For 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.
These more reactive forms are produced as powders. Cotton and Wilkinson's Advanced Inorganic Chemistry (third edition - page 316) suggests that the reactivity of one of these could be due to a very high surface area, or perhaps because the silicon exists in a graphite-like structure.
For phosphorus and sulphur, these have no reaction with water.
For, 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:
For argon, there is no reaction between argon and water.
Reactions with oxygen
For 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:
For magnesium, magnesium burns in oxygen with an intense white flame to give white solid magnesium oxide.
If magnesium is burned in air rather than in pure oxygen, it also reacts with the nitrogen in the air. Hence, a mixture of magnesium oxide and magnesium nitride will be formed.
For 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.
For silicon, silicon will burn in oxygen if heated strongly enough. Silicon dioxide is produced.
For 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:
For sulphur, sulphur burns in air or oxygen on gentle heating with a pale blue flame. It produces colourless sulphur dioxide gas.
Sulphur dioxide can be then converted further into sulphur trioxide in the presence of oxygen, but it needs the presence of a catalyst and fairly carefully controlled conditions.
For chlorine and argon, despite having several oxides, chlorine won't react directly with oxygen. Argon doesn't react either.
Reactions with chlorine
For sodium, sodium burns in chlorine with a bright orange flame. White solid sodium chloride is produced.
For magnesium, magnesium burns with its usual intense white flame to give white magnesium chloride.
For 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.
For 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.
For phosphorus, white phosphorus burns 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.
For sulphur, if a stream of chlorine is passed over some heated sulphur, it reacts to form an orange, evil-smelling liquid, disulphur dichloride, S2Cl2.
For chlorine and argon, it obviously doesn't make sense to talk about chlorine reacting with itself, and argon doesn't react with chlorine.
To conclude, as they belong to different groups, therefore, the form different products with water, oxygen and chlorine.