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The s-Block Elements

Short Answer Type

191.

Starting with CaCO₃, write balanced chemical equation showing the preparation of:
(i) CaO (ii) CaSO₄(iii) Ca(OH)₂ (iv) Ca(HCO₃)₂ solution.

111 Views

Long Answer Type

192.

Describe two important uses of the following;
(a) Caustic soda (b) Sodium carbonate (iii) Quick lime.

403 Views

193.

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?

318 Views

194.

Discuss the composition and manufacturing details of cement.
Or
Mention the main constituents of Portland cement.

363 Views

Short Answer Type

195.

Complete the following equations:
$left parenthesis straight i right parenthesis space Ca space plus space straight H subscript 2 straight O space space rightwards arrow space space left parenthesis ii right parenthesis space Ca left parenthesis OH right parenthesis subscript 2 space plus space Cl subscript 2 space rightwards arrow space left parenthesis iii right parenthesis space BeO space plus space NaOH space rightwards arrow space left parenthesis iv right parenthesis space BaO subscript 2 space plus space straight H subscript 2 SO subscript 4 space rightwards arrow$

105 Views

196.

Contrast the action of heat on the following and explain your answer:
(i) Na₂CO₃ and CaCO₃(ii) MgCl₂.6H₂O and CaCl₂.6H₂O
(iii) Ca(NO₃)₂ and NaNO₃.

226 Views

197.

Explain the significance of magnesium and calcium in biological fluids.

186 Views

198.

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

377 Views

199.

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

505 Views

200.
Compare the alkali metals and alkaline earth metals with respect to (i) ionisation enthalpy (ii) basicity of oxides and (iii) solubility of hydroxides.

Alkali metals	Alkaline earth metals
(i) Ionisation enthalpy: These have the lowest ionisation enthalpies in respective periods. This is because of their large atomic sizes. Also, they lose their only valence electron easily as they attain stable noble gas configuration after losing it.	(i) Ionisation enthalpy: Alkaline earth metals have smaller atomic size and higher effective nuclear charge as compared to alkali metals. This causes their first ionisation enthalpies to be higher than that of alkali metals. However, their second ionisation enthalpy is less than the corresponding alkali metals. This is because alkali metals, after losing one electron acquires noble gas configuration, which is very stable
(ii) Basicity of oxides: The oxides of alkali metals are very basic in nature. This happens due to the highly electropositive nature of alkali metals, which makes these oxides highly ionic. Hence, they readily dissociate in water to give hydroxide ions.	(ii) Basicity of oxides: The oxides of alkaline earth metals are quite basic but not as basic as those of alkali metals. This is because alkaline earth metals are less electropositive than alkali metals.
(iii) The solubility of hydroxides: The hydroxides of alkali metals are more soluble than those of alkaline earth metals.	(iii) The solubility of hydroxides: The hydroxides of alkaline earth metals are less soluble than those of alkali metals. This is due to the high lattice energies of alkaline earth metals. Their higher charge densities (as compared to alkali metals) account for higher lattice energies.