Matter

1. Matter

2. What is matter? • Something which occupies space and has mass • Can be sensed and measured

3. Is everything in the universe matter? No!

4. Describing Matter • Since the time of the Greeks, people have wondered about the nature of matter. • There were 2 main concepts.

5. Concepts of Matter • Matter is continuous. • It can be subdivided forever. • There is no smallest particle.

6. Concepts of Matter • Matter is NOT continuous. • Subdividing matter eventually must stop at the smallest particle. • This is theparticle theory of matter.

7. The Particle Model of Matter

8. How big are these particles? • Very, very tiny • 1 million particles laid side-by-side would not be as long as the thickness of a sheet of paper.

9. What are they called? • These smallest particles are called atoms. • Aristotle thought that they had no size at all. • We can image atoms with the STM (Scanning Tunneling Electron Microscope).

10. Particle Model Evidence A good model should match real-life observations.

11. Particle Model Evidence • Dissolving sugar into tea • Dissolving cherry drink mix into water

12. Particle Model Evidence • We can indirectly observe that these particles are moving.

13. Particle Model Evidence • The mixing caused by this motion is called diffusion. • Since Robert Brown first noticed evidence of the particle motion that causes diffusion, it is called Brownian motion.

14. Kinetic-Molecular Theory The evidence leads to the conclusion that matter is composed of tiny particles that are in random, constant motion.

15. Atom • Basic particle of matter • Made up of protons, neutrons and electrons

16. Protons • Located in the nucleus • Have a + charge • Have the same relative mass as the neutron

17. Neutrons • Located are in the nucleus • Have a neutral charge • Have the same relative mass as proton

18. Electrons • Located are outside the nucleus • Have a negative charge • Have a very tiny relative mass compared to protons and neutrons

19. Atom • Mass – protons and neutrons account for almost all of the mass of the atom • Volume – electrons account for the volume of the atom

20. Molecules • Molecules are formed when atoms bond together. • Molecules usually do not have a charge.

21. Ions • A charged atom • Formed with atoms lose or gain electrons

22. Ions • Cations – atoms lose electrons to form positive ions. • Anions – atoms gain electrons to form negative ions.

23. What is “mixing” due to particle motion? • Diffusion • Boiling • Freezing • Melting Question

24. T/F A molecule consists of atoms chemically bonded together. T Question

25. Classifying Matter

26. matter puresubstances mixtures

27. matter puresubstances compounds mixtures elements iron gold lead uranium sodium chloride glucose calcium carbonate water

28. matter puresubstances mixtures elements compounds iron gold lead uranium sodium chloride glucose calcium carbonate water

29. homogeneousmixtures heterogeneousmixtures mixtures air gasoline 14 karat gold seawater granite soil blood chocolate cake

30. matter puresubstances mixtures elements compounds homogeneousmixtures heterogeneousmixtures iron gold lead uranium sodium chloride glucose calcium carbonate water air gasoline 14 karat gold seawater granite soil blood chocolate cake

31. Pure Substances • contain only one kind of matter

32. Elements All atoms are the same.

33. Compounds • made up of two ore more atoms • have the same ratio of elements

34. Compounds 2 types Organic Inorganic • contain carbon • living things • do not have carbon • water, table salt

35. Mixtures • Contains two or more substances • physically placed together, not bonded • Variable composition

36. Mixtures 2 types Homogeneous Heterogeneous

37. Homogeneous • Particles are NOT visible separate. • called solutions Examples: saltwater, alloys

38. Heterogeneous • Particles are visible separate. Examples: soil, vegetable stew, wood, concrete

39. States of Matter • solid • liquid • gas

40. Solid • Particles are locked in place. They are rigid and have a definite shape. • Particles have low kinetic (motion) energy. • Particles are not very compressible and have a definite volume.

41. 3 Types of Solid Structures • crystalline – Particles are locked in a pattern. • amorphous – Particles lack a pattern; fluid • heterogeneous solid – no orderly pattern but not totally random

42. Liquid • Particles can flow around each other. They have no definite shape. • Particles have a higher kinetic energy than solids. • Particles are not very compressible. They have a definite volume.

43. Viscosity • the thickness of a liquid • High attraction between the particles and flows slowly. • Less viscous at higher temperatures

44. Lubricants liquids that reduce friction

45. Gas • Particles are separate from one another; no definite volume or shape. • Particles can be compressed because of the space between them.

46. Gas • Particles move very fast and have a very high kinetic energy. This allows them to overcome attractive forces. • Particles move a short distance before colliding with other gas particles.

47. Fluids (Liquids and Gases) substances that have the ability to flow

48. Fluids (Liquids and Gases) • Gas expands to fill a container; liquid does not. • Both gases and liquids will mix because the particles are not locked in place.

49. Fluids (Liquids and Gases) • A warmer substance mixes faster. • Particles colliding with a container cause pressure.

50. Plasma hot, ionized gas