Name

Class Color/ Period

Unit 0: Introduction to Chemistry (Measurement and Matter)

Regents Chemistry

Mrs. Young: Irondequoit High School

Learning Targets: By the end of this unit I Can…1. I can explain what chemistry is.2. I can describe how the nature of science is related to chemistry. 3. I can perform math calculations using proper significant figures.4. I can display numbers in both standard and scientific notation.5. I can explain how and why dimensional analysis can be a useful tool for completing metric unit conversions. 6. State that matter is classified as a pure substance or as a mixture of substances7. State that a pure substance (element or compound) has a constant composition and constant properties throughout a

given sample and from sample to sample. 8. Use particle models/ diagrams to differentiate among elements, compounds and mixtures.9. State that elements cannot be broken down by chemical change.10. State that mixtures are composed of two or more different substances that can be separated by physical means11. Distinguish between homogeneous and heterogeneous mixtures12. Explain that the proportions of components in a mixture can be varied. Each component in a mixture retains its original

properties.13. State that a physical change does not change the identity or properties of the substances(s) present, while a chemical

change results in the formation of different substances with changed properties. Identify changes as either physical or chemical.

14. State that differences in properties such as density, particle size, molecular polarity, boiling point & freezing point & solubility, allow physical separation of parts in a mixture.

15. Describe the process and use of filtration, distillation, and chromatography in the separation of a mixture.

Essential Questions:

What are particles and how can we model their

physical behavior?

How does the relative placement of particles

affect a substance’s properties?

How is matter classified and described?

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calendar

2

Introduction to Chemistry. What is Chemistry and how is it “done”?

BRIDGE: On the small sheet of paper you picked up on your way in, write one word, phrase or sentence that comes to mind when you hear the term “science” (1). MINI-LESSON:

Chemistry is the study of (anything that has ______________ and occupies ______________) and the _______________ that it undergoes.

One of my goals for you is that you will be able to think .

Pause for a challenge learning experience:

1. Share the word or phrase you wrote when you came in with your team (what comes to mind when you hear the term “science”)Keep this word in mind as you complete your next step.

2. Use the manipulatives that Mrs. Young gives you to complete task #1. a. On you intro sheet, write down at least one word about how you felt as you completed your task (2).

3. Once you’ve completed task #1 and reflection, ask for task #2.a. On you intro sheet, write down at least one word about how you felt as you completed your task (3).

4. Share the two word with your table and develop a sentence about how the words above connect to science that you will share with the class. Note: There are no “correct” answers here. One person needs to write this on their intro sheet.

5. After listening to your classmates write a reflection on your intro sheet about how this activity might be related to science

6.

Nature of science is defined as:

Nature of Science:

Directions: Use the information above, on the following pages, your prior work in science classes, and the internet (if needed write the website you used) to help you complete this assignment.

Vocabulary: Define the following words and concepts related to the scientific method in your own words.

1. Independent Variable: _____________________________________________________________________

2. Dependent Variable: ______________________________________________________________________

3. Control Variable (aka constants):_______________________________________________________________

4. Purpose of multiple trials:_____________________________________________________________________

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Workshop/ Assignment

0.1

Topic 0.2

the of information through various forms of direct and indirect and the testing of this information by methods including, but not limited to, . The principal product of science is knowledge in the form of naturalistic concepts and the laws and theories related to those concepts.

Deeper Understanding: 5. How is an observation different from a conclusion?

6. What should you see in a well-designed experiment? (Describe at least 3 things)

7. What is the difference between an independent variable and a dependent variable? If these variables had to be graphed, which would go on the X versus the Y axis?

Practice: Read the following scenarios and answer the questions that follow. Not sure if you “get it” with independent versus dependent? Go to this website https://tinyurl.com/gltodfv and try 4 before you write down your

answers to homework. 8. Eating breakfast increases performance in school.

Hypothesis: If ____________________________ ___, then _________________________________________

Independent Variable: ___________________________ Dependent Variable: ________________________

Control Group: ________________________________ Experimental Group: ________________________

9. Jack wants to find out which laundry detergent cleans the best. So, he takes a cotton sheet and cuts it up into equal squares. He stains four squares with chocolate, and four with grape juice. He washes one of each of the squares in each of the 3 detergents (tide, arm and hammer, and Wegmans brand). One from each set of squares is washed in water alone. For each wash load, he used: the same amount of water, the same amount of detergent, and the same temperature of water.

