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NAUMAN AHMAD
Lecturer Chemistry
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SOLID STATE
CHEMISTRY
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contents
• Introduction• Types of solids• Crystal Structures
• Elements of Symmetry• Bragg’s equation• Allotropes of carbon: Diamond, grapite !
"ullerene
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INTRODUCTION
Tree pases of matter: #as
$iquid Solid
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#asmolecules
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$iquid
molecules
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Solidmolecules
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What is solid?
• Definite sape%• Definite &olume%• 'igly incompressible%
• (igid%• Constituent particles eld closely by strong
intermolecular forces%
• "i)ed position of constituents%
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TYPES OF SOLIDS
T*o types +based upon atomic arrangement, binding energy, pysical ! cemical properties:
-% Crystalline.% Amorpous
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C!stalline solids
• Te building constituents arrange temsel&es in regularmanner trougout te entire tree dimensional net*or/%
• E)istence of crystalline lattice%• A crystalline lattice is a solid figure *ic as a definite
geometrical sape, *it flat faces and sarp edges%• Incompressible orderly arranged units%• Definite sarp melting point%•
Anisotropy%• Definite geometry%• #i&e )0ray diffraction bands%• E)amples: 1aCl, CsCl, etc%
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AMORPHOUS SOLIDS
• Deri&ed from #ree/ *ord 23morpe’ meaningsapeless%
• 1o regular but apa4ard arrangement of atoms ormolecules%
• Also considered as non0crystalline solids or super0cooled liquids%• 1o sarp m%p%• Isotropic%• 1o definite geometrical sape%• Do not gi&e )0ray diffraction bands%• E)amples: glass, rubber, plastics%
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T!"es o# c!stal st$ct$es
• Ionic crystals• Co&alent crystals• 5olecular crystals
• 5etallic crystals
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Ionic c!stals• $attice points are occupied by positi&e and negati&e ions%
• 'ard and brittle solids%• 'ig m%p% due to &ery strong electrostatic forces of
attraction%• 6oor conductors of electricity in solid state but good in
molten state%• 6ac/ing of speres depends upon:
presence of carged species present%
difference in te si4e of anions and cations%• T*o types: AB types% AB. types%
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Co%alent c!stals
• $attice points are occupied by neutral atoms%• Atoms are eld togeter by co&alent bonds• 'ard solids%
• 'ig m%p%• 6oor conductors of electricity%• T*o common e)amples: diamond ! grapite%
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Molec$la c!stals
• $attice points are occupied by neutral molecules%• Te molecules are eld togeter by &ander
7aal’s forces%
• 8ery soft solids%• $o* m%p%• 6oor conductors of electricity%
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Metallic c!stals
•
$attice points are occupied by positi&e metal ionssurrounded by a sea of mobile e0% • Soft to &ery ard%• 5etals a&e ig tensile strengt%
• #ood conductors of electricity%• 5alleable and ductile%• Bonding electrons in metals remain delocali4ed o&er
te entire crystal%• 'ig density%
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La&s o# s!''et!
• 6lane of symmetry•
Centre of symmetry• A)is of symmetry%
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Ele'ents o# s!''et!in c$(ic c!stal
• (ectangular planes of symmetry: 9• Diagonal planes of symmetry: •
A)es of four0fold symmetry: 9• A)es of tree0fold symmetry: ;• A)es of t*o0fold symmetry:
• Centre of symmetry: - Total symmetry elements: 23
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Planes o# s!''et!
(ectangular plane ofsymmetry: 9 Diagonal plane ofsymmetry:
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A)is o# s!''et!
"our0fold a)is ofsymmetry: 9 Tree0fold a)is ofsymmetry: ;
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A)is * cente o# s!''et!
