In the early version of the periodic table (by Newlands and then Mendeleev), how were the elements arranged?
|
|
- Branden Harrison
- 6 years ago
- Views:
Transcription
1 Page 1 In the early version of the periodic table (by Newlands and then Mendeleev), how were the elements arranged? What can we say about the elements in the same group of the periodic table? Why is the periodic table called the periodic table? What was the problem with the early periodic table, where elements were arranged in order of atomic weight? When Mendeleev proposed his early periodic table, what problem did he highlight? How did Mendeleev adjust his periodic table to take into account the problems he identified? How are the elements arranged in the modern periodic table? Which group was not featured on the early periodic table? What can we say about the electronic structure of elements in the same group of the periodic table? What do we call the elements in group 1 of the periodic table? What can we say about the density of the elements in group 1 (the alkali metals)? How do group 1 (alkali metals) react with non-metals?
2 Page 2 Elements in the same group of the periodic table have similar chemical and physical properties. In the early version of the periodic table (by Newlands and then Mendeleev), the elements were arranged by atomic weight. In the early periodic table, where elements were arranged in order of atomic weight, some elements were clearly in the wrong group (based on their properties). The periodic table is called the periodic table because elements with similar properties occur at regular intervals. Mendeleev sometimes switched the order of the elements if they were clearly in the wrong group. He also left gaps for elements which he realised had not been discovered. When Mendeleev proposed his early periodic table, he realised that some elements had not been discovered. Group 0 was not featured on the early periodic table as the group 0 (noble gases) had not been discovered In the modern periodic table, elements are arranged in order of atomic (proton) number. Now, all the elements were in the appropriate groups. Elements in group 1 of the periodic table are called the alkali metals. Group 1 (alkali metals) react with nonmetals to form ionic compounds. The alkali metal ion has a charge of +1. The compounds produced are white solids that dissolve in water, forming colourless solutions. Elements in the same group of the periodic table have the same number of electrons in their outer energy level (apart from group 0, where helium has 2 and the rest have 8). All of the elements in group 1 (alkali metals) are metals with low density (Li, Na, K are less dense than water).
3 Page 3 How do group 1 (alkali) metals react with water? What happens as we move down group 1, in terms of: reactivity of the elements melting and boiling points What can we say about transition metals compared to the metals in group 1. State three facts about transition metals. What do we call the elements in group 7? How do the halogens react with metals? What happens as we move down group 7, in terms of: reactivity of the elements melting and boiling points Complete this sentence: A more reactive halogen can.. a less reactive halogen from an aqueous solution of its salt What happens in the following reaction? chlorine + lithium bromide What happens in the following reaction? chlorine + lithium fluoride Explain why group 1 (alkali) metals become more reactive as we move down the group. Explain why group 7 elements (halogens) become less reactive as we move down the group.
4 Page 4 As we move down group 1, The elements get more reactive The melting and boiling points decrease Group 1 (alkali) metals react with water releasing hydrogen. They form hydroxides which dissolve in water, forming an alkaline solution. Many transition metals Can have ions with different charges Form coloured compounds Are useful as catalysts Compared to group 1 metals, transition metals: Are denser Have higher melting points (apart from mercury) Are stronger and harder Are much less reactive Do not react as vigorously with water and oxygen Halogens react with metals to form ionic compounds. The halogen ion (now called a halide) has a charge of -1. Elements in group 7 are called the halogens. A more reactive halogen can displace a less reactive halogen from an aqueous solution of its salt As we move down group 7, the elements get less reactive the melting and boiling points increase chlorine + lithium fluoride chlorine + lithium fluoride chlorine + lithium bromide bromine + lithium chloride Chlorine is less reactive than fluorine so it cannot displace the fluorine from the lithium fluoride. Chlorine is more reactive than bromine so it displaced the bromine from the lithium bromide. Group 7 elements (halogens) get less reactive as we move down the group because an electron is less easily gained into the outer energy level. The outer electron is further from the nucleus. Internal energy levels shield the outer electron from the nucleus. Group 1 (alkali) metals get more reactive as we move down the group because the outer electron is more easily lost. The outer electron is further from the nucleus. Internal energy levels shield the outer electron from the nucleus.
5 Page 5 How can we determine the hardness of a sample of water? How do soapless detergents react with hard water? What makes hard water hard? How is hard water formed? What is meant by temporary hard water? How can we tell the difference between permanent hard water and temporary hard water? How can hard water cost us money? What are the benefits of hard water? How can we soften hard water using sodium carbonate? How can we soften water using a water softener? State the three stages of preparing drinking water. Water filters contain carbon, silver and ion exchange resins. Describe the functions of these.
