Electroplating
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Electroplating is a process that uses electrical current to deposit metal ions from a solution onto an electrode. It allows precise control over deposition rate by adjusting current or voltage. Electroplating can be used to make nanostructures by depositing metal into a porous template, such as a polycarbonate filter or diblock copolymer. The amount deposited is directly proportional to the current over time. Electroplating is a simple way to make nanowires for applications such as data storage elements, where magnetic nanowires can store data through magnetization direction.
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Electrolysis and Electroplating
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.
electroplating
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.
Electroplating
Here is another creative presentation by your slide maker on the topic “ELECTROPLATING". Hope you like it. If you like it then please, *like*, *Download* and *Share*. By- Slide_maker4u (Abhishek Sharma) *******For presentation Orders, contact me on the Email addresses Written below
******** Email- Sharmaabhishek576@gmail.com or Sharmacomputers87@gmail.com
*******THANK YOU***************
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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.
electroplating
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.
Electroplating
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******** Email- Sharmaabhishek576@gmail.com or Sharmacomputers87@gmail.com
*******THANK YOU***************
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This document provides an overview of basic electrochemistry concepts. It discusses the charge and current involved in electrochemical processes. It introduces Faraday's laws relating the amount of material transformed to the quantity of electricity passed. It also covers conductivity, Nernst equation, different types of electrodes, potentiometry, and various electrochemical techniques including cyclic voltammetry. The key concepts covered include electron transfer processes, Butler-Volmer equation, mass transport by diffusion and convection, and reversible cyclic voltammograms.
Microteaching PPT.pptx
This document provides an overview of electrochemistry and electrolytic cells. It discusses:
- Electrochemistry involves the study of redox reactions and the transfer of electrons, including oxidation which is the loss of electrons and reduction which is the gain of electrons.
- Electrolytic cells use electrical energy to drive redox reactions in a direction that does not occur spontaneously, with examples of cathode and anode half reactions.
- Quantitative electrolysis allows control over the amount of substance undergoing a reaction, according to Faraday's laws - the amount of reaction is proportional to the charge passed, and different electrolytes require different amounts of electrons for the same reaction.
- An example problem calculates the mass of copper
electrochemistry-141128223112-conversion-gate02.pptx
Conductors and Non-Conductors
Substances can be classified as conductors and non-conductors based on their ability to conduct electricity.
Conductors: Substances that allow electric current to flow through them are called conductors. For example, Plastic, Wood, etc.
Non-Conductors: Non-conductors are insulators that do not allow electricity to pass through them. For example, Copper, Iron, etc.
Types of Conductors
Conductors are divided into two groups: Metallic conductors and Electrolytes.
Metallic Conductors: These conductors conduct electricity by the movement of electrons without any chemical change during the process. This type of conduction happens in solids and in the molten state.
Electrolytes: They conduct electricity by the movement of the ions in the solutions. It is present in the aqueous solution.
Distinguish between Metallic and Electrolytic Conduction
Metallic Conduction Electrolytic Conduction
The movement of electrons causes the electric current The movement of ions causes the electric current
There is no chemical reaction Ions get ionised or reduced at the electrodes
There is no transfer of matter It involves the transfer of matter in the form of ions
Follows Ohm’s law Follows Ohm’s law
Resistance increases with an increase in temperature Resistance decreases with an increase in temperature
Faraday’s law is not followed Follows Faraday’s law
Electrolytes
(a) Substances whose aqueous solutions allow the conductance of electric current and are chemically decomposed are called electrolytes.
(b) The positively charged ions furnished by the electrolyte are called cations, while the negatively charged ions furnished by the electrolyte are called anions.
Types of Electrolytes
(a) Weak electrolytes: Electrolytes that are decomposable to a very small extent in their dilute solutions are called weak electrolytes. For example, organic acids, inorganic acids and bases etc.
(b) Strong electrolytes: Electrolytes that are highly decomposable in aqueous solution and conduct electricity frequently are called electrolytes. For example, mineral acid and salts of strong acid.
Electrode
For the electric current to pass through an electrolytic conductor, the two rods or plates called electrodes are always needed. These plates are connected to the terminals of the battery to form a cell. The electrode through which the electric current flows into the electrolytic solution is called the anode, also called the positive electrode, and anions are oxidised here.
An electrode through which the electric current flows out of the electrolytic solution is called the cathode, also called the negative electrode, and cations are reduced there.
Electrolysis
Electrolysis is the process of chemical deposition of the electrolyte by passing an electric current. Electrolysis takes place in an electrolytic cell. This cell will convert the electrical energy to chemical energy.
UTK_Lecture1_March08.pdf
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This document summarizes an electrochemistry chapter that covers:
- Types of electrochemical cells including galvanic and electrolytic cells
- Reversible electrodes like metal-metal ion, gas, and metal-insoluble electrodes
- Determining standard electrode potentials and using the Nernst equation
- Examples of calculating cell potentials and writing electrode half reactions
Elec chem2.pptxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxddddddddddddddddddddddd...
This document summarizes an electrochemistry chapter that covers:
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- Reversible electrodes like metal-metal ion, gas, and metal-insoluble electrodes
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Lecture 5-6: Hydrogen, Storage & Batteries
This document discusses various topics related to hydrogen as a transport fuel, batteries, and fuel cells. It provides information on:
- Different types of vehicles that use hydrogen or batteries as their fuel/power source
- Methods for producing and storing hydrogen
- How electrochemical cells like batteries and fuel cells work through redox reactions
- Characteristics and reactions of different types of batteries including lead-acid, nickel-cadmium, and lithium-ion batteries.
Ch2 slides-1
This document summarizes key concepts from a chapter on the motion and recombination of electrons and holes in semiconductors.
