The document describes displacement reactions between metals and metal ion solutions. More reactive metals can displace less reactive metals from their solutions. For example, magnesium displaces iron from iron(II) nitrate, forming magnesium nitrate and iron. Magnesium is more reactive than iron. Lead also displaces copper from copper(II) sulphate, forming lead(II) sulphate and copper, as lead is more reactive than copper. However, copper does not displace lead, as copper is not more reactive than lead.
Reactions Of Metals And Metal Compoundsamr hassaan
The document discusses chemical reactions involving metals and their compounds. It explains that metals react with acids to produce salts and hydrogen gas. It also discusses how metals react with oxygen and carbon dioxide to form metal oxides and metal carbonates, which can then further react with acids. The document provides examples of word equations for common metal-acid reactions and identifies the products and reactants in various chemical changes involving metals and 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.
This document provides information on naming and writing formulas for ionic and molecular compounds. It discusses the characteristics of ionic compounds and how to name ionic compounds by writing the metal name followed by the nonmetal name with an "-ide" ending. It also covers transition metal naming conventions using Roman numerals to indicate charge. The document explains how to write formulas from compound names and discusses common polyatomic ions and how to write formulas containing polyatomic ions.
This chapter discusses the physical and chemical properties of metals. Metals are usually hard, shiny, malleable and ductile. They are good conductors of heat and electricity. Chemically, metals form positive ions and react with acids, oxygen, water and steam to form salts and release hydrogen gas. The reactivity of metals can be predicted based on their reactivity series, with more reactive metals displacing less reactive ones from their compounds. Alloys are stronger than pure metals due to disrupted atomic layers.
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.
Metals and non metals without animatiopnBalendu Kumar
The document discusses the properties and classification of metals and non-metals. It states that metals are good conductors of heat and electricity, can be molded and drawn into wires, and react with oxygen to form basic oxides. Non-metals may be solids, liquids or gases, are typically poor conductors, and react with oxygen to form acidic oxides. The document provides examples of chemical reactions to illustrate differences in how metals and non-metals react with water, acids, oxygen, and how displacement reactions occur between metals. It also lists some common uses of metals like iron, aluminum, and silver as well as non-metals like iodine, oxygen, sulfur, and phosphorus.
This document outlines key concepts about acids, bases, and salts. It defines acids as substances that produce hydrogen ions in water. There are strong acids that fully ionize and weak acids that partially ionize. Bases are oxides or hydroxides of metals. Alkalis are soluble bases that produce hydroxide ions in water. Acids and bases react to form salts and water in a neutralization reaction. The pH scale measures acidity and alkalinity. Indicators change color with pH. There are four types of oxides. Salts contain cations from bases and anions from acids. Common salts have various industrial and domestic uses.
Reactions Of Metals And Metal Compoundsamr hassaan
The document discusses chemical reactions involving metals and their compounds. It explains that metals react with acids to produce salts and hydrogen gas. It also discusses how metals react with oxygen and carbon dioxide to form metal oxides and metal carbonates, which can then further react with acids. The document provides examples of word equations for common metal-acid reactions and identifies the products and reactants in various chemical changes involving metals and 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.
This document provides information on naming and writing formulas for ionic and molecular compounds. It discusses the characteristics of ionic compounds and how to name ionic compounds by writing the metal name followed by the nonmetal name with an "-ide" ending. It also covers transition metal naming conventions using Roman numerals to indicate charge. The document explains how to write formulas from compound names and discusses common polyatomic ions and how to write formulas containing polyatomic ions.
This chapter discusses the physical and chemical properties of metals. Metals are usually hard, shiny, malleable and ductile. They are good conductors of heat and electricity. Chemically, metals form positive ions and react with acids, oxygen, water and steam to form salts and release hydrogen gas. The reactivity of metals can be predicted based on their reactivity series, with more reactive metals displacing less reactive ones from their compounds. Alloys are stronger than pure metals due to disrupted atomic layers.
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.
Metals and non metals without animatiopnBalendu Kumar
The document discusses the properties and classification of metals and non-metals. It states that metals are good conductors of heat and electricity, can be molded and drawn into wires, and react with oxygen to form basic oxides. Non-metals may be solids, liquids or gases, are typically poor conductors, and react with oxygen to form acidic oxides. The document provides examples of chemical reactions to illustrate differences in how metals and non-metals react with water, acids, oxygen, and how displacement reactions occur between metals. It also lists some common uses of metals like iron, aluminum, and silver as well as non-metals like iodine, oxygen, sulfur, and phosphorus.
This document outlines key concepts about acids, bases, and salts. It defines acids as substances that produce hydrogen ions in water. There are strong acids that fully ionize and weak acids that partially ionize. Bases are oxides or hydroxides of metals. Alkalis are soluble bases that produce hydroxide ions in water. Acids and bases react to form salts and water in a neutralization reaction. The pH scale measures acidity and alkalinity. Indicators change color with pH. There are four types of oxides. Salts contain cations from bases and anions from acids. Common salts have various industrial and domestic uses.
