6 ]

18. Change in composition of co-ordination sphere yields which type of isomers

Ans. Change in composition of co-ordination sphere yield ionisation isomers.

[Cr(H 2 O) 6 ]Cl 3 and [CrCl 3 (H 2 O) 3 ].3H 2 O

19. How many hydrate isomers are possible with the formula CrCl 3 .6H 2 O?

20. [Co(NH 3 ) 4 Cl 2 ]NO 2 and [Co(NH 3 ) 4 ClNO 2 ]Cl exhibit which type of isomerism?

Ans. The given compounds are the [Co(NH 3 ) 4 Cl 2 ]NO 2 and [Co(NH 3 ) 4 ClNO 2 ]Cl are the ionization isomers. Ionization isomers are identical except for a ligand has exchanged places with an anion or neutral molecule that was originally outside the coordination complex. The central ion and the other ligands are identical.

PDF Summary - Class 12 Chemistry Coordination Compounds Notes (Chapter 5)

1. introduction.

Coordination compounds are extremely important. It is important to recognize that life would not have been possible without the presence of chlorophyll (Mg - complex) in plants and haemoglobin (Fe- complex) in human blood. The study of these compounds will broaden our understanding of chemical bonding and the physical properties of coordination compounds such as magnetic properties.

2. Molecular or Addition Compounds

When a solution containing two or more simple stable compounds in molecular proportions is allowed to evaporate, it produces crystals of new substances known as molecular or addition compounds.

${\text{KCl + MgC}}{{\text{l}}_{\text{2}}}{\text{ + 6}}{{\text{H}}_{\text{2}}}{\text{O }} \to {\text{ }}\mathop {{\text{KCl}}{\text{.MgC}}{{\text{l}}_{\text{2}}}.6{{\text{H}}_{\text{2}}}{\text{O}}}\limits_{\left( {{\text{Camallite}}} \right)}$

${\text{CuS}}{{\text{O}}_{\text{4}}}{\text{ + 4N}}{{\text{H}}_{\text{3}}}{\text{ }} \to {\text{ }}\mathop {\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_3}} \right)}_4}} \right]{\text{S}}{{\text{O}}_4}}\limits_{\left( {{\text{Tetrammine copper }}\left( {{\text{II}}} \right){\text{ sulphate}}} \right)}$

2.1 Types of Molecular Compounds

2.1.1 double salt .

A double salt is a substance formed by combining two different salts that crystallize as a single substance but ionize as two distinct salts when dissolved in water. These salts lose their identity in solution, which means that when dissolved in water, they test positive for all of the ions present in the salt. eg. Mohr's salt, potash alum.

$\mathop {{\text{FeS}}{{\text{O}}_{\text{4}}}{\text{.}}{{\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}{\text{.6}}{{\text{H}}_{\text{2}}}{\text{O }}}\limits_{{\text{Mohr's salt }}} \to {\text{ F}}{{\text{e}}^{{\text{2 + }}}}_{\left( {aq} \right)}{\text{ + 6}}{{\text{H}}_{\text{2}}}{\text{O + 2N}}{{\text{H}}_{\text{4}}}{^{\text{ + }}_{\left( {aq} \right)}}{\text{ + 2S}}{{\text{O}}_{\text{4}}}{^{{\text{2--}}}_{\left( {aq} \right)}}$

2.2 Coordination Compounds

A coordination compound is a molecular compound formed by the combination of two or more simple molecular compounds that retains its identity both solid and dissolved.

$\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]{\text{S}}{{\text{O}}_{\text{4}}} \rightleftharpoons {\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]^{2 + }}{\text{ + S}}{{\text{O}}_{\text{4}}}^{2 - }$

3. Coordination Compounds

A ligand, a central atom, a complex ion, a cation, or an anion make up a coordination compound. In general, the complex ion is written in a square box, and the ion (cation or anion) is written outside the complex ion.

$\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}{\text{ }}} \right]{\text{ C}}{{\text{l}}_{\text{3}}}{\text{ }}$

$\left[ {{\text{Complex ion}}} \right]{\text{ anion}}$

General Formula: ${{\text{A}}_{\text{x}}}\left[ {{\text{M}}{{\text{L}}_{\text{n}}}} \right]{\text{/}}\left[ {{\text{M}}{{\text{L}}_{\text{n}}}} \right]{{\text{B}}_{\text{y}}}$ where M is the central metal atom/ion, L is the ligand, A is the cation and B is the anion.

Some Important Terms Pertaining to Coordination Compounds

3.1 coordination entity .

It is the fixed central metal atom or ion that is bonded to a specific number of ions or molecules. Six ammonia molecules, for example, are surrounded by three chloride ions in $\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}} \right]{\text{C}}{{\text{l}}_{\text{3}}}{\text{,}}$ a coordination entity.

3.2 Central Atom/Ion

In a specific geometrical arrangement, it is the central cation that is surrounded and coordinately bonded to one or more neutral molecules or negatively charged ions. In the complex $\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}} \right]{\text{C}}{{\text{l}}_{\text{3}}}{\text{,}}$ for example, ${\text{C}}{{\text{o}}^{{\text{3 + }}}}$ is the central metal ion that is positively charged and is coordinately bonded to six neutral NH 3 molecules within the coordination sphere. The central metal/ion is also known as Lewis acid.

3.3 Ligands

Ligands are ions or molecules that are bound to the coordination entity's central atom/ion. These can be simple ions like ${\text{C}}{{\text{l}}^{\text{--}}}{\text{,}}$ small molecules like ${{\text{H}}_{\text{2}}}{\text{O or N}}{{\text{H}}_{\text{3}}}{\text{,}}$ or larger molecules like ${{\text{H}}_{\text{2}}}{\text{NC}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{H}}_{\text{2}}}{\text{N}}{{\text{H}}_{\text{2}}}{\text{.}}$

3.4 Coordination Number (C.N)

The number of atoms in the ligands that are directly bound to the central metal atom or ion by coordinate bonds is known as the metal atoms or ion's coordination number. It is also the same as secondary valency.

${{\text{Complex }}} and {{\text{ Coordination number}}}$

${{{\text{K}}_{\text{4}}}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6 }}}} \right]} and {\text{ 6}}$

${{{\left[ {{\text{Ag}}{{\left( {{\text{CN}}} \right)}_{\text{2}}}} \right]}^ - }}{\text{2}}$

${\left[ {{\text{Pt}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{2}}}} \right]}{\text{4}}$

${{{\left[ {{\text{Ca}}\left( {{\text{EDTA}}} \right)} \right]}^{2 - }}}{\text{6}}$

3.5 Coordination Sphere

A square bracket surrounds the central metal atom or ion and the ligands that are directly attached to it. This was known as the coordination sphere or the first sphere of attraction. Because the metal ion tightly holds the ligands in the coordination sphere, it behaves as a single unit.