6 Page 6 Soapless detergents do not form a scum with hard water. They form a lather. Hard water forms a scum (rather than a lather) with soap so if a sample of water is very hard, it will need more soap to form a lather. The amount of soap needed to form a lather indicates the hardness of the water. When water flows over rocks containing calcium or magnesium compounds, these can dissolve in the water, making it hard. Hard water is hard because it contains dissolved compounds of calcium or magnesium. If we boil temporary hard water, it becomes soft. However, boiling permanent hard water has no effect on the hardness. Temporary hard water contains hydrogencarbonate ions (HCO3 - ). If we boil this water, these form carbonate ions. The carbonate ions react with the calcium ions / magnesium ions, forming a precipitate. This removes the calcium ions / magnesium ions from solution which makes the water soft. Hard water can contain calcium ions. These help us to develop strong bones and teeth. Calcium ions can also decrease the risk of heart disease. Hard water requires more soap to develop a lather. Also when temporary hard water is heated it forms scale (precipitate of calcium carbonate or magnesium carbonate). Scale reduces the efficiency of heating systems and kettles. Water softeners carry out ion-exchange. They contain either hydrogen ions or sodium ions. When hard water passes through, the calcium ions / magnesium ions in the water are switched for the hydrogen ions / sodium ions, making the water soft. If we add sodium carbonate to hard water, the carbonate ions react with the calcium ions /magnesium ions. This forms a precipitate, removing these ions from solution. This makes the water soft. Carbon removes impurities such as chlorine. Silver kills microbes. Ion exchange resins make hard water soft. Select a source of water e.g. an unpolluted river. Filter out any solids. Add chlorine to sterilise the water (kill microbes).
7 Page 7 Why is fluoride added to drinking water and why do some people object to this? How can completely pure water be produced? Which equation can we use to determine the amount of heat energy released / taken in during a reaction. We can measure the energy released from burning a fuel by using a calorimeter. State two issues with this. When we measure the energy change of a chemical reaction, why should we use a polystyrene cup rather than a glass beaker? Draw an energy level diagram for an exothermic reaction. Label the activation energy. Draw an energy level diagram for an endothermic reaction. Label the activation energy. Describe the bond energy changes that take place during a chemical reaction. What can we say about the bond energy changes taking place in an endothermic reaction? What can we say about the bond energy changes taking place in an exothermic reaction? How do catalysts speed up chemical reactions? Draw an energy level diagram showing the effect of a catalyst on a chemical reaction.
8 Page 8 Completely pure water can be produced by distillation. However, this requires a great deal of energy and is therefore extremely expensive. Adding fluoride to drinking water improves dental health. However, some people object as it prevents people from choosing whether they want to drink water with fluoride. 1. A great deal of heat energy is simply passed into the air, rather than the water in the calorimeter. 2. We should use a metal calorimeter rather than a glass beaker as metal is a better conductor of heat than glass. Q = m c ΔT Q = energy (J) m = mass (g) c = specific heat capacity (J/g/ o C) ΔT = temperature change ( o C) Polystyrene is a better insulator than glass. If we used a glass beaker then heat energy could pass in or out of the solution, giving us an incorrect reading. Breaking bonds requires energy (endothermic). Making bonds releases energy (exothermic). In an exothermic reaction, the energy released by forming new bonds is greater than the energy needed to break existing bonds. In an endothermic reaction, the energy needed to break existing bonds is greater than the energy released from forming new bonds. Catalysts provide a different pathway for a chemical reaction with a lower activation energy.
9 Page 9 State the equation for the combustion of hydrogen in engines. What happens when hydrogen is used in a fuel cell. State the advantages and disadvantages of using hydrogen in a fuel cell compared to combusting hydrogen in an engine. How can we test for calcium and magnesium ions by using sodium hydroxide solution? State the flame test results for the following metal ions: lithium sodium potassium calcium barium How can we test for aluminium ions by using sodium hydroxide solution? State the colours of the precipitates formed when the following ions react with sodium hydroxide solution: copper (II) iron (II) iron (III) How can we test for a metal carbonate (eg sodium carbonate)? How can we test for halide ions? What are the colours of the positive results? Describe how we can test for sulfate ions? Describe how we can use titration to determine the concentration of an acid or alkali. State the raw materials for producing ammonia by the Haber process and describe their sources.
10 Page 10 In a fuel cell, hydrogen reacts with oxygen to make water. This also produces electricity. The electricity can be used to power a vehicle. hydrogen + oxygen water (+energy) lithium = crimson sodium = yellow potassium = lilac calcium = red barium = green Hydrogen fuel cells are more efficient than combusting hydrogen. The water produced from a hydrogen fuel cell can be used for drinking water (eg in a space station). Hydrogen fuel cells require expensive catalysts. Aluminium ions will produce a white precipitate when reacted with sodium hydroxide solution. If we add excess sodium hydroxide solution, the white precipitate will redissolve. Both calcium and magnesium ions will produce a white precipitate when reacted with sodium hydroxide solution. First we add any dilute acid. Bubbles of gas will be produced. If we pass the gas through limewater and the limewater turns cloudy, the gas is carbon dioxide. This tells us that we had a metal carbonate. copper (II): blue precipitate iron (II): green precipitate iron (III): brown precipitate We can test for sulfate ions by adding barium chloride solution in the presence of hydrochloric acid. Sulfate ions will produce a white precipitate. We can test for halide ions by adding silver nitrate solution in the presence of dilute nitric acid. chloride ions = white precipitate bromide ions = cream precipitate iodide ions = yellow precipitate Nitrogen is extracted from the air. Hydrogen is extracted from natural gas (or by electrolysis of water). Fill a burette with the acid Use a pipette to measure a known volume of alkali into a conical flask Place the conical flask onto a white tile Add indicator to the alkali (eg phenolphthalein) Gradually add the acid, while swirling the alkali Add the acid in drops as you approach the endpoint Record the final volume of acid needed
11 Page 11 State the conditions for producing ammonia by the Haber process. What is meant when a reversible reaction reaches equilibrium? What happens to the yield of an exothermic (reversible) reaction if we increase the temperature? What happens to the yield of an endothermic (reversible) reaction if we increase the temperature? What happens to the yield of an exothermic (reversible) reaction if we decrease the temperature? What happens to the yield of an endothermic (reversible) reaction if we decrease the temperature? What happens to a gaseous reversible reaction if we increase the pressure? Describe how the conditions of the Haber process are a compromise. State the structural formula of methanol. State the structural formula of ethanol. State the structural formula of propanol. What is the functional group of the alcohols?
