17.2 Galvanic Cells
2 min read•june 25, 2024
convert chemical energy into electrical energy through redox reactions. These cells consist of two connected by a , with electrons flowing from the to the through an external circuit.
Understanding components is crucial for grasping concepts. The undergoes , releasing electrons, while the accepts electrons in a reaction. The salt bridge maintains charge balance, allowing for continuous .
Galvanic Cell Components and Function
Components of galvanic cells
Top images from around the web for Components of galvanic cells
17.2 Galvanic Cells | Chemistry View original
Is this image relevant?
Electrochemistry: cells and electrodes View original
Is this image relevant?
Electrochemical Cells | Boundless Chemistry View original
Is this image relevant?
17.2 Galvanic Cells | Chemistry View original
Is this image relevant?
Electrochemistry: cells and electrodes View original
Is this image relevant?
1 of 3
Top images from around the web for Components of galvanic cells
17.2 Galvanic Cells | Chemistry View original
Is this image relevant?
Electrochemistry: cells and electrodes View original
Is this image relevant?
Electrochemical Cells | Boundless Chemistry View original
Is this image relevant?
17.2 Galvanic Cells | Chemistry View original
Is this image relevant?
Electrochemistry: cells and electrodes View original
Is this image relevant?
1 of 3
- Anode occurs releases electrons negative electrode
- (in Zn-Cu cell)
- Cathode reduction occurs accepts electrons positive electrode
- (in Zn-Cu cell)
- Salt bridge allows ion flow maintains charge balance prevents mixing of half-cell solutions
- Contains or solution (in Zn-Cu cell)
- measures potential difference (voltage) between electrodes
- Typical values range from 0.1 V to 3 V (Zn-Cu cell ~1.1 V)
- each electrode immersed in solution containing its ions
- Oxidation half-cell contains anode species being oxidized ( in solution)
- Reduction half-cell contains cathode species being reduced ( in solution)
- Electron flow occurs from anode to cathode through external circuit
Cell notation for galvanic cells
- Shorthand representation of galvanic cells
- General format: Anode | Anode Electrolyte || Cathode Electrolyte | Cathode
- Anode on left cathode on right
- Single vertical line (|) separates electrode from electrolyte
- Double vertical line (||) separates two half-cells
-
- is anode is cathode
- and are in respective half-cells
Active vs inert electrodes
- Active electrodes participate in redox reaction
- Electrode material consumed or deposited during reaction
- , , ,
- Inert electrodes do not participate in redox reaction
- Electrode material acts as surface for electron transfer
- , ,
- In - galvanic cell:
- is active electrode (anode) oxidized and consumed
- is active electrode (cathode) reduced and deposited on electrode
Electrochemical Potentials and Calculations
- (E°) measures tendency of half-reaction to occur
- ranks half-reactions by standard reduction potentials
- relates cell potential to concentration and temperature
- Electrochemistry studies chemical reactions involving electric charges
Key Terms to Review (37)
Anode: The anode is the electrode where oxidation occurs in a galvanic cell. It is typically the negative terminal in such cells.
Anode: The anode is the electrode in an electrochemical cell where oxidation occurs, and electrons are released to flow through an external circuit. It is the negatively charged electrode that attracts positively charged ions and initiates the flow of electrons in a redox reaction.
Cathode: The cathode is the electrode where reduction occurs in an electrochemical cell. It is the positive terminal in a galvanic cell.
Cathode: A cathode is an electrode where reduction occurs during an electrochemical reaction. It plays a crucial role in various processes such as galvanic cells, where it attracts cations from the electrolyte, facilitating the flow of electric current. Understanding the function of the cathode is essential for grasping concepts like electrode potentials and energy transformations in electrochemical cells.
Cell Notation: Cell notation is a standardized way of representing the components and structure of an electrochemical cell, particularly in the context of galvanic or voltaic cells. It provides a concise and organized method for describing the essential elements of a cell and the direction of electron flow.
Cell notations: Cell notation is a shorthand representation of a galvanic cell, showing the components of each half-cell and their arrangement. It typically follows the format: anode | anode solution (concentration) || cathode solution (concentration) | cathode.
Cell schematics: Cell schematics are symbolic representations of electrochemical cells used to describe the components and reactions occurring within them. They illustrate the arrangement of electrodes, electrolyte solutions, and the direction of electron flow.
Chemical reduction: Chemical reduction is a process in which an element or compound gains electrons, resulting in a decrease in its oxidation state. It often occurs alongside oxidation in redox reactions.
Copper: Copper is a reddish-brown metallic element that is an essential mineral for human health and has numerous applications in various industries. It is a transition metal that exhibits unique chemical properties, making it an important component in many chemical processes and technological advancements.
Electrochemical Series: The electrochemical series, also known as the activity series or reactivity series, is a ranking of elements based on their tendency to lose or gain electrons during chemical reactions. This series is a fundamental concept in the understanding of galvanic cells and electrode potentials.
Electrochemistry: Electrochemistry is the study of the relationship between electrical energy and chemical energy, and the interconversion between the two. It involves the study of chemical reactions that produce electricity and the use of electrical energy to drive chemical reactions.
Electrolyte: An electrolyte is a substance that, when dissolved in a solvent such as water, dissociates into charged particles called ions. These ions are capable of conducting electricity and are essential for various chemical and physiological processes in the body and in electrochemical devices.
Electrolytes: Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. Common examples include salts, acids, and bases.
Electron Flow: Electron flow refers to the movement of electrons through a conductive material, such as a metal or a solution, driven by a difference in electrical potential. This flow of electrons is a fundamental concept in understanding the operation of electrochemical cells, particularly galvanic cells, where it is the driving force behind the generation of electrical energy.
