+ 10Cl 2Mn H 2 O + 5Cl 2. Deduce the half-equation for the oxidation of chloride ions to chlorine.
|
|
|
- Michael Rice
- 6 years ago
- Views:
Transcription
1 Q1.Chlorine is an important industrial chemical. (a) Chlorine is formed when KMnO 4 reacts with hydrochloric acid. The ionic equation for this redox reaction is 16H + + 2MnO Cl 2Mn H 2 O + 5Cl 2 (i) Deduce the half-equation for the oxidation of chloride ions to chlorine. (ii) Give the oxidation state of manganese in the MnO 4 ion. (iii) Deduce the half-equation for the reduction of the MnO 4 ions in acidified solution to manganese(ii) ions and water. Chlorine behaves as an oxidising agent in the extraction of bromine from seawater. In this process, chlorine gas is bubbled through a solution containing bromide ions. (i) Write the simplest ionic equation for the reaction of chlorine with bromide ions. (ii) Give one observation that would be made during this reaction. (iii) In terms of electrons, state the meaning of the term oxidising agent. In sunlight, chlorine can also oxidise water slowly to form oxygen. Write an equation for this reaction. Page 2
2 Give the oxidation state of chlorine in the chlorine-containing species that is formed. Equation Oxidation state of chlorine in the species formed... (2) (d) Explain why chlorine has a lower boiling point than bromine. (2) (Total 10 marks) Q2.The following pairs of compounds can be distinguished by simple test-tube reactions. For each pair, give a suitable reagent that could be added separately to each compound to distinguish between them. Describe what you would observe in each case. (a) AgBr(s) and AgI(s) Observation with AgBr(s)... Observation with AgI(s)... HCl(aq) and HNO 3(aq) Page 3
3 Observation with HCl(aq)... Observation with HNO 3(aq)... Cyclohexane and cyclohexene Observation with cyclohexane... Observation with cyclohexene... (d) Butanal and butanone Observation with butanal... Observation with butanone... (Total 12 marks) Q3.The following pairs of compounds can be distinguished by simple test tube reactions. For each pair of compounds, give a reagent (or combination of reagents) that, when added separately to each compound, could be used to distinguish between them. State what is observed in each case. (a) Butan 2 ol and 2 methylpropan 2 ol Page 4
4 Observation with butan 2 ol Observation with 2 methylpropan 2 ol Propane and propene Observation with propane Observation with propene Aqueous silver nitrate and aqueous sodium nitrate Observation with aqueous silver nitrate Observation with aqueous sodium nitrate (d) Aqueous magnesium chloride and aqueous barium chloride Page 5
5 Observation with aqueous magnesium chloride Observation with aqueous barium chloride (Total 12 marks) Q4.(a) Strontium chloride is used in toothpaste for sensitive teeth. Both strontium carbonate and strontium sulfate are white solids that are insoluble in water. (i) Write an equation for the reaction between strontium chloride solution and sodium sulfate solution. Include state symbols in your equation. (ii) Strontium carbonate reacts with nitric acid to produce a solution of strontium nitrate. Strontium sulfate does not react with nitric acid. Describe briefly how you could obtain strontium sulfate from a mixture of strontium carbonate and strontium sulfate. You are not required to describe the purification of the strontium sulfate. (2) A solution of magnesium sulfate is sometimes given as first aid to someone who Page 6
6 has swallowed barium chloride. Explain why drinking magnesium sulfate solution is effective in the treatment of barium poisoning. Medicines for the treatment of nervous disorders often contain calcium bromide. Silver nitrate, acidified with dilute nitric acid, can be used together with another reagent to test for the presence of bromide ions in a solution of a medicine. Describe briefly how you would carry out this test and state what you would observe. (Total 7 marks) Q5.Which of these substances reacts most rapidly to produce a silver halide precipitate with acidified silver nitrate? A B C D CH 3Br CH 3Cl CH 3F CH 3l (Total 1 mark) Q6.This question is about the chemical properties of chlorine, sodium chloride and sodium bromide. Page 7