Independent Variable: _______________________________________________________________________

Dependent Variable: ________________________________________________________________________

What is held constant? _______________________________________________________________________

Hypothesis: ________________________________________________________________________________

10. How can the above experiment be improved? _________________________________________________________ ____________________________________ ___

11. Read the nine statements on the next page about the nature of science (from NSTA: http://www.nsta.org/about/positions/natureofscience.aspx). After reading them all circle the one you believe is most true of science for YOU and put an “X” on the bullet that you find to be the most surprising or that you disagree with.

a. Write a reflection here about your choices. This should be at least 3 sentences in length and have an example of why you feel this way.

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Assignment 0.1 (cont)

5

Scientific Notation: How can Sharklet ® help us understand the importance of units?

Background Information: Let’s watch this video before we begin: https://www.youtube.com/watch?v=nyfsuXGMG4Q

Sharkskin has a nano-sized pattern of bumps and ridges on its dermal denticles.

A shark’s skin has 2 purposes:

1. It helps the shark swim quickly and quietly without much drag. (Mimicked in Olympic swimsuits)

2. It is a natural antimicrobial. It deters living organisms from growing onto it. (Mimicked in Sharklet® film)

Sharklet® is a new product inspired by sharkskin and is being used to create surfaces that will inhibit the growth of bacteria. Therefore, we can have desks, chairs, and other common areas that will not transmit germs from one person to another.

Soap, antibacterial cleaners, or other disinfectants are commonly used to sanitize areas. However, antibacterial products are washed down the drain and get into our waterways. Also, the use of these chemicals causes an increase in antibiotic-resistant bacteria.

In this lab, we will take a closer look at the Sharklet® film that is being used as a surface to inhibit the growth of bacteria.

Pre-Lab Questions:

1. What are bacteria, and how do bacteria grow?

2. How do people manage bacterial growth? Cite some traditional ways to manage bacterial growth.

3. What is Sharklet®? How does it work?

NOTES: In chemistry, we will be working with numbers that are very BIG and very small. The electron microscope that they used to look at sharklet (as well as shark skin) magnifies objects to be MUCH larger than they appear…

How much do you think it magnifies? . That’s a greater magnification than the number of people who live in Sweeden!!!

Scientific notation is a SHORTER way to write a number or a number.

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Topic 0.3

How do we create and use scientific notation?

1) Determine where the is.

2) Move the decimal to form a number between and .

3) Count how many places you moved the decimal.

4) note how many places you moved the decimal with a

- If the number was HUGE, your exponent should be .

- If the number was TINY, your exponent should be .

Examples/ Practice1. 3,647,000,000

2. 56,000,000,000,000

3. 200,000,000,000

4. 0.00000173

5. 0.000000502

Working Backwards- Can you go from scientific notation to standard form now???6. 3.78 x106 (number got because exponent was )

7. 1.0654 x 10-7 (number got because exponent was )

Application: Write in standard/ scientific notation. One sharklet “triangle” that help avoids all that bacteria is about 2.4 x 10-4 meters across

The number of molecules in a mole is 602,000,000,000,000,000,000,000

Decimal points are SO important in sci. notation. They move either to the LEFT or RIGHT to determine the #.

Practice with Scientific and Standard notation: If the number is in scientific notation (you see x10#) then convert to standard. If the number is in standard notation convert to scientific notation: 14) 101,000 19) 1.901 x10-7

15) 2.30 x 104 20) 0.000023

7

HW: 0.2 Once you get your answer, check it! Does it make sense?

16) 45.01

17) 3.2 x 101

18) 7110.07

Conversions and dimensional analysis: How can Sharklet ® help us understand the importance of units?

What’s important with conversions?Read the paragraph below and underline one phrase in EACH sentence that you think is the most important.

For the Regents, the most you will have to convert will be between the milli-/kilo-/base unit (g, L, etc.). This is always

a matter of three or six decimal places. You must also make sure you move the decimal the correct direction (right

or left, which depends on whether you are converting from small to big or vice versa).

What’s your TRICK? How do you “memorize” the order of the metric prefixes?

Kilo hecto deca base unit deci centi milli Practice! Show all work.

