1. Properties of Matter

2. Essential Questions How does the state of matter define its properties
Essential Questions How does the state of matter define its properties? What are the real-life examples of molecules, atoms & ions? How are atoms, molecules & ions alike and how are they different? How can matter be classified? What are the essential components of solutions? Why is water the universal solvent? In what ways can matter be quantified? What units should be used to quantify matter? What are the chemical & physical properties of pure substances? How can chemical and physical changes be determined in a laboratory setting?

3. The Breakdown of Matter
Anything with MASS & VOLUME
(solid, liquid, gas)
Pure Substances
Mixtures
EQ: How can matter be classified?

4. MIXTURES Mixtures = two or more substances PHYSICALLY combined.
Can be PHYSICALLY separated

5. Heterogeneous Mixtures
Hetero = different
Geneous = origin or beginning
has separations and/or boundaries
can see to different parts
Are ALL mixtures

6. Heterogeneous Mixtures
Physically combined substances

7. Homogeneous Mixtures Homeo = same Geneous = origin or beginning
matter of the SAME make-up
(no boundaries)

8. Others  alloys, colloids, etc.
Homogeneous Mixtures
Homogeneous
Mixtures
Solutions
Others  alloys, colloids, etc.

9. Homogeneous Mixtures
Homogeneous
Mixtures
Solutions
Solute
Solvent

10. Solutions EQ: What are the essential components of solutions?
Homogeneous mixtures
Physically NOT chemical combined
Solute = the substance BEING dissolved
Solvent = the substance DOING the dissolving

11. EQ: Why is water the universal solvent?
Examples of Solutions
Alloys = solid mixture or solution (brass, 14K gold, steel)
Air = gas mixture or solution
Liquid solutions = sweet tea, coffee, milk, tap water
EQ: Why is water the universal solvent?

12. Solution Properties
Soluble = the solute is able to dissolve in the solvent
Insoluble = the solute is NOT able to dissolve in the solvent

13. Descriptions of a Solution
Diluted Solutions = small amount of solute and/or a large amount of solvent
Concentrated Solutions = large amount of solute and/or a small amount of solvent
Saturated Solution = a solution that will NOT dissolve any more solute

14. An increase in temperature will allow more solute to dissolve in a solvent. The molecules of the solvent move faster and further apart allowing more room for more solute molecules.

15. 3 2 1 Name three properties of solutions:
1. __________________________________
2. __________________________________
3. __________________________________ 3
Name two types of mixtures & two types of pure substances.
1. ____________________________________
2. ____________________________________ 2 1
What is the one key in distinguishing between homogeneous and heterogeneous mixtures
1. _____________________________________

16. Pure Substances
Pure Substances
Elements
Compounds

17. EQ: How are atoms, molecules & ions alike and how are they different?
Pure Substances
chemically pure substances
only one part or one kind of matter
Elements = found on the periodic table
Compounds = 2 or more elements that have combined CHEMICALLY
EQ: How are atoms, molecules & ions alike and how are they different?

18. Elements EQ: What are the real-life examples of molecules, atoms & ions?
90 natural occurring elements
found on the periodic table
Atoms = smallest part of an element
represented by symbols

19. Compounds 2 or more elements that have combined CHEMICALLY
Molecules = smallest part of a compound
represented by formulas

20. Elements & Compounds Pure Substances Elements Atoms Symbols Compounds
Molecules
Formulas

21. States of Matter Also called Phases of Matter Solids Liquids
Vapors (gases)

22. Solids Have a definite shape Have a definite volume
Particles VIBRATE in place

23. Liquids Have NO definite shape Have definite volume
particles SLIDE freely

24. Gases (vapor) Have NO definite shape Have NO definite volume
particles fill the volume of the container

25. EQ: How does the state of matter define its properties?
Solids, Liquids & Gases
Solids = can form crystals = solid where the particle are arranged into repeating patterns.
Liquids = physical property of Viscosity = “thickness” – the resistance to flow.
Gases = volume of gases depend greatly on pressure and temperature.
EQ: How does the state of matter define its properties?

