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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) 500oC 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