1. What’s the MATTER,. Definition, States,. Change of State,
What’s the MATTER, Definition, States, Change of State, Types of Matter, and Properties and Changes
Unit 1B p. 2-5.

2. MATTER, Definition, States, and
MATTER, Definition, States, and Change of State At the conclusion of our time together, you should be able to:
Define matter
Define the various states of matter and draw an example of each state
Recognize that particle motion determines the state of matter

3. Matter: Anything that has mass and takes up space
Matter is made up of building blocks:
atom – smallest unit of an element.
element – a pure substance made of only one kind of atom.
compound – made of two or more atoms that are chemically combined.

4. FYI 90% of the Earth’s crust is made up of only 5 elements:
Oxygen 49.2%
Silicon %
Aluminum %
Iron %
Calcium %

5. States of Matter Solid- Definite volume and shape
Particles are tightly packed
Slight expansion when heated
Incompressible

6. Vibration around fixed points
Solid
Vibration around fixed points

7. States of Matter Liquid-
Has definite volume, but no definite shape (assumes the shape of the container)
Particles are loosely packed (can flow by sliding over each other)
Easily expand when heated
Considered incompressible

8. Vibration around sliding points
Liquid
Vibration around sliding points

9. States of Matter Gas- No definite shape or volume
Expand to fill the container
Particles are spaced far apart
Compressible

10. Gas
Vibration around moving points

11. States of Matter Plasma- Consists of electrically charged particles
It’s an ionized gas
Common in space, but very rare on Earth
Found in lightning, fluorescent lights and neon signs

12. Plasma When atoms are so hot, they lose ALL of their electrons.
“Super-heated Gas”

13. Energy Amounts in States of Matter
Solid- little energy, particles vibrate and rotate
Liquid- more energy, they move freely by sliding over each other
Gas- even more energy, move quickly
Plasma- most energy, move extremely fast

14. Solid Liquid Gas Plasma
Made of
Atoms
Holds
its shape
Atoms move
past each
other

15. States of Matter Changes of State
Energy
Gas
Energy
Liquid
Energy
Solid

16. Names of Phase Changes Solid to Liquid = Melting
Liquid to Gas = Boiling/evaporation
Gas to Liquid = Condensation
Liquid to Solid = Freezing
Solid to Gas = Sublimation
Gas to Solid = Deposition

17. Boiling Condensation Freezing Melting Gas Sublimation Liquid Solid
Deposition
Condensation
Liquid
Sublimation
Melting
Freezing
Solid

18. Gas Liquid Solid Sublimation When a solid turns directly into a gas.
Dry ice is
solid CO2
Solid

19. Moisture that collects on the outside of a cold glass results from the process of…
evaporation.
condensation.
sublimation.
vaporization.

20. Matter, Classify Matter At the conclusion of our time together, you should be able to:
Classify a mixture of matter based on their physical and chemical properties
Characterize various types of matter

21. Types of Matter Pure Substance- Matter with a fixed composition
It has distinct properties
Examples = elements
compounds

22. Types of Matter Mixtures- Most matter is a mixture
The composition is not fixed (changes from sample to sample)
Two Types –
Homogeneous
Heterogeneous

23. Homogeneous Mixtures Composition is uniform throughout Solution-
Particle size = 0.01 – 1 nm
Doesn’t settle out upon standing
Can’t be separated by filtering
Doesn’t scatter light
Example = salt water

24. Homogeneous Mixtures Colloid- Particle size = 1 – 1000 nm
Doesn’t settle out upon standing
Can’t be separated by filtering
Scatters light (Tyndall Effect)
Examples = milk, gelatin, smoke

25. Heterogeneous Mixtures - Suspension
The sample varies in composition, properties and appearance
No uniformity
If a suspension:
Particle size is greater than 1000 nm
Particles settle out upon standing
Can be separated by filtration
Might scatter light
Examples = soil, trail mix, pond water

26. Let’s Look at Some Examples:
Mixtures are variable combinations of 2 or more pure substances.
Heterogeneous – visibly separate phases
Homogeneous – Same throughout

