Chemistry for 14 -16 year olds: Non-metals and their compounds.

Slide 1 : 1 GCSE Questions and Answers Inorganic: Non-metals Includes Industrial Process:Contact, Ostwald, Haber-Bosch Remember that you can search using “edit”! 6 consecutive papers: 2002-7 You can find a video-cast lesson on this here

Slide 2 : 2 General Introduction.

Slide 3 : 3 Key Points. Reactivity increases as you go down a group of metals (Groups 1 and 2). Reactivity falls as you go down a group of non-metals (Group 7). As atoms get larger the outer shell gets further from the nucleus. The valence electrons are then held more weakly. It takes less energy to remove an electron from K than Na Cl can attract (and hold) an extra electron better than Br Metals can displace metals above then in their group Non-metals can displace non-metals below them in their group

Slide 4 : 4 Key facts about Carbon. Organic Carbon – Families of carbon compounds with (Organic chemistry) carbons in chains and rings. Inorganic Chemistry - Allotropes: Graphite, Diamond, C60 Charcoal, CO2, CO, CO32- & HCO3- Graphite and diamond discussed in “Atomic Structure and Bonding” C60 CO2 and CO consider here. Occurrence and reactions of carbonates and hydrogencarbonates considered in “Inorganic Metal Chemistry”.

Slide 5 : 5 Carbon Can you name its Allotropes and define “allotropes”?

Slide 6 : 6 Carbon Can you name its Allotropes and define “allotropes”? Allotropes. Diamond [1]; graphite [1]; and buckminsterfullerene [1] Definition. Allotropes are different forms [1] of same element in same physical state [1]

Slide 7 : 7 Identify these structures & outline bonding and properties

Slide 8 : 8 Identify these structures & outline bonding and properties

Slide 9 : 9 Why is diamond a very hard substance?   Why can graphite be used as a lubricant?

Slide 10 : 10 Why is diamond a very hard substance?   Strong bonds [1] in a giant/3D/macromolecular structure [1] Difficult to break bonds/very rigid structure [1] Not ionic/metallic bonding [0] (any two)   Why can graphite be used as a lubricant?   Made up of layers [1] Which can slide over each other/ which have weak attractive forces holding them together [1]

Slide 11 : 11 Charcoal (another form of carbon). Give three uses of charcoal.

Slide 12 : 12 Charcoal (another form of carbon). Can be produced by slowly smouldering wood under damp leaves. Used for decolourising and deodorising. Removing unpleasant odours in a car Charcoal in art WWIIGas mask BBQ Fuel

Slide 13 : 13 This third allotrope of carbon was only discovered in 1985. A spherical structure made up of both pentagonal and hexagonal rings of carbon atoms Consisting of discrete molecules of ‘just’ 60 atoms, they are NOT considered giant covalent structures Buckminster Fullerene (C60)

Slide 14 : 14 Properties and Uses of C60 This C60 structures do dissolve to some extent in some common solvents (e.g. CS2), and although solid, their melting points are not that high. Scientists are trying to make them as continuous tubes to form very strong fibres of 'pipe like' molecules called 'nanotubes'. These are incredibly tinny tubes (made of various materials) that can be used to direct particles efficiently in appropriate directions in microelectronics. They can be used to make structures harder then diamond

Slide 15 : 15 Solutions of pure Buckminsterfullerene have a deep purple colour. While there are few uses of fullerenes today, their structures suggest possible uses as superconductors, lubricants Yonex uses nano carbon, or fullerene, to create a faster performing shaft that is lighter yet more stable than traditional Graphite shaft

Slide 16 : 16 Chemical sponges: Medical researchers believe that fullerenes could be put to work as tiny chemical sponges, mopping up dangerous chemicals from injured brain tissue. Lubricants: Buckyballs can behaving as 'molecular ball bearings' allowing surfaces to glide over one another Molecular sieves Because of the way they stack, buckyballs could act as molecular sieves, trapping particles of particular sizes while leaving others unaffected. Buckycopiers? In the United States, Xerox owns patents for using buckyballs to improve resolution of photocopies. They are 1000 times smaller than the particles used in conventional photocopier toner.

Slide 17 : 17 Facts about silicon and silicates Would you classify silicon as a metal or non-metal. Comment on your answer. Yes/No/Neither Comment. _______________________________ _______________________________

Slide 18 : 18 Facts about silicon and silicates Would you classify silicon as a metal or non-metal. Comment on your answer. Yes/No/Neither Comment. Silicon is a semi-metal (metalloid). It is shiny like a metal, but is only a semi-conductor of electricity.

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Slide 20 : 20 State one use of silicon and explain what makes it suitable for this purpose.

Slide 21 : 21 State one use of silicon and explain what makes it suitable for this purpose. Used to make a wide variety of electronic devices, including transistors, integrated circuits and solar cells. This is because it is an excellent semi-conductor.

Slide 22 : 22 What is the formula of quartz Show a representative small part of the structure of

Slide 23 : 23 What is the formula of quartz SiO2 Show a representative small part of the structure of Each silicon [1] atom is attached to 4 [1] oxygen [1] atoms in a tetrahedral [1] arrangement

Slide 24 : 24 State two occurrences of silicates

Slide 25 : 25 State two occurrences of silicates In the manufacture of cement, porcelain, glass and ceramics.

Slide 26 : 26 Facts about Nitrogen and its compounds. Colourless, tasteless, odourless gas that consists of diatomic moles: N2 21% O2 1 78% N2 1% Argon

Slide 27 : 27 Liquid nitrogen as a temperature near to -200 oC Uses. Quick freezing of cooked pizza Removing warts Cryogenics (suspended animation) Obtained by the fractional distillation of Air.

Slide 28 : 28 Nitrogen, Nitrates , Ammonia and Ammonium Compounds. Nitrogen molecules have a strong N=N bond. Nitrogen will only react under extremes of condition. Nitrogen reacts with Hydrogen in the Haber-Bosch Industrial Process, forming Ammonia (NH3) N2 + 3H2 ? 2NH3 Catalyst = iron Temperature = 450oC Pressure = 200 atmospheres Cool to liquify ammonia Unreacted gases recycled

Slide 29 : 29 Ammonia is converted to Nitric Acid in the Ostwald Industrial Process. Stage 1: 4NH3 + 5O2 ? 4NO + 6H2O Conditions: Burnt (oxidised) at about 1000oC and several atmospheres pressure in the presence of a catalyst such as platinum with 10% rhodium Stage 2: 2NO + O2 ? 2NO2 Stage 3: 4NO2 + O2 + 2H2O ? 4HNO3 Stages 2 and 3 occur under normal conditions in an “absorption tower”. Catalyst gauze

Slide 30 : 30 Ammonia and Nitric Acid, together with Sulphuric and Phosphoric acids are used to produce most of our “artificial fertilizers” Ammonia + Acid ? Fertilizer Salt NH3 + NH4NO3 ? NH4NO3 Ammonium Nitrate 2NH3 + H2SO4 ? (NH4)2SO4 Ammonium Sulphate 3NH3 + H3PO4 ? (NH4)3PO4 Ammonium Phosphate Ammonia is used to manufacture explosives, including TNT, where the “N” is for “Nitro”. Most plants prefer N in NO3- to NH4+

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Slide 32 : 32 Nitrates entering rivers, lakes and drinking water supplies. Nitrate is a potential human health threat especially to infants, causing the condition known as methemoglobinemia, also called "blue baby syndrome. When Nitrate is taken in by eating food and drinking water,  Nitrate is converted in the gut to nitrite, which then combines with haemoglobin to form methemoglobin, thus decreasing the ability of the blood to carry oxygen. Infants are more susceptible to nitrate toxicity than older children or adults

