CHEMSHEETS.co.uk 20-May-12 Chemsheets AS 008 1

2y ago
70 Views
5 Downloads
1.44 MB
36 Pages
Last View : 1m ago
Last Download : 2m ago
Upload by : Brady Himes
Transcription

www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 0081

1 - FORMULASIf you are serious about doing A level Chemistry, you MUST be able to write a formula without asecond thought. It is the single most essential skill for an A level chemist.You have to know and be able to use the information on this page – you should not be looking itup. There is no data sheet with ion charges at A level.If you can’t write a formula in an instant, DROP CHEMISTRY NOW and choose something else.ElementsMonatomicSimple e are no ionicelements!!Giant covalentThe formula is just thesymbol, e.g.The formula is just imple molecularThere are no monatomiccompounds!!IonicSome commonmolecular compounds:Metalliccarbon monoxideThese have to beworked out using ioncharges – you have toknow these at AS/Alevel!nitrogen monoxideLEARN them ASAP.carbon dioxideGiant covalentThere are no metalliccompounds!!silicon dioxidenitrogen dioxidesulfur dioxideNote these acids:sulfur trioxidehydrochloric acidammoniasulfuric acidmethanenitric acidhydrogen sulfidephosphoric acidPositive ionsGroup 1 ions:Negative ionsGroup 3 ions:lithiumGroup 7 ions:aluminiumsodiumpotassiumOther common ionssilverGroup 2 carbonateiodidehydrogencarbonateGroup 6 ions:oxidehydrogenbarium May-12Other common ionshydroxidehydridephosphateChemsheets AS 0082

TASK 1 – WRITING FORMULAS OF IONIC COMPOUNDS1)silver bromide5555555555.9)lead (II) oxide5555555555.2)sodium carbonate5555555555.10) sodium phosphate5555555555.3)potassium oxide5555555555.11) zinc hydrogencarbonate 5555555555.4)iron (III) oxide5555555555.12) ammonium sulphate5555555555.5)chromium (III) chloride 5555555555.13) gallium hydroxide5555555555.6)calcium hydroxide5555555555.14) strontium selenide5555555555.7)aluminium nitrate555555555.5.15) radium sulfate5555555555.8)sodium sulfate5555555555.16) sodium nitride5555555555.TASK 2 – WRITING FORMULAS 11)lead (IV) oxide5555555555.11) barium hydroxide5555555555.2)copper5555555555.12) tin (IV) chloride5555555555.3)sodium5555555555.13) silver nitrate5555555555.4)ammonium chloride5555555555.14) iodine5555555555.5)ammonia5555555555.15) nickel5555555555.6)sulfur5555555555.16) hydrogen sulfide5555555555.7)sulfuric acid5555555555.17) titanium (IV) oxide5555555555.8)neon5555555555.18) lead5555555555.9)silica5555555555.19) strontium sulfate5555555555.5555555555.20) lithium5555555555.10) siliconTASK 3 – WRITING FORMULAS 21)silver carbonate5555555555.11) barium hydroxide5555555555.2)gold5555555555.12) ammonia5555555555.3)platinum (II) fluoride5555555555.13) hydrochloric acid5555555555.4)nitric acid5555555555.14) fluorine5555555555.5)ammonia5555555555.15) silicon5555555555.6)silicon (IV) hydride5555555555.16) calcium phosphate5555555555.7)phosphorus5555555555.17) rubidium5555555555.8)diamond5555555555.18) germanium (IV) oxide5555555555.9)vanadium (V) oxide5555555555.19) magnesium astatide5555555555.10) cobalt (II) hydroxide5555555555.20) nitrogen oxide5555555555. www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 0083

