This power point presentation focuses on the different intermolecular forces that binds molecules in order for solids to remain solids or liquid to remain liquids. This presentation also presents the different properties of liquid that can be explained through the concept of intermolecular forces. It also contains simple activities to test the understanding of the learners on the lesson.

1. General Chemistry 2
Presented by
Kristel Joy R. Somera
Subject Teacher

2. At the end of the lesson, you shall be
able to:
• Use the kinetic molecular model to explain
properties of liquids and solids
STEM_GC11IMFIIIa-c-99
• Describe the general types of
intermolecular forces STEM_GC11IMFIIIa-
c-100

3. Lesson 1: Kinetic Molecular Theory
on Liquids and Solids

4. Properties of Gases:
1.Gases have no definite shape and
volume.
2. Gases diffuse rapidly.
3. Gases can be readily compressed.
4. Gases have densities much lower
than solids and liquids.
Review:

5. Kinetic Molecular Theory:
Gases are composed of atoms or molecules
which are widely separated from
one another.
Gas molecules move at a very high speeds,
traveling in straight paths but in random
directions.
Gas molecules collide with one another and
with the walls of its container.
The average kinetic energy of the molecules is
determined by the gas temperature

7. Kinetic Molecular Theory of Solids and Liquids:
Criteria Solid Liquid
Particle
Arrangement
Movement
Density
• Particles are not
free to move
• Particles vibrate
in fixed position
• Particles are able
to slide pass one
another
Very High High

8. Kinetic Molecular Theory of Solids and Liquids:
Criteria Solid Liquid
Diffusibility
Compressibility
Volume and
shape
Thermal
Expansibility
Least Compressible
Fixed volume and
shape
Slightly
compressible
Assumes the shape
of the container it
occupies and has a
fixed volume
Expands slightly
when heated
Expands slightly
when heated
Extremely slow Slow

9. Lesson 2: Intermolecular Forces

10. Force which keeps
molecules together. It is
the force between the
atoms of a molecule or
compound.
Attractive force between
molecules. Responsible
for keeping matter in
solid or liquid phase.

11. Intramolecular forces
Intermolecular
forces

15. Intermolecular Forces
• The attractions between molecules are not nearly as
strong as the intramolecular attractions (bonds) that hold
compounds together.
• Many physical properties reflect intermolecular forces, like
boiling points, melting points, viscosity, surface tension,
and capillary action.

17. Types of Intermolecular Force
• Weakest to strongest forces:
dispersion forces (or London dispersion forces)
dipole–dipole forces
hydrogen bonding (a special dipole–dipole force)
ion–dipole forces
oNote: The first two types are also referred to collectively as
van der Waals forces.

20. These London dispersion forces are often found in the halogens
(e.g., F2 and I2), the noble gases (e.g., Ne and Ar), and in other
non-polar molecules, such as carbon dioxide and methane.
London dispersion forces are part of the van der Waals forces, or
weak intermolecular attractions.

24. • Dipole – dipole forces are formed
between neighboring molecules with
permanent dipoles.
• Polar covalent compounds usually
undergo dipole – dipole forces
• CCl4, HCl, SO2 are example of dipole –
dipole.

27. • H- bond is actually a dipole – dipole in
nature but for molecules containing O –
H, H- F and N-
• H2O, NH3, NH4 and HF are examples of
hydrogen bond.

31. • NaCl solution, CaCl2 solution, and KCl
solution are examples of ion - dipole.

32. Activity 2
Based on the discussion, determine the
intermolecular forces being described and
tell its level of strength (very weak, weak,
strong, very strong)

33. Description/ Nature of interaction Intermolecular Forces of
Attraction (IMFA)
Strength
1. Interaction of an ion with the
charge end of another molecule
2. A special type of dipole – dipole
formed between a partially positive
hydrogen and a neighboring
molecule with partially negative O,
N, F
3. An interaction between
molecules with temporary dipoles
4. An interaction between two polar
molecules other than N- H, O-H, and
H-F
ion - dipole Very strong
Hydrogen bond Strong
Dispersion Very weak
dipole – dipole Weak

