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The p-Block Elements Class 11 Notes Chemistry - Basic Subjective Questions
Section – A (1 Mark Questions)
1. How does metallic and non-metallic character vary in a group?
Ans. The non-metals and the metals exist only in the p-block of the periodic table. The non-metallic character of elements decreases down the group. In fact the heaviest element in each p-block group is the most metallic in nature.
2. Third-period elements can expand their covalence above four. Briefly explain.
Ans. The third-period elements of p-groups included d-orbital, which can be utilized to form bond and expand octet.
3. Give two examples of electron deficient molecules.
Ans. BF3, Al2Cl6
4. Arrange the following halides of boron in the increasing order of acidic character: BF3, BCl3, BBr3, BI3.
Ans. BF3 < BCl3 < BBr3 < BI3
Since in BF3 there is back -bonding due to which it is less acidic among all .
5. Why CCl4 behaves as an electron precise molecule?
Ans. Carbon in CCl4, the number of electrons around the central atom in a molecule is eight and thus is electron precise molecule.
6. Lead unaffected by water. Why?
Ans. Lead is unaffected by water, probable because of a protective oxide film formation.
7. Why Diamond is the hardest substance known?
Ans. Diamond is the hardest substance on the earth because it is very difficult to break extended covalent bonding.
8. What is water gas composed of ?
Ans. The mixture of CO and H2 is known as water gas or synthesis gas.
9. What is the maximum covalence shown by N?
Ans. Nitrogen shows a maximum covalence of +4 because only four orbitals, one S and three P-orbitals are available for bonding in Nitrogen.
10. Bi(V) is a stronger oxidizing agent than Bi(III). Why?
Ans. Bi is more stable in +3 oxidation state in comparison to +5 due to inert pair effect. Therefore, Bi(V) has a strong tendency to act as oxidizing agent.
Section – B (2 Marks Questions)
11. SiCl4 forms [SiCl6]2– while CCl4 does not form [CCl6]2– Explain.
Ans. Carbon does not have d-orbitals and hence CCl4 does not combine with Cl– ions to give [CCl6]2–. On the other hand, silicon has vacant 3d-orbitals and thus can expand its covalency from 4 to 6. Therefore SiCl4 combines with Cl ions to form [SiCl6]2–.
12. Why does carbon form covalent compounds whereas lead forms ionic compounds?
Ans. Carbon cannot lose electrons to form C4 because the sum of four ionization enthalpies is very high. It cannot gain four electrons to form C4 because energetically it is not favourable. Hence, C forms only covalent compounds. Down the group 14, ionization enthalpies decrease, Pb being the last element has so low I.E. that it can lose electrons to form ionic compounds.
13. What are halides of carbon? Give few examples.
Ans. Carbon combines with halogens to form both simple and mixed tetrahalides. In the case of simple halides, all the four expected tetrahalides (e.g. CF4, CCl4, CBr4 and CCl4) are known to exist. The stability of the simple tetrahalides decreases with the increasing atomic mass of the halogen.
(CF4 > CCl4 > CBr4 > Cl4)
Amongst the mixed halides the better-known compounds are (CFCl3, CF2Cl2 and CCl3Br).
14. Why are boron halides & diborane referred to as “Electron deficient compounds”?
Ans. Boron in its halides has only six electrons in its valence shell, therefore it is short by two electrons to complete its octet. As a result, a molecule of boron halide can accept a pair of electrons from any electron-rich compound that is why boron halides are called electron-deficient compounds. In diborane, the total no. of valence electrons is not sufficient to completely fill the available orbitals. This gives an electron-deficient character to diborane.
15. All the elements of group 13 except thallium show a +3 oxidation state while it, shows a +1 oxidation state. Give reasons.
Ans. The valence shells of group 13-elements have two electrons in s-subshell & 1-electron in p-subshell. Therefore, they are expected to show a +3-oxidation state. In thallium, the electrons of the s-subshell do not take part in bond formation due to the inert pair effect & only one electron of the p-orbital participates in bond formation, thus it shows +1 oxidation state only.
16. Carbon different from other member of the group. Why?
Ans. Carbon differs from rest of the members of its group due to its smaller size, higher electro negativity, higher ionization enthalpy and unavailability of d-orbitals.
17. Covalence of carbon not expand beyond four. Explain briefly.
Ans. In carbon, only s and p orbitals are available for bonding and therefore, it can accommodate only four pairs of electrons around it. This limit the maximum covalence to four whereas other members can expand their covalence due to the presence of d-orbitals.
18. Boron forms no compounds in a unipositive state but thallium in a unipositive state is quite unstable. Why?
Ans. Boron has electronic configuration 2s22p1 & therefore forms compounds in a trivalent state. However, thallium prefers to form compounds in the +1 oxidation state rather than in the +3 oxidation state as suggested by its group number. This is due to the inert pair effect. According to this effect, the 6s2 electrons in the case of heavy metals preferably do not take part in bonding.
19. Why Borazine is more reactive than benzene?
Ans. Both Borazine & Benzene are isoelectronic. In benzene C = C bonds are non-polar while N = B bonds in borazine are polar in nature due to the presence of a co-ordinate bond between N & B atoms. As a result, addition is quite frequent in borazine while it is less in benzene because of delocalisation of pi-electron charge.