Alkali metals react vigorously with chlorine to form metal chlorides. Lithium reacts with chlorine gas to form lithium chloride according to the chemical equation 2Li (s) + Cl2 (g) → 2LiCl (s). Sodium also reacts with chlorine gas in a similar reaction to form sodium chloride, represented by the equation 2Na (s) + Cl2 (g) → 2NaCl (s).
The document discusses minerals found in the Earth's crust, describing minerals as either natural elements or natural compounds. It provides examples of common elements like carbon and compounds like calcium carbonate that make up minerals. Properties of minerals like hardness and solubility in water are also examined, along with how heating can decompose some mineral compounds.
The document discusses learning outcomes about salts. It defines a salt as a compound formed when a hydrogen ion from an acid is replaced by a metal ion or ammonium ion. Examples of commonly used salts include NaCl, MSG, and CaCO3. Salts can be soluble or insoluble depending on their cation and anion. The document also describes different methods for preparing soluble and insoluble salts, such as titration, evaporation/heating, cooling/crystallization, filtration, and drying.
Metals are good conductors of electricity and heat, have high melting and boiling points, and can be hammered into shapes or pulled into wires. Examples include aluminum, copper, iron, and silver. Non-metals include gases like oxygen and neon at room temperature, liquids like bromine, and solids like carbon and phosphorus. Unlike metals, non-metals do not conduct electricity well and have low melting and boiling points.
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
This document discusses different types of bonding between atoms, including ionic and covalent bonding. It addresses why atoms form bonds, the types of bonds present in pure elements versus compounds, and examples of ionic compounds like NaCl, H2O and their structures. Multiple choice questions are also included to test understanding of ion formation, ionic compound formulas, and which processes contribute to making ionic bond formation energetically favorable.
A salt is formed when a hydrogen ion from an acid is replaced by a metal ion or ammonium ion. The solubility of a salt in water is important for determining the suitable method for preparing it. Common soluble salts include ammonium, sodium, and potassium salts as well as most nitrate, chloride, and sulfate salts. However, some chloride, sulfate, and carbonate salts are insoluble such as silver chloride, lead chloride, mercury chloride, calcium sulfate, lead sulfate, barium sulfate, and most metal carbonates. Knowing whether a salt is soluble or insoluble is crucial before preparing it.
This presentation follows metals and focuses on the transition metals over to the pure metals, non-metals and metalloids. If you are a teacher, I have a great lab to help students classify substances based on their physical and chemical properties. Just drop me a line at gjohnston@ssis.edu.vn
The document summarizes the periodic table, including who created it and how elements are organized. Dmitri Mendeleev and Lothar Meyer independently developed the periodic table around the same time, but Mendeleev published his first. The periodic table arranges elements by atomic number and groups them according to metal/non-metal properties and families such as noble gases, halogens, and transition metals. It also provides examples of the elements boron, aluminum, and beryllium, where they are found and some of their uses.
Metals, nonmetals, and metalloids can be distinguished by their physical properties. Metals are typically solids, shiny, malleable, and good conductors of heat and electricity. Nonmetals may be solids, liquids, or gases, have a dull luster, and are poor conductors. Metalloids have properties in between metals and nonmetals, and some are useful semiconductors. Most metals are found combined with other elements in minerals and ores in the Earth's crust. Carbon is unusual in that it can form graphite, which is brittle, or diamonds, the hardest natural material, depending on the arrangement of carbon atoms.
This document provides information about gold and introduces purple gold. It discusses the proportions of gold in different karats, the various colors of gold including yellow, white and pink, and how purple gold is an intermetallic compound of gold and aluminum. The document also summarizes that purple gold was invented in 2000 in Singapore, is low in malleability, and requires special care as it can react to acids and other contaminants.
This document provides the names and formulas of various ionic compounds. It lists the names of 40 ionic compounds along with their corresponding chemical formulas. The names provide the cation and anion present in each compound as well as the ionic charges. The formulas identify the elements and their ratios that make up each ionic compound.
1. The document discusses types of salts, how they are named, and methods of salt formation.
2. Common salt formation reactions include reactions between metals/metal compounds with acids/acid salts to form new salts and water.
3. The document provides examples of salt naming conventions and outlines several common salt formation methods like double displacement and acid-base reactions.
This document lists common metal compounds along with their chemical formulas and ion charges. It provides the names and formulas for metal oxides, hydroxides, chlorides, bromides, iodides, sulfates, carbonates, and nitrates of metals like sodium, potassium, calcium, zinc, aluminum, iron, copper, silver, and ammonium. The metals are listed with their common oxidation states and the ions are shown with their corresponding charges in the compounds.
This document lists common metal compounds along with their chemical formulas and ion charges. It provides the names and formulas for metal oxides, hydroxides, chlorides, bromides, iodides, sulfates, carbonates, and nitrates of metals like sodium, potassium, calcium, zinc, aluminum, iron, copper, silver, and ammonium. The metals are listed with their common oxidation states and the ions are shown with their associated charges in the compounds.
This document provides information about minerals, including their typical uses, definitions, groups, properties, and identification tests. It discusses the main mineral groups like silicates and non-silicates. It also describes several properties used to identify minerals, such as crystal form, luster, hardness, cleavage, specific gravity, and reactions to acid. Identification of minerals involves analyzing their physical and chemical properties.