12 Page 12 When a reversible reaction reaches equilibrium, both the forward and reverse reactions are taking place at the same rate. If we increase the temperature of an endothermic (reversible) reaction, the yield increases. 200 atmospheres pressure 450 o C Iron catalyst The ammonia is liquified by cooling and removed Unreacted gases are recycled back over the catalyst If we increase the temperature of an exothermic (reversible) reaction, the yield falls. If we decrease the temperature of an endothermic (reversible) reaction, the yield falls. If we decrease the temperature of an exothermic (reversible) reaction, the yield increases. We can favour the forward reaction by Increasing the pressure as there are fewer molecules on the right hand side Using a relatively low temperature as the forward reaction is exothermic However, a low temperature makes the reaction rate slow (ie a compromise). Using an iron catalyst increases the rate. If we increase the pressure of a gaseous reversible reaction, the position of the equilibrium shifts to the side with the fewest molecules. Ethanol has the following structural formula CH3CH2OH Methanol has the following structural formula CH3OH The functional group of the alcohols is OH Propanol has the following structural formula CH3CH2CH2OH
13 Page 13 Draw the structural formula of methanol. Draw the structural formula of ethanol. Draw the structural formula of propanol. State three uses of alcohols. What happens when alcohols are dissolved in water? What is produced when alcohols are reacted with sodium? Alcohols burn in air. True or false? How can alcohols be oxidised? What is vinegar and how is it produced? What is the functional group of carboxylic acids? What is the structural formula of methanoic acid? What is the structural formula of ethanoic acid?
14 Page 14 Ethanol Methanol Alcohols are used as fuels and solvents. Ethanol is found in alcoholic drinks. Propanol When alcohols are reacted with sodium, hydrogen gas is produced. When alcohols are dissolved in water, they form a neutral solution. Alcohols can be oxidised using chemical oxidising agents or by bacteria. When alcohols are oxidised, they form carboxylic acids. True: alcohols burn in air. The functional group of carboxylic acids is COOH Vinegar is a dilute solution of ethanoic acid in water. It is made by allowing bacteria to oxidise ethanol. The structural formula of ethanoic acid is CH3COOH The structural formula of methanoic acid is HCOOH
15 Page 15 What is the structural formula of propanoic acid? What is the displayed formula of methanoic acid? What is the displayed formula of ethanoic acid? What is the displayed formula of propanoic acid? What type of solution is produced when a carboxylic acid is dissolved in water? What is produced when carboxylic acids react with a metal carbonate. What is produced when carboxylic acids react with alcohols in the presence of an acid catalyst (eg sulfuric acid)? Carboxylic acids are weak acids. What does this mean? Why are esters used as flavourings and perfumes? What is the ester functional group? Draw the structure of the ester ethyl ethanoate. How is ethyl ethanoate produced?
16 Page 16 Methanoic acid The structural formula of propanoic acid is CH3CH2COOH Propanoic acid Ethanoic acid Carboxylic acids react with metal carbonates to produce carbon dioxide. When dissolved in water, carboxylic acids form an acidic solution. Weak acids (such as carboxylic acids) do not ionise completely when dissolved in water. This means that they have a higher ph (eg ph 5) than strong acids (which could be ph 1) when at the same concentration. In the presence of an acid catalyst (eg sulfuric acid), carboxylic acids react with alcohols to produce an ester. The ester functional group is: COO Esters are volatile (easily evaporate). They also have distinctive smells. Ethyl ethanoate is produced by reacting ethanol and ethanoic acid in the presence of an acid catalyst (eg sulfuric acid).
