With so many elements in the periodic table, don’t you get a little nervous? Well, it’s not that tricky! The scientists possibly knew how difficult it would be to remember all of the elements and their properties. That is why they grouped the elements into different groups. In this chapter, we will cover the p block elements. Nonetheless, let us just tell you, it is not THAT simple! You do have to focus on the subject honestly! Let us start with what p-block elements are.
The document provides guidelines for assigning oxidation numbers to elements in compounds, including:
- The oxidation number of free elements is zero.
- The oxidation number of ions is equal to the charge of the ion.
- The sum of oxidation numbers in a compound must equal zero.
- Exceptions to common oxidation numbers like fluorine = -1, oxygen = -2 are noted.
- Oxidation numbers can be determined from the periodic table group for many elements.
Examples are provided to demonstrate assigning oxidation numbers.
This document discusses acid-base reactions and concepts including:
- Conjugate acids and bases are the species that remain after an acid donates or a base accepts a proton.
- Stronger acids have weaker conjugate bases, and stronger bases have weaker conjugate acids. Reactions favor production of weaker acid/base pairs.
- Amphoteric compounds can act as both acids and bases, such as water and ammonia.
- Hydroxyl groups can make compounds acidic, basic, or amphoteric depending on other factors like electronegativity.
- Strong acid-strong base neutralization involves complete ionization to hydronium and hydroxide ions which then neutralize to form water.
Reaction of ferrous ion, ferric ion and chromium ion MUKULsethi5
1. Ionic compounds contain cations and anions that have specific chemical and physical properties. Transition metals like iron and chromium exist as cations in their ionic forms.
2. Iron can exist as the ferrous (Fe2+) or ferric (Fe3+) ion, with different electronic configurations, colors, and numbers of unpaired electrons depending on the ligand. Chromium typically exists as the Cr3+ ion.
3. Common iron and chromium compounds include salts containing the Fe2+, Fe3+, and Cr3+ ions. These compounds often have characteristic colors and are used in chemical tests and reactions that exploit the redox chemistry of iron and chromium.
The document discusses various topics related to reactions in aqueous solutions including:
- Solutions, solvents, solutes, electrolytes, and nonelectrolytes
- Strong and weak electrolytes and their ionization
- Acid-base theories and classifications of acids and bases
- Oxidation-reduction reactions and oxidation numbers
- Precipitation, acid-base, and redox reactions
- Solution stoichiometry, dilution, titrations, and gravimetric analysis
This document lists various anions and their identifying chemical properties. It groups the anions based on which precipitation agent can be used to identify them. For each anion, the symbol, identifying reagent, and expected color change or precipitate are provided. This allows for the identification of anions based on their reactions with specific reagents.
Redox reactions involve the transfer of electrons between reactants, resulting in changes to their oxidation states. Oxidation is the loss of electrons or gain of oxygen, while reduction is the gain of electrons or loss of oxygen. The document provides examples of redox reactions and identifies the oxidizing and reducing agents and species undergoing oxidation and reduction. It also gives the oxidation states of elements in ammonium sulfate.
F.Sc. Part 2 Chemistry Paper Rawalpindi Board 2008 (Malik Xufyan)Malik Xufyan
This document contains the questions from a chemistry exam for a student named Malik Xufyan. The exam has two parts - an objective multiple choice section with 17 questions worth 17 marks, and a subjective section with 33 questions worth 83 marks covering a range of chemistry topics. The subjective questions ask about properties of elements, organic chemistry reactions, inorganic compounds, industrial processes, and more. The document provides the context for a chemistry exam, but does not include any answers to the questions.
The document provides guidelines for assigning oxidation numbers to elements in compounds, including:
- The oxidation number of free elements is zero.
- The oxidation number of ions is equal to the charge of the ion.
- The sum of oxidation numbers in a compound must equal zero.
- Exceptions to common oxidation numbers like fluorine = -1, oxygen = -2 are noted.
- Oxidation numbers can be determined from the periodic table group for many elements.
Examples are provided to demonstrate assigning oxidation numbers.
This document discusses acid-base reactions and concepts including:
- Conjugate acids and bases are the species that remain after an acid donates or a base accepts a proton.
- Stronger acids have weaker conjugate bases, and stronger bases have weaker conjugate acids. Reactions favor production of weaker acid/base pairs.
- Amphoteric compounds can act as both acids and bases, such as water and ammonia.
- Hydroxyl groups can make compounds acidic, basic, or amphoteric depending on other factors like electronegativity.
- Strong acid-strong base neutralization involves complete ionization to hydronium and hydroxide ions which then neutralize to form water.
Reaction of ferrous ion, ferric ion and chromium ion MUKULsethi5
1. Ionic compounds contain cations and anions that have specific chemical and physical properties. Transition metals like iron and chromium exist as cations in their ionic forms.
2. Iron can exist as the ferrous (Fe2+) or ferric (Fe3+) ion, with different electronic configurations, colors, and numbers of unpaired electrons depending on the ligand. Chromium typically exists as the Cr3+ ion.
3. Common iron and chromium compounds include salts containing the Fe2+, Fe3+, and Cr3+ ions. These compounds often have characteristic colors and are used in chemical tests and reactions that exploit the redox chemistry of iron and chromium.
The document discusses various topics related to reactions in aqueous solutions including:
- Solutions, solvents, solutes, electrolytes, and nonelectrolytes
- Strong and weak electrolytes and their ionization
- Acid-base theories and classifications of acids and bases
- Oxidation-reduction reactions and oxidation numbers
- Precipitation, acid-base, and redox reactions
- Solution stoichiometry, dilution, titrations, and gravimetric analysis
This document lists various anions and their identifying chemical properties. It groups the anions based on which precipitation agent can be used to identify them. For each anion, the symbol, identifying reagent, and expected color change or precipitate are provided. This allows for the identification of anions based on their reactions with specific reagents.
