Question

16. (a) What is reactivity series of metals? What can you say about the reactivity of metals
which are placed:
(i) in the middle of reactivity series?
(ii) towards the bottom of reactivity series?
(iii) towards the top of reactivity series?
(b) A metal is placed in the middle of reactivity series. Suggest a chemical process to
obtain this metal from its oxide. Support your answer with one example,
metal is placed towards the top of the reactivity series. Suggest a chemical process to
obtain this metal from its oxide. Support your answer with one example,​

Answer 1

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(a) It is a series in which metals are arranged in order of their reactivity.

(i) Medium Reactive

(ii) In Bottom - They are least reactive metal.

(iii) Top - They are most reactive metal.

(b) Metal - Which is the middle of the reactive series.

Example- Zn

When we react ZnS with O2 this process is called roasting.

In this process ZnO obtained and SO2 Gas evolved.

2 ZnS + 3 O2 ----------> 2 ZuO + 2SO2

Now, When ZnO react with CO.

ZnS + CO -----------> Zu(s) + CO2(G)

(c) Sodium by Electrolysis process.

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Answer 2

Answer:

1 ) .Reactivity series :

It is series of decreasing order of metals' reactivity. Hydrogen is place in middle of series. Above hydrogen metals are more reactive in nature below are less. Metal which is more reactive it displaces a less reactive metal from its salt solution.

2 ) .

In order to obtaining a metal from its  oxides for metals in the middle of the reactivity series then metals towards oxides of such metals can be reduced with coke (carbon) which acts as a reducing agent.

For instance :

2 Fe₂O₃ + 3 C  ⇒ 4 Fe + 3 CO₂.

In order to obtaining a metal from its  oxides for metals in the high of the reactivity series their oxides are reduced to metals by the process of electrolysis

For instance :

Electrolysis of sodium chloride :

Na⁺ + e⁻  ⇒ Na   [ At cathode ]

2 Cl⁻ ⇒ Cl₂ + 2 e⁻   [ At anode ]