This document provides information about a chemistry GCSE exam involving questions on the periodic table, reactions of elements, preparation of salts, electrolysis, exothermic reactions, and hydrated sodium carbonate. The questions assess knowledge of key concepts like periodic trends, writing balanced equations, describing preparation methods and observations, redox reactions, and stoichiometry calculations. Step-by-step working is shown for multi-part questions involving calculations.
The document discusses the production of ammonia via the Haber process. Key points:
- Ammonia is produced by reacting nitrogen and hydrogen gases over an iron catalyst at high temperature (450°C) and pressure (200 atm).
- The balanced equation for the reaction is: N2 + 3H2 → 2NH3
- Unreacted gases are recycled in the process. Ammonia is then cooled to be liquified.
Chemistry perfect-score-module-form-4-set-4Mudzaffar Shah
This document discusses acids, bases, and salts. It defines acids as compounds that produce hydrogen ions (H+) or hydronium ions (H3O+) when dissolved in water. Bases are defined as substances that can neutralize acids to produce salts and water.
It discusses the properties of strong acids and bases versus weak acids and bases. Strong acids and bases fully dissociate in water, while weak acids and bases only partially dissociate.
The document also discusses monoprotic, diprotic, and triprotic acids based on the number of hydrogen ions they can donate. Equations are provided for the dissociation of several common acids like nitric acid, ethanoic acid, carbon
This document consists of a 14 page chemistry exam for the International General Certificate of Secondary Education. The exam contains multiple choice and free response questions testing knowledge of topics including:
- Gases in air and common air pollutants
- Classification of oxides
- Reactions of zinc and uses of zinc
- Electrochemistry of galvanic cells
- Allotropes and uses of oxygen
- Acid-base reactions involving iodine
- Structures and properties of group 14 elements
- Contact process for sulfuric acid production
- Hydrocarbon reactions to form alcohols
This document consists of exam questions related to chemistry. It includes 14 pages of multiple choice and free response questions testing knowledge of topics like the composition of air, classification of oxides, properties of metals like zinc and their compounds, organic compounds and reactions, and industrial processes like the contact process for producing sulfuric acid. The exam is for the International General Certificate of Secondary Education in Chemistry.
Marking scheme-chemistry-perfect-score-module-form-4-set-4Mudzaffar Shah
The document provides a marking scheme for an exam on acids, bases, and salts. It includes:
1) 11 multiple choice questions on acid-base concepts like neutralization reactions, ions present, calculating molarity, and distinguishing between strong/weak acids.
2) 9 more multiple choice questions testing identification of solutions, gas tests, and acid/base properties.
3) 10 essay questions requiring explanations of acid/base definitions, calculations of standard solutions, titration procedures, comparisons of acid types, and writing hypotheses and procedures for experiments.
4) Rubrics for grading lab reports with criteria like correctly recording burette readings, setting up tables, stating observations/inferences, and comparing
This document is a 16-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 exam questions testing knowledge of topics including the periodic table, atmospheric pollution, acid-base reactions, extraction of metals, organic compounds, and calcium compounds. Diagrams and tables are provided, and students are to show workings, complete equations, and answer short questions.
This document is the cover sheet and first 7 pages of a chemistry exam. It provides instructions for candidates to write their details, not use additional materials, and answer all questions. The exam consists of 7 multi-part chemistry questions testing understanding of topics like the contact process for sulfuric acid production, precipitation reactions, electrolysis, polymers, and stoichiometry.
The atomic radius is the distance from the atomic nucleus to the outermost stable electron orbital in an atom that is at equilibrium. The atomic radius tends to decrease as one progresses across a period from left to right because the effective nuclear charge increases, thereby attracting the orbiting electrons and lessening the radius. The atomic radius usually increases while going down a group due to the addition of a new energy level (shell). However, diagonally, the number of electrons has a larger effect than the sizeable radiu
The document discusses the production of ammonia via the Haber process. Key points:
- Ammonia is produced by reacting nitrogen and hydrogen gases over an iron catalyst at high temperature (450°C) and pressure (200 atm).
- The balanced equation for the reaction is: N2 + 3H2 → 2NH3
- Unreacted gases are recycled in the process. Ammonia is then cooled to be liquified.
Chemistry perfect-score-module-form-4-set-4Mudzaffar Shah
This document discusses acids, bases, and salts. It defines acids as compounds that produce hydrogen ions (H+) or hydronium ions (H3O+) when dissolved in water. Bases are defined as substances that can neutralize acids to produce salts and water.
It discusses the properties of strong acids and bases versus weak acids and bases. Strong acids and bases fully dissociate in water, while weak acids and bases only partially dissociate.
The document also discusses monoprotic, diprotic, and triprotic acids based on the number of hydrogen ions they can donate. Equations are provided for the dissociation of several common acids like nitric acid, ethanoic acid, carbon
This document consists of a 14 page chemistry exam for the International General Certificate of Secondary Education. The exam contains multiple choice and free response questions testing knowledge of topics including:
- Gases in air and common air pollutants
- Classification of oxides
- Reactions of zinc and uses of zinc
- Electrochemistry of galvanic cells
- Allotropes and uses of oxygen
- Acid-base reactions involving iodine
- Structures and properties of group 14 elements
- Contact process for sulfuric acid production
- Hydrocarbon reactions to form alcohols
This document consists of exam questions related to chemistry. It includes 14 pages of multiple choice and free response questions testing knowledge of topics like the composition of air, classification of oxides, properties of metals like zinc and their compounds, organic compounds and reactions, and industrial processes like the contact process for producing sulfuric acid. The exam is for the International General Certificate of Secondary Education in Chemistry.
