Some important types of redox reactions are being described as follows:
1. Combination Reactions
These are reactions in which two species (atoms or molecule) combine to form a single species. A combination reactions may be denoted in the manner:
A + B – C
For the above reaction to be a redox reaction. Either A or B or both A and B must be in the elemental form. Some important examples of this category are:
2. Decomposition Reactions
Decomposition reactions are just the reverse of combination reactions. A decomposition reaction involves the breakdown of a compound into two or more components at least one of which must be in the elemental state. Some example of this class of the reactions are:
3. Combustion Reactions
Combustion reaction is special category of combination reaction in which one of the element is oxygen. Some examples are:
4. Displacement Reactions
In these reactions, an atom or ion in a compound is replaced by an atom or ion of some other element. In general, it is represented by the equation,
X + YZ à XZ + Y
Here, from the compound YZ, the atom Y has been displaced by another atom X.
Types of displacement reactions. Displacement reactions are of the following two types:
(a) Metal-displacement reactions
(b) Non-metal displacement reactions
(a) Metal displacement reactions. In these reactions, a metal in the compound is displaced by some other metal in the elemental state. For example,
Here, the metal causing displacement is a better reducing agent than the metal undergoing displacement.
(b) Non-metal displacement reactions. In these reactions, a metal or a non-metal displaces another non-metal from its compound. In most of these reactions, the non-metal getting displaced is hydrogen. However, there are some reactions which involve the displacement of oxygen or halogens. Let us study some reactions in which hydrogen is being displaced. Depending upon the capability of the reducing metal or non-metal, the following cases arise:
(i) All alkali metals and some alkaline earth metals ( Ca, Sr and Ba) which are very good reducing agents displace hydrogen from cold water.
(ii) Less active metals such as magnesium and iron react with steam to produce hydrogen gas:
(iii) Many metals, including those which do not react with cold water, are capable of displacing hydrogen from acids. For example
Metals like cadmium and tin which do not react with steam also react with acids to displace dihydrogen gas.
(iv) Very less reactive metals such as silver (Ag) and gold (Au) which may occur in the native state do not react even with dilute hydrochloric acid.
Reactivity of Metals
From the above discussion, it follows that the rate of evolution of~ by metals from water and aqueous acids can be used to determine the order of reactivity of metals. For example, sodium (Na) reacts with water at the fastest rate, magnesium (Mg) reacts slowly, iron (Fe) reacts at the slowest rate while silver (Ag) and gold (Au) do not react at all.
The reactivity of metals is given in the form of activity series in Table 30.1.
Reactivity of Non. Metals
Like metals, activity series also exists for non-metals. Since non-metals have a tendency to accept electrons, therefore, this reactivity depends upon their oxidising power. For example, among halogens the oxidising power decreases as we move down the group 17 from fluorine to iodine. Thus, fluorine (F2) is the strongest oxidising agent. It displaces Cl2, Br2 and I2 from the solution of chloride, bromide and iodide ions respectively. In fact, F2 is so reactive that it even displaces oxygen from water.
On the other hand, chlorine can displace bromine from bromide ions and iodine from iodide ions.
Their corresponding ionic equations are:
Similarly, bromine can displace iodine from iodide ions
It may be noted that halogens can also be displaced by oxidation of their corresponding halide ions using suitable chemical oxidising agents.
Although a number of oxidising agents such as KMnO4 , JSCr2O 7, MnO2, etc., are available to oxidise CI-, Br-and lions to form Cl2, Br2 and I2 respectively, no oxidising agent is available to oxidise p-ions to F2 because F2 itself is the strongest oxidising agent. Therefore, the only way to prepare F2 is to oxidise F- ions electrolytically.
5. Disproportionation Reactions
A reaction in which the same species is simultaneously oxidised as well as reduced is called a disproportionation reaction. For such redox reactions to occur, the reacting species must contain an element which has atleast three oxidation states. The element in the reacting species is present in the intermediate oxidation state while the higher and lower oxidations states are available for reduction and oxidation to occur.
Some example, of disproportionation reactions are:
Reactivity of Halogens
Halogens are very good oxidising agents due to their tendency to gain electrons.
X2 + 2e – à 2X –
As discussed earlier in section 30.5, that the reactivity of halogens as oxidising agents decreases as Cl2> Br2 > I2
• Cl2 can oxidise Br as well as I- ions
Cl2(aq) + 2Br – (aq) à Br2 (aq) + 2 Cl
Cl2(aq) + 2l – (aq) à I2 (aq) + 2 Cl
• Br2 can oxidise only I- ions but not CI- ions
Br2(aq) + I –(aq) à I2 (aq) + 2Br –
Br2(aq) + CI –(aq) àNo reaction
Fill in the blanks
1. The reaction CaCO3 CaO + CO2 is a ........... reaction.
2. The reaction in which oxygen in added to the substance is called ............. reaction
3. Reaction in which hydrogen is added to a substance is called ............. reaction.
4. The process of loss of an electron in known as ............. and the process of gain of an electron is known as .............
