NCERT Class 11 Solutions States of Matter - NCERT Solutions prepared for CBSE students by the best teachers in Delhi.
Class XI Chapter 11 – The p-Block Elements Chemistry
Question 11.1: Discuss the pattern of variation in the oxidation states of
(i) B to Tl and (ii) C to Pb.
Answer (i) B to Tl
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 aluminium 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.
(ii) C to Pb
The electronic configuration of group 14 elements is ns2 np2. Therefore, the most common oxidation state exhibited by them should be +4. However, the +2 oxidation state becomes more and more common on moving down the group. C and Si mostly show the +4 state. On moving down the group, the higher oxidation state becomes less stable. This is because of the inert pair effect. Thus, although Ge, Sn, and Pb show both the +2 and + 4 states, the stability of the lower oxidation state increases and that of the higher oxidation state decreases on moving down the group.
Question 11.2: How can you explain higher stability of BCl3 as compared to TlCl3?
Answer Boron and thallium belong to group 13 of the periodic table. In this group, the +1 oxidation state becomes more stable on moving down the group. BCl3 is more stable than TlCl3 because the +3 oxidation state of B is more stable than the +3 oxidation state of Tl. In Tl, the +3 state is highly oxidising and it reverts back to the more stable +1 state.
Question 11.3: Why does boron trifluoride behave as a Lewis acid?
Answer The electric configuration of boron is ns2 np1. It has three electrons in its valence shell. Thus, it can form only three covalent bonds. This means that there are only six electrons around boron and its octet remains incomplete. When one atom of boron combines with three fluorine atoms, its octet remains incomplete. Hence, boron trifluoride remains electron-deficient and acts as a Lewis acid.
Question 11.4: Consider the compounds, BCl3 and CCl4. How will they behave with water? Justify.
Answer Being a Lewis acid, BCl3 readily undergoes hydrolysis. Boric acid is formed as a result. CCl4 completely resists hydrolysis. Carbon does not have any vacant orbital. Hence, it cannot accept electrons from water to form an intermediate. When CCl4 and water are mixed, they form separate layers.
Question 11.5: Is boric acid a protic acid? Explain.
Answer Boric acid is not a protic acid. It is a weak monobasic acid, behaving as a Lewis acid. It behaves as an acid by accepting a pair of electrons from –OH ion.
Question 11.6: Explain what happens when boric acid is heated.
Answer On heating orthoboric acid (H3BO3) at 370 K or above, it changes to metaboric acid (HBO2). On further heating, this yields boric oxide B2O3.
Question 11.7: Describe the shapes of BF3 and BH4 –. Assign the hybridisation of boron in these species.
(i) BF3 As a result of its small size and high electronegativity, boron tends to form monomeric covalent halides. These halides have a planar triangular geometry. This triangular shape is formed by the overlap of three sp2 hybridised orbitals of boron with the sp orbitals of three halogen atoms. Boron is sp2 hybridised in BF3.
(ii) BH4 – Boron-hydride ion (BH4 –) is formed by the sp3 hybridisation of boron orbitals. Therefore, it is tetrahedral in structure.
Question 11.8: Write reactions to justify amphoteric nature of aluminium.
Answer A substance is called amphoteric if it displays characteristics of both acids and bases. Aluminium dissolves in both acids and bases, showing amphoteric behaviour.
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