27. Pure substance vs. Mixture
Only ONE element has 2 or more
or compound elements/
(distilled water) compounds.

28. Distilled Water is
a compound.
an element.
a solution.
a mixture.

29. Air is a mixture of several gases.
Name Formula amount
Nitrogen N %
Oxygen O %
Argon Ar %
Carbon CO %
Dioxide

30. Noble (inert) Gas Air is a mixture of several gases
Name Formula Amount
Neon Ne %
Methane CH %
Helium He %
Krypton Kr %
Hydrogen H %
Xenon Xe %
Noble (inert) Gas

31. Atoms are NOT the same as molecules.
Air and oxygen are NOT the same.
Helium and hot air are NOT the same.

32. Helium and hot air are NOT the same.

33. What’s the MATTER Classify Matter
Let’s Put it All Together in a Chart!!

34. MATTER No Yes Can it be physically separated? MIXTURE PURE SUBSTANCE
This is on p. 5
MATTER No
Yes
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? No
Yes
Can it be chemically decomposed? No
Yes
Homo- geneous Mixture
(solution)
Hetero- geneous Mixture
Compound
Element
Colloids & Suspensions

35. Putting sand and salt together makes
a compound.
an element.
a mixture.
a solution.

36. Pure Water is
a compound.
an element.
a solution.
a mixture.

37. Tap Water is
a compound.
an element.
a solution.
a mixture.

38. An atom is to an element, as a molecule is to a
metal.
nonmetal.
metalloid.
compound.

39. If different kinds of atoms are represented by different colored dots, which picture represents a sample of a compound?

40. If different kinds of atoms are represented by different colored dots, which picture below represents a mixture?

41. Which of the following illustrations represents a pure substance?

42. Salt (NaCl) is a common substance. Salt is which of these?
atom
element
compound
mixture

43. A chocolate chip cookie is an example of a __________,
A chocolate chip cookie is an example of a __________, because ______________.
a. compound, the ingredients are chemically bonded.
b. compound, it is the same throughout.
c. mixture, you can separate out the chips.
d. mixture, you cannot distinguish between the ingredients.

44. Which of the following is a compound?
oxygen
water
nitrogen
air

45. Physical Change Physical
A change in matter from one form to another without changing its chemical properties
(most can be reversed)
No change in atoms/molecules

46. Physical Change Examples = Change in state or phase change Dissolving
Compressing
Light emission/absorption
Electrons passing through metals

47. Physical Change More Examples = boiling of a liquid melting of a solid
dissolving a solid in a liquid to give a homogeneous mixture
making a solution

48. 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

49. Physical Property Examples-
Color
Odor
Density
Melting Point
Boiling Point
Hardness
Solubility

50. 2 Chemical Change 1 Chemical
A change in matter from one form to another by changing its composition (most cannot be reversed)
Bonds are made / broken
Chemical change or chemical reaction — transformation of one or more atoms or molecules into one or more different molecules.

51. Sure Signs of a Chemical Change “Chemists Get Practice Trying Labs”
Color Change
Gas Produced (not from boiling!)
Precipitate – a solid formed by mixing two liquids together
Temperature Change
Light

52. Chemical Properties
Properties that describe the way a substance may change to form other substances
Only observed when a chemical reaction takes place

53. Chemical Properties
Properties that describe the way a substance may change to form other substances
Only observed when a chemical reaction takes place

54. Chemical Property Examples
Combustible
Reactive with water or acid
Flammable
Corrosive
Decomposes in air

55. Remember the Law of Conservation of Mass
In a physical change or a chemical reaction, mass is neither created or destroyed
(Antoine Lavoisier)

56. Physical vs. Chemical Change
Examples:
melting
flame produced
paper cut
dissolving salt in water
tarnishes in air

57. Physical vs. Chemical Change
Examples:
rusting iron
mixing mud and water
burning a log
freezing water
grinding spices

58. Physical vs. Chemical Properties
Physical Properties-
Properties that can be measured without changing the identity and composition of the substance
Chemical Properties-
Properties that can be measured by changing the identity and composition of the substance

59. Physical vs. Chemical Property
Examples:
melts at 55oF
flammable
will tear easily
will dissolve in water
will tarnish

60. Physical vs. Chemical Properties
Examples:
will rust
mixture can be separated by boiling
burns
freezes at -20oC
can be crushed