Redox reactions involve the transfer of electrons between reactants, resulting in changes to their oxidation states. Oxidation is the loss of electrons or gain of oxygen, while reduction is the gain of electrons or loss of oxygen. The document provides examples of redox reactions and identifies the oxidizing and reducing agents and species undergoing oxidation and reduction. It also gives the oxidation states of elements in ammonium sulfate.
F.Sc. Part 2 Chemistry Paper Rawalpindi Board 2008 (Malik Xufyan)Malik Xufyan
This document contains the questions from a chemistry exam for a student named Malik Xufyan. The exam has two parts - an objective multiple choice section with 17 questions worth 17 marks, and a subjective section with 33 questions worth 83 marks covering a range of chemistry topics. The subjective questions ask about properties of elements, organic chemistry reactions, inorganic compounds, industrial processes, and more. The document provides the context for a chemistry exam, but does not include any answers to the questions.
This document discusses qualitative inorganic analysis of anions, specifically focusing on carbonates/bicarbonates and sulfur-containing anions. It describes:
1) Carbonates and bicarbonates react with acids to produce carbon dioxide gas, which turns limewater milky. Sulfur-containing anions like sulfides, sulfites and thiosulfates are reducing and react with acids.
2) Common tests involve adding reagents like barium chloride, silver nitrate, and iron (III) chloride to detect anions via formation of insoluble precipitates.
3) The document provides details on solubility rules and characteristic reactions for each group of anions to allow their identification in mixtures
This document discusses acids and bases according to several theories. It begins by describing the properties of acids, including reacting with metals and carbonates, conducting electricity, turning litmus paper colors, and neutralizing bases. It then discusses the properties of bases. The Arrhenius theory defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. However, this theory has limitations and does not account for all acids and bases. The Brønsted-Lowry theory broadens the definition to any substance that can donate or accept protons. Strong acids fully dissociate in water while weak acids only partially dissociate. The pH scale measures the concentration of H+ ions on a
The study examined how iron cycling and reactive oxygen species (ROS) production are affected by particulates and solution conditions. Experiments showed that Fe(II) oxidation rate increased with iron oxide loading but hydrogen peroxide yield decreased, while hydroxyl radical yield increased. Buffers that restricted Fe(III) solubility limited ROS formation, while buffers that could donate electrons to ROS recycled Fe(III) to Fe(II). Surfaces accelerated Fe(II) oxidation by scavenging Fe(III), acting as Fe(III) sinks rather than catalysts. Conditions favoring Fe(III) precipitation limited ROS production by promoting faster precipitation over ROS-driven Fe(II) cycling.
The document discusses qualitative inorganic analysis of anions, specifically focusing on carbonates/bicarbonates and sulfur-containing anions. It describes the general characteristics, properties, reactions and tests to identify these anions. Carbonates and bicarbonates are identified through reactions with acids that produce carbon dioxide gas. Sulfur-containing anions like sulfides, sulfites and thiosulfates can be identified through reactions that produce hydrogen sulfide gas, sulfur dioxide gas or sulfur precipitates.
This document discusses chemical naming conventions. It explains that chemicals can have common names as well as systematic IUPAC names, and provides examples of chemicals referred to primarily by their common names. It also outlines rules for naming ionic compounds, including writing the metal cation and nonmetal anion, indicating transition metal ion charges with Roman numerals, and using Greek prefixes and suffixes like "-ate" or "-ite" to indicate atom counts and oxygen compounds.
The document discusses acid-base theories including Bronsted-Lowry acids and bases, Lewis acids and bases, and monoprotic and polyprotic acids. Under the Bronsted-Lowry definition, an acid is a proton donor and a base is a proton acceptor in a proton transfer reaction. A Lewis acid is an electron pair acceptor that forms a covalent bond, while a Lewis base is an electron pair donor. Monoprotic acids donate one proton, while polyprotic acids like sulfuric acid can donate multiple protons in successive reactions.
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 appears to be a list of chemistry questions and answers covering topics such as naming ions, ionic compounds, molecular compounds, acids and bases, and stoichiometry laws. The questions test knowledge of chemical formulas, naming conventions, and properties of different types of compounds.
1. The document discusses various topics related to carbon compounds including hydrocarbons, alkenes, isomers, homologous series, functional groups, and reactions such as fermentation, oxidation, esterification, and dehydration of alcohols.
2. An experiment is described to prepare the ester ethyl ethanoate from ethanol and ethanoic acid using concentrated sulfuric acid. Upon mixing and warming the reactants, a sweet smell is observed and an insoluble product forms in water.
3. Differences between alkanes and alkenes are compared, including molecular structure, physical properties, reactivity, and chemical tests. Alkenes contain carbon-carbon double bonds and
This document provides information about acids and bases. It defines acids and bases according to the Arrhenius and Bronstead-Lowry theories. The Arrhenius definition states that acids release hydrogen ions and bases release hydroxide ions in water. The Bronstead-Lowry definition expands this by defining acids as proton donors and bases as proton acceptors. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate, establishing an equilibrium. The acid dissociation constant and base dissociation constant describe the strength of acids and bases respectively.
The document provides an overview of naming chemical compounds. It discusses the rules for naming binary ionic compounds that contain metals and nonmetals (types I and II), binary covalent compounds between two nonmetals (type III), compounds containing polyatomic ions, and acids. Examples of applying the naming conventions are provided throughout. The overall strategies are to consider whether the compounds are ionic or covalent, identify cations and anions or elemental names, and apply prefixes or suffixes accordingly when arriving at the systematic name.
1. Qualitative inorganic analysis involves the detection and identification of anions in samples. Anions are divided into six groups including carbonates, sulphur-containing anions, halides, cyanogen, arsenic/phosphorus, and nitrogen-containing.
2. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions such as sulphides, sulphites, thiosulphates and sulphates are identified through reactions that produce precipitates, gases, or color changes with reagents like barium chloride, silver nitrate, and iron (III) chloride.
3. Common tests involve observing properties like solubility, as
The document discusses naming binary ionic compounds, binary covalent compounds, and ternary compounds. It provides examples of naming compounds containing metals and nonmetals such as NaCl, ZnI2, Al2O3. It also discusses naming transition metal compounds and compounds with variable metal ions using Roman numerals. The document provides examples and practice problems for naming various compound types.
