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Definition and meaning of rust

Definitions

rust (adj.)

1.of the brown color of rust

rust (n.)

1.any of various fungi causing rust disease in plants

2.the formation of reddish-brown ferric oxides on iron by low-temperature oxidation in the presence of water

3.a plant disease that produces a reddish-brown discoloration of leaves and stems; caused by various rust fungi

4.a red or brown oxide coating on iron or steel caused by the action of oxygen and moisture

rust (v. intr.)

1.become coated with oxide

2.become destroyed by water, air, or a corrosive such as an acid"The metal corroded" "The pipes rusted"

3.cause to deteriorate due to the action of water, air, or an acid"The acid corroded the metal" "The steady dripping of water rusted the metal stopper in the sink"

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Merriam Webster

RustRust (?), n. [AS. rust; akin to D. roest, G. & Sw. rost, Icel. ryð; -- named from its color, and akin to E. red. √113. See Red.]
1. (Chem.) The reddish yellow coating formed on iron when exposed to moist air, consisting of ferric oxide or hydroxide; hence, by extension, any metallic film of corrosion.

2. (Bot.) A minute mold or fungus forming reddish or rusty spots on the leaves and stems of cereal and other grasses (Trichobasis Rubigo-vera), now usually believed to be a form or condition of the corn mildew (Puccinia graminis). As rust, it has solitary reddish spores; as corn mildew, the spores are double and blackish.

Rust is also applied to many other minute fungi which infest vegetation, such as the species of Ustilago, Uredo, and Lecythea.

3. That which resembles rust in appearance or effects. Specifically: (a) A composition used in making a rust joint. See Rust joint, below. (b) Foul matter arising from degeneration; as, rust on salted meat. (c) Corrosive or injurious accretion or influence.

Sacred truths cleared from all rust and dross of human mixtures. Eikon Basilike.

Rust is used in the formation of compounds of obvious meaning; as, rust-colored, rust-consumed, rust-eaten, and the like.

Rust joint, a joint made between surfaces of iron by filling the space between them with a wet mixture of cast-iron borings, sal ammoniac, and sulphur, which by oxidation becomes hard, and impervious to steam, water, etc. -- Rust mite (Zoöl.), a minute mite (Phytopius oleivorus) which, by puncturing the rind, causes the rust-colored patches on oranges.

RustRust, v. i. [imp. & p. p. Rusted; p. pr. & vb. n. Rusting.] [AS. rustian.]
1. To contract rust; to be or become oxidized.

If gold ruste, what shall iron do? Chaucer.

Our armors now may rust. Dryden.

2. To be affected with the parasitic fungus called rust; also, to acquire a rusty appearance, as plants.

3. Fig.: To degenerate in idleness; to become dull or impaired by inaction.

Must I rust in Egypt? never more
Appear in arms, and be the chief of Greece?
Dryden.

RustRust, v. t.
1. To cause to contract rust; to corrode with rust; to affect with rust of any kind.

Keep up your bright swords, for the dew will rust them. Shak.

2. Fig.: To impair by time and inactivity. Johnson.

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Definition (more)