Coordination sphere

3.6 Coordination Polyhedron

The spatial arrangement of the ligand atoms that are directly attached to the central atom/ion is referred to as a coordination polyhedron. ${\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}} \right]^{{\text{3 + }}}}{\text{,}}$ for example, is octahedral, $\left[ {{\text{Ni}}{{\left( {{\text{CO}}} \right)}_{\text{4}}}} \right]$ is tetrahedral, and ${\left[ {{\text{PtC}}{{\text{l}}_{\text{4}}}} \right]_{\text{2}}}$ is square planar.

3.7 Oxidation Number of Central Metal Atom

It is defined as the charge that the central metal ion would have if all ligands and electron pairs were removed. It is computed as follows:

${{\text{K}}_{\text{4}}}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right] \to 4{{\text{K}}^ + } + {\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]^{4 - }}$

Charge on the complex ion is -4.

Let charge on Fe be x.

Now, the charge on cyanide ions is -1.

$\Rightarrow x + 6 \times \left( { - 1} \right) = - 4$

$\Rightarrow x = + 2 $

Hence, the oxidation number of Fe is +2 (II).

3.8 Homoleptic and Heteroleptic Complexes

Homoleptic complexes are those in which the central atom is coordinated with only one type of ligand, such as ${\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_6}} \right]^{{\text{3 + }}}}{\text{.}}$ Hetroleptic complexes are those in which the central atom is coordinated with more than one type of ligand, such as ${\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_4}{\text{C}}{{\text{l}}_2}} \right]^{\text{ + }}}{\text{.}}$

4. Nomenclature of Coordination Compounds

4.1 nomenclature .

The Following Rules are Followed When Naming a Complex Ion:

Cations are named first, followed by anions.

The central metal ion's oxidation state (O.S.) is denoted by a Roman numeral.

The ligand names are listed first, followed by the name of the central metal ion.

Anion ligand names that end in 'ide' are changed to 'o', 'ite' are changed to 'ito' and 'ate' are changed to 'ato'

The unmodified name is used for many ligands that are molecules.

Positive groups are terminated by –ium. For example: $\mathop {\text{N}}\limits^{ \cdot \cdot } {{\text{H}}_2} - {\text{N}}{{\text{H}}_3}^ + $ hydrazinium.

When there are multiple ligands of the same type, the prefixes di, tri, tetra, penta, and hexa are used to indicate the number of ligands of that type. An exception occurs when the name of the ligand contains a number, as in ethylenediamine (en). To avoid confusion, bis, tris, and tetrakis are used instead of di, tri, and tetra, and the ligand name is enclosed in brackets. as in bis (ethylenediamine)

If anion is a complex, metal is followed by 'ate'.

${\left[ {{\text{Ni}}{{\left( {{\text{CN}}} \right)}_4}} \right]^{2 - }}$: tetracyanonickelate (II) ion

Lead – plumbate

Gold – aurate

Zinc – zincate

Tin – stannate

Silver – argentate

Cobalt – cobaltate

Iron – ferrate

Aluminium – aluminate

Manganese – manganate

Copper – cuprate

Chromium – chromate

Platinum – platinate

A complex is said to be polynuclear if it contains two or more metal atoms. The prefix – $\mu $ denotes the bridging ligands that connect the two metal atoms.

Ambidentate ligands can be connected via different atoms.–

${\text{M}} \leftarrow {\text{N}}{{\text{O}}_{\text{2}}}$

${\text{M}} \leftarrow {\text{ONO}}$

When writing (not naming) the complex formula:

Complex ion should be enclosed by square brackets and

Ligands are placed alphabetically after metal, but first negative ligands, then neutral, then positive.

5. Werner’s Theory

Werner explained the nature of bonding in complexes and came to the conclusion that the metal in complexes has two different types of valency.

5.1 Primary Valency

The oxidation state of the central metal atom or ion determines the primary valency. These are asymmetrical.

Example: What are the primary valency of ${{\text{K}}_4}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]{\text{ and }}\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]{\text{S}}{{\text{O}}_{\text{4}}}$?

The primary valency of ${{\text{K}}_4}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]{\text{ and }}\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]{\text{S}}{{\text{O}}_{\text{4}}}$ is 2.

5.2 Secondary Valency

Secondary valency refers to the number of ligand atoms that are co-ordinated to the central metal atom. Because these are directional, a complex ion has a specific shape.

Example: What are the secondary valency of $\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}} \right]{\text{C}}{{\text{l}}_{\text{3}}}{\text{ and }}{{\text{K}}_{\text{4}}}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]$ ?

Sol. The secondary valency in $\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}} \right]{\text{C}}{{\text{l}}_{\text{3}}}$ is 6.

${{\text{K}}_{\text{4}}}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]$: six ligands are coordinated to Fe. As a result, the secondary valency is 6. Ions attached to complex ions satisfy the primary valency. It is represented by dotted lines. Ionisable valency is another name for primary valency. The ligands satisfy the secondary valency; they are non-ionisable and are represented by a solid line $\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}} \right]{\text{C}}{{\text{l}}_{\text{3}}}$

An anion found in the co-ordination and ionization sphere is represented by ……..

Every element is capable of satisfying both its primary and secondary valencies. When a negative ion is present in the coordination sphere, it exhibits dual behavior. It has the potential to satisfy both primary and secondary valencies.

The ligands that satisfy the secondary valencies are aimed at specific locations in space. The coordination number determines the geometry of the complex ion. If the metal has coordination number 6, the complex is octahedral, which means that six donor atoms of the ligands occupy six positions around the metal octahedrally. If, on the other hand, the coordination number is 4, the complex's geometry can be tetrahedral or square planar. This postulate predicted that different types of isomerism would exist in coordination compounds.

Three dimensional arrangement of ligand in octahedral, tetrahedral and square planar complex

Examples:

$(\mathrm{C} \cdot \mathrm{N}=6)$

${\left[\mathrm{Cr}\left(\mathrm{CH}_{3}\right)_{6}\right]^{3+}}$

${\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+} ;\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}}$

${\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{2-} ;\left[\mathrm{Fe}\left(\mathrm{F}_{6}\right)\right]^{3-}}$

${\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{6}\right]^{4+} ;\left[\mathrm{PtCl}_{6}\right]^{2-}}$

Square planar

$($ C. $N=4)$

$\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$

$\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$

$\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$

$\mathrm{X}=\mathrm{Cl}^{-}, \mathrm{Br}, \mathrm{I}^{-}$

Familiar C.N.’s of Some Common Metal Ions.

