Pls review

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CHAPTER 3: MATTER AND CHANGE
LESSON 1. PROPERTIES OF MATTER
Objectives
On completion of the lesson, you should be able to:
1. Describe matter.
2. Compare physical and chemical properties of matter
3. Distinguish between physical and chemical changes.
Introduction to Matter
Matter – anything that occupies space and has mass and weight.
Mass - the amount of matter present in an object. The more matter in an object, the
more mass it has. Keep in mind that weight is the effect of gravity on mass and are
not the same.
Volume- the amount of space occupied by matter. It is determined by its length, width and
height.
Composition- refers to what the object is made of (what atoms compose it and in what
proportion).
Property- refers to the characteristics of matter that we can use to distinguish one object from
another.
ACTIVITY 3.1.1: “BURNING MONEY”
Materials
1. Php 20.00 bill (higher denomination if you're brave)
2. tongs
3. matches or a lighter
4. salt (or one of these chemicals if you want a colored flame: lithium chloride, strontium
chloride, calcium chloride, sodium chloride, , copper sulfate, copper chloride, potassium
chloride, magnesium sulfate)
5. solution of 50% alcohol and 50% water (you can mix 95% alcohol with water in a 1:1 ratio,
if desired)
Procedure:
1. Prepare the alcohol and water solution. You can mix 50 ml of water with 50 ml of
95-100% alcohol.
2. Add a pinch salt or other colorant to the alcohol/water solution, to help produce a
visible flame.

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3. Soak a dollar bill in the alcohol/water solution so that it is thoroughly wet.
4. Use tongs to pick up the bill. Allow any excess liquid to drain. Move the damp bill
away from the alcohol-water solution.
5. Light the bill on fire and allow it to burn until the flame goes out.
DISCUSSION
1. What did you observe happened to the peso bill?
2. What is the property of alcohol that makes the magic on “burning money”
3. Explain why the money did not burn/ What is a physical property?
INPUT
A. Physical Property is the properties that do not involve the making of new substances. The
following are two (2) types of physical properties
1. Intensive property- physical properties that can be readily observed using the senses
( taste, smell, hearing, sight, touch.) It. is a characteristic of a substance that can be
described but not measured do not depend on the amount of matter present.
2. Extensive property- physical properties of a substance that can be measured
numerically( dependent on the amount of matter present).
Table 3.1 - Summary of Different Physical Properties of Matter
Physical Property Description
Boiling Point : temperature which the liquid form of a substance becomes a
gas.
Buoyancy The ability to float in certain fluids
Conductivity The ability of a material to allow heat or electricity to flow through
it
Density the ratio of mass to volume
Ductility The ability to be drawn into fine wires. Copper, gold and silver
are ductile.
Elasticity The ability to retain its original shape after it is stretched or
compressed
Flexibility The ability of a substance to bend without breaking. Rubber,
some plastics and metals are flexible.
Form Substances with a regular shape, such as cube-shaped grains of
salt, are said to be crystalline. Substances with an irregular form,
such as starch, are said to be amorphous.
Hardness measure of the resistance of a solid to being scratched or dented
Impenetrability The inability of two bodies to occupy the same space at the
same time.
Luster The ability of an object to reflect light. Chrome faucets are said
to have a high lust because they are e bright and shiny. A flat
paint, on the other hand, has a low luster.
Malleability The ability to be hammered into thin sheets. Because gold and
aluminum can be made into very thin sheets or foils, they are

