1. Electrons determine chemical behavior 2/24/14 2/24 Periodic Trends WB. 35-36 2/25 Electron Configuration WB: p 43-44 TB: 51-53HW: TB p.56 #4 a-f 2/26 Electron Configuration WB: p. 44-47 2/27 Valence Electrons WB: p. 48-50 HW: TB p. 66 # 4 a-f 2/28 Valence Electrons TB p. 51-53/ quiz

2. Date: 2/24/14Objective: I can explain atomic radius, electronegativity, and ionization energy and how they are connected. Bell Ringer: 1.Define ionization energy. 2.Why is the 2 nd ionization energy higher than the 1 st ionization energy?

3. Date: 2/24/14Objective: I can explain atomic radius, electronegativity, and ionization energy and how they are connected. Take out your note book Title :Notes 3/6

4. Date: 2/24/14Objective: I can explain atomic radius, electronegativity, and ionization energy and how they are connected Notes 2/24 Chemical groups – are the vertical columns Periods- are the horizontal rows

5. As we move from left to right in a period, the ionization energy increases As we move up a chemical group, the ionization energy increases

6. Bohr Models of atoms are drawings of atoms that identify the proton and neutrons in the nucleus and electrons in their energy levels (shell and orbits).

7. Notes 3/6 Bohr Models of atoms are drawings of atoms that identify the proton and neutrons in the nucleus and electrons in their energy levels (orbits). What atom?Draw K

8. Date: 2-25-14Objective: I can relate the position of elements on the periodic table with their electron arrangement. Bell Ringer 1. Which pair of elements has the most similar chemical properties? – Cl and Ar -K and N - Li and Na-C and Ca 2. Draw a Bohr Model of an Aluminum atom

9. Bohr Model of Atoms

10. Notes 2/25 Atomic Radius is the distance from the center of the atom to its furthest energy level.

11. Atomic Radius

12. Date: 3-11-13Objective: I can relate the position of elements on the periodic table with their electron arrangement. Bell Ringer 4. What is the total number of electrons in an atom of an element with an atomic number of 18 and a mass number of 40? 5. Which substance can be broken down by a chemical change? – Na - NH 3 - K - Mg 3.How do the charge and mass of an electron compare to the charge and mass of a proton?

13. Oxygen Electron Configuration1s 2 2s 2 2p 4 1 1 s value of energy level sublevel no. of electrons spdf NOTATION for H, atomic number = 1

14. 1 1 s value of energy level sublevel no. of electrons spdf NOTATION for H, atomic number = 1

15. Outer electron configuration for the elements

17. Date: 2-26-14Objective: I can relate the position of elements on the periodic table with their electron arrangement and their distance from the nearest noble gas. Fill in the blank periodic table Label each element 1- 36 Atomic number Atomic symbol Atomic mass

18. Date: 3-12-13Objective: I can relate the position of elements on the periodic table with their electron arrangement and their distance from the nearest noble gas. Workbook page 44-45 Complete page 44-45 #2-3a with your shoulder partner. Partner A completes information for one element and Partner B completes information for the next element. When you both finish, share your answers. Then go on to the next two elements using the same process.

19. Date: 3-12-13Objective: I can relate the position of elements on the periodic table with their electron arrangement and their distance from the nearest noble gas. Class discussion about p. 44-45 Next, complete page 46-47 #3b-4c with your shoulder partner. Partner A completes information for one element and Partner B completes information for the next element. When you both finish, share your answers. Then go on to the next two elements using the same process.

20. Date: 3-12-13Objective: I can relate the position of elements on the periodic table with their electron arrangement and their distance from the nearest noble gas. Class discussion about p. 46-47 Next, complete page 48-49 #4d-5h with your shoulder partner. Partner A completes information for one element and Partner B completes information for the next element. When you both finish, share your answers. Then go on to the next two elements using the same process.

21. Date: 3-13-13Objective: I can assign valence numbers to elements and organize the periodic table to valence numbers Bell Ringer- ACT practice handout Answer questions #14-17 on your bell ringer sheet

22. Date: 3-13-13Objective: I can assign valence numbers to elements and organize the periodic table to valence numbers Class discussion about p. 46-47 Next, complete page 48-49 #4d-5h with your shoulder partner. Partner A completes information for one element and Partner B completes information for the next element. When you both finish, share your answers. Then go on to the next two elements using the same process.