definition of Wikipedia

Synonyms

See also

Phrases

Adam's Rust • Albert Rust • Albert Rust (footballer) • American Rust • Armistead Rust • Art Rust, Jr. • As Friends Rust • As Friends Rust (album) • As Friends Rust Split with Discount • Athena Rust • Beauty and Rust • Beauty and Rust (Live in Leysin) • Bernhard Rust • Botany rust • Brian Rust • Bushrod Rust Johnson • Calcium Lime Rust • Canna rust • Carnival of Rust • Carnival of Rust (song) • Cedar-apple rust • Charles Rust-Tierney • Chrysanthemum white rust • De Rust • Donald L. Rust • Edward B. Rust, Jr. • Giacomo Rust • Graham Rust • Greg Rust • Hull-Rust-Mahoning Open Pit Iron Mine • Johann Nepomuk Rust • Kingdom of Rust • Kingdom of Rust (song) • Leaf rust (barley) • Live Rust • Lust 'n Rust • Mathias Rust • Matthias Rust • Meadowsweet Rust gall • Nathaniel Rust Mansion • No. 61 (Rust and Blue) • Obritzberg-Rust • October Rust • Paul Rust • Paula Rodriguez Rust • Peter Murray-Rust • Rebecca Rust • Reggie Rust • Richard Rust • Rod Rust • Rose rust • Rust (color) • Rust (comics) • Rust (disambiguation) • Rust (fungus) • Rust (song) • Rust Belt • Rust Belt Music • Rust Bowl • Rust Buckets • Rust College • Rust De Winter Nature Reserve • Rust Epique • Rust Hills • Rust Nashville • Rust Never Sleeps • Rust Records • Rust Township, Michigan • Rust and oxidation lubricant • Rust im Tullnerfeld • Rust in Peace • Rust monster • Rust v. Sullivan • Rust, Austria • Rust, Germany • Rust, Michigan • Rust-Oleum • Rust-and-yellow Tanager • Soybean rust • Stem rust • Stem rust (barley) • Stripe rust (barley) • Thomas Davis Rust • Thornton Rust • Val D. Rust • Walcott-Rust quarry • Wheat leaf rust • Wheat yellow rust • Where Moth and Rust Destroy • White Pine Blister Rust • White pine blister rust • White rust • Wilhelm Rust • William Ross Rust House • William Rust • William Rust Summit • You, You're a History in Rust

Analogical dictionary

rust (adj.)

rust[Dérivé]

chromatic[Similaire]




rust (n.)






Wikipedia

Rust

                   
  Colors and porous surface texture of rust

Rust is a general term for describing iron oxides. In colloquial usage, the term is applied to red oxides, formed by the reaction of iron and oxygen in the presence of water or air moisture. There are also other forms of rust, such as the result of the reaction of iron and chloride in an environment deprived of oxygen, such as rebar used in underwater concrete pillars, which generates green rust. Several forms of rust are distinguishable visually and by spectroscopy, and form under different circumstances.[1] Rust consists of hydrated iron(III) oxides Fe2O3·nH2O and iron(III) oxide-hydroxide FeO(OH)·Fe(OH)3.

Given sufficient time, oxygen, and water, any iron mass will eventually convert entirely to rust and disintegrate. Surface rust provides no protection to the underlying iron, unlike the formation of patina on copper surfaces. Rusting is the common term for corrosion of iron and its alloys, such as steel. Many other metals undergo equivalent corrosion, but the resulting oxides are not commonly called rust.

Contents

  Chemical reactions

  Heavy rust on the links of a chain near the Golden Gate Bridge in San Francisco; it was continuously exposed to moisture and salt spray, causing surface breakdown, cracking, and flaking of the metal.

  Oxidation of iron metal

When impure (cast) iron is in contact with water, oxygen, or other strong oxidants, or acids, it rusts. If salt is present, for example in seawater or salt spray, the iron tends to rust more quickly, as a result of electrochemical reactions. Iron metal is relatively unaffected by pure water or by dry oxygen. As with other metals, like aluminium, a tightly adhering oxide coating, a passivation layer, protects the bulk iron from further oxidation. The conversion of the passivating iron oxide layer to rust results from the combined action of two agents, usually oxygen and water.

Other degrading solutions are sulfur dioxide in water and carbon dioxide in water. Under these corrosive conditions, iron hydroxide species are formed. Unlike iron oxides, the hydroxides do not adhere to the bulk metal. As they form and flake off from the surface, fresh iron is exposed, and the corrosion process continues until either all of the iron is consumed or all of the oxygen, water, carbon dioxide, or sulfur dioxide in the system are removed or consumed.[2]

  Associated reactions

  A rusted (and dirt-encrusted) bolt; note the surface pitting and gradual shape-deformation, caused by severe oxidation
  Interior rust in old galvanized iron water pipes can result in brown and black water.

