Why does H⁺ ion always get associated with other atoms or molecules?

1.	Ionization enthalpy of hydrogen resembles that of alkali metals.
2.	Its reactivity is similar to halogens.
3.	It resembles both alkali metals and halogens.
4.	Loss of an electron from a hydrogen atom results in a nucleus of very small size as compared to other atoms or ions. Due to small size, it cannot exist free.

Metal hydrides are ionic, covalent or molecular in nature. Among LiH, NaH, KH, RbH, CsH, the correct order of increasing ionic character is

1.  LiH > NaH > CsH > KH>RbH

2.  LiH < NaH < KH < RbH < CsH

3.  RbH > CsH > NaH > KH > LiH

4.  NaH > CsH > RbH > LiH > KH

Which of the following hydrides is electron-precise hydride?

1.  ${\mathrm{B}}_2{\mathrm{H}}_6$

2.  ${\mathrm{NH}}_3$

3.  ${\mathrm{H}}_2\mathrm{O}$

4.  ${\mathrm{CH}}_4$

Radioactive elements emit α, β, and γ rays and are characterized by their half-lives. The radioactive isotope of hydrogen is:

1. Protium

2. Deuterium

3. Tritium

4. Hydronium

Consider the reactions

$\left(\mathrm{A}\right) H_2{O}_2 + 2HI \to {\mathrm{I}}_2+2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{B}\right) \mathrm{HOCl} + {\mathrm{H}}_2{\mathrm{O}}_2 \to {\mathrm{H}}_3{\mathrm{O}}^{+}{\mathrm{Cl}}^{-} + {\mathrm{O}}_2$

Which of the following statements is correct about ${\mathrm{H}}_2{\mathrm{O}}_2$ with reference to these reactions? Hydrogen perioxide is ________.

1.  An oxidising agent in both (A) and (B)

2.  An oxidising agent in (A) and reducing agent in (B)

3.  A reducing agent in (A) and oxidizing agent in (B)

4.  A reducing agent in both (A) and (B)

The oxide that gives ${\mathrm{H}}_2{\mathrm{O}}_2$ on treatment with dilute ${\mathrm{H}}_2{\mathrm{SO}}_4$ is ____

1.  ${\mathrm{PbO}}_2$

2.  ${\mathrm{BaO}}_2.8{\mathrm{H}}_2\mathrm{O}$

3.  ${\mathrm{MnO}}_2$

4.  ${\mathrm{TiO}}_2$

Which of the following equations depict the oxidising nature of ${\mathrm{H}}_2{\mathrm{O}}_2$?

1.  $2{{\mathrm{MnO}}_4}^{-} + 6{\mathrm{H}}^{+} + 5{\mathrm{H}}_2{\mathrm{O}}_2 \to 2{\mathrm{Mn}}^{2+} + 8{\mathrm{H}}_2\mathrm{O} + 5{\mathrm{O}}_2$

2.  $2{\mathrm{Fe}}^{3+} + 2{\mathrm{H}}^{+} + {\mathrm{H}}_2{\mathrm{O}}_2 \to 2{\mathrm{Fe}}^{2+} + 2{\mathrm{H}}_2\mathrm{O} + {\mathrm{O}}_2$

3.  $2{\mathrm{I}}^{-} + 2{\mathrm{H}}^{+}+ {\mathrm{H}}_2{\mathrm{O}}_2 \to {\mathrm{I}}_2+2{\mathrm{H}}_2\mathrm{O}$

4.  ${\mathrm{KIO}}_4 + {\mathrm{H}}_2{\mathrm{O}}_2 \to {\mathrm{KIO}}_3+{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

Which of the following equation depicts reducing nature of ${\mathrm{H}}_2{\mathrm{O}}_2$?

1.  $2{\left[\mathrm{Fe}{\left(\mathrm{CN}\right)}_6\right]}^{4-} + 2{\mathrm{H}}^{+}+{\mathrm{H}}_2{\mathrm{O}}_2 \to 2{\left[\mathrm{Fe}\left({\mathrm{CN}}_6\right)\right]}^{3-} + 2{\mathrm{H}}_2\mathrm{O}$

2.  ${\mathrm{I}}_2+{\mathrm{H}}_2{\mathrm{O}}_2+2{\mathrm{OH}}^{-} \to 2{\mathrm{I}}^{-}+2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

3.  ${\mathrm{Mn}}^{2+}+{\mathrm{H}}_2{\mathrm{O}}_2 \to {\mathrm{Mn}}^{4+}+2{\mathrm{OH}}^{-}$

4.  $\mathrm{PbS} + 4{\mathrm{H}}_2{\mathrm{O}}_2 \to {\mathrm{PbSO}}_4 + 4{\mathrm{H}}_2\mathrm{O}$

Hydrogen peroxide is-.

1.  An oxidising agent

2.  A reducing agent

3.  Both an oxidising and a reducing agent

4.  Neither oxidising nor reducing agent

When sodium peroxide is treated with dilute sulphuric acid, we get ______.

1.  Sodium sulphate and water

2.  Sodium sulphate and oxygen

3.  Sodium sulphate, hydrogen and oxygen

4.  Sodium sulphate and hydrogen peroxide