20. Why does CO2 have a linear shape with no dipole moment?
Ans. In CO2 molecule carbon atom undergoes sp hybridization. Two sp hybridized orbital of carbon atom overlap with two p-orbital’s of oxygen atoms to make two sigma bonds while other two electrons of carbon atom are involved in
PDF Summary - Class 11 Chemistry The p-Block Elements Notes (Chapter 13)
Introduction:
The p-block is made up of elements in groups 13 through 18 of the periodic table. Metals, metalloids, and non-metals are all found in the p-block. The electrical configuration of the p-block components is that of a generic valence shell configuration of
When compared to the other members of the same group, the first member of a group has a stronger capacity to establish
Trends in Properties of P-Block Elements:

(A) Group 13 Elements: The Boron Family:
Boron is a non-metal, while aluminium is a metal with numerous chemical similarities to boron, while gallium, indium, and thallium are virtually entirely metallic.
Electronic Configuration:
The valence shell electronic configuration of elements of boron family is
Atomic Radii:
As one moves along the group, an additional shell of electrons is added to each succeeding member, resulting in a rise in atomic radius.
Ionization Enthalpy:
The ionisation enthalpy values do not drop smoothly along the group as predicted from the overall patterns. The drop from
Electronegativity:
Electronegativity falls from
Physical Properties:
Boron is a non-metallic element. It's a solid black colour that's incredibly hard. It comes in a variety of allotropic forms. Boron has an extraordinarily high melting point due to its extremely strong crystalline lattice. Soft metals having a low melting point and good electrical conductivity make up the rest of the group. Gallium, which has a low melting point(
Chemical Properties:
Oxidation State and Trends in Chemical Reactivity:
The sum of boron's first three ionisation enthalpies is quite high due to its tiny size. This prohibits it from producing
These electron-deficient molecules have a proclivity to take a pair of electrons in order to reach a stable electronic state, and so act as Lewis acids. The inclination to act as Lewis acid reduces as the size of the group grows smaller. To create
Reactivity Towards Air:
Boron, in its crystalline state, is non-reactive. On the surface of aluminium, a very thin oxide layer develops, protecting the metal from further assault.
The character of these oxides changes as you move through the group. Boron trioxide is an acidic compound that forms metal borates when it combines with basic (metallic) oxides. The oxides of aluminium and gallium are amphoteric, while those of indium and thallium are basic.
Reactivity Towards Acids and Alkalies:
Even at moderate temperatures, boron does not react with acids and alkalies; nevertheless, aluminium dissolves in mineral acids and aqueous alkalies, giving it an amphoteric property. Dihydrogen is generated when aluminium is dissolved in dilute
Reactivity Towards Halogens:
These elements react with halogen to form trihalides (except
Important Trends and Anomalous Properties of Boron:
All of these elements' tri-chlorides, bromides, and iodides, which are covalent in nature, are hydrolysed in water. Except for boron, species like tetrahedral
Boron (B):
Occurrence:
Boron may be found in the following minerals in nature:
Borax
(Boron is part of an anionic complex),Boric acid
,Kernite
Colemanite
Extraction of Boron:
In the absence of oxygen, by reducing
with magnesium, sodium, or potassium:
The product is heated with
By heating potassium fluoroborate
with potassium metal, you can make boron.
It is then treated with dilute
In tiny amounts in pure form (crystalline boron) as a result of
Reduction of
with on a heated titanium metal filament at . The vapours of are absorbed in , and the vapours of boron that remain are condensed.Decomposition of
vapours using tungsten electrodes and a high-tension arc ( ).
Properties:
It comes in five different varieties, four of which are crystalline and one of which is amorphous. All crystalline forms are made up of clusters of
units and are extremely hard. All crystalline forms are chemically inert and appear black. Melting points are in the range of . The amorphous form, on the other hand, is brown and chemically active.Reaction With Air:
Action of Alkalies and Acids:
Reaction with
and :
Reducing Properties:
It decays in steam liberating hydrogen gas.
Uses:
Boron is utilised in the manufacture of high-impact steel and, since it absorbs neutrons, in reactor rods for atomic reaction control.
Compounds Of Boron:
Boron Trioxide
:
Preparation:
Properties:
It is a slightly acidic oxide that forms borates when it interacts with alkalies or bases.
(sodium orthoborate).It forms orthoboric acid after a gradual reaction with water. It generates coloured compounds when heated with transition metal salts.
Orthoboric Acid :
Among the oxyacids of boron are
Preparation:
A concentrated solution of borax is treated with sulphuric acid to precipitate it.
is made by suspending powdered colemanite in water and filtering the surplus . White crystals of are produced after filtering and chilling the filtrate.
Properties:
It is a weak monobasic acid, and the boron atom completes its octet in aqueous solution by eliminating
from water molecules:
As a result, it acts as a Lewis acid rather than a proton donor. When a polyhydroxy molecule like glycol or glycerol is added to its aqueous solution, it behaves as a strong acid. The great stability of the conjugate bone chelate complex accounts for the acidity.