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
This document contains a 27 question practice test on chemistry topics including:
- Balancing chemical equations
- Identifying limiting reactants and calculating theoretical yields
- Solubility rules
- Concentration calculations
- Acid-base reactions
- Nomenclature
The test covers chapters 3 and 4 of a general chemistry textbook, focusing on stoichiometry, types of chemical reactions, aqueous solutions, and acid-base chemistry. It provides multiple choice questions to assess understanding of these core chemistry concepts.
Certain anions like oxalate, tartrate, fluoride, borate, phosphate, and chromate can interfere with the qualitative analysis of cations if not removed. They are eliminated through processes like dry ignition (oxalate), treatment with hydrochloric acid (fluoride, borate), precipitation with zirconyl nitrate (phosphate), and evaporation with hydrochloric acid (chromate). Arsenate is first reduced to arsenite using ammonium iodide before both are eliminated by precipitation with hydrogen sulfide. The order of elimination is oxalate, tartrate, fluoride, borate, phosphate, and arsenate/arsenite to ensure accurate analysis of metal cations.
This document provides information on naming and writing formulas for different types of compounds. It discusses trends in the number of valence electrons for different groups of elements. It also explains how atoms gain or lose electrons to achieve stable octet configurations and the resulting ion charges. The document outlines rules for naming and writing formulas for ionic compounds, acids, and molecular compounds involving nonmetals. Key aspects covered include recognizing polyatomic ions in acids and using prefixes to indicate the number of nonmetal atoms in molecular compounds.
This document contains information from a chemistry class lecture on acids and bases. It includes the daily objectives, a quiz score from the previous class, examples of acid-base reactions identifying the acid and base in each, and practice problems for students to work through identifying acids and bases. The exit slip questions ask students to identify properties of acids, the Bronsted-Lowry definition of a base, and to analyze example acid-base reactions. The homework is to complete additional practice questions.
Redox reactions involve the transfer of electrons from a reducing agent to an oxidizing agent. The reducing agent is oxidized by donating electrons and the oxidizing agent is reduced by accepting electrons. Common oxidizing agents include potassium manganate(VII), potassium dichromate(VI), and hydrogen peroxide, while common reducing agents include metals and hydrogen peroxide. Examples of redox reactions provided include the displacement of copper from copper(II) sulfate by zinc and the reaction of potassium manganate(VII) with hydrogen peroxide.
This document contains 17 questions and answers about acids, bases and salts. Some key points covered include:
- Milk has a pH of 6, which decreases when it turns to curd due to lactic acid production.
- Solutions with pH values of 4, 7, 9, 11 and 1 are identified as weakly acidic, neutral, weakly alkaline, strongly alkaline and strongly acidic respectively.
- Toothpastes neutralize excess acid in the mouth and prevent tooth decay.
- Heating copper sulfate changes its color from blue to white as it loses water of crystallization.
chemistry exemplar class 12 d and f block elements pdfRohit Raj Ranjan
The d-block elements are found in the middle of the period table. The d-block elements are called transition metals and have valence electrons in d orbital's. The f-block elements,found in the two rows at the bottom of the periodic table, are called inner transition metals and have valence electrons in the f-orbital's.
This document discusses qualitative inorganic analysis of anions, specifically focusing on carbonates/bicarbonates and sulfur-containing anions. It describes:
1) Carbonates and bicarbonates react with acids to produce carbon dioxide gas, which turns limewater milky. Sulfur-containing anions like sulfides, sulfites and thiosulfates are reducing and react with acids.
2) Common tests involve adding reagents like barium chloride, silver nitrate, and iron (III) chloride to detect anions via formation of insoluble precipitates.
3) The document provides details on solubility rules and characteristic reactions for each group of anions to allow their identification in mixtures
This document discusses acids and bases according to several theories. It begins by describing the properties of acids, including reacting with metals and carbonates, conducting electricity, turning litmus paper colors, and neutralizing bases. It then discusses the properties of bases. The Arrhenius theory defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. However, this theory has limitations and does not account for all acids and bases. The Brønsted-Lowry theory broadens the definition to any substance that can donate or accept protons. Strong acids fully dissociate in water while weak acids only partially dissociate. The pH scale measures the concentration of H+ ions on a
The study examined how iron cycling and reactive oxygen species (ROS) production are affected by particulates and solution conditions. Experiments showed that Fe(II) oxidation rate increased with iron oxide loading but hydrogen peroxide yield decreased, while hydroxyl radical yield increased. Buffers that restricted Fe(III) solubility limited ROS formation, while buffers that could donate electrons to ROS recycled Fe(III) to Fe(II). Surfaces accelerated Fe(II) oxidation by scavenging Fe(III), acting as Fe(III) sinks rather than catalysts. Conditions favoring Fe(III) precipitation limited ROS production by promoting faster precipitation over ROS-driven Fe(II) cycling.
The document discusses qualitative inorganic analysis of anions, specifically focusing on carbonates/bicarbonates and sulfur-containing anions. It describes the general characteristics, properties, reactions and tests to identify these anions. Carbonates and bicarbonates are identified through reactions with acids that produce carbon dioxide gas. Sulfur-containing anions like sulfides, sulfites and thiosulfates can be identified through reactions that produce hydrogen sulfide gas, sulfur dioxide gas or sulfur precipitates.
This document discusses chemical naming conventions. It explains that chemicals can have common names as well as systematic IUPAC names, and provides examples of chemicals referred to primarily by their common names. It also outlines rules for naming ionic compounds, including writing the metal cation and nonmetal anion, indicating transition metal ion charges with Roman numerals, and using Greek prefixes and suffixes like "-ate" or "-ite" to indicate atom counts and oxygen compounds.