T*o0fold a)is ofsymmetry: Centre of symmetry: -
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T!"es o# c$(ic c!stals
"our types:-% Simple or primiti&e type.% Body0centered
9% "ace0centered;% End face0centered
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Simple or primiti&e type +sc Body0centered cell +bcc
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"ace0centered cell +fcc End face0centered cell
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N$'(e o# ato's "e $nit cellin a c$(ic lattice
• Simple cubic cell: -atom
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Simple cube
No of atoms per unit cell= 8 x 1/8=
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No of atoms per unit cell= 8 x 1/8 =
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Simple cubic arrangement
e.g.Polonium52% of the space is occupied by the atoms
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Body centered cubic lattice
No of atoms present per unit cell
= (8 x 1/8 ) + (1 x
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No of atoms per unit cell= (8 x 1/8) +1= 2
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Body centered cubic lattice
e.g. CsCl, CsBr
68% of the space is occupied by the atoms
" d bi l i
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"ace0centered cubic lattice
No of atoms present per unit cell
= (8 x 1/8 ) + (6 x
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"ace0centered cubic lattice
e.g. NaCl, NaF, KBr, MgO
74% of the space is occupied by the atoms
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End face0centered cubic lattice
# ato's "esent "e $nit cell
+ - ) . - 1 2 ) . 2 +
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Ato'ic adi$s o# a c$(ic lattice
• Simple cubic cell:r = a
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Radi$s atio $le
• (elation bet*een te radius, co0ordinationnumber and te structural arrangement of temolecule%
(adius ratio =
• #reater te radius ratio, larger te si4e of te
cation and ence te co0ordination number%
E l # di3 t t l
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E)a'"les o# di3eent c!stals!ste's
S.No. System Example
-% Cubic 1aCl, Cl, Ca"., Cu, nS, CsCl, Cu.3
.% 3rtorombic BaS3;, 139, 5gSi39, .S3;, CdS3;,AgBr
9% Tetragonal Sn3., Ti3., rSi3; ;% 5onoclinic CaS3;%.'.3, monoclinic S
% Triclinic CuS3;%'.3, 1a'S3;, '9639
% 'e)agonal 6bI., 5g, Cd, n, n3, B1, Si3., 'gS,CdS
% (omboedral or Trigonal #rapite, ICl, Al.39, calcite +CaC39, As,Sb, Bi
C bi l tti
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Cubic lattice
O th h bi l tti
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Orthorhombic lattice
T t l l tti
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Tetragonal lattices
li i l tti
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onoclinic lattice
T i li i l tti
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Triclinic lattice
!e agonal lattice
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!exagonal lattice
"hombohe#ral $Trigonal% lattice
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"hombohe#ral $Trigonal% lattice
St$ct$es o# i'"otant ionic
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St$ct$es o# i'"otant ionicco'"o$nds
-% AB type: 1aCl +roc/ salt CsCl nS +4inc blende < spalerite
.% AB. type: Ca". +fluorite
Ti3. +rutile
Si3.
# l , 4
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• "CC type%
• Co0ordination number :%
• Calculation o& no. o& atoms o&
NaCl'unitcell:Cl at corners: +? × -
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St$ct$e o# sodi$' choide
uic unit cell!mallest repeatale unit
Structure o& CsCl
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Structure o& CsCl
• bcc type%
• Co0ordination number ?:?%• 1umber of atoms
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Structure o& (nS •
fcc type%• Co0ordination number
;:;%• Calculation o& no. o&atoms'unit cell:
Total S = ?)-
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Structure o& Ca)2
• fcc type%• Co0ordination number: ?:;
+? for cation, ; for anion
G1ote: All te compounds of AB. type follo* te same pattern%
"#
Ca+
Structure o& * O
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Structure o& * 2O
• fcc type%• Co0ordination number: ;:?
; for cation ? for anion
Na+
$ #2
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St$ct$e o# i'"otantco%alent co'"o$nds
-% Diamond.% #rapite
%iamon&
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%iamon&
'tructure of &iamon&
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'tructure of &iamon&• fcc type%•
Tetraedral• C0C bond lengt = -%9;A• (efracti&e inde) = .%;
• 'ig dispersi&e po*er of ligt• 1on0conductor of electricity• 9d net*or/
• 'ardest substance e&er /no*n%• sed as abrasi&e%
3#+ structure o& #iamon#
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3#+ structure o& #iamon#
raphite
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raphite
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Structure o& raphite
•
3ne of te softest substances e&er /no*n%• .0d e)agonal layer structure• C0C bond lengt = -%;A• Inter layer distance = 9%;A• Sliding nature• sp. ybridisation *it one electron left o&er%• Specific gra&ity .%.• Electrical conductor • 5etallic lustre• sed as good lubricant%
2#+ structure o& graphite
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2#+ structure o& graphite