1. THE PERIODIC TABLE

2. STARTER: There are millions of substances in the world.
All these substances are made from about 100 different building blocks called elements.
These elements take a huge variety of forms:
From poison gases like chlorine
From reactive metals like sodium
to unreactive metals like gold
To the air we breathe

3. Properties of Elements
In science the word properties means, what the substance is like.
For example, here are some properties of sodium:
Metallic
Highly reactive
Solid but melts easily
Low density (light)
It would be really useful to be able to predict properties of elements instead of having to remember them!

4. Exploration Phet “Build an Atom” Simulation
LINK

5. Atomic Number Particle Charge Relative Mass Protons +1 1 Neutrons
Scientists found that the properties of elements seem to depend upon atomic number.
Atoms contain three types of particles:
Particle
Charge
Relative Mass
Protons +1 1
Neutrons
Electrons -1
0.0005
Atomic number = the number of protons in an atom.

6. Atomic Number and Electrons
In elements the atoms contain equal numbers of protons and electrons.
It follows that for an element the atomic number is equal both to the number of protons and to the number of electrons.
Atomic Number
Fluorine
9 protons 9+
9 electrons 9-
10 neutrons 0
Total Charge 0 19 F 9
Symbol
Atomic Mass

7. Atomic Number and Patterns
When scientists arranged elements in order of increasing atomic number (below) they found patterns in the properties.
Reactive Metals
Reactive Gases
Unreactive Gases K H Li Na Be Mg Al P N O S Cl F Ne Ar Si He B C

8. Do similar elements occur at regular intervals?
Reactive Metals
Reactive Gases K H Li Na Be Mg Al P N O S Cl F Ne Ar Si He B C 19 1 3 11 4 12 13 15 7 8 16 17 9 10 18 14 2 5 6
Count the number of elements to get from one reactive metal to the next? 8
Count the number of elements to get from one reactive gas to the next? 8

9. Putting elements in a table
If we divide the elements up and arrange them into a table we easily get patterns. K H Li Na Be Mg Al P N O S Cl F Ne Ar Si He B C 19 1 3 11 4 12 13 15 7 8 16 17 9 10 18 14 2 5 6
Cut here
and here
and here
And arrange these strips below each other H He Li Be N O F Ne B C Na Mg Al P S Cl Ar Si K Na Mg

10. Putting elements in a table
When we rearrange the strips elements that are similar go into the same columns. H He 1 2 Li Be N O F Ne B C 3 4 7 8 9 10 5 6 Na Mg Al P S Cl Ar Si 11 12 13 15 16 17 18 14 K 19 Li K Na
Reactive Metals Cl F
Reactive Gases Ar Ne He
Unreactive Gases Al P S Si Be N O B C Mg Na Mg

11. Putting elements in a table
Carrying on building up the elements by atomic number led to the creation of the periodic table shown below. H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As Na Mg

12. Groups – columns of elements
Downward columns are called groups. H Li Na K Rb Cs Fr
Group 1 Be Mg Ca Sr Ba Ra
Group 2 Ga In Tl Al B
Group 3 Ge Sn Pb Si C
Group 4 Sb Bi P N As
Group 5 Se Te Po O S
Group 6 Br At Cl F I
Group 7 He Kr Ne Ar Rn Xe
Group 0
Means in-between Sc Ti V Cr Mn Fe Co Ni Cu Zn Y Zr Nb Mo Tc Ru Pd Ag Cd Rh Hf Ta W Re Os Ir Au Hg La Pt Rf Db Sg Bh Hs Mt ? Ac
Transition Elements Na Mg

13. Periods – rows of elements
Rows of elements are called periods.
Period Number H He 1 Li Be N O F Ne B C 2 Na Mg Al P S Cl Ar Si 3 K Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr As 4 Rb Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh I Xe 5 Cs Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Rn 6 Fr Ra Rf Db Sg Bh Hs Mt ? Ac 7

14. What’s the group and Period? K C Cl MgGp 1 2 3 4 5 6 7 Pd H 1 He 2 Li Be B C C N O F Ne 3 Na Mg Mg Al Si P S Cl Cl Ar 4 K K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ?
What’s the group and Period? K C Cl Mg
Group 1 Period 4
Group 7 Period 3
Group 4 Period 2
Group 2 Period 3

15. Missing elements!
Below the chemical symbol have been replaced by atomic numbers. You will see some are missing! 1 3 11 19 37 55 87 4 21 22 12 23 24 25 26 27 28 29 30 31 32 34 35 20 36 39 40 41 42 43 44 46 47 48 49 50 51 38 52 45 56 72 73 74 75 76 77 79 80 81 82 83 84 57 85 78 88
104
105
106
107
108
109
111
112 89
110 13 15 7 8 16 17 9 10 18 86 53 14 54 2 5 6 33
Two further series of elements should go here but are only shown on some Periodic Tables. They are called the lanthanides and actinides.

