retelling of atomic structure

1. Atomic structure Mrs Griffiths Wellington School Visit www.teacherpowerpoints.com For 100’s of free powerpoints

2. Atomic Structure

3. The structure of the atom The Ancient Greeks used to believe that everything was made up of very small particles. I did some experiments in 1808 that proved this and called these particles ATOMS: Dalton ELECTRON – negative, mass nearly nothing PROTON – positive, same mass as neutron (“1”) NEUTRON – neutral, same mass as proton (“1”)

4. The Atom Nucleus Electron Shell or Orbit

5. The Atom Hydrogen Proton Electron Hydrogen has one proton, one electron and NO neutrons

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

7. Mass and atomic number -1 0 Electron 0 1 Neutron 1 1 Proton Relative Charge Relative Mass Particle He 2 4 MASS NUMBER = number of protons + number of neutrons SYMBOL PROTON NUMBER = number of protons (obviously)

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

9. The Atom Lithium Protons Neutrons Electrons

10. The Atom Beryllium Protons Neutrons Electrons Beryllium has four electrons, four protons and five neutrons.

11. The Atom Boron Protons Neutrons Electrons Boron has five electrons, five protons and six neutrons.

12. The Atom Carbon Protons Neutrons Electrons Carbon has six electrons, six protons and six neutrons.

13. The Atom Nitrogen Protons Neutrons Electrons Nitrogen has seven electrons, seven protons and seven neutrons.

14. The Atom Oxygen Protons Neutrons Electrons Oxygen has eight electrons, eight protons and eight neutrons.

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

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

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

18. H 1 1 B 5 11 O 8 16 Na 11 23 Cl 17 35 U 92 238 How many protons, neutrons and electrons?

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

21. 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) H Hg Au Pt Xe I Ag Kr Br Zn Cu Ni Fe Ca K Ar Cl S P Si Al Mg Na Ne F O N C B Be Li He 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

22. The Periodic Table Fact 2: As you move down through the periods an extra electron shell is added: H Hg Au Pt Xe I Ag Kr Br Zn Cu Ni Fe Ca K Ar Cl S P Si Al Mg Na Ne F O N C B Be Li He 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

23. The Periodic Table Fact 3: Most of the elements are metals: H Hg Au Pt Xe I Ag Kr Br Zn Cu Ni Fe Ca K Ar Cl S P Si Al Mg Na Ne F O N C B Be Li He These elements are metals This line divides metals from non-metals These elements are non-metals

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

26. 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)

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

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

30. Group 7 – The Halogens Some facts… 1) Reactivity DECREASES as you go down the group (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): 3) Because of this fluorine and chlorine are liquid at room temperature and bromine is a gas Decreasing reactivity Cl Cl

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

33. Electron structure Consider an atom of Potassium: Potassium has 19 electrons. These are arranged in shells… The inner shell has __ electrons The next shell has __ electrons The next shell has __ electrons The next shell has the remaining __ electron Electron structure = 2,8,8,1 K 19 39 Nucleus

34. How the shells fill with electrons 0 electron 0 electron 0 electron 2 electron Helium He 0 electron 0 electron 0 electron 1 electron Hydrogen H Shell 4 Shell 3 Shell 2 Shell 1 Element

35. How the shells fill with electrons 0 electron 0 electron 2 electron 2 electron Beryllium Be 0 electron 0 electron 1 electron 2 electron Lithium Li Shell 4 Shell 3 Shell 2 Shell 1 Element

36. How the shells fill with electrons 0 electron 0 electron 4 electron 2 electron Carbon C 0 electron 0 electron 3 electron 2 electron Boron B Shell 4 Shell 3 Shell 2 Shell 1 Element

37. How the shells fill with electrons 0 electron 0 electron 6 electron 2 electron Oxygen O 0 electron 0 electron 5 electron 2 electron Nitrogen N Shell 4 Shell 3 Shell 2 Shell 1 Element

38. How the shells fill with electrons 0 electron 0 electron 8 electron 2 electron Neon Ne 0 electron 0 electron 7 electron 2 electron Fluorine F Shell 4 Shell 3 Shell 2 Shell 1 Element

39. How the shells fill with electrons 0 electron 2 electron 8 electron 2 electron Magnesium Mg 0 electron 1 electron 8 electron 2 electron Sodium Na Shell 4 Shell 3 Shell 2 Shell 1 Element

40. How the shells fill with electrons 0 electron 4 electron 8 electron 2 electron Silicon Si 0 electron 3 electron 8 electron 2 electron Aluminium Al Shell 4 Shell 3 Shell 2 Shell 1 Element

41. How the shells fill with electrons 0 electron 6 electron 8 electron 2 electron Sulphur S 0 electron 5 electron 8 electron 2 electron Phosphorus P Shell 4 Shell 3 Shell 2 Shell 1 Element

42. How the shells fill with electrons 0 electron 8 electron 8 electron 2 electron Argon Ar 0 electron 7 electron 8 electron 2 electron Chlorine Cl Shell 4 Shell 3 Shell 2 Shell 1 Element

43. How the shells fill with electrons 2 electron 8 electron 8 electron 2 electron Calcium Ca 1 electron 8 electron 8 electron 2 electron Potassium Shell 4 Shell 3 Shell 2 Shell 1 Element

56. Four factors affecting Reaction Rate Surface Area Concentration Temperature Catalysts

64. Halogens 184 114 Solid Slate grey Iodine 59 -7 Liquid Brown Bromine -34 -101 Gas Green Chlorine B.P. -188 M.P. -220 State Gas Colour Pale Yellow Name Fluorine