1. MATTER
ANYTHING WITH MASS AND VOLUME

2. Classification of Matter
Elements
Pure Substances
Compounds
Matter
Homogeneous
Mixtures
Heterogeneous

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

4. Elements 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. Compounds A molecule is formed when two or more atoms combine.
Compounds are pure substances that are made of more than one element bound together.
Examples: water, table salt, and carbon dioxide.

6. MIXTURES Heterogeneous vs. Homogeneous
Homogeneous matter: matter that has identical properties throughout.
Examples: Sugar, salt, water, and whipped cream
Heterogeneous matter: matter that has parts with different properties.
Examples: granite, soil, potpourri

7. Conservation
Law of Conservation of Matter (Mass): matter 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.

8. Matter and energy MUST be conserved; it’s the LAW!

9. Virtually everything that is, is made up of atoms.

10. From the very large...

11. To the very small...

12. This includes you and me!
We are all made of atoms…and only atoms.
This includes you and me!

13. Making stuff nature never dreamed of.
Currently we have about 115 kinds of atoms. In the natural world there exists 88 different kinds of atoms.
The others have been artificially produced in laboratories.
Making stuff nature never dreamed of.
The Elements Song

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

15. Periodic Table

16. Abundance of the elements, by weight

17. The Earth’s interior is rich in iron

18. Sand is made of
Silicon & Oxygen

19. The ocean waters are made of oxygen & hydrogen

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

21. They don’t look anything like this either!
Different kinds of atoms, or elements, are different because they have different numbers of protons.
They don’t look anything like this either!

22. We list the elements by their atomic numbers - the number of protons they have.
Helium, number 2
Hydrogen, number 1

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

24. 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

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

26. 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

27. Indications of a Chemical Change…
Flames
Gas is given off (not to be confused with boiling)
Color Change

28. Evaporation is a physical change

29. Breaking is a physical change.

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

31. Rusting is a Chemical Change

32. Burning is a Chemical Change

33. 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.

34. SOLIDS Definite shape? YES Definite volume?
Molecules in a solid are tightly packed and constantly vibrating.

35. 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.

36. 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.

37. Phase Changes Changes in phase are examples of physical changes.
Melting: solid  liquid
Freezing: liquid  solid
Vaporization: liquid  gas
Condensation: gas  liquid
Sublimation: solid  gas

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

39. 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.

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

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

42. Evaporation
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 released by the liquid (Cooling of the liquid results)
Can happen at any temperature

43. Condensation
The change of state from gas to liquid. The opposite of evaporation.
Energy (heat) is absorbed by the liquid (Warming of the liquid results)

44. Boiling Change from state from a liquid to a gas.
Occurs throughout the liquid.
boiling point/temperature is determined by pressure
Energy (heat) is released by the liquid.

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

46. 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)
Label the points & temperatures on your graph.

47. Change the pressure  Change the Boiling Point

48. Phase Diagrams
a phase diagram shows the equilibria pressure-temperature relationship among the different phases of a given substance

49. WATER
Carbon Dioxide C
AD =
AB =
AC =

50. C
melting curve
AD =
AB =
AC =

51. C
melting curve
sublimation curve
AD =
AB =
AC =

52. C
vapor pressure curve
melting curve
sublimation curve
AD =
AB =
AC =

53. A D triple point = Point ______C A
triple point = Point ______
The point at which all 3 phases of a substance (solid, liquid, gas) can coexist at equilibrium. D
critical point = Point ______
The combination of critical temperature and critical pressure.
critical temp = temp. above which a gas cannot be liquefied. (H2O=374ºC)
critical pressure = press. required to liquefy a gas at its critical temperature. (H2O=218 atm)

54. Conditions for H2O on other planets…