The lemon battery How do batteries work ?. How can you get energy ?  Energy cannot be created or destroyed, but it can be saved in various forms. One.

Slides:



Advertisements
Similar presentations
Electrolytes: Conductors of Electricity Discovering the hidden secrets of lemons!
Advertisements

BatteriesBatteries How Batteries Work. Three Main Components of Batteries Negative terminal (anode): an electrode made of a metal such as zinc that accumulates.
Electrochemical & Voltaic Cells
Electrochemical Cells
Cells and Voltage.
Galvanic Cells What will happen if a piece of Zn metal is immersed in a CuSO 4 solution? A spontaneous redox reaction occurs: Zn (s) + Cu 2 + (aq) Zn 2.
Electrochemical Cells. Definitions Voltaic cell (battery): An electrochemical cell or group of cells in which a product-favored redox reaction is used.
VIII. Oxidation-Reduction J Deutsch An oxidation-reduction (redox) reaction involves the transfer of electrons (e - ). (3.2d) The oxidation numbers.
Batteries don’t store charge. They store energy. A chemical battery works because electrons like to leave some materials to go to others. The change in.
Electrochemistry The study of chemical reactions that produce electrical current or are driven to occur by applying an electrical current. Chemical potential.
Aim: What are electrochemical cells?
Section 18.1 Electron Transfer Reactions 1.To learn about metal-nonmetal oxidation–reduction reactions 2.To learn to assign oxidation states Objectives.
Electrochemistry AP Chapter 20. Electrochemistry Electrochemistry relates electricity and chemical reactions. It involves oxidation-reduction reactions.
Chapter 22 REDOX.
Electrochemistry. Electrochemical Cells  Electrons are transferred between the particles being oxidized and reduced  Two types –Spontaneous = Voltaic.
Batteries use chemical reactions to produce electricity, but how do the chemical reactions work? Chemicals used in batteries can do two things: i) release.
Section 10.3—Batteries & Redox Reactions
GALVANIC AND ELECTROLYTIC CELLS
ELECTROCHEMICAL CELLS
Electroplating. The electroplating of an object with metal is accomplished using an electrolytic cell. There are some basic rules for electroplating.
Electrochemistry.
Chapter 21.  Two types: ◦ Voltaic cell: electrons flow spontaneously ◦ Electrolytic cell: electrons are forced to flow.
Chapter 26 – Electricity from Chemical Reactions.
Electrochemical Cells - producing an electric current with a redox reaction.
 Learners must be able to define galvanic cell in terms of electrode reaction. e.g. salt bridge.(N.B. anode and cathode)  Learners must be able to do.
ELECTROCHEMICAL CELLS In redox reactions, there is a chemical reaction and an exchange of electrons between the particles being oxidized and reduced. An.
Topic: Redox Aim: What are electrochemical cells? Do Now: Which of the following ions is most easily reduced? 1)Li+ 2) K+ 3) Ca 2+ 4) Na+ HW:
REVISION ELECTROCHEMISTRY. OXIDATION is a loss of electrons An increase in oxidation number REDUCTION is a gain of electrons A decrease in oxidation number.
Current Electricity Part 2
10.3 Electric Potential. Electric Potential Electric potential refers to the amount of energy that electrons possess in a circuit.
Topic 10 Making Electricity. Aim: To learn more about the batteries we use everyday.
Electrochemistry Cells and Batteries.
Electrochemistry. Electrochemistry is the study of the relationship between the flow of electric current and chemical changes, including the conversion.
Electrolytic Cells. Endothermic.Use electricity to force a nonspontaneous reaction to occur. Endothermic. Electrolytic cells can be identified by the.
Electrolytic Cells Section 9.2. Vocabulary Electrolysis: electrical energy used to bring about a non-spontaneous redox reaction Electrolyte: any substance.
Electrochemical Reactions. Anode: Electrons are lost due to oxidation. (negative electrode) Cathode: Electrons are gained due to reduction. (positive.
ELECTROCHEMICAL CELLS. ELECTROCHEMISTRY The reason Redox reactions are so important is because they involve an exchange of electrons If we can find a.
Electrochemical Cells. Electrochemical Electrochemical cells are a way of storing chemical potential energy. When batteries operate, electrons in high.
Building a Lemon Battery To begin to understand how batteries work, I can help to build simple chemical cells using readily available materials which can.
ELECTROCHEMISTRY Electrochemistry relates electricity and chemical reactions. It involves oxidation-reduction reactions (aka – redox) They are identified.
Electrochemical Reactions. Anode: Electrons are lost due to oxidation. (negative electrode) Cathode: Electrons are gained due to reduction. (positive.
Electrolytic Cells utilizes electrical energy to create chemical energy.
ELECTROCHEMISTRY Presentation by: P.K. CHOURASIA K.V MANDLA, Jabalpur Region.
mr4iE. batteries containers of chemicals waiting to be converted to electricity the chemical reaction does not.
Voltaic Cells Notes A.) Spontaneous reaction 1.) In Voltaic Cells (Batteries), when the circuit is closed (turned on) electrons will move from anode.
Oxidation-Reduction Reactions
Electrochemical Cells
Chapter 10.7 Electrolysis.
Show Video:
Electrochemistry and The Chemical Cells.
Electrochemical Cells
utilizes electrical energy to create chemical energy
Electrolytic Cells.
Chemistry/Physical Setting
Electrochemistry.
The Electric Battery Volta discovered that electricity could be created if dissimilar metals were connected by a conductive solution called an electrolyte.
An electrolytic cell uses electricity to do a chemical reaction.
Electrochemistry i.e. This is the End!.
Chemical Potential Energy
Electrochemistry AP Chapter 20.
utilizes electrical energy to create chemical energy
Electrochemistry Lesson 3
Cells and Batteries.
Electrochemical Cells (Batteries)
AP Chem Get HW checked Work on oxidation # review
Chemical Potential Energy
AP Chem Get HW checked Take out laptops and go to bit.ly/GalCell
IX. Oxidation-Reduction
A. Oxidation-Reduction Reactions
Batteries How Batteries Work.
Presentation transcript:

