A simplified PPT for the students of class 8th to know about Electroplating, Conductivity of Liquid and chemical effects of electric current according to the syllabus. Ready to use material for assignments.
Its Is The Process By Which A Iron Nail Is Been Coated With Copper Plate.Electroplating is a process that uses electrical current to reduce dissolved metal cations so that they form a coherent metal coating on an electrode. The term is also used for electrical oxidation of anions onto a solid substrate, as in the formation silver chloride on silver wire to make silver/silver-chloride electrodes. Electroplating is primarily used to change the surface properties of an object (e.g. abrasion and wear resistance, corrosion protection, lubricity, aesthetic qualities, etc.), but may also be used to build up thickness on undersized parts or to form objects by electroforming.
The process used in electroplating is called electrodeposition. It is analogous to a galvanic cell acting in reverse. The part to be plated is the cathode of the circuit. In one technique, the anode is made of the metal to be plated on the part. Both components are immersed in a solution called an electrolyte containing one or more dissolved metal salts as well as other ions that permit the flow of electricity. A power supply supplies a direct current to the anode, oxidizing the metal atoms that comprise it and allowing them to dissolve in the solution. At the cathode, the dissolved metal ions in the electrolyte solution are reduced at the interface between the solution and the cathode, such that they "plate out" onto the cathode. The rate at which the anode is dissolved is equal to the rate at which the cathode is plated, vis-a-vis the current flowing through the circuit. In this manner, the ions in the electrolyte bath are continuously replenished by the anode.[1]
Other electroplating processes may use a non-consumable anode such as lead or carbon. In these techniques, ions of the metal to be plated must be periodically replenished in the bath as they are drawn out of the solution.[2] The most common form of electroplating is used for creating coins such as pennies, which are small zinc plates covered in a layer of copper. [3]Process[edit]
Electroplating of a metal (Me) with copper in a copper sulfate bath
The cations associate with the anions in the solution. These cations are reduced at the cathode to deposit in the metallic, zero valence state. For example, in an acid solution, copper is oxidized at the anode to Cu2+ by losing two electrons. The Cu2+ associates with the anion SO42- in the solution to form copper sulfate. At the cathode, the Cu2+ is reduced to metallic copper by gaining two electrons. The result is the effective transfer of copper from the anode source to a plate covering the cathode.
The plating is most commonly a single metallic element, not an alloy. However, some alloys can be electrodeposited, notably brass and solder.
This document discusses electrolysis, which is the process of using direct current to cause non-spontaneous chemical reactions. Electrolysis requires an electrolyte containing free ions, a direct current power supply, and two electrodes. During electrolysis, ions are oxidized or reduced at the electrodes through electron transfer. As an example, electrolysis can be used to purify copper by dissolving impure copper and conducting electrolysis, depositing pure copper at the cathode. Electrolysis equations describe the half-reactions that occur at each electrode. The document also provides an example of electrolyzing brine to produce chlorine gas, hydrogen gas, and sodium hydroxide.
Electrochemistry involves redox reactions in galvanic cells that convert chemical energy to electrical energy. In a galvanic cell, oxidation occurs at the anode and reduction occurs at the cathode. A salt bridge completes the circuit between the two half cells and maintains electrical neutrality. When a zinc rod is used as the anode in a copper sulfate solution with a copper cathode, the zinc rod loses weight as it oxidizes while copper precipitates and the solution warms due to heat released, demonstrating the spontaneous conversion of chemical to electrical energy in a galvanic cell.
A conduction tester is a simple device that uses a bulb or LED connected to a battery to determine if a material is a good or poor conductor of electricity. If the material completes the circuit between the two terminals, the bulb will glow or the LED will light, indicating it is a conductive material. Some solids and liquids like copper, salt water, and acids conduct electricity well while others like wood, rubber, and distilled water conduct poorly or not at all. Passing current through conducting liquids can cause chemical reactions and changes like producing gas bubbles or depositing metal on electrodes. Electrolysis and electroplating are examples of using electricity to drive chemical reactions.
The document discusses corrosion of metals and methods to prevent it. It focuses on the sacrificial anode cathode protection system. It explains that corrosion occurs via electrochemical reactions where the metal acts as the anode and transfers electrons to the cathode. Coupling iron with more electropositive metals like zinc and magnesium prevents rusting by providing preferential sites for the corrosion reactions. The project involves coupling iron nails with zinc, copper and magnesium to observe their effect on rusting. It is concluded that zinc and magnesium prevent rusting by being more electropositive than iron and corroding instead.
