Ionic Bond is a bond that is formed by the electrostatic force of attraction between atoms. In an ionic bond, a complete transfer of electrons takes place in the process of bond formation. This bond is formed by the attracting force between the cations and the anions that are formed by the donating and acceptance of the electrons.
Ionic Bond is also called the Electrovalent bond and is formed to complete the octet of the participating atoms. If an atom combines after forming a bond it releases some energy called the bond formation energy. The higher the energy released the higher the stability of the compound.
Table of Contents
Chemical Bond
The chemical bonds are formed when two or more two atoms transfer or share their electrons and combined completely to complete their octet. All the compounds around us are formed by the bonds. Now we define a bond as the force of attraction that joins two or more atoms together to form chemical compounds. We have about 120 elements known in the periodic table but there are billions of compounds known to us all these are formed by the joining of various elements together through bonds. There are generally three types of bonds that are,
Ionic Bonds: They are formed by the transfer of electrons from one atom to another.
Covalent Bonds: They are formed by sharing of the electrons.
Coordinate Bonds: They are formed when an atom donates its lone pair of electrons to another atom.
What is Ionic Bond?
The bond formed by losing or gaining electrons is called Ionic Bond. All the atoms form bonds to complete their octet or to achieve an inert gas configuration. An atom that has eight electrons in its outermost shell is called an inert gas which is highly stable and does not react with other atoms. If an atom has 1,2 or 3 electrons in its outermost shell it losses its electrons to form a cation with eight electrons in its penultimate shell, whereas if an atom has 5, 6, or 7 electrons in its outermost shell its accepts electrons forming an anion with eight electrons in its outermost (valance) shell. So the bond formed between these cations and the anion because of the electrostatic attraction force is called the Ionic bond.
The ionic bond is the strongest bond and all the compounds that are formed by the ionic bond are called the ionic compound. The ionic bond is also called an electrovalent bond as they are formed by the transfer of electrons. So simply an ionic or electrovalent bond is defined as the bond formed by the transfer and acceptance of the electrons. High electropositive elements like alkali and alkaline earth metals and high electronegative elements like halogens are combined easily by ionic bonds.
Electrovalent Bond
Ionic Bonds sometimes called Electrovalent bonds and they are also formed when electrons are transferred from one atom to another atom, resulting in positive and negative ions. The bond formed by the transfer of electrons between atoms is known as an electrovalent bond or an ionic bond. Electrovalent bonds can only be formed between a metal and a nonmetal. Two non-metals or two metals can neither form an electrovalent bond.
Factors Responsible for the Formation of Ionic Bonds
Various factors responsible for the formation of the ionic bond are discussed below,
The metal atom taken for the formation of the ionic bond should have low ionization enthalpy.
The non-metal atom taken for the formation of the ionic bond should have high electron gain enthalpy.
High energy must be released when the formation of the bond takes place, the higher the energy released the higher the strength of the ionic bond.
Electronegativity and Ionic Bonding
An ionic bond is a stable bond formed by the complete transfer of valence electrons. Ionic bond results in the formation of two oppositely charged ions – positive ions called cations and negative ions called anions. High electronegative compound forms very stable ionic compound as they can easily accept an electron to form anions. The ionic bond of highly electropositive and highly electronegative elements are much more stable as compared to other ionic compounds as they have a strong electrostatic force of attraction between them.
Properties of Ionic Bond
Ionic bonds have various properties that differentiate them from other bonds and some of the properties of the ionic compound are,
Ionic bonds are the most stable of all bonds.
As ionic bonds have charge separation, they are the most reactive of all the bonds in the appropriate medium.
The melting and boiling points of ionic-bonded molecules are extremely high.
Ionic-bonded molecules in aqueous solutions or molten states are good conductors of electricity because of the presence of ions, which act as charge carriers.
In nature, ionic-boned compounds are usually in a solid state.
Ionic-bonded molecules exist as crystal structures.
