1. The Periodic Table

2. MENDELEEV

3. Old image of periodic table

4. The following slides show the Structure of the atom and how this relates to the Modern Peiodic Table

5. The Atom Nucleus Electron Shell or Orbit

6. The structure of the atom ELECTRON negative, mass nearly nothing PROTON positive, same mass as neutron (“1”) NEUTRON neutral, same mass as proton (“1”)

7. Mass and atomic number ParticleRelative MassRelative Charge Proton11 Neutron10 Electron0 MASS NUMBER = number of protons + number of neutrons SYMBOL PROTON NUMBER = number of protons (obviously)

8. How many protons, neutrons and electrons?

9. Mendeleev Periodic table The periodic table arranges all the elements in groups according to their properties. Horizontal rows are called PERIODS Vertical columns are called GROUPS

10. HHe LiBeBCNOFNe Na MgMg AlSiPSClAr KCaFeNi CuCu ZnBrKr AgIXe Pt AuAu HgHg The Periodic Table Fact 1: Elements in the same group have the same number of electrons in the outer shell (this correspond to their group number) E.g. all group 1 metals have __ electron in their outer shell These elements have __ electrons in their outer shell These elements have __ electrons in their outer shells

11. HHe LiBeBCNOFNe Na MgMg AlSiPSClAr KCaFeNi CuCu ZnBrKr AgIXe Pt AuAu HgHg The Periodic Table Fact 2: As you move down through the periods an extra electron shell is added: E.g. Lithium has 3 electron in the configuration 2,1 Potassium has 19 electrons in the configuration __,__,__ Sodium has 11 electrons in the configuration 2,8,1

12. HHe LiBeBCNOFNe Na MgMg AlSiPSClAr KCaFeNi CuCu ZnBrKr AgIXe Pt AuAu HgHg The Periodic Table Fact 3: Most of the elements are metals: These elements are metals This line divides metals from non- metals These elements are non-metals

13. HHe LiBeBCNOFNe Na MgMg AlSiPSClAr KCaFeNi CuCu ZnBrKr AgIXe Pt AuAu HgHg The Periodic Table Fact 4: (Most important) All of the elements in the same group have similar PROPERTIES. This is how I thought of the periodic table in the first place. This is called PERIODICITY. E.g. consider the group 1 metals. They all: 1)Are soft 2)Can be easily cut with a knife 3)React with water

14. Group 0 – The Noble gases He Ne Ar Kr Xe Rn

15. The Nobel gases The Nobel gases have full outer shells and they are found in group 0 of the periodic table. Helium, Neon, Argon, Krypton, Xenon and Radon.

16. Group 0 These are the noble gases. They have complete electron shells. The electron shells are full. They are unreactive. They are inert. They do not react. They include, Helium, Neon, Argon, Krypton, Xenon and Radon

17. Group 0 – The Noble gases Some facts… 1) All of the noble gases have a full outer shell, so they are very _____________ 2) They all have low melting and boiling points 3) They exist as single atoms rather then diatomic molecules 4)Helium is lighter then air and is used in balloons and airships (as well as for talking in a silly voice) 5)Argon is used in light bulbs (because it is so unreactive) and argon, krypton and neon are used in fancy lights

18. The Atom Helium Electron Proton Neutron Helium has two electrons, two protons and two neutrons

19. The Atom Neon Protons Neutrons Electrons Neon has ten electrons, ten protons and ten neutrons.

20. Group 1 – The alkali metals Li Na K Rb Cs Fr

21. The Alkali metals Lithium, Sodium and Potassium have one electron in their outer shell and this is why they are found in group one of the periodic table.

22. Group 1 Lithium, sodium and potassium are all in group 1. They all have one electron in the outer shell. They are all metals. They react with group 7 to form metal halides.

23. Group 1 – The alkali metals 1) These metals all have ___ electron in their outer shell Some facts… 2) Reactivity increases as you go _______ the group. This is because the electrons are further away from the _______ every time a _____ is added, so they are given up more easily. 3) They all react with water to form an alkali (hence their name) and __________, e.g: Words – down, one, shell, hydrogen, nucleus Potassium + water potassium hydroxide + hydrogen 2K (s) + 2H 2 O (l) 2KOH (aq) + H 2(g)

24. The Atom Lithium Protons Neutrons Electrons

25. The Atom Sodium Protons Neutrons Electrons Sodium has eleven electrons, eleven protons and twelve neutrons.

26. Group 7 – The halogens F Cl Br I At

27. The Halogens Fluorine, Chlorine, Bromine and Iodine are the Halogens and they all have seven electrons in their outer shell. This is why they are found in group 7 of the periodic table.

28. Group 7 Fluorine,Chlorine, Bromine and Iodine. They all have 7 electrons in their outer shell. They are all coloured. They form metal halides with group 1 metals.

29. Group 7 – The Halogens Some facts… 1) Reactivity DECREASES as you go down the group Decreasing reactivity (This is because the electrons are further away from the nucleus and so any extra electrons aren’t attracted as much). 2) They exist as diatomic molecules (so that they both have a full outer shell): Cl 3) Because of this fluorine and chlorine are liquid at room temperature and bromine is a gas

30. Halogens Name Fluorine Colour Pale Yellow State Gas M.P. -220 B.P. -188 ChlorineGreenGas-101-34 BromineBrownLiquid-759 IodineSlate grey Solid114184

31. The Atom Fluorine Protons Neutrons Electrons Fluorine has nine electrons, nine protons and ten neutrons.

32. Uses of the Halogens Fluorine is put into water supplies to kill harmful bacteria and to help keep teeth healthy. Chlorine is used in swimming pools to bacteria in the water. Bromine is used in pesticides. Silver bromide is used in photography. Iodine is an antiseptic on cuts and grazes.

33. The halogens – some reactions 1) Halogen + metal: Na + Cl - Na Cl + 2) Halogen + non-metal: H Cl + H Halogen + metal ionic salt Halogen + non-metal covalent molecule

34. Reactions Sodium and Chlorine react to form  Sodium Chloride. Iron and Chlorine react to form  Iron Chloride. 2Na + Cl 2  2NaCl. Fe + Cl 2  FeCl 2.

35. Displacement Fluorine can displace Chlorine, Bromine and Iodine. F Cl Br I

36. Displacement Chlorine can displace Bromine and Iodine but it cannot displace Fluorine Cl Br I F

37. Displacement Bromine can displace Iodine but it cannot displace Fluorine or Chlorine Br I F Cl

38. Displacement Iodine cannot displace Iodine Fluorine, Chlorine or Bromine I F Cl Br

39. Fluorine reacts with sodium chloride. Which equation is correctly shows this reaction? F 2 + 2Na  2NaF F + Na  NaF 2F + 2Na  2NaF

40. Which will displace? 2NaF + Cl 2  Yes or No 2NaBr + Cl 2  Yes or No 2KI + I 2  Yes or No 2LiCl + I 2  Yes or No 2NaBr + I 2  Yes or No 2NaBr + F 2  Yes or No Cl 2 + 2NaBr  Yes or No