The document discusses the key differences between metals and non-metals, the sources and extraction of metals from ores, the formation of alloys through the addition of other metals, examples of main group metals important in biology, and the properties, electronic configurations, and common oxidation states of transition metals.
The document discusses acids, bases, and salts. It defines acids as substances that form hydrogen ions in water, such as hydrochloric acid, sulfuric acid, and nitric acid. Bases are defined as oxides and hydroxides of metals that react with acids to form salts and water. Common strong acids and their ions are listed, as well as common weak acids. The properties, naming, and formula writing of acids and bases are also covered.
Salts are formed when hydrogen ions in acids are replaced by metal ions or ammonium ions. There are two main types of salts - normal salts that do not contain replaceable hydrogen and acidic salts that contain replaceable hydrogen. Insoluble salts are prepared through precipitation reactions by mixing solutions of reactants containing the ions of the insoluble salt. Soluble salts can be prepared through filtration and crystallization using excess insoluble reactants or through titration using exact quantities of reactants.
The document provides examples of naming and writing formulas for various chemical compounds. It gives the names for 20 chemical formulas, such as sodium bromide for NaBr. It then gives the formulas for 20 chemical names, such as silicon dioxide for SiO2. Finally, it provides 20 more examples of naming or writing formulas for ionic and covalent compounds and identifies whether they are ionic or covalent.
The periodic table arranges elements in horizontal rows called periods and vertical columns called groups. It provides the symbol, name, and proton number of each element. Group 1 elements are alkali metals that react with oxygen and water. Transition metals are hard, colored solids that form complex compounds and are less reactive than alkali metals. The reactivity series lists metals in order of reactivity from most to least reactive. Displacement reactions occur when a more reactive metal displaces a less reactive one from a compound.
This document discusses the properties and reactivity of metals. It begins by describing the physical properties of metals, such as their hardness, malleability, conductivity and high melting points. It then discusses the chemical properties of metals, explaining how they form positive ions and react with oxygen, water and acids. Key points covered include the structure of pure metals and alloys, the reactivity series, and how the reactivity of metals relates to their tendency to form ions. Reactions of specific metals like magnesium, sodium and calcium are described. The document also addresses the passivating effect of metal oxides like aluminum oxide.
Alkali metals react vigorously with chlorine to form metal chlorides. Lithium reacts with chlorine gas to form lithium chloride according to the chemical equation 2Li (s) + Cl2 (g) → 2LiCl (s). Sodium also reacts with chlorine gas in a similar reaction to form sodium chloride, represented by the equation 2Na (s) + Cl2 (g) → 2NaCl (s).
The document discusses minerals found in the Earth's crust, describing minerals as either natural elements or natural compounds. It provides examples of common elements like carbon and compounds like calcium carbonate that make up minerals. Properties of minerals like hardness and solubility in water are also examined, along with how heating can decompose some mineral compounds.
The document discusses learning outcomes about salts. It defines a salt as a compound formed when a hydrogen ion from an acid is replaced by a metal ion or ammonium ion. Examples of commonly used salts include NaCl, MSG, and CaCO3. Salts can be soluble or insoluble depending on their cation and anion. The document also describes different methods for preparing soluble and insoluble salts, such as titration, evaporation/heating, cooling/crystallization, filtration, and drying.
Metals are good conductors of electricity and heat, have high melting and boiling points, and can be hammered into shapes or pulled into wires. Examples include aluminum, copper, iron, and silver. Non-metals include gases like oxygen and neon at room temperature, liquids like bromine, and solids like carbon and phosphorus. Unlike metals, non-metals do not conduct electricity well and have low melting and boiling points.
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
This document discusses different types of bonding between atoms, including ionic and covalent bonding. It addresses why atoms form bonds, the types of bonds present in pure elements versus compounds, and examples of ionic compounds like NaCl, H2O and their structures. Multiple choice questions are also included to test understanding of ion formation, ionic compound formulas, and which processes contribute to making ionic bond formation energetically favorable.
A salt is formed when a hydrogen ion from an acid is replaced by a metal ion or ammonium ion. The solubility of a salt in water is important for determining the suitable method for preparing it. Common soluble salts include ammonium, sodium, and potassium salts as well as most nitrate, chloride, and sulfate salts. However, some chloride, sulfate, and carbonate salts are insoluble such as silver chloride, lead chloride, mercury chloride, calcium sulfate, lead sulfate, barium sulfate, and most metal carbonates. Knowing whether a salt is soluble or insoluble is crucial before preparing it.
This presentation follows metals and focuses on the transition metals over to the pure metals, non-metals and metalloids. If you are a teacher, I have a great lab to help students classify substances based on their physical and chemical properties. Just drop me a line at gjohnston@ssis.edu.vn
The document summarizes the periodic table, including who created it and how elements are organized. Dmitri Mendeleev and Lothar Meyer independently developed the periodic table around the same time, but Mendeleev published his first. The periodic table arranges elements by atomic number and groups them according to metal/non-metal properties and families such as noble gases, halogens, and transition metals. It also provides examples of the elements boron, aluminum, and beryllium, where they are found and some of their uses.
