The document summarizes key concepts related to electrochemistry including electrolysis, electrolysis of molten and aqueous ionic compounds, electroplating, and hydrogen fuel cells. Electrolysis is the decomposition of ionic compounds using electricity. During electrolysis, ions are discharged at the electrodes. For molten compounds, the metal and non-metal products form. For aqueous solutions, the products depend on ion and metal reactivity. Electroplating coats objects with metal through electrolysis. Hydrogen fuel cells use hydrogen and oxygen to produce electricity and water.
This document discusses the electrolysis of brine solution (concentrated NaCl) to produce sodium hydroxide and chlorine gas. During electrolysis, sodium and hydrogen ions move to the cathode while chlorine and hydroxide ions move to the anode. At the cathode, only hydrogen ions are discharged to form hydrogen gas. At the anode, chlorine ions are discharged to form chlorine gas, leaving behind a solution of sodium hydroxide. A diaphragm cell is used to separately collect the chlorine gas and sodium hydroxide solution produced. Sodium hydroxide has uses including in soap production and paper making. Chlorine gas has uses as a bleaching agent and to produce hydrochlor
1. Electrolysis is the process of using electricity to cause non-spontaneous chemical reactions by passing a current through an electrolyte solution or molten compound.
2. An electrolytic cell contains two electrodes (an anode and a cathode), an electrolyte, and a power source like a battery.
3. During electrolysis, cations move toward the cathode and gain electrons through reduction reactions. Anions move toward the anode and lose electrons through oxidation reactions.
Electrolysis is the process of using electricity to cause a non-spontaneous chemical reaction. During electrolysis, ions migrate towards the electrodes and undergo oxidation or reduction reactions. At the cathode, positively charged ions are reduced and neutral atoms are formed. At the anode, negatively charged ions are oxidized and neutral atoms or molecules are formed. The products of electrolysis depend on factors like the ions present in the electrolyte, their concentration and position in the reactivity series, and the nature of the electrodes. Electrolysis has applications in purifying and extracting metals, and in electroplating.
This document discusses factors that determine which ions are discharged at the electrodes during electrolysis. For molten compounds containing one cation and one anion, the cation will be reduced at the cathode and the anion will be oxidized at the anode. For compounds in solution, the position of ions in the electrochemical series and concentration determine which ions are discharged. Ions higher in the anion series and lower in the metal series are preferentially discharged at the anode and cathode respectively. In dilute solutions, OH- and H+ ions are discharged but in concentrated solutions the ions from the compound may be discharged instead.
1. The document discusses the reactivity series and how it arranges metals in order of their reactivity based on their tendency to form positive ions.
2. Key reactions include displacement reactions where a more reactive metal can displace a less reactive one from a compound. Metals also react with oxygen to form metal oxides.
3. Extraction of metals using carbon and electrolysis is covered, where metals less reactive than carbon can be extracted from their oxides by reduction, and how electrolysis uses electricity to extract metals that are too reactive to be extracted by carbon.
Electrolysis is the process of using a direct electric current to drive nonspontaneous chemical reactions. It involves the decomposition of an electrolyte into its constituent ions by the removal or addition of electrons to the ions. During electrolysis, ions migrate to the electrodes where they undergo oxidation or reduction reactions. In the electrolysis of molten lead bromide, lead ions are reduced to metallic lead at the cathode, while bromide ions are oxidized to bromine gas at the anode. When an aqueous solution of copper sulfate is electrolyzed using copper electrodes, copper ions are reduced at the cathode to form metallic copper while oxygen gas forms at the anode. Electrolysis requires an electrolyte, electrodes, and a direct current power
During electrolysis, redox reactions occur where ions are reduced or oxidized at the electrodes. At the cathode, ions gain electrons through reduction reactions and at the anode, ions lose electrons through oxidation reactions. The overall reactions in electrolysis depend on the electrolyte, but generally involve the transfer of electrons between electrodes to split the electrolyte into separate elements or compounds.
During electrolysis, redox reactions occur where ions are reduced or oxidized at the electrodes. At the cathode, ions gain electrons through reduction reactions and at the anode, ions lose electrons through oxidation reactions. The overall reactions in electrolysis depend on the electrolyte, with common products including hydrogen, oxygen, chlorine and metals.
