Hydrated aluminium chloride is an ionic compound and soluble in water giving -

1. Al³⁺ and Cl^- ions

2. ${\left[\mathrm{Al}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+}$ and Cl^- ions

3. ${\left[{\mathrm{AlCl}}_2{\left({\mathrm{H}}_2\mathrm{O}\right)}_4\right]}^{+}$ and ${\left[{\mathrm{AlCl}}_4{\left({\mathrm{H}}_2\mathrm{O}\right)}_2\right]}^{-}$  ions

4. None of the above

${\mathrm{Al}}_4{\mathrm{C}}_3$ is an ionic carbide. It is also known as :

1. Acetylide

2. Methanide

3. Allyide

4. Alloy

Anhydrous aluminium chloride fumes in moist air owing to the formation of :

1. gaseous aluminium chloride

2. chlorine

3. chlorine dioxide

4. hydrogen chloride

The silicate anion in the mineral kinolte is a chain of three SiO₄ tetrahedra, that share corners with adjacent tetrahedra. The charge of the silicate anion is :

1. -4

2. -8

3. -6

4. -2

A compound that is sparingly soluble in cold water and fairly soluble in hot water is-

1. $\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2$

2. ${\mathrm{PbCl}}_2$

3. ${\mathrm{PbSO}}_4$

4. ${\mathrm{PbCrO}}_4$

Concentrated nitric acid reacts with iodine to give :

1. HOI

2. HI

3. HOIO₂

4. HOIO₃

The dipole moment of ${\mathrm{H}}_2{\mathrm{O}}_2$ is more than that of ${\mathrm{H}}_2\mathrm{O}$ but ${\mathrm{H}}_2{\mathrm{O}}_2$ is not a good solvent because :

1. It has a very high dielectric constant so that ionic compounds cannot be dissolved in it.

2. It does not act as an oxidising agent

3. It acts as a reducing agent

4. It dissociates easily and acts as an oxidising agent in chemical reactions 

The dissolution of $\mathrm{Al}{\left(\mathrm{OH}\right)}_3$ by a solution of NaOH results in the formation of :

1. ${\left[\mathrm{Al}{\left({\mathrm{H}}_2\mathrm{O}\right)}_4{\left(\mathrm{OH}\right)}_2\right]}^{+}$

2. $\left[\mathrm{Al}{\left({\mathrm{H}}_2\mathrm{O}\right)}_3{\left(\mathrm{OH}\right)}_3\right]$

3. ${\left[\mathrm{Al}{\left({\mathrm{H}}_2\mathrm{O}\right)}_2{\left(\mathrm{OH}\right)}_4\right]}^{-}$

4. $\left[\mathrm{Al}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6{\left(\mathrm{OH}\right)}_3\right]$

Sn crumbles to a powder in very cold weather, due to –

1. Expansion of the crystal lattice

2. Formation of SnO at low temperature

3. The conversion of Sn to powdery meta stannic acid

4. The transition from white tin to grey form, that is amorphous

The incorrect statement among the following is:

1.  SnF₄ is ionic in nature.

2.  PbF₄ is covalent in nature.

3.  SiCl₄ is easily hydrolysed.

4.  GeX₄ (X = F, Cl, Br, I) is more stable than GeX₂