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The carbon atoms in this form are each linear in geometry with sp orbital hybridisation.
When atoms interact to form a chemical bond, the atomic orbitals are said to mix in a process called orbital hybridisation.
In term of valence bond theory, these molecules can be described as adopting sp orbital hybridisation, featuring one sigma and two pi bonds.
Also, when the cation is formed the central carbon is rehybridised from sp to sp Orbital hybridisation.
Titanium(IV) hydride is the simplest transition metal molecule that displays sd orbital hybridisation.
Bent's rule was formulated in 1961 by American chemist Henry Bent to explain deviations in structures predicted from the orbital hybridisation theory.
Main article: Orbital hybridisation For transition metals as well as a more comprehensive quantum chemical description for both, Orbital hybridisation is used.
The importance of orbital overlap was emphasized by Linus Pauling to explain the molecular bond angles observed through experimentation and is the basis for the concept of orbital hybridisation.
His work on chemical bonding marks the beginning of modern quantum chemistry, and many of his contributions like Orbital hybridisation and electronegativity have become part of standard chemistry textbooks.
When a molecule cannot be represented by the standard tools of valence bond theory (promotion, orbital hybridisation, orbital overlap, sigma bond and pi bond formation) because no single structure predicted by VB can account for all the properties of the molecule, one invokes the concept of resonance.
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