Chapter 11 The P-Block Elements

Question 1. The element which exists in liquid state for a wide range of temperature and can be used for measuring high temperature is

(i) B

(ii) Al

(iii) Ga

(iv) In

Question 2. Which of the following is a Lewis acid ?

(i) $AlCl_3$

(ii) $MgCl_2$

(iii) $CaCl_2$

(iv) $BaCl_2$

Question 3. The geometry of a complex species can be understood from the knowledge of type of hybridisation of orbitals of central atom. The hybridisation of orbitals of central atom in $[Be(OH)_4]^–$ and the geometry of the complex are respectively

(i) $sp^3$, tetrahedral

(ii) $sp^3$, square planar

(iii) $sp^3d^2$, octahedral

(iv) $dsp^2$, square planar

Question 4. Which of the following oxides is acidic in nature?

(i) $B_2O_3$

(ii) $Al_2O_3$

(iii) $Ga_2O_3$

(iv) $In_2O_3$

Question 5. The exhibition of highest co-ordination number depends on the availability of vacant orbitals in the central atom. Which of the following elements is not likely to act as central atom in $MF_6^{3–}$?

(i) B

(ii) Al

(iii) Ga

(iv) In

Question 6. Boric acid is an acid because its molecule

(i) contains replaceable $H^+$ ion

(ii) gives up a proton

(iii) accepts $OH^–$ from water releasing proton

(iv) combines with proton from water molecule

Question 7. 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:

(i) C > Si > Ge > Sn

(ii) C >> Si > Ge $\approx$ Sn

(iii) Si > C > Sn > Ge

(iv) Ge > Sn > Si > C

Question 8. Silicon has a strong tendency to form polymers like silicones. The chain length of silicone polymer can be controlled by adding

(i) $MeSiCl_3$

(ii) $Me_2SiCl_2$

(iii) $Me_3SiCl$

(iv) $Me_4Si$

Question 9. Ionisation enthalpy ($\Delta_i H_1 \text{ kJ mol}^{–1}$) for the elements of Group 13 follows the order.

(i) B > Al > Ga > In > Tl

(ii) B < Al < Ga < In < Tl

(iii) B < Al > Ga < In > Tl

(iv) B > Al < Ga > In < Tl

Question 10. In the structure of diborane

(i) All hydrogen atoms lie in one plane and boron atoms lie in a plane perpendicular to this plane.

(ii) 2 boron atoms and 4 terminal hydrogen atoms lie in the same plane and 2 bridging hydrogen atoms lie in the perpendicular plane.

(iii) 4 bridging hydrogen atoms and boron atoms lie in one plane and two terminal hydrogen atoms lie in a plane perpendicular to this plane.

(iv) All the atoms are in the same plane.

Question 11. A compound X, of boron reacts with $NH_3$ on heating to give another compound Y which is called inorganic benzene. The compound X can be prepared by treating $BF_3$ with Lithium aluminium hydride. The compounds X and Y are represented by the formulas.

(i) $B_2H_6, B_3N_3H_6$

(ii) $B_2O_3, B_3N_3H_6$

(iii) $BF_3, B_3N_3H_6$

(iv) $B_3N_3H_6, B_2H_6$

Question 12. Quartz is extensively used as a piezoelectric material, it contains ___________.

(i) Pb

(ii) Si

(iii) Ti

(iv) Sn

Question 13. The most commonly used reducing agent is

(i) $AlCl_3$

(ii) $PbCl_2$

(iii) $SnCl_4$

(iv) $SnCl_2$

Question 14. Dry ice is

(i) Solid $NH_3$

(ii) Solid $SO_2$

(iii) Solid $CO_2$

(iv) Solid $N_2$

Question 15. Cement, the important building material is a mixture of oxides of several elements. Besides calcium, iron and sulphur, oxides of elements of which of the group(s) are present in the mixture?

(i) group 2

(ii) groups 2, 13 and 14

(iii) groups 2 and 13

(iv) groups 2 and 14

Question 16. 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

Question 17. The linear shape of $CO_2$ is due to _________.

(i) $sp^3$ hybridisation of carbon

(ii) sp hybridisation of carbon

(iii) $p\pi - p\pi$ bonding between carbon and oxygen

(iv) $sp^2$ hybridisation of carbon

Question 18. $Me_3SiCl$ is used during polymerisation of organo silicones because

(i) the chain length of organo silicone polymers can be controlled by adding $Me_3SiCl$

(ii) $Me_3SiCl$ blocks the end terminal of silicone polymer

(iii) $Me_3SiCl$ improves the quality and yield of the polymer

(iv) $Me_3SiCl$ acts as a catalyst during polymerisation

Question 19. Which of the following statements are correct?