Univalent	C.N	Divalent	C.N.
$\mathrm{Ag}^{+}$	2	$\mathrm{V}^{2+}$	6
$\mathrm{Au}^{+}$	2, 4	$\mathrm{Fe}^{2+}$	6
$\mathrm{Ti}^{+}$	2	$\mathrm{Co}^{2+}$	4, 6
$\mathrm{Cu}^{+}$	2, 4	$\mathrm{Ni}^{2+}$	4, 6
		$\mathrm{Cu}^{2+}$	4, 6
		$\mathrm{Zn}^{2+}$	4
		$\mathrm{Pd}^{2+}$	4
		$\mathrm{Pt}^{2+}$	4
		$\mathrm{Ag}^{2+}$	4

Trivalent	C.N.	Tetravalent	C.N.
$\mathrm{Sc}^{3+}$	6	$\mathrm{Pt}^{4+}$	6
$\mathrm{Cr}^{3+}$	6	$\mathrm{Pd}^{4+}$	6
$\mathrm{Fe}^{3+}$	6
$\mathrm{Co}^{3+}$	6
$\mathrm{Os}^{3+}$	6
$\mathrm{Ir}^{3+}$	6
$\mathrm{Au}^{3+}$	4

6. Effective Atomic Number (Ean)

Sidgwick proposed effective atomic number (EAN), which is defined as the number of electrons gained by the metal atom or ion after gaining electrons from the donor atoms of the ligands. In some cases, the effective atomic number (EAN) coincides with the atomic number of the next inert gas. The following relationship is used to calculate EAN:

EAN = Atomic number of the metal – number of electrons lost in ion formation + number of electrons gained from the donor atoms of the ligands. (2 × CN)

The EAN Values of Various Metals in Their Complexes Are Listed Below:

Complex	Metal (Oxidation state)	Atomic Number of Metal	Coordination Number	Effective Atomic Number
${{\text{K}}_{\text{4}}}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]$	+2	26	6	$\left( {26 - 2} \right) + \left( {6 \times 2} \right) = 36$
$\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]{\text{S}}{{\text{O}}_{\text{4}}}$	+2	29	4	$\left( {29 - 2} \right) + \left( {4 \times 2} \right) = 35$
$\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{6}}}} \right]{\text{C}}{{\text{l}}_{\text{4}}}$	+3	27	6	$\left( {27 - 3} \right) + \left( {6 \times 2} \right) = 36$
${\text{Ni}}{\left( {{\text{CO}}} \right)_{\text{4}}}$	0	28	4	$\left( {28 - 0} \right) + \left( {4 \times 2} \right) = 36$
${{\text{K}}_{\text{2}}}\left[ {{\text{Ni}}{{\left( {{\text{CN}}} \right)}_{\text{4}}}} \right]$	+2	28	4	$\left( {28 - 2} \right) + \left( {4 \times 2} \right) = 34$

7. Valence Bond Theory

Valence Bond Theory (VBT) can explain the bonding in coordination compounds because the d orbitals of the majority of transition metal complexes are incomplete. Valence bond considers orbital hybridization because penultimate d-orbitals are close in energy to s and p-orbitals of the outermost shell, allowing for various types of hybridization.

The Following Assumption is Made by VBT:

The central metal ion has a number of empty orbitals that can accept electrons donated by the ligands. The coordination number of the metal ion for the specific complex is equal to the number of empty d-orbitals.

Strong bonds are formed when the metal orbitals and ligand orbitals overlap. The greater the extent of overlapping, the more stable the complex. Different orbitals (s, p, or d) hybridize to form a set of equivalent hybridized orbitals that participate in ligand bonding.

Each ligand contributes two electrons to the central metal ion/atom.

The inner orbitals contain non-bonding metal electrons that do not participate in chemical bonding.

A complex is paramagnetic if it contains unpaired electrons. The complex is diamagnetic if it does not contain an unpaired electron.

Under the influence of a strong ligand (CN, CO), electrons can be forced to pair up, thereby violating Hund's rule of multiplicity.

Common Types of hybridization

Coordination Number	Hybridization	Shape	Geometry
2	sp	Linear	X-A-X
4	sp³	Tetrahedron
4	dsp²	Square Planar
5	sp³d or dsp³	Trigonal Bipyramidal
6	d²sp³ or sp³d²	Octahedral

Note: Inner d-orbitals (3d orbital) have been used for bonding in $\mathrm{d}^{2} \mathrm{sp}^{3}$ hybridisation; such complexes are known as inner orbital complexes or low spin complexes. The outer d-orbitals (4d orbital) have been used for bonding in $\mathrm{sp}^{3} \mathrm{~d}^{2}$ hybridisation; such complexes are known as outer orbital complexes or high spin complexes. $\sqrt {n\left( {n + 2} \right)} $ where n is the number of unpaired electrons, gives the magnetic moment.

7.1 Limitations of VBT

The change in ligand and metal ion properties could not be explained.

The valence bond theory is silent on why some complexes are more labile than others.

The VBT does not explain the existence of inner and outer orbital complexes satisfactorily.

The VBT was unable to explain the color of complexes.

8. Crystal Field Theory

The valence bond theory is less widely accepted than the Crystal Field Theory. It is assumed that the attraction between a complex's central metal and its ligands is purely electrostatic. The following assumptions are made in the crystal field.

Ligands are considered point charges.

Metal orbitals and ligand orbitals have no interaction.

In the free atom, all of the d orbitals on the metal have the same energy (that is, they are degenerate). However, when a complex is formed, the ligands destroy the degeneracy of these orbitals, resulting in different energies for the orbitals.

Degeneracy of d-orbital

8.1 Octahedral Complexes

The metal is at the center of an octahedral complex, and the ligands are at the six corners. As shown, the directions x, y, and z point to three adjacent corners of the octahedron. The lobes of the ${{\text{e}}_g}{\text{ and }}{{\text{d}}_{{{\text{x}}^{\text{2}}}{\text{ - }}{{\text{y}}^{\text{2}}}}}{\text{, }}{{\text{d}}_{{{\text{z}}^2}}}$ orbitals point along the x, y, and z axes and the lobes of the t2g ${{\text{t}}_{2g}}{\text{ and }}{{\text{d}}_{{\text{xy}}}}{\text{, }}{{\text{d}}_{{\text{xz}}}}{\text{, }}{{\text{d}}_{{\text{yz}}}}$ are located between the axes. The approach of six ligands along the x, y, z, –x, –y, and –z directions increases the energy of the ${{\text{d}}_{{{\text{x}}^{\text{2}}}{\text{ - }}{{\text{y}}^{\text{2}}}}}{\text{ and }}{{\text{d}}_{{{\text{z}}^2}}}$ orbitals (which point along the axes) much more than the energy of the dxy, d xz, and d yz orbitals (which point between the axes). Thus, the d orbitals split into two groups under the influence of an octahedral ligand field.

