metallic bonding

This is due to the effects of metallic bonding on small scales.

This process does not affect the communal metallic bonding very much.

Interstitial hydrides, which may be described as having metallic bonding.

Elements in this situation usually adopt metallic bonding.

Otherwise, metallic bonding can be very strong, even in molten metals, such as Gallium.

The electrical field is usually able to excite an elastic response from the electrons involved in the metallic bonding.

In metals, electrons are shared amongst the whole crystal in metallic bonding.

Molten gallium is therefore a very nonvolatile liquid thanks to its strong metallic bonding.

The metallic bonding in complicated compounds does not necessarily involve all constituent elements equally.

A special metallic bonding glue available from Eastman-Kodak will form a permanent bond in only 45 seconds.

The s-block elements have only metallic bonding.

Not all metals exhibit metallic bonding.

Thus metallic bonding is an extremely delocalized communal form of covalent bonding.

The goal of in-situ bonding is to create a metallic bonding between the foam core and face sheets.

Given high enough cooling rates and appropriate alloy composition, metallic bonding can occur even in glasses with an amorphous structure.

Metallic bonding bridges fairly easily from crystals of one compound to crystals of another.

Metallic bonding dissolves in liquid metal solvents.

There are a variety of known chemical bonding interactions including covalent, ionic, and metallic bonding among others.

As powerful as the concept of the band structure proved to be in the description of metallic bonding, it does have a drawback.

Metallic solids are held together by a high density of shared, delocalized electrons, known as "metallic bonding".

These include ionic bonding, covalent bonding, and metallic bonding.

Ionic bonds form between X and Z sites, but braggite also tends to exhibit metallic bonding characteristics.

Metallic bonding refers to the specific bonding between positive metal ions and surrounding valence electron clouds.

Thus, the transition from localized unpaired electrons to itinerant ones partaking in metallic bonding became more comprehensible.

This means that inside the metal one can generally not distinguish molecules, so that the metallic bonding is neither intra- nor intermolecular.