1. Complete spot the bonding worksheet Work in pairs/small groups Write answers on paper or whiteboards (not the sheet)

2. Structure and bonding review
Sunday, 16 April 2017

3. Specification links Metallic bonding
(p) describe, metallic bonding as the attraction of positive ions to delocalised electrons;
Bonding and Physical Properties
(q) describe structures as:
(i) giant ionic lattices, with strong ionic bonding ,i.e., as in NaCl,
(ii) giant covalent lattices, i.e., as in diamond and graphite,
(iii) giant metallic lattices,
(iv) simple molecular lattices, i.e., as in I2 and ice;
(r) describe, interpret and/or predict physical properties, including melting and boiling points, electrical conductivity and solubility in terms of:
(i) different structures of particles (atoms, molecules, ions and electrons) and the forces between them,
(ii) different types of bonding (ionic bonding, covalent bonding, metallic bonding, hydrogen bonding, other intermolecular interactions);
(s) deduce the type of structure and bonding present from given information.

4. Investigation What did we find out during the investigation?
Can you deduce the bonding in each substance?
Can you justify your answers?
Can you explain your observations/results in terms of the structure and bonding present in each substance

5. Results and conclusions
Substance
Test 1
Test 2
Test 3
Test 4 A
does not melt therefore high melting point
dissolves
conducts electricity B
melts readily therefore low melting point
does not dissolve C D
Does not dissolve
Conducts electricity

6. 6 marks
Could have been used in previous lessons

7. 6 marks

8. Exam question Compare and explain the electrical conductivities of sodium and sodium oxide in the solid and liquid states. [5 marks]

9. 3 marks

10. 5 marks

11. Specification links Electronegativity and Bond Polarity
(k) describe the term electronegativity as the ability of an atom to attract the bonding electrons in a covalent bond;
(l) explain that a permanent dipole polarity may arise when covalently-bonded atoms have different electronegativities, resulting in a polar bond;

12. Specification links Intermolecular Forces
(m) describe intermolecular forces based on permanent dipoles, as in hydrogen chloride, and instantaneous dipoles (van der Waals’ forces), as in the noble gases;
(n) describe hydrogen bonding, including the role of a lone pair, between molecules containing –OH and –NH groups, i.e. as in H2O, NH3 and analogous molecules;
(o) describe and explain the anomalous properties of water resulting from hydrogen bonding, e.g.:
(i) the density of ice compared with water,
(ii) its relatively high freezing point and boiling point;

13. 4 marks

14. Could have been used in previous lessons

19. Van der Waals’ exam questions Chlorine, bromine and iodine are halogens commonly used in school and college experiments. Describe how van der Waals’ forces arise (3 marks)
Could have been uesd in previous lessons

21. Exam question
(3 marks)

23. Exam questions
State and explain the trend in the boiling points of chlorine, bromine and iodine.
(3 marks)
b) The halogen astatine does not exist in large enough quantities to observe any of its reactions.
Why would astatine be expected to react similarly to other halogens?
(1 mark)

24. a)