Pure oxygen is a strong oxidizer. Magnesium is group 2, iron is group 8 and copper is group 11. This demo takes about three minutes to perform. There are a number of other ways to stop or slow down rust. Copper did not burn in air. They have been covered with a layer of chromium to protect the iron surface from contact with the air. Remove the hose and stopper the flask tightly. One way to protect the iron surface is to cover it with a metal that does not corrode, like chromium, for instance. Several repre-sentative reaction runs at a constant partial pressure of oxygen and at various pH values are plotted in Figure 1. Any two of the following: BeO, MgO, CaO, SeO, BaO. However, iron and rust (iron oxide) are completely different materials and therefore have different properties. Students can examine the reaction product afterwards to formulate their observations. You can then compare this reaction with the one that you did previously where iron was burned in oxygen in a combustion reaction. They had to be lit by hand and burned very brightly, for a very short period. A) Less reaction will take place. Lastly, give two examples of metals that you learnt about in this chapter which do not rust. Iron does not clearly alter in pure water or in dry air, but when both water and oxygen are present (moist air), iron corrodes. Tools, locks, hinges, screws and nails, garage doors... the list of items is almost endless! Bangladesh. This means that a metallic oxide is formed. This is a very versatile demonstration. Rusting is the common term for corrosion of iron and its alloys, such as steel. Can you see the oxygen that the metal will react with? Safety precautions to observe during the demonstrations: Steel wool is an alloy made mostly of iron. What do you observe during the reaction? The products are all metal oxides. You should make careful observations during the demonstration and write these down in the spaces provided below. For example, steel and cast-iron are made of iron. Carefully sprinkle a spatula of iron filings around the sides of the test tube. In this chapter we learnt how metal oxides form. The iron reacts with water and oxygen to form hydrated iron (III) oxide, which we see as rust. Use a clamp attached to a retort stand to hold the test tube in place. Look at the metal before it is burned. The iron is gradually 'eaten away' as it reacts slowly with the oxygen. Make sure that there is plenty of sand in the bottom of the Erlenmeyer flask. Calculate the mass of ferric oxide produced in this reaction. We can write a general word equation for reactions in which a metal reacts with oxygen: When we use words to describe a reaction, we are still operating on the macroscopic level. The iron will continue to corrode even if it has a thick layer of rust covering it. In air it smolders and burns with no flame. If we wanted to prevent the iron atoms and oxygen molecules from making contact, we would need to place a barrier between them. The oxide layer do not passivate the surface. Steel contains less than 2.14% carbon, and cast-iron not more than 7% carbon. All rights reserved. nH 2 O) and iron(III) oxide-hydroxide (FeO(OH), Fe(OH) 3), and is typically associated with the corrosion of refined iron.. Is there something present that is aiding or speeding up the reaction? Write the missing word on the line below. What do we call reactions where a substance burns in air? The purpose of these demonstrations is to give you a chance to make macroscopic observations of the chemical changes that take place during the reactions. What is rusting? You can see a video of steel wool burning here: Your teacher will perform a demonstration in which iron is burned in air. Rust is a different compound to the element iron and so it has different properties. 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