1. The document contains questions from a chemistry test on Chapter 5 covering topics like halogens, noble gases, oxides and compounds.
2. Short answers are provided for questions asking about bleaching powder preparation, disproportionation reactions, iodized salt, uses of halogens, noble gas properties and more.
3. Longer answers discuss similarities and differences of fluorine, oxidizing properties of halogens, reactions of chlorine with sodium hydroxide, and industrial bleaching powder manufacture.
F.Sc.2.Chemistry.Ch.6.Test Solved - Malik XufyanMalik Xufyan
This document contains the solved test questions from Class 12 Chemistry Chapter 5 on transition elements and coordination compounds. It includes short answer questions covering topics such as the properties of transition elements, oxidation states, corrosion prevention methods, and the nomenclature and preparation of coordination compounds. The test also has longer answer questions on the manufacturing of steel via open hearth and Bessemer processes, electrochemical theory of corrosion, and properties of transition elements such as binding energies and atomic radii.
i. The document contains the solved test questions from Class 12 Chemistry Chapter 7 on organic chemistry. It includes questions on the vital force theory, preparation of urea, catenation, fractions of petroleum, knocking in engines, types of hydrocarbons and cracking.
ii. Frederick Wohler disproved the vital force theory by preparing urea in the laboratory from inorganic compounds, opening up the field of organic chemistry synthesis. His work showed that organic compounds could be made artificially.
iii. The test questions cover topics like functional groups, isomerism, sources of organic compounds, uses of petroleum and its fractions, and cracking to produce motor fuels.
F.sc.2.Chemistry.Ch.01 Solved Test (Malik Xufyan)Malik Xufyan
i. The document is a chemistry test paper containing questions about the periodic table and properties of elements and compounds.
ii. It includes questions about periodic trends like ionization energy increasing along periods and decreasing down groups. It also asks about properties related to atomic structure like ionic radii being smaller for cations and larger for anions compared to their parent atoms.
iii. Questions are also asked about classification of elements into blocks based on electron configuration, properties of metals and non-metals like basic/acidic nature of their oxides, and chemical bonding properties like covalent and ionic bonding.
F.sc.Part.2.Chemistry.(Chapter Wise Tests& Their Solution) - Malik XufyanMalik Xufyan
This document provides the solutions to a chemistry exam on the periodic table and properties of elements. It includes answers to multiple choice and short answer questions testing knowledge of trends in the periodic table, atomic structure, ionization energy, atomic and ionic radii, and classification of different types of compounds. The summary focuses on key concepts:
- The document provides solutions to chemistry exam questions testing knowledge of periodic trends, atomic structure, ionization energy, and classification of compounds. Key concepts covered include trends in atomic and ionic radii, ionization energy, metallic character, and types of oxides and halides.
- Questions assess understanding of periodic table organization, Newlands' law of octaves, position of hydrogen, properties
F.sc.Part.2.Chemistry.(Chapter Wise Tests& Their Solution) - Malik XufyanMalik Xufyan
The document is a chemistry textbook solution manual providing answers to practice questions about periodic trends and properties of elements and compounds. It contains sample multiple choice and short answer questions, along with detailed explanations of periodic table concepts such as ionization energy, atomic and ionic radii, oxidation states, types of oxides, and conductivity. The summary is:
The document provides the solution manual for a chemistry textbook, with answers to practice questions about periodic trends, properties of elements and compounds, and explanations of key periodic table concepts.
F.Sc. Part 1 Chemistry.Ch.04.Test (Malik Xufyan)Malik Xufyan
The document appears to be part of a chemistry test for class 11th covering the topic of liquids and solids. It contains multiple choice and short answer questions testing concepts such as hydrogen bonding, intermolecular forces, boiling points, vapor pressure and properties of different states of matter. The test also includes several long answer questions requiring explanations of topics like ionic solids, crystals, liquid crystals, vapor pressure measurement and different types of intermolecular forces.
F.sc. Chemistry Part 2. (inorganic portion tests & solved - Malik XufyanMalik Xufyan
This document contains a chemistry test with multiple choice and subjective questions about periodic trends and properties of elements. It includes:
1) A 17 question multiple choice test on topics like periodic table groups, ionization energy, atomic radii, and alkali metals.
2) Six short answer questions defining terms and explaining periodic trends.
3) Three multi-part questions about improvements to the periodic table, classifying oxides, and discussing hydration energy and element positions.
The document provides an exam on fundamental concepts of chemistry and the periodic table to test a student's understanding.
F.Sc.2.Chemistry.Ch.6.Test Solved - Malik XufyanMalik Xufyan
This document contains the solved test questions from Class 12 Chemistry Chapter 5 on transition elements and coordination compounds. It includes short answer questions covering topics such as the properties of transition elements, oxidation states, corrosion prevention methods, and the nomenclature and preparation of coordination compounds. The test also has longer answer questions on the manufacturing of steel via open hearth and Bessemer processes, electrochemical theory of corrosion, and properties of transition elements such as binding energies and atomic radii.
i. The document contains the solved test questions from Class 12 Chemistry Chapter 7 on organic chemistry. It includes questions on the vital force theory, preparation of urea, catenation, fractions of petroleum, knocking in engines, types of hydrocarbons and cracking.
ii. Frederick Wohler disproved the vital force theory by preparing urea in the laboratory from inorganic compounds, opening up the field of organic chemistry synthesis. His work showed that organic compounds could be made artificially.
iii. The test questions cover topics like functional groups, isomerism, sources of organic compounds, uses of petroleum and its fractions, and cracking to produce motor fuels.
F.sc.2.Chemistry.Ch.01 Solved Test (Malik Xufyan)Malik Xufyan
i. The document is a chemistry test paper containing questions about the periodic table and properties of elements and compounds.
ii. It includes questions about periodic trends like ionization energy increasing along periods and decreasing down groups. It also asks about properties related to atomic structure like ionic radii being smaller for cations and larger for anions compared to their parent atoms.
iii. Questions are also asked about classification of elements into blocks based on electron configuration, properties of metals and non-metals like basic/acidic nature of their oxides, and chemical bonding properties like covalent and ionic bonding.