The early periodic table
3.5 Unit 3 Chemistry 3 Throughout this unit candidates will be expected to write word equations for reactions specified. Higher tier candidates will also be expected to write and balance symbol equations
More informationGCSE Chemistry 3 Summary Questions
GCSE Chemistry 3 Summary Questions Q1 Q2 Q3 Q4 Q5 Q6 Q7 Q8 Q9 Q10 Q11 Q12 Q13 Q14 Q15 Q16 Q17 Q18 Q19 C3.1.1 The early Periodic table (p73) Explain Newlands law of Octaves. Explain why Newlands law was
More informationChemistry CH3FP Unit Chemistry C3 Written Paper Monday 20 May pm to 2.30 pm For this paper you must have: Time allowed Instructions all
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Question Mark General Certificate of Secondary Education Foundation Tier June 2013 1 2 Chemistry
More informationCH3HP. (Jun15CH3HP01) General Certificate of Secondary Education Higher Tier June Unit Chemistry C3 TOTAL. Time allowed 1 hour
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Question Mark Chemistry Unit Chemistry C3 Thursday 14 May 2015 For this paper you must have:
More informationCH3FP. (Jun15CH3FP01) General Certificate of Secondary Education Foundation Tier June Unit Chemistry C3 PMT. Time allowed 1 hour TOTAL
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Question Mark A Chemistry Unit Chemistry C3 Thursday 14 May 2015 For this paper you must have:
More informationC3 TITRATIONS. Describe To recall facts, events or processes and give an ordered account. Connectives: firstly, next, finally,
C3 TITRATIONS Describe how a student could find the volume of hydrochloric acid that reacts with a known volume of sodium hydroxide solution. Include any measurements the student should make. (6) Pipette,
More informationFurther Additional Science
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Question Mark A Further Additional Science Unit 2 Chemistry C3 Thursday 14 May 2015 For this
More informationWJEC England GCSE Chemistry. Topic 4: The periodic table and properties of elements. Notes. (Content in bold is for Higher Tier only)
WJEC England GCSE Chemistry Topic 4: The periodic table and properties of elements Notes (Content in bold is for Higher Tier only) Reactions of elements Elements react in order to gain a stable arrangement
More informationGCSE Science Schemes of Work Chemistry
GCSE Science Schemes of Work Chemistry Unit 3: Chemistry Choose option *The suggested timings relate to the learning outcomes rather than to the activities. Communication C3.1 The periodic table. The modern
More informationQ1. Ammonia is used in the production of fertilisers. The flow diagram shows the main stages in the manufacture of ammonia.
Q1. Ammonia is used in the production of fertilisers. The flow diagram shows the main stages in the manufacture of ammonia. Study the flow diagram and then answer the questions. (a) What is the purpose
More informationC3 Revision Pack (Please keep this pack with you)
Name: C3 Revision Pack (Please keep this pack with you) Follow all the steps below... 1) Practice all the maths and working scientifically questions PRACTICE ALL THESE QUESTIONS! Maths and Science Skills
More information4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
More informationWhat are the two main steps used to treat water from reservoirs? (4)
C3b QUESTIONS 1. Water in Britain is taken from reservoirs to use as drinking water. KatieJonesPhotography/iStock/Thinkstock (a) What are the two main steps used to treat water from reservoirs? Give one
More informationAtoms, Elements, Atoms, Elements, Compounds and Mixtures. Compounds and Mixtures. Atoms and the Periodic Table. Atoms and the.
Atoms, Elements, Compounds and Mixtures Explain how fractional distillation can be used to separate a mixture. 1 Atoms, Elements, Compounds and Mixtures Fractional distillation is used to separate components
More informationSpecimen Paper. Further Additional Science Unit 2 Chemistry 3 [CODE] Time allowed 60 minutes
Centre Number Surname Candidate Number Specimen Paper For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Secondary Education Foundation Tier Question 1 Mark Further
More informationChapter 10 Organic Reactions
Chapter 0 Organic Reactions Name: Class: Date: Time: 85 minutes Marks: 85 marks Comments: Page of 32 This question is about organic compounds. (a) Ethanol burns in air. Use the correct answer from the
More informationUnit 4: Chemical Changes (Higher Content)
Metals react with oxygen to produce metal oxides. E.g. Copper + Oxygen > Copper Oxide The reactions are oxidation reactions because the metals gain oxygen. Reactivity of Metals Metal Extraction Metals
More information4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
More informationYEAR 10- Chemistry Term 1 plan
YEAR 10- Chemistry Term 1 plan 2016-2017 Week Topic Learning outcomes 1 1. The particulate nature of matter State the distinguishing properties of solids, liquids and gases. Describe the structure of solids,
More information4.4.1 Reactivity of metals Metal oxides The reactivity series. Key opportunities for skills development.
4.4 Chemical changes Understanding of chemical changes began when people began experimenting with chemical reactions in a systematic way and organising their results logically. Knowing about these different
More informationYear 8 Chemistry Knowledge Organiser Topic 1: Periodic Table
KPI 1.1: Identify, with reasons, differences between atoms, elements and compounds Key Terms Element Mixture Compound Elements Definitions A substance that contains only one type of atom A substance that
More informationEdexcel Chemistry Checklist
Topic 1. Key concepts in chemistry Video: Developing the atomic model Describe how and why the atomic model has changed over time. Describe the difference between the plum-pudding model of the atom and
More informationOCR Chemistry Checklist
Topic 1. Particles Video: The Particle Model Describe the main features of the particle model in terms of states of matter. Explain in terms of the particle model the distinction between physical changes
More informationQ1. Methane and oxygen react together to produce carbon dioxide and water.
