Electrons in covalent bonds are split equally between the atoms involved in the bond.

Electrons from the metal are used to bond to the ligand, in the process relieving the metal of excess negative charge.

Electrons that are bound to atoms possess a set of stable energy levels, or orbitals, and can undergo transitions between them by absorbing or emitting photons that match the energy differences between the levels.

Electrons can also be emitted from the electrodes of certain metals when light of frequency greater than the threshold frequency falls on it.

Electrons can absorb energy from photons when irradiated, but they usually follow an " all or nothing " principle.

Electrons can only exist in certain energy levels.

Electrons at these states can be easily excited to the conduction band, becoming free electrons, at room temperature.

Electrons in atoms and molecules can change ( make transitions in ) energy levels by emitting or absorbing a photon ( of electromagnetic radiation ) whose energy must be exactly equal to the energy difference between the two levels.

Electrons can also be completely removed from a chemical species such as an atom, molecule, or ion.

Electrons can take on any energy within an unfilled band.

Electrons can gain enough energy to jump to the conduction band by absorbing either a phonon ( heat ) or a photon ( light ).

Electrons can be exchanged between materials on contact ; materials with weakly bound electrons tend to lose them, while materials with sparsely filled outer shells tend to gain them.

* Electrons are fermions, but when they pair up into Cooper pairs they act as bosons, and so can collectively form a coherent state at low temperatures.

Electrons are fermions, and obey the exclusion principle, which means that no two electrons can share a single energy state within an atom ( if spin is ignored ).

Electrons can only reach ( and " illuminate ") a given plate element if both the grid and the plate are at a positive potential with respect to the cathode.

Electrons can move quite freely between energy levels without a high energy cost.

Electrons can transfer from one band to the other by means of carrier generation and recombination processes.

Electrons, within an electron shell around an atom, tend to distribute themselves as far apart from each other, within the given shell, as they can ( due to each one being negatively charged ).

Electrons released on impact escape to the layer of TiO < sub > 2 </ sub > and from there diffuse, through the electrolyte, as the dye can be tuned to the visible spectrum much higher power can be produced.

Electrons in the conduction band can respond to the electric field in the detector, and therefore move to the positive contact that is creating the electrical field.

Electrons can be used in these situations, whereas X-rays cannot, because electrons interact more strongly with atoms than X-rays do.

Electrons also have a long ballistic length at this temperature ; their mean free path can be several micrometres.

Electrons move according to the cross product of the magnetic field and the electron propagation vector, such that, in an infinite uniform field moving electrons take a circular motion at a constant radius dependent upon electron velocity and field strength according to the following equation, which can be derived from circular motion:

Electrons and positrons can be discriminated from other charged particles using the emission of transition radiation, X-rays emitted when the particles cross many layers of thin materials.

Electrons excited to the conduction band also leave behind electron holes, i. e. unoccupied states in the valence band.

Electrons form notional shells around the nucleus.

Electrons that populate a shell are said to be in a bound state.

# Electrons jump between orbitals in a particle-like fashion.

These he interpreted as " negative-energy electrons " and attempted to identify them with protons in his 1930 paper A Theory of Electrons and Protons However, these " negative-energy electrons " turned out to be positrons, and not protons.

Electrons in an s orbital benefit from closer proximity to the positively charged atom nucleus, and are therefore lower in energy.

Electrons ( the other major component of the atom ) are leptons.

Electrons are the charge carriers in metals and they follow an erratic path, bouncing from atom to atom, but generally drifting in the opposite direction of the electric field.

Electrons were first discovered as the constituents of cathode rays.

Electrons are extracted from metal electrodes either by heating the electrode, causing thermionic emission, or by applying a strong electric field and causing field electron emission.

Electrons which diffuse from the cathode into the P-doped layer, or anode, become what is termed " minority carriers " and tend to recombine there with the majority carriers, which are holes, on a timescale characteristic of the material which is the p-type minority carrier lifetime.

Electrons are responsible for emission of most EMR because they have low mass, and therefore are easily accelerated by a variety of mechanisms.

Electrons are at the heart of cathode ray tubes, which have been used extensively as display devices in laboratory instruments, computer monitors and television sets.

Electrons are bound by electromagnetic wave mechanics into orbitals around atomic nuclei to form atoms, which are the building blocks of molecules.

: Electrons are transferred from iron reducing oxygen in the atmosphere into water on the cathode, which is placed in another region of the metal.

Electrons flow in the external circuit.

Electrons flow from the source terminal towards the drain terminal if influenced by an applied voltage.

Electrons are drawn from the anode to the cathode through an external circuit, producing direct current electricity.

Electrons in this state are 45 % likely to be found within the solid body shown.

His most noted publication was the famous 1919 article " The Arrangement of Electrons in Atoms and Molecules " in which, building on Gilbert N. Lewis's cubical atom theory and Walther Kossel's chemical bonding theory, he outlined his " concentric theory of atomic structure ".

Electrons are particulate radiation and, hence, have cross section many times larger than photons, so that they do not penetrate the product beyond a few inches, depending on product density.

Electrons that belong to different molecules start " fleeing " and avoiding each other at the short intermolecular distances, which is frequently described as formation of " instantaneous dipoles " that attract each other.

Electrons and how they interact with electromagnetic fields are important in our understanding of chemistry and physics.

Electrons emitted from the filament move several times in back and forth movements around the grid before finally entering the grid.