The document is a guide about the halogens for GCSE chemistry students. It discusses the key properties and trends within group VII of the periodic table. The guide covers topics such as physical appearances, boiling points, electronic configurations, atomic sizes, and reactivity trends. It also describes reactions of halogens with metals and displacement reactions between halides.
The document discusses halogens and their medicinal uses. It covers the five halogens found in group 17 of the periodic table (fluorine, chlorine, bromine, iodine, astatine) and their physical properties like density and electronegativity decreasing from fluorine to iodine. Halogens and halogenides have medical importance, with chlorinated lime, iodine solutions, and salts like sodium chloride being used. Hypochlorites are also discussed as unstable compounds containing hypochlorite ion, used for bleaching, disinfection and water treatment when in aqueous solution.
Group VII elements are called halogens. They exist as diatomic molecules (F2, Cl2, Br2, I2) and have seven electrons in their outer shell. Fluorine has the smallest atomic radius while iodine has the largest due to more electron shells. Melting and boiling points decrease from fluorine to iodine due to weaker van der Waals forces between larger molecules. Electronegativity decreases from fluorine to iodine as the nucleus attracts electrons less. Halogens can gain electrons to form ions or share electrons to form covalent bonds. More reactive halogens can displace less reactive ones from solutions.
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.
1. The document discusses the reactions of halogens, including their reactions with metals like sodium and iron, and with non-metals like hydrogen.
2. It explains that the reactivity of the halogens decreases down the group, with fluorine being the most reactive and reacting violently with iron wool and hydrogen, while iodine reacts only slowly.
3. Halogen displacement reactions are described as redox reactions, where the more reactive halogen oxidizes the halide ion, gaining electrons itself and being reduced to form halide ions.
This document discusses the characteristic properties of s-block elements, which include the alkali metals (Group IA) and alkaline earth metals (Group IIA). Some key points discussed include:
- S-block elements have their outermost shell electrons in the s orbital.
- Alkali metals react vigorously with water to form alkaline hydroxides and hydrogen gas. Reactivity increases down the group.
- They form oxides, peroxides, and superoxides with oxygen. Oxidation states include -2, -1, and -1/2.
- Properties such as ionization energy, hydration energy, and metallic character generally decrease or increase moving down a group and across a period,
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.
This document discusses the properties and characteristics of alkaline earth metals. It begins by defining alkaline earth metals as group 2 elements with an outer electron configuration of ns2. Some key points made include:
- Alkaline earth metals have higher ionization energies than alkali metals. Ionization energy decreases down the group as atomic size increases.
- Their physical properties include being silvery-white, soft metals that are stronger oxidizers than alkali metals. They impart unique flame colors.
- Chemically, they readily react with oxygen, water and halogens. Reactivity increases down the group. They form basic hydroxides except for beryllium.
- The document also discusses trends
The document discusses halogens and their medicinal uses. It covers the five halogens found in group 17 of the periodic table (fluorine, chlorine, bromine, iodine, astatine) and their physical properties like density and electronegativity decreasing from fluorine to iodine. Halogens and halogenides have medical importance, with chlorinated lime, iodine solutions, and salts like sodium chloride being used. Hypochlorites are also discussed as unstable compounds containing hypochlorite ion, used for bleaching, disinfection and water treatment when in aqueous solution.
Group VII elements are called halogens. They exist as diatomic molecules (F2, Cl2, Br2, I2) and have seven electrons in their outer shell. Fluorine has the smallest atomic radius while iodine has the largest due to more electron shells. Melting and boiling points decrease from fluorine to iodine due to weaker van der Waals forces between larger molecules. Electronegativity decreases from fluorine to iodine as the nucleus attracts electrons less. Halogens can gain electrons to form ions or share electrons to form covalent bonds. More reactive halogens can displace less reactive ones from solutions.
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.
1. The document discusses the reactions of halogens, including their reactions with metals like sodium and iron, and with non-metals like hydrogen.
2. It explains that the reactivity of the halogens decreases down the group, with fluorine being the most reactive and reacting violently with iron wool and hydrogen, while iodine reacts only slowly.
3. Halogen displacement reactions are described as redox reactions, where the more reactive halogen oxidizes the halide ion, gaining electrons itself and being reduced to form halide ions.
This document discusses the characteristic properties of s-block elements, which include the alkali metals (Group IA) and alkaline earth metals (Group IIA). Some key points discussed include:
- S-block elements have their outermost shell electrons in the s orbital.
- Alkali metals react vigorously with water to form alkaline hydroxides and hydrogen gas. Reactivity increases down the group.
- They form oxides, peroxides, and superoxides with oxygen. Oxidation states include -2, -1, and -1/2.
- Properties such as ionization energy, hydration energy, and metallic character generally decrease or increase moving down a group and across a period,
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.
This document discusses the properties and characteristics of alkaline earth metals. It begins by defining alkaline earth metals as group 2 elements with an outer electron configuration of ns2. Some key points made include:
- Alkaline earth metals have higher ionization energies than alkali metals. Ionization energy decreases down the group as atomic size increases.
- Their physical properties include being silvery-white, soft metals that are stronger oxidizers than alkali metals. They impart unique flame colors.