Marking scheme-chemistry-perfect-score-module-form-4-set-4Mudzaffar Shah
The document provides a marking scheme for an exam on acids, bases, and salts. It includes:
1) 11 multiple choice questions on acid-base concepts like neutralization reactions, ions present, calculating molarity, and distinguishing between strong/weak acids.
2) 9 more multiple choice questions testing identification of solutions, gas tests, and acid/base properties.
3) 10 essay questions requiring explanations of acid/base definitions, calculations of standard solutions, titration procedures, comparisons of acid types, and writing hypotheses and procedures for experiments.
4) Rubrics for grading lab reports with criteria like correctly recording burette readings, setting up tables, stating observations/inferences, and comparing
This document is a 16-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 exam questions testing knowledge of topics including the periodic table, atmospheric pollution, acid-base reactions, extraction of metals, organic compounds, and calcium compounds. Diagrams and tables are provided, and students are to show workings, complete equations, and answer short questions.
This document is the cover sheet and first 7 pages of a chemistry exam. It provides instructions for candidates to write their details, not use additional materials, and answer all questions. The exam consists of 7 multi-part chemistry questions testing understanding of topics like the contact process for sulfuric acid production, precipitation reactions, electrolysis, polymers, and stoichiometry.
The atomic radius is the distance from the atomic nucleus to the outermost stable electron orbital in an atom that is at equilibrium. The atomic radius tends to decrease as one progresses across a period from left to right because the effective nuclear charge increases, thereby attracting the orbiting electrons and lessening the radius. The atomic radius usually increases while going down a group due to the addition of a new energy level (shell). However, diagonally, the number of electrons has a larger effect than the sizeable radiu
This document is a chemistry exam paper consisting of 10 printed pages and 2 blank pages. It contains questions on topics such as the Contact Process for making sulfuric acid, properties of manganese, Period 3 elements, alkenes, and electrolysis of copper sulfate. The exam is marked out of a total number of marks given at the end of each question.
This document consists of a 14 page chemistry exam with multiple choice and free response questions covering topics like the halogens, redox reactions, organic chemistry, acid-base reactions, and metals/alloys. It includes diagrams of lab setups and reagents/products. The exam provides space for students to show their work and includes a periodic table reference.
Jee mantra.iit jee advanced chemistry paper and solutionJEE MANTRA
This document contains sample questions from an IIT-JEE Advanced chemistry exam. It includes 12 questions on topics like oxidation-reduction reactions, isomerism, hydrogen bonding, electrochemistry, transition metals, and solutions. The total number of reagents that can oxidize iodide to iodine is 7. The molality of a 3.2 molar solution of a compound with molar mass 80 g/mol dissolved in a solvent with density 0.4 g/mL is 8.
This document appears to be an exam paper for a chemistry test. It consists of 7 multi-part questions covering various chemistry topics such as:
- Transition elements and the extraction of iron
- Reactivity of metals with water and acids
- Acids, bases and pH
- Oxides and their reactions
- Structures of carbon, silicon and germanium compounds
- Contact process for making sulfuric acid
- Combustion reactions and cell reactions
- Cracking of hydrocarbons
The questions require students to identify substances, write equations, describe processes, explain concepts, make predictions and draw structural formulas. An answer sheet is provided for students to write their responses.
Balancing equations worksheet and key, balancing equations, grade level varies, found on another site. This is high school level practice. This may be used for advanced chemistry practice, as well.
This document consists of a 14-page chemistry exam paper from the University of Cambridge International Examinations. The exam paper contains 8 multi-part chemistry questions testing students' knowledge of topics including the properties of gases, calcium carbonate, the Haber process, food chemistry, and reaction rates. It also includes a periodic table of elements.
Dear Students/Parents
We at 'Apex Institute' are committed to provide our students best quality education with ethics. Moving in this direction, we have decided that unlike other expensive and 5star facility type institutes who are huge investors and advertisers, we shall not invest huge amount of money in advertisements. It shall rather be invested on the betterment, enhancement of quality and resources at our center.
We are just looking forward to have 'word-of-mouth' publicity instead. Because, there is only a satisfied student and his/her parents can judge an institute's quality and it's faculty members coaching.
Those coaching institutes, who are investing highly on advertisements, are actually, wasting their money on it, in a sense. Rather, the money should be invested on highly experienced faculty members and on teaching gears.
We all at 'Apex' are taking this initiative to improve the quality of education along-with each student's development and growth.
Committed to excellence...
With best wishes.
S . Iqbal
( Motivator & Mentor)
This document outlines the syllabus statements and learning objectives for a unit on acids, bases and salts. It discusses the characteristic properties of acids and bases, including pH and indicators. It also covers the classification of oxides as acidic or basic, the preparation and purification of salts, and tests to identify aqueous cations, anions, and common gases. The objectives include describing acid-base reactions, the importance of pH in the environment, and suggesting methods to make salts from starting materials.
This document is a 16-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 multi-part chemistry questions testing knowledge of topics including the periodic table, atmospheric pollutants, acid-base reactions, extraction of metals, combustion reactions, organic compounds, and properties of group 1 and transition metals. It also includes a copy of the periodic table.
This document is a 14-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 multi-part questions testing knowledge of topics including fossil fuels, salt preparations, the periodic table, electrolysis of molten aluminum, esters and fats, and corrosion protection of steel structures. Blank pages are included at the end for calculations and diagrams.
This document contains the mark scheme for the May/June 2006 International General Certificate of Secondary Education (IGCSE) Chemistry exam. It provides guidance to examiners on how to award marks for students' answers, including identifying acceptable alternative responses. The mark scheme also indicates the minimum marks required to achieve different overall grades. CIE will not enter into discussions about the mark scheme.
