Delocalized in a sentence

The electrons in these delocalized orbitals have high mobility when the material is "doped" by oxidation, which removes some of these delocalized electrons.

The nature of metallic bonding The combination of two phenomena gives rise to metallic bonding: delocalization of electrons and the availability of a far larger number of delocalized energy states than of delocalized electrons.

Additionally, because they're delocalized and very fast, kinetic thermal energy conducts extremely quickly through metals with abundant conduction electrons.

Electrical conductivity arises due to the presence of electrons in states that are delocalized (extending through the material), however in order to transport electrons a state must be partially filled, containing an electron only part of the time.

For "conventional" cyclic compounds, aromaticity is conferred by the presence of 4n + 2 delocalized pi electrons, where n is an integer.

In this way, the negative charge on oxygen is delocalized on to the ortho and para carbon atoms.

Kinetic thermal energy adds to this speed and also causes delocalized electrons to travel farther away from the nuclei.

Metallic bonding main In metallic bonding, bonding electrons are delocalized over a lattice of atoms.

Metals take the delocalization principle to its extreme and one could say that a crystal of a metal represents a single molecule over which all conduction electrons are delocalized in all three dimensions.

Silver crystallizes in a face-centered cubic lattice with bulk coordination number 12, where only the single 5s electron is delocalized, similarly to copper and gold.

The electron density within a bond is not assigned to individual atoms, but is instead delocalized between atoms.

The strength of metallic bonds for different metals reaches a maximum around the center of the transition metal series, as those elements have large amounts of delocalized electrons in tight binding type metallic bonds.

The structure is alternatively illustrated as a circle around the inside of the ring to show six electrons floating around in delocalized molecular orbitals the size of the ring itself.

This is seen in, for example, phenol (C 6 H 5 –OH), which is acidic at the hydroxyl (OH), since a charge on this oxygen (alkoxide –O − ) is partially delocalized into the benzene ring.

This situation usually only occurs in relatively narrow (d-)bands, which are poorly delocalized.

Thus, not only do they become delocalized, forming a sea of electrons permeating the lattice, but they are also able to migrate through the lattice when an external electrical field is imposed, leading to electrical conductivity.