1. Complete Castle Learning, Check PAM Warm Up: 1) How are satellites used in remote sensing? 2) What is it called when a city expands quickly into low-density housing areas (spread out housing). Page 41 Homework : Complete Castle Learning and Check PAM for grade updates! Page 42 Friday, October 21, 2011 (A) Wednesday, October 26, 2011 Chemical vs. Physical Change Pre-Assessment

2. Complete Castle Learning and Turn in Late Work Warm Up: 1) Take out your study guide and review your notes for 5 minutes in preparation for your 1 st quarter exam. Page 43 Homework : Complete Castle Learning and Turn in Late Work Page 44 Monday, October 24, 2011 (B) Tuesday, October 25, 2011 1 st Quarter Exam Team Grading Monday, October 24, 2011 (B) Tuesday, October 25, 2011

3. Observe 5 physical and 5 chemical changes Warm Up: 1) Turn to your prospectus page and review the goals you set at the beginning of the year. 2) Reflect on your goals, did you meet them, did you perform the way you wanted to during 1 st quarter. 3) Make new goals, on a separate sheet of paper, designating areas that you are strong, weak and need work at. Page 45 Homework : Observe 5 real-life examples of chemical and physical changes (10 observations total) Page 46 Monday, October 31, 2011 (B) Tuesday, November 1, 2011 (A) Chemical vs. Physical Properties/Changes Booklet Project Rubric review Monday, October 31, 2011 (B) Tuesday, November 1, 2011 (A)

4. Finish Properties of Matter Foldable/Booklet Warm Up: Analyze the following questions: 1) Why do fish prefer the liquid state of water. Why is the solid and gaseous form not suitable? 2) Why is copper used to make wire? Why might iron not be suitable for this? 3) Why is lead used for a sinker in fishing? What isn’t a plastic bead suitable for a this? Page 47 Homework : Finish Properties of Matter Foldable/Booklet Page 48 Wednesday, November 2, 2011 (B) Thursday, November 3, 2011 (A) Properties of Matter Foldable/Booklet Wednesday, November 2, 2011 (B) Thursday, November 3, 2011 (A)

5. Complete Phase Changes Questions on Handout Warm Up: 1. Read the lab procedures for the Phase Change Lab. Write a hypothesis. (If…then, because…) 2. Identify the independent and dependent variables in the lab. Page 49 Homework : Complete Phase Changes Questions on Handout Page 50 Friday, November 4, 2011 (B) Monday, November 7, 2011 (A) Changes of State Lab(s) Friday, November 4, 2011 (B) Monday, November 7, 2011 (A)

6. Density Lab Report – Test Grade Warm Up: 1. See Phase Change Handout for warm up Page 51 Homework : Density Lab Report Page 52 Tuesday, November 8, 2011 (B) Wednesday, November 9, 2011 (A) Density Labs Tuesday, November 8, 2011 (B) Wednesday, November 9, 2011 (A)

7. Read Section 1.1 of Unit D in text and Answer Questions 1-3 Warm Up: (You Don’t Need to Write the Questions Today) 1. List the 7 specific physical properties with an example. 2. List the 2 specific chemical properties with an example 3. Why isn’t changing state a chemical property? 4. Think about our labs last period, why was the density of water the same for each trial, even though all the volumes weren’t the same? Page 53 Homework : 1.Define the vocabulary words from section 1.1 of Unit D by doing word triangles. ( Proton, Neutron, Nucleus, Electron, Atomic Number, Atomic Mass Number, Isotope, Ion) 2. Read the section and answer questions 1-3 at the end. Page 54 Physical and Chemical Properties Quiz Atomic Structure Pre-Assessment Atomic Structure Vocabulary Thursday, November 10, 2011 (B) Monday, November 14, 2011 (A) Use the information and the model of the atom below to answer the questions. 1.Shade the nucleus of the atom light blue. 2.How many protons are there in Fluorine? 3.Place a red to represent where the protons belong in this atom. 4.How many neutrons are in Fluorine? 5.Place a green dot where the neutrons belong in this atom. 6.How many electrons are in Fluorine? 7.Put an orange dot where each electron belongs 9 F Fluorine 18.998

8. Atomic Math Challenge Diagram Notes : Atomic Structure; Bohr Model; and Lewis Structure Tuesday, November 15, 2011 (B) Wednesday, November 16, 2011 (A) Page 55 Warm Up: 1. Read the “Atom’s Family Album found at your table and complete the family list in each of the boxes provided 2. Label the atom found on the back of the sheet using information from your reading. Bohr Model – displays the atomic structure with nucleus and electron clouds - Rule of the Rings: 1 st Ring/Shell = 2 electrons 2 nd Ring/Shell = 8 electrons 3 rd Ring/Shell = 18 electrons 4 th Ring/Shell = 32 electrons LET’S PRACTICE!!! Atomic Structure: Fluorine Atomic # 9 Atomic Mass Number: 18.998 Protons: 9 Neutrons: 10 Electrons: 9 Nucleus Valence Electrons: 7 Electron Cloud Atom – the smallest unit of matter Protons – Positively charged particles found in the nucleus of an atom - # can’t change without changing the atom Neutrons – Neutrally charged particles found in the nucleus of an atom - Number can change with isotopes Electrons – Negatively charged particles found in clouds surrounding the nucleus - # can change with ions

