1. Section 1.1: Matter has mass and volume

2. Matter - anything that has mass and takes up space (volume) Mass – the measure of the amount of matter an object contains Volume – the amount of space that an object occupies measured with a balance measured in grams (g) not the same as weight solids: cm 3 liquids: mL

3. Measuring Mass, Weight, and Volume MassWeightVolume Definition: The amount of matter an object contains. Definition: The downward pull on an object due to gravity Instrument: balance Instrument: scale Instrument: graduated cylinder, L x W x H, water displacement Metric unit: gram (g) Metric unit: newton (N) Metric unit: solids – cm 3 liquids – mL Definition: The amount of space an object occupies.

4. MassWeightVolume Other information: will not change with location Other information: weight of an object will change with location if the gravity changes Other information: solids, liquids, and gases all have volume

5. Your weight on different planets

6. Section 1.2: Matter is made of atoms Section 1.3: Matter combines to form different substances

7. An atom is the smallest particle of matter.

8. Democritus suggested:  Atoms were the smallest particles of any substance.  Atoms cannot be divided.  Atoms differed in size, shape, and, weight. Democritus’s Model

9. Solid Sphere Model John Dalton 1803 Dalton explained:  Atoms are the smallest particle and cannot be divided.  Atoms that make up the same elements are the same.  Atoms that make up different elements are different.  Atoms cannot be created or destroyed.

10. Plum Pudding Model J. J. Thomson 1897 Thomson proposed:  Atoms are made up of positively and negatively charged particles.  The negatively charged particles he called electrons.  The negative electrons are set in positively charged particles.

11. Planetary Model Ernest Rutherford 1911 Rutherford proposed:  An atom is made up of mostly empty space.  There is a center nucleus made up of positively charged protons.  Negatively charged electrons orbit around the nucleus.

12. Bohr Model Niels Bohr 1913 Bohr proposed:  Electrons orbit the nucleus at different energy levels.  Only a certain number of electrons could fit at each energy level.

13. Electron Cloud Model  Protons and neutrons are tightly packed into the nucleus of the atom.  The electrons are in a cloud around the nucleus but not indefinite orbits.

14. Two Parts of an Atom Electron cloud most of an atom’s volume nucleus most of an atom’s mass What is an atom?the smallest particle that makes up matter

15. Parts of an Atom protons – positively charged particles found in the nucleus of an atom neutrons – neutrally charged particles found in the nucleus of an atom electrons – negatively charged particles found orbiting the nucleus in the electron cloud

16.  Protons and neutrons have roughly the same mass, and each is about 2000 times more massive than an electron.

17. electron cloud nucleus electron proton neutron + + +

18. Electron CloudNucleus makes up most of an atom’s volume makes up most of an atom’s mass Contains: protons- positive charge neutrons - no charge electrons - negative charge

19. Normal atoms have no charge. - + + + + + - - - - the number of positive protons the number of negative electrons must equal =

20. http://web.visionlearning.com/custom/chemistry/animations/CHE1.3-an-atoms.shtml

22. Definition -matter that is made up of only one kind of atom

23. The Periodic Table of Elements is a chart used to organize and classify all of the elements.

24. All information about an atom can be found on the Periodic Table of Elements.

25. Symbol for the element: First letter always capitalized Second and third letters always lower case Periods are not used Atomic number: The number of protons in the nucleus Atomic mass: The number of protons and neutrons in the nucleus Name of the element

26. Information about atoms found on the Periodic Table of Elements: 18 Ar Argon 39.948 atomic number symbol element name atomic mass Round atomic mass to the nearest whole number ( 40 )

27. 27 atomic number Co element symbol cobalt element name 59 atomic mass atomic number number of protons protons = electrons element symbol element name atomic mass protons + neutrons

28. 27 atomic number number of protons protons = electrons Co element symbol cobalt element name 59 atomic mass protons + neutrons On the white paper:

