3. The structure of an atom LO: understand the structure of atoms In each atom, the number of protons will ALWAYS be the same as the number of electrons. This makes sure that the overall charge is zero. ParticleCharge Proton+1 Neutron0 Electron

4. Atomic and Mass number LO: understand how to interpret the periodic table The Atomic number is ALWAYS the smaller number next to the element. The mass number is always the bigger number.

5. Example Calculate the following quantities for the element below (i)Atomic number (ii)Mass number (iii)Number of protons (iv)Number of electrons (v)Number of neutrons LO: understand how to interpret the periodic table

6. Electron shells Consider Calcium. Calcium has an atomic number of 20. All of calcium’s 20 electrons can NOT fit in one orbit. Therefore, there must be multiple orbits for electrons to occupy LO: understand how to interpret the periodic table

7. Shell break down Atoms have 4 shells where electrons can live Shell 1 – 2 electrons Shell 2 – 8 electrons Shell 3 – 8 electrons Shell 4 – Whatever is left! LO: understand how to interpret the periodic table

8. Example 1 Draw the electron arrangement for sodium LO: understand how to interpret the periodic table

9. Example 2 Draw the electron arrangement for oxygen LO: understand how to interpret the periodic table

10. Reacting with oxygen When something reacts with oxygen, it always form an oxide. e.g. Magnesium  Magnesium oxide Sodium  Sodium oxide Calcium  Calcium oxide Potassium  Potassium oxide LO: understand why chemical reactions occur

11. Why do chemical reactions happen? When elements react together, they do so for a reason. They are trying to achieve a FULL OUTER ELECTRON SHELL. Consider the following reaction: LO: understand why chemical reactions occur

12. The Noble Gases LO: understand why chemical reactions occur The group 8 elements are also known as ‘Noble Gases’. These elements are very unreactive. Why do you think this is? They are unreactive as they already have a full outer shell. Therefore, they don’t need to try to gain/lose any electrons through reacting to get a full outer shell.

14. What is limestone? Limestone is a sedimentary rock that is formed over millions of years from the remains of dead sea creatures. The chemical name for limestone is CALCIUM CARBONATE and its formula is CaCO 3. LO: understand the uses and reactions of limestone

15. Quarrying To get limestone, it must be dug out of the ground through a process called quarrying. The limestone can be buried deep underground and the stone covering it must be removed using explosives. LO: understand the uses and reactions of limestone

16. The Limestone cycle The limestone cycle is a set of reactions that allow us to start at limestone and end up back with limestone. For your GCSE course, you need to know details of the three reactions, the word and symbol equations and how to balance them. LO: understand the reactions of limestone

17. Thermal decomposition Calcium carbonate  Calcium oxide + Carbon dioxide LO: understand the reactions of limestone

18. Calcium Hydroxide Calcium oxide + Water  Calcium Hydroxide LO: understand the reactions of limestone

19. Limewater Limewater can be made from calcium hydroxide solution by diluting it with additional water. LO: understand the reactions of limestone

20. Limewater Limewater is commonly used to test for carbon dioxide. When there is carbon dioxide present, the limewater goes from being clear to milky/cloudy LO: understand the reactions of limestone

21. Calcium Hydroxide Calcium Hydroxide + Carbon dioxide  Calcium Carbonate LO: understand the reactions of limestone

22. Check: LO: understand the reactions of limestone CaCO 3 CaO Ca(OH) 2 Limewater Ca(OH) 2

23. KEYWORDS: reactivity series, displacement

24. Reactivity Simple experiments can quite easily show us that some materials are more reactive than others. Metals such as magnesium and potassium are very reactive, whereas metals such as iron are quite unreactive. What metals can you think of that are quite unreactive? LO: understand the purpose of the reactivity series

25. Reactivity LO: understand the purpose of the reactivity series

26. The reactivity series This list shows the order of reactivity of common elements. Carbon and Hydrogen are highlighted in red as they are the only non- metals that are on the list. Do the results from our experiment agree with this list? LO: understand the purpose of the reactivity series

27. Using the reactivity series The reactivity series can help us work out if a reaction will happen or not. In our experiment, magnesium reacted with all of the solutions because it is more reactive than Aluminium, Zinc and Copper. It kicked these elements out of the sulphate solutions and replaced them, leading to a reaction. LO: understand the purpose of the reactivity series

28. The reactivity series Aluminium is more reactive than Zinc and Copper, so it could kick these elements out of the sulphate solutions and make a reaction. However, it is not reactive enough to kick magnesium out of the sulphate solution and so there was no reaction there! LO: understand the purpose of the reactivity series

29. Displacement reactions LO: understand the purpose of the reactivity series Magnesium + Copper Sulphate Copper + Magnesium Sulphate The reaction above is known as a displacement reaction. The Magnesium is displacing the copper out of the sulphate solution.