Slide 33 : 33 Use of Ammonia Solution to detect Cations in solution. MgCl2(aq)  +  2NH4OH(aq)  =Mg(OH)2(s)  +  2NH4Cl(aq)---------------------------------------------------------- ----------- ZnCl2(aq)  +  2NH4OH(aq)  = Zn(OH)2(s)  +  2NH4Cl(aq) Zn(OH)2(s)   +  2NH4OH(aq) = [Zn(NH3)4]2+(aq)  + 2OH-(aq) zinc tetra-ammine hydroxide ----------------------------------------------- AlCl3(aq)  +  3NH4OH(aq)  = Al(OH)3(s)  +  3NH4Cl(aq)  ----------------------------------------------- FeCl2(aq)  + 2NH4OH(aq)  =  Fe(OH)2(s)  +  2NH4Cl(aq) FeCl3(aq) + NH4OH(aq)  =  Fe(OH)3(s)  +  3NH4Cl(aq) --------------------------------------------------------------------- CuSO4(aq)  + 2NH4OH(aq)   =   Cu(OH)2(s)  +  (NH4)2SO4(aq) Cu(OH)2(s)  + 4NH3(aq)   =   [Cu(NH3)4]2+(aq)  + 2OH-(aq)                                        Copper tetra-ammine hydroxide ------------------------------------------------ White ppt White ppt Colourless Solution White ppt Green ppt Brown ppt Light blue ppt Dark blue solution

Slide 34 : 34 Copper (II) salts solutions with excess Ammonia

Slide 35 : 35 This is a 2-step reaction, involving 3 separate copper compounds. Copper (II) sulphate is a blue coloured salt solution Upon the addition of Ammonia Solution, insoluble Copper (II) Hydroxide is formed thus:CuSO4(aq)  + 2NH4OH(aq)   =   Cu(OH)2(s)  +  (NH4)2SO4(aq)Net Ionic Equation: Cu2+(aq)  +  2OH-(aq)  = Cu(OH)2(s)   Upon further addition of Ammonia solution the precipitate re-dissolves and a royal-blue solution is formedCu(OH)2(s)  + 4NH3(aq)   =   [Cu(NH3)4]2+(aq)  + 2OH-(aq)                                        Copper tetra-ammine ionNet Ionic Equation: Cu2+(s)  +  4NH3(aq)  =   [Cu(NH3)4]2+(aq)

d) Ammonia solution is used to detect the presence of metal cations in solution.(i) Describe what would be observed when ammonia solution is added slowly until it is in excess to a solution copper(II) sulphate. Blue solution [1] blue [1] precipitate [1] which redissolves in excess giving a dark blue [1] solution [1] (Max [4]) [4] : d) Ammonia solution is used to detect the presence of metal cations in solution.(i) Describe what would be observed when ammonia solution is added slowly until it is in excess to a solution copper(II) sulphate. Blue solution [1] blue [1] precipitate [1] which redissolves in excess giving a dark blue [1] solution [1] (Max [4]) [4]

(ii) When ammonia solution is added to a solution of an unknown metal chloride, a green precipitate is produced. What metal ion is present in the chloride solution? _______________________________ [1] : (ii) When ammonia solution is added to a solution of an unknown metal chloride, a green precipitate is produced. What metal ion is present in the chloride solution? _______________________________ [1]

Slide 38 : 38 Ammonia solution is a solution of NH3(aq) and Ammonium Hydroxide [NH4OH(aq)] Iron (II) salt solutions are generally green in colour. Iron (III) salt solutions are generally yellow/brown in colour. It is difficult to distinguish between dilute iron salts solutions using colour When an aqueous ammonia solution is added to each the results are clearly different. Iron (II) salt solution form a dark green precipitate of Fe(OH)2 Iron (III) salt solution form a dark brown precipitate of Fe(OH)3

Slide 39 : 39 Iron (II) salt solution form a green precipitate of Fe(OH)2. It does not dissolve in excess ammonia solution FeCl2(aq)  + 2NH4OH(aq)  =  Fe(OH)2(s)  +  2NH4Cl(aq) Net Ionic Equation: Fe2+(aq)  +  2OH-(aq)  = Fe(OH)2(s)    Iron (III) salt solution form a brown precipitate of Fe(OH)3. It does not dissolve in excess NH3 solution FeCl3(aq) + NH4OH(aq)  =  Fe(OH)3(s)  +  3NH4Cl(aq)   Net Ionic Equation: Fe3+(aq)  +  3OH-(aq)  = Fe(OH)3(s)

(ii) When ammonia solution is added to a solution of an unknown metal chloride, a green precipitate is produced. What metal ion is present in the chloride solution? Iron (II) / Fe2+ [1] : (ii) When ammonia solution is added to a solution of an unknown metal chloride, a green precipitate is produced. What metal ion is present in the chloride solution? Iron (II) / Fe2+ [1] 2006, Paper 2

Slide 41 : 41 Describe and explain what is observed when an excess of aqueous ammonia is added slowly to solutions of zinc and aluminium salts NH4OH NH3

Slide 42 : 42 Upon the addition of several drops of ammonia solution both form white gelatinous precipitates . These are insoluble hydroxides .ZnCl2(aq)  +  2NH4OH(aq)  = Zn(OH)2(s)  +  2NH4Cl(aq)Net Ionic Equation: Zn2+(aq)  +  2OH-(aq)  = Zn(OH)2(s)  AlCl3(aq)  +  3NH4OH(aq)  = Al(OH)3(s)  +  3NH4Cl(aq)   Net Ionic Equation: Al3+(aq)  +  3OH-(aq)  =  Al(OH)3(s)  Upon the addition of excess ammonia solution only the Zinc Precipitate re-dissolves.Zn(OH)2(s)   +  2NH4OH(aq) = [Zn(NH3)4]2+(aq)  + 2OH-(aq) The difference can be explained by the fact that zinc (like copper) is a transition element but aluminium is not. Aluminium is unable to form a complex similar to the tetra-ammine complexes of copper and zinc. Recall that with NaOH(aq) Zinc and Aluminium cannot be distinguished between as both form white precipitates that both redissolve

Slide 43 : 43 Magnesium salts solutions with excess Ammonia. Magnesium hydroxide is only sparingly soluble. Upon addition of several drops of ammonia solution the solution goes cloudy and a precipitate settles to the bottom of the test tube after several minutes. The reaction is:MgCl2(aq)  +  2NH4OH(aq)  =Mg(OH)2(s)  +  2NH4Cl(aq)  Excess ammonia does not re-dissolve the precipitate

Slide 44 : 44 Key Facts about Oxygen. Colourless, odourless, tasteless gas that exists as diatomic molecules O2. 21% of dry air. Materials that burn in air burn better, sometimes dangerously better, in pure or pressurised oxygen. Obtained by fractional distillation of Air Care: Risk of Explosion! Oxyacetylene

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Slide 46 : 46 Some Sulphur Chemistry. Name the three allotropes of sulphur

Slide 47 : 47 Some Sulphur Chemistry. Sulphur Allotropes Monoclinic sulphur needle-like crystals Rhombic sulphur S8 Puckered Ring Plastic Sulphur

Slide 48 : 48 Extraction of Sulphur. It is extrated by the Frasch Process. Can you outline how this works? Not tested in CCEA

Slide 49 : 49 Extraction of Sulphur. The Frasch Process.

Slide 50 : 50 Key Points on Group VII. The Halogens They all have 7 electrons in the outside shell. Fluorine F2 colourless gas Chlorine Cl2 green-yellow gas Bromine Br2 red-brown liquid Iodine I2 grey/black crystals

Slide 51 : 51 Group VII. The Halogens They all consist of diatomic molecules.   You could be asked what astatine, the next member of the group, looks like. You need to look for a pattern. Notice how they are gas at the top, then liquid, and then solid. So astatine will follow on the pattern and be a solid too.

