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+2 Gem Chemistry – For Complete Material - ���� 9080228421
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+2 Chemistry
Unit – 2 (New Syllabus)
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+2 Gem Chemistry – For Complete Material - ���� 9080228421
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UNIT-2: p-BLOCK ELEMENTS-I
EVALUATE
1. An aqueous solution of borax is (a) neutral (b) acidic (c) basic (d) amphoteric
Ans: (c) basic 2. Boric acid is an acid because its molecule (NEET) (a) contains replaceable H+ ion (b) gives up a proton (c) combines with proton to form water molecule (d) accepts OH- from water, releasing proton.
Ans: (d) accepts OH- from water, releasing proton. 3. Which among the following is not a borane?
(a) B2H6 (b) B3H6 (c) B4H10 (d) none of these Ans: (b) B3H6
4. Which of the following metals has the largest abundance in the earth’s crust? (a) Aluminium (b) calcium (c) Magnesium (d) Sodium
Ans: (a) Aluminium 5. In diborane, the number of electrons that accounts for
banana bonds is (a) Six (b) two (c) four (d) three
Ans: (c) four 6. The element that does not show catenation among the
following p-block elements is (a) Carbon (b) silicon (c) Lead (d) germanium
Ans: (c) Lead 7. Carbon atoms in fullerene with formula C60 have
(a) sp3 hybidised (b) sp hybridised (c) sp2 hybridised (d) partially sp2 and partially sp3 hybridised
Ans: (c) sp2 hybridised
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8. Oxidation state of carbon in its hydrides (a) +4 (b) -4 (c) +3 (d) +2
Ans: (a) +4 9. The basic structural unit of silicates is (NEET)
(a) (SiO3)2- (b) (SiO4)
2- (c) (SiO)- (d) (SiO4)4-
Ans: (d) (SiO4)4-
10. The repeating unit in silicone is v
(a) SiO2 (b)
Si O
R
R
(c)
Si O
R
OR
(d)
RSi O
R
O
Ans: (b)
Si O
R
R
11. Which of these is not a monomer for a high molecular
mass silicone polymer? (a) Me3SiCl (b) PhSiCl3 (c) MeSiCl3 (d) Me2SiCl2
Ans: (a) Me3SiCl 12. Which of the following is not sp2 hybridised?
(a) Graphite (b) Graphene (c) Fullerene (d) Dryice Ans: (d) Dryice
13. The geometry at which carbon atom in diamond are bonded to each other is (a) Tetrahedral (b) hexagonal (c) Octahedral (d) none of these
Ans: (a) Tetrahedral
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14. Which of the following statements is not correct? (a) Beryl is a cyclic silicate (b) Mg2SiO4 is an orthosilicate
(c) SiO44- is the basic structural unit of silicates
(d) Feldspar is not aluminosilicate
Ans: (d) Feldspar is not aluminosilicate 15. AlF3 is soluble in HF only in the presence of KF. It is due
to the formation of (NEET)
(a) [ ]3 3 3K AlF H (b) [ ]3 6K AlF (c) 3AlH (d) [ ]3K AlF H
Ans: (b) [ ]3 6K AlF
16. Match items in column-I with the items of column – II and assign the correct code.
Column-I Column-II A Borazole 1 B(OH)3
B Boric acid 2 B3N3H6
C Quartz 3 Na2[B4O5(OH)4]8H2O
A B C D
(a) 2 1 4 3
(b) 1 2 4 3
(c) 1 2 4 3
(d) None of these
Ans: (a) A-2, B-1, C-4, D-3
17. Duralumin is an alloy of (a) Cu, Mn (b) Cu, Al, Mg (c) Al, Mn (d) Al, Cu, Mn, Mg
Ans: (d) Al, Cu, Mn, Mg 18. Thermodynamically the most stable form of carbon is
(a) Diamond (b) graphite (c) Fullerene (d) none of these
Ans: (b) graphite
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19. The compound that is used in nuclear reactors as
protective shields and control rods is (a) Metal borides (b) metal oxides
(c) Metal carbonates (d) metal carbide
Ans: (a) Metal borides
20. The stability of +1 oxidation state increases in the sequence (a) Al < Ga < In < Tl (b) Tl > In < Ga < Al
(c) In < Tl < Ga < Al (d) Ga < In < Al < Tl
Ans: (a) Al < Ga < In < Tl
ANSWER THE FOLLOWING QUESTIONS
1. Write a short note on anamolous properties of the first
element of p-block. i) Small size of the first member.
ii) High ionisation enthalpy and high electronegativity.
iii) Absence of ‘d’ orbitals in their valence shell.