34. Activity 3
Identify the type of intermolecular forces of
attraction the given compound has.
1. CO2
2. MgCl2 Solution
3. ICl – Iodine monochloride
4. NH3
5. HCl
Dispersion
Ion - dipole
Dispersion
Hydrogen bond
Dipole - dipole

35. Arrange the following according to
decreasing intermolecular force of
attraction. Explain your answer
1. Carbon tetrachloride CCl4
2. Water H2O
3. Sodium Chloride solution
4. Iodine Chloride

36. Let us Review!

37. Determine the type of intermolecular
forces of attraction between the given
molecules
1. HF
2. PCl3
3. CO2
4. SO2
5. NaCl in water

38. 1. HF
2. PCl3
3. CO2
4. SO2
5. NaCl in water
H - bond
Dipole - dipole
London dispersion force
Dipole - dipole
Ion - dipole

39. Lesson 3: Properties of Liquids

40. Learning Competency:
• Describe the following properties of liquids, and explain
the effect of intermolecular forces on these properties:
surface tension, viscosity, vapor pressure, boiling point, and
molar heat of vaporization

41. What are the properties of liquid
according to Kinetic molecular theory?
1. Particles are not confined to a rigid position
since they have sufficient kinetic energy to
overcome their attractive forces. and they move
but not at a far distance, they roll and slide pass
each other.

42. 2. Since the molecules flow, they take the shape
of a container and diffuse moderately to occupy
a fixed volume.
3. They have high density but low
compressibility, and thermal expansion.
4. They are joined by intermolecular forces.

43. Special Physical Properties
of Liquids and
Intermolecular forces

44. Surface Tension

45. 1. Surface Tension
is the force that causes the surface of
a liquid to contract

46. Surface tension and Intermolecular
forces
 The strength of surface tension depends on the
intermolecular force of attraction.
 The stronger the IMFA, the greater the surface
tension
 However, an increase in temperature decreases
surface tension
Surface tension explains why a drop of
liquid is spherical in shape.

47. Viscosity

48. 2. Viscosity
is the resistance of
fluid to flow. This is
cause by the
intermolecular
attraction between
the molecules of
liquids.

49. Viscosity and Intermolecular forces
 A liquid with low intermolecular forces allows
molecules of liquid to move freely, therefore,
low viscosity
 A liquid with strong intermolecular forces
have high viscosity

50. Viscosity and Intermolecular forces
 Increasing the temperature causes the kinetic
energy of the molecules of liquid to increase.
Heat breaks the intermolecular forces causing
the molecules to move faster. Therefore,
increase in temperature will decrease the
viscosity.

51. Let us compare the viscosity and intermolecular forces
of the given liquids. Arrange them according to
increasing viscosity and IMF.
Water Toothpaste Honey Cooking Oil

52. Water Toothpaste
Honey
Cooking Oil
increasing viscosity and IMF.

53. Vapor pressure
and boiling point

54. 3. Vapor Pressure and Boiling Point
Vapor pressure of a liquid is the
pressure of the vapor resulting
from evaporation of a liquid.

55. Let us determine which of the following
samples of liquid has high vapor pressure
Water

56. samples of liquid in increasing vapor
pressure
Water

57. 3. Vapor Pressure and IMF
 If a liquid has a weak IMF, the escaping
tendency of the molecules is high (molecules
easily breaks apart/ turn into its gaseous state)
 Weak IMF means high vapor pressure and
strong IMF means low vapor pressure
 Liquids have different vapor pressure at
different temperature.

58. 3. Vapor Pressure and Boiling Point
Boiling Point of a liquid is the temperature at
which the vapor pressure of the liquid is equal to
the atmospheric pressure. At this temperature,
the amount of heat added to the system by
heating the liquid is equal to the amount of heat
escaping through evaporation. This is why the
temperature remains constant at boiling point.

