Argon: Discover, Extraction, Properties, Isotopes and Uses

Argon is commonly present in the atmosphere and was discovered in the year1894, when Lord Rayleigh and William Ramsay isolated it from liquid air for the first time. Argon is classified as a noble gas and makes up about 0.94% of the atmosphere. The level of argon has subsequently increased in the atmosphere due to the formation of the Earth from radioactive potassium-40 turning into argon by decaying. It is commercially acquired through the process of distillation of liquid air.

Key Terms: Argon, noble gas, atmosphere, air, liquid,  nitrogen, oxygen, carbon dioxide, earth, temperature

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Discovery and Naming of Argon

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In 1785, British scientist Henry Cavendish succeeded in isolating the gas and found that it makes about 1% of air, remaining unreactive even in severe temperatures. However, he was unable to identify the gas and completely comprehend its qualities. Argon was undetected for many years despite being prevalent in the Earth's atmosphere until William Ramsay and Lord Rayleigh isolated it from liquid air in 1894.

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Lord Rayleigh discovered in 1893 that nitrogen taken from the air has a higher density than nitrogen extracted from ammonia or other nitrogen compounds. Rayleigh and Ramsay conducted additional tests to understand this anomaly and kept each other updated on their progress. Ramsay isolated all of the components of the air, including nitrogen, oxygen, and carbon dioxide, in 1894. The nitrogen in the gas was eliminated by reacting it with magnesium, yielding solid magnesium nitride. The gas that remained was chemically inert and occupied 1/80th of the original volume. Ramsay discovered new red and green spectral lines after analyzing the spectrum. Ramsay and Rayleigh announced their discoveries to the rest of the world in 1895.

Physical Properties

• Argon is a noble gas that is colorless, odorless, and tasteless. 
• Argon has a density of 1.784 grams per liter, making it a noble gas. 
• The density of argon is around 1.29 grams per liter when compared to the density of air. 
• At -185.86°C (-302.55°F), argon transforms from a gas to a liquid. 
• At -189.3°C (-308.7°F), it transforms from a liquid to a solid.

Chemical Properties

The noble gas is a type of gas that has no chemical activity. It creates weak, compound-like structures in rare cases and under extreme conditions.

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Occurrence in Nature

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Argon is the third most abundant gas in the atmosphere, accounting for 0.94 percent of the Earth's atmosphere. When naturally occurring 40K (radioactive potassium) decays to 40Ar, it produces 40Ar. It is commercially generated via fractional distillation, which separates it and other gases from liquid air.

Extraction

The noble-gas mixture Fractional distillation can be used to create argon from liquid air. Argon can also be made by combining heated magnesium or calcium with nitrogen gas from the atmosphere. A nitride is formed when magnesium or calcium reacts with nitrogen:

With nitrogen gas, a little amount of argon is always present as an impurity. It does not react with magnesium or calcium, therefore it stays behind. Argon can also be found in natural gas wells. Some argon can be recovered as a by-product of the natural gas purification process.

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Isotopes

The three isotopes of argon are found in nature. Argon-36, Argon-38, and Argon-40 are the isotopes in question. Isotopes are formed when an element splits into two or more isotopes. Isotopes differ from one another based on their mass number. The mass number is the number printed to the right of the element name. The number of protons plus neutrons in the nucleus of an element's atom is used to calculate its mass number. The element is defined by its number of protons, however, the number of neutrons in an atom of any given element can vary. Each isotope element represents a change.

A radioactive isotope breaks apart and emits radiation when it decays. When tiny particles are fired at atoms, radioactive isotopes are created. These particles cling to the atoms, making them radioactive. There are no practical uses for radioactive argon isotopes. However, one non-radioactive isotope can be used to determine the age of extremely old rocks. The potassium entry describes this method of dating and determining the age of rocks.