Metals, nonmetals, and metalloids can be distinguished by their physical properties. Metals are typically solids, shiny, malleable, and good conductors of heat and electricity. Nonmetals may be solids, liquids, or gases, have a dull luster, and are poor conductors. Metalloids have properties in between metals and nonmetals, and some are useful semiconductors. Most metals are found combined with other elements in minerals and ores in the Earth's crust. Carbon is unusual in that it can form graphite, which is brittle, or diamonds, the hardest natural material, depending on the arrangement of carbon atoms.
This document provides information about gold and introduces purple gold. It discusses the proportions of gold in different karats, the various colors of gold including yellow, white and pink, and how purple gold is an intermetallic compound of gold and aluminum. The document also summarizes that purple gold was invented in 2000 in Singapore, is low in malleability, and requires special care as it can react to acids and other contaminants.
This document provides the names and formulas of various ionic compounds. It lists the names of 40 ionic compounds along with their corresponding chemical formulas. The names provide the cation and anion present in each compound as well as the ionic charges. The formulas identify the elements and their ratios that make up each ionic compound.
1. The document discusses types of salts, how they are named, and methods of salt formation.
2. Common salt formation reactions include reactions between metals/metal compounds with acids/acid salts to form new salts and water.
3. The document provides examples of salt naming conventions and outlines several common salt formation methods like double displacement and acid-base reactions.
This document lists common metal compounds along with their chemical formulas and ion charges. It provides the names and formulas for metal oxides, hydroxides, chlorides, bromides, iodides, sulfates, carbonates, and nitrates of metals like sodium, potassium, calcium, zinc, aluminum, iron, copper, silver, and ammonium. The metals are listed with their common oxidation states and the ions are shown with their corresponding charges in the compounds.
This document lists common metal compounds along with their chemical formulas and ion charges. It provides the names and formulas for metal oxides, hydroxides, chlorides, bromides, iodides, sulfates, carbonates, and nitrates of metals like sodium, potassium, calcium, zinc, aluminum, iron, copper, silver, and ammonium. The metals are listed with their common oxidation states and the ions are shown with their associated charges in the compounds.
This document provides information about minerals, including their typical uses, definitions, groups, properties, and identification tests. It discusses the main mineral groups like silicates and non-silicates. It also describes several properties used to identify minerals, such as crystal form, luster, hardness, cleavage, specific gravity, and reactions to acid. Identification of minerals involves analyzing their physical and chemical properties.
The document discusses the key differences between metals and non-metals, the sources and extraction of metals from ores, the formation of alloys through the addition of other metals, examples of main group metals important in biology, and the properties, electronic configurations, and common oxidation states of transition metals.
The document discusses acids, bases, and salts. It defines acids as substances that form hydrogen ions in water, such as hydrochloric acid, sulfuric acid, and nitric acid. Bases are defined as oxides and hydroxides of metals that react with acids to form salts and water. Common strong acids and their ions are listed, as well as common weak acids. The properties, naming, and formula writing of acids and bases are also covered.
Salts are formed when hydrogen ions in acids are replaced by metal ions or ammonium ions. There are two main types of salts - normal salts that do not contain replaceable hydrogen and acidic salts that contain replaceable hydrogen. Insoluble salts are prepared through precipitation reactions by mixing solutions of reactants containing the ions of the insoluble salt. Soluble salts can be prepared through filtration and crystallization using excess insoluble reactants or through titration using exact quantities of reactants.
The document provides examples of naming and writing formulas for various chemical compounds. It gives the names for 20 chemical formulas, such as sodium bromide for NaBr. It then gives the formulas for 20 chemical names, such as silicon dioxide for SiO2. Finally, it provides 20 more examples of naming or writing formulas for ionic and covalent compounds and identifies whether they are ionic or covalent.
The periodic table arranges elements in horizontal rows called periods and vertical columns called groups. It provides the symbol, name, and proton number of each element. Group 1 elements are alkali metals that react with oxygen and water. Transition metals are hard, colored solids that form complex compounds and are less reactive than alkali metals. The reactivity series lists metals in order of reactivity from most to least reactive. Displacement reactions occur when a more reactive metal displaces a less reactive one from a compound.
This document discusses the properties and reactivity of metals. It begins by describing the physical properties of metals, such as their hardness, malleability, conductivity and high melting points. It then discusses the chemical properties of metals, explaining how they form positive ions and react with oxygen, water and acids. Key points covered include the structure of pure metals and alloys, the reactivity series, and how the reactivity of metals relates to their tendency to form ions. Reactions of specific metals like magnesium, sodium and calcium are described. The document also addresses the passivating effect of metal oxides like aluminum oxide.
This document is a chapter from a textbook on metals and their reactivity. It discusses the physical and chemical properties of metals, including their structure and properties of alloys. It introduces the reactivity series of metals and how their reactivity relates to their tendency to form ions. The chapter describes displacement reactions between metals and explains how the reactivity series can be used to predict these reactions. It also discusses the reduction of metal oxides by carbon and hydrogen as well as the thermal stability of different metal compounds. In summary, the chapter provides an overview of metals and uses the reactivity series to explain and predict their chemical behaviors.
