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iGCSE chemistry Section 2 lesson 1

iGCSE chemistry Section 2 lesson 1. Content. The iGCSE Chemistry course. Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3 Organic Chemistry Section 4 Physical Chemistry Section 5 Chemistry in Society. Content. Section 2

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iGCSE chemistry Section 2 lesson 1

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  1. iGCSE chemistrySection 2 lesson 1

  2. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3 Organic Chemistry Section 4 Physical Chemistry Section 5 Chemistry in Society

  3. Content Section 2 Chemistry of the Elements • The Periodic Table • Group 1 Elements • Group 7 Elements • Oxygen and Oxides • Hydrogen and Water • Reactivity Series • Tests for ions and gases

  4. Content • The Periodic Table • 2.1 understand the terms group and period • 2.2 recall the positions of metals and non-metals in the Periodic Table • 2.3 explain the classification of elements as metals or non-metals on the basis of their electrical conductivity and the acid-base character of their oxides • 2.4 understand why elements in the same group of the Periodic Table have similar chemical properties • 2.5 understand that the noble gases (Group 0) are a family of inert gases and explain their lack of reactivity in terms of their electronic configurations. • b) Group 1 elements — lithium, sodium and potassium • 2.6 describe the reactions of these elements with water and understand that the reactions provide a basis for their recognition as a family of elements • 2.7 describe the relative reactivities of the elements in Group 1 • 2.8 explain the relative reactivities of the elements in Group 1 in terms of distance between the outer electrons and the nucleus. • Lesson 1 • The Periodic Table • Group 1 elements

  5. The Periodic Table

  6. The Periodic Table Groups

  7. The Periodic Table Groups 1 2 3 4 5 6 7 8 (0)

  8. The Periodic Table Periods

  9. The Periodic Table 1 2 3 4 5 6 7 Periods

  10. The Periodic Table Noble gases Alkali metals Alkaline Earth metals Halogens Transition metals

  11. The Periodic Table Sn = tin Group 4 Period 5

  12. The Periodic Table Non-metals Metals

  13. The Periodic Table The chemical elements are arranged in order of increasing atomic number

  14. The Periodic Table Elements in the same group have the same number of electrons in their outermost shell. This is the same as the group number

  15. The Periodic Table Elements in the same period have the same number of shells. This is the same as the period number

  16. Metals and non-metals

  17. Metals and non-metals More than ¾ of the elements in the Periodic Table are metals

  18. Metals and non-metals More than ¾ of the elements in the Periodic Table are metals So what defines a metal?

  19. Metals and non-metals Metals, such as gold, are good electrical conductors. This is because they have a giant structure in which electrons in the highest energy level are free to move through the entire structure.

  20. Metals and non-metals Metals, such as gold, are good electrical conductors. This is because they have a giant structure in which electrons in the highest energy level are free to move through the entire structure. Non-metals, such as sulphur, are very poor conductors of electricity, or do not conduct at all.

  21. Metals and non-metals Both metals and non-metals form oxides. For example: copper oxide CuO sulphur dioxide SO2

  22. Metals and non-metals Both metals and non-metals form oxides. For example: copper oxide CuO sulphur dioxide SO2 Oxides of metallic elements are bases, those which dissolve in water form alkalis.

  23. Metals and non-metals Both metals and non-metals form oxides. For example: copper oxide CuO sulphur dioxide SO2 Oxides of metallic elements are bases, those which dissolve in water form alkalis. Oxides of non-metallic elements tend to be acids.

