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the P-block Elements Class 11 Notes For Chemistry Chapter 11

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The p- Block Element

Elements in which the last electron enters in the any one of the three p- orbital of their outermost shells – p-block elements

•  Gen. electronic configuration of outer shell is  ns2np1-6 The inner core of e-config.may differ which greatly influences their physical & to some extent chemical properties.

•   The block of elements in the periodic table consisting of the main groups :

• Group13

(B to Tl)
• Group14 (C to Pb)
• Group15 (N to Bi)
• Group 16  (O to Po)
• Group17   (F to At)
• Group18 (He to Rn)

(1)   Members at the top and on the right of the p-block are nonmetals (C, N,   P, O, F, S, Cl, Br, I, At).
(2) Those on the left and at the bottom are metals (Al, Ga, In,Tl, Sn, Pb, Sb Bi, Po).
(3)     Between the two, from the top left to bottom right, lie an ill-defined group of metalloid elements (B, Si, Ge, As, Te)

GROUP 13  : The boron group

 • Outer Electronic Configuration:-ns2np1

•   group  members:  boron  (B),  aluminum  (Al),  gallium  (Ga),  indium  (In) & thallium (Tl) .  All, except boron, are metals.

•   Boron show  diagonal relationship with  Silicon;    both are  semiconductors metalloids & forms covalent compounds.

•    Boron compounds are electron deficient, they are lack of an octet of electrons about the B atom .

•   diborane B2H6 is  simplest boron hydride
•   Structure: three-center two-electron: the H atoms are simultaneously bonded to two B atoms the B-H bridging bond lengths are greater than B-H terminal.

•   - Boron oxide is acidic (it reacts readily with water to form boric acid)

•   aluminium compounds:aluminium oxide is amphoteric

•   aluminum  halides,  e.g.,  AlCl3   is  dimer,  an  important  catalyst  in  organic chemistry have anincomplete octet, acts as Lewic acid by accepting lone pairs from Lewic bases, forming adduct

•   aluminum hydride, e.g., LiAlH4, a reducing agent

•   Atomic Properties - Electronic Configurations





Abundance   in   Earth’s
Crest (in ppm)




[He]2s2 2p1





[Ne]3s2 3p1





[Ar]3d104s2 4p1





[Kr] 4d105s2 5p1





[Xe] 5d106s2 6p1


 Atomic and ionic radii

•   The   atomic  and   ionic   radii  of   group   13   elements  are   compared  to corresponding elements of group 2.     From left to right in the period, the magnitude of nuclear charge increases but the electrons are added to, the same shell.    These  electrons do  not  screen  each  other,  therefore,  the  electrons experience greater nuclear charge.

•    In other words, effective nuclear charge increases and thus, size decreases. Therefore, the elements of this group have smaller size than the corresponding elements of second group.

•   On  moving down the  group  both atomic  and  ionic  radii are  expected to increase due to the addition of new shells. However, the observed atomic radius of Al (143 pm) is slightly more than that of Ga (l35 pm).

Ionization energies

The first ionization energies of group 13 elements are less than the corresponding members of the alkaline earths.

The sharp decrease in I.E. from B to Al is due to increase in size. In case of Ga, there are ten d-electrons in its inner electronic configuration.

The very high value of 3rd I. E. of thallium indicates that +3 O.N. state is not stable, rather +1 is more stable for thallium .

Electropositive (or metallic) character

the elements of group 13 are less electropositive as compared to elements of group 2. On moving down the group the electropositive (metallic) character increases because ionization energy decreases. For e.g., Boron is a non-metal white the other elements are typical metals.

Oxidation states

The common oxidation states of group 13 elements are +3 and + l .The stability of the + 1 oxidation state increases in the sequence Al <Ga< In <Tl, Due to Inert pair effect.







