KINETIC MOLECULAR MODEL OF SOLIDS AND LIQUIDS

Activity 1: Color Drop

1. The moment when you drop the food coloring into the water it slowly goes down,
spreads out, and after a few seconds it will totally stain the water. This happened
because water molecules have continuous motion due to their kinetic energy.

2. When you compare the rate of diffusion of the two glasses, the hot water has faster
rate of diffusion than cold water. It is because the molecules of hot water have greater
kinetic energy that cold water. Therefore, the molecules move faster and the food
coloring will diffuse quicker. The diffusion process is simply explained by the kinetic
molecular theory, the higher the temperature, the higher the kinetic energy.

3. The Kinetic Molecular Energy is related to the experiment because it explains the
process of it. The spaces between water molecules which causes the constant motion
present in the water. When the temperature increases, the kinetic energy will increase
as well, this will cause the increase in speed of the water molecules. That is why when
you put a liquid substance in water, it will eventually spread-out even without stirring.

4. The food color would not be spread out in the water because there is no kinetic energy
that will trigger the color to spread out and dye the water.

Activity 2: What’s the Matter?

Activity 3: Describe Me
Characteristic Solid Liquid
Intermolecular force Strong Strong but weaker than solid
Shape Definite indefinite
Volume definite definite
Density high high
Compressibility none slight
Arrangement of Particles Regular and fixed Irregular and random
Motion of Molecules Vibrate in fixed position Particles are free to move
Fluidity Does not flow Flows freely

Activity 4
Solids have higher densities compared to their liquid form because the solid particles 
are more compact. However, ice is less dense than water since the volume of ice is greater
than that of liquid with the same amount of matter. This is often due to the anomalous
behavior of the water when it reaches 4 degrees Celsius. Normally, as things are cooled, they
contract. But this is not what water obeys when it crosses 4 degrees Celsius. That's why the
ice is less dense than the liquid. This phenomenon has a biological meaning. In areas like
Antarctica, where temperatures are below temperature, fish and other marine life have
survived. Because the ice has less density than the water, it can float and stay on the surface,
preventing the underside from freezing. This will encourage marine life to flourish in these
regions.

Activity 5
1. B
2. A
3. B
4. D
5. C
6. B
7. A
8. B
9. B
10. D

Reflection
I learned about the kinetic molecular model of solids and liquids. I enjoyed answering
what’s the matter part because it was easy and it was already discussed during our junior high
school days. I want to learn more on how I can use these in real life.
 INTERMOLECULAR FORCES

Activity 1: OPERATION: Crossword Puzzle

1. Hydrogen bonding
2. Ion dipole
3. Van der waals force
4. Intramolecular
5. Dipole dipole
6. London dispersion
7. Hydrogen
8. Inetermolecular
Activity 2: Go With the Flow

Activity 3: Classify Me
1. Dipole-dipole force and London Dispersion
2. London dispersion force
3. Ion-dipole force and London Dispersion
4. London Dispersion force
5. Hydrogen Bonding and London Dispersion
6. Hydrogen bonding and London Dispersion
7. Dipole-Dipole interaction and London Dispersion
8. Ion-dipole force and London Dispersion
9. London Dispersion force
10. Dipole-dipole force and London Dispersion

Activity 4: Describe Me
 Compound Type of Strongest type of Reason for
Intramolecular force/ intermolecular force classifying
chemical bond present
1. Hydrogen Covalent bond Hydrogen Bonding The compound
exhibits hydrogen
fluoride HF
bonding
because hydrogen is
bonded to highly
electronegative
fluorine.
2. Magnesium MgCl2 – ionic Ion-dipole force The compound
compound exhibits ion-dipole
chloride
force because there is
(MgCl2) in Water – Covalent an attraction
compound between ions and
Water polar molecule.
3. Hydrogen Dipole-dipole force The compound
Covalent compound exhibits
bromide HBr
dipole-dipole
interaction
because the molecule
is polar.
4. Silicon Covalent compound London The compound
Dispersion forces exhibits London
dioxide SiO2
dispersion force
because it is a
nonpolar covalent
compound.
5. Fluorine Covalent compound London The compound
molecule F2 Dispersion forces exhibits London
dispersion force
because it is a
nonpolar covalent
compound.

Activity 5: What If?

Water is the most abundant molecule in living cells and the one most critical to life as
we know it. If hydrogen bonding did not exist in water, everybody would die. What will
happen is water would vanish instantly and turn into separate hydrogen and oxygen gas.
Lack of hydrogen bonding (and therefore) water would also mean that life would have to
revolve around other compounds, since water is important to all living things. Every single
cell die, therefore there’ll be no life. Plants will not be able to absorb water into their xylem
vessels and die, potentially ending all life on Earth.
REFLECTION

I learned about the intermolecular forces. I also learned the different types of
intermolecular forces including london dispersion, dipole-dipole, hydrogen bonding, and
ion-dipole. I enjoyed most on answering the crossword puzzle. I want to learn more on the
intermolecular forces.

PROPERTIES OF LIQUIDS AND INTERMOLECULAR FORCES

Activity 1: KNOW ME!

1. C
 2. D
3. A
4. B
5. a. A
b. B
c. B
d. B

Activity 2: I CAN DO IT!

1. Surface tension
2. Fluid
3. Capillary action
4. Viscosity
5. Vapor
6. Vaporization
7. Vapour pressure
8. Boiling point
9. Molar heat of vaporization

Activity 3: PICTURE SHOWS WHAT I KNOW!