In group 13: 1) Boron is metalloid.
2) Boron shows diagonal relationship with silicon of group 14.
3) The oxides of boron and silicon are acidic is nature.
Group 14: The carbon is non metals others are metalloids or
metals.
Carbon form multiple bonds and shows catenation.
The Catenation property decreases down the group.
Group 15: The Nitrogen form multiple bonds. Nitrogen is
diatomic molecule.
Group 16: Oxygen is diatomic. Due to its high electro
negativity, it forms hydrogen bonds.
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Group 17: Fluorine is most electronegative and forms
hydrogen bonds.
It shows –1 oxidation state. Fluorine is Strongest oxidizing
agent and most reactive elements.
2. Describe briefly allotropism in p-block elements with
specific reference to carbon. Some elements exists in more than one crystalline or molecular
forms in the same physical state.
The phenomenon is called allotropism and the different
forms of an element are called allotropes.
Allotropes of Carbon: Diamond, Graphite, Graphene, Fullerenes,
Carbon nano tubes.
3. Boron does not react directly with hydrogen. Suggest one
method to prepare diborane form BF. The gaseous boron trifluoride reacts with sodium hydride at
450K gives diborane. 450K
3 2 62BF + 6NaH B H + 6NaF→
diborane
4. Give the uses of Borax.
Uses of Borax: 1. Borax is used for the identification of coloured metal ions.
2. In the manufacture of optical and borosilicate glass,
enamels and glaze for pottery.
3. It is also used as a flux in metallurgy and also acts as a
good preservative.
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5. What is catenation? Describe briefly the catenation
property of carbon. Catenation is an ability of an element to form chain for
catenation.
1. The valency of element is greater than or equal to two
2. Element should have an ability to bond with itself.
3. The self bond must be strong as its bond with other elements.
4. Kinetic inertness of catenated compound towards other
molecules.
6. Write a note on Fisher tropsch synthesis. The reaction of Carbon monoxide with hydrogen using
metal catalysts at 500-700K and 50 atm gives saturated and
unsaturated hydro carbons.
2 n 2n+2 2nCO + (2n +1) H C H + nH O→
2 n 2n 2nCO + 2nH C H + nH O→
Carbon monoxide forms numerous complex compounds
with transition metals.
4[Ni(CO) ] ∆
4Ni + 4 CO [Ni (CO) ]→
7. Give the structure of CO and CO2. If has linear structure. Three electron are shared between
carbon and oxygen.
The structure has two canonical forms of resonance hybrid.
Carbon dioxide 2(CO )
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Carbon dioxide has a linear structure with equal bond
distance for the both C-O bonds. In this molecule, one C-O
sigma bond and 3c-4e bond covering all the three atoms.
8. Give the uses of silicones. 1. Silicones are used for low temperature lubrication and in
vacuum pump.
2. It is used in high temperature oil bath.
3. They are used for making water proofing clothes.
4. They are used as insulating material in electrical motor
and other appliances.
5. They are mixed with paints and enamels to make them
resistant towards high temperature, sun light, dampness
and chemicals.
9. AlCl3 behaves like a Lewis acid. Substantiate this
statement. It forms addition compounds with ammonia phosphine and
carbonyl chloride etc., So it behaves as Lewis acid 3 3AlCl .6NH .
10. Describe the structure of diborane. In diborane two BH2 units are linked by two bridged
hydrocarbons. It has eight B-H bonds.
Diborane has only 12 valence electrons and are not sufficient
of form covalent bonds.
The four terminal B-H bonds are normal covalent bonds.
The remaining four electrons used for bridged bonds is two
three center B-H-B bonds. Utilize two electrons each.
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The bridged hydrogen atoms are in a plane.
In diborane, Boron is sp2 hybridized orbital contain single
electron and fourth orbital is empty.
The three centre-two electron B-H-B bond formation
involves overlapping the half filled hybridised orbital of one
boron, the empty hybridised orbital of the other boron and
the half filled 1s orbital of hydrogen.
