NCERT Solutions For Class 11 Chemistry Chapter 10 The S Block Elements

Class 11 Chemistry Chapter 10 The S Block Elements

NCERT Solutions For Class 11 Chemistry Chapter 10 The S Block Elements, (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 10 The S Block Elements

Class 11 Chemistry Chapter 10 The S Block Elements


10.1. What are the common physical and chemical features of alkali metals?


Physical properties of alkali metals:

  • Alkali metals have low ionization enthalpies.
  • Alkali metals are highly electropositive in nature.
  • Alkali metals exhibit +1 oxidation states in their compounds.
  • Alkali metals impart characteristic colours to the flame.

Chemical properties of alkali metals:

  • Alkali metals are highly reactive in nature.
  • Alkali metals hydroxides are highly basic in nature.
  • Alkali metals dissolve in liquid ammonia to form blue and conducting solution.

10.2. Discuss the general characteristics and gradation in properties of alkaline earth metals.


  • Atomic size goes on increasing down the group.
  • Ionisation energy goes on decreasing down the group.
  • They are harder than alkali metals.
  • They are less electropositive than alkali metals.
  • Electropositive character increases on going down the group.

10.3. Why are alkali metals not found in nature?


Alkali metals are highly reactive in nature. That’s why they always exist in combined state in nature.

10.4. Find out the oxidation state of sodium in Na2O2.


Let x be the oxidation state of Na in Na2O2     2x + 2 (-1) = 0  2x – 2 = 0    2x = 2 x = +1.

10.5. Explain why is sodium less reactive than potassium.


It is because ionization enthalpy ∆Hi of potassium = 419 kJ mol -1.
Ionization enthalpy of sodium = 496 KJ mol. Since Ionization enthalpy of potassium is less than that of sodium, potassium is more reactive than sodium.

10.6. Compare the alkali metals and alkaline earth metals with respect to (i) ionization enthalpy, (ii) basicity of oxides, (iii) solubility of hydroxides.


(i) Ionization enthalpy. Because of high nuclear charge the ionization enthalpy
of alkaline earth metals are higher than those of the corresponding alkali metals.

(ii) Basicity of oxides. Basicity of oxides of alkali metals are higher than that of alkaline earth metals.

(iii) Solubility of hydroxides of alkali metals are higher than that of alkaline earth metals. Alkali metals due to lower ionization enthalpy are more electropositive than the corresponding group 2 elements.

10.7. In what ways lithium shows similarities to magnesium in its chemical behaviour?


  • Both react with nitrogen to form nitrides.
  • Both react with 02 to form monoxides.
  • Both the elements have the tendency to form covalent compounds.
  • Both can form complex compounds.

10.8. Explain why can alkali and alkaline earth metals not be obtained by chemical reduction method.


Alkali and alkaline earth metals are themselves better recucing agents, and reducing agents better than alkali metals are not available. That is why these metals are not obtained by chemical reduction methods.

10.9. Why are potassium and calcium, rather than lithium used in photoelectric cells?


Potassium and calcium have much lower ionization enthalpy than that of lithium. As a result, these metals easily emit electrons on exposure to light. Due to this, K and Cs are used in photoelectric cells rather than lithium.

10.10. When alkali metal dissolves in liquid ammonia, the solution can acquire different colours. Explain the reason for this type of colour change.


Alkali metals dissolve in liquid ammonia and give deep blue solutions which are conducting in nature because ammoniated electrons absorb energy in the visible region of light and impart blue colour.

10.11. Beryllium and magnesium do not give colour to flame whereas other alkaline earth metals do so. Why?


Due to small size, the ionization enthalpies of Be and Mg are much higher than those of other alkaline earth metals. Therefore, a large amount of energy is needed to excite their valence electron, and that’s why they do not impart colour to the flame.

10.12. Discuss the various reactions that occur in the Solvay process.


10.13. Potassium carbonate cannot be prepared by Solvay process. Why?


Potassium carbonate being more soluble than sodium bicarbonate does not get precipitated when CO2 is passed through a concentrated solution of KCl saturated with ammonia.

10.14. Why is Li2CO3 decomposed at a lower temperature whereas Na2CO3 at higher temperature?


Li2COis a covalent compound whereas Na2CO3 is an ionic compound. Therefore, Lattice energy of Na2CO3 is higher than that of Li2CO3. Thus, LiCO3 is decomposed at a lower temperature.

