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प्रश्न
Explain the reactions of nonmetals with water with the help of examples.
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उत्तर
Generally, nonmetals do not react with water, except halogens.
E.g. Chlorine on dissolving in water gives the following reaction:
\[\ce{\underset{\text{Chlorine}}{Cl_{2(g)}} + \underset{\text{Water}}{H2O_{(l)}} -> \underset{\text{acid}}{\underset{\text{Hypochlorous}}{HOCl_{(aq)}}} + \underset{\text{acid}}{\underset{\text{Hydrochloric}}{HCl_{(aq)}}}}\]
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संबंधित प्रश्न
Name one metal which is extracted by:
Electrolytic reduction.
Bronze is an alloy of copper and ______.
How is manganese extracted from manganese dioxide, MnO2? Explain with the help of an equation.
Name the gas produced when calamine ore is calcined.
Explain how, mercury is extracted from its sulphide ore (cinnabar). Give equations of the reactions involved.
Zinc blende ore can be converted into zinc oxide by the process of ______.
An element has its electron configuration as 2,8,8,2. Now answer the following questions.
a) What is the atomic number of this element?
b) What is the group of this element?
c) To which period does this element belong?
Which method of refining is used to get 99.8% pure aluminium?
Name a non- metal that has a metallic luster and sublimes on heating.
Define calcination.
Gold and silver are active metals.
Explain concept with example/explain with the help of a balanced equation.
Calcination
Explain in brief types of extraction of highly reactive metals according to their reactivity.
Which of the statements about the reaction, \[\ce{ZnO + CO -> Zn + CO2}\] is correct?
Which of the following metals exist in their native state in nature?
- Cu
- Au
- Zn
- Ag
- Given below are the steps for extraction of copper from its ore. Write the reaction involved.
- Roasting of copper (I) sulphide
- Reduction of copper (I) oxide with copper (I) sulphide.
- Electrolytic refining
- Draw a neat and well labelled diagram for electrolytic refining of copper
On the basis of reactivity metals are grouped into three categories:
- Metals of low reactivity
- Metals of medium reactivity
- Metals of high reactivity
Therefore metals are extracted in pure form from their ores on the basis of their chemical properties.
Metals of high reactivity are extracted from their ores by electrolysis of the molten ore.
Metals of low reactivity are extracted from their sulphide ores, which are converted into their oxides. The oxides of these metals are reduced to metals by simple heating.
(a) Name the process of reduction used for a metal that gives vigorous reaction with air and water both.
(b) Carbon cannot be used as a reducing agent to obtain aluminium from its oxide? Why?
(c) Describe briefly the method to obtain mercury from cinnabar. Write the chemical equation for the reactions involved in the process.
OR
(c) Differentiate between roasting and calcination giving chemical equation for each.
The given reaction shows one of the processes to extract the metals like Iron and Manganese.
\[\ce{MnO2(s) + Al(s) -> Mn(l) + Al2O3(s) + Heat}\]
Give a reason why Aluminium is preferably used in thermite reactions.
A mineral from which the metal can be extracted economically and conveniently is known as ______.