- Chemically, they readily react with oxygen, water and halogens. Reactivity increases down the group. They form basic hydroxides except for beryllium.
- The document also discusses trends
This document provides information about alkali metals and describes the extraction and uses of sodium and sodium compounds. It discusses the periodic table classification of alkali metals. Key points include:
- Alkali metals are soft, silvery-white reactive metals found in Group 1 of the periodic table.
- Sodium is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride.
- Sodium reacts violently with water and is used to produce sodium hydroxide and other sodium compounds.
- Sodium hydroxide and sodium carbonate are manufactured via electrolysis or other chemical processes and have various industrial and household applications.
The document discusses the lanthanide series of f-block elements. It provides the electronic configurations of the lanthanide elements from Lanthanum to Lutetium. It describes the lanthanide contraction effect where atomic and ionic radii decrease across the series. Key effects of lanthanide contraction include decreased basicity and similar ionic radii of post-lanthanide elements to those in the previous period. The document also briefly introduces the actinide series and notes their similar properties to lanthanides but with 5f electrons instead of 4f.
The document provides information about electrolysis, including:
1) Electrolysis is the chemical effect of electricity on ionic compounds, causing them to break up into simpler substances like elements.
2) During electrolysis, ions move to electrodes of opposite charge where chemical reactions occur - non-metals form at the anode and metals or hydrogen form at the cathode.
3) Examples of electrolysis include molten lead(II) bromide producing lead at the cathode and bromine at the anode, and aqueous copper(II) chloride producing copper at the cathode and chlorine at the anode.
The document discusses the properties and reactions of alkali metals. It notes that there are 6 alkali metals - lithium, sodium, potassium, rubidium, cesium, and francium. Alkali metals are found in common items like salt and play an important role in sustaining life. They have low melting and boiling points compared to other metals. All alkali metals vigorously react with water, producing hydrogen gas and the metal hydroxide, with the reaction speed and violence increasing down the group. Salt is produced through the vigorous reaction of sodium with chlorine gas.
The electronegativity of an element is a measure of how strongly it attracts electrons in a covalent bond. Electronegativity increases left to right and top to bottom in a period, and metals have the lowest values while nonmetals have the highest. The difference in electronegativity between two bonded atoms indicates bond type - ionic bonds form when difference is >1.7, covalent bonds form when difference is <1.7, and polar covalent bonds form for differences in between. Electronegativity values can be used to predict and investigate bond types.
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIESsarunkumar31
periodic table, modern periodic law, nomenclature of elements greater than 100,electronic configuration and types of elements,periodic trends in properties of elements.ionization enthalpy, effective nuclear charge, electronegativity, s, p d and f block elements, covalent radius, ionic radius, predicition of group, period and block, electron gain enthalpy, periodic trends and chemical reactivity
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.
Introduction, position in periodic table, transition elements & inner transition elements, lanthanoids & actinoids, General trends in properties, atomic radii, atomic volume, melting points, boiling points, density, standard electrode potentials, oxidation states, Some practice questions.
The document provides information about the elements in Group 14 of the periodic table. It begins by introducing the group and listing the elements carbon, silicon, germanium, tin, and lead. It then provides details about each element, including their physical properties, oxidation states, occurrence in nature, and important uses. The document discusses topics like allotropes of carbon, silicon semiconductor applications, germanium use in electronics, tin uses in alloys and solder, and properties of lead like its low melting point.
Revision Slides for AQA A-Level Chemistry on the Group Two Elements. Designed for the new Exam Series of June 2017, but relevant for all series and exam boards.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
This document discusses chemical bonding and macromolecular structures. It begins by explaining the different types of bonds - ionic bonds formed between metals and non-metals by electron transfer, and covalent bonds formed between non-metals by electron sharing. It describes the properties of ionic and covalent compounds. It then discusses macromolecular structures found in substances like diamond, graphite and metals. It explains metallic bonding and compares the structures and properties of diamond and graphite. In the end, it discusses the different uses of diamond and graphite based on their properties.
The document discusses the periodic table of elements, explaining how the elements are organized according to properties like atomic number and mass and describing important groups of elements including metals, non-metals, noble gases, and families like alkali metals and halogens. It provides details on the development of the periodic table and key aspects of classifying and understanding the elements.
The document discusses the properties of group 16 (chalcogen) elements (oxygen, sulfur, selenium, tellurium, polonium). Key points include:
- They have the general electronic configuration of ns2np4 and can exhibit oxidation states of -2, +2, +4, and +6.
- Properties vary periodically down the group with atomic size increasing and ionization energy/electronegativity decreasing.
- Oxygen is a gas that forms strong diatomic bonds while sulfur exists as solid rings.
- Important compounds formed include hydrides, halides like sulfur hexafluoride, and oxoacids such as sulfuric acid.