Slide 52 : 52 Laboratory Preparation of Chlorine Gas. 2HCl + [O] ? H2O +Cl2 This is an OXIDATION reaction. Potassium Permanganate is a suitable OXIDISING AGENT

Slide 53 : 53 Laboratory Preparation of Hydrogen Chloride Gas HCl(g) and Hydrochloric Acid 2NaCl(s) + H2SO4(l) ? NaHSO4 (aq) + HCl(g) HCl(aq)

Slide 54 : 54 Reactivity. Saying fluorine is dangerous is an understatement. Halogens react especially well with metals Iron reacts very violently when heated with chlorine iron + chlorine = iron (III) chloride 2Fe + 3Cl2 = 2FeCl3 Iron reacts quite vigorously when heated with bromine iron + bromine = iron (III) bromide 2Fe + 3Br2 = 2FeBr3 iron does not react when heated with iodine

Slide 55 : 55 From the video-cast showing the preparation of Chlorine and its reaction with Iron Wool Iron + Chlorine ? Iron (III) Chloride 2Fe + 3Cl2 ? 2FeCl3 Chlorine

Slide 56 : 56 Reactivity. To say that fluorine is dangerous is an understatement. Halogens react especially well with metals Halogens get less reactive as you go down the group. A halogen can displace a less reactive halogen (one lower in the group) from its compound. 2NaBr + Cl2 ? 2NaCl + Br2 2NaBr + I2 ? No reaction

Slide 57 : 57 Group VII. The Halogens Explanation of why the halogens get less reactive as you go down the group All the halogens react by gaining one electron to fill their outer shell - the more easily they are gained, the more reactive the halogen

Slide 58 : 58 Identifying halide ions in solution The equations for the reactions are represented thus:NaX(aq)  +  AgNO3(aq)   =   AgX(s)  +  NaNO3(aq) Na

Slide 59 : 59 NaCl(aq)  +  AgNO3(aq)   =   AgCl(s)  +  NaNO3(aq)                                                white ppt NaBr(aq)  +  AgNO3(aq)   =   AgBr(s)  +  NaNO3(aq)                                                cream ppt NaI(aq)  +  AgNO3(aq)   =   AgI(s)  +  NaNO3(aq)                                              yellow ppt Why Can’t You hite ream ellow

Slide 60 : 60 Both AgCl and AgBr are light sensitive. They have darkened noticeably after 5 minutes AgBr

Slide 61 : 61 Other things to know about Chlorine. Chlorine’s Test is that itbleaches litmus paper Chlorine reacts with cold dilute NaOH to form sodium chlorate (I). Its formula is NaClO Sodium + Chlorine ? Sodium + Sodium + Water Hydroxide Chloride Chlorate (I) 2NaOH(aq) + Cl2(g) ? NaCl(aq) + NaOCl(aq) + H2O(l) Sodium chlorate (I) solution is used on a large scale for surface purification, bleaching, odour removal and water disinfection.

Slide 62 : 62 Other uses to know for Chlorine. A bleach (whitener) for cotton, linen and wood pulp To manufacture domestic bleaches like “domestos” Treat water in swimming pools To manufacture thepolymer PVC, where the “C” is “chloride” To manufacture insecticides. DDT, banned in most countries is one example

Slide 63 : 63 Chemical Warfare The first shells containing chlorine were produced by the Germans in 1916. Cl2 + H2O ? HCl + HClO Hydrochloric & hypochlorous acids

Slide 64 : 64 Iodine can be used for its antiseptic properties. It can be used to treat cuts and grazes. Drops can be added contaminated water to help sterilise it.

Slide 65 : 65 Key points on Group 8 Noble Gases. Unreactive (chemically inert) compared with the other elements. They all have full outer shells of electrons and are therefore very stable. XX

Slide 66 : 66 Uses of the noble gases . Noble gases in Lighting. Ordinary filament lamps contain argon or nitrogen and argon. High-energy fluorescent lighting tubes and airport runway lights contain krypton or argon and krypton. Lighthouse lamps contain xenon or argon and krypton.

Slide 67 : 67 Neon Sign

Slide 68 : 68 Source: wikipedia

Slide 69 : 69 Helium. Airships and Party Balloons Much less dense than air and non-combustible

Slide 70 : 70 Helium is used by Deep-Sea Divers. Breathing gas mixtures to prevent deep sea divers suffering from 'the bends'. The pressure increases as a diver descends, so breathing gases have to be supplied under pressure. Nitrogen in air causes 'nitrogen narcosis' below 30 m, a dangerous condition similar to being drunk.

5 Ammonia is an important industrial chemical in many different manufacturing processes.a) Give two uses of ammonia. 1. ___________________________ 2. ________________________ [2] : 5 Ammonia is an important industrial chemical in many different manufacturing processes.a) Give two uses of ammonia. 1. ___________________________ 2. ________________________ [2]

Slide 72 : 72 NH3 + HNO3 ? NH4NO3 Ammonia + Nitric ? Ammonium Nitrate Acid ------------------------------------ 2NH3 + H2SO4 ? (NH4)2SO4 Ammonia + Sulphuric ? Ammonium Acid Sulphate ----------------------------------------- 3NH3 + H3PO4 ? (NH4)3PO4 Ammonia + Phosphoric ? Ammonium Acid Nitrate From “Learning Outcomes” Making fertilizers

5 Ammonia is an important industrial chemical in many different manufacturing processes. a) Give two uses of ammonia. Fertilizers / Nitric Acid / Explosives/ Dyes [2] : 5 Ammonia is an important industrial chemical in many different manufacturing processes. a) Give two uses of ammonia. Fertilizers / Nitric Acid / Explosives/ Dyes [2]

b) Ammonia is prepared industrially from nitrogen and hydrogen gases. The equation for the reaction is: N2 + 3H2 = 2NH3(i) What is the name of the industrial process used to manufacture ammonia? ______________________________ [1] : b) Ammonia is prepared industrially from nitrogen and hydrogen gases. The equation for the reaction is: N2 + 3H2 = 2NH3(i) What is the name of the industrial process used to manufacture ammonia? ______________________________ [1]

b) Ammonia is prepared industrially from nitrogen and hydrogen gases. The equation for the reaction is: N2 + 3H2 ? 2NH3(i) What is the name of the industrial process used to manufacture ammonia? Haber [1] (Bosch) process : b) Ammonia is prepared industrially from nitrogen and hydrogen gases. The equation for the reaction is: N2 + 3H2 ? 2NH3(i) What is the name of the industrial process used to manufacture ammonia? Haber [1] (Bosch) process

Slide 76 : 76 Haber-Bosch Process Source:IB

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(ii) Give the temperature and pressure which are used in this process. Temperature __________?C [1] Pressure _____________ atmospheres [1](iii) What catalyst is used for this process? _______________________________ [1] : (ii) Give the temperature and pressure which are used in this process. Temperature __________?C [1] Pressure _____________ atmospheres [1](iii) What catalyst is used for this process? _______________________________ [1]

(ii) Give the temperature and pressure which are used in this process. Temperature 450?C (accept 350-500) [1] Pressure 250 atmospheres [1] (accept 200- 1000) (iii) What catalyst is used for this process? Iron [1] : (ii) Give the temperature and pressure which are used in this process. Temperature 450?C (accept 350-500) [1] Pressure 250 atmospheres [1] (accept 200- 1000) (iii) What catalyst is used for this process? Iron [1]

Slide 80 : 80 Influence of Temperature and Pressure on the % Yield N2(g) + 3 H2(g) ? 2 NH3(g) Energy Change = – 76 kJ/mol

Ammonia : P block group V 81 Ammonia The formula is NH3 Lone pair not involved in bonding Can dative bond with a H+ ion to form an ammonium ion

Ammonia : P block group V 82 Ammonia NH3 + H2O = NH4OH Depending on the circumstance we may represent ammonia solution as either: - NH3(aq) or NH4OH(aq) -

c) Give a chemical test for ammonia and the observations you would make if ammonia was present. Test: ______________________ [1] Observations: __________________ __________________________ [2] : c) Give a chemical test for ammonia and the observations you would make if ammonia was present. Test: ______________________ [1] Observations: __________________ __________________________ [2]

c) Give a chemical test for ammonia and the observations you would make if ammonia was present. Test: Hydrogen chloride [1] Observations: white [1] fumes / cloud / smoke [1] : c) Give a chemical test for ammonia and the observations you would make if ammonia was present. Test: Hydrogen chloride [1] Observations: white [1] fumes / cloud / smoke [1]

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Slide 86 : 86 Manufacture of Hydrogen Chloride. 2NaCl + H2SO4 ? NaHSO4 + HCl sodium sulphuric sodium hydrogen chloride acid hydrogen chloride chloride

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d) Ammonia is an alkaline gas and it reacts readily with dilute sulphuric acid to produce a solution of ammonium sulphate.(i) Describe the test you would carry out to confirm the presence of the sulphate ion. Name of reagent used: ____________ [1] Result of test: ______________________ _______________________________ [2] : d) Ammonia is an alkaline gas and it reacts readily with dilute sulphuric acid to produce a solution of ammonium sulphate.(i) Describe the test you would carry out to confirm the presence of the sulphate ion. Name of reagent used: ____________ [1] Result of test: ______________________ _______________________________ [2]

