1. Create your “Water Droplet Obituary” Page 41 Thursday, October 25, 2012 Friday, October 26, 2012 Page 42 Water Quality Indicators/Treatment Quick Check Water Droplet Obituary Warm Up: 1.Take out the EOG Prep Book, place it between you and your should buddy and turn to page 157. Read Chapter 21 silently. 2.Answer “Lesson Review” Questions 1-3 3.Also, answer the “Discussion Question” on page 160. *LAST SCIENCE CLASS OF THE 1 st QUARTER!* Homework: 1.Create your Water Droplet Obituary o Be sure to include 1. A specific start point 2.Your path through the water cycle 3.A specific end point Thursday, October 25, 2012 Friday, October 26, 2012 Water Droplet Obituary – Describes the series of locations, events and experiences that droplet had in its “lifetime”. Possible Starting Points: Headwaters of Catawba River Basin Precipitation from a rain cloud into a forest Puddle near a factory Hydroelectric Power Plant at Lake Norman Carowinds Water Park Possible Ending Points: Pfiesteria infested swamp Hog waste lagoon In a bottle from a drinking water treatment facility Waste water treatment center Puddle in front of JMR

2. Read Section 1.1 of Unit D in Text Answer Q 1-3 Page 43 Tuesday, October 30, 2012 Wednesday, October 31, 2012 Page 44 Intro to Chemistry and Atoms Warm Up: Wait for video questions Homework: 1. Read Section 1.1 of Unit D in Text Answer Q 1-3 Chemistry – The study of matter and atoms and the changes they can undergo Atoms – The building block and basic unit of all matter - Consist of a small charged particles Subatomic Particles – Atoms contain charged particles Nucleus Electron Cloud (rings) Positive – Protons Negative – Electrons Neutral – Neutrons Parts of an Atom : Tuesday, October 30, 2012 Wednesday, October 31, 2012 Nucleus Electron Cloud

3. Atomic Number – Number of Protons - This is how elements are arranged on the periodic table Neutral Atom –Protons = the number of Electrons Atomic Mass Number – Number of Protons + Neutrons - The total mass of the nucleus Connection to the Periodic Table of Elements (p. 20 D) 6 C Carbon 12.001 Atomic Number = # of Protons / Electrons Symbol = 1 st letter always capital Atomic Mass = Protons + Neutrons

4. Page 46 Reading Atoms on the Periodic Table 16 S Sulfur 32.066 13 Al Aluminum 26.982 11 Na Sodium 22.990 Protons: Neutrons: Electrons: Protons: Neutrons: Electrons: Protons: Neutrons: Electrons:

5. Page 46 Atomic Structure Notes Continued Bohr Model - model that shows where particles are located in atoms. Valence electrons – outermost energy level Carbon: 6 Protons How many valence electrons? 6 Neutrons 6 Electrons

6. Page 46 Bohr Model Practice: Use the information to make a Bohr model Carbon: 6 Protons 6 Neutrons 6 Electrons Nitrogen: 7 Protons 7 Neutrons 7 Electrons Oxygen: 8 Protons 8 Neutrons 8 Electrons

7. Page 46 Practice: Determine Protons, Neutrons and Electrons, Draw a Bohr Diagram 5 B Boron 10.811 10 Ne Neon 20.180 12 Mg Magnesium 24.305

8. Page 45 Thursday, November 1, 2012 Friday, November 2, 2012 Page 46 Thursday, November 1, 2012 Friday, November 2, 2012 Homework: 1.Practice Bohr Models 2.Finish Pure Substances vs. Mixtures Graphic Organizer Warm up: 1.Atoms of the same element are alike / different. 2.Protons are positive / neutral / negative. 3.Protons are inside / outside the nucleus. 4.Neutrons are positive / neutral / negative. 5.Neutrons are inside / outside the nucleus. 6.Electrons are inside / outside the nucleus. 7.The overall charge of the nucleus is positive / neutral / negative. Practice Bohr Models Finish Pure Substances vs. Mixtures Graphic Organizer Bohr Models Pure Substances vs. Mixtures Pure Substances – same composition throughout (atoms, elements, compounds) Mixtures – physical combinations