9. Page 56 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

10. Page 56 Atomic Number – Number of Protons - Does not change - How elements are arranged on the periodic table Neutral Atom – When the number of Protons equals the number of Electrons Atomic Mass Number – Number of Protons + Neutrons - The total mass of the nucleus Atomic Structure Notes Continued 6 C Carbon 12.001 Atomic Number = # of Protons / Electrons Symbol = 1 st letter always capital Atomic Mass = Protons + Neutrons

11. Page 56 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:

12. Page 56 Atomic Structure Notes Continued Valence Electrons – The number of electrons in the outermost energy level of a particular element. The number of valence electrons matches the family number of the element Lewis Structure – A method of writing the chemical structure of an element using the element’s symbol and the number of electrons located in the outermost energy level or the valence electrons. (no more than 2 dots per side!) C Carbon: 6 Protons How many valence electrons? 6 Neutrons 6 Electrons

13. Page 56 Practice: Determine Protons, Neutrons and Electrons, Draw a Bohr Diagram and Lewis Structure 5 B Boron 10.811 10 Ne Neon 20.180 12 Mg Magnesium 24.305

14. Read Section 1.2 of Unit D and Answer Questions 1-3 Practice Atomic Structure Isotope and Ion Notes Thursday, November 17, 2011 (B) Friday, November 18, 2011 (A) Page 57 Warm Up: 1.Practice creating a Bohr model and Lewis structure for the following elements: 1.Potassium 2.Scandium 3.Beryllium 2. How is this Lewis structure different from the ones we did last period? What should you do to not violate the “8 dot rule” for your Lewis structure? Thursday, November 17, 2011 (B) Friday, November 18, 2011 (A) Page 58

15. Isotopes or Different Elements?

16. What is an Isotope? Isotope – atoms (elements) with the same number of protons (atomic number) but with different numbers of neutrons

17. Examples Let’s look at Hydrogen… How many protons, neutrons and electrons does Hydrogen typically have?

18. Examples of an Isotope

19. So, what exactly is an isotope? When an element has a fixed number of protons, but has more than one combination of neutrons Example: Hydrogen can have 0, 1, or 2 neutrons, but it always has 1 proton!

20. Now you try! I will give you two scenarios, you and your table must determine if the pair of elements are isotopes or different elements. Remember, they will be different elements if there are different number of protons!!!

21. Review 1.Element D has 6 protons and 7 neutrons Element F has 7 protons and 7 neutrons DIFFERENT ELEMENT!!! 2. Element J has 27 protons and 32 neutrons Element L has 27 protons and 33 neutrons ISOTOPE!!!

22. Review 3.Element X has 17 protons and 18 neutrons Element Y has 18 protons and 17 neutrons DIFFERENT ELEMENT! 4. Element Q has 56 protons and 81 neutrons Element R has 56 protons and 82 neutrons ISOTOPE!!

23. Review 5. Element T has an atomic number of 20 and an atomic mass of 40. Element Z has 20 protons and an atomic mass of 41. ISOTOPE!!!

24. Review 6. Element W has 8 protons and 8 neutrons. Element V has 7 protons and 8 neutrons. DIFFERENT ELEMENTS!

25. Review 7. Element P has an atomic number of 92 and an atomic mass of 238. Element S has 92 protons and 143 neutrons. ISOTOPES!!!

26. Color and Answer: Understanding Periodic Table Sheet Ions, Periodic Table, Metals, Nonmetals and Metalloids Monday, November 21, 2011 (B) Tuesday, November 22, 2011 (A) Page 59 Warm Up: 1. Complete the “check for understanding” at your table in the plastic sheet. Page 60 Homework: Color and Answer: Understanding Periodic Table Sheet Monday, November 21, 2011 (B) Tuesday, November 22, 2011 (A)

27. All atoms aren’t neutral Ions Atoms that have lost or gained an electron Lose an electron = overall positive charge Gain an electron = overall negative charge

28. Take a Closer Look Let’s see how Sodium (Na) becomes an ion Start with 11 electrons Neutral One valence Lose one electron Now there are 11 protons and 10 electrons Overall positive charge

29. Now Chlorine (Cl) Chlorine = atomic # 17 17 electrons and protons When chlorine bonds with Sodium, Chlorine gains an electron One extra electron (-) Now there are more electrons than protons Overall negative charge

30. Study for Quiz on Atomic Structure and Periodic Table Metals, Nonmetals, and Metalloids Notes Monday, November 28, 2011 (B) Tuesday, November 29, 2011 (A) Page 61 Warm Up: 1.Turn to page 35 of Unit D and Complete the following sections of your Chapter Review: #’s 1-3, 5 and 8-18 (you need to write the question for 8-18!) Page 62 Homework: Study for Quiz on Atomic Structure and Periodic Table Monday, November 28, 2011 (B) Tuesday, November 29, 2011 (A)

31. Understanding the Periodic Table