The following power point discusses about the Chemical Effects of Electric Current. In this, we study about how electricity is conduced in liquids, electrolysis and the uses and applications of it
Its Is The Process By Which A Iron Nail Is Been Coated With Copper Plate.Electroplating is a process that uses electrical current to reduce dissolved metal cations so that they form a coherent metal coating on an electrode. The term is also used for electrical oxidation of anions onto a solid substrate, as in the formation silver chloride on silver wire to make silver/silver-chloride electrodes. Electroplating is primarily used to change the surface properties of an object (e.g. abrasion and wear resistance, corrosion protection, lubricity, aesthetic qualities, etc.), but may also be used to build up thickness on undersized parts or to form objects by electroforming.
The process used in electroplating is called electrodeposition. It is analogous to a galvanic cell acting in reverse. The part to be plated is the cathode of the circuit. In one technique, the anode is made of the metal to be plated on the part. Both components are immersed in a solution called an electrolyte containing one or more dissolved metal salts as well as other ions that permit the flow of electricity. A power supply supplies a direct current to the anode, oxidizing the metal atoms that comprise it and allowing them to dissolve in the solution. At the cathode, the dissolved metal ions in the electrolyte solution are reduced at the interface between the solution and the cathode, such that they "plate out" onto the cathode. The rate at which the anode is dissolved is equal to the rate at which the cathode is plated, vis-a-vis the current flowing through the circuit. In this manner, the ions in the electrolyte bath are continuously replenished by the anode.[1]
Other electroplating processes may use a non-consumable anode such as lead or carbon. In these techniques, ions of the metal to be plated must be periodically replenished in the bath as they are drawn out of the solution.[2] The most common form of electroplating is used for creating coins such as pennies, which are small zinc plates covered in a layer of copper. [3]Process[edit]
Electroplating of a metal (Me) with copper in a copper sulfate bath
The cations associate with the anions in the solution. These cations are reduced at the cathode to deposit in the metallic, zero valence state. For example, in an acid solution, copper is oxidized at the anode to Cu2+ by losing two electrons. The Cu2+ associates with the anion SO42- in the solution to form copper sulfate. At the cathode, the Cu2+ is reduced to metallic copper by gaining two electrons. The result is the effective transfer of copper from the anode source to a plate covering the cathode.
The plating is most commonly a single metallic element, not an alloy. However, some alloys can be electrodeposited, notably brass and solder.
This document discusses electrolysis, which is the process of using direct current to cause non-spontaneous chemical reactions. Electrolysis requires an electrolyte containing free ions, a direct current power supply, and two electrodes. During electrolysis, ions are oxidized or reduced at the electrodes through electron transfer. As an example, electrolysis can be used to purify copper by dissolving impure copper and conducting electrolysis, depositing pure copper at the cathode. Electrolysis equations describe the half-reactions that occur at each electrode. The document also provides an example of electrolyzing brine to produce chlorine gas, hydrogen gas, and sodium hydroxide.
Electrochemistry involves redox reactions in galvanic cells that convert chemical energy to electrical energy. In a galvanic cell, oxidation occurs at the anode and reduction occurs at the cathode. A salt bridge completes the circuit between the two half cells and maintains electrical neutrality. When a zinc rod is used as the anode in a copper sulfate solution with a copper cathode, the zinc rod loses weight as it oxidizes while copper precipitates and the solution warms due to heat released, demonstrating the spontaneous conversion of chemical to electrical energy in a galvanic cell.
A conduction tester is a simple device that uses a bulb or LED connected to a battery to determine if a material is a good or poor conductor of electricity. If the material completes the circuit between the two terminals, the bulb will glow or the LED will light, indicating it is a conductive material. Some solids and liquids like copper, salt water, and acids conduct electricity well while others like wood, rubber, and distilled water conduct poorly or not at all. Passing current through conducting liquids can cause chemical reactions and changes like producing gas bubbles or depositing metal on electrodes. Electrolysis and electroplating are examples of using electricity to drive chemical reactions.
The document discusses corrosion of metals and methods to prevent it. It focuses on the sacrificial anode cathode protection system. It explains that corrosion occurs via electrochemical reactions where the metal acts as the anode and transfers electrons to the cathode. Coupling iron with more electropositive metals like zinc and magnesium prevents rusting by providing preferential sites for the corrosion reactions. The project involves coupling iron nails with zinc, copper and magnesium to observe their effect on rusting. It is concluded that zinc and magnesium prevent rusting by being more electropositive than iron and corroding instead.
The following power point discusses about the Chemical Effects of Electric Current. In this, we study about how electricity is conduced in liquids, electrolysis and the uses and applications of it
CBSE Class 8 / VIII General Ccience Power Point Presentation
Prepared By
Praveen M Jigajinni
DCSc & Engg,PGDCA,ADCA,MCA,MSc(IT),MTech(IT), M.Phil (Comp Sci)
For Any Queries Please feel free to contact:
Email Id : praveenkumarjigajinni@gmail.com
Cell No: 9431453730
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7 and describes their properties such as neutralizing bases and forming hydrogen ions in solution. Strong acids like hydrochloric acid are described as ionizing completely, while weak acids only partially ionize. Common acids are also listed such as hydrochloric acid found in stomachs. Bases are defined as having a pH greater than 7 and their properties are outlined. The document further discusses pH scales, indicators, buffers, and examples of acid-base reactions. Digestion and pH levels in different parts of the digestive system are briefly covered.
