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NCERT solutions Chemistry Class 11 Part 2 chapter 10 The s-Block Elements

Chapters

NCERT Chemistry Class 11 Part 2

Chemistry Textbook for Class 11 Part 2

Chapter 10 - The s-Block Elements

Pages 305 - 306

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

Q 1 | Page 305

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

Q 2 | Page 305

Why are alkali metals not found in nature?

Q 3 | Page 305

Find the oxidation state of sodium in Na2O2.

Q 4 | Page 305

Explain why is sodium less reactive than potassium?

Q 5 | Page 305

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

Q 6 | Page 305

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

Q 7 | Page 305

Explain why alkali and alkaline earth metals cannot be obtained by chemical reduction methods?

Q 8 | Page 305

Why are potassium and cesium, rather than lithium used in photoelectric cells?

Q 9 | Page 305

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

Q 10 | Page 305

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

Q 11 | Page 305

Discuss the various reactions that occur in the Solvay process.

Q 12 | Page 305

Potassium carbonate cannot be prepared by Solvay process. Why?

Q 13 | Page 305

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

Q 14 | Page 305

Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals

Nitrates

Q 15.1 | Page 306

Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals

Carbonates 

Q 15.2 | Page 306

Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals

Sulphates

Q 15.3 | Page 306

Starting with sodium chloride how would you proceed to prepare sodium metal

Q 16.1 | Page 306

Starting with sodium chloride how would you proceed to prepare sodium hydroxide

Q 16.2 | Page 306

Starting with sodium chloride how would you proceed to prepare sodium peroxide

Q 16.3 | Page 306

Starting with sodium chloride how would you proceed to prepare sodium carbonate?

Q 16.4 | Page 306

What happens when magnesium is burnt in air.

Q 17.1 | Page 306

What happens when quick lime is heated with silica 

Q 17.2 | Page 306

What happens when chlorine reacts with slaked lime

Q 17.3 | Page 306

What happens when calcium nitrate is heated?

Q 17.4 | Page 306

Describe two important uses of each of the following Caustic soda

Q 18.1 | Page 306

Describe two important uses of the following - sodium carbonate

Q 18.2 | Page 306

Describe two important uses of the following - quicklime

Q 18.3 | Page 306

Draw the structure of BeCl2 (vapour)

Q 19.1 | Page 306

Draw the structure of BeCl2 (solid).

Q 19.2 | Page 306

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.

Q 20 | Page 306

Describe the importance of the following limestone

Q 21.1 | Page 306

Describe the importance of the following cement 

Q 21.2 | Page 306

Describe the importance of the following plaster of paris.

Q 21.3 | Page 306

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

Q 22 | Page 306

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

Q 23 | Page 306

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

Q 24 | Page 306

What happens when sodium metal is dropped in water?

Q 25.1 | Page 306

What happens when sodium metal is heated in the free supply of air?

Q 25.2 | Page 306

What happens when sodium peroxide dissolves in water?

Q 25.3 | Page 306

Comment on each of the following observations:

The mobilities of the alkali metal ions in aqueous solution are Li+ < Na+ < K< Rb+ < Cs+

Q 26.1 | Page 306

Comment on each of the following observations:

Lithium is the only alkali metal to form a nitride directly.

Q 26.2 | Page 306

Comment on each of the following observations:

 Ee for M2+ (aq) + 2e —> M(s) (where M = Ca, Sr or Ba) is nearly constant.

Q 26.3 | Page 306

State as to why a solution of Na2CO3 is alkaline?

Q 27.1 | Page 306

State as to why alkali metals are prepared by electrolysis of their fused chlorides?

Q 27.2 | Page 306

State as to why sodium is found to be more useful than potassium?

Q 27.3 | Page 306

Write balanced equations for reactions between

 Na2Oand water

Q 28.1 | Page 306

Write balanced equations for reactions between

KO2 and water

Q 28.2 | Page 306

Write balanced equations for reactions between Na2O and CO2

Q 28.3 | Page 306

How would you explain the following observations?

BeO is almost insoluble but BeSO4 in soluble in water,

Q 29.1 | Page 306

How would you explain the following observations?

 BaO is soluble but BaSO4 is insoluble in water,

Q 29.2 | Page 306

How would you explain the following observations?

LiI is more soluble than KI in ethanol.

Q 29.3 | Page 306

Which of the alkali metal is having least melting point?

(a) Na

(b) K

(c) Rb

(d) Cs

Q 30 | Page 306

Which one of the following alkali metals gives hydrated salts?

(a) Li

(b) Na

(c) K

(d) Cs

Q 31 | Page 306

Which one of the alkaline earth metal carbonates is thermally the most stable?

a) MgCO3 

(b) CaCO3 

(c) SrCO3 

(d) BaCO3

Q 32 | Page 306

NCERT Chemistry Class 11 Part 2

Chemistry Textbook for Class 11 Part 2
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