Oxidation state



+3, +1

+3, +1

+3, +1

Chemical reactivity of Gr.13 Elements

All elements in their compounds exhibit the oxidation state of + 3 and +1. Hydrides
•   None of the group 13 elements reacts directly with hydrogen. However, a no.
of hydrides of these elements have been prepared by indirect methods. The boron hydrides are called boranes& classified in two series:   (a)          BnHn+4 called nidoboranes            (b)       BnHn+6 called arachnoboranes


2BF3(g) + 6LiH(s) → B2H6(g) + 6LiF(s)

•   Laboratory method:

(i) By the reaction of iodine with sodium borohydride in a high boiling solvent. 2NaBH4 + I2   → B2H6   + 2NaI   + H2
(ii) By reduction of BCl3 with LiAlH4 4BCl3 +  3LiAlH4 → 2 B2H6  + 3AlCl3   + 3 LiCl

Structure of Diborane, B2H6

structure of diborane 26H6
Structure of Diborane, B2H6

Some important characteristics of boranes:

i) Lower boranes are colourless gases while higher boranes are volatile liquids or solids.

ii) They undergo spontaneous combustion in air due to strong affinity of boron for oxygen. B 2H6   + 3O2   → B2O3   + 3H2O + Heat

iii)  Boranes react with alkali metal hydrides in diethyl ether to form borohydride complexes. B2H6   + 2MH →2M+[BH4]-  (M= Li or Na) Metal borohydride
(iv) Diborane reacts with ammonia to give borazine at 450 K. B2H6   + 6NH3    → 3B3N3H   + 12H2

•   Borazine has a cyclic structure similar to benzene and thus is  called inorganic benzene

•   The other elements of this group form only a few stable hydrides. The thermal stability decreases as we move down the group.

•   AlH3 is a colourless solid polymerized via Al - H - Al bridging units. These hydrides are weak Lewis acids and readily form adducts with strong Lewis base (B:) to give compounds of the type MH3 (M = Al or Ga). They also form complex-tetrahydrido anions, [MH4]-. The most important tetrahydrido compound is  Li[AlH4]

tetrahydrido compound is  Li[AlH4]


•   M2O 3   & M(OH)3

basic Character increases

HALIDES: Structure of boron trihalides

 Structure of boron trihalides

Dimeric structure of aluminium chloride

–  Boron halides do not form dimers because the size of boron is so small that it is unable to coordinate four large-sized halide ions.

structure of aluminium chloride

•  Anomalous properties of boron

1. Boron is a non-metal & bad conductor of electricity whereas aluminium is a metal& good conductor. B is  hard but Al is a soft metal.
2.  Boron exists in two forms-crystalline and amorphous. But Al does not exist in different forms.
3. The melting and boiling point of boron are much higher than that of Al .
4. Boron forms only covalent compounds whereas Al forms even some ionic compounds.
5. The hydroxides and oxides of boron are acidic in nature whereas those of aluminium are amphoteric.
6. The trihalides of boron exist as monomers. On the other hand, aluminium halides exist as dimers .
7. The hydrides of boron are quite stable while those of aluminium are unstable

•   Boron and silicon exhibit the typical properties of non-metals. These do not form cations. Both exist in amorphous as well as crystalline forms.

•   Boron oxide (B2O3) and silic a (SiO2) both are acidic and dissolve in alkali solutions to form borates and silicates respectively. B2O3   + 6NaOH → 2Na2BO3    + 3H2O SiO2 +  2NaOH → Na2SiO3    + H2O
•   The chlorides of both B and Si get hydrolyzed by water to boric acid and silicic acid respectively. BCl3   + 3H2O →H3BO3    + 3HCl        SiCl4   + 3H2O   → H2SiO3    + 4HCl

  The  hydrides  of  Boron  and  Silicon  are  quite  stable.  Numerous  volatile hydrides are also known which catch fire on exposure to air and are easily hydrolyzed.  Both elements are semiconductors.

