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- Chemical Bond. The force that holds different atoms in a molecule is called chemical bond.
- Octet Rule. Atoms of different elements take part in chemical combination in order to complete their octet or to attain the noble gas configuration.
- Valence Electrons. It is the outermost shell electron which takes part in chemical combination.
- Facts Stated by Kossel in Relation to Chemical Bonding. — In the periodic table, the highly electronegative halogens and the highly electro-positive alkali metals are separated by noble gases.
Learn the basics of chemical bonding and molecular structure with free CBSE notes for class 11 chemistry. The notes cover topics such as octet rule, covalent bond, polarity, valence bond theory, molecular orbital theory and more.
The Chemical Bonding and Molecular Structure Class 11 Notes is an appropriate study resource because it compiles the entire lesson of Chemical Bonding and Molecular Structure into a short yet precise document.
- Section – A
- Section – B
- Chemical Bond
- Lewis Symbols
- Covalent Bond
- Formal Charge
- Hybridisation
- Valence Bond Theory
- Molecular Orbital Theory
- Metallic Bond
- GeneratedCaptionsTabForHeroSec
1. The given statement is True or False: The shape of SF6molecule is octahedral whereas that of IF7is square pyramidal. Ans. False shape of IF7is pentagonal bipyramidal 2. Why is NaCl a bad conductor of electricity in the solid state? Ans. In the solid state, Na+and Cl–ions are strongly held together and are not free to move. 3. Out of HF, HCl, HBr...
11. Write the significance of plus and minus sign shown in representing the orbitals. Ans.Molecular orbitals are represented by wave functions. A plus sign in an orbital indicates a positive wave function while a minus sign in an orbital represents a negative wave function. 12. Define electronegativity. How does it differ from electron gain enthalp...
Chemical bonding is the creation of a chemical compound by forming a chemical link between two or more atoms, molecules, or ions. The atoms in the resulting molecule are held together by chemical bonds.
In 1916, Kossel and Lewis were successful in providing a successful explanation for why atoms unite to form molecules based on the concept of an electrical configuration of noble gases. Noble gas atoms have little or no inclination to mix with other noble gas atoms or atoms of other elements. This implies that the electronic arrangements of these a...
In nature, covalent bonds can be either polar or nonpolar. Electrons are shared unequally in Polar Covalent chemical bonding because the more electronegative atom pulls the electron pair closer to itself and away from the less electronegative atom. A polar molecule like water is an example. The irregular spacing of electrons between the atoms cause...
A charge on an individual atom(s) in a polyatomic molecule is known as formal charge. It's a deceptive charge that's linked to only one atom in the structure. We term it fake because a molecule or compounds true charge is distributed across the species' structure. Formal charge is caused by flaws in the configuration of an atom involved in the synt...
Hybridisation is defined as the mixing of atomic orbitals belonging to the same atom but with slightly varying energies, resulting in an energy redistribution between them and the production of new orbitals with identical energies and shapes. Hybrid orbitals are the novel orbitals that result from this process. Hybridisation: Some Important Points:...
Types of Covalent Bond:
1. Sigma (σ) Bond. 2. Pi (π) Bond.
1. Sigma (σ) Bond:
Head-on positive (same phase) overlap of atomic orbitals along the internuclear axis forms this sort of covalent connection. Due to the direct overlapping of the participating orbitals, sigma bonds are the strongest covalent bonds. The electrons that participate in a bond are referred to as electrons. All single bonds are, in general, sigma bonds. The following atomic orbital combinations can be used to make them. S-S Overlapping: One “s” orbital from each participating atom undergoes head-on...
2. The Pi (π) Bond:
Sidewise positive (same phase) overlap of atomic orbitals in a direction perpendicular to the internuclear axis forms pi bonds. The axes of the atomic orbitals are parallel to one another during bond formation, whereas the overlapping is perpendicular to the internuclear axis. This sort of covalent bonding is depicted in the diagram below. Showing p-p Overlapping to form Pi (π) Bond Due to the substantially smaller degree of overlapping, pi bonds are often weaker than sigma bonds. A typical t...
The orbitals of the connected atoms lose their distinct character and merge (overlap) to form bigger orbitals called molecular orbitals when the atoms to be joined get near together. A molecule has molecular orbitals, which are similar to atomic orbitals. The sole distinction is that electrons in atomic orbitals travel under the influence of only o...
Metal atoms are the constituent particles of metallic solids, which are bound together by metallic bonds. A metal atom is said to be made up of two parts: valence electrons and the remaining kernel (the nucleus and inner shells). Metal atom kernels occupy the lattice sites, while valence electrons occupy the space between the kernels. Metal atoms' ...
Download free PDF of revision notes for Chemical Bonding and Molecular Structure, a chapter from CBSE Class 11 Chemistry textbook. Learn about ionic, covalent, coordinate and metallic bonds, hybridization, molecular orbitals and more.
Mar 18, 2024 · The main topics covered in Class 11 Chemistry chapter 4 notes are KÖssel-Lewis’s approach to chemical bonding, the octet rule, and its limitations, drawing Lewis structures of simple molecules, VSEPR theory, valence bond theory, molecular orbital theory of homonuclear diatomic molecules, and concepts of hydrogen bonding.
- Sumit Saini
Learn about the types, formation and properties of chemical bonds, such as ionic, covalent, coordinate and hydrogen bonds. Find out the VSEPR theory, dipole moment, resonance, valence bond theory and more with examples and diagrams.
Download free PDF notes for CBSE Class 11 Chemistry Chapter 4 on chemical bonding and molecular structure. Learn about ionic, covalent, hydrogen, and resonance bonds, VSEPR, valence bond, and molecular orbital theories.