Chemistry C3 Higher Questions Part 2 Q1. Methane and oxygen react together to produce carbon dioxide and water. The methane gas will not burn in oxygen until a flame is applied, but once lit it continues
More informationAdditional Science Chemistry
Additional Science Chemistry C2 Core Questions and Keywords and Definitions Question How did Mendeleev arrange the elements known at the time into a periodic table? How did Mendeleev use his table? Where
More informationOCR Chemistry Checklist
Topic 1. Particles Video: The Particle Model Describe the main features of the particle model in terms of states of matter. Explain in terms of the particle model the distinction between physical changes
More informationGCSE OCR Revision Chemistry. GCSE OCR Revision Chemistry. GCSE OCR Revision Chemistry. Bonding. GCSE OCR Revision Chemistry
Particle Model and Atomic Structure The following symbols describe two different substances. Deduce all the information you can from these symbols. 13 C 12 6 6 C 1 Particle Model and Atomic Structure The
More informationOrchard School. New Document 1 Name: Class: Date: 129 minutes. Time: 126 marks. Marks: Comments: Page 1
New Document Name: Class: Date: Time: Marks: 29 minutes 26 marks Comments: Page Q. The ph scale is a measure of the acidity or alkalinity of a solution. (a) Solution Draw one line from each solution to
More informationEdexcel Chemistry Checklist
Topic 1. Key concepts in chemistry Video: Atomic Structure Recall the different charges of the particles that make up an atom. Describe why atoms have no overall charge. Use the periodic table to identify
More informationEdexcel Chemistry Checklist
Topic 1. Key concepts in chemistry Video: Developing the atomic model Describe how and why the atomic model has changed over time. Describe the difference between the plum-pudding model of the atom and
More informationThe table shows the results of some tests carried out on three solutions, A, B and C. Hydrochloric acid is added. Solution
1 Chemical tests can be used to identify compounds. The table shows the results of some tests carried out on three solutions, A, B and C. Solution Flame Test Hydrochloric acid is added Sodium hydroxide
More informationDraw one line from each solution to the ph value of the solution. Solution ph value of the solution
1 The ph scale is a measure of the acidity or alkalinity of a solution. (a) Draw one line from each solution to the ph value of the solution. Solution ph value of the solution 5 Acid 7 9 Neutral 11 13
More information5.4 Chemical changes Reactivity of metals Metal oxides The reactivity series. Key opportunities for skills development
5.4 Chemical changes Understanding of chemical changes began when people began experimenting with chemical reactions in a systematic way and organising their results logically. Knowing about these different
More informationPaper Atomic structure and the periodic table
Paper 1 4.1 Atomic structure and the periodic table 4.1.1 A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes Use the names and symbols of the first 20 elements in
More informationWrite down everything that the word equation tells you about the reaction (Total 4 marks)
Q1. Here is a word equation for a chemical reaction. copper oxide + sulphuric acid copper sulphate + water Write down everything that the word equation tells you about the reaction.......... (Total 4 marks)
More informationOrganic Chemistry. Alkanes are hydrocarbons in which the carbon atoms are joined by single covalent bonds.
Organic Chemistry Organic compounds: The branch of chemistry which deals with the study of carbon compounds is called organic chemistry. Catenation: The carbon atom has a property to undergo self linking
More informationBoardworks GCSE Separate Sciences: Chemistry
Boardworks GCSE Separate Sciences: Contents Guide Boardworks GCSE Separate Sciences: CFCs and Alcohols 51 slides 21 Flash activities What are CFCs? Introducing CFCs Naming CFCs Properties and uses of CFCs
More informationQualitative Analysis is where you find out what type of substance you have present.
C3 Revision C3.1 Water Testing Qualitative Analysis is where you find out what type of substance you have present. Quantitative Analysis is when you deduce the amount of unknown sample you have. Water
More informationSummer revision calculations for AS chemists September 2016
Summer revision calculations for AS chemists September 206 Q.Dilute nitric acid reacts with potassium hydroxide solution. The equation for the reaction is: HNO 3 + KOH KNO 3 + H 2O A student investigated
More informationName: New Document 1. Class: Date:
New Document 1 Name: Class: Date: Atomic Structure Q1. The figure below shows magnesium burning in air. Charles D Winters/Science Photo Library (a) Look at the figure above. How can you tell that a chemical
More informationEXPERIMENTS. Testing products of combustion: Reducing Copper(III) Oxide to Copper. Page 4
APPARATUS Page 2 APPARATUS Page 3 Reducing Copper(III) Oxide to Copper EXPERIMENTS Page 4 Testing products of combustion: EXPERIMENTS Showing that oxygen and water is needed for rusting iron Page 5 Showing
More informationUnit C1: Chemistry in our world Page 1 of 5
Unit C1: Chemistry in our world Page 1 of 5 Lesson Specification learning outcomes Edexcel 360 Science Specification match Edexcel 360 Science GCSE Science Students Book page reference Additional information
More informationMendeleev arranged the elements in order of their atomic mass (atomic weight).