1. A car travels 845 km. How many meters is this?

2. Convert 0.0290 L to milliliters.

3. Convert 2500mL to L.

3. 6.3 g = _______ kg

4. 7.1 km = ______ m

5. 8.1 kg = _______ g

6. 1 L = ________ mL

7. 7 m = _______ mm

8. 12 mL = ______ L Compare by placing a < ,> or = on the line provided:

9. 56 cm ____ 6 m 11. 7 g _____ 698 mg

What about the Sharklet? Here is an Image of Sharklet® film from under an electron microscope

8

K__________

H__________

D__________

U(base

unit______)

D__________

C__________

M__________

Topic 0.4

What is the length of one diamond pattern on the surface of the Sharklet® film in microns (micrometers)?

Is “Micro” in our mnemonic device? What do we do?

Dimensional Analysis notes In chemistry, you will develop skills necessary to solve

problems. One method to problem solving that is extremely useful in

chemistry is:

- Use to your advantage by labeling (no naked numbers)!- We can convert between units by using .

o These are

o For example

The Metric System The metric system is a standardized system of measurement used by scientists throughout the world. It is also the measurement system used in everyday life in most countries. Unlike the English system with which you are already familiar, the metric system is based on units of ten, thus simplifying interconversions. This base-ten system is similar to our monetary system, in which 10 cents equals a dime, 10 dimes equals a dollar, and so on. Units of ten in the metric system are indicated by Latin and Greek prefixes placed before the base units:

1. What is a Base Unit & what table are they on?

2. Find the “selected units” table on your reference tables. What are the SI Base Units for:Volume = ____________________

Length = ____________________

Mass = ____________________

Energy = ____________________

3. What table can you find Metric Prefixes on?

4. Check out how the exponent # is different from the chart. What does this mean in terms of the decimal place and what we’ve learned with scientific notation?

Exponent #

1x106 1x103 1 x 100 1x10 –1 1x10 –2 1x10 -3 1x10 –6 1 x 10 -9 1x10 –12

Whole # 1,000,000.

1,000. 1 .1 .01 .001 .000001

.000000001 .000000000001

Abbrev. M k Base Unit

d c m u n p

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Topic 0.4

Prefix Name

Mega kilo Base Unit

deci centi milli micro nano pico

5. How do you convert in the metric system? – Use dimensional analysis and multiply given unit by a conversion factor using Table C

Sample Problem: Convert 170.2 kilo grams to micro grams

Step 1: List all conversion factors necessary (use reference table C as necessary)

103g = 1 kg 10-6 g = 1microgram

Step 2: Set up your “Railroad Tracks” and include your given value with units

Step 3: Find the conversion factor can be used to cancel the initial units using division and enter into chart.

Step 4: Continue to determine which conversion factor can be used to cancel the units to end up with the final correct units when done cancelling (what unit does the problem ask for in the end).

Step 5: Multiply across the top and divide by the bottom:

6. What about the length of the sharklet? We know that each diamond is about 2.4 x 10-5 meters. How many micrometers is this and is it close to our predicted value from the bottom of page 8?

Directions: Use dimensional analysis to solve the following problems. Show your work & include units in final answer!!1. How many dollars are in 27 quarters? Be sure to list your conversion factors.

2. 3 days seconds

3. 9,474 mm cm

10

Is it our predicted value?

4. 1 year minutes

Dimensional Analysis is basically a very simple type of algebra that lets us take measurements and convert them into other units in a relatively foolproof way.

1) What are the final units?

Yellow jacket x Dawg 3 x Seminole 2 x _Blue Devil x Gators x _Yellow Jacket = Gators2 Yellow Jacket2 Seminole Seminole Blue Devil

To get credit you MUST show your dimensional analysis work (like above, but using these conversion factors). Be sure to START with the number given in the problem

2) Convert 22 quackzils to dabbles using the following conversion factors:9.3 dabbles= 1.2 flapzits12 quackzils= 1.5 buttons4 flapzit = 3.2 buttons

3) Convert 2.02 lier to kneiew19 kneiew = 2.3 eiooe 5.34 lier = 7.6 koeilel 9 koeilel = 3 eiooe

4) Convert 8.01 kilement to flapereioe 2 flapereioe = 7 waltlere 5 kilement = 0.25 unbuclle2 waltlere = 1.5 unbuclle

5) Convert 101 Dalmatians to spots4.5 Dalmatians have 18 pawsFor every 4 paws there are on average 10.45 grams of drool For every 5.02 grams of drool it is expected there are 3.2 spots

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Assignment 0.3

EXTRA CHALLENGE: Sally Leadfoot was pulled over on her way from Syracuse to Ithaca by an officer claiming she was speeding. The speed limit is 65 mi/hr and Sally had traveled 97 km in 102 minutes (start with the bolded value). How fast was Sally’s average speed? Does she deserve a ticket? ***

Significant Figures (“Sig Figs”)

1) In chemistry class, we will be doing many labs and experiments whereit’s important to be accurate and precise.