The document discusses acid-base theories including Bronsted-Lowry acids and bases, Lewis acids and bases, and monoprotic and polyprotic acids. Under the Bronsted-Lowry definition, an acid is a proton donor and a base is a proton acceptor in a proton transfer reaction. A Lewis acid is an electron pair acceptor that forms a covalent bond, while a Lewis base is an electron pair donor. Monoprotic acids donate one proton, while polyprotic acids like sulfuric acid can donate multiple protons in successive reactions.
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 appears to be a list of chemistry questions and answers covering topics such as naming ions, ionic compounds, molecular compounds, acids and bases, and stoichiometry laws. The questions test knowledge of chemical formulas, naming conventions, and properties of different types of compounds.
1. The document discusses various topics related to carbon compounds including hydrocarbons, alkenes, isomers, homologous series, functional groups, and reactions such as fermentation, oxidation, esterification, and dehydration of alcohols.
2. An experiment is described to prepare the ester ethyl ethanoate from ethanol and ethanoic acid using concentrated sulfuric acid. Upon mixing and warming the reactants, a sweet smell is observed and an insoluble product forms in water.
3. Differences between alkanes and alkenes are compared, including molecular structure, physical properties, reactivity, and chemical tests. Alkenes contain carbon-carbon double bonds and
This document provides information about acids and bases. It defines acids and bases according to the Arrhenius and Bronstead-Lowry theories. The Arrhenius definition states that acids release hydrogen ions and bases release hydroxide ions in water. The Bronstead-Lowry definition expands this by defining acids as proton donors and bases as proton acceptors. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate, establishing an equilibrium. The acid dissociation constant and base dissociation constant describe the strength of acids and bases respectively.
The document provides an overview of naming chemical compounds. It discusses the rules for naming binary ionic compounds that contain metals and nonmetals (types I and II), binary covalent compounds between two nonmetals (type III), compounds containing polyatomic ions, and acids. Examples of applying the naming conventions are provided throughout. The overall strategies are to consider whether the compounds are ionic or covalent, identify cations and anions or elemental names, and apply prefixes or suffixes accordingly when arriving at the systematic name.
1. Qualitative inorganic analysis involves the detection and identification of anions in samples. Anions are divided into six groups including carbonates, sulphur-containing anions, halides, cyanogen, arsenic/phosphorus, and nitrogen-containing.
2. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions such as sulphides, sulphites, thiosulphates and sulphates are identified through reactions that produce precipitates, gases, or color changes with reagents like barium chloride, silver nitrate, and iron (III) chloride.
3. Common tests involve observing properties like solubility, as
The document discusses naming binary ionic compounds, binary covalent compounds, and ternary compounds. It provides examples of naming compounds containing metals and nonmetals such as NaCl, ZnI2, Al2O3. It also discusses naming transition metal compounds and compounds with variable metal ions using Roman numerals. The document provides examples and practice problems for naming various compound types.
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
This document contains a 27 question practice test on chemistry topics including:
- Balancing chemical equations
- Identifying limiting reactants and calculating theoretical yields
- Solubility rules
- Concentration calculations
- Acid-base reactions
- Nomenclature
The test covers chapters 3 and 4 of a general chemistry textbook, focusing on stoichiometry, types of chemical reactions, aqueous solutions, and acid-base chemistry. It provides multiple choice questions to assess understanding of these core chemistry concepts.
Certain anions like oxalate, tartrate, fluoride, borate, phosphate, and chromate can interfere with the qualitative analysis of cations if not removed. They are eliminated through processes like dry ignition (oxalate), treatment with hydrochloric acid (fluoride, borate), precipitation with zirconyl nitrate (phosphate), and evaporation with hydrochloric acid (chromate). Arsenate is first reduced to arsenite using ammonium iodide before both are eliminated by precipitation with hydrogen sulfide. The order of elimination is oxalate, tartrate, fluoride, borate, phosphate, and arsenate/arsenite to ensure accurate analysis of metal cations.
This document provides information on naming and writing formulas for different types of compounds. It discusses trends in the number of valence electrons for different groups of elements. It also explains how atoms gain or lose electrons to achieve stable octet configurations and the resulting ion charges. The document outlines rules for naming and writing formulas for ionic compounds, acids, and molecular compounds involving nonmetals. Key aspects covered include recognizing polyatomic ions in acids and using prefixes to indicate the number of nonmetal atoms in molecular compounds.
This document contains information from a chemistry class lecture on acids and bases. It includes the daily objectives, a quiz score from the previous class, examples of acid-base reactions identifying the acid and base in each, and practice problems for students to work through identifying acids and bases. The exit slip questions ask students to identify properties of acids, the Bronsted-Lowry definition of a base, and to analyze example acid-base reactions. The homework is to complete additional practice questions.
Redox reactions involve the transfer of electrons from a reducing agent to an oxidizing agent. The reducing agent is oxidized by donating electrons and the oxidizing agent is reduced by accepting electrons. Common oxidizing agents include potassium manganate(VII), potassium dichromate(VI), and hydrogen peroxide, while common reducing agents include metals and hydrogen peroxide. Examples of redox reactions provided include the displacement of copper from copper(II) sulfate by zinc and the reaction of potassium manganate(VII) with hydrogen peroxide.
This document contains 17 questions and answers about acids, bases and salts. Some key points covered include:
- Milk has a pH of 6, which decreases when it turns to curd due to lactic acid production.
- Solutions with pH values of 4, 7, 9, 11 and 1 are identified as weakly acidic, neutral, weakly alkaline, strongly alkaline and strongly acidic respectively.
- Toothpastes neutralize excess acid in the mouth and prevent tooth decay.
- Heating copper sulfate changes its color from blue to white as it loses water of crystallization.
chemistry exemplar class 12 d and f block elements pdfRohit Raj Ranjan
The d-block elements are found in the middle of the period table. The d-block elements are called transition metals and have valence electrons in d orbital's. The f-block elements,found in the two rows at the bottom of the periodic table, are called inner transition metals and have valence electrons in the f-orbital's.
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.