Catechol and salicylic acids create comparable complexes, but ethanol does not.

When heated, it produces metaboric acid
Orthoboric acid is oily to the touch and is less soluble in cold water than hot water. It has a multilayer structure with hydrogen bonds connecting planar units of
Test For Borate Radical:
The evolved gas is burnt when boric acid is heated with ethyl alcohol, creating a green edged flame.
Uses:
It's an antiseptic, and the water solution may be used to cleanse your eyes. In addition, it is utilised in the glass, enamel, and pottery industries.
Borax
Preparation:
Borax can be found in nature, but it can also be produced using the methods listed below.
From Colemanite mineral. When colemanite powder is heated in a solution of
, the precipitation of takes place.
When white crystals of borax precipitate, the filterate is cooled. On treatment with
From orthoboric acid. The action of
on orthoboric acid produces borax.
Properties:
Borax is a white powder that is more soluble in hot water than cold water.
Because of its hydrolysis to weak acid
and strong alkali , its aqueous solution is alkaline.
When borax powder is heated, it expands at first owing to water loss in the form of steam, but then it transforms into a colourless clear borax bead at
.
Action of Acids:
The white flakes of boric acid are produced by heating.
Correct formula of borax is
Bead Test: Boric anhydride reacts with certain metal salts such as,
To form coloured metaborates. The colour of the metaborates can be used to identify the metallic ions (cations) in salts.
Uses: It is utilised in borax bead test, in gold purification, as flux during welding of metals and in glass production process.
Diborane
: Binary compounds of with are called boron hydrides or boranes. These compounds form following two types of series:
The chemistry of diborane has piqued attention due to its use in a variety of synthetic processes, as well as the fact that the structure's elucidation aided in the clarification of fundamental ideas regarding the structure of electron deficient compounds.
Preparation:
It can also be obtained by addition of
to concentrated or .
(Industrial method)
Properties:
Diborane is a colourless gas having boiling point
which is briskly decomposed by water with the formation of :
Diborane mixtures with air or oxygen spontaneously combust, releasing a substantial quantity of heat. Most other fuels have a lower heat of combustion per unit weight of fuel than diborane. As a result, it is utilised as a rocket fuel.
Pyrolysis of diborane in sealed containers at temperatures above
is a complicated process that results in a mixture of boranes. eg, , and .Organoboranes are formed when diborane reacts easily with alkenes and alkynes in ether solvents at normal temperature. The hydroboration reaction is the name given to this process.
Cleavage reactions
(borane carbonyl) or
Aluminium
Extraction (Hall-Heroult Process):
Bauxite
Properties:
Aluminium is a silvery metal with a density of
Action of Air: Dry air has no effect on aluminium. However, wet air creates a thin coating of
on its surface, which dulls its brilliance. It burns to create and at extremely high temperatures.Reaction with Halogens:
When gaseous halogens travel through aluminum, the halide forms in an anhydrous state.
Action of Alkalies: When heated with concentrated
, it releases gas and forms a colorless sodium aluminate solution.
Action of Acids: Aluminium interacts with both dilute
and but not with concentrated , since concentrated causes aluminium to become passive, producing a protective oxide coating on the surface.
Reaction with
: Aluminum nitride is produced when gas is passed over heated aluminum. As a result, hot aluminum functions as a absorber.
Reaction with Water: Cold water has no effect on aluminium. Boiling water or steam attacks it extremely slowly.
Action of
Solution: Mercury is released when aluminium is added to a solution of .
Reduction of Oxides of Metals: When less reactive metal oxides are heated with aluminium; the less reactive metal is released.
Uses:
Aluminium is utilized for plating tanks, pipes, iron bars, and other steel items to prevent corrosion, manufacturing of aluminium cables, precise instruments, surgical apparatus, aircraft bodies, train coaches, motorboats, and automobiles.
Compounds of Aluminium:
Aluminium Oxide
:
It's also known as alumina. It may be found in the form of bauxite and corundum in nature. It can also be found in gemstones. Topaz yellow, sapphire blue, ruby red, amethyst violet, and emerald green are some of the most important aluminium oxide stones.
Preparation:
Pure
Properties:
It's a white amorphous powder that's insoluble in water but soluble in acids (forming, for example
Uses:
It is employed in the extraction of aluminium, the creation of fake gems, the production of aluminium compounds, and the fabrication of furnace linings. As a catalyst in organic processes, it is a refractory substance.
Aluminium Chloride
:
It is a colourless crystalline solid that is water soluble. It has a covalent bond. Anhydrous
Preparation:
By mixing aluminium,
, or in dilute :
The solution gained is filtered and crystallized and the crystals of
Anhydrous
is obtained by the action of on heated aluminium.By heating a mixture of
and coke and passing chlorine over it.
Properties:
Action of Heat:
When heated at a high temperature, hydrated salt is transformed to
Action of Moisture on Anhydrous
:
When open to air, anhydrous
Action of
: Anhydrous absorbs since the latter is a Lewis acid. (white solid)Action of
Solution:
When solution of
This reaction is useful for determining the difference between an aluminium salt and salts of
Action of
Solution:
When
To differentiate an
Hydrolysis with Water:
When
The complex cation has a great affinity to undergo dimerization.