7 (a) Sodium bromide reacts with concentrated sulfuric acid in a different way from sodium chloride. Write an equation for this reaction of sodium bromide and explain why bromide ions react differently from chloride ions. Equation... Explanation... A colourless solution contains a mixture of sodium chloride and sodium bromide. Using aqueous silver nitrate and any other reagents of your choice, develop a procedure to prepare a pure sample of silver bromide from this mixture. Explain each step in the procedure and illustrate your explanations with equations, where appropriate. (6) Write an ionic equation for the reaction between chlorine and cold dilute sodium hydroxide solution. Give the oxidation state of chlorine in each of the chlorine-containing ions formed. Page 8
8 (2) (Total 11 marks) Page 9
(09) WMP/Jun10/CHEM1
Group 2 and Group 7 9 5 The alkane butane is used as a fuel. 5 (a) (i) Write an equation for the complete combustion of butane. 5 (a) (ii) State a condition which may cause carbon to be formed as a product
3.2.5 Group VII. Trends in reducing abilities. 222 minutes. 218 marks. Page 1 of 21
3..5 Group VII Trends in reducing abilities minutes 18 marks Page 1 of 1 Q1. (a) Samples of solid sodium fluoride, sodium chloride, sodium bromide and sodium iodide are each warmed separately with concentrated
Page 2. Q1.The following pairs of compounds can be distinguished by simple test tube reactions.
Q1.The following pairs of compounds can be distinguished by simple test tube reactions. For each pair of compounds, give a reagent (or combination of reagents) that, when added separately to each compound,
3.2.5 Group VII. Trends in oxidising abilities. 167 minutes. 167 marks. Page 1 of 19
3..5 Group VII Trends in oxidising abilities 167 minutes 167 marks Page 1 of 19 Q1. (a) Samples of solid sodium fluoride, sodium chloride, sodium bromide and sodium iodide are each warmed separately with
white precipitate white precipitate, dissolves in excess of NaOH brown precipitate Identity of Q Identity of R Identity of S...
Q1.The table below shows observations of changes from some test-tube reactions of aqueous solutions of compounds Q, R and S with five different aqueous reagents. The initial colours of the solutions are
Describe 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
+ 10Cl 2Mn H 2 O + 5Cl 2. Deduce the half-equation for the oxidation of chloride ions to chlorine.... (1)... (1)
Chlorine is an important industrial chemical. (a) Chlorine is formed when KMnO 4 reacts with hydrochloric acid. The ionic equation for this redox reaction is 6H + + 2MnO 4 + 0Cl 2Mn 2+ + 8H 2 O + 5Cl 2
Some standard enthalpies of formation are given in the table below
Q1. Barium can be extracted from barium oxide (BaO) in a process using aluminium. A mixture of powdered barium oxide and powdered aluminium is heated strongly. The equation for this extraction process
... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3
![... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3](/thumbs/76/73434679.jpg "... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3")
1 Chemists have developed models for bonding and structure which are used to explain different properties. (a) Ammonia, NH 3, is a covalent compound. Explain what is meant by a covalent bond. Draw a dot-and-cross
3.2.5 Group VII. Trends in Physical Processes. 70 minutes. 70 marks. Page 1 of 7
3.2.5 Group VII Trends in Physical Processes 70 minutes 70 marks Page 1 of 7 Q1. (a) State and explain the trend in electronegativity down Group VII from fluorine to iodine. Trend... Explanation... (i)
Anhydrous 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
AS Paper 1 Group VII: The Halogens
AS Paper 1 Group VII: The Halogens South Axholme School Q1.Which one of the following statements is true? A B C D Bromine liberates iodine from aqueous sodium iodide. Chlorine liberates fluorine from aqueous
PRACTICAL 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
Strontium is extracted from strontium oxide (SrO) by heating a mixture of powdered strontium oxide and powdered aluminium.
