padasalai trbtnpsc …...jun 12, 2019 · unit 2 p- block elements answer the following questions:...
TRANSCRIPT
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
14
UNIT 2 p- BLOCK ELEMENTS
Answer the following questions:
1. Write a short note on anamolous properties of the first element of p-block.
In p-block elements, the first member of each group differs from the other elements of the
corresponding group. The factors responsible for this anomalous behaviour are
1. Small size of the first member
2. High ionisation enthalpy and high electronegativity
3. Absence of d orbitals in their valance shell
2. Describe briefly allotropism in p- block elements with specific reference to carbon.
Some elements exist in more than one crystalline or molecular forms in the same physical
state. For example, carbon exists as diamond and graphite. This phenomenon is called
allotropism and the different forms of an element are called allotropes.
3. Boron does not react directly with hydrogen. Suggest one method to prepare diborane
from BF3.
• Boron does not react directly with hydrogen.
• But, it forms a variety of hydrides called boranes.
• The simplest borane is diborane - B2H6. Other larger boranes are prepared from this
diborane.
• Gaseous boron trifluoride with sodium hydride around 450 K gives diborane.
• To prevent subsequent pyrolysis, the product diborane is trapped immediately.
450 K
2BF3 + 6NaH B2H6 + 6NaF
4. Give 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 also used as a flux in metallurgy and also acts as a good preservative
5. What is catenation ? describe briefly the catenation property of carbon.
Catenation is an ability of an element to form chain of atoms.
The following conditions are necessary for catenation.
i. the valency of element is greater than or equal to two,
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
15
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.
v.Carbon possesses all the above properties and forms a wide range of compounds with itself
and with other elements such as H, O, N, S and halogens.
6. Write a note on Fisher tropsch synthesis. Fischer Tropsch synthesis:
The reaction of carbon monoxide with hydrogen at a pressure of less than 50 atm using
metal catalysts at 500 - 700 K yields saturated and unsaturated hydrocarbons.
nCO + (2n+1)H2 CnH(2n+2) + nH2O
nCO + 2nH2 CnH2n + nH2O
Carbon monoxide forms numerous complex compounds with transition metals in which the
transition meal is in zero oxidation state. These compounds are obtained by heating the metal
with carbon monoxide.
Eg. Nickel tetracarbonyl [Ni(CO)4], Iron pentacarbonyl [Fe(CO)5], Chromium hexacarbonyl
[Cr(CO)6].
7. Give the structure of CO and CO2.
Structure of CO
• It has a linear structure. In carbon monoxide, three electron pairs are shared between carbon
and oxygen.
• The C-O bond distance is 1.128Å.
• The structure can be considered as the resonance hybrid of the following two canonical
forms.
Structure of CO2 :
Carbon dioxide has a liner structure with equal bond distance for the both C-O bonds.
In this molecule there is one C-O sigma bond. In addition there is 3c-4e bond covering all the
three atoms.
C CO
_+ ..
:..
:
..
..O C O
+_
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
16
8. Give the uses of silicones.
1. Silicones are used for low temperature lubrication and in vacuum pumps and 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 is electron deficient. It has three electrons in its valence shell.
• So when it forms a covalent compound with chlorine it forms three single bonds with
chlorine.
• It doesn't form an octet by doing so thus it can take two more electrons by forming a
coordinate bond to become an octet
• Thus it behaves as Lewis acid.
• Lewis acid is an electron donor
10. Write a short note on hydroboration.
• hydroboration is the addition of a hydrogen-boron bond to C-C, C-N, and C-O double
bonds, as well as C-C triple bonds
• Diborane adds on to alkenes and alkynes in ether solvent at room temperature. This reaction
is called hydroboration and is highly used in synthetic organic chemistry, especially for anti
Markovnikov addition.
B2H6 + 6 RCH = CHR 2 B(CH - CHR)3
11. Describe the structure of diborane.
• In diborane two BH2 units are linked by two bridged hydrogens.
• Therefore, it has eight B-H bonds.
C CO
+ _..
:
..:
..OCO
O
_
:
+
....O: O ::
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
• Diborane has only 12 valance electrons
• The four terminal B-H bonds are normal covalent bonds
• Hence, these bonds are two
• The remaining four electrons
• Hence, these bonds are three centre
• The bridging hydrogen atoms are in a plane as shown in the figure.
