2.  To consider how the properties of titanium relate to its uses  To consider the development of the periodic table and the position of elements within it  To appreciate grouping of elements by physical and chemical properties  To recap on how the extraction processes for metals relate to their reactivity

3. PropertiesUses Low density Strong Can be alloyed with Iron, Aluminium, Vanadium, Molybdenum Lustrous / high strength to weight ratio/Silver colour Corrosion-resistant Biocompatable (non-toxic to or rejected by the body) Can make strong lightweight alloys for aircraft and aerospace manufacture Jewellery, sporting goods, mobile phones Reaction Vessels and pipes Medical prostheses, orthopedic and dental implants and instruments

4.  By mid 1600s only 10 elements had been identified – most had been known since prehistoric times  1669- While searching for the ‘Elixir of Life’ Hennig Brand heated urine and discovered Phosphorus  Over next 150 years – 30 new elements discovered

5.  Titanium – discovered in 1791 by William Gregor from the mineral ilmenite  Martin Heinrich Klaproth separated Titanium oxide and named it after the Titans of Greek Mythology  Isolated as impure titanium in 1825 by Jons Jakob Berzelius  difficult to isolate due to stability of its oxides

6.  First published by Russia chemist Dmitri Mendeleev  arranges elements in rows (periods) by increasing atomic number  In columns or groups by chemical properties and electron arrangement

7. Trends in the Periodic Table and Bonding

8. The periodic table is a very useful arrangement of all of the known chemical elements. It can be used to observe patterns and relationships between different elements, and the table is arranged in several important ways.

9. Horizontal rows in the periodic table are called periods. Elements are arranged in the periodic table in order of increasing atomic number. Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 The outer electron shell becomes filled as we move from left to right. Li 2,1 Be 2,2 B 2,3 C 2,4 N 2,5 O 2,6 F 2,7 Ne 2,8 The atomic number of the elements increases by one moving left to right along a period.

10. METALS NON- METALS We can divide the periodic table with a ‘staircase’ line to show elements that are metals and non-metals. As we move along a period from left to right we see a shift from metal to non-metal characteristics.

11. Numbered vertical columns of elements in the periodic table are called groups. 1234567012345670

12. Some groups are known by special names Alkali Metals Transition Metals Halogens Noble Gases 12345670

13. 13456702 Elements in the same group have similar chemical properties The alkali metals are all soft, very reactive metals. Li 3 Na 11 K 19 Rb 37 Cs 55 They all have one electron in their outer shell and show a gradual trend in both chemical and physical properties as we move down the group 1

14. 13456702 Elements in the same group have similar chemical properties The halogens are all very reactive non-metal elements. They all have seven electrons in their outer shell. The halogens are the only group to contain all three states of matter at room temperature. F 9 Cl 17 Br 35 I 53 At 85 7

15. 13456702 Elements in the same group have similar chemical properties The noble gases are all unreactive gaseous elements. He 2 Ne 10 Ar 18 Kr 36 Xe 54 They all have a full outer electron shell and are all odourless, colourless monatomic gases. Rn 86 0

16. MetalMelting Point KDensityRelative Strength Titanium900 Aluminium483 Iron (steel)531 Copper220

17.  Heat Alone – relatively unreactive metals can be obtained from their ores by simply heating to drive off the oxygen  Using a Reducing Agent e.g. Carbon Monoxide – for metals in the mid-range of the Reactivity Series-Carbon monoxide ‘grabs’ the oxygen from the metal forming carbon dioxide  Using Electrolysis of a melt – the Most reactive metals require high voltage electrical energy to separate them from their ores