1. Write a 3 mark definition for the first ionisation energy.

2. The Periodic Table 1) Explain the changes in ionisation energy of elements across each period, and down each group (refer to nuclear charge, atomic radius and electron shielding). 2) Describe and explain the variations in melting and boiling points across periods 2 and 3 in terms of structure and bonding. 3) Be able to interpret data on electron configuration, atomic radii, first ionisation energies, m.p. and b.p. to describe periodicity

3. History (learn the details) 1) In the 1800s, scientists grouped the elements by mass. 2) John Newlands (1863) came up with the law of octaves (putting elements in rows of 8) 3) Mendeleev designed the current periodic table, and left gaps. Ordered by atomic number and properties (based on valance electrons)

4. Periodic Table Which are the s-block, p-block and d-block elements?

5. Why the different name blocks? S-Block Na – 1s 2 2s 1 P-Block Chlorine - 1s 2 2s 2 2p 6 3s 2 3p 5 D-block Titanium – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2

7. Atomic Radius – down a group?

8. In periodic table answers, mention: 1)Nuclear charge – number of protons 1)Electron shielding – more complete inner shells, more of the positive nuclear charge is shielded 2)Atomic radius – size of the atom

9. Your turn 1) Explain the trend in first ionisation energies for period 2 and 3. 2) Explain the trend down group 1. 3) Describe the patterns for melting and boiling points across period 2 and 3 (you will need to talk about different bonding)

11. The Periodic Table 1) Explain the changes in ionisation energy of elements across each period, and down each group (refer to nuclear charge, atomic radius and electron shielding). 2) Describe and explain the variations in melting and boiling points across periods 2 and 3 in terms of structure and bonding. 3) Be able to interpret data on electron configuration, atomic radii, first ionisation energies, m.p. and b.p. to describe periodicity