14 chemical effects of electric currentCHEKIT SHARMA
this is the best chapter in science as it is my favioratie as i love chemistry and even i think that the people who would view this will like so i request to plese like share and comment so ok today only this much is enough so i'll leave bye
This document is a chemistry project report by Utkarsh Varshney of class 12 on the topic of rusting of iron. It includes an introduction to rusting and its mechanisms, experiments conducted on rusting of iron under different conditions, and methods to prevent rusting. The project was completed under the guidance of the teacher Mr. Vikram Bhambhu to fulfill CBSE practical requirements.
The document discusses metals and non-metals. It describes the physical and chemical properties of metals and non-metals. Metals are lustrous, malleable, ductile and are good conductors of heat and electricity, while non-metals have opposite properties. It also discusses how metals and non-metals react with oxygen, water, acids and how displacement reactions can be used to determine reactivity order. Metals are extracted from ores through processes like enrichment, extraction using chemical/electrochemical methods depending on their reactivity.
Electrolysis is an electrochemical process where an electric current is passed through an ionic substance like molten salt or electrolyte solution, causing a non-spontaneous chemical reaction to occur. During electrolysis, ions migrate to the electrodes where they undergo oxidation or reduction reactions. Cations migrate to the cathode and gain electrons through reduction. Anions migrate to the anode and lose electrons through oxidation. The document defines key terms related to electrolysis like electrodes, electrolyte, ions, and provides examples of the half-reactions and overall reaction that occur during the electrolysis of molten sodium chloride.
The document discusses the extraction of metals from ores. It begins by explaining that metals are found either in their free state or combined as compounds in minerals and ores. It then outlines some common metal ores such as bauxite (Al2O3.2H2O) for aluminum, zinc blende (ZnS) for zinc, and hematite (Fe2O3) for iron. Finally, it notes that the steps in extracting metal from ore depend on the reactivity of the metal. Highly reactive metals require more processing steps since they must be extracted from their ionic compounds in the ore. Less reactive metals like gold and silver are sometimes found in their free state.
This document provides an overview of electrochemistry. It begins by defining electrochemistry as the study of chemical reactions at the interface of an electrode and electrolyte involving the interaction of electrical and chemical changes. The document then discusses the history and founders of electrochemistry, including Faraday's two laws of electrolysis. It explains key concepts such as oxidation-reduction reactions, balancing redox equations, and the Nernst equation. The document also covers applications including batteries, corrosion, electrolysis, and branches of electrochemistry like bioelectrochemistry and nanoelectrochemistry.
Chemistry(class11)-CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIESPawan Kumar
The document discusses the history and development of the periodic table. It explains that:
1) Elements have been organized into the periodic table based on their atomic weights and properties in order to systematically study and predict chemical behavior.
2) Early periodic tables were proposed by scientists like Dobereiner, Newlands, and Mendeleev based on trends in atomic weights, though Mendeleev's 1869 table was the most successful in predicting new elements.
3) Modern periodic tables are arranged by atomic number according to the periodic law proposed by Moseley, with elements grouped into blocks based on their electron configurations. The table better explains trends in physical and chemical properties.
The document discusses solutions and solution chemistry. It begins by defining solutions as homogeneous mixtures of two or more pure substances, with the solute dispersed uniformly throughout the solvent. It then discusses how solutions form and the energy changes that occur, including the enthalpy changes of separating solute and solvent particles and forming new interactions between them. The rest of the document discusses various factors that affect solubility, such as the nature of the solute and solvent, intermolecular forces, temperature, and pressure. It also covers colligative properties of solutions like vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
This document contains information about various metals and non-metals. It lists the elements sodium through scandium and several other metals and non-metals. It then compares the properties of metals and non-metals such as their physical state, hardness, conductivity and reactivity. Specific metals like gold, silver, aluminum and copper are discussed along with their common uses like making jewelry, aircraft, utensils and wires. Nitrogen and graphite are given as examples of non-metals and their uses by plants and in pencils respectively. The document concludes by presenting the reactivity series of some common metals.
Acid Bases and Salts and Chemical EquationsSanchit Duseja
1) The document discusses chemical reactions and equations, focusing on chemical changes, types of chemical equations, and balanced chemical equations.
2) It then covers the five main types of chemical reactions - combination, decomposition, displacement, double displacement, and oxidation-reduction reactions.
3) Finally, it discusses acids, bases, and salts. It defines acids and bases, lists their key properties, methods of classification, common examples, and uses.
