Why Silver (Ag) is Classified as a Transition Metal Despite a Fully Filled d^10 Orbital

Silver (Ag) is classified as a transition metal, even though its elemental state has a fully filled d10 orbital configuration. This classification is based on the element's ability to form variable oxidation states and have partially filled d orbitals in at least one of its oxidation states.

Definition of Transition Metals

Transition metals are defined as elements that have an incomplete d subshell in one or more of their oxidation states. While elemental silver has a filled d subshell in its ground state, it can exist in oxidation states where the d subshell is not fully occupied, aligning with this definition.

Variable Oxidation States

Silver commonly exhibits a 1 oxidation state, denoted as Ag , with a d10 configuration. However, in some complex compounds and under specific conditions, it can exhibit oxidation states involving the d orbitals. These states, while less common, are indicative of potential d orbital involvement in its chemistry.

Chemical Behavior

Silver can participate in various chemical reactions, including coordination with ligands, where its d electrons play a significant role in bonding and complex formation. This behavior is characteristic of transition metals, highlighting the element's transition metal properties.

Position in the Periodic Table

Silver is located in the d-block of the periodic table, which is designated for transition metals. This placement is based on its electron configuration and the properties it shares with other transition metals. The periodic table classification also supports its classification as a transition metal.

Electronic Configuration and Oxidation States

The electronic configuration of silver is [Kr]5s1 4d10. In its 1 oxidation state, silver has an electronic configuration [Kr], indicating a partially filled d orbital. Despite the full d orbital in its ground state, the presence of unpaired electrons in its valence configuration and similar properties to transition metals support its classification as a transition metal.

In summary, while silver has a fully filled d orbital in its most stable form, its classification as a transition metal is supported by its ability to engage in chemical reactions involving d orbitals, its position in the periodic table, and the presence of variable oxidation states in complex chemistry.

Keywords: silver, transition metal, d^10, electron configuration