The document discusses the extraction of metals from ores. It begins by explaining that metals are found either in their free state or combined as compounds in minerals and ores. It then discusses the various types of ores containing different metals such as oxides, sulfides, halides, etc. It also provides examples of common ores for metals like aluminum, zinc, iron, copper, sodium, potassium, lead, tin, and silver. Finally, it notes that the extraction process involves grouping metals based on their reactivity in the reactivity series, with less reactive metals sometimes found in their free state and more reactive metals requiring extraction from ionic compounds in their ores.
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals react with oxygen, water, acids and metal salt solutions. Metals are listed in a reactivity series from most reactive to least reactive. The document outlines how ionic compounds form and their properties. The extraction, refining and corrosion of metals is summarized along with methods for preventing corrosion.
The document describes non-metals and their properties. It discusses the physical and chemical properties of non-metals, and describes the industrial preparation of chlorine, sulfuric acid, and ammonia. It also lists common uses of non-metals like carbon, sulfur, phosphorus, chlorine, and nitrogen and their compounds.
This chapter discusses the properties and preparation of non-metals. It describes the differences between metals and non-metals, and the physical and chemical properties of common non-metals like hydrogen, oxygen, nitrogen, carbon, chlorine and sulfur. It also explains methods of preparing gases like chlorine, oxygen, ammonia and collecting them based on their solubility and density. Industrial production of chlorine using the mercury cell and membrane cell processes is also covered.
Metallurgy involves extracting metals from their ores in their pure state. Most reactive metals are found combined as sulfates, carbonates, or oxides, while less reactive metals occur naturally in their free metallic state. The process of metallurgy includes mining ores, concentrating the ores to remove impurities, oxidizing and reducing the ores, and refining the reduced metals. Electrolytic refining is used to remove soluble and insoluble impurities from reduced metals to produce pure metals.
Chapter 3.metals and non metals priya jhaPriya Jha
An element is the simplest form of matter that cannot be split into simpler substances or built from simpler substances by any ordinary chemical or physical method. There are 118 elements known to us, out of which 92 are naturally occurring, while the rest have been prepared artificially. Elements are further classified into metals, non-metals, and metalloids based on their properties, which are correlated with their placement in the periodic table.Metals
With the exception of hydrogen, all elements that form positive ions by losing electrons during chemical reactions are called metals. Thus metals are electropositive elements with relatively low ionization energies. They are characterized by bright luster, hardness, ability to resonate sound and are excellent conductors of heat and electricity. Metals are solids under normal conditions except for Mercury.Nonmetals
Elements that tend to gain electrons to form anions during chemical reactions are called non-metals. These are electronegative elements with high ionization energies. They are non-lustrous, brittle and poor conductors of heat and electricity (except graphite). Non-metals can be gases, liquids or solids.Metalloids
Metalloids have properties intermediate between the metals and nonmetals. Metalloids are useful in the semiconductor industry. Metalloids are all solid at room temperature. They can form alloys with other metals. Some metalloids, such as silicon and germanium, can act as electrical conductors under the right conditions, thus they are called semiconductors. Silicon for example appears lustrous, but is not malleable nor ductile (it is brittle - a characteristic of some nonmetals). It is a much poorer conductor of heat and electricity than the metals. The physical properties of metalloids tend to be metallic, but their chemical properties tend to be non-metallic. The oxidation number of an element in this group can range from +5 to -2, depending on the group in which it is located.
The document discusses the structure and properties of metals. Metals have a metallic lattice structure where the metal atoms are arranged in a regular pattern with their valence electrons delocalized in a "sea of electrons". This structure results in several properties including conductivity of heat and electricity, malleability, lustrous appearance, and high melting points. The structure can be modified through processes like work hardening, heat treatment, and alloying to achieve desired material properties for different applications.
The document discusses the extraction of metals from ores. It begins by explaining that metals are found either in their free state or combined as compounds in minerals and ores. It then outlines some common metal ores such as bauxite (Al2O3.2H2O) for aluminum, zinc blende (ZnS) for zinc, and hematite (Fe2O3) for iron. Finally, it notes that the steps in extracting metal from ore depend on the reactivity of the metal. Highly reactive metals require more processing steps since they must be extracted from their ionic compounds in the ore. Less reactive metals like gold and silver are sometimes found in their free state.
The document discusses the extraction of metals from ores. It begins by explaining that metals are found either in their free state or combined as compounds in minerals and ores. It then discusses the various types of ores containing different metals such as oxides, sulfides, halides, etc. It also provides examples of common ores for metals like aluminum, zinc, iron, copper, sodium, potassium, lead, tin, and silver. Finally, it notes that the extraction process involves grouping metals based on their reactivity in the reactivity series, with less reactive metals sometimes found in their free state and more reactive metals requiring extraction from ionic compounds in their ores.
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals react with oxygen, water, acids and metal salt solutions. Metals are listed in a reactivity series from most reactive to least reactive. The document outlines how ionic compounds form and their properties. The extraction, refining and corrosion of metals is summarized along with methods for preventing corrosion.
The document describes non-metals and their properties. It discusses the physical and chemical properties of non-metals, and describes the industrial preparation of chlorine, sulfuric acid, and ammonia. It also lists common uses of non-metals like carbon, sulfur, phosphorus, chlorine, and nitrogen and their compounds.
This chapter discusses the properties and preparation of non-metals. It describes the differences between metals and non-metals, and the physical and chemical properties of common non-metals like hydrogen, oxygen, nitrogen, carbon, chlorine and sulfur. It also explains methods of preparing gases like chlorine, oxygen, ammonia and collecting them based on their solubility and density. Industrial production of chlorine using the mercury cell and membrane cell processes is also covered.
