unit 1 chemistry: classifying matter matters · unit 1 chemistry: classifying matter matters what...

Science 7 Mrs. Clement

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Unit 1 Chemistry: Classifying Matter Matters

What You Will Learn:

Who’s Who in the world of

Chemistry.

Atomic Theory is a law that

governed the universe

The history of chemistry.

An element is matter made up of

only one kind of atom.

The list of elements is known as

the Periodic Table of Elements.

Elements are pure substances.

Compounds are pure substances

that are made up of two or more

different elements.

All matter can be classified as pure

substances or mixtures.

Pure substances can be classified

as elements or compounds.

Mixtures can be separated by a

variety of methods.

Solutions can be measured by

concentration, solubility and

acidity.

Why chemistry is AMAZING:

Have you ever stared at frost crystals, watched a pot of water boil, or

melted an ice cube in a drink? Well, you are officially a chemist!

Chemistry is all about finding out WHY things do what they do. You will

observe, measure, and compare different types of matter, and conduct

some bubbly, fizzy, viscos, and, perhaps, even explosive experiments.

Without an understanding of chemistry, our world would be drastically

different: we would slip on icy sidewalks, plant blueberries in the wrong

type of soil, burn our skin with soap and would not, I am afraid to say,

have astronaut ice cream, non-stick frying pans, nail polish, computers or

microwaves!


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A Glance into the Future

Pre-quiz

check in

Lesson

Key Words

HW

Check

Post-quiz

check in

1.1 Why Matter Matters

Use Your Senses!

LAB #1: Mystery

Material

HW: Intro to Chemistry

Matter

Chemistry

p.9-10

Lab

p 11

HW

1.2 Historical Perspectives

Who’s Who chemists

Guess Who ACTIVITY

HW: Quick Check

Archimedes

Dmitri Mendeleev

John Dalton

p. 19

HW

1.3 Chemistry

Intro

LAB #3: Oil Spill

HW: Lab Q&A

Suspension

Emulsion

Solution

Picking apart

Filtering

Density

Magnetism

Dissolving

Evaporating

p.23-24

Lab

p.25-26

HW

1.4 Describing Matter

Qualitative properties

Quantitative properties

Lab #4: Observing and

Describing Materials

HW: Class Prep

Property

Quantitative

property

Qualitative

property

p.34-36

Lab

p.37 HW

1.5 Pure Substances and

Mixtures

Classifying

Pure Substances

Mixtures

LAB #5: Sort Em’

HW: Mixture Methods

Pure substance

Mixture

Alloy

Solution

Emulsion

Suspensions

Mechanical

mixtures

p. 40 Lab

P. 46-47

HW


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Date of miniquizes

#____: ______________________________

#____: ______________________________

1.6 Elements & Compounds

Periodic Table

Elements, Elements,

Elements

LAB #6: Atoms Model

HW: Reading to Find out

Elements

Compounds

Particles

Properties

p. 52

LAB

p.53-54

HW

1.7 Comparing Elements,

compounds and mixtures

Table

Review

HW: Elementary, my

dear

p. 63-64

HW

Unit Review & Quiz

Recap

Key words

Recap

p. 64


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How Do They Know That???

What do you already know about the properties of matter?

What do you want to know?

Follow up: who’s got the answers?

How can you tell the

difference between

gold and pyrite?

Why does ice melt on

metal plates faster

than plastic?

Why does water boil

at 100 C but silver

melts at 962 C?

Why does my bike

rust when I leave it

outside?

What is viscosity?

What is the

difference between

mass and volume?


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1.1 Use Your Senses (Textbook p. 102)

Which of the jars below is filled with water?

What is in the other jar?

What are the limits of this observation?

What would make the experiment easier to conduct?

Why should you never taste matter in the science lab? In science

class you are likely to work with materials that are toxic or

poisonous. For instance, there are several substances that are

similar to water in that they are colourless and often odorless:

bleach, hydrogen peroxide, salt water and so forth


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What is Chemistry?

What is Chemistry?

Where does chemistry take place?

What tools and equipment are involved?

What is Matter? What is Energy?

What is Matter? What is Energy?


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Examine the list of words below and sort them into two groups: one for

those things that you think would be classified as matter, and the other for

those that you think are non-matter. Once you are finished, explain why you

classified the list the way you did. In other words, what do the things in

each group have in common?

pizza air silk beauty juice x-rays

atom love soil heat hope sunshine

cold trees water people bacteria salt

Matter Non-Matter

What do these things all have in

common?

What do these things have in

common?


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Everything that you __________, ____________, _____________ and

___________ is made up of ______________. Matter makes up every

living thing and every material object. _____________ is the study of

matter and its changes.

Which of the words on the sign

do NOT describe matter? Which

words on the sign describe

matter? What is the difference?

Sense word Words that describe matter

Sight

Touch

Smell


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LAB #1 Mystery Material

Driving Question: How can you use your experience

to infer the identity of different materials?

Getting Started How well can you use your experiences and senses to infer the identity of

different materials?

Infer, or inference means _________________________________

In this activity you will be given 6 containers, each filled with a mystery material. Your

job is to use your senses and your experiences with everyday substances to identify each

mystery material. The first time around you will not be given any clues. After your initial

observations and your first inferences, you will then be told what the mystery materials

are. With this information make your second inferences.

Materials: - 5 containers, each filled with mystery material

- pencil to record results

1. Use the table on the following page to complete your observations.

Give your table a title.

2. Do not open the containers. Work with a partner, picking

up the containers one by one. Observe how heavy or light each

container feels. Rank the containers from lightest to heaviest.

Record your findings.

3. Infer what material might be inside each container. Record your

inferences.

4. Check with your teacher to find out the material inside each

container. Record the final outcomes on your table.


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Table: Observations of Five Mystery Materials

Rank from lightest

to heaviest

(Relative

mass)

Identity of Materials

1st Inference 2nd Inference Actual Identity

Lightest

Heaviest

Which material did you correctly identify? Did any materials surprise you?

