NCERT Solutions For Class 11 Chemistry Chapter 9 Hydrogen

Class 11 Chemistry Chapter 9 Hydrogen

NCERT Solutions For Class 11 Chemistry Chapter 9 Hydrogen, (Chemistry) exam are Students are taught thru NCERT books in some of the state board and CBSE Schools. As the chapter involves an end, there is an exercise provided to assist students to prepare for evaluation.  Students need to clear up those exercises very well because the questions withinside the very last asked from those.

Sometimes, students get stuck withinside the exercises and are not able to clear up all of the questions.  To assist students to solve all of the questions and maintain their studies without a doubt, we have provided step-by-step NCERT Solutions for the students for all classes.  These answers will similarly help students in scoring better marks with the assist of properly illustrated solutions as a way to similarly assist the students and answering the questions right.

NCERT Solutions For Class 11 Chemistry Chapter 9 Hydrogen

Class 11 Chemistry Chapter 9 Hydrogen


Chapter 9 Hydrogen

9.1. Justify the position of hydrogen in the periodic table on the basis of its electronic configuration.


Hydrogen has been placed at the top of the alkali metal in group, but it is not a member of the group.

Its position is not justified properly because of its electronic configuration as (1s1). It can be placed with alkali metals because it also has similar configuration (ns1) as alkali metals.

However, it can also be placed along with halogen in group 17 since just like halogen it can acquire inert gas configuration by accepting one electron.

9.2. Write the names of isotopes of hydrogen. What is the mass ratio of these isotopes?


9.3. Why does hydrogen occur in a diatomic form rather than in a monoatomic form under normal conditions?


In diatomic form, the K-shell of hydrogen is complete (1s2) and so it is quite stable.

9.4. How can the production of dihydrogen obtained from ‘Coal gasification’ be increased?


The production of dihydrogen in coal gasification can be increased by reacting CO(y) present in syngas with steam in the presence of iron chromate catalysts.

With the removal of C02 the reaction shifts in the forward direction and thus, the production of dihydrogen will be increased.

9.5. Describe the bulk preparation of dihydrogen by electrolytic method. What is the role of an electrolyte in this process?


In bulk, hydrogen can be produced by electrolysis of acidified water using Pt electrodes.

Electrolyte is added to increase the dissociation of water.

9.6. Complete the following reactions.


9.7. Discuss the consequences of high enthalpy of H-H bond, in terms of chemical reactivity of dihydrogen.


This is due to its small atomic size and also small bond length (74 pm) of H-H bond.

9.8. What do you understand by (i) Electron-deficient (ii) Electron-precise (iii) Electron-rich compounds of hydrogen? Provide justification with suitable examples.


(i) Electron deficient hydrides: Compounds in which central atom has incomplete octet, are called electron deficient hydrides. For example, BeH2, BH3 are electron deficient hydrides.

(ii) Electron precise hydrides: Those compounds in which exact number of electrons are present in central atom or the central atom contains complete octet are called precise hydrides e.g., CH4, SiH4, GeH4 etc. are precise hydrides.

(iii) Electron rich hydrides: Those compounds in which central atom has one or more lone pair of excess electrons are called electron rich hydrides, e.g.,NH3, H2O.

9.9. What characteristics do you expect from an electron-deficient hydride with respect to its structure and chemical reaction?


It is expected to be a Lewis acid. They are likely to accept electrons to become stable. They can form coordinate bond with electron rich compound.

9.10. Do you expect the carbon hydride of type Cn H2n+2 to act as ‘Lewis’ acid or base? Justify your answer.


Carbon hydrides of the type Cn H2n+2 are electron precise hydrides. Because they have atom with exact number of electrons to form covalent bonds. Thus, they do not behave as Lewis acid or base. Since they have no tendency to accept or lose electrons.

9.11. What do you understand by the term ‘non-stoichiometric hydrides’? Do you expect this type of hydrides to be formed by alkali metals? Justify your answer.


Those hydrides which do not have fix composition are called non-stoichiometric hydrides, and the composition varies with temperature and pressure. This type of hydrides are formed by d and /block elements. They cannot be formed by alkali metals because alkali metal hydrides form ionic hydrides.

9.12. How do you expect the metallic hydrides to be useful for hydrogen storage? Explain.


In metallic hydrides, hydrogen is adsorbed as H-atoms. Due to the adsorption of H atoms the metal Lattice expands and become unstable. Thus, when metallic hydride is heated, it decomposes to form hydrogen and finely divided metal. The hydrogen evolved can be used as fuel.