F.sc.Part.2.Chemistry.(Chapter Wise Tests& Their Solution) - Malik XufyanMalik Xufyan
This document provides the solutions to a chemistry exam on the periodic table and properties of elements. It includes answers to multiple choice and short answer questions testing knowledge of trends in the periodic table, atomic structure, ionization energy, atomic and ionic radii, and classification of different types of compounds. The summary focuses on key concepts:
- The document provides solutions to chemistry exam questions testing knowledge of periodic trends, atomic structure, ionization energy, and classification of compounds. Key concepts covered include trends in atomic and ionic radii, ionization energy, metallic character, and types of oxides and halides.
- Questions assess understanding of periodic table organization, Newlands' law of octaves, position of hydrogen, properties
F.sc.Part.2.Chemistry.(Chapter Wise Tests& Their Solution) - Malik XufyanMalik Xufyan
The document is a chemistry textbook solution manual providing answers to practice questions about periodic trends and properties of elements and compounds. It contains sample multiple choice and short answer questions, along with detailed explanations of periodic table concepts such as ionization energy, atomic and ionic radii, oxidation states, types of oxides, and conductivity. The summary is:
The document provides the solution manual for a chemistry textbook, with answers to practice questions about periodic trends, properties of elements and compounds, and explanations of key periodic table concepts.
F.Sc. Part 1 Chemistry.Ch.04.Test (Malik Xufyan)Malik Xufyan
The document appears to be part of a chemistry test for class 11th covering the topic of liquids and solids. It contains multiple choice and short answer questions testing concepts such as hydrogen bonding, intermolecular forces, boiling points, vapor pressure and properties of different states of matter. The test also includes several long answer questions requiring explanations of topics like ionic solids, crystals, liquid crystals, vapor pressure measurement and different types of intermolecular forces.
F.sc. Chemistry Part 2. (inorganic portion tests & solved - Malik XufyanMalik Xufyan
This document contains a chemistry test with multiple choice and subjective questions about periodic trends and properties of elements. It includes:
1) A 17 question multiple choice test on topics like periodic table groups, ionization energy, atomic radii, and alkali metals.
2) Six short answer questions defining terms and explaining periodic trends.
3) Three multi-part questions about improvements to the periodic table, classifying oxides, and discussing hydration energy and element positions.
The document provides an exam on fundamental concepts of chemistry and the periodic table to test a student's understanding.
F.sc. Part 1 Chemistry Chapterwise Test Solved by Malik XufyanMalik Xufyan
1. The document discusses test series and publications for chemistry from class 9 to MSc from Maliks Chemistry and Jhang Institute for Advanced Studies.
2. It provides the chapter list and page numbers for the chemistry test series covering topics such as basic concepts, gases, liquids, atomic structure, chemical bonding, and electrochemistry.
3. Contact information is given for Malik Xufyan and Jhang Institute for Advanced Studies for their chemistry publications and test series.
Muhammad Sufyan from Chenab College Jhang presented on ionization energy. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom to form a cation. Across a period, ionization energy increases as atomic number increases because the nuclear charge is stronger, attracting electrons more tightly. Down a group, ionization energy decreases as atomic size increases with more electron shells, holding electrons more loosely. Factors that influence ionization energy include atomic size, nuclear charge, orbital nature, and shielding effects. Ionization energy can indicate metallic character and help predict elemental valency.
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 contains a chapter on periodic classification of elements and periodicity. It includes 93 multiple choice questions testing knowledge of periodic trends, properties of elements and compounds, electronic configuration and the development of the periodic table. The questions cover topics such as ionization energy, atomic and ionic radii, electronegativity, oxidation states, types of oxides and hydrides, and classification of elements into blocks and groups.
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 is a chapter about compounds from a chemistry textbook. It begins with an outline of topic areas including ionic compounds, molecular compounds, naming ions, and naming compounds. It then covers the key topics in more detail: ionic compounds form between metals and nonmetals and have ionic bonds, while molecular compounds form between nonmetals by sharing electrons in covalent bonds. It discusses the names of common monoatomic and polyatomic ions and how to write formulas and name ionic and molecular compounds. It concludes with examples of writing formulas, naming compounds, and discussing the law of definite proportions in compounds.
The document provides the electronic configurations of various ions of transition metals and lanthanides. It also provides answers to questions related to oxidation states, stability, and properties of transition metal ions and compounds. The key points are:
1) Electronic configurations of ions such as Cr3+, Cu+, Co2+, Mn2+, Pm3+, Ce4+, Lu2+, and Th4+ are given.
2) Mn2+ compounds are more stable than Fe2+ towards oxidation due to the half filled d orbital of Mn2+, making it more stable.
3) Oxidation states of transition metals increase from +2 to higher states with an increase in atomic number due to increasing number of d electrons
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.
The document discusses the physical and chemical properties of alkali metals and alkaline earth metals. It provides details about their ionization energies, reactivity, reactions with water and other substances, and color imparted to flames. Alkali metals have low melting points due to weak metallic bonding. Their reactivity increases down the group as ionization energy decreases. Alkaline earth metals have higher melting points than alkali metals due to smaller atomic size and stronger metallic bonds. Their reactivity is also less than alkali metals.
The document discusses the oxidation states of elements in groups 13 and 14 of the periodic table. It notes that the +3 oxidation state is most common for group 13 but becomes less stable down the group due to the inert pair effect. For group 14, the +4 state is most common for carbon and silicon but the +2 state becomes more stable down the group also due to the inert pair effect. The document also contains sample questions and answers regarding the structures, properties, and reactions of boron- and carbon-containing compounds.