23. Date: 3-13-13Objective: I can assign valence numbers to elements and organize the periodic table to valence numbers Read workbook page 51-52 and take cornell notes

24. Date: 3-15-13Objective: I can assign valence numbers to elements and organize the periodic table to valence numbers Bell ringer Write the electron configuration and draw the Bohr model for Fluorine

26. General Periodic Trends Atomic and ionic size Atomic and ionic size Ionization energy Ionization energy Electron affinity Electron affinity Higher effective nuclear charge. Electrons held more tightly Smaller orbitals. Electrons held more tightly.

27. Atomic Size Size goes UP on going down a group. Size goes UP on going down a group. Because electrons are added farther from the nucleus, there is less attraction. Because electrons are added farther from the nucleus, there is less attraction. Size goes DOWN on going across a period. Size goes DOWN on going across a period. Size goes UP on going down a group. Size goes UP on going down a group. Because electrons are added farther from the nucleus, there is less attraction. Because electrons are added farther from the nucleus, there is less attraction. Size goes DOWN on going across a period. Size goes DOWN on going across a period.

28. Atomic Radii Figure 8.9

29. Trends in Atomic Size See Figures 8.9 & 8.10

30. Electron Configurations The electron configuration of an atom is a shorthand method of writing the location of electrons by sublevel. The sublevel is written followed by a superscript with the number of electrons in the sublevel. – If the 2p sublevel contains 2 electrons, it is written 2p 2

31. Writing Electron Configurations First, determine how many electrons are in the atom. Iron has 26 electrons. Arrange the energy sublevels according to increasing energy: – 1s 2s 2p 3s 3p 4s 3d … Fill each sublevel with electrons until you have used all the electrons in the atom: – Fe: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 The sum of the superscripts equals the atomic number of iron (26)

32. The periodic table can be used as a guide for electron configurations. The period number is the value of n. Groups 1A and 2A have the s-orbital filled. Groups 3A - 8A have the p-orbital filled. Groups 3B - 2B have the d-orbital filled. The lanthanides and actinides have the f-orbital filled. Electron Configurations and the Periodic Table

33. Valence Electrons When an atom undergoes a chemical reaction, only the outermost electrons are involved. These electrons are of the highest energy and are furthest away from the nucleus. These are the valence electrons. The valence electrons are the s and p electrons beyond the noble gas core.

34. Predicting Valence Electrons The Roman numeral in the American convention indicates the number of valence electrons. – Group IA elements have 1 valence electron – Group VA elements have 5 valence electrons When using the IUPAC designations for group numbers, the last digit indicates the number of valence electrons. – Group 14 elements have 4 valence electrons – Group 2 elements have 2 valence electrons

35. Electron Dot Formulas An electron dot formula of an elements shows the symbol of the element surrounded by its valence electrons. We use one dot for each valence electron. Consider phosphorous, P, which has 5 valence electrons. Here is the method for writing the electron dot formula.

36. Ionic Charge Recall, that atoms lose or gain electrons to form ions. The charge of an ion is related to the number of valence electrons on the atom. Group IA/1 metals lose their one valence electron to form 1+ ions. – Na → Na + + e - Metals lose their valence electrons to form ions.

37. Predicting Ionic Charge Group IA/1 metals form 1+ ions, group IIA/2 metals form 2+ ions, group IIIA/13 metals form 3+ ions, and group IVA/14 metals from 4+ ions. By losing their valence electrons, they achieve a noble gas configuration. Similarly, nonmetals can gain electrons to achieve a noble gas configuration. Group VA/15 elements form -3 ions, group VIA/16 elements form -2 ions, and group VIIA/17 elements form -1 ions.

38. Ion Electron Configurations When we write the electron configuration of a positive ion, we remove one electron for each positive charge: Na → Na + 1s 2 2s 2 2p 6 3s 1 → 1s 2 2s 2 2p 6 When we write the electron configuration of a negative ion, we add one electron for each negative charge: O → O 2- 1s 2 2s 2 2p 4 → 1s 2 2s 2 2p 6

39. Conclusions Continued We can Write the electron configuration of an element based on its position on the periodic table. Valence electrons are the outermost electrons and are involved in chemical reactions. We can write electron dot formulas for elements which indicate the number of valence electrons.

40. Conclusions Continued We can predict the charge on the ion of an element from its position on the periodic table.

42. (c) 2007 brainybetty.com ALL RIGHTS RESERVED. 42 Electron configurations-ways electrons arranged around nuclei Aufbau principle- each electron occupies lowest energy orbital available