which of the following statements best describes the relationship between atoms and conductivity
atoms with few electrons make good conductors
atoms with many electrons make good insulators
atoms with a nearly empty valence shell make good conductors
atoms with a full velence shell make good conductors
The correct statement that describes the relationship between atoms and conductivity is "atoms with a nearly empty valence shell make good conductors." To understand why this is the case, it's important to consider the concept of valence electrons.
Valence electrons are the electrons in the outermost shell of an atom. They are involved in chemical reactions and determining the atom's properties, including its conductive properties. Atoms with a nearly empty valence shell have a small number of valence electrons, typically one or a few, and tend to be good conductors.
When a material conducts electricity, it allows the flow of electric charge. This flow of charge occurs due to the movement of electrons. In conductive materials, such as metals, the valence electrons are not tightly bound to individual atoms but are instead free to move throughout the material. These "free" or "delocalized" electrons are responsible for the material's conductivity. They can easily move in response to an applied electric field, allowing the flow of electric charge.
In contrast, atoms with a full valence shell, often referred to as noble gases, tend to be good insulators. Noble gases, like helium or neon, have a completely filled valence shell, making it difficult for electrons to move freely and conduct electricity.
To summarize, atoms with a nearly empty valence shell, characterized by just a few valence electrons, make good conductors because these electrons are free to move and facilitate the flow of electric charge through the material.