Slide 89 : 89 Complete Formula Equation:    BaCl2(aq) + CuSO4(aq) BaSO4(s) + CuCl2(aq) Complete Ionic Equation:        Ba2+(aq) +2 Cl-(aq) + Cu2+(aq) +SO42-(aq) = BaSO4(s) + Cu2+(aq) +2 Cl-(aq) Establishing the Net Ionic Equation:                Ba2+ + 2 Cl- + Cu2+ + SO42-  = BaSO4(s) + Cu2+ + 2 Cl-                                              Ba2+(aq) + SO42-(aq) BaSO4(s) White ppt BaCl2 CuSO4

d) Ammonia is an alkaline gas and it reacts readily with dilute sulphuric acid to produce a solution of ammonium sulphate.(i) Describe the test you would carry out to confirm the presence of the sulphate ion. Name of reagent used: barium chloride [1] Result of test: white [1] ppt [1] : d) Ammonia is an alkaline gas and it reacts readily with dilute sulphuric acid to produce a solution of ammonium sulphate.(i) Describe the test you would carry out to confirm the presence of the sulphate ion. Name of reagent used: barium chloride [1] Result of test: white [1] ppt [1]

(ii) Ammonia sulphate reacts with sodium hydroxide when heated. Write a balanced equation for the reaction. ___________________________ [2] : (ii) Ammonia sulphate reacts with sodium hydroxide when heated. Write a balanced equation for the reaction. ___________________________ [2]

(ii) Ammonia sulphate reacts with sodium hydroxide when heated. Write a balanced equation for the reaction. (NH4)2 SO4 + 2NaOH ? Na2 SO4 + 2NH3 + 2H2O [2] : (ii) Ammonia sulphate reacts with sodium hydroxide when heated. Write a balanced equation for the reaction. (NH4)2 SO4 + 2NaOH ? Na2 SO4 + 2NH3 + 2H2O [2]

e) Ammonia dissolves readily in water to form aqueous ammonia. Aqueous ammonia is used to test for metal cations in solution.(i) What would you observe if aqueous ammonia was added dropwise to a solution of copper (II) sulphate CuSO4(aq)? __________________________________ _______________________________ [2] : e) Ammonia dissolves readily in water to form aqueous ammonia. Aqueous ammonia is used to test for metal cations in solution.(i) What would you observe if aqueous ammonia was added dropwise to a solution of copper (II) sulphate CuSO4(aq)? __________________________________ _______________________________ [2]

e) Ammonia dissolves readily in water to form aqueous ammonia. Aqueous ammonia is used to test for metal cations in solution.(i) What would you observe if aqueous ammonia was added dropwise to a solution of copper (II) sulphate CuSO4(aq)? Blue [1] ppt [1] : e) Ammonia dissolves readily in water to form aqueous ammonia. Aqueous ammonia is used to test for metal cations in solution.(i) What would you observe if aqueous ammonia was added dropwise to a solution of copper (II) sulphate CuSO4(aq)? Blue [1] ppt [1]

(ii) What further observations would you make if an excess of aqueous ammonia was added? _____________________________ ___________________________ [3] : (ii) What further observations would you make if an excess of aqueous ammonia was added? _____________________________ ___________________________ [3]

(ii) What further observations would you make if an excess of aqueous ammonia was added? ppt re-dissolves [1] dark [1] blue [1] solution [1] : (ii) What further observations would you make if an excess of aqueous ammonia was added? ppt re-dissolves [1] dark [1] blue [1] solution [1]

4a) Ammonia is used in many household cleaning products. It has a very strong penetrating smell. State two other physical properties of ammonia. __________________________ [2] : 4a) Ammonia is used in many household cleaning products. It has a very strong penetrating smell. State two other physical properties of ammonia. __________________________ [2] 2003, Paper 2

4a) Ammonia is used in many household cleaning products. It has a very strong penetrating smell. State two other physical properties of ammonia. Gas / low melting point / low boiling point [1] Higher than air [1] (very) soluble in water [1] colourless [1] Max [2] : 4a) Ammonia is used in many household cleaning products. It has a very strong penetrating smell. State two other physical properties of ammonia. Gas / low melting point / low boiling point [1] Higher than air [1] (very) soluble in water [1] colourless [1] Max [2]

b) The diagram shows some of the essential reactions and industrial processes associated with ammonia. : b) The diagram shows some of the essential reactions and industrial processes associated with ammonia.

(i) Describe a chemical test for ammonia, giving the result of the test. _____________________________ ___________________________ [3](ii) Name the compound A. ___________________________ [1] : (i) Describe a chemical test for ammonia, giving the result of the test. _____________________________ ___________________________ [3](ii) Name the compound A. ___________________________ [1]

(i) Describe a chemical test for ammonia, giving the result of the test. Hydrogen chloride / concentrated hydrochloric acid [1] white [1] smoke/fumes/solid [1] (ii) Name the compound A. Ammonium Chloride [1] : (i) Describe a chemical test for ammonia, giving the result of the test. Hydrogen chloride / concentrated hydrochloric acid [1] white [1] smoke/fumes/solid [1] (ii) Name the compound A. Ammonium Chloride [1]

(iii) Describe the production of ammonia in the Haber-Bosch process. Your answer should include the name of the catalyst used, the approximate temperature and pressure and a balanced, symbol equation. __________________________________ __________________________________ __________________________________ ______________________________ [7] : (iii) Describe the production of ammonia in the Haber-Bosch process. Your answer should include the name of the catalyst used, the approximate temperature and pressure and a balanced, symbol equation. __________________________________ __________________________________ __________________________________ ______________________________ [7]

(iii) Describe the production of ammonia in the Haber-Bosch process. Your answer should include the name of the catalyst used, the approximate temperature and pressure and a balanced, symbol equation. The key points of this answer are: nitrogen [1] hydrogen [1] catalyst = iron [1], temperature = 450oC [1], pressure = 200 atm [1], N2 + 3H2 ? 2NH3 [2] reversible arrow not essential Cool to liquify ammonia [1] Unreacted gases recycled [1] Max [7] from [9] but some parts marked essential : (iii) Describe the production of ammonia in the Haber-Bosch process. Your answer should include the name of the catalyst used, the approximate temperature and pressure and a balanced, symbol equation. The key points of this answer are: nitrogen [1] hydrogen [1] catalyst = iron [1], temperature = 450oC [1], pressure = 200 atm [1], N2 + 3H2 ? 2NH3 [2] reversible arrow not essential Cool to liquify ammonia [1] Unreacted gases recycled [1] Max [7] from [9] but some parts marked essential

c) Garden lawn fertiliser often contains ammonium nitrate in addition to iron(II) sulphate, which is used to kill moss. (i) write a balanced, symbol equation for the reaction of ammonia and nitric acid to produce ammonium nitrate. ___________________________ [2] : c) Garden lawn fertiliser often contains ammonium nitrate in addition to iron(II) sulphate, which is used to kill moss. (i) write a balanced, symbol equation for the reaction of ammonia and nitric acid to produce ammonium nitrate. ___________________________ [2]

c) Garden lawn fertiliser often contains ammonium nitrate in addition to iron(II) sulphate, which is used to kill moss. (i) write a balanced, symbol equation for the reaction of ammonia and nitric acid to produce ammonium nitrate. NH3 + HNO3 ? NH4NO3 [2] : c) Garden lawn fertiliser often contains ammonium nitrate in addition to iron(II) sulphate, which is used to kill moss. (i) write a balanced, symbol equation for the reaction of ammonia and nitric acid to produce ammonium nitrate. NH3 + HNO3 ? NH4NO3 [2]

(ii) Describe, giving practical details, how you would prove that lawn fertiliser pellets contain iron(II) sulphate and not iron(III) sulphate. Give the expected result. _____________________________ _____________________________ __________________________ [5] : (ii) Describe, giving practical details, how you would prove that lawn fertiliser pellets contain iron(II) sulphate and not iron(III) sulphate. Give the expected result. _____________________________ _____________________________ __________________________ [5]

(ii) Describe, giving practical details, how you would prove that lawn fertiliser pellets contain iron(II) sulphate and not iron(III) sulphate. Give the expected result. Add water [1], add ammonia solution/NaOH solution [1], green [1], ppt [1], red brown (ppt) indicates Fe3+ [1] : (ii) Describe, giving practical details, how you would prove that lawn fertiliser pellets contain iron(II) sulphate and not iron(III) sulphate. Give the expected result. Add water [1], add ammonia solution/NaOH solution [1], green [1], ppt [1], red brown (ppt) indicates Fe3+ [1]

