Metals are good conductors of electricity because they have free electrons (option A). In metallic bonds, the outer electrons of metal atoms are not bound to any specific atom and can move freely throughout the metal. This “sea of free electrons” allows electrical charge to flow with minimal resistance, making metals highly efficient conductors. This property distinguishes metals from other materials whose electrons are more tightly bound to their atoms, resulting in poorer conductivity. While factors such as atomic weight, melting point, and other physical properties might influence a metal’s overall characteristics, the presence of free electrons is the primary reason for their superior electrical conductivity. This is why metals are commonly used in electrical wiring, components, and various applications where efficient electricity conduction is essential.