The document describes non-metals and their properties. It discusses the physical and chemical properties of non-metals, and describes the industrial preparation of chlorine, sulfuric acid, and ammonia. It also lists common uses of non-metals like carbon, sulfur, phosphorus, chlorine, and nitrogen and their compounds.
The document summarizes the acid-base behavior of the highest oxidation state oxides of the period 3 elements (sodium to chlorine). It finds that the oxides trend from strongly basic on the left (Na2O) to strongly acidic on the right (Cl2O7), with Al2O3 in the middle being amphoteric. Each oxide is then discussed individually in terms of its reaction with water and whether it demonstrates acidic, basic, or no reactivity.
The document discusses the periodic table and its development over time. It describes how early scientists like Dobereiner, Meyer, Newlands, and Mendeleev contributed to organizing the elements. Key developments include recognizing that elements with similar properties recur periodically and leaving gaps in the table for undiscovered elements. The document then analyzes various groups of elements, including the noble gases, Group 1 and 17 elements, and transition metals. It describes their characteristic properties and representative uses.
B.sc(microbiology and biotechnology and biochemistry) ii inorganic chemistry ...Rai University
This document provides information on alkaline earth metals and alkali metals. It discusses their isolation methods, physical properties, reactivity, oxides, carbonates, and other salts. It also covers diagonal relationships between elements, hydrides, solvation of alkali metal ions, alkyls and aryls, complexation behavior, and biological importance of alkali metals. Specifically, it notes that alkaline earth metals like calcium, barium and strontium are isolated through electrolysis of their stable salts, while beryllium and magnesium are obtained through electrolysis of their chlorides. It also discusses how lithium shows stronger tendencies toward covalency than other alkali metals in forming covalent alkyls and aryls.
Alkali metals are elements found in Group 1 of the periodic table, including lithium, sodium, potassium, rubidium, cesium, and francium. They have low melting and boiling points, are soft, and become liquid or gas at room temperature as you move down the group. Their density increases as atomic mass increases more than atomic radius.
revision on chapter periodic table, chemical bonding and electrolysis with an...MRSMPC
The document contains information about the periodic table including:
1) It lists the elements hydrogen through argon and their symbols in the periodic table.
2) It explains that noble gases are chemically non-reactive because they have a stable electron configuration with a full outer shell.
3) Sodium undergoes reactions with oxygen, water, and chlorine that produce sodium oxide, sodium hydroxide, and sodium chloride, respectively.
The document discusses alkaline earth metals, including their extraction methods and properties. It describes:
- Calcium is extracted via electrolysis of molten calcium chloride. Strontium and barium are similarly extracted through electrolysis of their molten chlorides.
- Radium is obtained by electrolysis of molten radium chloride using a mercury cathode and platinum anode.
- Alkaline earth metal salts impart characteristic flame colors from brick red (calcium) to apple green (barium).
- Their reactivity decreases down the group as ionization energy decreases.
1) A chemical reaction is a process where one or more new substances are formed. Chemical equations represent reactions using symbols for reactants and products.
2) Balanced chemical equations ensure the same number and type of atoms for each element on both sides of the reaction arrow.
3) Common reaction types include combination, decomposition, displacement, and double displacement. Combination reactions form one product from two or more reactants while decomposition reactions break down one reactant into multiple products.
This document contains questions from the UP Board English Medium 12th Class chemistry exam, including:
- Questions about the formula of a cubic structured compound made of elements A and B.
- Questions about Kohrausch's law and its applications, and about defining and limitations of Raoult's law.
- Questions asking to classify crystalline solids based on intermolecular forces and give examples.
- Questions differentiating between true and colloidal solutions with examples.
- Questions about p-block elements and nucleic acids with examples.
- Questions about IUPAC names for coordination compounds and writing structural formulas for glucose and its reaction with Tollen's reagent.
It also
F.sc. Part 1 Chemistry Chapterwise Test Solved by Malik XufyanMalik Xufyan
1. The document discusses test series and publications for chemistry from class 9 to MSc from Maliks Chemistry and Jhang Institute for Advanced Studies.
2. It provides the chapter list and page numbers for the chemistry test series covering topics such as basic concepts, gases, liquids, atomic structure, chemical bonding, and electrochemistry.
3. Contact information is given for Malik Xufyan and Jhang Institute for Advanced Studies for their chemistry publications and test series.
Muhammad Sufyan from Chenab College Jhang presented on ionization energy. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom to form a cation. Across a period, ionization energy increases as atomic number increases because the nuclear charge is stronger, attracting electrons more tightly. Down a group, ionization energy decreases as atomic size increases with more electron shells, holding electrons more loosely. Factors that influence ionization energy include atomic size, nuclear charge, orbital nature, and shielding effects. Ionization energy can indicate metallic character and help predict elemental valency.
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 contains a chapter on periodic classification of elements and periodicity. It includes 93 multiple choice questions testing knowledge of periodic trends, properties of elements and compounds, electronic configuration and the development of the periodic table. The questions cover topics such as ionization energy, atomic and ionic radii, electronegativity, oxidation states, types of oxides and hydrides, and classification of elements into blocks and groups.
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 is a chapter about compounds from a chemistry textbook. It begins with an outline of topic areas including ionic compounds, molecular compounds, naming ions, and naming compounds. It then covers the key topics in more detail: ionic compounds form between metals and nonmetals and have ionic bonds, while molecular compounds form between nonmetals by sharing electrons in covalent bonds. It discusses the names of common monoatomic and polyatomic ions and how to write formulas and name ionic and molecular compounds. It concludes with examples of writing formulas, naming compounds, and discussing the law of definite proportions in compounds.
The document provides the electronic configurations of various ions of transition metals and lanthanides. It also provides answers to questions related to oxidation states, stability, and properties of transition metal ions and compounds. The key points are:
1) Electronic configurations of ions such as Cr3+, Cu+, Co2+, Mn2+, Pm3+, Ce4+, Lu2+, and Th4+ are given.
