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February 2016 © Copyright The PiXL Club Ltd, 2016 This resource is strictly for the use of member schools for as long as they remain members of The PiXL Club. It may not be copied, sold nor transferred to a third party or used by the school after membership ceases. Until such time it may be freely used within the member school. All opinions and contributions are those of the authors. The contents of this resource are not connected with nor endorsed by any other company, organisation or institution. www.pixl.org.uk The PiXL Club Ltd, Company number 07321607

How to deliver the DTT Booster Administer the short diagnosis test. Mark the test (peer assess) Work through the therapy slides completing the model questions and answers. Complete the question slides for students to self assess. Administer the final test (peer assess)

Conduction and convection Edexcel Topic 6 – Reacting masses Model Question How many protons in P? How many neutrons in P? Model Answer Protons = 15 Neutrons = 31 – 15 = 16 Information from the periodic table. Atomic mass – how heavy the atom is. Symbol – First letter always a capital, second lower case. Full name Atomic or proton number Occasionally you see the two numbers reversed, the rule is, if you want the mass look for the BIGGEST number. 31 P Phosphorus 15 27 Al Aluminium 13 CLICK to reveal MODEL ANSWER Atomic mass is the number of protons added to the number of neutrons. The atomic number tells you how many protons, so you can work out the number of neutrons. Neutrons = mass number - proton number Some atomic masses are not whole numbers, this is because of averaging for isotopes – don’t worry about it, just use it as it is written. P1.1.3a/P1.1.1

Conduction and convection Edexcel Topic 6– Reacting masses Model Question What is the formula mass of: a) Fe(OH)3 b) Fe2O3 c) Ca(NO3)2 Model Answer a) 107 b) 160 c) 164 Calculating the formula mass (Mr) Remember: Atomic mass is the top number / bigger number on the periodic table. When you have a formula with more than one type of atom there is a subscript / small number after the atoms symbol. H2O – the 2 means two of the atom before, so two hydrogens. If there is no number there it means there is one of them. Brackets are used to group things together. Numbers after the bracket mean that many of whatever is inside the bracket. Ca(OH)2 means that there are two OH groups attached to the Ca. CLICK to reveal MODEL ANSWER CH4 – 1 carbon mass= 12 =12 4 Hydrogens mass = 1 x 4 = 4 16 The formula mass of CH4 = 16 Al(OH)3 1 Al = 27 OH : 1 O = 16 + 1 H = 1 = 17 And the bracket has a 3 after it so it is mass of OH x 3, 17 x 3 = 51 The formula mass of Al(OH)3 27 + 51= 78 P1.1.3a/P1.1.1

Conduction and convection Edexcel Topic 6– Reacting masses MgO Mg = 24, O = 16 so MgO = 40 In MgO 24/40 is magnesium 24 x100 = 60% 40 Magnesium oxide is 60% magnesium Percentage composition If you made some shortcrust pastry, here is the ingredients list: 125g flour 55g butter 40g water After mixing them all together you would have a total of 220g of pastry (125g + 55g + 40g) In my 220g of pastry there are still 55g of butter. 55/220 of my pastry is butter. 55 x 100 = 25% 220 Atoms are no different, only we call the mixing a reaction. From the previous slide Fe2O3 Mg = 56, O = 16 so Fe2O3 = 160 There are 2 Fe atoms so 112 is Fe 112 x100 = 70% 160 Fe2O3 is 70% Fe Model Question What % aluminium is in Al2O3? Model Answer Al2O3 = (27x2) + (16x3) = 102 2 x Al = 54 54 x 100 = 52.9% 102 CLICK to reveal MODEL ANSWER P1.1.3a/P1.1.1

Conduction and convection Edexcel Topic 6 – Reacting masses Model Question Mg + H2SO4  MgSO4 + H2 If I reacted 24g of magnesium with excess H2SO4. How much MgSO4 will be produced? Model Answer 24g  24+32+(4x16) = 120 Reacting masses – How much do you get? Magnesium + chlorine  magnesium chloride Mg + Cl2  MgCl2 24 + (2x35.5)  95 If you reacted 24g of magnesium with 71g of chlorine you would get 95g of magnesium chloride…. In theory! CLICK to reveal MODEL ANSWER Reasons why you might not get what you expected: Some is lost when transferring or separating mixtures. It gets left on the sides of beakers or in a filter paper. The reaction may not have finished. You may have wrongly measured or written down something, a weight for example. Your chemicals might have reacted to produce something unexpected. As you are well aware, experiments never quite turn out as planned, what you should get in theory is not what you might get Exam hint In some questions it may say something like, 24g of magnesium was reacted with excess chlorine….. They say excess to tell you that there was enough chlorine to react with all of the magnesium. P1.1.3a/P1.1.1

Conduction and convection Edexcel Topic 6 – Reacting masses Percentage yield This is comparing how much product we did get compared to how much we expected to get. Model Question A student mixed 5.4g lead nitrate with excess potassium iodide. After filtering and drying he obtained 6.9g of lead iodide product. His teacher said that he should have got 9.2g. What is his percentage yield? (Hint, just look for actual and expected) Model Answer % yield = 6.9g x 100 = 75% 9.2g Percentage yield = Actual amount produced Amount you should have got The amount we should have got is also called the theoretical yield. CLICK to reveal MODEL ANSWER If you get a percentage yield of more than 100% you put numbers the wrong way around! In a reaction of calcium with hydrochloric acid, a student expected to obtain 8g of calcium chloride, at the end of the experiment she obtained 2g, what is her percentage yield? % yield = actual amount produced x 100 = 2g = 25% amount expected 8g P1.1.3a/P1.1.1

Zn Edexcel Topic 6 – Reacting masses What is the atomic mass of zinc? What is the relative formula mass of: nitric acid HNO3 calcium sulfate CaSO4 lithium carbonate Li2CO3 Zinc nitrate Zn(NO3)2 What is the percentage of: tin in tin oxide, Sn in SnO2 carbon in pentane, C in C5H10 copper in copper carbonate, Cu in CuCO3 Zinc metal can be reacted with sulfur to make zinc sulfide in an experiment 3.25g of zinc was reacted with excess sulfur and 8.57g of zinc sulfide was obtained. The expected mass of zinc sulfide was 9.85g. What is the % yield and why is it not 100% 65 Zn Zinc 30 Atomic masses H=1 N=14 O=16 S = 32 Li=7 C=12 Cu=63.5 Zn=65 Sn=119 Ca=40

Edexcel Topic 6 – Reacting masses What is the atomic mass of Zinc?? 65 What is the relative formula mass of: nitric acid HNO3 63 calcium sulfate CaSO4 136 lithium carbonate Li2CO3 74 Zinc nitrate Zn(NO3)2 177 What is the percentage of: tin in tin oxide, Sn in SnO2 84.4% carbon in pentane, C in C5H10 85.7 copper in copper carbonate, Cu in CuCO3 51.4% Zinc metal can be reacted with sulfur to make zinc sulfide in an experiment 3.25g of zinc was reacted with excess sulfur and 8.57g of zinc sulfide was obtained. The expected mass of zinc sulfide was 9.85g. What is the % yield and why is it not 100% % yield = 87%, not 100% some Zn did not react, product was lost, different product formed.

Final test DTT Booster Students now complete the final test. Compare this to what they achieved in the diagnostic test.