[1] Carriers in semiconductors undergo both thermal motion due to temperature as well as drift motion in the presence of an electric field. The drift velocity depends on factors like carrier mobility and the electric field.
[2] Carriers can also diffuse from regions of higher concentration to lower concentration. The diffusion current depends on the diffusion constant which is related to carrier mobility via the Einstein relation.
[3] When carriers recombine, they restore equilibrium conditions by decaying over time with a characteristic lifetime. Recombination involves traps and centers that facilitate the process.
Opto electronic presentation 01 ecx5243
1. The document contains information about an electronics student named T.M.M. Chanaka, including their registration number and centre. It discusses concepts like conductivity, thermal equilibrium, and the location of the Fermi level in semiconductors.
2. The second part of the document answers questions about how conductivity depends on doping and temperature. It calculates the position of the Fermi level for n-type and p-type semiconductors at different temperatures.
3. The last part explains how the energy bands move when a diode is forward biased and briefly compares the i-v relationships of silicon and gallium arsenide diodes.
2nd Year Undergraduate Practical
1. The document describes an experiment to test the validity of the Nernst equation by measuring the voltage of electrochemical cells containing varying concentrations of zinc or magnesium ions.
2. Results show cell voltage decreases with decreasing log of the concentration of zinc ions, following the linear relationship predicted by the Nernst equation.
3. A magnesium-copper cell is also constructed, producing enough voltage to power a small LED, demonstrating a spontaneous redox reaction and energy conversion.
chemical kinetics.pdf
This document provides information on various topics in electrochemistry. It defines electrolytes and non-electrolytes, and discusses different types of conductors. It also explains electrochemical cells and electrolytic cells. Key concepts covered include electrode potential, the electrochemical series, Faraday's laws of electrolysis, and different types of batteries.
Electrochemistry
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.
Band edge engineering of composite photoanodes for dye sensitized solar cells
This document discusses engineering the band edges of composite photoanodes for dye-sensitized solar cells through doping. Specifically, it doped ZnO nanorods with cobalt to lower its conduction band minimum and doped TiO2 nanoparticles with zirconium to raise its conduction band minimum in order to overcome an energy barrier preventing electron transfer. Characterization with diffuse reflectance spectroscopy and open circuit voltage measurements under illumination confirmed the doping shifted the band edges as intended. However, dye-sensitized solar cells fabricated with the composite nanostructures did not show improved performance. The paper details a methodology for producing and measuring band edge shifts but notes limitations in applying it to improve device operation.
Zr doped TiO2 nanocomposites for dye sensitized solar cells
This document discusses engineering the band edges of a composite photoanode for dye-sensitized solar cells through doping. ZnO nanorods were doped with cobalt to lower their conduction band minimum energy, and TiO2 nanoparticles were doped with zirconium to raise their conduction band minimum energy. This was done to overcome an energy barrier that previously prevented electron transfer from TiO2 to ZnO in the composite. Characterization showed the doping incorporated into the materials as desired without other changes. Open circuit photovoltage measurements indicated the doping shifted the band energies to enable electron transfer, but devices using the materials did not show improved performance. The methodology for producing and measuring band edge shifts through doping is detailed.
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Electroplating
- 1. Electroplating to makeElectroplating to make nanostructuresnanostructures
- 2. Electroplating - The chemical conversion of ions in solution into a solid deposit of metal atoms with the work of a electrical power supply Cu2+ Cu2+ Cu2+ Cu solid Cu ions in solution 2e- Cu2+ + 2e- –> Cu(0) Mz+ + ze- –> M(0)
- 3. Electroplating Cell V I Cu2+ + 2e- –> Cu(0) "reduction" CuSO4 dissolved in water Cu(0) –> Cu2+ + 2e- "oxidation" anodecathode If using an inert Pt electrode: 2 H2O –> O2 + 4H+ + 4e- Working Electrode (WE) Counter Electrode (CE)
- 4. Amount of Deposition The number of atoms deposited is proportional to the number of electrons passed through the circuit - We can determine this by measuring the current I = dq dt Q = I dt 0 t ∫ = It If I is constant # electrons = Q/e = It/e where e = 1.6 x 10-19 C # atoms = # electrons/z = It/ez # moles of atoms = # atoms/NA = It/ezNA eNA = (1.6 x 10-19 C)(6.02 x 1023 ) = 96,500 C = F = "1 Faraday" # moles of atoms = It/Fz Cu2+ 2e- ammeter I
- 5. Amount of Deposition (cont.) # moles of atoms = It/Fz m = mass = (It/Fz)(gram atomic weight) t = film thickness = (mass)/(density • area) = m/(ρA) e.g., AWCu = 63.55 g/mole Cu2+ 2e- ammeter I Note that these equations assume 100% current efficiency (CE) - that is, assuming that all of the electrons are used for converting metal ions. However, another reduction reaction may compete for electrons making the CE less than 100%. For example, 2H+ + 2e- –> H2 . CE must be determined by an independent measurement.
- 6. Why choose electroplating toWhy choose electroplating to make nanostructures??make nanostructures?? The process is easy to operate and only needs simple equipment. It’s simple to control the deposition rate by controlling the voltage or current. It’s a good way to make Nanowires in a porousIt’s a good way to make Nanowires in a porous template.template.
- 7. Electrodeposited Nanowires nanoporous template nanowires in a polycarbonate filter nanowires in a diblock copolymer template
- 8. Application Data storage elementsData storage elements 1 0 0 1 1 If the nanowires are magnetic, they can be used to store data (arrow indicates the direction of magnetization)
Editor's Notes
- Pulse reverse electrodeposition results in improved microcrystalline structure and improved magnetic properties (larger perpendicula magnetocrystalline anisotropy)