Chemical Properties
The metal silver is described as a white, lustrous solid. In its pure form it has the highest thermal and electrical conductivity and lowest contact resistance of all metals. With the exception of gold, silver is the most malleable metal.
Silver (symbol Ag) is one of the basic elements present in the earth's crust. Silver is rare, but occurs naturally in the environment as a soft, “silver”-colored metal or as a white powdery compound (silver nitrate). Metallic silver and silver alloys are used to make jewelry, eating utensils, electronic equipment, and dental fillings. Nanoparticles of silver have been developed into meshes, bandages, and clothing as an antibacterial. Silver is used in photographic materials, electric and electronic products, brazing alloys and solders, electroplated and sterling ware, as a catalyst, and in coinage. Silver is alloyed with many other metals to improve strength and hardness and to achieve corrosion resistance.
History
Silver is one of the oldest metals, known since ancient times. It is a precious metal worldwide, used in ornaments, coins, and utensils. The symbol Ag for this element is derived from the Latin word, argentum. Silver occurs in nature in native form, commonly associated with gold. It is found in most lead and copper ores. The principal mineral of silver is argentite, Ag2S [1332-04-3]. Some other silver minerals include pyrargyrite, Ag3SbS3 [15123-77-0]; proustite, Ag3AsS3 [15152-58-4]; polybasite, Ag16Sb2S11 [53810-31-4]; cerargyrite, AgCl [14358-96-4]; stephanite, Ag5SbS4 [1302-12-1]; and tetrahedrite, Cu3(AsSb)S3. Abundance of silver in the earth’s crust is estimated to be 0.075 mg/kg and its average concentration in sea water is 0.014 µg/L.
Crystal System
The space lattice of Ag belongs to the cubic system, and its face-centered cubic lattice has a lattice constant of a=0.40705 nm.
Uses
Silver and its alloys and compounds have numerous applications. As a precious metal, silver is used in jewelry. Also, one of its alloys, sterling silver, containing 92.5 weight % silver and 7.5 weight % copper, is a jewelry item and is used in tableware and decorative pieces. The metal and its copper alloys are used in coins. Silver-copper brazing alloys and solders have many applications. They are used in automotive radiators, heat exchangers, electrical contacts, steam tubes, coins, and musical instruments.
Some other uses of silver metal include its applications as electrodes, catalysts, mirrors, and dental amalgam. Silver is used as a catalyst in oxidation-reductions involving conversions of alcohol to aldehydes, ethylene to ethylene oxide, and ethylene glycol to glyoxal.
Production Methods
Many processes are known for recovery of silver from its ores. These depend mostly on the nature of the mineral, its silver content, and recovery of other metals present in the ore. A few processes are briefly outlined below.
Silver is usually extracted from high-grade ores by three common processes that have been known for many years. These are amalgamation, leaching, and cyanidation. In one amalgamation process, ore is crushed and mixed with sodium chloride, copper sulfate, sulfuric acid, and mercury, and roasted in cast iron pots. The amalgam is separated and washed. Silver is separated from its amalgam by distillation of mercury.
In the cyanidation process the ore is crushed and roasted with sodium chloride and then treated with a solution of sodium cyanide. Silver forms a stable silver cyanide complex, [Ag(CN)2]–. Adding metallic zinc to this complex solution precipitates silver. Several leaching processes are known. One such process, known as the Patera process, developed in the mid 19th century, involves roasting ore with sodium chloride followed by leaching with sodium thiosulfate solution. Silver 834 SILVERis precipitated as silver sulfide, Ag2S, by adding sodium sulfide to the leachate. In the Clandot process, leaching is done with ferric chloride solution. Addition of zinc iodide precipitates silver iodide, AgI. AgI is reduced with zinc to obtain silver.
The above processes are applied for extraction of silver from high-grade ores. However, with depletion of these ores, many processes were developed subsequently to extract silver from low-grade ores, especially lead, copper, and zinc ores that contain very small quantities of silver.
