General Chemistry
Unit 9
Matter

Atom, Element, Compound

Solid, Liquid, Gas, Plasma

Intrinsic property vs Extrinsic property

Pure substance vs Mixture

Homogeneous mixture (true solution or colloid) vs Heterogeneous mixture (suspension)

Physical change vs Chemical change
1
We are learning to:
1.
Compare and contrast the characteristics of different types of matter.
2.
Differentiate between a physical change and a chemical change.
We are looking for:
1a. Describe the various types of properties of matter.
1b. Recognize that particles of matter are in constant motion that determines their state (solid, liquid, gas).
1c. Separate a mixture of matter based on its physical and chemical properties
1d. Characterize various types of matter (suspension, colloid, true solution)
2a. Physical changes do not change the chemical makeup of the material while chemical changes do.
2
What’s the MATTER, part I
Matter:
 Anything that has _______ and takes up __________.
States of Matter
 Solid Definite __________ and ___________
 Particles are __________ packed
 Slight expansion when ___________
 Incompressible
 Liquid Has definite __________, but no definite __________ (assumes the shape of the
container)
 Particles are ____________ packed (can flow)
 Easily expands when ___________
 Considered incompressible
 Gas No definite ___________or ___________
 ___________ to fill the container
 Particles are spaced _______ apart
 Compressible
3
FYI:
Composition of Air
Name
Nitrogen
Oxygen
Argon
Carbon Dioxide
Neon
Methane
Helium
Krypton
Hydrogen
Xenon
Symbol
N2
O2
Ar
CO2
Ne
CH4
He
Kr
H2
Xe
% by volume
78.084
20.9476
0.934
0.0314
0.001818
0.0002
0.000524
0.000114
0.00005
0.0000087
 Plasma Consists of _______________ charged particles
 It’s an ionized _________
 Common in __________, but very rare on ____________
 Found in lightning, fluorescent lights and neon signs
A lit candle shows all 4 states of matter…so they say
(right above wick) = __________
4
Energy Amounts in States of Matter
 ________- little energy, particles vibrate and rotate
 ________- more energy, they move freely
 ________- even more energy, move quickly
 ________- most energy, move extremely fast
Phases of Matter
Names of Phase Changes
 Solid to Liquid
= ______________
 Liquid to Gas
= ______________
 Gas to Liquid
= ______________
 Liquid to Solid
= ______________
 Solid to Gas
= ______________
 Gas to Solid
= ______________
5
Properties of Matter
 2 Types: Extrinsic and Intrinsic
 _______________ – depend on the amount of the sample
 Examples =
volume
mass
length
weight
 _____________ – does not depend on the amount of the sample ( I AM NOT)
 Examples =
density
melting point
boiling point
malleability
ductility
color
odor
What’s the MATTER, part II
Types of Matter
 Pure Substance Matter with a ________ composition
 It has distinct properties
 Examples =
elements
compounds
 Mixtures Most matter is a mixture
 The composition is not fixed (changes from sample to sample)
 Two Types –
____________________
____________________
6
Homogeneous Mixtures:
 Composition is ______________ throughout
 True Solution Particle size = 0.01 – 1 nm
 Doesn’t settle out upon ________________
 Can’t be separated by __________________
 Doesn’t scatter _____________
 Example = distilled water
 Colloid Particle size = 1 – 1000 nm
 Doesn’t settle out upon standing
 Can’t be separated by filtering
 Scatters light ( ____________________ )
 Examples = milk, gelatin, smoke
Heterogeneous Mixtures
 The sample varies in composition, properties and _______________
 No _______________
 Particle size is greater than 1000 nm
 Particles ____________________ upon standing
 Can be separated by filtration
 Might scatter light
 Examples = soil, trail mix, _________________
7
True Solution
Colloids
Suspensions
8
Observing Solutions, Suspensions and Colloids
Make at least three "good" observations about the material in each container. Do
not include the container in your observations!
Container “A”
Container “B”
1.
1.
2.
2.
3.
3.
4.
4.
mixture type:
mixture type:
Container “C”
Container “D”
1.
1.
2.
2.
3.
3.
4.
4.
mixture type:
Container “E”
mixture type:
Container “F”
Container “G”
1.
1.
1.
2.
2.
2.
3.
3.
3.
4.
4.
4.
Mixture type:
mixture type:
mixture type:
9
Classification of colloids
Because the size of the dispersed phase may be difficult to measure, and because colloids have
the appearance of solutions, colloids are sometimes identified and characterized by their
properties. For example, if a colloid consists of a solid phase dispersed in a liquid, the solid
particles will not diffuse through a membrane, whereas with a solution the dissolved ions or
molecules will diffuse through a membrane.
Colloids can be classified as follows:
Dispersed Phase
Gas
Continuous
Medium
Gas
Liquid
Solid
NONE
(All gases are mutually
miscible)
Liquid Aerosol
Examples: fog, mist, clouds
Solid Aerosol
Examples: smoke, air
particulates
Emulsion
Examples: milk,
mayonnaise, hand cream
Sol
Examples:, pigmented
ink
Gel
Examples: gelatin, jelly,
cheese, opal
Solid Sol
Example: cranberry
glass
Foam
Liquid
Example: whipped cream
Solid
Solid Foam
Examples: aerogel,
styrofoam, pumice
In some cases, a colloid can be considered as a homogeneous, (not heterogeneous [meaning not
the same]) mixture. This is because the distinction between "dissolved" and "particulate" matter
can be sometimes a matter of approach.
10
Physical vs. Chemical Properties
 Every substance has a unique set of properties (characteristics that identify
that substance)
 Physical Properties Properties that can be measured without changing the identity and
composition of the substance
 Physical Property Examples Color
 Odor
 Density
 Melting Point
 Boiling Point
 Hardness
 Solubility
Physical Change A change in matter from one form to another without changing its
______________________________ (most can be reversed)
 Examples =
 Mixing
 Dissolving
 Compressing
 Evaporating
 Cutting
11
Chemical Properties Properties that describe the way a substance may change to form other
substances
 Only observed when a _______________________takes place
Chemical Property Examples