Behavior in Aqueous Solutions

1   Al, Ga, In and Tl exhibit a well-defined aqueous chemistry in their tripositive states. Species like [M(OH)4]-, [M(H2O)2(OH)4]-, [M(OH2)6]3+ for M = Al, Ga, In, exist in aqueous solution.

2.  Al, Ga. In and T1 ions exist as octahedral aqua ions, [M(OH2)6]3 + in aqueous solution and many salts like halides, sulphates, nitrates and perchlorates exist as hydrates.

3. Aluminiumsulphate forms double salts -  called alum, having the general formula M2SO4. Al2(SO4)3.12H2O, where M=Na+ or K+. USES OF BORON & ALUMINIUM

•   Aluminium is used extensively in industry and everyday life. It forms many useful alloys with Cu. Mn, Mg, Si and Zn. Hence, aluminium and its alloys find use in packaging, utensil making, construction, aerospace and other transportation industries. It is used as a conductor for transmission of electricity. Aluminium is alsoused in the alumino-thermite process for production of chromium and manganese from their ores.

Group 14 Elements:-The Carbon Family

Group 14 includes carbon (C), silicon (Si), germanium (Ge), tin (Sn) and lead (Pb). General electronic configuration of carbon family is ns2np2. Covalent radius:-Covalent radius expected to increase from Cto Si, From Si to Pb small increase is found.
Ionization Enthalpy:-The first ionization enthalpies of group 14 elements are higher than those of the corresponding group 13 elements. Electronegativity:-Group 14 elements are smaller in size as compared to group 13 elements that’s why this group elements are slightly more electronegative than group13

Chemical properties:-

Carbon and silicon mostly show +4 oxidation state. Germanium forms stable compounds in +4 state and only few compounds in +2 state.

Tin forms compounds in both oxidation states. Lead compounds in +2 state are stable and in +4 state are strong oxidizing agents.

Exception:-Pb4 and SnF4 are ionic in nature.

Except CCl4 other tetrachlorides are easily hydrolysed by water.

Since carbon does not have d-orbitals and hence cannot expand its coordination number beyond 4

CCl4 +H2O           No Reaction

SiCl4+4H2O         Si(OH)4+4HCl Silicic acid

Allotropes of Carbon:-The three types of allotropes are –


Diamond :-

In diamond each carbon atom undergas SP3hybridisation. Each carbon is tetrahedrally linked to four other carbon atoms.

Graphite :-

In graphite, carbon is SP2-hyberdized graphite has a two-dimensional sheet like structure consisting of a number of hexagonal rings fused together. Graphite conducts electricity along the sheet.It is very soft and Slippery FullerenceFullerence was  discovered collectively by  three  scientists namely R.E Smalley,R.F Curl and H.W Kroto SOME Important Compounds Of Carbon and Silicon

Carbon monoxide :-

It I  prepared by  direct oxdisation of C  in  limited supply of oxygen. 2C+O2(g)  →   2CO(g Commercially it is prepared by the passage of steam over hot coke

Carbon Dioxide :-

It is prepared by complete combustion of carbon and carbon fuels in excess of air.C(s) +O2(g)  → CO2(g)

Laboratory method:-

In laboratory it is prepared by the treatment of dilHCl on CaCO3 CaCO3(s) +2HCl(aq) → CaCl2(aq) +CO2>/(g)+H2O(l) Silicon  

Dioxide :-

Each silicon atom is covalently bonded in a tetrahedral manner to four oxygen atoms. Silicones:-Silicones   are   the   synthetic   organo-siliconpolymers   having   general formulae (R2SiO)n in which R = alkyl (methyl,ethyl or phenyl) Silicates:-Silicates are  exist  in  nature in  the  form of feldspar, zeolites,mica and asbestos etc. The basic structure of silicates is SiO44

Zeolite s:

-Zeolites  is  aalumino-silicate  of  metal.  Metal  cations  participating  in formationof Zeolite are use usually Na+,K+,or Ca2+. Zeolites are used to remove permanent hardness of water.

ncert notes for class 11 chapter 11 p block elements

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