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3. plasma
Bonse einstein
condensate
Fermionic
condensate
Quark condensate
thought wave

4. By changing T and P it is interconvertable.

5. Characteristics of solid

6. -Ice has hexagonal 3D crystal structure formed due to to
intermolecular H-Bonding which leave almost half the space
vacant.
-Both ice and water structure almost same.
-On melting of ice some H-bond are broken and vacant spaces
are occupied by water molecules, and they are joint more
closely.
-In solid ice, vacant space is
more then liquid water.
-Therefore the
density of ice is less then
water.

7. moderate

10. Characteristics of solid
1. Solid fixed composition- has fixed mass, volume,
shape and Density. Order of density: Solid >Liquid
>Gas. Exception: Dice < Dwater
2. in solids- Intermolecular distance is shortest. hence
solid are incomopressible.
3. Solid are HARD and .
4. Solid have strongest intermolecular force of
attraction.
-Solid with weak IMF - Low M.P.
-Solid with strong IMF - high M.P.
5. Soilid fixed position and posses Oscillatory motion.
becouse of low thermal energy- means Temperature.
Soild with weak IMF - Thermal energy high.
Soild with strong IMF- Thermal energy low.

11. Classification Solid
Crytalline Solid Amorphous Solid
Greek - No formGreek- Stone
Eg:- Metals And
Non metals
Eg: Rubber ,Glass
,Plastic

12. What is the
common
formula of
salt?
NaCl

13. How is
Na+ and
Cl- are
arrange.

14. Such
arrange
ment is
been
observed
in
crystallin
e solid.
3D figure

15. This
structure
also
represent
in
different
form..

17. It represent
continuity.

38. Why is glass considered a supercooled liquid?
Ans: Glass is an amorphous solid. Like liquids, it has a tendency to
flow, though very slowly. This can be seen from the glass panes of
windows or doors of very old buildings which are thickerat the bottom
than at the top. Therefore, glass is considered as a supercooled liquid.
Glass are the transparant
medium obtain by fuseing
together SiO2, Na2O, B2O3.
Amorphouse
solid.
800 varities of
glass.

39. Composition
of Glass
Quartz
Glass/Silica gel
Green Glass
Blue GlassYellow GlassRed Glass
Sodalime
Glass
Pyrex Glass
60-80% SiO2+10-
25% B2O3+ Al2O3.
75% SiO2+15% Na2O
+ 10% CaO.
SiO2+trace amount
Cu & Au
SiO2 + UO2. SiO2 + CuO/CoO.
SiO2 +
CuO/Fe2O3.
SiO2

40. constituent particles are
atoms. closely packed
atoms by London forces.
eg. noble gases. soft,
low M.P and poor
conductor.

41. Dry ice (solid,
methane

44. Bonding in Ice and Water
-Structure of liquid water and solid ice are almost identical.
-ice has hexagonal 3D crystal structure formed due to H-bonding.
-Each O-H bond is polar, hence H2O is polar molecule. contain dipole
dipole interaction.
-in ice, H2O molecules are linked forming a tetrahedral arrangement.
-in this arrangement, 2 covalently bonded H-atom and 2 H-atoms
bonded by H-bonding are at 4 corners of the tetrahedral.
O
H
H
HH

47. In this structure
No. of Na+ = No. of
Cl-

48. If we look at any one
face of NaCl structure.

53. Crystal undergo distortion and fractured. by shearing force.

54. Covalent Solid-
Carbon are in 3 allotropes form

73. M ion(kernel)

74. Cations in
electron cloud

75. All metallic
elements,
for example,
Cu, Fe, Zn

76. Unit cell and Crystal
lattice

82. Primitive and its variation
with centred unit cell

89. Cubic Unit Cell

97. Packing of Solid

107. Note- the no.
of hole are
double.

112. Voids are free
space or empty
space or holes
present in the
crystal.

128. how many
NaCl
molecule is
present in
one unit
cell?
No. of Na atom = 4

136. rCs

137. Packing efficiency in cubic unit cell

139. r
a

141. No . Of fcc is 4.

142. Relation for the density of unit cell
In a cubic crystal, let
a = Edge length of the unit cell.
d = Density of the solid substance.
M = Molar mass of the substance.
Then, volume of the unit cell = a3
Again, let
z = Number of atoms present in
one unit cell
m = Mass of each atom
mass of the unit cell = Number of atoms
in the unit cell × Mass of each atom
= z × m
But, mass of an atom, m
Therefore, density of the unit
cell,