Why or why not?


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Due Date: _______________

Introduction to Chemistry

1. What is matter: _____________________________

____________________________________________________

2. What is chemistry: _____________________________________

____________________________________________________

3. Complete the following table:

Property Describing the property

Clarity It is clear, cloudy, opaque, translucent…

It is black, white, colourless, red, blue and

greenish yellow…

Taste

Texture

It is spicy, sharp, odorless, sour…

Lustre


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1.2 Historical Perspectives

Science as an organized body of knowledge began with the Ionian School

of Greek Philosophers. Alchemy, one of the earliest forms of chemistry,

combines religion, science, philosophy, and magic. It developed in Alexandria,

Egypt, China and Greece sometime after the sixth century B.C.

Archimedes (287-212 BC) Discovered the Low of Buoyancy called Archimedes’

Principle. Archimedes’ Principle states that an object

placed into a liquid seems to lose an amount of weight

equal to the amount of fluid it displaces. Archimedes

conducted an experiment to determine how much

gold was in the king’s crown. He did so by measuring

the amount of water the crown displaced when it was

submerged in water. If the crown displaced the same

amount of water as an equal amount of gold, he could

determine if the crown was made of pure gold. Unfortunately for the king,

the crown was found to be impure and the goldsmith found to have skipped

town.

Democritus (460-370 BC) Developed the Atomic Theory of Matter, which

states that substances in the universe are make of

particles that could not be broken down further.

Later, these particles were called atoms, which is the

Greek word for “indivisible.” Democritus also

explained that atoms could not be created or

destroyed but could be rearranged in different

combinations. This was the beginning of the

development of the Law of Conservation of Mass and Energy.

Alchemy was the main source of chemical knowledge until 1600. Some of the

discoveries made during this time included producing chemical changes in

natural substances, improving methods for taking metal from ore, making and

using acids, and designing balances and crucibles.


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Al Razi (880-909 AD) The first to classify chemical substances into mineral,

vegetable, animal and derivative groups. He also

subdivided minerals into metals, spirits, salts and

stones.

Paracelsus (1500s) In the 1500’s, knowledge of

chemistry was used to fight

diseases. In the 1500’s and 1600s some alchemists were

called iatrochemists because they had begun to study the

chemical effects of medicine on the body. Paracelsus

accepted the belief that the four basic substances were

air, fire, water and earth. He believed these four basic

substances were made of mercury, sulfur and salt.

Andreas Libavius (1555-1616 AD) A follower of Paracelsus and wrote the first accurate

chemistry book called Alchemia, in 1597, which included

recipes for the preparation of several strong acids.

Jan Baptista van Helmont

(1580-1644) Believed only air and water were elements, and water was the

basic element of all plants. He invented the word gas and

studied gases released by burning charcoal and fermenting

wine.

Galileo Galilei (1564-1642) In 1592, Galileo developed a theomoscope, a

precursor to the thermometer. By the 1600’s,

chemistry became a science. Galileo was also famous

for his inventions in mathematics, astronomy,

physics and medicine.


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Jean Beguin (1550-1620) Wrote the first textbook of chemistry in 1611. He

defined chemistry as the search for medications. His

chemistry was therefore practical and experimental,

with a minimum of theory.

Francis Bacon (1561–1626) In the thirteenth century, Francis

Bacon had begun to use the experimental method of

chemical research by planning his experiment and

carefully interpreting his results. He died in April 1626

of pneumonia after experiments with ice.

Robert Boyle (1627-1691) Believed that theory must be supported

by experimentation. Boyle considered Van

Helmont’s study of gases, and through his

experiments, found that air, earth, fire,

and water were not elements. The

publication of his book, The Sceptical Chymist (1661), was the beginning of the

end of alchemy. In 1662, Boyle

discovered that there is an inverse relationship between the volume of gas

and its pressure, now referred to as Boyle’s Law. Boyle also rejected current

thought that matter was made of earth, air, water, and fire. He proposed

that matter considered of primary particles that could collect together to

make what he called “corpuscles.”

Joseph Priestly (1733-1804) During the 1700’s, many elements were discovered,

including oxygen and its role in chemical reactions. This

was one of the keys to modern chemistry. Priestly

conducted research on gases and discovered that what

would later be known as carbon dioxide,. While living next

door to a brewery, he discovered that the fermentation of


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grain gave off a gas that was heavier than air and put out fire. He also

discovered that when it was mixed with water, it made a refreshing drink,

soda water, which was the precursor to what is now

known as soft drinks.

Antoine-Laurent Lavoisier (1743-1794) Was considered the founder of modern chemistry

because of his strict approach to research. He drew up

the first rational system of chemical nomenclature. He

also studied combustion, and when he heard of the gas

that encouraged the burning process, he called it oxygen.

He defined burning as the uniting of substance with

oxygen.

Sir Humphry Davy (1778-1829) During the 1800’s, fifty element were discovered. Sodium

and potassium were discovered when Davy ran electricity

through substances containing them. This process was called

electrolysis. He also experimented with gases and

discovered nitrous oxide and its properties; however, he is

most well known for inventing a safely lamp for miners.

Friedrich Wöhler (1800-1882) Conducted research in organic and inorganic

chemistry. He and Justus von Leibig discovered that

the spatial organization of atoms within a molecule

was important in determining the kind of substance it

made.

Chemistry was later divided into three main

branches; inorganic, organic and physical chemistry.

Inorganic chemistry is the study of compounds

without carbon. Organic chemistry is the study of substances with carbon.

Physical chemistry deals with the study of heat, electricity, and other

forms of energy in chemical processes.


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John Dalton (1766-1844) In 1808, Dalton published an atomic theory suggesting

that each element was made up af certain kinds of

elements. His atomic weights were not correct;

however, he did formulate the Atomic Theory of

Matter. The Theory states that all matter is made up

of atoms. His theories were based on three

propositions: 1) all matter is made of extremely small

particles called atoms; 2) atoms of one element are

exactly alike; 3) when elements combine, they form compounds- their atoms

combine in simple numerical proportions.