This document provides an overview of electrochemical cells. It defines oxidation and reduction reactions and describes how electrons are transferred in these reactions. It explains the basic components and workings of electrolytic cells, which use an external power source to drive non-spontaneous chemical reactions, and galvanic cells, which generate electricity from spontaneous reactions. Reversible and irreversible electrodes are also discussed. Thermodynamics relationships for electrochemical cells are outlined.
The document discusses the extraction and processing of various metals. It describes how most metals are found in ores and require concentration and extraction of the pure metal. The extraction method depends on the metal's reactivity. Less reactive metals can be directly extracted from ores, while more reactive metals require electrolysis or reduction using carbon or other reagents. Common extraction techniques are also outlined for a number of metals including iron, aluminum, and zinc.
1. Magnetism arises from the magnetic moments of electrons, both from their orbital motion and spin.
2. Magnetic materials can be classified as diamagnetic, paramagnetic, ferromagnetic, antiferromagnetic, or ferrimagnetic based on their magnetic properties.
3. Ferromagnetic materials exhibit hysteresis, where magnetization lags behind an applied magnetic field, leading to a hysteresis loop. Hard magnetic materials have large hysteresis loops while soft magnetic materials have small loops.
The document discusses electroplating, which involves using electrolysis to coat a thin layer of one metal onto another. It explains that electroplating can be used to protect against corrosion or improve appearance. It then provides details on the electroplating process, where the metal to be plated is the cathode and connects to the negative terminal, while the metal used for plating is the anode and connects to the positive terminal. Ions of the anode metal dissolve and deposit onto the cathode. Copper plating of other metals like copper is provided as an example.
Various factors that affecting the rate of corrosion by Ariful IslamArifulIslam665
This presentation summarizes various factors that influence the rate of corrosion. It discusses primary factors related to the metal, including the nature of the metal, surface state of the metal, and nature of corrosion products. Secondary environmental factors are also covered, such as pH of the medium, temperature, presence of oxidizing agents, humidity, and area effect. The presentation was delivered by Ariful Islam to the Department of Chemistry at Khulna University of Engineering & Technology in Bangladesh.
class-10th
subject-chemistry
topic name-chemical reaction and chemical equation
most important notes for class 10th student that slide cover two chemistry topics chemical reaction and periodic table classification
The document discusses ionic bonding between metals and non-metals. Ionic bonding occurs when metals give up electrons to form positive ions and non-metals gain electrons to form negative ions. The positive and negative ions are then attracted to each other, forming an ionic compound. Metals are usually found on the left side of the periodic table and easily give up valence electrons. Non-metals are usually on the right side and readily gain electrons to achieve a full valence shell. When ions form, they arrange in a crystalline lattice structure with positive and negative ions alternating. Ionic compounds have properties like being crystalline solids, having high melting points, and being able to conduct electricity when melted or
This document discusses the basics of electricity and chemical effects of electric current. It begins by explaining what charges are and how they relate to atoms. It then defines electric current as the flow of electrons. It discusses the differences between conductors and insulators, and how certain materials allow electric current to flow through them while others do not. It also explains the direction of electric current flow and some of the chemical changes that can occur when electric current passes through solutions. Additional topics covered include electrical conductivity, electrolysis, electroplating, and an example of electroplating an iron key.
chemical effects of current for students of class 8amansirdav
This document provides an overview of a lesson on the chemical effects of electric current. The key points covered include:
- Recalling the differences between conductors and insulators.
- Understanding what causes conductivity in liquids and defining strong and weak electrolytes.
- Explaining the chemical effects of electric current and its applications, including electrolysis, electroplating, and electromagnetic induction.
- Discussing activities and demonstrations to help students learn the concepts.
CBSE Class 8 / VIII General Ccience Power Point Presentation
Prepared By
Praveen M Jigajinni
DCSc & Engg,PGDCA,ADCA,MCA,MSc(IT),MTech(IT), M.Phil (Comp Sci)
For Any Queries Please feel free to contact:
Email Id : praveenkumarjigajinni@gmail.com
Cell No: 9431453730
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7 and describes their properties such as neutralizing bases and forming hydrogen ions in solution. Strong acids like hydrochloric acid are described as ionizing completely, while weak acids only partially ionize. Common acids are also listed such as hydrochloric acid found in stomachs. Bases are defined as having a pH greater than 7 and their properties are outlined. The document further discusses pH scales, indicators, buffers, and examples of acid-base reactions. Digestion and pH levels in different parts of the digestive system are briefly covered.
14 chemical effects of electric currentCHEKIT SHARMA
this is the best chapter in science as it is my favioratie as i love chemistry and even i think that the people who would view this will like so i request to plese like share and comment so ok today only this much is enough so i'll leave bye
This document is a chemistry project report by Utkarsh Varshney of class 12 on the topic of rusting of iron. It includes an introduction to rusting and its mechanisms, experiments conducted on rusting of iron under different conditions, and methods to prevent rusting. The project was completed under the guidance of the teacher Mr. Vikram Bhambhu to fulfill CBSE practical requirements.
