1. Chemical Properties

2. Syllabus Statements 3.3 Chemical properties 3.3.1 Discuss the similarities and differences in the chemical properties of elements in the same group. 3.3.2 Discuss the changes in nature, from ionic to covalent and from basic to acidic, of the oxides across period 3.

3. Trends across period 3 The elements we are talking about are: Sodium Na Magnesium Mg Aluminium Al Silicon Si Phosphorous P Sulfur S Chlorine Cl We ignore Argon because it doesn’t really have any chemistry!!

4. As we move across the period, we change from metals to non metals. Its actually a gradual change and is best illustrated by the way in which elements bond with oxygen. Sodium, magnesium and aluminium are metallic. (shiny, conductors etc.) They form oxides which contain ionic bonds and which have a giant ionic structure

6. The oxides of phosphorous, sulfur and chlorine contain covalent bonds. They are molecular covalent These elements are non-metals (don’t conduct)

8. Silicon is a metalloid From Wikipedia, the free encyclopedia A metalloid is a chemical element with properties that are in-between or a mixture of those of metals and nonmetals, and which is considered to be difficult to classify as either a metal or a nonmetal. There is no standard definition of a metalloid nor is there agreement as to which elements are appropriately classified as such. The six elements commonly recognized as metalloids are boron, silicon, germanium, arsenic, antimony and tellurium.

9. Silicon forms an oxide which has a giant covalent structure

10. There is also a trend from basic oxides to acidic oxides.

11. FormulaNa 2 OMgOAl 2 O 3 SiO 2 P2O5P2O5 SO 3 Cl 2 O 7 Type of bonding Ionic Highly polar covalent Polar covalent Acid/base character Basic AmphotericWeakly acidic Acidic acidic Other oxides Na 2 O 2 P2O3P2O3 SO 2 ClO 2 Cl 2 O Amphoteric – a substance which can react with both acids and bases

12. Basic oxides Sodium oxide will dissolve in water to give a basic solution which contains hydroxide ions Na 2 O + H 2 O  2Na + 2OH - Magnesium oxide is only slightly soluble, but will react with acid to make salt + water Write the equation for it reacting with Hydrochloric acid. Include state symbols MgO (s) + HCl (aq)  MgCl 2(aq) + H 2 O (l)

13. Amphoteric oxides Aluminium oxide is insoluble. It will react with (and hence dissolve in) both acids and alkalis Al 2 O 3 + 6H +  2Al 3+ + 3H 2 O Al 2 O 3 + 2OH - + 3H 2 O  2Al(OH) 4 -

15. Acidic Oxides Silicon oxide doesn’t really show much behaviour as an acid or a base, But it will slowly react with a hot, concentrated alkali (i.e. it shows slightly acidic properties) SiO 2 + 2OH -  SiO 3 2- + H 2 O

16. The remaining period 3 oxides react fully with water to give acidic solutions. P 4 O 10 + 6H 2 O  4H 3 PO 4 SO 3 + H 2 O  H 2 SO 4 Cl 2 O 7 + H 2 O  2HClO 4 Note that this is a dimer!

17. Syllabus Statements 3.3 Chemical properties 3.3.1 Discuss the similarities and differences in the chemical properties of elements in the same group. 3.3.2 Discuss the changes in nature, from ionic to covalent and from basic to acidic, of the oxides across period 3.