Jöns Jacob Berzelius (1779-1848) Calculated more accurate atomic weights based

on Dalton’s atomic theory and Joseph Louis Gay-

Lussac’s (1778-1850) Law of Combining Volumes.

This law states that elements combine in definite

proportions by volume to form compounds.

Berzelius also introduced the used of atomic

symbols.

Mary Lyon (1797–1849) Founded Mount Holyoke College in Massachusetts, one of

the first women's colleges. At the time, most colleges

taught chemistry as a lecture-only class. Lyon made lab

exercises and experiments an integral part of

undergraduate chemistry education. Her method became

popular. Most modern chemistry classes include a lab

component.

Amedeo Avogadro (1776-1856)

In 1811 he discovered that there was a difference

between atoms and molecules. Stanislao Cannizzaro (1826-1910) demonstrated how Avogadro’s theory

applied to the measurement of atomic weights. This

work led to the development of the Periodic Law by

Dmitri Mendeleev and Lother Meyer.


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Dmitri Mendeleev (1834-1907) Developed the Periodic Law that states that elements

properties depend on its atomic weight. Mendeleev

developed this discovery into the Periodic Table the 63

elements known at this time. He left gaps in the table to

show that there were still more elements to be

discovered. There are currently 118 known elements.

Marie Curie (1867-1939) Pioneered radioactivity research. She was the first

two-time Nobel laureate and the only person to win the

award in two different sciences (Linus Pauling won

Chemistry and Peace). She was the first woman to win a

Nobel Prize. Marie Curie was the first female professor

at the Sorbonne.

Niels Bohr (1885-1962) Proposed the first model of the atom to incorporate into

quantum physics. Bohr devised the concept of having

electrons in different energy levels in an atom.

Alice Hamilton (1869-1970) Was a chemist and physician who directed the first

governmental commission to investigate industrial

hazards in the workplace, such as exposure to dangerous

chemicals. Because of her work, laws were passed to

protect employees from occupational hazards. In 1919

she became the first female faculty member of Harvard

Medical School.


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Marie Daly (1921–2003) Became the first African American woman to earn a

Ph.D. in chemistry. The majority of her career was

spent as a college professor. In addition to her

research, she developed programs to attract and aid

minority students in medical and graduate school.

Ruth Benerito (1916-) Invented wash-and-wear cotton fabric. Chemical

treatment of the cotton surface not only reduced

wrinkles, but could be used to make it flame

resistant and stain resistant.

Joan Berkowitz (1931- A chemist and environmental consultant.

She uses her command of chemistry to

help solve problems with pollution and

industrial waste.


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Due Date: _______________

Who’s Who Chemistry Quick Check

Matching

___________ 1. Archimedes a. developed Periodic Law

___________ 2. Democritus b. discovered Law of Buoyancy

___________ 3. Jean Beguin c. developed Atomic Theory of Matter

___________ 4. Antoine-Laurent

Lavoisier

d. founded the first women’s college

___________ 5. Dmitri Mendeleev e. founder of modern chemistry

___________ 6. Mary Lyon f. wrote the first chemistry textbook

Fill in the Blanks 6. The ________ ________ of matter states that all matter is made up

of atoms.

7. __________________ is the study of substances containing carbon.

8. Inorganic chemistry is the study of compounds without

_____________.

9. Joseph Priestly conducted research on gases and discovered what

would later be called __________________.

10. Niels Bohr proposed the first model of the _____________ to

incorporate quantum _____________________.

Timeline

Use the following statements to complete the timeline:

11. In the 1500’s, chemistry was used to fight diseases.

12. Between 1800 and 1900, 50 elements were discovered.

13. In 1611, Jean Beguin wrote the first accurate textbook

14. In 1661, Robert Boyle publishes The Sceptical Chemist

15. Oxygen and carbon are discovered by Joseph Priestly during the

1700’s.


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1.3 Chemistry

The term chemistry was used for the first time around 400-409 AD,

and it was used in reference to changing matter. Chemistry and the

__________________________ really has its roots in the kitchen-

pounding grain and other foods, boiling food in pots, straining to separate

solids and liquids, fermentation, etc. _________ was probably

one of the first chemicals used. Salt is found in the seas

and inside the earth. Salt has been used for many things,

including:

flavoring and preserving foods

melting snow and ice

softening water

processing fabrics and leather

mummification

making pottery

building churches

Salt was also used as a medicine in ointments, powders and syrups. Another

commonly used early chemical was ___________. It was used as a

preservative, in glasses and glazes for pottery, and in cleaning textiles.

Other chemicals were plant and animal dyes.

_____________ is the study of _____________ and how they interact

with other substances. The scientific definition of chemistry is the study of

the composition of matter and the changes that the matter undergoes.


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Chemistry is related to many areas of science including ___________,

______________, ____________, _____________, ___________, and

so on. There are many practical applications of chemistry in the world around

us. Clothes are made out of synthetic fibers and natural or man-made dyes.

Cooking is chemistry. For example, when baking a cake, several different

substances are mixed and baked, which results in a new substance.

In the 1800’s, chemistry was divided into three main branches:

_____________, ___________, and ____________ chemistry. Inorganic

chemistry is the study of compounds ______________________. Organic

chemistry is the study of substances ____________________. Physical

chemistry deals with the study of __________, _____________, and

other forms of __________________ in chemical processes. Two more

branches of chemistry were added: analytical chemistry, which deals with

the composition of substances, and biochemistry, which is the study of

chemistry of living things.

Some of the processes used by chemists are _____________,

_________________, _________________, and ________________..

Filtration uses ___________ materials to separate solids from

liquids. For example, the coffee filter allows the coffee oils through

but not the grounds.

Distillation is a process by which a _______________________ and

condensed back into a liquid. This process is used to separate liquids

from dissolved solids or volatile liquids from less volatile ones. For


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example, salt can be removed from seawater by allowing the water to

evaporate and re-condense in another container.

