Hydrogen is the simplest and lightest element. It has one proton and one electron. Hydrogen exists as diatomic hydrogen gas (H2) and is the first element in the periodic table. It can form compounds with almost all elements by gaining, losing or sharing electrons. Water (H2O) is an important compound of hydrogen that is essential for life. The largest use of hydrogen is in the production of ammonia, which is used to make fertilizers and other chemicals.
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Oxygen is the most abundant element in the earth's crust and air, making up 21% of the atmosphere. It exists in two allotropes: O2 (molecular oxygen) and O3 (ozone). O2 is colorless and odorless as a gas but pale blue as a liquid or solid. It is a strong oxidizing agent. Commercial oxygen is prepared through electrolysis of water or air separation processes. Oxygen has many industrial uses including combustion processes like welding and engines, iron and steel production through the basic oxygen process, water treatment to reduce biochemical oxygen demand, and in respiration devices that require high purity oxygen.
This document provides information about the boron family (Group 13) of the periodic table. It discusses the elements in Group 13 - boron (B), aluminium (Al), gallium (Ga), indium (In), and thallium (Tl). It details their electronic configurations, occurrence in nature, extraction methods, and chemical and physical properties. In particular, it focuses on the extraction of aluminium via the Bayer process and discusses the uses of aluminium and its environmental impacts.
It comprises the study of Hydrogen Chemistry and their applications.
Apart from these, It contains The stoarge, transportation of hydrogen along with the preparation of hydrogen.
Hydrogen is the simplest and lightest element. It has one proton and one electron. Hydrogen exists as diatomic hydrogen gas (H2) and is the first element in the periodic table. It can form compounds with almost all elements by gaining, losing or sharing electrons. Water (H2O) is an important compound of hydrogen that is essential for life. The largest use of hydrogen is in the production of ammonia, which is used to make fertilizers and other chemicals.
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Oxygen is the most abundant element in the earth's crust and air, making up 21% of the atmosphere. It exists in two allotropes: O2 (molecular oxygen) and O3 (ozone). O2 is colorless and odorless as a gas but pale blue as a liquid or solid. It is a strong oxidizing agent. Commercial oxygen is prepared through electrolysis of water or air separation processes. Oxygen has many industrial uses including combustion processes like welding and engines, iron and steel production through the basic oxygen process, water treatment to reduce biochemical oxygen demand, and in respiration devices that require high purity oxygen.
This document provides information about the boron family (Group 13) of the periodic table. It discusses the elements in Group 13 - boron (B), aluminium (Al), gallium (Ga), indium (In), and thallium (Tl). It details their electronic configurations, occurrence in nature, extraction methods, and chemical and physical properties. In particular, it focuses on the extraction of aluminium via the Bayer process and discusses the uses of aluminium and its environmental impacts.
It comprises the study of Hydrogen Chemistry and their applications.
Apart from these, It contains The stoarge, transportation of hydrogen along with the preparation of hydrogen.
This document provides information about acid-base chemistry including:
1. Acids and bases are defined, and indicators like litmus paper are described for testing acidity and basicity.
2. The pH scale is introduced to measure acidity and alkalinity, and examples of strong and weak acids and bases are given.
3. Common acids, bases, and salts are described including their properties and reactions. Processes like neutralization, ionization, and the formation of soap as a salt are explained.
The document outlines a 12 lesson plan on acids and bases, covering core concepts like different acid definitions, pH calculations, buffers, salt hydrolysis, and acid-base titration curves and calculations. Lessons involve quizzes, examples, explanations of concepts, and some practical activities like investigating buffer capacity and generating titration curves. The goal is to help students develop an understanding of acids and bases from a foundational to applied level.
Chemical bonding xi , dr.mona srivastava , founder masterchemclassesDR MONA Srivastava
Viewers,
This ppt of chemical bonding is designed to give a complete idea and though conceptual extract of the topic for the students of XI to help them understand the basics of chemical bonding in chemistry. Hope it covers all important aspects and points .
Dr Mona Srivastava
Founder-
Masterchemclasses
O documento apresenta um capítulo sobre química geral. Aborda tópicos como introdução à química, áreas de estudo da química, experimentação, modelos atômicos, radioatividade, tabela periódica, ligações químicas, ácidos, bases, reações químicas e propriedades da matéria.
RELATÓRIO DE AULA PRÁTICA: REAÇÕES DE HIDRÓXIDOS DOS METAIS ALCALINOS TERROSOSEzequias Guimaraes
1. O documento descreve um relatório de uma aula prática sobre as reações dos hidróxidos dos metais alcalinos terrosos.
2. Foram analisadas as reações dos óxidos de Mg, Ca, Ba com água, formando hidróxidos. Também foram observadas as reações dos hidróxidos com sulfato de cobre, formando precipitados de cores diferentes.
