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Do Now: What is Matter? TURN IN Current Events – Bigfoot Today :

Thursday 3/20/14. New Chapter New Notebook. Do Now: What is Matter? TURN IN Current Events – Bigfoot Today : Video – Bill Nye, Atoms & Molecules Class read 4.1 & 4.1 GRWS Homework : Complete 4.1 GRWS.

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Do Now: What is Matter? TURN IN Current Events – Bigfoot Today :

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  1. Thursday 3/20/14 New Chapter New Notebook • Do Now: • What is Matter? • TURN IN Current Events – Bigfoot • Today: • Video – Bill Nye, Atoms & Molecules • Class read 4.1 & 4.1 GRWS • Homework: • Complete 4.1 GRWS Unit 2 Chapter 4 Day 1 OBJECTIVE: Explain how the Study of Atoms has changed in the last century

  2. Friday 3/21/14 • Do Now: • The Elements in the Body – a graph • Today: • Chapter 4 Notes – Part 1 Atoms and Atomic Structure • P-N-E worksheets • Homework: • Missing Assignments? • Enjoy the weekend! Unit 2 Chapter 4 Day 2 OBJECTIVE: Identify subatomic particles and distinguish the atomic number and mass of an element

  3. Monday 3/24/14 2 hour delay • Do Now: • The Atom – Graphic Organizer • Today: • More P-N-E practice • Thomson’s and Rutherford’s experiments • Chemistry Unit Project Intro- Due Date Fri 4/4 • Chapter 4 Notes – Part 2Ions, Isotopes and Excited Electrons • Homework: • Read Chapter 4.2 & 4.2 GRWS • Advertise-the-Elements project Due Fri 4/4 Unit 2 Chapter 4 Day 3 OBJECTIVE: Identify subatomic particles and distinguish the atomic number and mass of an element

  4. Tuesday 3/25/14 • Do Now: • Atoms and Parts crossword puzzle • Today: • Finish Chapter 4 Notes – Part 2 Ions, Isotopes and Excited Electrons • What happens to Carbon if… • Modeling Isotopes Activity • Homework: • R & R Structure of the Atom • Advertise-the-Elements project Due Fri 4/4 Unit 2 Chapter 4 Day 4 OBJECTIVE: Discuss variations of atoms and Investigate the structural differences of hydrogen isotopes

  5. Wednesday 3/26/14 • Do Now: • Element Word Find • Today: • Bohr’s Model of the Atom • “Bohr”ing practice • Constructing a Lewis Dot Diagram • Homework: • Read Chapter 4.3 & Complete 4.3 GRWS • Advertise-the-Elements project Due Fri 4/4 Unit 2 Chapter 4 Day 5 OBJECTIVE: Construct and interpret Bohr’s models and Lewis dot diagrams for multiple elements

  6. Thursday 3/27/14 • Do Now: • Word Wise Chapter 4 • Today: • Chemistry Unit Project • Atomic Basics Review • Modeling the Location of an Electron Lab • Homework: • Finish Electron Cloud Lab • Advertise-the-Elements project Due Fri 4/4 Unit 2 Chapter 4 Day 6 OBJECTIVE: Demonstrate understanding of atomic structure basics. Model the Electron Cloud using probability.

  7. Chapter 4 ATOMS and AtomicStructure

  8. 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

  9. Matter is made of atoms

  10. 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

  11. Early Models of the AtomDemocritus • Universe was made of empty space and tiny bits of stuff • Called these tiny bits of stuff atomos • Atoms could not be divided

  12. Early Models of the AtomDalton • 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

  13. Early Models of the AtomThomson • Plum pudding model • Atom made of a positively charged material with the negatively charged electrons scattered through it.

  14. Early Models of the AtomRutherford • Mostly empty space • Small, positive nucleus • Contained protons • Negative electrons scattered around the outside

  15. Early Models of the AtomBohr • Atom as a planetary arrangement • Electrons move in definite orbits around the nucleus

  16. Modern Model of the AtomThe 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)

  17. Atomic Structure • Nucleus • Protons • Neutrons • Electrons

  18. Atomic Structure • Electrons • 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

  19. Atomic Structure • 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

  20. Atomic Structure • 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

  21. Atomic Structure

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

  23. Chapter 4 Atoms andAtomic Structure • Part 2

  24. 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

  25. 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)

  26. 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.

  27. 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)

  28. Isotopes

  29. 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.

  30. 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

  31. 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!

  32. Bohr’s Model of the Atom

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

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

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

  36. Lewis Dot Structures • Rules for filling the model: ONLYVALENCE ELECTRONS ARE USED 2 • 1 4

  37. Lewis Dot Structures

  38. Advertise-the-ElementsGeneral Information • Due date is Wed 10/30 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! • The Unit Project is worth as much as the Unit Test. Make that work for you.

  39. 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/ OR even places like… http://www.elementsales.com/pl_element.htm

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

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