The document discusses metals and non-metals. It describes the physical and chemical properties of metals and non-metals. Metals are lustrous, malleable, ductile and are good conductors of heat and electricity, while non-metals have opposite properties. It also discusses how metals and non-metals react with oxygen, water, acids and how displacement reactions can be used to determine reactivity order. Metals are extracted from ores through processes like enrichment, extraction using chemical/electrochemical methods depending on their reactivity.
Electrolysis is an electrochemical process where an electric current is passed through an ionic substance like molten salt or electrolyte solution, causing a non-spontaneous chemical reaction to occur. During electrolysis, ions migrate to the electrodes where they undergo oxidation or reduction reactions. Cations migrate to the cathode and gain electrons through reduction. Anions migrate to the anode and lose electrons through oxidation. The document defines key terms related to electrolysis like electrodes, electrolyte, ions, and provides examples of the half-reactions and overall reaction that occur during the electrolysis of molten sodium chloride.
The document discusses the extraction of metals from ores. It begins by explaining that metals are found either in their free state or combined as compounds in minerals and ores. It then outlines some common metal ores such as bauxite (Al2O3.2H2O) for aluminum, zinc blende (ZnS) for zinc, and hematite (Fe2O3) for iron. Finally, it notes that the steps in extracting metal from ore depend on the reactivity of the metal. Highly reactive metals require more processing steps since they must be extracted from their ionic compounds in the ore. Less reactive metals like gold and silver are sometimes found in their free state.
This document provides an overview of electrochemistry. It begins by defining electrochemistry as the study of chemical reactions at the interface of an electrode and electrolyte involving the interaction of electrical and chemical changes. The document then discusses the history and founders of electrochemistry, including Faraday's two laws of electrolysis. It explains key concepts such as oxidation-reduction reactions, balancing redox equations, and the Nernst equation. The document also covers applications including batteries, corrosion, electrolysis, and branches of electrochemistry like bioelectrochemistry and nanoelectrochemistry.
Chemistry(class11)-CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIESPawan Kumar
The document discusses the history and development of the periodic table. It explains that:
1) Elements have been organized into the periodic table based on their atomic weights and properties in order to systematically study and predict chemical behavior.
2) Early periodic tables were proposed by scientists like Dobereiner, Newlands, and Mendeleev based on trends in atomic weights, though Mendeleev's 1869 table was the most successful in predicting new elements.
3) Modern periodic tables are arranged by atomic number according to the periodic law proposed by Moseley, with elements grouped into blocks based on their electron configurations. The table better explains trends in physical and chemical properties.
The document discusses solutions and solution chemistry. It begins by defining solutions as homogeneous mixtures of two or more pure substances, with the solute dispersed uniformly throughout the solvent. It then discusses how solutions form and the energy changes that occur, including the enthalpy changes of separating solute and solvent particles and forming new interactions between them. The rest of the document discusses various factors that affect solubility, such as the nature of the solute and solvent, intermolecular forces, temperature, and pressure. It also covers colligative properties of solutions like vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
This document contains information about various metals and non-metals. It lists the elements sodium through scandium and several other metals and non-metals. It then compares the properties of metals and non-metals such as their physical state, hardness, conductivity and reactivity. Specific metals like gold, silver, aluminum and copper are discussed along with their common uses like making jewelry, aircraft, utensils and wires. Nitrogen and graphite are given as examples of non-metals and their uses by plants and in pencils respectively. The document concludes by presenting the reactivity series of some common metals.
Acid Bases and Salts and Chemical EquationsSanchit Duseja
1) The document discusses chemical reactions and equations, focusing on chemical changes, types of chemical equations, and balanced chemical equations.
2) It then covers the five main types of chemical reactions - combination, decomposition, displacement, double displacement, and oxidation-reduction reactions.
3) Finally, it discusses acids, bases, and salts. It defines acids and bases, lists their key properties, methods of classification, common examples, and uses.
This document provides an overview of electrochemical cells. It defines oxidation and reduction reactions and describes how electrons are transferred in these reactions. It explains the basic components and workings of electrolytic cells, which use an external power source to drive non-spontaneous chemical reactions, and galvanic cells, which generate electricity from spontaneous reactions. Reversible and irreversible electrodes are also discussed. Thermodynamics relationships for electrochemical cells are outlined.
The document discusses the extraction and processing of various metals. It describes how most metals are found in ores and require concentration and extraction of the pure metal. The extraction method depends on the metal's reactivity. Less reactive metals can be directly extracted from ores, while more reactive metals require electrolysis or reduction using carbon or other reagents. Common extraction techniques are also outlined for a number of metals including iron, aluminum, and zinc.
