p-Block Elements-I: Answer the following questions

Chemistry : p-Block Elements-I

Answer the following questions:

1.        Write a short note on anamolous properties of the first element of p-block.

Anamolous properties are due to

1. Small size of the first element

2. High ionisation enthalpy and high electronegativity

3. Absence of d orbitals in their valence shell

2.     Describe briefly allotropism in p- block elements with specific reference to carbon.

Carbon exhibits the following allotropic form

(i) Graphite

(ii) Diamond

(iii) Fullerene

(iv) Carbon nanotubes

(v) Graphene

(i) Graphite

• It is More stable form, soft and conducts electricity.

• It is composed of flat two dimensional sheets of carbon atoms. Each sheet is a hexagonal and posses sp² hybridised carbon atoms. The C - C bond length is 1.41 Ǻ

• Each carbon atom forms three σ bonds and the fourth electron present in the unhybridised p orbital is free and responsible for conductivity.

• The successive carbon sheets are held together by weak van der Waals forces. The distance between two successive layers is 3.40 Ǻ.

• It is used as a lubricant.

(ii) Diamond

• Diamond is very hard.

• sp³ hybridised and bonded to four neighbouring carbon atoms by σ bonds.

• It has a tetrahedral arrangement in the entire lattice. C - C bond length is 1.54 Ǻ.

• Since all four valence electrons of carbon are involved in bonding there is no free electrons for conductivity.

• It used for sharpening hard tools, cutting glasses, making bores and rock drilling.

(iv) Fullerenes

• These allotropes are discrete molecules such as C₃₂, C₅₀, C₆₀, C₇₀, C₇₆ etc.

• These molecules have cage like structures.

• C₆₀ molecule has 20 six membered rings and 12 five membered rings.

• Each carbon atom is sp² hybridised and has a delocalised π bond giving aromatic character to these molecules. C - C bond distance is 1.44 Ǻ.

(iv) Carbon nanotubes

• It have graphite like tubes with fullerence ends.

• Nanotubes are stronger than steel and conduct electricity.

• It is applied in nanoscale electronics, catalysis, polymers and medicine.

(v) Graphene

It has a single planar sheet of sp² hybridised carbon atoms that are densely packed in a honeycomb crystal lattice.

3.     Boron does not react directly with hydrogen. Suggest one method to prepare diborane from BF3.

Boron does not react directly with hydrogen. Treatment of gaseous boron trifluoride with sodium hydride around 450 K gives diborane.

2BF₃ + 6NaH ^{__ 450 K}→ B₂H₆ + 6NaF

4.     Give the uses of Borax.

1. Identification of coloured metal ions.

2. Manufacture of optical and borosilicate glass, enamels and glazes for pottery

3. Used as a flux in metallurgy

4. Food preservatives

5.     What is catenation ? describe briefly the catenation property of carbon.

Catenation is an ability of an element to form chain of atoms.

Carbon possesses the following properties and forms a wide range of compounds with itself.

(i) The valency of element is greater than or equal to two

(ii) Element should have an ability to bond with itself

(iii) The self bond must be as strong as its bond with other elements

(iv) Kinetic inertness of catenated compound towards other molecules.

6.     Write a note on Fisher tropsch synthesis.

Carbon monoxide reacts with hydrogen at a pressure of less than 50 atm using metal catalysts at 500 - 700 K yields saturated and unsaturated hydrocarbons is known as Fisher tropsch synthesis.

nCO + (2n+l)H₂ → C_nH_(2n+2) + nH₂O

nCO + 2nH₂ → C_nH_2n + nH₂O

7.     Give the structure of CO and CO2.

8.     Give the uses of silicones.

1. Silicones are used for low temperature lubrication and in vacuum pumps, high temperature oil baths.

2. They are used for making water proofing clothes

3. They are used as insulting material in electrical motor and other appliances

4. They are mixed with paints and enamels to make them resistant towards high temperature, sunlight, dampness and chemicals.

9.     AlCl3 behaves like a lewis acid. Substantiate this statement.

AlCl₃ behaves like a Lewis acid and forms addition compounds with ammonia, phosphine and carbonylchloride.

Eg. AlCl₃.6NH₃.

10. Describe the structure of diborane.

• Two BH₂ units are linked by two bridged hydrogens with eight B - H bonds.

• Diborane has only 12 valence electrons and are not sufficient to form normal covalent bonds.

• 8 electrons used for 2c-2e bonds and the remaining four elections used for 3c-2e bond.

• The boron is sp³ hybridised. Three of the four sp³ hybridised orbitals contains single electron and the fourth orbital is empty.

• Two of the half filled hybridised orbitals of each boron overlap with the two hydrogens to form four terminal 2c-2e bonds, leaving one empty and one half filled hybridised orbitals on each boron.

• The bridging hydrogen atoms are in a plane.

• The three centre - two electron bonds, involves overlapping the half filled hybridised orbital of one boron, the empty hybridised orbital of the other boron and the half filled is orbital of hydrogen.

11. Write a short note on hydroboration.

Diborane adds on to alkenes and alkynes in ether solvent at room temperature is called hydroboration. It is highly used in synthetic organic chemistry, especially for anti Markovnikov addition.