How do you account for the reducing behaviour of h3 po2 on the basis of its s...Bibek Chouhan
This document contains questions for a chemistry exam. It states that questions 1-10 are worth 1 mark each, questions 11-20 are worth 2 marks each, and question 21 is worth 5 marks. The questions cover various topics in chemistry including acids and bases, oxidation and reduction reactions, properties of elements and compounds, and preparation of chemicals.
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.
This document contains a chemistry revision paper with 30 questions covering topics related to p-block elements. The paper provides general instructions, indicating that all questions are compulsory and marks are provided for each question. It includes questions ranging from 1 to 5 marks on topics such as the structures and properties of various p-block elements and compounds, including their reactions, electronic structures, acid-base properties, and oxidation states.
This document discusses various types of reactions that occur in liquid ammonia, including precipitation, complex formation, ammonolysis, solvation, and amphoteric reactions. Precipitation reactions in ammonia differ from those in water, as most metal chlorides are insoluble except for NaCl, NH4Cl, and BeCl2. Complex formation reactions also occur similarly to those in water, such as the formation of potassium hydroxozincate from zinc chloride and potassium hydroxide. Ammonolysis reactions involve ammonia acting as a reactant in place of water. Solvation involves the formation of ammoniates through coordination bonds, ion dipole interactions, or hydrogen bonding between ammonia molecules and other compounds. Amphoteric behavior
1. The document discusses naming ionic and covalent compounds according to IUPAC rules. It provides examples of determining formulas from names and vice versa.
2. Rules are given for naming acids, including binary acids like HCl and oxyacids containing polyatomic ions like H2SO4. Examples of naming acids based on their formulas are provided.
3. Hydrates are discussed, which contain water molecules as part of their chemical structure. Their names indicate the number of water molecules using Greek prefixes.
This document contains multiple choice and other types of chemistry questions related to chemical bonding and molecular structure. Some of the questions assess understanding of concepts like hybridization, shapes of molecules, bond order calculations using valence shell electron pair repulsion (VSEPR) theory and molecular orbital theory. Other questions test application of concepts to determine molecular geometry, bond type, dipole moments and relative bond strengths. The document also includes comprehension passages to provide context for subsequent multiple choice questions.
F.sc.2.Chemistry.Ch.05 Solved Test (Malik Xufyan)Malik Xufyan
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.
Similar to chemistry exemplar class 12 p-Block Elements pdf (10)
Atoms consist of three basic particles: protons, electrons, and neutrons. The nucleus (center) of the atom contains the protons (positively charged) and the neutrons (no charge). The outermost regions of the atom are called electron shells and contain the electrons (negatively charged).
Class room work sheet (Crws) some basic concept of chemistryRohit Raj Ranjan
A mole is defined as the amount of substance containing the same number of discrete entities (atoms, molecules, ions, etc.) ... The molar mass of an element (or compound) is the mass in grams of 1 mole of that substance, a property expressed in units of grams per mole (g/mol)
A chemical bond is a lasting attraction between atoms, ions or molecules that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between oppositely charged ions as in ionic bonds or through the sharing of electrons as in covalent bond
chemistry exemplar class 12 chemical kinetics pdfRohit Raj Ranjan
1. The role of a catalyst is to change the activation energy of reaction by providing an alternate reaction pathway that requires less energy.
2. In the presence of a catalyst, the heat evolved or absorbed during the reaction remains unchanged as the catalyst does not alter the enthalpy change of the reaction.
3. Activation energy of a chemical reaction can be determined by determining the rate constants at two temperatures.
4. For a general reaction A → B, if the concentration of A decreases exponentially with time, the reaction is first order with respect to A.
chemistry exemplar class 12 electrochemistry pdfRohit Raj Ranjan
Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction ("redox") reaction
Solid-state chemistry, also sometimes referred as materials chemistry, is the study of the synthesis, structure, and properties of solid phase materials, particularly, but not necessarily exclusively of, non-molecular solids. It therefore has a strong overlap with solid-state physics, mineralogy, crystallography, ceramics, metallurgy, thermodynamics, materials science and electronics with a focus on the synthesis of novel materials and their characterisation. Solids can be classified as crystalline or amorphous on basis of the nature of order present in the arrangement of their constituent particles,
Alcohol, phenol, ether are classes of organic compounds which find wide usage in a broad range of industries as well as for domestic purposes. Alcohol is formed when a saturated carbon atom is bonded to a hydroxyl (-OH) group. Phenol is formed when a hydrogen atom in a benzene molecule is replaced by the -OH group.
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
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Therefore, human intervention has significantly influenced land use patterns over many
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9
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chemistry exemplar class 12 p-Block Elements pdf
1. 1. On addition of conc. H2
SO4
to a chloride salt, colourless fumes are evolved
but in case of iodide salt, violet fumes come out. This is because
(i) H2
SO4
reduces HI to I2
(ii) HI is of violet colour
(iii) HI gets oxidised to I2
(iv) HI changes to HIO3
2. In qualitative analysis when H2
S is passed through an aqueous solution of
salt acidified with dil. HCl, a black precipitate is obtained. On boiling the
precipitate with dil. HNO3
, it forms a solution of blue colour. Addition of excess
of aqueous solution of ammonia to this solution gives _________.
(i) deep blue precipitate of Cu (OH)2
(ii) deep blue solution of [Cu (NH3
)4
]
2+
(iii) deep blue solution of Cu(NO3
)2
(iv) deep blue solution of Cu(OH)2
.Cu(NO3
)2
3. In a cyclotrimetaphosphoric acid molecule, how many single and double
bonds are present?
(i) 3 double bonds; 9 single bonds
(ii) 6 double bonds; 6 single bonds
(iii) 3 double bonds; 12 single bonds
(iv) Zero double bonds; 12 single bonds
4. Which of the following elements can be involved in pπ–dπ bonding?
(i) Carbon
(ii) Nitrogen
I. Multiple Choice Questions (Type-I)
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2. (iii) Phosphorus
(iv) Boron
5. Which of the following pairs of ions are isoelectronic and isostructural?
(i) CO3
2–
, NO3
–
(ii) ClO3
–
, CO3
2–
(iii) SO3
2–
, NO3
–
(iv) ClO3
–
, SO3
2–
6. Affinity for hydrogen decreases in the group from fluorine to iodine. Which of
the halogen acids should have highest bond dissociation enthalpy?
