2. Unit 2 Chapter 4 Day 1 OBJECTIVE : Explain how the Study of Atoms has changed in the last century and identify subatomic particles Do Now: The Elements in the Body – a graph TURN IN: Current Events Today: Chapter 4 Notes – Part 1 Atoms and Atomic Structure Thomson’s and Rutherford’s experiments P-N-E worksheets Homework: Read Chapter 4.1 & complete 4.1 GRWS New Chapter New Notebook

3. Unit 2 Chapter 4 Day 2 OBJECTIVE : Explain how the Study of Atoms has changed in the last century and identify subatomic particles Do Now: The Atom – Graphic Organizer Today: Homework check and review 4.1 GRWS More P-N-E practice What is Matter? Video: Bill Nye-Atoms & Molecules Chapter 4 Notes – Part 2 Ions, Isotopes and Excited Electrons Homework: Chapter 4.2 GRWS

4. Unit 2 Chapter 4 Day 3 OBJECTIVE : Discuss variations of atoms and Investigate the structural differences of hydrogen isotopes Do Now: Atoms and Parts crossword puzzle Today: Homework check and review 4.2 GRWS Finish Chapter 4 Notes – Part 2 Ions, Isotopes and Excited Electrons LAB: Modeling Isotopes of Hydrogen R & R Structure of the Atom Homework: Finish R & R

5. Unit 2 Chapter 4 Day 4 OBJECTIVE : Construct and interpret Bohr’s models and Lewis dot diagrams for multiple elements Do Now: What happens to Carbon if… TURN IN HOMEWORK Today: Return Unit 1 Test – Corrections Due TOMORROW Intro - Chemistry Unit Project - Due Date = 4/1/15 Bohr and Lewis - Electron Models of the Atom “Bohr”ing practice and Making Lewis Dot Diagrams Homework: Advertise-the-Elements project – Select your Elements! Read Chapter 4.3 & complete GRWS Progress Reports signed

6. Unit 2 Chapter 4 Day 5 OBJECTIVE : Construct and interpret Bohr’s models and Lewis dot diagrams for multiple elements. Do Now: Word Wise Chapter 4 What are YOUR Elements? Today: Homework check and Review 4.3 GRWS Element Practice What Atom am I? Review Bohr’s /Lewis Models LAB: Modeling the Location of an Electron in a Cloud Homework: Textbook Chapter 4 Assessment pg 121+ #1 – 32 Complete sentences

7. PARCC BREAK 5 days of PARCC testing – no instructional classes!

8. Unit 2 Chapter 4 Day 6 OBJECTIVE : Demonstrate understanding of atomic structure basics. Do Now: Chapter Assessment Homework Check and Review Today: Atomic Basics – Chapter 4 Quiz Homework: Everyday Elements! Advertise-the-Elements project Due 4/1/15 POP

10. Chapter 4 ATOMS and AtomicStructure

11. Matter The term matter describes all of the physical substances around us: your table, your body, a pencil, water, and so forth Anything that has mass and takes up space (has volume) Made up of different kinds of atoms Includes all things that can be seen, tasted, smelled, or touched

12. Matter is made of atoms

14. Models Models are often used for things that are too small or too large to be observed or that are too difficult to be understood easily

15. Early Models of the Atom Democritus Universe was made of empty space and tiny bits of stuff Called these tiny bits of stuff atomos Atoms could not be divided

16. Early Models of the Atom Dalton All elements are composed of indivisible particles. Atoms of the same element are the same Atoms of different elements are different. Compounds consisted of atoms of different elements combined together

17. Early Models of the Atom Thomson Plum pudding model Atom made of a positively charged material with the negatively charged electrons scattered through it. He discovered the ELECTRON!

19. Early Models of the Atom Rutherford Mostly empty space Small, positive nucleus Contained protons Negative electrons scattered around the outside He discovered the PROTON!

21. Early Models of the Atom Bohr Atom as a planetary arrangement Electrons move in definite orbits around the nucleus

22. Modern Model of the Atom The Electron Cloud Sometimes called the wave model Spherical cloud of varying density Shows where an electron is more or less likely to be (quantum mechanics)

23. Atomic Structure Nucleus –Protons –Neutrons Electrons

24. Tiny, very light particles Have a negative electrical charge (-) Move around the outside of the nucleus Always moving – can move in any direction within their shell Is equal to the number of protons

25. Protons Much larger and heavier than electrons Protons have a positive charge (+) Located in the nucleus of the atom Identifies the Atomic Number Made up of smaller particles called quarks

27. Neutrons Large and heavy like protons –1840 times the mass of an electron Neutrons have no electrical charge Located in the nucleus of the atom Made up of smaller particles called quarks