Weak field ligands are those that cause only a minor amount of crystal field splitting. Strong field ligands are ligands that cause a large splitting. The common ligands can be arranged in ascending crystal field splitting $\Delta .$

Spectrochemical Series

$\mathrm{I}^{-}<\mathrm{Br}^{-}<\mathrm{S}^{2-}<\mathrm{Cl}^{-}<\mathrm{NO}_{3}^{-}<\mathrm{F}^{-}<\mathrm{OH}^{-}<\mathrm{EtOH}<\text { oxalate }<\mathrm{H}_{2} \mathrm{O}$

$\text { (weak field ligands) }<\mathrm{EDTA}<\left(\mathrm{NH}_{3}=\text { pyridine }\right)<\text { ethylenediamine }<\text { dipyridy }<0 \text { - phenanthroline }<\mathrm{NO}_{2}<\mathrm{CN}^{-}$

$<\mathrm{CO} \text { (strong field ligands) }$

A pattern of increasing donation is followed:

$\text { Halide donors }<\mathrm{O} \text { donors }<\mathrm{N} \text { donors }<\mathrm{C} \text { donors }$

The total crystal field stabilization energy is given by

${\text{CFS}}{{\text{E}}_{\left( {{\text{octahedral}}} \right)}} = - 0.4{n_{\left( {{t_{2g}}} \right)}} + 0.6{n_{\left( {{e_g}} \right)}}$

where ${n_{{t_{2g}}}}{\text{ and }}{n_{{e_g}}}$ are the number of electrons occupying the$t_{2g}$ and $e_g$ orbitals respectively. The CFSE is zero for ions with $d^0$ and $d^{10}$ configurations in both strong and weak ligand fields. The CFSE is also zero for $d^5$ configurations in a weak field.

Effects of Crystal Field Splitting

CFSE and electronic arrangements in octahedral complexes

Arrangement of electrons weak ligand field and strong ligand field

8.2 Tetrahedral Complexes

A cube is related to a regular tetrahedron. As shown, one atom is in the center of the cube, and four of the cube's eight corners are occupied by ligands.

Degeneracy of d-orbital in tetrahedral complex

The directions x, y, and z point to the cube's face centers. The e orbitals are oriented along the x, y, and z axes (that is to the centres of the faces). The t 2 orbitals are located between the x, y, and z axes (that is towards the centres of the edges of the cube). The ligands' approach directions do not exactly coincide with the e or t 2 orbitals.

As a result, the t 2 orbitals are closer to the ligand direction than the e orbitals. The ligands' approach raises the energy of both sets of orbitals. Because they are closest to the ligands, the energy of the t 2 orbitals is increased the most. The crystal field splitting in octahedral complexes is the inverse of that in octahedral complexes.

The t 2 orbitals are $0.4{\Delta _t}$ higher than the weighted average energy of the two groups (the Bari center), while the e orbitals are $0.6{\Delta _t}$ lower.

In tetrahedral complexes, the magnitude of the crystal field splitting t is much smaller than in octahedral fields. This is due to two factors:

Because there are only four ligands rather than six, the ligand field is only two-thirds the size; consequently, the ligand field splitting is also two-thirds the size.

The orbital direction does not coincide with the ligand direction. This reduces the crystal field splitting by about two-thirds.

Thus the tetrahedral crystal field splitting ${\Delta _t}$ is roughly 2/3 × 2/3 = 4/9 of the octahedral crystal field splitting ${\Delta _t}.$

9. Organometallic Compounds

Organometallic compounds are those that contain at least one carbon-metal bond. The Grignard reagent, RMgX, is a well-known example of an organometallic compound in which $\mathrm{R}$ is an alkyl group. Organometallic compounds include diethyl zinc $\left[\mathrm{Zn}\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2}\right]$, lead tetraethyl $\left[\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{4}\right]$, ferrocene $\left[\mathrm{Fe}\left(\mathrm{C}_{5} \mathrm{H}_{5}\right)_{2}\right]$, dibenzene chromium $\left[\mathrm{Cr}\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)_{2}\right]$, and metal carbonyls. Organometallic compounds are divided into three types:

Complexes with the sigma $\left( \sigma \right)$

Bonded complexes of Pi $\left( \pi \right)$

Complexes with both sigma and pi bonding properties.

9.1 Sigma Bonded Complexes

The metal atom and carbon atom of the ligand are joined together with a sigma bond in these complexes, i.e., the ligand contributes one electron and is thus referred to as a one electron donor.

Grignard reagent, $R-M g-X$, where $R$ is an alkyl or aryl group and $X$ is halogen.

Zinc compounds with the formula $\mathrm{R}_{2} \mathrm{Zn}$, for example, $\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{Zn}$. Frankland was the first to isolate this in 1849 . Other comparable compounds include $\left(\mathrm{CH}_{3}\right)_{4} \mathrm{Sn},\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{4} \mathrm{~Pb}$, $\mathrm{Al}_{2}\left(\mathrm{CH}_{3}\right)_{6}, \mathrm{Al}_{2}\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{6}$, and $\mathrm{Pb}\left(\mathrm{CH}_{3}\right)_{4}$

9.2 Pi Bonded Organometallic Compounds

These are the compounds of metals that are combined with alkenes, alkynes, benzene, and other ring compounds. In these complexes, the metal and ligand form a bond that involves the pi electrons of the ligand. Three common examples are Zeise’s salt, ferrocene and dibenzene chromium. These are shown here :

Pi bonded organometallic compounds

9.3 Sigma– and Pi–Bonded Organometallic Compounds

This class includes metal carbonyls, which are compounds formed by combining metal and carbon monoxide. These compounds have sigma and pi bonding. Metal atoms in these compounds have no oxidation state. Carbonyls can be monomeric, bridged, or polynuclear in nature.

Sigma– and pi–bonded carbonyl compounds

The metal–carbon bond in a metal carbonyl has both the sigma– and pi–character. When a vacant hybrid orbital of the metal atom overlaps with an orbital on the C atom of carbon monoxide containing a lone pair of electrons, a sigma bond is formed.

Sigma– overlap in carbonyl compounds

When a filled orbital of a metal atom overlaps with a vacant antibonding pi* orbital of a carbon monoxide atom, a pi–bond is formed. This overlap is also known as metal atom back donation of electrons to carbon. As an example, consider the following:

pi– overlap in carbonyl compounds

The pi–overlap is perpendicular to the sigma–bond nodal plane.

In olefinic complexes, bonding pi–orbital electrons are donated to the metal atoms' empty orbital while back bonding occurs from the metal atoms' filled orbital to the antibonding pi–orbital of the olefin.

10. Isomerism

Isomers are compounds that have the same molecular formula but a different structural formula.

