What is meant by hybridisation of atomic orbitals? Describe the shapes of \(sp, sp ^2 , sp ^3\) hybrid orbitals.
Solution and Explanation
Hybridization is defined as an intermixing of a set of atomic orbitals of slightly different energies, thereby forming a new set of orbitals having equivalent energies and shapes.
For example, one \(2s-orbital\) hybridizes with two \(2p-orbitals\) of carbon to form three new \(sp ^2\) hybrid orbitals.
These hybrid orbitals have minimum repulsion between their electron pairs and thus, are more stable. Hybridization helps indicate the geometry of the molecule.
Shape of sp hybrid orbitals: sp hybrid orbitals have a linear shape. They are formed by the intermixing of s and porbitals as:
Shape of \(sp ^2\) hybrid orbitals:
\(sp ^2\) hybrid orbitals are formed as a result of the intermixing of one \(s-orbital\) and two \(2p-orbitals\). The hybrid orbitals are oriented in a trigonal planar arrangement as:
Shape of \(sp ^3\) hybrid orbitals:
Four \(sp ^3\) hybrid orbitals are formed by intermixing one \(s-orbital\) with three \(p-orbitals\). The four \(sp ^3\) hybrid orbitals are arranged in the form of a tetrahedron as:
Top Questions on Hybridisation
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Concepts Used:
Chemical Bonding and Molecular Structure
Such a group of atoms is called a molecule. Obviously, there must be some force that holds these constituent atoms together in the molecules. The attractive force which holds various constituents (atoms, ions, etc.) together in different chemical species is called a chemical bond.
Types of Chemical Bonds:
There are 4 types of chemical bonds which are formed by atoms or molecules to yield compounds.
- Ionic Bonds - Ionic bonding is a type of chemical bonding which involves a transfer of electrons from one atom or molecule to another.
- Covalent Bonds - Compounds that contain carbon commonly exhibit this type of chemical bonding.
- Hydrogen Bonds - It is a type of polar covalent bonding between oxygen and hydrogen wherein the hydrogen develops a partial positive charge
- Polar Bonds - In Polar Covalent chemical bonding, electrons are shared unequally since the more electronegative atom pulls the electron pair closer to itself and away from the less electronegative atom.
Factors Affecting Bond Enthalpy in Chemical Bonding:
- Size of the Atom
- Multiplicity of Bonds
- Number of Lone Pair of Electrons Present
- Bond Angle