1. MATTER
ANYTHING WITH MASS AND VOLUME

2. Classification of Matter
Elements
Draw this chart!, leave space to define the terms
Pure Substances
Compounds
Matter
Homogeneous
Mixtures
Heterogeneous

3. Pure Substances vs. Mixtures
A pure substance is made of only one kind of material and has definite properties.
Matter that consists of two or more substances mixed together but not chemically combined is called a mixture.

4. Pure Substances: Elements are the simplest pure substance.
Examples: hydrogen, carbon, and oxygen.
The smallest particle of an element that has the properties of that element is called an atom.

5. Pure substances:
Compounds are pure substances that are made of more than one element bound together.
Examples: water (H2O), and carbon dioxide.
A molecule is formed when two or more atoms chemically combine.
Example: water (H2O), O2

6. MIXTURES Heterogeneous vs. Homogeneous
Homogeneous matter (solutions): matter that has identical properties throughout.
Examples: salt water, gravy, whipped cream
Heterogeneous matter: matter that has parts with different properties.
Examples: granite, soil, potpourri, cookies

7. LIQUID MIXTURES Miscible vs. Immiscible
Miscible Mixture: liquids that mix evenly, forming a homogeneous solution. Example: Soda mixed with Koolaid
Immiscible Mixture: liquids that DO NOT mix evenly, forming a heterogeneous mixture. Example: Oil mixed with Water

8. EXAMPLES
What type of matter are each of the following… ?

9. SAND

10. SAND
Heterogeneous mixture

11. Salt (NaCl)

12. Salt (NaCl)
Pure Substance: COMPOUND

13. Air

14. Air Homogeneous mixture of: Nitrogen, N2 78.08% Oxygen, O2 20.95%
Argon, Ar 0.93%
Carbon dioxide, CO %
Neon, Ne %
Helium, He %
Methane, CH %
Krypton, Kr %
Nitrogen(I) oxide, N2O %
Hydrogen, H %
Xenon, Xe %
Ozone, O %
Homogeneous mixture of:
Many gases make up mixture, but it looks like it is all one gas.

15. Gold

16. Gold
Pure Substance: ELEMENT: Au

17. Bronze

18. Bronze
Homogeneous mixture of copper and tin (alloy: mixture of metals)

19. Salad Dressing:

20. Salad Dressing:
Heterogeneous Mixture

21. Conservation Law of Conservation of Mass:
Mass cannot be created or destroyed.
Law of Conservation of Energy: Energy cannot be created or destroyed; it may only change from one form to another.

22. Matter and Energy MUST be conserved is the LAW!

23. Virtually everything is made up of atoms.

24. From the very large...

25. To the very small...

26. This includes you and me! Giggitty, Giggitty, Goo!
We are all made of atoms…and only atoms.
This includes you and me! Giggitty, Giggitty, Goo!

27. Currently we have about 117 kinds of atoms
Currently we have about 117 kinds of atoms. In the natural world there exists 92 different kinds of atoms.
The others have been artificially produced in laboratories.
The Elements Song

28. We call each kind of atom an element, and give it a specific name and symbol.
Copper Cu
Gold Au

29. Periodic Table

30. Abundance of the elements, by weight

31. The Earth’s interior is rich in iron

32. Sand is made of
Silicon & Oxygen

33. The ocean waters are made of oxygen & hydrogen

34. Of course real atoms don’t look anything like this you imbecile!
Atoms are made up of protons, neutrons, and electrons.
Of course real atoms don’t look anything like this you imbecile!
Protons and neutrons are found in the nucleus of atoms -- roughly at the center
Electrons travel around the nucleus.

35. It would be sweet if atoms really were this huge!
Different kinds of atoms, or elements, are different because they have different numbers of protons.
It would be sweet if atoms really were this huge!