10.1 Structural Isomerism

10.1.1 ionisation isomerism : .

This isomerism occurs when the coordination compounds produce different ions in solution. For example, the formula has two isomers.

$\underset{violet}{[Co(NH_3)_5Br]SO_4} \rightleftharpoons \underset{Pentaamine Bromide}{[Co(NH_3)_5Br]^{2+}} - cobalt(III)\,\, ion + {So_4}^{2-}$

This isomer produces a white precipitate of $BaSO_4$ in a solution of $BaCl_2$.

$\underset{Red}{[Co(NH_3)_5 SO_4]Br} \rightleftharpoons \underset{Pentaamine Sulphato}{[Co(NH_3)_5SO_4]^{+}} - cobalt(III)\,\, ion + {Br}^{-}$ With $\mathrm{AgNO}_{3}$ solution, the above isomer produces a light yellow precipitate.

10.1.2 Hydrate Isomerism:

When different numbers of water molecules are present inside and outside the coordination sphere, this type of isomerism occurs. This isomerism is best exemplified by the three isomers with the formula ${\text{CrC}}{{\text{l}}_{\text{3}}}{\text{.6}}{{\text{H}}_{\text{2}}}{\text{O}}{\text{.}}$

$\left[ {{\text{Cr}}{{\left( {{{\text{H}}_{\text{2}}}{\text{O}}} \right)}_{\text{6}}}} \right]{\text{C}}{{\text{l}}_{\text{3}}}{\text{ , }}\left[ {{\text{Cr}}{{\left( {{{\text{H}}_{\text{2}}}{\text{O}}} \right)}_{\text{5}}}{\text{Cl}}} \right]{\text{C}}{{\text{l}}_{\text{2}}}{\text{.}}{{\text{H}}_{\text{2}}}{\text{O, and }}\left[ {{\text{Cr}}{{\left( {{{\text{H}}_{\text{2}}}{\text{O}}} \right)}_{\text{4}}}{\text{C}}{{\text{l}}_{\text{2}}}} \right]{\text{Cl}}{\text{.2}}{{\text{H}}_{\text{2}}}{\text{O}}$ are its Hydrate Isomers.

10.1.3 Coordination Isomerism:

This type of isomerism can be found in coordination compounds that contain both cationic and anionic complex ions. To form isomers, the ligands in both the cationic and anionic ions are exchanged. Here are some examples:

$\left[ {{\text{Pt}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]\left[ {{\text{CuC}}{{\text{l}}_{\text{4}}}} \right]{\text{ and }}\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]\left[ {{\text{PtC}}{{\text{l}}_{\text{4}}}} \right]$

10.1.4 Linkage Isomerism:

This isomerism occurs in complex compounds containing ambidentate ligands such as ${\text{N}}{{\text{O}}_{\text{2}}}{\text{, C}}{{\text{N}}^{\text{ - }}}{\text{, SC}}{{\text{N}}^{\text{ - }}}{\text{, }}{{\text{S}}_{\text{2}}}{\text{O}}_3^{2 - }{\text{, and CO}}{\text{.}}$ For example, $\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{5}}}{\text{N}}{{\text{O}}_{\text{2}}}} \right]{\text{C}}{{\text{l}}_{\text{2}}}{\text{ and }}\left[ {{\text{Co}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{5}}}{\text{ONO}}} \right]{\text{C}}{{\text{l}}_{\text{2}}}$ are linkage isomers because ${\text{NO}}_{\text{2}}^{\text{ - }}$ can be linked via N or O.

10.1.5 Ligand Isomerism:

Some ligands can exist as isomers; for example, diamino propane can exist as both 1, 2-diamino propane (pn) and 1, 3-diamino propane, also known as trimethylene diamine (tn).

When these ligands (pn and tn) combine to form complexes, the complexes are isomers of each other. This ligand is found in isomeric complexes such as ${\left[ {{\text{Co}}{{\left( {{\text{pn}}} \right)}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{2}}}} \right]^{\text{ + }}}{\text{ and }}{\left[ {{\text{Co}}{{\left( {{\text{tn}}} \right)}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{2}}}} \right]^{\text{ + }}}$ ions.

10.1.6 Coordination Position Isomerism:

This type of isomerism is exhibited by polynuclear complexes by changing the position of ligands with respect to different metal atoms present in the complex. For example,

Coordination position isomerism

10.2 Stereo Isomerism

Compounds with stereo isomerism have the same number of atoms or groups in the same position, but the atoms or groups are arranged differently around the central atom.

10.2.1 Geometrical Isomerism

Complex compounds with the same ligands in the coordination sphere but different relative positions of the ligands around the central metal atom are referred to as geometrical isomers, and the phenomenon is referred to as geometrical isomerism.

10.2.1.1 Geometrical Isomerism in Square Planar Complexes

A square planar complex with two similar ligands at opposite positions (180 o a part) is called a trans-isomer, while a square planar complex with two similar ligands at adjacent positions (90 o a part) is called a cis - isomer.

Geometrical isomers (cis and trans) of $\left.\mathrm{Pt}\left[\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]$

Geometrical isomerism

Geometrical isomers (cis and trans) $o f\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} C l_{2}\right]^{+}$

Isomerism in complex

10.2.1.2 Geometrical Isomerism in Octahedral Complexes

Geometrical isomerism in complex

Mabcdef: They form 15 isomers

$M(AA)_2b_2$

$M(AA)_2bc$

$M(AA)a_2b_2$

$Ma_2b_2c_2$

Optical Isomerism in octahedral complexes

Example: Draw the optical isomers of $\left[ {{\text{Pt}}\left( {{\text{Cl}}} \right)\left( {{\text{Br}}} \right)\left( {\text{I}} \right)\left( {{\text{py}}} \right)\left( {{\text{N}}{{\text{O}}_{\text{2}}}} \right)\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)} \right]$

Optical Isomerism in octahedral complex Mabcdef

Example: Draw the optical isomers of ${\left[ {{\text{Co}}{{\left( {{\text{en}}} \right)}_{\text{3}}}} \right]^{{\text{3 + }}}}$

Optical Isomerism in octahedral complex

The two optical isomeric forms of the complex ${\left[ {{\text{Co}}{{\left( {{\text{en}}} \right)}_{\text{3}}}} \right]^{{\text{3 + }}}}$

Isomerism in octahedral complexes

cis $M(AA)_2b_2$

Example: Draw the optical isomers of $\left[ {{\text{RhC}}{{\text{l}}_{\text{2}}}{{\left( {{\text{en}}} \right)}_{\text{2}}}} \right]{{\text{ }}^{\text{ + }}}$