This document provides information on typical chemical reactions including displacement reactions between metals and between halogens. It discusses how reactivity series can predict which reactants will undergo displacement, with the more reactive element displacing the less reactive one. General equations for displacement reactions and other common reactions like metals reacting with acids are given. Word and balanced chemical equations are provided as examples.
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 metals reacting with acids to form salts and hydrogen gas. The key points are:
1) Metals react with acids according to the general equation: Metal + Acid → Salt + Hydrogen.
2) Salts have the metal as the first name and acid as the last name, such as magnesium chloride from magnesium and hydrochloric acid.
3) Copper is less reactive than magnesium and zinc based on experiments showing these metals reacting with hydrochloric and sulfuric acids to form salts and hydrogen while copper did not react.
This document provides information on synthesizing and qualitatively analyzing salts. It discusses how salts are formed by replacing hydrogen ions in acids with metal ions or ammonium ions. Common salt reactions and solubility rules for various salts are presented. Methods for synthesizing soluble and insoluble salts are described. Qualitative salt analysis involves tests to identify cations using sodium hydroxide and ammonium hydroxide solutions and tests to identify anions using reagents like barium chloride and silver nitrate solutions. Color changes, gas evolution and precipitate formation are observed to determine the present ions.
The document discusses the reactivity and extraction of various metals. It introduces the reactivity series, which ranks metals based on their reactivity with oxygen, acids, and water. More reactive metals are higher in the series and displace less reactive ones. Extraction methods depend on reactivity - less reactive metals like copper can be extracted by heating their ores with carbon, while very reactive metals require electrolysis.
The document discusses metals, non-metals, and chemical reactions. It provides examples of displacement reactions using various metals and metal sulfates. It also discusses the corrosion of iron, copper, and silver when exposed to atmospheric gases and moisture. Key points covered include the displacement of less reactive metals by more reactive ones in a reactivity series, and how iron rusts and copper and silver develop colored coatings from corrosion.
This document provides information on metals and the periodic table. It discusses the layout and components of the periodic table. It then focuses on Group 1 alkali metals, their properties, and reactions with water. It also covers transition metals, common element symbols, and reactions of metals with oxygen, water, and acids. Displacement reactions and the reactivity series are explained. The document concludes with information on extracting metals, including the blast furnace process and electrolysis.
This document discusses reactivity of metals and minerals. It begins by describing the different types of minerals found in rocks and ores, including natural elements like gold and compounds like limestone. It then explains how the reactivity of metals can be determined by observing their reactions with oxygen and other substances. Experiments are described to determine the position of carbon and hydrogen in the reactivity series by observing whether they can displace metals from metal oxides when heated. The document concludes that understanding the reactivity series is important for extracting metals from their ores.
The document provides information about the reactivity series of metals and oxidation-reduction reactions. It begins by defining key terms like displacement reaction, alkali metals, oxidation, and reduction. It then describes several classroom activities where students observe demonstrations of alkali metal reactions and determine the reactivity order. Students also write word and balanced equations for metal reactions with oxygen, water, and acids. The activities help students understand that more reactive metals displace less reactive ones and form positive ions more easily. The document emphasizes that oxidation involves gain of oxygen while reduction involves loss of oxygen.
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 reactions of metals with acids and their uses. It explains that metals are found naturally in ores and can be extracted. Certain metals like aluminum, steel, and iron have specific uses like in aircraft, cooking pots, etc. due to their properties. It also describes how most metals react with acids to produce salts and hydrogen gas. The reactivity of metals follows certain patterns that allow predictions of how a metal will react with acid.
This document provides information on metals and the periodic table. It discusses the layout and components of the periodic table. It then focuses on Group 1 alkali metals, their properties, and reactions with water. It also covers transition metals, common element symbols, and reactions of metals with oxygen, water, and acids. Displacement reactions and the reactivity series are explained. The document concludes with information on extracting metals, electrolysis, and rusting.
The document provides information about extracting iron from its ore, hematite. It describes the process of reduction, where iron oxide is heated with carbon to produce iron and carbon dioxide. The reaction works through oxidation of carbon and reduction of iron. Iron is extracted through the reduction of its ore, hematite (iron oxide), using carbon as the reducing agent. The carbon is oxidized, removing oxygen from the iron oxide and producing iron and carbon dioxide.
Metals and non-metals.pptx CLAA 8 COLLINSansul23jan
This chapter discusses the physical and chemical properties of metals and non-metals. It defines metals as hard, shiny, malleable and ductile materials, while non-metals are dull, brittle materials. The chapter describes the physical properties of metals and non-metals such as state, hardness, lustre, malleability, conductivity. It also discusses their chemical properties including reactions with oxygen, water, acids, and bases. Finally, it outlines some common uses of metals like in machinery and non-metals like oxygen in breathing and iodine as an antiseptic.
The document discusses the properties and reactivity of metals. It describes experiments to determine the reactivity series of metals by observing their reactions with water, steam, and dilute acids. Metals react differently in each test based on their positions in the reactivity series, from most reactive to least reactive. The reactivity series allows prediction of other reactions like reduction of metal oxides and decomposition of metal carbonates.