Low grade ores are concentrated by floatation. The concentrates are fed into smelters (copper, lead, and zinc smelters). The concentrates are subjected to various treatments before and after smelting including sintering, calcination, and leaching. Copper concentrates are calcined for removal of sulfur and smelted in a reverberatory furnace to convert into blister copper containing 99 wt% Cu. The blister copper is fire-refined and cast into anodes. The anodes are electrolytically refined in the presence of cathodes containing 99.9% copper. Insoluble anode sludges from electrolytic refining contain silver, gold, and platinum metals. Silver is recovered from the mud by treatment with sulfuric acid. Base metals dissolve in sulfuric acid leaving silver mixed with any gold present in the mud. Silver is separated from gold by electrolysis.
Lead and zinc concentrates can be treated in more or less the same manner as copper concentrates. Sintering lead concentrates removes sulfur and following that smelting with coke and flux in a blast furnace forms impure lead bullion. The lead bullion is drossed with air and sulfur and softened with molten bullion in the presence of air to remove most impurities other than silver and gold. Copper is recovered from the dross and zinc converts to its oxide and is recovered from blast furnace slag. The softened lead obtained above also contains some silver. The silver is recovered by the Parkes Process. The Parkes process involves adding zinc to molten lead to dissolve silver at temperatures above the melting point of zinc. On cooling, zinc-silver alloy solidifies, separating from the lead and rising to the top. The alloy is lifted off and zinc is separated from silver by distillation leaving behind metallic silver.
The unsoftened lead obtained after the softening operation contains silver in small but significant quantities. Such unsoftened lead is cast into anode and subjected to electrolytic refining. The anode mud that is formed adhering to these anodes is removed by scraping. It contains bismuth, silver, gold, and other impurity metals. Silver is obtained from this anode mud by methods similar to the extraction of anode mud from the copper refining process discussed earlier.
If the low–grade ore is a zinc mineral, then zinc concentrate obtained from the flotation process is calcined and leached with water to remove zinc. Silver and lead are left in leach residues. Residues are treated like lead concentrates and fed into lead smelters. Silver is recovered from this lead concentrate by various processes described above.
Description
Silver is one of the earliest known metals. Silver has no known
physiologic or biologic function, though colloidal silver is
widely sold in health food stores. Silver has high thermal and
electrical conductivity and resists oxidation in air that is devoid
of hydrogen sulfide.
Chemical Properties
Elemental silver has a face-centered cubic crystal structure. Silver is a white metal, softer than copper and harder than gold. When molten, silver is luminescent and occludes oxygen, but the oxygen is released upon solidification. As a conductor of heat and electricity, silver is superior to all other metals. Silver is soluble in HNO3 containing a trace of nitrate; soluble in hot 80% H2SO4; insoluble in HCl or acetic acid; tarnished by H2S, soluble sulfides and many sulfur-containing organic substances (e.g., proteins); not affected by air or H2O at ordinary temperatures, but at 200 C, a slight film of silver oxide is formed; not affected by alkalis, either in solution or fused. There are two stable, naturally occurring isotopes, 107Ag and 109Ag. In addition, there are reported to be 25 less stable isotopes, ranging in half-life from 5 seconds to 253 days.
Chemical Properties
Silver is a white lustrous metal that is extremely ductile and malleable. Silver does not oxidize in O2 by heating. It becomes Ag2O3 in O3 and black Ag2S3 in S2 and H2S. It is soluble in HNO3 and concentrated H2SO4 . It is not soluble in alkali.
Physical properties
Silver is located in group 11 (IB) of period 5, between copper (Cu) above it in period 4 andgold (Au) below it in period 6. Thus, silver’s chemical and physical properties are somewhatsimilar to these two group 11 partners.Silver is a soft, while, lustrous metal that can be worked by pounding, drawing througha die, rolling, and so forth. It is only slightly harder than gold. It is insoluble in water, but it will dissolve in hot concentrated acids. Freshly exposed silver has a mirror-like shine thatslowly darkens as a thin coat of tarnish forms on its surface (from the small amount ofnatural hydrogen sulfide in the air to form silver sulfide, AgS). Of all the metals, silver isthe best conductor of heat and electricity. This property determines much of its commercialusefulness. Its melting point is 961.93°C, its boiling point is 2,212°C, and its density is10.50 g/cm
3.
Isotopes
There are 59 isotopes of silver, ranging from Ag-93 to Ag-130 with half-livesfrom a few milliseconds to a few days to 418 years. All but two of these 59 isotopes areradioactive and are produced synthetically. The two stable isotopes found in nature areAg-107 and Ag-109. These two make up 100% of the element’s existence in the Earth’scrust.