- O
The document discusses the halogens, which are the elements in group 17 of the periodic table (fluorine, chlorine, bromine, iodine, astatine). It provides details about their general properties, including their electron configuration, existence as diatomic molecules, colors, reactivity, and ability to gain electrons to achieve stable electronic structures. It also describes their physical and chemical properties such as ionization energy, electronegativity, electron affinity, and oxidizing power (which decreases down the group). Peculiar properties of fluorine are highlighted. Uses of halogens and facts about their presence in humans are also mentioned. Interhalogen compounds and pseudohalides/pseudohalogens
The halogens are a group of non-metals that all have seven electrons in their outer shell, making them highly reactive as they only need one more electron to fill their outer shell. The halogens featured are fluorine, chlorine, bromine, iodine, and astatine. Fluorine is used in toothpaste as fluoride. Chlorine is mostly used to kill bacteria or as a bleach. Bromine is a main ingredient in camera film as silver bromide. Iodine dissolved in water can be used as an antiseptic or starch test.
The document discusses the properties and uses of noble gases. It defines noble gases as elements that do not interact with other elements due to their complete electron orbits. It lists the noble gases as helium, neon, argon, krypton, xenon, and radon. It then discusses their physical properties, including being odorless and colorless gases at room temperature with low melting and boiling points. Finally, it provides examples of uses for some noble gases, such as using helium for balloons due to its light weight and neon for lighting due to its bright white color.
The document discusses neutralization in chemistry. It lists the group members and learning objectives which are to explain neutralization, write equations for neutralization reactions, and explain applications of neutralization. It then covers definition of neutralization, examples of neutralization equations, and applications like insect stings, indigestion, soil treatment, and factory waste neutralization.
Embrace digital chemistry data with expert insights
How will chemistry data change in the coming years? Do research practices need to morph alongside it?
In the second webinar in the series, join Professor Simon Coles (University of Southampton), Lynn Kamerlin (Georgia Tech), May Copsey and Anna Rulka (Royal Society of Chemistry) as they explore what the future holds for chemistry data.
IB Chemistry on Chemical Properties, Oxides and Chlorides of Period 3Lawrence kok
The document provides a tutorial on the chemical properties of oxides and chlorides of period 3 elements. It discusses periodic trends in properties across period 3, including increases in size and decreases in ionization energy, electronegativity, and reactivity from left to right. For group 1 metals, reactivity increases down the group with reactions like ignition in water. For group 17 halogens, reactivity decreases with color changes from yellow to violet. Oxides range from ionic metal oxides to acidic nonmetal oxides, while chlorides show a mix of ionic and covalent bonding.
This document provides information about alkali metals and describes the extraction and uses of sodium and sodium compounds. It discusses the periodic table classification of alkali metals. Key points include:
- Alkali metals are soft, silvery-white reactive metals found in Group 1 of the periodic table.
- Sodium is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride.
- Sodium reacts violently with water and is used to produce sodium hydroxide and other sodium compounds.
- Sodium hydroxide and sodium carbonate are manufactured via electrolysis or other chemical processes and have various industrial and household applications.
The document discusses the lanthanide series of f-block elements. It provides the electronic configurations of the lanthanide elements from Lanthanum to Lutetium. It describes the lanthanide contraction effect where atomic and ionic radii decrease across the series. Key effects of lanthanide contraction include decreased basicity and similar ionic radii of post-lanthanide elements to those in the previous period. The document also briefly introduces the actinide series and notes their similar properties to lanthanides but with 5f electrons instead of 4f.
The document provides information about electrolysis, including:
1) Electrolysis is the chemical effect of electricity on ionic compounds, causing them to break up into simpler substances like elements.
2) During electrolysis, ions move to electrodes of opposite charge where chemical reactions occur - non-metals form at the anode and metals or hydrogen form at the cathode.
3) Examples of electrolysis include molten lead(II) bromide producing lead at the cathode and bromine at the anode, and aqueous copper(II) chloride producing copper at the cathode and chlorine at the anode.
The document discusses the properties and reactions of alkali metals. It notes that there are 6 alkali metals - lithium, sodium, potassium, rubidium, cesium, and francium. Alkali metals are found in common items like salt and play an important role in sustaining life. They have low melting and boiling points compared to other metals. All alkali metals vigorously react with water, producing hydrogen gas and the metal hydroxide, with the reaction speed and violence increasing down the group. Salt is produced through the vigorous reaction of sodium with chlorine gas.
The electronegativity of an element is a measure of how strongly it attracts electrons in a covalent bond. Electronegativity increases left to right and top to bottom in a period, and metals have the lowest values while nonmetals have the highest. The difference in electronegativity between two bonded atoms indicates bond type - ionic bonds form when difference is >1.7, covalent bonds form when difference is <1.7, and polar covalent bonds form for differences in between. Electronegativity values can be used to predict and investigate bond types.
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIESsarunkumar31
periodic table, modern periodic law, nomenclature of elements greater than 100,electronic configuration and types of elements,periodic trends in properties of elements.ionization enthalpy, effective nuclear charge, electronegativity, s, p d and f block elements, covalent radius, ionic radius, predicition of group, period and block, electron gain enthalpy, periodic trends and chemical reactivity
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.
Introduction, position in periodic table, transition elements & inner transition elements, lanthanoids & actinoids, General trends in properties, atomic radii, atomic volume, melting points, boiling points, density, standard electrode potentials, oxidation states, Some practice questions.
The document provides information about the elements in Group 14 of the periodic table. It begins by introducing the group and listing the elements carbon, silicon, germanium, tin, and lead. It then provides details about each element, including their physical properties, oxidation states, occurrence in nature, and important uses. The document discusses topics like allotropes of carbon, silicon semiconductor applications, germanium use in electronics, tin uses in alloys and solder, and properties of lead like its low melting point.
