Chemistry Chemical Bonding and Molecular Structure

O? (15) will have configuration σ1s²σ1s²σ2s²σ2s²σ2p? ² (π2p? ²=π2p? ²) (π*2p? ¹). This ion is paramagnetic.

The concept of delocalization or resonance can be explained for quantum mechanical atomic models in which electrons are considered to be spread over the entire molecular orbital.

The fundamental assumption of the valence bond theory contradicts the delocalization. The valence bond theory assumes that a covalent bond forms from the overlap of atomic orbitals on adjacent atoms, and electron density is localized between two specific nuclei.

That is why VBT cannot explain energy stabilization due to the resonance property.

H? O has a tetrahedral geometry and a bent shape with a bond angle of 104.5°, which is smaller than 109.5°. This is because of the presence of two lone pairs in H? O.

ClF? and XeF? have two lone pairs of electrons on central atom.

Hybridisation of carbon a, b, and c respectively are sp³, sp² and sp².

A central atom having two lone pairs and three bond pairs reflects sp³d hybridization and a corresponding T-shaped geometry.

As you know, electrovalent bonds result very strong electrostatic attraction force. All the factors that help maximize this electrostatic attraction are important for the formation of the ionic bond. Here are the important factors;

• Low ionization energy Metal
• High electron affinity Non Metal
• Large-sized cations
• Small-sized anions
• Electronegativity equal to or greater than 1.7

Covalent and electrovalent bonding are the two major chemical bonding processes. These two bonds are different from each other in multiple aspects. Check the table below to know a concise summary of the differences.