The rusting of iron is an electrochemical process that begins with the transfer of electrons from iron to oxygen.[3] The rate of corrosion is affected by water and accelerated by electrolytes, as illustrated by the effects of road salt on the corrosion of automobiles. The key reaction is the reduction of oxygen:

O2 + 4e + 2H2O → 4OH

Because it forms hydroxide ions, this process is strongly affected by the presence of acid. Indeed, the corrosion of most metals by oxygen is accelerated at low pH. Providing the electrons for the above reaction is the oxidation of iron that may be described as follows:

Fe → Fe2+ + 2e

The following redox reaction also occurs in the presence of water and is crucial to the formation of rust:

4Fe2+ + O2 → 4Fe3+ + 2O2−

In addition, the following multistep acid-base reactions affect the course of rust formation:

Fe2+ + 2H2O Fe(OH)2 + 2H+
Fe3+ + 3H2O Fe(OH)3 + 3H+

as do the following dehydration equilibria:

Fe(OH)2 FeO + H2O
Fe(OH)3 FeO(OH) + H2O
2FeO(OH) Fe2O3 + H2O
  Rusted pyrite cubes embedded in a stony matrix

From the above equations, it is also seen that the corrosion products are dictated by the availability of water and oxygen. With limited dissolved oxygen, iron(II)-containing materials are favoured, including FeO and black lodestone (Fe3O4). High oxygen concentrations favour ferric materials with the nominal formulae Fe(OH)3-xOx/2. The nature of rust changes with time, reflecting the slow rates of the reactions of solids.

Furthermore, these complex processes are affected by the presence of other ions, such as Ca2+, both of which serve as an electrolyte, and thus accelerate rust formation, or combine with the hydroxides and oxides of iron to precipitate a variety of Ca-Fe-O-OH species.

A chemical rust indicator can be used for testing the presence of Fe2+. Fe2+ turns the rust indicator from yellow to blue.

  Prevention

Because of the widespread use and importance of iron and steel products, the prevention or slowing of rust is the basis of major economic activities in a number of specialized technologies. A brief overview of methods is presented here; for detailed coverage, see the cross-referenced articles.

Rust is permeable to air and water, therefore the interior metallic iron beneath a rust layer continues to corrode. Rust prevention thus requires coatings that preclude rust formation.

  Rust-resistant alloys

Stainless steel forms a passivation layer of chromium(III) oxide. Similar passivation behavior occurs with magnesium, titanium, zinc, zinc oxides, aluminium, polyaniline, and other electroactive conductive polymers.

Special "weathering steel" alloys such as Cor-Ten rust at a much slower rate than normal, because the rust adheres to the surface of the metal in a protective layer. Designs using this material must include measures that avoid worst-case exposures, since the material still continues to rust slowly even under near-ideal conditions.

  Galvanization

Galvanization consists of an application on the object to be protected of a layer of metallic zinc by either hot-dip galvanizing or electroplating. Zinc is traditionally used because it is cheap, adheres well to steel, and provides cathodic protection to the steel surface in case of damage of the zinc layer. In more corrosive environments (such as salt water), cadmium plating is preferred. Galvanization often fails at seams, holes, and joints where there are gaps in the coating. In these cases, the coating still provides some partial cathodic protection to iron, by acting as a galvanic anode and corroding itself instead of the underlying protected metal. The protective zinc layer is consumed by this action, and thus galvanization provides protection only for a limited period of time.

More modern coatings add aluminium to the coating as zinc-alume; aluminium will migrate to cover scratches and thus provide protection for a longer period. These approaches rely on the aluminium and zinc oxides re-protecting a once-scratched surface, rather than oxidizing as a sacrificial anode as in traditional galvanized coatings. In some cases, such as very aggressive environments or long design life, both zinc and a coating are applied to provide enhanced corrosion protection.

  Plating

  Rusting can completely degrade iron. Note the remaining dull silver-colored galvanization on the unrusted portions.
  • Zinc plating (galvanized iron/steel): iron or steel coated with zinc metal layer. Hot-dipped method or zinc-blasting method may be used.
  • Tin plating: mild steel sheet coated with a tin layer.
  • Cadmium plating
  • Chrome plating: a thin layer of chromium is electrolytically applied to the steel, providing both rust protection and a highly polished, bright appearance. Often used on the bright silver-colored components of bicycles, motorbikes, and automobiles.

