2. Catalyst 1.What would J.J. Thomson say to Dalton to prove that his plum pudding model is superior? 2.What would Ernest Rutherford say to J.J. Thomson to prove that his atomic model is superior? 3.What would Niels Bohr say to those other dead white guys to prove that his orbiting model is the superior? End

4. Review - Important Point #1 The atom is mostly empty space. This is why most of the alpha particles went through The majority of the atom does not have anything in it.

5. Review - Important Point #2 The atom has very small, but very dense nucleus. Alpha particles that bounced back were coming into contact with nucleus. Alpha particles were deflected back because nucleus is positive.

7. Lecture 1.9 – Bohr’s Electron Shells

8. Today’s Learning Targets 1.15 – I can define atomic/ionic radius and explain how it relates to the charge of the nucleus and the electron. Furthermore, I can explain how this trend changes as you move throughout the Periodic Table.

9. Niels Bohr Refined Rutherford’s model of the atom with his discovery in 1913.

12. What Bohr Knew Shooting electricity through the hydrogen excited electrons. Color produced only for specific values Problem – If electrons were free to roam, then we should get all sorts of colors

14. Bohr’s Solution Electrons are not free to roam in the electron cloud, electrons are restricted to orbits or energy levels.

15. The Modern Model Rutherford ’ s space and nucleus Dalton ’ s atom Bohr ’ s energy levels Thompson ’ s electrons

16. SUMMARIZE

17. Magnets! How do they work?

18. Nuclear Attraction The negatively charged electrons are attracted towards the positively charged nucleus. The negatively charged electrons are attracted towards the positively charged nucleus. The more the electron “feels” the nucleus. The tighter it is held The more the electron “feels” the nucleus. The tighter it is held

19. What do the arrows represent? How does the thickness of the arrows relate to nuclear attraction? How does the size of the atom relate to the positive and negative charges in an atom?

20. a As you move from the smallest atom to the largest atom, how does the distance between the valence electrons and the nucleus change? As you move from the smallest atom to the largest atom, how does the attractive force between the valence electrons and the nucleus change? What direction does this go on the periodic table? Why are the atoms getting bigger?

21. Stop and Jot Order the elements from smallest to largest IE: phosphorus, arsenic, nitrogen.

22. SUMMARIZE

23. Master Chef - White Board Races

24. White Board Relay Race Problems 1.Which has a larger atomic radius: chlorine or silicon? 2.Which has a smaller atomic radius magnesium or calcium? 3.Put the following elements in order from smallest atomic radius to largest: B, F, N, O. 4.Put the following elements in order from smallest atomic radius to largest: N, As, Bi, P. 5.Why does bromine do a worse job of attracting electrons than fluorine?

25. Atomic Radius Atomic Radius – The distance from the center of the nucleus to the outermost edge of the electron cloud Outer edge of electron cloud Nucleus

26. Atomic Radius Trends Atomic radius increases as you go down a group on the Periodic Table. Atomic radius decreases as you go across a period on the Periodic Table

27. Why Atomic Radius Increases Down a Group As you add more electron shells to an element, the element becomes “bulkier”. This means that as you go down a group, more orbits are added, so the radius becomes bigger.

28. Why Atomic Radius Decreases Across a Period As you move across a period, more protons are added to the nucleus. Also, more electrons are added within the same orbit. This means there is a larger positive and negative charge, which results in a higher attraction and a decrease in the radius.

30. SUMMARIZE

31. Master Chef - White Board Races

32. Whiteboard Questions (T/F) 1.Atomic radius is the distance from the center of the nucleus to the first electron orbit. 2.Atomic radius increases across a period and down a group. 3.Atomic radius decreases down a group because you are adding more electron orbits. 4.Atomic radius decreases across a period because there are less electrons in the same orbit.

33. Whiteboard Questions (cont) 5. Order the following from largest to smallest atomic radius: Ca, Se, Ni - Answer: Se, Ni, Ca 6. Order the following from largest to smallest atomic radius: O, Po, S - Answer: O, S, Po 7. Order the following from smallest to largest atomic radius: Cs, F, Ga - Answer: F, Ga, Cs

34. Exit Ticket 1. Define atomic radius 2. Define electronegativity. 3. Order from largest to smallest electronegativity: Ca, Se, Ni 4. Order from smallest to largest atomic radius: O, Po, S

35. Rate Yourself Based on the exit ticket and your current level of understanding, rate yourself 1 – 4 on LT 1.8 and 1.9

37. Closing Time 1.9 – Electronegativity and Atomic Radius UNIT 1 EXAM Thursday/Friday (9/19/2014)!