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Roupya Bhasma: An Ayurvedic Silver Preparation

Roupya Bhasma is an Ayurvedic metallic preparation derived from silver. It’s a highly refined form of silver, processed through specific Ayurvedic methods to make it suitable for internal consumption.

Key Benefits of Roupya Bhasma

• Nervous system: Supports the nervous system and improves mental clarity.
• Skin health: May be beneficial for certain skin conditions.
• Detoxification: Helps cleanse the body of toxins.
• General well-being: Promotes overall health and vitality.

How to Use Roupya Bhasma

Roupya Bhasma is typically administered orally in small doses. It’s crucial to consult with an Ayurvedic practitioner to determine the appropriate dosage and usage, as it is a potent substance.

Precautions and Considerations

• Individual variations: The response to Roupya Bhasma may vary from person to person. It is essential to observe any unusual reactions and consult a healthcare professional if necessary.
• Pregnancy and lactation: Pregnant and breastfeeding women should seek medical advice before using Roupya Bhasma.
• Digestive sensitivity: In some individuals, it might cause digestive discomfort initially.
• Medical supervision: Roupya Bhasma should be used under the guidance of an Ayurvedic physician.

Roupya Bhasma offers a traditional approach to addressing various health concerns. However, it is crucial to remember that it is not a substitute for medical treatment. If you are experiencing persistent health issues, it is essential to consult a qualified healthcare professional for a comprehensive evaluation and appropriate treatment.

By understanding the therapeutic properties and proper usage of Roupya Bhasma, individuals can harness its potential to improve overall health and well-being.

Silver is a chemical element; it has symbol Ag (from Latin argentum ‘silver’, derived from Proto-Indo-European *h₂erǵ ‘shiny, white’)) and atomic number 47. A soft, white, lustrous transition metal, it exhibits the highest electrical conductivity, thermal conductivity, and reflectivity of any metal.[8] The metal is found in the Earth’s crust in the pure, free elemental form (“native silver”), as an alloy with gold and other metals, and in minerals such as argentite and chlorargyrite. Most silver is produced as a byproduct of copper, gold, lead, and zinc refining.

Silver has long been valued as a precious metal. Silver metal is used in many bullion coins, sometimes alongside gold:[9] while it is more abundant than gold, it is much less abundant as a native metal.[10] Its purity is typically measured on a per-mille basis; a 94%-pure alloy is described as “0.940 fine”. As one of the seven metals of antiquity, silver has had an enduring role in most human cultures.

Other than in currency and as an investment medium (coins and bullion), silver is used in solar panels, water filtration, jewellery, ornaments, high-value tableware and utensils (hence the term “silverware”), in electrical contacts and conductors, in specialized mirrors, window coatings, in catalysis of chemical reactions, as a colorant in stained glass, and in specialized confectionery. Its compounds are used in photographic and X-ray film. Dilute solutions of silver nitrate and other silver compounds are used as disinfectants and microbiocides (oligodynamic effect), added to bandages, wound-dressings, catheters, and other medical instruments.
Silver is similar in its physical and chemical properties to its two vertical neighbours in group 11 of the periodic table: copper, and gold. Its 47 electrons are arranged in the configuration [Kr]4d105s1, similarly to copper ([Ar]3d104s1) and gold ([Xe]4f145d106s1); group 11 is one of the few groups in the d-block which has a completely consistent set of electron configurations.[12] This distinctive electron configuration, with a single electron in the highest occupied s subshell over a filled d subshell, accounts for many of the singular properties of metallic silver.[13]

Silver is a relatively soft and extremely ductile and malleable transition metal, though it is slightly less malleable than gold. Silver crystallizes in a face-centered cubic lattice with bulk coordination number 12, where only the single 5s electron is delocalized, similarly to copper and gold.[14] Unlike metals with incomplete d-shells, metallic bonds in silver are lacking a covalent character and are relatively weak. This observation explains the low hardness and high ductility of single crystals of silver.[15]

Silver has a brilliant, white, metallic luster that can take a high polish,[16] and which is so characteristic that the name of the metal itself has become a color name.[13] Protected silver has greater optical reflectivity than aluminium at all wavelengths longer than ~450 nm.[17] At wavelengths shorter than 450 nm, silver’s reflectivity is inferior to that of aluminium and drops to zero near 310 nm.[18]

Very high electrical and thermal conductivity are common to the elements in group 11, because their single s electron is free and does not interact with the filled d subshell, as such interactions (which occur in the preceding transition metals) lower electron mobility.[19] The thermal conductivity of silver is among the highest of all materials, although the thermal conductivity of carbon (in the diamond allotrope) and superfluid helium-4 are higher.[12] The electrical conductivity of silver is the highest of all metals, greater even than copper. Silver also has the lowest contact resistance of any metal.[12] Silver is rarely used for its electrical conductivity, due to its high cost, although an exception is in radio-frequency engineering, particularly at VHF and higher frequencies where silver plating improves electrical conductivity because those currents tend to flow on the surface of conductors rather than through the interior. During World War II in the US, 13540 tons of silver were used for the electromagnets in calutrons for enriching uranium, mainly because of the wartime shortage of copper.[20][21][22]

Silver readily forms alloys with copper, gold, and zinc. Zinc-silver alloys with low zinc concentration may be considered as face-centred cubic solid solutions of zinc in silver, as the structure of the silver is largely unchanged while the electron concentration rises as more zinc is added. Increasing the electron concentration further leads to body-centred cubic (electron concentration 1.5), complex cubic (1.615), and hexagonal close-packed phases (1.75).[14]
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