Metallurgy involves extracting metals from their ores in their pure state. Most reactive metals are found combined as sulfates, carbonates, or oxides, while less reactive metals occur naturally in their free metallic state. The process of metallurgy includes mining ores, concentrating the ores to remove impurities, oxidizing and reducing the ores, and refining the reduced metals. Electrolytic refining is used to remove soluble and insoluble impurities from reduced metals to produce pure metals.
Chapter 3.metals and non metals priya jhaPriya Jha
An element is the simplest form of matter that cannot be split into simpler substances or built from simpler substances by any ordinary chemical or physical method. There are 118 elements known to us, out of which 92 are naturally occurring, while the rest have been prepared artificially. Elements are further classified into metals, non-metals, and metalloids based on their properties, which are correlated with their placement in the periodic table.Metals
With the exception of hydrogen, all elements that form positive ions by losing electrons during chemical reactions are called metals. Thus metals are electropositive elements with relatively low ionization energies. They are characterized by bright luster, hardness, ability to resonate sound and are excellent conductors of heat and electricity. Metals are solids under normal conditions except for Mercury.Nonmetals
Elements that tend to gain electrons to form anions during chemical reactions are called non-metals. These are electronegative elements with high ionization energies. They are non-lustrous, brittle and poor conductors of heat and electricity (except graphite). Non-metals can be gases, liquids or solids.Metalloids
Metalloids have properties intermediate between the metals and nonmetals. Metalloids are useful in the semiconductor industry. Metalloids are all solid at room temperature. They can form alloys with other metals. Some metalloids, such as silicon and germanium, can act as electrical conductors under the right conditions, thus they are called semiconductors. Silicon for example appears lustrous, but is not malleable nor ductile (it is brittle - a characteristic of some nonmetals). It is a much poorer conductor of heat and electricity than the metals. The physical properties of metalloids tend to be metallic, but their chemical properties tend to be non-metallic. The oxidation number of an element in this group can range from +5 to -2, depending on the group in which it is located.
The document discusses the structure and properties of metals. Metals have a metallic lattice structure where the metal atoms are arranged in a regular pattern with their valence electrons delocalized in a "sea of electrons". This structure results in several properties including conductivity of heat and electricity, malleability, lustrous appearance, and high melting points. The structure can be modified through processes like work hardening, heat treatment, and alloying to achieve desired material properties for different applications.
The document discusses the extraction of metals from ores. It begins by explaining that metals are found either in their free state or combined as compounds in minerals and ores. It then outlines some common metal ores such as bauxite (Al2O3.2H2O) for aluminum, zinc blende (ZnS) for zinc, and hematite (Fe2O3) for iron. Finally, it notes that the steps in extracting metal from ore depend on the reactivity of the metal. Highly reactive metals require more processing steps since they must be extracted from their ionic compounds in the ore. Less reactive metals like gold and silver are sometimes found in their free state.
all about metal and nonmetal of class 10 from physical to chemical....
last minute suggestion and preparation notes
made by student of 10th class only ..
short and sweet slides for quick revision...
HOPE IT MAY HELP U ...☺☻☺☻☺☻
Metals react with oxygen, water, acids, and salt solutions of metals. They tend to lose electrons during chemical reactions, forming positive ions. Metal oxides are formed when metals react with oxygen. Amphoteric oxides like zinc oxide and aluminum oxide can react with both acids and bases to form salts and water. Non-metals do not react with water because they cannot donate electrons to break the hydrogen-oxygen bonds. They also do not react with dilute acids but some exceptions exist, such as sulfur reacting with nitric acid. Aluminum undergoes various reactions including anodizing when treated with acids or steam in the laboratory.
This is a summary of the topic "metals" in the GCE O levels subject: Chemistry. Students taking either the combined science (chemistry/physics) or pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
The document discusses the properties and characteristics of metals and non-metals. It states that metals are generally found in the earth's crust in ores associated with other elements, and are also present in rocks, water, and dust. Non-metals lack metallic properties and are mostly gases or solids like carbon, sulfur, and phosphorus. A metalloid has properties between metals and non-metals. The document then discusses various physical and chemical properties of metals and non-metals such as conductivity, ductility, hardness, luster, malleability, physical state, sonority, examples, and their reactions with oxygen, water, acids, and other metal salts. It provides examples of these reactions and exceptions.
The document discusses the Downs Process for extracting sodium through the electrolysis of molten sodium chloride, where sodium ions are reduced to sodium atoms at the cathode and chlorine gas is produced at the anode. It also describes how sodium hydroxide is produced through the electrolysis of sodium chloride solutions, and lists some common uses of sodium and sodium hydroxide such as in soap production, as a drain cleaner, and for lighting.
This document provides information on the chemical properties of metals. It discusses how metals react with oxygen, water, acids, and metal salt solutions. It explains that the reactivity of metals varies, with metals like sodium and potassium being the most reactive due to losing their outer shell electrons easily. The document also discusses the formation of ionic compounds through the transfer of electrons from metals to non-metals, and provides examples of how ionic compounds like NaCl and MgCl2 are formed.
The document provides information about grade 10 IGCSE chemistry content related to properties and reactions of metals. It discusses distinguishing metals from non-metals, reactivity series, extraction of metals like iron from ores, and uses of metals such as aluminum and zinc. It also describes physical and chemical properties of metals, structure and properties of alloys, and reactions of metals with water, steam, and acids to determine reactivity order.
Metals react with oxygen, water, and acids to form metal oxides, hydroxides, or salts. They lose electrons and become positively charged ions. Non-metals react with oxygen to form non-metal oxides, gaining electrons and becoming negatively charged ions. Corrosion occurs as metals react with substances like oxygen and water in the air, forming coatings or rust. Corrosion can be prevented by applying protective coatings like oil, paint, zinc plating, or by alloying metals.
