Classification of elements and Periodicity in properties MCQs for NEET — Chemistry Questions with Answers

,

,

and

:

S : Sulphate is estimated as ${\mathrm{BaSO}}_4$ and not as ${\mathrm{MgSO}}_4$.

E : Ionic radius of ${\mathrm{Mg}}^{2+}$ is smaller than ${\mathrm{Ba}}^{2+}$.

1.  S is correct but E is wrong
2.  S is wrong but E is correct
3.  Both S and E are correct and E is correct explanation of S
4.  Both S and E are correct but E is not correct explanation of S

Hydrogen can form compounds with all other elements

Hydrogen is much lighter element than the alkali metals or the halogens

The IE of hydrogen is too high for group of alkali metals but too low for halogen group

None of these

sodium contains only one electron in outermost shell

first ionisation potential is small and the difference in first and second ionisation potential is very large

radius of Na⁺ is much smaller than of Na⁺

none of the above

Lithium is the strongest reducing agent

Density of potassium is more than sodium

Cs is used in devising photoelectric cells.

All alkali metals give blue solution in liquid ammonia

Rb⁺

Na⁺

K⁺

Li⁺

I.P.

EN

Atomic radius

Hydration energy of univalent ion

Basic strength of oxides                                 ${\mathrm{Cs}}_2\mathrm{O}<{\mathrm{Rb}}_2\mathrm{O}<{\mathrm{K}}_2\mathrm{O}<{\mathrm{Na}}_2\mathrm{O}<{\mathrm{LiO}}_2$

Stability of peroxides                                      ${\mathrm{Na}}_2\mathrm{O} <{\mathrm{K}}_2{\mathrm{O}}_2<{\mathrm{Rb}}_2{\mathrm{O}}_2<{\mathrm{Cs}}_2{\mathrm{O}}_2$

Stability of bicarbonate                                   ${\mathrm{LiHCO}}_3<{\mathrm{NaHCO}}_3<{\mathrm{KHCO}}_3<{\mathrm{RbHCO}}_3<\mathrm{Cs} {\mathrm{HCO}}_3$

Melting Point                                                  $\mathrm{NaF}<\mathrm{NaCl}<\mathrm{NaBr}<\mathrm{Nal}$

(A) 1 and 4                                           

(B) 1 and 3

(C) 1 and 2                                           

(D) 2 and 3

The solubility, thermal stability, and the basic character of the hydroxides of alkaline earth

      metals increases from $\mathrm{Mg}{\left(\mathrm{OH}\right)}_2 \mathrm{to} \mathrm{Ba}{\left(\mathrm{OH}\right)}_2.$

The dehydration of hydrated chlorides, bromides, bromides and iodides of Ca, Sr and Ba can be

      achieved on heating.

The chlorides of both beryllium and aluminium are soluble in organic solvents and are strong

      Lewis acids.

(A) (1) and (2) only                                     

(B) (1) and (3) only

(C) (1), (2) and (3)                                     

none