Advertisements
Advertisements
Question
Discuss the pattern of variation in the oxidation states of B to Tl.
Advertisements
Solution 1
The electric configuration of group 13 elements is ns2 np1. Therefore, the most common oxidation state exhibited by them should be +3. However, it is only boron and aluminum which practically show the +3 oxidation state. The remaining elements, i.e., Ga, In, Tl, show both the +1 and +3 oxidation states. On moving down the group, the +1 state becomes more stable. For example, Tl (+1) is more stable than Tl (+3). This is because of the inert pair effect. The two electrons present in the s-shell are strongly attracted by the nucleus and do not participate in bonding. This inert pair effect becomes more and more prominent on moving down the group. Hence, Ga (+1) is unstable, In (+1) is fairly stable, and Tl (+1) is very stable
| Group 13 element | Oxidation state |
| B | +3 |
| Al | +3 |
| Ga, In, Tl | +1, +3 |
The stability of the +3 oxidation state decreases on moving down the group.
Solution 2
Common oxidation states are +1 and +3. The stability of +3 oxidation state decreases from B to Tl. +1 oxidation state increases from B to Tl.
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.
Elements of group 14 ________.
Rationalise the given statement and give a chemical reaction:
Lead is known not to form an iodide, PbI4.
Classify the following oxide as neutral, acidic, basic or amphoteric:
PbO2
Classify the following oxide as neutral, acidic, basic or amphoteric:
Tl2O3
Write suitable chemical equations to show the nature of the following oxide.
CO2
Write suitable chemical equations to show the nature of the following oxide.
Al2O3
Which of the following is a Lewis acid?
Catenation i.e., linking of similar atoms depends on size and electronic configuration of atoms. The tendency of catenation in Group 14 elements follows the order:
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.
Explain the following:
Silicon forms \[\ce{SiF^{2-}6}\] ion whereas corresponding fluoro compound of carbon is not known.
The +1 oxidation state in group 13 and +2 oxidation state in group 14 becomes more and more stable with increasing atomic number. Explain.
Carbon and silicon both belong to the group 14, but inspite of the stoichiometric similarity, the dioxides, (i.e., carbon dioxide and silicon dioxide), differ in their structures. Comment.
Explain the following:
Carbon shows catenation property but lead does not.
Explain the following:
BF3 does not hydrolyse.
Explain the following:
Why does the element silicon, not form a graphite like structure whereas carbon does.
The principal ore of lead is ______.
\[\ce{SiCl4 ->[H2O] (A) ->[\Delta] (B) ->[Na2CO3][heat] (C)}\]. The Compound C is ______.