The lemon battery How do batteries work ?

How can you get energy ?  Energy cannot be created or destroyed, but it can be saved in various forms. One way to store it is in the form of chemical energy in a battery. When connected in a circuit, a battery can produce electricity.  What is a circuit ?Play the game below.  ps/ages/10_11/changing_circuits.shtml ps/ages/10_11/changing_circuits.shtml

How do batteries work ?  Batteries convert Chemical Energy into Electrical Energy  A battery has two ends -- a positive terminal (cathode) and a negative terminal (anode). If you connect the two terminals with wire, a circuit is formed. Electrons will flow through the wire and a current of electricity is produced. Inside the battery, a reaction between chemicals take place. But the reaction takes place only if there is a flow of electrons. Batteries can be stored for a long time and still work because the chemical process doesn't start until the electrons flow from the negative to the positive terminals through a circuit. How does a lemon battery work?

How does the lemon battery work ? How do I make one ?  A lemon battery is made with a lemon and two metallic electrodes of different metals such as a copper penny or wire and a galvanized (zinc coated) nail.  The energy for the battery does not come from the lemon, but rather the chemical change in zinc (or other metal). The zinc is oxidized inside the lemon, exchanging some of its electrons in order to reach a lower energy state, and the energy released provides the power. The lemon merely provides an environment where this can happen, but they are not used up in the process..  /watch?v=mS8Zw4JOvvg /watch?v=mS8Zw4JOvvg  /watch?v=olhfjvUE- Fo&feature=related /watch?v=olhfjvUE- Fo&feature=related  /watch?v=2uncoL3R34c&f eature=related /watch?v=2uncoL3R34c&f eature=related  /watch?v=REZQES5XuAY& feature=related /watch?v=REZQES5XuAY& feature=related

Lab directions  y.org/franklin/fun/l emon.htm y.org/franklin/fun/l emon.htm  Click on the above link and read how to do the lab. Turn to lesson #4 in your student book.

When the lab is over…take this test, we will discuss answers together.  What causes electrons to flow through the wire is:  a) a gravitational potential forces electrons through the wire  b) acids push the electrons through the wire  c) a potential difference between anode and cathode pushes electrons through the wire  d) electrons do not flow through the wire but through the electrolyte  Which statement is true about a lemon battery?  a) The energy for the battery does not come from the lemon, but rather the chemical change in zinc (or other metal)  b) The battery is made with two metallic electrodes of different metals such as a copper penny or wire and a galvanized nail.  c) In a lemon battery, both oxidation (loss of electrons) and reduction (gain of electrons) occur.  d) All of the above are correct