Q1.Group 2 metals and their compounds are used commercially in a variety of processes. (a) Strontium is extracted from strontium oxide (SrO) by heating a mixture of powdered strontium oxide and powdered
3.2.6 Group II. Trends in Chemical properties. 164 minutes. 161 marks. Page 1 of 19
3.2.6 Group II Trends in Chemical properties 164 minutes 161 marks Page 1 of 19 Q1. (a) A small sample of barium metal was added to water in a flask. When the reaction had ceased, the contents of the flask
For 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
1 Two white powders, A and B, known to be Group 2 carbonates, are investigated.
1 Two white powders, A and B, known to be Group 2 carbonates, are investigated. (a) (i) The presence of the carbonate ion is usually confirmed using a simple test carried out in two stages at room temperature.
Draw the structure of the alkene that would form 1,2-dibromo-3-methylbutane when reacted with bromine.
Q1.In each of the following questions, you should draw the structure of the compound in the space provided. (a) Draw the structure of the alkene that would form 1,2-dibromo-3-methylbutane when reacted
Complete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion.
1 This question is about the elements with atomic numbers between 58 and 70 (a) Cerium, atomic number 58, is a metal Complete the table to show the relative charge of each particle and the number of each
Page 2. Q1.Which of these species is the best reducing agent? A Cl 2 C I 2
Q1.Which of these species is the best reducing agent? l 2 l I 2 I Q2.Which of these substances reacts most rapidly to produce a silver halide precipitate with acidified silver nitrate? H 3r H 3l H 3F H
Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. ... [3] ...
![Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. ... [3] ...](/thumbs/78/76733031.jpg "Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. ... [3] ...")
3 Gallium is a metallic element in Group III. It has similar properties to aluminium. (a) (i) Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer.
Page (Extra space) (4) Benzene can be converted into amine U by the two-step synthesis shown below.
Q1. The hydrocarbons benzene and cyclohexene are both unsaturated compounds. Benzene normally undergoes substitution reactions, but cyclohexene normally undergoes addition reactions. (a) The molecule cyclohexatriene
2.3 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).
1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation
NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,
CHEM2. General Certificate of Education Advanced Subsidiary Examination January Unit 2 Chemistry in Action (JAN12CHEM201) PMT
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Subsidiary Examination January 2012 Question 1 2
A cream precipitate formed
Q1. (a) Some scientists thought that the waste water from a waste disposal factory contained two sodium halides. They tested a sample of the waste water. They added three reagents, one after the other,
Chem!stry. Assignment on Redox
Chem!stry Name: ( ) Class: Date: / / Assignment on Redox Question 1: Which one of the following elements is the most powerful reducing agent? A Aluminium B Copper C Lead D Potassium Question 2: Which of
F321: Atoms, Bonds and Groups Redox
F321: Atoms, Bonds and Groups Redox 39 Marks 1. The element strontium forms a nitrate, Sr(NO 3 ) 2, which decomposes on heating as shown below. 2Sr(NO 3 ) 2 (s) 2SrO(s) + 4NO 2 (g) + O 2 (g) Using oxidation
AS Paper 1 Group II: The Alkaline Earth Metals
AS Paper 1 Group II: The Alkaline Earth Metals Q1.An aqueous solution of a sodium salt gave no precipitate when treated with either silver nitrate solution or barium chloride solution. Which one of the
The Use of Dilute Nitric Acid in the Qualitative Analysis of Anions
The Use of Dilute Nitric Acid in the Qualitative Analysis of Anions Background Information Aqueous barium nitrate is primarily used in qualitative analysis to test for the presence of sulfate ions. If
Show by calculation that the starting concentration of the manganate(vii) ions was mol dm 3.
