Which of the following is soluble in pyridine:-

(1) LiCl

(2) CsCl

(3) NaCl

(4) KCl

Ionic mobility of which of the following alkali metal ions is lowest when an aqueous solution of their salts are put under an electric field?

(1) Na                       

(2) K

(3) Rb                       

(4) Li

The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. Amongst fluorides of alkali metals, the lowest solubility of LiF in water is due to:

(a) Ionic nature of lithium fluoride             

(b) High lattice enthalpy

(c) High hydration enthalpy of lithium ion

(d) Low ionisation enthalpy of lithium atom

By adding gypsum to cement:

(1) Setting time of cement becomes less       

(2) Setting time of cement increases

(3) Colour of cement becomes light               

(4) Shining surface is obtained

Property of all the alkaline earth metals that increases with their atomic number is :

(A) Solubility of their carbonates

(B) Thermal stability of their sulphates

(C) Ionisation energy

(D) Electronegativity

A metal [x] on heating on nitrogen gas gives [Y]. [Y] on treatment with ${\mathrm{H}}_2\mathrm{O}$ gives a colourless gas which when passed through ${\mathrm{CuSO}}_4$ solution gives a blue colour. [Y] is

(A) $\mathrm{Mg}{\left({\mathrm{NO}}_3\right)}_2$                                     

(B) ${\mathrm{Mg}}_3{\mathrm{N}}_2$

(C) ${\mathrm{NaN}}_3$                                             

(D) $\mathrm{MgO}$

The density of-

1. Na > K                                                     

2. Na = K

3. K > Na                                                     

4. Li > K

Lattice energy is lowest for –

(A) LiF                                                       

(B) NaCl

(C) KBr                                                       

(D) CsI

Which of the following halides has the highest melting point-

(A) NaCl                                           

(B) KCl

(C) NaBr                                           

(D) NaF

Alkaline earth metals form hydrated crystalline solids such as $MgC{l}_2.6H_{2}O, CaC{l}_2.6H_{2}O$. This is due to-

(1) Smaller ionic size

(2) Increased charge on ions

(3) Higher hydration enthalpies

(4) High oxidation potential