Origin of Name
Silver’s modern chemical symbol (Ag) is derived from its Latin word
argentum, which means silver. The word “silver” is from the Anglo-Saxon world “siolfor.”
Ancients who first refined and worked with silver used the symbol of a crescent moon to
represent the metal.
Occurrence
Silver is the 66th most abundant element on the Earth, which means it is found at about0.05 ppm in the Earth’s crust. Mining silver requires the movement of many tons of ore torecover small amounts of the metal. Nevertheless, silver is 10 times more abundant than gold.And though silver is sometimes found as a free metal in nature, mostly it is mixed with theores of other metals. When found pure, it is referred to as “native silver.” Silver’s major ores areargentite (silver sulfide, Ag
2S) and horn silver (silver chloride, AgCl). However, most silver isrecovered as a by-product of the refining of copper, lead, gold, and zinc ores. Although silveris mined in many countries, including the United States, Mexico, and Canada, most silver isrecovered from the electrolytic processing of copper ores. Silver can also be recovered throughthe chemical treatment of a variety of ores.
Characteristics
Silver is somewhat rare and is considered a commercially precious metal with many uses.Pure silver is too soft and usually too expensive for many commercial uses, and thus it isalloyed with other metals, usually copper, making it not only stronger but also less expensive.The purity of silver is expressed in the term “fitness,” which describes the amount of silverin the item. Fitness is just a multiple of 10 times the silver content in an item. For instance,sterling silver should be 93% (or at least 92.5%) pure silver and 7% copper or some othermetal. The fitness rating for pure silver is 1000. Therefore, the rating for sterling silver is 930,and most sliver jewelry is rated at about 800. This is another way of saying that most silverjewelry is about 20% copper or other less valuable metal.
Many people are fooled when they buy Mexican or German silver jewelry, thinking theyare purchasing a semiprecious metal. These forms of “silver” jewelry go under many names,including Mexican silver, German silver, Afghan silver, Austrian silver, Brazilian silver, Nevadasilver, Sonara silver, Tyrol silver, Venetian silver, or just the name “silver” with quotes aroundit. None of these jewelry items, under these names or under any other names, contain anysilver. These metals are alloys of copper, nickel, and zinc.
History
Silver was first discovered by prehistoric people in large amounts around 5000 BC, when they dug the first copper mines (Silver is often found alongside copper veins.). Slag dumps in Asia Minor and on islands in the Aegean Sea indicate that man learned to separate silver from lead as early as 3000 B.C. Silver occurs native and in ores such as argentite (Ag2S) and horn silver (AgCl); lead, lead-zinc, copper, gold, and copper-nickel ores are principal sources. Natural silver contains two stable isotopes. Fifty-six other radioactive isotopes and isomers are known. Silver compounds can be absorbed in the circulatory system and reduced silver deposited in the various tissues of the body. In recent times, however, consumption of silver has at times greatly exceeded the output. On June 24, 1968, the U.S. Government ceased to redeem U.S. Silver Certificates with silver. Since that time, the price of silver has fluctuated widely. As of January 2002, the price of silver was about $4.10/troy oz. (13￠/g); however the price has fluctuated considerably due to market instability.
Uses
For coinage, most frequently alloyed with copper or gold; for manufacture of tableware, mirrors, jewelry, ornaments; for electroplating; for making vessels and apparatus used in manufacture of medicinal chemicals, in processing foods and beverages, in handling organic acids; as catalyst in hydrogenation and oxidation processes; as ingredient of dental alloys. Has been used for purification of drinking water because of toxicity to bacteria and lower forms of life. Some salts used in photography.
Uses
Silver has a multitude of uses and practical applications both in its elemental metallic formand as a part of its many compounds. Its excellent electrical conductivity makes it ideal for usein electronic products, such a computer components and high-quality electronic equipment.It would be an ideal metal for forming the wiring in homes and transmission lines, if it weremore abundant and less expensive.
Metallic silver has been used for centuries as a coinage metal in many countries. Theamount of silver now used to make coins in the United States has been reduced drastically byalloying other metals such as copper, zinc, and nickel with silver.
Silver is used as a catalyst to speed up chemical reactions, in water purification, and inspecial high-performance batteries (cells). Its high reflectivity makes it ideal as a reflectivecoating for mirrors.
