This document provides an introduction to the alkaline earth metals in Group II of the periodic table. It summarizes the key trends across the group, including increases in atomic and ionic radius and decreases in ionization energy and melting point down the group. The reactivity of the elements increases due to the greater ease of forming cations. Their oxides, hydroxides, carbonates and sulfates also show trends in solubility and other properties corresponding to the size of the metal ions.
Be Mg Ca Sr Ba
The document discusses the trends in properties of elements in Group II of the periodic table. It explains that atomic radius, ionic radius, and first ionization energy decrease down the group, while melting point decreases. Successive ionization energies increase due to decreased shielding. Reactivity also increases as it becomes easier to form cations with larger atomic size and lower ionization energy. The elements react with oxygen and water to form oxides, hydroxides, carbonates, and sulfates.
This document discusses the properties and reactions of Group II elements and their compounds. It describes how atomic radius and ionization energy increase down the group, while electronegativity decreases. Group II elements react vigorously with oxygen and water to form oxides and hydroxides. Their oxides are basic and react with acids, while hydroxides are sparingly soluble bases. Thermal decomposition stability increases down the group for nitrates and carbonates. Important uses include magnesium oxide as a refractory and calcium compounds to make cement and treat acidic soil.
This document discusses various battery technologies including primary and secondary cells. It provides details on dry cells, lead-acid batteries, nickel-cadmium batteries, and fuel cells. The key points are:
- Primary cells cannot be recharged while secondary cells can be recharged by passing current in the opposite direction.
- Dry cells are inexpensive but have a limited shelf life. Lead-acid batteries are rechargeable and commonly used in vehicles. Nickel-cadmium batteries can be recharged hundreds of times.
- Fuel cells directly convert chemical energy to electrical energy and include hydrogen-oxygen and methanol-oxygen types. They do not require recharging and have applications in space, military, and stationary power
This document discusses the properties and characteristics of alkaline earth metals. It begins by defining alkaline earth metals as group 2 elements with an outer electron configuration of ns2. Some key points made include:
- Alkaline earth metals have higher ionization energies than alkali metals. Ionization energy decreases down the group as atomic size increases.
- Their physical properties include being silvery-white, soft metals that are stronger oxidizers than alkali metals. They impart unique flame colors.
- Chemically, they readily react with oxygen, water and halogens. Reactivity increases down the group. They form basic hydroxides except for beryllium.
- The document also discusses trends
New chm-152-unit-9-power-points-sp13-140227172048-phpapp02Cleophas Rwemera
This document discusses electrolysis and Faraday's law of electrolysis. It begins by introducing electrolytic cells and predicting the products of electrolysis. It then explains that according to Faraday's law, the amount of substance produced at each electrode is directly proportional to the quantity of electricity passing through the cell. The document provides an example calculation applying Faraday's law to determine the current needed in an electrolysis process. It also discusses some key aspects of Faraday's law, such as defining the faraday as one mole of electrons.
Group 2 and thier properties and reactions.pptxHarisAwan33
Group 2 elements include beryllium, magnesium, calcium, strontium, barium, and radium. They are shiny, silvery-white metals that are reactive at standard temperature and pressure. The elements have similar electron configurations with their outer electron shells being filled with two electrons. Properties of the elements, such as atomic radius, reactivity, and melting point, follow trends down the group as the principal energy level increases. Group 2 elements react readily with oxygen, water, and acids to form metal oxides, hydroxides, and salts. The reactivity of these reactions increases down the group as ionization energy decreases.
This document provides an overview of redox reactions and electrochemistry applications. It discusses oxidation-reduction concepts like oxidation states and the OIL RIG mnemonic. Examples of redox reactions and electrochemistry applications are given, including galvanic cells, corrosion, electrolysis, and batteries. Key concepts covered include cell potential, the Nernst equation, and how concentration affects cell potential. Diagrams illustrate galvanic cells and how they function.