Revision Slides for AQA A-Level Chemistry on the Group Two Elements. Designed for the new Exam Series of June 2017, but relevant for all series and exam boards.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
This document discusses chemical bonding and macromolecular structures. It begins by explaining the different types of bonds - ionic bonds formed between metals and non-metals by electron transfer, and covalent bonds formed between non-metals by electron sharing. It describes the properties of ionic and covalent compounds. It then discusses macromolecular structures found in substances like diamond, graphite and metals. It explains metallic bonding and compares the structures and properties of diamond and graphite. In the end, it discusses the different uses of diamond and graphite based on their properties.
The document discusses the periodic table of elements, explaining how the elements are organized according to properties like atomic number and mass and describing important groups of elements including metals, non-metals, noble gases, and families like alkali metals and halogens. It provides details on the development of the periodic table and key aspects of classifying and understanding the elements.
The document discusses the properties of group 16 (chalcogen) elements (oxygen, sulfur, selenium, tellurium, polonium). Key points include:
- They have the general electronic configuration of ns2np4 and can exhibit oxidation states of -2, +2, +4, and +6.
- Properties vary periodically down the group with atomic size increasing and ionization energy/electronegativity decreasing.
- Oxygen is a gas that forms strong diatomic bonds while sulfur exists as solid rings.
- Important compounds formed include hydrides, halides like sulfur hexafluoride, and oxoacids such as sulfuric acid.
- O
The document discusses the halogens, which are the elements in group 17 of the periodic table (fluorine, chlorine, bromine, iodine, astatine). It provides details about their general properties, including their electron configuration, existence as diatomic molecules, colors, reactivity, and ability to gain electrons to achieve stable electronic structures. It also describes their physical and chemical properties such as ionization energy, electronegativity, electron affinity, and oxidizing power (which decreases down the group). Peculiar properties of fluorine are highlighted. Uses of halogens and facts about their presence in humans are also mentioned. Interhalogen compounds and pseudohalides/pseudohalogens
The halogens are a group of non-metals that all have seven electrons in their outer shell, making them highly reactive as they only need one more electron to fill their outer shell. The halogens featured are fluorine, chlorine, bromine, iodine, and astatine. Fluorine is used in toothpaste as fluoride. Chlorine is mostly used to kill bacteria or as a bleach. Bromine is a main ingredient in camera film as silver bromide. Iodine dissolved in water can be used as an antiseptic or starch test.
The document discusses the properties and uses of noble gases. It defines noble gases as elements that do not interact with other elements due to their complete electron orbits. It lists the noble gases as helium, neon, argon, krypton, xenon, and radon. It then discusses their physical properties, including being odorless and colorless gases at room temperature with low melting and boiling points. Finally, it provides examples of uses for some noble gases, such as using helium for balloons due to its light weight and neon for lighting due to its bright white color.
The document discusses neutralization in chemistry. It lists the group members and learning objectives which are to explain neutralization, write equations for neutralization reactions, and explain applications of neutralization. It then covers definition of neutralization, examples of neutralization equations, and applications like insect stings, indigestion, soil treatment, and factory waste neutralization.
Embrace digital chemistry data with expert insights
How will chemistry data change in the coming years? Do research practices need to morph alongside it?
In the second webinar in the series, join Professor Simon Coles (University of Southampton), Lynn Kamerlin (Georgia Tech), May Copsey and Anna Rulka (Royal Society of Chemistry) as they explore what the future holds for chemistry data.
IB Chemistry on Chemical Properties, Oxides and Chlorides of Period 3Lawrence kok
The document provides a tutorial on the chemical properties of oxides and chlorides of period 3 elements. It discusses periodic trends in properties across period 3, including increases in size and decreases in ionization energy, electronegativity, and reactivity from left to right. For group 1 metals, reactivity increases down the group with reactions like ignition in water. For group 17 halogens, reactivity decreases with color changes from yellow to violet. Oxides range from ionic metal oxides to acidic nonmetal oxides, while chlorides show a mix of ionic and covalent bonding.
This document is a lecture on carbon-carbon bond formation reactions in organic chemistry. It covers various main group and transition metal reagents that can be used to form C-C bonds, including organolithium, organomagnesium, organozinc, organocopper, organochromium, organocobalt and organopalladium reagents. Specific reactions discussed include alkylation of enolates, aldol reactions, conjugate additions, Grignard additions, Reformatsky reactions, Heck reactions and more. Examples are provided to illustrate reaction mechanisms and strategies for controlling stereochemistry.
This document provides an overview of a PowerPoint presentation on structure and bonding for GCSE chemistry students. It introduces ionic bonding, metallic bonding, and covalent bonding. The document explains that the presentation covers how different types of chemical bonding affect the physical properties of elements and compounds. It also provides website information for additional resources on this topic.
This document is a slide presentation on chapter 5 from a general chemistry textbook. It covers the following topics:
- The nature of aqueous solutions, including strong/weak electrolytes and non-electrolytes.
- Precipitation reactions that form insoluble compounds. Net ionic equations are introduced.
- Acid-base reactions defined by Brønsted-Lowry theory. Examples of acid-base reactions are given.