5. The species undergoing oxidation acts as a ............. agent.
6. The reducing agent undergoes ............. of electrons.
7. Formation of Nitric oxide from nitrogen and oxygen is a ............. reaction.
8. The potato chips manufacturers uses ............. gas to flush the chips bags to prevent the chips getting oxidised.
9. Reaction in which energy is absorbed is known as ............. reaction.
10. The reaction in which heat is given out along with products is known as ............. reaction.
11. Digestion of food in our body is an example of ............. reaction.
Fill in the blanks
1. Decomposition 2. Oxidation 3. Reduction 4. Oxidation, reduction
5. Reducing 6. loss 7. combination 8. Nitrogen
9. Endothermic 10. Exothermic 11. Combustion
Match the following
1. Column-A Column-B
Types of chemical reaction Chemical equation
(A) Combination reactoin (i) Zn + H2SO4 → ZnSO4 + H2
(B) Oxidation & reduction reaction (ii) 2H2O 2H2 + O2
(C) Decomposition reaction (iii) CaO + CO2 → CaCO3
(D) Displacement reaction (iv) H2 + Cl2 → 2HCl
(E) Double displacement reaction (v) BaCl2 + Na2SO4 → BaSO4 ¯ + NaCl
Match the following
(A) → (iii), (iv) ; (B) → (ii). (iv) ; (C) → (ii) ; (D) → (i) ; (E) → (v)
Very Short Answer Questions
1. Is it possible to have combustion without oxygen?
2. Can a double displacement reaction be a redox reaction?
3. What happens when a strip of zinc is dipped in a copper sulphate solution?
4. Is copper more reactive than iron? Give a reaction in support of your answer _
5. In which type of reaction does an exchange of partner takes place?
6. (Based on activities)
Why a dilute acid is added to water during electrolysis of water?
7. Name the product obtained on cathode during electrolysis of water
8. Is the volume of gases produced during electrolysis of water is same? If not than what is the ratio in between them?
9. What will happen if silver bromide is kept for some time in sunlight?
10. Write names of three metals which do not corrode?
11. Name two antioxidants which are usually added to fat and oil containing foods to prevent rancidity.
Short Answer Questions :_
1. What do you mean by a precipitation reaction?
2. Why should a magnesium ribbon be cleaned before burning in air?
3. Write a balanced chemical equation with symbols for the following reactions _
(i) Solutions of barium chloride and sodium sulphate in water react to give insoluble barium sulphate and the solution of sodium chloride.
(ii) Sodium hydroxide solution (in water) reacts with hydrochloric acid solution (in water) to produce sodium chloride solution and water.
4. Write the balanced equation for the following chemical reactions.
(i) Hydrogen + chlorine → Hydrogen chloride.
(ii) Barium chloride + Aluminium Sulphate → Barium sulphate + Aluminium chloride.
(iii) Sodium + water ¾® Sodium hydroxide + Hydrogen.
5. How can you say that respiration is an exothermic process?
Name two biochemical reaction which are exothermic.
6. Why blue colour of copper sulphate solution becomes faded when iron fillings are added to it?
7. What happens when copper turnings are added to silver nitrate solution?
8. Why the solution of silver nitrate becomes blue in colour after some time when copper turnings are added to it?
9. A solution of a substance 'X' is used for white washing _
(i) Name the substance 'X' and write the formula.
(ii) Write the reaction of the above substance 'X' with water.
10. Why is the amount of gas double in one of the test tube during the electrolytic decomposition of water? Name the gas?
11. When a green iron salt is heated strongly, its colour finally changes to black and odour of burning sulphur is given out.
(i) Name the iron salt
(ii) Name the type of reaction that takes place during the heating of iron salt.
(iii) Write the chemical equation for the reaction involved.
12. Write one equation each for decomposition reactions where energy is supplied by heat, light and electricity.
13. What is the difference between displacement and double displacement reactions? Write equations for these reactions.
14. Classify each of the following reactions as combination, decomposition, displacement or double displacement reaction.
(i) H2 + Cl2 → 2HCl
(ii) 2KClO3 2KCl + 3O2
(iii) Zn + CuSO4 → ZnSO4 + Cu
Blue Colour less
(iv) 2Pb(NO3)2 2PbO(s) + 4NO2(g) + O2(g)
(v) NaOH + HCl → NaCl + H2O
(vi) BaCl2 + H2SO4 → BaSO4 + 2HCl
(vii) CaO + CO2 → CaCO3
(viii) CaCO3 CaO + CO2
(ix) 2KI + Cl2 → 2KCl + I2
Chemical reaction & equation
Very short answer type
1. No 2. No 3. Blue colour of solution fade up.
4. No, because iron is more reactive metal than copper.
Fe + CuSO4 ¾® FeSO4 + Cu
5. Double displacement reaction. 6. To increase the ionization of water.
7. Hydrogen gas 8. No, H2 : O2 (2 : 1)
9. Photochemical reaction takes place.
2AgBr ¾® 2Ag(s) + Br2(g)
10. Silver, Gold, Platinum.
11.(a) BHA (Butylated Hydroxy Anisole)
(b) BHT (Butylated Hydroxy Toluene)
14. (i) Combination reaction (ii) Decomposition reaction (iii) Displacement reaction
(iv) Decomposition reaction] (v) In double displacement reaction Neutralization reaction
(vi) Double displacement reaction (vii) Combination reaction (viii) Decomposition reaction
(ix) Displacement reaction (x) Decomposition reaction