3. Atomic Structure The basic structure of an atom The term ‘isotope’ Identify elements on the periodic table and calculate P/E/N

4. The basic structure of an atom Atom, element, electron, proton, neutron TASK 1: Recap Write down 3 things you can remember about the periodic table. 1) 2) 3)

5. Keywords atomshows what happens to the atoms in a chemical reaction elementthe smallest part of an element compoundshows the symbols of the elements Mixturetwo or more atoms chemically joined together chemical formulasubstance that cannot be split into simpler substances balanced equationtwo or more elements not chemically joined together The basic structure of an atom Atom, element, electron, proton, neutron

6. TASK 2: Structure of the atom The basic structure of an atom Atom, element, electron, proton, neutron Atoms are tiny building blocks. They are made from protons, electrons and neutrons. The protons and neutrons exist in the centre part of the atom called the nucleus.

7. The basic structure of an atom Atom, element, electron, proton, neutron

8. The basic structure of an atom Atom, element, electron, proton, neutron TASK 3: Protons, electrons, neutrons Subatomic particle Relative charge Relative mass Proton+11 Electron0.0005 Neutron01

9. The term ‘isotope’ Atom, element, electron, proton, neutron Isotopes Isotopes are varieties of an element that have the same atomic number, but different mass numbers.

10. Identify elements on the periodic table and calculate P/E/N Atom, element, electron, proton, neutron P.E.N. Protons = atomic number Electrons = atomic number Neutrons = mass number – atomic number

11. Identify elements on the periodic table and calculate P/E/N Atom, element, electron, proton, neutron P.E.N. Calculate the number of each on this table. SymbolAtomic number Mass number Number of protons Number of electrons Number of neutrons 4 He 2 24 12 C 6 16 O 8 56 Fe 26

12. Electronic Structure How to calculate P/E/N That electrons occupy different shells Construct dot and cross diagrams of different elements

13. AtomProtonsNeutronsElectronsAtomic number Mass Number Boron Potassium Chromium Mercury Argon Starter Activity: How to calculate P/E/N Atom, element, electron, proton, neutron

14. How Are Electrons Arranged? Electrons are not evenly spread. The exist in layers known as shells. electron configuration. The arrangement of electrons in these shells is often called the electron configuration. 2nd Shell 1st Shell 3rd Shell 4th Shell

15. Each shell has a maximum number of electrons that it can hold. 1st Shell: 2 electrons 2 nd Shell: 8 electrons 3 rd Shell: 8 electrons The maximum How Are Electrons Arranged?

16. Which Shells Do Electrons go into? Opposites attract. Protons are + and electrons are – charged. Electrons will occupy the shells nearest the nucleus unless these shells are already full. 1st Shell: Fills this first 2 nd Shell: Fill this next 3 rd Shell: And so on

17. Working Out Electron Arrangements 1.How many electrons do the element atoms have? (This will equal the atomic number). 2.Keeping track of the total used, feed them into the shells working outwards until you have used them all up. 1st Shell: Fills this first 2 nd Shell: Fill this next Drawing neat diagrams helps you keep track!

18. identify types of change as chemical or physical reaction, reversible, irreversible TASK 4: What is it? Copy both questions into your exercise book and answer.

19. Chemical reactions - investigation how to identify a chemical reaction the importance of lab safety investigate different reactions

20. Bonding There are 3 types of bonding How ionic bonding occurs Draw the electronic configuration for ionic bonding in sodium chloride (NaCl)

21. Ionic Compounds The structure of ionic compounds The physical properties of NaCl and MgO Work out the formulae for ionic compounds

22. The structure of ionic compounds Ionic compound, giant ionic lattice Task 1: Show how bonding occurs in magnesium oxide. O Mg 2.8.2. 2.6 Magnesium atom Oxygen atom Mg2+ O2- 2.8 Magnesium Oxide

23. The structure of ionic compounds Ionic compound, giant ionic lattice Task 2: Show how bonding occurs in lithium oxide. Li O Li+ O2-

24. The physical properties of NaCl and MgO Ionic compound, giant ionic lattice Ionic compounds: Read page 134/5 and answer the questions below. (write the question and the answer) Under what conditions does NaCl conduct electricity? Suggest why magnesium oxide bricks are used to line furnaces. Describe the structure of sodium chloride, including information on physical properties.

25. Covalent Bonding The properties of CO 2 and H 2 O How covalent bonding occurs Draw dot and cross diagrams for covalent bonds

26. Group 1 The properties of elements in group 1 Why elements are placed in groups Make observations of group 1 reactions

27. ElementObservationObservation in waterExplanation Li Na K

28. The Flame Tests Why we use the flame tests to identify substances Information from the flame tests Make observations using the flame tests

29. Recap 1)Write a word and balanced symbol equation for the reaction of sodium with water. 2)Write a word and balanced symbol equation for the reaction of caesium with water. Why we use the flame tests to identify substances Flame test, metal ion, hydrochloric acid

30. ElementSymbolObservation before flame test Observation in flame Lithium Sodium Potassium Copper Calcium Why we use the flame tests to identify substances Flame test, metal ion, hydrochloric acid

