Uses of Silver in Chemistry and Everyday Applications

Silver is a chemical element that is represented by the symbol (silver formula) “Ag” is a white lustrous metal that is sold at a high price because of its decorative beauty and electrical conductivity. Silver is located in Group 11 and 5th period of the periodic table. It is placed between copper (element of 4th period) and gold ( element of 6th period) as a result its physical and chemical properties are intermediate between these two metals. The atomic number of silver is 47.  In the most abundant isotope of silver, atoms have 47 electrons, 47 protons and also 60 neutrons.

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Properties of Silver Element

• Silver element is a relatively shiny and soft metal. It tarnishes slowly in the air as sulphur compounds react with the surface forming black silver sulfide.

• The atomic weight of silver is 107.8682 u and the silver atomic number is 47.

• 960.8℃ (1,861.4℉) is the melting point and 2,212℃ (4,014℉) is the boiling point of silver.

• The variable oxidation state of silver is +1, +2, +3.

• Electronic configuration of silver (Kr)4d¹⁰5s¹ and silver symbol is Ag.

• Pure silver metal is one of the best conductors of electricity as well as heat. 

• Silver is present in high concentrations in some compounds such as argentite, but most of it is recovered in other metals such as copper refining processes. 

• Most of the compounds of silver are sensitive to light because of this the photographic industry uses silver bromide and silver chloride in excessive amounts.

• Silver that occurs naturally is composed of two stable isotopes,  ¹⁰⁷Ag and ¹⁰⁹Ag.

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Compounds of Silver

Different types of compounds of the silver elements with other elements are given below.

1. Oxides and Chalcogenides - Silver element has comparatively had low chemical affinities for oxygen than other elements, therefore silver oxides are thermally unstable. Upon the addition of alkali, soluble salts of silver(I) precipitate dark-brown coloured silver(I) oxide (Ag₂O). Silver(I) oxide decomposes to silver and oxygen above 160℃ as it has the tendency to easily reduce to metallic silver.In non-integral oxidation states, some other mixed oxides with silver are namely Ag₂O₃ and Ag₃O₄.

2. Halides - Silver difluoride (AgF₂) is the only found dihalide of silver but all four silver(I) halides are known. AgF₂ is a thermally stable compound and safe fluorinating agent. Silver(II) fluoride is used to synthesize hydrofluorocarbons.

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3. Inorganic Compounds - White silver nitrate (AgNO₃) is used in many ways in organic syntheses such as for deprotection and oxidations. Alkenes are bound reversibly by silver ion (Ag⁺) and by selective absorption silver nitrate has been used in order to separate mixtures of alkenes. In order to release the free alkene, the resulting adduct can be decomposed with ammonia. The reaction of aqueous solutions of sodium carbonate with a deficiency of silver nitrate produces yellow silver carbonate. It can be reduced with formaldehyde (CH₂O) and produce silver free alkali metals.

4. Coordination Compounds - Silver(III) coordination compounds are found rarely and can be easily reduced to the more stable lower oxidation states. The compounds of the square planar geometry such as silver periodate and tellurate complexes may be prepared by oxidising silver(I) with alkaline peroxodisulfate. The yellow coloured and diamagnetic complex compound [AgF₄]⁻ is much less stable that fumes in moist air and reacts with the glass. Silver(II) complexes are more common. Aqueous silver ion (Ag⁺²) is produced by oxidation of Ag⁺ by ozone. It is a very strong oxidising agent, even in acidic solutions, it has the ability to stabilize phosphoric acid due to complex formation. 

Uses of Silver

Silver is used for different purposes in daily life as well as in industries because of its chemical and physical properties. Some of the uses of silver elements are given below.

• Sterling silver is an alloy which consists of almost  92.5% silver and the rest is other metals, generally copper. This alloy is popularly used for jewellery and silver tableware for its fascinating appearance. Pure silver metal is very soft for the making of jewellery and utensils hence in order to make it hard it is generally alloyed with at least one other metal.

• Silver is the best reflector of visible light known hence it is used to make mirrors, but it does tarnish with time. 

• Silver is also used in solder, dental alloys, brazing alloys, batteries and electrical contacts. Printed circuits are developed with the help of silver paints.

• Silver bromide and iodide compounds are sensitive to light. These were important in the history of photography. Now in modern days, digital photography has risen but salts of silver are still for the production of high-quality photographs and protecting against illegal copying.

• Silver also possesses antibacterial properties. Therefore nanoparticles of Ag are used in clothing in order to stop bacterias from forming and digesting sweat and unpleasant odours. Threads of silver metal are used in weaving the fingertips of gloves to use it with touchscreen phones.

Conclusion

Silver is an important and rare metal. We get information about symbols, uses, compounds, properties and occurrence of silver. It forms compounds that are important for photography, jewellery, antibacterial and electronic devices.