Uses:
It is employed as a catalyst in petroleum cracking, Friedel-Crafts processes, and the preparation of aluminium compounds.
Alums
Alums are clear crystalline solids with the generic formula, where is a trivalent metal
Potash alum
Alums are double salts that generate metal ions (or ammonium ions) and sulphate ions when dissolved in water.
Preparation:
Alums may be made by fusing
Uses:
It's used in the dye business as a mordant, as a germicide for water purification, and as a coagulating agent for removing colloidal contaminants from water.
(B) Group 14 Elements: The Carbon Family
Group 14 includes carbon (
Electronic Configuration:
The valence shell electronic configuration of these elements is
Covalent Radius:
From
Ionization Enthalpy:
The initial Ionization Enthalpy of members of group 14 is greater than that of members of group 13. The impact of the inner core electron may also be seen here. In general, the ionisation enthalpy
Electronegativity:
The elements in this group are slightly more electronegative than those in group 13 due to their tiny size. From
Physical Properties:
All of the members of Group 14 are solids. Non-metals include carbon and silicon, metalloids include germanium, and soft metals like tin and lead have low melting points. The melting and boiling values of group 14 elements are significantly greater than those of group 13 elements.
Chemical Properties:
Oxidation States and Trends in Chemical Reactivity:
The outermost shell of group 14 elements has four electrons. These elements show
It is owing to the valence shell electrons
Reactivity Towards Oxygen:
When heated in oxygen, all components produce oxides. There are primarily two forms of oxides:
Reactivity Towards Water:
Water has no effect on carbon, silicon, or germanium. Tin decomposes steam to produce dihydrogen gas and dioxide. Water has little effect on lead, owing to the development of a protective oxide coating.
Reactivity Towards Halogen:
These elements can create halides with the formula
Important Trends And Anomalous Behaviour Of Carbon
Carbon, like the initial member of other groupings, is distinct from the rest of its peers. Its smaller size, greater electronegativity, higher ionisation enthalpy, and lack d- orbitals, all contribute to this anomalous behaviour of carbon. Only four pairs of electrons can be accommodated around it. Carbon has the unique ability to form
Allotropes of Carbon
Carbon exists in a variety of allotropic forms, both crystallic and amorphous. Two well-known crystalline forms of carbon are diamond and graphite. H.W. Kroto, E. Smalley, and R.F. Curl discovered fullerenes, a third form of carbon, in 1985.
Diamond:
Its lattice is crystalline. Each carbon atom in a diamond undergoes sp hybridisation and is connected to four other carbon atoms in a tetrahedral manner utilising hybridised orbitals. The length of the C-C bond is
Graphite:
The structure of graphite is layered. Van der Waal's forces hold the layers together, and the distance between them is 340 pm. Each layer is made up of carbon atoms arranged in planar hexagonal rings. Within the layer, the C - C bond length is 141.5 pm. Each carbon atom in a hexagonal ring goes through sp2 hybridisation and forms three sigma bonds with three carbon atoms nearby. A
Fullerenes:
Fullerenes are created by heating graphite in the presence of inert gases such as helium or argon in an electrical arc. Because of its smooth shape and lack of 'dangling' connections, fullerenes are the only pure form of carbon. Fullerenes are a kind of molecule that resembles a cage. Buckminsterfullerene is a
Uses of Carbon:
High-strength, lightweight composites are made from graphite fibres embedded in plastic. Tennis rackets, fishing rods, aeroplanes, and canoes are all made from composites. Graphite is used for electrodes in batteries and industrial electrolysis because it is an excellent conductor. Graphite crucibles are inert to dilute acids and alkalies. Activated charcoal is used to absorb harmful gases, as well as in water filters to remove organic contaminants and air conditioning systems to regulate smell. Carbon black is used as a filler in car tyres and as a dark pigment in black ink. Coke is primarily utilised as a reducing agent in metallurgy and as a fuel. Diamond is a valuable stone that is used in jewellery.
Properties Of Carbon:
Carbon in any form will react with oxygen at a sufficiently high temperature to give carbon dioxide; in a deficiency of oxygen, carbon monoxide is formed as well.
It will decrease steam, creating water gas and a variety of metal oxides; these reductions are important for industry.
It is not attacked by dilute acids, but concentrated nitric acid and sulphuric acid are reduced if warmed with carbon according to the equations:
Oxides Of Carbon:
Carbon Dioxide :
Preparation:
It is easily produced in the laboratory by the action of weak hydrochloric acid on marble chips:
It is generated as a by-product in the manufacturing of quicklime and in fermentation operations in the industrial sector:
Properties:
At normal temperature and pressure, it is a colourless, odourless, and heavy gas that dissolves in its own volume of water. When the pressure is increased, it dissolves considerably more quickly in water, as do all gases, and this concept is employed in the production of soda water and fizzy beverages.
is quickly liquefied (critical temperature ), and a cylinder of the gas under pressure serves as a handy fire extinguisher. Solid carbon dioxide ('dryice') is created when a highly compressed gas is allowed to expand fast. Because no massy liquid is generated when solid carbon dioxide sublimes at , it is a handy way to produce low temperatures.Carbon dioxide is the anhydride of carbonic acid, a weak dibasic acid that ionises in the following order:
The buffer system of
Carbon dioxide readily reacts with alkalis forming the carbonate and, if
is in excess, the hydrogen carbonate. This is the basis of the lime-water test for gas.
