1. Chemistry
The Periodic Table

2. The elements in the periodic table

3. Names of groups in the periodic table

4. Solids, liquids and gases

5. Matching elements and groups

6. Hydrogen does not belong to any group –because it does not fit easily to any trends shown in any one group

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

8. Missing elements!
In this periodic table the symbols are replaced by atomic numbers. Some of the numbers are missing – where?
Two more rows of elements fit here. 87 88 89
104
105
106
107
108
109
110
111
112
113
114
115
116
117
118 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 37 38 39 40 41 42 43 44 45 46 47 49 50 51 52 53 54 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 11 12 13 14 15 16 17 18 3 4 5 6 7 8 9 10 1 2
They are called the lanthanides and actinides and are only shown on some periodic tables.

9. Atomic number, charge and electrons
Atoms contain equal numbers of protons and electrons. This means that atoms are neutral.
What is the charge of a fluorine atom?
9 protons = +9
9 electrons = -9
10 neutrons = 0
Total charge = 0
What links atomic number and the number of electrons?
atomic number = the number of electrons in an atom

10. Atomic structure revisited

11. Mendeleev and the periodic table
Mendeleev created the first modern periodic table by grouping together elements with similar properties.

12. Properties of elements
What is a property of an element?
A property is any characteristic of an element.
For example, here are some properties of sodium:
metallic
highly reactive
solid but melts easily
feels light (low density)
It would be really useful to be able to predict properties of elements instead of having to remember them!

13. Properties of elements
From sodium, a reactive metal…
…to gold, an unreactive metal.
From chlorine, a poisonous gas…
…to oxygen, a life-giving gas.

14. Columns of elements What are columns of elements called? 1 2 groups 34 5 6 7 Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Rg ? Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Na Mg Al Si P S Cl Ar Li Be B C N O F Ne H He

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

16. Groups and periods

17. What’s the electron arrangement?

18. Atomic number and patterns of behaviour
If the elements are arranged in order of increasing atomic number, patterns in their properties can be seen.
reactive gases
reactive metals H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K
unreactive gases

19. Positions of similar elements
Compare the positions of similar elements:
reactive gases
reactive metals H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K
unreactive gases
How many elements from one reactive gas to the next? 8
How many elements from one reactive metal to the next? 8
How many elements from one unreactive gas to the next? 8

20. Arranging elements
Divide the elements at set intervals into separate rows:
cut here
cut here
cut here H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K
Arrange these rows so elements with matching properties are together: H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K

21. Arranging elements into columns
When elements are arranged according to their properties what patterns do you see?
hydrogen is a special case H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K
reactive gases
unreactive gases
reactive metals
Similar elements go into the same columns.
Hydrogen is an exception – it is best positioned above the reactive metals.

22. note Compare the positions of similar elements: reactive gases
reactive metals H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K
unreactive gases
Group 0 is very close to group 1 and 7 : both groups can easily achieve a noble gas electron structure . Group 1 : lose electron to be like the near noble gas .
Group 7 : gain or share electrons to be like the near noble gas.

23. H He Electrons in period 1
Elements in period 1 only have electrons in the first shell.
Why are there only two elements in period 1? 1 2 3 4 5 6 7 H He 1 1 2
The first shell can only hold a maximum of two electrons,
so period 1 only includes the elements hydrogen and helium.
What is special about the outer shell of helium?

24. Li Be B C N O F Ne Electrons in period 2
Elements in period 2 all have a complete first shell.
What happens to electrons in the second shell in period 2? 1 2 3 4 5 6 7 Li Be B C N O F Ne 2
2,1
2,2
2,3
2,4
2,5
2,6
2,7
2,8
The second shell is completed one electron at a time going across the period from left to right.
What is special about the outer shell of neon?

25. Na Mg Al Si P S Cl Ar Electrons in period 3
Elements in period 3 have complete first and second shells.
What happens to electrons in the third shell in period 3? 1 2 3 4 5 6 7 Na Mg Al Si P S Cl Ar 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
The third shell is completed one electron at a time going across the period from left to right.
What is special about the outer shell of argon?

26. Patterns of electron arrangements
Consider the electron arrangements of the first 20 elements in the periodic table. 1 2 3 4 5 6 7 1 1 2 2
2,1
2,2
2,3
2,4
2,5
2,6
2,7
2,8 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 4
2,8,8,1
2,8,8,2
What is the pattern of outer shell electrons in a group?
What is the pattern of outer shell electrons across a period?
What is the pattern of full electron shells in a group?

27. Electron trends in the periodic table
Trends down a group:
the number of complete electron shells increases by one;
the number of outer shell electrons is the same.
The number of a group is the same as the number of electrons in the outer shell of elements in that group, except for group 0.
Trends across a period:
the number of outer shell electrons increases by one;
the number of complete electron shells stays the same.
The point at which a new period starts is the point at which electrons begin to fill a new shell.

28. Electrons and groups

29. Patterns: reactivity of metals
What happens to the reactivity of metals along a period?
What happens to the reactivity of metals down a group?
Which is the most reactive metal?
increase in reactivity Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Rg Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Na Mg Al Li Be
increase in reactivity

30. Which metal is more reactive?

31. Boardworks GCSE Additional Science: Chemistry
Reacting with water
Boardworks GCSE Additional Science: Chemistry
Group 1 – Alkali Metals
Teacher notes
This virtual experiment illustrates how each of the alkali metals reacts with water. You may want to show the reaction for two or three of these metals and then ask students to predict the other reactions using what they have learned about the reactivity trends in the periodic table.

32. Patterns: reactivity of non-metals
Group 0 elements are the most unreactive of all elements.
For the remaining non-metals and metalloids, reactivity increases up a group and along a period from left to right. At Rn Sb Te I Xe Ge As Se Br Kr Si P S Cl Ar B C N O F Ne He
increase in reactivity
Which is the most reactive non-metal ?
unreactive
increase in reactivity

33. Which non-metal is more reactive?

34. Halogen reaction with iron wool
Teacher notes
This virtual experiment compares the reactivity of the halogens with iron wool. It could be used as a precursor to running the practical in the lab, or as a revision exercise. When using this activity, it should be made clear that with iodine, the reaction takes several minutes of strong heating before it reacts. This is illustrated by the stop watch, but is not shown in real time.

35. Multiple-choice quiz

36. Anagrams

37. Glossary
atomic number – The number of protons in an atom. Sometimes called the proton number.
electron arrangement – A shorthand way of writing the number of electrons in an atom’s electron shells.
element – A substance made up of only one type of atom.
group – A column in the periodic table containing elements with the same number of outer shell electrons and similar chemical properties.
period – A row in the periodic table containing elements with the same number of full electron shells.
periodic table – A table that lists all the elements in order of increasing atomic number, arranged into groups and periods.
property – Any characteristic of an element.