This document discusses the electrolysis of brine solution (concentrated NaCl) to produce sodium hydroxide and chlorine gas. During electrolysis, sodium and hydrogen ions move to the cathode while chlorine and hydroxide ions move to the anode. At the cathode, only hydrogen ions are discharged to form hydrogen gas. At the anode, chlorine ions are discharged to form chlorine gas, leaving behind a solution of sodium hydroxide. A diaphragm cell is used to separately collect the chlorine gas and sodium hydroxide solution produced. Sodium hydroxide has uses including in soap production and paper making. Chlorine gas has uses as a bleaching agent and to produce hydrochlor
1. Electrolysis is the process of using electricity to cause non-spontaneous chemical reactions by passing a current through an electrolyte solution or molten compound.
2. An electrolytic cell contains two electrodes (an anode and a cathode), an electrolyte, and a power source like a battery.
3. During electrolysis, cations move toward the cathode and gain electrons through reduction reactions. Anions move toward the anode and lose electrons through oxidation reactions.
Electrolysis is the process of using electricity to cause a non-spontaneous chemical reaction. During electrolysis, ions migrate towards the electrodes and undergo oxidation or reduction reactions. At the cathode, positively charged ions are reduced and neutral atoms are formed. At the anode, negatively charged ions are oxidized and neutral atoms or molecules are formed. The products of electrolysis depend on factors like the ions present in the electrolyte, their concentration and position in the reactivity series, and the nature of the electrodes. Electrolysis has applications in purifying and extracting metals, and in electroplating.
This document discusses factors that determine which ions are discharged at the electrodes during electrolysis. For molten compounds containing one cation and one anion, the cation will be reduced at the cathode and the anion will be oxidized at the anode. For compounds in solution, the position of ions in the electrochemical series and concentration determine which ions are discharged. Ions higher in the anion series and lower in the metal series are preferentially discharged at the anode and cathode respectively. In dilute solutions, OH- and H+ ions are discharged but in concentrated solutions the ions from the compound may be discharged instead.
1. The document discusses the reactivity series and how it arranges metals in order of their reactivity based on their tendency to form positive ions.
2. Key reactions include displacement reactions where a more reactive metal can displace a less reactive one from a compound. Metals also react with oxygen to form metal oxides.
3. Extraction of metals using carbon and electrolysis is covered, where metals less reactive than carbon can be extracted from their oxides by reduction, and how electrolysis uses electricity to extract metals that are too reactive to be extracted by carbon.
Electrolysis is the process of using a direct electric current to drive nonspontaneous chemical reactions. It involves the decomposition of an electrolyte into its constituent ions by the removal or addition of electrons to the ions. During electrolysis, ions migrate to the electrodes where they undergo oxidation or reduction reactions. In the electrolysis of molten lead bromide, lead ions are reduced to metallic lead at the cathode, while bromide ions are oxidized to bromine gas at the anode. When an aqueous solution of copper sulfate is electrolyzed using copper electrodes, copper ions are reduced at the cathode to form metallic copper while oxygen gas forms at the anode. Electrolysis requires an electrolyte, electrodes, and a direct current power
During electrolysis, redox reactions occur where ions are reduced or oxidized at the electrodes. At the cathode, ions gain electrons through reduction reactions and at the anode, ions lose electrons through oxidation reactions. The overall reactions in electrolysis depend on the electrolyte, but generally involve the transfer of electrons between electrodes to split the electrolyte into separate elements or compounds.
During electrolysis, redox reactions occur where ions are reduced or oxidized at the electrodes. At the cathode, ions gain electrons through reduction reactions and at the anode, ions lose electrons through oxidation reactions. The overall reactions in electrolysis depend on the electrolyte, with common products including hydrogen, oxygen, chlorine and metals.
This document provides an overview of electrolysis. It discusses the history of electrolysis, the process which involves using a direct electric current to drive a non-spontaneous chemical reaction. It also covers Faraday's laws of electrolysis, industrial uses such as producing aluminum and chlorine, and reactions that occur during electrolysis like the oxidation and reduction at electrodes. Specific techniques like electrolysis of water and electrocrystallization are also summarized.