9.13. How does the atomic hydrogen or oxy-hydrogen torch function for cutting and welding purposes ? Explain.


When hydrogen is burnt in oxygen the reaction is highly exothermic, it produces very high temperature nearly 4000°C which is used for cutting and welding purposes.

9.14.  Among NH3 H2O and HE, which would you expect to have highest magnitude of hydrogen bonding and why?


HF is expected to have highest magnitude of hydrogen bonding since, ‘F’ is most electronegative. Therefore, HF is the most polar.

9.15. Saline hydrides are known to react with water violently producing fire. Can C02, a well known fire extinguisher, be used in this case? Explain.


No. Because if saline hydrides react with water the reaction will be highly exothermic thus the hydrogen evolved in this case can catch fire. C02 cannot be used as fire extinguisher because C02 will get absorbed in alkali metal hydroxides.

9.16. Arrange the following:

(i) CaH2, BeH2 and TiH2 in order of increasing electrical conductance.

(ii) LiH, NaH and CsH in order of increasing ionic character.

(iii) H-H, D—D and F—F in order of increasing bond dissociation enthalpy.

(iv) NaH, MgH2 and H2O in order of increasing reducing property.


(i) BeH2< TiH2 < CaH2

(ii) LiH < NaH < CsH

(iii) F—F < H—H < D—D

(iv) H2O < MgH2 < NaH

9.17. Compare the structures of H2O and H2O2


In water, O is sp3 hybridized. Due to stronger lone pair-lone pair repulsions than bond pair-bond pair repulsions, the HOH bond angle decreases from 109.5° to 104.5°. Thus water molecule has a bent structure.

H2O2 has a non-planar structure. The O—H bonds are in different planes. Thus, the structure of H2O2 is like an open book.

9.18. What do you understand by the term ‘auto-protolysis’ of water? what is its significance?


Auto-protolysis means self-ionisation of water. It may be represented as

Due to auto-protalysis water is amphoteric in nature, i.e., it can act as an acid as well as base.

9.19. Consider the reaction of water with F2 and suggest, in terms of oxidation and reduction, which species are oxidised/reduced ?


2F2(ag) + 2H20(l)—————> O2(g) + 4H+(aq) + 4F(aq)

In this reaction water acts as a reducing agent and itself gets oxidised to O2 while F2 acts as an oxidising agent and hence itself reduced to F ions.

9.20. Complete the following chemical reactions.

(i) PbS(s) + H2O2 (aq) ————->

(ii) MnO4 (aq) + H2O2 (aq) ————->

(iii) CaO(s) + H2O(g) ————->

(iv) AlCl3(g) + H2O(l)————->

(v) Ca3N2(S) + H2O(l) ————->

Classify the above into (a) hydrolysis, (b) redox and (c) hydration reactions.


(i) PbS(s) +4H2O2(aq) ————-> PbSO4(s) + 4H2O(l)

(ii) 2MnO4 (aq) +H2O2(aq) + 6H+(aq) ————-> 2Mn (aq) + 8H2O(l) + 5O2(g)

(iii) CaO(s) + H2O(g) ————->Ca(OH)2(aq)

(iv) AlCl3(aq) + 3H2O(l) ————-> Al(OH)3(S) + 3HCl (aq)

(v) Ca3N2(s) + H2O(l) ————->3Ca(OH)2(aq) + 2NH3(aq)

(a) Hydrolysis reactions, (iii) (iv) and (v)

(b) Redox reactions (i) and (ii)

9.21. Describe the structure of common form of ice.


Ice crystallizes in the normal hexagonal form. However, at very low temperatures it condenses in cubic form. In the normal hexagonal ice each oxygen atom is tetrahedrally surrounded by four other hydrogen atoms.

9.22. What causes the temporary and permanent hardness of water?


Temporary hardness of water is due to the presence of bicarbonates of calcium and magnesium in water i.e., Ca(HCO3)2 and Mg(HCO3) in water. Permanent hardness of water is due to the presence of soluble chlorides and sulphates of calcium and magnesium i.e., CaCl2, CaS04, MgCl2 and MgS04.

9.23. Discuss the principle and method of softening of hard water by synthetic ion-exchange resins.


Cation exchange resins have large organic molecule with S03H group which are insoluble in water. Ion exchange resin (RS03H) is changed to RNa on treatment with NaCl. The resin exchange Na+ ions with Ca2+ and Mg2+ ions present in hard water and make it soft.

2RNa(s) + M2+(aq) ——> R2M(s) + 2Na+(aq)

where, M = Mg, Ca.

The resins can be regenerated by adding aqueous NaCl solution.