Cis $Ma_2b_2c_2$

Optical Isomerism in cis

cis $M(AA)b_2c_2$

Example: Draw the optical isomers of ${\left[ {{\text{CoC}}{{\text{l}}_{\text{2}}}\left( {{\text{en}}} \right){{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{2}}}} \right]^{\text{ + }}}$

cis $M(AA)_2 bc$

11. Stability Of Coordination Compounds

The degree of association between the two species involved in the state of equilibrium is referred to as the stability of a complex in solution. If we get a reaction like this:${\text{M + 4L\;}} \rightleftharpoons {\text{\;M}}{{\text{L}}_{\text{4}}}$

The greater the stability constant, the greater the proportion of ML 4 in solution. Because free metal ions are rare in solution, M is usually surrounded by solvent molecules, which compete with and eventually replace the ligand molecules, L. To keep things simple, we ignore the solvent molecules and write the four stability constants as follows:

${\text{M + L }} \rightleftharpoons {\text{ ML }}{{\text{K}}_{\text{1}}}{\text{ = }}\left[ {{\text{ML}}} \right]{\text{/}}\left[ {\text{M}} \right]\left[ {\text{L}} \right]$

${\text{ML + L }} \rightleftharpoons {\text{ M}}{{\text{L}}_{\text{2}}}{\text{ }}{{\text{K}}_{\text{2}}}{\text{ = }}\left[ {{\text{M}}{{\text{L}}_{\text{2}}}} \right]{\text{/}}\left[ {{\text{ML}}} \right]\left[ {\text{L}} \right]$

${\text{M}}{{\text{L}}_{\text{2}}}{\text{ + L }} \rightleftharpoons {\text{ M}}{{\text{L}}_{\text{3}}}{\text{ }}{{\text{K}}_{\text{3}}}{\text{ = }}\left[ {{\text{M}}{{\text{L}}_{\text{3}}}} \right]{\text{/}}\left[ {{\text{M}}{{\text{L}}_{\text{2}}}} \right]\left[ {\text{L}} \right]$

${\text{M}}{{\text{L}}_{\text{3}}}{\text{ + L }} \rightleftharpoons {\text{ M}}{{\text{L}}_{\text{4}}}{\text{ }}{{\text{K}}_{\text{4}}}{\text{ = }}\left[ {{\text{M}}{{\text{L}}_{\text{4}}}} \right]{\text{/}}\left[ {{\text{M}}{{\text{L}}_{\text{3}}}} \right]\left[ {\text{L}} \right]$

where $\mathrm{K}_{1}, \mathrm{~K}_{2}$, etc are known as stepwise stability constants. Alternatively, we can express the overall stability constant as follows:

${\text{M + 4L }} \rightleftharpoons {\text{ M}}{{\text{L}}_{\text{4}}}{\text{ }}{{\text{\beta }}_4} = \left[ {{\text{M}}{{\text{L}}_{\text{4}}}} \right]/\left[ {\text{M}} \right]{\left[ {\text{L}} \right]^4}$

12. Importance and Applications of Coordination Compounds

Analytical chemistry: .

The analytical applications of coordination chemistry are in

a. Qualitative and Quantitative Analysis :

Metal ions react with a variety of ligands to form colored coordination compounds. These reactions are used to detect metal ions. The formed colored complexes can be used to estimate metals using traditional or instrumental methods such as gravimetry or colorimetry. The following are some examples:

The addition of potassium ferrocyanide solution detects the presence of iron ions ($Fe^{3+}$), resulting in the formation of the Prussian blue complex.

${\text{F}}{{\text{e}}^{{\text{2 + }}}}{\text{ + }}{{\text{K}}_{\text{3}}}{\text{ Fe}}{\left( {{\text{CN}}} \right)_{{\text{6\;}}}} \to {\text{KFe}}\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]{\text{ + 2}}{{\text{K}}^{\text{ + }}}$

b. Volumetric Analysis:

Titration with EDTA can be used to determine the hardness of water. $\mathrm{Ca}^{2+}$ and $\mathrm{Mg}^{2+}$, the metal ions that cause hardness, form stable complexes with EDTA.

Metal Extraction and Purification:

Metals such as silver and gold are extracted by forming water-soluble cyanide complexes with the ore. By adding zinc to the solution, pure gold can be extracted. Metals can also be purified by forming and then decomposing their coordination compounds. For example, after extraction, impure nickel can be converted to pure nickel by first converting it to nickel carbonyl and then decomposing it.

Catalysts for coordination compounds are used in critical commercial processes. For example,

In the formation of polyethene, the Ziegler-Natta catalyst ($TiCl_4$ and trialkyl aluminium) is used as a catalyst.

In the hydrogenation of alkenes, the Wilkinson catalyst - $\operatorname{RhCl}\left(\mathrm{PPh}_{3}\right)_{3}$ is used.

Various rhodium complexes, such as $\left[\mathrm{Rh}(\mathrm{CO})_{2} \mathrm{I}_{2}\right],\left[\mathrm{Rh}(\mathrm{Cl})(\mathrm{CO})\left(\mathrm{PPh}_{3}\right)_{2}\right]$, or $\left[\mathrm{Rh}(\mathrm{Cl})(\mathrm{CO})_{2}\right]_{2}$ are used as catalysts in the Monsanto acetic acid process in the presence of $\mathrm{CH}_{3} \mathrm{l}, \mathrm{I}_{2}$, or HI as activator.

Electroplating:

Gold, silver, and copper coordination compounds are used as components in baths used for electroplating articles made of other metals with these metals. $\mathrm{K}\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]$ is used as an electrolyte in silver plating; $\mathrm{K}\left[\mathrm{Au}(\mathrm{CN})_{2}\right]$ is used as an electrolyte in gold plating; and $\mathrm{K}_{3}$ $\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]$ is used as an electrolyte in copper plating.

Coordination complexes are important biological compounds. Chlorophyll, for example, is a $\mathrm{Mg}^{2+}$ complex. This green pigment is essential for photosynthesis in plants. Similarly, haemoglobin, the red pigment found in blood, is a $\mathrm{Fe}^{2+}$ coordination complex, and vitamin B12, an essential nutrient, is a $\mathrm{Co}^{3+}$ complex.

6. Medicinal uses: In the treatment of metal poisoning, complexing or chelating agents are used, in which a coordination complex is formed between the toxic metal in excess metal and the complexing agent. EDTA, for example, is used to treat lead poisoning. When EDTA is injected intravenously into the bloodstream, it traps lead, forming a compound that is excreted in the urine. Mercury, arsenic, aluminum, chromium, cobalt, manganese, nickel, selenium, zinc, tin, and thallium are other heavy metal poisonings that can be treated similarly with chelation therapy. Similarly, D-penicillamine and desferrioxamine B, chelating ligands, are used to remove excess copper and iron, respectively.