Heating to combustion
Reactivity with water or acid
Flammability
Corrosion
Decomposition
_______________________________ = In a physical change or a chemical
reaction, mass is neither created nor destroyed (Antoine Lavoisier)
12
Physical and Chemical Changes
Place a check in the appropriate column
Change
1
Salt dissolves in water
2
Hydrochloric acid reacts with magnesium to produce hydrogen gas
3
A piece of copper is cut in half
4
A sugar cube is ground up
5
Water is heated and changed to steam
6
Iron rusts
7
Ethyl alcohol evaporates
8
Ice melts
9
Milk sours ( goes bad)
10
Potassium reacts violently with water
11
Pancakes cook on a griddle
12
Grass grows on a lawn
13
A tire is inflated with air
14
Food in digested in the stomach
15
Water is absorbed by a paper towel
16
Ethyl alcohol boils at 79oC
17
Paper burns
18
Water freezes at 0oC
19
Fireworks explode
20
Alka-Seltzer gives off carbon dioxide when added to water
21
Clouds form in the sky
Physical
Change
Chemical
Change
13
Chemical or Physical Changes Activity
In this activity you will investigate various changes. It is your task to determine if the changes are
physical or chemical, based on the indications you have learned. Fill in the table as you complete each
test. Be detailed in your observations; be sure to identify all indicators. Clean all glassware and
equipment after each test.
What are the 5 indicators that we observe as signs of a chemical reaction?
(Chemists Get Practice Trying Labs)
1.
2.
Test
3.
Observations
4.
5.
Indicators
Type of
Change
1) Fill a test tube 5 ml of KI
solution. Add 8 drops of Pb(NO3)2
to the test tube. Observe.
□ Physical
□ Chemical
2) Add two squirts of solution B to
a test tube. Record its
temperature. Add 2 small scoops of
powder A to the test tube.
Observe and record the
temperature again.
□ Physical
□ Chemical
3) Add a small scoop of sodium
polyacrylate to an evaporating dish.
Add 4 squirts of water to the
powder. Observe. Add 4 more
squirts of water. Observe.
Add lots more squirts of water!
PLEASE DISCARD IN TRASH
CAN!
□ Physical
□ Chemical
4) Add 5 ml of 3M NaOH to a test
tube. Record the temperature. Add
2 small scoops of citric acid to the
beaker. Record the temperature
again. Observe.
□ Physical
□ Chemical
14
Test
Observations
Indicators
Type of
Change
5) Fill a test tube ½ full of milk.
Add 2 squirts of Solution B. Mix
well with scoopula. Pour into small
beaker. Observe.
□ Physical
□ Chemical
6) Add a small scoop of CaCl2
powder and a small scoop of powder
A to an evaporating dish. Using the
spatula, mix the powders together.
Add 5 drops of Universal indicator
to the powders. Observe.
□ Physical
□ Chemical
7) Add one small piece of
magnesium metal to a evaporating
dish. Add 3 drops of solution B.
Observe.
□ Physical
□ Chemical
8) Add a small scoop of powder B
to an evaporating dish. Add 10
drops of water to the powder. Mix
well. Observe.
□ Physical
□ Chemical
9) Properly light the Bunsen
burner. Observe.
(KEEP BURNER LIT FOR NEXT
TEST)
□ Physical
□ Chemical
10) Obtain a small piece of
magnesium ribbon. Using a crucible
tongs, ignite the magnesium with
the Bunsen burner. (DO NOT LOOK
DIRECTLY AT THE LIGHT AS IT
CAN CAUSE RETINAL DAMAGE).
Observe.
□ Physical
□ Chemical
15
Introduction: The purpose of this experiment is to relate the major concepts of the properties of
matter. Using the physical properties and changes of various substances you are going to separate a
mixture.
Your goal is to design an experiment that will separate a mixture of sand,
salt, iron filings, and
pieces of cork.
Here are some points to keep in mind:
You will perform this experiment with your partner.
You and your partner will design an experiment to separate the mixture.
Think before you manually pick out each item
Do not use more than 50 mL of water.
You must include a material list and a detailed procedure list.
You must include a table of your collected data.