(iii) State two environmental problems which occur when excess fertiliser is leached out of the soil and into lakes and rivers. _____________________________ __________________________ [2] : (iii) State two environmental problems which occur when excess fertiliser is leached out of the soil and into lakes and rivers. _____________________________ __________________________ [2]

(iii) State two environmental problems which occur when excess fertiliser is leached out of the soil and into lakes and rivers. Eutrophication [1] Contamination of water supply [1] : (iii) State two environmental problems which occur when excess fertiliser is leached out of the soil and into lakes and rivers. Eutrophication [1] Contamination of water supply [1]

Slide 110 : 110 From our “Learning Outcomes”

d) Ammonia is used to manufacture nitric acid. This process involves the catalytic oxidation of ammonia and occurs in three stages. Stage 1 _____________________ Stage 2 _____________________ Stage 3 _____________________[6] : d) Ammonia is used to manufacture nitric acid. This process involves the catalytic oxidation of ammonia and occurs in three stages. Stage 1 _____________________ Stage 2 _____________________ Stage 3 _____________________[6]

Slide 112 : 112

Slide 113 : 113

d) Ammonia is used to manufacture nitric acid. This process involves the catalytic oxidation of ammonia and occurs in three stages. Stage 1 4NH3 + 5O2 ? 4NO + 6H2O Stage 2 2NO + O2 ? 2NO2 Stage 3 4NO2 + O2 + 2H2O ? 4HNO3 : d) Ammonia is used to manufacture nitric acid. This process involves the catalytic oxidation of ammonia and occurs in three stages. Stage 1 4NH3 + 5O2 ? 4NO + 6H2O Stage 2 2NO + O2 ? 2NO2 Stage 3 4NO2 + O2 + 2H2O ? 4HNO3

Slide 115 : 115 4NO2 + O2 + 2H2O ? 4HNO3

(ii) Name the material used as a catalyst in this process. ___________________________ [1](iii) Which stage, 1, 2 or 3 involves use of the catalyst? ___________________________ [1] : (ii) Name the material used as a catalyst in this process. ___________________________ [1](iii) Which stage, 1, 2 or 3 involves use of the catalyst? ___________________________ [1]

Slide 117 : 117

(ii) Name the material used as a catalyst in this process.Platinum /platinum-rhodium [1](iii) Which stage, 1, 2 or 3 involves use of the catalyst? Stage 1 [1] : (ii) Name the material used as a catalyst in this process.Platinum /platinum-rhodium [1](iii) Which stage, 1, 2 or 3 involves use of the catalyst? Stage 1 [1]

4a) Air is a mixture of nitrogen, oxygen, carbon dioxide, water vapour and noble gases. The diagram below shows how an impure sample of nitrogen gas may be prepared from air. The conical flask containing the sodium hydroxide is used to absorb carbon dioxide from the air. : 4a) Air is a mixture of nitrogen, oxygen, carbon dioxide, water vapour and noble gases. The diagram below shows how an impure sample of nitrogen gas may be prepared from air. The conical flask containing the sodium hydroxide is used to absorb carbon dioxide from the air. 2005, Paper 1

Slide 120 : 120

Slide 121 : 121 Industrial preparation of Nitrogen, Oxygen, Argon and other gases

Slide 122 : 122 Finding the fraction of Normal Air that is Oxygen

(i) Write a balanced symbol equation for the reaction of carbon dioxide with sodium hydroxide solution. _______________________________ _______________________________ [3] : (i) Write a balanced symbol equation for the reaction of carbon dioxide with sodium hydroxide solution. _______________________________ _______________________________ [3]

Slide 124 : 124 NaOH pellets. They begin to glisten within a minute and within several hours have turned to a solution of sodium carbonate. A few days later a white solid remains - Na2CO3 CO2 + 2NaOH ? Na2CO3 + H2O

(i) Write a balanced symbol equation for the reaction of carbon dioxide with sodium hydroxide solution. CO2 + 2NaOH ? Na2CO3 + H2O [3] : (i) Write a balanced symbol equation for the reaction of carbon dioxide with sodium hydroxide solution. CO2 + 2NaOH ? Na2CO3 + H2O [3]

Slide 126 : 126 Industrial Sources of CO2

(ii) What is the purpose of the heated copper in the diagram. _______________________________ _______________________________ [2](iii) Name one impurity in the gas collected. _______________________________ [1] : (ii) What is the purpose of the heated copper in the diagram. _______________________________ _______________________________ [2](iii) Name one impurity in the gas collected. _______________________________ [1]

(ii) What is the purpose of the heated copper in the diagram. Remove [1] oxygen [1] [2](iii) Name one impurity in the gas collected. Argon/neon/helium/krypton/water vapour Any one [1] : (ii) What is the purpose of the heated copper in the diagram. Remove [1] oxygen [1] [2](iii) Name one impurity in the gas collected. Argon/neon/helium/krypton/water vapour Any one [1]

b) Nitrogen can be converted into ammonia in the Haber-Bosch Process through a reaction with hydrogen gas.(i) Write a balanced symbol equation for the production of ammonia gas in the Haber- Bosch Process. _______________________________ _______________________________ [3] : b) Nitrogen can be converted into ammonia in the Haber-Bosch Process through a reaction with hydrogen gas.(i) Write a balanced symbol equation for the production of ammonia gas in the Haber- Bosch Process. _______________________________ _______________________________ [3]

b) Nitrogen can be converted into ammonia in the Haber-Bosch Process through a reaction with hydrogen gas.(i) Write a balanced symbol equation for the production of ammonia gas in the Haber- Bosch Process. N2 + 3H2 ? 2NH3 [3] : b) Nitrogen can be converted into ammonia in the Haber-Bosch Process through a reaction with hydrogen gas.(i) Write a balanced symbol equation for the production of ammonia gas in the Haber- Bosch Process. N2 + 3H2 ? 2NH3 [3]

(ii) Complete the table below to give the operating conditions which are used in the Haber-Bosch Process. : (ii) Complete the table below to give the operating conditions which are used in the Haber-Bosch Process.

(ii) Complete the table below to give the operating conditions which are used in the Haber-Bosch Process. : (ii) Complete the table below to give the operating conditions which are used in the Haber-Bosch Process.

c) Ammonia may be prepared by heating ammonium chloride with solid calcium hydroxide and collecting the gas as shown in the diagram. : c) Ammonia may be prepared by heating ammonium chloride with solid calcium hydroxide and collecting the gas as shown in the diagram.

(i) Suggest why ammonia gas is collected in the way shown. _______________________________ [1](ii) Write a balanced symbol equation for the reaction of ammonium chloride with calcium hydroxide. _______________________________ [3] : (i) Suggest why ammonia gas is collected in the way shown. _______________________________ [1](ii) Write a balanced symbol equation for the reaction of ammonium chloride with calcium hydroxide. _______________________________ [3]

(i) Suggest why ammonia gas is collected in the way shown. Less dense than air [1](ii) Write a balanced symbol equation for the reaction of ammonium chloride with calcium hydroxide. 2NH4Cl + Ca(OH)2 ? 2NH3 + CaCl2 + 2H2O [3] : (i) Suggest why ammonia gas is collected in the way shown. Less dense than air [1](ii) Write a balanced symbol equation for the reaction of ammonium chloride with calcium hydroxide. 2NH4Cl + Ca(OH)2 ? 2NH3 + CaCl2 + 2H2O [3]

(iii) A glass rod, dipped in concentrated hydrochloric acid is held under test tube A. What observations would you make? _______________________________ [2] : (iii) A glass rod, dipped in concentrated hydrochloric acid is held under test tube A. What observations would you make? _______________________________ [2]

(iii) A glass rod, dipped in concentrated hydrochloric acid is held under test tube A. What observations would you make? White [1] fumes / smoke [1] [2] : (iii) A glass rod, dipped in concentrated hydrochloric acid is held under test tube A. What observations would you make? White [1] fumes / smoke [1] [2]

d) Ammonia solution is used to detect the presence of metal cations in solution.(i) Describe what would be observed when ammonia solution is added slowly until it is in excess to a solution copper(II) sulphate. _______________________________ _______________________________ _______________________________ [4] : d) Ammonia solution is used to detect the presence of metal cations in solution.(i) Describe what would be observed when ammonia solution is added slowly until it is in excess to a solution copper(II) sulphate. _______________________________ _______________________________ _______________________________ [4]

