2. KMT in liquid and solid.pdf and properties

kinetic molecular theory in solid and liquid as well as their properties

1. KINETICMOLECULAR MODEL
ANDINTERMOLECULAR FORCES
KineticMolecularModelof
LiquidsandSolids

2. As was the case for gaseous substances, the kinetic
molecular theory may be used to explain the behavior
of
solids and liquids. In the following description, the term
particle will be used to refer to an atom, molecule, or
ion. Note that we will use the popular phrase
“intermolecular attraction” to refer to attractive forces
between
the particles of a substance, regardless of whether these
particles are molecules, atoms, or ions.

3. Kinetic Molecular Theory
The KMT explains the properties of solids and liquids
in terms of intermolecular forces of attraction and the
kinetic energy of the individual particles.

4. Recalling the concept:
Solid Liquid Gas
Arrangement of
particles
Closely and
orderly packed
Less closely
packed
Very far apart
Kinetic energyVibrate and rotate
about a fixed
position
Particle slide over
each other
Particles move
at great speed
Particle motionVery low Low High
Attractive forcesVery strong Strong Low

6. Plasma
•Like gas, plasma does not have a definite shape or
volume.
•Produce magnetic fields and electric current and
respond to strong electromagnetic forces.

8. The 4
th
state of matter (Plasma)
•Formed by providing heat to the gas
•It is an ionized gas consisting of
positive ions and free electrons,
typically at low pressures
(fluorescent lamp) or at very high
temperatures (Sun)
•It is where all the states of matter
arises from.

9. Thermal vs. non-thermal plasma
Thermal Plasma
•Have electrons and
heavy particles at the
same temperature; they
are in thermal
equilibrium with each
other.
Non-thermal Plasma
•Have ions and neutrals
at a much lower
temperature, whereas
electrons are much
hotter.

11. Types of plasma
Natural plasma
•Stars, solar wind,
interstellar nebulae
Artificial plasma
•TV screens, fluorescent
lamps, Laser-produced
plasmas, Plasma used in
semiconductor device
fabrication.
Natural plasma
•Lightning, Polar
aurora, Blue jets

17. Compressibility of gas
Gaseous butane is
compressed within the
storage compartment of
a disposable lighter,
resulting in
its condensation to the
liquid state.

18. Intermolecular Forces of Attraction
Intermolecular Forces are
attractive forces between
molecules or particles in
the solid or liquid states

19. Intermolecular Forces of Attraction
Intermolecular Forces (IMF) are relatively
weaker than the forces within the molecules
forming bonds (intramolecular forces)
Intramolecular Forces holds atoms together
in a molecule

20. Intermolecular Forces of Attraction
The intermolecular forces of attraction in a
pure substance are collectively known as
van der Waals forces
1.Dipole-dipole
2.Hydrogen bonding
3.Ion-dipole
4.London dispersion
5.Dipole-induced dipole forces

21. vanderWaalsforces:
❑Thetermforallknown
Intermolecular forces.
❑Named after a Dutch
scientist: Johannes van
der Waals (1837 –
1932)

22. TypesofvanderWaalsforces:
Dipole–dipole
Exist between polar molecules. One end of a
dipole attracts the oppositely charged end of
the other dipole.
Weaker force compared to ion-dipole
(depending on size)
Example:
a.Dichloromethane
b.HydrochloricAcid

23. TypesofvanderWaalsforces:
HydrogenBonds
⦿Playsanimportantroleinlife processes
⦿Itcaneasilybebrokenandreformed
⦿Occursinwater,DNAmolecules,and protein
⦿It is an attractive interaction between a hydrogen atom
bonded to an electronegative Fluorine, Oxygen and
Nitrogen atom and an unshared electron pair of another
nearby electronegative atom.