1 In 1869 there were 60 known elements. Mendeleev arranged the elements in order of their atomic mass (atomic weight). He realised that elements with similar properties occurred at regular intervals. (a)
More informationChemical measurements QuestionIT
Chemical measurements QuestionIT 1. What is the law of conservation of mass? Mass of reactants = mass products. 2. Why might some reactions appear to show a change in mass? A reactant or a product is a
More informationCHY3F. (Jun10CHY3F01) General Certificate of Secondary Education Foundation Tier June Unit Chemistry C3 TOTAL. Time allowed 45 minutes
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Question Mark General Certificate of Secondary Education Foundation Tier June 2010 1 2 Chemistry
More informationREVISION CARDS. Chemistry C2. Modified 09/12/2015 (PB)
REVISION CARDS Chemistry C2 www.chemistryinfo.co.uk Modified 09/12/2015 (PB) INDEX 3 Periodic table 4 Structure of the atom 5 Relative Atomic Mass 6 Electron shells 7 Ions 8 Ionic compounds 9 Solubility
More informationA level Chemistry Preparation Work
A level Chemistry Preparation Work This booklet is designed to help you prepare for you re A level studies in chemistry. Tasks have been selected to improve your grounding in key skills and concepts that
More informationFor the element X in the ionic compound MX, explain the meaning of the term oxidation state.
1. (a) By referring to electrons, explain the meaning of the term oxidising agent.... For the element X in the ionic compound MX, explain the meaning of the term oxidation state.... (c) Complete the table
More informationSeparate Science: Chemistry Paper 1. Knowledge Organisers. Chemistry Paper 1 17 th May AM 1h 45min. Atomic Structure The Periodic Table
Separate Science: Chemistry Paper 1 Chemistry Paper 1 17 th May AM 1h 45min Topics in the Paper: C1 C2 Atomic Structure The Periodic Table Knowledge Organisers C3 C4 C5 C6 C7 Structure and Bonding Chemical
More informationPage 2. Q1.This question is about mixtures and analysis. Which two substances are mixtures? Tick two boxes. Air. Carbon dioxide.
Q1.This question is about mixtures and analysis. (a) Which two substances are mixtures? Tick two boxes. Air Carbon dioxide Graphite Sodium Chloride Steel (2) (b) Draw one line from each context to the
More informationElectrodes are normally made out of inert (unreactive) materials. Graphite and platinum are common electrode materials.
Electrolysis Electrolysis is using an electric current to break up an ionic compound to form elements. Covalent compounds can t be split up by electrolysis. Terms used in electrolysis: Electrolyte - the
More informationDushan [δβ] BOODHENA 1
CHEMISTRY SUMMARY FOR THE FORM 3 NATIONAL ASSESSMENT 1. Define the term element. An element is a pure substance that cannot be broken down into simpler substances by any ordinary chemical process. 2. Define
More informationAQA Chemistry (Combined Science) Specification Checklists. Name: Teacher:
AQA Chemistry (Combined Science) Specification Checklists Name: Teacher: Paper 1-4.1 Atomic structure and the periodic table 4.1.1 A simple model of the atom, symbols, relative atomic mass, electronic
More informationDescribe in full the colour change at the end-point of this titration. ... (1)
Q1. (a) A solution of barium hydroxide is often used for the titration of organic acids. A suitable indicator for the titration is thymol blue. Thymol blue is yellow in acid and blue in alkali. In a titration
More informationGCE O' LEVEL PURE CHEMISTRY (5073/02) Suggested Answers for 2016 O Level Pure Chemistry Paper 2
Section A (50 M) Aa) trend The number of electron shell increases The number of valence electrons increases Proton number increases There is a change in character from metallic to non-metallic Only true
More informationAnhydrous strontium chloride is not used in toothpaste because it absorbs water from the atmosphere. The hexahydrate, SrCl 2.6H 2O, is preferred.
Q1.(a) Anhydrous strontium chloride is not used in toothpaste because it absorbs water from the atmosphere. The hexahydrate, SrCl 2.6H 2O, is preferred. A chemist was asked to determine the purity of a
More information1 Principles of chemistry
1 Principles of chemistry The following sub-topics are covered in this section. (a) States of matter (b) Elements, compounds and mixtures (c) Atomic structure (d) The Periodic Table (e) Chemical formulae,
More informationfor sodium ion (Na + )
3.4 Unit 2 Chemistry 2 Throughout this unit candidates will be expected to write word equations for reactions specified. Higher tier candidates will also be expected to write and balance symbol equations
More informationAQA Chemistry Checklist
Topic 1. Atomic structure Video: Atoms, elements, compounds, mixtures Use the names and symbols of the first 20 elements in the periodic table, the elements in Groups 1 and 7, and other elements in this
More informationYEAR 10 CHEMISTRY TIME: 1h 30min
YEAR 10 CHEMISTRY TIME: 1h 30min NAME: CLASS: Useful data: Q = It. Faraday Constant = 96,500 C mol -1. Use the Periodic table, given below, where necessary. Marks Grid [For Examiners use only] Question
More information# Ans Workings / Remarks
# Ans Workings / Remarks 1 B Atomic mass and temperature affects the rate of diffusion of gas. The lower the atomic mass, the lighter the substance. The higher the temperature, the higher the rate of collision
More informationflame test acidified silver nitrate solution added