2) Why sig figs?a. Consider the following measurements:

8 cm 8.0 cm 8.00 cm3) More digits indicate a more precise measurement4) We are limited by our equipment!5) Significant figures in a measurement include the known digits plus

one final estimated digit

Why Do significant figures matter? A Significant Win: You may recognize this famous gold medalist. He’s

Michael Phelps, the world-champion swimmer. The times of world-class athletes like Michael Phelps may be measured to the hundredths of a

second. That’s important because the times are often very close. A new world record may be set by just a split-second difference in time.

Why It Matters: The need for accuracy in timing athletic events makes significant figures important. Significant figures are the correct number of digits for reporting a measurement or calculation. Just the thought of significant figures may make you cringe, but using them really isn’t difficult. You just need to apply a few simple rules.

We must rely on high-speed cameras to capture race times to the hundredth of a second [Figure2]

How accurately must swimming times be measured, and how many significant figures are required? To answer this question, watch the video below. It shows Michael Phelps setting a new world record in an exciting 100-meter race. Notice how little time separates his time in this race from the previous world record. (answer these questions below)

https://tinyurl.com/y9j784sx1. In the swimming competition in the video , what was Michael Phelps’ time? What was the previous world record? How much time did he shave off the previous world record?

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Topic 0.5

2. In this swimming competition, swimmer’s times were measured digitally. How many significant figures are there in Michael Phelps’ winning time? Why?

How do we count Significant Figures?

0.003560006200

0.3403 30,000

3.2000001 0.0003

If the number is written in scientific notation 2.30 x102 has ____ significant figures, but if it was in standard notation would have Sig figs because now the point is _____ !

Practice by rounding the following measurements to 3 significant figures:a) 6755 mL = __________

b) 4,507 g = __________

c) 10,595 km = __________

d) 0.06782 g = __________

e) 1.0549 m = __________

f) 0.10649 kJ = __________

g) 45,949 mm = __________

When multiplying and dividing : Determine the number of significant figures in the numbers and report your answer to the of the two.

42.506 x 320 = (in calculator) with correct significant figures

5.00 ÷1.223= (in calculator) with correct significant figures

When adding and subtracting: Determine the number of digits and report your answer to the of the two.

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4.05241 ____ DP+1.008 ___ DP

1025.4 ____ DP-4.4208 ___ DP

When the POINT is , start at the

.0.3400 has _________ sig figs

When the POINT is , start at the .

3400 has _________sig figs

Determine the number of significant figures in each of the numbers below.

1. ______105.02. ______ 0.005400

3. ______ 5600

4. ______0.025. ______0.000009

6. ______1020

Still not sure how they work? Before moving on learn more about significant figures at the link below then answer the questions that follow. https://tinyurl.com/ybojqhll

7. True or false: The number of significant figures is the minimum number of figures required to report a value without loss of accuracy.

8. Which figures are significant?i. all non-zero figures

ii. any zeros between significant figuresiii. trailing zeros to the right of a decimal pointiv. all of the above

9. Which figures are not significant?i. trailing zeros to the left of a decimal point

ii. leading zeros to the right of a decimal pointiii. leading zeros to the left of a decimal pointiv. two of the above

How many significant figures are there in each of the following numbers?10. 1000_______ 11. 1000.0_______ 12. 10.005_______

13. Why is it important to use significant figures when recording a measurement, such as an athlete’s time in a race? (think back to the video we started with)

Complete the following operation and express your answer to the correct number of significant digits.14. ____________4285.75 - 520.1 - 386.255

15. ____________(9.825)/(8.20)

16. ____________(0.0167) x (8.525)

17. ____________0.00526 - 0.52

18. ____________ (8.215) x(9.00)

19. When using an analog (non-digital) measuring device, how many figures are significant? (What is a general rule? See #5 on the top of page 11)

20. When using a digital measuring device, do you estimate or record the exact value? (ask your teacher if you’re unsure)

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Assignment 0.4

Putting it all together

Directions: Do the following questions. Give all answers in scientific notation with correct sig figs.