When carbon dioxide interacts with alkalies, it forms carbonate and
The above reaction accounts for the formation of temporarily hard water.
Carbon dioxide, which is normally present to the extent of 0.03% by volume in the atmosphere, is removed from it by the process known as photosynthesis. It is the process by which green plants convert atmospheric
into carbohydrates such as glucose. The overall chemical change can be expressed as:
The process of photosynthesis removes carbon dioxide from the atmosphere, which is typically present to the level of 0.03% by volume. It is the process by which green plants transform
Plants use this process to produce food for themselves, as well as animals and humans. However, recent increases in fossil fuel burning and limestone breakdown for cement manufacturing appear to have increased
Carbonation of soft drinks is commonly done using gaseous
. It is used as a fire extinguisher since it is heavy and does not encourage combustion. The production of urea consumes a significant amount of .
Carbon Monoxide (Co):
Preparation:
When carbon or carbonaceous materials is oxidised by air or oxygen, it produces carbon monoxide with
. It is also generated when is reduced using red-hot carbon; this reaction is important in metal extractions.
It may be made in the lab by dehydrating methanoic acid and mixing it with concentrated sulphuric acid:
When oxalic acid is dehydrated in the same way, oxalic acid is also produced.
Steam is passed over heated coke on a commercial scale to prepare it. Water gas, also known as synthesis gases, is the combination of
and .
When air is utilized instead of steam, it produces a combination of
Industrial fuels such as water gas and producer gas are highly essential. With the release of heat, carbon monoxide in water gas or producer gas can be further combusted to generate carbon dioxide.
(absorbed by
Properties:
Carbon monoxide is a colourless, odourless gas that forms a blue flame when burned in air. It is very toxic, interacting with haemoglobin in the blood more readily than oxygen, causing rapid obstructing of normal breathing. Because the gas is not quickly absorbed by active charcoal, ordinary gas masks provide no protection. because it does not readily bind to active charcoal A combination of manganese (IV) oxide and copper (II) oxide catalytically oxidises it to
in the presence of air, and this combined catalyst is employed in the breathing equipment worn by rescue crews during mining catastrophes.Carbon monoxide is a strong reducing agent that is used in the extraction of iron and nickel in industry:
It interacts with a variety of transition metals to produce volatile carbonyls; the production of nickel carbonyl followed by its breakdown is the foundation of Mond's technique for getting extremely pure nickel:
Carbon monoxide reacts with sulphur to form carbonyl sulphide, and with chlorine in the presence of light to form carbonyl chloride (phosgene), which is used in the manufacture of polyurethane foam plastics. Phosgene is an extremely toxic gas.
Although carbon monoxide is not a genuine acid anhydride since it does not generate an acid when it interacts with water, it does produce sodium methanoate when it reacts under pressure with fused sodium hydroxide:
It combines with hydrogen under pressure in the presence of a zinc oxide or chromium (III) oxide catalyst to produce methanol; this is an important industrial process.
is readily absorbed by an ammoniacal solution of copper (I) chloride to give . It reduces an ammonical solution of silver nitrate to silver (black) and, in the absence of other gaseous reducing agents, this serves as a test for the gas. It can be estimated byreaction with iodine pentoxide, the iodine which is produced quantitatively being titrated with standard sodium thiosulphate solution.
An ammoniacal solution of copper (I) chloride easily absorbs by
Carbon Suboxide
The anhydride of propanedioic acid (malonic acid), of which it is the anhydride, may be produced by dehydrating it with phosphorus pentoxide:
When heated to about
The molecule is thought to have a linear structure:
Carbonates And Bicarbonates
Carbonic acid is a dibasic acid that produces two types of salts: carbonates (normal salts) and bicarbonates (acid salts) when the replacement hydrogens from
Preparation:
With
:
By Precipitation:
Carbides:
Carbides are carbon-based binary compounds with additional elements that are less electronegative or have equivalent electronegativity. They are divided into three groups: ionic, covalent, and interstitial (or metallic)
Ionic Carbides (or Salt like Carbides): Usually made up of components from the I, II, and III groups (Boron is an exception). They are further sub-classified into three categories based on the hydrolysis product.
Methanides These give
on reaction with .
These carbides contain
Acetylides: These give
on reaction with .
Such compounds contain
Allylides These give 1-propyne on reaction with
.
Such compounds contain
Covalent Carbides Compounds (like
) these are some giant molecules like are also examples of covalent carbides.Interstitial or metallic carbides: Transition metals, in which carbon atoms occupy interstitials in the crystal structure of metals, create such carbides.
Carborundum .
Preparation:
Properties:
It's a brittle material(Hardness
). It does not melt when heated, but rather decomposes into components. Acids have no effect on it. At high temperatures, however, it produces the following two reactions. Each atom is hybridised, giving it a diamond-like structure. As a result, each atom is surrounded by four atoms of the opposite kind.