1 The results of two tests on solid X are shown. test aqueous sodium hydroxide added acidified silver nitrate added observation green precipitate formed yellow precipitate formed What is X? copper(ii)
More informationIdentification of Ions and Gases
Identification of Ions and Gases Question Paper 1 Level IGSE Subject hemistry (0620/0971) Exam oard ambridge International Examinations (IE) Topic cids, bases and salts Sub-Topic Identification of ions
More information4 Inorganic chemistry and the periodic table Answers to Exam practice questions
Pages 116 118 Exam practice questions 1 a) Atomic radius increases down the group [1] because of the increasing number of inner full shells of electrons. [1] The more full shells the larger the atom. [1]
More informationName: Periodic Table. Class: Foundation revision questions. Date: 39 minutes. Time: 39 marks. Marks: Comments: Page 1 of 12
Periodic Table Foundation revision questions Name: Class: Date: Time: 39 minutes Marks: 39 marks Comments: Page of 2 Lithium is a very reactive metal. Lithium reacts with cold water. (i) Which physical
More informationST EDWARD S OXFORD. Lower Sixth Entrance Assessment. November Chemistry. 1 Hour. Candidates name:... St Edward's School 1
ST EDWARD S OXFORD Lower Sixth Entrance Assessment November 2013 Chemistry 1 Hour Candidates name:... St Edward's School 1 St Edward's School 2 1. Complete the table below. Element calcium Symbol Pb S
More informationGCSE Additional Science Chemistry Contents Guide
GCSE Additional Science Contents Guide Copyright Boardworks Ltd 2007 Boardworks Ltd The Gallery 54 Marston Street Oxford OX4 1LF 08703 50 55 60 enquiries@boardworks.co.uk www.boardworks.co.uk 04-07 contains
More informationusing simple distillation and paper chromatography practical to obtain a
2.11 Core practical: Investigate the composition of inks using simple distillation and paper chromatography Paper 1 & 2 Topic 1 What do you need to be able to do? Practical: Description Investigate the
More informationGCSE Chemistry. CH3HP Mark scheme June Version/Stage: 1.0 Final
GCSE Chemistry CH3HP Mark scheme 4402 June 206 Version/Stage:.0 Final Mark schemes are prepared by the Lead Assessment Writer and considered, together with the relevant questions, by a panel of subject
More informationCH3HP. (Jun14CH3HP01) General Certificate of Secondary Education Higher Tier June Unit Chemistry C3 PMT TOTAL. Time allowed 1 hour
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Question Mark Chemistry Unit Chemistry C3 Thursday 15 May 2014 For this paper you must have:
More informationMetal + water -> metal hydroxide + hydrogen Metal + acid -> metal salt + hydrogen
Name of Formula Formula of ion Name of salt Hydrochloric Sulphuric HCl Cl - Chloride H 2 SO 4 SO 4-2 Sulphate Key words: Oxidation: loss of electrons Reduction: gain of electrons Displacement reaction:
More informationPersonalised Learning Checklists AQA Chemistry Paper 1
AQA Chemistry (8462) from 2016 Topics C4.1 Atomic structure and the periodic table State that everything is made of atoms and recall what they are Describe what elements and compounds are State that elements
More informationOCR Chemistry Checklist
Topic 1. Particles Video: The Particle Model Describe the main features of the particle model in terms of states of matter. Explain in terms of the particle model the distinction between physical changes
More informationGCSE Chemistry. Module C7 Further Chemistry: What you should know. Name: Science Group: Teacher:
GCSE Chemistry Module C7 Further Chemistry: What you should know Name: Science Group: Teacher: R.A.G. each of the statements to help focus your revision: R = Red: I don t know this A = Amber: I partly
More informationLondon Examinations IGCSE
Centre No. Candidate No. Paper Reference 4 3 3 5 2 H Paper Reference(s) 4335/2H London Examinations IGCSE Chemistry Paper 2H Higher Tier Wednesday 21 May 2008 Afternoon Time: 2 hours Surname Signature
More informationChemistry Co-teaching Combined Science and Chemistry
Chemistry Co-teaching Combined Science and Chemistry April 2016 Area Spec reference Combined Chemistry Both specifications Chemistry only 4.1 Atomic structure and the periodic table 4.1.1 A simple model
More informationChemistry Summer Holiday Homework Year Y9 & 10
Chemistry Summer Holiday Homework Year Y9 & 10 1. An atom of aluminium has the symbol (a) Give the number of protons, neutrons and electrons in this atom of aluminium. Number of protons... Number of neutrons...
More informationICSE Board. Class X Chemistry. Board Paper Time: 1½ hrs Total Marks: 80
ICSE Board Class X Chemistry Board Paper 2013 Time: 1½ hrs Total Marks: 80 General Instructions: 1. Answers to this paper must be written on the paper provided separately. 2. You will NOT be allowed to
More informationEdexcel GCSE Chemistry. Topic 3: Chemical changes. Acids. Notes.
Edexcel GCSE Chemistry Topic 3: Chemical changes Acids Notes 3.1 Rec that acids in solution are sources of hydrogen ions and alkalis in solution are sources of hydroxide ions Acids produce H + ions in
More information2.3 Group 7 The Halogens
2.3 Group 7 The Halogens Physical properties of the Halogens: The melting and boiling point of the halogens increases with atomic number due to increased van der Waals (from increased number of electrons).
