1. Chapter 1 Section 6 Atoms with More than One Electron

2. February 1, 2012 HW: 1.6 CTG p. 57 #1-8, Due Monday LO Graph the ionization energies of the first 36 elements. Use electron configurations to describe the number of electrons around an atom. SC View the spectra of various materials. Graphically analyze patterns in the amounts of energy required to remove electrons from different kinds of atoms. Compare trends in stability of atoms in the periodic table. Compare the structure of the periodic table with the patterns of levels and sublevels to which electrons can be assigned. Develop a shorthand notation to describe the configuration of electrons in an atom. Do Now: 1.4 & 1.5 Honors 1.5 Quiz Copy LO and SC WDYS, WDYT p. 46 Agenda: WDYS, WDYT Investigation Chem Talk Summary Quiz

3. Investigate 1) Teacher will demo the spectra of a few elements, you should complete number 1 for each of them!

4. Investigate Read through number 2 Graph paper will be provided, you will be expected to plot the 1 st and 2 nd ionization energies on the graph paper.

5. February 3, 2012 HW: 1.6 CTG p. 57 #1-8 LO Graph the ionization energies of the first 36 elements. Use electron configurations to describe the number of electrons around an atom. SC View the spectra of various materials. Graphically analyze patterns in the amounts of energy required to remove electrons from different kinds of atoms. Compare trends in stability of atoms in the periodic table. Compare the structure of the periodic table with the patterns of levels and sublevels to which electrons can be assigned. Develop a shorthand notation to describe the configuration of electrons in an atom. Do Now: Finish graphing ionization energies-pg. 47 What are ionization energies? Are there any trends on the periodic table? If so, describe them. Agenda: Investigation Chem Talk Summary Quiz

7. Investigate Complete numbers 3- 5 as a class. ▫Be sure to answer all of the questions!

8. Investigate Read through numbers 6 and 7 and complete them, answering all of the questions as a class! ▫This part is very important.

9. Blank Periodic Table Fill in and color code orbitals

11. Chem Talk Take 5 minutes and skim through the chem talk ▫You do not have to take notes!

12. Chem Notes What is ionization energy? What is an ion?

13. Chem Notes What is ionization energy? What is an ion? The amount of energy required to remove an electron from an atom.

14. Chem Notes What is ionization energy? What is an ion? The amount of energy required to remove an electron from an atom. Atoms that have lost or gained electrons: Na + energy  Na + + e -

15. Chem Notes What is the first ionization energy? What is the second ionization energy?

16. Chem Notes What is the first ionization energy? What is the second ionization energy? Energy required to remove the first electron from the atom: Ca + energy  Ca + + e -

17. Chem Notes What is the first ionization energy? What is the second ionization energy? Energy required to remove the first electron from the atom: Ca + energy  Ca + + e - Energy Required to remove the second electron from the atom: Ca + + energy  Ca 2+ + e -

18. Chem Notes Which electron is harder to remove, the first or second? Why?

19. Chem Notes Which electron is harder to remove, the first or second? Why? The Second! The second electron is closer to the nucleus (more tightly bound), therefore since there is greater magnetic attraction to the positive nucleus, it is harder. The second ionization energy is ALWAYS harder

20. Chem Notes What is the periodic trend for atomic radius? What is the periodic trend for ionization energy?

21. Chem Notes What is the periodic trend for atomic radius? What is the periodic trend for ionization energy? As you go up and to the right, the radius decreases Since atoms are more tightly bound as radius decreases, it becomes more difficult to remove the electron Therefore, up and to the right, IE increases

22. Radius Decreases, IE Increases

23. Date: HW: CTG p. 57 #1-8 LO Graph the ionization energies of the first 36 elements. Use electron configurations to describe the number of electrons around an atom. SC View the spectra of various materials. Graphically analyze patterns in the amounts of energy required to remove electrons from different kinds of atoms. Compare trends in stability of atoms in the periodic table. Compare the structure of the periodic table with the patterns of levels and sublevels to which electrons can be assigned. Develop a shorthand notation to describe the configuration of electrons in an atom. Do Now: Which element has a bigger radius: As or At? Why? Agenda: Chem Talk Summary Quiz

24. Chem Notes What is an electron configuration? What are the 4 sublevels?

25. Chem Notes What is an electron configuration? What are the 4 sublevels? The arrangement of electrons around a given atom s, p, d, and f

26. Chem Notes Rule 1: The first energy level has only one type of orbital, labeled 1s, where 1 identifies the energy level and s identifies the orbital.

