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Why are metallic compounds good conductors?

Md Ariful Islam

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Md Ariful Islam

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$"Metallic bonding"$ consists of an array of close-packed metal atoms, which each contribute one or two or more electrons to the overall metallic lattice. And the result is the familiar description of metals: $"positive ions in a sea of electrons"$.

The formally positively charged metal nuclei can move with respect to each other WITHOUT disrupting the metallic bond. And this gives rise to typical metallic properties: $"malleability"$, the ability to beaten into a sheet (cf. Latin $"malleus"="hammer"$); and $"ductility"$, the ability to be drawn into a wire.

But the free electrons are delocalized across the entire lattice, and thus they give rise to two other bulk properties: the capacity to conduct electrical charge and heat. Most metals are excellent conductors. The free electrons are competent to conduct both charge and heat....

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Why metals are good conductors of electricity?

Metals are excellent conductors because the atoms in a metal form a matrix through which their outer electrons can move freely. Instead of orbiting their respective metal atoms, they form...

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Are metals or nonmetals better conductors of electric current? Why?

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Metals are good conductors because they have many free electrons. How are these free electrons obtained?

Take Sodium for an example. Each sodium because of its low electronegativity wants to lose or donate one electron to the other sodium atoms in the metallic matrix. By losing...

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What are metallic compounds and why are they conductive?

The reason as to why metallic posses these properties is because the electrons do not stay in their assigned orbitals, they become delocalised and move all over the place....

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What properties do metallic compounds have?

In General: Very High melting and boiling points Very Good Conductors of heat and electricity Malleable (can be made into different shapes without breaking) Ductile (can be molded...

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Which have higher melting points ionic or metallic compounds?

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What do compounds that are ductile and excellent conductors of electricity have?

Metals are $"malleable"$, capable of being hammered into a sheet, and $"ductile"$, capable of being drawn out into a wire. This workability makes metals the premier materials for making tools....

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Why are ionic solids poor conductors of electricity?

..........and, therefore, cannot carry a current. In a melt (for which typical ionic solids must be raised to very high temperatures), or solvated by polar molecules in a solution (typically...

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Why are covalent bonds poor conductors of electricity?

because covalent bonds are formed by sharing of electrons..they don't have a free electron that is required for electricity transfer(electricity is the flow of free electrons!) thus they re bad...

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Why are metallic compounds solid at room temperature?

But caesium and mercury are certainly room temperature LIQUIDS. That metals exist in condensed phases under standard conditions is a consequence of , which is a non-molecular force of interaction,...

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