10.15. Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals.
(a) Nitrates (b) Carbonates (c) Sulphates


(a) Nitrates of both group 1 and group 2 elements are soluble in water because hydration energy is more than the lattice energy.
Nitrates of both group 1 and group 2 elements are thermally unstable but they decompose differently except LiCO3 e.g.

(b) Carbonates of group 1 elements are soluble in water except Li2CO3 They are also thermally stable except Li2CO3

Group 2 carbonates are insoluble in water because their Lattice energy are higher than hydration energy.
Thermal stability of carbonates of group 2 increases down the group because Lattice energy goes no increasing due to increase in ionic character.
(c) Sulphates of group 1 are soluble in water except Li2SO4. They are thermally stable.
Solubility of sulphates of group 2 decreases down the group because Lattice energy dominates over hydration energy.
Sulphates of group 2 elements are thermally stable and increasing down the group due to increases in Lattice energy.

10.16. Starting with sodium chloride how would you proceed to prepare.
(i) Sodium metal (ii) Sodium hydroxide
(iii) Sodium peroxide (iv) Sodium carbonate?


(i) Sodium metal is manufactured by electrolysis of a fused mass of NaCl 40% and CaCl2 60% in Down’s cell at 873 K, using iron as cathode and graphite as anode. Na is liberated at the cathode.
At cathode:
Na+ + e —–> Na (l)
At anode:
2Cl (melt) ——-> Cl2 (g) + 2e.
(ii) Sodium hydroxide is manufactured by electrolysis of an aqueous solution of NaCl (brine) in Castner-Kellner cell.
At cathode:
Na+ + e —–> Na
2Na + Hg ——->Na – Hg + 2H20
2Na- Hg + 2H20——>2NaOH +H2 +Hg
At anode:
Cl – e ——->Cl
Cl + Cl——–>Cl2
(iii) Sodium peroxide:
4Na + 02 2Na2O + 02
(iv)Sodium carbonate is obtained by Solvay ammonia process.

10.17. What happens when (i) magnesium is burnt in air, (ii) Quick lime is heated with silica (iii) chlorine reacts with slaked lime (iv) calcium nitrate is heated?


10.18. Describe two important uses of each of the following: ,
(i) caustic soda (ii) sodium carbonate (iii) quick lime


(i) Caustic soda
(a) It is used in the manufacturing of soap paper, artificial silk etc.
(b) It is used in textile industries.

(ii) Sodium carbonate
(a) Used in the softening of water, for laundry and cleaning purposes.
(b) It is used in glass manufacturing.

(iii) Quick lime
(a) It is used in the preparation of bleaching powder.
(b) Used in the purification of sugar and in the manufacturing of cement.

10.19. Draw the structure of (i) BeCl2 (vapour), (ii) BeCl2 (solid).


BeCl2 (vapour)
In the vapour state, it exists as a chlorobridged dimer.

10.20. The hydroxides and carbonates of sodium and potassium are easily soluble in water while the corresponding salts of magnesium and calcium are sparingly soluble in water. Explain.


Since group 1 hydroxides and carbonates due to large size contain higher hydration energy than the lattice energy so, they are easily soluble in water. Whereas, in magnesium and calcium due to small size their lattice energy dominates over hydration energy they are sparingly soluble in water.

10.21. Describe the importance of the following:
(i) Limestone (ii) Cement (iii) Plaster of Paris.



  • Extensively used in the manufacturing of high quality paper.
  • Used as mild abrasive in toothpaste.
  • As a filler in cosmetics.
  • Used as an antacid.


  • An important building material.
  • Used in concrete and reinforced cement.

Plaster of Paris:

  • Used in plasters.
  • In dentistry, in ornamental work for making statues.

10.22. Why are lithium salts commonly hydrated and those of the other alkali metal ions usually anhydrous?


Due to smallest size, Li+ can polarize water molecules easily than the other alkali metal ions.

10.23. Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone?


It is due to high lattice energy of LiF as compared to LiCl.
LiCl is soluble in water because its hydration energy is higher than its lattice energy.

