Arrange the following metals in the order in which they displace each other from the solution of their salts.
Al, Cu, Fe, Mg and Zn.
Al, Cu, Fe, Mg and Zn.
Solution and Explanation
A metal of stronger reducing power displaces another metal of weaker reducing power from its solution of salt.
The order of the increasing reducing power of the given metals is
\(Cu < Fe < Zn < Al < Mg\).
Hence, we can say that Mg can displace \(Al\) from its salt solution, but Al cannot displace \(Mg\).
Thus, the order in which the given metals displace each other from the solution of their salts is given below:
\(Mg>Al> Zn> Fe>Cu\)
Top Questions on Redox Reactions In Terms Of Electron Transfer Reactions
- Number of electrons exchanged during the following reaction are/is
2Fe3+(aq) + 2I-(aq) → 2Fe2+(aq) + I2(s)- CUET (UG) - 2023
- Chemistry
- Redox Reactions In Terms Of Electron Transfer Reactions
- Why does the following reaction occur?
\(XeO_6^{4-}(aq) + 2F^ - (aq) + 6H^ + (aq) \rightarrow XeO_3(g) + F_2(g) + 3H_2O(l)\) What conclusion about the compound \(Na_4XeO_6\)(of which \(XeO_6^{4-}\) is a part) can be drawn from the reaction.- CBSE Class XI
- Chemistry
- Redox Reactions In Terms Of Electron Transfer Reactions
- Calculate the oxidation number of Sulphur, chromium, and nitrogen in
\(H_2SO_5\), \(Cr_2O_7^{2−}\) and \(NO_3^−\). Suggest structure of these compounds. Count for the fallacy.- CBSE Class XI
- Chemistry
- Redox Reactions In Terms Of Electron Transfer Reactions
- The Mn3+ ion is unstable in solution and undergoes disproportionation to give Mn2+ , MnO2, and H+ ion. Write a balanced ionic equation for the reaction.
- CBSE Class XI
- Chemistry
- Redox Reactions In Terms Of Electron Transfer Reactions
- Consider the reactions:
- H3PO2(aq) + 4 AgNO3(aq) + 2 H2O(l) \(\rightarrow\) H3PO4(aq) + 4Ag(s) + 4HNO3(aq)
- H3PO2(aq) + 2CuSO4(aq) + 2 H2O(l) \(\rightarrow\) H3PO4(aq) + 2Cu(s) + H2SO4(aq)
- C6H5CHO(l) + 2[Ag (NH3)2]+(aq) + 3OH- (aq) \(\rightarrow\) C6H5COO- (aq) + 2Ag(s) + 4NH3(aq) + 2 H2O(l)
- C6H5CHO(l) + 2Cu2+(aq) + 5OH-(aq) \(\rightarrow\) No change observed.
What inference do you draw about the behaviour of Ag+ and Cu2+ from these reactions?
- CBSE Class XI
- Chemistry
- Redox Reactions In Terms Of Electron Transfer Reactions
Questions Asked in CBSE Class XI exam
- Find the sum to indicated number of terms in each of the geometric progressions in 1, – a, \(a^2\), –\(a^3\), ... n terms (if a ≠ – 1).
- CBSE Class XI
- geometric progression
- Find n if n-1P3: nP3 = 1: 9.
- CBSE Class XI
- Permutations
- Give a brief description of the principles of the following techniques taking an example in each case.(a) Crystallisation (b) Distillation (c) Chromatography.
- CBSE Class XI
- Organic Chemistry- Some Basic Principles and Techniques
- Three reasons why the author’s grandmother was disturbed when he started going to the city school.
- CBSE Class XI
- The Portrait of a lady
- Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in \(C_2H_4\) and \(C_2H_2\) molecules.
- CBSE Class XI
- Bond Parameters
Concepts Used:
Redox Reactions
Redox Reaction:
Redox reactions are chemical reactions where oxidation and reduction take place simultaneously. In this type of reaction, there is a gain of electrons for one chemical species while the other loses electrons or simply involves transfer of electrons. The species that loses electrons is oxidized while the one that gains electrons is reduced.
Types of Redox Reactions:
Redox reactions can be differentiated into 4 categories namely combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions. Each is explained separately below:
Combination Reaction:
In this, the molecules combine to form new compounds. For example, when magnesium reacts to nitrogen.
Decomposition Reaction:
Opposite to the combination reaction, here there is a breakdown of compounds to simpler substances. For example, electrolysis of water.
Displacement Reaction:
In this, the more reactive metal will displace the less reactive one in a chemical reaction. The reactivity of an element is represented in a series called the reactivity series (arranged in decreasing order of reactivity) which makes it easier to determine the chemical reaction and its products.
Disproportionation Reaction:
This is a peculiar type of reaction where an element showing a particular oxidation state will be oxidized and reduced simultaneously. Another thing to note is that these reactions will always have an element that can exhibit three oxidation states.