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B. Chemical Properties: are the properties that involve the formation of a new substance.
(example: when iron rusts or propane burns). It is an irreversible change that produces
one or several new kinds of matter apart from the original.
Table 3.2 - Summary of Different Chemical Properties of Matter
Chemical Property Description
Combustibility the ability of a substance to burn (requires oxygen)
Flammability the ability of a substance to burn when exposed to a
flame
Light Sensitivity: the ability of a substance to change to a new
substance in the presence of visible light
burning
The ability to undergo rapid combustion or consume
fuel in such a way as to give off heat, gases, and,
usually, light; be on fire: The fire burned in the grate.
rusting
to decay or corrode and become unusable through the
action of rust ; to deteriorate or become impaired, as
through inaction or disuse.
fermentation
a change brought about by a ferment, as yeast
enzymes, which convert grape sugar into ethyl alcohol.
tarnishing
to dull the luster of (a metallic surface), especially by
oxidation; discolor.
Digestion
the process in the alimentary canal by which food is
broken up physically, as by the action of the teeth, and
chemically, as by the action of enzymes, and converted
into a substance suitable for absorption and
assimilation into the body
malleable substances.
Mass The amount of matter in an object
Melting Point Temperature which the solid form of a substance becomes
liquid.
Odor A substance can be described as odorless, burnt, flowery,
putrid, spicy, sharp, choking, nauseating
and suffocating
Physical State The condition of being a solid, a liquid or a gas.
Solubility The ability of a substance to dissolve in a solvent like water
Taste : There are four tastes: sweet, like sugar; sour like vinegar, salty,
like table salt; and bitter, like coffee. All flavors are either
combinations of these four tastes, or combinations of tastes and
odors
Temperature The hotness or coldness of a body
Texture: The feel of a substance to the fingers: fine, coarse, smooth,
gritty, silky, fluffy, waxy, etc.
. Viscosity: The measure of how easily a liquid flows. Liquids may be thin,
thick, runny, syrupy, etc.
The thicker the liquid, the more viscous it is. Tar or molasses are
viscous, water is not.

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respiration
 the process in living organisms of taking in oxygen
from the surroundings and giving out carbon dioxide
( external respiration ). In terrestrial animals this is
affected by breathing air.
 the chemical breakdown of complex organic
substances, such as carbohydrates and fats, that
takes place in the cells and tissues of animals and
plants, during which energy is released and carbon
dioxide produced ( internal respiration )
PHYSICAL AND CHEMICAL CHANGES
ACTIVITY 3.1.2: Boil Water in a Paper Cup –
Materials : 1)Plastic with water
2) box of match
3) Candle
Procedure: Boil water in a paper cup filled with water. What happens?
Tips: Be sure that cup must have a flat bottom without a lip The cup should be filled nearly to
the top.
DISCUSSION
PROBEX (Predict-Observe- Explain)
Write your predictions, observation and explanation
Predict ______________________________________
Observe _____________________________________
Explain ______________________________________
Activity 3.1.3: “Clear Solution Mixture”
Materials : 1) betadine solution
2) sodium ascorbate (Vit C)
Procedure: Mix betadine solution (betadine & water) with sodium ascorbate.
What do you think will happen?
PROBEX (Predict-Observe- Explain)
Write your predictions, observation and explanation
Predict ______________________________________
Observe _____________________________________
Explain ______________________________________
Physical change - a reversible change that affects the physical property or form but not the
identity of matter. It does not produce new substances.
Example: Tearing a piece of paper, breaking a glass into pieces, molding clay
Chemical change - an irreversible change that produces one or several new kinds of matter
apart from the original.
Example: Rusting of iron, souring of milk

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APPLICATION:
Direction. Classify each of the properties listed below as extensive or intensive. Then classify
each property as physical or chemical. Write the word out to earn full credit.
Property
Extensive or Intensive
Property
Physical or Chemical
Property
color
combustibility
hardness
density
mass
melting point
ductility
volume
reactivity with acid
odor
weight
malleability
tendency to corrode
Directions, Part 2: Some measurements or descriptions of properties are listed below.
Write which property is being described in each case. Select properties that are listed in
the table from Part 1.
1) 15 dm3
A. ________________
2) can easily be hammered into sheets B. ________________
3) 2.8 g/cm3
C. ________________
4) burns when heated in the presence of O2 D. ________________
5) shiny metal forms a chalky white layer on its surface E. ________________
6) can be scratched by a diamond F. ________________
7) 500o
C G. ________________
8) can easily be drawn into a wire H. _______________

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LESSON 2: PHASE CHANGES OF MATTER
Objectives
On completion of the unit you should be able to:
1. Compare the different 4 phases of matter: changes: solid, liquid, gas and plasma
2. Explain the phase change diagram in relation to phase change.
PHASE CHANGE
A phase is a state of being, with the possibility of making a transition to another state
or phase. Phase of matter pertain to how the particles of the object are arranged and how
they interact with each other. As the phase ranges, these arrangement and interaction also
changes. The following tables compare the four (4) states of matter
Table 3.3 Summary of Four (4) States of Matter & Their Properties
4 States of Matter Solid Liquid Gas Plasma
Volume/ Mass/
Density
Definite Volume
Definite Mass
Definite Density
Definite Volume
Definite Mass
Definite Density
Changes volume
Definite mass
Changes density
Changes volume
Definite mass
Changes density
Shape Definite shape Changes shape
depending on
the container.
Indefinite shape Indefinite shape
Movement and
collisions
Vibrate in place Roll or slide over
each other.
A few collisions
Bounce and collide Fairly fast
Electrons
stripped
Energy Low Medium High Extremely high
Examples Rock, paper,
scissors
Water, juice, tea Oxygen, hydrogen,
water vapor
Star, lightening,
incandescent
bulb
Compressibility
force or pressure
required
High Little Very little extreme pressure
- stars - gravity,
magnetic
Measured with Cubic meters... Liter, ml, qt. Gal. Cubic ...

