Valence Bond Theory Examples
Valence bond theory (VBT) is used to explain how covalent bonds form in many compounds. Here are some examples of VBT:
- Water (H2O): Water is made up of two hydrogen atoms bound to an oxygen atom. Each hydrogen atom has an s-orbital with one lone electron, and oxygen has an s-orbital with an electron pair.
- Fluorine Molecule (F2): The F-F bond in the diatomic fluorine molecule is formed by the intersection of the two F atoms’ pz orbitals, each of which contains an unpaired electron.
- Ethylene (C2H4): Both C atoms have three bonding pairs and no lone pairs, meaning they are both sp2 hybridized.
- Methylamine (CH3NH2): Both the carbon and the nitrogen atom are sp3-hybridized. The C-N sigma bond is an overlap between two sp3 orbitals
VBT can also explain the difference in the length and strength of the chemical bonds in H2 and F2 molecules.
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Valence Bond Theory
Valence bond theory (VBT) describes the formation of covalent bonds and the electronic structure of molecules. It assumes that electrons occupy atomic orbitals of individual atoms within a molecule, and that the electrons of one atom are attracted to the nucleus of another atom.
VBT states that the overlap of incompletely filled atomic orbitals leads to the formation of a chemical bond between two atoms. The unpaired electrons are shared and a hybrid orbital is formed. VBT views bonds as weakly coupled orbitals (small overlap). When the orbitals overlap along an axis containing the nuclei, they form a σ bond. VBT accounts for the directional nature of covalent bonds.
In this article, we will learn about Valance Bond Theory, Valance Bond Theory Class 12, its various postulates, limitations, and other details. Before learning about VBT (Valance Bond Theory), let’s first learn about Hybridization.
Table of Content
- What is Hybridization?
- Number of Orbitals and Types of Hybridization
- What is Valence Bond Theory?
- Postulates of Valence Bond Theory
- Applications
- Limitations