Difference between Ionic Bond and Covalent Bond
Ionic Bonds and Covalent Bonds are two types of bonds that form various chemical compounds that we use or see in our daily life. Some of the differences between the ionic bond and the covalent bond are discussed in the table below,
Ionic Bond
Covalent Bond
Ionic bonds are formed by the attraction of positive and negative ions in a crystal, and compounds held together by ionic bonds are known as ionic compounds.
When two atoms share one or more electron pairs, they form a covalent bond. Each atom contributes an equal number of electrons to the formation of the bond.
In the formation of ionic bonds cations and anions are formed as intermediates ions.
No such intermediates are formed in the formation of covalent bonds.
Ionic bonds are formed between two atoms in which one atom is electronegative and the other is electropositive.
As atoms with higher ionization potential do not lose their valence electrons easily, they prefer to form covalent bonds by sharing electrons.
If the electronegativity difference between the atom is very high they form ionic bonds. For instance, bonds formed in the KCl compound.
If the electronegativities of the combining atoms are not significantly different, the bond formed between them is most likely covalent. For instance, bonds formed in the HCl compound
Examples of the compound with ionic bonds are,
Examples of the compound with covalent bonds are,
Examples of Ionic Bonds
There are various compounds which are formed by ionic compounds and these compounds are called ionic bonds. Various examples of the ionic bond are discussed in the table below,
Compound
Cation
Anion
Reaction
Electronic Configuration
NaCl
Na+
Cl–
Na → Na+ + e– Cl + e–→ Cl–
Na = 2, 8, 1 Cl = 2, 8, 7
CaCl2
Ca2+
2Cl–
Ca → Na2+ + 2e– 2Cl + 2e–→ 2Cl–
Ca = 2, 8, 8, 2 Cl = 2, 8, 7
CaO
Ca2+
O2-
Ca → Na2+ + 2e– O + 2e– → O2-
Now we explain the formation of NaCl in detail
Bonding in NaCl
NaCl is an ionic compound that is formed by the formation of Na+ ions and Cl– ions.
The electronic configuration of Sodium is (2,8,1) and it has 1 electron more than a stable noble gas configuration (2,8). So it easily forms Na+ ion by losing an electron.
The electronic configuration of Chlorine is (2,8,7) and it has 1 electron short to achieve a stable noble gas configuration (2,8,8). So it easily forms Cl– ion by gaining an electron.
Now one electron from Na goes to Cl and they both form the Na+ cation and Cl– anion respectively, which are joined together by the electrostatic force of attraction. Forming NaCl ionic compound, the formation of the NaCl compound by the ionic bond is shown in the image below,
FAQs on Ionic Bonds
Q1: What are Chemical Bonds?
Answer:
Chemical bonds are the forces between two or more two atoms that allow atoms to combine to form compounds, they are the results of the interaction between the electrons of the atoms. We charged particles of two atoms interact they form bonds which hold atoms together two form chemical compounds.
Q2: What are the Types of Chemical Bonds?
Answer:
The chemical bond is the force that joins atoms together to form chemical compounds. There are generally three types of chemical bonds that join various atoms together to form the chemical compounds that are,
Ionic Bonds
Covalent Bonds
Coordinate Bonds
Q3: What are Ionic Bonds?
Answer:
Ionic bonds are the bonds formed by the complete transfer of electrons. These are the strongest type of bond and are formed when an atom completely transfers its electron to another atom to form a bond between them. They are formed by joining cations and anions together by electrostatic force. Some examples of the compound where an ionic bond is formed are,
Q4: What are Covalent Bonds?
Answer:
Covalent bonds are the bonds formed by the sharing of electrons. They are weaker than ionic compounds in strength and are formed when two or more two atoms share their electrons to complete their octet. Some examples of the compound where a covalent bond is formed are,
Q5: What are Examples of the Ionic Bond?
