1. 1 Unit 1: Atoms, Elements, and Compounds Pages 3-105 Lithium Atom Element Lithium By Lester Green Smallwood Academy Gambo

2. 2 Chapter 1: Atomic theory explains composition and behaviour of matter Pp 6-35

3. 3 Section 1.1 Laboratory Safety Pp 8-13

4. 4 1.01 Demonstrate knowledge of WHMIS standards Safety rules for Science Lab (pp 10-11) General Safety Rules Glassware Safety Rules Chemical Safety Rules Hot Plates and Open Flames Safety Rules Electrical Equipment Safety Rules

5. 5 1.01 continued… Know the WHIMS symbols Worksheet: WHMIS

6. 6 1.01 continued… Dangerous Container Dangerous Product

7. Science Lab Safety 1.1 A Page 9 7

8. Pp 16-19 8 Section 1.2 Investigating matter

9. 1.02 Describe earlier conceptions of the structure of matter with current conceptions Early Conceptions: Composed of four “elements”…earth, air, wind, fire. See Did you know, page 24 9

10. 1.02 continued… Current Conception: Matter is composed of atoms and atoms contain electrons, protons, and neutrons See also outcomes 1.10 and 1.11 10

11. 1.02.1 Define matter Matter Anything that has mass and volume. Mass The amount of matter in a substance Measured in grams or kilograms Volume The amount of space a substance occupies Measured in litres or cubic metres 11

12. 1.03 Investigate materials and describe them in terms of physical and chemical properties. Activity 1-2A, page 17 12

13. 1.03.1 Distinguish between chemical and physical properties. Chemical properties Observations and measurements of a substance when its reacts with another substance. Example: reactivity 13

14. 1.03.1 continued… Physical properties characteristic that can be observed or measured on its own. Examples State Color Density 14

15. 1.03.2 List examples of physical and chemical properties. (see p.18-19) PhysicalChemical ColorCombustibility MalleabilityReactivity Electrical ConductivityFlammability Magnetism Luster Density Melting and boiling points Texture 15

16. 1.04 Investigate materials and describe their physical and chemical properties. Core Lab 1-2C (p 20) 16

17. 1.05 State a prediction and hypothesis based on observed patterns. Core Lab 1-2C (p 20) 17

18. 1.06 Compile and display data collected on properties of materials Core Lab 1-2C (p 20) 18

19. 1.07 Organize data using a format that is appropriate to the experiment. Core Lab 1-2C (p 20) 19

20. 1.08 State a conclusion based on experimental data. Core Lab 1-2C (p 20) 20

21. Pp 24-29 Section 1.3: Atomic Theory 21

22. 1.09 Explain the importance of using the terms laws and theory in science  Allows scientist to communicate their observations  Theories are proposed ideas that are supported by reliable evidence  Unlike laws, theories are subject to change if new evidence is found 22

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24. 1.09.1 Distinguish between a theory and a law Theory Explanations of observations that are supported by reliable evidence Theories are subject to change given new evidence 24

25. 1.09.1 continued Laws Describes events, patterns, or relationships that have been observed. They state what happens with no explanation Laws are constant and do not change 25

26. 1.10 Identify major changes in atomic theory up to and including Bohr model 26

27. 1.10.1 Describe the contributions of scientists to the development of the atomic theory. Early Greeks Empedocles claimed matter was composed of four “elements”…air, wind, earth and fire. 27

28. Early Greeks continued… Democritus Substance can be divided into smaller and smaller pieces until it could be no longer divided. He called the smallest piece “atomos” Today we use the word atom 28

29. Early Greeks continued... Aristole A greed with the theory proposed by early Greeks but suggested there was a fifth element. Belief of the Greek scholars FOUR elements 29

30. 1.10.1 continued Dalton (Billard Ball Theory) Matter composed of small, hard spheres that are different for each type of elements. Gold spheres are not like lead spheres He defined the atom as the smallest particle of an element and it could not be divided. 30

31. 1.10.1 continued J.J Thomson (Raisin Bun Model)  He determined that there were streams of negatively charged particles (electrons)  He concluded that all atoms must contain these smaller particles. 31

32. 1.10.1 continued J.J Thomson (Raisin Bun Model). He proposed a “raisin bun” model of the atom. The bun was positively charged and the raisins were negatively charged 32

33. 1.10.1 continued Rutherford His team noticed that when highly charged particles were fired at gold foil, some bounced back. Reasoned that there was a concentration of particles 33

34. 1.10.1 continued Rutherford An atom was much more than just empty space of scattered electrons. (as opposed to what the "plum pudding model" proposed) An atom must have a positively charged center that contains most of its matter He called this dense, concentrated center the nucleus The positively charged center (nucleus) was relatively small in reference to the total size of the atom 34

35. 1.10.1 continued Rutherford (Planetary Model) Inside the nucleus there are two kinds of particles 1 Protons…positively charged 2 Neutrons…neutral or no electric charge 35

36. 1.10.1 continued Neils Bohr (Orbital Model) Discovered that electrons in an atom are arranged in energy levels or shells. Electrons have different amounts of energy 36

37. 1.11 Describe Rutherford’s experiment to test Thomson’s atomic model See previous slides on Rutherford’s gold foil experiment See page 27 and take brief notes 37

38. 1.11.1 Recognize that the atomic theory continues to be defined Equipment used today were not available to early scientist. This allows scientist to do different experiment and to collect data that were not possible in the past. New data allows scientist to continuously redefined their knowledge 38

39. 1.12 Use models in describing the structure and components of atoms 39

40. 1.12.1 Define atom The smallest particle of an element that retains the properties of the element. 40

41. 1.12.2 Distinguish among protons, neutrons and electrons. Charge  Neutrons neutral  Protons positive charge  Electrons negative charge 41

42. 1.12.2 continued Relative Mass Neutron…1837 times more than an electron Proton…1836 times more than an electron Electron…1 42

43. 1.12.2 continued Location in the atom Neutron nucleus Proton nucleus Electron surrounding the nucleus 43

44. 1.13 Give examples of group settings and individual activities related to atomic structure Worksheets: Atomic structure 44