This document discusses the properties and reactivity of metals. It begins by describing the physical properties of metals, such as their hardness, malleability and conductivity. It then discusses the chemical properties of metals, including how they form positive ions and react with oxygen, water and acids. The document introduces metal alloys and explains why they are stronger than pure metals. It also defines the reactivity series and uses it to predict and describe the reactions of different metals. The document discusses the reactions of various metal compounds and how the position of metals in the reactivity series affects their reactivity and the stability of their compounds.
This document discusses a science presentation about the properties and reactions of metals and non-metals. It lists the group members giving the presentation and describes several properties of metals like malleability and conductivity. It then discusses how metals react with oxygen, water, acids, salt solutions, chlorine, hydrogen and how alloys are formed and used. For non-metals, it summarizes their reactions with oxygen, water, acids, salt solutions, chlorine, hydrogen and describes ionic compounds.
1. The Down's cell is an electrolytic cell that operates at 800°C to produce sodium metal through the electrolysis of molten sodium chloride.
2. It consists of a graphite anode and iron cathode separated by an iron screen inside a lined steel chamber. Molten sodium chloride mixed with calcium chloride and barium chloride is used as the electrolyte.
3. During electrolysis, chloride ions are oxidized at the anode to produce chlorine gas while sodium ions are reduced at the cathode to produce molten sodium metal. Some calcium is also produced but separates from the sodium due to differences in density.
Metals can be extracted from their ore through various processes depending on the reactivity of the metal. Less reactive metals can be manually separated from crushed ore, while more reactive metals require more energy-intensive processes like electrolysis or extraction in a blast furnace. In a blast furnace, ore, limestone flux and coke fuel are continuously fed into the top while hot air is blown into the bottom, allowing extraction of the metal in molten form from the bottom. Roasting is also used as a preliminary step, where sulfide ores are heated in air to transform the metal into an oxide and release sulfur dioxide gas. These processes can release toxic fumes and pollutants if not properly controlled.
1) Metals react with oxygen to form metal oxides, with reactivity varying between metals. The most reactive metals, such as sodium and potassium, burn vigorously while copper is the least reactive.
2) Metals also react with water and acids, producing hydrogen gas and salt solutions. More reactive metals like sodium and potassium react violently with water, while less reactive metals do not react or react slowly.
3) When metals react with non-metals, they form ionic compounds through transfer of electrons from the metal to the non-metal. Ionic compounds have high melting points, are brittle solids, and dissolve in water but not organic solvents.
Metals can be summarized as follows:
1) Metals are malleable, ductile, good conductors of heat and electricity, and have high melting points.
2) Alloys are mixtures of metals that are stronger and harder than pure metals due to interfering atomic layers.
3) Metals are extracted from ores via chemical and thermal processes, with the most common being the extraction of iron in a blast furnace.
The document discusses the process of extracting metals from ores. It begins by explaining how the reactivity of metals determines whether they are found in nature in elemental form or as compounds in ores. Extraction involves removing impurities from the ore, converting metal compounds to oxides, and then reducing the oxides to elemental metals. Less reactive metals can be extracted by heating while more reactive metals require electrolysis or displacement by other reactive metals. The pure metals may then be refined electrolytically to remove remaining impurities.
The document discusses alkaline earth metals, including their extraction methods and properties. It describes:
- Calcium is extracted via electrolysis of molten calcium chloride. Strontium and barium are similarly extracted through electrolysis of their molten chlorides.
- Radium is obtained by electrolysis of molten radium chloride using a mercury cathode and platinum anode.
- Alkaline earth metal salts impart characteristic flame colors from brick red (calcium) to apple green (barium).
- Their reactivity decreases down the group as ionization energy decreases.
This document outlines the key topics and concepts covered in a syllabus for a C5 Electricity & Chemistry course. It includes 9 points that describe electrolysis processes, products, and principles. Specifically, it covers how electrolysis breaks ionic compounds into simpler substances through the chemical effects of electricity. It also describes the use of electrodes, electrolytes, anodes and cathodes and how they relate to the reactions and products in different electrolysis examples, including molten salts, aqueous solutions, and metal refining. Finally, it mentions electroplating of metals and the industrial production of aluminum, chlorine, hydrogen and sodium hydroxide.
Metals and non-metals have distinct physical and chemical properties. Physically, metals tend to be solid, shiny, malleable, and good conductors of heat and electricity, while non-metals are usually brittle solids, liquids, or gases that are poor conductors. Chemically, metals react with non-metals like sulfur to form compounds called metal sulfides, and they react with oxygen to form metal oxides, which may dissolve in water to form bases. Non-metals also react with oxygen to form oxides, which dissolve in water to form acids like sulfurous acid. Common metals and non-metals have a variety of industrial and domestic uses based on their properties.
Ncert class 10 - science - chapter 3 - metals and non-metalsEswariKumaravel
The document discusses the properties of metals and non-metals. It describes how metals are lustrous, malleable, ductile, and good conductors of heat and electricity, while non-metals lack these properties. Experiments are presented to demonstrate that metals are lustrous, hard except for a few, malleable by hammering into thin sheets, and ductile by pulling into wires. Other experiments show that metals conduct heat by melting wax and conduct electricity by lighting a bulb. The document contrasts how metals and non-metals react with oxygen, water, acids, and how metals react in salt solutions in displacement reactions.
This document provides information on the physical and chemical properties of metals and non-metals. It discusses how metals are generally solids with high melting and boiling points that are malleable and good conductors, while non-metals exist in different physical states and have lower melting/boiling points. It also describes how metals react with oxygen, water, and acids to form metal oxides, hydroxides, and salts. Common extraction methods for metals from their ores include concentration, reduction, and refining. Corrosion of metals and methods to prevent it are also outlined.
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals react with oxygen, water, and acids. A reactivity series of metals is provided from most reactive to least. The document explains how ionic compounds form and their properties. The extraction of metals from ores is summarized including concentration, reduction, and refining steps. Common extraction methods are outlined for metals of high, medium, and low reactivity in the series.
all about metal and nonmetal of class 10 from physical to chemical....
last minute suggestion and preparation notes
made by student of 10th class only ..
short and sweet slides for quick revision...