This document consists of a chemistry exam paper containing multiple choice and short answer questions testing knowledge of chemical apparatus, reactions, and experimental procedures. The questions cover topics such as identifying experimental set ups, describing chemical reactions and tests, planning investigations, analyzing results, and drawing conclusions from experiments.
This document provides instructions for candidates taking an International General Certificate of Secondary Education (IGCSE) Chemistry exam. It includes the exam paper with multiple choice and free response questions covering topics like the periodic table, chemical reactions, organic compounds, and atmospheric pollution. Candidates are to write their answers directly on the exam paper and show all working for calculations and diagrams.
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 contains mark schemes for Chemistry examinations from June 2004, including:
- The mark scheme and maximum marks for multiple choice, core, and extended papers.
- Details on how examiners were instructed to award marks and handle unexpected responses.
- Grade thresholds for each exam component.
- Sample exam questions and answers with marks allocated.
The document discusses changes made by CIE to use different variants of some question papers for assessments with large candidatures, where previously there was only one variant, in order to provide more past examination material. It explains that the content and question types remain unchanged between variants, and that the relationships between question papers, mark schemes, and principal examiner's reports have been established. Candidates will typically only see one variant of a question paper for their country.
The document is the mark scheme for the October/November 2013 International General Certificate of Secondary Education (IGCSE) Chemistry exam. It provides the answers and allocation of marks for questions 1 through 7 on the exam. For each question or part of a question, it specifies the marks awarded for correct responses. It also provides guidance to examiners on acceptable alternative answers and use of examiners' discretion. The mark scheme is intended to be used along with the exam paper and examiner's report to ensure fair and consistent marking of students' responses.
The document contains summaries of several diagrams showing different scientific processes and experiments. It provides answers to questions about the diagrams, identifying variables, materials, observations, and conclusions. The key information summarized is that the document contains expert summaries and explanations of multiple scientific diagrams and experiments.
The document discusses CIE's use of variant question papers for some popular assessments with large candidatures. It explains that while the content and question types remain the same, there are now two variants of the question paper, mark scheme, and principal examiner's report for one component. Centres will use only one variant, but this provides access to more past examination material. It includes a diagram showing the relationship between the question papers, mark schemes, and reports for the two variants. The document also provides contact information for questions about these changes.
This document is a 16-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 exam questions testing students' knowledge of topics including the periodic table, atmospheric pollution, acid-base reactions, extraction of metals, combustion reactions, organic compounds, and properties of calcium chloride. Diagrams and tables are provided to aid in answering multiple-choice and written response questions.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against developing mental illness and improve symptoms for those who already suffer from conditions like anxiety and depression.
This document is a chemistry exam from Puntland State of Somalia consisting of 9 sections with a total of 100 marks. It covers various chemistry concepts such as the electronic configurations of elements, chemical equations, enthalpy, organic compounds, and industrial processes like the Haber process. The exam tests the students' understanding of fundamental chemistry principles through multiple choice and structured questions requiring explanations and calculations.
This document is a chemistry exam paper consisting of 10 printed pages and 2 blank pages. It contains questions on topics such as the Contact Process for making sulfuric acid, properties of manganese, Period 3 elements, alkenes, and electrolysis of copper sulfate. The exam is marked out of a total number of marks given at the end of each question.
This document consists of a 14 page chemistry exam with multiple choice and free response questions covering topics like the halogens, redox reactions, organic chemistry, acid-base reactions, and metals/alloys. It includes diagrams of lab setups and reagents/products. The exam provides space for students to show their work and includes a periodic table reference.
Jee mantra.iit jee advanced chemistry paper and solutionJEE MANTRA
This document contains sample questions from an IIT-JEE Advanced chemistry exam. It includes 12 questions on topics like oxidation-reduction reactions, isomerism, hydrogen bonding, electrochemistry, transition metals, and solutions. The total number of reagents that can oxidize iodide to iodine is 7. The molality of a 3.2 molar solution of a compound with molar mass 80 g/mol dissolved in a solvent with density 0.4 g/mL is 8.
This document appears to be an exam paper for a chemistry test. It consists of 7 multi-part questions covering various chemistry topics such as:
- Transition elements and the extraction of iron
- Reactivity of metals with water and acids
- Acids, bases and pH
- Oxides and their reactions
- Structures of carbon, silicon and germanium compounds
- Contact process for making sulfuric acid
- Combustion reactions and cell reactions
- Cracking of hydrocarbons
The questions require students to identify substances, write equations, describe processes, explain concepts, make predictions and draw structural formulas. An answer sheet is provided for students to write their responses.
Balancing equations worksheet and key, balancing equations, grade level varies, found on another site. This is high school level practice. This may be used for advanced chemistry practice, as well.
This document consists of a 14-page chemistry exam paper from the University of Cambridge International Examinations. The exam paper contains 8 multi-part chemistry questions testing students' knowledge of topics including the properties of gases, calcium carbonate, the Haber process, food chemistry, and reaction rates. It also includes a periodic table of elements.
Dear Students/Parents
We at 'Apex Institute' are committed to provide our students best quality education with ethics. Moving in this direction, we have decided that unlike other expensive and 5star facility type institutes who are huge investors and advertisers, we shall not invest huge amount of money in advertisements. It shall rather be invested on the betterment, enhancement of quality and resources at our center.
We are just looking forward to have 'word-of-mouth' publicity instead. Because, there is only a satisfied student and his/her parents can judge an institute's quality and it's faculty members coaching.
