Final answer:
The statement is false because the physical properties of metals such as conductivity and malleability are dependent on the number of delocalized electrons within the metallic bonding model.
Step-by-step explanation:
The statement 'Physical properties for metals are independent of the number of delocalized electrons they have' is false. The metallic bonding model, which describes the sea of delocalized electrons within a metal, explains several physical properties of metals such as conductivity, malleability, and luster. These properties are heavily influenced by the number of delocalized electrons. For example, conductivity is affected by how easily electrons flow through the metal, and the malleability depends on the ability to deform under stress without breaking, which requires movable electrons that are not bound too tightly to the atomic lattice.
The number of delocalized electrons indeed affects the metallic character, which is reflected in an element's position on the periodic table. As one moves down a group, metallic character increases due to the ease of removing electrons that are farther from the nucleus. Conversely, the metallic character decreases across a period as the effective nuclear charge increases, making it harder to remove electrons. Therefore, the number of delocalized electrons contributes significantly to the metal's physical properties, making the initial statement incorrect.