HOPE IT MAY HELP U ...☺☻☺☻☺☻
Metals react with oxygen, water, acids, and salt solutions of metals. They tend to lose electrons during chemical reactions, forming positive ions. Metal oxides are formed when metals react with oxygen. Amphoteric oxides like zinc oxide and aluminum oxide can react with both acids and bases to form salts and water. Non-metals do not react with water because they cannot donate electrons to break the hydrogen-oxygen bonds. They also do not react with dilute acids but some exceptions exist, such as sulfur reacting with nitric acid. Aluminum undergoes various reactions including anodizing when treated with acids or steam in the laboratory.
This is a summary of the topic "metals" in the GCE O levels subject: Chemistry. Students taking either the combined science (chemistry/physics) or pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
The document discusses the properties and characteristics of metals and non-metals. It states that metals are generally found in the earth's crust in ores associated with other elements, and are also present in rocks, water, and dust. Non-metals lack metallic properties and are mostly gases or solids like carbon, sulfur, and phosphorus. A metalloid has properties between metals and non-metals. The document then discusses various physical and chemical properties of metals and non-metals such as conductivity, ductility, hardness, luster, malleability, physical state, sonority, examples, and their reactions with oxygen, water, acids, and other metal salts. It provides examples of these reactions and exceptions.
The document discusses the Downs Process for extracting sodium through the electrolysis of molten sodium chloride, where sodium ions are reduced to sodium atoms at the cathode and chlorine gas is produced at the anode. It also describes how sodium hydroxide is produced through the electrolysis of sodium chloride solutions, and lists some common uses of sodium and sodium hydroxide such as in soap production, as a drain cleaner, and for lighting.
This document provides information on the chemical properties of metals. It discusses how metals react with oxygen, water, acids, and metal salt solutions. It explains that the reactivity of metals varies, with metals like sodium and potassium being the most reactive due to losing their outer shell electrons easily. The document also discusses the formation of ionic compounds through the transfer of electrons from metals to non-metals, and provides examples of how ionic compounds like NaCl and MgCl2 are formed.
The document provides information about grade 10 IGCSE chemistry content related to properties and reactions of metals. It discusses distinguishing metals from non-metals, reactivity series, extraction of metals like iron from ores, and uses of metals such as aluminum and zinc. It also describes physical and chemical properties of metals, structure and properties of alloys, and reactions of metals with water, steam, and acids to determine reactivity order.
Metals react with oxygen, water, and acids to form metal oxides, hydroxides, or salts. They lose electrons and become positively charged ions. Non-metals react with oxygen to form non-metal oxides, gaining electrons and becoming negatively charged ions. Corrosion occurs as metals react with substances like oxygen and water in the air, forming coatings or rust. Corrosion can be prevented by applying protective coatings like oil, paint, zinc plating, or by alloying metals.
This document discusses the properties and reactivity of metals. It begins by describing the physical properties of metals, such as their hardness, malleability and conductivity. It then discusses the chemical properties of metals, including how they form positive ions and react with oxygen, water and acids. The document introduces metal alloys and explains why they are stronger than pure metals. It also defines the reactivity series and uses it to predict and describe the reactions of different metals. The document discusses the reactions of various metal compounds and how the position of metals in the reactivity series affects their reactivity and the stability of their compounds.
This document discusses a science presentation about the properties and reactions of metals and non-metals. It lists the group members giving the presentation and describes several properties of metals like malleability and conductivity. It then discusses how metals react with oxygen, water, acids, salt solutions, chlorine, hydrogen and how alloys are formed and used. For non-metals, it summarizes their reactions with oxygen, water, acids, salt solutions, chlorine, hydrogen and describes ionic compounds.
1. The Down's cell is an electrolytic cell that operates at 800°C to produce sodium metal through the electrolysis of molten sodium chloride.
2. It consists of a graphite anode and iron cathode separated by an iron screen inside a lined steel chamber. Molten sodium chloride mixed with calcium chloride and barium chloride is used as the electrolyte.
3. During electrolysis, chloride ions are oxidized at the anode to produce chlorine gas while sodium ions are reduced at the cathode to produce molten sodium metal. Some calcium is also produced but separates from the sodium due to differences in density.
Metals can be extracted from their ore through various processes depending on the reactivity of the metal. Less reactive metals can be manually separated from crushed ore, while more reactive metals require more energy-intensive processes like electrolysis or extraction in a blast furnace. In a blast furnace, ore, limestone flux and coke fuel are continuously fed into the top while hot air is blown into the bottom, allowing extraction of the metal in molten form from the bottom. Roasting is also used as a preliminary step, where sulfide ores are heated in air to transform the metal into an oxide and release sulfur dioxide gas. These processes can release toxic fumes and pollutants if not properly controlled.
1) Metals react with oxygen to form metal oxides, with reactivity varying between metals. The most reactive metals, such as sodium and potassium, burn vigorously while copper is the least reactive.
2) Metals also react with water and acids, producing hydrogen gas and salt solutions. More reactive metals like sodium and potassium react violently with water, while less reactive metals do not react or react slowly.
3) When metals react with non-metals, they form ionic compounds through transfer of electrons from the metal to the non-metal. Ionic compounds have high melting points, are brittle solids, and dissolve in water but not organic solvents.
Metals can be summarized as follows:
1) Metals are malleable, ductile, good conductors of heat and electricity, and have high melting points.
2) Alloys are mixtures of metals that are stronger and harder than pure metals due to interfering atomic layers.
3) Metals are extracted from ores via chemical and thermal processes, with the most common being the extraction of iron in a blast furnace.
