For Class 11 students who want to get precise and comprehensive NCERT Solutions for Chemistry, we are providing here the accurate details for all questions given in Chemistry NCERT book.
NCERT books are written in the most lucid and clear manner that helps to break the complex problems in most efficient way possible. The questions given at the end of a chapter are based on every conceptual topic. Students must solve all these NCERT questions to keep a track of their understanding.
Benefits of solving NCERT exercise questions:
Solving the NCERT exercise problems will help you
- clear all the concepts you learned in a chapter
- familiarise with different types of questions that might be asked in exams
- get enough practice which is key to perform well in exams
Practicing the NCERT questions will assure good results as most of the questions in annual examinations are asked from NCERT textbooks.
CBSE Class 11 Chemistry NCERT Solutions for Chapter- Chemical Bonding and Molecular Structure
Here we are providing NCERT solutions for CBSE Class 11 Chemistry Chapter 4, Chemical Bonding and Molecular Structure. All the questions have been solved in the most appropriate and simple way so as to help students access the right study material for the exam preparation.
Students may download the NCERT solutions for Class 11 Chemistry in PDF format.
Main topics discussed in Class 11 Chemistry chapter- Chemical Bonding and Molecular Structure, are:
- Kossel-Lewis approach to chemical bonding
Octet rule and its limitations
Ionic or electrovalent bond
Lewis structures of molecules
- Lattice enthalpy
- Bond parameters
- Resonance structures
- Polarity of bonds
- Valence Shell Electron Pair Repulsion (VSEPR) theory
Valence bond theory
Orbital overlap concept
Directional properties of bonds
Overlapping of atomic orbitals
Types of overlapping and nature of covalent bonds
Strength of sigma and pi bonds
- Hybridisation and its types
Examples of sp3, sp2 and sp hybridisation
Hybridisation of elements involving d orbitals
- Molecular orbital theory
Linear combination of atomic orbitals
Conditions for the combination of atomic orbitals
Types of molecular orbitals
Energy level diagram for molecular orbitals
Electronic configuration and molecular behaviour
- Bonding in some homonuclear diatomic molecules
- Hydrogen bonding
Cause of formation of hydrogen bond
Types of H-bonds.
Some of the questions and their solutions from NCERT Solutions for Class 11: Chemical Bonding and Molecular Structure, are as follows:
Q. Explain the formation of a chemical bond.
Sol. A chemical bond is defined as an attractive force that holds the constituents (atoms, ions, etc.) together in a chemical species. Various theories have been suggested for the formation of chemical bonds such as the electronic theory, Valence shell electron pair repulsion theory, valence bond theory and molecular orbital theory. A chemical bond is attributed to the tendency of a system to attain stability. It was observed that the inertness of noble gases was because of their fully filled outermost orbitals. Hence, it was postulated that the elements having incomplete outermost shells are unstable (reactive). Atoms therefore, combine with each other and complete their octets or duplets to attain stable configuration of the nearest noble gases. This combination can occur either by sharing of electrons or by transferring one or more electrons from one atom to another. The chemical bond formed as a result of sharing of electrons between atoms is called covalent bond. An ionic bond is formed as a result of the transference of electrons from one atom to another.
Q. Explain with help of a suitable example polar covalent bond.
Sol. When two dissimilar atoms having different electronegativities combine to form a covalent bond, the bond pair of electrons is not shared equally. The bond pair shifts towards the nucleus of an atom having greater electronegativity. As a result electron distribution gets distorted and the electron cloud is displaced towards the electronegative atom.
As a result, the electronegative atom becomes slightly negatively charged while the other atom becomes slightly positively charged. Thus, opposite poles are developed in the molecule and this type of bond is called polar covalent bond.
HCl, for example contains a polar covalent bond. Chlorine atom is more electronegative than the hydrogen atom. Hence, the bond pair lies towards chlorine therefore, it acquires a partial negative charge.
Q. Write the significance of a plus and minus shown in representing the orbitals.
Sol. Molecular orbitals are represented by wave functions. A plus sign in an orbital represents positive wave function while a negative sign indicates a negative wave function.
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