Silicon:
Silicon is the second most prevalent element in the earth's crust (approximately 28% by weight) and may be found as the oxide silica in a number of forms, such as sand, quartz, and flint, as well as silicates in rocks and clays.
Preparation:
By reducing silica with carbon in an electric furnace, the element can be obtained:
The process of zone refining is used to generate very pure silicon from 'chemically' pure silicon. (2)
Properties:
Silicon is a high-melting-point solid with a diamond-like structure. The lack of an allotrope with the graphite structure demonstrates silicon atoms' inability to multiple bind with one another. Silicon is chemically inert in its bulk state, but halogens and alkalies attack it when it is powdered:
Except for hydrofluoric acid, with which it produces hexafluorosilicic acid, it is unaffected by acids.
(Magnesium silicide)
Compounds of Silicon:
Silicon dioxide,
Silicon dioxide,
Quartz is widely utilised as a piezoelectric material, allowing for the development of ultra-reliable clocks, contemporary radio and television transmission, and mobile radio communications. Silica gel is a drying agent that may also be used to support chromatographic materials and catalysts. In filtration facilities, Kieselghur, an amorphous type of silica, is utilised.
Silicates:
Silicates are binary silicon-oxygen compounds that also contain additional metals in their atomic structures.
Because the difference in negativity between
and is roughly 1.7, the link can be classified as ionic & covalent.If we calculate the radius ratio
It suggests that the co-ordination no. of silicon must be 4 and from VBT point of view we can say that Si is sp hybridized. Therefore silicate structures must be based upon tetrahedral units tetrahedral units may exist as discrete units or may polymerise into larger units by sharing corners.
Classification Of Silicates:
Orthosilicates:
As seen in the picture, these include distinct units of
Pyrosilicate:
Two tetrahedral units are linked in these silicates by sharing oxygen at one comer, resulting in
The oxygen atoms that are coupled with one Siatom will have a negative charge. Thorteveitite
Cyclic Silicates:
The silicates containing these anions are known as cyclic silicates because two oxygen atoms per tetrahedron are shared to form closed rings, resulting in the structure with general formula
Chain Silicates:
Simple chain and double chain chain silicates are two types of chain silicates. In simple chains, two corners of each tetrahedron are shared, resulting in a lengthy tetrahedron chain. They have the same general formula as cyclic silicates, i.e.
Double chain silicates, in which two simple chains are linked together by shared oxygen, can also be drawn. Amphiboles are another name for such compounds. Asbestos is a well-known example of a double chain silicate mineral. The general formula for the anions of double chain silicates is
e.g. Synthetic silicates
Enstatite
Two dimensional sheet silicates in such silicates, Each tetrahedral shares three oxygen atoms with neighbouring
tetrahedrals. This sharing results in a two-dimensional sheet structure with a generic formula, such as Talc.Three Dimensional Sheet Silicates:
All four oxygen atoms are shared by neighbouring
e.g. Quartz, Tridymite, Crystobalite, Feldspar, Zeolite and Ultramarines.
Silicones:
Silicones are synthetic organosilicon compounds with Si-O-Si bonds that hold repeating units of
The silicones are made by polymerizing alkyl or aryl substituted chlorosilanes after they have been hydrolysed. The following processes produce alkyl or aryl substituted chlorosilanes.
The silane derivatives are hydrolysed during fractional distillation, and the resulting 'hydroxides' rapidly condense due to intermolecular water elimination. The amount of hydroxyl groups originally linked to the silicon atom determines the ultimate product:
Several molecules can be combined in this way to produce a long chain polymer with
A little amount of the monochlorosilane derivative is added to the hydrolysis mixture to terminate the polymer chain seen above.
Only the following chemicals can be used to make silicones.
Silicones from the hydrolysis of
Silicones from the hydrolysis of a combination of
As is customary, the dichloro derivative will form a long chain polymer. However, the hydrolysis product of the mono-chloro derivative might stifle the development of this polymer at any point.
Silicones produced through trichloro derivative hydrolysis When a chemical like
Silicones are water-repellent due to the hydrocarbon layer that runs along the silicon-oxygen chain. Silicones may be used to make products with the physical characteristics of oils, rubbers, and resins. Silicone fluids (such as those used in plane hydraulic systems) are thermally stable and their viscosity changes very little as a function of temperature; silicone rubbers, on the other hand, keep their flexibility at lower temperatures than regular rubber. Silicone varnishes are such good insulators and heat-resistant that using them to insulate wire allowed motors to run at over-loads that would have caused the insulation to catch fire. The discovery of silicones has opened up a whole new sector of science and technology, both civilian and military.
Tin and Lead:
Compounds of Tin:
Stannous Oxide
:
Preparation:
In the absence of air, stannous hydroxide,
is heated.
By heating stannous oxalate,
in absence of air.
Properties:
is an insoluble in water amphoteric dark grey or black solid oxide. It forms stannous salts when it dissolves in acids.
In a heated solution of
, SnO dissolves to create (soluble) sodium stannite and water.
Only aqueous solutions are known to contain stannites. Stannites take oxygen from the air and oxidise to stannate, which is a naturally stable compound.
