What are the common physical and chemical features of alkali metals?
Discuss the general characteristics and gradation in properties of alkaline earth metals.
Why are alkali metals not found in nature?
Find out the oxidation state of sodium in Na2O2.
Explain why is sodium less reactive than potassium.
Compare the alkali metals and alkaline earth metals with respect to (i) ionization enthalpy (ii) basicity of oxides and (iii) solubility of hydroxides.
In what ways lithium shows similarities to magnesium in its chemical behaviour?
Explain why can alkali and alkaline earth metals not be obtained by chemical reduction methods?
Why are potassium and caesium, rather than lithium used in photoelectric cells?
When an alkali metal dissolves in liquid ammonia the solution can acquire different colours. Explain the reasons for this type of colour change.
Beryllium and magnesium do not give colour to flame whereas other alkaline earth metals do so. Why?
Discuss the various reactions that occur in the Solvay process.
Potassium carbonate cannot be prepared by Solvay process. Why?
Why is Li2CO3 decomposed at a lower temperature whereas Na2CO3 at higher temperature?
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.
Starting with sodium chloride how would you proceed to prepare
sodium metal
sodium hydroxide
sodium peroxide
sodium carbonate?
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?
Describe two important uses of each of the following: (i) caustic soda (ii) sodium carbonate (iii) quicklime.
Draw the structure of (i) BeCl2 (vapour) (ii) BeCl2 (solid).
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.
Describe the importance of the following: (i) limestone (ii) cement (iii) plaster of paris.
Why are lithium salts commonly hydrated and those of the other alkali ions usually anhydrous?
Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone?
Explain the significance of sodium, potassium, magnesium and calcium in biological fluids.
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 ?
Comment on each of the following observations:
The mobilities of the alkali metal ions in aqueous solution are Li+ < Na+ < K+ < Rb+ < Cs+
Lithium is the only alkali metal to form a nitride directly.
for M2+ (aq) + 2e– → M(s) (where M = Ca, Sr or Ba) is nearly constant.
State as to why
a solution of Na2CO3 is alkaline?
alkali metals are prepared by electrolysis of their fused chlorides?
sodium is found to be more useful than potassium?
Write balanced equations for reactions between
(a) Na2O2 and water
(b) KO2 and water
(c) Na2O and CO2.
How would you explain the following observations?
(i) BeO is almost insoluble but BeSO4 is soluble in water,
(ii) BaO is soluble but BaSO4 is insoluble in water,
(iii) LiI is more soluble than KI in ethanol.
Which of the alkali metal is having least melting point?
Which one of the following alkali metals gives hydrated salts?
Which one of the alkaline earth metal carbonates is thermally the most stable?