B₂H₆ + 3RCH = CHR → 2B(CH₂CH₂R)₃ + 6H₂

12. Give one example for each of the following

(i) icosogens (ii) tetragen (iii) prictogen (iv) chalcogen

(i) Icosogens (ii) Tetragen (iii) Pnictogen (iv) Chalcogen

(i) Icosogens - Boron

(ii) Tetragen - Carbon

(iii) Pnictogen - Nitrogen

(iv) Chalcogen - Oxygen

13. Write a note on metallic nature of p-block elements.

• The tendency of an element to form a cation by loosing electrons is known as metallic character. On descending a group the ionisation energy decreases and hence the metallic character increases.

• The elements present in lower left part are metals while the elements in the upper right part are non metals.

• Due to higher ionisation energy all the elements of group 17 and 18 are non metals.

• Higher nuclear charge is responsible for nonmetallic character of boron.

14. Complete the following reactions

a. B ( OH)3 +NH3 →

b. Na2B4O7 + H2SO4 + H2O  →

c. B2H6 + 2NaOH + 2H2O  →

d. B2H6 + CH3OH  →

e. BF3 + 9 H2O  →

f . HCOOH + H2SO4  →

g . SiCl4 + NH3  →

h. SiCl4 + C2H5OH →

i. B + NaOH  →

j. H2B4O7 Red hot→

Answer:

a) B(OH)₃ + NH₃ ^___Δ→ BN+3H₂O

b) Na₂B₄O₇ + H₂SO₄ + 5H₂O → 4 H₃BO₃ + Na₂SO₄

c) B₂H₆ + 2NaOH + 2H₂O → 2NaBO₂ + 6H₂

d) B₂H₆ + 6CH₃OH → 2B(OCH₃)₃ + 6H₂

e) BF₃ + H₂O → F₃B ← OH₂

f) HCOOH + H₂SO₄ → CO + H₂O. H₂SO₄

g) 2SiCl₄ + NH₃ ^___33Ok__Ether^__→ Cl₃SiNHSiCl₃ + 2HCl

h) SiCl₄ + 4C₂H₅OH → Si(OC₂H₅)₄ + 4HCl

i) 2B + 6NaOH → 2Na₃BO₃ + 3H₂

j) H₂B₄O₇ ^{___Red box} → 2B₂O₃ + H₂O

15. How will you identify borate radical?

Trialkylborate is formed when borate salt is heated with ethyl alcohol in presence of conc.sulphuric acid. The vapour of trialkylborate burns with a green edged flame and this reaction is used to identify the presence of borate.

H₃BO₃ + 3C₂H₅OH ^{___Conc. H2SO4__}→ B(OC₂H₅)₃ + 3H₂O

16. Write a note on zeolites.

• Zeolites are three-dimensional crystalline solids containing aluminium, silicon, and oxygen in their regular three dimensional framework. They are hydrated sodium alumino silicates with general formula Na₂O.(Al₂O₃).x(SiO₂).yH₂O

(x=2 to 10; y=2 to 6)

• Zeolites have porous structure in which the monovalent sodium ions and water molecules are loosely held. The Si and Al atoms are tetrahedrally coordinated with each other through shared oxygen atoms.

• Zeolites have a three dimensional crystalline structure consisting of a network of interconnected tunnels and cages. Water molecules moves freely in and out of these pores but the zeolite framework remains rigid.

• The pore /channel sizes are nearly uniform, allowing the crystal to act as a molecular sieve.

17. How will you convert boric acid to boron nitride?

Fusion of urea with boric acid in ammonia atmosphere at 800 −1200 K gives boron nitride

B(OH)₃ [Boric acid] + NH₃ ^____Δ__→ BN [Boron nitride] + 3H₂O

18. A hydride of 2nd period alkali metal (A) on reaction with compound of Boron (B) to give a reducing agent (C). identify A , B and C.

Alkali metal present in second period is Li and its hydride is LiH(A). LiH(A) reacts with boron compound B₂H₆(B) gives a reducing agent LiBH₄ (C).

2LiH + B₂H₆  ^___Ether_→ 2LiBH₄

   (A)    (B)                                     (C)

A : LiH - Lithium hydride

B : B₂H₆ - Diborane

C : LiBH₄ - Lithium borohydride

19. A double salt which contains fourth period alkali metal (A) on heating at 500K gives (B). aqueous solution of (B) gives white precipitate with BaCl2 and gives a red colour compound with alizarin. Identify A and B.

Alkali metal present in fourth period is potassium. Its double salt is potash alum.

K₂SO₄. Al₂(SO₄)₃. 24H₂O

A is K₂SO₄. Al₂(SO₄)₃. 24H₂O

A on heating at 500 K gives burnt alum.

K₂SO₄ Al₂(SO₄)₃. 24 H₂O ^{___500 K_}→ K₂SO₄.Al₂(SO₄)₃ + 24 H₂O

      Potash Alum (A)                                        Burnt Alum (B)

In aqueous solution B ionizes and gives sulphate ion. While adding BaCl₂, sulphate ion reacts with BaCl₂ gives BaSO₄ precipitate which is white colour. B also gives red colour with alizarin due to the presence of Al³⁺.

A : K₂SO₄. Al₂(SO₄)₃. 24 H₂O - Potash alum

B : K₂SO₄. Al₂(SO₄)₃ - Burnt alum

20.   CO is a reducing agent . justify with an example.

Carbon monoxide acts as a strong reducing agent. It reduces iron oxide into iron.

3CO + Fe₂O₃ ^___Heat__→ 2Fe + 3CO₂