13. Coordination Compounds and Complex Ions

Coordination compounds are those in which the central metal atom is linked to a number of ligands (ions or neutral molecules) via coordinate bonds, i.e. by these ligands donating lone pairs of electrons to the central metal atom ion.

If such a compound has a positive or negative charge, it is referred to as a complex ion, for example, ${\left[ {{\text{Fe}}{{\left( {{\text{CN}}} \right)}_{\text{6}}}} \right]^{{\text{4--}}}}{\text{, }}{\left[ {{\text{Cu}}{{\left( {{\text{N}}{{\text{H}}_{\text{3}}}} \right)}_{\text{4}}}} \right]^{{\text{2 + }}}}{\text{.}}$ Hence Co-ordination compounds are also those that contain complex ions, such as $K_4 [Fe(CN)_6]$, $[Cu(NH_3)_4]SO_4$, and so on. In general, a complex ion is denoted by ${\left[ {{\text{M}}{{\text{L}}_{\text{n}}}} \right]^{ \pm x}}$ where M is the metal ion, L represents ligands, n is the coordination number of metal ion and x is the net charge on the complex.

Four types of complexes are shown below:

Cation as complex ion, (carrying a net positive charge) e.g., $\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}$ in $\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right.$ ] $\mathrm{Cl}_{3} .$

Anion as complex ion, (carrying a net negative charge) e.g., $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}$ in $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$.

Cation and anion both as complex ions. Carrying both positive and negative change.

For e.g., $\left[\mathrm{Pt}(\mathrm{Py})_{4}\right]\left[\mathrm{PtCl}_{4}\right]$

Neutral complex (A complex carrying no net charge) e.g., $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ etc.

14. Terminology of Coordination Compounds

14.1 centre of coordination (central atom/ion or acceptor atom/ion): .

The centre of coordination is the cation or neutral atom to which one or more ligands (neutral molecules or anions) are attached or coordinated. As an acceptor, the central atom/ion must have empty orbitals in order to accommodate electron pairs donated by the ligand's donor atom. This explains why transition metals with empty d-orbitals readily form coordination compounds.

For example in the complexes $\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right) 6\right]^{2+}$ and $\left[(\mathrm{CN})_{6}\right]^{3-}, \mathrm{Ni}^{2+}$ and $\mathrm{Fe}^{3+}$ respectively are the central ions.

14.2 Ligands

A ligand or coordinating group is an atom, ion, or molecule that can donate at least two electrons to the central atom to form a coordinate bond (or dative linkage). The atom in a ligand that actually donates the electron pair is referred to as the donor atom. The ligands function as Lewis bases by donating one or more electron pairs to the central metal atoms or ions, which function as Lewis acids by accepting electrons.

14.2.1 Types of Ligands:

Ligands are classified based on how many lone pair electrons they donate to the central metal atom or ion.

Monodentate or Unidentate Ligands: These ligands have a single donor atom that donates only one electron pair to the central metal atom.

Bidentate Ligands: Ligands with two donor atoms and the ability to link with the central metal in two positions are referred to as bidentate ligands.

Tridentate Ligand: The ligands that possess three donor atoms are called tridentate ligands

Tetradentate Ligand: These ligands have four donor atoms.

Pentadentate Ligands: They have five donor atoms

Hexadentate Ligands: They have six donor atoms.

14.2.2 Chelating Ligands:

A bidentate or polydentate ligand is referred to as a chelating ligand if it forms a cyclic ring structure upon coordination. Chelates are the complexes that result from this process. Chelates with 5 or 6 membered rings are more stable. Due to steric hindrance, larger group ligands form more unstable rings than smaller group ligands.

14.2.3 Ambidentate Ligands:

The ligands that have two donor atoms but only one donor atom are attached to the metal atom at a time when forming complexes. These ligands are known as ambidentate ligands. As an example:

$\mathrm{M} \leftarrow \mathrm{NO}_{2}$ Nitrito-N

$\mathrm{M} \leftarrow \mathrm{CN}$ Cyano-C

$\mathrm{M} \leftarrow \mathrm{SCN}$ Thiocyanato-S

$\mathrm{M} \leftarrow \mathrm{ONO}$ Nitrito-O

$\mathrm{M} \leftarrow \mathrm{NC}$ Isocyano

$\mathrm{M} \leftarrow \mathrm{NCS}$ Thiocyanato-N

15. Coordination Number (C.N)

Chemistry class 12 revision notes for chapter 5 - coordination compounds.

You can download the CBSE class 12th revision notes for chapter 5 Coordination Compounds for free in PDF format. Also, students can download the revision notes for Coordination Compounds class 12 Notes and can be able to score high in exams. These are the Coordination Compounds class 12 Notes prepared by the team of expert teachers of Vedantu. The revision notes help you revise the whole chapter in just a few minutes. Recalling the revision notes on just a day before or the exam days is one of the best tips recommended and advised by the teachers during exam days.

What are Coordination Compounds?

Coordination compounds contain ions or molecules linked or coordinated to a transition metal. A few examples of the coordination compounds include [Ni(H 2 O) 6 ]Cl 2 , [Cr(NH 3 ) 5 (NO 2 )] 2+ . Ag(CN) 2- , CuCl42- are called the coordination complexes or the complex ions. Ligands are the ions or molecules that combine with the transition metal ions to produce these complexes further.

The coordination number of any of the Coordination compounds is given by the total number of ligands that are associated with the transition metal ion. Coordination compounds include substances such as chlorophyll, haemoglobin, vitamin B12, catalysts, and dyes, used in the preparation of the organic substances. The Coordination compounds are also used as catalysts for several biological and industrial processes having much importance in the qualitative and quantitative chemical analysis within the field of analytical chemistry.

Important Applications of the Coordination Compounds

Let us look at the essential applications of the Coordination Compounds.

Because of the formation of cyanide complexes (dicyanoargentate and dicyanoaurate), noble metals, such as silver and gold are extracted from their ore

The haemoglobin is one of the coordination compounds of iron

In the ethene polymerization, the Ziegler Natta catalyst (a combination of titanium tetrachloride and the triethyl aluminum) is used

A catalyst of a complex metal is used in the hydrogenation of alkenes

When the aqueous ammonia is mixed with the copper sulphate solution, a deep blue complex is formed, which is soluble in water. This reaction is helpful to detect the cupric ions present in the salt

Sub-Topics Covered under the Coordination Compounds

The necessary sub-topics that cover under Coordination Compounds are listed below:

Bonding in Metal Carbonyls - This topic discusses the concept of bonding in different metal carbonyls

Definition of Some Important Terms that are About Coordination

Crystal Field Theory - This unit explains what is meant by Crystal Field Theory and its significance

Geometric and Optical Isomerism - It describes the basic concept of what isomerism is and the geometric and optical part

Compounds - Students will study the crucial terms on what they mean in coordination chemistry

Introduction and Werner’s Theory of Coordination Compounds - In this concept, the students will study theory and look at its postulates including examples

Importance, Applications of Coordination Compounds - By this topic, you will learn about the applications and importance of coordination compounds including the applications of these important compounds

Nomenclature of Coordination Compounds - From this, the students will learn how the different complex compounds get their names

Isomerism in Coordination Compounds - This topic digs deep the isomerism topic and the coordination compounds

Valence Bond Theory in Coordination Compounds - This one will explore the valence bond theory and its respective important postulates

Importance of Revision Notes

It is always important and advised the students to keep Revision Notes either prepared by them or by the other digital platforms with them. Because it will help the students to get an in-depth understanding of the topics when they go through the notes before going to the exam.