2) Mn2+ compounds are more stable than Fe2+ towards oxidation due to the half filled d orbital of Mn2+, making it more stable.
3) Oxidation states of transition metals increase from +2 to higher states with an increase in atomic number due to increasing number of d electrons
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.
The document discusses the physical and chemical properties of alkali metals and alkaline earth metals. It provides details about their ionization energies, reactivity, reactions with water and other substances, and color imparted to flames. Alkali metals have low melting points due to weak metallic bonding. Their reactivity increases down the group as ionization energy decreases. Alkaline earth metals have higher melting points than alkali metals due to smaller atomic size and stronger metallic bonds. Their reactivity is also less than alkali metals.
The document discusses the oxidation states of elements in groups 13 and 14 of the periodic table. It notes that the +3 oxidation state is most common for group 13 but becomes less stable down the group due to the inert pair effect. For group 14, the +4 state is most common for carbon and silicon but the +2 state becomes more stable down the group also due to the inert pair effect. The document also contains sample questions and answers regarding the structures, properties, and reactions of boron- and carbon-containing compounds.
The document describes non-metals and their properties. It discusses the physical and chemical properties of non-metals, and describes the industrial preparation of chlorine, sulfuric acid, and ammonia. It also lists common uses of non-metals like carbon, sulfur, phosphorus, chlorine, and nitrogen and their compounds.
The document summarizes the acid-base behavior of the highest oxidation state oxides of the period 3 elements (sodium to chlorine). It finds that the oxides trend from strongly basic on the left (Na2O) to strongly acidic on the right (Cl2O7), with Al2O3 in the middle being amphoteric. Each oxide is then discussed individually in terms of its reaction with water and whether it demonstrates acidic, basic, or no reactivity.
The document discusses the periodic table and its development over time. It describes how early scientists like Dobereiner, Meyer, Newlands, and Mendeleev contributed to organizing the elements. Key developments include recognizing that elements with similar properties recur periodically and leaving gaps in the table for undiscovered elements. The document then analyzes various groups of elements, including the noble gases, Group 1 and 17 elements, and transition metals. It describes their characteristic properties and representative uses.
B.sc(microbiology and biotechnology and biochemistry) ii inorganic chemistry ...Rai University
This document provides information on alkaline earth metals and alkali metals. It discusses their isolation methods, physical properties, reactivity, oxides, carbonates, and other salts. It also covers diagonal relationships between elements, hydrides, solvation of alkali metal ions, alkyls and aryls, complexation behavior, and biological importance of alkali metals. Specifically, it notes that alkaline earth metals like calcium, barium and strontium are isolated through electrolysis of their stable salts, while beryllium and magnesium are obtained through electrolysis of their chlorides. It also discusses how lithium shows stronger tendencies toward covalency than other alkali metals in forming covalent alkyls and aryls.
Alkali metals are elements found in Group 1 of the periodic table, including lithium, sodium, potassium, rubidium, cesium, and francium. They have low melting and boiling points, are soft, and become liquid or gas at room temperature as you move down the group. Their density increases as atomic mass increases more than atomic radius.
revision on chapter periodic table, chemical bonding and electrolysis with an...MRSMPC
The document contains information about the periodic table including:
1) It lists the elements hydrogen through argon and their symbols in the periodic table.
2) It explains that noble gases are chemically non-reactive because they have a stable electron configuration with a full outer shell.
3) Sodium undergoes reactions with oxygen, water, and chlorine that produce sodium oxide, sodium hydroxide, and sodium chloride, respectively.
The document discusses alkaline earth metals, including their extraction methods and properties. It describes:
- Calcium is extracted via electrolysis of molten calcium chloride. Strontium and barium are similarly extracted through electrolysis of their molten chlorides.
- Radium is obtained by electrolysis of molten radium chloride using a mercury cathode and platinum anode.
- Alkaline earth metal salts impart characteristic flame colors from brick red (calcium) to apple green (barium).
- Their reactivity decreases down the group as ionization energy decreases.
1) A chemical reaction is a process where one or more new substances are formed. Chemical equations represent reactions using symbols for reactants and products.
2) Balanced chemical equations ensure the same number and type of atoms for each element on both sides of the reaction arrow.
3) Common reaction types include combination, decomposition, displacement, and double displacement. Combination reactions form one product from two or more reactants while decomposition reactions break down one reactant into multiple products.
This document contains questions from the UP Board English Medium 12th Class chemistry exam, including:
- Questions about the formula of a cubic structured compound made of elements A and B.
- Questions about Kohrausch's law and its applications, and about defining and limitations of Raoult's law.
- Questions asking to classify crystalline solids based on intermolecular forces and give examples.
- Questions differentiating between true and colloidal solutions with examples.
- Questions about p-block elements and nucleic acids with examples.
- Questions about IUPAC names for coordination compounds and writing structural formulas for glucose and its reaction with Tollen's reagent.
It also
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02 DIOXYGEN.ppt 16th group elements presentationtharshdharsh
Ozone (O3) is an allotrope of oxygen that is present in the upper atmosphere where it absorbs harmful UV rays from the sun. It is prepared in the lab by passing oxygen through a silent electric discharge or electrolyzing acidified water. Ozone is a pale blue gas that is heavier than air and slightly soluble in water. It decomposes to oxygen at 30°C. Ozone exhibits strong oxidizing properties by decomposing to nascent oxygen that can oxidize compounds like HCl to Cl2 and ferrous sulfate to ferric sulfate. Ozone in the upper atmosphere protects life on Earth by absorbing UV radiation.
This tackles the basics and the easiest concept of Chemical reactions. This features only the four basic types of chemical reactions: synthesis, decomposition, metathesis, and ion - exchange reaction.
This is a basic concept because there is a pattern to be followed in each type of reaction.
More types of chemical reactions will be given on my next set of presentation entitled, "Everything You Want to Know About Chemical Reactions."
1) Noble gases have completely filled outer electron shells which makes them chemically inert. However, under certain conditions some can form compounds.
