1. Matter

2. a substance changes some physical property…
During a
“__________ change”
a substance changes some physical property…
PHOTO of iceberg
H2O

3. …but it is still the same material with the same ____________ composition.
gas
H2O
solid
liquid

4. ______________ Property:
The tendency of a substance to change into another substance.
Photo:
Steel rusting:
caused by iron (Fe)
reacting with oxygen (O2)
to produce rust (Fe2O3)
4 Fe O Fe2O3

5. _____________ Change:
Any change involving a rearrangement of ________.

6. Chemical ____________:
The process of a chemical change...

7. During a
“chemical reaction”
new materials are formed by a change in the way atoms are ____________ together.

8. Physical and Chemical Properties
Examples of Physical Properties
Boiling point Color Slipperiness Electrical conductivity
Melting point Taste Odor Dissolves in water
Shininess (luster) Softness Ductility Viscosity (resistance to flow)
Volatility Hardness Malleability Density (mass / volume ratio)
Examples of Chemical Properties
Burns in air Reacts with certain acids Decomposes when heated
Explodes Reacts with certain metals Reacts with certain nonmetals
Tarnishes Reacts with water Is toxic
Chemical properties can ONLY be observed during a chemical reaction!
Ralph A. Burns, Fundamentals of Chemistry 1999, page 23

9. Physical & Chemical Changes
CO2
crushing
heating
Pyrex
_______________
_____________
CaO
Limestone,
CaCO3
Crushed limestone,
CaCO3
The crushing of limestone is a physical change; it does not alter the chemical composition of the limestone. The heating of limestone is a chemical change; the limestone decomposes into two other substances, lime and carbon dioxide.
Lime and
carbon dioxide,
CaO + CO2

10. Light hastens the decomposition of hydrogen peroxide, H2O2.
Sunlight
energy O2
Pyrex
Pyrex
H2O2
H2O
Light hastens the decomposition of hydrogen peroxide, H2O2.
The dark bottle in which hydrogen peroxide is usually stored
keeps out the light, thus protecting the H2O2 from decomposition.

11. Solid, Liquid, Gas
(a) Particles in _____ (b) Particles in _______ (c) Particles in ______

12. _________
H2O(s) Ice
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 31

13. Ice H2O(s) Ice Photograph of ice model Photograph of snowflakes
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.

14. _________ In a ________ H2O(l) Water molecules are in
constant ________
molecules are close
together
Liquids are almost
incompressible
Liquids do not fill the
container
some writing from Kotz (PowerPoint online)
H2O(l) Water
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 31

15. _________
H2O(g) Steam
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 31

16. ____ ________ ______
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 441

17. States of Matter _____ ________ ________ Holds Shape Fixed Volume
Solid
In a solid the molecules are closely bound to one another by molecular forces. A solid holds its shape and the volume of a solid is fixed by the shape of the solid.
Liquid
In a liquid the molecular forces are weaker than in a solid. A liquid will take the shape of its container with a free surface in a gravitational field. In microgravity, a liquid forms a ball inside a free surface. Regardless of gravity, a liquid has a fixed volume.
Gas
In a gas the molecular forces are very weak. A gas fills its container, taking both the shape and the volume of the container
_____
________
________
heat
heat
Holds Shape
Fixed Volume
Shape of Container
Free Surface
Fixed Volume
Shape of Container
Volume of Container

18. MATTER yes no _________ _________ yes no yes no _________ Mixture
Can it be physically separated?
_________
_________
yes
Is the composition uniform? no
yes
Can it be chemically decomposed? no
_________ Mixture
(solution)
_____________ Mixture
_________
__________
Colloids
Suspensions
Courtesy Christy Johannesson

19. Matter Flowchart Examples: graphite pepper element sugar (sucrose)
paint
soda
element
hetero. mixture
compound
hetero. mixture
Graphite image: geology.about.com/.../bl/images/blgraphite.htm
solution
homo. mixture
Courtesy Christy Johannesson

20. Pure Substances ______________ composed of identical __________
EX: copper wire, aluminum foil
Courtesy Christy Johannesson

21. Pure Substances ______________
composed of 2 or more __________ in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)
Courtesy Christy Johannesson

22. ______________ Variable combination of two or more pure substances.
________________
________________
Courtesy Christy Johannesson

23. Methods of ____________ Mixtures
Magnet
Filter
Decant
Evaporation
Centrifuge
Chromatography
Distillation

24. _________ separates a liquid from a solid
Mixture of
solid and
liquid
Stirring
rod
Filtrate (liquid
component
of the mixture)
Filter paper
traps solid
Funnel
_________ separates a liquid from a solid
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 40

25. ___________________ Tie-dye t-shirt Black pen ink DNA testing
Tomb of Unknown Soldiers
Crime scene
Paternity testing

26. Paper Chromatography

27. A _____________ Apparatus
liquid with a solid
dissolved in it
thermometer
condenser
tube
distilling
flask
pure
liquid
receiving
hose connected to
cold water faucet
“A Distillation Apparatus”
Description: This transparency shows an apparatus used for laboratory distillations.
Basic Concepts
The separation of substances by distillation occurs because the boiling point of the substances differ. The substance with the lowest boiling point boils away first.
Distillation is based on the principle that a substance will change from a liquid to a vapor during heating and from a vapor back to a liquid while cooling.
Teaching Strategies
Use this slide to explain to students how a distillation apparatus is used to purify liquids and to separate the components of liquid mixtures. Begin by reviewing the phases of matter, stressing the processes of evaporation and condensation. Remind students that different liquids have different boiling points. Point out that substances that are solids at room temperature usually have higher boiling points than do substances that are liquids at room temperature.
Questions
If the distilling flask shown in the diagram were open to the air (rather than being connected to the condensor), what would happen to each component of the mixture in the flask as boiling continued?
Explain your answer to question 1 in terms of the boiling points of the liquid and the dissolved solid.
In the distillation apparatus, the vaporized liquid must enter the condenser. The condenser consists of a long tube within another tube (the jacket). The substance in the central tube and the jacket cannot mix. Cold water enters at the bottom of the jacket and exits at the top.
What is the function of the condenser jacket?
How would changing the length of the condenser jacket affect how well it performs this function?
Explain why the liquid entering the receiving flask is pure.
To separate a mixture of methanol and water, you set up a distillation apparatus and heat the mixture to the boiling point of methanol, 65 oC.
What substance would you expect to collect at the receiving flask?
When you finish the experiment, you discover that the substance in the receiving flask is not pure. It still contains both water and methanol. Can you explain why? (Hint: Think about vapor pressures.)
Before automobiles were invented, crude petroleum was used mainly as a source of kerosene. The petroleum was heated in a device called a still. Gasoline, then considered to be useless, evaporated first into the air. Kerosene boiled off next and was condensed and collected. A tar-like residue remained in the still. From this information, what can you deduce about the boiling points of gasoline, kerosene, and the residue?
How will you know when all of one component has been separated?
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 282

28. Separation of a sand-saltwater mixture.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 40