28. Describing Atoms Atomic Number = number of protons Mass Number = number of protons plus neutrons. Atomic Mass (or Weight) = average mass of the naturally occurring isotopes of an element. In a neutral atom, the # of protons = # of electrons

29. 5678 BCNO 11121416 BoronCarbonNitrogenOxygen 13141516 AlSiPS 27283132 AluminumSiliconPhosphorusSulfur

31. Chapter 4 Atoms and Atomic Structure Part 2

32. Ions An atom that carries an electrical charge is called an ion –The number of protons does not change in an ion –The number of neutrons does not change in an ion SO…both the atomic number and the atomic mass remain the same

33. Ions If the atom loses electrons, the atom becomes positively charged (because the number of positively charged protons will be more the number of electrons) If an atom gains electrons, the atom becomes negatively charged (more negative charges than positive charges)

34. Ions This atom has lost an electron. Now it has one more proton than electron. One more proton means one more positive charge. This makes the total charge of the atom POSITIVE. This atom has gained an electron. Now it has one less proton than electron. One less proton means one less positive charge. This makes the total charge of the atom NEGATIVE.

35. Isotopes Have the same atomic number (number of protons) The number of protons for a given atom never changes. The number of neutrons can change. Two atoms with different numbers of neutrons are called isotopes Have different atomic mass numbers (number of protons + neutrons)

36. Three Isotopes of Hydrogen

37. Write symbols for each of the three Isotopes of Hydrogen? H H H Protium Deuterium Tritium

38. Isotopes

39. Add or Subtract a PROTON NEW ELEMENT Add or Subtract a NEUTRON ISOTOPE Add or Subtract an ELECTRON ION

40. Atomic Orbitals An orbital is the region of space around the nucleus where an electron is likely to be found The electron cloud model approximates how electrons behave in their orbitals.

41. Electrons and Energy Levels Each electron in an atom has a specific amount of energy Possible energies that electrons can have in an atom are called energy levels An electron can move from one energy level to another when the atom gains or loses energy

42. Electron Configuration Electron configuration is the specific arrangement of electrons in orbitals. –Each energy level can only hold a specific amount of electrons –Each energy level must be completely filled before electrons fill the next level The number of electrons in the outermost level are called valence electrons –These are the electrons used for bonding!

43. Electron Diagrams Bohr and Lewis

44. Bohr’s Model of the Atom

45. Rules for filling the model –Start at the lowest energy level 1 st energy level = 2 electrons (electrons #1 and 2) Place them opposite each other 2 nd energy level = 8 electrons (electrons #3 to 10) Place them opposite each other -and- Make pairs for easier counting 3 rd energy level = 18 electrons (electrons #11 to 28) Bohr’s Model of the Atom

46. ELEMENT _____________ # Protons ________ # Neutrons ________ Bohr’s Model of the Atom ELEMENT _____________ # Protons ________ # Neutrons ________

47. Lewis Dot Structures Lewis dot diagrams are a simple way to show how the electrons are arranged in their outer shell. This is where chemical reactions take place and how elements bond together.

48. Lewis Dot Structures Rules for filling the model: ONLY VALENCE ELECTRONS ARE USED 2 3 1 4 WHAT ARE VALENCE ELECTRONS ?

49. Lewis Dot Structures VALENCE ELECTRONS are the electrons found in the OUTERMOST shell of the Bohr’s model. ELEMENT _____________ # electrons (total) _______ # Valence electrons _______ ELEMENT _____________ # electrons (total) _______ # Valence electrons _______ ELEMENT _____________ # electrons (total) _______ # Valence electrons _______

50. Lewis Dot Structures Rules for filling the model: ONLY VALENCE ELECTRONS ARE USED 2 3 1 4

51. Lewis Dot Structures

52. Advertise-the-Elements General Information Due date is Wed 4/1 at the beginning of class…Not after you finish gluing this on, or tying that together…Nor after you borrow my scissors and tape…NO…you must walk in here with it ready to turn in or it will be LATE! (Projects turned in after Spring Break cannot earn more than 50% credit MAX) The Unit Project is worth as much as the Unit Test. Make that work for you.

54. Internet Sources Wikipedia (or Wiki-anything) is NOT an acceptable scientific source for this project and cannot be used as a source. Cost for elements can be found on various sites. Try: Periodic Table of Elements: Los Alamos National Laboratory at http://periodic.lanl.gov/http://periodic.lanl.gov/ OR even places like… http://www.elementsales.com/pl_element.htm

55. Cool interactive periodic tables can be found at lots of sites…Try: http://www.chemicalelements.com/ http://elements.wlonk.com/ElementUses.htm http://www.chemicalelements.com/ http://elements.wlonk.com/ElementUses.htm http://education.jlab.org/itselemental/ Repeat…wiki-ANYTHING is not acceptable Try searching for your element in Science Journals. You could find innovative uses and new discoveries.