  Cathodic protection

Cathodic protection is a technique used to inhibit corrosion on buried or immersed structures by supplying an electrical charge that suppresses the electro-chemical reaction. If correctly applied, corrosion can be stopped completely. In its simplest form, it is achieved by attaching a sacrificial anode, thereby making the iron or steel the cathode in the cell formed. The sacrificial anode must be made from something with a more negative electrode potential than the iron or steel, commonly zinc, aluminium, or magnesium. The sacrificial anode will eventually corrode away, ceasing its protective action unless it is replaced in a timely manner.

Cathodic protection can also be provided by using a special-purpose electrical device to appropriately induce an electric charge on the metal to be protected.

  Coatings and painting

  Flaking paint, exposing a patch of surface rust on sheet metal

Rust formation can be controlled with coatings, such as paint, lacquer, or varnish that isolate the iron from the environment. Large structures with enclosed box sections, such as ships and modern automobiles, often have a wax-based product (technically a "slushing oil") injected into these sections. Such treatments usually also contain rust inhibitors. Covering steel with concrete can provide some protection to steel because of the alkaline pH environment at the steel-concrete interface. However rusting of steel in concrete can still be a problem, since expanding rust can fracture or slowly "explode" concrete from within.

As a closely related example, iron bars were used to reinforce stonework of the Parthenon in Athens, Greece, but caused extensive damage by rusting, swelling, and shattering the marble components of the building.

When only temporary protection is needed for storage or transport, a thin layer of oil, grease, or a special mixture such as Cosmoline can be applied to an iron surface. Such treatments are extensively used when "mothballing" a steel ship, automobile, or other equipment for long-term storage.

Special anti-seize lubricant mixtures are available, and are applied to metallic threads and other precision machined surfaces to protect them from rust. These compounds usually contain grease mixed with copper, zinc, or aluminum powder, and other proprietary ingredients.[citation needed]

  Bluing

Bluing is a technique that can provide limited resistance to rusting for small steel items, such as firearms; for it to be successful, a water-displacing oil is rubbed onto the blued steel.

  Inhibitors

Corrosion inhibitors, like gas-phase or volatile inhibitors, can be used to prevent corrosion inside sealed systems. They are not effective when air circulation disperses them, and brings in fresh oxygen and moisture.

  Humidity control

Rust can be avoided by controlling the moisture in the atmosphere. An example of this is the use of silica gel packets to control humidity in equipment shipped by sea.

  Economic impact

  The collapsed Silver Bridge, as seen from the Ohio side

Rust is associated with degradation of iron-based tools and structures. As rust has a much higher volume than the originating mass of iron, its build-up can also cause failure by forcing apart adjacent parts — a phenomenon sometimes known as "rust smacking". It was the cause of the collapse of the Mianus river bridge in 1983, when the bearings rusted internally and pushed one corner of the road slab off its support. Rust was also an important factor in the Silver Bridge disaster of 1967 in West Virginia, when a steel suspension bridge collapsed in less than a minute, killing 46 drivers and passengers on the bridge at the time.

  The Kinzua Bridge after it collapsed

The Kinzua Bridge in Pennsylvania was blown down by a tornado in 2003, largely because the central base bolts holding the structure to the ground had rusted away, leaving the bridge anchored by gravity alone.

Like exposed steel, reinforced concrete is also vulnerable to rust damage. Internal pressure caused by expanding corrosion of concrete-covered steel and iron can cause the concrete to spall, creating severe structural problems. It is one of the most common failure modes of reinforced concrete bridges and buildings.

  Cultural symbolism

Rust is a commonly-used metaphor for slow decay, since it gradually converts robust iron and steel metal into a soft crumbling powder. A wide section of the industrialized American Midwest and American Northeast, once dominated by steel foundries, the automotive industry, and other manufacturers, has experienced harsh economic cutbacks that have caused the region to be dubbed the "Rust Belt".

In music, literature, and art, rust is associated with images of faded glory, neglect, decay, and ruin.

  See also

  A blacksmith removing rust with sand prior to welding

  References

  1. ^ "Interview, David Des Marais". http://nasa.gov/centers/ames/multimedia/audio/MER/mer13.html. 
  2. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  3. ^ Gräfen, H.; Horn, E. M.; Schlecker, H.; Schindler, H. (2000). "Corrosion". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. DOI:10.1002/14356007.b01_08.  edit

  External links

   
               

 

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