- Oxidation-reduction reactions are introduced through examples. Half-reactions and balancing redox equations using the half-reaction method are covered.
- Oxidizing and reducing agents are defined based on whether the element is gaining or losing electrons in a
This PowerPoint presentation covers group 7 (halogens) of the periodic table. It discusses trends in properties down the group such as appearance, boiling point, atomic radius, electronegativity, and oxidizing power. These trends are demonstrated through displacement reactions where a more reactive halogen will displace a less reactive one from a halide salt. Other reactions covered include the reaction of chlorine with water and alkalis. Methods for testing for halides using silver nitrate and concentrated sulfuric acid are also outlined.
Halogens are elements in group 17 of the periodic table that include fluorine, chlorine, bromine, iodine, and astatine. They exist as diatomic molecules and have seven electrons in their outer shell. The general characteristics of halogens are that their melting and boiling points increase as you go down the group, as does their atomic radius due to increasing nuclear charge. Their reactivity generally decreases down the group as atomic size increases and electronegativity decreases. Halogens react with water and alkalis to form acids and salts. They are powerful oxidizing agents and can displace other elements from their compounds. Common uses of halogens include water purification, bleaching, and synthesis of compounds
Nabamita is a master teacher at Vedantu who has an MSc and B.Ed. She enjoys traveling and Biryani but is often sleepy. She is currently working as a project associate at IIT Guwahati while teaching at Vedantu.
This chapter discusses alkenes, which are hydrocarbons containing carbon-carbon double bonds. It covers the structure and bonding of ethylene as well as the IUPAC nomenclature used for naming alkenes. The chapter also examines methods for synthesizing alkenes, including dehydrohalogenation reactions and dehydration of alcohols. It discusses factors that influence the stability of alkenes such as substitution and ring size. The chapter concludes by exploring some physical properties and commercial uses of alkenes.
07 - Structure and Synthesis of Alkenes - Wade 7thNattawut Huayyai
This chapter discusses alkenes, which are hydrocarbons containing carbon-carbon double bonds. It covers the structure and bonding of ethylene as well as the IUPAC nomenclature used for naming alkenes. The chapter also examines methods for synthesizing alkenes, including dehydrohalogenation reactions and dehydration of alcohols. It discusses substituent effects on the stability of double bonds and various physical properties of alkenes.
D-block elements are those elements belonging to groups 3 through 12 that have their last electron entering the d subshell. Transition elements are defined as elements that have partially filled d orbitals. While all transition elements are d-block elements, not all d-block elements are transition elements as some like zinc have a filled d10 configuration. D-block elements form complex compounds by binding metal ions to anions or neutral molecules through available d orbitals. They also commonly show paramagnetism and catalytic properties due to unpaired electrons in their d orbitals.
The document is a guide to chemical bonding for GCSE students produced by Knockhardy Publishing. It provides an overview of the types of chemical bonds formed between atoms, including ionic bonds formed through electron transfer between atoms with configurations just short and just over a noble gas, and covalent bonds formed through electron pair sharing between atoms with configurations short of a noble gas. Examples of ionic compounds like sodium chloride and covalent compounds like water and methane are given to illustrate how bonding allows atoms to achieve stable noble gas configurations.
The halogens are the most reactive nonmetals and exist as diatomic molecules. Their reactivity decreases down the group due to the increasing atomic radius and decreasing electronegativity. They readily react with metals to form ionic halide salts. Halogens have an oxidation state of -1 but can expand their octet to form bonds with oxidation states up to +7 by using d-orbitals.
This document is an introduction to the chemistry of alkanes presented as a PowerPoint by Knockhardy Publishing. It covers the key topics of alkane structure, properties, reactions and industrial processes. The presentation is intended for A-level chemistry students and follows the requirements of major exam boards. It provides an overview of the structure and hybridization of carbon atoms in alkanes, physical properties related to intermolecular forces, combustion reactions, and cracking and chlorination processes.
This document provides an introduction to the alkaline earth metals in Group II of the periodic table. It summarizes the key trends across the group, including increases in atomic and ionic radius and decreases in ionization energy and melting point down the group. The reactivity of the elements increases due to the greater ease of forming cations. Their oxides, hydroxides, carbonates and sulfates also show trends in solubility and other properties corresponding to the size of the metal ions.
Chemistry zimsec chapter 9 chemical periodicityalproelearning
This document summarizes key concepts about chemical periodicity, including the various blocks and periods in the periodic table. It describes trends in atomic properties like atomic radius, ionization energy, and electronegativity across periods and down groups. These trends are explained by factors like nuclear charge, atomic size, and shielding effects. Common reactions of representative elements like formation of oxides and chlorides from the third period are presented, along with equations. Structures and bonding of these compounds are discussed as well as their reactions with water.
Stereo-preference in the degradation of the erythro and threo isomers of b-O-4-type lignin model compounds in oxidation processes Ⅲ: in the reaction with chlorine- and manganese-based oxidants
The document summarizes key aspects of lead-acid and lithium-ion batteries. It discusses the electrochemistry of lead-acid batteries, including the reactions, voltages, energies, and equivalent circuit models. It also examines the structures of battery components like lead dioxide electrodes and how they are affected by factors like rate of reaction. For lithium-ion batteries, it reviews the redox potentials of various metal systems and highlights some early cathode materials used like lithium titanium disulfide, noting the advantages it provided like a smooth galvanostatic curve.
