VIDEOS 1 TO 50

Visualizing Natural Bond Orbitals

Published: 2013/03/05

Channel: ccclabmit

Avogadro with Gaussian + NBO

Published: 2015/05/06

Channel: IaNiusha

Jmol Viewer and display of NBOs in web browsers

Published: 2012/11/18

Channel: Org Med Chem

Multiple NBOS With GaussView and WebMO

Published: 2016/04/12

Channel: John Keller

Comparing an MO with the Corresponding NBO Using WebMO

Published: 2016/04/10

Channel: John Keller

03.03 Localized Molecular Orbitals and NBO Theory

Published: 2017/11/16

Channel: Michael Evans

03.04 NBO Analysis of Methane

Published: 2017/11/16

Channel: Michael Evans

03.05 Shapes of Natural Bond Orbitals

Published: 2017/11/16

Channel: Michael Evans

KNIME UGM 2013 Bernd Wiswedel talk- Part 3 NBO

Published: 2013/03/22

Channel: KNIMETV

Discovering Chemistry With Natural Bond Orbitals

Published: 2016/10/15

Channel: Verbeke

Download Valency and Bonding A Natural Bond Orbital Donor Acceptor Perspective PDF

Published: 2017/02/07

Channel: N. Octari

Books of Discovering Chemistry With Natural Bond Orbitals 2

Published: 2015/09/23

Channel: Katherine Morris

Download Discovering Chemistry With Natural Bond Orbitals PDF eBook

Published: 2016/07/02

Channel: Janet De Morgan J

(Redirected from Natural Bond Orbital)

In quantum chemistry, a **natural bond orbital** or **NBO** is a calculated *bonding orbital* with maximum electron density. The NBOs are one of a sequence of natural localized orbital sets that include "natural atomic orbitals" (NAO), "natural hybrid orbitals" (NHO), "natural bonding orbitals" (NBO) and "natural (semi-)localized molecular orbitals" (NLMO). These natural localized sets are intermediate between basis atomic orbitals (AO) and molecular orbitals (MO):

- Atomic orbital → NAO → NHO →
**NBO**→ NLMO → Molecular orbital

Natural (localized) orbitals are used in computational chemistry to calculate the distribution of electron density in atoms and in bonds between atoms. They have the "maximum-occupancy character" in localized 1-center and 2-center regions of the molecule. Natural bond orbitals (NBOs) include the highest possible percentage of the electron density, ideally close to 2.000, providing the most accurate possible “natural Lewis structure” of ψ. A high percentage of electron density (denoted %-ρ_{L}), often found to be >99% for common organic molecules, correspond with an accurate natural Lewis structure.

The concept of *natural orbitals* was first introduced by Per-Olov Löwdin in 1955, to describe the unique set of orthonormal 1-electron functions that are intrinsic to the *N*-electron wavefunction.^{[1]}

Each bonding NBO σ_{AB} (the donor) can be written in terms of two directed valence hybrids (NHOs) h_{A}, h_{B} on atoms A and B, with corresponding polarization coefficients *c*_{A}, *c*_{B}:

- σ
_{AB}=*c*_{A}*h*_{Α}+*c*_{B}*h*_{B}

The bonds vary smoothly from covalent (*c*_{A} = *c*_{B}) to ionic (*c*_{A} >> *c*_{B}) limit.

Each valence bonding NBO σ must be paired with a corresponding valence antibonding NBO σ* (the acceptor) to complete the span of the valence space:

- σ
_{AB}* =*c*_{A}*h*_{Α}−*c*_{B}*h*_{B}

The bonding NBOs are of the "Lewis orbital"-type (occupation numbers near 2); antibonding NBOs are of the "non-Lewis orbital"-type (occupation numbers near 0). In an idealized Lewis structure, full Lewis orbitals (two electrons) are complemented by formally empty non-Lewis orbitals. Weak occupancies of the valence antibonds signal irreducible departures from an idealized localized Lewis structure, which means true "delocalization effects".^{[1]}

With a computer program that can calculate NBOs, optimal Lewis structures can be found. An optimal Lewis structure can be defined as that one with the maximum amount of electronic charge in Lewis orbitals (Lewis charge). A low amount of electronic charge in Lewis orbitals indicates strong effects of electron delocalization.

In resonance structures, major and minor contributing structures may exist. For amides, for example, NBO calculations show that the structure with a carbonyl double bond is the dominant Lewis structure. However, in NBO calculations, "covalent-ionic resonance" is not needed due to the inclusion of bond-polarity effects in the resonance structures.^{[2]} This is similar to other modern valence bond theory methods.

- ^
^{a}^{b}Weinhold, Frank; Landis, Clark R. (2001). "Natural Bond Orbitals and Extensions of Localized Bonding Concepts" (PDF).*Chemistry Education Research and Practice*.**2**(2): 91–104. doi:10.1039/B1RP90011K. **^**Weinhold, Frank; Landis, Clark R. (2012).*Discovering Chemistry With Natural Bond Orbitals*. New Jersey: John Wiley & Sons. pp. 132–133. ISBN 978-1-118-22916-3.

- Homepage for the NBO computer program: http://nbo6.chem.wisc.edu/
- IUPAC Gold Book definition: natural bond orbital (NBO)
- Free, open-source implementation for Atomic orbital → NAO transformation and Natural Population Analysis methods: JANPA package

None of the audio/visual content is hosted on this site. All media is embedded from other sites such as GoogleVideo, Wikipedia, YouTube etc. Therefore, this site has no control over the copyright issues of the streaming media.

All issues concerning copyright violations should be aimed at the sites hosting the material. This site does not host any of the streaming media and the owner has not uploaded any of the material to the video hosting servers. Anyone can find the same content on Google Video or YouTube by themselves.

The owner of this site cannot know which documentaries are in public domain, which has been uploaded to e.g. YouTube by the owner and which has been uploaded without permission. The copyright owner must contact the source if he wants his material off the Internet completely.

Wikipedia content is licensed under the GFDL and (CC) license