Several of its compounds were not only useful but even essential for the predigital photographicindustry. Several of the silver salts, such as silver nitrate, silver bromide, and silverchloride, are sensitive to light and, thus, when mixed with a gel-type coating on photographicfilm or paper, can be used to form light images. Most of the silver used in the United Statesis used in photography.
Photochromic (transition) eyeglasses that darken as they are exposed to sunlight have asmall amount of silver chloride imbedded in the glass that forms a thin layer of metallic silverthat darkens the lens when struck by sunlight. This photosensitive chemical activity is thenreversed when the eyeglasses are removed from the light. This chemical reversal results from asmall amount of copper ions placed in the glass. This reaction is repeated each time the lensesare exposed to sunlight.
Uses
This malleable white metal is found as argentite (Ag2S) and
horn silver (AgCl) or in lead and copper ore. Copper plates
coated with a thin layer of elemental silver and fumed with
iodine were used by Niépce and Daguerre. Aside from the
heliograph and physautotype, silver halide compounds were
the basis of all photographic processes used in the camera and
most of the printing processes during the 19th century.
Uses
Silver is a precious metal, used in jewelryand ornaments Other applications includeits use in photography, electroplating, dentalalloys, high-capacity batteries, printed circuits,coins, and mirrors. Silver is stable in air, and it is utilized in reflecting mirrors. The film vacuum evaporated on a quartz plate with the thickness of 2–55 nm shows the transmittance maximum at λ: 321.5 nm and works as a narrow band filter.
Definition
A transition metal that occurs native and as the sulfide (Ag
2S) and chloride (AgCl). It is extracted as a by-product in refining copper and lead ores. Silver darkens in air due to the formation of silver sulfide. It is used in coinage alloys, tableware, and jewelry. Silver compounds are used in photography. Symbol: Ag; m.p. 961.93°C; b.p. 2212°C; r.d. 10.5 (20°C); p.n. 47; r.a.m. 107.8682.
Definition
silver: Symbol Ag. A white lustroussoft metallic transition element; a.n.47; r.a.m. 107.87; r.d. 10.5; m.p.961.93°C; b.p. 2212°C. It occurs as theelement and as the minerals argentite(Ag
2S) and horn silver (AgCl). It isalso present in ores of lead and copper,and is extracted as a by-productof smelting and refining these metals.The element is used in jewellery,tableware, etc., and silver compoundsare used in photography.Chemically, silver is less reactivethan copper. A dark silver sulphideforms when silver tarnishes in air becauseof the presence of sulphurcompounds. Silver(I) ionic salts exist(e.g. AgNO
3, AgCl) and there are anumber of silver(II) complexes.
Biosynthesis
Silver nanoparticles (AgNPs) are biosynthesized using the aqueous leaf extract of Azadirachta indica (Neem)[1]. Diagrammatic representation of the production of AgNPs utilizing extracts from plants is showed below[2].
General Description
Silver is a noble metal, extensively used in SERS, photocatalysis and solar cells. The surface of silver can be functionalized to attain specific properties such as biocompatibility and vapor selectivity of sensors.3 Iodized silver foils and thin films find potential use as SERS-active metal substrates.1 Cu substrates laminated with Ag foils, have compatible coefficient of thermal expansion (CTE), to be used for electronic packaging. Porous ZnO nanoplates deposited on silver foil with tunable hydrophobicity may be fabricated.3
Reactivity Profile
Silver reacts violently with chlorine trifluoride (in the presence of carbon) [Mellor 2 Supp. 1 1956]. Bromoazide explodes on contact with Silver foil. Acetylene forms an insoluble acetylide with Silver [Von Schwartz 1918 p. 142 ]. When Silver is treated with nitric acid in the presence of ethyl alcohol, Silver fulminate, which can detonated may be formed. Ethyleneimine forms explosive compounds with Silver, hence Silver solder should not be used to fabricate equipment for handling ethyleneimine. Finely divided Silver and strong solutions of hydrogen peroxide may explode [Mellor 1:936 1946-47)]. Incompatible with oxalic acid and tartaric acid [Nav Aer. 09-01-505 1956]. Silver can form explosive salts with azidrine. ("Ethyleneimine" Brocure 125-521-65, Midland (Mich.), Dow Chemical Co., 1965). Ammonia forms explosive compounds with gold, mercury, or Silver. (Eggeman, Tim. "Ammonia" Kirk-Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc. 2001.). Acetylene and ammonia can form explosive Silver salts in contact with Ag. (Renner, Hermann, Gunther Schlamp. “Silver, Silver Compounds, and Silver Alloys." Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH Verlag GmbH & Co. KGaA. 2001.)
