Q. Describe two important uses of each of the following: (i) caustic soda (ii) sodium carbonate (iii) quicklime.

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

Q. Why are alkali metals not found in nature?

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

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

Q. Why are potassium and caesium used, rather than lithium used in photoelectric cells?

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

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

Q. Explain why is sodium less reactive than potassium.

Q. Find out the oxidation state of sodium in $N{a}_2{O}_2$.

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

Q. Why is $L{i}_{2}C{O}_3$ decomposed at a lower temperature whereas $N{a}_{2}C{O}_3$ at higher temperature?

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

Q. Draw the structure of

Q. What happens when:

Q. 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.

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

Q. 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.

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