Chemical bonding

lasting attraction between atoms that enables the formation of chemical compounds

chemical bond that involves the sharing of electron pairs between atoms

chemical bond involving electron transfer

thumb|alt=A water molecule is put into a see-through egg shape, which is color-coded by electrostatic potential. A concentration of red is near the top of the shape, where the oxygen atom is, and gradually shifts through yellow, green, and then to blue near the lower-right and lower-left corners of the shape where the hydrogen atoms are.|upright=1.5|right|Electrostatic potential map of a water molecule, where the oxygen atom has a more negative charge (red) than the positive (blue) hydrogen atoms Electronegativity, symbolized as χ, is the tendency for an atom of a given chemical element to att

measure of an element's combining capacity with other atoms when it forms chemical compounds or molecules

quantum mechanical principle that two identical fermions cannot occupy the same quantum state simultaneously

atom, molecule, or ion that has an unpaired valence electron; typically highly reactive

form of association between an electronegative atom and a hydrogen atom attached to a second, relatively electronegative atom

mathematical function describing the location and behavior of an electron within an atom

principal energy levels in atomic physics

type of chemical bond in metals, sharing conduction electrons among a lattice of cations

outer shell electron that is associated with an atom, and that can participate in the formation of a chemical bond if the outer shell is not closed

measure of the size of an atom that forms part of one covalent bond

covalent chemical bond linking two consecutive amino acid monomers along a peptide or protein chain

chemical rule of thumb

mixing (superposition) of atomic orbitals in chemistry

forces of attraction or repulsion which act between neighboring particles

thumb|200px|Cobalt complex cobalt tetracarbonyl hydride|HCo(CO)4 with five ligands

amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion

chemical bond involving four bonding electrons; has one sigma plus one pi bond

chemistry term; way of describing bonding in molecules or ions by the combination of several contributing structures into a resonance hybrid in valence bond theory

wave-like behavior of an electron in a molecule

chemical bond involving six bonding electrons; one sigma plus two pi bonds

diagrams for the bonding between atoms of a molecule and lone pairs of electrons

covalent bond in a coordination complex in which the shared electrons are donated by one of the atoms and also known as dative bond

strongest type of covalent chemical bond; formed by head-on overlapping between atomic orbitals.

method for describing the electronic structure of molecules using quantum mechanics

type of covalent chemical bond

number of atoms, molecules or ions bonded to in a molecule or crystal

one of two foundational theories of quantum chemistry

two electrons that occupy the same orbital but have opposite spins

covalent bond joining a sugar molecule to another group

substance that forms a complex with a biomolecule

pair of valence electrons that are not shared with another atom; concept used in valence shell electron pair repulsion theory (VSEPR theory) which explains the shapes of molecules

principle of atomic physics

electron in a molecule not associated with a single atom or covalent bond

chemical bond between two atoms involving two valence electrons (atoms share one pair of electrons where the bond forms, therefore, a single bond is a type of covalent bond); usually a sigma bond

type of force acting between atoms and molecules

mathematical model that approximates the interaction between a pair of neutral atoms or molecules

mechanism of spontaneous symmetry breaking in molecular and solid-state systems

type of chemical bond

local change in the electron density of a molecule due to electron-withdrawing or electron-donating groups elsewhere in the molecule, resulting in a permanent dipole in a bond

model that describes the breaking of degeneracies of electron orbital states, usually d or f orbitals, due to a static electric field produced by a surrounding charge distribution (anion neighbors)

type of chemical bond

aggregation of non-polar molecules in aqueous solutions

type of molecular orbital (MO) that weakens the bond between two atoms and helps to raise the energy of the molecule relative to the separated atom; is normally higher in energy than bonding molecular orbital

covalent bond between two carbon atoms

number of valence electrons of an atom in isolation

type of chemical bond between two atoms involving eight electrons

technique in quantum chemistry

Net positive charge experienced by an electron in a polyelectronic atom

decrease of ionic radii across the lanthanide series

rule used primarily for predicting formulae for stable metal complexes

instability in molecules with bonds at unnatural angles

region on a protein or piece of DNA or RNA to which ligands may form a chemical interaction

covalent bond between carbon and hydrogen

electron-deficient chemical bond where three atoms share one of two electrons

a covalent bond involving 12 bonding electrons

attractive, noncovalent interactions between aromatic rings

molecular orbital theory applied to transition metal complexes