![]() ![]() ![]() Extension work based on the reactivity of metals practical Printable results tables are provided in the supporting resources booklet to save time in your practical lessons. This section of the video also looks at how to do a fair test. Caution learners against using the thermometer to agitate the metal in the acid as there is a risk of making a hole in the cup as well as damaging the thermometer. In the metal acid reactions observe the recommended concentration for the acid as there will not be a significant temperature rise at lower concentrations. TIP You may need to remove the metal in the copper(II) sulfate solution to see that it has a brown layer of solid on it – it will look black when in the blue solution. Consider demonstrating the copper(II) sulfate reactions on a larger scale, so learners can clearly see a change in the colour of solution – it may be harder to spot in the dimple tray. This minimises the amount of chemicals used. The displacement reactions are carried out in microscale using a spotting tile. These investigations may be spread over two or three lessons to make the content manageable. Exothermic reactions of metals and acid and metal displacement reactions are experiments that learners can carry out themselves. The first explores the reactions of the alkali metals in water and is a teacher demonstration. The video offers three experiments that investigate the relative reactivity of metals. Notes on running the practical experiments Plus technician notes and integrated instructions. Editable versions of all worksheets and key documents are provided.įull teacher notes are available in the supporting resources booklet, including ideas for how to use this video and the supporting resources as part of your teaching. Supporting resources booklet including pause-and-think questions with answers, teacher notes, intended outcomes, follow-up worksheets and structure strips. RSC Yusuf Hamied Inspirational Science Programme.Introductory maths for higher education.The physics of restoration and conservation.As both elements have undergone a change in their oxidation state, we can identify the reaction as a redox reaction. Chlorine has gained 1 electron to gain a -1 charge. After the reaction, sodium has lost 1 electron to gain a +1 charge. Much like balancing a reaction, we can tally the oxidation states of the reactants and products to see if there has been a change in oxidation state:īoth reactants start out with an oxidation state of 0 (i.e. In this process (known as smelting) iron (III) oxide is heated to a very high temperature (above 1200\degree \text One common example of this method is the the reduction of iron (III) oxide to produce pure iron. Reduction by carbon is a preferable method of extraction, as this is much less expensive than extraction using electrolysis. This is because metal oxides will not lose their oxygen when the metal is more reactive than carbon. Those lower in the reactivity series and so are less reactive will be reduced by reaction with carbon. Metals that come higher in the reactivity series and so are more reactive than carbon will be reduced using electrolysis. Which method is used will depend on the position of the metal in the reactivity series relative to that of carbon. This is typically done in one of two ways: To extract pure metals from their oxide ores, they must be reduced (i.e. ![]()
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