Health Hazard
The acute toxicity of silver metal is low. The acute toxicity of soluble silver
compounds depends on the counterion and must be evaluated case by case. For
example, silver nitrate is strongly corrosive and can cause burns and permanent
damage to the eyes and skin.
Chronic exposure to silver or silver salts can cause a local or generalized darkening
of the mucous membranes, skin, and eyes known as argyria. The other chronic
effects of silver compounds must be evaluated individually.
Fire Hazard
Dust is flammable.
Flammability and Explosibility
Silver and most soluble silver compounds are not combustible. However, silver
nitrate and certain other silver compounds are oxidizers and can increase the
flammability of combustible materials.
Silver acetylide, azide, fulminate, oxalate mixtures, styphnate, tartarate mixtures,
and tetrazene are all explosives and must be handled as such.
Pharmaceutical Applications
The name silver is derived from the Saxon word ‘siloflur’, which has been subsequently transformed into
the German word ‘Silabar’ followed by ‘Silber’ and the English word ‘silver’. Romans called the element
‘argentum’, and this is where the symbol Ag derives from.
Silver is widely distributed in nature. It can be found in its native form and in various ores such as argentite
(Ag
2S), which is the most important ore mineral for silver, and horn silver (AgCl). The principal sources of
silver are copper, copper–nickel, gold, lead and lead–zinc ores, which can be mainly found in Peru, Mexico,
China and Australia.
Silver has no known active biological role in the human body, and the levels of Ag
+ within the body are
below detection limits. The metal has been used for thousands of years mainly as ornamental metal or for
coins.
Furthermore, silver has been used for medicinal purposes since 1000 BC. It was known that water would
keep fresh if it was kept in a silver pitcher; for example, Alexander the Great (356–323 BC) used to transport
his water supplies in silver pitchers during the Persian War. A piece of silver was also used, for example,
to keep milk fresh, before any household refrigeration was developed. In 1869, Ravelin proved that silver
in low doses acts as an antimicrobial. Around the same time, the Swiss botanist von Ngeli showed that
already at very low concentration Ag+ can kill the green algae spirogyra in fresh water. This work inspired
the gynaecologist Crede to recommended use of AgNO
3
drops on new born children with conjunctivitis.
Safety Profile
Human systemic effects by inhalation: skin effects. Inhalation of dusts can cause argyrosis. Questionable carcinogen with experimental tumorigenic data. Flammable in the form of dust when exposed to flame or by chemical reaction with C2H2, NH3, bromoazide, ClF3 ethyleneimine, H2O2, oxalic acid, H2SO4, tartaric acid. Incompatible with acetylene, acetylene compounds, aziridine, bromine azide, 3-bromopropyne, carboxylic acids, copper + ethylene glycol, electrolytes + zinc, ethanol + nitric acid, ethylene oxide, ethyl hydroperoxide, ethyleneimine, iodoform, nitric acid, ozonides, peroxomonosulfuric acid, peroxyformic acid. See also POWDERED METALS and SILVER COMPOUNDS.
Potential Exposure
Silver may be alloyed with copper, aluminum, cadmium, lead, or antimony. The alloys are used in the manufacture of silverware, jewelry, coins, ornaments, plates, commutators, scientific instruments; automobile bearing; and grids in storage batteries. Silver is used in chromenickel steels, in solders and brazing alloys; in the application of metallic films on glass and ceramics, to increase corrosion resistance to sulfuric acid, in photographic films, plates and paper; as an electroplated undercoating for nickel and chrome; as a bactericide for sterilizing water; fruit juices; vinegar, etc.; in bus bars and windings in electrical plants; in dental amalgams; and as a chemical catalyst in the synthesis of aldehydes. Because of its resistance to acetic and other food acids, it is utilized in the manufacture of pipes, valves, vats, pasteurizing coils and nozzles for the milk, vinegar, cider, brewing, and acetate rayon silk industries.