2 - EQUATIONSFrom an early age you should have been able to balance chemical equations. However, at A level, you will often need to:work out the formulas yourselves work out what is made (so you need to know some basic general equations) for reactions involving ions in solution, write ionic equationsSome general reactions you should know:General ReactionExamplessubstance oxygen oxides2 Mg O2 2 MgO2 H2S 3 O2 2 H2O 2 SO2C3H8 5 O2 3 CO2 4 H2Ometal water metal hydroxide hydrogen2 Na 2 H2O 2 NaOH H2metal acid salt hydrogenMg 2 HCl MgCl2 H2oxide acid salt waterMgO 2 HNO3 Mg(NO3)2 H2Ohydroxide acid salt water2 NaOH H2SO4 Na2SO4 H2Ocarbonate acid salt water carbon dioxideCuCO3 2 HCl CuCl2 H2O CO2hydrogencarbonate acid salt water carbon dioxideKHCO3 HCl KCl H2O CO2ammonia acid ammonium saltNH3 HCl NH4Clmetal carbonate metal oxide carbon dioxide (on heating)CaCO3 CaO CO2TASK 4 – WRITING BALANCED EQUATIONS1)Balance the following equations.a) Mg HNO3 Mg(NO3)2 H2b) CuCl2 NaOH Cu(OH)2 NaClc) SO2 O2 SO3d) C4H102) O2 CO2 H2OGive balanced equations for the following reactions.a) sodium oxygen sodium oxideb) aluminium chlorine aluminium chloridec) calcium hydrochloric acid calcium chloride hydrogend) ammonia sulphuric acid ammonium sulphate www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 0084

TASK 5 – WRITING BALANCED EQUATIONS 2Write balance equations for the following reactions:1)burning aluminium2)burning hexane (C6H14)3)burning ethanethiol (CH3CH2SH)4)reaction of lithium with water5)reaction of calcium carbonate with nitric acid6)thermal decomposition of lithium carbonate7)reaction of ammonia with nitric acid8)reaction of potassium oxide with water9)reaction of calcium hydroxide with hydrochloric acid10)reaction of zinc with phosphoric acid11)reaction of sodium hydrogencarbonate with sulfuric acid12)reaction of potassium hydroxide with sulfuric acidIonic equationsNa When an ionic substance dissolves in water, the positive andnegative ions separate and become hydrated (they interact withwater molecules rather than each other). For example, a solutionof sodium chloride could also be described as a mixture ofhydrated sodium ions and hydrated chloride ions in water.Cl–Na Cl–Cl–Na In reactions involving ionic compounds dissolved in water, some ofthe ions may not be involved in the reaction. These are calledspectator ions. For such reactions, we can write an ionicequation that only shows the species that are involved in thereaction.Cl–Cl–Na Cl–Simple examples are equations for which ionic equations can bewritten include:Na Na Na Cl–Reactions of acids:Common ionic equations are: -acid hydroxideH (aq) OH (aq) H2O(l)acid carbonate2 H (aq) CO3 (aq) H2O(l) CO2(g)acid hydrogencarbonateH (aq) HCO3 (aq) H2O(l) CO2(g)acid ammoniaH (aq) NH3(aq) NH4 (aq) 2-- We can even use these ionic equations to work out the ratio in which acids react without writing any equation. For example, in the reaction of H2SO4(aq) with NaOH(aq) we know that one lot of H2SO4 contains two lots of H ions. As H ions react with OH ions in the ratio 1:1 [H (aq) OH (aq) H2O(l)] we know that we need two lots of NaOH to provide two lots of OH ions to react with the two lots of H ions. Therefore, one lot of H2SO4 reacts with two lots of NaOH, i.e. thereacting ratio of H2SO4 : NaOH 1:2 www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 0085

Na OH–Na NaNaNa SO4 SO4OH–Na NaOH– Na NaOH–SO42–OH–SO42–SO4 Na OH–NaNa NaOH– OH–Na 2–SO42–Na SO42–SO42– Na NaNaH2SO4 (aq)-contains H (aq) the Na (aq) and SO42-(aq) ions are not involvedcontains OH (aq) NaCONa 2-Na 3 Na NaNa Na CO2-Na 3SO42–NaSO42–2–SO4 Na SO42–CONa2- Na 3Na SO42–Na SO42–Na Na Na NaNa H (aq) OH-(aq) H2O(l)NaOH (aq) NaNa SO42–Na NaNa NaNaNa 2–OH–2–NaOH–Na SO42–NaNa NaCO2-Na3 SO42–SO42– NaSO4SO42–NaNa Na CO 2-H2SO4 (aq)Na 2 H (aq) CO32-(aq) H2O(l) CO2(g)Na2CO3 (aq) contains H (aq)CO32-(aq)containsNa Na3NaNa 2– the Na (aq) and SO42-(aq) ions are not involvedPrecipitation reactionsSome salts are insoluble in water. If solutions containing those ions are mixed, the insoluble salt forms as a solid as thesolutions are mixed. This solid is known as a precipitate, and the reaction as precipitation. NO3–NaNO3–Ba2 Na NaNaNO3NO3–– NaNaNO3–Na2 BaNO3–NaNO3 Na Na NaNa – NO3Ba2 SO42– Ba2 SO 2– Ba2 4 Na– 2 2–2 SO4 BaSO42–SO42– BaNaBa(NO3)2 (aq)contains Ba2 (aq)NO3NO3–NaNO3– Na SO42–NO3–NO3–NO3–NaSO42–2 2 BaNO3– –NO3–Ba NO3– SO42–NO3–– Na2SO4 –NaNO3NaSO42–NO3–Ba2 Ba2 (aq) SO42-(aq) BaSO4(s)Na2SO4 (aq)contains SO42-(aq)Most salts are soluble in water. Often when solutions of two salts are mixed, no such precipitation reaction will take placeand the ions will remain dissolved in water. NO3–NaNO3–Mg2 NaNO3 NaNa–Na NO3–Na2–NaNO3– NO3Na Na NO3SO42––SO42– NaMg2 NO3–Na NaNaNa Mg(NO3)2 (aq) www.CHEMSHEETS.co.uk NaNa2SO4 (aq)20-May-12Na Mg2 SO42–SO42–NO3–NO3–2 Mg2 NO3–2–SO4NO3––MgSO42––NO3 SO4 NaMg2 Mg2 NO3– SO42–NO3– NaNO3–NO3–Mg2 SO42– Na NO3– NaNO3–NO3–Mg2 Mg2 SO42–Nothing happens – solutions just mix togetherChemsheets AS 0086