9.24. Write chemical reaction to show the amphoteric nature of water.


Water is amphoteric in nature because it acts as an acid

9.25. Write chemical reactions to justify that hydrogen peroxide can function as an oxidising as well as reducing agent.


As an oxidising agent

2Fe2+  (aq) + 2H+(aq) +H2O2(aq) ———–> 2Fe3+  (aq) + 2 H2O(l)

As a reducing agent

I2(s) + H2O2 (aq) + 2OH (aq) ———> 2I (aq) + 2 H2O(l) + O2(g)

9.26. What is meant by ‘demineralised water’ and how can it be obtained?


Demineralised water is free from all soluble mineral salts which is obtained by passing water successively through a cation exchange (in the form of H+) and an anion exchange in the form of OH resins.

H+ exchanges for Na+, Ca2+, Mg2+ and other cations present in water. This process results in release of proton which makes the water acidic.

OH exchanges, for anions like Cl, HCO3,SO42-etc.

OH ions thus liberated neutralize the H+ ions set free in the cation exchange process. H+(aq) + OH(aq) ——-> H2O(l)

9.27. Is demineralised or distilled water useful for drinking purposes? If not, how can it be made useful ?


No, demineralised water is not fit for drinking purposes. It can be made useful by adding required amount of ions which are useful for our body.

9.28. Describe the usefulness of water in biosphere and biological systems.


(i) Major part of all living system is made of water.

(ii) It constitutes about 65 – 70% of body weights of animals and plants.

(iii) Some properties of water like high specific heat, thermal conductivity, surface tension, high polarity allow water to play a major role in biosphere.

(iv) Because of high heat of vaporisation it is responsible ro regulate temperature of living beings.

(v) It is an excellent fluid for the transportation of minerals and nutrients in plants.

(vi) It is also required for photosynthesis in plants.

9.29. What properties of water make it useful as a solvent? What types of compound can it (i) dissolve (ii) hydrolyse?


Water is highly polar in nature thats why it has high dielectric constant and high dipole moment. Because of these properties, water is a universal solvent.

It can hydrolyse many oxides metallic or non-metallic, hydrides, carbides, nitrides etc.

9.30. Knowing the properties of H2O and D2O, do you think D2O can be used for drinking purpose.


No, D2O is injurious to human beings, plants and animals.

9.31. What is the difference between the terms ‘hydrolysis’ and ‘hydration’?


Hydrolysis is a chemical reaction in which a substance reacts with water under neutral, acidic or alkaline conditions.

9.32. How can saline hydrides remove traces of water from organic compounds?


Saline hydrides (i.e, CaH2 NaH etc.) react with water and form the corresponding metal hydroxide with the liberation of Hgas. Thus, these hydrides can be used to remove traces of water from the organic compounds.

NaH(s) + H2O(l) ———–> NaOH(aq) + H2(g)

CaH2(s) + 2H2O(l) ———> Ca(OH)2(aq) + H2(g)

9.33. What do you expect the nature of hydrides is, if formed by elements of atomic numbers 15,19, 23 and 44 with dihydrogen? Compare their behaviour towards water.


Atomic No. 15 is of phosphorus. The hydride is PH3 and its nature is covalent. Atomic No. (Z = 19) is of potassium. The hydride is KH and it is ionic in nature. Atomic No. (Z = 23) is of vanadium. The hydride is VH. It is interstitial or metallic. Atomic No. 44 is of ruthenium, its hydride is interstitial or metallic.

9.34. Do you expect different products in solution when aluminium (III) chloride and potassium chloride treated separately with (i) normal water (ii) acidified water (iii) alkaline water? Write equation wherever necessary.


9.35. How does H2O2 behave as a bleaching agent?


Bleaching action of H2O2 is due to the oxidation of colouring matter by nascent oxygen.

H2O2(Z) ———> H2O(Z) + O(g)

9.36. What do you understand by the terms:

(i) Hydrogen economy (ii) hydrogenation (iii) syngas (iv) water-gas shift reaction (v) fuel-cell?


(i) Hydrogen economy: The basic principle of hydrogen economy is the storage and transportation of energy in the form of liquid or gaseous dihydrogen.

(ii) Hydrogenation: Hydrogenation means addition of hydrogen across double and triple bonds in presence of catalyst to form saturated compounds.

(iii) Syngas: The mixture of CO and H2 are called synthesis or syngas. It can be produced by the reaction of steam on hydrocarbon or coke at high temperature in the presence of nickel catalyst

(iv) Water-gas shift reaction: The amount of hydrogen in the syngas can be increased by the action of CO of syngas mixture with steam in the presence of iron chromate as catalyst.This is called water-gas shift reaction.

(v) Fuel-Cell: It is a cell which converts chemical energy of fuel directly into electrical energy.

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