Structure of diborane
11. Write a short note on hydroboration. Diborane reacts with alkenes and alkynes in ether solvent at
room temperature is known as hydroboration
2 6 2 2 3B H + 6RCH = CHR 2B(RCH - CH R)→
12. Give one example for each of the following
i) icosogens ii) tetragen iii) prictogen iv) chalcogen (i) Icosogens - Boron
(ii) Tetragen - Carbon
(iii) prictogen - Nitrogen
(iv) chalcogen - Oxygen
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13. Write a note on metallic nature of p-block elements. The tendency of an element to form a cation by losing
electrons is known as electropositive or metallic character.
On descending the group, the ionization energy decreases
and hence metallic character increases.
In P- block, the elements present in lower part are metals.
In Group 13, all elements are metals except boron which is
metalloid.
In Group 14, tin and lead are metal
In Group 15, Bismuth is metal.
14. Complete the following reactions.
a. ( ) →33B OH + NH
3 3 2800-1200KB(OH) + NH BN + 3H O∆→
Boron Nitride
b. →2 4 7 2 4 2Na B O + H SO + H O
2 4 7 2 4 2 3 3 2 4Na B O + H SO + 5H O 4H BO + 2Na SO→
Boric Acid
c. →2 6 2B H + 2NaOH + 2H O
2 6 2 2 2B H + 2NaOH + 2H O 2NaBO + 6H→
Sodium Meta Borate
d. →2 6 5B H + CH OH
2 6 3 2 3 3 2B H + 6CH OH + H O 2B(OCH ) + 6H→
Trimethyl borate
e. →3 2BF + 9H O
+3 2 3 3 44BF + 3H O H BO + 3H + 3(BF )−→
Boric Acid
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f. →2 4HCOOH + H SO
2 4 2 2 4HCOOH + H SO CO + H O + H SO→
(In this reaction, sulphuric acid is a dehydrating agent)
g. →4 3SiCl + NH 330k
4 3 3 3Ether2SiCl + NH Cl Si NH SiCl→ − −
Chloro siloxone
h. →4 2 5SiCl + C H OH
4 2 5 2 5 4SiCl + 4C H OH Si(OC H ) + 4HCl→
Tetra Ethoxy silane
i. →B + NaOH
3 3 22B + 6NaOH 2Na BO + 3H→
Sodium Borate
j. Red hot→2 4 7H B O Red hot
2 4 7 2 3 2Temperature H B O B O + H O→
Borax bead
15. How will you identify borate radical? When boric acid or borate salt is heated with ethyl alcohol in
presence of Con. Sulphuric acid, trialkyl borate is formed.
The vapour of this ester burns with green edged flame and
this reaction is used to identify the presence of borate
2 4
Con3 3 2 5 2 5 3 2H So
H BO + 3C H OH B(OC H ) + 3H O→
16. Write a note on zeolites. Zeolites are three dimensional crystalline solids containing
aluminum, silicon and oxygen in their regular three dimensional
frame work.
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The general formula is
2 3 2 2NaO(Al O ) x(SiO ) y(H O) (x = 2 to 10, y = 2 to 6)
Zeolites have porous structure in which sodium ions and
water molecules are loosely held.
The silicon and aluminum atoms are tetrahedrally coordinated
with each other through shared oxygen atoms.
Zeolites are similar to clay minerals but they differ in their
crystalline structure.
Zeolites have three dimensional crystalline structure looks
like a honeycomb consisting of a network of inter connected
tunnels and catges.
Water molecules moves freely in and out of these pores but
the zeolites framework remain rigid.
Zeolites are useful to remove permanent hardness of water.
17. How will you convert boric acid to boron nitride?
Fusion of urea with 3B(OH) , in an atmosphere of 800-1200K
gives boron Nitride. 800-1200K
3 3 2B(OH) + NH BN + 3H O→
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.
( ) ( )ndA hydride of 2 period
+ compound of Boron B (Re )alkali metal A
C ducing Agent →
2LiH + B2H6 →2LiBH4
A B C
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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.
