Metal

Metal is any of a class of substances characterized by high electrical and [|thermal conductivity] as well as by malleability, [|ductility], and high reflectivity of light. Approximately three-quarters of all known [|chemical elements] are metals. The most abundant varieties in the [|Earth’s crust] are [|aluminum], [|iron] , [|calcium] , [|sodium] ,[|potassium] , and [|magnesium]. The vast majority of metals are found in ores (mineral-bearing substances), but a few such as [|copper], [|gold] , [|platinum] , and [|silver] frequently occur in the free state because they do not readily react with other elements. <span style="font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif;">Metals are usually <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|crystalline solids]. In most cases, they have a relatively simple <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|crystal] structure distinguished by a close packing of atoms and a high degree of symmetry. Typically, the atoms of metals contain less than half the full complement of electrons in their outermost shell. Because of this characteristic, metals tend not to form compounds with each other. They do, however, combine more readily with nonmetals (e.g., oxygen and sulfur), which generally have more than half the maximum number of <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|valence electrons]. Metals differ widely in their chemical reactivity. The most reactive include lithium, potassium, and radium, whereas those of low reactivity are gold, silver, palladium, and platinum. <span style="font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif;">The high electrical and thermal conductivities of the <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|simple metals] (i.e., the non-transition metals of the <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|periodic table] ) are best explained by reference to the free-electron theory. According to this concept, the individual atoms in such metals have lost their <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|valence] electrons to the entire <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|solid], and these <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|free electrons] that give rise to conductivity move as a <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|group] throughout the solid. In the case of the more complex metals (i.e., the <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|transition elements] ), conductivities are better explained by the <span style="background-color: transparent; color: #004d99; font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif; font-size: 12px; text-decoration: none;">[|band theory], which takes into account not only the presence of free electrons but also their interaction with so-called // d // electrons. <span style="font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif;">The mechanical properties of metals, such as hardness, ability to resist repeated stressing (fatigue strength), ductility, and malleability, are often attributed to defects or imperfections in their crystal structure. The absence of a layer of atoms in its densely packed structure, for example, enables a metal to deform plastically, and prevents it from being brittle

<span style="font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif;">Metal the key component in Sword Making: <span style="font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif;">Here is the Process... <span style="font-family: Arial,"Arial Unicode MS",Helvetica,sans-serif;">First you need to form the Metal, then you need to heat treat it, then you need to sharpen it, then it needs to be finished. Forming is making the metal so it is in a relatively malleable state. From here you can give the sword a shape (curved, straight, 90 degree angle etc.) Next the metal is heat treated, meaning you beat it until it becomes stronger and stronger. Next there is the matter of making it sharp. This is done by industrial sharpeners. Lastly the swrod need to be finished, you can polish the blade and add a nice handle. Noe, the sword is complete and can be used for decoration, battle, or recreation.

Chemical
Metals are usually inclined to form [|cations] through electron loss, [|[4]] reacting with oxygen in the air to form [|oxides] over changing timescales (iron [|rusts] over years, while [|potassium] burns in seconds). Examples:

4 Na + O2 → 2 Na2O (sodium oxide)2 Ca + O2 → 2 CaO (calcium oxide)4 Al + 3 O2 → 2 Al2O3 (aluminium oxide). The [|transition metals] (such as [|iron], [|copper] , [|zinc] , and [|nickel] ) take much longer to oxidize. Others, like [|palladium], [|platinum] and [|gold] , do not react with the atmosphere at all. Some metals form a barrier layer of [|oxide] on their surface which cannot be penetrated by further oxygen molecules and thus retain their shiny appearance and good conductivity for many decades (like [|aluminium], magnesium, some [|steels] , and [|titanium] ). The [|oxides] of metals are generally [|basic], as opposed to those of nonmetals, which are [|acidic].

[|Painting], [|anodizing] or [|plating] metals are good ways to prevent their [|corrosion]. However, a more reactive metal in the [|electrochemical series] must be chosen for coating, especially when chipping of the coating is expected. Water and the two metals form an [|electrochemical cell], and if the coating is less reactive than the coatee, the coating actually //promotes// corrosion.

Base metal
In [|chemistry], the term //base metal// is used informally to refer to a metal that [|oxidizes] or [|corrodes] relatively easily, and reacts variably with dilute [|hydrochloric acid] (HCl) to form [|hydrogen]. Examples include iron, [|nickel], [|lead] and zinc. Copper is considered a base metal as it oxidizes relatively easily, although it does not react with HCl. It is commonly used in opposition to [|noble metal]. In [|alchemy], a //base metal// was a common and inexpensive metal, as opposed to [|precious metals] , mainly gold and silver. A longtime goal of the alchemists was the transmutation of base metals into precious metals. In [|numismatics], coins used to derive their value primarily from the [|precious metal] content. Most modern currencies are [|fiat currency], allowing the coins to be made of //base metal//.

Ferrous metal
The term "ferrous" is derived from the [|Latin word] meaning "containing iron". This can include pure iron, such as [|wrought iron], or an alloy such as [|steel]. Ferrous metals are often [|magnetic], but not exclusively.

Noble metal
//Noble metals// are metals that are resistant to [|corrosion] or [|oxidation], unlike most [|base metals]. They tend to be precious metals, often due to perceived rarity. Examples include gold, platinum, silver and [|rhodium].