1. If a gas has a density of 4.36 grams / liter, what is the density in a. mg/mL?

b. kg/µL?

c. lbs/cubic inch?

4. How many kg in 32 nanograms?

5. How many µg (micrograms) in 256.3 kg?

6. How many square feet in 43 square inches?

7. How many square mm in 0.12 square inches?

8. The density of air under normal conditions is 1.19 g/Liter. 15

What is the mass of the air in a room that measures 8 x 12 x 20 feet?

DENSITYHow can we mathematically represent “closeness” of particles?

One of the key differences between solids, liquids, and gases is just how far apart the individual particles are. We describe that closeness using density, which is a physical property.

REFERENCE TABLES Table T

At STP, King Joffrey has a crown that weighs 1060 g. When tested, it displaced 430 mL of water. According to Reference Table S, is this crown made of gold? Explain in terms of density.

Density can be thought of as a conversion factor (recall dimensional analysis from the intro unit). For every 1 cm3 chunk of gold, it would weigh 19.3 grams. Use dimensional analysis to solve the problem below.How many grams of copper are needed to fill a 10 cm3 container at STP?

REFERENCE TABLES Table S

In lab, you will be calculating the density of various objects. Want to know how close you are to the actual value? You can! By finding your percent error.

REFERENCE TABLES Table T

16

TOPIC

MORE DENSITY NOTES:

Density: Regents Practice

1. Explain, in terms of density, why oil floats on water.

__________________________________________________________________________________________________

____________________________________________________________________________________________

2. At STP, which physical property of aluminum always remains the same from sample to sample?(1) Mass(2) Density(3) Length(4) Volume

3. A 10.0-gram sample of which element has the smallest volume at STP?(1) Aluminum(2) Magnesium(3) Titanium(4) Zinc

4. A 10.0-gram sample of gaseous nitrogen is at STP. Which property will increase when the sample is cooled down enough to become a liquid?

(1) Mass(2) Volume(3) Density(4) Temperature

5. The volume of a platinum chain is found to be 15.0 mL by water displacement. Calculate the mass of the chain.

____________________ g

In the solid phase, arsenic occurs in two forms. One form, yellow arsenic, has a density of 1.97 g/cm3. The other form, gray arsenic, has a density of 5.78 g/cm3. Although arsenic is toxic, it is needed by the human body in very small amounts.6. Explain, in terms of the arrangement of atoms, why one form of arsenic has a lower density.

__________________________________________________________________________________________________

____________________________________________________________________________________________

Some properties of three elements, represented by D, E, and Q, are listed in the table below.

7. Identify the physical property in the table that could be used to differentiate the samples of the three elements from each other.

17

ASSIGN.0.5

Note: these are only 3 out of the 6 topics your quiz is on—we’ll review more in class before quiz.Review for Unit 0 quiz Measurements and Matter1. Look at the ruler below:

1 2 3 4 cm5

What is the correct measurement for the length of the black line? __________

2. Look at the ruler below:

1 2 3 4 cm5

What is the correct measurement for the length of the black line? __________

3. Use a plastic ruler (if you don’t grab one before class starts). The length of this line is:

4. What is the correct measurement for the volume of water?_________________

Change the following to Scientific Notation: Change the following to standard notation

5. 5.28 = _______________ 10. 2.56 x103 = _______________

6. 2,000 = _______________ 11. 9.0 x10-3 = _______________

7. 15 = _______________ 12. 8.9 x106 = _______________

8. .006589 = _______________ 13. 9.2 x10-2 = _______________

9. .00009 = _______________ 14. 6.3 x104 = _______________

15. What are the following conversion factors?1 m = _____ cm 1 m = _______ mm 1 km = _________ m

You may use either dimensional analysis or your “King Henry” mnemonic device (show your work in both cases.)16. Convert 2570 cm into km:

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ASSIGN. 0.6

17. Convert 0.000335 km into cm:

18. Convert 2.58 x 105 mm into kmMODELING IN CHEMISTRYHow can we learn about stuff we can’t see?

Since chemistry is basically the study of things we can’t see, it involves the use of modeling: ways of showing or describing what happens at the molecular level. We will be using models of visible and invisible systems nearly every day, and they’ll come in two main forms:

Modeling using diagrams Modeling using formulas and equations

POGIL Time!!!