Those coaching institutes, who are investing highly on advertisements, are actually, wasting their money on it, in a sense. Rather, the money should be invested on highly experienced faculty members and on teaching gears.
We all at 'Apex' are taking this initiative to improve the quality of education along-with each student's development and growth.
Committed to excellence...
With best wishes.
S . Iqbal
( Motivator & Mentor)
This document outlines the syllabus statements and learning objectives for a unit on acids, bases and salts. It discusses the characteristic properties of acids and bases, including pH and indicators. It also covers the classification of oxides as acidic or basic, the preparation and purification of salts, and tests to identify aqueous cations, anions, and common gases. The objectives include describing acid-base reactions, the importance of pH in the environment, and suggesting methods to make salts from starting materials.
This document is a 16-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 multi-part chemistry questions testing knowledge of topics including the periodic table, atmospheric pollutants, acid-base reactions, extraction of metals, combustion reactions, organic compounds, and properties of group 1 and transition metals. It also includes a copy of the periodic table.
This document is a 14-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 multi-part questions testing knowledge of topics including fossil fuels, salt preparations, the periodic table, electrolysis of molten aluminum, esters and fats, and corrosion protection of steel structures. Blank pages are included at the end for calculations and diagrams.
This document contains the mark scheme for the May/June 2006 International General Certificate of Secondary Education (IGCSE) Chemistry exam. It provides guidance to examiners on how to award marks for students' answers, including identifying acceptable alternative responses. The mark scheme also indicates the minimum marks required to achieve different overall grades. CIE will not enter into discussions about the mark scheme.
This document consists of a chemistry exam paper containing multiple choice and short answer questions testing knowledge of chemical apparatus, reactions, and experimental procedures. The questions cover topics such as identifying experimental set ups, describing chemical reactions and tests, planning investigations, analyzing results, and drawing conclusions from experiments.
This document provides instructions for candidates taking an International General Certificate of Secondary Education (IGCSE) Chemistry exam. It includes the exam paper with multiple choice and free response questions covering topics like the periodic table, chemical reactions, organic compounds, and atmospheric pollution. Candidates are to write their answers directly on the exam paper and show all working for calculations and diagrams.
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 contains mark schemes for Chemistry examinations from June 2004, including:
- The mark scheme and maximum marks for multiple choice, core, and extended papers.
- Details on how examiners were instructed to award marks and handle unexpected responses.
- Grade thresholds for each exam component.
- Sample exam questions and answers with marks allocated.
The document discusses changes made by CIE to use different variants of some question papers for assessments with large candidatures, where previously there was only one variant, in order to provide more past examination material. It explains that the content and question types remain unchanged between variants, and that the relationships between question papers, mark schemes, and principal examiner's reports have been established. Candidates will typically only see one variant of a question paper for their country.
The document is the mark scheme for the October/November 2013 International General Certificate of Secondary Education (IGCSE) Chemistry exam. It provides the answers and allocation of marks for questions 1 through 7 on the exam. For each question or part of a question, it specifies the marks awarded for correct responses. It also provides guidance to examiners on acceptable alternative answers and use of examiners' discretion. The mark scheme is intended to be used along with the exam paper and examiner's report to ensure fair and consistent marking of students' responses.
The document contains summaries of several diagrams showing different scientific processes and experiments. It provides answers to questions about the diagrams, identifying variables, materials, observations, and conclusions. The key information summarized is that the document contains expert summaries and explanations of multiple scientific diagrams and experiments.
The document discusses CIE's use of variant question papers for some popular assessments with large candidatures. It explains that while the content and question types remain the same, there are now two variants of the question paper, mark scheme, and principal examiner's report for one component. Centres will use only one variant, but this provides access to more past examination material. It includes a diagram showing the relationship between the question papers, mark schemes, and reports for the two variants. The document also provides contact information for questions about these changes.
This document is a 16-page exam for the International General Certificate of Secondary Education in Chemistry. It contains 7 exam questions testing students' knowledge of topics including the periodic table, atmospheric pollution, acid-base reactions, extraction of metals, combustion reactions, organic compounds, and properties of calcium chloride. Diagrams and tables are provided to aid in answering multiple-choice and written response questions.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against developing mental illness and improve symptoms for those who already suffer from conditions like anxiety and depression.
This document is a chemistry exam from Puntland State of Somalia consisting of 9 sections with a total of 100 marks. It covers various chemistry concepts such as the electronic configurations of elements, chemical equations, enthalpy, organic compounds, and industrial processes like the Haber process. The exam tests the students' understanding of fundamental chemistry principles through multiple choice and structured questions requiring explanations and calculations.
This document provides instructions for candidates taking an International General Certificate of Secondary Education (IGCSE) Chemistry exam. It includes:
1. Instructions for candidates to write their details and to answer all questions.
2. A 15 page exam paper with multiple choice and structured questions covering topics like the periodic table, chemical reactions, organic compounds, acids and bases, electrolysis and fertilizers.
3. A notice that the exam consists of 15 printed pages and 1 blank page.
This document provides a chemistry revision programme that includes:
1. Lists of cation and anion names and formulas.
2. Instructions to construct chemical formulas for compounds.
3. Information on chemical properties of acids and reactions with metals, carbonates, and basic oxides.
4. Examples of balanced chemical and ionic equations for acid-base reactions.
5. Tables of chloride, nitrate, and sulfate salts formed from the example equations.
The document discusses the use of variant question papers by CIE (Cambridge International Examinations) for some of their popular assessments. It explains that while the content and standard of assessment remains the same, there are now two variants of the question papers, mark schemes, and principal examiner reports available for one component. This provides centers with more past examination material than usual to access. It includes both variants in the document. It also provides contact information for any questions about these changes and instructions for identifying the relevant parts of the document.