Stay consistent with practice and avoid skipping it during CBSE (NCERT) preparation.

Develop a study plan that includes dedicated time slots for practicing different sections., take short breaks in between study sessions, but ensure they are not excessively long., make use of offline or online mock tests to evaluate your weaknesses and strengths accurately., analyze the results of mock tests to identify areas that require improvement and make necessary adjustments., ensure to revise each chapter multiple times for better retention and understanding., thorough revision is a key strategy for excelling in the exams., implement effective revision techniques such as creating concise notes, using flashcards, and solving previous years' question papers., seek clarification on any doubts or concepts that are unclear through additional resources or assistance from teachers., practice solving sample papers to get acquainted with the exam format and time management., stay organized and maintain a proper study schedule to effectively cover all the topics before the exam., conclusion .

Vedantu's Coordination Compounds Class 12 Notes for CBSE Chemistry Chapter 5 provide a comprehensive and well-structured resource for students studying coordination compounds. The notes cover all the essential topics, including the concept of coordination compounds, nomenclature, isomerism, bonding, and coordination number. The content is concise yet informative, making it easier for students to grasp complex concepts. The inclusion of examples and illustrations further enhances understanding. The notes also emphasize the application of coordination compounds in various fields. Overall, Vedantu's Class 12 Notes on Coordination Compounds are a valuable tool for students, offering a solid foundation and aiding in their preparation for examinations.

FAQs on Coordination Compounds Class 12 Notes CBSE Chemistry Chapter 5 (Free PDF Download)

1. List Out the Topics of Coordination Compounds?

The topics that fall under the topic, coordination compounds are listed below for the flexibility of students:

Crystal Field Theory

Bonding in Metal Carbonyls

Definition of the Important Terms concerning Coordination Compounds

Importance and Applications of the Coordination Compounds

Geometric and Optical Isomerism

Isomerism in Coordination Compounds

Introduction and Werner’s Theory of Coordination Compounds

Valence Bond Theory in Coordination Compounds

Nomenclature of Coordination Compounds

2. Where Can I Download the Revision Notes for Chemistry Coordination Compounds?

You can download the Coordination Compounds Revision Notes from Vedantu by reaching out to www.vedantu.com . Besides, you can also download the same from the official website as well.

3. Explain the Optical Isomerism in Coordination Compounds?

The isomer that forms a non-super imposable mirror image is called enantiomers or optical isomers. These are of two types as given below.

Isomer, that rotates the plane-polarized light in a clockwise direction is called a ‘d’ or ‘+’ or dextro isomer.

Isomer, that rotates the plane-polarized light in a counterclockwise direction is referred to as levo isomer or ‘l’, ‘-‘ isomer.

The equimolar mixture of ‘l’ and ‘d’ isomer is called the racemic mixture.

An example of Optical Isomerism can be given as follows.

(Image will be Uploaded Soon)

4. What are the Polydentate Ligands?

A few ligands have various donor atoms that can bind to the coordination centre. These ligands are often known as polydentate ligands.

A good example of a polydentate ligand can be given as the EDTA4- ion (which is a ethylene diamine tetraacetate ion), can bind to the coordination centre via its two nitrogen atoms and four oxygen atoms.

5. What points should be kept in mind while making a study plan for Chapter 5 of Class 12 Chemistry?

Follow the given procedure to make an effective study plan for Chapter 5 of Class 12 Chemistry:

Create a timetable. This will help you to divide your time so that you can focus on Chapter 5 of Class 12 Chemistry .

Go thoroughly through your syllabus. If you're unaware of your syllabus, you will not be able to start your preparation.

Practice sample papers and previous years question papers so that you can understand the concepts easily.

Use NCERT books and guidebooks while preparing for your exams. Students can also use the study material available on the vedantu app.

6. Write the limitations of the Valence Bond Theory.

Some Limitations of the Valence Band Theory are Given Below:

This theory is based on assumptions.

Quantitative understanding of magnetic data is not given in this theory.

Differences between strong and weak ligands are not discussed through the Valence Band Theory.

The theory does not explain the colour exhibited by complexes.

The explanation about the kinetic stabilities of the coordination compounds is not given by this theory.

The exact predictions regarding the square planar and tetrahedral structures of the coordinated complexes are not made through this theory.

7. What are the features of the Crystal Field Theory?

The Features of the Crystal Field Theory are as Follows:

The Crystal Field Theory states that the bond between the central metal ion and the ligand is simply ionic.

In this theory, the ligand is considered as the point negative charge.

The CMI is pondered as a positive charge.

In the case of anions, the ligands are treated as point charges.

The ligands are regarded as dipoles in the case of neutral molecules.

There is an electrostatic force of attraction between CMI and ligands.

8. What is isomerism in coordination compounds? What are the different types of isomerism?

The phenomenon in which two or more compounds have a different structural formula but have the same molecular formula differing in one or more chemical or physical properties is known as isomerism.

The types of isomerism are:

Structural Isomerism
Solvate isomerism
Linkage isomerism
Ionisation isomerism
Coordination isomerism
Stereoisomerism
Optical isomerism

These various types of isomerism are explained in detail in the NCERT book. Students can also download the Notes of Chapter 5 of Class 12 Chemistry free of cost from the vedantu website (vedantu.com).

9. What are the postulates of Werner's Theory of Coordination Compounds?

Beneath are the Postulates of Werner’s Theory of Coordination Compounds:

According to this theory, metals exhibit two types of valencies in coordination compounds. These valencies are primary and secondary.

The primary valencies get fulfilled by negative ions. These valencies are ionisable.

The secondary valencies are regarded as non-ionisable and get fulfilled by the neutral molecules or by negative ions.

The coordination number is equivalent to the secondary valence and this is fixed for a metal.

There is a spatial arrangement of metal when ions are bounded by secondary linkages.

Previous Year Question Papers CBSE Class 12

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NCERT Solutions for Class 12 Chemistry Chapter 5 Coordination Compound
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