explain the following reactions: 1) reactivity of aluminum with steam.
2) reactivity of zinc with sodium hydroxide
3) reactivity of non metals with acids
4) electrolytic refining
5) reactivity of non metals with water.
Answers
Answer:
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Explanation:
is the correct answer
Answer:
1.)Like the reaction between magnesium and water, it is possible to react aluminium with steam. However, the aluminium oxide produced forms a barrier on the surface of the aluminium which prevents further reaction.
2.)Zinc react with excess sodium hydroxide to form sodium zincate(Na2ZnO2) along with hydrogen gas. Zinc is a transition metal which shows moderate reactivity. Zinc reacts with NaOH to form sodium zincate with the evolution of hydrogen gas.
3.)Non-metals do not react with acids. This is due to the fact that a substance undergoing reaction with acids, donates electrons to the H+ ions produced by the acids. But non-metals are acceptor of electrons and hence they do not donate electron to the hydrogen ion of the acid.
4.)electrolytic refining, the plates of crude metal are anodically dissolved in a suitable electrolyte, while “pure” metal is deposited on the adjacent cathodes. The electrorefining process was introduced about a hundred years ago to produce a substitute to fire-refined copper.
5.)They form stable compound with hydrogen. Their chlorides are completely hydrolyzed by water. Reaction of non-metals with oxygen: They react with oxygen to form acidic oxides or neutral oxides. Reaction of non-metals with water: They do not react with water (steam) to evolve hydrogen gas.