29. neonsodium calciumphosphorous

30. copperarsenic seaborgiumiodine

31. 7Nitrogen 226138 126 5927 42 4Lithium 2412 13355 atomic mass number of neutrons number of protons element 14 88Radium 6Carbon Cobalt Helium Magnesium Cesium 7 32 78 2 3 12 7

32. 88 11969 117Platinum 14692 35Chlorine 5931 10847 3116 atomic mass number of neutrons number of protons element Oxygen Tin Uranium Nickel Silver Phosphorous 16 195 238 18 61 50 78 17 28 15

33. ElementProtonsNeutrons Atomic Number Electrons Atomic Mass Calcium Neon Fluorine Cobalt 777714 20 40 2412 171817 35 10 2010 6530 3530 4018 2218 9991019 5224 2824 27 82207 59 8212582 3227 Nitrogen Magnesium Chlorine Zinc Argon Chromium Lead

34. Periodic Table of Elements #1: Web Elements Periodic Table of Elements #2: Chemical Elements Periodic Table of Elements #3: Jefferson Lab Periodic Table #4: Los Alamos National Lab Jefferson Lab: Element Games

35. Step 1:Glue your white paper to the TOP of your colored paper. Step 2:Write your research information on the white paper.

36. Step 3:Fold the top of your paper to the bottom of the WHITE paper. Step 4:Fold up bottom flap. Step 5: Add periodic table information. atomic number symbol name atomic mass

38. Definition : a particle that is made up of two or more atoms bonded together  Molecules can be made up of atoms that are alike or atoms that are different.

41. Definition : a particle that is made up of two or more atoms bonded together  Molecules can be made up of atoms that are alike or atoms that are different.

42. Molecules in Air

43. Definition – a substance that consists of two or more different types of atoms bonded together  A compound has different properties from the individual elements that make up the compound.

44. Sodium chloride: salt chlorine – a poisonous gas sodium – a dangerous metal

45. carbon – dark solid element oxygen – invisible gas element

47. Water Molecule A water molecule contains: 2 hydrogen (H) atoms 1 oxygen (O) atom A chemical formula is used to identify the composition of a compound. The chemical formula for water is: H2OH2OH2OH2O

49. Chemical formula oooooooo NH 3 C 4 H 10 CO 2

50. C 6 H 12 O 6 Chemical formula: llllllllllll

51. Definition – a combination of different substances that remain the same individual substances and can be separated by physical means

52. Matter can be Mixed Mixed substances are made of different atoms and or molecules.Pure Pure substances are made of only one type of atom or molecule. element atommolecule compound homogeneous(uniformedmixture)heterogeneous(nonuniformmixture) looks the same throughout can see the different parts

53. Cover Elements, Compounds, and Mixtures

54. Pocket #1 Pure substances: substances made up of only one kind of atom or molecule 1.atom/element 2.molecule/compound

55. Pocket #2 Mixed substances: substances made up of different atoms and/or molecules 1.uniform mixtures 2.nonuniform mixtures

56. Card definitions atom – the smallest particle that makes up matter element – matter made of one kind of atom Card #1 Card #2 molecule – the smallest particle of a compound compound – a substance that is made up of two or more different kinds of atoms that are chemically combined

57. Uniform mixture - looks the same throughout Nonuniform mixture - can see the different parts ocean waterair cake batter bronze brass chocolate milk soda soil blood Card #1 Card #2 (homogeneous) (heterogeneous)

58. Comparing Compounds and Mixtures Compound: Mixture: 1.New substances are formed by atoms that chemically combine together. 1. Substances in a mixture physically combine and remain the same substances. and remain the same substances.

59. Compound: Mixture: 2.Elements in a compound are always in the same proportions or in a fixed amount. or in a fixed amount. 2. Substances in a mixture can be combined in any amount.

60. Compound: Mixture: 3. Substances cannot be physically separated. 3. Substances can be physically separated.

61. elements compounds

62. 123 456

63. 7 8 9 10 11 1213

64. 1415