31. Information from the flame tests Flame test, metal ion, hydrochloric acid The Flame Tests Describe how you carried out the flame tests Outline how you carried out the flame tests, including results and explain why the flame tests are useful

32. Group 7 The appearance and uses of group 7 elements The reactions that occur with group 7 and group 1 Balance chemical equations show group 1 and 7 reactions

33. The appearance and uses of group 7 elements Halogens, metal halide, reaction Recap: CalciumRed CopperLilac SodiumGreen Potassiumorange lithiumorange Match the element with the correct flame test result:

34. Group 7: The Halogens The appearance and uses of group 7 elements Halogens, metal halide, reaction

35. Group 7: The Halogens The appearance and uses of group 7 elements Halogens, metal halide, reaction HalogenSymbolAppearanceUses Fluorine Chlorine Bromine Iodine

36. Reactions with metals The reactions that occur with group 7 and group 1 Halogens, metal halide, reaction Why do group 7 elements react vigorously with group 1 elements?

37. Reactions with metals Balance chemical equations show group 1 and 7 reactions Halogens, metal halide, reaction Li + I 2 LiI

38. The Transition Elements Where to locate the transition elements on the periodic table The transition metals are often used as catalysts Describe the thermal decomposition of carbonates of transition elements

39. Transition elements Where to locate the transition elements on the periodic table Transition element, catalyst, thermal Identify some transition elements and give uses for 5 of them.

40. Thermal decomposition What do you understand by the term ‘thermal decomposition’? Describe the thermal decomposition of carbonates of transition elements Transition element, catalyst, thermal copper carbonatecopper oxide +carbon dioxide Write balanced symbol equations for the thermal decomposition of manganese (II) carbonate, MnCO 3 and iron (II) carbonate, FeCO 3

41. Precipitation Reactions What a precipitation reaction is How NaOH is used to identify transition metal ions Investigate the precipitation reactions and construct balanced symbol equations

42. Precipitation Reactions What a precipitation reaction is Precipitate, reaction, Sodium Hydroxide A precipitation reaction happens when a mixture of solutions reacts to make an insoluble salt. The insoluble solid is called the precipitate.

43. How NaOH is used to identify transition metal ions Precipitate, reaction, Sodium Hydroxide Balanced equations Cu 2+ +2OH - Cu(OH) 2

44. Metallic Structure The properties of metals The link between the properties of metals and its uses Describe metallic bonding

45. Metal properties Properties of metals The properties of metals Tensile strength, metallic bond

46. Metal properties Properties of metals hard Shiny/lust rous Good conductor s of heat Good conductor s of electricity High Density High tensile strength High melting and boiling points The properties of metals Tensile strength, metallic bond

47. Describe metallic bonding Tensile strength, metallic bond

48. Superconductors That some metals are superconductors at low temperatures What a superconductor is Describe the potential benefits of superconductors

49. http://www.bbc.co.uk/education/clips/zjcrkqt The discovery of superconductors 1)Name a METAL. 2)What are wires made out of? 3)What percentage of electrical energy is absorbed by copper wires as the energy travels from the power station to your plug? 4)In which year was Dutch Physicist Onnes investigating the conductivity of materials at low temperatures ? 5)To what temperature was mercury cooled down to? 6)What did Onnes discover? 7)What happens to electrons at normal temperatures? 8)What happens to electrons at extremely low temperatures ? What a superconductor is Crystal, resistance, superconductor

50. The pros and cons Benefits of superconductorsDrawbacks of superconductors Describe the potential benefits of superconductors Crystal, resistance, superconductor Use page 155 of your textbook to help with this task

51. Exam Tips How to answer an exam question What the examiner is looking for Grade an exam paper and produce a set of ‘exam tips’

57. TASK 1: Using only your exercise book, grade the exam paper using red pen. If you think an answer is incorrect, you must provide a correct answer! TASK 2: Now remark the paper using the mark scheme provided. Did you get a different score? Why was the score different? TASK 3: Now that you know what the examiner is looking for, produce a ‘top 5 tips’ list for answering exam questions

58. You’re the teacher! How to answer an exam question What the examiner is looking for Grade an exam paper and produce a set of ‘exam tips’

60. Group 1 elements Group 7 elements Bonding Atomic Structure Transition metals Water treatment

61. Testing water The tests for sulphate ions and halide ions Why it is important to test water samples Produce word equations for precipitation reactions

62. Substances in water: Why it is important to test water samples Pollutant, chlorination, sedimentation Using page 157 of your textbook give an overview of 1)how water can become polluted 2)How water can be purified http://www.treehugger.com/clean-water/why-bill-gates- drinking-poop-water-video.html

64. The tests for sulphate ions and halide ions Pollutant, chlorination, sedimentation Testing water Testing for sulphate ionsTesting for halide ions Draw the table below. Briefing overview how you test for sulphates and halide ions

65. Produce word equations for precipitation reactions Pollutant, chlorination, sedimentation Equations Sodium sulphate Barium chloride Sodium chloride Barium sulphate + +

66. Produce word equations for precipitation reactions Pollutant, chlorination, sedimentation Equations Sodium chloride Silver nitrate Sodium nitrate Silver chloride + +