In gaseous phase, water molecule has a bent form.

Bond angle of water is $109.0°$

 Hydrogen peroxide has a non-planar structure.

 The dihedral angle of H₂O₂ in gas phase is 111.5° 

 $\mathrm{PbS}\left(\mathrm{s}\right) +{\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{aq}\right) \to {\mathrm{PbSO}}_4\left(\mathrm{s}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

 $\mathrm{CaO}\left(\mathrm{s}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right) \to \mathrm{Ca}{\left(\mathrm{OH}\right)}_2 \left(\mathrm{aq}\right)$

 ${\mathrm{AlCl}}_3\left(\mathrm{g}\right) + 3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) \to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right) + 6\mathrm{HCl}\left(\mathrm{aq}\right)$

 ${\mathrm{Ca}}_3{\mathrm{N}}_2\left(\mathrm{s}\right) + 6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) \to 3\mathrm{Ca}{\left(\mathrm{OH}\right)}_2\left(\mathrm{aq}\right) + 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

$$ {}^{}{}^{}$$ {}^{}\mathrm{O has\; a\; bent\; structure\; .}$$

NaH > H₂O < MgH₂

_{${\mathrm{H}}_2\mathrm{O}$ > ${\mathrm{MgH}}_2$> NaH}

_{${\mathrm{H}}_2\mathrm{O}$< ${\mathrm{MgH}}_2$ < NaH}

_{${\mathrm{H}}_2\mathrm{O}$ $\simeq$ ${\mathrm{MgH}}_2$ < NaH}

  Ionisation enthalpy of hydrogen resembles that of alkali metals

  Its reactivity is similar to halogens

  It resembles both alkali metals and halogens

  Loss of an electron from 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

(a), (b) and (c)

(b) and (c)

(a) and (c)

(a) and (b)

 $O^{-2}$

 $O{H}^{-}$

 $O_2^{-}$

 $O_2$

Protium, Deuterium, Tritium ; 3:2:3

Protium, Deuterium, Tritium ; 1:2:3

Protium, Deuterium, Tritium ; 2:2:3

Protium, Deuterium, Tritium ; 3:2:1

Due to high ionization enthalpy

Due to low ionization enthalpy

Due to high electron gain enthalpy

Due to low electron gain enthalpy

It cools down the temperature.

None of the above

It lowers the availability of ions available in the process for the conduction of electricity.

It makes the ions available in the process for conduction of electricity.

Hydrogen has a low tendency to form ${\mathrm{H}}^{+}$ions.

It forms diatomic molecules ($H_2$), and a large number of covalent hydrides.

Hydrogen does not possess metallic characteristics.

All of the above.

Lewis acid.

Lewis base.

Both 1 and 2

None of the above

Hydrogen-deficient compounds formed by the reaction of a hydrogen atom with d-block and f-block elements.

Hydrogen-deficient compounds formed by the reaction of dihydrogen with d-block and f-block elements.

Electron-deficient compounds formed by the reaction of dihydrogen with d-block and f-block elements.

Hydrogen-deficient compounds formed by the reaction of dihydrogen with s-block and p-block elements.

Metallic hydrides are oxygen-rich.

Metallic hydrides are oxygen-deficient.

Metallic hydrides are hydrogen-rich.

Metallic hydrides are hydrogen-deficient.

Atomic hydrogen converts into molecular hydrogen and generates a large amount of energy

 Atomic hydrogen converts into molecular hydrogen and generates a low amount of energy

Molecular hydrogen converts into atomic hydrogen and generates a large amount of energy

Molecular hydrogen converts into atomic hydrogen and generates a low amount of energy

HF > ${\mathrm{H}}_2\mathrm{O}$ > ${\mathrm{NH}}_3$

 ${\mathrm{H}}_2\mathrm{O}$ > HF > ${\mathrm{NH}}_3$

HF > ${\mathrm{NH}}_3$ > ${\mathrm{H}}_2\mathrm{O}$

 ${\mathrm{NH}}_3$ > HF > ${\mathrm{H}}_2\mathrm{O}$

 ${\mathrm{CO}}_2$ has high lattice energy.

 ${\mathrm{CO}}_2$ will be effective in isolating the burning surface from dihydrogen and dioxygen.

 ${\mathrm{CO}}_2$ is lighter than dioxygen.

 ${\mathrm{CO}}_2$ is lighter than dihydrogen.

Physical reaction in which two water molecules react to produce a hydroxide ion (OH^–) and a hydronium ion (${\mathrm{H}}_3{\mathrm{O}}^{+}$).

Chemical reaction in which five water molecules react to produce a hydroxide ion (OH^–) and a hydronium ion (${\mathrm{H}}_3{\mathrm{O}}^{+}$).

Chemical reaction in which two water molecules react to produce a hydroxide ion (OH^–) and a hydronium ion (${\mathrm{H}}_3{\mathrm{O}}^{+}$).

Chemical reaction in which two water molecules react to produce three hydroxide ions (OH^–)

O is reduced from 0 to -1 oxidation state, whereas F is oxidized from –2 to 0

F is reduced from 0  to -1 oxidation state, whereas O is oxidized from –2 to 0

F is reduced from 0 to –2 oxidation state, whereas O is oxidized from – 2 to -1

O is reduced from 0 to –2 oxidation state, whereas F is oxidized from –3 to 0

Each hydrogen atom is surrounded tetrahedrally by four other oxygen atoms at a distance of 540 pm.

Each hydrogen atom is surrounded tetrahedrally by four other oxygen atoms at a distance of 276 pm.

Each oxygen atom is surrounded tetrahedrally by four other oxygen atoms at a distance of 276 pm.

Each oxygen atom is surrounded tetrahedrally by four other oxygen atoms at a distance of 540 pm.

Increasing the lattice energy.

Physical separation.

Lowering the activation energy.

Exchange of cations and anions.

Reaction with ${\mathrm{H}}_2\mathrm{S}$

Reaction with ${\mathrm{NH}}_3$

Reaction with NaOH

All of the above

Passing water successively through an anion exchange (in the K⁺ form) and cation exchange (in the Mn^- form) resin

Passing water successively through a cation exchange (in the H⁺ form) and an anion exchange (in the OH^- form) resin

Passing water successively through an anion exchange (in the O⁺ form) and cation exchange (in the OH^- form) resin

Passing water successively through a cation exchange (in the OH^- form) and an anion exchange (in the H⁺ form) resin

Demineralised water contains all insoluble minerals. 

Demineralised water is free of all soluble minerals. 

Demineralised water contains soluble minerals. 

Demineralised water contains soluble anion only.