(i) Fullerenes have dangling bonds

(ii) Fullerenes are cage-like molecules

(iii) Graphite is thermodynamically most stable allotrope of carbon

(iv) Graphite is slippery and hard and therefore used as a dry lubricant in machines

Question 20. Which of the following statements are correct. Answer on the basis of Fig.11.1.

(i) The two birdged hydrogen atoms and the two boron atoms lie in one plane;

(ii) Out of six B–H bonds two bonds can be described in terms of 3 centre 2-electron bonds.

(iii) Out of six B-H bonds four B-H bonds can be described in terms of 3 centre 2 electron bonds;

(iv) The four terminal B-H bonds are two centre-two electron regular bonds.

Question 21. Identify the correct resonance structures of carbon dioxide from the ones given below :

(i) $O – C \equiv O$

(ii) $O = C = O$

(iii) $^–O \equiv C – O^+$

(iv) $^–O – C \equiv O^+$

Question 22. Draw the structures of $BCl_3 \cdot NH_3$ and $AlCl_3$ (dimer).

Question 23. Explain the nature of boric acid as a Lewis acid in water.

Question 24. Draw the structure of boric acid showing hydrogen bonding. Which species is present in water? What is the hybridisation of boron in this species?

Question 25. Explain why the following compounds behave as Lewis acids?

(i) $BCl_3$

(ii) $AlCl_3$

Question 26. Give reasons for the following:

(i) $CCl_4$ is immiscible in water, whereas $SiCl_4$ is easily hydrolysed.

(ii) Carbon has a strong tendency for catenation compared to silicon.

Question 27. Explain the following :

(i) $CO_2$ is a gas whereas $SiO_2$ is a solid.

(ii) Silicon forms $SiF_6^{2–}$ ion whereas corresponding fluoro compound of carbon is not known.

Question 28. The +1 oxidation state in group 13 and +2 oxidation state in group 14 becomes more and more stable with increasing atomic number. Explain.

Question 29. 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.

Question 30. If a trivalent atom replaces a few silicon atoms in three dimensional network of silicon dioxide, what would be the type of charge on overall structure?

Question 31. When $BCl_3$ is treated with water, it hydrolyses and forms $[B(OH)_4]^–$ only whereas $AlCl_3$ in acidified aqueous solution forms $[Al(H_2O)_6]^{3+}$ ion. Explain what is the hybridisation of boron and aluminium in these species?

Question 32. Aluminium dissolves in mineral acids and aqueous alkalies and thus shows amphoteric character. A piece of aluminium foil is treated with dilute hydrochloric acid or dilute sodium hydroxide solution in a test tube and on bringing a burning matchstick near the mouth of the test tube, a pop sound indicates the evolution of hydrogen gas. The same activity when performed with concentrated nitric acid, reaction doesn’t proceed. Explain the reason.

Question 33. Explain the following :

(i) Gallium has higher ionisation enthalpy than aluminium.

(ii) Boron does not exist as $B^{3+}$ ion.

(iii) Aluminium forms $[AlF_6]^{3–}$ ion but boron does not form $[BF_6]^{3–}$ ion.

(iv) $PbX_2$ is more stable than $PbX_4$.

(v) $Pb^{4+}$ acts as an oxidising agent but $Sn^{2+}$ acts as a reducing agent.

(vi) Electron gain enthalpy of chlorine is more negative as compared to fluorine.

(vii) $Tl(NO_3)_3$ acts as an oxidising agent.

(viii) Carbon shows catenation property but lead does not.

(ix) $BF_3$ does not hydrolyse.

(x) Why does the element silicon, not form a graphite like structure whereas carbon does.

Question 34. Identify the compounds A, X and Z in the following reactions :

(i) $A + 2HCl + 5H_2O \rightarrow 2NaCl + X$

$X \xrightarrow{>370K} HBO_2 \xrightarrow{>370K} Z$

Question 35. Complete the following chemical equations :

$Z + 3LiAlH_4 \rightarrow X + 3LiF + 3AlF_3$

$X + 6H_2O \rightarrow Y + 6H_2$

$X + 3O_2 \rightarrow B_2O_3 + 3H_2O$

Question 36. Match the species given in Column I with the properties mentioned in Column II.