Electron volts (eV): An electron volt (eV) is a unit of energy equal to the amount of kinetic energy gained by an electron when it is accelerated through an electric potential difference of one volt. It is commonly used in nuclear and particle physics to express small amounts of energy.
Galvanic Cell: A galvanic cell, also known as a voltaic cell, is an electrochemical cell that generates an electric current through a spontaneous redox (reduction-oxidation) reaction. It is a device that converts the chemical energy of a spontaneous redox reaction into electrical energy.
Galvanic cells: Galvanic cells, also known as voltaic cells, are electrochemical cells that convert chemical energy into electrical energy through spontaneous redox reactions. They consist of two half-cells connected by a salt bridge and an external circuit.
Gold: Gold is a precious, dense, and highly valued metal that has been prized throughout human history for its unique properties and applications. It is a transition metal that is widely used in various industries, from jewelry and electronics to medicine and dentistry.
Graphite: Graphite is a crystalline form of carbon, known for its unique layered structure and excellent electrical conductivity. Its arrangement allows for the easy movement of electrons, making it useful in various applications, such as batteries and lubricants. In addition to its electrical properties, graphite also exhibits remarkable thermal stability and mechanical strength, distinguishing it from other carbon allotropes.
Half-cells: Half-cells are the two sections of an electrochemical cell where oxidation and reduction reactions occur separately. Each half-cell contains a conductive electrode and an electrolyte solution.
Half-Cells: A half-cell is an electrochemical system consisting of a metal or ion in a solution of its own ions, with an electrode immersed in the solution. Half-cells are the fundamental building blocks of galvanic cells, which are devices that generate electrical energy through spontaneous redox reactions.
Inert electrode: An inert electrode is a conductive material that does not participate in the chemical reaction of an electrochemical cell. It serves as a surface for the transfer of electrons.
Magnesium: Magnesium is a chemical element with the symbol Mg and atomic number 12. It is an essential mineral that plays a vital role in numerous bodily functions and is closely connected to the topics of periodic variations in element properties and galvanic cells.
Nernst Equation: The Nernst equation is a fundamental relationship in electrochemistry that describes the relationship between the reduction potential of an electrochemical half-reaction and the activities of the chemical species involved. It is a crucial tool for understanding and predicting the behavior of galvanic cells, electrode potentials, and the spontaneity of electrochemical processes.
Oxidation: Oxidation is a chemical reaction where an atom, ion, or molecule loses electrons. It often involves gaining oxygen or losing hydrogen.
Oxidation: Oxidation is a fundamental chemical process in which an element or compound loses electrons, resulting in an increase in its oxidation state. This term is central to understanding redox (reduction-oxidation) reactions, the functioning of electrochemical cells, corrosion, and the properties and behavior of oxygen, sulfur, and various organic compounds.
Platinum: Platinum is a rare, silvery-white metal that is highly valued for its catalytic properties and use in various electrochemical applications. Its unique chemical and physical characteristics make it an essential element in numerous industries and scientific fields.
Platinum metals: Platinum metals, also known as the platinum group metals (PGMs), are a group of six transition metals that include platinum, palladium, rhodium, ruthenium, iridium, and osmium. These metals are known for their excellent catalytic properties and resistance to wear and tarnish.
Potassium Chloride: Potassium chloride is an ionic compound consisting of the elements potassium and chlorine. It is an essential mineral that plays a crucial role in various physiological processes within the body, including nerve and muscle function, as well as fluid balance regulation.
Potassium Nitrate: Potassium nitrate is an inorganic salt with the chemical formula KNO3. It is a colorless, crystalline solid that is widely used in various applications, including the production of fertilizers, pyrotechnics, and as an oxidizing agent in chemical reactions.
Reduction: Reduction is a chemical process in which a substance gains electrons, resulting in a decrease in its oxidation state. It is a key concept in redox (reduction-oxidation) reactions, where substances are either reduced or oxidized to facilitate the transfer of electrons.
Salt bridge: A salt bridge is a device used in electrochemical cells to maintain electrical neutrality by allowing the transfer of ions. It typically consists of a tube filled with a salt solution or gel that connects the two half-cells.
Silver: Silver is a lustrous, soft, and malleable transition metal with a wide range of applications in various industries, including electronics, jewelry, and photography. It is known for its unique properties, such as high electrical and thermal conductivity, as well as its antimicrobial and corrosion-resistant characteristics.
Standard Electrode Potential: The standard electrode potential is a measure of the tendency of an electrode to gain or lose electrons when it is in its standard state, which is defined as the potential of the electrode when it is in its standard state and the reaction is at standard conditions (25°C, 1 atm pressure, and 1 M concentration of all solutes). It is a fundamental concept in electrochemistry and is used to predict the direction and spontaneity of redox reactions.
Volt: The volt (symbol: V) is the derived unit for electric potential difference and electromotive force in the International System of Units (SI). It is named after the Italian physicist Alessandro Volta, who invented the first electric battery. The volt is the potential difference across a resistance of one ohm when a current of one ampere is flowing through it.
Voltmeter: A voltmeter is an electronic instrument used to measure the potential difference, or voltage, between two points in an electrical or electronic circuit. It is a crucial tool in the study of galvanic cells, which are electrochemical cells that generate electricity through spontaneous redox reactions.
Zinc: Zinc is a metallic element that plays a crucial role in various biological processes within the human body. It is an essential mineral required for the proper functioning of numerous enzymes and is involved in a wide range of physiological activities, including immune system function, wound healing, and protein synthesis.