The document discusses the activity series of metals and how it can be used to predict products of displacement reactions. It provides examples of reactions that can occur between different metals and solutions like aluminum displacing hydrogen from acid, sodium displacing hydrogen from water, and magnesium displacing zinc from a solution. The document then describes a procedure for developing an activity series based on laboratory observations of reactions between metal strips and salt solutions. Observations such as gas evolution, color changes, and precipitate formation are noted. The results are recorded in a table showing reactions between various metals and solutions of salts like aluminum sulfate, copper sulfate, zinc sulfate, nickel sulfate, lead sulfate, and iron sulfate.
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 defines and explains various types of numbers. It describes perfect squares as whole numbers squared, and square roots as factors of a number whose product equals that number. Radical signs represent nonnegative square roots. Irrational numbers cannot be expressed as fractions, while real numbers include both irrational and rational numbers. Natural numbers are positive whole numbers, and whole numbers include zero, with integers extending to negative numbers as well. Rational numbers can be expressed as fractions of integers.
This document lists 40 problems that identify properties of mathematics such as addition, subtraction, multiplication, and variables. Each problem identifies a specific property being demonstrated such as the commutative property, associative property, identity property, inverse property, closure property, and distributive property. The problems cover properties as they relate to numbers, fractions, and variables.
The document discusses prime numbers and how to identify them. It defines prime numbers as integers whose only factors are 1 and itself. It then walks through a process of eliminating composite numbers from 1 to 100 by sequentially removing numbers with factors of 2, 3, 5, 7 and so on. This leaves only the prime numbers, which cannot be arranged into rectangles with other numbers.
The halogens are a group of non-metals that have seven electrons in their outer shell, making them highly reactive as they need only one more electron to fill their outer shell. The document describes the properties and uses of four halogens: fluorine is used in toothpaste as fluoride; chlorine is used as a disinfectant and bleach; bromine is used in camera film; and iodine can be used as an antiseptic or test for starch when dissolved in water.
There are two main ways to classify triangles: by their sides and by their angles. Triangles can be scalene, isosceles, or right based on their sides. They can be acute, obtuse, or right based on their angles. The document provides definitions and examples of each type of triangle classification.
The document describes a mathematical treasure hunt activity involving sequences. Students are given clues about various mathematical sequences and must determine subsequent terms. The correct sequence of answers is: 47, 15, 2, 12, 1, 3, 9, 27, 81, 64, 11, 4, 54, 85, 5, 16.
The document discusses the transition metals, lanthanides, and actinides. It describes the iron triad elements of iron, cobalt, and nickel which have similar properties. It also discusses the platinum group elements ruthenium, rhodium, palladium, osmium, iridium, and platinum which have similar properties and do not combine easily with other elements. The actinides are all radioactive and have unstable nuclei that decay to form other elements.
The document discusses energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and standard enthalpy change. It provides examples of how to calculate enthalpy changes from experimental temperature change data using concepts like specific heat capacity. Hess's law, which states the enthalpy change of a reaction is equal to the sum of enthalpy changes of the steps in a reaction mechanism, is also introduced.
Stoichiometry is the quantitative study of reactants and products in chemical reactions. Given the amount of one reactant, stoichiometry can be used to determine the amount of products that can be formed. The key steps involve balancing the chemical equation, converting between moles and mass using molar ratios and molar masses, and setting up and solving mole ratios from the balanced equation and problem statement.
This document provides an overview of key math concepts related to areas of shapes, exponents, square roots, and the Pythagorean theorem. It defines the area formulas for squares, rectangles, and triangles. It also explains the different types of triangles, how exponents relate to multiplying a base number by itself, and how to calculate square roots using a scientific calculator.
1) The document provides an overview of solving various types of linear equations, including equations with fractions and variables on both sides.
2) Step-by-step methods are demonstrated for solving equations with parentheses, fractions, and variables on both sides of the equal sign.
3) Examples show how to use the root of an equation to then solve for a related expression.
1) The document discusses various methods for solving linear equations, including using inverse operations, distributing terms, cross multiplying fractions, and using roots of equations.
2) It provides examples of solving equations with parentheses, fractions, and multiple terms as well as determining values based on the solutions to equations.
3) The examples cover a range of equation types and solution methods to illustrate how to systematically solve for unknown variables.
Slope describes the steepness of a line, with a positive slope indicating a line rising from left to right and a negative slope a line falling from left to right. Slope is calculated by finding the change in the vertical distance over the change in the horizontal distance between two points on the line, using the formula m=(change in y)/(change in x). Horizontal lines have a slope of zero while vertical lines have no defined slope.
This document provides an overview of key concepts for simplifying expressions including expressions, equations, inequalities, results of operations, powers, grouping symbols, and order of operations. It assigns practice problems from pages 10-11 and even numbered problems from 2-44 to complete without a calculator.
The document provides an overview of some key concepts related to even, odd, composite, and prime numbers. It explains that even numbers can be divided by 2, odd numbers cannot, and composite numbers can be divided by another number other than 1 or itself. Prime numbers can only be divided by 1 and itself. The document then walks through systematically removing composite numbers from 1 to 100 to show the prime numbers remaining.
