Transition metals typically exhibit superior electrical conductivity compared to Group 1 metals, primarily due to the presence of multiple valence electrons.

Transition metals, which encompass elements such as iron, copper, and gold, are renowned for their excellent ability to conduct electricity. This characteristic arises mainly from their atomic structure. Transition metals possess multiple valence electrons in their outer shells, which are free to move. These mobile electrons facilitate the flow of electricity through the metal. Generally, the greater the number of free electrons in a metal, the higher its conductivity.

In contrast, Group 1 metals—also referred to as alkali metals—such as lithium, sodium, and potassium, contain only one electron in their outermost shell. This limited number of valence electrons results in fewer free electrons available for conduction. Consequently, these metals typically demonstrate lower electrical conductivity compared to transition metals.

It is crucial to acknowledge that while transition metals are generally better conductors, exceptions exist. For instance, manganese, a transition metal, is a poor conductor of electricity. Conversely, some Group 1 metals, like potassium, can exhibit relatively good conductivity. Thus, although this trend generally holds true, chemistry is rife with exceptions.

In summary, the electrical conductivity of a metal is predominantly influenced by the number of free electrons available for conduction. Transition metals, with their multiple valence electrons, are generally more effective conductors than Group 1 metals. However, it is essential to consider that individual metal conductivity can vary due to other influencing factors.