- Alkali metals have low ionization energies and readily lose their outer electron to form cations with a +1 oxidation state. They are soft, reactive metals that form ionic compounds.
- Sodium is the second alkali metal and is found abundantly in nature as the mineral sodium chloride. It is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride at lower temperatures using calcium chloride. This allows pure sodium to be produced at the cathode and chlorine gas to be collected at the anode.
The document outlines key concepts in electrochemistry including:
1. Electrolysis involves using electricity to break down ionic compounds or solutions into their components. It occurs when ions are able to move freely in molten or aqueous states.
2. During electrolysis, cations move to the cathode where they gain electrons and undergo reduction reactions. Anions move to the anode where they lose electrons and undergo oxidation reactions.
3. The electrolysis of molten ionic compounds produces metals at the cathode and non-metals at the anode. Electrolysis of aqueous solutions can produce hydrogen and oxygen from water or discharge other ions depending on their reactivity.
Electrolytes are substances that can conduct electricity in the molten or liquid state and undergo chemical changes. Electrolysis is a process where electrolytes are broken down into their constituent elements by passing electricity through them. During electrolysis, ions migrate to the oppositely charged electrodes. At the anode, ions lose electrons and form gases or dissolve. At the cathode, ions gain electrons and form solid elements. Examples of electrolysis of molten lead(II) bromide and lead(II) oxide are described through their half reactions at the anode and cathode and overall reactions.
This document outlines learning outcomes for a chapter on electrochemistry. It describes key concepts such as classifying substances as conductors or non-conductors, different types of electrical conduction, electrolysis, oxidation and reduction reactions, and industrial applications of electrolysis. The document also defines important terms like electrolyte, cathode, anode, cation, anion, and Faraday's constant. It explains how to calculate masses and volumes of substances liberated during electrolysis.
The document outlines key concepts in electrochemistry including:
- Conductors and electrolytes allow electric currents through movement of charged particles. Electrolytes must be molten or dissolved.
- During electrolysis, cations move to the cathode and are reduced while anions move to the anode and are oxidized.
- Products depend on the electrolyte - molten salts produce metals at the cathode and nonmetals at the anode, while solutions can produce gases from water. Reactions follow selective discharge principles.
1. Electrochemistry involves chemical reactions caused by the introduction of electrical energy. Alessandro Volta discovered batteries in 1793 by placing different metals in water. (2) Berzelius later proposed that atoms are electrified, with metals being positive and non-metals negative. (3) Galvanic cells convert chemical energy to electrical energy through spontaneous redox reactions between two half-cells separated by a salt bridge.
Electrolysis is a process that uses electricity to separate substances. When an ionic substance is melted or dissolved in water, ions are free to move and an electric current can break them down into elements. During electrolysis, positive ions move to the negative cathode where they gain electrons and negative ions move to the positive anode where they lose electrons. Electrolysis of brine produces chlorine gas, hydrogen gas, and sodium hydroxide solution which have important industrial uses.
Electrochemistry is the study of electricity and how it relates to chemical reactions. In electrochemistry, electricity can be generated by movements of electrons from one element to another in a reaction known as redox or oxidation-reduction reaction.
The document discusses electrolysis and the principles behind it. It explains that electrolysis involves passing electricity through an electrolyte, which causes chemical decomposition. Ions migrate to the electrodes and are discharged. Metals are formed at the cathode by reduction, while non-metals or oxygen form at the anode by oxidation. It provides examples of electrolysis such as molten salts like NaCl and aqueous solutions like copper sulfate. Factors affecting ion discharge are also discussed.
The document outlines learning outcomes for a chapter on electrochemistry. It will describe investigations into classifying substances as conductors or non-conductors, distinguish between metallic and electrolytic conduction, define key terms like electrolysis, electrodes, and ions. It will also cover predicting reactions and products of electrolysis, calculating quantities produced using Faraday's constant, and discussing industrial applications of electrolysis.
This slide was prepared by me for I was given project on the course applied electro-chemistry. Am student at Addis Ababa university institute of technology , addis ababa Ethiopia
1. Electrolysis is the process of using electricity to cause non-spontaneous chemical changes.
2. During electrolysis, ions migrate towards the oppositely charged electrode - cations move towards the cathode and anions move towards the anode.