( )A double salt Present in
fourth period alkalimetal A
500K B→
500K2 4 2 4 3 2 2 4 2 4 3 2K SO . Al (SO ) .24H O K SO .Al (SO ) + 24H O→
Aqueous solution of (B) + BaCl2 → White Precipitate
2 4 2 4 3 2K SO .Al (SO ) .24H O + BaCl2 → BaSO4
A) Potash Alum - 2 4 2 4 3 2K SO .Al (SO ) .24H O
B) Anhydrous potash alum - 2 4 2 4 3K SO .Al (SO )
20. CO is a reducing agent, justify with an example. Carbon monoxide reduces Iron (III) oxide to Iron. So it is a
powerful reducing agent.
2 3 23CO + Fe O 2Fe + 3CO→
For Complete Materials
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Additional Questions
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UNIT-2: P Block Elements - I
CHOOSE THE BEST ANSWER
1. In borax bead test which compound is formed? (a) Double Oxide (b) Tetra borate (c) Meta-borate (d) Ortho- borate
Ans: (c) Meta-borate 2. The stability of +1 oxidation state increase in the sequence: (a) Al < Ga < In < Tl (b) TI < In < Ga < Al (c) ln < Tl < Ga < Al (d) Ga < In < Al < Tl
Ans: (a) Al < Ga < In < Tl 3. Which one of the following anions is present in the chain
structure of silicates?
(a) 6-2 7Si O (b) 2-
2 5 n(Si O ) (c) 2-3 n(SiO ) (d) 4-
4SiO
Ans: (c)))) 2-3 n(SiO )
4. Which of the following oxide is amphoteric? (a) SiO2 (b) CO2 (c) SnO2 (d) CaO
Ans: (c) SnO2 5. Which of these is not a manomer for a high molecular
mass silicon polymer? (a) MeSiCl3 (b) Me2SiCl2 (c) Me3SiCl (d) PhSiCl-3
Ans: (c) Me3SiCl
TWO AND THREE MARK QUESTION AND ANSWER
1. 18-group elements are called as inert gases why? Write the electronic configuration. In 18-group, the p-orbitals are completely filled and stable due to symmetry.
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They are having less reactivity.
The common electronic configuration is ns2np6.
2. Write the ores of Boron.
Borax ⇒ [ ]2 4 5 4 2Na B O (OH) .8H O
Kernite ⇒ [ ]2 4 5 4 2Na B O (OH) .2H O
3. Write the reduction of Boron trihalides. Reduction of boron trichloride with tungsten at 1500K gives
tungsten boride.
BCl3 + W 2
1500K
H→ WB + Cl2 + HCl
4. Write the action of oxygen with boron on heating? When born is heated with oxygen around 900K gives boron
trioxide.
4B + 3O2 900K→ 2B2O3
5. What is action of boron with acids and bases? Boron does not react with halo acids. But it reacts with sulphuric
acid and Nitric acid gives boric acid.
2B + 3H2SO4 →2H3BO3 + 3SO2
Boron reacts with sodium hydroxide gives sodium borate
2B + 6NaOH →2Na3BO3 + 3H2
6. Write the uses of boron.
1. Isotope of Boron ( )105B is used as moderator in nuclear
reactors.
2. Amorphous Boron is used as rocket fuel igniter
3. Boron is essential for the cell walls of plants
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4. Compounds of boron such as boric acid and borax are used in eye drops, antiseptics, and washing powders.
7. How borax is obtained from its ore? Borax is obtained from colemanite ore by boiling with sodium
carbonate.
2Ca2B6O11+2Na2CO3+H2O∆→3Na2B4O7 + 3CaCO3 + Ca(OH)2
8. What is the action of heat on borax? On heating of borax gives borax beads.
Na2B4O7. 10H2O 2
∆ ∆
2 4 7 2 2 3-10H ONa B O 2NaBO + B O→ →
9. Write the uses of Borax. 1. Borax is used for the identification of coloured metal ions
2. In the manufacture optical and borosilicate glass, enamels and glazes for pottery
3. It is used as a flux in metallurgy and acts as good preservative.
10. Write preparation of Boric acid. Boric acid is prepared by treating borax with sulphuric acid
Na2B
4O
7 + H
2SO
4 + 5H
2O → Na
2SO
4 + 4H
3BO
3
11. What is the action of heat on Boric acid?
H3BO3 373K→ HBO2 + H2O
Boric acid Meta boric acid
H2B4O7 Red Hot
Temp→2B2O3 + H2O
boric anhydride
12. Explain the structure of Boric acid. Boric acid has a two dimensional layered structure.
It consist of [ ]3-
3BO unit.
