11.2

What are the structures of Group 14 Tetrachlorides?

• Simple Molecules

• Giant Covalent Molecules

• Simple Covalent Molecules

The tetrachlorides exist as simple covalent molecules

that are held together by .

• Strong van der Waals forces

• Weak van der Waals forces

• Covalent bonds

Going down Group 14, thermal stability of the tetrachlorides .

(a)  

Tetrachlorometehane, CCl₄ does not undergo hydrolysis because
(Choose the most suitable answer)

• carbon atom does not have d orbitals to receive lone pairs from oxygen atoms in water molecules

• carbon atom does not have empty d orbitals

These tetrachlorides are stable at high temperatures.

• SiCl₄, SnCl₄, PbCl₄

• SiCl₄, CCl₄, GeCl₄

• SnCl₄, CCl₄, GeCl₄

• SiCl₄, PbCl₄, GeCl₄

All the tetrachlorides except for CCl₄,

are readily hydrolysed by water to liberate of hydrogen chloride.

• Yellow Fumes

• Brown Fumes

• White Fumes

• Red-Brown Fumes

SiCl₄, GeCl₄, SnCl₄, and PbCl₄ form dative bonds with water molecules because

• They do not have d orbitals

• They have partially filled orbitals

• They have empty d orbitals

Arrange the elements according to atomic size down the group.

• Si, Ge, C, Sn, Pb

• Pb, Ge, Si, C, Sn

• C, Si, Ge, Sn, Pb

• Sn, Pb, Si, Ge, C

The only tetrachloride that cannot be hydrolysed.

• SnCl₄

• GeCl₄

• SiCl₄

• CCl₄

Going down group 14:

• Both melting point and electrical conductivity increases.

• Both melting point and electrical conductivity decreases.

• Melthing point decreases but electrical conductivity increases.

• Melting point increases but electrical conductivity decreases.