3. At the cathode, cations gain electrons and are reduced. At the anode, anions lose electrons and are oxidized.
4. The products of electrolysis depend on the electrolyte. Molten salts yield elements, while aqueous solutions yield hydrogen or oxygen along with other possible products.
This document discusses electrochemistry, including electrolytes, non-electrolytes, and electrolysis. It explains that electrolytes can conduct electricity because they contain free-moving ions, while non-electrolytes cannot conduct electricity. Electrolysis is the process of using electricity to break down compounds, and can be done on molten or aqueous solutions using an electrolytic cell with an anode and cathode. Factors like the position of ions in the electrochemical series and concentration affect which ions are discharged. Electrolysis has industrial applications like metal extraction and electroplating. Voltaic cells convert chemical energy to electrical energy and examples are given. The electrochemical series arranges elements by their tendency to release electrons,
Electrochemical cells convert chemical energy into electrical energy (voltaic/galvanic cells) or use electrical energy to drive non-spontaneous chemical reactions (electrolytic cells). Voltaic cells consist of two half-cells where oxidation occurs at the anode and reduction at the cathode. A salt bridge allows ion flow between cells while preventing mixing. The Daniell cell uses a zinc anode and copper cathode with oxidation of zinc and reduction of copper ions. Electrolytic cells use a power source to force non-spontaneous reactions like the electrolysis of molten lead bromide into elemental lead and bromine gas.
Chapter2- akjkjkkaaCorrosion Basics.pptxSrikanth S
This document provides an overview of key concepts in chemistry and electrochemistry as they relate to corrosion. It defines matter, elements, atoms, ions, and compounds. It describes the structure of atoms including electrons, protons, and neutrons. It introduces concepts like the periodic table, valence electrons, and ionic charge. It then discusses electrochemical reactions, corrosion processes, cathodic and anodic reactions, and how surface area affects corrosion rates. Key topics covered include electrolysis, Faraday's law for relating current to mass loss, and the effects of acidity, oxygen, and dissolved ions on corrosion mechanisms.
Chapter2- akjkjkkaaCorrosion Basics.pptxSrikanth S
This document provides an overview of key concepts in chemistry and electrochemistry as they relate to corrosion. It defines matter, elements, atoms, ions, and compounds. It describes the structure of atoms including electrons, protons, and neutrons. It introduces concepts like the periodic table, valence electrons, and ionic charge. It then discusses electrochemical reactions, corrosion processes, cathodic and anodic reactions, and how surface area affects corrosion rates. Key topics covered include electrolysis, Faraday's law for relating current to mass loss, and the effects of acidity, oxygen, and dissolved ions on corrosion mechanisms.
The document provides information about electrochemistry. It discusses oxidation-reduction reactions and how they involve the transfer of electrons between species. It explains how to assign oxidation numbers to keep track of electrons gained and lost. Balancing oxidation-reduction reactions using the half-reaction method is also covered. Finally, the document discusses voltaic cells, electrolytic cells, and applications of electrochemistry such as electroplating.
Electrolysis is a process where an electric current is passed through an ionic substance, causing the substance to decompose. During electrolysis, the substance being electrolyzed (called the electrolyte) contains positive and negative ions. Positive ions move to the negative electrode where they gain electrons through reduction reactions. Negative ions move to the positive electrode where they lose electrons through oxidation reactions. This process is used industrially for processes like refining metals and producing chemicals.
This document provides an overview of electrolysis. It discusses the history of electrolysis, the process which involves using a direct electric current to drive a non-spontaneous chemical reaction. It also covers Faraday's laws of electrolysis, industrial uses such as producing aluminum and chlorine, and reactions that occur during electrolysis like the oxidation and reduction at electrodes. Specific techniques like electrolysis of water and electrocrystallization are also summarized.
- Alkali metals have low ionization energies and readily lose their outer electron to form cations with a +1 oxidation state. They are soft, reactive metals that form ionic compounds.
- Sodium is the second alkali metal and is found abundantly in nature as the mineral sodium chloride. It is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride at lower temperatures using calcium chloride. This allows pure sodium to be produced at the cathode and chlorine gas to be collected at the anode.