26. Phase Changes Melting Freezing Vaporization Condensation Sublimation
physical changes

27. Melting the process of changing from a solid to a liquid
energy is being put into the substance
melting point = the temperature at which melting occurs – physical property
the melting point of water is 0ºC

28. Freezing the process of changing from a liquid to a solid
energy is being pulled out of the substance
freezing point = same temperature as the melting point
(used mainly in weather)

29. Vaporization the process of changing from a liquid to a gas
energy is being put into the substance
evaporation
boiling

30. Evaporation
vaporization that occurs at the surface of the liquid

31. Boiling vaporization that occurs throughout the liquid
boiling point = the temperature at which boiling occurs
the boiling point of water is 100ºC

32. Condensation the process of changing from a gas to a liquid
energy is being pulled out of the substance

33. Sublimation the process of changing from a solid to a gas
energy is being put into the substance
ex: dry ice (CO2)

34. 3 2 1 Name three phases of matter:
1. __________________________________
2. __________________________________
3. __________________________________ 3
Name two types of vaporization.
1. ____________________________________
2. ____________________________________ 2 1
What is the so different about sublimation?
1. _____________________________________

35. EQ: What are the chemical & physical properties of pure substances?
Properties of Matter
characteristics that can identify and describe matter.
Physical Properties
Chemical Properties
EQ: What are the chemical & physical properties of pure substances?

36. Physical Properties observable properties
physical change = changes that occur while the substance remains the same.
ex: phase change

37. Examples of Physical Properties
density (d=m/v)
color
melting point & boiling point
hardness
phase of matter
malleable
ductile
taste
conductivity
luster
texture
solubility

38. Chemical Properties
properties that describes how the substance interacts with other substances or will act chemically
chemical change = an actual chemical reaction takes place and a NEW substance is formed
ex: combustion

39. Examples of Chemical Properties
flammability
reactivity
combustion
oxidation
reacts with _____
endothermic
exothermic
forms a precipitate

40. Chemical Change EQ: How can chemical and physical changes be determined in a laboratory setting?
Color change
Temperature change = reaction is either endothermic or exothermic
Gas given off
Precipitate formed = solid formed in the reaction of two liquids

41. Energy (temperature) Changes in Reactions
Endothermic reactions
Energy is put into the reaction
Reaction stops as soon as energy is no longer put into the reaction
Ex: cooking
Exothermic reactions
Energy is given off in the reactions
Ex: burning

42. Exothermic Reactions
May require energy to be put into to the reaction in order to start or activate the reaction
Activation Energy = energy required to start an exothermic reaction

43. Reducing Activation Energy
Catalysts are often used to reduce the activation energy required to start an exothermic reaction

44. Chemical change vs. Physical change
ask the question, “Has a new substance been formed?”
“yes” = chemical change
“no” = physical change

45. Examples of Problems ex: 2H2 + O2  2H2O
hydrogen gas combines with oxygen gas to form water
a new substance is formed
a chemical reaction occurs
EQ: How can chemical and physical changes be determined in a laboratory setting?

46. Examples of Problems : N2 + O2 + CO2 = air
nitrogen gas combines with oxygen gas and carbon dioxide gas and a few other gases mix
NO chemical reaction takes place
physical change has taken place in the gases

47. Examples of Problems Ice melting Phases change Solid  Liquid
No new substance is formed…it is still water
Physical change

48. Malleable
A physical property that describes being able to be flatten or pounded onto sheets
This property is associated with metals.

49. Ductile
A physical property that describes being able to be drawn into a wire.
This property is associated with metals.

50. Luster
A physical property that describes how a substance reflects light
This property is often associated with minerals, gem stones, metals and nonmetals.

51. Oxidation
A chemical property describing a substance reaction with oxygen
slow oxidation = rusting, tarnish, corrosion
fast oxidation = burning, exploding, combustion

52. Density The amount of matter in a given amount of space
Density = mass ÷ volume
D = m/v D = ?
Mass = m = 96.5 grams
Volume = v = 5 cm3
D = 96.5 g / 5 cm3 = 19.3 g/cm3
19.3 g/cm3 is the density of gold
The density of water = 1.0 g/mL
Density

53. BUOYANCE
The ability of a fluid (liquid or gas) to exert an upward force on an object immersed in it.
If buoyant force = object’s weight
the object will float

54. GAS LAWS Boyle’s Law: pressure and volume
Volume decreases as Pressure increases
Pressure decreases as Volume increases

55. Gas Laws Charles’s Law: temperature & volume
Volume increases as Temperature increases
Volume decreases as Temperature decreases