(i) HF
(ii) HCl
(iii) HBr
(iv) HI
7. Bond dissociation enthalpy of E—H (E = element) bonds is given below. Which
of the compounds will act as strongest reducing agent?
Compound NH3
PH3
AsH3
SbH3
Δdiss
(E—H)/kJ mol–1
389 322 297 255
(i) NH3
(ii) PH3
(iii) AsH3
(iv) SbH3
8. On heating with concentrated NaOH solution in an inert atmosphere of CO2
,
white phosphorus gives a gas. Which of the following statement is incorrect
about the gas?
(i) It is highly poisonous and has smell like rotten fish.
(ii) It’s solution in water decomposes in the presence of light.
(iii) It is more basic than NH3
.
(iv) It is less basic than NH3
.
9. Which of the following acids forms three series of salts?
(i) H3
PO2
(ii) H3
BO3
(iii) H3
PO4
(iv) H3
PO3
10. Strong reducing behaviour of H3
PO2
is due to
(i) Low oxidation state of phosphorus
(ii) Presence of two –OH groups and one P–H bond
91 p-Block Elements
www.tiwariacademy.com
3. 92
Exemplar Problems, Chemistry
(iii) Presence of one –OH group and two P–H bonds
(iv) High electron gain enthalpy of phosphorus
11. On heating lead nitrate forms oxides of nitrogen and lead. The oxides formed
are ______.
(i) N2
O, PbO
(ii) NO2
, PbO
(iii) NO, PbO
(iv) NO, PbO2
12. Which of the following elements does not show allotropy?
(i) Nitrogen
(ii) Bismuth
(iii) Antimony
(iv) Arsenic
13. Maximum covalency of nitrogen is ______________.
(i) 3
(ii) 5
(iii) 4
(iv) 6
14. Which of the following statements is wrong?
(i) Single N–N bond is stronger than the single P–P bond.
(ii) PH3
can act as a ligand in the formation of coordination compound
with transition elements.
(iii) NO2
is paramagnetic in nature.
(iv) Covalency of nitrogen in N2
O5
is four.
15. A brown ring is formed in the ring test for NO3
–
ion. It is due to the formation of
(i) [Fe(H2
O)5
(NO)]
2+
(ii) FeSO4
.NO2
(iii) [Fe(H2
O)4
(NO)2
]
2+
(iv) FeSO4
.HNO3
16. Elements of group-15 form compounds in +5 oxidation state. However,
bismuth forms only one well characterised compound in +5 oxidation state.
The compound is
(i) Bi2
O5
(ii) BiF5
(iii) BiCl5
(iv) Bi2
S5
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4. 93 p-Block Elements
17. On heating ammonium dichromate and barium azide separately we get
(i) N2
in both cases
(ii) N2
with ammonium dichromate and NO with barium azide
(iii) N2
O with ammonium dichromate and N2
with barium azide
(iv) N2
O with ammonium dichromate and NO2
with barium azide
18. In the preparation of HNO3
, we get NO gas by catalytic oxidation of ammonia.
The moles of NO produced by the oxidation of two moles of NH3
will be ______.
(i) 2
(ii) 3
(iii) 4
(iv) 6
19. The oxidation state of central atom in the anion of compound NaH2
PO2
will
be ______.
(i) +3
(ii) +5
(iii) +1
(iv) –3
20. Which of the following is not tetrahedral in shape?
(i) NH4
+
(ii) SiCl4
(iii) SF4
(iv) SO4
2–
21. Which of the following are peroxoacids of sulphur?
(i) H2
SO5
and H2
S2
O8
(ii) H2
SO5
and H2
S2
O7
(iii) H2
S2
O7
and H2
S2
O8
(iv) H2
S2
O6
and H2
S2
O7
22. Hot conc. H2
SO4
acts as moderately strong oxidising agent. It oxidises both
metals and nonmetals. Which of the following element is oxidised by conc.
H2
SO4
into two gaseous products?
(i) Cu
(ii) S
(iii) C
(iv) Zn
23. A black compound of manganese reacts with a halogen acid to give greenish
yellow gas. When excess of this gas reacts with NH3
an unstable trihalide is
formed. In this process the oxidation state of nitrogen changes from _________.
(i) – 3 to +3
(ii) – 3 to 0
(iii) – 3 to +5
(iv) 0 to – 3
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5. 94
Exemplar Problems, Chemistry
24. In the preparation of compounds of Xe, Bartlett had taken O2
+
Pt F6
–
as a base
compound. This is because
(i) both O2
and Xe have same size.
(ii) both O2
and Xe have same electron gain enthalpy.
(iii) both O2
and Xe have almost same ionisation enthalpy.
(iv) both Xe and O2
are gases.
25. In solid state PCl5
is a _________.
(i) covalent solid
(ii) octahedral structure
(iii) ionic solid with [PCl6
]+
octahedral and [PCl4
]–
tetrahedra
(iv) ionic solid with [PCl4
]
+
tetrahedral and [PCl6
]
–
octahedra
26. Reduction potentials of some ions are given below. Arrange them in decreasing
order of oxidising power.
Ion ClO4
–
IO4
–
BrO4
–
Reduction E
V
=1.19V E
V
=1.65V E
V
=1.74V
potential E
V
V
V
/V
(i) ClO4
–
> IO4
–
> BrO4
–
(ii) IO4
–
> BrO4
–
> ClO4
–
(iii) BrO4
–
> IO4
–
> ClO4
–
(iv) BrO4
–
> ClO4
–
> IO4
–
27. Which of the following is isoelectronic pair?
(i) ICl2
, ClO2
(ii) BrO2
–
, BrF2
+
(iii) ClO2
, BrF
(iv) CN
–
, O3
II. Multiple Choice Questions (Type-II)
Note : In the following questions two or more options may be correct.
