MCQ Detailed View

Coinage metals refer to a small group of metallic elements that have historically been used to make coins due to their resistance to corrosion, high luster, and good electrical conductivity. These metals include copper (Cu), silver (Ag), and gold (Au). In the periodic table, all three elements are classified as transition metals. They are placed in Group 11 of the periodic table, which is part of the d-block elements.

Transition metals are characterized by having partially filled d-orbitals in either their elemental state or in one or more of their oxidation states. Coinage metals share this property. For example, copper has an electron configuration ending in 3d104s13d^{10}4s^13d104s1, silver has 4d105s14d^{10}5s^14d105s1, and gold has 5d106s15d^{10}6s^15d106s1. These electron arrangements explain their ability to form metallic bonds and conduct electricity efficiently.

The other options do not fit coinage metals. Alkali metals (such as sodium and potassium) are highly reactive and do not have the corrosion resistance needed for coinage. Halogens are non-metals that form salts with metals and are not metallic in nature. Alkaline earth metals (such as magnesium and calcium) are also reactive and not suitable for minting coins.

Transition metals like copper, silver, and gold are ideal for coinage because they do not easily oxidize or tarnish in normal environmental conditions. They are also malleable, meaning they can be shaped into coins without breaking. Additionally, their relatively high densities and appealing colors have made them valuable for currency throughout history.

Thus, coinage metals are scientifically and chemically classified as transition metals, specifically belonging to Group 11 of the periodic table.