Give Reasons.
1. P pie - P pie bonding is absent in Si02
2. BH3 dimerises but BCl3 doesnt
3. SiCl4 can be hydrolysed but CCl4 cannot be
4. PbCl4 acts as an oxidising agent
Give Reasons.
1. P pie - P pie bonding is absent in Si02
2. BH3 dimerises but BCl3 doesnt
3. SiCl4 can be hydrolysed but CCl4 cannot be
4. PbCl4 acts as an oxidising agent
1) p pi -p pi bonding is absent in SiO2 because silicon has vacant d orbital and it has to use its d orbital for accepting p electrons of the oxygen atoms and therefore forms d pi-p pi bonding instead of p pi- p pi bonding.
2) BH3 dimerizes because of the small size of hydrogen atom so boron can easily accommodates six hydrogen atoms around us as compared to the six bigger chlorine atoms.
3) SiCl4 can be hydrolyzed because of the presence of vacant d orbitals in the Si so it can increase its coordination number beyond 4.
4) PbCl4 acts as a oxidizing agent because after reduction it comes to the lower oxidation state of +2 from +4 oxidation state, which is more stable because of the inert pair effect.
1) p pi -p pi bonding is absent in SiO2 because silicon has vacant d orbital and it has to use its d orbital for accepting p electrons of the oxygen atoms and therefore forms d pi-p pi bonding instead of p pi- p pi bonding.
2) BH3 dimerizes because of the small size of hydrogen atom so boron can easily accommodates six hydrogen atoms around us as compared to the six bigger chlorine atoms.
3) SiCl4 can be hydrolyzed because of the presence of vacant d orbitals in the Si so it can increase its coordination number beyond 4.
4) PbCl4 acts as a oxidizing agent because after reduction it comes to the lower oxidation state of +2 from +4 oxidation state, which is more stable because of the inert pair effect.