The document summarizes key topics about the atmosphere and environment, including:
1) The composition of air is approximately 78% nitrogen, 21% oxygen, and the remainder being noble gases like argon.
2) Common air pollutants include carbon monoxide, nitrogen oxides, sulfur dioxide, and their sources include incomplete combustion of fuels and vehicles.
3) Air pollution can harm health and the environment, and acid rain forms from air pollutants dissolving in water. Increased carbon dioxide and methane in the atmosphere may contribute to global warming.
This document provides an overview of chemical equations and reactions. It discusses:
- Chemical equations, reactants, products, and how atoms rearrange during reactions.
- Balancing chemical equations by ensuring equal numbers of each atom on both sides.
- Information that can be obtained from a balanced chemical equation, such as moles of substances.
- Four main types of chemical reactions: combination, decomposition, displacement, and double displacement. Examples of each type are provided along with general reaction equations.
This document is a chemistry exam paper that consists of 7 questions testing knowledge of various chemistry concepts. It provides instructions for candidates on how to answer the questions, including writing in boxes provided and not writing in barred code or grey areas. It also lists the number of marks allocated for each question or part of a question. Finally, it states that the exam paper is made up of 14 printed pages and 2 blank pages.
1. The document describes 6 experiments involving chemical reactions and properties. It includes questions about the experiments and reactions.
2. Experiment 1 involves electrolysis of silver nitrate and copper sulfate solutions. Observations and half reactions are asked about.
3. Experiment 2 involves heating lead(II) carbonate and identifying the gas produced. Calculations of moles of gas are required.
This document provides information about salts in chemistry. It defines a salt as an ionic substance formed by the replacement of hydrogen ions in an acid by metal ions or ammonium ions. Salts consist of cation and anion parts from the base and acid respectively. The document also includes tables and diagrams showing solubility rules for common salts and their reactions with heat. It describes methods for preparing and purifying soluble and insoluble salts, as well as qualitative analysis of salts through observation of physical properties and chemical tests.
This document contains a chemistry document about coordination compounds with questions for practice. It includes:
- Very short answer (1 mark) questions testing definitions and names of coordination compounds.
- Short answer (2 mark) questions requiring explanations and examples of coordination compound concepts.
- Short answer (3 mark) questions requiring explanations, drawings of structures, and applications of coordination compounds using concepts like isomerism, crystal field theory and magnetic properties.
Chemical formula and equation, mol conceptRossita Radzak
1. This document provides information on chemical formulas, equations, mole concept and stoichiometry calculations. It includes examples of writing chemical formulas and balancing equations, as well as mole calculations to determine the number of particles, moles of substances, and masses involved in various chemical reactions.
2. Key concepts covered are the mole, molar mass, molar volume, empirical formulas, and stoichiometric calculations to determine limiting reactants, products formed and reaction yields. Sample problems demonstrate mole calculations for common reactions like metal-acid or carbonate reactions.
3. The document serves as a reference for students to learn essential concepts and skills in writing formulas, balancing equations, and solving a wide range of stoichiometric problems.
Cambridge IGCSE Chemistry 0620 solved past paper . For solved papers for over 10 years along with thousands of resources, join yearly membership : www.smartexamresources.com. USE coupon code: FREEDOM40 to get 40% discount on all products that you purchase
The document discusses rusting of iron and how zinc plates protect iron ships from rusting. It also discusses oxidation states of aluminum and copper in their compounds aluminum oxide and copper(I) oxide. Finally, it describes an experiment using potassium manganate as an oxidation agent and iron as the reducing agent.
This document provides information on naming and writing formulas for inorganic compounds. It begins by discussing binary ionic compounds formed from a metal and nonmetal. It explains that the name of the cation (metal) comes first, followed by the anion (nonmetal) with the "-ide" suffix. Examples of naming compounds of common metals like calcium, magnesium, and sodium are provided. The document then discusses polyatomic ions and compounds containing them. It also covers compounds where the metal forms more than one ion. Finally, it discusses acids and naming compounds containing oxoanions. In summary, the document outlines the system for systematically naming inorganic compounds based on their formulas as well as writing formulas from IUPAC names.
This document contains a mock chemistry test with multiple choice and short answer questions covering various topics:
1) The questions cover topics like duralumin alloys, methods of producing hydrogen chloride, reactions producing copper, addition reactions of bromine with alkenes, IUPAC and common names of organic compounds, isomers, production of chloroform and ethyne.
2) There are also questions about the chief ore of aluminum, its concentration process, electrolytic reduction, neutral oxides, catalysts, drying agents, balanced equations, properties of acids and the Ostwald process.
3) The final questions ask for IUPAC names and to identify muriatic acid and the main ore of iron.
Profiles of Iconic Fashion Personalities.pdfTTop Threads
The fashion industry is dynamic and ever-changing, continuously sculpted by trailblazing visionaries who challenge norms and redefine beauty. This document delves into the profiles of some of the most iconic fashion personalities whose impact has left a lasting impression on the industry. From timeless designers to modern-day influencers, each individual has uniquely woven their thread into the rich fabric of fashion history, contributing to its ongoing evolution.
The Genesis of BriansClub.cm Famous Dark WEb PlatformSabaaSudozai
BriansClub.cm, a famous platform on the dark web, has become one of the most infamous carding marketplaces, specializing in the sale of stolen credit card data.
