Chemical Properties and Uses of Silver in Chemistry
Silver is essential in chemistry and helps students understand various practical and theoretical applications related to this topic. It is a precious metal with immense historical and scientific importance, and its unique properties make it valuable in fields like medicine, electronics, and material science.
What is Silver in Chemistry?
A silver refers to a chemical element with the symbol Ag and atomic number 47. This concept appears in chapters related to metals and nonmetals, transition elements, and periodic properties, making it a foundational part of your chemistry syllabus.
Silver is classified as a transition metal and is famous for its high electrical and thermal conductivity, lustrous white appearance, and strong antimicrobial activity.
Molecular Formula and Composition
The molecular formula of pure silver is Ag. Each atom contains 47 protons, 47 electrons, and typically 61 or 62 neutrons, depending on the isotope. Silver is categorized under element metals, specifically as a noble or coinage metal in Group 11 of the periodic table alongside copper and gold.
Preparation and Synthesis Methods
Industrially, silver is commonly obtained as a byproduct during the extraction of copper, lead, or zinc from their ores. In the laboratory, silver can be prepared by reducing silver salts, such as silver nitrate, using reducing agents.
The most common industrial method is the cyanide process, where silver-containing ores are treated with sodium cyanide, followed by zinc, to precipitate metallic silver. Refinement is achieved through electrolysis or chemical methods.
Physical Properties of Silver
Silver is a lustrous, white, and soft metal. It has the highest electrical and thermal conductivity of all metals. The melting point of silver is about 961°C, and its boiling point is approximately 2212°C. Its density is around 10.5 g/cm³.
In its pure form, silver is too soft for utensils and jewelry, so it is typically blended with other metals like copper (as in sterling silver) to increase hardness.
Chemical Properties and Reactions
Silver is stable in air and water but tarnishes when exposed to sulfur compounds, forming a black coating of silver sulfide. It shows low chemical reactivity, does not react with oxygen or water easily, but dissolves in nitric acid to form silver nitrate (AgNO₃) and in concentrated sulfuric acid.
Common oxidation states include +1, with rare +2 and +3 states. Silver readily forms compounds with halogens, such as silver nitrate and silver chloride.
Frequent Related Errors
- Confusing silver with nonmetals or less conductive metals.
- Assuming all silver compounds are non-toxic.
- Ignoring that silver tarnishes due to sulfur, not oxygen.
- Mixing up silver’s extraction with that of gold or copper.
Uses of Silver in Real Life
Silver is widely used in jewelry and silverware due to its attractive shine. It is also used in electronics for wires, contacts, and conductors because of its excellent conductivity.
In medicine, silver is effective against bacteria and is included in wound dressings and creams. Industrially, it plays a role in photographic films (silver halides), mirrors, and renewable energy (solar panels). Silver is also used in currency, coins, and investment.
Relation with Other Chemistry Concepts
Silver is closely related to topics such as transition elements and properties of metals, helping students build a conceptual bridge between material science, periodic trends, and electrochemistry. Its extraction and alloys introduce metallurgy and real-world applications of chemical principles.
Step-by-Step Reaction Example
- Reacting Silver Nitrate with Copper:
AgNO₃ (aq) + Cu (s) → Cu(NO₃)₂ (aq) + Ag (s) - Copper displaces silver from silver nitrate solution and deposits pure silver metal.
This is a classic displacement reaction demonstrating the relative reactivity of metals.
Lab or Experimental Tips
Remember silver by its brilliant white color and ease of forming a “mirror” deposit on glass (used in Tollens’ test). Vedantu educators often highlight that silver’s compounds—like silver nitrate—are photosensitive, turning black when exposed to light due to silver formation.
Try This Yourself
- Write the balanced equation for extraction of silver by cyanide process.
- Name two important silver compounds used in everyday applications.
- Find silver’s placement in the periodic table and list its group and period.
Final Wrap-Up
We explored silver—its structure, properties, reactions, and real-life importance. Silver stands out for its brilliant luster, high conductivity, and valuable uses from jewelry to electronics and medicine. For more in-depth explanations and exam-prep tips, explore live classes and expert notes on Vedantu.
FAQs on Silver – Properties, Atomic Structure, and Everyday Uses
1. What is silver in chemistry?
Silver is a chemical element with the symbol Ag and atomic number 47. It is a soft, lustrous metal known for its high electrical and thermal conductivity, malleability, and valuable uses in jewelry, electronics, coins, and photography.
2. What are the physical and chemical properties of silver?
Silver possesses distinctive physical and chemical properties:
- Appearance: Shiny, white, and metallic luster.
- Conductivity: Highest among all metals for electricity and heat.
- Malleability and ductility: Easily shaped and stretched.
- Oxidation state: Commonly +1 in compounds.
- Reactivity: Resistant to corrosion but reacts with sulfur compounds to form silver sulfide (tarnish).
3. How is silver used in everyday life?
Silver is utilized in various everyday applications:
- Jewelry and silverware – for its beauty and luster.
- Coins and investments – as a precious metal.
- Electronics – in conductors, contacts, and solar panels due to high conductivity.
- Photography – in traditional film as silver halide crystals.
- Medicine – for antibacterial coatings and wound dressings.
4. Why is silver considered valuable?
Silver is valuable due to its rarity, unique physical properties, and wide industrial uses:
- Scarcity: Naturally limited availability in Earth’s crust.
- Industrial demand: Widely used in electronics, medical, and photographic industries.
- Monetary history: Used historically as currency and investment for wealth preservation.
5. What is the current price of silver per ounce?
The market price of silver per ounce fluctuates daily based on global demand and supply. To find the latest price, check reliable financial sources or precious metals markets. The price reflects silver’s role as an investment and industrial material.
6. What are common compounds of silver?
Major silver compounds include:
- Silver nitrate (AgNO3): Used in analytical chemistry and photography.
- Silver chloride (AgCl): Forms a white precipitate, sensitive to light.
- Silver bromide (AgBr): Key in photographic films.
- These compounds exhibit important chemical properties and practical uses.
7. Where is silver found naturally?
Silver is found in the Earth's crust both as a native element and in ores such as argentite (Ag2S), galena (PbS with silver), and native mixed with other metals. Silver is often recovered as a byproduct during the extraction of copper, lead, and zinc.
8. How is silver extracted from its ores?
Silver is extracted from ores using processes like:
- Roasting and leaching (often with cyanide or thiosulfate solutions).
- Electrolytic refining
- Smelting
9. What oxidation states does silver exhibit?
Silver commonly exhibits the +1 oxidation state (+1), written as Ag+. Less commonly, silver can show a +2 oxidation state in certain compounds, but +1 is typical in almost all its chemical reactions.
10. What are the environmental impacts of silver mining?
Silver mining can have environmental impacts such as:
- Water pollution from chemicals used in extraction.
- Soil degradation and habitat disturbance.
- Use of cyanide or mercury (in some methods) poses ecological risks.
11. Can silver be used as an antimicrobial agent?
Yes, silver has strong antimicrobial properties. Silver ions disrupt the function of bacteria, making it useful in medical dressings, coatings on medical devices, and water purification systems to inhibit microbial growth.
12. How does silver differ from other group 11 metals (copper and gold)?
Silver differs from copper and gold in several ways:
- Conductivity: Silver is the most conductive of all elements.
- Color: Silver is white, copper is reddish, gold is yellow.
- Reactivity: Silver tarnishes, copper corrodes, gold is the least reactive.