143. Defects in Crystal

148. This defect cause
by absence of
cation and anion.
Schottky defect
Eg. NaCl, KCl, CsCl

150. It is due to cation
or anion leaves
there regular site
and moves to
occupy the
interstitial site.

151. The density of
crystal is an altered.

153. Impurity
defect change
the original
properties of
Crystalline
solid
Substitution Intertitial

158. Electrical properties and
Band theory

161. Eg. Silicon
The variation inthe electerical properties of solid
can be explain on the basis of band theroy.

162. Lets take an
example of Mg

165. Distribution of
electrons can
be written as

166. Distribution of
electrons can
be written like
this

167. Let us
consider 1
more Mg
atom
The 2 atom of Mg
interact with each
other

178. Conduction band
either empty or
partially
completely filled.

179. Depending on this
energy gap,
generally there
can be three type
of solids…

180. On the basis of electrical conductivity the solids can be
classified into three types

191. Atomic no.- 14
E.C.-
1s2,2s2,2p6,3s2,3p2
Valency- 4

193. In this solid
structure
there is only
one free
electron.

194. Here in the
given solid,
1 atom
contributes
1 free
electron.

195. Thus Due to large no. of
negative charge electron
present, is called n-type
semi conductor.

203. Magnetic properties of solid

207. Magnetic Properties of solid

212. Example- Fe3O3, Fe3O4 (magnetite), ferrites such as MgFe2O4 and
ZnFe2O4.
Substance which are expected to posses large magnetism on the
basis of the unpaired electrons but actually have small net magnetic
moments are called Ferrimagnetic substances.
Ferrimagnetic substances are weakly attracted by a magnetic
field as compared to ferromagnetic substances.
On heating, these substances become paramagnetic.

213. Anti-ferromagnetism
Substances which are expected to possess paramagnetism
or Ferromagnetism on the basis of unpaired electron but
actually they posses zero net magnetic moment are called
anti Ferromagnetic substances.
e.g. MnO, Mn2O3, MnO2.

220. Dielectric
properties

221. High electric resistivities but good supporter of electric field.
This is due to the reason that electrons in a dielectric substances are
tightly pack to each other.
Can store energy /charges.
Polarization takes place because nuclei are attracted to one side and
the electron cloud to the other side.
There may also be permanent dipoles in the crystal called Dipole
Dipole interaction.
Dielectric properties
Since the molecule is linear, these two bond dipoles cancel each other
out then overall dipole moment ( μ=0).

222. Electric field generate
Electric field generate Electric field generate

223. Piezoelectricity (or pressure electricity)
Conversely, if electric field is applied to such crystals, atomic
displacement takes place resulting into mechanical strain. This is
sometimes called Inverse piezoelectric effect.

224. ammonium dihydrogen phosphate (NH4H2PO4) and quartz.
The crystals are used as pick – ups in record
players where they produce electrical signals
by application of pressure.
titanates of barium and lead, lead zirconate
(PbZrO3) - It is used in capacitors,
electromechanical transducers(converts an
electrical signal into sound waves (as in a
loudspeaker) or converts a sound wave into
an electrical signal (as in the
microphone,ultrasonic generators and sonar
detectors). and nonlinear optics.

225. It is a Greek word derived, means electricity generated by heat.
Some piezoelectric crystals when heated or cooled produce a small
electric current. The electricity thus produced is called
pyroelectricity.
Pyroelectricity:
TV switch Temporary
voltage stored karte hai.

226. e.g. Barium titanate (BaTiO3) sodium potassium tartarate (Rochelle
salt) and potassium dihydrogen phosphate (KH2PO4).
In some of the piezoelectric crystals, the dipoles are permanently
polarized even in the absence of the electric field. However on
applying electric field, the direction of polarization changes
Ferroelectricity:
Ferromagnetic
All ferroelectric solids are
piezoelectric but the reverse is
not true.

227. e.g. Lead zirconate (PbZrO3)
In some crystals, the dipoles align themselves in such a way, that
alternately, they point up and down so that the crystal does not
posses any net dipole moment. Such crystal are said to be anti
Ferroelectric
Anti Ferroelectricity:
All ferroelectric solids are
piezoelectric but the reverse is
not true.

228. Super Conductivity

229. Electrical resistance decreases with decreases in temperature and
becomes almost zero near the absolute zero.
A substance is said to be superconducting when it offers no
resistance to the flow of electricity.
Super Conductivity
The phenomenon was first discovered by Kammerlingh Onnesin 1913
when he found that mercury becomes superconducting at 4 K.
The temperature at which a substance starts
behaving as super conductor is called
transition temperature.

230. Most metals have transition temperatures between 2K -5K. Certain
organic compounds also becomes superconducting below 5K. Such
low temperature can be attained only with liquid helium which is
very expensive.
Super Conductivity
Super conductivity materials have great technical potentials.
power transmission
levitation transportation (trains which
move in air without rails).magnetic train.
Uses

231. Certain alloys of niobium have been found to be superconducting at
temperature as high as 23 K.
Super Conductivity
Since 1987, many complex metal oxides have been found to possess
super conductivity at some what higher temperature.