Brian Fitzsimmons on the Business Strategy and Content Flywheel of Barstool S...Neil Horowitz
On episode 272 of the Digital and Social Media Sports Podcast, Neil chatted with Brian Fitzsimmons, Director of Licensing and Business Development for Barstool Sports.
What follows is a collection of snippets from the podcast. To hear the full interview and more, check out the podcast on all podcast platforms and at www.dsmsports.net
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Presentation by Herman Kienhuis (Curiosity VC) on Investing in AI for ABS Alu...Herman Kienhuis
Presentation by Herman Kienhuis (Curiosity VC) on developments in AI, the venture capital investment landscape and Curiosity VC's approach to investing, at the alumni event of Amsterdam Business School (University of Amsterdam) on June 13, 2024 in Amsterdam.
The Steadfast and Reliable Bull: Taurus Zodiac Signmy Pandit
Explore the steadfast and reliable nature of the Taurus Zodiac Sign. Discover the personality traits, key dates, and horoscope insights that define the determined and practical Taurus, and learn how their grounded nature makes them the anchor of the zodiac.
Discover timeless style with the 2022 Vintage Roman Numerals Men's Ring. Crafted from premium stainless steel, this 6mm wide ring embodies elegance and durability. Perfect as a gift, it seamlessly blends classic Roman numeral detailing with modern sophistication, making it an ideal accessory for any occasion.
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Part 2 Deep Dive: Navigating the 2024 Slowdownjeffkluth1
Introduction
The global retail industry has weathered numerous storms, with the financial crisis of 2008 serving as a poignant reminder of the sector's resilience and adaptability. However, as we navigate the complex landscape of 2024, retailers face a unique set of challenges that demand innovative strategies and a fundamental shift in mindset. This white paper contrasts the impact of the 2008 recession on the retail sector with the current headwinds retailers are grappling with, while offering a comprehensive roadmap for success in this new paradigm.
Industrial Tech SW: Category Renewal and CreationChristian Dahlen
Every industrial revolution has created a new set of categories and a new set of players.
Multiple new technologies have emerged, but Samsara and C3.ai are only two companies which have gone public so far.
Manufacturing startups constitute the largest pipeline share of unicorns and IPO candidates in the SF Bay Area, and software startups dominate in Germany.
How are Lilac French Bulldogs Beauty Charming the World and Capturing Hearts....Lacey Max
“After being the most listed dog breed in the United States for 31
years in a row, the Labrador Retriever has dropped to second place
in the American Kennel Club's annual survey of the country's most
popular canines. The French Bulldog is the new top dog in the
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The APCO Geopolitical Radar - Q3 2024 The Global Operating Environment for Bu...APCO
The Radar reflects input from APCO’s teams located around the world. It distils a host of interconnected events and trends into insights to inform operational and strategic decisions. Issues covered in this edition include:
2. 1 A part of the Periodic table is shown below. a) Name the Russian scientist whose work led to the development of the modern Periodic Table. ___________________________ [1]
3. 1 A part of the Periodic table is shown below. a) Name the Russian scientist whose work led to the development of the modern Periodic Table. Mendeleev (similar spelling accepted) [1]
4. b) Using only the elements shown above name: (i) the most reactive Alkali Metal: ___________________________ [1] (ii) the least reactive Halogen: ___________________________ [1]
5. b) Using only the elements shown above name: (i) the most reactive Alkali Metal: rubidium [1] (ii) the least reactive Halogen: iodine [1]
6. (iii) the least dense Noble Gas: ___________________________ [1] (iv) a semi-metal ___________________________ [1]
7. (iii) the least dense Noble Gas: helium [1] (iv) a semi-metal silicon or germanium [1]
8. (v) a metal of valency 3: ___________________________ [1] (vi) two different elements which can exist as allotropes: ___________________________ [1]
9. (v) a metal of valency 3: aluminium [1] (vi) two different elements which can exist as allotropes: carbon [1] and sulphur [1] (Accept oxygen, phosphorus. Accept symbols for all (b) )
10. c) (i) Complete the table below to show the observations which could be made when the two selected elements react under the conditions shown. [13] Reaction with Magnesium Sulphur Oxygen Water/Steam No reaction Dilute hydrochloric acid
11. c) (i) Complete the table below to show the observations which could be made when the two selected elements react under the conditions shown. [13] Reaction with Magnesium Sulphur Oxygen Burns with (bright) white flame [1]; white [1] solid ash [1] remains Burns with blue flame [1]; pungent choking [1] gas [1] forms Water/Steam Burns in steam with (bright) white flame [1]; white [1] accept white/grey solid [1] remains No reaction Dilute hydrochloric acid Bubbles of colourless [1] gas/heat [1]; magnesium disappears [1] No reaction [1] accept an “X” blank box – no marks
12. (ii) Write balanced symbol equations for those reactions you think occur. _____________________________ _____________________________ _____________________________ __________________________ [8]
13. (ii) Write balanced symbol equations for those reactions you think occur. Mg + 2HCl -> MgCl 2 + H 2 [2] 2Mg + O 2 -> 2MgO [2] Mg + H 2 O -> MgO + H 2 [2] S + O 2 -> SO 2 [2] [1] – Correct symbols used throughout [1] – Correct balancing Accept correct ionic equation
14. 2 The methods used to prepare salts depend on whether the required salt is soluble or insoluble. Zinc sulphate, for example, is soluble while barium sulphate is insoluble.
