1. + Reactions Noadswood Science, 2011

2. + Reactions To be able to describe how similar metals react with water and oxygen, and why noble gases do not react Sunday, August 16, 2015

3. + Reactivity What metals are reactive and which are not? Can you make a list of reactive metals? Why is sodium not used for cutlery? Why is magnesium not used for car bodies? Why can people wear gold? How are these metals produced?

4. + Reactivity Some metals are extremely reactive, whilst others are not – the reactivity series shows how reactive metals are… Potassium Sodium Calcium Magnesium Aluminium (Carbon) Zinc Iron Lead (Hydrogen) Copper Silver Gold Platinum

5. + Metal + Water Some metals do not react with water (such as gold and silver), but others do… Watch the demo of some more reactive metals being placed in water – the metal reacts with the water forming a metal hydroxide, and as it does it releases hydrogen (which can sometimes catch alight)!

6. + Metal + Water When a metal reacts with water the products are a metal hydroxide and hydrogen gas… Metal + Water  Metal Hydroxide + Hydrogen Write out the equations for the following (word and symbol) Sodium reacting with water Potassium reacting with water Lithium reacting with water

7. + Metal + Water Metal + Water  Metal Hydroxide + Hydrogen Sodium + Water  Sodium Hydroxide + Hydrogen 2Na (s) + 2H 2 O (l)  2NaOH (aq) + H 2 (g) Potassium+ Water  Potassium Hydroxide + Hydrogen 2K (s) + 2H 2 O (l)  2KOH (aq) + H 2 (g) Lithium + Water  Lithium Hydroxide + Hydrogen 2Li (s) + 2H 2 O (l)  2LiOH (aq) + H 2 (g)

8. + Metal + Oxygen Some metals do not react with water (such as gold and silver), but others do… Watch the videos of some metals reacting in oxygen…

9. + Reactivity Potassium Burning In Air

10. + Reactivity Sodium Burning In Oxygen

11. + Metal + Oxygen When a metal reacts with oxygen the product is a metal oxide Metal + Oxygen  Metal Oxide What is the word and symbol equation for the reaction between sodium and oxygen? + 

12. + Metal + Oxygen Metal + Oxygen  Metal Oxide Sodium + Oxygen  Sodium Oxide 4Na (s) + O 2 (g)  2Na 2 O (s) + 

13. + Reactivity Compare the reactivity series to where the elements are found within the periodic table – what relationship is there?

14. + Electron Structure & Reactivity There is a definite pattern between the placement of a metal on the periodic table and how reactive it is – the most reactive metals are located in groups I and II, with the least reactive metals being within the transition metals, placed in the centre of the periodic table, between groups II and III – they are generally hard and dense, and less reactive than the alkali metals

15. + Reactivity – Very Reactive The electron structure of an atom affects how reactive it is – a shell with just one electron in is it keen to ‘get rid’ of this so they have a full outer shell Elements within group I (lithium, sodium, potassium etc…) and group II (magnesium, calcium, strontium etc…) have just one or two electrons to ‘get rid of’ before they have a full outer shell, and as such are extremely reactive The most reactive metals are found within group I and II

16. + Reactivity – Not Reactive Electron structure of an atom affects how reactive it is – a shell with three of four electrons will find it very difficult to gain / loose enough electrons to have a full outer shell Elements within group III and group IV (including the transition metals such as zinc, silver and gold) have lots of electrons to gain / lose before they have a full outer shell, and as such as quite un-reactive This is why metals such as gold can be found as ‘pure’ – they are so un-reactive that they have not reacted with other chemicals for billions of years

17. + Reactivity In Groups As atoms get bigger they have more full shells of electrons – each new row has one more full shell The number of outer electrons is the same for each element within a group As you go do the group the outer shell of electrons is further from the nucleus – the inner shells provide shielding from the attraction of the +ve nucleus As metal atoms get bigger the outer electron is more easily lost – metals are more reactive as you descend down group I and group II