16. Patterns 1. Metals and Non-metals
Metals are on the left and centre.
Non-metals are mostly on the right
In between are metalloids.
These are like metals in some ways and like no-metals in others.

17. Patterns 1. Metals and Non-metals

18. Say whether these elements are metals, non-metals or metalloids.
Cobalt (Co)
Krypton (Kr)
Scandium (Sc)
Francium (Fr)
Silicon (Si)
Metal
Metal
Non-metal
Metal
Metalloid H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As

19. Physical State Physical state means – is it a solid, liquid or gas.
There are only 2 liquid elements.
Notice how most of the gases are on the far right.

20. Physical State

21. Say whether these elements are solids, liquids or gases.
Bromine (Br)
Barium (Ba)
Nitrogen (N)
Niobium (Nb)
Krypton (Kr)
Solid
Solid
Gas
Gas
Liquid H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As N Br Kr Nb Ba

22. Patterns 2. Reactivity of Metals
As a general, but not perfect, rule: the further to the left and the further down the table - the more reactive the metal is.
More Reactive
More Reactive

23. Which metal is most reactive?
Potassium (K) or Lithium (Li)
Calcium (Ca) or Iron (Fe)
Calcium (Ca) or Magnesium (Mg)
Copper (Cu) or Barium (Ba) Ca K Ba Ca H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Ca Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al

24. Patterns 3. Reactivity of Non-Metals
This is more complicated.
At the very end of the periodic table is the most unreactive group of elements in the table.
Apart from that – the further up and the further right – the more reactive the non-metal.
More reactive
Unreactive
More reactive

25. Which non-metal is most reactive?
Neon (Ne) or Iodine (I)
Carbon (C) or Oxygen (O)
Fluorine (F) or Chlorine (Cl)
Oxygen (O) or Silicon (Si) I O F O Se Br Kr Te At P N O S Cl F Ne Ar Rn I Si Xe He B C As

26. Patterns and Electron Structures
The physical and chemical properties of elements are hugely influenced by the number and arrangement of electrons in the atom.
This is why patterns in properties are linked to atomic number.
If the atomic number increases by one it means that the atom has one extra electron. 1 H 4 He 2 7 Li 3 9 Be 10 B 5
Each element has one more electron
Atomic number = number of protons
For atoms of an element it is also = number of electrons

27. Patterns and Electron Structures
The places where we start a new period is to do with the arrangement of the electrons.
It is the point at which electrons start entering a new shell further from the nucleus. K H Li Na Be Mg Al P N O S Cl F Ne Ar Si He B C 19 1 3 11 4 12 13 15 7 8 16 17 9 10 18 14 2 5 6
Cut here
and here
and here
We shall look at these electron arrangements in the next few slides.

28. Patterns of Electron Arrangements
We can imagine building up atoms by adding protons, neutrons and electrons as we cross the periodic table. 1 2
2,1
2,2
2,5
2,6
2,7
2,8
2,3
2,4
2,8,1
2,8,2
2,8,3
2,8,5
2,8,6
2,8,7
2,8,8
2,8,4
2,8,8,1
2,8,8,2 Sc Ti V Cr Mn Fe Co Ni Cu Zn
2,8,8,2
Electrons
in 1st shell
Electrons
in 2nd shell
Electrons
in 3rd shell
Electrons
in 4th shell

29. What’s the electron arrangement C Mg K ClGp 1 2 3 4 5 6 7 Pd H 1 He 2 Li Be B C C N O F Ne 3 Na Mg Mg Al Si P S Cl Cl Ar 4 K K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ?
What’s the electron arrangement C Mg K Cl
2.8.7
2.4
2.8.2

