The oxidising property of ${\mathrm{H}}_2{\mathrm{O}}_2$ is best explained by assuming that two oxygen atoms in its molecule are.

(1) Bonded differently

(2) Bonded similarly

(3) Bonded covalently

(4) Bonded by hydrogen bonds

${\mathrm{H}}_2\mathrm{O}$ has higher boiling point than ${\mathrm{H}}_2\mathrm{S}$ because.

(1) ${\mathrm{H}}_2\mathrm{O}$ is a smaller molecule and hence more closely packed

(2) The bond angle in ${\mathrm{H}}_2\mathrm{O}$ is more than in ${\mathrm{H}}_2\mathrm{S}$ and hence the former molecules are more tightly packed

(3) Of intermolecular hydrogen bonding in liquid ${\mathrm{H}}_2\mathrm{O}$

(4) The latent heat of vaporisation is higher for ${\mathrm{H}}_2\mathrm{O}$ than for ${\mathrm{H}}_2\mathrm{S}$

On partial hydrolysis of one mole of peroxodisulphuric acid produces

1. two moles of sulphuric acid

2. two moles of peroxomonosulphuric acid

3. one mole of sulphuric acid and one mole of peroxomonosulphuric acid

4. one mole of sulphuric acid, one mole of peroxomonosulphuric acid and one mole of hydrogen peroxide.

The maximum possible number of hydrogen bonds a water molecule can form is –

(1) 2                                         

(2) 4

(3) 3                                         

(4) 1

${\mathrm{H}}_2{\mathrm{O}}_2$ acts as antiseptic due to its –

(1) Reducing property                           

(2) Oxidising property

(3) Bleaching property                           

(4) Acidic property

A compound that has both polar and non-polar bonds is  –

1. ${\mathrm{NH}}_4\mathrm{Cl}$                                    

2. $\mathrm{HCN}$

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

4. ${\mathrm{CH}}_4$

In which of the following reactions is ${\mathrm{H}}_2{\mathrm{O}}_2$ acting as an acid.

(A) $2{\mathrm{KMnO}}_4+3{\mathrm{H}}_2{\mathrm{SO}}_4+5{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{K}}_2{\mathrm{SO}}_4+{\mathrm{MnO}}_4+2{\mathrm{MnSO}}_4+8{\mathrm{H}}_2\mathrm{O}+5{\mathrm{O}}_2$

(B) $2{\mathrm{K}}_3\mathrm{Fe}{\left(\mathrm{CN}\right)}_6+2\mathrm{KOH}+{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{K}}_4\mathrm{Fe}{\left(\mathrm{CN}\right)}_6+2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

(C) ${\mathrm{O}}_3+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{H}}_2\mathrm{O}+2{\mathrm{O}}_2$

(D) $\mathrm{Ba} {\left(\mathrm{OH}\right)}_2+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{BaO}}_2+{\mathrm{H}}_2\mathrm{O}$

Exhausted permutit does not contain ............ ion –

(A) ${\mathrm{Na}}^{+}$                                      

(B) ${\mathrm{Mg}}^{2+}$

(C) ${\mathrm{Al}}^{3+}$                                    

(D) ${\mathrm{Si}}^{4+}$

Which of the following metal cannot absorb hydrogen –

(1) Pd                                     

(2) Al

(3) Ni                                     

(4) Co

The best explanation for not placing hydrogen with the group of alkali metals or halogens is.

1. Hydrogen can form compounds with all other elements

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

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

4. None of these