1. Tuesday Oct 14 Objective: Describe different models of the atom. Checkpoint: Draw a picture of a copper atom, including electrons in the correct energy levels. Does copper want to gain or lose electrons to be come stable? What ion will it form when it does this to become stable? HW: Study for Nuclear Chem re-take exam on Wednesday (after school), 12:30 PM Read pp 104-108 in book (Section 4.2) Answer questions 8-14 on pp 108. Due Friday.

2. Copper 29 p 35 n

3. Copper 29 p 35 n Cu 2+

4. Nuclear Chem make-up exam Wednesday 12:30 PM

6. Ba(NO 3 ) 2 Ca(NO 3 ) 2 Cu(NO 3 ) 2 Pb(NO 3 ) 2 LiNO 3 KNO 3 NaNO 3 Sr(NO 3 ) 2 Yellow/Green Orange Green/Blue Light blue Red Pink/Purple Bright yellow Orange/Red

7. CuSO 4 Cu(NO 3 ) 2

8. Cu Cu 2+

9. 9 Thomson Model Created the “Plum-pudding model” Electrons are surrounded by a sea of evenly distributed positive charge

10. 10 Rutherford Model Small, dense, positive nucleus surrounded by cloud of electrons

11. 11 Bohr Model Proposed that electrons orbit the nucleus in a fixed, circular path Orbit path has specific energy that prevents electrons from falling into the nucleus Quantum of energy is the amount of energy needed to move an electron between energy levels

12. 12 Bohr Model Picture

13. 13 Erwin Schrödinger Quantum Mechanical Model – Modern model – Estimates the probability of finding an electron within a certain volume of space surrounding the nucleus – Where you find the electron 90% of the time

14. 14 Electron Cloud Picture

15. 15 Energy Levels - 1 Electrons exist within energy levels or shells – General location around the nucleus where the electron is moving – Energy levels are not equally spaced apart, they become more tightly packed the farther you get from the nucleus

16. 16 Energy Levels - 2 Principal quantum numbers (n) identify the energy levels in an atom – Tells you how far away the electron is from the nucleus – There are 1-7 energy levels, correlates with period numbers – Each level has same n number of sublevels – Maximum number of 2n 2 electrons per level

17. 17 Atomic Orbitals - 1 Atomic orbitals are more specific regions within each energy level where electrons are found – Highest probability of finding an electron – Also called sublevels, subshells, azimuthal quantum number, or angular momentum quantum number (l) Number of orbitals for each energy level equals n 2

18. 18 Atomic Orbitals - 2 Sublevels are designated by letters – s,p,d,f Each sublevel has a unique shape and number of orbitals related to different spatial orientations Each sublevel orbital can hold a maximum of 2 electrons

19. 19 Orbital Shapes

20. Orbital Shapes cont.

21. 21 Summary Each principal energy level consists of one or more sublevels and each sublevel consists of one or more orbitals Orbitals  Sublevels  Energy Level

22. Thought of the Week The joy of life comes from our encounters with new experiences, and hence there is no greater joy than to have an endlessly changing horizon, for each day to have a new and different sun. Christopher McCandless