1. Magnetism arises from the magnetic moments of electrons, both from their orbital motion and spin.
2. Magnetic materials can be classified as diamagnetic, paramagnetic, ferromagnetic, antiferromagnetic, or ferrimagnetic based on their magnetic properties.
3. Ferromagnetic materials exhibit hysteresis, where magnetization lags behind an applied magnetic field, leading to a hysteresis loop. Hard magnetic materials have large hysteresis loops while soft magnetic materials have small loops.
The document discusses electroplating, which involves using electrolysis to coat a thin layer of one metal onto another. It explains that electroplating can be used to protect against corrosion or improve appearance. It then provides details on the electroplating process, where the metal to be plated is the cathode and connects to the negative terminal, while the metal used for plating is the anode and connects to the positive terminal. Ions of the anode metal dissolve and deposit onto the cathode. Copper plating of other metals like copper is provided as an example.
Various factors that affecting the rate of corrosion by Ariful IslamArifulIslam665
This presentation summarizes various factors that influence the rate of corrosion. It discusses primary factors related to the metal, including the nature of the metal, surface state of the metal, and nature of corrosion products. Secondary environmental factors are also covered, such as pH of the medium, temperature, presence of oxidizing agents, humidity, and area effect. The presentation was delivered by Ariful Islam to the Department of Chemistry at Khulna University of Engineering & Technology in Bangladesh.
class-10th
subject-chemistry
topic name-chemical reaction and chemical equation
most important notes for class 10th student that slide cover two chemistry topics chemical reaction and periodic table classification
The document discusses ionic bonding between metals and non-metals. Ionic bonding occurs when metals give up electrons to form positive ions and non-metals gain electrons to form negative ions. The positive and negative ions are then attracted to each other, forming an ionic compound. Metals are usually found on the left side of the periodic table and easily give up valence electrons. Non-metals are usually on the right side and readily gain electrons to achieve a full valence shell. When ions form, they arrange in a crystalline lattice structure with positive and negative ions alternating. Ionic compounds have properties like being crystalline solids, having high melting points, and being able to conduct electricity when melted or
This document discusses the basics of electricity and chemical effects of electric current. It begins by explaining what charges are and how they relate to atoms. It then defines electric current as the flow of electrons. It discusses the differences between conductors and insulators, and how certain materials allow electric current to flow through them while others do not. It also explains the direction of electric current flow and some of the chemical changes that can occur when electric current passes through solutions. Additional topics covered include electrical conductivity, electrolysis, electroplating, and an example of electroplating an iron key.
chemical effects of current for students of class 8amansirdav
This document provides an overview of a lesson on the chemical effects of electric current. The key points covered include:
- Recalling the differences between conductors and insulators.
- Understanding what causes conductivity in liquids and defining strong and weak electrolytes.
- Explaining the chemical effects of electric current and its applications, including electrolysis, electroplating, and electromagnetic induction.
- Discussing activities and demonstrations to help students learn the concepts.
this presentation is based on magnetic effect of electric current, a which many of us have studies or will be studying in higher classes.this presentation is a better way of understanding the topic and in a visual way
This document is a student project on studying the effect of metal coupling on rusting of iron. It includes an introduction on corrosion, the electrochemical mechanism of rusting, and common prevention methods. The aim is to investigate how coupling iron with different metals affects rusting. The procedure involves coupling iron nails with zinc, copper, or magnesium and observing any rust formation. The results showed that coupling with more electropositive metals like zinc and magnesium prevented rusting, while coupling with less electropositive copper facilitated rusting.
There are several types of electrodes classified by their composition and function. Reference electrodes like the standard hydrogen electrode (SHE) and saturated calomel electrode (SCE) maintain a known and constant potential used for comparison. The SHE represents the standard reduction potential but is difficult to maintain at standard conditions. The SCE uses a mercury/mercury chloride mixture and is easier to construct and maintain compared to the SHE. Indicator electrodes like the glass electrode are used in titration analysis, with the glass electrode potential indicating pH. Electrodes can also be classified as anodes, which experience oxidation, or cathodes, which undergo reduction.
Conductors allow electric current to pass through them, while insulators do not. A conduction tester uses a circuit with a battery, bulb, and wires to determine if a substance is a conductor or insulator based on whether the bulb lights. When electric current passes through a conducting solution, chemical reactions can occur like gas bubble formation, metal deposition, or color changes - this is the chemical effect of electric current. Electrolysis is the process where electric current splits water into hydrogen and oxygen gases. Electroplating uses electric current to deposit a thin layer of metal onto another material.