Be Mg Ca Sr Ba
The document discusses the trends in properties of elements in Group II of the periodic table. It explains that atomic radius, ionic radius, and first ionization energy decrease down the group, while melting point decreases. Successive ionization energies increase due to decreased shielding. Reactivity also increases as it becomes easier to form cations with larger atomic size and lower ionization energy. The elements react with oxygen and water to form oxides, hydroxides, carbonates, and sulfates.
This document discusses the properties and reactions of Group II elements and their compounds. It describes how atomic radius and ionization energy increase down the group, while electronegativity decreases. Group II elements react vigorously with oxygen and water to form oxides and hydroxides. Their oxides are basic and react with acids, while hydroxides are sparingly soluble bases. Thermal decomposition stability increases down the group for nitrates and carbonates. Important uses include magnesium oxide as a refractory and calcium compounds to make cement and treat acidic soil.
This document discusses various battery technologies including primary and secondary cells. It provides details on dry cells, lead-acid batteries, nickel-cadmium batteries, and fuel cells. The key points are:
- Primary cells cannot be recharged while secondary cells can be recharged by passing current in the opposite direction.
- Dry cells are inexpensive but have a limited shelf life. Lead-acid batteries are rechargeable and commonly used in vehicles. Nickel-cadmium batteries can be recharged hundreds of times.
- Fuel cells directly convert chemical energy to electrical energy and include hydrogen-oxygen and methanol-oxygen types. They do not require recharging and have applications in space, military, and stationary power
This document discusses the properties and characteristics of alkaline earth metals. It begins by defining alkaline earth metals as group 2 elements with an outer electron configuration of ns2. Some key points made include:
- Alkaline earth metals have higher ionization energies than alkali metals. Ionization energy decreases down the group as atomic size increases.
- Their physical properties include being silvery-white, soft metals that are stronger oxidizers than alkali metals. They impart unique flame colors.
- Chemically, they readily react with oxygen, water and halogens. Reactivity increases down the group. They form basic hydroxides except for beryllium.
- The document also discusses trends
New chm-152-unit-9-power-points-sp13-140227172048-phpapp02Cleophas Rwemera
This document discusses electrolysis and Faraday's law of electrolysis. It begins by introducing electrolytic cells and predicting the products of electrolysis. It then explains that according to Faraday's law, the amount of substance produced at each electrode is directly proportional to the quantity of electricity passing through the cell. The document provides an example calculation applying Faraday's law to determine the current needed in an electrolysis process. It also discusses some key aspects of Faraday's law, such as defining the faraday as one mole of electrons.
Group 2 and thier properties and reactions.pptxHarisAwan33
Group 2 elements include beryllium, magnesium, calcium, strontium, barium, and radium. They are shiny, silvery-white metals that are reactive at standard temperature and pressure. The elements have similar electron configurations with their outer electron shells being filled with two electrons. Properties of the elements, such as atomic radius, reactivity, and melting point, follow trends down the group as the principal energy level increases. Group 2 elements react readily with oxygen, water, and acids to form metal oxides, hydroxides, and salts. The reactivity of these reactions increases down the group as ionization energy decreases.
This document provides an overview of redox reactions and electrochemistry applications. It discusses oxidation-reduction concepts like oxidation states and the OIL RIG mnemonic. Examples of redox reactions and electrochemistry applications are given, including galvanic cells, corrosion, electrolysis, and batteries. Key concepts covered include cell potential, the Nernst equation, and how concentration affects cell potential. Diagrams illustrate galvanic cells and how they function.
B.tech. ii engineering chemistry unit 2 water technologyRai University
This document discusses various sources and types of water as well as common impurities found in water. It describes surface water sources like rain, river, lake and sea water and mentions their typical compositions. It also discusses underground water sources like spring and well water. The document then lists major ionic, non-ionic and gaseous impurities that may be present in water. It provides details on hard water, including what causes hardness and its effects on soap lathering. Methods to soften hard water like the lime soda process are also summarized.
This document discusses electrochemistry and voltaic cells. It begins by defining electrochemistry as the interconversion of chemical and electrical energy. It then discusses electrolysis and voltaic cells. Electrolysis involves using electricity to break down substances, while voltaic cells convert chemical energy to electrical energy. The document goes on to describe the components and reactions of voltaic cells, including simple voltaic cells and Daniell cells. It also discusses applications of electrolysis in industries such as metal extraction and electroplating.
