1. MATTER
Does it Really MATTER?
YES

2. The Four States of Matter
Solid
Liquid
Gas
Plasma
Based upon particle arrangement
Based upon energy of particles
Based upon distance between particles

3. States of Matter

4. States of Matter
A. The Kinetic Theory
1. All matter is composed of small particles (atoms, molecules, or ions).
2. They are in constant, random motion.
3. They constantly collide with each other and with the walls of their container.

5. STATES OF MATTER SOLIDS
Particles of solids are tightly packed, vibrating about a fixed position.
Solids have a definite shape and a definite volume.

6. STATES OF MATTER LIQUID
Particles of liquids are tightly packed, but are far enough apart to slide over one another.
Liquids have an indefinite shape and a definite volume.

7. STATES OF MATTER GAS
Particles of gases are very far apart and move freely.
Gases have an indefinite shape and an indefinite volume.

8. B. Phase Properties Particle Properties Phase Proximity Energy Motion
Volume
Shape
Solid
close
little
vibrational
definite
definite
Liquid
close
moderate
rotational
definite
indefinite
Gas
far apart
a lot
translational
indefinite
indefinite

9. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Solid to liquid
Melting
Heat goes into the solid as it melts.
Liquid to solid
Freezing
Heat leaves the liquid as it freezes.

10. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Liquid to gas
Vaporization, which includes boiling and evaporation
Heat goes into the liquid as it vaporizes.
Gas to liquid
Condensation
Heat leaves the gas as it condenses.
Solid to gas
Sublimation
Heat goes into the solid as it sublimates.

11. "Bunsen! my flame! I melt whenever I see you" said the ice.
Chemistry Joke
A small piece of ice which lived in
a test tube fell in love with a
Bunsen burner.
"Bunsen! my flame! I melt whenever I see you" said the ice.
The Bunsen burner replied :
"It's just a phase you're going through".

12. Thermal E x p a n s i o n
1. Particles in any state expand when heated (generally).
2. Examples of solids:
a. Expansion joints
b. Power lines
c. Thermostats
3. Different materials expand at different rates.

13. 4. Mercury and alcohol are liquids that expand in thermometers
5. Air expands when heated (becoming less dense)
6. Water reaches maximum density at about 4 C.
Ice particles are farther apart than liquid water (so it floats).

14. Will everything just be a gas?
But what happens if you raise the temperature to super-high levels… between 1000°C and 1,000,000,000°C ?
Will everything just be a gas?

15. a. Hot, ionized gas particles.
Plasma
a. Hot, ionized gas particles.
b. Electrically charged.
c. Most common state in universe.

16. Some places where plasmas are found…
1. Flames

17. 2. Lightning

18. 3. Aurora (Northern Lights)

19. The Sun is an example of a star in its plasma state

20. Plasma

21. STATES OF MATTER LIQUID PLASMA SOLID GAS
Tightly packed, in a regular pattern
Vibrate, but do not move from place to place
Close together with no regular arrangement.
Vibrate, move about, and slide past each other
Well separated with no regular arrangement.
Vibrate and move freely at high speeds
Has no definite volume or shape and is composed of electrical charged particles

22. Physical Properties What are some physical properties? color
melting and boiling point
odor

23. Physical Changes Some physical changes would be boiling of a liquid
can be observed without changing the identity of the substance
Some physical changes
would be
boiling of a liquid
melting of a solid
dissolving a solid in a liquid

25. Chemical Properties and Chemical Change
Burning hydrogen (H2) in oxygen (O2) gives H2O.
Chemical change or chemical reaction — transformation of one or more atoms or molecules into one or more different molecules.

26. Sure Signs of a Chemical Change
Heat
Light
Gas Produced (not from boiling!)
Precipitate – a solid formed by mixing two liquids together

27. Physical vs. Chemical physical chemical melting point flammable
Examples:
melting point
flammable
density
magnetic
tarnishes in air

28. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

29. What Are Substances ??
Substances can be identified as either an element, compound, or a mixture.

30. A substance is matter of a particular kind.
A substance cannot be further broken down or purified by physical means.
A substance is matter of a particular kind.
Each substance has its own characteristic properties that are different from the set of properties of any other substance.
Definition of a substance.

31. Pure substances Elements
Compounds
Can be decomposed into simpler substances by chemical changes, always in a definite ratio
A compound is a substance that contains two or more elements chemically combined in a fixed proportion
Elements
The simplest form of matter that has a unique set of properties.
Cannot be decomposed into simpler substances by chemical changes
The two categories of pure chemical substances.

32. Elements, Molecules and Compounds
Some elements, such as the noble gases, exist as individual atoms.
Often, elements consist of two or more atoms joined together. We call these molecules.
If more than one type of atom is in a molecule, we call it a compound.

33. Definitions A solution is a homogeneous mixture
A solute is dissolved in a solvent.
A saturated solution is one where the concentration is at a maximum - no more solute is able to dissolve.
A saturated solution represents an equilibrium: the rate of dissolving is equal to the rate of crystallization. The salt continues to dissolve, but crystallizes at the same rate so that there “appears” to be nothing happening.

34. solute - is the substance being dissolved
Solvent - is the liquid in which the solute is dissolved
an aqueous solution has water as solvent

35. Variable combination of 2 or more pure substances.
Types of Mixtures
Variable combination of 2 or more pure substances.
Heterogeneous – visibly separate phases
Homogeneous – Same throughout

36. Mixtures Atom, molecule or compound? atom molecule compound
This is a mixture of elements made up of atoms, elements made up of molecules, and compounds.
In a mixture, the particles are not joined together.
Atom, molecule or compound?
atom
molecule
compound

37. HOMOGENEOUS MIXTURES
Homogenous mixtures look the same throughout but can be separated by physical means (dissolution, centrifuge, gravimetric filtering, etc.).
Examples: milk, yogurt

38. INDICATORS OF A HOMOGENEOUS MIXTURE
Have the same composition throughout
Components are indistinguishable
May or may not scatter light
Examples: milk, yogurt, etc.
Brainstorm more examples of homogenous mixtures.

39. HETEROGENEOUS MIXTURES
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie. density, polarity, metallic properties).

40. INDICATORS OF A HETEROGENEOUS MIXTURE
Do not have same composition throughout
Components are distinguishable
Examples: fruit salad, vegetable soup, etc.
Brainstorm more examples of heterogenous mixtures.

41. WHAT ARE COLLOIDS?
Colloids are solutions. They can be described as a substance trapped inside another substance. They can be identified by their characteristic scattering of light.
For example: air trapped inside the fat molecules in whipped cream.
Brainstorm more ideas of colloids: fog, egg merangue, jello, smoke, etc.

42. TYNDALL EFFECT

43. Intensive and Extensive Properties
Physical and chemical properties may be intensive or extensive.

44. What are intensive properties?
Intensive properties such as density, color, and boiling point do not depend on the size of the sample of matter and can be used to identify substances.

46. What are extensive properties?
Extensive properties such as mass and volume do depend on the quantity of the sample.