28. If chlorine gas is passed through hot NaOH solution, two changes are observed
in the oxidation number of chlorine during the reaction. These are ________
and _________.
(i) 0 to +5
(ii) 0 to +3
(iii) 0 to –1
(iv) 0 to +1
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6. 95 p-Block Elements
29. Which of the following options are not in accordance with the property
mentioned against them?
(i) F2
> Cl2
> Br2
> I2
Oxidising power.
(ii) MI > MBr > MCl > MF Ionic character of metal halide.
(iii) F2
> Cl2
> Br2
> I2
Bond dissociation enthalpy.
(iv) HI < HBr < HCl < HF Hydrogen-halogen bond strength.
30. Which of the following is correct for P4
molecule of white phosphorus?
(i) It has 6 lone pairs of electrons.
(ii) It has six P–P single bonds.
(iii) It has three P–P single bonds.
(iv) It has four lone pairs of electrons.
31. Which of the following statements are correct?
(i) Among halogens, radius ratio between iodine and fluorine is maximum.
(ii) Leaving F—F bond, all halogens have weaker X—X bond than X—X'
bond in interhalogens.
(iii) Among interhalogen compounds maximum number of atoms are present
in iodine fluoride.
(iv) Interhalogen compounds are more reactive than halogen compounds.
32. Which of the following statements are correct for SO2
gas?
(i) It acts as bleaching agent in moist conditions.
(ii) It’s molecule has linear geometry.
(iii) It’s dilute solution is used as disinfectant.
(iv) It can be prepared by the reaction of dilute H2
SO4
with metal sulphide.
33. Which of the following statements are correct?
(i) All the three N—O bond lengths in HNO3
are equal.
(ii) All P—Cl bond lengths in PCl5
molecule in gaseous state are equal.
(iii) P4
molecule in white phohsphorus have angular strain therefore white
phosphorus is very reactive.
(iv) PCl is ionic in solid state in which cation is tetrahedral and anion is
octahedral.
34. Which of the following orders are correct as per the properties mentioned against
each?
(i) As2
O3
< SiO2
< P2
O3
< SO2
Acid strength.
(ii) AsH3
< PH3
< NH3
Enthalpy of vapourisation.
(iii) S < O < Cl < F More negative electron gain enthalpy.
(iv) H2
O > H2
S > H2
Se > H2
Te Thermal stability.
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7. 96
Exemplar Problems, Chemistry
35. Which of the following statements are correct?
(i) S–S bond is present in H2
S2
O6
.
(ii) In peroxosulphuric acid (H2
SO5
) sulphur is in +6 oxidation state.
(iii) Iron powder along with Al2
O3
and K2
O is used as a catalyst in the
preparation of NH3
by Haber’s process.
(iv) Change in enthalpy is positive for the preparation of SO3
by catalytic
oxidation of SO2
.
36. In which of the following reactions conc. H2
SO4
is used as an oxidising reagent?
(i) CaF2
+ H2
SO4
⎯→ CaSO4
+ 2HF
(ii) 2HI + H2
SO4
⎯→ I2
+ SO2
+ 2H2
O
(iii) Cu + 2H2
SO4
⎯→ CuSO4
+ SO2
+ 2H2
O
(iv) NaCl + H2
SO4
⎯→ NaHSO4
+ HCl
37. Which of the following statements are true?
(i) Only type of interactions between particles of noble gases are due to
weak dispersion forces.
(ii) Ionisation enthalpy of molecular oxygen is very close to that of xenon.
(iii) Hydrolysis of XeF6
is a redox reaction.
(iv) Xenon fluorides are not reactive.
III. Short Answer Type
38. In the preparation of H2
SO4
by Contact Process, why is SO3
not absorbed
directly in water to form H2
SO4
?
39. Write a balanced chemical equation for the reaction showing catalytic oxidation
of NH3
by atmospheric oxygen.
40. Write the structure of pyrophosphoric acid.
41. PH3
forms bubbles when passed slowly in water but NH3
dissolves. Explain
why?
42. In PCl5
, phosphorus is in sp3
d hybridised state but all its five bonds are not
equivalent. Justify your answer with reason.
43. Why is nitric oxide paramagnetic in gaseous state but the solid obtained on
cooling it is diamagnetic?
44. Give reason to explain why ClF3
exists but FCl3
does not exist.
45. Out of H2
O and H2
S, which one has higher bond angle and why?
46. SF6
is known but SCl6
is not. Why?
47. On reaction with Cl2
, phosphorus forms two types of halides ‘A’ and ‘B’. Halide
A is yellowish-white powder but halide ‘B’ is colourless oily liquid. Identify A
and B and write the formulas of their hydrolysis products.
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8. 97 p-Block Elements
48. In the ring test of NO3
–
ion, Fe
2+
ion reduces nitrate ion to nitric oxide, which
combines with Fe
2+
(aq) ion to form brown complex. Write the reactions involved
in the formation of brown ring.
49. Explain why the stability of oxoacids of chlorine increases in the order given
below:
HClO < HClO2
< HClO3
< HClO4
50. Explain why ozone is thermodynamically less stable than oxygen.
51. P4
O6
reacts with water according to equation P4
O6
+ 6H2
O ⎯→ 4H3
PO3
.
Calculate the volume of 0.1 M NaOH solution required to neutralise the acid
formed by dissolving 1.1 g of P4
O6
in H2
O.
52. White phosphorus reacts with chlorine and the product hydrolyses in the
presence of water. Calculate the mass of HCl obtained by the hydrolysis of the
product formed by the reaction of 62 g of white phosphorus with chlorine in
the presence of water.
53. Name three oxoacids of nitrogen. Write the disproportionation reaction of that
oxoacid of nitrogen in which nitrogen is in +3 oxidation state.
54. Nitric acid forms an oxide of nitrogen on reaction with P4
O10
. Write the reaction
involved. Also write the resonating structures of the oxide of nitrogen formed.
55. Phosphorus has three allotropic forms — (i) white phosphorus (ii) red
phosphorus and (iii) black phosphorus. Write the difference between white
and red phosphorus on the basis of their structure and reactivity.