The document defines oxidation and reduction (redox) reactions in terms of oxygen/hydrogen gain or loss, electron transfer, and changes in oxidation state. It provides examples of redox reactions like combustion and corrosion. Oxidation is defined as gaining oxygen, losing hydrogen, losing electrons, or increasing oxidation state. Reduction is the opposite - gaining electrons or decreasing oxidation state. Mnemonics like "OIL-RIG" are given to help remember the definitions.
The document defines oxidation and reduction (redox) reactions in terms of oxygen/hydrogen gain or loss, electron transfer, and changes in oxidation state. It provides examples of redox reactions like combustion and corrosion. Redox involves both oxidation, defined as gaining oxygen, losing hydrogen, losing electrons, or increasing oxidation state, and reduction, defined as the opposite of these processes. Common oxidizing and reducing agents can be identified through color changes using potassium iodide and dichromate solutions.
1. The document discusses the general principles and processes involved in isolating elements from minerals, including concentration/purification of ores, isolation of metals from concentrated ores, and purification of metals.
2. Key steps in concentration/purification of ores include hand picking, hydraulic washing, electromagnetic separation, and froth flotation. Isolation of metals involves converting ores to metal oxides through roasting or calcination, then reducing metal oxides to metals using thermal or electrolytic processes.
3. Thermal reduction relies on coupling reduction reactions using an appropriate reducing agent based on Gibbs free energy values from Ellingham diagrams, which predict feasibility of reductions at different temperatures. Common extraction methods are also summarized for iron and
1. The document discusses the general principles and processes involved in isolating elements from minerals, including concentration/purification of ores, isolation of metals from concentrated ores, and purification of metals.
2. Key steps in concentration/purification of ores include hand picking, hydraulic washing, electromagnetic separation, and froth flotation. Isolation of metals involves converting ores to metal oxides through roasting or calcination, then reducing metal oxides to metals using thermal or electrolytic processes.
3. Thermal reduction relies on coupling reduction reactions using an appropriate reducing agent based on Gibbs free energy values from Ellingham diagrams. Examples demonstrate determining suitable reducing agents for different metal oxides at varying temperatures.
Chemistry zimsec chapter 9 chemical periodicityalproelearning
This document summarizes key concepts about chemical periodicity, including the various blocks and periods in the periodic table. It describes trends in atomic properties like atomic radius, ionization energy, and electronegativity across periods and down groups. These trends are explained by factors like nuclear charge, atomic size, and shielding effects. Common reactions of representative elements like formation of oxides and chlorides from the third period are presented, along with equations. Structures and bonding of these compounds are discussed as well as their reactions with water.
The document summarizes the properties of elements in Group 13 (boron family) of the periodic table. It discusses their electron configurations, occurrence in nature, extraction methods, and chemical and physical properties. Boron is the only nonmetal in the group. Aluminum is the most abundant and widely used member. The properties of these elements trend from nonmetallic (boron) to metallic (thallium) down the group. Their compounds typically exhibit oxidation state of +3, forming oxides, halides, and other salts with the formula MX3 where M is the group 13 element.
The document summarizes extraction and uses of magnesium. It describes common magnesium minerals like dolomite and magnesite. It discusses challenges in extracting magnesium through pyrometallurgical and electrometallurgical processes. The Pidgeon and Magnetotherm processes are described for pyrometallurgical extraction. The Dow process extracts magnesium from seawater through precipitation and electrolysis. Magnesium has non-structural uses like alloying, deoxidation, and cathodic protection. Structural uses include aircraft and transportation applications due to magnesium's high strength to weight ratio.
The document provides an introduction to key concepts in electrochemistry including oxidation/reduction reactions, oxidation numbers, and definitions of terms like oxidizing agent and reducing agent. It then discusses rules for assigning oxidation numbers, types of redox reactions like disproportionation, electrochemical cells, and how to determine the potential of a cell.