The document discusses the process of extracting metals from ores. It begins by explaining how the reactivity of metals determines whether they are found in nature in elemental form or as compounds in ores. Extraction involves removing impurities from the ore, converting metal compounds to oxides, and then reducing the oxides to elemental metals. Less reactive metals can be extracted by heating while more reactive metals require electrolysis or displacement by other reactive metals. The pure metals may then be refined electrolytically to remove remaining impurities.
The document discusses alkaline earth metals, including their extraction methods and properties. It describes:
- Calcium is extracted via electrolysis of molten calcium chloride. Strontium and barium are similarly extracted through electrolysis of their molten chlorides.
- Radium is obtained by electrolysis of molten radium chloride using a mercury cathode and platinum anode.
- Alkaline earth metal salts impart characteristic flame colors from brick red (calcium) to apple green (barium).
- Their reactivity decreases down the group as ionization energy decreases.
This document outlines the key topics and concepts covered in a syllabus for a C5 Electricity & Chemistry course. It includes 9 points that describe electrolysis processes, products, and principles. Specifically, it covers how electrolysis breaks ionic compounds into simpler substances through the chemical effects of electricity. It also describes the use of electrodes, electrolytes, anodes and cathodes and how they relate to the reactions and products in different electrolysis examples, including molten salts, aqueous solutions, and metal refining. Finally, it mentions electroplating of metals and the industrial production of aluminum, chlorine, hydrogen and sodium hydroxide.
Metals and non-metals have distinct physical and chemical properties. Physically, metals tend to be solid, shiny, malleable, and good conductors of heat and electricity, while non-metals are usually brittle solids, liquids, or gases that are poor conductors. Chemically, metals react with non-metals like sulfur to form compounds called metal sulfides, and they react with oxygen to form metal oxides, which may dissolve in water to form bases. Non-metals also react with oxygen to form oxides, which dissolve in water to form acids like sulfurous acid. Common metals and non-metals have a variety of industrial and domestic uses based on their properties.
Ncert class 10 - science - chapter 3 - metals and non-metalsEswariKumaravel
The document discusses the properties of metals and non-metals. It describes how metals are lustrous, malleable, ductile, and good conductors of heat and electricity, while non-metals lack these properties. Experiments are presented to demonstrate that metals are lustrous, hard except for a few, malleable by hammering into thin sheets, and ductile by pulling into wires. Other experiments show that metals conduct heat by melting wax and conduct electricity by lighting a bulb. The document contrasts how metals and non-metals react with oxygen, water, acids, and how metals react in salt solutions in displacement reactions.
This document provides information on the physical and chemical properties of metals and non-metals. It discusses how metals are generally solids with high melting and boiling points that are malleable and good conductors, while non-metals exist in different physical states and have lower melting/boiling points. It also describes how metals react with oxygen, water, and acids to form metal oxides, hydroxides, and salts. Common extraction methods for metals from their ores include concentration, reduction, and refining. Corrosion of metals and methods to prevent it are also outlined.
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals react with oxygen, water, and acids. A reactivity series of metals is provided from most reactive to least. The document explains how ionic compounds form and their properties. The extraction of metals from ores is summarized including concentration, reduction, and refining steps. Common extraction methods are outlined for metals of high, medium, and low reactivity in the series.
This document provides information on the physical and chemical properties of metals and non-metals. It discusses how metals react with oxygen, water, and acids. A reactivity series of metals is presented from most reactive to least reactive. The document also describes how ionic compounds form and their properties. Extraction and refining of metals from their ores is outlined, including concentration, reduction, and electrolytic processes. Corrosion of metals and methods to prevent it are also summarized.
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals are generally solids, malleable, and good conductors, while non-metals can be solids, liquids, or gases and are not malleable. It explains how metals react with oxygen, water, and acids to form metal oxides, hydroxides, and salts. The reactivity of common metals is ranked in a reactivity series. The document also summarizes how metals are extracted from their ores through concentration, reduction, and refining processes. Electrolytic extraction and refining methods are described for reactive metals.
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals react with oxygen, water, and acids. A reactivity series of metals is provided. The document also discusses how ionic compounds form and their properties. The extraction of metals from ores and the refining process is explained. Corrosion of metals and methods to prevent it are covered. Alloys are defined as homogeneous mixtures of metals or metals with non-metals.
1. The document discusses the physical and chemical properties of metals and non-metals. It describes how metals react with oxygen, water, acids and metal salt solutions.
2. A reactivity series of metals is presented, ranking them from most reactive (potassium) to least reactive (gold). The extraction processes for obtaining metals from their ores is also outlined.
3. Metals are extracted via concentration, reduction, and refining steps. Extraction methods depend on the reactivity of the metal, involving processes like roasting, calcination, or electrolysis of molten ores.
The document discusses the physical and chemical properties of metals and non-metals. Metals are typically solid, malleable, ductile and good conductors of heat and electricity. They form basic oxides and displace less reactive metals from salt solutions. Non-metals can be solid, liquid or gas, are typically soft, brittle and poor conductors. Metals react with oxygen to form metal oxides, with water to form metal hydroxides and hydrogen gas, and with acids to form salts and hydrogen gas. The reactivity of metals determines how they are extracted from their ores.
This document summarizes the physical and chemical properties of metals and non-metals. It discusses how metals react with oxygen, water, and acids. It also describes the reactivity series of metals, how ionic compounds form, and how metals are extracted from their ores. Key points include:
- Metals are malleable and conductive while non-metals vary in state and are not usually malleable.
- Metals react with oxygen to form metal oxides, with water to form hydroxides and hydrogen, and with acids to form salts and hydrogen.
- The reactivity series arranges metals from most reactive (e.g. potassium) to least reactive (e.g. gold
The document discusses the physical and chemical properties of metals and non-metals. It describes how metals are generally solids, malleable, good conductors of heat and electricity, and react with oxygen, water, acids, and displace less reactive metals. It also discusses how non-metals can be solids, liquids or gases, are not malleable, and are generally poor conductors. The document then explains the extraction of metals from ores through concentration, reduction, and refining processes.