This document defines key terms related to quadratic equations, complex numbers, and parabolas. It explains that a quadratic equation can be written in the form ax2 + bx + c = 0 and involves real numbers a, b, and c with a ≠ 0. It also defines the discriminant, complex numbers as a + bi, imaginary numbers as complex numbers with b ≠ 0, and the real and imaginary parts of complex numbers. Additionally, it states that the graph of a quadratic equation in two variables is called a parabola, and that the axis of symmetry of a parabola is its vertical or horizontal line through the vertex.
1. Limestone is a sedimentary rock formed from sea creatures that can be used as a building material or to make other materials like cement and glass through thermal decomposition.
2. Crude oil is formed from ancient organisms and plants that were buried over millions of years, producing hydrocarbons through heat and pressure. It is separated into fractions with different boiling points through fractional distillation to produce useful products like gasoline and diesel.
3. These fractions can also undergo catalytic cracking to break larger hydrocarbons into smaller, more useful ones for fuels and plastics.
There are several techniques used in chemistry labs to separate mixtures, including filtration, chromatography, distillation, and centrifugation. Filtration uses a filter paper to separate insoluble residue from soluble filtrate. Chromatography separates dyes based on their differing stickiness to paper as they move up the paper with a solvent front. Distillation involves boiling a liquid mixture and condensing the vapor to separate components with different boiling points.
The document summarizes key points about the periodic table of elements:
1) Elements in the same group have the same number of electrons in their outer shell.
2) As you move down a period, an extra electron shell is added.
3) Most elements are metals, with non-metals on the right side of the table.
4) Elements in the same group have similar properties, called periodicity.
The document discusses the noble gases, which are unreactive elements in Group 18 of the periodic table. They rarely combine with other elements and are found in nature as uncombined atoms due to their low reactivity. Examples of noble gases discussed include helium, neon, argon, krypton, and radon. Common uses of the noble gases mentioned are balloons, lightbulbs, neon signs, and strobe lights. Radon gas requires special attention due to its radioactivity and potential to cause lung cancer if inhaled over long periods of time.
3. METALS AND ACIDS Metals Magnesium Iron Sodium Calcium Acids Hydrochloric acid Sulphuric acid Nitric acid Ethanoic acid
4. METALS AND ACIDS Metal + Acid Salt + Hydrogen Metals Magnesium Iron Sodium Calcium Acids Hydrochloric acid Sulphuric acid Nitric acid Ethanoic acid
5. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid iron iron nitrate ethanoic acid sodium ethanoate calcium calcium sulphate copper nitric acid nitric acid iron nitrate sodium sodium chloride calcium ethanoic acid magnesium sulphuric acid
6. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron iron nitrate ethanoic acid sodium ethanoate calcium calcium sulphate copper nitric acid nitric acid iron nitrate sodium sodium chloride calcium ethanoic acid magnesium sulphuric acid
7. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate ethanoic acid sodium ethanoate calcium calcium sulphate copper nitric acid nitric acid iron nitrate sodium sodium chloride calcium ethanoic acid magnesium sulphuric acid
8. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate sodium ethanoic acid sodium ethanoate calcium calcium sulphate copper nitric acid nitric acid iron nitrate sodium sodium chloride calcium ethanoic acid magnesium sulphuric acid
9. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate sodium ethanoic acid sodium ethanoate calcium sulphuric acid calcium sulphate copper nitric acid nitric acid iron nitrate sodium sodium chloride calcium ethanoic acid magnesium sulphuric acid
10. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate sodium ethanoic acid sodium ethanoate calcium sulphuric acid calcium sulphate copper nitric acid No Reaction nitric acid iron nitrate sodium sodium chloride calcium ethanoic acid magnesium sulphuric acid
11. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate sodium ethanoic acid sodium ethanoate calcium sulphuric acid calcium sulphate copper nitric acid copper nitrate iron nitric acid iron nitrate sodium sodium chloride calcium ethanoic acid magnesium sulphuric acid
12. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate sodium ethanoic acid sodium ethanoate calcium sulphuric acid calcium sulphate copper nitric acid copper nitrate iron nitric acid iron nitrate sodium hydrochloric acid sodium chloride calcium ethanoic acid magnesium sulphuric acid
13. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate sodium ethanoic acid sodium ethanoate calcium sulphuric acid calcium sulphate copper nitric acid copper nitrate iron nitric acid iron nitrate sodium hydrochloric acid sodium chloride calcium ethanoic acid calcium ethanoate magnesium sulphuric acid
14. FORMING SALTS METAL ACID SALT magnesium hydrochloric acid magnesium chloride iron nitric acid iron nitrate sodium ethanoic acid sodium ethanoate calcium sulphuric acid calcium sulphate copper nitric acid copper nitrate iron nitric acid iron nitrate sodium hydrochloric acid sodium chloride calcium ethanoic acid calcium ethanoate magnesium sulphuric acid magnesium sulphate
15. DISPLACEMENT REACTIONS Metal soln Metal Iron (III) nitrate Magnesium nitrate Copper (II) sulphate Zinc sulphate Lead (II) nitrate Iron Magnesium Copper Zinc Lead
16.