This document discusses electrolysis and Faraday's law of electrolysis. It provides examples of predicting products of electrolysis for molten salts, aqueous salt solutions, and applying Faraday's law calculations. Key points include:
- During electrolysis, the cation is reduced at the cathode and the anion is oxidized at the anode
- In molten salts, the more easily oxidized/reduced species reacts at each electrode
- In aqueous solutions, overvoltage must be considered in addition to electrode potentials
- Faraday's law states the amount of substance reacted is directly proportional to the quantity of electricity passed through the cell
- Calculations can determine current, time, charge or mass from the other variables using Faraday's constant
Sulfur has an oxidation number of +4 in SO2 and Na2SO4. Carbon has an oxidation number of +4 in CO32-. Oxygen has an oxidation number of -2 in all cases. Sodium has an oxidation number of +1 in Na2SO4. Nitrogen has an oxidation number of -3 and hydrogen has an oxidation number of +1 in (NH4)2S.
The document is a guide about the halogens for GCSE chemistry students. It discusses the key properties and trends within group VII of the periodic table. The guide covers topics such as physical appearances, boiling points, electronic configurations, atomic sizes, and reactivity trends. It also describes reactions of halogens with metals and displacement reactions between halides.
Manufacture of caustic soda and chlorine using electrolysis process ...Ankush Gupta
This document discusses the manufacture of chlorine and caustic soda using electrolysis processes. It provides background on the chlor-alkali industry and describes the three main electrolysis processes: diaphragm cell, mercury cell, and membrane cell. The membrane cell process is highlighted as the most energy efficient and environmentally friendly option. Properties and production details of chlorine, caustic soda, and hydrogen are also outlined. A literature review covers previous research on improving chlor-alkali cell efficiency and treating wastewater from the process.
Introduction
Magnesium extraction
a. Pidgeon process
b. Magnotherm process
Extraction of metals from oxide members
c. Electrolytic process (Dow process )
Aluminum extinction
a. Baye’s process
b. Hall- heraoult process
c. Methods of titrating low grades ores
d. Newer process for Aluminum production
Tantalum extraction
1. Precipitation is an easy and cost-effective process to produce nano-sized particles using inexpensive source materials like inorganic chemicals.
2. Precipitation often results in hard aggregation of primary particles during washing, filtration, and drying which must be addressed.
3. Methods to prevent aggregation include controlling crystal growth, maintaining a constant pH washing solution to encourage electrostatic repulsion, and ball milling dried aggregates with less polar solvents.
1. The document discusses various external water softening processes including lime-soda, zeolite, and ion exchange processes.
2. The lime-soda process uses lime and soda ash to precipitate calcium and magnesium ions from water.
3. The zeolite process involves exchanging sodium ions in zeolite minerals with calcium and magnesium ions in hard water.
4. Ion exchange uses cation and anion exchange resins to remove ions from water and produce deionized water with hardness of only 2 ppm.
There are 6 types of electronic transitions that can occur in molecules: 1) σ→ σ* transition, 2) π → π* transition, 3) n→σ* transition, 4) n→π* transition, 5) σ→π* transition, and 6) π→σ* transition. These electronic transitions can be represented graphically using an energy level diagram.
Hittorf's method is a moving boundary method used to determine the transport numbers of ions in an electrolyte solution. Kohlrausch's law of independent migration of ions states that the equivalent conductance of an electrolyte at infinite dilution is equal to the sum of the equivalent conductances of the individual ions that make up the electrolyte. A formula is provided to calculate the transport numbers of ions based on the distance traveled by the boundary, concentration of the electrolyte solution, and total number of ions.
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This document discusses various sources and types of water as well as common impurities found in water. It describes surface water sources like rain, river, lake and sea water and mentions their typical compositions. It also discusses underground water sources like spring and well water. The document then lists major ionic, non-ionic and gaseous impurities that may be present in water. It provides details on hard water, including what causes hardness and its effects on soap lathering. Methods to soften hard water like the lime soda process are also summarized.