15. Energy Applications II. Batteries.pptssuser0680bd
The document summarizes key aspects of lead-acid and lithium-ion batteries. It discusses the electrochemistry of lead-acid batteries, including the reactions, voltages, energies, and equivalent circuit models. It also examines the structures of battery components like lead dioxide electrodes and how they are affected by factors like rate of reaction. For lithium-ion batteries, it reviews the redox potentials of various metal systems and highlights some early cathode materials used like lithium titanium disulfide, noting the advantages it provided like a smooth galvanostatic curve.
Daltons DYME Presentation - Beyond Al: Group 13 Salphen catalysts for efficie...RyanLewis164
This was the presentation given at the RSC Dalton's DYME meeting on 29/06/2021. The background of the presentation is using Group 13 Salphen catalysts for the cycloaddition between terminal epoxides and CO2 to form cyclic carbonates.
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
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1. GROUP VIIGROUP VII
The HalogensThe Halogens
A guide for GCSE studentsA guide for GCSE students
KNOCKHARDY PUBLISHINGKNOCKHARDY PUBLISHING
20102010
SPECIFICATIONSSPECIFICATIONS
2. GROUP VIIGROUP VII
INTRODUCTION
This Powerpoint show is one of several produced to help students
understand selected GCSE Chemistry topics. It is based on the requirements
of the AQA specification but is suitable for other examination boards.
Individual students may use the material at home for revision purposes and
it can also prove useful for classroom teaching with an interactive white
board.
Additional Powerpoints, and the full range of AS and A2 Chemistry topics,
are available from the KNOCKHARDY WEBSITE at...
www.knockhardy.org.uk
All diagrams and animations in this Powerpoint are original and
created by Jonathan Hopton. Permission must be obtained for their
use in any commercial work.
All diagrams and animations in this Powerpoint are original and
created by Jonathan Hopton. Permission must be obtained for their
use in any commercial work.
3. CONTENTSCONTENTS
• Introduction
• Group trends
• Group similarities
• Reaction with metals
• Displacement reactions
• Summary
• Quick quiz
GROUP VIIGROUP VII
6. GROUP PROPERTIESGROUP PROPERTIES
GENERAL • non-metals
• exist as separate diatomic molecules… eg Cl2
• have seven electrons in their outer shells
• form negative ions with a 1- charge
• reaction with metals and halides
7. GROUP PROPERTIESGROUP PROPERTIES
GENERAL • non-metals
• exist as separate diatomic molecules… eg Cl2
• have seven electrons in their outer shells
• form negative ions with a 1- charge
• reaction with metals and halides
TRENDS • appearance
• boiling point
• electronic configuration
• atomic size
• ionic size
• reactivity
10. GROUP TRENDSGROUP TRENDS
INCREASES down Group because more energy is required to separate
the larger molecules.
F2
Yellow
Cl2
Green
Br2
Red/brown
I2
Grey
GAS GAS LIQUID SOLID
Colour
State (at RTP)
APPEARANCEAPPEARANCE
BOILING POINTBOILING POINT
F2
- 188
Cl2
- 34
Br2
58
I2
183Boiling point / °C
Yellow Green Red/brown PurpleVapour colour
11. GROUP TRENDSGROUP TRENDS
• electrons go into shells further from the nucleus
F Cl Br I
2,7 2,8,7 2,8,18,7 2,8,18,18,7Configuration
ELECTRONIC CONFIGURATIONELECTRONIC CONFIGURATION
9 17 35 53Atomic Number
12. GROUP TRENDSGROUP TRENDS
F Cl Br I
ATOMIC & IONIC RADIUSATOMIC & IONIC RADIUS
0.064 0.099 0.111 0.128Atomic radius / nm
NOT TO SCALE
13. GROUP TRENDSGROUP TRENDS
ATOMIC RADIUS INCREASES down Group
IONIC RADIUS INCREASES down Group
• the greater the atomic number the more electrons there are
these go into shells increasingly further from the nucleus
• ions are larger than atoms - the added electron repels the
others so radius gets larger
F Cl Br I
ATOMIC & IONIC RADIUSATOMIC & IONIC RADIUS
0.064 0.099 0.111 0.128Atomic radius / nm
F¯ Cl¯ Br¯ I¯
0.136 0.181 0.195 0.216Ionic radius / nm
15. GROUP SIMILARITIESGROUP SIMILARITIES
• all the atoms have seven electrons in their outer shell
• ions are larger than atoms - the added electron repels the
others so radius gets larger
ELECTRONIC CONFIGURATIONELECTRONIC CONFIGURATION
F Cl Br I
2,7 2,8,7 2,8,18,7 2,8,18,18,7Configuration
9 17 35 53Atomic Number
17. GROUPGROUP SIMILARITIESSIMILARITIES
ION FORMATIONION FORMATION
F Cl Br I
Configuration
Ion F¯ Cl¯ Br¯ I¯
2,8 2,8,8 2,8,18,8 2,8,18,18,8
• all gain one electron to form a negative ion of charge 1-
• ions are larger than atoms
• the smaller the atom the easier it forms an ion
18. GROUPGROUP SIMILARITIESSIMILARITIES
ION FORMATIONION FORMATION
F Cl Br I
Configuration
Ion F¯ Cl¯ Br¯ I¯
2,8 2,8,8 2,8,18,8 2,8,18,18,8
• all gain one electron to form a negative ion of charge 1-
• ions are larger than atoms
• the smaller the atom the easier it forms an ion
REACTIVITYREACTIVITY
F Cl Br I
Reactivity Increasingly reactive
• reactivity decreases down the Group / increases up the Group