(example; substance separated, method of separation, mass of separated substance)
The team will submit the experiment BEFORE the experiment can be done
The team will then test their separation design.
You must turn in the final products (hand in each separated product in a plastic "dish")
DO NOT mix back together BEFORE handing the product in.
Materials you can choose from but are not limited to:
Graduate cylinder
Beaker
Beaker tongs
Test tubes
Test tube holders
scoopula
forceps
funnel
filter paper
pipets
hot plate
magnets
water
goggles
plastic "dish"
You will be graded on the:
Cover page
Purpose
Background
Materials list and Procedure
Data Analysis: Data table
Conclusion
Be sure to label each section in the lab report. See page 19 for details of each section.
16
Post-Lab Questions
(include the answers to these questions in your conclusion section)
1) The chemical formulas of iron and salt are Fe and NaCl, respectively. Are these substances
elements or compounds? Explain.
2) Are any of the substances in the mixture magnetic? Is magnetism a physical or chemical
property? Explain.
3) Which substances dissolved in water? Is solubility a physical or chemical property? Explain.
4) Is the combination of salt and sand a new compound or a mixture? Explain.
5) Describe the results of the filtration process. Which substance remained on the filter paper
after filtration? Is the filtrate (the liquid that passed through) a pure substance? Explain.
17
Details for writing up the
Separation Inquiry Lab
A typed (size 12 font, double spaced) lab report is due on _____________________________.
The only pieces of information to be shared between lab partners are the procedure and the separation values
for each component. All students are responsible for writing their own lab report. A letter grade will be lost for
every section that is shared between students.
Cover page: Lab title, your name and class period… color and creativity welcome!
Purpose:
 To separate a physical mixture into its original components
Background Information:
In a physical mixture, each component retains its own characteristics and can be removed from the mixture.
The mixture you are given contains iron, cork, salt, and sand.
Procedure:
Lab partners are to create a procedure on how you will separate the mixture. You must write a detailed step –
by – step procedure. These steps should be numbered.
Data Analysis:
Create a data table to summarize the amounts of each of the 4 components, including the total amount of
sample you had. You should also include a column for percent error for each component. The original values
for each material will be given to you after you have completed the separation of the components.
Component
Amount by separation (g)
Original amount (g)
% error
Percent Error = {(original value – your value) / (original value)} x 100
Conclusion:
Based on your data and percent error calculations, discuss where and why error was introduced into your
component values. Did you have problems with any of the separations? Do you have any suggestions as to
how these errors could be eliminated if you had to do this lab again?
The lab questions from page 18 should also be answered in this section.
18
Matter is made up of building blocks:
_______
– smallest unit of an element.
_________ – a pure substance made of only one kind of atom.
_________ – made of two or more atoms that are chemically combined.
Paper Clip Compounds
I. Problem: Can one determine a difference between elements, compounds and mixtures by considering
the atomic structure with models made from paper clips and other items?
1. On your table you will need 3 wood splints (Ws), 12 paper clips (Pc) and a 2 foot strip of
masking tape (Mt). These three items represent three different types of atoms.
Before you use the wood splints, break them into quarters so each one is about
3 cm long.