Column I

(i) $BF_4^–$

(ii) $AlCl_3$

(iii) SnO

(iv) $PbO_2$

Column II

(a) Oxidation state of central atom is +4

(b) Strong oxidising agent

(c) Lewis acid

(d) Can be further oxidised

(e) Tetrahedral shape

Question 37. Match the species given in Column I with properties given in Column II.

Column I

(i) Diborane

(ii) Gallium

(iii) Borax

(iv) Aluminosilicate

(v) Quartz

Column II

(a) Used as a flux for soldering metals

(b) Crystalline form of silica

(c) Banana bonds

(d) Low melting, high boiling, useful for measuring high temperatures

(e) Used as catalyst in petrochemical industries

Question 38. Match the species given in Column I with the hybridisation given in Column II.

Column I

(i) Boron in $[B(OH)_4]^–$

(ii) Aluminium in $[Al(H_2O)_6]^{3+}$

(iii) Boron in $B_2H_6$

(iv) Carbon in Buckminsterfullerene

(v) Silicon in $SiO_4^{4–}$

(vi) Germanium in $[GeCl_6]^{2–}$

Column II

(a) $sp^2$

(b) $sp^3$

(c) $sp^3d^2$

Question 39. Assertion (A): If aluminium atoms replace a few silicon atoms in three dimensional network of silicon dioxide, the overall structure acquires a negative charge.

Reason (R) : Aluminium is trivalent while silicon is tetravalent.

(i) Both A and R are correct and R is the correct explanation of A.

(ii) Both A and R are correct but R is not the correct explanation of A.

(iii) Both A and R are not correct

(iv) A is not correct but R is correct.

Question 40. Assertion (A): Silicons are water repelling in nature.

Reason (R) : Silicons are organosilicon polymers, which have $(–R_2SiO–)$ as repeating unit.

(i) A and R both are correct and R is the correct explanation of A.

(ii) Both A and R are correct but R is not the correct explanation of A.

(iii) A and R both are not true.

(iv) A is not true but R is true.

Question 41. Describe the general trends in the following properties of the elements in Groups 13 and 14.

(i) Atomic size

(ii) Ionisation enthalpy

(iii) Metallic character

(iv) Oxidation states

(v) Nature of halides

Question 42. Account for the following observations:

(i) $AlCl_3$ is a Lewis acid

(ii) Though fluorine is more electronegative than chlorine yet $BF_3$ is a weaker Lewis acid than $BCl_3$

(iii) $PbO_2$ is a stronger oxidising agent than $SnO_2$

(iv) The +1 oxidation state of thallium is more stable than its +3 state.

Question 43. When aqueous solution of borax is acidified with hydrochloric acid, a white crystalline solid is formed which is soapy to touch. Is this solid acidic or basic in nature? Explain.

Question 44. 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.

(i) $TlCl_3, TlCl$

(ii) $AlCl_3, AlCl$

(iii) $InCl_3, InCl$

Question 45. $BCl_3$ exists as monomer whereas $AlCl_3$ is dimerised through halogen bridging. Give reason. Explain the structure of the dimer of $AlCl_3$ also.

Question 46. Boron fluoride exists as $BF_3$ but boron hydride doesn’t exist as $BH_3$. Give reason. In which form does it exist? Explain its structure.

Question 47.

(i) What are silicones? State the uses of silicones.

(ii) What are boranes? Give chemical equation for the preparation of diborane.

Question 48. A compound (A) of boron reacts with $NMe_3$ to give an adduct (B) which on hydrolysis gives a compound (C) and hydrogen gas. Compound (C) is an acid. Identify the compounds A, B and C. Give the reactions involved.

Question 49. A nonmetallic element of group 13, used in making bullet proof vests is extremely hard solid of black colour. It can exist in many allotropic forms and has unusually high melting point. Its trifluoride acts as Lewis acid towards ammonia. The element exihibits maximum covalency of four. Identify the element and write the reaction of its trifluoride with ammonia. Explain why does the trifluoride act as a Lewis acid.

Question 50. A tetravalent element forms monoxide and dioxide with oxygen. When air is passed over heated element (1273 K), producer gas is obtained. Monoxide of the element is a powerful reducing agent and reduces ferric oxide to iron. Identify the element and write formulas of its monoxide and dioxide. Write chemical equations for the formation of producer gas and reduction of ferric oxide with the monoxide.