Your Online "Chemical Bonding" Teacher
Home » Chemistry » Chemical Bonding »
Water is the best example of hydrogen bonding. We all know that how much water is important in our life. So hydrogen bonding is very important for sustaining life. Water is recognized as a natural solvent. Because without hydrogen bond water would not be ...
The bond which is formed between hydrogen atom and a higher electronegative atom (F, O or N) is known as Hydrogen bond. This bond involves dipole to dipole movement. The bond strength of hydrogen is very small e.g. H….F bond is 41.83 KJmol -1. Hydrogen ...
Metallic bond is formed due to the attraction between kernels and the mobile electrons in a metal lattice. Metallic bond is a non-directional bond. This bond is helpful in making the substances malleable and ductile. This is a weak bond due to the simultaneous attraction ...
Bonding Molecular Orbital: Bonding molecular orbital is formed by the addition of overlapping of atomic orbitals. The wave function of the bonding MO may be written as: Ψ (MO) = ΨA + ΨB. Atomic orbitals having same sign forms the Bonding molecular orbital when the ...
Sigma bond: sigma bond is formed due to the axial overlapping of two orbital’s (‘s-s’, ‘s-p’or’p-p’). Only one sigma bond can exists between two atoms. Sigma bond is denoted as’ σ ‘bond. In Sigma bond the electron density is maximum and it is cylindrically ...
The valence bond theory was developed by W.Heitler and F.London in 1927. Then it was further amended by the Linus Pauling and J.C. Slater. For this Linus Pauling get the Chemistry Nobel Prize in 1954. Valence bond theory is based on wave mechanical expression of the ...
Fajan gives the following four rules for the Polarisation: Polarization will be increased by: 1. High charge and small size of the cation. 2. High charge and large size of the anion. 3. The polarizability of an anion is related to the deformability of its electron cloud (i.e. its ...
The relative energies of molecular orbitals depend upon the following two factors: (i) Atomic orbitals energies for the combination to form molecular orbitals. (ii) The extent of overlapping between the atomic orbitals. The greater the overlap, the more the bonding orbital is lowered and the anti-bonding orbital is ...