56. Give an example to show the effect of concentration of nitric acid on the
formation of oxidation product.
57. PCl5
reacts with finely divided silver on heating and a white silver salt is
obtained, which dissolves on adding excess aqueous NH3
solution. Write the
reactions involved to explain what happens.
58. Phosphorus forms a number of oxoacids. Out of these oxoacids phosphinic
acid has strong reducing property. Write its structure and also write a reaction
showing its reducing behaviour.
IV. Matching Type
Note : Match the items of Column I and Column II in the following questions.
59. Match the compounds given in Column I with the hybridisation and shape
given in Column II and mark the correct option.
Column I Column II
(A) Xe F6
(1) sp3
d3
– distorted octahedral
(B) Xe O3
(2) sp3
d2
- square planar
(C) Xe OF4
(3) sp3
- pyramidal
(D) Xe F4
(4) sp3
d2
- square pyramidal
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9. 98
Exemplar Problems, Chemistry
Code :
(i) A (1) B (3) C (4) D (2)
(ii) A (1) B (2) C (4) D (3)
(iii) A (4) B (3) C (1) D (2)
(iv) A (4) B (1) C (2) D (3)
60. Match the formulas of oxides given in Column I with the type of oxide given in
Column II and mark the correct option.
Column I Column II
(A) Pb3
O4
(1) Neutral oxide
(B) N2
O (2) Acidic oxide
(C) Mn2
O7
(3) Basic oxide
(D) Bi2
O3
(4) Mixed oxide
Code :
(i) A (1) B (2) C (3) D (4)
(ii) A (4) B (1) C (2) D (3)
(iii) A (3) B (2) C (4) D (1)
(iv) A (4) B (3) C (1) D (2)
61. Match the items of Columns I and II and mark the correct option.
Column I Column II
(A) H2
SO4
(1) Highest electron gain
enthalpy
(B) CCl3
NO2
(2) Chalcogen
(C) Cl2
(3) Tear gas
(D) Sulphur (4) Storage batteries
Code :
(i) A (4) B (3) C (1) D (2)
(ii) A (3) B (4) C (1) D (2)
(iii) A (4) B (1) C (2) D (3)
(iv) A (2) B (1) C (3) D (4)
62. Match the species given in Column I with the shape given in Column II and
mark the correct option.
Column I Column II
(A) SF4
(1) Tetrahedral
(B) BrF3
(2) Pyramidal
(C) BrO3
–
(3) Sea-saw shaped
(D) NH
+
4
(4) Bent T-shaped
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10. 99 p-Block Elements
Code :
(i) A (3) B (2) C (1) D (4)
(ii) A (3) B (4) C (2) D (1)
(iii) A (1) B (2) C (3) D (4)
(iv) A (1) B (4) C (3) D (2)
63. Match the items of Columns I and II and mark the correct option.
Column I Column II
(A) Its partial hydrolysis does not (1) He
change oxidation state of central atom
(B) It is used in modern diving apparatus (2) XeF6
(C) It is used to provide inert atmosphere (3) XeF4
for filling electrical bulbs
(D) Its central atom is in sp 3
d
2
hybridisation (4) Ar
Code :
(i) A (1) B (4) C (2) D (3)
(ii) A (1) B (2) C (3) D (4)
(iii) A (2) B (1) C (4) D (3)
(iv) A (1) B (3) C (2) D (4)
V. Assertion and Reason Type
Note : In the following questions a statement of assertion followed by a
statement of reason is given. Choose the correct answer out of the following
choices.
(i) Both assertion and reason are correct statements, and reason is the correct
explanation of the assertion.
(ii) Both assertion and reason are correct statements, but reason is not the
correct explanation of the assertion.
(iii) Assertion is correct, but reason is wrong statement.
(iv) Assertion is wrong but reason is correct statement.
(v) Both assertion and reason are wrong statements.
64. Assertion : N2
is less reactive than P4
.
Reason : Nitrogen has more electron gain enthalpy than phosphorus.
65. Assertion : HNO3
makes iron passive.
Reason : HNO3
forms a protective layer of ferric nitrate on the surface
of iron.
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11. 100
Exemplar Problems, Chemistry
66. Assertion : HI cannot be prepared by the reaction of KI with concentrated
H2
SO4
Reason : HI has lowest H–X bond strength among halogen acids.
67. Assertion : Both rhombic and monoclinic sulphur exist as S8
but oxygen
exists as O2
.
Reason : Oxygen forms pπ – pπ multiple bond due to small size and
small bond length but pπ – pπ bonding is not possible in
sulphur.
68. Assertion : NaCl reacts with concentrated H2
SO4
to give colourless fumes
with pungent smell. But on adding MnO2
the fumes become
greenish yellow.
Reason : MnO2
oxidises HCl to chlorine gas which is greenish yellow.
69. Assertion : SF6
cannot be hydrolysed but SF4
can be.
Reason : Six F atoms in SF6
prevent the attack of H2
O on sulphur
atom of SF6
.
VI. Long Answer Type
70. An amorphous solid “A” burns in air to form a gas “B” which turns lime water
milky. The gas is also produced as a by-product during roasting of sulphide
ore. This gas decolourises acidified aqueous KMnO4
solution and reduces
Fe3+
to Fe2+
. Identify the solid “A” and the gas “B” and write the reactions
involved.
71. On heating lead (II) nitrate gives a brown gas “A”. The gas “A” on cooling
changes to colourless solid “B”. Solid “B” on heating with NO changes to a
blue solid ‘C’. Identify ‘A’, ‘B’ and ‘C’ and also write reactions involved and
draw the structures of ‘B’ and ‘C’.
72. On heating compound (A) gives a gas (B) which is a constituent of air. This
gas when treated with 3 mol of hydrogen (H2
) in the presence of a catalyst
gives another gas (C) which is basic in nature. Gas C on further oxidation in
moist condition gives a compound (D) which is a part of acid rain. Identify
compounds (A) to (D) and also give necessary equations of all the steps involved.
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