4a) Chlorine gas can be prepared in the laboratory using concentrated hydrochloric acid. The reaction can be represented by the equation. 2HCl + [O] ? H2O +Cl2(i) State the name and type of substance represented by [O]. Name: ____________________________ Type: __________________________ [2] : 4a) Chlorine gas can be prepared in the laboratory using concentrated hydrochloric acid. The reaction can be represented by the equation. 2HCl + [O] ? H2O +Cl2(i) State the name and type of substance represented by [O]. Name: ____________________________ Type: __________________________ [2]

Slide 140 : 140

4a) Chlorine gas can be prepared in the laboratory using concentrated hydrochloric acid. The reaction can be represented by the equation. 2HCl + [O] ? H2O +Cl2(i) State the name and type of substance represented by [O]. Potassium permanganate / manganese dioxide [1] oxidising agent [1] : 4a) Chlorine gas can be prepared in the laboratory using concentrated hydrochloric acid. The reaction can be represented by the equation. 2HCl + [O] ? H2O +Cl2(i) State the name and type of substance represented by [O]. Potassium permanganate / manganese dioxide [1] oxidising agent [1]

(ii) Describe the appearance of the chlorine gas produced. _______________________________ [1]b) In industry, chlorine can be produced by the electrolysis of concentrated sodium chloride solution using carbon electrodes.(i) State the electrode at which chlorine is produced. _______________________________ [1] : (ii) Describe the appearance of the chlorine gas produced. _______________________________ [1]b) In industry, chlorine can be produced by the electrolysis of concentrated sodium chloride solution using carbon electrodes.(i) State the electrode at which chlorine is produced. _______________________________ [1]

(ii) Describe the appearance of the chlorine gas produced. Green [1]b) In industry, chlorine can be produced by the electrolysis of concentrated sodium chloride solution using carbon electrodes.(i) State the electrode at which chlorine is produced. Anode [1] : (ii) Describe the appearance of the chlorine gas produced. Green [1]b) In industry, chlorine can be produced by the electrolysis of concentrated sodium chloride solution using carbon electrodes.(i) State the electrode at which chlorine is produced. Anode [1]

(ii) The electrodes cannot be made from iron, since iron reacts with chlorine. Write a balanced symbol equation for the reaction of iron with chlorine. _______________________________ [1] : (ii) The electrodes cannot be made from iron, since iron reacts with chlorine. Write a balanced symbol equation for the reaction of iron with chlorine. _______________________________ [1]

(ii) The electrodes cannot be made from iron, since iron reacts with chlorine. Write a balanced symbol equation for the reaction of iron with chlorine. 2Fe + 2Cl2 ? 2FeCl3 [1] [1] [1] +[1] for balancing : (ii) The electrodes cannot be made from iron, since iron reacts with chlorine. Write a balanced symbol equation for the reaction of iron with chlorine. 2Fe + 2Cl2 ? 2FeCl3 [1] [1] [1] +[1] for balancing

c) Chlorine is a reactive gas. Write balanced symbol equations and give the observations for the following reactions.(i) Chlorine + sodium hydroxide solution. Equation: _______________________ [3] Observations: ____________________ [1] : c) Chlorine is a reactive gas. Write balanced symbol equations and give the observations for the following reactions.(i) Chlorine + sodium hydroxide solution. Equation: _______________________ [3] Observations: ____________________ [1]

c) Chlorine is a reactive gas. Write balanced symbol equations and give the observations for the following reactions.(i) Chlorine + sodium hydroxide solution. Equation: Cl2 + 2NaOH ? NaCl + NaOCl + H2O [1] [1] +[1] for balancing [3] Observations: Heat evolved/temperature increases, smell of bleach [1], yellow/green colour fades [1], colourless solution [1] (Maximum [1]) : c) Chlorine is a reactive gas. Write balanced symbol equations and give the observations for the following reactions.(i) Chlorine + sodium hydroxide solution. Equation: Cl2 + 2NaOH ? NaCl + NaOCl + H2O [1] [1] +[1] for balancing [3] Observations: Heat evolved/temperature increases, smell of bleach [1], yellow/green colour fades [1], colourless solution [1] (Maximum [1])

(ii) Chlorine + sodium bromide solution Equation: _______________________ [3] Observations: ____________________ [2] : (ii) Chlorine + sodium bromide solution Equation: _______________________ [3] Observations: ____________________ [2]

Slide 149 : 149

Slide 150 : 150 2NaI(aq) + Br2(g) ?    2NaCl(aq) + I2(aq) ?

(ii) Chlorine + sodium bromide solution Equation: Cl2 + 2NaBr ? Br2 + 2NaCl [1] [1] + [1] for balancing [3] Observations: Colourless solution [1], changes to red brown [1], yellow/green colour disappears [1] (Maximum [2]) : (ii) Chlorine + sodium bromide solution Equation: Cl2 + 2NaBr ? Br2 + 2NaCl [1] [1] + [1] for balancing [3] Observations: Colourless solution [1], changes to red brown [1], yellow/green colour disappears [1] (Maximum [2])

d) Large amounts of liquid chlorine are transported in tankers by road to water treatment works.(i) How is the chlorine gas turned into liquid chlorine? _______________________________ [1](ii) Why is chlorine transported as a liquid and not as a gas? _______________________________ [1] : d) Large amounts of liquid chlorine are transported in tankers by road to water treatment works.(i) How is the chlorine gas turned into liquid chlorine? _______________________________ [1](ii) Why is chlorine transported as a liquid and not as a gas? _______________________________ [1]

d) Large amounts of liquid chlorine are transported in tankers by road to water treatment works.(i) How is the chlorine gas turned into liquid chlorine? Cooled/pressure applied [1](ii) Why is chlorine transported as a liquid and not as a gas? Ease of transportation/takes up less space [1] : d) Large amounts of liquid chlorine are transported in tankers by road to water treatment works.(i) How is the chlorine gas turned into liquid chlorine? Cooled/pressure applied [1](ii) Why is chlorine transported as a liquid and not as a gas? Ease of transportation/takes up less space [1]

Every tanker transporting chlorine must have a Hazchem warning label as shown below. : Every tanker transporting chlorine must have a Hazchem warning label as shown below.

(iii) What word is missing from Box A on the Hazchem label to describe the hazard associated with chlorine? _______________________________ [1](iv) Why are small amounts of chlorine added to water at the water treatment works? _______________________________ [1] : (iii) What word is missing from Box A on the Hazchem label to describe the hazard associated with chlorine? _______________________________ [1](iv) Why are small amounts of chlorine added to water at the water treatment works? _______________________________ [1]

(iii) What word is missing from Box A on the Hazchem label to describe the hazard associated with chlorine? Toxic [1](iv) Why are small amounts of chlorine added to water at the water treatment works? Kills [1] germs, microbes, bacteria [1] or sterilise [2] : (iii) What word is missing from Box A on the Hazchem label to describe the hazard associated with chlorine? Toxic [1](iv) Why are small amounts of chlorine added to water at the water treatment works? Kills [1] germs, microbes, bacteria [1] or sterilise [2]

(v) Give another use of chlorine. _______________________________ [1] : (v) Give another use of chlorine. _______________________________ [1]

(v) Give another use of chlorine. Bleach (for cotton, lined, wood pulp)/PVC manufacture [1] : (v) Give another use of chlorine. Bleach (for cotton, lined, wood pulp)/PVC manufacture [1]

e) Hydrochloric acid can also be transported by road in tankers. The tanker has the Hazchem warning label shown below. : e) Hydrochloric acid can also be transported by road in tankers. The tanker has the Hazchem warning label shown below.