TASK 6 – IONIC EQUATIONS1)Use your knowledge of ionic equations to give the molar ratio in which the following acids react with bases.Complete the table to show your answers.Acid2)Formula of acidBasehydrochloric acidlithium hydroxidesulphuric acidsodium hydrogencarbonatenitric acidammoniasulphuric acidpotassium carbonatenitric acidstrontium hydroxideFormula of baseMolar ratio ofacid:baseWrite ionic equations for each of the following reactions.a) reaction of hydrochloric acid (aq) with potassium hydroxide (aq)b) precipitation of silver iodide from reaction between silver nitrate (aq) and potassium iodide (aq)c) reaction of potassium carbonate (aq) with nitric acid (aq)d) precipitation of calcium hydroxide from reaction between sodium hydroxide (aq) and calcium chloride (aq)e) reaction of ammonia (aq) with hydrochloric acid (aq)f) reaction of sodium hydrogencarbonate (aq) with sulfuric acid (aq)g) precipitation of calcium sulfate from reaction between calcium chloride (aq) and sulfuric acid (aq)h) precipitation of lead (II) chloride from reaction between lead nitrate (aq) and sodium chloride (aq)i)reaction of barium hydroxide (aq) with nitric acid (aq) www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 0087

3 – SIGNIFICANT FIGURES & STANDARD FORMSome general rules in chemistry: usually give final answers to 3 significant figures (but it is best to keep the whole number on your a during the calculation) give Mr’s to 1 decimal placeNote:-30.00346678 0.00347 (3 sig fig) 3.47 x 10 (3 sig fig)5346678 347000 (3 sig fig) 3.47 x 10 (3 sig fig)TASK 7 – SIGNIFICANT FIGURES & STANDARD FORM1)2)3)Write the following numbers to the quoted number of significant figures.a) 3457894 sig figs5555555d) 63 sig figs5555555.b) 2973003 sig figs5555555e) 0.0015633 sig figs5555555.c) 0.078963 sig figs5555555f) 0.014 sig figs5555555.Complete the following sums and give the answers to 3 significant figures.a) 6125 x 3845555555d) 750 255555555.b) 25.00 x 0.015555555e) 0.000152 x 135555555.c) 13.5 0.185555555f) 0.0125 x 0.0255555555.Write the following numbers in non standard form.a) 1.5 x 104)5)-35555555.d) 0.0534 x 10455555555b) 0.046 x 10-2555555.e) 10.3 x 10555555555c) 3.575 x 105555555.f) 8.35 x 10-355555555Write the following numbers in standard form.a) 0.0001675555555.d) 3450055555555b) 0.0524555555.e) 0.6255555555c) 0.000000015555555.f) 8700000055555555Complete the following calculations and give the answers to 3 significant figures.a) 6.125 x 10b) 4.3 x 10-3-4x 3.55555555555555555555555. 7.05555555555555555555555.8c) 4.0 x 10 35000d) 0.00156 2.4 x 10555555.35555555555555555555555.e) 6.10 x 10-2– 3.4 x 10-5f) 8.00 x 10-3x 0.100 x 105555555555555555555555.-3 12Chemsheets AS 0088