30. Arrangement of Electrons1 2 3 4 5 6 7 8 1 2 3
Click on action buttons to reveal how electron configuration is built-up.
The transition metals
Skip this

31. Electrons in Period 1 1 2 3 4 5 6 7 8 1 1 2
Skip this

32. Electrons in Period 2
Elements in the second period contain 2 electrons in the first shell (complete) and the second shell is completed one electron at a time as you cross the period from left to right. 1 2 3 4 5 6 7 8 2
2,1
2,2
2,3
2,4
2,5
2,6
2,7
2,8
This atom is
special it has a complete outer shell
Skip this

33. Electrons in Period 3
Elements in the third period have complete first and second shells. The third shell is completed one electron at a time as you cross the period from left to right. 1 2 3 4 5 6 7 8 3
2,8,1
2,8,2
2,8,3
2,8,4
2,8,5
2,8,6
2,8,7
2,8,8
Skip this

34. Group 1 Elements 1
Group 1 elements have 1 electron in the outermost shell which they lose in chemical reactions.
The outer electron is further from the nucleus and so more easily lost as you go down the group.
This is why reactivity increases going downwards 1 1 2
2,1 3
Skip this
2,8,1

35. Group 2 Elements
In chemical reactions metals tend to lose their outer shell electrons to form positive ions.
So, these elements all form ions with a 2+ charge.
The further the outer shell is from the nucleus the more easily electrons are lost. 2
2,2
2,8,2
Skip this

36. Group 3 Elements 3
Metals lose their outer electrons to form ions. The charge on the ion produced by Group 3 metals will be +3.
2,3
Skip this
2,8,3

37. Group 4 Elements 4
The elements at the top of Group 4 are non-metals. They bond covalently, i.e. by sharing electrons with another atom.
2,4
Skip this
2,8,4

38. Group 5 Elements 5
The number of electrons in the outermost shell is the same as the group number.
They need 3 more electrons to achieve a full electron shell.
2,5
Skip this
2,8,5

39. Group 6 Elements
The atoms in Group 6 form negative ions (2-) by the addition of two extra electrons. This completes their outer most shell. 6
2,6
Skip this
2,8,6

40. Group 7 Elements
Group 7 elements form 1- ions by the addition of 1 extra electron.
They are most reactive at the top of the group because incoming electrons are pulled into shells that are closer to the nucleus. 7
2,7
Skip this
2,8,7

41. Group 0 Elements 8
The elements in Group 8 (or 0) have complete outer shells.
They are very unreactive and are called NOBLE (or inert) GASES. 2
2,8
Skip this
2,8,8

42. Periodic Table and Reactivity
The fact that in each group the number of outer shell electrons is the same leads to similar types of chemical reactivity.
For example, all group 1 elements react with water to give hydrogen and an alkali.
The fact that the outer shell electrons get progressively further from the nucleus leads to trends (patterns).
For example, Group 1 elements get more reactive as you go down the group.

43. Broad Types of Element

44. In the Periodic Table elements are arranged in order of?
Atomic mass
Atomic number
Density
Boiling point

45. Neutral atoms of an element contain?
Equal numbers of protons and neutrons
Equal numbers of electrons and neutrons
Equal numbers of protons and electrons
Equal numbers of protons, neutrons and electrons

46. A vertical collection of elements in the Periodic Table are called?
Groups
Periods
Columns
Gases

47. A horizontal collection of elements in the Periodic Table are called?
Groups
Periods
Rows
Gases

48. In the Periodic Table gases occur?
On the left
On the left and middle
On the right and middle
On the right

49. In the Periodic Table metals occur?
On the left
On the left and middle
On the right and middle
On the Right

50. The Group 7 Elements are also called?
The halogens
The transition elements
The alkali metals
The noble gases

51. The Group 1 Elements are also called?
The halogens
The transition elements
The alkali metals
The noble gases

52. In the Periodic Table metals get more reactive going towards?
Top left
Top right
Bottom left
Bottom right

53. Which of these electron arrangements could be a noble gas?
2.1,
2.5
2.7
2.8

54. Which of these electron arrangements could be a halogen?
2.1,
2.5
2.7
2.8

55. Teacher Resources

56. THE PERIODIC TABLE H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni CuZn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As

57. H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As