(i) What is the word missing from Box B on this Haschem label to describe the hazard associated with hydrochloric acid? _______________________________ [1](ii) Hydrocholoric acid can be made by using sodium chloride. What other substance reacts with sodium chloride to produce hydrogen chloride gas? _______________________________ [2] : (i) What is the word missing from Box B on this Haschem label to describe the hazard associated with hydrochloric acid? _______________________________ [1](ii) Hydrocholoric acid can be made by using sodium chloride. What other substance reacts with sodium chloride to produce hydrogen chloride gas? _______________________________ [2]

Slide 161 : 161 2NaCl(s) + H2SO4(l) ? NaHSO4(aq) + HCl(g) HCl(g) (add water) ? HCl(aq)

(i) What is the word missing from Box B on this Haschem label to describe the hazard associated with hydrochloric acid? Corrosive [1](ii) Hydrocholoric acid can be made by using sodium chloride. What other substance reacts with sodium chloride to produce hydrogen chloride gas? Concentrated [1] sulphuric acid [1] [2] : (i) What is the word missing from Box B on this Haschem label to describe the hazard associated with hydrochloric acid? Corrosive [1](ii) Hydrocholoric acid can be made by using sodium chloride. What other substance reacts with sodium chloride to produce hydrogen chloride gas? Concentrated [1] sulphuric acid [1] [2]

(iii) Describe the test for hydrogen chloride gas and give the expected result. _______________________________ _______________________________ _______________________________ _______________________________ [4] : (iii) Describe the test for hydrogen chloride gas and give the expected result. _______________________________ _______________________________ _______________________________ _______________________________ [4]

(iii) Describe the test for hydrogen chloride gas and give the expected result. Glass rod [1] dipped in concentrated [1] ammonia [1] white [1] fumes/smoke [1] (Maximum [4]) : (iii) Describe the test for hydrogen chloride gas and give the expected result. Glass rod [1] dipped in concentrated [1] ammonia [1] white [1] fumes/smoke [1] (Maximum [4])

1 In the laboratory, a student carried out experiments using the elements sulphur and magnesium.a) Complete the table below, stating the colour of each element. : 1 In the laboratory, a student carried out experiments using the elements sulphur and magnesium.a) Complete the table below, stating the colour of each element. 2007, Paper 2

1 In the laboratory, a student carried out experiments using the elements sulphur and magnesium.a) Complete the table below, stating the colour of each element. : 1 In the laboratory, a student carried out experiments using the elements sulphur and magnesium.a) Complete the table below, stating the colour of each element.

b) The student burned some sulphur and then some magnesium in air. Complete the table below, giving observations which occur during heating and describe the products of each reaction. : b) The student burned some sulphur and then some magnesium in air. Complete the table below, giving observations which occur during heating and describe the products of each reaction.

b) The student burned some sulphur and then some magnesium in air. Complete the table below, giving observations which occur during heating and describe the products of each reaction. : b) The student burned some sulphur and then some magnesium in air. Complete the table below, giving observations which occur during heating and describe the products of each reaction.

c) Write balanced symbol equations for the following reactions:(i) Sulphur burning in air _______________________________ [2](ii) Magnesium burning in air _______________________________ [3] : c) Write balanced symbol equations for the following reactions:(i) Sulphur burning in air _______________________________ [2](ii) Magnesium burning in air _______________________________ [3]

c) Write balanced symbol equations for the following reactions:(i) Sulphur burning in air S + O2 ? SO2 [2] [1] [1](ii) Magnesium burning in air 2Mg + O2 ? 2MgO [3] [1] [1] +[1] for balancing : c) Write balanced symbol equations for the following reactions:(i) Sulphur burning in air S + O2 ? SO2 [2] [1] [1](ii) Magnesium burning in air 2Mg + O2 ? 2MgO [3] [1] [1] +[1] for balancing

d) Many laboratory reactions involve oxidation.(i) Explain why the burning of sulphur in air is an oxidation reaction. _______________________________ _______________________________ [2] : d) Many laboratory reactions involve oxidation.(i) Explain why the burning of sulphur in air is an oxidation reaction. _______________________________ _______________________________ [2]

d) Many laboratory reactions involve oxidation.(i) Explain why the burning of sulphur in air is an oxidation reaction. Sulphur gains oxygen [1] gain of oxygen is oxidation [1] [2] : d) Many laboratory reactions involve oxidation.(i) Explain why the burning of sulphur in air is an oxidation reaction. Sulphur gains oxygen [1] gain of oxygen is oxidation [1] [2]

e) Most fossil fuels contain sulphur impurities. When these fossil fuels burn the sulphur is oxidised to sulphur dioxide.(i) Write a balanced symbol equation for the oxidation of sulphur to sulphur dioxide. _______________________________ [2] : e) Most fossil fuels contain sulphur impurities. When these fossil fuels burn the sulphur is oxidised to sulphur dioxide.(i) Write a balanced symbol equation for the oxidation of sulphur to sulphur dioxide. _______________________________ [2]

e) Most fossil fuels contain sulphur impurities. When these fossil fuels burn the sulphur is oxidised to sulphur dioxide.(i) Write a balanced symbol equation for the oxidation of sulphur to sulphur dioxide. S + O2 ? SO2 [2] : e) Most fossil fuels contain sulphur impurities. When these fossil fuels burn the sulphur is oxidised to sulphur dioxide.(i) Write a balanced symbol equation for the oxidation of sulphur to sulphur dioxide. S + O2 ? SO2 [2]

Sulphur dioxide leads to the formation of acid rain. (ii) What are the three main harmful effects of acid rain? _______________________________ _______________________________ _______________________________ [3] : Sulphur dioxide leads to the formation of acid rain. (ii) What are the three main harmful effects of acid rain? _______________________________ _______________________________ _______________________________ [3]

Sulphur dioxide leads to the formation of acid rain. (ii) What are the three main harmful effects of acid rain? Trees damaged/killed [1], fish killed/harmed, buildings/statues corroded [1] [3] : Sulphur dioxide leads to the formation of acid rain. (ii) What are the three main harmful effects of acid rain? Trees damaged/killed [1], fish killed/harmed, buildings/statues corroded [1] [3]

(iii) Give two measures which can be taken to reduce the formation of acid rain. _______________________________ _______________________________ _______________________________ _______________________________ [2] : (iii) Give two measures which can be taken to reduce the formation of acid rain. _______________________________ _______________________________ _______________________________ _______________________________ [2]

(iii) Give two measures which can be taken to reduce the formation of acid rain. Burn less fossil fuels [1], remove sulphur from fuels [1], alternative energy forms [1], remove acidic gases from power station emissions [1], catalytic converters in cars [1] (Max [2]) [2] : (iii) Give two measures which can be taken to reduce the formation of acid rain. Burn less fossil fuels [1], remove sulphur from fuels [1], alternative energy forms [1], remove acidic gases from power station emissions [1], catalytic converters in cars [1] (Max [2]) [2]

6a) The quantity of sulphuric acid produced by a country has been linked to economic stability.(i) Name the industrial process used to produce sulphuric acid. _______________________________ [1] : 6a) The quantity of sulphuric acid produced by a country has been linked to economic stability.(i) Name the industrial process used to produce sulphuric acid. _______________________________ [1] 2007, Paper 2

Slide 180 : 180 Sulphuric Acid Plant

Slide 181 : 181 + H2SO4 H2SO4 H2S2O7 + H2O

6a) The quantity of sulphuric acid produced by a country has been linked to economic stability.(i) Name the industrial process used to produce sulphuric acid. Contact [1] process [1] : 6a) The quantity of sulphuric acid produced by a country has been linked to economic stability.(i) Name the industrial process used to produce sulphuric acid. Contact [1] process [1]

(ii) Complete the table below to give the operating conditions which are used in the industrial manufacture of sulphuric acid. : (ii) Complete the table below to give the operating conditions which are used in the industrial manufacture of sulphuric acid.

(ii) Complete the table below to give the operating conditions which are used in the industrial manufacture of sulphuric acid. : (ii) Complete the table below to give the operating conditions which are used in the industrial manufacture of sulphuric acid.

(iii) The sulphuric acid obtained in this process is concentrated. Describe in detail how a sample of concentrated acid should be safely diluted using water. _______________________________ _______________________________ _______________________________ [3] : (iii) The sulphuric acid obtained in this process is concentrated. Describe in detail how a sample of concentrated acid should be safely diluted using water. _______________________________ _______________________________ _______________________________ [3]

(iii) The sulphuric acid obtained in this process is concentrated. Describe in detail how a sample of concentrated acid should be safely diluted using water.Safety glasses / gloves [1]add acid to water [1] (essential) dropwise/slowly [1]with stirring [1]. Maximum [3] : (iii) The sulphuric acid obtained in this process is concentrated. Describe in detail how a sample of concentrated acid should be safely diluted using water.Safety glasses / gloves [1]add acid to water [1] (essential) dropwise/slowly [1]with stirring [1]. Maximum [3]

b) Some of the reactions of concentrated sulphuric acid are summarised in the diagram below. : b) Some of the reactions of concentrated sulphuric acid are summarised in the diagram below.