3. O pH de cada solução foi medido para analisar a relação ácido-base.
Hydrogen is the first element with one electron. It resembles alkali metals and halogens due to its ability to gain or lose electrons. Hydrogen forms covalent, ionic, and interstitial compounds called hydrides with other elements. Water has many unique properties due to hydrogen bonding between molecules. Hard water contains calcium and magnesium ions that can be removed by boiling, using limewater, or sodium carbonate to produce soft water suitable for household use.
This document discusses the alkali and alkaline earth metals. It provides information on their properties and classification in the periodic table. The alkali metals are soft, reactive, and have one outer electron. They include lithium, sodium, potassium, rubidium, cesium, and francium. The alkaline earth metals have a +2 oxidation state and include beryllium, magnesium, calcium, strontium, barium, and radium. Each metal is then described individually, noting their discovery, physical properties, and common uses. Melting and boiling points are also listed for comparison.
Acids produce hydrogen ions (H+) in aqueous solutions, have a pH below 7, taste sour, and react with bases. Examples include citric acid and hydrochloric acid. Bases produce hydroxide ions (OH-) in water, have a pH above 7, taste bitter, and feel soapy. Examples include sodium hydroxide and potassium hydroxide. The strength of acids and bases is determined by their level of ionization, with strong acids and bases having near complete ionization and weak ones having little ionization. The pH scale is used to measure acidity and alkalinity.
This document provides information about the s-block elements lithium (Li) through francium (Fr) and the alkaline earth metals beryllium (Be) through radium (Ra). It discusses their electronic configurations, atomic and ionic radii, ionization energies, hydration enthalpies, physical properties, and important compounds such as oxides, hydroxides, halides, and salts. It notes the similarities and differences between lithium and other alkali metals, as well as the similarities between lithium and magnesium. The biological importance of sodium and potassium is also mentioned.
6.3 (a) electrolysis of an aqueous solutionAzieda Dot
The document discusses the electrolysis of aqueous solutions. It explains that during electrolysis, only one ion is selectively discharged at each electrode based on its position in the electrochemical series, the nature of the electrode, and the concentration of ions. The ion discharged at the anode depends on which is easier to oxidize, while the ion discharged at the cathode depends on which is easier to reduce. Different products are formed depending on these factors and the specific electrolyte used.
O documento descreve os diferentes tipos de óxidos, incluindo suas propriedades, classificações e exemplos. Discute óxidos básicos, ácidos, neutros, mistos e anfóteros, fornecendo detalhes sobre sua nomenclatura e reações. Também destaca alguns óxidos importantes como CaO, CO2 e SOx.
Hydrogen is the simplest and most abundant element. It exists as three isotopes and can be prepared through the electrolysis of water or through reactions between acids and reactive metals like zinc. Hydrogen burns readily with oxygen to form water and is highly flammable, making its handling and storage require safety precautions. It has various industrial uses including energy production, oil refining, and ammonia synthesis.
This document provides information about acid-base chemistry including:
1. Acids and bases are defined, and indicators like litmus paper are described for testing acidity and basicity.
2. The pH scale is introduced to measure acidity and alkalinity, and examples of strong and weak acids and bases are given.
3. Common acids, bases, and salts are described including their properties and reactions. Processes like neutralization, ionization, and the formation of soap as a salt are explained.
The document outlines a 12 lesson plan on acids and bases, covering core concepts like different acid definitions, pH calculations, buffers, salt hydrolysis, and acid-base titration curves and calculations. Lessons involve quizzes, examples, explanations of concepts, and some practical activities like investigating buffer capacity and generating titration curves. The goal is to help students develop an understanding of acids and bases from a foundational to applied level.
Chemical bonding xi , dr.mona srivastava , founder masterchemclassesDR MONA Srivastava
Viewers,
This ppt of chemical bonding is designed to give a complete idea and though conceptual extract of the topic for the students of XI to help them understand the basics of chemical bonding in chemistry. Hope it covers all important aspects and points .
Dr Mona Srivastava
Founder-
Masterchemclasses
O documento apresenta um capítulo sobre química geral. Aborda tópicos como introdução à química, áreas de estudo da química, experimentação, modelos atômicos, radioatividade, tabela periódica, ligações químicas, ácidos, bases, reações químicas e propriedades da matéria.
RELATÓRIO DE AULA PRÁTICA: REAÇÕES DE HIDRÓXIDOS DOS METAIS ALCALINOS TERROSOSEzequias Guimaraes
1. O documento descreve um relatório de uma aula prática sobre as reações dos hidróxidos dos metais alcalinos terrosos.
2. Foram analisadas as reações dos óxidos de Mg, Ca, Ba com água, formando hidróxidos. Também foram observadas as reações dos hidróxidos com sulfato de cobre, formando precipitados de cores diferentes.
