Related Concept Videos
01:27¹H NMR: Long-Range Coupling
The coupling interactions of nuclei across four or more bonds are usually weak, with J values less than 1 Hz. While these are usually not observed in spectra, the presence of multiple bonds along the coupling pathway can result in observable long-range coupling.
In alkenes, spin information is communicated via σ–π overlap, as seen in allylic (four-bond) and homoallylic (five-bond) couplings. These coupling interactions are stronger when the σ bond is parallel to the alkene π orbitals.
In alkenes, spin information is communicated via σ–π overlap, as seen in allylic (four-bond) and homoallylic (five-bond) couplings. These coupling interactions are stronger when the σ bond is parallel to the alkene π orbitals.
01:08Covalent Bonds
Overview
When two atoms share electrons to complete their valence shells, they create a covalent bond. An atom's electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally, creating polar bonds.
When two atoms share electrons to complete their valence shells, they create a covalent bond. An atom's electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally, creating polar bonds.
01:29Covalent Bonds
When two atoms share electrons to complete their valence shells they create a covalent bond. An atom’s electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally, creating polar bonds.A Covalent...
02:40Chemical Bonds
Atoms participate in a chemical bond formation to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest to it in atomic number. Ionic, covalent, and metallic bonds are some of the important types of chemical bonds. Bond energy and bond length determine the strength of a chemical bond.
Types of Chemical Bonds
An ionic bond is formed due to electrostatic attraction between cations and anions. Often, the ions are formed by the transfer of electrons from...
02:45Valence Bond Theory
Overview of Valence Bond Theory
02:42Valence 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...
You might also read
Related Articles
Articles linked to this work by shared authors, journal, and citation graph.
Sort by
Same author
Polar covalent bonds: an AIM analysis of S,O bonds.
The journal of physical chemistry. A·2009
Related Experiment Video
Updated: Jul 20, 2026
10:51
The Synthesis, Characterization and Reactivity of a Series of Ruthenium N-triphosPh Complexes
Published on: April 10, 2015
Characteristics of multiple N,O bonds.
1National University of Lesotho, PO ROMA 180, Lesotho. i.love@nul.ls
The Journal of Physical Chemistry. A
|September 1, 2006
Summary
Nitrogen-oxygen bonds often exhibit higher bond orders than expected, suggesting nitrogen can be pentavalent and exceed the octet rule in simple molecules. This analysis uses atoms in molecules theory to study electron distribution.
Area of Science:
- Quantum Chemistry
- Chemical Bonding
- Computational Chemistry
Background:
- Understanding electron distribution in chemical bonds is crucial for predicting molecular properties.
- The octet rule is a fundamental concept in chemistry, but exceptions exist.
Purpose of the Study:
- To analyze the electron distribution in nitrogen-oxygen (N,O) bonds using advanced theoretical methods.
- To investigate the bond orders and valency of nitrogen in various simple molecules.
Main Methods:
- Bader's atoms in molecules (AIM) theory was employed.
- Analysis of electron density and its Laplacian.
- Calculation of bond orders and correlation with bond lengths.
Main Results:
- Electron density derived parameters show strong correlation with bond length and bond order.
- A significant number of N,O bonds exhibit bond orders near or exceeding 2.
- Nitrogen atoms frequently display pentavalency, deviating from the classical octet rule.
Conclusions:
- Nitrogen's hypervalence is demonstrated in many simple N,O-containing molecules.
- The classical octet rule is not universally obeyed by nitrogen.
- Atoms in molecules theory provides valuable insights into chemical bonding and electron distribution.