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The metallic bonding which is basically a "sea" or cloud of electrons.
Some are, but not usually. They are typically insulators (exceptions are large polymers with conjugated bonding, but these are quite unique and not commonly found).
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measurable you can measure it and observable you can see and observe it
Types of bonding: ionic (in salts), covalent (in organic compounds), metallic (in metals).
Malleability, Ductile, Luster, Electrical Conductivity, and Thermal Conductivity.
The metallic bonding which is basically a "sea" or cloud of electrons.
Three properties of metals that are caused by metallic bonding are electrical conductivity, malleability, and ductility.
ionic compund
Yes. Graphite is covalently bonded but is moderately conductive, as are some poly-aromatic compounds.
It would help if you specify whether you are talking about thermal conductivity, or electrical conductivity. Diamond certainly doesn't has the highest electrical conductivity. Its thermal conductivity is one of the highest known, and - if a synthetic diamond is made from pure (99.9%) C-12, it is indeed the highest. The Wikipedia article attributes this to a strong covalent bonding.
The metallic bonding which is basically a "sea" or cloud of electrons.
Some are, but not usually. They are typically insulators (exceptions are large polymers with conjugated bonding, but these are quite unique and not commonly found).
Metals have high electrical conductivity because they have alot of free mobile electrons. Metals have metallic bonding in which a sea of electrons is created. It is this sea of electrons that enables metals to conduct electricity so well.
Ionic bonding forms compounds.
The metallic bond is a delocalised bond with free electrons and also may include some covalent interaction This bonding is the cause of the luster, opacity, electrical conductivity, thermal conductivity, strength, malleability, ductility generally associated with the metals.
the electrons involved in metallic bonding are delocalised - they are free to move which accounts for electrical conductivity. In ionic bonds the electrons are tightly bound to individual atoms. Generally covalent bonds have localised electrons, in pairs in individual bonds. However there are delocalised electrons in some situations - take graphite extensive pi bonds allow for delocalisation and electrical conductivity.