2. Using the appropriate item, make the materials below and scotch tape them on a piece
of paper properly labeled with a letter and the formula as listed below. Have a onefoot strip of scotch tape at your table for you to tear off a small piece.
A. WsMt2
D. Mt2
B. Ws2Mt and Pc
E. 2Ws2Pc
C. Mt2 and 3Pc
F. 4Pc
G. 2Ws(PcMt3)2
3. You are to work individually but you can confer with your lab partner. Represent bonds
by having the items touch each other. Metallic bonds are not represented, only
ionic or covalent bonds. The weaker bonds between compounds are not represented.
4. Once you have completed the lab practical on the back of this paper, take your models
apart and return the wood splints and paper clips to their original locations.
V. Observations:
When you have completed building the models and added their labels, you will need to be checked off.
Once you have the “stamp of approval” you are to complete the back of this paper.
19
Questions:
A
B
C
D
E
F
G
1. How many total atoms are there in each of
the above materials? One answer per box.
2. How many total molecules are there in each
of the above materials? One answer per box.
3. Place an "e" for the material(s) that would
best be classified as an element.
4. Place an "c" for the material(s) that would
best be classified as a compound.
5. Place an "m" for the material(s) that would
best be classified as a mixture.
6. Place an "x" for the one element that is
monatomic.
7. Place an "x" for the one element that is
diatomic.
8. If the charge on Mt in substance A is -1,
what is the charge on Ws? Answer in column A.
9. If the charge on Ws in material G is +4,
what is the charge on PcMt3? Answer in column
G.
10. In material E, is the charge on Pc positive
or negative? Answer in column E.
11. If the charge on Ws in material B is +2,
what is the charge on Mt? Answer in column B.
12. If Ws were removed from G, what kind of
ion would the remainder be called? Answer in
column G.
13. If Ws were removed from E, what kind of
ion would the remainder be called? Answer in
column E.
14. Put an "x" in the appropriate column(s) for
material(s) that is (are) made up of 2 identical
compounds.
15. Put an "x" in the appropriate column(s) for
material(s) that is (are) made up of 4 identical
elements.
20
Matter Review Sheet
1. Define matter
2. What are the 2 major categories of matter?
A.
B.
3. Mixtures can be classified as _H____________________ or H_______________________
4. What are the two types of homogeneous mixtures?
5. What is the Tyndall effect?
6. Which type(s) of mixtures will have the Tyndall effect?
7. Which type of mixture has the largest sized particles?
8. Which type of mixture has the smallest sized particles?
9. Which type of mixture will have all of its particles settle out ?
10. Which type of mixture can the particles not be filtered out and will not have the Tyndall effect?
11. Classify the following as element (E), Compound (Cd), True Solution (TS), Colloid (Cl), or Suspension (S)
a. ___Oil and Vinegar
e. ___NaCl
b. ___Salt water
f. ___Hydrogen
c. ___Jello (has Tyndall effect)
g. ___Fog
d. ___Sandy water
h. ___ Carbon dioxide
12. Which type of property (physical or chemical) can be used to separate components of a mixture?
21
13. What is the difference between the solute and solvent? Which one will typically be the larger amount?
14. What is the difference between a physical change and a chemical change?
15. What does the law of conservation of mass say?
16. What are the 4 states of matter and how can you tell the difference between them? Which is the most common
one in the universe???
17. Define the following terms related to states of matter or changes in states of matter:
a. Condensation
b. Sublimation
c. Vaporization
d. Deposition
e. Freezing
f.
Melting
18. What is the difference between an intensive and an extensive property?
19. What are the five clues/evidences that a chemical change has occurred?
a.
b.
c.
d.
e.
22