The document outlines key concepts in electrochemistry including:
1. Electrolysis involves using electricity to break down ionic compounds or solutions into their components. It occurs when ions are able to move freely in molten or aqueous states.
2. During electrolysis, cations move to the cathode where they gain electrons and undergo reduction reactions. Anions move to the anode where they lose electrons and undergo oxidation reactions.
3. The electrolysis of molten ionic compounds produces metals at the cathode and non-metals at the anode. Electrolysis of aqueous solutions can produce hydrogen and oxygen from water or discharge other ions depending on their reactivity.
Electrolytes are substances that can conduct electricity in the molten or liquid state and undergo chemical changes. Electrolysis is a process where electrolytes are broken down into their constituent elements by passing electricity through them. During electrolysis, ions migrate to the oppositely charged electrodes. At the anode, ions lose electrons and form gases or dissolve. At the cathode, ions gain electrons and form solid elements. Examples of electrolysis of molten lead(II) bromide and lead(II) oxide are described through their half reactions at the anode and cathode and overall reactions.
This document outlines learning outcomes for a chapter on electrochemistry. It describes key concepts such as classifying substances as conductors or non-conductors, different types of electrical conduction, electrolysis, oxidation and reduction reactions, and industrial applications of electrolysis. The document also defines important terms like electrolyte, cathode, anode, cation, anion, and Faraday's constant. It explains how to calculate masses and volumes of substances liberated during electrolysis.
The document outlines key concepts in electrochemistry including:
- Conductors and electrolytes allow electric currents through movement of charged particles. Electrolytes must be molten or dissolved.
- During electrolysis, cations move to the cathode and are reduced while anions move to the anode and are oxidized.
- Products depend on the electrolyte - molten salts produce metals at the cathode and nonmetals at the anode, while solutions can produce gases from water. Reactions follow selective discharge principles.
1. Electrochemistry involves chemical reactions caused by the introduction of electrical energy. Alessandro Volta discovered batteries in 1793 by placing different metals in water. (2) Berzelius later proposed that atoms are electrified, with metals being positive and non-metals negative. (3) Galvanic cells convert chemical energy to electrical energy through spontaneous redox reactions between two half-cells separated by a salt bridge.
Electrolysis is a process that uses electricity to separate substances. When an ionic substance is melted or dissolved in water, ions are free to move and an electric current can break them down into elements. During electrolysis, positive ions move to the negative cathode where they gain electrons and negative ions move to the positive anode where they lose electrons. Electrolysis of brine produces chlorine gas, hydrogen gas, and sodium hydroxide solution which have important industrial uses.
Electrochemistry is the study of electricity and how it relates to chemical reactions. In electrochemistry, electricity can be generated by movements of electrons from one element to another in a reaction known as redox or oxidation-reduction reaction.
The document discusses electrolysis and the principles behind it. It explains that electrolysis involves passing electricity through an electrolyte, which causes chemical decomposition. Ions migrate to the electrodes and are discharged. Metals are formed at the cathode by reduction, while non-metals or oxygen form at the anode by oxidation. It provides examples of electrolysis such as molten salts like NaCl and aqueous solutions like copper sulfate. Factors affecting ion discharge are also discussed.
The document outlines learning outcomes for a chapter on electrochemistry. It will describe investigations into classifying substances as conductors or non-conductors, distinguish between metallic and electrolytic conduction, define key terms like electrolysis, electrodes, and ions. It will also cover predicting reactions and products of electrolysis, calculating quantities produced using Faraday's constant, and discussing industrial applications of electrolysis.
This slide was prepared by me for I was given project on the course applied electro-chemistry. Am student at Addis Ababa university institute of technology , addis ababa Ethiopia
1. Electrolysis is the process of using electricity to cause non-spontaneous chemical changes.
2. During electrolysis, ions migrate towards the oppositely charged electrode - cations move towards the cathode and anions move towards the anode.
3. At the cathode, cations gain electrons and are reduced. At the anode, anions lose electrons and are oxidized.
4. The products of electrolysis depend on the electrolyte. Molten salts yield elements, while aqueous solutions yield hydrogen or oxygen along with other possible products.
