Advertisements
Advertisements
Question
Match the species given in Column I with the properties mentioned in Column II.
| Column I | Column II |
| (i) \[\ce{BF^{-}4}\] | (a) Oxidation state of central atom is +4 |
| (ii) AICI3 | (b) Strong oxidising agent |
| (iii) SnO | (c) Lewis acid |
| (iv) PbO2 | (d) Can be further oxidised |
| (e) Tetrahedral shape |
Solution
| Column I | Column II |
| (i) \[\ce{BF^{-}4}\] | (e) Tetrahedral shape |
| (ii) AICI3 | (c) Lewis acid |
| (iii) SnO | (d) Can be further oxidised |
| (iv) PbO2 | (b) Strong oxidising agent |
Explanation:
(i) \[\ce{BF^{-}4}\]: Tetrahedral shape, sp3 hybridisation, regular geometry.
(ii) AlCl3: Octet of Al not complete, acts as Lewis acid.
(iii) SnO: Sn2+ can show +4 oxidation state.
(iv) PbO2: Due to inert pair effect, Pb4+ is less stable than Pb2+ and hence acts as strong oxidising agent.
APPEARS IN
RELATED QUESTIONS
How can you explain higher stability of BCl3 as compared to TlCl3?
What happens when BF3 is reacted with ammonia?
What do you understand by inert pair effect?
Write a balanced equation for Al + NaOH → ?
Which of the following oxides is acidic in nature?
When BCl3 is treated with water, it hydrolyses and forms [B[OH]4]– only whereas AlCl3 in acidified aqueous solution forms [Al(H2O)6]3+ ion. Explain what is the hybridisation of boron and aluminium in these species?
Explain the following:
Electron gain enthalpy of chlorine is more negative as compared to fluorine.
Match the species given in Column I with the hybridisation given in Column II.
| Column I | Column II |
| (i) Boron in [B(OH)4]– | (a) sp2 |
| (ii) Aluminium in [Al(H2O)6]3+ | (b) sp3 |
| (iii) Boron in B2H6 | (c) sp3d2 |
| (iv) Carbon in Buckminsterfullerene | |
| (v) Silicon in \[\ce{SiO^{4-}4}\] | |
| (vi) Germanium in [GeCl6]2– |
Describe the general trends in the following properties of the elements in Groups 13 and 14.
Nature of halides
Three pairs of compounds are given below. Identify that compound in each of the pairs which has group 13 element in more stable oxidation state. Give reason for your choice. State the nature of bonding also.
AlCl3 , AlCl