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals are generally solid, malleable, and good conductors, while non-metals can be solid, liquid, or gas and are not malleable. It also explains how metals react with oxygen, water, and acids, forming ionic compounds. Common extraction methods are outlined, such as electrolysis for reactive metals and roasting/reduction for others. The document concludes by discussing corrosion prevention through methods like galvanization and alloying.
Metal-and-Non-metal-10 BEST FOR CBSE STUDENTS.pptxravisharma1308
This document discusses the physical and chemical properties of metals and non-metals. It describes how metals are generally solid, malleable, good conductors of heat and electricity, and react with oxygen, water, and acids. Non-metals can be solid, liquid, or gas, are not malleable, conduct heat and electricity poorly, and do not react the same as metals. The reactivity of different metals is explained through the activity series. Common extraction methods include concentration, reduction, and refining. Corrosion and prevention methods are also outlined.
Metals and non-metals differ in their physical and chemical properties. Physically, metals are typically solid, hard, shiny, malleable and ductile with high melting and boiling points, while non-metals can be solid, liquid or gas with varying hardness, luster, malleability and melting/boiling points. Chemically, metals react with oxygen to form metal oxides, with water to form metal hydroxides and hydrogen gas, and with acids to form salts and hydrogen gas. Metals also displace less reactive metals in salt solutions. Non-metals gain electrons to form negative ions while metals lose electrons to form positive ions. Ionic bonds form when positive metal ions attract negative non-
The document discusses the physical and chemical properties of metals and non-metals. Physically, metals are typically solid, malleable, ductile, and good conductors of heat and electricity, while non-metals can be solid, liquid, or gas and are not malleable, ductile, or good conductors. Chemically, metals react with oxygen to form metal oxides, react with water or acids, and can corrode in air/moisture. Non-metals typically burn when reacting with oxygen to form non-metal oxides. The reactivity series lists metals in order of their reactivity from most (potassium) to least (gold, platinum) reactive.
The document discusses metals and non-metals. It describes the physical and chemical properties of metals and non-metals. Metals are lustrous, malleable, ductile and are good conductors of heat and electricity, while non-metals have opposite properties. It also discusses how metals and non-metals react with oxygen, water, acids and how displacement reactions can be used to determine reactivity order. Metals are extracted from ores through processes like enrichment, extraction using chemical/electrochemical methods depending on their reactivity.
The document describes the physical and chemical properties of metals and non-metals. Physically, metals are malleable and ductile, have metallic luster, and are good conductors of heat and electricity, while non-metals lack these properties. Chemically, metals are reactive and form basic oxides, reacting with acids to produce salts and hydrogen gas. They also react with water. Metals exist higher in the reactivity series and must be extracted through electrolysis, while less reactive metals can be extracted from their ores by heating. Common metals like iron, copper and aluminum are used to make containers and wires, while non-metals like silicon, sulfur and hydrogen have various industrial applications.
This document discusses the physical properties and reactions of metals and non-metals. Metals are solid, malleable, and good conductors of heat and electricity, while non-metals can be solid, liquid, or gas and are not malleable. Metals react differently with oxygen, water, and metal salt solutions depending on their reactivity. Most metals are found naturally as ores and must be extracted from impurities. Corrosion of metals can be prevented through various coatings and by forming alloys.
Metals react with oxygen, water, and acids to form metal oxides, hydroxides, or salts. They lose electrons and become positively charged ions. Non-metals react with oxygen to form non-metal oxides, generally do not react with water or acids, and gain electrons to become negatively charged ions. Corrosion occurs as metals react with substances like oxygen and water, forming coatings like rust. Corrosion can be prevented by applying protective coatings like oil, paint, zinc plating, or by alloying metals.
Alloys are mixtures of metals or metals with nonmetals that enhance properties like hardness and corrosion resistance. Common alloys include brass, bronze, and solder. Corrosion is the deterioration of metals due to reactions with air, moisture or chemicals. It can be prevented through methods like coating, alloying, galvanization, and electroplating. Metals are good conductors, malleable, and have high melting points, while nonmetals are brittle, poor conductors, and exist as solids, liquids or gases. Metals react with oxygen, acids, water and displacement reactions. Extraction methods depend on a metal's reactivity and include electrolysis, smelting, and self-reduction
Metals and non-metals have unique properties. Sodium and potassium have low melting points while mercury is liquid. Most metals like gold and silver are malleable and ductile, allowing them to be formed into wires. Electric wires are coated in plastic to prevent electric shock from conduction. Non-metals like carbon exist in different allotropes with varying properties. Metals react with oxygen to form metal oxides, and react with water to form metal hydroxides and hydrogen gas. More reactive metals can displace less reactive metals from their salt solutions. Metals are extracted from ores through processes like enrichment, roasting, and electrolytic refining.
1. The document discusses various properties and reactions involving metals and non-metals. It describes the structure of alloys and how they are stronger than pure metals.
2. Key extraction methods are related to a metal's position in the reactivity series, such as electrolysis of reactive metals and blast furnaces for less reactive metals.
3. Common uses of metals such as aluminum, zinc, and iron alloys are explained in terms of the metals' properties including strength, corrosion resistance, and galvanization.
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4. i) Reaction with oxygen :-
Metals react with oxygen to form metal oxides.
When copper is heated it combines with oxygen to form copper oxide.
2Cu + O2 2CuO
When aluminium is heated it combines with oxygen to form aluminium
oxide. 4Al + 3O2 2Al2O3
Some metal oxides are basic oxides because they react with water to
form bases.
4Na + O2 2Na2O
Na2O + H2O 2NaOH
K + O2 K2O
K2O + H2O 2KOH
Some metal oxides show acidic and basic properties. They are called
amphoteric oxides. Eg :- Aluminium oxide, Zinc oxide etc.