4 – THE MOLE & AVOGADRO CONSTANT23 One mole of anything contains 6.02 x 10 of those things. One mole of2323bananas is 6.02 x 10 bananas. One mole of water molecules is 6.02 x 10water molecules This number is known as the Avogadro constant. The Avogadro number was chosen so that the mass of one mole of particlesof a substance equals the Mr in grams. For example, the Mr of water is 18.0,and the mass of one mole of water molecules in 18.0 grams.Moles Mass (in grams)Mr1 ton 1,000,000 g1 kg 1,000 g1 mg 0.001 gRemember Mr Moles!TASK 8 – MOLES1)2)3)How many moles are there in each of the following?a) 72 g of Mgb)4 kg of CuOd) 1 tonne of NaCle)20 mg of Cu(NO3)2c)39 g of Al(OH)3c)0.01 moles of AgWhat is the mass of each of the following?a) 5 moles of Cl2b)0.2 moles of Al2O3d) 0.002 moles of (NH4)2SO4e)0.3 moles of Na2CO3.10H2Oa) Calculate the number of moles of CO2 molecules in 11 g of carbon dioxide.b) Calculate the number of moles of C atoms in 11 g of carbon dioxide.a) Calculate the number of moles of O atoms in 11 g of carbon dioxide.4)a) Calculate the number of moles of Al2O3 in 5.1 g of Al2O3.b) Calculate the number of moles of Al3 ions in 5.1 g of Al2O3.2-a) Calculate the number of moles of O ions in 5.1 g of Al2O3.5)An experiment was carried out to find the Mr of vitamin C (ascorbic acid). It was found that 1 g contains 0.00568moles of Vitamin C molecules. Calculate the Mr of vitamin C.6)Use the following data to calculate the mass of the particles shown.Mass of proton 1.6726 x 10-24g-24Mass of neutron 1.6749 x 10-28gAvogadro constant 6.0221 x 1023Mass of electron 9.1094 x 10g1a) Calculate the mass of a H atom.1 b) Calculate the mass of an H ion.3c) Calculate the mass of a H atom. www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 0089

5 – REACTING MASS CALCULATIONSWhat a chemical equation means N2 3 H22 NH3 1 molecule N23 molecules H22 molecules NH312 molecules N22 dozen molecules N236 molecules H23 dozen molecules H224 molecules NH32 dozen molecules NH312 molecule N22 dozen molecules N236 molecules H23 dozen molecules H224 molecules NH32 dozen molecules NH32323236 x 10 molecule N22 moles N218 x 10 molecules H23 moles H212 x 10 molecules NH32 moles NH310 moles N23 moles H22 moles NH30.5 moles N21.5 moles H21 mole NH3TASK 9 – WHAT EQUATIONS MEAN4 Na O2 2 Na2O 3 Cl2 2 AlCl3 6½ O2 4 CO2 5 H2O 3 O2 2 N2 6 H2O12 mol0.1 mol2 Al5 mol0.1 molC4H100.5 mol20 mol4 NH30.5 mol10 mol www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 00810

Reacting mass calculations You can use balanced chemical equations to find out what mass of chemicals (or volume of gases) react or areproduced in a chemical reaction. To do this, calculate:(a) moles of e.g.(b) moles of ? (c) mass of ?What mass of iron is produced when 32 kg of iron (III) oxide is heated with CO? ?Fe2O3(s) 3 CO(g) 2 Fe(s) 3 CO2(g)moles of Fe2O3 mass (g) 32,000 200.5 molMr159.61 mole of Fe2O3 forms 2 moles of Fe moles of Fe 2 x 200.5 401.0 mol mass of Fe moles x Mr 401.0 x 55.8 22,400 g (3 sig fig)e.g.What mass of oxygen is needed to convert 102 g of ammonia into nitrogen? ?4 NH3(g) 3 O2(g) 2 N2(g) 6 H2O(g)moles of NH3 mass (g) 102 6.00 molMr17.04 moles of NH3 reacts with 3 moles of O2 1 mole of NH3 reacts with ¾ mole of O2 moles of O2 6.00 x ¾ 4.00 mol mass of O2 moles x Mr 4.00 x 32.0 128 g (3 sig fig)e.g.When 5.00 g of crystals of hydrated tin (II) chloride, SnCl2.xH2O, are heated, 4.20 g of anhydrous tin (II) chlorideare formed. Calculate the number of molecules of water of crystallisation are in SnCl2.xH2O (i.e. the value of x).SnCl2.xH2O SnCl2 x H2Omoles of SnCl2 mass (g) 4.20 0.02214 molesMr189.7 moles of SnCl2.xH2O 0.02214 mol Mr of SnCl2.xH2O mass 5.00 225.8moles0.02214 Mr of xH2O 225.8 – 189.7 36.1 x 36.1 2 (x is a whole number)18.0 www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 00811