59. Boiling Point= temperature where
vapor pressure = Atmospheric
pressure

60. Boiling Point and Vapor pressure and IMF
 The lower atmospheric pressure, the faster it is to
equalize the vapor pressure of the liquid and the
atmospheric pressure, the lower the boiling point.
 A liquid that has weak intermolecular forces has
high vapor pressure evaporates easily, therefore it
has a low boiling point.
 A liquid with strong IMF has low vapor pressure,
does not evaporate easily and with high boiling
point

61. Let us study and compare the different Boiling
Point of some liquids. Let us arrange the liquids
into increasing boiling point, IMFA and increasing
vapor pressure
Liquid Boiling Point
Water 100 ºC
Isopropyl Alcohol 82.5 ºC
Soy bean Cooking Oil 300ºC
acetone 56 ºC

62. Arrangement of the sample liquids into increasing
boiling point and IMFA
Liquid Boiling Point
Acetone 56ºC
Isopropyl Alcohol 82.5 ºC
Water 100ºC
Soy bean Cooking Oil 300 ºC

63. Arrangement of the sample liquids into increasing
vapor pressure
Liquid Boiling Point
Soy bean cooking oil 300ºC
Water 100 ºC
Isopropyl Alcohol 82.5ºC
Acetone Soy bean
Cooking Oil
56 ºC

64. The amount of heat needed to vaporize a
given amount of liquid at its boiling
point.
4. Molar heat of Vaporization

65. What is the most
abundant liquid on
Earth?
WATER!

66. Common Uses of Water

69. Propertie
s of
Water

70. 1. Water has high boiling
point (100ºC)
Reason
Consequenc
e

71. 2. Water has high
specific heat
Reason
Consequenc
e

72. 3. Water has high density
in its liquid form
Reason
Consequenc
e

73. 4. Water has high surface
tension
Reason
Consequenc
e

74. 5. Water has high heat of
vaporization
Reason
Consequenc
e

75. Water has:
1. high boiling point
2. high specific heat
3. high density in its liquid form
4. high surface tension; and
5. high heat of vaporization

76. Test your mastery!

77. Water plays a vital role in our
life. Determine the
property/ies of water where
the given situation or
illustration can be attributed.

78. 1.
Answer

79. Water moves from roots of
a tree to the top of very tall
trees.
2.
Answer

80. Perspiration lowers body
temperature.
3.
Answer

81. preventions of
temperature variations
that are outside the range
suitable for life
4.
Answer

82. Water is liquid at room
temperature.
5.
Answer

83. Water resist sharp changes
in temperature so earth
would not experience great
temperature variations.
6.
Answer
Back

84. The high boiling point of
water is due to its strong
intermolecular forces of
attraction caused by the
formation of the H - bond

86. The high specific heat of
water is due to its strong
intermolecular forces of
attraction caused by the
formation of the H - bond

88. The high surface
tension of water is
due to the formation
of the h – bond on
the surface of the
water molecules

89. The high heat of vaporization
of water is due to its strong
intermolecular forces of
attraction caused by the
formation of the H – bond.

90. Water is not easily vaporize
or turn into its gaseous state

91. Water can absorb or release
large quantities of heat
without change in
temperature.

92. Ice floats in water.

93. Water can be able to move
against gravity or flow into
fibers

94. Large amount of heat is
needed to vaporize a given
amount of water.

100. 1.
Water has high density in its
liquid form
Back to mastery

101. Water moves from roots of
a tree to the top of very tall
trees.
2.
Water has high surface
tension Back to mastery

102. Water has high molar heat of vaporization/
high specific heat
Perspiration lowers body
temperature.
3.
Back to mastery

103. preventions of
temperature variations
that are outside the range
suitable for life
4.
Water has high molar heat of vaporization/
high specific heat Back to mastery

104. Water is liquid at room
temperature.
5.
Water has high boiling
point Back to mastery

105. Water resist sharp changes
in temperature so earth
would not experience great
temperature variations.
6.
Water has high molar heat of vaporization/
high specific heat Back to mastery

106. Connecting to real –
life

107. How does the molecular
structure and intermolecular
forces affect the properties of
water?

108. Evaluation!

109. Assignment:
-Follow- up
1. Search for more applications of the properties of
water in daily life not mentioned during the lesson.
-Advance
1. What are the processes involving phase change?
2. Draw/plot the phase diagram of water and
interpret.