• In diborne, the boron is sp3
• 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
• It leaves one empty and one half
• The Three centre - two electron bridging bond H
half filled hybridised orbital of
boron and the half filled 1s orbital of
12. Give one example for each of the following
(i) Icosogens Eg. B
(iii) Prictogen Eg. N
13. Write a note on metallic nature of p
Along the period the metallic character decreases
It is because on moving across the period, the atomic size decreases due to the increased nuclear
charge and hence, ionization energy increases.
On moving down the group the metallic character increases
It is because on moving down a group, the atomic size increases.
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
17
iborane has only 12 valance electrons
H bonds are normal covalent bonds.
two centre- two electron bonds. (2c-2e bond).
The remaining four electrons are used for bridging . (B-H-B )
Hence, these bonds are three centre- two electron bonds. (3c-2e bond).
The bridging hydrogen atoms are in a plane as shown in the figure. . 3 hybridised.
hybridised orbitals contains single electron and the fourth orbital is
Two of the half filled hybridised orbitals of each boron overlap with the two hydrogens
2e bonds.
one empty and one half filled hybridised orbitals on each boron.
two electron bridging bond H-B-H, is formed by the
half filled hybridised orbital of one boron, the empty hybridised orbital of the
1s orbital of hydrogen.
12. Give one example for each of the following
(ii) Tetragen Eg. C
(iv) Chalcogen Eg. O
13. Write a note on metallic nature of p-block elements.
he metallic character decreases.
It is because on moving across the period, the atomic size decreases due to the increased nuclear
charge and hence, ionization energy increases.
he metallic character increases.
It is because on moving down a group, the atomic size increases.
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
hybridised orbitals contains single electron and the fourth orbital is
Two of the half filled hybridised orbitals of each boron overlap with the two hydrogens
is formed by the overlap of the
, the empty hybridised orbital of the other
It is because on moving across the period, the atomic size decreases due to the increased nuclear
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
18
As a result the ionization energy decreases and tendency to lose electrons increases. Therefore,
metallic character increases
14. Complete the following reactions
∆
a B(OH)3 + NH3 BN + 3H2O
b. Na2B4O7 + H2SO4 + 5H2O 4H3BO3 + 2Na2SO4
c. B2H6 + 2NaOH +2H2 O 2NaBO2 + 6H2
d. 4BF3 + 9H2O 4H3BO3 + 3H+ + 3[BF4]- e. B2H6 + 6CH3 OH 2B(OCH3)3 + 6H2
f HCOOH + H2SO4 CO + H2O + H2SO4 330 K g. 2SiCl4 + NH3 Cl3 Si-NH-SiCl3 Ether h SiCl4 + C2H5OH Si(OC2H5)4 + 2Cl2 Tetraethoxy silane i. 2B + 6NaOH 2Na3BO3 + 3H2 Red hot j. H2B4O7 2B2O3 + H2O
15. How will you identify borate radical?
When boric acid or borate salt is heated with ethyl alcohol in presence of conc. sulphuric
acid, an ester, is formed. The vapour of this ester burns with a green edged flame and this
reaction is used to identify the presence of borate.
4H3BO3 + 3C2H5OH B(OC2H5)3 + 3H2O ethyl borate
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
NaO.(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.
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
19
• The Si and Al 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 a three dimensional crystalline structure looks like a honeycomb 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.
• Another special aspect of this structure is that 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 B(OH)3, in an atmosphere of ammonia at 800 - 1200 K gives boron nitride.
B(OH)3 + NH3 BN + 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.
• A hydride of 2nd period alkali metal (lithium) that is lithium hydride
• It reacts with compound of Boron that is boron tri fluoride to give a lithium
borohydride as a reducing agent and lithium fluoride.
• Lithium borohydride is used in organic synthesis as a reducing agent for esters.
The balanced chemical reaction will be,
4Li H + BF3 LiBH4 + 3 LiF
Result: A = lithium hydride , B= boron trifluoride , C = 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.