TASK 10 – REACTING MASS CALCULATIONS 11)What mass of hydrogen is needed to react with 40 g of copper oxide?CuO H2 Cu H2O2)What mass of oxygen reacts with 192 g of magnesium?2 Mg O2 2 MgO3)What mass of sulfur trioxide is formed from 96 g of sulfur dioxide?2 SO2 2 SO3 O24)What mass of carbon monoxide is needed to react with 480 kg of iron oxide?Fe2O3 3 CO 2 Fe 3 CO25)What mass of carbon dioxide is produced when 5.6 g of butene is burnt.C4H8 6 O2 4 CO2 4 H2O6)What mass of oxygen is needed to react with 8.5 g of hydrogen sulphide (H2S)?2 H2S 3 O2 2 SO2 2 H2O7)4.92 g of hydrated magnesium sulphate crystals (MgSO4.nH2O) gave 2.40 g of anhydrous magnesium sulphate onheating to constant mass. Work out the formula mass of the hydrated magnesium sulphate and so the value of n.MgSO4.nH2O 8)In an experiment to find the value of x in the compound MgBr2.xH2O, 7.30 g of the compound on heating to constantmass gave 4.60 g of the anhydrous salt MgBr2. Find the value of x.MgBr2.xH2O 9)MgSO4 n H2OMgBr2 x H2OWhat mass of glucose must be fermented to give 5.00 kg of ethanol?C6H12O6 2 C2H5OH 2 CO210) The pollutant sulfur dioxide can removed from the air by reaction with calcium carbonate in the presence of oxygen.What mass of calcium carbonate is needed to remove 1 ton of sulfur dioxide?2 CaCO3 2 SO2 O2 2 CaSO4 2 CO211) What mass of potassium oxide is formed when 7.8 mg of potassium is burned in oxygen?4 K O2 2 K2O12) What mass of hydrogen is produced when 10.0 g of aluminium reacts with excess hydrochloric acid?2 Al 6 HCl 2 AlCl3 3 H213) What mass of sodium just reacts with 40.0 g of oxygen?4 Na O2 2 Na2O14) What mass of nitrogen is produced when 2.00 tonnes of ammonia gas decomposes?2 NH3 N2 3 H215) What mass of oxygen is produced when 136 g of hydrogen peroxide molecules decompose?2 H2O2 2 H2O O216) What mass of lead (II) oxide is produced when 0.400 moles of lead (II) nitrate decomposes?2 Pb(NO3)2 2 PbO 4 NO2 O2 www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 00812

Limiting reagents In the real world of chemistry, it is rare that we react the exact right amount of chemicals together. Usually, we have morethan we need of one of the reactants and so it doesn’t all react – it is in excess. Sometimes in calculations, we need to work out if one of the reactants is in excess. The reactant that is not in excess issometimes called the limiting reagent.e.g. 1 - Starting point - Working out how much reacts in terms of moles:Moles at the startMoles reactingMoles SO2Moles O2Moles SO2Moles O2Reagent inexcess4342O210100.10.0220.42102 SO2 O2 2 SO3Moles at the endMoles SO2Moles O2Moles SO3014And then you usually have to work out the mass of one of the substances.e.g. 2Ba(OH)2 2 HCl BaCl2 2 H2OMoles at the startMoles reactingMol Ba(OH)2Moles HClMol Ba(OH)2Moles HClReagent inexcess552.55Ba(OH)20.10.050.20.50.0250.0375e.g. 3Moles at the endMol Ba(OH)2Moles HClMoles BaCl2In the manufacture of titanium, what mass of titanium can theoretically be formed when 1 kg of titanium chloridereacts with 0.1 kg of magnesium?TiCl4 2 Mg Ti 2 MgCl2Moles TiCl4 1000 5.266189.9Moles Mg 100 4.11524.35.266 moles of TiCl4 needs 10.53 moles of Mg to react, TiCl4 is in XS and does not all react, so Mg is the limiting reagent 2.058 moles of TiCl4 reacts with 4.115 moles of Mg 2.058 moles of Ti is producedMass of Ti 2.058 x 47.9 98.6 g www.CHEMSHEETS.co.uk20-May-12Chemsheets AS 00813