Al2O3 + 6HCl 2AlCl3 + 3H2O
(basic)
Al2O3 + NaOH NaAlO2 + H2O
(acidic) (Sodium aluminate)
* 2) Chemical properties of metals :-
6. Metals react with water to form metal oxides or metal hydroxides and
hydrogen.
2Na + 2H2O 2NaOH + H2
2K + H2O 2KOH + H2
Ca + H2O Ca(OH)2 + H2
2Al + 3H2O Al2O3 + H2
3Fe + 4H2O Fe2O3 + 4H2
The reactivity of different metals with water is different :-
- Sodium and potassium react violently with cold water to form sodium
hydroxide and hydrogen and catches fire.
- Calcium reacts less violently with water to form calcium hydroxide
and water and does not catch fire.
- Magnesium reacts only with hot water to form magnesium hydroxide
and hydrogen.
- Metals like aluminium, iron and zinc react only with steam to form
the metal oxides and hydrogen.
- Metals like lead, copper, silver and gold do not react with water.
* ii) Reaction with water :-
7. Metals react with dilute acids to form salts and hydrogen.
Mg + 2HCl MgCl2 + H2
2Al + 6 HCl 2AlCl3 + 3H2
Zn + 2HCl ZnCl2 + H2
Fe + 2HCl FeCl2 + H2
The reactivity varies from metal to metal. For the above
metals the decreasing order of reactivity is Mg > Al > Zn > Fe.
Copper, silver and gold do not react with dilute HCl.
Hydrogen gas is not evolved when metals react with
nitric acid (HNO3) because it is a strong oxidising agent and
it oxidises the H2 produced to water and is itself reduced to
oxides of nitrogen.
3Cu + 8HNO3 3Cu(NO3)2 + 4H2O + 2NO2
* iii) Reaction with acids :-
8. A more reactive metal displaces a less reactive metal from its salt
solution. (Displacement reaction)
Magnesium displaces copper from copper sulphate solution.
Mg + CuSO4 MgSO4 + Cu
Zinc displaces copper from copper sulphate solution.
Zn + CuSO4 ZnSO4 + Cu
Iron displaces copper from copper sulphate solution
Fe + CuSO4 FeSO4 + Cu
* iv) Reaction of metals with metal salt solutions
:-
after 15 – 20 minutes
9. The arranging of metals in the decreasing order of their
reactivity is called reactivity series of metals.
K - Potassium Most reactive
Na - Sodium
Ca - Calcium
Mg - Magnesium
Al - Aluminium
Zn - Zinc Reactivity decreases
Fe - Iron
Pb - Lead
H - Hydrogen
Cu - Copper
Hg - Mercury
Ag - Silver
Au - Gold Least reactive
* 3) Reactivity series of metals :-
10. Metals :- lose electrons and become positive ions. So they are
called electropositive elements.
Eg :- The atomic number of sodium is 11, its electronic configuration is
2,8,1, it has 1 valence electron. It loses 1 electron and forms a sodium
ion Na +
Na Na + + 1 e-
AN = 11
EC = 2,8,1 2,8
Mg Mg 2+ + 2 e-
AN = 12
EC = 2,8,2 2,8
Non metals :- gain electrons and become negative ions. So they
are called electro negative elements.
Eg:- The atomic number of chlorine is 17, its electronic configuration is
2,8,7, it has 7 valence. It gains 1 electron and forms a chloride ion Cl -
Cl + 1 e- Cl -
AN = 17
EC = 2,8,7 2,8,8
O + 2e- O 2-
AN = 8
EC = 2,6 2,8
* 4) How do metals an non metals react ?
11. Na . + Cl Na Cl NaCl
AN = 11 AN = 17
EC = 2,8,1 EC = 2,8,7
The atomic number of Na is 11, its electronic
configuration is 2,8,1, it has 1 valence electron, it loses 1
electron to form Na + ion. The atomic number of Cl is 17, its
electronic configuration is 2,8,7, it has 7 valence electrons,
it gains 1 electron to form Cl - ion. Then the attraction
between the Na + ion and Cl - ion results in the formation of
sodium chloride molecule – NaCl.
* 5a) Formation of sodium chloride molecule – NaCl
x
x
x
x
x
x
x
.
x
xx
x
x x
x
+ -
12. Mg Mg 2+ + 2e -
AN = 12
EC = 2,8,2 2,8
Cl + 1e - Cl -
AN = 17
EC = 2,8,7 2,8,8
Mg + Mg MgCl2
The AN of Mg is 12, its EC is 2,8,2, it has 2 valence electrons, it loses
2 electrons to form Mg 2+ . The AN of Cl is 17, its EC is 2,8,7, it has 7
valence electrons, it gains 1 electron to form Cl -. Then the attraction
between Mg 2+ ion and 2 Cl - ions results in the formation of Magnesium
chloride molecule – MgCl2 .
* b) Formation of Magnesium chloride molecule – MgCl2
.
.
x
x
x
x
x
x
x
x
x
x
x
x
x
x
2+
-
x
xx
x
x
x
x
.
Cl
Cl
-
x
xx
x
x
x
x
.
Cl
Cl
13. Ionic compounds are compounds formed by the transfer of
electrons from a metal to a non metal.
Properties of ionic compounds :-
i) They are formed by the transfer of electrons and are made up of
ions.
i) They are crystalline solids.
ii) They have high melting points and boiling points.
iii) They are soluble in water but insoluble in organic solvents (like
petrol, kerosene etc.)
iv) They conduct electricity in molten state or in solution.
* 6) Ionic compounds (Electrovalent compounds) :-
14. Some metals like gold, silver, platinum etc are found in the free
state in the earth’s crust because they are least reactive. Most metals
are found as oxides, carbonates, sulphides, halides etc.