Uses:
It's used to make stannous chloride and stannous sulphate.
Stannous Chloride :
It's a colourless solid that dissolves in water. Its solution becomes milky over a period of time owing to hydrolysis to
Preparation:
On crystallisation, the solution yields colourless crystals of
Properties:
Reaction with
solution: When solution is added to an aqueous mercuric chloride solution, a silky white mercurous chloride precipitate is produced, which becomes black when the mercury is reduced further to black mercury.
It reduces ferric chloride,
to ferrous chloride,It is hydrolyzed in water, resulting in a white precipitate of
(white)
Its aqueous solution is acidic because it creates a weak basic and a strong acid. Hydrolysis can be avoided by adding concentrated
Uses:
It's utilised as a reducing agent in the dye business, as well as for mercuric salt testing and the production of various stannous compounds.
Stannic Oxide :
Preparation:
By burning Sn in air
By heating Sn with concentrated
Properties:
It's a white solid that won't dissolve in water. It has a low acidity. It forms stannic sulphate when dissolved in
Stannic Chloride
Preparation:
By the action of
gas on heated
By the action of
on stannous chloride
Properties:
It's a colourless, flammable liquid.
. It has a covalent bond.Action of Moisture It absorbs moisture and converts to hydrated stannic chlorides,
, and which is why it's called "butter of tin" or "oxymercurate of tin."It is quickly hydrolyzed in water and generates a powerful acid
. As a result, litmus finds its aqueous solution acidic. It hydrolyzes at a faster rate than
is a Lewis acid. Hence it has a tendency to accept lone pair of electrons from etc. and form adducts such asIt dissolves in concentrated
forming and in presence of ammonium chloride, it forms ammonium salts of this acid.
Uses:
For the preparation of stannic compounds.
Compounds Of Lead:
Litharge
:
It's an amphoteric oxide that dissolves in both acids and alkalis.
It's utilised in the rubber sector, as well as flint glasses, enamels, and storage batteries.
Lead Dioxide
:
The fact that
Preparation:
Properties:
It's an insoluble powder with a chocolate color. It produces monoxide when heated at
:
It oxidizes
to :
It dissolves in conc.
solution:
It oxidises Mn salt to permanganic acid:
It reacts with
at red heat to form lead sulphate:
It reacts with conc.
to evolve oxygen gas.
Uses:
It's used in the match business to make the igniting surface of match boxes and to make match powder
Red Lead
:
Preparation:
It is prepared by heating
Properties:
It is a red powder that is insoluble in water but produces a red precipitate of
when heated with conc.
When heated above
, it undergoes decomposition into and liberate oxygen gas.
It oxidizes conc.
to chlorine
When heated with conc.
it evolves oxygen
Uses:
It is employed as an oxidising agent, in the production of red paint, in the production of special lead cement, and in the production of flint glass.
Lead Chloride
:
Preparation:
Properties:
It's a crystalline white substance that's insoluble in cold water but soluble in hot water. It forms a complex ion when dissolved in strong HCl.
Uses:
It's utilised in the production of paint pigments.
Lead Tetrachloride
:
Preparation:
The following procedures are used to make it:
By dissolving
in cold conc. HCl
When
is introduced to a chloroplumbic acid solution, a yellow precipitate of ammonium chloroplumbate is produced.
Lead tetrachloride is produced when crystals of ammonium chloroplumbate are introduced to ice cold conc.
and separate as a yellow oily liquid.
By the action of
on a solution of in conc.
Properties:
It's a yellow oily liquid that freezes at
and dissolves in organic solvents like ethanol and benzene.Precipitation of
is formed by rapid hydrolysis with water.
Uses: It's utilised in the production of stannic compounds.
About The p-Block Elements
The p-block elements are the interesting group of elements found usually on the right side of the periodic table from column number 3A to 8A (including the segments 13-18). A few of the p-block elements include noble gases, metalloids, halogens, and metals. Therefore, in chemistry, class 11, the topic p-Block elements are dealt with in more detail. The students need to learn the anomalous properties, general trends, allotropes, and important compounds of p-block elements.
The p-block elements topics deal with the elements present in the p-block of the modern periodic table. Also, there are variations in the properties of the p-block elements due to the influence of d-block and f-block electrons present in the heavier elements of the inner core.
Also, once this chapter is done, students can learn about the trends in the chemistry of p-block elements. They will also know about the trends in physical and chemical properties of group 13 and group 14 elements and can know the anomalous behavior of Boron and Carbon.
Even they will describe the allotropic forms of Carbon and get an idea about the compounds of Carbon, Silicon, and Boron. A few of the concepts described in group 13 elements are the boron family, the atomic radii, electronegativity, physical and chemical properties, some important compounds of boron, borax, and more.
In addition to these, the concepts used in group 14 elements are carbon family, electronic configuration, covalent radius, physical and chemical properties, electronegativity, allotropes of carbon, diamond, graphite, and more.
Sub-Topics Covered Under The p-Block Elements
The chemistry class 11, Chapter 11 of, The p-block elements falls under the part of unit 11. The total weight of the unit is 8, 9, 10, 11, and carries 16 marks. The student, by studying this chapter, can become 100 percent accurate on the NCERT solutions for class 11 Chemistry at Vedantu, solved by our subject experts.