24. TypesofvanderWaalsforces:
HydrogenBonds
Example:
a.Water(H
2O)
b.Ammonia
c.AmmoniaandWater(NH
3)
d.HydrofluoricAcid(HF)
Ammonia

25. TypesofvanderWaalsforces:
Ion–dipole
⦿Resultswhenanionandthepartialcharge
foundattheendofthepolarmoleculeattract
eachother.
⦿Positiveionsareattractedtothenegative
endofadipoleandviceversa.This
explains the solubility of ionic
compounds in water which is polar
molecule.
Example:
a.Salt(NaCl)DissolvedinWater(H
2O)
b.Potassim(K+)DissolvedinHydrochloric
Acid(HCl)

26. TypesofvanderWaalsforces:
Ion–dipole
Example:
a.Salt(NaCl)Dissolved
inWater(H
2O)
b.Potassim(K+)
Dissolvedin
Hydrochloric
Acid(HCl)

27. TypesofvanderWaalsforces:
LondonDispersionForces
⦿It is the weakest type of intermolecular forces
⦿When two non-polar molecules approach each other,
an instantaneous dipole moment forms.
⦿Cl
2 and CH
4

28. London Dispersion Forces
Even distribution
of e-
Uneven
distribution of e-
due to constant
movement making
one side partially +
(Polarization)
Temporary
Partial + attracts
nonpolar and form
forces of attraction
Atom will be
distorted

29. TypesofvanderWaalsforces:
LondonDispersionForces
⦿Dipolecanbeinducedmorelikelyon
moleculeshavinglargermolecularmasses.
(Polarizability)
-Thisalsoaffectsthemeltingandboiling
pointsofthemolecules.

30. INTERMOLECULAR
FORCES AND
PROPERTIESOFLIQUIDS
What factors determine
the physical
properties of liquids?

33. POPERTIESOFLIQUIDS
A.VISCOSITY
⦿Whatisthedifferencebetweenfluid
andviscousliquids?
⦿VISCOSITYistheabilityofafluidto
resistflowing.

34. POPERTIESOFLIQUIDS
A.VISCOSITY
⦿Viscosityofa
liquiddependson
intermolecular
forcesthatis
present.
⦿The stronger the
IMF, the higher
the viscosity

35. POPERTIESOFLIQUIDS
A.VISCOSITY
⦿Non-polarmoleculeshavelow
viscositiesbecauseofweakLondon
Force.Example:Benzene,pentaneand
carbontetrachloride.
⦿Polarmolecules
suchasglycerol
andaqueous
sugarsolution
havehigh
viscosities.

36. POPERTIESOFLIQUIDS
A.VISCOSITY
⦿Long-chained substances
like oil have greater IMF
because there are more
atoms that can attract one
another, contributing to the
substance’s total attractive
forces.

37. POPERTIESOFLIQUIDS
A.VISCOSITY
Whatdoyouthinkistheeffectofan
increasingtemperaturetotheviscosityof
aliquid?
The viscosity
decreases as
thetemperature
increases

39. POPERTIESOFLIQUIDS
B.SURFACETENSION

40. POPERTIESOFLIQUIDS
B.SURFACETENSION
⦿Themeasureoftheresistanceofa liquidto
spreadout.
⦿The higher IMF means higher surface tension
⦿Thehigherthe temperature,
the lessthestrength ofthe
attractive forcethatholds
themolecule together

41. POPERTIESOFLIQUIDS
B.SURFACETENSION
⦿Allows needles and paper clips to
float in water if placed carefully on
the surface. It also explains why
drop of water are spherical in
shaped

42. POPERTIESOFLIQUIDS
B.SURFACETENSION
⦿Molecules within a liquid are
pulled in all directions by IMF
⦿Molecules at the surface are
pulled downward and
sideways by other molecules,
not upward away from the
surface

45. POPERTIESOFLIQUIDS
C.CAPILLARITY
⦿The tendency of a liquid to
rise in narrow tubes or to be
drawn into small openings
such as in plants transport
system.
⦿Resultsfrom competition
between liquid’s
intermolecular forceandthe
wallsof thetube.