15. a) (i) Describe in detail how you would prepare a pure dry sample of zinc sulphate crystals in the laboratory starting from solid zinc carbonate and dilute sulphuric acid. ________________________________ ________________________________ ________________________________ ________________________________ ____________________________ [10]
16. a) (i) Describe in detail how you would prepare a pure dry sample of zinc sulphate crystals in the laboratory starting from solid zinc carbonate and dilute sulphuric acid. Place a volume of dilute sulphuric acid in a beaker [1]. Warm acid [1]. Add/react/mix [1] zinc carbonate with stirring [1] until o more solid dissolves/no more gas is given off [1]. Filter [1] the mixture into an evaporating basin/beaker/crystallising dish [1]. Heat [1] the solution to reduce the volume [1]. Allow to cool [1], filter [1] decant off the crystals, desiccator/low temperature oven [1]. Do not accept – heat to dryness. (Max [10]/[13])
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19. b) (i) Describe in detail how you would prepare a pure dry sample of barium sulphate in the laboratory starting with solutions of barium chloride and magnesium sulphate. ____________________________ ____________________________ ____________________________ ____________________________ _________________________ [5]
20. b) (i) Describe in detail how you would prepare a pure dry sample of barium sulphate in the laboratory starting with solutions of barium chloride and magnesium sulphate. Mix [1] the solutions of barium chloride and magnesium sulphate. A white [1] precipitate [1] formed. Filter [1] the mixture, rinse/wash with cold water [1] and dry in an oven [1]. Accept suitable drying method. (Max [5]/[6])
21. (ii) Give a balanced symbol equation for the preparation of barium sulphate. ________________________ [2] (iii) Give the names of two other compounds which could be used to make barium sulphate instead of barium chloride and magnesium sulphate. ________________________ [2]
22. (ii) Give a balanced symbol equation for the preparation of barium sulphate. BaCl 2 + MgSO 4 -> BaSO 4 + MgCl 2 Ba 2+ + SO 4 2- -> BaSO 4 [2] (iii) Give the names of two other compounds which could be used to make barium sulphate instead of barium chloride and magnesium sulphate . Barium nitrate [1] Any soluble sulphate [1] accept correct formula.
23. 3 Electrolysis plays an important part in extracting some metals from their ores and in purifying others. a) Define what is meant by the term electrolysis. _________________________________ ______________________________ [2] b) Name one metal which is obtained from its ore by electrolysis. ______________________________ [1]
24. 3 Electrolysis plays an important part in extracting some metals from their ores and in purifying others. a) Define what is meant by the term electrolysis. Electrolysis is decomposition [1] of a substance using an electric current [1] b) Name one metal which is obtained from its ore by electrolysis. Any reactive metal at the top of the reactivity series. Specification refers to aluminium [1]; but could accept sodium, potassium, calcium, magnesium, zinc.
25. c) Draw a labelled diagram of simple laboratory apparatus which shows how copper can be purified .
26. c) Draw a labelled diagram of simple laboratory apparatus which shows how copper can be purified . Complete circuit (1) (1) (1) Electrolyte (1) (1) (1) Accept any soluble copper salt
27. d) Write balanced , ionic equations to show the electrode reactions which occur when copper is purified. (i) At the anode ________________ [2] (ii) At the cathode ______________ [2]
28. d) Write balanced , ionic equations to show the electrode reactions which occur when copper is purified . (i) At the anode Cu -> Cu 2+ + 2e - [2] (ii) At the cathode Cu 2+ + 2e - -> Cu [2]
29. e) Which particles are responsible for the conductivity of electricity in: (i) metals? ____________________ [1] (ii) electrolytes? ________________ [1]
30. e) Which particles are responsible for the conductivity of electricity in: (i) metals? Electrons [1] (ii) electrolytes? Ions [1]
31. f) Give two uses of copper metal apart from its use in electrical wiring. _____________________________ ___________________________ [2]
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33. g) The electrolysis of dilute sulphuric acid using inert electrodes produces two gases as products. (i) Name a material which could be used as the electrodes in this experiment. ___________________________ [1] (ii) Name the product formed at the anode _______________ cathode _____________ [2]
37. g) The electrolysis of dilute sulphuric acid using inert electrodes produces two gases as products. (i) Name a material which could be used as the electrodes in this experiment. Graphite (or platinum) [1] (ii) Name the product formed at the anode oxygen [1] accept O 2 cathode hydrogen [1] accept H 2
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40. 4 a) What term is used to describe a reaction which gives out heat? __________________________ [1]
41. 4 a) What term is used to describe a reaction which gives out heat? Exothermic [1]
42. b) When drops of water are added to anhydrous copper sulphate heat is given out. (i) Describe what would be observed during this reaction. _________________________________ ______________________________ [2] (ii) The addition of water to anhydrous copper sulphate is called ______________________________ [1]
43. b) When drops of water are added to anhydrous copper sulphate heat is given out. (i) Describe what would be observed during this reaction. The white [1] solid would turn blue [1] (ii) The addition of water to anhydrous copper sulphate is called Hydration [1]
44. c) Heat is also given out during the reaction of sodium hydroxide with hydrochloric acid. (i) Give a balanced symbol equation for this reaction. ______________________________ [2] (ii) The reaction of an acid with an alkali is called ________________________ [1]
45. c) Heat is also given out during the reaction of sodium hydroxide with hydrochloric acid. (i) Give a balanced symbol equation for this reaction. NaOH + HCl -> NaCl + H 2 O [2] (ii) The reaction of an acid with an alkali is called Neutralisation [1]
46. d) The redox reaction of zinc with copper sulphate solution also gives out heat. (i) Describe what would be observed during this reaction. _________________________________ ______________________________ [2] (ii) Give a balanced symbol equation for this equation. _____________________ [2]
47. d) The redox reaction of zinc with copper sulphate solution also gives out heat. (i) Describe what would be observed during this reaction. The silvery/grey[1] zinc would become coated with red/brown[1] copper metal. The blue [1] solution fades / colourless / zinc disappears / bubbles[1] / green[1]. Max [2] (ii) Give a balanced symbol equation for this equation. Zn + CuSO 4 -> ZnSO 4 + Cu or Zn + Cu 2+ -> Zn 2+ + Cu [2]
48. (iii) The reaction of zinc with copper sulphate solution is an example of ______________________________ [1] (iv) Explain this redox reaction in terms of electron transfer. _________________________________ _________________________________ _________________________________ ______________________________ [5]
49. (iii) The reaction of zinc with copper sulphate solution is an example of Displacement [1] (iv) Explain this redox reaction in terms of electron transfer. The zinc has lost electrons [1] and is therefore oxidised [1]. The copper ions have gained electrons [1] and are therefore reduced [1]. Redox is reduction and oxidation taking place together [1]
50. To obtain full marks in this question, you must show your working out 5 When washing soda crystals, Na 2 CO 3 .10H 2 O, are left exposed to the atmosphere they lose water of crystallisation. The longer they are left, the more water is lost. The amount of water of crystallisation remaining can be found in two ways: either by heating to remove all the remaining water or by titration.