Fermentation is the production of ________________________

through the action of yeast of bacteria.

Sublimation is when a __________________________ without

changing to a liquid. For example, mothballs.

It is important to understand the basic concepts of chemistry and its

application because it is part of everyday life. One way the study of

chemistry is important is in trying to change the __________

effects of some ________________ of industry, such as

the impact that aerosols sprays have had on the ozone layer.


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LAB #3 Oil Spill

Question: Is it possible to clean oil spills?

Vegetable oil

Tablespoon

3 baking pans

Tap water

Spoon

String

Stir sticks

Cocoa powder

Salt

Blue food colouring

SORBENTS

Cheesecloth or gauze

Cotton balls

Cotton socks

Dish soap

Feathers

Materials:

1. Fill three different baking dishes with cold tap water within 1 cm of rim.

a. Dish A: Crude Oil

i. Add 2 tbsp. of cocoa powder.

ii. Mix cocoa powder and oil thoroughly with a paddle pop stick.

iii. Very slowly pour simulated crude oil from a height of 1 cm onto

the top of the fresh water Dish A. If you pour the oil too

quickly, the experiment won't work.

b. Dish B: Fresh water

i. Add 3 drops of blue food colouring

c. Dish C: Salt water

i. Add 2 tbsp. of salt

2. Place 3 tbsp. of vegetable oil in all three dishes.

3. Place a small sorbent sample into the centre top of the contaminated fresh

water. Record observations.

4. Remove sorbent with tweezers or tongs.

5. Repeat step 3 with other sorbent samples.

Part II

6. Clean out contaminated dishes.

7. Prepare new simulated water following instructions above.

8. Dip a feather into each oil-contaminated dish. Record Observations.

9. Add detergent to water to each dish. Record observations.


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Scientific Question: Is it possible to clean oil spills?

Hypothesis: ________________________________________________

_________________________________________________________

_________________________________________________________

_________________________________________________________

Observations: (include each solvents, feathers and soap)

Conclusion: ________________________________________________

_________________________________________________________

_________________________________________________________

_________________________________________________________

Fresh Water Crude Oil Salt Water

Solvent A

Solvent B

Solvent C

Soap

Feather


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Due Date: _______________

Quick Check Science LAB #2

1. What happened to the oil when you dropped it on the fresh

water/salt water/ crude oil? Did it sink? Float? Mix in?

2. How much oil did the sorbent clean up? How quickly?

3. Does the sorbent pick up water too? If so, how can you tell?

4. Does the sorbent sink or float?

5. What is the condition of the contaminated sorbent?

6. How would you pick up the oil-contaminated material in a "real" oil spill in

fresh water/the ocean?


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7. How would you dispose of the oil-contaminated material in a real oil spill?

8. Of the sorbents you tested, which one worked the fastest? The best?

9. What other materials could you use as sorbents?

10. What happened when the detergent was added to the contaminated

fresh water/ocean?

11. What happens when a feather gets oil on it?

12. How might an oiled feather affect a bird?


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1.4 Describe Matter using Observable Properties (textbook p. 106)

Qualitative and Quantitative Properties of Matter

What is a Property?

Each type of matter has its own set of _____________. A property is a

_________________ or feature of the matter.

Early bycicles were made almost entirely of wood -including the wheels.

Later models had wheels made of iron! Needless to say, early bicycles were

known as “boneshakers” and must have been very uncomfortable for the

cyclist to ride.

What properties of wood and iron make

these materials unsuitable for bicycle

tires?

Today, bicycle tires are made of rubber

filled with air. What properties of rubber

and air make them much more suitable for

bicycle tires?

Two Types of Properties

____________________ properties are those that can usually be

described using your _____________ (sight, smell, hearing, touch, but

never taste!)

_______________ properties are those that can be measured using simple

___________ and ________________.


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The photos below show two materials that share some of the same

properties. The one on the right is gold, and the one on the left is pyrite

which is also known as fool’s gold because it looks so much like gold.

Gold and pyrite have similar qualitative properties. What are the shared

_____________________ of gold and pyrite that may have contributed to

the confusion?

Any property of matter that can be ______________ using your

_____________ and described in words is called a QUALITATIVE

PROPERTY.

If you where given a piece of gold and a piece of pyrite and asked to tell

them apart, what other properties could you use to distinguish them?

Any property of matter that can be ______________________

______________________ is called a QUANTITATIVE PROPERTY.

Pyrite (Fool’s Gold) Gold

http://images.google.ca/imgres?imgurl=http://oneyearbible.blogs.com/photos/uncategorized/foolsgold.jpg&imgrefurl=http://www.oneyearbibleblog.com/2005/04/&h=277&w=425&sz=49&tbnid=lK7WStkIVbXNWM:&tbnh=79&tbnw=122&hl=en&start=10&prev=/images?q=fool's+gold&svnum=10&hl=en&lr=&sa=G


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Examples of Qualitative & Quantitative Properties of Matter

Classify the following properties of matter as either qualitative or

quantitative. (Note: some properties could be classified as both types.)

temperature, boiling point, melting point, bright, heavy, light, small, red, green, viscosity, elasticity, malleability, hardness, plasticity, state of matter (solid, liquid or gas), colour, odour, texture, density, texture (e.g., 80 vs 220 grit sand paper), conductivity, shape (e.g., 1 cm3 sugar cube), hot, cold, dark, rough, smooth, round, sharp, small, big, shiny, dull, odourless, mass, volume

Qualitative Properties of Matter Quantitative Properties of Matter

Properties can also be used to help you describe or identify unknown materials. Suppose you are given two beakers filled with a colourless liquid

and you are told that one of the liquids is water. How can you find out which

one is water?


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Why are qualitative properties not very useful for describing matter?

As you can see, there are many, many quantitative properties of matter.

Some of these properties we use every day (e.g., air temperature). Others

are used mainly by people in specialized fields such as metalworking,

engineering or materials science.

Challenge Yourself: Use the Internet to find out if the

following properties of matter are

qualitative or quantitative.