46. POPERTIESOFLIQUIDS

47. POPERTIESOFLIQUIDS

48. POPERTIESOFLIQUIDS
C.CAPILLARITY
Two types of forces are involved in capillary action
⦿Cohesion –intermolecular attraction between like liquid
molecules
⦿Adhesion –attraction between unlike molecules(water
and the one that make up the glass tube)
⦿These forces also define the shape of the surface of a
liquid in a cylindrical container (meniscus)

49. POPERTIESOFLIQUIDS
C.CAPILLARITY
⦿When the cohesive force between the liquid molecules
is greater than the adhesive forces between the liquid
and the walls of the container, the surface of the liquid
is convex.
⦿When the cohesive forces between the liquid molecules
are lesser than the adhesive forces between the liquid
and the walls of the container, the surface of the liquid
is concave.

51. POPERTIESOFLIQUIDS
D.VAPOR PRESSURE
⦿It is the pressure exerted by its
vapor when in equilibrium with
liquid or soilid.
⦿Example: when liquid or solid
substances is made to evaporate in
a closed container, the gas exerts a
pressure above the liquid.

52. POPERTIESOFLIQUIDS
D.VAPOR PRESSURE
⦿Substances with relatively strong IMF
will have low vapor pressure because
the particles will have difficulty
escaping as a gas.
Example:
⦿Water(H bonding) has vapor pressure of
0.03 atm
⦿Ethyl Ether Dipole-dipole and London
forces has vapor pressure of 0.68 atm

54. POPERTIESOFLIQUIDS
E.BOILING POINT
⦿The boiling point of a liquid is the
temperature at which its vapor pressure
is equal to the external or atmospheric
pressure
⦿Increasing the temperature of a liquid
raises the KE of its molecules, until
such a point where the energy of the
particle movement exceeds the IMF that
holds them together.

55. POPERTIESOFLIQUIDS
E.BOILING POINT
⦿The liquid molecules then transform to
gas and are seen as bubbles that rises
to the surface of the liquids and escape
to the atmosphere.
⦿Temperature at which a liquid boils
under 1 atmospheric pressure is
referred to as its normal boiling point.

56. POPERTIESOFLIQUIDS
E.BOILING POINT
⦿At higher altitudes, the atm is lower,
hence, the boiling point will
subsequently decrease.
⦿The greater IMF, the higher the energy
needed to increase the KE of the
molecules to break these forces.

58. POPERTIESOFLIQUIDS
F.HEAT OF VAPORIZATION
⦿Molar Heat of vaporization is the
amount of heat required to vaporize one
mole of substance at its boiling point.
⦿The application of heat disrupts the IMF
of attraction of the liquid molecules and
allows them to vaporize

59. POPERTIESOFLIQUIDS
F.HEAT OF VAPORIZATION
⦿Boiling point generally increases as
molar heat of vaporization increases.
⦿The heat of vaporization is also
determined by the strength of IMF
between molecules.

61. POPERTIESOFLIQUIDS
ANALYSIS
⦿Normalboilingpointhappenswhena
liquidreachesaninternaltemperature
of100
OCunder
1atm(atmosphericpressure)
Whichlevelwithrespecttosea
levelfoodscooksfasterand
slower?

62. POPERTIESOFLIQUIDS
Athigheraltitude,
atmosphericpressureis
lesser.
Thuswaterboilsfasterata
lowertemperaturebecause
lesspressureisexertedon
watermolecules.
Inefficientdeliveryofheatto
cookthefoodandittakestime
forthefoodtobe cooked.