A double salt which contains fourth group alkali metal is Potash alum (A) on heating at 500K
loses water of hydration and swells up and gives burnt alum(B) Due to the presence of sulphate
ions B gives white precipitate with BaCl2 and the same contains aluminium ion and hence gives
red colour with alizarin
500 K
K2SO4 .Al2(SO4)3.24 H2O K2SO4.Al2(SO4)3 + 24 H2 O
20. CO is a reducing agent . justify with an example.
Carbon monoxide acts as a strong reducing agent. It reduces iron oxide to iron
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
20
CO + Fe2O3 2Fe + 3CO2
21. What are the uses of boron
1. Boron has the capacity to absorb neutrons. Hence, its isotope 10B5 is used as moderator in
nuclear reactors.
2. Amorphous boron is used as a rocket fuel igniter.
3. Boron is essential for the cell walls of plants.
4. Eye drops, antiseptics and washing powders contain boric acid and borax.
5. In the manufacture of Pyrex glass, boric oxide is used.
22. What is inert pair effect ?
In heavier post-transition metals, the outer s electrons (ns) have a tendency to remain inert and
show reluctance to take part in the bonding, which is known as inert pair effect. This effect is
also observed in groups 14, 15 and 16.
23 How is borax prepared? Mention its form
Borax is a sodium salt of tetraboric acid.
It is obtained from colemanite ore by boiling its solution with sodium carbonate.
2Ca2B6O11 + 2NaCO3 + H2O 3Na2B4O7 + 3CaCO3 + Ca(OH)2
Borax is normally formulated as Na2B4O7.10H2O.
Borax exists as prismatic form, jeweller or octahderal borax (Na2B4O7.5H2O) and borax glass
(Na2B4O7).
24. Explain the structure of boric acid.
Boric acid has a two dimensional layered structure. It consists of [BO3]3- unit and
these are linked to each other by hydrogen bonds as shown in the Figure
25. What are the Uses of boric acid?
1. Boric acid is used in the manufacture of pottery glazes, glass, enamels and pigments.
2. It is used as an antiseptic and as an eye lotion.
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
3. It is also used as a food preservative
26. What is alum how is it prepared from alunite?
• The name alum is given to the double salt of potassium aluminium sulphate
• K2SO4. Al2(SO4)3.24.H2O
• The alunite is the naturally occurring form and it is K
• When it is treated with excess of sulphuric acid, the aluminium hydroxide is converted to
aluminium sulphate.
• A calculated quality of potassium sulphate is added and the solution is crystallised to
generate potash alum.
• It is purified by recrystallisation.
K2SO4. Al2(SO4)3 .4Al(OH)
K2SO4 + Al2(SO4)3
27. Give the Uses of Alum.
1. It is used for purification of water
2. It is also used for water proofing and textiles
3. It is used in dyeing, paper and leather tanning industries
4. It is employed as a styptic agent to arrest bleeding.
28. Write note on graphite and diamond.
Graphite is soft and conducts electricity.
• It is composed of flat two dimensional sheets of ca
• Each sheet is a hexagonal net of sp
• Carbon atoms are with a C-C bond length of 1.41 Å
• Each carbon atom forms three
neighbouring carbon atoms using three of its valence
electrons .
• The fourth electron present in the unhybridised p orbital
forms a π-bond.
• These π electrons are delocalised
its electrical conductivity.
• The successive carbon sheets are held together by weak van der Waals forces.
• The distance between successive sheet is 3.40 Å.
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
21
3. It is also used as a food preservative.
prepared from alunite?
The name alum is given to the double salt of potassium aluminium sulphate
is the naturally occurring form and it is K2SO4. Al2(SO4)3.4Al(OH)
is treated with excess of sulphuric acid, the aluminium hydroxide is converted to
A calculated quality of potassium sulphate is added and the solution is crystallised to
It is purified by recrystallisation.
.4Al(OH)3 + 6H2SO4 K2SO4 + Al2(SO4)3 + 12 H
3 + 24 H2O K2SO4.Al2(SO4)3.24 H2O
1. It is used for purification of water
2. It is also used for water proofing and textiles
3. It is used in dyeing, paper and leather tanning industries
4. It is employed as a styptic agent to arrest bleeding.
Write note on graphite and diamond.
is soft and conducts electricity.