Property Qualitative or

Quantitative

Description

clarity

lustre

brittleness

ductility

Quantitative Properties of Matter You Must Know!

temperature

melting point

boiling point

mass

volume

density


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Qualitative Observation:

See Touch Smell Hear

Appearance

LUSTRE:

shiny/dull,

reflective

CLARITY:

transparent (clear)

opaque

translucent, cloudy,

milky, foggy, smoky,

COLOUR:

colourless

burning, powdery,

granular, bubbling,

fizzing,

Shape:

round, flat, oval,

spherical, square,

brick-shaped, egg-

shaped, oblong,

irregular, clumping,

symmetrical

State of matter:

solid, liquid, gas,

takes on shape of

container, moves, flows

Viscosity:

thick, watery, like

molasses

Temperature:

warm to the touch, cold to

the touch, freezing, hot,

room temperature, luke-

warm, (but, its still better

to measure temperature

using a thermometer)

Texture:

rough, smooth, bumpy, like

sand paper, furry, greasy,

feathery, slippery, jagged,

cottony, fluffy, leafy,

billowy, sharp,

Hardness:

hard, soft, malleable,

brittle, strength,

malleability, elasticity,

plasticity

ODOUR:

odourless,

acrid,

sour, rotting,

sweet,

overpowering,

floral, putrid,

cheesy, cedar-

scented,

choking, burning

sizzling,

popping

bubbling,

hissing,

cracking,

snapping

humming,

singing,

ringing,

thudding

booming,

burping

crunching,

clicking


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Quantitative Observation:

Quantitative

Property

Measuring Instrument Units Used

Mass Beam Balance or

electronic Balance

Milligrams: mg

Grams: g (= 1000 mg)

Kilograms: kg (= 1000g)

Tonnes: t

Volume

For regular solids: use a ruler to

measure dimensions of solid then use

formula:

V = l x w x h

For irregular shaped solids use the

water displacement method.

For liquids, use the appropriate sized

graduated cylinder.

Generally we use ...

mL, L, kL for liquids

and ...

mm3, cm3, m3 for solids,

although there are

exceptions to this rule.

Density

Calculated using the formula: D =

mass ÷ Volume

Note: Each pure substance at a given

temperature and pressure has its own

unique density. For example the density of water at room temperature and pressure

is 1.0 g/mL

For most gases, liquids or

irregular solids use:

g/mL

mg/mL

mg/L

g/L

For regular solids:

g/cm3

mg/cm3

mg/mm3

g/mm3

Varies depending upon the

volume and/or mass of

the material you are

measuring.


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Temperature

Thermometer degrees Celsius (˚C)

degrees Kelvin (K)

Absolute zero is the temperature at

which atoms stop moving-it’s very cold!

Absolute zero is equal to 0 K (read as

zero Kelvin).

0 K is equal to -273 ˚C

Melting point

(Freezing point)

Thermometer All materials have a characteristic

temperature at which they melt to

become a liquid or freeze to become a

solid. Most often measured in degrees

Celsius (˚C).

The melting point of water is _____

Boiling Point Thermometer All materials have a characteristic

temperature at which they boil to

become a gas. Most often measured in

degrees Celsius (˚C).

The boiling point of water is ____

Acidity (pH)

Note: pH is the

measure of the

percent of

Hydrogen ions in

a solution.

Litmus paper and

Chemical Indicators

such phenolphthalein,

bromothymol blue

Methyl orange

Using the pH scale: 0-14

7 is neutral pH (neither acidic nor basic)

Note: Pure water has a

neutral pH

Acids have a pH less than 7

Bases have a pH greater than 7

Note: You’ve probably realized that most properties of matter such as

strength, hardness, viscosity, malleability, elasticity, plasticity can also be

quantified. Even, colour, texture, and lustre can also be quantified (measured

and converted to a number value).


34

LAB #4 Observing and Describing Matter

Properties of matter that can be observed directly using your senses

are called ______________________ properties. (Note: These

properties are also refered to as observable properties.)

Materials:

- containers #1-17

- observation worksheet

- word bank

1. Work with a partner.

2. Choose 2 objects to analyze.

3. Observe the first material.

4. Describe the material’s qualitative attribute: sight, touch the smell

5. Find another team. Give them your description words and ask them

to identify your materials. Were they correct? How could you

improve your descriptions?

6. Complete the Q&A.

Observations:

Describe two (2) objects using your senses and the Word Bank for

Qualitative Properties of Matter. Use as many words as you can to

describe the object’s properties. Make an inference about the identity of

the object.


35

Object Sense

Used

Qualitative (Observable)

Properties

Inference Actual

Identity

Sight

Touch

Smell

Sight

Touch

Smell

Part II: What is it?

Find two students who did not observe the same materials you did. You are

to give them a few clues (qualitative properties) from your observation lists

to see if they can guess what material you are describing. Start with two

qualities and then keep adding until they can infer the material correctly.

1. How successful were the students at inferring the identities of the

objects when only a few qualitative properties were given? Explain.

____________________________________________________

____________________________________________________

____________________________________________________


36

2. Check with four or more other students to determine approximately how

many clues people needed in order to make an accurate guess. What did

you find out?

_______________________________________________________

_______________________________________________________

_______________________________________________________

3. Did you find that sense-related words led to more successful inferences?

Explain.

_______________________________________________________

_______________________________________________________

_______________________________________________________

_______________________________________________________

4. What did you learn about identification of materials by doing this

investigation?

_______________________________________________________

_______________________________________________________

_______________________________________________________

_______________________________________________________


37

Due Date: _______________

Class Prep Be prepared to share your answers with the class next day.

1. Are water, ice and water vapor the same type of matter? Explain.

2. How is a mixture of sugar and water different from a mixture of

sand and water?

3. How does pure water differ from tap water?

4. What are the similarities and differences between mass and weight?

____________________________________________________

____________________________________________________

BONUS: 10 ClementBucks

Find out what the words putrescine and cadavarine mean?