Minerals :- are elements or compounds which occur naturally inside
the earth’s crust.
Ore :- is a mineral from which metals can be extracted profitably.
Gangue :- is the impurities present in the ore like rock particles,
sand particles, clay particles etc.
b) Extraction of metals from their ores :-
Metals are extracted from their ores in three main steps. They are :-
i) Concentration of the ore (Enrichment of the ore).
ii) Reduction to the metal.
iii) Refining (Purification of the metal).
Concentration of the ore :- is the removal of gangue (impurities)
from the ore by different methods.
* 7a) Occurence of metals :-
15. Metals of Metals of Metals of
high reactivity medium reactivity low reactivity
Electrolysis of
molten ore Carbonate ore Sulphide ore Sulphide ore
Pure metal Calcination Roasting Roasting
Oxide of metal Metal
Reduction to metal Refining
Refining
* 8) Steps involved in the extraction of metals from their ores :-
Ore
16. Metals which are low in the activity series can be
reduced to the metals by heating in the presence of oxygen
(Roasting).
Eg :- Mercury is obtained from its ore Cinnabar (HgS) by
heating in the presence of oxygen. When it is heated in the
presence of oxygen it is first converted into mercuric oxide
(HgO) and on further heating it is reduced to mercury.
2HgS + 3O2 2HgO + 2O2
2HgO 2Hg + O2
Copper is obtained from its sulphide ore (CuS) by
heating in the presence of oxygen.
2CuS + 3O2 2Cu2O + 2SO2
2Cu2O + Cu2S 6Cu + SO2
* i) Extraction of metals low in the activity series :-
heat
heat
heat
heat
17. Metals in the middle of the activity series like Zn, Fe, Pb, are found as
oxide, sulphide or carbonate ores.
It is easier to obtain metals from their oxides than from their
sulphides or carbonates. So non oxide ores are converted into oxide
form before reduction. Non oxide ores can be converted into oxide form
by roasting or calcination.
Roasting :- is heating of an ore in the presence of oxygen. It is used to
convert suphide ores into oxide form.
Eg :- 2 ZnS + 3O2 2 ZnO + 2SO2
Calcination :- is heating of an ore in the absence of oxygen. It is used to
convert sulphide ores into oxide form.
Eg :- ZnCO3 ZnO + CO2
The oxide ore is then reduced to the metal by heating with a reducing
agent. The most common reducing agent is coke (carbon).
Eg :- ZnO + C Zn + CO
* ii) Extraction of metals in the middle of the activity
series :-
heat
heat
heat
18. Sometimes reactive metals like Na, Ca, Al etc. are used
as reducing agents to obtain metals from their oxides.
Eg :- 3MnO2 + 4Al Mn + 3Al2O3 + Heat
(Manganese (Manganese)
dioxide)
The reaction between metal oxides and aluminium is
highly exothermic and the metals are obtained in molten
state. Such reactions are called thermit reactions.
The reaction between iron oxide and aluminium
produces molten iron. This reaction is used to join rail
tracks, broken machine parts etc.
Fe2O3 + 2Al Al2O3 + 2Fe + Heat
* Thermit reactions :-
20. Metals at the top of the activity series like K, Na, Ca, Al etc. cannot
be obtained from their ores by simple heating or by heating with
reducing agents. They are obtained by electrolytic reduction of their
molten chlorides.
Eg :- When electric current is passed through molten sodium
chloride, sodium metal is deposited at the cathode and chlorine gas is
deposited at the anode.
At cathode :- Na + + e - Na (Sodium metal)
At anode :- 2Cl - Cl2 + 2e - (Chlorine gas)
* iii) Extraction of metals at the top of the activity series :-
21. The removal of impurities from the metal to obtain the pure metal is
called refining of metals. The most common method for refining of
metals is electrolytic refining.
In this method a block of the impure metal is made the anode and a
thin sheet of the pure metal is made the cathode. The electrolyte is a salt
solution of the metal to be purified.
Eg :- In the electrolytic refining of copper, a block of impure copper is
made the anode and a thin sheet of pure copper is made the cathode.
The electrolyte is acidified copper sulphate solution. When electric
current is passed through the electrolyte, pure copper from the anode is
deposited at the cathode and the impurities settle down as anode mud.
* 9) Refining of metals :-
22. Corrosion is the damage caused to metals due to the reaction of metals
with oxygen, moisture, carbon dioxide etc.
Eg :- Formation of brown coating of rust over iron.
Formation of green coating of basic copper carbonate over copper.
Formation of black coating of silver sulphide over silver.
To show that air and moisture are necessary for the rusting of iron :-
Take three test tubes marked 1,2,3 and put iron nails in each of them. Put some
anhydrous calcium chloride in test tube 1 to absorb moisture. Pour some boiled distilled
water in test tube 2 and pour some oil over it to prevent air into the test tube. Pour some
water in test tube 3. Cork the test tubes and leave them for a few days. The nails in test
tube 1 does not get rusted because it had only air and no water. The nails in test tube 2
does not rust because it had only water and no air. The nails in test tube 3 gets rusted
because it had air and water.
* 10a) Corrosion :-
23. Corrosion of metals can be prevented by :-
i) Applying oil or grease.
ii) Applying paint.
iii) By galvanisation. (Coating with zinc)
iv) By tinning. (Coating with tin)
v) By electroplating. (Coating a less reactive metal like chromium)
vi) By alloying. (Making alloys)
c) Alloy :-
An alloy is a homogeneous mixture of a metal with other metals or
non metal.
Eg :- Steel – iron, carbon
Stainless steel – iron, carbon, cobalt, nickel
Brass – copper, zinc
Bronze – copper, tin
Solder – Lead, tin (used for welding electrical wires together)
If one of the metals in an alloy is mercury, it is called an amalgam.
* b) Prevention of corrosion :-