Advertisements
Advertisements
Question
The +1 oxidation state in group 13 and +2 oxidation state in group 14 becomes more and more stable with increasing atomic number. Explain.
Solution
In group 13 and 14, as we move down the group, the tendency of s-electrons of the valence shell to participate in bond formation decreases. This is due to ineffective shielding of s-electrons of the valence shell by the intervening d- and f-electrons. This is called inert pair effect.
Due to this, s-electrons of the valence shell of group 13 and 14 are unable to participate in bonding. Hence, +1 and +2 oxidation states, in group 13 and 14 respectively, become -more stable with increasing atomic number.
APPEARS IN
RELATED QUESTIONS
Discuss the pattern of variation in the oxidation states of C to Pb.
Explain the difference in properties of diamond and graphite on the basis of their structures.
Explain why is there a phenomenal decrease in ionisation enthalpy from carbon to silicon?
Classify the following oxide as neutral, acidic, basic or amphoteric:
B2O3
Classify the following oxide as neutral, acidic, basic or amphoteric:
SiO2
Classify the following oxide as neutral, acidic, basic or amphoteric:
Tl2O3
Write suitable chemical equations to show the nature of the following oxide.
PbO2
The reason for small radius of Ga compared to Al is:
(i) poor screening effect of d and f orbitals.
(ii) increase in nuclear charge.
(iii) presence of higher orbitals.
(iv) higher atomic number.
The linear shape of CO2 is due to:
(i) sp3 hybridisation of carbon.
(ii) sp hybridisation of carbon.
(iii) pπ – pπ bonding between carbon and oxygen.
(iv) sp2 hybridisation of carbon.
Explain the following:
Silicon forms \[\ce{SiF^{2-}6}\] ion whereas corresponding fluoro compound of carbon is not known.
