i think ionic bond why because if more ions are there more is the conductivity.
Metallic bond structure
electron negativity
Ability to conduct a current electric mabeability
-U.S. Treasury bonds -Corporate bonds -Junk bonds
The other four forms of energy are thermal, electrical, chemical, and nuclear. Thermal energy refers to the energy associated with heat, electrical energy is the energy of electric charges, chemical energy is stored in chemical bonds, and nuclear energy is released during nuclear reactions.
Thermal energy cause thermal decomposition of a compound; the bonds between atoms are weakened.
electron negativity
Properties of metals as high boiling point, high melting point, malleability, ductility, electrical conductivity, thermal conductivity, lustre are explained by the theory of metallic bonds.
Properties of metals as high boiling point, high melting point, malleability, ductility, electrical conductivity, thermal conductivity, lustre are explained by the theory of metallic bonds.
electrical conductivity, malleability, & ductility.
electrical conductivity, malleability, & ductility.
Generally: - they have a low thermal and electrical conductivity; - their deformation is very temperature dependent; - low Young module (they deform a lot for low tensions/strenghts); - the atoms are bond by covalent and secondary bonds (Van der Walls and hydrogen bonds)
Examples: low density, hardness, melting point, boiling point, exist frequently as a gas, form covalent bonds, bad electrical and thermal conductivity, lack of elasticity, bad mechanical properties, etc.
Examples: low density, hardness, melting point, boiling point, exist frequently as a gas, form covalent bonds, bad electrical and thermal conductivity, lack of elasticity, bad mechanical properties, etc.
Examples: density, boiling point, melting point, electrical resistivity, thermal conductivity etc.
are often metals.have high conductivity
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.
Electrical conductivity, water solubility, crystalline structure