Electroplating. The electroplating of an object with metal is accomplished using an electrolytic cell. There are some basic rules for electroplating.

Slides:

Advertisements

Similar presentations

Types of cells – – – Overview Cells are containers of liquid with electrodes: In electrolytic cells, electricity is used to force chemicals to.

Advertisements

BatteriesBatteries How Batteries Work. Three Main Components of Batteries Negative terminal (anode): an electrode made of a metal such as zinc that accumulates.

Electric cells  a simple electric cell consists of two different metal electrodes placed in an electrolyte  metals high up in the reactivity series give.

Oxidation Reduction Regents Review.

Cells and Voltage.

Cells and Voltage.

Balance Redox Rxns: Fe(OH) 3 + [Cr(OH) 4 ] -1 Fe(OH) 2 + CrO 4 -2 in base.

Electrolytic Cell and Electroplating Chapter 19 Page Chem 12.

OB: Redox Class #4 Voltaic vs. Electrolytic cells Voltaic cells has chemistry spontaneously produce electricity. The other kind of electrochemical cell,

What does this?. Have to do with this? NOTHING!!!

Oxidation Reduction Chemisty: Redox Chemistry

Yr 10 Electrolysis project. Yr 10 Electrolysis project.

Electroplating By: Matthew Nerhing. What is Electroplating? Electroplating- It is the deposition of a thin layer of metal on a surface by an electrical.

Electroplating Aims: Describe how to electroplate an object

ELECTROLYSIS. Compare and contrast voltaic (galvanic) and electrolytic cells Explain the operation of an electrolytic cell at the visual, particulate.

Chapter 20 Preview Multiple Choice Short Answer Extended Response

Aim: What are electrochemical cells?

Redox: Oxidation and Reduction Definitions Oxidation: loss of e- in an atom increase in oxidation number (ex: -1  0 or +1  +2)  Reduction: gain of.

Electrolysis Electrolysis of Water.

Chapter 22 REDOX.

Balance Redox Rxns: Fe(OH) 3 + [Cr(OH) 4 ] -1 Fe(OH) 2 + CrO 4 -2 in base.

An Introduction to Electroanalytical Chemistry Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of.

Balance Redox Rxns: Fe(OH) 3 + [Cr(OH) 4 ] -1 Fe(OH) 2 + CrO 4 -2 in base.

GALVANIC AND ELECTROLYTIC CELLS

ELECTROCHEMICAL CELLS

Electrochemistry.

Chapter 21.  Two types: ◦ Voltaic cell: electrons flow spontaneously ◦ Electrolytic cell: electrons are forced to flow.

JUST REMEMBER... “OIL RIG” (oxidation is losing, reduction is gaining)

Electrochemistry or REDOX Unit 9. I. The Vocabulary of Electrochemistry A] Electrochemsitry is…… The field of chemistry studying reactions resulting from.

Electrochemical Cells - producing an electric current with a redox reaction.

1 AnodeCathode Basic Concepts of Electrochemical Cells.

Mr. Chapman Chemistry 30 ELECTROCHEMICAL CELLS AND REDOX REACTIONS.

Electrochemical cell. Parts of a Voltaic Cell The electrochemical cell is actually composed to two half cells. Each half cell consists of one conducting.

ELECTROCHEMICAL CELLS In redox reactions, there is a chemical reaction and an exchange of electrons between the particles being oxidized and reduced. An.

Voltaic Cells/Galvanic Cells and Batteries. Background Information Electricity is the movement of electrons, and batteries are an important source of.

Galvanic Cells ELECTROCHEMISTRY/CHEMICAL REACTIONS SCH4C/SCH3U.

Electrochemistry. Electrochemistry is the study of the relationship between the flow of electric current and chemical changes, including the conversion.

Electroplating By: Matthew Nerhing. What is Electroplating? Electroplating- It is the deposition of a thin layer of metal on a surface by an electrical.

Unit 2: Electrochemistry Electrolysis

Electrolytic Cells. Endothermic.Use electricity to force a nonspontaneous reaction to occur. Endothermic. Electrolytic cells can be identified by the.

By: Steph Magill.  Electroplating- The process of coating an electrically conducting surface with a thin layer (seldom more than in [0.025 mm]

Electrolytic Cells.

Electrolytic Cells Section 9.2. Vocabulary Electrolysis: electrical energy used to bring about a non-spontaneous redox reaction Electrolyte: any substance.

In many applications, a very pure form of a specific metal is required. One method used to purify a metal is called electrorefining. It uses a Type 3 Electrolytic.

