Final answer:
The statement is false. Metals are flexible and conductive due to a 'sea of electrons' that enables free movement and provides many of their distinctive properties such as conductivity, malleability, and ductility. The free-electron model explains these behaviors by describing the electrons as freely moving within the metal.
Step-by-step explanation:
The statement that metals have a strong hold on their electrons, so they are not flexible and not free-floating is false. In reality, metals are characterized by a sea of electrons that are delocalized and free to move around. This quality allows metals to conduct electricity and heat efficiently. The malleability (flexibility) and ductility (ability to be drawn into wires) of metals stem from the ability of these delocalized electrons to act like a 'glue', facilitating the movement of the positive metal ions within the structure without breaking the metallic bond.
Therefore, it's not the strong hold on electrons that defines the metallic properties but rather the presence of free-floating electrons within the metallic bonds. These bonds are what give metals their characteristic properties such as conductivity, malleability, ductility, and a high melting point. The shiny appearance of metals, their conductivity, and their ability to be shaped are related to the structure of metallic bonds where delocalized electrons play a significant role.
The free-electron model of metals explains these behaviors by suggesting that the electrons move freely through the metal, hence the name 'sea of electrons'. It is this feature, rather than a strong hold on electrons, that contributes to the flexibility and other properties of metals.