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Examples ofvalence bond theory
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Invalencebondtheory, covalent bonds are assumed to consist of two electrons lying in overlapping, usually hybridised, atomic orbitals from bonding atoms.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Invalencebondtheory, it is described as a resonance hybrid with equal contributions from two canonical forms that are mirror images of each other.
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This example is from Wikipedia and may be reused under a CC BY-SA license.It is conventional in organic chemistry to write isocyanates with two double bonds, which accords with a simplisticvalencebondtheoryof the bonding.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Invalencebondtheory, delocalization in benzene is represented by resonance structures.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Avalencebondtheoryapproach which just considered s and p orbitals would describe the bonding in terms of resonance between two resonance structures.
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This example is from Wikipedia and may be reused under a CC BY-SA license.This is similar to other modernvalencebondtheorymethods.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Invalencebondtheory, the two electrons on the two atoms are coupled together with the bond strength depending on the overlap between them.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Simplevalencebondtheorywould predict a quadruple bond as the only way to satisfy the octet rule for carbon in dicarbon.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Covalent bonds are better understood byvalencebondtheoryor molecular orbital theory.
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This example is from Wikipedia and may be reused under a CC BY-SA license.If a single set of these orbitals is combined with all linear independent combinations of the spin functions, we have spin-coupledvalencebondtheory.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Orbital hybridisation allowedvalencebondtheoryto successfully explain the geometry and properties of a vast number of molecules.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Formal charges are used invalencebondtheoryfor some canonical forms used to construct a resonance hybrid.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Valencebondtheoryconcerns itself with the formation of sigma and pi bonds.
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This example is from Wikipedia and may be reused under a CC BY-SA license.With more complicated compounds, such as metal complexes,valencebondtheoryis less applicable and alternative approaches, such as the molecular orbital theory, are generally used.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Valencebondtheoryproposes that covalent bonds consist of two electrons lying in overlapping, usually hybridised, atomic orbitals from two bonding atoms.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Valencebondtheoryfurther describes the composition of each orbital in a molecule.
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This example is from Wikipedia and may be reused under a CC BY-SA license.More sophisticated theories arevalencebondtheorywhich includes orbital hybridization and resonance, and the linear combination of atomic orbitals molecular orbital method which includes ligand field theory.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Valencebondtheorygives us a model for benzene where each carbon atom makes two sigma bonds with its neighbouring carbon atoms and one with a hydrogen atom.
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This example is from Wikipedia and may be reused under a CC BY-SA license.Valencebondtheoryproposes that molecular structures are due to covalent bonds between the atoms and that each bond consists of two overlapping and typically hybridised atomic orbitals.
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This example is from Wikipedia and may be reused under a CC BY-SA license.These examples are from corpora and from sources on the web. Any opinions in the examples do not represent the opinion of the Cambridge Dictionary editors or of Cambridge University Press or its licensors.