It is composed of flat two dimensional sheets of carbon atoms.
Each sheet is a hexagonal net of sp2 hybridised
C bond length of 1.41 Å
Each carbon atom forms three σ bonds with three
neighbouring carbon atoms using three of its valence
fourth electron present in the unhybridised p orbital
electrons are delocalised and it is responsible for
The successive carbon sheets are held together by weak van der Waals forces.
ween successive sheet is 3.40 Å.
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
.4Al(OH)3.
is treated with excess of sulphuric acid, the aluminium hydroxide is converted to
A calculated quality of potassium sulphate is added and the solution is crystallised to
+ 12 H2O
O
The successive carbon sheets are held together by weak van der Waals forces.
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
• It is used as a lubricant either on its own or as a graphited oil.
• Diamond is very hard.
• The carbon atoms in diamond are sp
atoms by σ bonds with a C-C bond length of 1.54 Å.
• This results in a tetrahedral arrangement around each
carbon atom that extends to the entire lattice
• Since all four valance electrons of carbon are
involved in bonding there is no free electrons for
conductivity.
• Being the hardest element, it used for sharpening hard
tools, cutting glasses, making bores and rock drilling
29. Explain the structure of Fullerenes
• Fullerenes are discrete molecules such as C
• These molecules have cage like structures
• The C60 molecules have a soccer ball like structure and is called
buckminster or buckyballs.
• It has a fused ring structure consists of 20 six membered rings
and 12 five membered rings.
• Each carbon atom is sp2 hybridised and forms thee
delocalised π bond giving aromatic character to these molecules.
• The C-C bond distance is 1.44 Å and C=C distance is 1.38 Å.
30. Distinguish between graphite and diamond
S.NO. Graphite
1 Graphite is soft and conducts electricity.
2 The carbon atoms in graphite
hybridised
3 C-C bond length is 1.41 Å
4 These π electrons are delocalised
it is responsible for its electrical
conductivity
5 It is used as a lubricant either on
own or as a graphited oil.
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
22
It is used as a lubricant either on its own or as a graphited oil.
The carbon atoms in diamond are sp3 hybridised and bonded to four neighbouring carbon
C bond length of 1.54 Å.
This results in a tetrahedral arrangement around each
carbon atom that extends to the entire lattice
Since all four valance electrons of carbon are
ed in bonding there is no free electrons for
Being the hardest element, it used for sharpening hard
tools, cutting glasses, making bores and rock drilling.
Explain the structure of Fullerenes
are discrete molecules such as C32, C50, C60, C70, C76 etc.
These molecules have cage like structures
molecules have a soccer ball like structure and is called
It has a fused ring structure consists of 20 six membered rings
hybridised and forms thee σ bonds & a
bond giving aromatic character to these molecules.
C bond distance is 1.44 Å and C=C distance is 1.38 Å.
30. Distinguish between graphite and diamond
Diamond
is soft and conducts Diamond is very hard. and does not conduct electricity.
graphite are sp2 The carbon atoms in diamond are sp
hybridised
1.41 Å C-C bond length is 1.54 Å
electrons are delocalised and
is responsible for its electrical
Valance electrons of carbon are involved in
bonding there is no free electrons for
conductivity.
It is used as a lubricant either on its
It used for sharpening hard tools, cutting
glasses, making bores and rock drilling
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
hybridised and bonded to four neighbouring carbon
does not conduct
The carbon atoms in diamond are sp3
alance electrons of carbon are involved in
bonding there is no free electrons for
It used for sharpening hard tools, cutting
glasses, making bores and rock drilling
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
31. Write note on nanotubes and graphene
Carbon nanotubes, have graphite like tubes with fullerene ends.
Along the axis, these nanotubes are stronger than steel
They conduct electricity.
They have many applications in nanoscale electronics, catalysis,
polymers and medicine.
Another allotrophic form of carbon is
It has a single planar sheet of sp2 hybridised carbon atoms
They are densely packed in a honeycomb crystal lattice.
