Starter Activity

1. Starter Activity • State the 3 main properties of metals. • Explain in terms of metallic structure how these properties arise.

2. Structures of Ionic and Covalent Compounds • Describe and explain the physical properties of a giant ionic lattice. • Describe and explain the physical properties of simple covalent and giant covalent lattices.

3. IONIC COVALENT eg sodium chloride (salt) PURE substances have different STRUCTURES depending on the type of BONDING they have METALLIC eg copper SIMPLE MOLECULAR eg carbon dioxide, water GIANT MOLECULAR eg diamond, graphite The structure of a substance influences what its PHYSICAL PROPERTIES will be.

4. Ionic Compounds Positive sodium ion Na+ Negative chloride ion Cl- Ionic substances are compounds of metals and non-metals (eg sodium chloride, copper oxide, magnesium sulphide etc) They are made of IONS: atoms which have lost or gained electrons giving them a positive or negative CHARGE The + ions and – ions STRONGLY ATTRACT each other to make a regular crystal structure

5. Strong ionic bond Because of the very STRONG BONDS between the IONS, ionic compounds have high melting & boiling points. All ionic compounds are solids at room temperature. Sodium chloride melts at over 800°C

6. The greater the charge the stronger the electrostatic forces between ions. Therefore more energy is needed to break up the lattice.

7. H2O MELT DISSOLVE - - - - - - - - - - - - - - - - - - + + + + + + + + + + + + + + + + + + + As ionic compounds are made of CHARGED IONS, they can conduct electricity but ONLY if the ions can MOVE. If it is MOLTEN the ions can move If it is DISSOLVED the ions can move 800°C 20°C

8. - - - - - - - + + + + + + + + MOLTEN IONIC COMPOUND MOLTEN ionic compounds CONDUCT ELECTRICITY

9. H20 molecule Ions free to move around When salt is put in water, H2O molecules pull the ions apart to make a solution. This lets the ions move around.

10. PURE WATER SOLID SALT SALT SOLUTION DISSOLVED ionic compounds also CONDUCT ELECTRICITY

11. H20 molecule Ions free to move around When salt is put in water, H2O molecules pull the ions apart to make a solution. This lets the ions move around.

12. Solubility Ionic lattices can dissolve in polar solvents, such as water. Polar molecules break down the lattice by surrounding each ion to form a solution. • When NaCl dissolved in water the giant ionic lattice breaks down. • Water molecules attract the Na+ and Cl- ions. • The ionic lattice breaks down as it dissolves. Water molecules surround the ions • Na+ attracts the δ- on the O in the water molecules • Cl- attracts the δ+ on the H in the water molecules

13. Questions Why do ionic compounds have high melting and boiling points? Explain the different electrical conductivities of an ionic compound in different states. Explain why water is a good solvent for ionic compounds

14. H atom O atom Whole thing = H2O molecule SIMPLE MOLECULAR SUBSTANCES These are substances like carbon dioxide CO2, water H2O and methane CH4 which are always made of simple molecules whether they are SOLIDS, LIQUIDS OR GASES

15. MOLECULES ONLY WEAKLY ATTRACT EACH OTHER VERY STRONG bonds BETWEEN ATOMS (so molecule is very hard to break up) WEAK bonds BETWEEN MOLECULES (so molecules are easy to separate)

16. LIQUID SOLID GAS Simple molecular substances can only be a liquid or a solid when the temperature is LOW enough for the WEAK BONDS to pull the molecules together

17. This means simple molecular substances have LOW melting and boiling points Liquid oxygen boiling at -183°C Solid oxygen at -240°C

18. As the bonds between the molecules are weak, simple molecular substances are weak and soft when solid. As the molecules are NOT CHARGED simple molecular substances DON’T CONDUCT ELECTRICITY when solids, liquids or gases.

19. Solubility – simple molecular structures are soluble in non-polar solvents, such as hexane. Because van der Waals’ forces form between the solvent and the molecule. The formation of the van der Waals’ forces weakens the lattice structure.

20. Carbon atom Only STRONG bonds GIANT MOLECULAR SUBSTANCES In these materials strong covalent bonds join atoms together with other atoms of the same type to make giant structures, rather than little groups. Every C atom joined to 4 others DIAMOND (this is only part of the structure - the same pattern carries on in every direction)

21. SILICA (Silicon dioxide SiO2) has a similar structure to diamond Every Si atom joined to 4 O atoms Silica is the main substance in ROCKS. Pure silica is called QUARTZ

22. Because all the atoms in Giant Structures are joined by STRONG BONDS they: • Have HIGH melting / boiling points • Are usually HARD and STRONG Because all the atoms in Giant Structures are UNCHARGED, they will not conduct electricity.

23. GRAPHITE – a special case WEAK BONDS STRONG BONDS Common form of carbon found in soot, charcoal, pencil leads etc Carbon atoms each joined to 3 others with STRONG bonds to make hexagonal sheets of atoms The sheets of atoms are joined to other sheets by WEAK bonds

24. As the bonds between the layers of atoms are weak, they can easily slide over each other As the C atoms are only bonded to 3 others, the extra electrons form clouds of ‘free electrons’ between the layers

25. GRAPHITE - Properties The STRONG BONDS between the ATOMS mean it has HIGH MELTING and BOILING POINTS The WEAK BONDS between the LAYERS mean it is SOFT and SLIPPERY as the layers SLIDE over each other easily (used in pencils and as a solid lubricant) The FREE ELECTRONS between the layers mean that graphite CONDUCTS ELECTRICITY (used as sliding contacts in electric motors)

26. Solubility – Giant covalent structures are not soluble in both polar and non-polar solvents. Because the covalent bonds in the lattice are too strong to be broken by either polar or non-polar solvents.

27. SUMMARY - Descriptions METALLIC Strong malleable solids Don’t dissolve eg copper IONS ONLY IONIC Crystals Dissolve in water eg sodium chloride (salt) IONS + FREE ELECTRONS SIMPLE MOLECULAR Usually Gases eg CO2, H2O ATOMS joined into GIANT MOLECULES GIANT MOLECULAR Hard strong solids Don’t dissolve eg diamond (graphite – special case) MOLECULES ONLY

28. Write a summary of the physical properties of different structures with reasons.

29. SUMMARY - PROPERTIES

30. Questions • For each of the following substances • NaCl ii) SiO2 (sand) iii) Br2 iv) C2H5OH • Predict the; • structure b) melting point • c)electrical conductivity d) solubility • 2. Explain the different properties of diamond and graphite in terms of their structure.