2) Xenon can form various fluorides like XeF2, XeF4, and XeF6. It can also form oxides like XeO3 and XeO4. The structures of these compounds range from linear to octahedral depending on the number of electron pairs and lone pairs.
3) Xenon compounds are typically prepared through reactions involving elemental xenon, fluorine and oxygen under high temperatures and pressures. Many are unstable and decompose to form xenon and other products.
Lecture 9.3 through 9.5- Naming molecules & acidsMary Beth Smith
The document discusses naming binary molecular compounds and acids and bases. It provides guidelines for naming compounds based on their formulas or vice versa. The key points are:
- Binary molecular compounds are named with prefixes to indicate the number of atoms and the suffix "-ide" for the second element.
- Acids are named after their anions and have formulas starting with hydrogen and ending with the anion formula. Their names indicate the anion stem.
- Bases are named by the cation name followed by the hydroxide anion name and have the hydroxide formula.
- The laws of definite and multiple proportions describe the consistent element ratios in compounds.
Noble Gases
Introduction, isolation of Helium
from Natural gas, applications of
Noble gases. Preparation,
properties and structures of
fluorides and oxides of Xenon
(XeF2 , XeF4 , XeF6 , XeO3, XeO4 ).
Group 18 of the periodic table comprises helium(He), neon(Ne), argon (Ar), krypton (Kr),xenon (Xe), radon (Rn) and oganesson (Og).
FellowBuddy.com is a platform which has been setup with a simple vision, keeping in mind the dynamic requirements of students.
Our Vision & Mission - Simplifying Students Life
Our Belief - “The great breakthrough in your life comes when you realize it, that you can learn anything you need to learn; to accomplish any goal that you have set for yourself. This means there are no limits on what you can be, have or do.”
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This document provides the instructions and questions for a chemistry exam. It is divided into short answer questions worth 1-3 marks each and long answer questions worth 5 marks each. The short answer questions cover topics like organic reactions, electrolytes, thermodynamics, and acid-base chemistry. The long answer questions require explaining concepts like crystal structures, isomerism, and corrosion processes. Students have 3 hours to complete the exam, which is out of a total of 70 marks. Calculators are not allowed.
Here are the answers to the practice questions:
1. Displacement reaction
2. (g) indicates the substance is in gaseous state
3. By storing in air tight containers to prevent reaction with oxygen
4. CO2 dissolves in water to form carbonic acid which reacts with calcium hydroxide to form calcium carbonate, making the solution milky
5. Nitrogen
6. By the direction of the gas bubbles - oxygen bubbles up and hydrogen bubbles down
7. Photodecomposition of hydrogen chloride to form hydrogen and chlorine
8. In the displacement reaction, iron displaces copper from its solution. The iron nail becomes coated with copper and the blue
Chlorine and its compounds are discussed. Chlorine can be prepared in the laboratory by reacting concentrated hydrochloric acid with manganese(IV) oxide or potassium manganate(VII). Chlorine is a greenish-yellow gas that is denser than air and acts as a strong oxidizing agent and bleach. It reacts with many metals and non-metals to form chlorides. Common uses of chlorine include water disinfection and manufacturing of bleaches, plastics and pesticides.
This document provides a sample question paper for Chemistry (Class XII). It includes:
1. Details on the types of questions and their marks, totaling 70 marks.
2. The first few questions of the paper on topics like gas adsorption, noble gas species, and salt dissociation.
3. Instructions for the exam, including the time allowed and that calculators are not permitted.
This document provides information on naming ionic and covalent compounds. It discusses how to name ionic compounds based on their cation and anion. It also discusses naming transition metal ions based on their charge. For covalent compounds, it describes naming binary molecular compounds and compounds containing hydrogen or carbon. It provides examples of naming ionic compounds, transition metal compounds, and molecular compounds systematically. It also discusses writing chemical formulas, identifying common polyatomic ions, and recognizing ionic versus covalent character.
The document describes the process for selecting the German team for the International Chemistry Olympiad (IChO), which involves 4 rounds of testing. Students first complete problems at home, then the top scorers advance to chemistry camps involving theoretical and practical exams. The top 15 students then participate in a final week-long practical training camp, after which the IChO team is selected. The document also provides the problems and solutions for each round of the national competition.
Noble gas-ppt-,inert gas, group 18 elements# inert gas # nobal gas xenon com...RAHUL SINWER
The document discusses the noble gases, which are located in group 0 of the periodic table. It provides details on the properties and chemical composition of the noble gases, which include helium, neon, argon, krypton, xenon, and radon. It also discusses the discovery of the noble gases and their incorporation into the periodic table. The document further summarizes the chemical properties and reactivity of the noble gases, noting that under certain conditions some can form compounds, especially xenon, which can form a variety of fluorides, oxides, and oxyfluorides.
Science Subject for Middle School - 8th Grade_ Chemical Reactions by Slidesgo...septinarestu1
Here are the answers:
a. The reactants are zinc and hydrochloric acid.
b. The products are hydrogen gas and zinc(II)chloride.
c. Zinc + Hydrochloric acid → Hydrogen gas + Zinc(II)chloride
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1. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Name: Class: 12 Portion inorganic
Paper: Chemistry Objective Part Marks: 17
Time: 20 Minutes. Test: 15 Chapter no: 5
Q 1. Each question has FOUR possible answers. Choose the correct answer and encircle it. 17
Sr#. Statement. A B C D
1. The color F2 is: Yellow Pale yellow Reddish
yellow
Greenish yellow
2. The oxidation state of F is: -1 +1 -2 +2
3. The color of HCl at room temperature is: Greenish
yellow
Violet Colorless Yellow
4. What type of bonding is present in HF? Ionic Covalent Dipole Hydrogen
5. The Cl2O7 is _____ liquid. Oily Concentrated Dilute All
6. The formula of bleaching powder is: CaOCl2 CaCO3 NaOH Ca(OH)2
7. Which is used to prepare chlorine? Caustic soda Baking soda Bleaching
powder
None of theses
8. Fluorine is used to prepare: Ferons Nylon Fibers PVA
9. The melting point of XeF4 is: 141◦C 146◦C 114◦C 104◦C
10. The mixture used for breathing by the sea
divers contain oxygen to about:
80% 20% 40% 50%
11. Which of the following HX is the weaker
acid in solution?
