Lithium has the minimum tendency to form ${\mathrm{Li}}^{+}$ ion. The aqueous solution of lithium is the

1. Strongest reducing agent.                      

2. Poorest reducing agent.

3. Strongest oxidising agent.                

4. Poorest oxidising agent.

Calcium hydride can be obtained by heating : 

1. Calcium oxide with hydrogen.

2. Calcium oxide with hydrogen under pressure.

3. Calcium with hydrogen under pressure.

4. Calcium with hydrogen at a very low temperature.

Calcium hydroxide upon reacting with moist chlorine forms-

1. ${\mathrm{CaCl}}_2$                                 

2. $\mathrm{Ca}{\left(\mathrm{OCl}\right)}_2$

3. ${\mathrm{CaCl}}_2.2{\mathrm{H}}_2\mathrm{O}$                       

4. ${\mathrm{CaCl}}_2.7{\mathrm{H}}_2\mathrm{O}$

A blue colored solution of an alkali metal in liq NH₃ is due to the presence of -

1. ${\mathrm{M}}^{-}$atoms.                                         

2. ${\mathrm{M}}^{+}$ ions .

3. Solvated anions  .                           

4. Solvated electrons.

Alkali metal ions are- 

1. Diamagnetic and coloured.

2. Diamagnetic and colourless.

3. Paramagnetic and coloured.

4. Paramagnetic and colourless.

A compound X on heating gives a colourless gas. The residue is dissolved in water to obtain Y. Excess $C{O}_2$ is bubbled through an aqueous solution of Y, and Z is formed. Z on gentle heating gives back X. The compound X is-

1. ${\mathrm{CaCO}}_3$                                           

2. ${\mathrm{Na}}_2{\mathrm{CO}}_3$

3. ${\mathrm{CaSO}}_4.2{\mathrm{H}}_2\mathrm{O}$                                 

4. ${\mathrm{K}}_2{\mathrm{CO}}_3$

Magnesia can be prepared by -

1. Burning Mg in air.

2. Heating hydroxide, nitrate, sulphate or carbonate of magnesium.

3. Heating Mg in steam.

4. All of the above.

A compound insoluble in acetic acid is  -

1. Calcium oxide.                    

2. Calcium carbonate.

3. Calcium oxalate.                      

4. Calcium hydroxide.

The incorrect statement regarding Be(II group) is -

1. It forms an ionic carbide.

2. Its carbonate decomposes on heating.

3. Its halides are covalent.

4. It is easily attacked by water.

Ca, on exposure of the moist air, forms a layer on its surface as : 

1. ${\mathrm{CaCO}}_3$                                             

2. $\mathrm{Ca}{\left(\mathrm{OH}\right)}_2$

3. ${\mathrm{CaCO}}_3.\mathrm{Ca}{\left(\mathrm{OH}\right)}_2$                               

4. CaO