17. DISPLACEMENT REACTIONS Metal ion soln Metal Iron (III) nitrate Magnesium nitrate Copper (II) sulphate Zinc sulphate Lead (II) nitrate Iron Magnesium Copper Zinc Lead
18. DISPLACEMENT REACTIONS Metal ion soln Metal Iron (III) nitrate Magnesium nitrate Copper (II) sulphate Zinc sulphate Lead (II) nitrate Iron X X X Magnesium Copper Zinc Lead
19. DISPLACEMENT REACTIONS Metal ion soln Metal Iron (III) nitrate Magnesium nitrate Copper (II) sulphate Zinc sulphate Lead (II) nitrate Iron X X X Magnesium X Copper Zinc Lead
20. DISPLACEMENT REACTIONS Metal ion soln Metal Iron (III) nitrate Magnesium nitrate Copper (II) sulphate Zinc sulphate Lead (II) nitrate Iron X X X Magnesium X Copper X X X X X Zinc Lead
21. DISPLACEMENT REACTIONS Metal ion soln Metal Iron (III) nitrate Magnesium nitrate Copper (II) sulphate Zinc sulphate Lead (II) nitrate Iron X X X Magnesium X Copper X X X X X Zinc X X Lead
22. DISPLACEMENT REACTIONS Metal ion soln Metal Iron (III) nitrate Magnesium nitrate Copper (II) sulphate Zinc sulphate Lead (II) nitrate Iron X X X Magnesium X Copper X X X X X Zinc X X Lead X X X X
24. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate
25. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron
26. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron magnesium is more reactive than iron
27. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate
28. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate lead (II) sulphate + copper
29. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate lead (II) sulphate + copper lead is more reactive than copper
30. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate lead (II) sulphate + copper lead is more reactive than copper but copper + lead (II) sulphate
31. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate lead (II) sulphate + copper lead is more reactive than copper but copper + lead (II) sulphate no reaction
32. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate lead (II) sulphate + copper lead is more reactive than copper but copper + lead (II) sulphate no reaction copper is not more reactive than lead
Editor's Notes
Electrons can spin. In a similar way, all nuclei can spin (except those with an even atomic number and an even mass number). These positively charged spheres behave like magnets. When placed into a strong magnetic field, each nucleus can either align with the external magnetic field or against it. The lower energy state occurs when the nucleus is spinning in alignment with the magnetic field, and the high energy state occurs when the nucleus is spinning out of alignment with the magnetic field Given sufficient energy, the nuclei can ‘flip’ between the two states. In an NMR spectrometer, the magnetic field strength can be varied. The magnetic field strength at which the nucleus flips can thus be measured. The strength of magnetic field at which a particular nucleus flips is dependant upon the environment of that nucleus.
Electrons can spin. In a similar way, all nuclei can spin (except those with an even atomic number and an even mass number). These positively charged spheres behave like magnets. When placed into a strong magnetic field, each nucleus can either align with the external magnetic field or against it. The lower energy state occurs when the nucleus is spinning in alignment with the magnetic field, and the high energy state occurs when the nucleus is spinning out of alignment with the magnetic field Given sufficient energy, the nuclei can ‘flip’ between the two states. In an NMR spectrometer, the magnetic field strength can be varied. The magnetic field strength at which the nucleus flips can thus be measured. The strength of magnetic field at which a particular nucleus flips is dependant upon the environment of that nucleus.
Electrons can spin. In a similar way, all nuclei can spin (except those with an even atomic number and an even mass number). These positively charged spheres behave like magnets. When placed into a strong magnetic field, each nucleus can either align with the external magnetic field or against it. The lower energy state occurs when the nucleus is spinning in alignment with the magnetic field, and the high energy state occurs when the nucleus is spinning out of alignment with the magnetic field Given sufficient energy, the nuclei can ‘flip’ between the two states. In an NMR spectrometer, the magnetic field strength can be varied. The magnetic field strength at which the nucleus flips can thus be measured. The strength of magnetic field at which a particular nucleus flips is dependant upon the environment of that nucleus.
Electrons can spin. In a similar way, all nuclei can spin (except those with an even atomic number and an even mass number). These positively charged spheres behave like magnets. When placed into a strong magnetic field, each nucleus can either align with the external magnetic field or against it. The lower energy state occurs when the nucleus is spinning in alignment with the magnetic field, and the high energy state occurs when the nucleus is spinning out of alignment with the magnetic field Given sufficient energy, the nuclei can ‘flip’ between the two states. In an NMR spectrometer, the magnetic field strength can be varied. The magnetic field strength at which the nucleus flips can thus be measured. The strength of magnetic field at which a particular nucleus flips is dependant upon the environment of that nucleus.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
We say that these show different chemical shifts - ie they flip at different field strengths. The observed chemical shift is measured against a standard - usually tetramethylsilane (TMS). The example above shows methanol. Methanol has three H nuclei which have an identical environment (labelled 1) and one hydrogen in a different environnment (labelled 2). Two peaks due to methanol can be observed. The smallest is due to the hydrogen labelled 1. The second is due to the three other hydrogens. It is three times the size of the first.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.
Balance the following half-equations using either H+ or H2O (and, of course, e-) on either side of the equation.