1. In the picture, as the temperature of the container increases, the water molecules
evaporate and transform into a vapor state. Any of the water molecules in the vapor
process have a chance to go out into the flask and then suddenly vanish into the
atmosphere.
2. Container B has a closed environment, so when the liquid evaporates and transforms
to its vapor phase, the water molecules did not have the opportunity to escape from
the container.

Activity 4: MIND THE GRAPH

a. When the temperature increases, the vapor pressure of water also increases.

b. The graph contains the vapor pressures of the four common liquids: diethyl ether,
ethyl alcohol, water and ethylene glycol with regards of the temperature. Base on the
graph, the vapor pressure increases as temperature increases, it applies to all these
four liquids.

Activity 5: CRITICAL THINKER

1. a. Acetic acid 🡪 Water 🡪 Ethanol 🡪 Acetone
 b. Acetone 🡪 Ethanol 🡪 Water 🡪 Acetic acid
c. Acetone 🡪 Ethanol 🡪 Water 🡪 Acetic acid
2. The reason why glycerol has a higher viscosity than water is because of its higher
number of – OH groups, which helps it to form more H-bonds with other glycerol
molecules. Because of this, its intermolecular forces are greater than those of water,
and its resistance to flow is higher.

REFLECTION
I learned about properties of liquids and intermolecular forces. I enjoyed most
on identifying the words being described. I want to learn more how can I apply this in
real life and what are the circumstances.
 PROPERTIES OF WATER AND INTERMOLECULAR FORCES

Activity 1: MIND POWER

Part A

1. Heat of Vaporization

2. Density in its liquid form

3. Surface Tension

4. pH

5. Boiling point

Part B

1. Cohesion refers to the attraction of molecules for other molecules of the same

kind,
and water molecules have strong cohesive forces thanks to their ability to form
hydrogen bonds with one another.

2. The weight of the insect and the structure of its legs in combination with the
surface tension of the water allow certain insects to walk on the water. Water
molecules are more drawn to each other than to other materials, so they create a force
to remain together called surface tension.

3. Adhesion is the attraction of molecules of one kind for molecules of a

different kind, and it can be quite strong for water, especially with other
molecules bearing positive or negative charges.

4. Cohesion and adhesion helps plants move materials because cohesion is where

molecules are attracted to each other due to covalent bonds, and adhesion
forms hydrogen bonds once the molecules become attracted to each other.

5. Water is most dense at its freezing point.

6. Ice floats because it is about 9% less dense than liquid water. In other words,
ice takes up about 9% more space than water, so a liter of ice weighs less than liter water.
The heavier water displaces the lighter ice, so ice floats to the top. 

7. Ice serves as a barrier between the water and the cold air above.

8. Capillary action. It is the rise of water against force of gravity

9. Ice actually has a very different structure than liquid water, in that the
molecules align themselves in a regular lattice rather than more randomly as in
the liquid form. It happens that the lattice arrangement allows water molecules to be
more spread out than in a liquid, and, thus, ice is less dense than water.
Activity 2: EXPLORING PROPERTIES

1. D and F

2. B

3. A and B

4. E and C

5. A

6. A

7. B

8. F

9. C

10. B

Activity 3: WORD HUNT

Part A

1. Covalent

2. Polar

3. Dissolve

4. Cohesion

5. Positively, negatively

Part B

1. Oil will heat up faster than water because the heat capacity of oil is lower than
the heat capacity of water. Water requires more energy per gram of liquid to change its
temperature. 

2. apples, wood, and sponges 

3. When the heat is raised as water is boiled, the higher kinetic energy of
the water molecules causes the hydrogen bonds to break completely and
allows water molecules to escape into the air as gas.
REFLECTION
I learned about the properties of water and intermolecular forces. I enjoyed most on
answering the activities. I want to learn more on the importance of this topic.

THE STRUCTURE OF CRYSTALLINE AND AMORPHOUS SOLIDS

Activity 1: CRYSTALLINE SOLID

1. Ionic

2. Covalent network

3. Molecular

4. Metallic

5. Covalent network

6. Molecular

7. Molecular

8. Ionic

9. Ionic

10. J

1. Ice has a crystalline structure that is stabilized by hydrogen bonding. These

intermolecular forces are of equal strength and thus take the same amount of energy
to resolve. As a result, the ice melts at a single temperature and not a temperature
range. The different, very large molecules that make up butter undergo varied van der
Waals attractions of different strengths that are overcome at different temperatures, and
therefore the process of melting takes place over a wide temperature range.
Activity 2: CONCEPTUAL PROBLEMS

1. The arrangement of the constituent atoms or molecules are more important in

determining the properties of a solid due to the greater long range, persistent order of 
the solids. Gases and liquids can not easily be defined by the spatial arrangement of
their components because rapid molecular motion and rearrangement determines
many of the properties of liquids and gases.

2. The initial solid contained the desired compound in an amorphous state, as

shown by the broad temperature range over which the melting occurred. The slow cooling of
the liquid caused it to crystallize, as shown by the sharp second melting point
observed at the predicted temperature.

Activity 6: Multiple Choices

1. B

2. B

3. A

4. D

5. B

6. A

7. C

8. B

Reflection
I learned that solids have different structures and the explanation why solids are
sometimes hard or soft. I enjoyed most on analyzing situations and multiple choices. It made
me read and learn more from the module and activities. I want to learn more on gases because
I’m done reading the module for solids and liquids. It interests me more to explore and
curious about the matter.