This document discusses electrochemistry, including electrolytes, non-electrolytes, and electrolysis. It explains that electrolytes can conduct electricity because they contain free-moving ions, while non-electrolytes cannot conduct electricity. Electrolysis is the process of using electricity to break down compounds, and can be done on molten or aqueous solutions using an electrolytic cell with an anode and cathode. Factors like the position of ions in the electrochemical series and concentration affect which ions are discharged. Electrolysis has industrial applications like metal extraction and electroplating. Voltaic cells convert chemical energy to electrical energy and examples are given. The electrochemical series arranges elements by their tendency to release electrons,
Electrochemical cells convert chemical energy into electrical energy (voltaic/galvanic cells) or use electrical energy to drive non-spontaneous chemical reactions (electrolytic cells). Voltaic cells consist of two half-cells where oxidation occurs at the anode and reduction at the cathode. A salt bridge allows ion flow between cells while preventing mixing. The Daniell cell uses a zinc anode and copper cathode with oxidation of zinc and reduction of copper ions. Electrolytic cells use a power source to force non-spontaneous reactions like the electrolysis of molten lead bromide into elemental lead and bromine gas.
Chapter2- akjkjkkaaCorrosion Basics.pptxSrikanth S
This document provides an overview of key concepts in chemistry and electrochemistry as they relate to corrosion. It defines matter, elements, atoms, ions, and compounds. It describes the structure of atoms including electrons, protons, and neutrons. It introduces concepts like the periodic table, valence electrons, and ionic charge. It then discusses electrochemical reactions, corrosion processes, cathodic and anodic reactions, and how surface area affects corrosion rates. Key topics covered include electrolysis, Faraday's law for relating current to mass loss, and the effects of acidity, oxygen, and dissolved ions on corrosion mechanisms.
Chapter2- akjkjkkaaCorrosion Basics.pptxSrikanth S
This document provides an overview of key concepts in chemistry and electrochemistry as they relate to corrosion. It defines matter, elements, atoms, ions, and compounds. It describes the structure of atoms including electrons, protons, and neutrons. It introduces concepts like the periodic table, valence electrons, and ionic charge. It then discusses electrochemical reactions, corrosion processes, cathodic and anodic reactions, and how surface area affects corrosion rates. Key topics covered include electrolysis, Faraday's law for relating current to mass loss, and the effects of acidity, oxygen, and dissolved ions on corrosion mechanisms.
The document provides information about electrochemistry. It discusses oxidation-reduction reactions and how they involve the transfer of electrons between species. It explains how to assign oxidation numbers to keep track of electrons gained and lost. Balancing oxidation-reduction reactions using the half-reaction method is also covered. Finally, the document discusses voltaic cells, electrolytic cells, and applications of electrochemistry such as electroplating.
Electrolysis is a process where an electric current is passed through an ionic substance, causing the substance to decompose. During electrolysis, the substance being electrolyzed (called the electrolyte) contains positive and negative ions. Positive ions move to the negative electrode where they gain electrons through reduction reactions. Negative ions move to the positive electrode where they lose electrons through oxidation reactions. This process is used industrially for processes like refining metals and producing chemicals.
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3. WHAT IS ELECTROLYSIS?
Electrolysis is the decomposition of ionic compounds using electricity.
Ionic compounds contain metals combined with non-metals. Examples
include
● sodium chloride (NaCl) – a combination of the metal sodium with the non-metal
chlorine
● copper sulfate (CuSO4) – a combination of the metal copper with the non-metals sulfur
and oxygen.
Ionic compounds are made up of positive and negative ions. As solids,
ionic compounds cannot conduct electricity because the ions cannot
move around. However, when ionic compounds are melted or dissolved,the ions are free
to move and conduct electricity. These liquids or solutions are called electrolytes because
they are able to conduct electricity.
4. EXPLANATION
If two electrodes connected to a supply of electricity are
put into the electrolyte, the negative ions are attracted
to the positive electrode and the positive ions are
attracted to the negative electrode .
This happens because opposite charges attract each other.
When the ions reach the electrodes they are discharged.
This means that they gain or lose electrons so that they
lose their charge and become neutral. Positive ions gain
electrons. Negative ions lose electrons.
The negative ions are discharged by losing electrons
at the positive electrode. These electrons move around
the circuit through the wires to the negative electrode.