Answer:
The various examples of the compounds where the ionic bond is formed are,
NaCl, in the NaCl Na atom, loses an electron to form the Na+ ion and Cl atom gains an electron to form Cl– now these Na+ cations and Cl– anions combine together by electrostatic force to form an ionic bond. Some other compounds formed by the ionic bonds are,
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Er. Neeraj K.Anand is a freelance mentor and writer who specializes in Engineering & Science subjects. Neeraj Anand received a B.Tech degree in Electronics and Communication Engineering from N.I.T Warangal & M.Tech Post Graduation from IETE, New Delhi. He has over 30 years of teaching experience and serves as the Head of Department of ANAND CLASSES. He concentrated all his energy and experiences in academics and subsequently grew up as one of the best mentors in the country for students aspiring for success in competitive examinations.
In parallel, he started a Technical Publication "ANAND TECHNICAL PUBLISHERS" in 2002 and Educational Newspaper "NATIONAL EDUCATION NEWS" in 2014 at Jalandhar. Now he is a Director of leading publication "ANAND TECHNICAL PUBLISHERS", "ANAND CLASSES" and "NATIONAL EDUCATION NEWS".
He has published more than hundred books in the field of Physics, Mathematics, Computers and Information Technology. Besides this he has written many books to help students prepare for IIT-JEE and AIPMT entrance exams. He is an executive member of the IEEE (Institute of Electrical & Electronics Engineers. USA) and honorary member of many Indian scientific societies such as Institution of Electronics & Telecommunication Engineers, Aeronautical Society of India, Bioinformatics Institute of India, Institution of Engineers. He has got award from American Biographical Institute Board of International Research in the year 2005.
CBSE Class 11 Chemistry Syllabus is a vast which needs a clear understanding of the concepts and topics. Knowing CBSE Class 11 Chemistry syllabus helps students to understand the course structure of Chemistry.
Unit-wise CBSE Class 11 Syllabus for Chemistry
Below is a list of detailed information on each unit for Class 11 Students.
UNIT I – Some Basic Concepts of Chemistry
General Introduction: Importance and scope of Chemistry.
Nature of matter, laws of chemical combination, Dalton’s atomic theory: concept of elements, atoms and molecules.
Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.
UNIT II – Structure of Atom
Discovery of Electron, Proton and Neutron, atomic number, isotopes and isobars. Thomson’s model and its limitations. Rutherford’s model and its limitations, Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals – Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.
UNIT III – Classification of Elements and Periodicity in Properties
Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100.
UNIT IV – Chemical Bonding and Molecular Structure
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.
UNIT V – Chemical Thermodynamics
Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics – internal energy and enthalpy, measurement of U and H, Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Second law of Thermodynamics (brief introduction) Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes. Third law of thermodynamics (brief introduction).
UNIT VI – Equilibrium
Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle, ionic equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization, ionization of poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).
UNIT VII – Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.
UNIT VIII – Organic Chemistry: Some basic Principles and Techniques
General introduction, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.
UNIT IX – Hydrocarbons
Classification of Hydrocarbons Aliphatic Hydrocarbons: Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions. Alkenes – Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition. Alkynes – Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of – hydrogen, halogens, hydrogen halides and water.
Aromatic Hydrocarbons:
Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Craft’s alkylation and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.
To know the CBSE Syllabus for all the classes from 1 to 12, visit the Syllabus page of CBSE. Meanwhile, to get the Practical Syllabus of Class 11 Chemistry, read on to find out more about the syllabus and related information in this page.
CBSE Class 11 Chemistry Practical Syllabus with Marking Scheme
In Chemistry subject, practical also plays a vital role in improving their academic scores in the subject. The overall weightage of Chemistry practical mentioned in the CBSE Class 11 Chemistry syllabus is 30 marks. So, students must try their best to score well in practicals along with theory. It will help in increasing their overall academic score.
CBSE Class 11 Chemistry Practical Syllabus
The experiments will be conducted under the supervision of subject teacher. CBSE Chemistry Practicals is for 30 marks. This contribute to the overall practical marks for the subject.
The table below consists of evaluation scheme of practical exams.
Evaluation Scheme
Marks
Volumetric Analysis
08
Salt Analysis
08
Content Based Experiment
06
Project Work
04
Class record and viva
04
Total
30
CBSE Syllabus for Class 11 Chemistry Practical
Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used.