38

1.5 Pure Substances and Mixtures

(textbook p.132)

Substances

A substance that contains only

_________________________ __is called a pure

substance. There are millions of substances, but only a few

can be found in nature. For example, water is a pure

substance, but pure water is hard to find in nature. Even the

clearest spring water contains _____________________. In

nature, pure substances tend to mix with other substances. Diamonds are

one of the few exceptions. They are formed deep within the earth, in only a

few areas.

Most of the pure substances you encounter in your daily life have been made

purely by people through ___________. Aluminum foil is a pure substance,

and so is table sugar.


39

Mixtures

Almost all the natural substances and manufactured products in the world

are mixtures and pure substances. A mixture contains two or more pure

substances.

Whenever you see a sample of matter that has more than ones set of

properties, you know for sure that it is a mixture. For example, a sandy

beach, concrete, a bag of nuts.

There are two types of mixtures:

Homogeneous Heterogeneous The Greek word “homo” means the

same. Completely even mixing of the

components so that every part is

exactly the same composition. Cannot

detect different parts under a

microscope. Pure substance

The Greek word “hetero” means

different. Mixing of components is

uneven, even though it may appear

homogeneous. Sometimes a

microscope may be needed to see the

different parts.


40

Classifying Mixtures

As you have discovered, most of the substances in your

daily life are not pure substances. For example, hand lotion,

shampoo, makeup, and soap are all mode of many

substances (food colouring, perfumes, etc.). Food contains

preservatives and other additives. Even juice that is

labeled 100% pure is actually a mixture of water,

citric acid and other substances.

What are other common “pure substances”?

Mixtures can be categorized according to their

LAB #5 Sort Em’

Question: Is it possible to classify mixtures?

Materials: - photo cards with various types of mixtures

(i.e. homogeneous and heterogeneous)

- poster paper

- glue

- markers


41

Appearances

Mechanical

Mixture

- Heterogeneous Mixture.

- Parts are large and noticeably

different.

- Substances are easily seen.

Suspension - Heterogeneous mixture.

- Particles are large enough to be

seen and are mixed and

suspended in another substance

such as air or a liquid.

- Particles settle out quickly, or

within half an hour, and separate

into a mechanical mixture.

- Any substance that states

“Shake Well Before Using” is

likely a suspension.

Solutions - mixture that appears to be only

one substance.

- Parts of the solution are so

mixed that they cannot be seen,

even under a microscope.

- This is because the particles

that dissolve fill the spaces

between the particles od the

substances it dissolves in.

- Solutions are made up of two or

more metals, that are known as

alloys

Emulsion - Heterogeneous mixture. A type

of colloid where one liquid is

permanently suspended in

another liquid.

- Often an emulsifying agent is

needed to create this type of

colloid.

- Emulsions are opaque and usually

look creamy.


42

Other Mixtures:

Colloid - Heterogeneous mixture,

although appears to be

homogeneous.

- Particles are smaller than

those in suspensions and thus

do not settle out, but remain

permanently suspended.

- Colloids can be any

combination of phases (solid,

liquid, gas).

Emulsifier - A substance used to suspend

a liquid in another liquid. For

example, mustard or egg yolk

is used to suspend oil in

vinegar.

- The resulting substance

becomes a creamy emulsion.

- Mayonnaise is an example of

an emulsion.

Solution or Mechanical Mixture?

How can you tell if a mixture is a solution or mechanical mixture? Often you

can tell just by looking at it. What if you cannot?

- Use a microscope. If the mixture is a solution, you will be able to see

only one type of matter, even under a microscope

- If the mixture is a liquid, pour it through a filter. If anything is

caught in the filter, then the mixture is definitely not mechanical.

- Shine a light through it. Solutions contain no undissolved particles and

do not scatter light. Therefore, you will not see a beam running

through the solution. A heterogeneous mixture, however, does contain

undissolved particles that can scatter light.


43

Classifying Matter

1. Place an X beside the types of matter that correctly applies to

each example.

Type of

Matter

Sugar

water

Mayo Tap

water

Pizza Nitrogen

gas

Salt &

Water

Oil

and

H2O

Carbon

dioxide

Tin

in

lead

100%

Lead

O2

dissolved

in water

Pure

Substance

Element

Hetero-

geneous

Mixture

Homo-

geneous

Mixture

Mechanical

Mixture

Suspension

Emulsion

Colloid

Solution


44

Separating Mixtures

Do you have a “junk drawer”? Have you ever tried to sort out all the items

that have collected in it? In every day life, there are many situations in

which people want to separate the parts of mixtures. For example, you do

not want to drink water that contains fish or algae, or dissolved chemicals

from factories.

Depending on the mixture involved, separating the parts can be easy or

difficult. What are the ways you can separate mixtures, do you think?

A physical mix of pure substances can be separated by physical means such

as: picking and sorting large substances, magnetism, sifting, evaporation,

filtration, distillation, or chromatography.


45


46

Due Date: _______________

Mixture Methods

Describe the method you would use to separate each

mixture.

Mixture Method Marbles and

foam balls

Soil and water

Salt and pepper

mix

Sand and water

Wood chips and pieces of brick


47

Sand and pebbles

Sugar and water

Aluminum nails

and iron nails


48

1.6 Elements and Compounds (Textbook p. 145)

Elements are substances made up

of only __________________that

cannot be divided by ordinary

laboratory means. Ordinary laboratory

means might include _____________

_____________, ____________ or

_________. The _______________

states that an element’s properties

depend upon its atomic weight. Dmitri Mendeleev developed this discovery

into the _______________ of the 63 elements known during his time. He

left gaps in the Periodic Table showing that there were still more elements

to be discovered. Currently there are 118 known elements. By organizing the

elements by ______________ in the Periodic Table, groups of elements

emerged. The _____________ rows are periods. The Periodic Law states

that when elements are arranged by increasing atomic number, their

_______________________________________ are the same. These

periods are arranged according to the atomic number, which is the number

of protons in the nucleus. The columns represent groups or families that

have similar physical and chemical properties.