27. The s-orbital:

28. 1 st energy level

29. Chem Notes Rule 2: The second energy level has two types of orbitals (an s orbital and p orbitals) which are labeled the 2s and 2p orbitals.

30. The p-orbitals

31. Chem Notes Rule 3: The third energy level has three types of orbitals (an s orbital, p orbitals, and d orbitals) and are labeled as the 3s, 3p, and 3d orbitals

32. The d-orbitals

33. Chem Notes Rule 4 The number of orbitals corresponds to the energy level you are considering. For example: 4 th energy level has 4 types of orbitals (s, p, d, and f) 5 th energy level has 5 types of orbitals (s, p, d, f, g)

34. Chem Notes Rule 5 The s orbital has a maximum of 2 electrons The d orbital has a maximum of 6 electrons The number of electrons is indicated by a superscript following the orbital designation. Ex: 2p 5 means that there are five electrons in the p- orbitals in the 2 nd energy level. 1s 2 means that there are 2 electrons in the s-orbital of the 1 st energy level.

35. Chem Notes Electrons are placed into the lowest energy levels first and then ‘built up’ from there. Ex: Carbon has 6 electrons. 2 electrons are in the 1 st energy level, s-orbital: 1s 2 2 electrons are in the 2 nd energy level, s-orbital: 2s 2 2 electrons are in the 2 nd energy level, p-orbital: 2p 2 So, finally: 1s 2 2s 2 2p 2

36. Chem Notes The electron configuration for argon (Ar with 18 electrons) is:

37. Chem Notes The electron configuration for argon (Ar with 18 electrons) is: 1s 2 2s 2 2p 6 3s 2 3p 6

38. Chem Notes The electron configuration for argon (Ar with 18 electrons) is: 1s 2 2s 2 2p 6 3s 2 3p 6 The electron configuration for arsenic (As, with 33 electrons is)

39. Chem Notes The electron configuration for argon (Ar with 18 electrons) is: 1s 2 2s 2 2p 6 3s 2 3p 6 The electron configuration for arsenic (As, with 33 electrons is) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3

40. Chem Notes The electron configuration for argon (Ar with 18 electrons) is: 1s 2 2s 2 2p 6 3s 2 3p 6 The electron configuration for arsenic (As, with 33 electrons is) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3

41. Chem Notes The electron configuration for argon (Ar with 18 electrons) is: 1s 2 2s 2 2p 6 3s 2 3p 6 The electron configuration for arsenic (As, with 33 electrons is) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3 Becomes: [Ar] 4s 2 3d 10 4p 3

42. Chem Notes What is the ground state? What is the excited state?

43. Chem Notes What is the ground state? What is the excited state? The most stable energy configuration where all electrons are in the lowest orbitals possible An electron of an atom that has absorbed enough energy to be raised into a higher energy sublevel

44. Date: HW: CTG p. 57 #1-8 LO Graph the ionization energies of the first 36 elements. Use electron configurations to describe the number of electrons around an atom. SC View the spectra of various materials. Graphically analyze patterns in the amounts of energy required to remove electrons from different kinds of atoms. Compare trends in stability of atoms in the periodic table. Compare the structure of the periodic table with the patterns of levels and sublevels to which electrons can be assigned. Develop a shorthand notation to describe the configuration of electrons in an atom. Do Now: What is the electron configuration for: Si Be Fe Agenda: Chem Talk Summary Quiz

45. Chem Notes What are the orbitals?

46. Chem Notes What are the orbitals?Probability that you can find the electrons in a given space Hard to determine due to wave and particle behavior This is quantum mechanics! A model (like the think tube!)

47. Chem Notes What is the Heisenberg uncertainty principle You cannot know exactly where an electron is, either its momentum is high and its position is known, or is momentum is known, but the position is unkown…

48. Practice Complete the worksheet on electron configuration and ask for help if needed

49. Summary Essential Questions, p. 55 --How do you know? --Why do you believe --Why should you care LO and SC reflection