How would you expect a metalloid like arsenic to conduct electricity, compared to a metal?
To understand how a metalloid like arsenic would conduct electricity compared to a metal, we need to consider their respective electronic structures and conducting properties. Metals generally have a high electrical conductivity due to their unique characteristics, while metalloids exhibit intermediate conductivity.
In metals, the atoms are arranged in a closely-packed crystal lattice structure, and they typically have a few valence electrons that are loosely held by the atomic nuclei. These valence electrons are referred to as "delocalized" because they are free to move throughout the lattice. When an electric field is applied, these mobile electrons can flow in response, creating an electric current.
On the other hand, metalloids like arsenic have electronic structures that lie between metals and non-metals. Arsenic has five valence electrons, which is more than most metals and fewer than non-metals. While some of these electrons are involved in bonding, there are still some partially delocalized electrons that can contribute to electrical conduction to some extent.
However, the electrical conductivity of arsenic is lower compared to pure metals due to a higher degree of electron localization. The presence of localized electron states makes it harder for electrons to move freely, leading to decreased conductivity.
One significant factor affecting conductivity in metalloids like arsenic is temperature. As the temperature rises, the thermal energy allows more electrons to overcome localized states and participate in conduction, thereby increasing conductivity.
In summary, while metals have high electrical conductivity due to their delocalized electrons within a lattice structure, metalloids like arsenic possess intermediate conductivity because of a higher degree of electron localization.