1. Chemistry Revision 3

2. Electronic configurations State which block in the periodic table you find the following elements: Sulphur Vanadium Strontium

3. Electronic configurations Sulphur = p Vanadium = d Strontium = s Write the full electronic configurations of the following elements (in terms of 1s 2 etc) Chlorine (17e), Cobalt (27e), Copper (29e)

4. Electronic configurations Chlorine 1s 2 2s 2 2p 6 3s 2 3p 5 Cobalt 1s 2 2s 2 2p 6 3s 2 3p 6 3d 7 4s 2 Copper 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 1 Note this is an exception along with CHROMIUM

5. Group 7 Chemistry Complete the following table HalogenColour at 298K State at 298K Fluorine Chlorine Bromine Iodine

6. More on group 7 What do I see if I add sodium bromide solution to a solution of silver nitrate? Write the IONIC equation for this reaction, including state symbols.

7. The answer- A cream precipitate would form on mixing the two colourless solutions. Ag + (aq) + Br - (aq)  AgBr (s) Remember that an ionic equation does not include spectator ions!!

8. Oxidation numbers Identify oxidation numbers in the following, and thus deduce whether it is oxidation or reduction or neither! StartEndOx? red? Br 2 KBr KMnO 4 Mn 2+ AgNO 3 AgI Fe 2+ Fe 3+ NH3NH3 NO2NO2

9. And the answers StartEnd Br 2 0KBrReduction KMnO 4 +7Mn 2+ +2Reduction AgNO 3 +1AgI+1Neither Fe 2+ +2Fe 3+ +3Oxidation NH 3 -3NO 2 +4Oxidation

10. Half equations Write the overall equation and the two half equations for the reactions occurring when chlorine water is added to potassium iodide solution Identify what has been reduced.

11. Half equations Cl 2 (aq) + 2I - (aq)  2Cl - (aq) + I 2 (aq) Reduced: Cl 2 (aq) + 2e -  2Cl - (aq) Oxidised: 2I - (aq)  2e - + I 2 (aq) Remember half equations do as they say- they show what is happening in half the equation!

12. Economic importance of Cl + Br Give 2 uses of chlorine or its compounds Give 2 uses of bromine or its compounds Remember you are expected to know the redox chemistry of the extraction of bromine from sea water.

13. Ionic Lattices Draw a labelled diagram to show the structure of an ionic lattice, as exemplified by sodium chloride

14. Solution calculations It takes 12.30cm3 of 0.05M NaOH to neutralise 25.00cm3 of HCl. 1) Write the balanced chemical equation 2) Work out the number of moles of NaOH used 3) Work out the concentration of HCl

15. Now try the exam q. More next week. Remember- I am here to help and support- BUT I can’t do the work for you. Are you “striving for the best of yourself always”??