HF HI HCl HBr
12. Which is the strongest acid? HClO HClO2 HClO3 HClO4
13. Structure of OF2 is: Linear Planer Trigonal Bent
14. Halothane is used as? Antiseptic Antipyretic Anesthetic Anti-
inflammatory
15. The XeO3 is ____ . Weakly
acidic
Strongly
acidic
Basic Neutral
16. Electronegative of fluorine is: 3 2.5 4 2.58
17. Perchloric acid is ________ agent. Reducing Oxidizing Dehydrating Dehydrogenating
2. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Name: Class: 12 Portion Inorganic
Paper: Chemistry Subjective Part Marks: 68
Time: 2:40 Test: 15 Chapter no: 5
SECTON –I
Q 2. Give the short answers of the any EIGHT
questions. 16
i. What is bleaching powder? How it is
prepared give names of different
methods.
ii. Discuss the oxides of chlorine.
iii. What are disportionation reactions? Give
an example.
iv. What is iodized salt?
v. What are ferons and Teflon?
vi. Why iodine has metallic lustre?
vii. Give the various uses of halogens and
their derivatives.
viii. Name the gas, which is used for earth
quack prediction.
ix. What are noble gases? Explain their
inertness on the basis of their electronic
configuration.
x. What do you know about oxyflourides of
xenon?
xi. Write down the names and formulas of
ores of halogens.
xii. Give some chemical properties of
Perchloric acid.
Q 3. Give the short answers of the any EIGHT
questions. 16
i. Give the applications of noble gases.
ii. Give the preparation of xenon
oxytetraflourides.
iii. Give the physical properties of noble
gases.
iv. What do you know about noble gases
write down?
v. What is meant by the available chlorine?
Give some uses of chlorine.
vi. Give general features of oxyacids of
halogens.
vii. What do you know about decolorization
of halogens?
viii. Discuss the preparation and properties of
iodine pentoxides.
ix. Write down about chlorine dioxides.
x. Give the preparation of bromine
monoxides.
xi. Give the uses of Beckmann’s method.
xii. Give the general features of oxyacids of
halogens.
Q 4. Give the short answers of the any SIX
questions.
12
i. What is meant by the bond dissociation
energy of halogens?
ii. What factors affecting the oxidizing
power of halogens?
iii. Give the trends in oxidizing power of
halogens.
iv. Give the properties of HF.
v. Give the preparation and properties of
oxides of fluorine.
vi. Give the physical properties of bleaching
powder and uses of bleaching powder.
vii. Give the construction of Beckmann’s
method.
viii. How bleaching powder acts as an
oxidizing agent?
SECTION-ll
Give the answers of the following THREE
questions. Each question is of FOUR marks.
24
Q 5.A) Give the similarities and dissimilarities of
fluorine to their groups.
B) Give the oxidizing properties of halogens.
Q 6.A) Discuss in detail of compounds of halogens.
B) Give the reaction of chlorine with cold and hot
NaOH.
Q 7.A) How bleaching powder is manufactured on
industrial scale?
B) Discuss in detail about compounds of xenon.
3. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Name: Class: 12 Portion Inorganic
Paper: Chemistry Subjective Part Marks: 68
Time: 2:40 Test: 15 Chapter no: 5
SECTON –I
Q 2. Give the short answers of the any EIGHT questions.
16
xiii. What is bleaching powder? How it is prepared give names of different methods.
Chemical formula of bleaching powder is CaOCl2 or Ca( OCl )Cl. It can be prepared on
industrial scale. Different methods are used for the manufacturing of bleaching powder.
These methods are
1. Hasenclever’s method.
2. Beckmann’s method.
Hasenclever’s method is an old method while Beckmann’s method is a modern method.
xiv. Discuss the oxides of chlorine.
Oxides of chlorine are unstable. They are not prepared by the direct reaction of chlorine aand
oxygen. These are used extensively for bleaching wood, paper pulp in industry and for water
treatment. There are two oxides of chlorine. These are chlorine dioxide and chlorine
heptaoxide.ClO2 is prepared by the following reaction.
2ClO3ˉ + 2Clˉ + 4H⁺ 2ClO2 + Cl2 + 2H2O
Chlorine heptachloride is prepared by the following reaction.
2HClO4 + P2O5
-10 o
C
Cl2O7 + 2HPO3
ClO2 used as antiseptic. It is used for purification of water. it is also used to bleach cellulose
material.
xv. What are disproportion reactions? Give an example.
A reaction in which specie (atom, ion or molecule) is oxidized and reduced simultaneously is
called disproportion reaction. For example:
Reaction of Cl2 with cold and hot NaOH is an example of disproportion reaction.
xvi. What is iodized salt?
When some amount of iodide ions are added in common salt (NaCl) , this is called iodized
salt. Usually, for this purpose NaI or KI is mixed with NaCl. Insufficient amount of iodine
causes the enlargement of thyroid glands.
xvii. What are ferons and Teflon?
Flourochlorocarbons are called ferons. These are CCl2F2 (diflourodichloromethane) & CClF3
(tifluorochloromethane). These gases are used as refrigerant and aerosol poll ants. Teflon is a
polymer of ( [ CF2-CF2 ]n ). It is an important plastic.
xviii. Why iodine has metallic lustre?
Metallic luster in iodine is due to the excitation of electrons of iodine at room temperature.
Due to the bigger size of iodine the electrons of iodine at room temperature take energy and
go to higher energy states. When excited electrons come back, they emit some radiations of
particular wavelength. Therefore, they appear as luster grayish black solid.
4. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
xix. Give the various uses of halogens and their derivatives.
Uses of halogens or their derivatives are
Fluorine is used in the preparation of ferons and Teflon.
Fluorides in toothpastes build a protective coating on teeth.
Chlorine is used in the manufacturing of bleaching powder, PVC, CHCl3 and CCl4.
Bromine is used as fungicide and as AgBr in photography.
Iodine is used in pharmaceutical company. It is added as NaI or KI as a table salt.
xx. Name the gas, which is used for earthquake prediction.
Radon is used for earthquake prediction.
xxi. What are noble gases? Explain their inertness on the basis of their electronic
configuration.
Elements Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe) and Radon (Ra)
that are placed in zero group or VIII group or periodic table are called noble gases. These are
also called inert gases or rare gases because they are chemically inert and present in very
small amount in atmosphere. All noble gases have their complete octet. Therefore, they are
chemically inert.
xxii. What do you know about oxyflourides of xenon?
Oxytetraflourides are colorless volatile liquid. It can be kept in nickel vessel. it reacts with
water to give XeO3. Xenon oxytetraflourides are prepared rapidly by the rapid reaction of
XeF6 with silica.
2XeF6 + SiO2 2XeF4 + SiF4
xxiii. Write down the names and formulas of ores of halogens.
Ores of fluorine are Fluorspar (CaF), Cryolite (Na3AlF6) and Apatite [(CaF2.3Ca3(PO4)2].
Ores of chlorine are Halite (NaCl), Carnallite (KCl.MgCl2.6H2O) (salt beds, brine wells, sea
water).
Ores of bromine are Brine wells, sea water, NaBr, KBr and MgBr2.
Ores of iodine are NaIO3, NaIO4 deposits in Chile brine walls.
xxiv. Give some chemical properties of Perchloric acid.
It reacts with organic compounds violently.
Dissolving power of HClO4 is enhanced due to increase in oxidizing strength.
Cold and dilute Perchloric acid is a very weak oxidizing agent.
It is the strongest of all acids in aqueous medium.
Q 3. Give the short answers of the any EIGHT questions.
16
xiii. Give the applications of noble gases.
Application of noble gases is
He is used in weather balloons, in welding and in traffic signal lights.
Ne and He arc is used in making glass lasers.
Xe is used in bactericidal lamps.
Radon being radioactive is used in radiotherapy for cancer and for earth quack prediction.
5. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Krypton is used to fill fluorescent tubes and in flash lamps for high speed.
xiv. Give the preparation of xenon oxytetraflourides.
1. Xenon oxytetraflourides are prepared rapidly by the rapid reaction of XeF6 with silica.
2XeF6 + SiO2 2XeF4 + SiF4
2. Hydrolysis of XeF6 with small amount of water gives XeOF4.
XeF6 + H2O XeOF4 + 2HF
xv. Give the physical properties of noble gases.
All noble gases are colorless and odourless gases. They are chemically inert. Due to complete
shell it is difficult to remove electrons from valance shell. Therefore, they have high
ionization energy. They have low melting and boiling point and heat of vaporization. They
are less soluble in water. Their solubility increases down the group due to increase in atomic
size.
xvi. What do you know about noble gases write down?
Elements Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe) and Radon (Ra)
that are placed in zero group or VIII group or periodic table are called noble gases. These are
also called inert gases or rare gases because they are chemically inert and present in very
small amount in atmosphere. All noble gases have their complete octet. Therefore, they are
chemically inert.
All noble gases are colorless and odourless gases. They are chemically inert. Due to
complete shell it is difficult to remove electrons from valance shell. Therefore, they have high
ionization energy. They have low melting and boiling point and heat of vaporization. They are
less soluble in water. Their solubility increases down the group due to increase in atomic size.
xvii. What is meant by the available chlorine? Give some uses of chlorine.
The amount of chlorine which is set free during the reaction of bleaching powder with an
acid is called available chlorine. Chlorine is used in:
Chlorine is used in the manufacturing of bleaching powder.
It is also used in the manufacturing of HCl, which is cheapest industrial acid. It is
used in the manufacturing of antiseptics and insecticides, weed killer.
It is used in the manufacturing of PVC plastics.
It is used as disinfectant in swimming pool and water treatment plants.
xviii. Give general features of oxyacids of halogens.
General features of oxyacids of halogens are
Stable oxyacids of fluorine do not exist. HOF has been prepared but is highly
unstable.
Most of oxyacids of halogens are unstable compound. They generally exist only in
aqueous solution in the form of their salts. They cannot be isolated.
xix. What do you know about decolorization of halogens?
F2 and Cl2 can oxidize colored dyes to colorless substances e.g. litmus, universal indicators
etc. during bleaching Cl also act as oxidizing agent.
xx. Discuss the preparation and properties of iodine pentoxides.
6. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Iodine penta oxide is prepared by heating acidic acid at 240˚C.
2HIO3
240 o
C
I2O5 + H2O
Iodine penta oxide is a white crystalline solid.
It is stable up to 300˚C.
It has polymeric structure.
It is insoluble in organic solvents.
xxi. Write down about chlorine dioxides.
Chlorine dioxide is a pale yellow gas. On warming, it explodes into Cl2 and O2. It is soluble
in water. it is stable in dark. It is used as antiseptic and for the purification of water. it is
prepared by the following reaction.
2ClO3ˉ + 2Clˉ + 4H⁺ 2ClO2 + Cl2 + 2H2O
xxii. Give the preparation of bromine monoxides.
It can be prepared by reaction of bromine vapours with mercuric oxide.
HgO + 2Br2
50 o
C
HgBr2 + Br2O
It is also prepared by the treating suspension of HgO in CCl4 with bromine.
HgO + 2Br2 HgBr2 + Br2O
xxiii. Give the uses of Beckmann’s method.