63. PROPERTIESOFSOLIDS
How are the structures and
properties of
solids related?
https://www.slideshare.net/marvinnbustamante1/general-
chemistry-2-chapter-1-the-kinetic-molecular-model-and-
intermolecular-forces-of-attraction-in-matter

64. POPERTIESOFSOLIDS
⦿ASOLIDisformedwhen
thetemperatureofa
liquidislowandthe
pressureissufficiently
highcausingthe
particlestocomevery
closetooneanother.
⦿Theyarerigid
⦿Theirparticleshardly
diffuse

65. POPERTIESOFSOLIDS
NATUREOFSOLIDS
Crystalline
Solids
Amorphous
Solids

66. POPERTIESOFSOLIDS
A. CRYSTALLINE
⦿Atoms,ions,ormoleculesarearranged
inwelldefinedarrangement
⦿Havingflatsurfaceandsharpedges
⦿Example:gems,salts,sugarandice.

67. POPERTIESOFSOLIDS
TYPESOF CRYSTALLINE SOLIDS
Ionic
Molecular
CovalentNetwork
Metallic

68. POPERTIESOFSOLIDS
1.IonicCrystallineSolids
⦿Composedof(+)and(-)ions
⦿Heldbyelectrostaticattractions
⦿Theyarehard,brittleandpoor
electricalandthermalconduction
⦿Example:NaCl

69. POPERTIESOFSOLIDS
2.MolecularCrystallineSolids
⦿Composedofatomsandmolecules
⦿Heldtogetherby:H-Bond,dipole-
dipole,andLondondispersionforces
⦿Soft,lowtomoderatemeltingpointand
poorthermalandelectrical
conductivity
⦿Examples:CH
4,C
12H
22O
11,CO
2,H
2O
andBr
2

70. POPERTIESOFSOLIDS
3.CovalentNetwork Crystalline
Solids
⦿Atomsconnectedinanetworkof
covalentmolecules
⦿Heldtogetherbycovalentbonds
⦿Veryhard,veryhighmeltingpointand
oftenpoorthermalandelectrical
conductivity.
⦿Examples:Plastics,Allotropesof
carbon,siliconcarbide

71. POPERTIESOFSOLIDS
4.MetallicCrystallineSolids
⦿Composedofatomsandmolecules
⦿Heldtogetherbymetallicbonds
⦿Softtohard,lowtohighmeltingpoint,
malleable,ductileandgoodthermal
andelectricalconduction
⦿Allmetallicelements:Cu,Na,Zn,Fe
andAl

72. POPERTIESOFSOLIDS
Howaremoleculesbeing
arrangedinmicroscopiclevel?
UnitCell
Crystal
Lattice
Thesmallestportionofthe
crystalwhichshowsthe
completepatternofits
particles
Therepetitionofunitcells
inall directions

73. POPERTIESOFSOLIDS
Structural
Representations
ofMolecules:
1.NaCl
2.Ice
3.Diamond
4.MetallicBond
in(Fe)

74. POPERTIESOFSOLIDS
B.AMORPHOUS SOLIDS
⦿FromtheGreekwordfor“without
form”
⦿Solidparticleswhichdonothave
orderlystructures.
⦿Theyhavepoorlydefinedshapes
⦿arerigid,buttheylackrepeated
periodicityorlong-rangeorderintheir
structure.
⦿examplesincludethinfilmlubricants,
metallicglasses,polymers,andgels

75. POPERTIESOFSOLIDS
STRUCTURE OF AMORPHOUS SOLID:

76. POPERTIESOFSOLIDS
CRYSTALLINEVERSUSAMORPHOUS SOLIDS

77. POPERTIESOFSOLIDS
⦿Itcanbenotedthatastemperatureof
crystallinesolidisincreased,the
particlesvibratebackandforthabout
itslatticepoint.
⦿Thecrystalbecomeslessordered.
⦿Theheataddedincreasesthekinetic
motionoftheparticles.
⦿Untilthecrystallinestructureis
completelydestroyedbythevibrations
oftheparticles,meltingisachieved.

78. POPERTIESOFLIQUIDS
ANALYSIS
⦿Whatwillhappenifheatingstopsand
noheatisallowedtoescape?
Bothsolidandliquidphasesare
presentinequilibrium.