Sodium reacts with water less vigorously than potassium because-

1. It has a higher atomic weight.

2. It is less electropositive .

3. It is more electronegative. 

4. It is a metal .

The correct relation about the density of Na and K is 

1. Na > K                                                     

2. Na = K

3. K > Na                                                     

4. Li > K

Which of the following does not give an oxide on heating-

(1) $MgC{O}_3$                                                   

(2) $L{i}_{2}C{O}_3$

(3) $ZnC{O}_3$                                                   

(4) $K_{2}C{O}_3$ 

The reason for a lower basicity of hydroxides of alkaline earth metals than alkali metals is : 

1. Alkali metals form ionic compounds.

2. The bond strength of oxygen is more for alkali metals.

3. The electropositivity of alkali metals is more than alkaline earth metals.

4. The electropositivity of alkali metals is less than alkaline earth metals.

In $K^{+}{F}^{-}$ ionic radius of $F^{-}$ is more while atomic radius of $K^{+}$ is –

(1) Less than $F^{-}$

(2) More than $F^{-}$

(3) Equal to $F^{-}$

(4) None of these

Lattice energy is lowest for –

1. LiF                                                       

2. NaCl

3. KBr                                                       

4. CsI

MgO is a-

(1) Acidic oxide                                     

(2) Basic oxide

(3) Neutral oxide                                   

(4) Amphoteric oxide

Which of the following statements is wrong ?

(1) Lithium nitrate on heating gives lithium nitrite and $O_2$.

(2) Sodium oxide, $N{a}_{2}O$ is obtained on heating sodium azide with sodium nitrite.

(3) Potassium cyanide dissolves silver in presence of air or $O_2$.

(4) Potassium formate is formed when moist $C{O}_2$ reacts with potassium hydride.

Ionic conductances of hydrated M+ ions are in the order-

(1) $L{i}^{+}\left(aq\right)>N{a}^{+}\left(aq\right)>K^{+}\left(aq\right)>R{b}^{+}\left(aq\right)>C{s}^{+}\left(aq\right)$

(2) $L{i}^{+}\left(aq\right)>N{a}^{+}\left(aq\right)<K^{+}\left(aq\right)<R{b}^{+}\left(aq\right)<C{s}^{+}\left(aq\right)$

(3) $L{i}^{+}\left(aq\right)>N{a}^{+}\left(aq\right)>K^{+}\left(aq\right)>R{b}^{+}\left(aq\right)<C{s}^{+}\left(aq\right)$

(4) $L{i}^{+}\left(aq\right)<N{a}^{+}\left(aq\right)<K^{+}\left(aq\right)<R{b}^{+}\left(aq\right)<C{s}^{+}\left(aq\right)$

Among the following groups of oxides, the group containing oxides that cannot be reduced by carbon to give the respective metals is –

(1) PbO, $F{e}_3{O}_4$                                   

(2) CaO, $K_{2}O$

(3) $C{u}_{2}O, Sn{O}_2$                                   

(4) $F{e}_2{O}_3, ZnO$