what is matter? - web viewa substance that contains only one kind of particle is called a pure...

Science 7 Mrs. Clement

Unit 1 Chemistry: Classifying Matter Matters

What You Will Learn:

Who’s Who in the world of Chemistry.

Atomic Theory was a law that governed the universe… until recently.

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.

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

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3

Pre-quiz check

inLesson Key Words

HW Check

Post-quiz check in

1.1 Why Matter Matters Use Your Senses! LAB #1: Mystery

Material HW: Intro to Chemistry

MatterChemistry

p.9-10 Lab

p 11HW

1.2 Historical Perspectives Who’s Who chemists Guess Who ACTIVITY HW: Quick Check

ArchimedesDmitri MendeleevJohn Dalton

p. 20HW

1.3 Chemistry Intro LAB #4: Oil Spill HW: Lab Q&A

SuspensionEmulsionSolutionPicking apartFilteringDensityMagnetismDissolvingEvaporating

p.34-35 Lab

p.36-37HW

1.4 Describing Matter Qualitative properties Quantitative properties Lab #3: Observing and

Describing Materials

PropertyQuantitative propertyQualitative property

p.28-30 Lab

1.5 Pure Substances and Mixtures Classifying Pure Substances Mixtures LAB #5: Sort Em’ HW: Mixture Methods

Pure substanceMixtureAlloySolutionEmulsionSuspensionsMechanical mixtures

p. 40 Lab

P. 46HW

1.6 Elements & Compounds Periodic Table Elements, Elements,

Elements HW: Elementary, my

dear

ElementsCompoundsParticlesProperties

p. 57-58 HW

1.7 Comparing Elements, compounds and mixtures Table Review

Unit Review & Quiz

Recap Key words


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 if filled with water?What is in the other jar?

What are the limits of this observation?

What would make the experiment easier to conduct?

What is Chemistry?

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?

Where does chemistry take place?

What tools and equipment are involved?

What is Matter? What is Energy?

What is Matter? What is Energy?

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

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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-raysatom love soil heat hope sunshinecold trees water people bacteria

salt

Matter Non-Matter

What do these things all have in common?

What do these things have in common?

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.

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Which of the words on the sign do NOT describe matter? Which words on the sign describe matter? What is the difference?

LAB #1 Mystery Material

Driving Question: How can you use your experience to infer the identity of different materials?

Getting StartedHow 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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Sense word

Words that describe matter

Sight

Touch

smell


Table: Observations of Five Mystery MaterialsRank 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?

LAB #1 Mystery Material

Driving Question: How can you use your experience to infer the identity of different materials?

Getting StartedHow 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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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…

TasteTexture

It is spicy, sharp, odorless, sour…Lustre

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

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

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

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3. How does pure water differ from tap water?

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

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1.2 Historical PerspectivesScience 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. Al Razi (880-909 AD)

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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.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.

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

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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. Physical chemistry deals with the study of heat, electricity, and other forms of energy in chemical processes.

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

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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.

Dmitri Mendeleev (1834-1907)Developed the Periodic Law that states that an elements properties depend on its atomic weight. Mendeleev developed this discovery into the Periodic Table the of 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.

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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.

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

Lavoisierd. 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 Blanks6. 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 textbook14. In 1661, Robert Boyle publishes The Sceptical Chemist15. Oxygen and carbon are discovered by Joseph Priestly

during the 1700’s.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

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__________________________ 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. 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

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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 condescended back into a liquid. This process is used to separate liquids from dissolved solids or volatile liquids from less volatile ones. For 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 #4 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 Oili. 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 wateri. Add 3 drops of blue food colouring

c. Dish C: Salt wateri. 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: ________________________________________________ ___________________________________________________________________________________________________________________________________________________________________________

Due Date: _______________Quick Check Science LAB #2

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Fresh Water Crude Oil Salt Water

Solvent A

Solvent B

Solvent C

Soap

feather


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?

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

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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

Qualitative and Quantitative Properties of Matter

What is a Property?Each type of matter has its own set of PROPERTIES. A property is a characteristic or feature of the matter.

Early bicylces 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 PropertiesQUALITATIVE properties are those that can usually be described using your

senses (sight, smell, hearing, touch, but never taste!)

QUANTITATIVE properties are those that can be measured using simple tests and equipment.

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.

Pyrite (Fool’s Gold)

Gold

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Gold and pyrite have similar qualitative properties. What are the shared qualitative properties of gold and pyrite that may have contributed to the confusion?

Any property of matter that can be observed using your senses 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 distinquish them?

Any property of matter that can be measured or describe with a numerical value is called a QUANTITATIVE PROPERTY.

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

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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


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?

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.