The document discusses corrosion, including its types, why we prevent it, and various electrochemical principles related to corrosion. It defines corrosion as the destruction of metals by chemical and electrochemical attack from the environment. There are two main types of corrosion: chemical (dry) corrosion which occurs without moisture, and electrochemical (wet) corrosion, which is the most common and occurs in the presence of moisture via an electrochemical cell. The document outlines several electrochemical concepts like the Pilling Bedworth rule, electrochemical series, Nernst equation, standard electrodes, and Pourbaix and Ellingham diagrams which can be used to understand and predict corrosion reactions and products.
The document discusses corrosion, including its types, why we prevent it, and several related concepts from electrochemistry. It defines corrosion as the destruction of metals by chemical and electrochemical attack from the environment. There are two main types: chemical corrosion from oxygen and electrochemical corrosion, which occurs in the presence of moisture and produces an electrochemical cell. The document outlines several concepts to understand and control corrosion, including the Pilling-Bedworth rule, electrochemical series, Nernst equation, standard electrodes, and Pourbaix and Ellingham diagrams.
The document discusses corrosion, including its types, why we prevent it, and several related concepts from electrochemistry. It defines corrosion as the destruction of metals by chemical and electrochemical attack from the environment. There are two main types: chemical corrosion from oxygen and electrochemical corrosion, which occurs in the presence of moisture and produces an electrochemical cell. The document outlines several electrochemical concepts like the Pilling Bedworth rule, electrochemical series, Nernst equation, standard electrodes, and Pourbaix and Ellingham diagrams, which can be used to understand and predict corrosion reactions.
The document discusses conductivity (or specific conductance) of metal ions in solution, which is a measure of its ability to conduct electricity. It explains that conductivity is higher for strong electrolytes that nearly completely dissociate into ions in solution, while weak electrolytes only partially dissociate. Several factors influence conductivity, including the nature of the solute and solvent, concentration, and temperature. Conductivity measurements are used in various industrial applications like water treatment and leak detection.
IT IS A NICE VEDIO AND PPT ABOUT CHEMICAL EFFECTS OF ELECTRIC CURRENT EVEN I WAS NOT KNOWING ABOUT THIS FIRST AND NOW I AM THE CHAMP OF THIS CHAPTER KNOWN AS CHEMICAL EFFECT OF ELECTRIC CURRENT.
The document discusses various metal plating processes. It describes electroplating as coating metal onto another surface using electricity, where metal ions dissolve from the anode and deposit on the cathode. Electroless plating uses chemical reactions without electricity to deposit metal alloys like nickel-phosphorus. Galvanization coats iron or steel with zinc to prevent rusting. Post-plating processes like rinsing remove chemical residues. The electroplating industry generates various solid, liquid, and gaseous wastes that must be properly managed to reduce environmental pollution.
Corrosion And Its Prevention (Electrochemical Interpretation) Awais Chaudhary
This document discusses corrosion and its prevention through an electrochemical interpretation. It begins by defining corrosion as the deterioration of materials through chemical interaction with the environment, and notes that while it affects many materials, the discussion will focus on iron and steel corrosion. It then provides examples of corrosion, explains why metals corrode in terms of thermodynamics, and outlines the general scheme of corrosion when a metal is immersed in an aqueous solution. The document continues by explaining the electrochemistry of corrosion, including the components of a corrosion cell, current flow, and the mechanism of rusting. It classifies types of corrosion such as uniform, galvanic, crevice, pitting and intergranular corrosion. Finally, it discusses some
This document provides a summary of a presentation on conductometry. It discusses electrochemical cells, types of electrodes including reference and indicator electrodes. It also describes the Nernst equation and its applications in determining solubility products and for analytical chemistry purposes such as measuring ion concentrations using cell potentials. Electrode types including electrodes of the first, second and third kind are explained along with examples like the silver/silver chloride electrode.
This document provides information about electrochemistry. It discusses how electrochemistry deals with oxidation-reduction reactions that produce or utilize electrical energy. There are two main types of electrochemical cells: galvanic cells which convert chemical energy to electrical energy, and electrolytic cells which use electrical energy to drive non-spontaneous chemical reactions. The document explains the basic setup and workings of these two cell types.
Metallic bonding allows metals to have unique properties. Metals form a regular lattice structure where the outer electrons separate from the metal atoms to form a "sea of electrons". This delocalizes the electrons and allows them to move freely through the metal. The metal atoms become positively charged ions that are attracted to the sea of electrons, called metallic bonding. This strong bonding allows metals to conduct heat and electricity well and be hard and malleable. Band theory can explain these properties by describing the states that form from the overlapping atomic orbitals in a metal lattice.
1. All materials are composed of 92 elements that combine to form compounds or molecules. Elements cannot be broken down further, while compounds and molecules can.
2. Atoms are the smallest particles of elements and join together to form molecules. Atoms themselves contain electrons, protons and neutrons.