The positive ions are discharged by gaining electrons
at the negative electrode.
5. KEY TERMS Electrolysis Decomposition of compounds
using electricity.
Electrolyte A liquid that conducts electricity.
Discharge Gain or lose electrons to
become electrically neutral.
Anode An electrode where oxidation
takes place (oxidation is the loss of
electrons) – in electrolysis it is the
positive electrode.
Cathode An electrode where
reduction takes place (reduction is the
gain of electrons) – in electrolysis it is
the negative electrode.
6. ELECTROLYSIS OF MOLTEN IONIC COMPOUND
Binary ionic compounds are ones made from one metal
combined with
one non-metal. Examples include lead bromide (PbBr2)
,sodium chloride (NaCl) and aluminium oxide (Al2O3) . The
electrolysis of these compounds when molten produces
the metal and
non-metal.
Molten lead bromide, PbBr2(l), is an electrolyte.
During electrolysis:
Pb2+ ions gain electrons at the cathode and become Pb
atoms
Br- ions lose electrons at the anode and become Br atoms,
which pair up to form Br2 molecules
So lead forms at the negative electrode and bromine
forms at the positive electrode.
7. ELECTROLYSIS OF MOLTEN SODIUM CHLORIDE
• ELECTROLYSIS INVOLVES THE MOVEMENT OF IONS TO THE ELECTRODE. SOLID-STATE DOES NOT
ALLOW THE MOVEMENT OF IONS AND IS UNSUITABLE FOR ELECTROLYSIS. WHEN MELTED AT HIGH
TEMPERATURES, SODIUM CHLORIDE SEPARATES INTO SODIUM AND CHLORIDE IONS SO THAT
ELECTROLYSIS CAN TAKE PLACE TO FORM SODIUM ATOMS AND CHLORINE GAS
NaCl → Na +(l) + Cl–(l)
At cathode: reduction of 2Na+(l) + e– → Na(l)
At anode: oxidation of 2Cl–(l) → Cl2(g) + 2e–
Net reaction is written as: 2Na +(l) + 2Cl–(l) → 2Na(l) + Cl2(g)
8. ELECTOLYSIS OF ALUMINIUM OXIDE
• THE DIAGRAM SHOWS AN ALUMINIUM OXIDE ELECTROLYSIS CELL. THE
NEGATIVE ELECTRODES (CATHODES) AND THE POSITIVE ELECTRODES
(ANODES) ARE MADE OF GRAPHITE, A FORM OF CARBON.
• DURING ELECTROLYSIS:
• POSITIVELY CHARGED ALUMINIUM IONS GAIN ELECTRONS FROM THE
CATHODE, AND FORM MOLTEN ALUMINIUM.
• OXIDE IONS LOSE ELECTRONS AT THE ANODE, AND FORM OXYGEN
MOLECULES.
• THE OXYGEN REACTS WITH THE CARBON IN THE ELECTRODES, FORMING
CARBON DIOXIDE WHICH BUBBLES OFF. CARBON IS THEREFORE LOST FROM
THE POSITIVE ELECTRODES, SO THEY MUST BE REPLACED FREQUENTLY. THIS
ADDS TO THE COST OF THE PROCESS.
Al3+ + 3e– → Al (reduction – gain electrons)
2O2– → O2 + 4e– (oxidation – lose electrons)
9. ELECTROLYSIS OF AQUEOUS IONIC COMPOUND
When an ionic compound is dissolved in water, the products of
electrolysis are often different to those when the compound is molten.
In water, a small fraction of the molecules break down into hydrogen
ions (H+) and hydroxide ions (OH−). These ions can be discharged
instead of the ions in the ionic compound. More water molecules can
break down if these ions are used up.
At each electrode there are two ions that could discharge, one from the
ionic compound and one from the water. The one that is easier to discharge
is the one that is discharged.Also the Inert electrodes are
electrodes that will allow the electrolysis to take place but do not react
themselves. Graphite electrodes are the most common inert electrodes used.
10. ELECTROLYSIS OF AQUEOUS IONIC COMPOUND
For example, the electrolysis of copper(II) chloride solution produces copper at
the negative electrode
. However, the electrolysis of sodium chloride solution produces hydrogen. Note
that the electrolysis of sodium chloride solution produces chlorine gas and
hydrogen gas but also leaves a solution of sodium hydroxide as well.