30. Extracting metals Metals play a very important role in our society. Building, planes, trains, cars, electronics, furniture and miles of miles of wiring are all made out of metals. It is essential, therefore, that we are able to get a continuous supply of them. LO: understand how to extract metals from their ores

31. Extracting metals So you have your ore. Now what? How do you go about getting the nice, pure metal that is locked inside it? To extract the metal, you must use an element that is higher up the reactivity series. This will kick out the metal that YOU WANT, leaving you free to sell it on or use it. LO: understand how to extract metals from their ores

32. Extracting Iron Iron is an EXTREMELY important metal. It was a vital part of the industrial revolution that happened in Britain in the 1700s and 1800s, which allowed Britain to become the dominant superpower at the time. It is still widely used today to make buildings and bridges. What elements could we use to extract iron from its ore? LO: understand how to extract metals from their ores

33. Copper LO: understand the extraction of copper Copper is one of the most widely used metals in the world. It is most commonly used in piping and electrical wires. Copper, however, is a very expensive metal to extract

34. Smelting LO: understand the extraction of copper In the first part of the process, copper ore is heated in a furnace. This makes a substance called crude copper, which still contains a lot of impurities

35. Electrolysis LO: understand the extraction of copper The impure copper is purified using electricity in a process called electrolysis. The impure copper separates and goes into the solution and attaches itself to the pure copper leaving the impurities behind as a sludge.

36. Phytomining LO: understand the extraction of copper Phytomining is the extraction of copper using plants. Plants absorb copper ions through their roots. These copper ions collect in the plants and become concentrated.

37. Phytomining LO: understand the extraction of copper Phytomining is the extraction of copper using plants. When the plants are burnt, the copper ions combine with oxygen to form copper compounds in the left over ash.

38. Phytomining LO: understand the extraction of copper Phytomining is the extraction of copper using plants. The copper compounds are dissolved and electrolysis is performed on the solution. This way, pure copper is extracted

40. Refining crude oil Crude oil is a dark, smelly liquid which is a mixture of lots of different chemicals The majority of these chemicals are hydrocarbons – chemicals made of JUST hydrogen and carbon In its raw state, crude oil is useless. It must be refined through a process called fractional distillation before it can be put to use LO: understand the process and product of fractional distillation

41. Refining crude oil – Fractional distillation 1.Crude oil is vaporised at 450°C and pumped into the bottom of the tower 2.The temperature of the tower decreases as the height increases. As the vaporised oil rises, it cools and condenses 3.Heavy fractions contain large molecules and have a high b.p. They condense near the bottom 4.Light fractions contain small molecules and have a low b.p. They condense near the top of the column LO: understand the process and product of fractional distillation

42. Alkanes Alkanes are one type of hydrocarbon that crude oil is mainly made up of. For your GCSE course, you need to know the formula of the first four alkanes and how to draw them The first two alkanes are: CH 4 – Methane C 2 H 6 – Ethane WHAT IS THE GENERAL FORMULA OF AN ALKANE? LO: understand the products of combustion of hydrocarbons

43. Alkanes The first five alkanes are: CH 4 – Methane C 2 H 6 – Ethane C 3 H 8 – Propane C 4 H 10 – Butane C 5 H 12 – Pentane LO: (i) understand the structure of alkanes (ii) be able to explain the products of combustion

44. Combustion Combustion is the process of reacting a fuel with oxygen. It releases energy from fuels! LO: understand the products of combustion

45. Complete combustion When a hydrocarbon burns in the presence of lots of oxygen, the ONLY products are carbon dioxide and water LO: understand the products of combustion

46. Incomplete combustion Incomplete combustion occurs when there is not enough oxygen. This causes the formation of two extra products along with carbon dioxide and water: 1.Carbon monoxide 2.Carbon (soot) You DON’T need to know how to do these balanced equations! LO: understand the products of combustion