3. Materials exist in solid, liquid and gas states depending on the strength of electrostatic forces between atoms and molecules. Stronger forces lead to solids with fixed shapes, while weaker forces allow liquids and gases to flow freely.
STUDY OF THE EFFECT OF METAL COUPLING ON THE RUSTING OF IRONKrishna Yadav
In this project the aim is to investigate effect of the metals coupling on the rusting of iron. Metal coupling affects the rusting of iron. If the nail is coupled with a more electro-positive metal like zinc, magnesium or aluminium rusting is prevented but if on the other hand, it is coupled with less electro –positive metals like copper, the rusting is facilitated.
Similar to Electroplating & conductivity of liquid (20)
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
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LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
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How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
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আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
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Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
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2. Electroplating is a plating process that uses electrical current to
reduce cat-ions of a desired material from a solution and coat a conductive
object with a thin layer of the material, such as a metal. Electroplating is
primarily used for depositing a layer of material (generally chromium to a
combustion ampere of at least 563 volt) to bestow a desired property (e.g.,
abrasion and wear resistance, corrosion protection, lubricity, aesthetic qualities,
etc.) to a surface that otherwise lacks that property.
Another application uses electroplating to build up thickness on
undersized parts. The process used in electroplating is called electro deposition.
It is analogous to a galvanic cell acting in reverse. The part to be plated is the
cathode of the circuit. In one technique, the anode is made of the metal to be
plated on the part. Both components are immersed in a solution called an
electrolyte containing one or more dissolved metal salts as well as other ions
that permit the flow of electricity. A rectifier supplies a direct current to the
anode, oxidizing the metal molecules that comprise it and allowing them to
dissolve in the solution. At the cathode, the dissolved metal ions in the
electrolyte solution are reduced at the interface between the solution and the
cathode, such that they "plate out" onto the cathode. The rate at which the
anode is dissolved is equal to the rate at which the cathode is plated, vis-à-vis
the current flowing through the circuit. In this manner, the ions in the electrolyte
bath are continuously replenished by the anode.
Electroplating
3. Other electroplating processes may use a non consumable anode such as
lead. In these techniques, ions of the metal to be plated must be periodically
replenished in the bath as they are drawn out of the solution.
There are two main reasons for electroplating objects:
(a) To protect the metal underneath;
(b) To produce an attractive finish.
Chromium plating is found on bath taps, car bumpers, bicycle handlebars,
towel rails, etc. Chromium does not corrode. It can be polished to give a bright
attractive appearance, and it is a hard metal which resists scratches and wear.
Silver plating is also common for the same reasons. Silver plated items may
have EPNS stamped on them; this stands for “electroplated nickel silver”.
Cutlery and jewellery items are often silver plated - they have the
appearance of silver but are much less expensive.
Electroplating
4. To test whether a liquid allows electric current to pass through it or not, we
can use the tester. When the liquid between the two ends of the tester allows the
electric current to pass, the circuit of the tester becomes complete. The current flows
in the circuit and the bulb glows. When the Liquid does not allow the electric
current to pass, the circuit of the tester is not complete and the bulb does not glow.
In some situations even though the liquid is conducting, the bulb may not
glow. Due to the heating effect of current, the filament of the bulb gets heated to a
high temperature and it starts glowing. However, if the current through a circuit is
too weak, the filament does not get heated sufficiently and it does not glow. Though
a material may conduct electricity, it may not conduct it as easily as a metal. As a
result, the circuit of the tester may be complete and yet the current through it may
be too weak to make the bulb glow.
Most liquids that conduct electricity are solutions of acids, bases and salts.
Conductivity of Liquid
5. The passage of electric currents through liquids causes heating just as it
does in solids. More importantly, chemical activity may occur in the liquids around
the electrodes.
Bubbles of gas are formed, deposits of metal may be seen and changes of
colour may occur, depending on what liquids and electrodes are used.
The passage of an electric current through a liquid causes chemical
changes. This process is known as electrolysis.
Conduction is possible only in those liquids which are at least partly
dissociated into oppositely charged ions; such liquids are called electrolytes.
Solutions of many inorganic chemical compounds (e.g. common salt,
sulphuric acid, etc.) are examples of this type of liquid. In electrolysis, the whole
arrangement of electrodes, electrolyte and the vessel containing them is called a
voltmeter. In the case of the copper voltmeter, which involves copper electrodes in
copper sulphate solution, the net effect is that copper is dissolved off the anode and
deposited on the cathode, with the electrolyte remaining unchanged.
Chemical Effects of Electric Current
6. Some liquids are good conductors of electricity and some are
poor conductors.
Most liquids that conduct electricity are solutions of acids,
bases and salts.
The passage of an electric current through a conducting liquid
causes chemical reactions. The resulting effects are called
chemical effects of currents.
The process of depositing a layer of any desired metal on
another material, by means of electricity, is called
electroplating.
Summary