1. STATES OF MATTER
CH. 1

4. Property Examples
odor
taste
color
texture
shape

5. PROPERTIES
Physical properties:Characteristics of a substance that can be determined without changing it into a new substance.
Chemical properties:Characteristics of a substance that determine how it will react with other substances.

6. Physical Change-a change that doesn’t produce a new kind of substance.

7. CHEMICAL CHANGE
A Chemical change is the process of forming a new substance that has different properties by chemically combining atoms.

8. Iron Oxide

10. Mass-the amount of matter in an object.

11. Volume-the amount of space an object takes up.

13. Density-the amount of matter in a given space.

14. Matter-anything that has mass and volume.

15. States of Matter

17. Solid-a substance that has a definite volume and shape.
Tightly packed in a definite pattern.

18. Types of Solids
Crystalline-particles arranged in a specific repeating pattern. (diamond)
Amorphous-particles are arranged in a random pattern. (charcoal)

19. Liquid-a substance that has a definite volume but no definite shape.
Close together but free to flow.

20. Viscosity The measurement of a liquid’s resistance to flow.
-Honey Water

21. Viscosity
The stronger the force of attraction, the higher the viscosity. Heat weakens the forces to lower viscosity.

22. Surface Tension
The uneven forces acting on the particles on the surface of a liquid.

23. Surface Tension
The stronger the attractive forces between particles, the greater the surface tension.
-The water molecules at the surface have a higher downward pull, creating tension on the surface.

24. Gas-a substance that has neither a definite shape nor volume.
Spread apart and move about freely.

25. Changing States

26. Melting-Solid to Liquid

27. Freezing-Liquid to Solid

28. Vaporization-Liquid to Gas

29. Evaporation-Vaporization from the surface.

30. Condensation-Gas to a Liquid

31. Sublimation-solid directly to a gas.

32. Deposition-Gas directly to a solid

33. Vapor
Vapor-The gas state of a substance that is normally a solid or liquid at room temperature.

34. Behavior of Gases
Pressure-the amount of force applied per unit of area(volume).
Boyle’s Law-pressure of a gas increases if the volume decreases and decreases if the volume increases, when the temperature remains constant.
Charles’ Law-the volume of gas increases with increasing temperature, if the pressure is constant.

35. Plasma-a substance made of high energy particles.

38. Energy
Kinetic-Energy of motion. The faster the particles move the more kinetic energy they have.
Potential-Stored energy(chemical potential). The farther apart the particles, the more the greater the potential energy.

39. Thermal Energy
Matter changes from one state to another by adding or taking away heat.

40. Kinetic Molecular Theory
-How particles in matter behave.
Small particles make up all matter.
Particles are in constant, random motion.
Particles collide.
No energy is lost when they collide.

41. Conservation of Mass and Energy

42. Dalton’s Atomic Theory
Atoms are the basic
building blocks of all
matter. They are the
smallest form of a
substance and cannot
be broken down any
further.

43. Atomic Structure

44. Atoms

45. Make up of an atom (subatomic particles)
An atom has a nucleus made of positively charged protons and neutral neutrons. An electron cloud surrounds the nucleus. The electron cloud contains negative electrons. The cloud has three energy levels. The 1st contains up to 2 electrons.
The 2nd and 3rd contain up to 8 electrons.

47. Atom
Nucleus Protons-Positive Neutrons-Neutral Electron Cloud(7 levels) Electrons-Negative Level 1-up to 2 electrons Level 2-up to 8 electrons Level 3-up to 8 electrons

48. Periodic Table

49. Atomic Number-the number of protons in the nucleus of an atom.

51. Mass Number(Atomic Mass)-the total number of protons and neutrons in the nucleus of an atom.

52. Mass Number

53. Atomic Mass

54. Atoms

55. Energy Levels

58. Ions-charged atoms that occur when electrons are gained or lost creating a difference between the number of protons and electrons.

59. Ions

60. Ionic Bonding-transfer

63. Covalent Bonding-share

65. Isotopes-atoms of the same element(same # protons) that have a different number neutrons.

66. Classifications of Matter
Elements
Compounds
Mixtures

67. Elements-matter that cannot be broken down by ordinary chemical means.

68. Elements/Compounds

69. Compound-two or more kinds of atoms chemically combined.

70. Sodium

71. Chlorine

72. NaCl

73. Mixture-two or more substances physically combined.

74. Mud