Leaving Out the d-block

Size Matters Which is the bigger out of the following pairs of atoms: 1.N or P 2.Se or Br 3.Na or Cl

Melting and boiling of Periods Elements Remember the recent flow chart?? What are we overcoming when we boil (or melt) each of the following elements?: Li, Be, B (giant), C, N, O, F, Ne Na, Mg, Al, Si (giant), P, S, Cl, Ar Which of the above should have very high boiling points? which should have very low boiling points?

Give the biggest atom in period 2 Which is the biggest out of: Al, Ga, Br Which will conduct electricity Which will have the lowest melting point and what are we overcoming? Which will form positive ions most readily?

Giant Covalent Breaking Covalent bonds Very high B.Pt. Metallic Overcoming metallic ‘bonds’ Quite to very high B.Pt. Simple Molecular Element Overcoming Van der Waals forces only Low B.Pt. Giant Covalent Breaking Covalent bonds Very high B.Pt. Metallic Overcoming metallic ‘bonds’ Quite to very high B.Pt. Simple Molecular Element Overcoming Van der Waals forces only Low B.Pt.

Giant Covalent Breaking Covalent bonds Very high B.Pt. Metallic Overcoming metallic ‘bonds’ Quite to very high B.Pt. Simple Molecular Element Overcoming Van der Waals forces only Low B.Pt. Giant Covalent Breaking Covalent bonds Very high B.Pt. Metallic Overcoming metallic ‘bonds’ Quite to very high B.Pt. Simple Molecular Element Overcoming Van der Waals forces only Low B.Pt.

More Predictions! Strength of metallic bonding: the greater the charge on the ions the stronger the bonding. Van der Waals forces: the more electrons in total in the molecule the stronger these forces are. They will still be pretty weak overall though. Arrange the metals within each period into order of bpt. Arrange the molecules within each period into order of b.pt. Note N 2 O 2 and F 2 have very similar numbers of electrons so the VDW forces will be approx equal. Sketch your predicted graph of Bpt. across Pd 3 Sketch your predicted graph of Bpt. across Pd 2

NaMgAlSiP 4 S 8 Cl 2 Ar

Could you fully explain this graph?

LiBeBCN 2 O 2 F 2 Ne

Could you fully explain this graph?

Just shown to help spot the periodic trends

Ionisation Energies – Across a Period These can be affected by: Atomic Size Shielding Nuclear Charge Which of the above change across a period from left to right? What do you predict will be the trend in 1 st IE across any given period?

Ionisation Energies – Down a Group These can be affected by: Atomic Size Shielding Nuclear Charge How will each of the above change down a group from top to bottom? What do you predict will be the trend in 1 st IE down any given group?

Give the symbols of the following element with the: Highest 1 st IE from group 2 Lowest 1 st IE from period 3 Lowest 1 st IE (from the first 6 periods) Highest 1 st IE (from the first 6 periods) Link to all elements in order of 1 st IELink

Using the Text Book… Pages are really just background and you don’t need to learn this for the exam. Maybe read it at some point though?? Pages are very relevant, you should work through these. –Add to your notes, learn definitions and tackle all the questions. As always check your answers in the back and try incorrect ones again at a later date. –Page 97 Q1,2,3, Pages 98,99 Q1,2,3,