What is the general outer configuration of the coinage metals? (a) \(\mathrm{ns}^{2} \mathrm{np}^{6}\) (b) \((\mathrm{n}-1) \mathrm{d}^{9} \mathrm{~ns}^{2}\) (c) \((\mathrm{n}-1) \mathrm{d}^{10} \mathrm{~ns}^{1}\) (d) \((\mathrm{n}-1) \mathrm{d}^{10} \mathrm{~ns}^{2}\)

Coinage metals include copper (Cu), silver (Ag), and gold (Au), famously known for their historical use in making coins, hence their name. Apart from being good conductors of electricity and heat, they have a high luster and resistance to corrosion which make them ideal for currency and jewelry. Their unique properties stem from their electronic arrangement, which is a critical aspect of their chemistry and physical behavior.

Understanding the electronic configuration of coinage metals not only helps in predicting their chemical reactions but also contributes to various applications in electronics, catalysis, and decorative art. These metals, located in group 11 of the periodic table, share similarities in their chemistry, including their oxidation states and their ability to form complex ions.

Group 11 of the periodic table is significant, comprising coinage metals—Cu, Ag, and Au—that exhibit a blend of transition metal and post-transition metal properties. This group is characterized by the full d-subshell in their penultimate electron shell alongside a partially filled s-orbital in their outermost shell. Group 11 metals possess a unique standing within the periodic table due to their d10s1 electronic configuration, which imparts distinctive physical properties such as high malleability, ductility, and electrical conductivity.

• Copper has been paramount in electrical wiring due to its excellent electrical conductivity.
• Silver, the best conductor of heat and electricity, is crucial in high-value electronics and solar panels.
• Gold, as the least reactive, finds its use in high-end electronic connectors and satellites.

These uses underscore the importance of their specific electron configuration in their technological applications.

The electron configuration of an element is a representation of the arrangement of electrons distributed among the orbital shells and subshells. Group 11 elements have an electron configuration pattern that falls under the noble gas configuration, with a completely filled d-subshell \textbf{(n-1)d\(^{10}\)}\ and a single electron in the s-subshell of the valence shell \textbf{ns\(^{1}\)}\.

This configuration plays a pivotal role in the properties of the coinage metals: the stability of the filled d-shell along with the availability of the outer s-electron for bond formation. This electron configuration results in a +1 oxidation state typically observed in compounds of these metals, although higher oxidation states can sometimes be achieved due to the involvement of d-electrons.

Electronic Configurations of Coinage Metals:

• Copper: \textbf{[Ar] 3d\(^{10}\) 4s\(^{1}\)}\
• Silver: \textbf{[Kr] 4d\(^{10}\) 5s\(^{1}\)}\
• Gold: \textbf{[Xe] 4f\(^{14}\) 5d\(^{10}\) 6s\(^{1}\)}\

The position of the coinage metals in the periodic table, their electron configuration, and its subsequent influence on their properties is not only fundamental to understanding their chemistry but also vital to the many industries that depend on these metals.