2. Electron Energy Level Notes

3. Electrons do not travel around the nucleus of an atom in orbits They are found in ____ ____at different distances away from the nucleus. (kind of like shells or layers). energy levels

4. The Quantum Mechanical Model of the Atom (cont.) The wave function predicts a three-dimensional region around the nucleus called an _______. orbital

5. Hydrogen Atomic Orbitals The ______ _______ ______(n) indicates the relative size and energy of atomic orbitals. principal quantum number n specifies the atom’s major energy levels. Electrons cannot exist between energy levels (just like the rungs of a ladder).

6. Electron Energy Level Notes Energy levels are broken up into sublevels: There are at least 4 possible types of sublevels—given labels: __, __, __,or __. s, p, d, f

7. Hydrogen Atomic Orbitals (cont.) Energy sublevelsEnergy sublevels are contained within the principal energy levels.

8. Energy Levels and Sub-levels d)Ex. Orbitals around the Nucleus of a Neon Atom

9. Electron Energy Level Notes Only a certain number of electrons may exist in an energy level, but the number varies. It can be determined by: # of electrons in level = 2 x (# of energy level) 2 Therefore: energy level 1 = 2 (1) 2 = 2 energy level 2 = 2 (2) 2 = 8 energy level 3 = 18 energy level 4 = 32 etc...

10. Electron Energy Level Notes In each energy level, electrons fill sublevels in a certain order Level 1: only has one s sublevel (a spherical shape) 2 electrons may fit in this sublevel--each one has an opposite “spin”, allowing them to take up the same space Pauli exclusion principle—no more than 2 electrons may be found in the same orbital (“orbital” means a particular location)

11. s-Orbital Image

12. Electron Energy Level Notes Level 2: has two sublevels: s and p 2 electrons in s there are 3 different p orbitals, and may hold 2 electrons each—6 total. total of 8 overall in Level 2

13. p-Orbital Image

14. Electron Energy Level Notes Level 3: has 3 sublevels: s, p, and d 2 electrons in s 6 electrons in p there are 5 different d orbitals, and 2 electrons can fit in each—total of 10. (look at picture of d orbitals, imagine how they can fit together) total of 18

15. d-orbital notes

16. Hydrogen Atomic Orbitals (cont.) Each energy sublevel relates to orbitals of different shape.

17. Image of orbitals

18. Electron Energy Level Notes Level 4: has 4 sublevels: s, p, d, and f 2 electrons in s 6 electrons in p 10 electrons in d 14 electrons in f (7 different orbitals for f) total of 32

19. s s s s p p p d d f 1 2 3 4 1 sublevel 1 orbital 2e - 2 sublevels 1+3=4 orbitals 2 + 6 = 8e - 3 sublevels 1+3+5=9 orbitals 2 + 6 + 10 = 18e - 4 sublevels 1+3+5+7=16 orbitals 2 + 6 + 10 + 14 = 32e -

20. Hydrogen Atomic Orbitals (cont.)

21. Electron Energy Level Notes The order that electrons fill up orbitals does not follow the logical order of all 1’s, then all 2’s, then all 3’s, etc. They follow the order found on pg. 156.

22. Order of Orbitals

23. Electron Energy Level Notes An easy way to remember this is to use the periodic table--it is arranged to show how these orbitals are filled.

24. Order of Orbitals—Periodic Table

25. Ground-State Electron Configuration The arrangement of electrons in the atom is called the electron configuration.electron configuration The aufbau principle states that each electron occupies the lowest energy orbital available.aufbau principle

26. Ground-State Electron Configuration (cont.) The Pauli exclusion principle states that a maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins.Pauli exclusion principle Hund’s ruleHund’s rule states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same energy level orbitals.

27. Electron Energy Level Notes Hund’s rule is used for filling orbitals with electrons. It states that only one electron will be put in each orbital of a sublevel until all of them are filled, and after that, they may be paired up until the sublevel is full.

28. Section 5-3 Ground-State Electron Configuration (cont.)

29. Section 5-3 Ground-State Electron Configuration (cont.) Noble gas notation uses noble gas symbols in brackets to shorten inner electron configurations of other elements.

30. Section 5-3 Ground-State Electron Configuration (cont.) The electron configurations (for chromium, copper, and several other elements) reflect the increased stability of half-filled and filled sets of s and d orbitals.

31. Section 5-3 Valence Electrons Valence electronsValence electrons are defined as electrons in the atom’s outermost orbitals—those associated with the atom’s highest principal energy level. Electron-dot structureElectron-dot structure consists of the element’s symbol representing the nucleus, surrounded by dots representing the element’s valence electrons.

32. Section 5-3 Valence Electrons (cont.)