A. Basic Laboratory Techniques 1. Cutting glass tube and glass rod 2. Bending a glass tube 3. Drawing out a glass jet 4. Boring a cork
B. Characterization and Purification of Chemical Substances 1. Determination of melting point of an organic compound. 2. Determination of boiling point of an organic compound. 3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.
C. Experiments based on pH
1. Any one of the following experiments:
Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
Comparing the pH of solutions of strong and weak acids of same concentration.
Study the pH change in the titration of a strong base using universal indicator.
2. Study the pH change by common-ion in case of weak acids and weak bases.
D. Chemical Equilibrium One of the following experiments:
1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions. 2. Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.
E. Quantitative Estimation i. Using a mechanical balance/electronic balance. ii. Preparation of standard solution of Oxalic acid. iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid. iv. Preparation of standard solution of Sodium carbonate. v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonatesolution.
F. Qualitative Analysis 1) Determination of one anion and one cation in a given salt Cations‐ Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+ Anions – (CO3)2‐ , S2‐, NO2‐ , SO32‐, SO2‐ , NO ‐ , Cl‐ , Br‐, I‐, PO43‐ , C2O2‐ ,CH3COO‐ (Note: Insoluble salts excluded)
2) Detection of ‐ Nitrogen, Sulphur, Chlorine in organic compounds.
G) PROJECTS Scientific investigations involving laboratory testing and collecting information from other sources.
A few suggested projects are as follows:
Checking the bacterial contamination in drinking water by testing sulphide ion
Study of the methods of purification of water.
Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional variation in drinking water and study of causes of presence of these ions above permissible limit (if any).
Investigation of the foaming capacity of different washing soaps and the effect of addition of Sodium carbonate on it.
Study the acidity of different samples of tea leaves.
Determination of the rate of evaporation of different liquids Study the effect of acids and bases on the tensile strength of fibres.
Study of acidity of fruit and vegetable juices.
Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with theapproval of the teacher.
Practical Examination for Visually Impaired Students of Class 11
Below is a list of practicals for the visually impaired students.
A. List of apparatus for identification for assessment in practicals (All experiments) Beaker, tripod stand, wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand, dropper, test tube holder, ignition tube, china dish, tongs, standard flask, pipette, burette, conical flask, clamp stand, dropper, wash bottle • Odour detection in qualitative analysis • Procedure/Setup of the apparatus
B. List of Experiments A. Characterization and Purification of Chemical Substances 1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid B. Experiments based on pH 1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper 2. Comparing the pH of solutions of strong and weak acids of same concentration.
C. Chemical Equilibrium 1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of eitherions. 2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the concentration of either of the ions.
D. Quantitative estimation 1. Preparation of standard solution of oxalic acid. 2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
E. Qualitative Analysis 1. Determination of one anion and one cation in a given salt 2. Cations – NH+4 Anions – (CO3)2-, S2-, (SO3)2-, Cl-, CH3COO- (Note: insoluble salts excluded) 3. Detection of Nitrogen in the given organic compound. 4. Detection of Halogen in the given organic compound.
Note: The above practicals may be carried out in an experiential manner rather than recording observations.
We hope students must have found this information on CBSE Syllabus useful for their studying Chemistry. Learn Maths & Science in interactive and fun loving ways with ANAND CLASSES (A School Of Competitions) App/Tablet.
Frequently Asked Questions on CBSE Class 11 Chemistry Syllabus
Q1
How many units are in the CBSE Class 11 Chemistry Syllabus?
There are 9 units in the CBSE Class 11 Chemistry Syllabus. Students can access various study materials for the chapters mentioned in this article for free at ANAND CLASSES (A School Of Competitions).
Q2
What is the total marks for practicals examination as per the CBSE Class 11 Chemistry Syllabus?
The total marks for the practicals as per the CBSE Class 11 Chemistry Syllabus is 30. It includes volumetric analysis, content-based experiment, salt analysis, class record, project work and viva.
Q3
Which chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry?
The organic chemistry chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry.
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