1. Atomic structure

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
Electron
Nucleus
Shell or Orbit

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

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

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

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

9. The Atom Lithium
Electrons
Protons
Neutrons

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

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

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

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

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

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

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

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

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

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

20. 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 He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg
These elements have __ electrons in their outer shells
These elements have __ electrons in their outer shell
E.g. all group 1 metals have __ electron in their outer shell

21. 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 H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg
Sodium has 11 electrons in the configuration 2,8,1
Potassium has 19 electrons in the configuration __,__,__

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

23. 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. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn Br Kr Ag I Xe Pt Au Hg
E.g. consider the group 1 metals. They all:
Are soft
Can be easily cut with a knife
React with water

24. Group 1 – The alkali metalsNa K Rb Cs Fr

25. Group 1 – The alkali metals
Some facts…
1) These metals all have ___ electron in their outer shell
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:
Potassium + water potassium hydroxide + hydrogen
2K(s) H2O(l) KOH(aq) H2(g)
Words – down, one, shell, hydrogen, nucleus

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

27. 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
Helium is lighter then air and is used in balloons and airships (as well as for talking in a silly voice)
Argon is used in light bulbs (because it is so unreactive) and argon , krypton and neon are used in fancy lights

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

29. Group 7 – The Halogens Some facts… Decreasing reactivity
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): Cl Cl
3) Because of this fluorine and chlorine are liquid at room temperature and bromine is a gas

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

31. How shells fill
The first electron shell can only hold a maximum of two electrons.
The second electron shell can hold a maximum of eight electrons.
The third electron shell can also hold a maximum of eight electrons.
The fourth electron shell can also hold eight electrons.

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

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

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

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

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

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

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

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

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

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

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

43. The First Twenty Elements
Hydrogen 1,0,0,0
Helium ,0,0,0
Lithium ,1,0,0
Beryllium 2,2,0,0
Boron ,3,0,0
Carbon ,4,0,0
Nitrogen ,5,0,0

44. First 20 Elements continued
Oxygen ,6,0,0
Fluorine ,7,0,0
Neon ,8,0,0
Sodium ,8,1,0
Magnesium 2,8,2,0
Aluminium 2,8,3,0
Silicon ,8,4,0

45. First 20 Elements continued
Phosphorus ,8,5,0
Sulphur ,8,6,0
Chlorine ,8,7,0
Argon ,8,8,0
Potassium ,8,8,1
Calcium ,8,8,2

46. 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.

47. 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.

48. 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.

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

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

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

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

53. Fluorine reacts with sodium chloride
Fluorine reacts with sodium chloride. Which equation is correctly shows this reaction?
F2 + 2Na  2NaF
F + Na  NaF
2F + 2Na  2NaF

54. Which will displace? 2NaF + Cl2  Yes or No 2NaBr + Cl2  Yes or No
2KI + I2  Yes or No
2LiCl + I2  Yes or No
2NaBr + I2  Yes or No
2NaBr + F2 Yes or No
Cl2 + 2NaBr  Yes or No

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

56. Catalyst
A catalyst speeds up or slows down a reaction but does not get used up by the reaction.

57. Temperature
If we increase the temperature of a reaction by 100C the rate will double this means the reaction will be complete in half the time.

58. Concentration
If we increase the concentration of a reactant the number of particles increase that in turn increases the chance of a collision and initiates a chemical reaction.

59. Surface area
The larger the particle size the smaller the relative area the slower the reaction.
The smaller the particle size the greater the relative surface area and the faster the reaction.

60. 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.

61. 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.

62. 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

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

64. Reactions Sodium and Chlorine react to form  Sodium Chloride.
Iron and Chlorine react to form 
Iron Chloride.
2Na + Cl2  2NaCl.
Fe + Cl2  FeCl2.

65. 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.