36. We list the elements by their atomic numbers - the number of protons they have.
Helium, number 2
Hydrogen, number 1
In several cases the atomic weights are in parentheses.  This indicates that these elements have no stable isotopes; that is, they are radioactive.  The value enclosed in parentheses and used for the atomic weight is the atomic mass number of the most stable known isotope, as indicated by the longest half-life.

37. Physical Properties
Physical properties: characteristics that can be observed without changing the identity of the substance.
Examples:
mass
volume
color
shape
texture
density

38. Physical Changes
Physical change: a change in the physical form or properties of a substance that occurs without a change in composition.
Examples:
melting
freezing
grinding
dissolving

39. Chemical Properties
Chemical property: describes a substance’s ability to change into a different substance.
Examples:
flammability
reactivity

40. Chemical Changes
Chemical change: occurs when a substance changes composition by forming one or more new substances. (bonds are broken and bonds are formed)
Example:
HCl + NaOH  NaCl + H2O

41. Indications of a Chemical Change…
Heat in Endothermic (feels cold)
Heat out Exothermic (feels hot)
Gas is given off (fizzing or bubbles)
Color Change
New Substance is Formed

42. Evaporation is a physical change

43. Breaking is a physical change.

44. Boiling is a change of state, and therefore a physical change!

45. Rusting is a Chemical Change

46. Burning is a Chemical Change

47. Kinetic Theory
All matter is made of atoms and molecules that act like tiny particles.
These tiny particles are always in motion. The higher the temp., the faster the particles move.
At the same temp., more massive (heavier) particles move slower than less massive (lighter) particles. (inertia)

48. SOLIDS Definite shape? YES Definite volume?
Molecules in a solid are tightly packed and constantly vibrating.
Eureka: Molecules in Solids

49. LIQUIDS Definite shape? NO Definite volume? YES
Some liquids flow more easily than others. The resistance of a liquid to flow is called viscosity.
Honey has a high viscosity compared to water.
Eureka: Molecules in Liquids

50. GASES Definite shape? NO Definite volume?
The particles in a gas are spread very far apart, but can be compressed by pumping them into a restricted volume.
Eureka: Molecules in Gases

51. Phase Changes (Changes of State)
Changes in phase are examples of physical changes.
Melting: solid  liquid
Freezing: liquid  solid
Vaporization: liquid  gas
Condensation: gas  liquid
Sublimation: solid  gas
Deposition: gas  solid

52. Changes of State SOLID GAS LIQUID Melting Vaporization Condensation
Deposition
Sublimation
Vaporization
Condensation
Melting
Freezing
LIQUID

53. Energy Transfers ENERGY is the ability to change or move matter.
Energy is ABSORBED when substances melt or evaporate.
NOTE: our bodies cool down when our sweat evaporates.
Energy is RELEASED when substances freeze or condense.

54. Melting The change of state from solid to liquid.
Energy (heat) is absorbed by the substance that is melting.

55. Freezing
The change of state from liquid to solid. Opposite of melting.
Energy (heat) is released by the substance undergoing freezing.

56. Evaporation Energy (heat) is absorbed by the liquid
The change of state at the surface of a liquid as it passes to a vapor. This results from the random motion of molecules that occasionally escape from the liquid surface.
Energy (heat) is absorbed by the liquid
Can happen at any temperature

57. Condensation
The change of state from gas to liquid. The opposite of evaporation.
Energy (heat) is released by the gas to become a liquid.

58. Boiling Change from state from a liquid to a gas.
Occurs throughout the liquid.
boiling point/temperature is determined by pressure
Energy (heat) is absorbed by the liquid for it to boil and produce gas.

59. Phase Change Graph
*Boiling & freezing points depend on the pressure.

60. Water at normal pressure (1 atm):
For water at normal (every day) pressures:
Melting/freezing point:
Condensing/boiling point:
0 oC (32oF)
100 oC (212oF)

61. Phase Change Graph 0°C 100°C
*Boiling & freezing points depend on the pressure.

62. Change the pressure  Change the Boiling Point