ELECTROCHEMICAL CELLS. ELECTROCHEMISTRY The reason Redox reactions are so important is because they involve an exchange of electrons If we can find a.

Electrolytic Cells Chemistry Chapter 19 E.

Electrochemistry Introduction Voltaic Cells. Electrochemical Cell  Electrochemical device with 2 half-cells with electrodes and solutions  Electrode—metal.

Electrochemical Cells. Electrochemical Electrochemical cells are a way of storing chemical potential energy. When batteries operate, electrons in high.

Electrolytic Cells. An electrolytic cell is an electrochemical cell that undergoes a redox reaction when electrical energy is applied. It is most often.

1 REVERSIBLE ELECTROCHEMISTRY 1. Voltaic Or Galvanic Cells Voltaic or Galvanic cells are electrochemical cells in which spontaneous oxidation- reduction.

Oxidation-Reduction (aka Redox) Reactions These are electron- transfer reactions! om/ICT/rr/redox1.html.

mr4iE. batteries containers of chemicals waiting to be converted to electricity the chemical reaction does not.

Electrochemistry Chapter 18. Electrochemistry –the branch of chemistry that studies the electricity- related application of oxidation-reduction reactions.

Electro-chemistry: Batteries and plating Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of electrons.

Aim: What are electrochemical cells? DO Now: 1.Complete sheet from yesterday. If done compare answers with partner. 2.Pass down homework.

You will have to completely label a diagram to look like this

Redox in Action: Voltaic cells

Electrochemical cells

Chapter 15 Oxidation and Reduction

Au Au3+ - ELECTROLYSIS SLIDE ONE OVERVIEW ANIMATION 3e- +

Electrolytic Cells Aim: Write half reactions for electrolysis of a salt and electroplating.

Chapter 10 Electrolytic Cells 10.7.

1. Introduction to Electrochemical Cells

10.2 Electrochemistry Objectives S2

Electrolytic Cells.

Chapter 10 ELECTROLYTIC CELLS 10.7.

Aim # 36: What is the difference between a

Electrochemistry Lesson 3

Write the oxidation half reaction for lithium oxidizing

Batteries How Batteries Work.

Presentation transcript:

Electroplating

The electroplating of an object with metal is accomplished using an electrolytic cell. There are some basic rules for electroplating.  The object to be plated must always be the cathode in the electrolytic cell. Thus, it must always be connected to the negative pole of the electric source.  The anode in the electrolytic cell must be made from the plating metal.  The electrolyte used in the electrolytic cell must contain the cation of the plating metal.

off Ag AgNO 3(aq) Ag + -+ power source on Ag NO 3 - e-e- e-e- e- e-  e- e-  e- e-   e- e- e-e- e-e- Ag Ag + Copper spoon Electroplating cathodeanode

Electroplating Ex.1) Electrons enter into the ____ (+/-) pole of a battery and exit out from the ____(+/-) pole of the a battery. Ex.2) When electroplating, the electrolyte used needs to contain the same metal as the _______________ __________ Ex.3) In the electrolytic process used to plate pure copper onto the surface of a material, the material should be connected in the electroplating device as the (1) cathode which is positive (2) cathode which is negative (3) anode which is positive (4) anode which is negative + _ plating metal

Electroplating Ex.4) Which of the following cells is set up properly to electroplate a silver spoon with gold? (1) (3) (2)(4) battery - + AgNO 3(aq) Ag (s) battery - + Au(NO 3 ) 3(aq) Au (s) battery + - AgNO 3(aq) Ag (s) battery + - Au(NO 3 ) 3(aq) Au (s)

Electroplating Ex.5) Complete the set up in order to electroplate the piece of zinc pipe with copper. [DRAW LINES TO REPRESENT THE WIRES] The metal strip is made of ____________ What salt would you add? ____________ Battery + - copper Cu(NO 3 ) 2

Electroplating Ex. (6) The diagram below shows a key to be plated with silver in an electrolytic cell. Draw lines from the battery to the key and from the battery to the silver electrode to correctly set-up the electrolytic cell. + - Battery  Silver electrode AgNO 3 solution A B

Electroplating Ex. (7) Given the reduction reaction for the cell above: Ag 1+ (aq) + 1e - → Ag (s) This reaction occurs at (1) A, which is the anode (2) A, which is the cathode (3) B, which is the anode (4) B, which is the cathode  + - Battery Silver electrode AgNO 3 solution A B