1. Manganate(VII) ions react with ethanedioate ions in acidic solution. MnO 4 (aq) + 16H + (aq) + 5C O 4 (aq) Mn + (aq) + 8H O(l) + 10CO (g) (a) In a particular experiment 00 cm of aqueous potassium manganate(vii),
Chemical Reactions CHAPTER Reactions and Equations
CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number
Fluorine Gas. Chlorine Gas. Bromine Liquid. Iodine Solid
Halogens Fluorine (F 2 ): very pale yellow gas. It is highly reactive Chlorine : ( ) greenish, reactive gas, poisonous in high concentrations Bromine ( ) : red liquid, that gives off dense brown/orange
Group 7: The Halogens
Group 7: The Halogens Fluorine (F), Chlorine (), Bromine (Br), Iodine (I-) and Astatine (At). The halogens are very reactive elements and so, just like the Group 2 metals, they are not found in nature
3.2.9 Alkenes. Addition Reactions. 271 minutes. 268 marks. Page 1 of 35
..9 Alkenes Addition Reactions 71 minutes 68 marks Page 1 of 5 Q1. Propene reacts with bromine by a mechanism known as electrophilic addition. (a) Explain what is meant by the term electrophile and by
Elements in the Periodic Table show a periodic trend in atomic radius. In your answer you should use appropriate technical terms, spelled correctly.
1 The Periodic Table is arranged in periods and groups (a) Elements in the Periodic Table show a periodic trend in atomic radius State and explain the trend in atomic radius from Li to F In your answer
(a) Explain what is happening in stages 1 and 2. (3) (b) (i) Identify the products formed in stages 5, 6 and 7.
1 Hydrated magnesium nitrate, Mg(NO 3 ) 2.6H 2 O, is heated in a boiling tube and the following observations are made. Stage 1 Stage 2 Stage 3 Stage 4 Stage 5 Stage 6 Stage 7 The white solid forms a clear,
Chem!stry. Assignment on Acids, Bases and Salts #
Chem!stry Name: ( ) Class: Date: / / Assignment on Acids, Bases and Salts #5 Write your answers in the spaces below: 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 1. Which of the
QUESTIONSHEETS GROUPS 1 AND 2 REACTIONS OF THE ELEMENTS WITH WATER REACTIONS OF THE ELEMENTS WITH DILUTE ACIDS
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 10 GROUPS 1 AND 2 Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
F321: Atoms, Bonds and Groups Group 7
F321: Atoms, Bonds and Groups Group 7 93 Marks 1. Chlorine and bromine are elements in Group 7 of the Periodic Table. Chlorine is used in water treatment. State one advantage and one disadvantage of using
4 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]
Draw 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
(24) WMP/Jun12/CHEM2
24 Do not write outside the box 9 A student investigated the chemistry of the halogens and the halide ions. 9 (a) In the first two tests, the student made the following observations. Test 1. Add chlorine
sodium carbonate. sodium hydrogencarbonate. sodium nitrate. D sodium sulfate. (Total for Question 9 = mark)
1 ompound X is an anhydrous, white solid which decomposes on heating to form a white solid residue, a colourless gas, and a colourless vapour which condenses to a colourless liquid. ompound X is sodium
AQA A2 CHEMISTRY TOPIC 5.3 REDOX EQUILIBRIA BOOKLET OF PAST EXAMINATION QUESTIONS
AQA A2 CHEMISTRY TOPIC 5.3 REDOX EQUILIBRIA BOOKLET OF PAST EXAMINATION QUESTIONS 1. (a) Define the term oxidising agent in terms of electrons.... 2. Use the data in the table below, where appropriate,
The Periodic Table consists of blocks of elements
The Periodic Table consists of blocks of elements s block d block p block There is a clear link between the Periodic Table and the electronic configuration of an element 1s 2s 2p 3s 3p 4s 3d 4p 1s ATOMIC
TYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS http://www.youtube.com/watch?v=te4668aarck&feature=related The Five Major Class of Chemical Reaction http://www.youtube.com/watch?v=i HHvx1VC_8 Jan 2 8:07 PM 1 Nov 19 8:48 AM
Types of Reactions: Reactions
1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous
IB Topics 9 & 19 Multiple Choice Practice
IB Topics 9 & 19 Multiple Choice Practice 1. What are the oxidation states of chromium in (NH 4) 2Cr 2O 7 (s) and Cr 2O 3 (s)? 2. Which of the following is a redox reaction? 3Mg (s) + 2AlCl 3 (aq) 2Al
F321: Atoms, Bonds and Groups Moles and Equations
F321: Atoms, Bonds and Groups Moles and Equations 108 Marks 1. (a) A student carries out a titration to find the concentration of some sulfuric acid. The student finds that 25.00 cm 3 of 0.0880 mol dm
This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24
Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives
least reactive magnesium
1 One way of establishing a reactivity series is by displacement reactions. (a) A series of experiments was carried out using the metals lead, magnesium, zinc and silver. Each metal was added in turn to
The presence of these ions can be confirmed by reacting separate samples of solution X with aqueous ammonia and with aqueous sodium carbonate. ...
