Final answer:
Metallic materials do not dissolve in water but are stably maintained in solid state due to metallic bonding and a sea of delocalized electrons. They possess characteristics like high electrical and thermal conductivity and malleability. The melting points of metals vary based on the strength of their metallic bonds.
Step-by-step explanation:
Metallic materials do not dissolve in water, but they remain stable and intact in their solid state because of the metallic bonding and sea of delocalized electrons surrounding their atomic nuclei. Metallic solids like crystals of copper, aluminum, and iron consist of metal atoms in a structure often described as a uniform distribution of atomic nuclei within a 'sea' of delocalized electrons. These electrons, capable of moving through the entire crystal, foster electrical conductivity. Metallic bonds induce several important properties in metals such as high thermal and electrical conductivity metallic luster, and malleability. These solids can exhibit a range of hardness and strength and have varying melting points dependent on the metallic bonding's strength.
Some examples include: sodium and potassium which are relatively soft metals and transition metals like iron that have high melting points above 1000 °C.While pure water and dry table salt are insulators, metallic solids are good conductors of heat and electricity which differentiates them from ionic solids that do not conduct electricity. Metals like copper are not only known for their electrical conductivity but also their ability to be beaten into thin sheets or drawn into wires demonstrating their malleability and ductility.