(i) Identify Solid A and Gas B. Solid A _________________________ [1] Gas B __________________________ [1](ii) What would you observe during Reaction 1? _______________________________ _______________________________ [3] : (i) Identify Solid A and Gas B. Solid A _________________________ [1] Gas B __________________________ [1](ii) What would you observe during Reaction 1? _______________________________ _______________________________ [3]

(i) Identify Solid Carbon / Charcoal [1] Gas B Steam / Water [1](ii) What would you observe during Reaction 1? Solid rises up/swells [1] heat/warms up [1] pungent/caramel smell [1] reaction not immediate. Maximum [3] A and Gas B. Solid A : (i) Identify Solid Carbon / Charcoal [1] Gas B Steam / Water [1](ii) What would you observe during Reaction 1? Solid rises up/swells [1] heat/warms up [1] pungent/caramel smell [1] reaction not immediate. Maximum [3] A and Gas B. Solid A

(iii) Name the white powder C. _______________________________ [1](iv) What property of concentrated sulphuric acid is demonstrated in Reactions 1 and 2? _______________________________ [1] : (iii) Name the white powder C. _______________________________ [1](iv) What property of concentrated sulphuric acid is demonstrated in Reactions 1 and 2? _______________________________ [1]

Slide 191 : 191 From our “learning Outcomes”

(iii) Name the white powder C. anhydrous [1] copper(II) sulphate [1](iv) What property of concentrated sulphuric acid is demonstrated in Reactions 1 and 2? Dehydrating [1] : (iii) Name the white powder C. anhydrous [1] copper(II) sulphate [1](iv) What property of concentrated sulphuric acid is demonstrated in Reactions 1 and 2? Dehydrating [1]

(v) Write a balanced symbol equation for Reaction 3. _______________________________ [2] : (v) Write a balanced symbol equation for Reaction 3. _______________________________ [2]

(v) Write a balanced symbol equation for Reaction 3. H2SO4 + NaCl ? NaHSO4 + HCl [2] : (v) Write a balanced symbol equation for Reaction 3. H2SO4 + NaCl ? NaHSO4 + HCl [2]

(vi) Describe how you would carry out a chemical test for the presence of hydrogen chloride gas, stating the observations you would make for a positive test. Test: _____________________________ _________________________________ Observations: ______________________ _______________________________ [4] : (vi) Describe how you would carry out a chemical test for the presence of hydrogen chloride gas, stating the observations you would make for a positive test. Test: _____________________________ _________________________________ Observations: ______________________ _______________________________ [4]

(vi) Describe how you would carry out a chemical test for the presence of hydrogen chloride gas, stating the observations you would make for a positive test. Test: glass rod [1] dipped in concentrated [1] ammonia [1] Observations: White [1] smoke [1] (Maximum [4]) : (vi) Describe how you would carry out a chemical test for the presence of hydrogen chloride gas, stating the observations you would make for a positive test. Test: glass rod [1] dipped in concentrated [1] ammonia [1] Observations: White [1] smoke [1] (Maximum [4])

7 Sulphuric acid is used in the production of many chemicals. It is used to make ammonium sulphate, an important fertiliser.a) Write a balanced symbol equation for the reaction of sulphuric acid with ammonia to produce ammonium sulphate. _______________________________ [3] : 7 Sulphuric acid is used in the production of many chemicals. It is used to make ammonium sulphate, an important fertiliser.a) Write a balanced symbol equation for the reaction of sulphuric acid with ammonia to produce ammonium sulphate. _______________________________ [3] 2007, Paper 2

7 Sulphuric acid is used in the production of many chemicals. It is used to make ammonium sulphate, an important fertiliser. a) Write a balanced symbol equation for the reaction of sulphuric acid with ammonia to produce ammonium sulphate. 2NH3 + H2SO4 ? (NH4)2SO4 [3] [1] [1] +[1] for balancing. Accept equation using NH4OH : 7 Sulphuric acid is used in the production of many chemicals. It is used to make ammonium sulphate, an important fertiliser. a) Write a balanced symbol equation for the reaction of sulphuric acid with ammonia to produce ammonium sulphate. 2NH3 + H2SO4 ? (NH4)2SO4 [3] [1] [1] +[1] for balancing. Accept equation using NH4OH

b) The method shown below is used to find out if ammonium sulphate would be washed out of soil by rain. : b) The method shown below is used to find out if ammonium sulphate would be washed out of soil by rain.

(i) Describe how you would find the pH of the water that has run through the soil. _______________________________ _______________________________ [2] : (i) Describe how you would find the pH of the water that has run through the soil. _______________________________ _______________________________ [2]

(i) Describe how you would find the pH of the water that has run through the soil. Use pH paper/universal indicator paper/universal indicator solution [1] compare to colour chart [1]. Accept use a pH meter for a full [2] : (i) Describe how you would find the pH of the water that has run through the soil. Use pH paper/universal indicator paper/universal indicator solution [1] compare to colour chart [1]. Accept use a pH meter for a full [2]

(ii) A sample of this water was heated with some sodium hydroxide solution in a boiling tube and the gas evolved was tested with damp universal indicator paper as shown below. What happens to the damp universal indicator paper if ammonium sulphate is present in the water? ___________________________________ [1] : (ii) A sample of this water was heated with some sodium hydroxide solution in a boiling tube and the gas evolved was tested with damp universal indicator paper as shown below. What happens to the damp universal indicator paper if ammonium sulphate is present in the water? ___________________________________ [1]

(ii) A sample of this water was heated with some sodium hydroxide solution in a boiling tube and the gas evolved was tested with damp universal indicator paper as shown below. What happens to the damp universal indicator paper if ammonium sulphate is present in the water? Changes to blue [1] : (ii) A sample of this water was heated with some sodium hydroxide solution in a boiling tube and the gas evolved was tested with damp universal indicator paper as shown below. What happens to the damp universal indicator paper if ammonium sulphate is present in the water? Changes to blue [1]

(iii) Explain your answer to part (b)(ii) above. _______________________________ _______________________________ [2](iv) Describe how you would test the water to shown that sulphate ions are present. State the observations you would make for a positive test. Test: _____________________________ Result: ____________________________ _______________________________ [3] : (iii) Explain your answer to part (b)(ii) above. _______________________________ _______________________________ [2](iv) Describe how you would test the water to shown that sulphate ions are present. State the observations you would make for a positive test. Test: _____________________________ Result: ____________________________ _______________________________ [3]

(iii) Explain your answer to part (b)(ii) above. Forms ammonia [1] gas which is alkaline [1] [2](iv) Describe how you would test the water to shown that sulphate ions are present. State the observations you would make for a positive test. Test: Barium chloride solutions [1] Result: White [1] ppt [1] [3] : (iii) Explain your answer to part (b)(ii) above. Forms ammonia [1] gas which is alkaline [1] [2](iv) Describe how you would test the water to shown that sulphate ions are present. State the observations you would make for a positive test. Test: Barium chloride solutions [1] Result: White [1] ppt [1] [3]

Slide 206 : 206 Nitrogen readily dissolves in blood under these increased pressure condition. If the diver returns to the surface too quickly, nitrogen bubbles form and block blood vessels. Helium is much less soluble than nitrogen: ‘Heliox', a mixture of 80% helium and 20% oxygen, reduces the chance of these potentially fatal problems happening.

Slide 207 : 207 Hydrogen and the Hindenburg Disaster

Slide 208 : 208

Slide 209 : 209

Slide 210 : 210 Thanks for viewing. Do consider using others in this Series. Atomic Structure and Bonding. Inorganic: Metal Chemistry Inorganic: Non-metal Chemistry Redox and Electrolytic Chemistry Organic Chemistry Hard Water Acids Bases & Salt Preparations Kinetics and Energetics Miscellaneous Also, check back on this video-lesson from time-to-time during the duration of your course. F.Scullion