3. O pH de cada solução foi medido para analisar a relação ácido-base.
Hydrogen is the first element with one electron. It resembles alkali metals and halogens due to its ability to gain or lose electrons. Hydrogen forms covalent, ionic, and interstitial compounds called hydrides with other elements. Water has many unique properties due to hydrogen bonding between molecules. Hard water contains calcium and magnesium ions that can be removed by boiling, using limewater, or sodium carbonate to produce soft water suitable for household use.
This document discusses the alkali and alkaline earth metals. It provides information on their properties and classification in the periodic table. The alkali metals are soft, reactive, and have one outer electron. They include lithium, sodium, potassium, rubidium, cesium, and francium. The alkaline earth metals have a +2 oxidation state and include beryllium, magnesium, calcium, strontium, barium, and radium. Each metal is then described individually, noting their discovery, physical properties, and common uses. Melting and boiling points are also listed for comparison.
Acids produce hydrogen ions (H+) in aqueous solutions, have a pH below 7, taste sour, and react with bases. Examples include citric acid and hydrochloric acid. Bases produce hydroxide ions (OH-) in water, have a pH above 7, taste bitter, and feel soapy. Examples include sodium hydroxide and potassium hydroxide. The strength of acids and bases is determined by their level of ionization, with strong acids and bases having near complete ionization and weak ones having little ionization. The pH scale is used to measure acidity and alkalinity.
This document provides information about the s-block elements lithium (Li) through francium (Fr) and the alkaline earth metals beryllium (Be) through radium (Ra). It discusses their electronic configurations, atomic and ionic radii, ionization energies, hydration enthalpies, physical properties, and important compounds such as oxides, hydroxides, halides, and salts. It notes the similarities and differences between lithium and other alkali metals, as well as the similarities between lithium and magnesium. The biological importance of sodium and potassium is also mentioned.
6.3 (a) electrolysis of an aqueous solutionAzieda Dot
The document discusses the electrolysis of aqueous solutions. It explains that during electrolysis, only one ion is selectively discharged at each electrode based on its position in the electrochemical series, the nature of the electrode, and the concentration of ions. The ion discharged at the anode depends on which is easier to oxidize, while the ion discharged at the cathode depends on which is easier to reduce. Different products are formed depending on these factors and the specific electrolyte used.
O documento descreve os diferentes tipos de óxidos, incluindo suas propriedades, classificações e exemplos. Discute óxidos básicos, ácidos, neutros, mistos e anfóteros, fornecendo detalhes sobre sua nomenclatura e reações. Também destaca alguns óxidos importantes como CaO, CO2 e SOx.
Hydrogen is the simplest and most abundant element. It exists as three isotopes and can be prepared through the electrolysis of water or through reactions between acids and reactive metals like zinc. Hydrogen burns readily with oxygen to form water and is highly flammable, making its handling and storage require safety precautions. It has various industrial uses including energy production, oil refining, and ammonia synthesis.
4. Vlastnosti vodíku
Vodík je bezbarvý plyn, bez chuti a zápachu.
Je 14,5x lehčí než vzduch. Se vzduchem
tvoří výbušnou směs.
Požár vzducholodi Hindenburg,
plněné vodíkem.
6.května 1937 na letišti Lakehurst v New Jersey
5. Příprava vodíku:
Vodík se připravuje reakcí zinku a kyseliny chlorovodíkové
Zn + 2 HCl → H2+ ZnCl2
Rozkladem vody pomocí elektrolýzy (stejnosměrný el. proud)
2 H2O → 2H2 + O2
Termickým rozkladem methanu při 10000C
CH4 → C + 2 H2
Katalytické štěpení methanolu vodní parou při 2500C
CH3OH + H2O → CO2 + 3 H2
7. Izotopy vodíku
Deuterium - 2H (někdy se označuje jako „D“)
Atom s jádrem 2H, který obsahuje v jádře jeden proton a
jeden neutron a od běžného vodíku se liší především
atomovou hmotností. Deuterium je stabilní izotop, který
nepodléhá radioaktivní přeměně. Ve spojení s kyslíkem
tvoří deuterium těžkou vodu D2O. Využívá se v určitém
typu jaderných rektorů k přípravě plutonia z uranu.
Tritium – 3H
Tritium (čti trícium) je izotop 3H, který má jádro složeno z
jednoho protonu a 2 neutronů a bývá někdy označován
chemickou značkou T. Je nestabilní s poločasem rozpadu
12,4 roku. Uměle je tritium získáváno v těžkovodních
jaderných reaktorech při výrobě plutonia z přírodního
uranu. Tritium slouží jako jedna složka náplně
ternonukleární bomby, nejničivější lidmi vyrobené zbraně.