1. This method is used in the manufacturing of chloroform.
2. This method is used for bleaching cotton, linen and paper pulp
3. This method is used for making unshrinkable wool.
4. This method is used for the laboratory preparation of chlorine and oxygen.
xxiv. Give the general features of oxyacids of halogens.
1. Stable oxyacids of fluorine do not exist. HOF has been prepared but is highly
unstable.
2. Most of the oxyacids of halogens are unstable compound. They generally exist only
in aqueous solution in the form of their salts. They cannot be isolated.
Q 4. Give the short answers of the any SIX questions.
12
ix. What is meant by the bond dissociation energy of halogens?
Bond dissociation energy of halogens decreases with increase in size of halogen atoms.
Dissociation occurs in the following order.
HF < HCl < HBr < HI
Thus HI is dissociated more and HF is dissociated least.
x. What factors affecting the oxidizing power of halogens?
Following factors affect oxidizing power.
Energy of dissociation.
Electron affinities of atoms
Hydration energy of ions.
7. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Heats of vaporization.
xi. Give the trends in oxidizing power of halogens.
If a halogen has low energy of dissociation, high electron affinity and high hydration energy
of its ions, then it will be a better oxidizing agent. Thus oxidizing power of F2 is high due to
low dissociation energy and high hydration energy of Fˉ ion.
Thus general trend of oxidizing power is
F2 > Cl2 > Br2 > I2
xii. Give the properties of HF.
Properties of HF are
HF is a colorless volatile liquid. HF attacks glass. It is handled in teflon (poly tetra
flour ethylene) containers. In dry state, it can be stored in copper stainless-steel
containers under vacuum.
It is strongly fuming liquid.
It is used as non-aqueous solvent.
HF is a strongly hydrogen bonded liquid.
xiii. Give the preparation and properties of oxides of fluorine.
Trioxygen di fluoride (O3F2) is prepared by passing electric discharge through a mixture of
oxygen and fluorine. 2F2 + 3O2 2O3F2
Properties of oxides of fluorine are
At 363˚C, it is dark red viscous liquid but turns to reddish brown solid at 350˚C.
It decomposes on heating to give oxygen gas and other oxides of fluorine.
2O3F2 2O2F2 + O2
xiv. Give the physical properties of bleaching powder and uses of bleaching powder.
It is yellowish white powder. It has strong smell of chlorine. It is used for the preparation of
chlorine and oxygen. It is used in the manufacturing of chloroform. It is used as disinfectant
and in the sterilization of water. it is used for making unshrinkable wool.
xv. Give the construction of Beckmann’s method.
The apparatus of Beckmann’s method consists of;
Cast iron tower.
This tower has eight horizontal shelves.
Each shelve has a rotating rake.
There is a hopper is present at the top.
Bleaching powder is collected at the bottom of the tower.
There are inlets for Cl2 and hot air, at the base of tower.
xvi. How bleaching powder acts as an oxidizing agent?
Bleaching powder acts as an oxidizing agent due to the generation of hypochlorite ion (OCl-
)
in water.
Ca(OCl)Cl
H2O
Ca2+
+ Cl-
+ ClO-
SECTION-ll
8. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Give the answers of the following THREE questions. Each question is of FOUR marks.
24
Q 5.A) Give the similarities and dissimilarities of fluorine to their groups.
See the topic of peculiar behavior of fluorine.
B) Give the oxidizing properties of halogens.
See the topic of oxidizing properties.
Q 6.A) Discuss in detail of compounds of halogens
See the topic of compounds of halogens.
B) Give the reaction of chlorine with cold and hot NaOH.
See the topic of reactions of chlorine with cold and hot NaOH.
Q 7.A) How bleaching powder is manufactured on industrial scale?
See the topic of manufacturing of bleaching powder.
B) Discuss in detail about compounds of xenon.
See the topic of compounds of xenon.
9. F.sc.2.Chemistry.Ch.05. Solved Test (Malik Xufyan)
Cell # 0313-7355727
Exercise
Q 7. (a) How the halogen acids are ionized in water.
Halogen acids are ionized in water to give H+
ions.
HX + H2O H3O+
+ OH-
The order of acid strength is given below.
HF > HCl > HBr > HI
Q 13. Give the short answers of the following.
(i) What is “Iodized salt”?
When some amount of iodide ions added in common salt (NaCl), this is called iodized salt.
Usually, for this purpose NaI or KI is mixed with NaCl. Insufficient amount of iodine causes
the enlargement of thyroid glands.
(ii) What are Ferons and Teflon?
Flourochlorocarbons are called ferons. These are CCl2F2 (diflourodichloromethane) & CClF3
(tifluorochloromethane). These gases are used as refrigerant and aerosol poll ants. Teflon is a
polymer of ( [ CF2-CF2 ]n ). It is an important plastic.
(iii) Arrange the following ions in order of increasing size.
F-
, Cl-
, I-
, Br-
I-
> Br-
> Cl-
> F-
Ionic radii increase downward from top to bottom in a group. F-
Has smallest size while I-
has greater size.
(iv) Why iodine has metallic lustre?
Metallic luster in iodine is due to the excitation of electrons of iodine at room temperature.
Due to the bigger size of iodine the electrons of iodine at room temperature take energy and
go to higher energy states. When excited electrons come back, they emit some radiations of
particular wavelength. Therefore, they appear as luster grayish black solid.
(v) Which halogen sublimes to violets vapours?
Iodine is grayish black solid and emits vapours of violet color.
(vi) Which halogen is used as an antiseptic?
Iodine is used as antiseptic in the form of iodine tincture and iodex.
(vii) Which halogen is used in water treatment to kill bacteria?
Chlorine is disinfectant and used to kill pathogenic bacteria. It is used in drinking water and
swimming pools as disinfectant.
(viii) Name the gas, which is used for earth quack prediction.
Radon is used for earth quack prediction.
(ix) Name the gas, which is used in bacterial lamps.
Xenon is used in bacterial lamps.