At the positive electrode
If the negative ion from the ionic compound is simple (eg Cl– or Br–), then that element is
produced. If the negative ion is a compound ion (eg NO3–, SO4-22, CO32–), then oxygen is
produced from the hydroxide ion present instead.
11. ELECTROLYSIS OF AQUEOUS IONIC COMPOUND
At the negative electrode
Metal ions and hydrogen ions are positively charged. Whether you get the
metal or hydrogen during electrolysis depends on the position of the metal
in the
reactivity serier
the metal will be produced if it is less reactive than hydrogen
hydrogen will be produced if the metal is more reactive than hydrogen
The relative reactivity of selected elements from most to least: potassium,
sodium, calcium, magnesium, aluminium, carbon, zinc, iron, tin, lead,
hydrogen, copper, silver, gold, platinum.
12. ELECTROLYSIS OF AQUEOUS NACL
As shown , the electrolysis of sodium chloride solution
will produce chlorine gas at the anode and hydrogen gas
at the cathode.
at the anode, 2Cl– → Cl2 2e– (oxidation)
at the cathode, 2H+ + 2e– → H2 (reduction)
During the electrolysis, hydrogen and chloride ions are
removed from solution whereas sodium and hydroxide
ions are left behind in solution. This means that sodium
hydroxide is also formed during the electrolysis of sodium
chloride solution. This process is carried out on an
industrial scale using sea water to produce hydrogen gas,
chlorine gas and sodium hydroxide solution.
13. Electrolysis is used to electroplate objects (coat them with a thin layer of metal). This is useful for coating a cheaper metal with
a more expensive one, such as copper or silver.
The negative electrode should be the object to be electroplated.
The positive electrode should be the metal that you want to coat the object with.
The electrolyte should be a solution of the coating metal, such as its metal nitrate or sulfate.
Here are two examples.
Electroplating with silver
The object to be plated, such as a metal spoon, is connected to the negative terminal of the power supply. A piece of silver is
connected to the positive terminal. The electrolyte is silver nitrate solution.
Electroplating with copper
The object to be plated, such as a metal pan, is connected to the negative terminal of the power supply. A piece of copper is
connected to the positive terminal. The electrolyte is copper(II) sulfate solution.
Purifying copper by electrolysis [Higher tier only]
Copper is purified by electrolysis. Electricity is passed through solutions containing copper compounds, such as copper(II)
sulfate. The anode (positive electrode) is made from impure copper and the cathode (negative electrode) is made from pure
copper.
Pure copper forms on the cathode.
ELECTROPLATING
14. HYDROGEN FUEL CELL
A fuel is a substance which releases energy when burned
Hydrogen is used as a fuel in rocket engines and in fuel cells to power some cars
A fuel cell is an electrochemical cell in which a fuel donates electrons at one
electrode and oxygen gains electrons at the other electrode
H2 → 2H+ + 2e–
O2 + 4e– → 2O2–
The hydrogen-oxygen fuel cell produces electricity by combining
both elements, releasing energy and water
The overall equation for the reaction within a hydrogen fuel cell is:
hydrogen + oxygen → water
The diagram shows the setup of a hydrogen fuel cell
The air entering provides the oxygen
The fuel entering is hydrogen
The only chemical product made is water
15. HYDROGEN FUEL CELL
Advantages
• They do not produce any pollution: the only product is water whereas petrol engines
produce carbon dioxide, and oxides of nitrogen
• They release more energy per kilogram than either petrol or diesel
• No power is lost in transmission as there are no moving parts, unlike an internal
combustion engine
• Quieter so less noise pollution compared to a petrol engine
Disadvantages
• Materials used in producing fuel cells are expensive
• Hydrogen is more difficult and expensive to store compared to petrol as it is very
flammable and easily explodes when under pressure
• Fuel cells are affected by low temperatures, becoming less efficient
• There are only a small number of hydrogen filling stations across the country
• Hydrogen is often obtained by methods that involve the combustion of fossil fuels,
therefore releasing carbon dioxide and other pollutants into the atmosphere