CBSE Class 11-science Chemistry Chemical Bonding and Molecular Structure
The Lewis dot structures show the arrangement of bonded pairs and lone pairs around
The octet rule is a simple chemical rule of thumb that states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas.
Ionic bond is electrostatic force of attraction between two oppositely charged atoms or group of atoms.
Covalent bond is formed by sharing of valence electrons.
Bond enthalpy is the energy required to break one mole of bond and is significant in determining the property of molecules.
Enthalpy of reaction is calculated from bond enthalpies of the reactants and the products.
Hybrid orbitals result from the mixing of atomic orbitals on the same atom.
The orbitals undergoing hybridisation should have only a small difference in energy and they should be present in the valence shell of the atom.
Geometry and Shapes of Molecules
VSEPR Theory predicts the shapes of molecules based on least possible energy.
Resonance and Hydrogen Bond
Pair of electrons in the multiple bonds are delocalised and structures so formed are called resonating or canonical structures.
Molecular Orbital Theory
Bonding molecular orbitals are at lower energy than the atomic orbitals and anti-bonding molecular orbitals with higher energy than the atomic orbital.
The stability and magnetic character of the molecule depends on the number of electrons in the bonding and anti-bonding.
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