Q1.A green solution, X, is thought to contain [Fe(H 2 O) 6 ] 2+ ions. The presence of these ions can be confirmed by reacting separate samples of solution X with aqueous ammonia and with aqueous sodium
Reactants: Products: Definition:
Definition: A chemical reaction is a process in which one or more substances are changed to form new chemical substance(s) with different physical and chemical properties. Definition: A chemical reaction
Q1. The following pairs of compounds can be distinguished by simple test tube reactions.
Q1. The following pairs of compounds can be distinguished by simple test tube reactions. For each pair of compounds, give a reagent (or combination of reagents) that, when added separately to each compound,
4.4. 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
Q1.Which one of the following contains the metal with the lowest oxidation state? [Mn(CN) 6] 3 (Total 1 mark)
![Q1.Which one of the following contains the metal with the lowest oxidation state? [Mn(CN) 6] 3 (Total 1 mark)](/thumbs/78/76732680.jpg "Q1.Which one of the following contains the metal with the lowest oxidation state? [Mn(CN) 6] 3 (Total 1 mark)")
AS Paper 1 Redox South Axholme School Q1.Which one of the following contains the metal with the lowest oxidation state? A CrO 2F 2 B [Cr 2O 7] 2 C D [MnCl 6] 2 [Mn(CN) 6] 3 (Total 1 mark) Q2. (a) Samples
Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind.
Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. 1. calcium + oxygen 2. cupric carbonate 3. aluminum + hydrochloric
(10) WMP/Jan12/CHEM2
0 Do not write outside the box 5 Iodine reacts with concentrated nitric acid to produce nitrogen dioxide (NO 2 ). 5 (a) (i) Give the oxidation state of iodine in each of the following. I 2... HIO 3...
CHERRY HILL TUITION AQA CHEMISTRY A2 PAPER Section A (2 marks) (1 mark) (Extra space) Property
2 Section A Answer all questions in the spaces provided. 1 (a) Define the term lattice enthalpy of dissociation. 1 (b) Lattice enthalpy can be calculated theoretically using a perfect ionic model. Explain
International Advanced Level Chemistry Advanced Subsidiary Unit 2: Application of Core Principles of Chemistry
Write your name here Surname Other names Pearson Edexcel International Advanced Level Centre Number Candidate Number Chemistry Advanced Subsidiary Unit 2: Application of Core Principles of Chemistry Friday
CHM152LL Solution Chemistry Worksheet
Name: Section: CHM152LL Solution Chemistry Worksheet Many chemical reactions occur in solution. Solids are often dissolved in a solvent and mixed to produce a chemical reaction that would not occur if
burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3
1 Crystals of sodium sulphate-10-water, Na 2 SO 4.10H 2 O, are prepared by titration. burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3 (a)
Core practical 15: Analyse organic and inorganic unknowns
Core practical 15 Teacher sheet Core practical 15: Objectives To research the tests for ions and organic compounds To successfully test unknown substances to establish their identity Safety Wear goggles.
