Chemical bonding Chemical bonding A 3-center-2-electron bond is an electron deficient chemical bond where three atoms share two electrons. The combination of three atomic orbitals form one bonding, one non-bonding, and one anti-bonding molecular orbital. Since the two electrons go into the bonding orbital this constitutes a chemical bond between the three atoms. The resulting molecular orbital, when visualised in 3D, looks like a banana, hence it is often called a banana bond. ...more on Wikipedia about "3-center-2-electron bond"
3-center-4-electron bond is a term for the axial bonds on a trigonal bypyramidal or octahedral molecule such as Phosphorous V Chloride. In this molecule, Phosphorous has an expanded octet, which is a violation of molecular orbital theory. So, the central atom shares a pi bond between the two atoms, creating resonant Lewis structures with ionic-covalent bonding. ...more on Wikipedia about "3-center-4-electron bond"
Antibonding (or anti-bonding) is a type of chemical bonding. An antibonding orbital is a form of molecular orbital (MO) that is located outside the region of two distinct nuclei. The overlap of the constituent atomic orbitals is said to be 'out of phase' and as such the electrons present in each antibonding orbital are repulsive and act to destabilize the molecule as a whole. ...more on Wikipedia about "Antibonding"
In supramolecular chemistry, an aromatic interaction (or π-π interaction) is a noncovalent interaction between organic compounds containing aromatic moieties. π-π interactions are caused by intermolecular overlapping of p- orbitals in π-conjugated systems, so they become stronger as the number of π-electrons increases. Other noncovalent interactions include hydrogen bonds, van der Waals forces, charge-transfer interactions, and dipole-dipole interactions. ...more on Wikipedia about "Aromatic interaction"
Atomic orbitals are the quantum states of the individual electrons in the electron cloud around a single atom. Classically, the atomic orbitals can be thought of as similar to the orbits of the planets around the Sun. However, it is important to note that the atomic orbitals cannot actually be described classically. In fact, explaining the behaviour of the electrons that orbit an atom was one of the driving forces behind quantum mechanics. In quantum mechanics, the atomic orbitals are the quantum states that electrons surrounding an atom may exist in. These can be described as a wave function over space, as shown in the diagram on the right, by the n, l, and m quantum numbers of the orbital, or by the names of the orbitals, as used in electron configurations. ...more on Wikipedia about "Atomic orbital"
Banana bonds or bent bonds are a special type of chemical bonding in which the ordinary hybridization state of two atoms making up a chemical bond are modified with increased or decreased s-orbital character in order to accommodate a particular molecular geometry. Bent bonds are found in strained organic compounds such as cyclopropane, oxirane and aziridine. In these compounds it is not possible for the carbon atoms to assume the 109.5° bond angles with standard sp3 hybridization. Increasing the p character makes it possible to reduce the bond angles to 60°. At the same time the carbon to hydrogen bonds gain more s-character and shorten. In cyclopropane the maximum electron density between two carbon atoms does not correspond to the internuclear axis hence the name bent bond. In cyclopropane the interorbital angle is 104°. ...more on Wikipedia about "Banana bond"
A chemical bond is the physical phenomenon of chemical substances being held together by attraction of atoms to each other through electrons or by electrostatic forces. Classically, strong chemical bonds are found in molecules, crystals or in solid metal and they organize the atoms in ordered structures. Weak chemical bonds are classically explained to be effects of polarity, or the lack of it, of strong bonds. ...more on Wikipedia about "Chemical bond"
Chemical polarity refers how polar a chemical bond is. To find the polarity, take the difference in the electronegativity. If the result is below 1.7 and above 0.5, the bond is polar. Ionic bonds are considered to be extremely polar. A commonly recognised polar molecule is Water (H2O). ...more on Wikipedia about "Chemical polarity"
Cohesion or cohesive attraction or cohesive force in chemistry is the intermolecular attraction between like- molecules. Cohesion explains phenomena such as surface tension. Capillary action for example described in the Cohesion-tension theory related to botany is considered a mix of cohesion and adhesion. Cohesion is produced by the intermolecular forces. ...more on Wikipedia about "Cohesion (chemistry)"
A coordinate covalent bond (also known as dative covalent bond) is a special type of covalent bond in which the shared electrons come from one of the atoms only. Once the bond has been formed, its strength is no different from that of a covalent bond. ...more on Wikipedia about "Coordinate covalent bond"
In chemistry, the coordination number is the sum of the total number of neighbors of a central atom in a chemical compound and the number of lone pairs on it. In methane the coordination number for the carbon atom is 4. In inorganic chemistry the number of sigma bonds between ligand and the central atom count but not the number of pi bonds. ...more on Wikipedia about "Coordination number"