9. Page 47 Monday, November 5, 2012 Wednesday, November 7 2012 Page 48 Monday, November 5, 2012 Wednesday, November 7, 2012 Homework: 1.Finish Periodic Table Worksheet - Parts 1 and 2 ONLY Warm up: Finish Periodic Table worksheet Introduction, Organization and History of the Periodic Table 1.Determine what element this Bohr model is representing. 2.How did you come to this conclusion? 3.Draw a Bohr model for Helium and Neon – can you make any observations that make these two alike in any way? 4.Make a t-chart and compare and contrast mixtures and pure substances.

10. Matter Has mass or weight Takes up space (volume) Cannot occupy the same space as other matter at the same time Pure Substances Has the same composition throughout Can Occur Naturally Mixtures Formed when two or more substances are physically combined Parts can be physically separated Substances in a mixture retain their original properties Element Cannot be broken down into simper substances Compound Chemical combination of two or more different elements Cannot be physically separated Properties are entirely different properties of each element alone Homogeneous Parts of the mixture are evenly distributed Heterogeneous Parts of the mixture are not evenly distributed

11. Group or Family (All have same number of valence electrons) Period or Row (One proton is added from left to right) Metaloids Nobel Gasses Non-Metals Metals

12. Chinese Periodic Table

14. Chemistry Careers Food Chemistry Make up Gatorade Fireworks Forensic Detectives Pharmacist Cologne/Perfume Toothpaste/mouthwa sh/hand lotion, etc

15. Page 49 Thursday, November 8, 2012 Friday, November 9, 2012 Page 50 Thursday, November 8, 2012 Friday, November 9, 2012 Homework: 1.Finish Periodic Table Basics Activity Periodic Table Families – Part 3 Metals, Non-Metals and Metalloids Periodic Table Basics Activity Warm Up: Identify each container as a beaker full of elements, compounds, heterogeneous mixture or homogeneous mixture. Finish Periodic Table Basics Activity

16. Families of Elements on the Periodic Table – Part 3

18. Properties of …. Metals Metalloids Most are solids Can be shaped & pulled into wires Shiny / lustrous Good conductors of electricity/heat Tend to lose electrons in chemical reactions Most are Solids Can be shiny or dull Can be shaped & pulled into wires Conducts better than nonmetals but not as well as metals Most are gases Solid non-metals are brittle Not shiny, but dull Poor conductors of electricity and heat Tend to gain electrons in chemical reactions Non-metals

19. Page 51 Tuesday, November 13, 2012 Wednesday, November 14, 2012 Page 52 Homework: 1.Study for Quiz on Atomic Structure, Periodic Table and Pure Substances/Mixtures next class History of the Periodic Table Periodic Eggs/Atomic Cube Activities Warm Up: 1)What are some characteristics the “Carbon Family” shares? 2) Study for Quiz Tuesday, November 13, 2012 Wednesday, November 14, 2012 History of the Periodic Table Dimitri Mendeleev (1834 – 1907) Siberian Founded the periodic table (1869) Organized by Atomic Mass and properties Could predict where new elements would go on the table Henry Moseley (1887-1915) Studied elements using x-rays Was able to slightly reposition the periodic table because he could see protons Killed in WWI at age of 28 Britain made a policy that restricts scientists from fighting in wars

20. Mendeleev’s Original Periodic Table

21. Moseley’s Modern Periodic Table

22. Page 53 Thursday, November 15, 2012 Friday, November 16, 2012 Page 54 Homework: Reflect on 1 st Quarter, especially your science grade, and crate a t-chart that lists things you did well with and things you need to improve. Nuts and Bolts Activity Announced Chemistry Quiz Warm Up: 1)Create a concept map that has the topic of Chemistry in the middle and branches out into Atoms, Periodic Table, History and Matter. Then expand on each topic. See below for example: Reflect on 1 st Quarter – Make a T-Chart Thursday, November 15, 2012 Friday, November 16, 2012 Chemistry Atoms Periodic Table History Types of Matter