21. REACTION OF HALOGENS WITH METALSREACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
22. REACTION OF HALOGENS WITH METALSREACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
THE EASE OF REACTION DECREASES DOWN THE GROUP F > Cl > Br > I
23. REACTION OF HALOGENS WITH METALSREACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
THE EASE OF REACTION DECREASES DOWN THE GROUP F > Cl > Br > I
THIS IS BECAUSE ‘THE LARGER THE HALOGEN ATOM, THE LESS
EASILY IT ATTRACTS THE ELECTRON IT NEEDS
TO FILL ITS OUTER SHELL’
24. REACTION OF HALOGENS WITH METALSREACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
THE EASE OF REACTION DECREASES DOWN THE GROUP F > Cl > Br > I
THIS IS BECAUSE ‘THE LARGER THE HALOGEN ATOM, THE LESS
EASILY IT ATTRACTS THE ELECTRON IT NEEDS
TO FILL ITS OUTER SHELL’
THE HALIDES OF GROUP I ARE… WHITE IONIC SOLIDS
VERY SOLUBLE IN WATER
SODIUM CHLORIDE (NaCl) IS A TYPICAL GROUP I HALIDE
26. REACTION WITH ALKALI METALS - EquationsREACTION WITH ALKALI METALS - Equations
SODIUM CHLORINE SODIUM CHLORIDE+
27. REACTION WITH ALKALI METALS - EquationsREACTION WITH ALKALI METALS - Equations
Na + Cl2 NaCl
SODIUM CHLORINE SODIUM CHLORIDE
28. REACTION WITH ALKALI METALS - EquationsREACTION WITH ALKALI METALS - Equations
Na + Cl2 NaCl
SODIUM CHLORINE SODIUM CHLORIDE
The equation doesn’t balance - multiply the formulae until it doesThe equation doesn’t balance - multiply the formulae until it does
29. REACTION WITH ALKALI METALS - EquationsREACTION WITH ALKALI METALS - Equations
2Na + Cl2 2NaCl
Na + Cl2 NaCl
SODIUM CHLORINE SODIUM CHLORIDE
Balanced equationBalanced equation
31. Cl
SODIUM ION
2,8
Na
CHLORIDE ION
2,8,8
both species now have ‘full’ outer shells; ie they
have the electronic configuration of a noble gas
+
11 protons; 10 electrons 17 protons; 18 electrons
SODIUM CHLORIDE FORMATIONSODIUM CHLORIDE FORMATION
34. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
35. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS DECREASE IN REACTIVITY DOWN THE GROUP CAN BE
DEMONSTRATED USING DISPLACEMENT REACTIONS...
A DISPLACEMENT REACTION IS WHERE ONE SPECIES TAKES THE PLACE
OF ANOTHER IN A COMPOUND.
36. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
BROMIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
A SOLUTION OF THE HALOGEN IS ADDED TO A SOLUTION OF A HALIDE
HALIDES ARE SALTS FORMED BETWEEN ELEMENTS AND HALOGENS
37. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SODIUM
BROMIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
CHLORIDE
SOLUTION
Colourless
NO VISIBLE
REACTION
Experiment 1
38. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
BROMINE
WATER
Orange
CHLORINE
WATER
Pale green
SODIUM
BROMIDE
SOLUTION
Colourless
BROMINE
produced
Experiment 2
39. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
BROMIDE
SOLUTION
Colourless
BROMINE
WATER
Orange
CHLORINE
WATER
Pale green
SODIUM
IODIDE
SOLUTION
Colourless
IODINE
produced
Experiment 3
40. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SODIUM
BROMIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
CHLORIDE
SOLUTION
Colourless
NO VISIBLE
REACTION
Experiment 4
41. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
BROMIDE
SOLUTION
Colourless
NO VISIBLE
REACTION
Experiment 5
42. DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
BROMIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
IODIDE
SOLUTION
Colourless
IODINE
produced
Experiment 6
43. SODIUM CHLORIDE
CHLORINE
SODIUM BROMIDE SODIUM IODIDE
Solution stays
colourless
NO REACTION
Solution goes from
colourless to orange-
yellow
NO REACTION
Solution goes from
colourless to orange-
yellow
BROMINE FORMED
Solution goes from
colourless to orange-
yellow
NO REACTION
Solution goes from
colourless to red
IODINE FORMED
BROMINE
Solution goes from
colourless to orange-
red
IODINE FORMED
DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SUMMARY OF OBSERVATIONS
1
65
2 3
4
The colour change in Experiments 4 and 5 is
due to dilution – there is no reaction
51. CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM
BROMIDE
THIS SHOWS THAT A MORE REACTIVE HALOGEN WILL DISPLACE
A LESS REACTIVE ONE FROM AN AQUEOUS
SOLUTION OF ITS SALT
DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
SUMMARY
52. CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM
BROMIDE
THIS SHOWS THAT A MORE REACTIVE HALOGEN WILL DISPLACE
A LESS REACTIVE ONE FROM AN AQUEOUS
SOLUTION OF ITS SALT
HOWEVER, THIS REACTION DOES NOT TAKE PLACE
BROMINE + SODIUM CHLORIDE CHLORINE + SODIUM BROMIDE
(Bromine is below chlorine in the Group so is less reactive)
DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
53. PRESS THE SPACE BAR TO SEE WHAT HAPPENS
DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
EXPLANATION
17+
CHLORINE ATOM
17 PROTONS
17 ELECTRONS
2,8,7
35+
BROMIDE ION
35 PROTONS
36 ELECTRONS
2,8,18,8
THE CHLORINE ATOM PULLS AN ELECTRON OUT OF THE OUTER SHELL OF
THE BROMIDE ION – THE CHLORINE ATOM BECOMES A CHLORIDE ION AND
THE BROMIDE ION BECOMES A BROMINE ATOM.