Let us look at the topics and subtopics in the p-block elements chapter below:
Group 13 Elements - The Boron Family
Ionization Enthalpy
Atomic Radii
Electronegativity
Electronic Configuration
Physical and Chemical Properties
Important Trends & Anomalous Properties of Boron
Some Important Compounds of Boron
Borax
Diborane, B2H6
Orthoboric Acid
Uses of Boron & Aluminium & Their Compounds
Group 14 Elements: The Carbon Family
Covalent Radius
Electronic Configuration
Ionization Enthalpy
Physical and Chemical properties
Electronegativity
Important Trends & Anomalous Behaviour of Carbon
Allotropes of Carbon
Graphite
Diamond
Fullerenes
Uses of Carbon
Some Important Compounds of Carbon & Silicon
Carbon Monoxide and
Carbon Dioxide
Silicon Dioxide, Sio2
Silicates
Silicones
Zeolites
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Importance of a Revision Notes
A revision notes is the one which can be either prepared by the students or by other third-party providers and is so important. It is used to note the important points, formulas, points to be remembered. Also, it can be very helpful during the exams, where the students can make the most of it by carrying easily because it is handy.
FAQs on The P Block Elements Class 11 Notes CBSE Chemistry Chapter 11 (Free PDF Download)
1. Explain some points about p-Block Elements?
In the chapter, The p-block elements, the last electron enters the outermost p-orbital. There are 6 groups of p-block elements in the Periodic Table, ranging and numbering from 13 to 18. Their valence shell electronic configuration is given by ns2np1 – 6 (except for He or Helium).
2. List out some topics of The p-Block Elements?
Some of the topics that are related to p-Block Elements are given as follows:
Atomic Radii
Electronic Configuration
Group 13 Elements - The Boron Family
Ionization Enthalpy
Electronegativity
CovalantRadius
3. What are the subjects that can be found from the site, Vedantu?
Vedantu is one of the larger online learning platforms. Students can get many of the information such as Revision Notes, Practice Papers, Model Papers, Mock Test Papers, Exam Preparation Tips, and How to prepare for the exams. They can avail this information from various subjects, including Maths, Physics, Chemistry, Regional Languages, Economics, Business Studies, and so forth.
4. Why is The p-Block Elements topic more important in the exams?
The p-Block Elements concept is the most important topic because it comprises many subtopics of both Group 13 and Group 14. It also carries good weightage, and students can make a good score by preparing well for this chapter without a miss.
5. What is a p-block element?
Chapter 11 of Chemistry talks about the P-block element. In simple words, elements whose last electron enters any of the three p-orbitals of their respective shells are known as p-block elements. P-blocks begin from the 13th group up until the 18th group in the periodic table. They are called p-blocks because their valence electrons are in the p orbital. There are a total of 35 p-block elements. You can look for a detailed explanation in Class 11 Chemistry Revision Notes for Chapter 11.
6. What are the properties of p-block elements?
P-block elements are composed of metal, nonmetals, and metalloids. P-block elements consist of classic metal properties. P-block elements are good conductors of electricity, have a very shiny appearance, have a high melting point, are good conductors of heat, and react quickly with the non-metals to form ionic compounds. Examples of metals in p-block are Gallium, tin, etc. Some of the known metalloids are found in p-block as well, such as silicon, boron, etc. The nonmetals in p-blocks are opposites of metals. They have a low boiling point, poor conductor of electricity. Examples are phosphorus, sulfur, selenium, etc.
7. What are the elements of s and p-block Combinedly called?
S and p blocks are presented on the opposite sides of the periodic table. S block is composed of metals whereas the p-block elements include metals, nonmetals and metalloids. S and p elements when combined are represented by the term 'representative elements'. The inert gases are present in a and I blocks are an exception to this term. Elements in the block are highly electromotive while elements of the p block are electronegative. Class 11 Chemistry Revision Notes for Chapter 11 is a step by step explanation to understand the concept of representative better at Vedantu.
8. What is chemical bonding?
Any interactions that state the association of atoms into molecules, crystals, ions and other stable species in chemicals that build up the substances of everyday life can be called chemical bonding. These bonds are generally of four types; ionic bonds, covalent bonds, hydrogen bonds and Van der Waals interactions. To understand the process of chemical bonding in detail you can visit Vedantu's revision notes, summary and explanation of important topics. You can find all the required study material for Chemistry Chapter 11 free of cost on the Vedantu app as well.
9. What are the fundamental concepts in Class 11 Chemistry Chapter 11?
Chapter 11 of Class 11 Chemistry briefs us about the P-block elements and other concepts related to them. Some of the fundamental concepts that are covered in the chemistry NCERT book are- introduction to the group 13 elements which is known as the Boron family, important trends and anomalous properties of Boron, some important compounds of Boron, uses of Boron and Aluminium, group 14 elements: the Carbon family, important trends and anomalous behaviour of Carbon, allotropes of Carbon and some important compounds of Carbon and Silicon.

