Name: Class: Redox revision questions. 50 minutes. Time: Marks: 50. Comments: Page 1 of 17
Name: Class: Redox revision questions Time: 50 minutes Marks: 50 Comments: Page of 7 Aqueous C 2 O ions react with MnO ions in acidic solution according to the equation 5 C 2 O + 2MnO + 6H + 2Mn 2+ + 0CO
SO 4... [2], to an excess of dilute sulfuric acid. A student adds a sample of solid potassium carbonate, K [3]
![SO 4... [2], to an excess of dilute sulfuric acid. A student adds a sample of solid potassium carbonate, K [3]](/thumbs/83/87669036.jpg "SO 4... [2], to an excess of dilute sulfuric acid. A student adds a sample of solid potassium carbonate, K [3]")
1 Chemicals called acids have been known throughout history The word acid comes from the Latin acidus meaning sour Dilute sulfuric acid, H 2 SO 4, is a common laboratory acid (a) State the formulae of
UNIT F321: ATOMS, BONDS AND GROUPS REVISION CHECKLIST. Miscellaneous Questions
UNIT F321: ATOMS, BONDS AND GROUPS REVISION CHECKLIST Miscellaneous Questions 1.1 Module 1: Atoms and Reactions 1.1.1 Atoms Candidates should be able to: Atomic structure (a) describe protons, neutrons
Types of Reactions: Reactions
1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous
11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds
Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most
Identification of ions and gases Assignment
Name: ( ) ate: lass: Identification of ions and gases ssignment 1. n excess of sodium hydroxide is added to an aqueous solution of salt X and boiled. mmonia gas is only given off after aluminium foil is
Chemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions
Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In
Stoichiometry Chapter 9 Practice Assessment B
NAME Hour Date Stoichiometry Chapter 9 Practice Assessment B Objective 1: Interpret balanced chemical equations in terms of interacting moles, representative particles, masses, and gas volume at STP. Directions:
AS CHEMISTRY (7404/1)
SPECIMEN MATERIAL AS CHEMISTRY (7404/1) Paper 1: Inorganic and Physical Chemistry Specimen 2015 Session Time allowed: 1 hour 30 minutes Materials For this paper you must have: the Data Sheet, provided
INSTRUCTIONS ON EVERY AP EXAM:
Most Common Reaction Types: 1. Acid-base neutralization (both weak & strong) 2. Nonmetal and metal oxides with water 3. Active metals with water 4. Single replacement redox 5. Double replacement precipitation
TIME 1 hour 30 minutes, plus your additional time allowance.
Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education 2012 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC112] WEDNESDAY
Net Ionic Equations. Making Sense of Chemical Reactions
Making Sense of Chemical Reactions Now that you have mastered writing balanced chemical equations it is time to take a deeper look at what is really taking place chemically in each reaction. There are
2 Answer all the questions. How many neutrons are there in an atom of chlorine-37?... [1] How many electrons are needed to fill one orbital?
![2 Answer all the questions. How many neutrons are there in an atom of chlorine-37?... [1] How many electrons are needed to fill one orbital?](/thumbs/87/96035070.jpg "2 Answer all the questions. How many neutrons are there in an atom of chlorine-37?... [1] How many electrons are needed to fill one orbital?")
2 Answer all the questions 1 The answer to each part of this question is a number (a) (i) How many neutrons are there in an atom of chlorine-37? [1] (ii) How many electrons are needed to fill one orbital?
Qualitative Analysis Part Two Anions & Gases
Qualitative Analysis Part Two Anions & Gases Qualitative Tests for Anions Which anions must I know the tests for? Describe tests to identify the following anions: Carbonate CO 3 2 (by the addition of dilute
CHEM2. General Certificate of Education Advanced Subsidiary Examination June Unit 2 Chemistry in Action. Friday 27 May pm to 3.
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Subsidiary Examination June 2011 Question 1 2 Mark
4.4.1 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
The following pairs of compounds can be distinguished by simple test tube reactions.
The following pairs of compounds can be distinguished by simple test tube reactions. For each pair of compounds, give a reagent (or combination of reagents) that, when added separately to each compound,
An equation for the decomposition of hydrogen peroxide is shown below.
