- such a substance in its pure state, as distinguished from alloys.
- an element yielding positively charged ions in aqueous solutions of its salts.
verb (used with object), met·aled, met·al·ing or (especially British) met·alled, met·al·ling.
Origin of metal
Examples from the Web for metalled
Historical Examples of metalled
It was not metalled until 1859, and nearly all the buildings were frame.Some Reminiscences of old Victoria
Lumps of limestone with which roads are metalled in Northern India.Birds of the Plains
The barn had a slate roof; the railings were new; the pathways had been metalled.Bouvard and Pcuchet, part 2
Take the metalled road on the right leading to Tavannes fort.Verdun Argonne-Metz 1914-1918
There is no railway in the district, and only 29 m. of metalled road.
- any of a number of chemical elements, such as iron or copper, that are often lustrous ductile solids, have basic oxides, form positive ions, and are good conductors of heat and electricity
- an alloy, such as brass or steel, containing one or more of these elements
- the total weight of projectiles that can be shot by a ship's guns at any one time
- the total weight or number of a ship's guns
verb -als, -alling or -alled or US -als, -aling or -aled (tr)
Word Origin for metal
mid-13c., from Old French metal "metal; material, substance, stuff" (12c.), from Latin metallum "metal; mine, quarry, mineral, what is got by mining," from Greek metallon "metal, ore" (senses only in post-classical texts; originally "mine, quarry, pit"), probably from metalleuein "to mine, to quarry," of unknown origin, but related somehow to metallan "to seek after." Cf. Greek metalleutes "a miner," metalleia "a searching for metals, mining."
late 14c., from metal (n.).
Usage: Most metallic elements are lustrous or colorful solids that are good conductors of heat and electricity, and readily form ionic bonds with other elements. Many of their properties are due to the fact that their outermost electrons, called valence electrons, are not tightly bound to the nucleus. For instance, most metals form ionic bonds easily because they readily give up valence electrons to other atoms, thereby becoming positive ions (cations). The electrical conductivity of metals also stems from the relative freedom of valence electrons. In a substance composed of metals, the atoms are in a virtual sea of valence electrons that readily jump from atom to atom in the presence of an electric potential, creating electric current. With the exception of hydrogen, which behaves like a metal only at very high pressures, the elements that appear in the left-hand column of the Periodic Table are called alkali metals. Alkali metals, such as sodium and potassium, have only one electron in their outermost shell, and are chemically very reactive. (Hydrogen is exceptional in that, although it is highly reactive, its other metallic properties are manifest only at very high pressures.) Metals farther toward the right side of the Periodic Table, such as tin and lead, have more electrons in their outermost shell, and are not as reactive. The somewhat reactive elements that fall between the two extremes are the transition elements, such as iron, copper, tungsten, and silver. In most atoms, inner electron shells must be maximally occupied by electrons before an outer shell will accept electrons, but many transition elements have electron gaps in the shell just inside the valence shell. This configuration leads to a wide variety of available energy levels for electrons to move about in, so in the presence of electromagnetic radiation such as light, a variety of frequencies are readily emitted or absorbed. Thus transition metals tend to be very colorful, and each contributes different colors to different compounds.