The characteristic that allows some metals to be better conductors of electricity is that they have 'free electrons'. Free Electrons simply means that there is a weaker bond between the electrons on the outer valence shell to the nucleus of the atom, than other atoms. This weak bond allows electrons in metals to become more easily excited (when mechanical means of generation occurs), where the electrons are able to transfer from one atom to another.
I imagine this is what the question is asking. Basically, electricity is inherent in the material. Metals have weak bonds in their outer valence electron shell.
A: In metals, the atoms move freely, allowing heat to travel faster. :)
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plasma
The wavelength that will cause electrons to travel faster when hitting uranium is 100nm. If the wavelength was any lower, electrons would not move as fast.
Flowing electrons makes electricity (they flow from negative to positive. ). You need a circuit or a path for the electrons to move through, a power source like a battery or a generator, and something to use the electricity, like a light bulb...
Good Insulator are those substance which has almost no free electrons to move freely and thus, cannot conduct electricity. When EMF (Electro motive force) is applied along the length of the insulator, high resistance of the insulator causes no motion of the electrons due to which the electrons cannot flow.
They move throught the matel
Electrons move freely among many metal nuclei
metal atoms being so close to one another that their outermost level overlap. Cause of the overlapping metallic bonds extend throughout the metal in all direction, so valence electrons can move throughout the metal.
During this type of reaction, the electrons would move from the metal to the non-metal. The transfer of electrons allows both material to maintain a full outer valence.
The number of valence electrons increases.
In a metal the valence electrons delocalize into the conduction band, becoming an "electron gas" that fills the metal's bulk volume.In covalent bonds the valence electrons are shared between local pairs of atoms.In ionic bonds the valence electrons leave the "metal" and move to the "nonmetal" creating a pair of separate oppositely charged ions.In resonance bonds the valence electrons oscillate between being shared between two nearby local pairs of atoms.etc.To summarize in metals the valence electrons become delocalized, in other bonds the valence electrons stay local.
Every atom in Column 2 of a wide form periodic table has two valence electrons.
When a metal reacts with a non-metal, the electrons move from the metal to the non-metal. This is because the metal can achieve valence when it loses the electrons in its outer shell. The non-metal can also achieve full valence by gaining the electron in its outer shell.
metal atoms being so close to one another that their outermost level overlap. Cause of the overlapping metallic bonds extend throughout the metal in all direction, so valence electrons can move throughout the metal.
Atoms being so close to one-another that their outermost energy overlap
Valence electrons in a metallic bond are delocalized and can move freely within the metal atoms. This gives metals their malleability and luster.
metal conducts electricity because it allows electrons to move freely as well as it has free electrons, unlike insulators(non-metals) which do not have free electrons. When the electrons are allowed to move freely in a substance, it is a good conductor and allows electric charge to flow.