electron deficiency

As the most extreme form of electron deficiency one can consider the metallic bond.

In these cations the electron deficiency is spread over the central cyclobutane ring.

By adding other impurities such as gallium, an electron deficiency or hole is created.

The electron deficiency is an important point in distinguishing metallic from more conventional covalent bonding.

The chlorophyll traps make up their electron deficiency by grabbing them from water molecules sited close by.

The relative electron-richness and electron deficiency of the reactants can best be described visually, in a molecular orbital diagram.

Ring strain and electron deficiency in the oxanorbornadiene increase reactivity towards the cycloaddition rate-limiting step.

Electron deficiency occurs when a compound has too few valence electrons for the connections between atoms to be described as covalent bonds.

Unlike carbon, boron cannot form a honeycomb hexagonal framework (like graphene) because of its electron deficiency.

The instability of this molecule results from the high Lewis acidity of the boron atom due to its electron deficiency.

Current flow can be understood in two forms: as negatively charged electrons, and as positively charged electron deficiencies called holes.

Therefore it is rare for bridging alkyl or aryl groups to occur due to the weak electron deficiency of the zinc atom.

Oxygen, more electronegative than carbon, pulls the electrons in the carbon-oxygen bond towards itself, creating an electron deficiency at the carbon atom.

N-type semiconductors have mobile electrons that carry electrical current, while p-type semiconductors have electron deficiencies or holes that act as carriers of electrical current.

Electron deficiency can also be used to describe molecules with highly polarized bonds such as boron trifluoride or silicon tetrafluoride which have a strong tendency to act as Lewis acids.

When zinc lacks electron donating ligands it is unable to obtain coordination saturation, which is a consequence of the large atomic radius and low electron deficiency of zinc.

If the cations have multiple possible oxidation states, then it is possible for cation vacancies to compensate for electron deficiencies on cation sites with higher oxidation numbers, resulting in a non-stoichiometric compound.

The electron deficiency of the carbonyl carbon is the result of the greater electronegativity of the oxygen due to which the bonding electrons to a greater extent are pulled in the direction of the oxygen.

This largely attributed to the electron deficiency of the monomer and the small size of the hydride ligands; which allows dimerisation to take place with a very low energy barrier as there is a negligible increase in inter-ligand repulsion.

The electronegativity of boron (2.04 on the Pauling scale) compared to that of nitrogen (3.04) and also the electron deficiency on the boron atom and the lone pair on nitrogen favor alternative mesomer structures for borazine.

A silicon crystal is different from an insulator because at any temperature above absolute zero, there is a finite probability that an electron in the lattice will be knocked loose from its position, leaving behind an electron deficiency called a "hole".