Jove
Visualize
Contact Us
JoVE
x logofacebook logolinkedin logoyoutube logo
ABOUT JoVE
OverviewLeadershipBlogJoVE Help Center
AUTHORS
Publishing ProcessEditorial BoardScope & PoliciesPeer ReviewFAQSubmit
LIBRARIANS
TestimonialsSubscriptionsAccessResourcesLibrary Advisory BoardFAQ
RESEARCH
JoVE JournalMethods CollectionsJoVE Encyclopedia of ExperimentsArchive
EDUCATION
JoVE CoreJoVE BusinessJoVE Science EducationJoVE Lab ManualFaculty Resource CenterFaculty Site
Terms & Conditions of Use
Privacy Policy
Policies

Related Concept Videos

MO Theory and Covalent Bonding02:40

MO Theory and Covalent Bonding

The molecular orbital theory describes the distribution of electrons in molecules in a manner similar to the distribution of electrons in atomic orbitals. The region of space in which a valence electron in a molecule is likely to be found is called a molecular orbital. Mathematically, the linear combination of atomic orbitals (LCAO) generates molecular orbitals. Combinations of in-phase atomic orbital wave functions result in regions with a high probability of electron density, while...
Molecular Orbital Theory I02:35

Molecular Orbital Theory I

Overview of Molecular Orbital Theory
Molecular Orbital Theory II03:51

Molecular Orbital Theory II

Molecular Orbital Energy Diagrams
Valence Bond Theory02:45

Valence Bond Theory

Overview of Valence Bond Theory
Valence Bond Theory02:42

Valence Bond Theory

Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
Valence Bond Theory and Hybridized Orbitals02:38

Valence Bond Theory and Hybridized Orbitals

According to valence bond theory, a covalent bond results when: (1) an orbital on one atom overlaps an orbital on a second atom, and (2) the single electrons in each orbital combine to form an electron pair. The strength of a covalent bond depends on the extent of overlap of the orbitals involved. Maximum overlap is possible when the orbitals overlap on a direct line between the two nuclei.
A σ bond (single bond in a Lewis structure) is a covalent bond in which the electron density is...

You might also read

Related Articles

Articles linked to this work by shared authors, journal, and citation graph.

Sort by
Same author

1-Fluoropropane. Torsional Potential Surface.

Journal of chemical theory and computation·2015
Same author

Single Electron Transfer and SN2 Reactions: The Importance of Ionization Potential of Nucleophiles.

Journal of chemical theory and computation·2015
Same author

Radical cations and triplet states of 1,2-disubstituted cyclopropanes: comparison of potential surfaces.

Photochemical & photobiological sciences : Official journal of the European Photochemistry Association and the European Society for Photobiology·2012
Same author

Properties of the Nucleic-acid Bases in Free and Watson-Crick Hydrogen-bonded States: Computational Insights into the Sequence-dependent Features of Double-helical DNA.

Biophysical reviews·2011
Same author

Innermolecular reactions of fluorophenylcarbene inside a hemicarcerand.

Organic letters·2009
Same author

Competing gas-phase substitution and elimination reactions of gemini surfactants with anionic counterions by mass spectrometry. Density functional theory correlations with their bolaform halide salt models.

The journal of physical chemistry. B·2008

Related Experiment Video

Updated: Jul 18, 2026

Analyzing Melts and Fluids from Ab Initio Molecular Dynamics Simulations with the UMD Package
06:37

Analyzing Melts and Fluids from Ab Initio Molecular Dynamics Simulations with the UMD Package

Published on: September 17, 2021

Diffuse functions in natural bond orbital analysis.

Lionel Goodman1, Ronald R Sauers

  • 1Department of Chemistry and Chemical Biology, Wright and Rieman Laboratories, Rutgers, the State University of New Jersey, New Brunswick, New Jersey 08903, USA. goodman@rutchem.rutgers.edu

Journal of Computational Chemistry
|December 7, 2006
PubMed
Summary

Diffuse function augmentation significantly alters natural bond orbital (NBO) analysis, especially with Pople basis sets. This can lead to nonphysical results for larger molecules, highlighting the importance of basis set selection in computational chemistry.

More Related Videos

Diffuse Reflectance Infrared Spectroscopic Identification of Dispersant/Particle Bonding Mechanisms in Functional Inks
10:31

Diffuse Reflectance Infrared Spectroscopic Identification of Dispersant/Particle Bonding Mechanisms in Functional Inks

Published on: May 8, 2015

Controlled Synthesis and Fluorescence Tracking of Highly Uniform Poly(N-isopropylacrylamide) Microgels
11:34

Controlled Synthesis and Fluorescence Tracking of Highly Uniform Poly(N-isopropylacrylamide) Microgels

Published on: September 8, 2016

Related Experiment Videos

Last Updated: Jul 18, 2026

Analyzing Melts and Fluids from Ab Initio Molecular Dynamics Simulations with the UMD Package
06:37

Analyzing Melts and Fluids from Ab Initio Molecular Dynamics Simulations with the UMD Package

Published on: September 17, 2021

Diffuse Reflectance Infrared Spectroscopic Identification of Dispersant/Particle Bonding Mechanisms in Functional Inks
10:31

Diffuse Reflectance Infrared Spectroscopic Identification of Dispersant/Particle Bonding Mechanisms in Functional Inks

Published on: May 8, 2015

Controlled Synthesis and Fluorescence Tracking of Highly Uniform Poly(N-isopropylacrylamide) Microgels
11:34

Controlled Synthesis and Fluorescence Tracking of Highly Uniform Poly(N-isopropylacrylamide) Microgels

Published on: September 8, 2016

Area of Science:

  • Computational Chemistry
  • Quantum Chemistry
  • Theoretical Chemistry

Background:

  • Natural Bond Orbital (NBO) analysis is crucial for understanding chemical bonding.
  • Basis set choice significantly influences computational chemistry results.
  • Diffuse function augmentation is used to improve descriptions of electron density.

Purpose of the Study:

  • To investigate the impact of diffuse function augmentation on NBO analysis.
  • To compare the effects of augmentation on different basis sets (Pople vs. Dunning).
  • To identify conditions under which augmentation may lead to erroneous results.

Main Methods:

  • Utilized Pople basis sets (6-311G and 6-31G) with RHF and B3LYP.
  • Employed diffuse function augmentation.
  • Performed NBO analysis.
  • Compared results with Dunning-type correlation consistent orbitals.

Main Results:

  • Diffuse augmentation of 6-311G Pople basis sets strongly impacts NBO analysis.
  • Augmentation introduces anomalies, particularly for molecules with >= 4 heavy atoms, leading to nonphysical results.
  • Lesser anomalies were observed for 6-31G basis sets.
  • NBO analysis with Dunning basis sets showed weaker basis set dependence.

Conclusions:

  • Diffuse function augmentation of Pople basis sets can compromise the validity of NBO analysis.
  • The choice of basis set and augmentation strategy is critical for accurate chemical interpretations.
  • Dunning-type basis sets offer greater robustness against augmentation artifacts in NBO analysis.