describe the reactions of the Period 3 elements from sodium to argon with water, oxygen and chlorine

Reactions with water

Sodium

Sodium has a very exothermic reaction with cold water producing hydrogen and a colourless solution of sodium hydroxide.

Magnesium

Magnesium has a very slight reaction with cold water, but burns in steam.

A very clean coil of magnesium dropped into cold water eventually gets covered in small bubbles of hydrogen which float it to the surface. Magnesium hydroxide is formed as a very thin layer on the magnesium and this tends to stop the reaction.

Magnesium burns in steam with its typical white flame to produce white magnesium oxide and hydrogen

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Aluminium

Aluminium powder heated in steam produces hydrogen and aluminium oxide. The reaction is relatively slow because of the existing strong aluminium oxide layer on the metal, and the build-up of even more oxide during the reaction.

Silicon

There is a fair amount of disagreement in the books and on the web about what silicon does with water or steam. The truth seems to depend on the precise form of silicon you are using.

The common shiny grey lumps of silicon with a rather metal-like appearance are fairly unreactive. Most sources suggest that this form of silicon will react with steam at red heat to produce silicon dioxide and hydrogen.

But it is also possible to make much more reactive forms of silicon which will react with cold water to give the same products.

Phosphorus and sulphur

These have no reaction with water.

Chlorine

Chlorine dissolves in water to some extent to give a green solution. A reversible reaction takes place to produce a mixture of hydrochloric acid and chloric(I) acid (hypochlorous acid).

In the presence of sunlight, the chloric(I) acid slowly decomposes to produce more hydrochloric acid, releasing oxygen gas, and you may come across an equation showing the overall change: Argon There is no reaction between argon and water. Reactions with oxygen Sodium Sodium burns in oxygen with an orange flame to produce a white solid mixture of  sodium oxide and sodium peroxide. For the simple oxide: For the peroxide: Magnesium Magnesium burns in oxygen with an intense white flame to give white solid magnesium oxide.

In the presence of sunlight, the chloric(I) acid slowly decomposes to produce more hydrochloric acid, releasing oxygen gas, and you may come across an equation showing the overall change: Argon There is no reaction between argon and water. Reactions with oxygen Sodium Sodium burns in oxygen with an orange flame to produce a white solid mixture of sodium oxide and sodium peroxide. For the simple oxide: For the peroxide: Magnesium Magnesium burns in oxygen with an intense white flame to give white solid magnesium oxide.

Aluminium

Aluminium will burn in oxygen if it is powdered, otherwise the strong oxide layer on the aluminium tends to inhibit the reaction. If you sprinkle aluminium powder into a Bunsen flame, you get white sparkles. White aluminium oxide is formed.

Silicon

Silicon will burn in oxygen if heated strongly enough. Silicon dioxide is produced.

 

Phosphorus

White phosphorus catches fire spontaneously in air, burning with a white flame and producing clouds of white smoke - a mixture of phosphorus(III) oxide and phosphorus(V) oxide.

The proportions of these depend on the amount of oxygen available. In an excess of oxygen, the product will be almost entirely phosphorus(V) oxide.

For the phosphorus(III) oxide:

For the phosphorus(V) oxide:

Sulphur Sulphur burns in air or oxygen on gentle heating with a pale blue flame. It produces colourless sulphur dioxide gas.
Chlorine and argon Despite having several oxides, chlorine won't react directly with oxygen. Argon doesn't react either. Reactions with chlorine Sodium Sodium burns in chlorine with a bright orange flame. White solid sodium chloride is produced. Magnesium Magnesium burns with its usual intense white flame to give white magnesium chloride. Aluminium Aluminium is often reacted with chlorine by passing dry chlorine over aluminium foil  heated in a long tube. The aluminium burns in the stream of chlorine to produce very  pale yellow aluminium chloride.  This sublimes (turns straight from solid to vapour and back again) and collects further  down the tube where it is cooler. Silicon If chlorine is passed over silicon powder heated in a tube, it reacts to produce  silicon tetrachloride. This is a colourless liquid which vaporises and can be condensed  further along the apparatus. Phosphorus White phosphorus burns spontaneously in chlorine to produce a mixture of two  chlorides, phosphorus(III) chloride and phosphorus(V) chloride (phosphorus trichloride  and phosphorus pentachloride). Phosphorus(III) chloride is a colourless fuming liquid. Phosphorus(V) chloride is an off-white (going towards yellow) solid.		Sulphur If a stream of chlorine is passed over some heated sulphur, it reacts to form an orange, evil-smelling liquid, disulphur dichloride, S2Cl2.	Note:  Sulphur dioxide can, of course, be converted further into sulphur trioxide in the presence of oxygen, but it needs the presence of a catalyst and fairly carefully controlled conditions. If you are interested in this, see the page on the Contact Process. This isn't particularly relevant to the current topic, but if you do feel the urge to follow this link, use the BACK button on your browser to return to this page.