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Uses of Argon

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• Argon lasers are employed in the treatment of diabetic retinal detachment and diabetic phototherapy, as well as in surgeries to fuse arteries and eliminate tumors. The medical field is the primary application for the argon laser system, as it can target areas with exceptional precision.
• Cryo-needles are used to treat kidney tumors, and they are cooled during argon cryosurgery as part of the technique. This means that sick or aberrant tissue is frozen and killed or eliminated. Argon is also used to treat other issues, such as heart arrhythmias, which are irregular heartbeats.
• In neon tubes, argon is employed as a gas. When electricity is transmitted through argon, a purple-blue glow is produced. It begins to emit light at a considerably lower voltage as it charges. Because it saves money, it quickly became the favored gas for this application.
• This is also true of fluorescent illumination. Argon is used in incandescent light bulbs to keep the filament from oxidizing too quickly. The bulb's life is extended as a result of this.
• Argon is used in the food and beverage industries because of its inertness. Argon is used in drinks to displace air from wine barrels. Because it is denser than air, it settles above the liquid, protecting it from oxidation and sourness. In pubs and restaurants, the same rule applies to open wine and beverage bottles.
• Argon is widely utilized in the welding and casting industries, particularly in the production of specialized alloys and titanium. Because it protects the metal being worked on from oxygen, it is also employed as a shielding gas during arc welding. TIG stands for tungsten inert gas, and it works with either pure argon or argon mixes.
• Because argon decreases chromium losses during steel production in a converter, the appropriate carbon content can be achieved at a lower temperature. Argon is also utilized to remove hydrogen and degasify aluminum throughout the manufacturing process.
• The preservation of old documents is one of the most exciting applications of argon gas. Because of its inert properties, argon gas can be used to create a protective environment. This helps in keeping them from deteriorating and getting damaged during storage and exhibition.
• You may not have considered argon in this light, but it is really useful in the home! It's utilized for thermal insulation in energy-efficient windows; specifically, argon is used to fill the space between the panes in the double-glazed windows that are so widespread in the UK.
• Look for two little holes along with the spacer material if you want to make sure your windows have this gas. In production, these holes are required - one for pumping argon in, and the other for allowing air to be forced out as the gas is pumped in.
• For cold-water diving, this noble gas can be employed as drysuit insulation. This is because argon is inert and has a limited thermal conductivity. It can also be used in its argox form, which is the informal name for an argon-oxygen scuba diving breathing gas. However, this is a pretty uncommon application.

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Health Effects of Argon

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• Exposure routes: The chemical can be inhaled and absorbed into the body.
• Inhalation risk: When the containment is lost, this liquid evaporates quickly, generating air supersaturation and a substantial risk of asphyxia in tight spaces.
• Exposure's effects include Dizziness on inhalation. Dullness. Headache. Suffocation. Frostbite occurs when the skin comes into touch with fluids. Frostbite occurs when the eyes come into contact with fluids.
• Inhalation: This gas is categorized as a simple asphyxiant because it is inert. Excessive concentrations of argon can cause dizziness, nausea, vomiting, loss of consciousness, and can even lead to death. Errors in judgment, confusion, or loss of consciousness can all lead to death if self-rescue is not possible. When oxygen levels are low, unconsciousness and death can happen quickly and without warning.
• Simple asphyxiant gases have an effect proportionate to how much they reduce the amount (partial pressure) of oxygen in the air that is breathed. Before noticeable symptoms appear, oxygen levels in the air may be reduced to 75% of their usual levels. This necessitates the presence of a simple asphyxiant in the mixture of air and gas at a concentration of 33 percent. When the simple asphyxiant reaches a concentration of 50%, it can cause severe symptoms. In a couple of minutes, a concentration of 75% is lethal.
• Symptoms: Rapid respirations and a lack of oxygen are the first indications of a simple asphyxiant. Mental acuity is lowered, and muscle coordination is hampered. Later on, judgment is skewed, and all sensations are suppressed. Emotional instability is common, and weariness sets in quickly. Nausea and vomiting, prostration and loss of consciousness, and lastly convulsions, deep coma, and death may occur as the asphyxia continues.

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Points To Remember 

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• Argon is a noble gas that does not accept or release electrons. As a result, it is unknown if it has an ionic charge.
• Its graphical representation emphasizes its usage in the welding sector, where argon gas is often utilized to prevent the oxidation of welded metals.
• The IUPAC changed Argon's chemical symbol from A to Ar in 1957.
• Researchers in Pennsylvania found the pollution of groundwater by methane from leaking fracking wells (holes designed to recover oil from shale rocks) in 2014 by introducing argon and other noble gases into the wells.

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