51. 5a) 2.675g of a sample of crystals were heated to constant mass. The mass of the residue was 1.325g. (i) Why was the sample heated to constant mass? ______________________________ [1] (ii) Calculate the number of moles of anhydrous sodium carbonate in the residue. ______________________________ [2]
52. Consequential marking applies throughout 5a) 2.675g of a sample of crystals were heated to constant mass. The mass of the residue was 1.325g. (i) Why was the sample heated to constant mass ? To ensure that all water [1] (of crystallisation) was lost. (ii) Calculate the number of moles of anhydrous sodium carbonate in the residue. Na 2 CO 3 = 1.325 = 0.0125 [1] 106 [1]
53. (iii) Calculate the mass of water lost and from this calculate the number of moles of water lost. _________________________________ ______________________________ [3] (iv) From your answers to part (a)(ii) and (iii) above, calculate the value of x in the formula Na 2 CO 3 .xH 2 O. _________________________________ ______________________________ [2]
54. (iii) Calculate the mass of water lost and from this calculate the number of moles of water lost. Mass of water lost = (2.765-1.325) g = 1.35g [1] Number of moles lost = 1.35 = 0.075 [1] 18 [1] (iv) From your answers to part (a)(ii) and (iii) above, calculate the value of x in the formula Na 2 CO 3 .xH 2 O. Ratio of moles Na 2 CO 3 : H 2 O 0.0125 : 0.075 [1] 1 : 6 [1]
55. b) 1.775g of a different sample of washing soda was dissolved in distilled water and made up of a total volume of 250cm 3 . 25.0cm 3 of this solution were titrated with 0.08 mol/dm 3 (moles per litre) nitric acid. 31.25cm 3 of acid were required. The equation for the reaction is: Na 2 CO 3 + 2HNO 3 -> 2NaNO 3 + H 2 O + CO 2 (i) Calculate the number of moles of nitric acid used in the titration. ______________________________________ ___________________________________ [2]
56. b) 1.775g of a different sample of washing soda was dissolved in distilled water and made up of a total volume of 250cm 3 . 25.0cm 3 of this solution were titrated with 0.08 mol/dm 3 (moles per litre) nitric acid. 31.25cm 3 of acid were required. The equation for the reaction is: Na 2 CO 3 + 2HNO 3 -> 2NaNO 3 + H 2 O + CO 2 (i) Calculate the number of moles of nitric acid used in the titration. Number of moles HNO 3 = 31.25 x 0.08 1000[1] = 2.5 x 10 -3
57. (ii) Calculate the number of moles of sodium carbonate present in the 25.0cm 3 sample. _______________________________________ ____________________________________[2] (iii) Calculate the number of moles of sodium carbonate present in 250cm 3 of solution. _______________________________________ ____________________________________[2]
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61. c) Sodium hydrogencarbonate decomposes when it is heated into sodium carbonate according to the equation: 2NaHCO 3 -> NaCO 3 + H 2 O + CO 2 1.68g of sodium hydrogencarbonate were placed in a test tube and heated in a Bunsen flame for some time. (i) Calculate the number of moles of sodium hydrogencarbonate used. _______________________________________ ____________________________________ [2]
62. c) Sodium hydrogencarbonate decomposes when it is heated into sodium carbonate according to the equation: 2NaHCO 3 -> NaCO 3 + H 2 O + CO 2 1.68g of sodium hydrogencarbonate were placed in a test tube and heated in a Bunsen flame for some time. (i) Calculate the number of moles of sodium hydrogencarbonate used. Number of moles NaHCO 3 = 1.68 84 [1] = 0.02 [1]
63. (ii) Calculate the number of moles of sodium carbonate formed. ___________________________________ ________________________________ [2] (iii) Calculate the mass of sodium carbonate expected to be formed. ___________________________________ ________________________________ [2]
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65. (iv) Calculate the volume of carbon dioxide produced in this experiment. (1 mole of gas occupies 24dm 3 at room temperature and pressure) _____________________________________ __________________________________ [2]
66. (iv) Calculate the volume of carbon dioxide produced in this experiment. (1 mole of gas occupies 24dm 3 at room temperature and pressure) Mole ratio NaHCO 3 : CO 2 2 : 1 [1] Number of moles CO 3 expected = 0.02 = 0.01 [1] 2 Volume of CO 3 expected = 24 x 0.01 = 0.24dm 3 [1] or 240cm 3