Covalent bonding is an intramolecular form of chemical bonding characterized by the sharing of one or more pairs of electrons between two species, producing a mutual attraction that holds the resultant molecule together. Atoms tend to share electrons in such a way that their outer electron shells are filled. Such bonds are always stronger than the intermolecular hydrogen bond and similar in strength to or stronger than the ionic bond. ...more on Wikipedia about "Covalent bond"
Covalent radius in chemistry corresponds to half of the distance between two identical atomic nuclei, bound by a covalent bond. It is expressed in terms of picometres (pm) or angstroms (Å). ...more on Wikipedia about "Covalent radius"
Cross-conjugation is a special type of conjugation in a molecule, when in a set of three Pi bonds only two pi-bonds interact with each other by conjugation, the third one is excluded from interaction. In classical terms it means that the strict alternation of single and double bonds --CH=CH–CH=CH–CH-- (i.e., conjugated) is interrupted by two consecutive single bonds at each cross-conjugated point in the cross-conjugated pathway: --CH=CH–C(=CH)–CH=CH--. Examples of cross-conjugation can be found in molecules such as benzophenone, divinylether and Dendralenes. The type of conjugation has an impact on reactivity and molecular electronic transitions. ...more on Wikipedia about "Cross-conjugation"
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Crystal field theory is used to describe the electronic structure of transition metal complexes. It is successful in describing the magnetic properties, colors, hydration enthalpies and spinel structures of transition metal complexes, but it cannot provide an adequate description of bonding. Crystal field theory was developed by the physicists Hans Bethe and John Hasbrouck van Vleck. It was combined with molecular orbital theory to form ligand field theory, which delivers insight into the process of chemical bonding in transition metal complexes. ...more on Wikipedia about "Crystal field theory"
In chemistry, delocalized electrons are electrons in a molecule that do not belong to a single atom or a covalent bond. Delocalized electrons are part of a pi electron system that extends over several adjacent atoms. Delocalized electrons can be found in conjugated systems of double bonds and in aromatic systems. A case of delocalized electrons occurs also in solid metals, where the d-subshell interferes with the above s-subshell, and contributes to the properties of a metal. ...more on Wikipedia about "Delocalized electron"
Delta bonds are bonds which contain two nodal planes, whose intersection is a line containing the segment joining the two bonded species. Delta bonds are so named because their orbital symmetry is the same as d-orbitals (except for 2z^2-x^2-y^2, which is sigma-like, and xy, xz which are pi-like) when looking down the bond axis. ...more on Wikipedia about "Delta bond"
In chemistry, a dihydrogen bond is a kind of hydrogen bond, an interaction between a metal hydride bond and an OH or NH group or another proton donor. A transition metal complex including this type of bonding was first synthesized by G.J. Kubas et al. in 1984. ...more on Wikipedia about "Dihydrogen bond"
In chemistry a donor number or DN is a qualitative measure of lewis basicity. A donor number is defined as the negative enthalpy value for the 1:1 adduct formation between ...more on Wikipedia about "Donor number"
The effective nuclear charge is the net positive charge experienced by an electron in a multielectron atom. The term "effective" is used because the shielding effect of negative electrons prevents higher orbital electrons from experiencing the full nuclear charge. ...more on Wikipedia about "Effective nuclear charge"
A compound that is electron deficient has too few valence electrons for the connections between atoms to be described as covalent bonds. Electron deficient bonds are often better described as 3-center-2-electron bonds. Examples of compounds that are electron deficient are the boranes, including diborane. ...more on Wikipedia about "Electron deficient"
In chemistry, a formal charge (FC) on an atom in a molecule is defined as: ...more on Wikipedia about "Formal charge"
In chemistry, a glycosidic bond is a certain type of chemical bond that joins a sugar molecule to another molecule. ...more on Wikipedia about "Glycosidic bond"
In chemistry, a hydrogen bond is a type of attractive intermolecular force that exists between two partial electric charges of opposite polarity. Although stronger than most other intermolecular forces, the typical hydrogen bond is much weaker than both the ionic bond and the covalent bond. Within macromolecules such as proteins and nucleic acids, it can exist between two parts of the same molecule, and figures as an important constraint on such molecules' overall shape. ...more on Wikipedia about "Hydrogen bond"
In chemistry a hydrogen donor is any chemical compound that has a hydrogen atom available for chemical interaction. Hydrogen donor is synonimous with a active hydrogen compound. A wide range of compounds fall within this category, from simple mineral acids to ordinary acids, carboxylic acids, amines, sulfonic acids to less obvious ones like carbon acids such as ethyl acetoacetate or Meldrum's acid. The pKa is a measure of the quality of a hydrogen donor. ...more on Wikipedia about "Hydrogen donor" If you like you could tell us your opinion about www.shortopedia.com
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