Which of the following metal atoms would have the highest conductivity? the atom with the smallest radius and the fewest valence electrons the atom with the smallest radius and the most valence electrons the atom with the largest radius and the fewest valence electrons the atom with the largest radius and the most valence electrons

Atoms with the largest radius and the fewer valence electrons

Explanation:

Conductivity is the ability of atoms to conduct electricity. This is due to the presence of loose electrons in their outermore shell, aslo known as valence electrons. These valence electrons are those that move from one medium to another transporting the electricity they possess (negative charges). Metals are the most conductive elements, and they also tend to have fewer valence electrons.

Ionization energy is the amount of energy needed to strip electrons from the atom. For small atoms (smallest radius), ionization energy is bigger because forces between the nucleus and the electrons are higher. For large atoms (largest radius) ionization energy is smaller, meaning it's easier to remove electrons from the atom.

In this sense, atoms with fewer valence electrons (metals) and with smaller ionization energy (greater ease of movement for the electrons) would have highest conductivity. So, the correct answer will be atoms with the largest radius and the fewer valence electrons.

The correct answer is D: the atom with the largest radius and the most valence electrons

not the one above^ which is C