  24. Metals and non-metals Metallic elements Non-metallic elements Combine with oxygen to form oxides Oxides of metallic elements are solids Many non-metallic oxides are gases, some are liquids and some solids Oxides of metallic elements are all bases Bases soluble in water are called alkalis Some bases are insoluble Most dissolve in water to form acids Some are insoluble and neutral

  25. Metals and non-metals Non-metal oxides as acids: Sulphur dioxide + Water  Sulphurous acid SO2 + H2O  H2SO3

  26. Metals and non-metals Metal oxides as bases: Base + Acid  Salt + Water eg. CuO + H2SO4 CuSO4 + H2O

  27. Groups and chemical properties

  28. The Group Number tells you how many electrons there are in the outer shell (orbit) of an element. For example, oxygen is in Group 6, so has 6 electrons in its outermost shell (2:6)

  29. The Period Number tells you how many shells (orbits) there are around the nucleus. For example, Calcium is in Period 4, so will have 4 shells around the nucleus

  30. The Period Number tells you how many shells (orbits) there are around the nucleus. For example, Calcium is in Period 4, so will have 4 shells around the nucleus

  31. Groups and chemical properties why do elements in the same group of the Periodic Table have similar chemical properties

  32. Groups and chemical properties why do elements in the same group of the Periodic Table have similar chemical properties It’s all to do with their electronic configuration.

  33. Groups and chemical properties why do elements in the same group of the Periodic Table have similar chemical properties It’s all to do with their electronic configuration. In order to be stable, atoms need a full outer shell of electrons

  34. Groups and chemical properties Elements in the same group have the same number of electrons in their outermost shell

  35. Groups and chemical properties Atoms need to lose or gain electrons in order to become stable

  36. Groups and chemical properties Metals lose their outer electron or electrons when they react, and non-metals gain

  37. Groups and chemical properties The fewer electrons that need to be lost or gained, the more reactive the element

  38. Groups and chemical properties The fewer electrons that need to be lost or gained, the more reactive the element

  39. Groups and chemical properties Non-metals

  40. Groups and chemical properties Group 1 elements lose one electron to become stable

  41. Groups and chemical properties Group 1 elements lose one electron to become stable Group 2 elements lose two electrons to become stable

  42. Groups and chemical properties Group 1 elements lose one electron to become stable Group 2 elements lose two electrons to become stable Group 3 elements lose three electrons to become stable

  43. Groups and chemical properties Group 5 elements gain three electrons to become stable Group 6 elements gain two electrons to become stable Group 7 elements gain one electron to become stable

  44. Groups and chemical properties The fewer electrons that need to be lost or gained, the more reactive the element

  45. Groups and chemical properties Group 1 are the most reactive metals Group 7 are the most reactive non-metals

  46. Groups and chemical properties What about the elements in Group 8 (0) ? Why are they so unreactive?

  47. Groups and chemical properties What about the elements in Group 8 (0) ? Why are they so unreactive? 2 2:8 2:8:8 Look at their electron configurations – can you see why they don’t react?

  48. Groups and chemical properties What about the elements in Group 8 (0) ? Why are they so unreactive? 2 2:8 2:8:8 Look at their electron configurations – can you see why they don’t react? They already have full outer shells of electrons, so they don’t need to lose or gain any more. This is why they are called the inert gases. They don’t usually react. (They are also know as the rare or noble gases)

  49. Content • The Periodic Table • 2.1 understand the terms group and period • 2.2 recall the positions of metals and non-metals in the Periodic Table • 2.3 explain the classification of elements as metals or non-metals on the basis of their electrical conductivity and the acid-base character of their oxides • 2.4 understand why elements in the same group of the Periodic Table have similar chemical properties • 2.5 understand that the noble gases (Group 0) are a family of inert gases and explain their lack of reactivity in terms of their electronic configurations. • b) Group 1 elements — lithium, sodium and potassium • 2.6 describe the reactions of these elements with water and understand that the reactions provide a basis for their recognition as a family of elements • 2.7 describe the relative reactivities of the elements in Group 1 • 2.8 explain the relative reactivities of the elements in Group 1 in terms of distance between the outer electrons and the nucleus. • Lesson 1 • The Periodic Table • Group 1 elements

  50. Group 1 – The Alkali Metals

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