TASK 11 – REACTING MASS CALCULATIONS 21)In each case work out the limiting reagent and moles of ammonia formed (assuming complete reaction).N2 3 H2 2 NH3a) 3 moles of N2 3 moles of H2b) 3 moles of N2 10 moles of H2c) 0.1 moles of N2 0.2 moles of H2d) 0.5 moles of N2 2.0 moles of H2e) 2 moles of N2 10 moles of H22)In each case work out the limiting reagent and moles of ammonia formed (assuming complete reaction.2 SO2 O2 2 SO3a) 3 moles of SO2 3 moles of O2b) 3 moles of SO2 2 moles of O2c) 0.1 moles of SO2 0.02 moles of O2d) 2.0 moles of SO2 0.4 moles of O2e) 2 moles of SO2 10 moles of O23)5.00 g of iron and 5.00 g of sulphur are heated together to form iron (II) sulphide. Which reactant is in excess andwhat is the maximum mass of iron (II) sulphide that can be formed?Fe S FeS4)In the manufacture of the fertiliser ammonium sulphate, what is the maximum mass of ammonium sulphate that canbe obtained from 2.00 kg of sulphuric acid and 1.00 kg of ammonia?H2SO4 2 NH3 (NH4)2SO45)In the Solvay process, ammonia is recovered by the reaction shown. What is the maximum mass of ammonia thatcan be recovered from 2 tonnes of ammonium chloride a

metal carbonate metal oxide carbon dioxide (on heating) CaCO 3 CaO CO 2 TASK 4 – WRITING BALANCED EQUATIONS 1) Balance the following equations.

Related Documents:

www.CHEMSHEETS.co.uk 14-Jul-12 Chemsheets A2 009 7 TASK 3 – pH of strong bases 1) Calculate the pH of the following solutions. a) 0.15 mol dm-3 KOH b) 0.05 mol .

www.CHEMSHEETS.co.uk 23-Feb-2016 Chemsheets A2 1001 Page 3 As the temperature changes, the average energy of the particles increases and so the

www.CHEMSHEETS.co.uk 10-Mar-2016 Chemsheets A2 1014 Page 7 Example 2 Ethanol has the formula C 2 H 5 OH and is used as a fuel (e.g. for cars in Brazil). It burns .

www.CHEMSHEETS.co.uk 10-Jul-12 Chemsheets AS 029 3 CALORIMETRY The enthalpy change for a reaction can be found by measuring the temperature change in a reaction.File Size: 1MB

a) [Co(H 2O) 6] 2 Co 2 e) [FeO 4] 2– Fe 6 i) K 2[CoCl 4] Co 2 b) [CrCl 6] 3– Cr 3 f) [Mn(CN) 6] 4– Mn 2 j) K 3[AuF 6] Au 3 c) [Co(NH 3) 6]Cl 2 Co 2 g) [Ni(CO) 4] Ni 0 k) (NH 4) 2[IrCl 6] Ir 4 d) [Co(NH 3) 5Cl]Cl 2 Co 3 h) [Ni(EDTA)] 2– Ni 2 l) Na[Mn(CO) 5] Mn -1 TASK 2 – Writing half equations a) 2I– I 2 2e – b .

www.CHEMSHEETS.co.uk 16-July-2016 Chemsheets A2 1078 b) By reduction of nitrile compounds This is the commonest way as it only forms one amine rather than a mixture.

May 3 – Nicole Fetzer–Bryan. May 5 – Eli Wilhelm. May 5 – Shelby Conger. May 6 – Jeff Vaverka. May 7 – Mitchell Bryan. May 8 – Eric Leonard. May 8 – Chad Sailors. May 10 – Cale Foster. May 11 – Faye Brand. May 12 – James Westbrook. May 13 – Peter Smith. May 14 – Jack Rumer. May 15 – Justin Kriegel. May 16 – Jodi .

First aid at work – your questions answered Page 3 of 8 Health and Safety Executive The findings of your first-aid needs assessment (see Q3) will identify whether first-aiders should be trained in FAW, EFAW, or some other appropriate level of training. EFAW training enables a first-aider to give emergency first aid to someone who is injured or becomes ill while at work. FAW training includes .