Each box on the Periodic Table has the atomic number, which

represents the number of protons, or ___________ charged particles, in

the nucleus. The number of electrons _____________________the


49

number of protons in an electrically balanced atom. Atoms of the same

element have the ________ number of protons but may have

____________ number of neutrons. Elements with different numbers of

neutrons are called isotopes. Atomic weights are determined by comparing

the element with an atom of carbon 12, which is assigned the weight of 12

units. The atomic mass numbers are often used in place of atomic weights.

Atomic mass is the number of protons and neutrons found in the atom.

Atoms can combine to

form new substances called

_________. Chemical ______

hold the atom of the molecule

together. Molecules are in

_______________. Molecules

are the smallest part of a

compound that still has the properties of the compound. Molecules are the

smallest part of a compound that still has the properties of the compound. A

molecule is a _________, chemically bonded group of atoms that act as one

unit. Molecules are in constant motion in all states of matter. Molecules are

a solid are packed tightly together, have strong cohesive force, and move

slowly. Cohesion is the attraction of _______________ Molecules of a

liquid are spread farther apart and have a lower cohesive force that allows

the molecules to slide over one another, and they move rapidly. In a _____,

molecules have very little cohesive force, and spread further apart, and

move very rapidly.


50

________________ allow substances to chemically react to other

substances to form new substances. These changes occur at the atomic or

molecular schedule. ______________ states that matter is made of atoms.

Atoms are the smallest part of an element and are the building blocks of all

matter; they combine to form elements and molecules. Atoms consist of

electrons, protons, and neutrons. Electrons have a

________________ and circle around the nucleus

of the atom. The nucleus contains protons and

neutrons. Protons have _____________, and

neutrons are neutral or have ____________.

Most of the mass of an atom is from the protons

and neutrons and is in the nucleus.

Models of the atom are changing as more is learned about them.

John Dalton: Atomic Theory stated that atoms were solid, indivisible

mass.

Dalton’s Atomic Theory


51

J.J. Thomson: discovered atoms contained neutrons. He described

the “plum pudding” model of an atom with charged electrons stuck into

a lump of positively charged material (i.e. A ball of peanut brittle with

the candy part making up the positively charged material and the

peanuts as the electrons). However, this model did not describe the

number of elements and protons, their arrangement, or that electrons

could be removed to form ions.

Ernest Rutherford: discovered that atoms contained a nucleus. He

proposed that atoms had a nucleus surrounded by electrons. He

thought the rest of the atom was empty space.

Niels Bohr: suggested that the electrons moved around the nucleus in

concentric circular paths or orbits. He further stated that electrons

in a particular path have a fixed energy. In order for them to move

from one orbit to another, they gain and lose energy. A quantum of

energy is the amount of energy needed to move an electron from its

current level to the next higher level. This concept is where the term

quantum leap, which describes an abrupt change, originates.

James Chadwick: discovered that he nuclei of atoms contained

neutrons that carried no charge.

Erwin Schrodinger: used quantum theory to develop the quantum

mechanical model of the atom. In this model, electrons have a

restricted value, but the do not have a specified path around the

nucleus. They are in a cloud around the nucleus.

Since the current theory of atomic structure consists of electrons,

protons, neutrons, and hundreds of subatomic particles, Bohr’s model is

the easiest level to understand.


52

LAB #6 Model of an Atom

Question: How can we model atoms

Materials: - Table of elements

- Balloons (3 different colours)

- String

- tape

Procedure:

1. Choose 4-6 elements from the Periodic Table

2. On the cue cards provided, make a detailed sketch of each

atom. Display the correct neutrons, protons, and electrons.

3. Gather material to create an accurate model for each atom.

4. Colour-code the balls so that it is easier to identify the each

part of the model.


53

Due Date: _______________

Reading to Find Out Read about elements and the periodic table on pages 146-147, and

then answer the questions below.

1. How many elements are listed in the periodic table? ____

2. How many of these exist naturally? _____

3. How many of these are made in the laboratory? ___

The periodic table is organized into groups (columns) and periods (rows).

The atomic number of the element Hydrogen is 1 and its symbol is H.

The elements in the periodic table are grouped based on their __________

and _______________ ________________ into four kinds of elements:

Metals like copper, sodium, and titanium

Non-metals like carbon, oxygen, fluorine and sulfur

Metalloids like boron, silicon, and antimony

Noble Gases like neon, argon, and krypton

GROUPS = VERTICAL COLUMNS

All elements in a particular group have the same number of electrons

in their outermost energy level. The Roman Numerals equal the

outermost electrons.

o Group 1 (IA) Alkali Metals: H, Li, Na, K…. all have 1 outer

electron

o Group 2 (IIA) Alkaline Earth Metals: Be, Mg, Ca… all have 2

outer electrons

o Groups 3 to 12 (IB to VIIB) Transition Metals: Fe, Ni, Cu, Zn,

Au, Ag…. Electrons vary

o Group 13 (IIIA) B, Al, Ga… all have 3 outer electrons

o Group 17 (VIIA) Halogens: F, Cl, Br, I… all have 7 outer

electrons


54

o Group 18 (VIIIA) Noble Gases: He, Ne, Ar,… all have 8 outer

electrons (except He has 2)

PERIODS = HORIZONTAL ROWS All elements in a particular period have the same number of electron

energy levels

o Period 1 - H and He have 1 energy level (can hold 2 electrons)

o Period 2 – Li, Be, B, C, N,… have 2 energy levels (1st holds 2 and

2nd holds 8 electrons)

o Period 3 – Na, Mg, Al, Si, P, S, Cl, Ar have 3 energy levels (2, 8,

and 8)

The 1st energy level holds 2 electrons

The 2nd energy level holds 8 electrons

The 3rd energy level holds 8 electrons at first, but later can hold 18

Look at the table below to see the patterns that are created in each group and

period

Alkali Metals

Group 1 (IA)

