![]() ![]() ![]() Sulphur burns in Oxygen quite readily and produces a blue flame and gaseous Sulphur Dioxide which is an acidic gas.Ĭhlorine and Argon do not actually directly react with Oxygen despite the fact that Chlorine has several oxides. White Phosphorus (P 4) burns spontaneously in air with a white flame and releases white smoke containing Phosphorus(III) Oxide and Phosphorus(V) Oxide which are simple molecules, not giant structures like the previous products. Silicon is similarly unreactive, and only burns in Oxygen if heated strongly with a high concentration of Oxygen to form Silicon Dioxide. Magnesium also burns in Oxygen in much the same manner, with an intense white flame to form Magnesium Oxide, and thus continues the trend.Īluminium is far less reactive with Oxygen as the Al 2O 3 surface layer inhibits oxidation, however when powdered it is far more reactive and produces white sparks upon reaction with Aluminium(III) Oxide being formed. Sodium burn in Oxygen with an orange flame to form a white solid which is a mixture of Sodium Oxide and Sodium Peroxide. ![]() The overall trend is that reactivity with water decreases across Period 3 from left to right, with Chlorine being the slight exception.Īnother trend across Period 3 is each elements reaction with Oxygen to form an Oxide. Chloric(I) Acid and Hydrochloric Acid is formed from this reaction, however in the presence of Sunlight an alternate reaction occurs, which is a result of Chloric(I) Acid decomposition and Hydrochloric Acid and diatomic Oxygen is formed instead. Chlorine on the other hand does react with water, first by dissolving in it as Cl 2 to form a green solution where a reversible reaction takes place. However it is important to note that Phosphorus and Sulphur do not react with water directly, and neither does Argon which is a noble gas and thus has a stable electronic configuration, as its outermost electron shell filled to capacity with electrons meaning it does not tend to form chemical bonds. Silicon Dioxide and Hydrogen gas is formed by the reaction, which continues the trend with Aluminium and Magnesium (under higher temperatures) in regards to their reactions with water as an oxide is formed instead of a hydroxide, unlike Sodium. Silicon is very unreactive in its standard elemental form, it only reacts with water under high temperatures. Notice that an Oxide forms instead of a Hydroxide, which breaks the trend with Sodium, and is slightly similar the reaction between Magnesium and steam. However Magnesium reacts with steam to form insoluble Magnesium Oxide (an even stronger base) and Hydrogen gas.Īluminium also reacts with steam to form Aluminium(III) Oxide and Hydrogen gas, however the reaction is very slow due to the unreactive layer of Aluminium(III) Oxide which already exists on its surface, so the steam has to penetrate deeper to react. Sodium reacts vigorously with water in a very exothermic reaction to form a basic solution (a metal hydroxide) and bubbles of Hydrogen gas, Magnesium does much the same thing in cold water but slightly less vigorously due to the lower reactivity, which is a direct result of the greater nuclear charge holding valence electrons more strongly to the Magnesium atom, thus making it more difficult for them to be lost during a reaction. ![]() The first example of such trends concerns Sodium and Magnesium(s-block metals) and to a lesser extent Aluminium (p-block metal), and their reaction with water. They can be roughly divided into metals (Na, Mg and Al), metalloids (Si) and non-metals (P, S, Cl, and Ar), and the elements within these groups tend to have similar chemical properties and form similar compounds such as oxides, which in turn have similar reactions. Period 3 of the Periodic Table consists of the elements Sodium, Magnesium, Aluminium, Silicon, Phosphorus, Sulphur, Chlorine and Argon. ![]()
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