More informationAQA TRILOGY Chemistry (8464) from 2016 Topics T5.1 Atomic structure and the periodic table (Paper 1) To pic. Student Checklist
Personalised Learning Checklist AQA TRILOGY Chemistry (8464) from 2016 s T5.1 Atomic structure and the periodic table (Paper 1) State that everything is made of atoms and recall what they are 5.1.1 A simple
More informationExtracting metals QuestionIT
Extracting metals QuestionIT 1. What is an ore? Metal compound in a rock. 2. What is produced when metals react with oxygen? Metal oxide. 3. What is this process called and why? Oxidation, gain of oxygen.
More informationPhysical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
More informationUnit: KCH0/4CH0 Science (Double Award) KSC0/4SC0 Paper: 1C
Write your name here Surname Other names Edexcel Certificate Edexcel International GCSE Centre Number Chemistry Unit: KC0/4C0 Science (Double Award) KSC0/4SC0 Paper: 1C Monday 20 May 2013 Afternoon Time:
More informationNational 4/5 Chemistry
National 4/5 Chemistry Homework Unit 1 Chemical Changes and Structure Please do not write on these booklets questions should be answered in homework jotters. Part 1 Introduction to Unit 1 1. Which box
More informationCombined Science Chemistry Academic Overview
Combined Science Chemistry Academic Overview 2018-2019 Science Term 1.1 Term 1.2 Term 2.1 Term 2.2 Term 3.1 Term 3.2 Year 9 States of Matter Methods of Separating and Purifying Substances Atomic Structure
More informationSame theme covered in Combined but extra content Extra parts atomic symbols (first 20, Group 1 and Group 7)
Co-teaching document new ELC Science 5960 and Foundation Level GCSE Combined Science: Trilogy (8464) Chemistry: Component 3 Elements, mixtures and compounds ELC Outcomes Summary of content covered in ELC
More information2B Air, Oxygen, Carbon Dioxide and Water
Air, Oxygen, Carbon Dioxide and Water Air, oxygen and carbon dioxide are important chemicals in our everyday lives. Knowledge of their properties helps us to develop an understanding of the role they play.
More informationM1. (a) Mendeleev 1. atomic weight 1. undiscovered 1. electronic structures 1 [5] (b) (i) A 1
M. (a) Mendeleev atomic weight (c) groups (d) undiscovered (e) electronic structures [5] M. (a) sodium is a metal sodium forms ions with a + charge (i) A B (iii) hydrogen [5] M3. (a) (i) argon and potassium
More informationQ1. Methane and oxygen react together to produce carbon dioxide and water.
Q1. Methane and oxygen react together to produce carbon dioxide and water. The methane gas will not burn in oxygen until a flame is applied, but once lit it continues to burn. (a) Explain why energy must
More informationName Date Class STUDY GUIDE FOR CONTENT MASTERY
Chemical Reactions Section 10.1 Reactions and Equations In your textbook, read about evidence of chemical reactions. For each statement, write yes if evidence of a chemical reaction is present. Write no
More informationPRACTICAL QUESTIONS TEST TUBE REACTIONS 4&11 Questions. Dr Chris Clay
PRACTICAL QUESTIONS TEST TUBE REACTIONS 4&11 Questions Dr Chris Clay http://drclays-alevelchemistry.com/ Q1.(a) A sample of solid chromium(iii) hydroxide displays amphoteric character when treated separately
More informationCovalent (sharing of electron pairs) Ionic ( electrostatic attraction between oppositely charged ions)
Covalent (sharing of electron pairs) Ionic ( electrostatic attraction between oppositely charged ions) Metallic (electrostatic attraction between + metal ions and delocalised electrons) Group 1 ions 1+
More informationNational 4 Unit Rates of Reaction 2. Atomic Structure 3. Acids & Bases 4. Energy Changes. Homework
National 4 Unit 1 1. Rates of Reaction 2. Atomic Structure 3. Acids & Bases 4. Energy Changes Homework 1 2 Homework 1 - Rates of Reaction Decide which of the following are True or False: 1. Increasing
More informationAQA GCSE CHEMISTRY (9-1) Topic 1: Atomic Structure and the Periodic Table
AQA GCSE CHEMISTRY (9-1) Topic 1: Atomic Structure and the Periodic Table 4.1.1 Atoms, elements and compounds 4.1.1.1 Atoms, elements and compounds All substances are made of atoms. An atom is the smallest
More informationAtomic Structure and the Periodic Table. AQA Chemistry topic 1
Atomic Structure and the Periodic Table AQA Chemistry topic 1 1.1 Atoms, elements and compounds The structure of the atom Everything in the universe is basically made up of atoms. An atom is the smallest
More informationPage 2. Q1.The electronic structure of the atoms of five elements are shown in the figure below. The letters are not the symbols of the elements.
Q1.The electronic structure of the atoms of five elements are shown in the figure below. The letters are not the symbols of the elements. Choose the element to answer the question. Each element can be
More informationAngel International School - Manipay 1 st Term Examination November, 2015
Grade 11B Angel International School - Manipay 1 st Term Examination November, 2015 Chemistry - I Duration: 1.00 Hour Part 1 1) A liquid boils at a temperature of 100 o C. Which other property of the liquid
More information