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The following Figure 1 below shows the processes involved in phase change:
Figure 1 Phase Change and Processes of Changes
The processes involved in phase change are:
1. Melting = changing solid ------> liquid
2. Evaporation = changing liquid------> gas
3. Ionization = changing gas--------> plasma
4. Deionization = changing plasma ---> gas
6. Freezing = changing liquid-------> solid
7. Sublimation = changing solid--------> gas
8. Deposition = changing gas---------> solid
APPLICATION
Below is an illustration of water Cycle. Explain the phase change involved in water cycle.

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LESSON 3: CLASSIFICATION OF MATTER
Objectives
On completion of the lesson, you should be able to:
1. Draw a concept map on classification scheme for matter.
2. Explain the difference between pure substances and mixtures;
3. Classify matter as elements, compounds and mixtures.
4. Distinguish, metals, nonmetals and metalloids
5. Compare acid and bases in compounds
ACTIVITY3.3.1: Video Presentation on Elements, Compounds and Mixtures
To start your journey on exploring the kinds of matter, watch the video entitled Elements,
Compounds and Mixtures. After watching the video, answer the questions that follow.
DISCUSSION
1. How is an element different from a compound?
2. How is an element similar to a compound?
3. What is a mixture?
4. What is the difference between a homogeneous mixture and a heterogeneous mixture?
5. Give examples of elements, compounds and mixtures.
INPUT
The concept map illustrates the major classifications of matter:
CLASSIFICATION OF MATTER
A. PURE SUBSTANCE- matter having a definite set of properties and composition that cannot
be separated by physical means.

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1. Elements- substances made up only of one kind
of atom that cannot be separated chemically.
Table 3.4 - Summary of the Characteristics of Metals, Nonmetals and Metalloids
Metals Nonmetals Metalloids
They are typically shiny,
good conductors of heat
and electricity, have a
high density, and only
melt at high
temperatures.
Metals are ductile and
malleable, so their shape
can be easily changed
into thin wires or sheets
. Metals will corrode,
gradually wearing away
like rusting iron.
Their surface is dull and they
are poor conductor of heat
and electricity. As compared
to metals, they have low
density and will melt at low
temperatures.
The shape of a nonmetal
cannot be changed easily as
they tend to be brittle and will
break.
They have properties of both
metals and non-metals.
Some of the metalloids, such
as silicon and germanium,
are semi-conductors. This
means that they can carry an
electrical charge under
special conditions. This
property makes metalloids
useful in computers and
calculators.
Ex. Iron, Gold, Silver,
Platinum, Copper,
Mercury
Ex.Sulfur, Chlorine, Nitrogen,
Phosphorus, etc... .
The 7 diatomic elements
are: Hydrogen (H2); Nitrogen
(N2), Oxygen O2), Fluorine
(F2), Chlorine (Cl2) Iodine (I2),
Bromine (Br2)
Ex. There only 7 metalloids
such as Silicon(Si), Arsenic
As), Germanium (Ge)
Antimony (Sb), Tellurium (Te)
and Polonium( Po)
COMPOUNDS - chemical combinations of various kinds of element. They are made up of two
or more elements chemically combined.They have fixed or uniform composition and unique
properties of their own. When elements combine to form compounds, they do not retain their
unique properties. They can be break down into simpler substance only by chemical separation
methods.
Example: Water is a compound. It can be broken down
into simpler substances – hydrogen and oxygen.
Compounds are generally classified into three – the acids, bases, and salts.
Table 3.5 - Summary of Comparison of the Different Classes of Compounds
ACID BASE SALT
sour taste taste bitter usually a compound of a
metal with a single non-
metal other than oxygen
react with active
metals to produce
hydrogen(H)
react with active nonmetals to
produce hydroxide (OH)
give color changes
with indicators ( blue
litmus paper turns red
in the presence of an
acid substance
reverses the color change
produced by acids on
indicators (red litmus paper
turns blue in basic
substances