Alkaline Earth

Group 2 (IIA)

Halogens

Group 17 (VIIA)

Noble Gases

Group 18

(VIIIA)

Period 1 H 1 He 2

Period 2 Li 2-1 Be 2-2 F 2-7 Ne 2-8

Period 3 Na 2-8-1 Mg 2-8-2 Cl 2-8-7 Ar 2-8-8

Period 4 K 2-8-8-1 Ca 2-8-8-2 Br 2-8-18-7 Kr 2-8-18-8

Period 5 Rb 2-8-18-1 Sr 2-8-18-2 I 2-8-18-18-

7

Xe 2-8-18-18-8

Period 6 Cs 2-8-18-18-8-

1

Ba 2-8-18-18-

8-2

At 2-8-18-32-

18-7

Rn 2-8-18-32-

18-8

Period 7 Fr 2-8-18-32-

18-8-1 Ra 2-8-18-

32-18-8-2 Uus 2-8-18-32-

32-18-7 Uuo 2-8-18-32-

32-18-8


55

Elements, Elements, Elements…

1. For each of the following elements...

Give their symbol.

Place an M beside those that are metals,

Place an G beside those that are a gas at standard temperature

and pressure,

Place a S beside those that are a solid at standard temperature

and pressure

Place a NM beside those that are non-metals,

Place a NG beside those that are noble gases,

Circle the heaviest element in the group,

Shade the lightest element in the group

Lead Silver

Silicon Neon

Phosphorus Aluminum

Flourine Oxygen

Sodium Gold


56


57

2. 2. Use your periodic table to list the missing information for each

element. Note: Be sure to include units for melting point and density values.

20 40

Ca

_________

Element Name:

_______________

Atomic Number: _____

Atomic Mass: ______

Number of Protons _____

Number of Electrons _____

Number of Neutrons _____

Melting point ______________

Density _____________

54 131

Xe

_________

Element Name: _______________


Atomic Mass: ______





Density _____________


58

Element Name: _______________


Atomic Mass: ______





Density _____________

5 11

B

_________

Check out the following website for more information on the Periodic

Table:

http://www.colorado.edu/physics/2000/periodic_table/index.html

http://www.colorado.edu/physics/2000/periodic_table/index.html


59

1.7 Comparing Elements, Compounds and Mixtures

Substance Can it be

broken

down into

a simpler

substance?

If it can be broken down

into a simpler substance, is

this accomplished physically

or chemically?

Is it a(n) element,

compound/mixture?

Water

(H2O)

Epsom salt

(magnesium

sulfate)

Graphite

(carbon)

Oil and

vinegar

1. Which type of matter cannot be broken down into a simpler substance?

Give three examples of this type of matter.

2. Which types of matter can be broken down into simpler substances?

_______________________________________________________

3. Which type of matter can be broken down into simpler substances by

chemical means? _________________________________________

_______________________________________________________

_______________________________________________________

4. Which type of matter can be broken down into simpler substances by

physical means? _________________________________________

______________________________________________________

5. Which type(s) of matter are pure substances? Which are not?

_______________________________________________________

_______________________________________________________


60

6. Use the information from the table above to help you explain the

difference between an element, a compound and a mixture. ____________________________________________________________________________________________________________________________________________________________________________________________________________________________

Subatomic Particles and their Characteristics.

Subatomic

Particle

Electrical

Charge

Relative Mass

Where in the atom is it

located?

Protons

Neutrons

Electrons

7. What do scientists believe the atom looks like? Draw a sketch labelling,

the nucleus, orbits, protons, neutron, and electron.

8. What makes an atom stable?

9. How do atoms become stable?


61

10. What is electron affinity?

11. What is atomic number? What is atomic mass?

12. How are elements in the periodic table organized?

13. Which group of elements is most reactive? Give three examples.

14. Which group of elements is least reactive? Why are these elements non-

reactive? Give three examples.


62

Due Date: _______________

Elementary, my dear

Complete the following chart (Textbook p.150)

Look at the two-dimensional model of the atom to

answer questions 1-2:

1. The atom has _______ protons.

a. 9

b. 0

c. 1

d. 10

Matter

Solution (heterogeneous)

Pure Substance

(homogenious)


63

2. The atom has ______ electrons.

a. 9

b. 0

c. 1

d. 10

3. Write the symbol or name for each of the following elements. Refer to

the Periodic Table on page 56 of this workbook or page 147 of the

textbook.

a. Fe _____________

b. Potassium _________

c. Ca _______

d. Gold ___________

e. B __________

4. Match the following terms with the correct definitions.

___________ 1. Attraction to substances a. elements

___________ 2. States that all matter is made of atoms b. protons

___________ 3. Have a positive charge c. Atomic Theory

___________ 4. Have a negative charge d. electrons

___________ 5. Substances made up od only one kind of

atom

e. cohesion

Bonus: $10 ClementBucks

True or False

1. _______ Smog is heterogeneous

2. _______ Soda is heterogeneous

3. _______ Gold is homogeneous

4. _______ The human body is homogeneous


64

To Recap

Mixtures can be separated through:

o filtration

o sifting

o magnetism

o evaporation

o flotation

o dissolving

o panning

An element cannot be broken down into simpler substances by a

chemical change.

Each element is made of a different kind of atom

The 116 known elements are listed in the Periodic Table

A molecule is made of more than one atom linked together

A compound is made of chemically combined material.

Mixtures can be classified as heterogeneous or homogeneous solutions

Mechanical mixtures, suspensions, emulsions or solutions are types of

heterogeneous mixtures

Matter can be classified through a flowchart

Homogenous materials have the same properties throughout

Heterogeneous materials have different parts with different

properties

Pure substances contain only one type of matter. They are

homogeneous

Mixtures contain two or ore types of matter. Mixtures can be

heterogeneous or homogeneous.

Date of Unit 1 Chemistry Quiz: ______________________________

unit 1 chemistry: classifying matter matters · unit 1 chemistry: classifying matter matters what...

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