32.What are the uses of carbondioxide
1. Carbon dioxide is used to produce an inert atomosphere for chemical processing.
2. Biologically, it is important for photosynthesis.
3. It is also used as fire extinguisher and as a propellent gas.
4. It is used in the production of carbonated beverages and in the production of foam.
33. What are Silcones?
Silicones or poly siloxanes are organo silicon polymers with general empirical
This formula is similar to that of ketone (R
These silicones may be linear or cross linked.
Because of their very high thermal stability they are called
34. How are Silcones prepared?
Silicones are prepared by the hydrolysis of dialkyldichlorosilanes (R
diaryldichlorosilanes Ar2SiCl2, which are prepared by passing vapours of RCl or ArCl over
silicon at 570 K with copper as a catalyst.
2RCl+
The hydrolysis of dialkylchloro silanes R
from both the sides
Cl Si
R
__ __
R
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
23
and graphene
have graphite like tubes with fullerene ends.
are stronger than steel.
have many applications in nanoscale electronics, catalysis,
Another allotrophic form of carbon is graphene.
hybridised carbon atoms
are densely packed in a honeycomb crystal lattice.
uses of carbondioxide?
1. Carbon dioxide is used to produce an inert atomosphere for chemical processing.
2. Biologically, it is important for photosynthesis.
3. It is also used as fire extinguisher and as a propellent gas.
4. It is used in the production of carbonated beverages and in the production of foam.
Silicones or poly siloxanes are organo silicon polymers with general empirical formula (R
formula is similar to that of ketone (R2CO), they were named “silicones”.
These silicones may be linear or cross linked.
Because of their very high thermal stability they are called as high –temperature polymers.
Silcones prepared?
Silicones are prepared by the hydrolysis of dialkyldichlorosilanes (R
, which are prepared by passing vapours of RCl or ArCl over
silicon at 570 K with copper as a catalyst.
Cu / 570 K 2RCl+ Si R2SiCl2
The hydrolysis of dialkylchloro silanes R2SiCl2 yields to a straight chain polymer which
H2O
-2HCl
Cl Si
R
__ __
R
HO OH
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
1. Carbon dioxide is used to produce an inert atomosphere for chemical processing.
4. It is used in the production of carbonated beverages and in the production of foam.
formula (R2SiO).
temperature polymers.
Silicones are prepared by the hydrolysis of dialkyldichlorosilanes (R2SiCl2) or
, which are prepared by passing vapours of RCl or ArCl over
yields to a straight chain polymer which grown
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
24
The hydrolysis of monoalkylchloro silanes RSiCl3 yields to a very complex cross linked
polymer.
Linear silicones can be converted into cyclic or ring silicones when water molecules is removed
from the terminal –OH groups.
35. Mention the Uses of silicones
1. Silicones are used for low temperature lubrication
2 They are used in vacuum pumps and in high temperature oil baths.
3. They are used for making water proofing clothes
4. They are used as insulting material in electrical motor and other appliances
5. They are mixed with paints and enamels to make them resistant towards high temperature,
sunlight, dampness and chemicals.
36. What are the types of silicates ?
The mineral which contains silicon and oxygen in tetrahedral [SiO4]4- units linked together
in different patterns are called silicates.
SiO
R
__ __
R
HO OH Si
R
__ __
R
Si
R
__ __
R
OHHO
- H2O
Si
R
__ __
R
HO OH+
OSi
R
__ __
R
Si
R
__ __
R
HO
+ Si
R
__ __
R
HO OH
Si
R
__ __
R
OHOEtc.
- H2O
Si__ __
Si__ __
O
Me
O
O __
Si__ __
Si__
O
Me
Me
Me
MeMe
Me
Me
Si__ __
Si__ __
O
Me
O
O__
Si__ __
Si__
O
Me
Me
Me
MeMe
Me
Me
O
Si
Me
Me
Si
Me
MeO O
Si
MeMe
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Padasalai TrbTnpsc
+2 CHEMISTRY Dr. C. ARUL JOSEPH RAJ
25
1.Ortho silicates (Neso silicates) 2. Pyro silicate (or) Soro silicates) 3. Cyclic silicates (or
Ring silicates) 4. Inosilicates : 5. Double chain silicates (or amphiboles) 6. Sheet or phyllo
silicates 8. Asbestos 9. Three dimensional silicates (or tecto silicates)
&&&&&&&&&&
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