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These are linked to each other by hydrogen bonds.
Structure of boric acid
13. Write the uses of Boric acid. 1) It is used in the manufacture of pottery glazes. glass,
enamels and pigments.
2) It is used as antiseptic and eye lotion.
3) Used as food preservative.
14. Write the industrial manufacture of diborane? Diborane is obtained by reaction of sodium boro hydride
with Iodine in diglyme.
4 2 2 6 22NaBH + I B H + 2NaI + H→
diborane
15. What is organic benzene? How is it produced? Borazole or borazine is known as inorganic benzene.
Diborane is treated with excess ammonia at high temperature
gives borazole.
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High temperature2 6 3 Closed vessel
3B H + 2NH →B3N3H6
Borozole
16. Write the uses of Diborane? 1) used as a high energy fuel for propellant.
2) used as reducing agent in organic chemistry.
3) used in welding torches.
17. Explain the preparation of boron trifluoride. Calcium fluoride is treated with boron trioxide in presence
of conc. sulphuric acid gives boron trifluoride.
B2O3 + 3CaF2 + 3H2SO4 ∆→2BF3 + 3CaSO4 + 3H2O
18. Give the uses of boron trifluoride 1) used for preparing catalyst HBF4
2) used as fluorinating agent
19. Explain McAfee process of preparation of Aluminium
chloride. By heating a mixture of alumina and coke in a current of
chlorine gives aluminium chloride.
Al2O3 + 3C + 3Cl2 →2AlCl3 + 3CO2
20. Write the uses of aluminium chloride. 1) Anhydrous aluminium chloride is used as catalyst in
Friedal – crafts reaction
2) used for manufacture of petrol by cracking the mineral
oils.
3) used as catalyst for manufacture of dye, drugs and
perfumes
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21. Write the preparation of Alum. When alum stone is treated with excess of sulphuric acid,
the aluminium hydroxide is converted to aluminum sulphate. On adding calculated quantity of potassium sulphate, potash
alum is crystallised.
2 4 2 4 3 3 2 4K SO .Al (SO ) .4Al(OH) + 6H SO →
2 4 2 4 3 2K SO + 3Al (SO ) +12H O
2 4 2 4 3 2K SO + Al (SO ) + 24H O→
2 4 2 4 3 2K SO .Al (SO ) .24H O
22. What Burnt alum? How is it prepared? Potash alum melts on heating at 365K. Further heating at 457K, losses water of hydration and
swells up.
The swollen mass is known as burnt kum 475K
2 4 2 4 3 2 2 4 2 4 3K SO .Al (SO ) .24H O K SO .Al (SO ) +→ 24H2O
Burnt alum
23. Write the uses of alum. 1) used for purification of water 2) used for water proofing and textiles
3) used in dyeing, and leather tanning industries 4) used as a styptic agent to arrest bleeding
24. Graphite conducts electricity why?
Each carbon atom forms three σ bonds with three neighbouring
carbon atoms using three valence electrons and the fourth
electron present in unhybridised ‘p’-orbital forms a π bond.
These π-electrons are delocalised over the entire sheet and
responsible for electrical conductivity.
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25. What are carbon nanotubes? 1. It is an allotrope of carbon.
2. It has graphite like tubes with fullerene ends.
3. The nonotubes are stronger than steel and conduct
electricity.
4. It is used in nanoscale electronics, catalysis, polymers and
medicine.
26. What is producer gas? It is mixture of carbon monoxide and Nitrogen.
27. What is water gas (or) Synthetic gas? It is mixture of carbon monoxide and hydrogen.
28. What is phosgene? How is it prepared? Carbonyl chloride is known as phosgene
When carbon monoxide is treated with chlorire in presence
of light or charcoal, phosgene is obtained.
CO + Cl2 light→COCl2
29. Write the uses of carbon monoxide 1) Water gas (CO+H2) and producer gas (CO + N2) are
important industrial fuels.
2) used as good reducing agent
3) It is an important ligand
30. How silicic esters are prepared? Silicon tetra chloride is treated with alcohols gives silicic
esters.
SiCl4 + 4C2H5OH →Si (OC2H5)4 + 4HCl
Tetra ethoxy silane
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31. Write the uses of silicon tetra chloride. 1) used in the production of semiconducting silicon.