Quantitative Properties of Matter You Must Know!

temperaturemelting pointboiling point

massvolumedensity

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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

britteness

ductility

Qualitative Observation:

See Touch Smell Hear

Quantitative Properties of Matter You Must Know!

temperaturemelting pointboiling point

massvolumedensity

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AppearanceLUSTRE:shiny/dull,reflective

CLARITY:transparent (clear)opaquetranslucent, 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, poppingbubbling, hissing,cracking, snappinghumming, singing,ringing, thuddingbooming, burpingcrunching, clicking

Quantitative Observation:

Quantitative Property

Measuring Instrument Units Used

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Mass Beam Balance orelectronic Balance

Milligrams: mgGrams: 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/mLmg/mLmg/Lg/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 andChemical Indicators

such phenolphthalein,

bromothymol blueMethyl orange

Using the pH scale: 0-147 is neutral pH (neither acidic nor

basic)Note: Pure water has a

neutral pHAcids 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).

LAB #3 Observing and Describing Matter

Properties of matter that can be observed directly using your senses are called ______________________ properties. (Note: These

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Object Sense

Used

Qualitative (Observable)

Properties

Inference ActualIdentity

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.____________________________________________________________________________________________________________________________________________________________

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?

LAB #3 Observing and Describing Matter

Properties of matter that can be observed directly using your senses are called ______________________ properties. (Note: These

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_____________________________________________________________________________________________________________________________________________________________________

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?____________________________________________________________________________________________________________________________________________________________________________________________________________________________

BONUS: 10 ClementBucks

Find out what the words putrescine and cadavarine mean?

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1.5 Pure Substances and Mixtures(textbook p.132)

A substance that contains only one kind of particle 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 dissolved materials. 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 refining. Aluminum foil is a pure substance, and so is table sugar.

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.

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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 HeterogeneousThe 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.

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http://www.bing.com/images/search?q=different+coloured+balls&view=detail&id=AA72D7162303D51B57BE678E9DAA5AEFA0A7E234&first=301&FORM=IDFRIR

http://www.bing.com/images/search?q=different+coloured+balls&view=detail&id=490659D133A68D0E3DD30E2318F7F50DDDB404BF&first=271&FORM=IDFRIR


Classifying MixturesAs 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 Appearances

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

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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.

Other Mixtures:

Colloid - Heterogeneous mixture, although appears to be homogeneous.

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- 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.

Classifying Matter

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

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Separating MixturesDo 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?

Type of Matter

Sugar

water

Mayo

Tap water

Pizza

Nitrogen gas

Silt &

Water

Oil and

H2O

Carbon

dioxide

Tin in lead

100%

Lead

O2 dissolved in water

Pure Substance

Element

Hetero-geneous MixtureHomo-geneousMixtureMechanical Mixture

Suspension

Emulsion

Colloid

Solution

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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.

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Due Date: _______________Mixture Methods

Describe the method you would use to separate each mixture.

Marbles and foam balls

Sand and water

Soil and water

Salt and pepper mix

Wood chips and pieces of brick

Sand and pebbles

Sugar and water

Aluminum nails and iron nails

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1.6 Elements and Compounds(Textbook p. 145)

Elements are substances made up of only one kind of atom 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 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

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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 sill has the properties of the compound. A molecule is a _________, chemically bonded group of atoms that acts 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 farther apart, and move very rapidly.

________________ 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

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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

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

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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 electronics, protons, neutrons, and hundreds of subatomic particles, Bohr’s model is the easiest level to understand.

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Elements and the Periodic Table

Reading to Find OutRead 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 electronso Group 17 (VIIA) Halogens: F, Cl, Br, I… all have 7 outer

electrons

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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 levelso 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 MetalsGroup 1 (IA)

Alkaline EarthGroup 2 (IIA)

HalogensGroup 17 (VIIA)

Noble GasesGroup 18 (VIIIA)

Period 1 H 1 He 2Period 2 Li 2-1 Be 2-2 F 2-7 Ne 2-8Period 3 Na 2-8-1 Mg 2-8-2 Cl 2-8-7 Ar 2-8-8Period 4 K 2-8-8-1 Ca 2-8-8-2 Br 2-8-18-7 Kr 2-8-18-8Period 5 Rb 2-8-18-1 Sr 2-8-18-

2I 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

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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

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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 _____________

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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

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


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. 9b. 0

c. 1d. 10

2. The atom has ______ electrons.a. 9b. 0

c. 1d. 10

Matter

Solution (heterogeneous

)

Pure Substance(homogenious)

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3. Write the symbol for each of the following elements. Refer to the Periodic Table on page 30 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 ClementBucksTrue or False

1. _______ Smog is heterogeneous2. _______ Soda is heterogeneous3. _______ Gold is homogeneous4. _______ The human body is homogeneous

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1.7 Comparing Elements, Compounds and Mixtures

Substance

Can it be

broken down into a

simpler substan

ce?

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? ______________________________________________________________________________________________________________

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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?

10. What is electron affinity?

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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.

To Recap

Mixtures can be separated through:o filtrationo siftingo magnetismo evaporationo flotationo dissolvingo panning

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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: ______________________________

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what is matter? - web viewa substance that contains only one kind of particle is called a pure...

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