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neutralize bases neutralizes acids
Ex, hydrochloric acid
(H2SO4)
Ex Sodium hydroxide (NAOH) Ex. Sodium chloride (NaCl)
Toilet bowl cleaner
acid; vinegar
Toothpaste, shampoo &
conditioner
B. MIXTURES- matter made up of two or more substances that are physically combined where
each component still retains its own characteristics.
1. Homogeneous Mixtures or Solutions- are mixtures that are uniform in composition and
properties in a given sample but composition and properties may vary with different samples.
2 .Heterogeneous mixtures have components that are very easy to distinguish from one
another. They exist in two or more phases.
Table 3.6 - Summary of the Different Types of Mixtures
Solution Suspension Colloid
 solute particles have dissolved to
the point of ions, atoms, or
molecules
 solute particles are evenly
dispersed through solvent
 particles do not settle out with time
 solute particles do
not dissolve fully
 particles form
groups of ions,
atoms, or molecules
 are evenly dispersed
through solvent, but
solution appears
cloudy
 particles do not
settle out with time
 really a mixture,
solute particles do
not dissolve
 particles form large
groups of insoluble
particles
 particles settle out
with time
 particles are too small to see with
naked eye (less than 1 nanometer
= 0.000000001 m)
 particles are usually
not seen with naked
eye (1 - 100
nanometers)
 particles can be seen
with naked eye
(larger than 100 nm)
 solute particles will pass through a
paper filter and a semipermeable
membrane; cannot be separated
except through distillation
 solute particles will
pass through a
paper filter; can be
separated by a
semipermeable
membrane, i.e.,
cellophane and cell
walls
 can be easily
separated by
filtering
 may be dilute or concentrated;
 may be unsaturated, saturated, or
supersaturated
 degree of saturation is dependent
on temperature; ex, more sugar
will dissolve when tea is hot)
 parts of a colloid
may be separated
by an
ultracentrifuge (spin
at very high speeds;
used to separate
blood)
 there are 9 types of solutions,
based on the solute (1st) and the
solvent (2nd) + example:
solute solvent example
gas gas air
 there are 3 types of
colloids:
 gels - liquid
particles in a
solid, flow slowly
 examples include
Italian salad
dressing, liquid
medicines that
require shaking

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gas liquid soda water
gas solid hydrogen in Pt
liquid gas water vapor in air
liquid liquid alcohol in water
liquid liquid silver amalgam
solid gas sulfur vapor in air
solid liquid sugar in water
solid solid brass
(gelatin, jelly,
stick deodorant)
 emulsions - two
liquids
(mayonnaise,
hand cream,
milk)
 aerosols - solid
or liquid in a gas
(fog, smoke,
paint-spray can)
before being taken;
and some paint
Separating mixtures
Sometimes it is important to be able to separate a mixture. There are lots of different ways to
do this. These are some examples:
a) Filtration
A piece of filter paper in a funnel can be used to separate a mixture of sand and water.
b) Heating / evaporation
Sometimes, heating a solution causes the water to evaporate, leaving the other part of
the mixture behind. You can try this using a salt solution.
c) Centrifugation
This is a laboratory process which uses the centrifugal force of spinning objects to
separate out the heavier substances from a mixture. This process is used to separate
the cells and plasma in blood. When the test tubes that hold the blood are spun round in
the machine, the heavier cells sink to the bottom of the test tube.
d) Dialysis
This is an interesting way of separating a mixture because it can be used in some
important applications. Dialysis works using a process called diffusion. Diffusion takes
place when one substance in a mixture moves from an area where it has a high
concentration to an area where its concentration is lower. This movement takes place
across a semi-permeable membrane. A semi-permeable membrane is a barrier that lets
some things move across it, but not others. This process is very important for people
whose kidneys are not functioning properly, an illness called renal failure.
APPLICATION
1. What happens is someone experience kidney failure?
2. How can you avoid kidney failure?

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SYNTHESIS
Part I .Complete the following diagram that shows the classification of matter
Part II. Classify each of the following substances as; an element, a compound, a solution, or a
heterogeneous mixture.
1. Sand 2. Salt 3. Pure Water 4. Soil
5. Soda 6. Pure Air 7. Carbon Dioxide 8. Gold
9. Bronze 10. Oxygen 11. Salad Dressing 12. Salt Water