54. BECAUSE BROMINE ATOMS ARE LARGER THAN CHLORINE ATOMS, IT IS
EASIER TO PULL ONE OF THEIR OUTER SHELL ELECTRONS OUT.
CHLORINE NOW HAS THE OUTER SHELL ELECTRONIC CONFIGURATION OF
A NOBLE GAS.
DISPLACEMENT REACTIONS OF HALOGENSDISPLACEMENT REACTIONS OF HALOGENS
EXPLANATION
CHLORINE ATOM
17 PROTONS
17 ELECTRONS
BROMIDE ION
35 PROTONS
36 ELECTRONS
CHLORIDE ION
17 PROTONS
18 ELECTRONS
BROMINE ATOM
35 PROTONS
35 ELECTRONS
55. SYMBOL
MOLECULAR
FORMULA
APPEARANCE
STATE (room temp)
F
PALE YELLOW
GAS
Cl
FLUORINE IODINE
ELECTRONIC
CONFIGURATION
BOILING POINT
2,7
INCREASES
2,8,7
GAS
ION
(electronic config)
F¯
2,8
Cl¯
2,8,8
REACTION WITH
SODIUM LESS REACTIVE
PRODUCT OF REACTION
WITH SODIUM
SODIUM
FLUORIDE (NaF)
SODIUM
CHLORIDE (NaCl)
PALE GREEN
Br I
BROMINECHLORINE
F2 Cl2 Br2 I2
RED-BROWN GREY-BLACK
LIQUID SOLID
2,8,18,7 2,8,18,18,7
Br¯
2,8,18,8
I¯
2,8,18,18,8
SODIUM
BROMIDE (NaBr)
SODIUM IODIDE
(NaI)
GROUP VII - SUMMARYGROUP VII - SUMMARY
COLOUR OF VAPOUR PALE YELLOW GREEN RED-BROWN PURPLE
56. QUICK QUIZQUICK QUIZ
1. ELEMENTS IN GROUP 7 ARE KNOWN AS THE ………
2. WHAT ARE THE NAMES OF THE ELEMENTS
3. HOW DOES THE ATOMIC NUMBER CHANGE DOWN THE GROUP?
4. HOW DOES THE ELECTRONIC CONFIGURATION CHANGE?
5. HOW DOES THE ATOMIC SIZE (RADIUS) CHANGE?
6. HOW MANY ELECTRONS DO THEY HAVE IN THE OUTER LEVEL?
7. ARE THEY METALS OR NON-METALS?
8. WHAT HAPPENS TO THEIR COLOUR DOWN THE GROUP?
9. DO THEY GO AROUND IN PAIRS OR AS MONATOMIC GASES?
10. WHAT HAPPENS TO THEIR STATE AT ROOM TEMPERATURE?
11. WHAT TYPE OF COMPOUNDS DO THEY FORM WITH METALS?
12. HOW CAN EXPLAIN THEIR RELATIVE REACTIVITY IN TERMS OF THE
ATOMIC STRUCTURE?
57. QUICK QUIZ - ANSWERSQUICK QUIZ - ANSWERS
1. HALOGENS.
2. FLUORINE, CHLORINE, BROMINE, IODINE, ASTATINE.
3. ATOMIC NUMBER INCREASES DOWN THE GROUP.
4. GET MORE SHELLS DOWN THE GROUP.
5. ATOMIC SIZE INCREASES DOWN THE GROUP.
6. THEY ALL HAVE SEVEN ELECTRONS IN THE OUTER LEVEL.
7. THEY ARE NON-METALS.
8. COLOUR DARKENS DOWN THE GROUP.
9. ATOMS GO AROUND IN PAIRS OR AS DIATOMIC GASES.
10. GO FROM GAS TO SOLID DOWN THE GROUP.
11. THEY FORM IONIC COMPOUNDS WITH METALS.
12. THE LARGER THEY ARE THE LESS EASILY ELECTRONS ARE GAINED
AND THE LESS REACTIVE THEY BECOME.