2) used as a starting material in the synthesis of silica gel,
silicic esters.
32. What are silicones? How is it prepared? Silicones or poly siloxanes are organo silicon polymers.
The hydrolysis of dialkylchloro silanes gives silicones
Cl Si
R
R
Cl HO Si
R
R
OH22
2
H O
HCl
+−
33. Explain the types of silicones. (i) Linear silicone: Hydrolysis and subsequent condensation
of dialkyl or diaryl silicon chlorides.
(a) Silicone rubber: Silicones are bridged together by methylene
or similar groups.
(b) Silicone resins: Prepared by blending silicones with organic
resins such as acrylic esters.
(ii) Cyclic silicones: Obtained by hydrolysis of R2SiCl2
(iii) Cross linked silicones: Obtained by hydrolysis of
RSiCl3.
FIVE MARK QUESTION ANSWERS
1. Write the action of heat on diborane at different
temperature? 388K
2 6 5 11 25B H 2B H + 4H→
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198-373K2 62B H →B4H10 + H2
5B2 H6 373
sealed tube
K→ B10 H14 + 8H2
5B2H6 473 523K−→2B5H9 + 6H2
10B2H6 523K→2B5H9 + 2B5H10 + 11H2
B2H6 Red hot
Temp→2B + 3H2
2. Write a note on Diamond. 1. It is an allotrope of carbon
2. The carbon atoms are sp3 hybridised
3. The C-C bond length is 1.54A°
4. The carbon atoms are tetraedrally arranged
5. All four valence electrons of carbon are involved in bonding
and free electrons are not available for conductivity.
6. used for sharpening hard tools, cutting tools, cutting
glasses, making bores and rock drilling.
3. Explain the carbon allotrope fullerenes. 1. It is an allotrope of fullerene
2. C60 molecules have a soccer ball like structure and is
called bucky balls or buck minister fullerene
3. It has a fused ring structure consist of 20 six membered
rings and 12 five membered rings
4. Each carbon atom is sp2 hybridised
5. It forms three σ bonds and a delocalised π bond gives
aromatic character.
6. C-C bond distance is 1.44A° C = C bond distance is 1.38A°
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4. Explain the types of silicates. (Any two types may be
asked in board exam) Silicones are classified into various types based on linking
of tetrahedral units of [SiO4]4-.
1) Ortho silicate (Neso Silicates) The simplest silicates contains discrete [SiO4]
4- tetrahdral units.
Ortho Silicate
2) Pyso silicate or Soro silicate
It contains ( )6-
2 7Si O units.
It is formed by joining two ( )4-
4SiO tetrahedral units by
having one oxygen atoms at one corner.
(E.g) Thortiveitite. Sc2Si2O7
Structure of Pyro silicate
3) Cyclic silicates or Ring silicates
It contains ( )2n-
3 nSiO ions formed by linking three or more
tetrahedral ( )4-
4SiO unit.
Each silicate unit shares two of its oxygen atoms with other units.
(E.g) Beryl Be3 Al2 (SiO3)6
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Structure of Cyclic silicates
4) Iono silicates They contains ‘n’ number of silicate units by sharing two or
more oxygen atoms.
They are classified into two types
a) Chain silicates (or) Pyroxenes: They contain [ ]2n-
3 n(SiO )
ions formed by ‘n’ number of tetrahedral (SiO4)4- units linearly.
Each silicate unit shares two of its oxygen atoms with other
unit (E.g) spodumene LiAl(SiO3)2.
Structure of Chain silicates
b) Double chain silicates or amphiboles
It contains ( )6n-
4 11 nSi O ions. It is classified into two types
(i) Those sharing 3 vertices.
(ii) Those sharing only 2 vertices.
(E.g) Asbestos
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Structure of Double chain silicates
5) Sheet silicates or phyllo silicates
It contains ( )2n-
2 5 nSi O
Each ( )4-
4SiO tetrahedron units shares three oxygen atoms
with others.
It forms two dimensional sheets.
Structure of Sheet or phyllo silicates
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6) Three dimensional silicates All oxygen atoms of (SiO4)
2- tetrahedra are share with other
tetrahedra to form three – dimensional net work.
They have general formule (SiO2)n
(E.g) Quartz
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