An equation for the decomposition of hydrogen peroxide is shown below. 2H 2 O 2 2H 2 O + O 2 State the measurements you would take in order to investigate the rate of this reaction............. (Total
Year 10 Chemistry. Practice questions. Topics
Year 10 Chemistry Practice questions Topics 1 Group 1 2 Group 7 3 Reactivity series 4 Air and Water 5 Rates of reaction 6 Electrolysis 7 Acids, Alkali and Salts Objective: Evaluate group 1 & 7 reactivity
Page 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
The first ionisation energies of the elements Li to Na are shown in the figure below.
1 Ionisation energies have been used to develop the model of the atom. The first ionisation energies of the elements Li to Na are shown in the figure below. 2500 1st ionisation energy / kj mol 1 2000 1500
4. a) Complete the nuclear equation below. (1mk) b) 37 37
KCSE 2006 CHEMISTRY PAPER 1 QUESTIONS 1. (a) What is meant by isomerism? (1mark) (b) Draw and name two isomers of butane. (2 marks) 2. The diagram below represent a set-up that was used to show that part
Chapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
Reactions (Chapter 4) Notes 2016.notebook. October 14, Chemical Reactions. Chapter 4 Notes. Oct 21 8:44 AM. Oct 22 10:14 AM
Chemical Reactions Chapter 4 Notes Oct 21 8:44 AM Oct 22 10:14 AM 1 There are several things to keep in mind writing reactions and predicting products: 1. States of matter of elements/compounds 2. Diatomics
Advanced Placement Chemistry, SCH4UAP EXAMINATION REVIEW. Equations. Page 1
Advanced Placement Chemistry, SCH4UAP EXAMINATION REVIEW Equations Page 1 Page 2 Page 3 Page 4 Page 5 Page 6 4.2 - Precipitation Reactions Question 1 Give the formulas to show the reactants and the products
AQA A2 CHEMISTRY TOPIC 5.4 TRANSITION METALS PART 2 REDOX REACTIONS AND CATALYSIS BOOKLET OF PAST EXAMINATION QUESTIONS
AQA A2 CHEMISTRY TOPIC 5.4 TRANSITION METALS PART 2 REDOX REACTIONS AND CATALYSIS BOOKLET OF PAST EXAMINATION QUESTIONS 1. Chemical reactions can be affected by homogeneous or by heterogeneous catalysts.
2 Answer all the questions. CO, in the presence of aqueous hydrochloric acid, HCl(aq).
2 Answer all the questions. 1 A student investigates the reaction between iodine, I 2, and propanone, (CH 3 ) 2 CO, in the presence of aqueous hydrochloric acid, HCl(aq). The results of the investigation
Unit 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
4.4. 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
1 A solution contains barium ions and silver ions and one type of anion. What could the anion be? chloride only. nitrate only.
For more awesome resources, visit us at www.savemyexams.co.uk/ Identification of Ions and Gases Question Paper 2 Level IGSE Subject hemistry (0620/0971) Exam oard ambridge International Examinations (IE)
Acids and Bases. Properties of Acids. Properties of Bases
Chemistry 2A/2B Term 3 Notes B 1 Coghlan Chemistry 2A/2B Term 3 Notes B Properties of Acids Acids and Bases 1. Neutralise. 2. Turns litmus red. 3. Conducts when in with water form an (acids ). 4. React
Formulae and Equations
Formulae and Equations 1 of 41 Boardworks Ltd 2016 Formulae and Equations 2 of 41 Boardworks Ltd 2016 Forming different compounds 3 of 41 Boardworks Ltd 2016 Elements are made up of just one type of atom.
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *4827396477* CHEMISTRY 9701/35 Advanced Practical Skills October/November
At 298 K and 100 kpa, the oxygen gas produced in this decomposition occupied a volume of m
Q1. Potassium nitrate, KNO 3, decomposes on strong heating, forming oxygen and solid Y as the only products. (a) 1.00 g sample of KNO 3 (M r = 101.1) was heated strongly until fully decomposed into Y.
Name 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