Shown below are four models (diagrams) of four different things on a microscopic level. With a partner, compare and contrast the models. Work together to circle the numbers of the models you would consider to be “pure.”

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TOPIC

0.7

ELEMENTS, COMPOUNDS, AND MIXTURES

How is matter classified and described?

MATTER is ______________________________________________________________________________.

COMPOUND MIXTURE

Example

Proportions (Amount)

Properties

Particle Diagram

Particle Diagrams

element compound

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TOPIC 0.8/ HW

Mixture of two elements

Mixture of an element & compound

Mixture of two compounds

HOMOGENEOUS VS. HETEROGENEOUS MATTER & Classification

How does the arrangement of particles in a mixture affect what we see?

Let’s recall what a mixture is-____________________________________________________ _ _

__________________________________________________________________ _

air – ____________________________________________________

sand – __________________________________________________

There are two types of mixtures:

1) heterogenous –_______________________________________________ex. chicken soup, __________________, and _________________

2) homogenous –_______________________________________________ex: milk- cream, fat and water vinegar – acetic acid and water

___________________, and _________________

** A SOLUTION is also a homogenous mixture. Most solutions are liquids. Air and stainless steel are also solutions.

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TOPIC

0.9

22

Matter

Can it be separated

__________________?

(Pure)

NO! YES!

Can it be separated

__________________?

Are particles distributed

__________________?

NO! YES! NO! YES!

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ASSIGN. 0.7

24

PHYSICAL & CHEMICAL PROPERTIESWhat are physical and chemical properties and how do they help to identify a substance?

How can we identify a substance?

by its

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TOPIC

0.10

We want to make sense of four terms: chemical properties, physical properties, chemical changes, and physical changes. Sometimes, it is easier to look at examples of these terms before we construct definitions.

Instructions: Work with your team and organize the terms into four groups:Physical Changes Chemical Changes Physical Properties Chemical Properties

Physical Chemical

Changes

Properties

STOP and have your teacher check your responses. Copy the statements into the boxes above. Be able to justify your answers.

Definitions: Create definitions based on your examples above. Note that you should NOT have the same definition for the changes and properties column. If you are stuck, obtain a text book and use the glossary.

Physical Chemical

Changes

26

Properties

PHYSICAL & CHEMICAL CHANGESHow can we distinguish between a physical and chemical change?

Phase ChangesPhase changes are physical changes. When you fill an ice cube tray with water and put it in the freezer, the liquid water changes into a solid –but it is still just water (H2O). Since no new substance was created, it is considered a physical change. You will need to know the names of the different phase changes.SOLID LIQUID GAS

CHANGES

What you might see for a __________________________ change:

________________________________

________________________________

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TOPIC

0.11

Is a

___________________

produced?NO! YES!

________________________________

________________________________

**A precipitate is a solid that forms and settles out of a liquid. The clues DO NOT indicate that a chemical reaction ABSOLUTLY took place.

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ASSIGN. 0.8

ASSIGN. 0.8 (cont)

9. A student used a balance and determined the mass to be 10.23 and was given the density of the object to be 6.82 g/ mL.

a) Calculate the VOLUME of the element and show your work.

b) If the accepted value for volume is 1.72 mL, calculate the percent error.

c) If the student were to measure the volume of the object using water displacement and then find the mass, what error is introduced by doing this?

10. In the boxes below, draw particle diagrams to represent an element, a compound, and a mixture using the key provided.

Element X The Compound X2Y A mixture of Element X and Y

11. Argon is an example of a(n) (element, compound, mixture)

12. Salts, such as sodium chloride, are examples of (elements, compounds, mixtures)

13. Solutions are examples of (elements, compounds, mixtures)

14. Air is an example of a(n) element, compound, solution)

15. Which of the following are examples of pure substances? bromine air NaCl(aq) water

Ca(OH)2 carbonic acid NaCl(s) neon

PHYSICAL SEPARATIONSHow can we use physical properties to isolate useful substances?

29

TOPIC

0.12

Key:

Element X:

Element Y:

Technique Physical Property Used to Separate

Examples

Distillation also sometimes described as _______________________

Filtration

Chromatography

What happens to the matter? It has _________________________, not disappeared.

CONSERVATION OF MASS

30

Mass of products MUST _________________ the mass of reactants. Mass is neither created nor destroyed. What you start with you must end up with.

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