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1. The document discusses the general principles and processes involved in isolating elements from minerals, including concentration/purification of ores, isolation of metals from concentrated ores, and purification of metals.
2. Key steps in concentration/purification of ores include hand picking, hydraulic washing, electromagnetic separation, and froth flotation. Isolation of metals involves converting ores to metal oxides through roasting or calcination, then reducing metal oxides to metals using thermal or electrolytic processes.
3. Thermal reduction relies on coupling reduction reactions using an appropriate reducing agent based on Gibbs free energy values from Ellingham diagrams, which predict feasibility of reductions at different temperatures. Common extraction methods are also summarized for iron and
1. The document discusses the general principles and processes involved in isolating elements from minerals, including concentration/purification of ores, isolation of metals from concentrated ores, and purification of metals.
2. Key steps in concentration/purification of ores include hand picking, hydraulic washing, electromagnetic separation, and froth flotation. Isolation of metals involves converting ores to metal oxides through roasting or calcination, then reducing metal oxides to metals using thermal or electrolytic processes.
3. Thermal reduction relies on coupling reduction reactions using an appropriate reducing agent based on Gibbs free energy values from Ellingham diagrams. Examples demonstrate determining suitable reducing agents for different metal oxides at varying temperatures.
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This document summarizes key concepts about chemical periodicity, including the various blocks and periods in the periodic table. It describes trends in atomic properties like atomic radius, ionization energy, and electronegativity across periods and down groups. These trends are explained by factors like nuclear charge, atomic size, and shielding effects. Common reactions of representative elements like formation of oxides and chlorides from the third period are presented, along with equations. Structures and bonding of these compounds are discussed as well as their reactions with water.
The document summarizes the properties of elements in Group 13 (boron family) of the periodic table. It discusses their electron configurations, occurrence in nature, extraction methods, and chemical and physical properties. Boron is the only nonmetal in the group. Aluminum is the most abundant and widely used member. The properties of these elements trend from nonmetallic (boron) to metallic (thallium) down the group. Their compounds typically exhibit oxidation state of +3, forming oxides, halides, and other salts with the formula MX3 where M is the group 13 element.
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- In molten salts, the more easily oxidized/reduced species reacts at each electrode
- In aqueous solutions, overvoltage must be considered in addition to electrode potentials
- Faraday's law states the amount of substance reacted is directly proportional to the quantity of electricity passed through the cell
- Calculations can determine current, time, charge or mass from the other variables using Faraday's constant
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This document discusses the manufacture of chlorine and caustic soda using electrolysis processes. It provides background on the chlor-alkali industry and describes the three main electrolysis processes: diaphragm cell, mercury cell, and membrane cell. The membrane cell process is highlighted as the most energy efficient and environmentally friendly option. Properties and production details of chlorine, caustic soda, and hydrogen are also outlined. A literature review covers previous research on improving chlor-alkali cell efficiency and treating wastewater from the process.
Introduction
Magnesium extraction
a. Pidgeon process
b. Magnotherm process
Extraction of metals from oxide members
c. Electrolytic process (Dow process )
Aluminum extinction
a. Baye’s process
b. Hall- heraoult process
c. Methods of titrating low grades ores
d. Newer process for Aluminum production
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1. Precipitation is an easy and cost-effective process to produce nano-sized particles using inexpensive source materials like inorganic chemicals.
2. Precipitation often results in hard aggregation of primary particles during washing, filtration, and drying which must be addressed.
3. Methods to prevent aggregation include controlling crystal growth, maintaining a constant pH washing solution to encourage electrostatic repulsion, and ball milling dried aggregates with less polar solvents.
1. The document discusses various external water softening processes including lime-soda, zeolite, and ion exchange processes.
2. The lime-soda process uses lime and soda ash to precipitate calcium and magnesium ions from water.
3. The zeolite process involves exchanging sodium ions in zeolite minerals with calcium and magnesium ions in hard water.
4. Ion exchange uses cation and anion exchange resins to remove ions from water and produce deionized water with hardness of only 2 ppm.
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