Carcinogenicity
The U.S. Department of Health
and Human Resources has extensively monitored published
studies on the occupational therapeutic and domestic exposures
to metals over many years, but has failed so far to
identify unequivocal clinical evidence that silver is carcinogenic
to humans under any circumstances. On the basis of
human experience and supportive studies in experimental
animals, silver is currently classified as a noncarcinogen
(62, 94, 141). On occasions patients exposed to silver in
antibiotic prostheses and other devices have died from
cancer, but in each case the role of silver in the etiology
of the malignancies was not proven.
It is expected that human contact with any of the radioactive
isotopes of silver may lead to local or other carcinogenic
changes in humans through the action of the radioactive
emissions as have been reported with gold in jewelry. No
cases have been seen to date.
Environmental Fate
Silver is a rare element, which occurs naturally in its pure form. It
is a white, lustrous, relatively soft, and very malleable metal.
Silver has an average abundance of about 0.1 ppm in the Earth’s
crust and about 0.3 ppm in soils. It exists in four oxidation states
(0,+1,+2,and +3). Silver occurs primarily as sulfides with iron,
lead, tellurides, and with gold. Silver is found in surface waters
as sulfide, bicarbonate, or sulfate salts, as part of complex ions
with chlorides and sulfates and adsorbed onto particulate
matter. Silver is released through natural processes, for example,
erosion of soils. Sources of atmospheric contamination arise
from processing of ores, steel refining, cement manufacture,
fossil fuel combustion, and municipal waste incineration. Of
anthropomorphic release, over 75% was estimated to be from
disposal of solid waste. Ore smelting and fossil fuel combustion
can emit fine particulates that may be transported long distances
and deposited with precipitation. The major source of release to
surface waters is effluent from photographic processing.
Releases from the photographic industry and from disposal of sewage sludge and refuse are the major sources of soil contamination
with silver. Silver can leach into groundwater, which can
be extenuated in acidic conditions. Silver can bioconcentrate in
fish and invertebrates.
storage
Most silver compounds should be protected from light during
storage or while in use.
Purification Methods
For purification by electrolysis, see Craig et al. [J Res Nat Bur Stand 64A 381 1960]. For purification of crude, or silver residues to pure silver see Glemser & Sauer in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 1028-1030 1963, and for the preparation of colloidal silver see ibid (Ed. Brauer) p 1034.
Structure and conformation
Silver has the electron configuration as [Kr] 4d
10 5s
1
Toxicity evaluation
Ag+ is the biologically active form. Silver is not an essential
mineral supplement and has no known physiologic function.
While specific mechanisms of toxicity are unclear, silver has
high affinity for sulfhydryl groups and proteins. The deposition
of silver in tissues is the result of precipitation of insoluble
silver salts, such as silver chloride and silver phosphate. These
insoluble salts appear to be transformed into soluble silver
sulfide albuminates; to form complexes with amino or carboxyl
groups in RNA, DNA, and proteins; or to be reduced to metallic
silver by ascorbic acid or catecholamines. These could lead to
alteration of a number of cellular processes.
Incompatibilities
Dust may form explosive mixture with air. Powders are incompatible with strong oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions. Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides May react and/or form dangerous or explosive compounds, with acetylene, ammonia, halogens, hydrogen peroxide; bromoazide, concentrated or strong acids, oxalic acid, tartaric acid, chlorine trifluoride, ethyleneimine.
Toxics Screening Level
The initial threshold screening level for silver metal dust and fume and soluble silver compounds (as silver) is 0.1 μg/m3 based on an 8 hour averaging time.
Waste Disposal
Recovery, wherever possible, in view of economic value of silver. Techniques for silver recovery from photoprocessing and electroplating wastewaters have been developed and patented.
References
[1] Eco-Friendly Synthesis and Evaluation of Silver Nanoparticles (AgNPs) Using Azadirachta indica: A Greener Approach to Boosting Antimicrobial Power.
[2] Selvam, K., Prasath, A. R., & Alanazi, A. K. (2025). A Review of Recent Developments in Green Synthesis of Silver Nanoparticles: Antioxidant and Antibacterial Applications. Microscopy Research and Technique, 89 1, 134–147.
https://doi.org/10.1002/jemt.70060