10.24. Explain the significance of sodium, potassium, magnesium and calcium in biological fluids.


Sodium ions:

  • Na+ ions participate in the transmission of nerve signals, in regulating the flow of water across cell membranes.
  • In the transport of sugars and amino acids into cell.

Potassium ions:

  • They activate many enzymes.
  • Participate in the oxidation of glucose to produce ATP.

Magnesium ions:

  •  All enzymes that utilise ATP in phosphate transfer require magnesium as a cofactor.
  • Mg is the main pigment for the absorption of light in plants.


  •  Ca2+ ions are present in bones.
  •  plays important roles in neuromuscular function.

10.25. What happens when
(i) Sodium metal is dropped in water?
(ii) Sodium metal is heated in free supply of air?
(iii) Sodium peroxide dissolves in water?


(i) 2Na + 2H2O ——–> 2NaOH + H2
(ii) 2Na + O2 ———> Na2O2
(iii) Na2O2 + 2H20 ———> 2NaOH + H2O2

10.26. Comment on each of the following observations:
(a) The mobilities of the alkali metal ions in aqueous solution are Li+ < Na+ <K+ < Rb+ < Cs+
(b) Lithium is the only alkali metal to form a nitride directly.
(c) Ee for M2+ (aq) + 2e —> M(s) (where M = Ca, Sr, or Ba) is nearly constant.


(a) Smaller the size of the ion, more highly it is hydrated and hence greater is the mass of the hydrated ion and thus the ionic mobility become lesser. The extent of hydration decreases in the order.
Li+ < Na+ <K+ < Rb+ < Cs+
Thus the mobility of Cs+ will be the highest.
(b) Due to its smaller size lithium can form nitride directly.
(c) It is because reduction potential depends upon sublimation energy, ionisation energy and hydration energy. Their resultant is almost constant for these ions.

10.27. State as to why
(a) a solution of Na2CO3 is alkaline?
(b) alkali metals are prepared by electrolysis of their fused chlorides?
(c) Sodium is found to be move useful than potassium?


(a) Na2CO3 is a salt of a weak acid, carbonic acid (H2CO3) and a strong base NaOH. Thus it undergoes hydrolysis to produce strong base NaOH and its aqueous solution is alkaline in nature.
Na2CO3(s) + H2O(l)———–>2NaOH
(b) Because the discharge potential of alkali metals is much higher than that of hydrogen, therefore when the aqueous solution of any alkali metal chloride is subjected to electrolysis, H2, instead of the alkali metal, is produced at the cathode. Therefore alkali metals are prepared by electrolysis of their fused chlorides.
(c) Since potassium is move reactive than sodium and it is found in nature to a less extent than Na, sodium is found to be more useful.

10.28.Write balanced equations for reactions between.
(a) Na2O2 and water
(b) KO2 and water
(c) Na2O and CO2


(a) Na2O2 + 2H2O ——-> 2Na0H + H2O2
(b) 2KO2 + 2H2O ———-> 2K0H + O2+ H2O2
(c) Na2O+ CO2 ———–>Na2CO3

10.29.  How would you explain the following observations?
(i) BeO is almost insoluble but BeSO4 is soluble in water.
(ii) BaO is soluble but BaSO4is insoluble in water.
(iii) Lil is more soluble than KI in ethanol.


(i) Lattice energy of BeO is compartively higher than the hydration energy. Therefore, it is almost insoluble in water. Whereas  BeSO4 is ionic in nature and its hydration energy dominates the lattice energy.
(ii) Both BaO and BaSOare ionic compounds but the hydration energy of BaO is higher than the lattice energy therefore it is soluble in water.
(iii) Since the size of Li+ ion is very small in comparison to K+ ion, it polarises the electron cloud of I ion to a great extent. Thus Lil dissolves in ethanol more easily than the KI.

10.30. Which of the alkali metal is having least melting point?
(a) Na (b) K (c) Rb (d) Cs


Size of Cs is the biggest thus, its melting point is the lowest, (d) is correct.

10.31. Which one of the following alkali metals give hydrated salts?
(a) Li (b) Na (c) K (d) Cs


Li+ is the smallest. Thus, it has the highest charge density and hence attracts the water molecules more strongly.

10.32. Which one of the following alkaline earth metal carbonates is thermally most stable?
(a) MgCO3 (b) CaCO3 (c) SrCO3 (d) BaCO3


(d) BaCO3

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