Don't lose sight of the overall trend in the period with respect to the highest oxides when you are looking at all this detail. Warning: The rest of this page contains quite a lot of detail about the various oxides. These reactions are all explored in detail on the rest of this page. They will, however, all react with bases such as sodium hydroxide to form salts such as sodium sulphate. The pattern isn't so simple if you include the other oxides as well.įor the non-metal oxides, their acidity is usually thought of in terms of the acidic solutions formed when they react with water - for example, sulphur trioxide reacting to give sulphuric acid. Those are the ones on the top row above, and are where the element is in its highest possible oxidation state. An amphoteric oxide is one which shows both acidic and basic properties.įor this simple trend, you have to be looking only at the highest oxides of the individual elements.
The trend is from strongly basic oxides on the left-hand side to strongly acidic ones on the right, via an amphoteric oxide (aluminium oxide) in the middle. The trend in acid-base behaviour is shown in various reactions, but as a simple summary:
Use the BACK button on your browser to return quickly to this page later if you choose to follow this link. Note: If you haven't already been there, you might be interested in looking at the page about the structures and physical properties of the Period 3 oxides as a useful introduction before you go any further. The oxides we'll be looking at are: Na 2O Argon is obviously omitted because it doesn't form an oxide. This page looks at the reactions of the oxides of Period 3 elements (sodium to chlorine) with water, and with acids or bases where relevant. From the results obtained, the writers believe that oxygen is a primary product of the reaction, while carbon dioxide is a secondary product, the carbon acting primarily as a catalyst.In experiments with tungstic oxide, also, oxygen was produced, but, contrary to the findings of other investigators, carbon dioxide was also formed.Acid-base behaviour of the period 3 oxidesĪCID-BASE BEHAVIOUR OF THE PERIOD 3 OXIDES In a number of experiments, less carbon was consumed than should have been for the amount of aluminium oxide that reacted, if it be assumed that carbon dioxide, rather than oxygen, was a primary product. The temperature at which reaction started, as shown by the formation of a sublimate of aluminium chloride in the reaction tube, decreased as the proportion of carbon to aluminium oxide increased. No carbon monoxide was obtained when a stream of chlorine was used, but small amounts were formed in a static atmosphere of chlorine. This occurred when a mixture of aluminium oxide and carbon was heated either in a stream of chlorine or in a static atmosphere of chlorine. The reaction aluminium oxide–carbon–chlorine has been investigated and found to produce aluminium chloride, oxygen and carbon dioxide.
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